Chem; Semester 1 Review-M2

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• If the polyatomic ion ends with "-ite" it will be an

"-ous acid"

v... symbol for wavelegth...

"nu" "lambda"

Orbital ("electron cloud")

("electron cloud")

Elemental Anions

(Main Group) "Pulled of the Table" anions/negatives ◦Have one particular negative charge

◦What is the equation that relates these values?

(e=hv)

DeBroglie and Schrodinger electron as wave 39 Louis DeBroglie (1924) suggested that es have wave properties so the Bohr model needs to be modified. Erwin Schrodinger (1926) devised an eqn that treated es moving around the nucleus as waves.

(electrons have properties of light and matter)

Bohr's Experiment

(excited state) energy into electrons photons out (ground state)

• Schrödinger Wave Equation (1926) - Used to determine the probability of finding the H electron at any given distance from the nucleus - finite # of solutions quantized energy levels - defines probability of finding an electron

(standardized) (5th theory of atom)

• Write what ion would form from each atom and then choose • K

For each of the following atoms, determine the ion each atom will form: b. K, Se, Kr

+1, -2, 0

For each of the following atoms, determine the ion each atom will form: a. Sr, Mg, Ba, Be

• Write what ion would form from each atom and then choose • Ca

• Write what ion would form from each atom and then choose • b

Photoelectric effect: (releases electrons)

- Radiation profiles of heated objects The emission of electrons from a material when light of certain frequencies shines on the surface of the material

• Flame tests are only 1 example of spectroscopy(test of diagnostic) • Different kinds of spectroscopy have different sensitivities.

- Test water for metal contaminate - Find composition of materials - Test hair, blood, and urine for poisons

What is alchemy? A medieval philosophy & early form of chemistry whose aims were...

- the transmutation of base metals into gold - the discovery of a cure for all diseases - the preparation of a potion that gives eternal life

Electromagnetic radiation (EMR), or light:

-- a form of energy that exhibits wavelike behavior as it travels through space.

Robert Millikan (1909): Conducted experiments to determine the charge -to-mass ratio, and ultimately the mass of the electron.

-- the electron is 9.109x10-31kg, about 2000x smaller than the positive piece -- all atoms are able to produce electrons and atoms are NOT indivisible Supports Thompson's plum putting model rather than creating his own

• Write what ion would form from each atom and then choose • Ci

-1

• Write what ion would form from each atom and then choose • S

-2

• Write what ion would form from each atom and then choose • P

-3

Quantum Numbers 3. Magnetic Q# (ml) →

-3, -2, -1, 0, 1, 2, 3 s=0 p=-1 - 1 d=-2 - 2 (CONFIRM THIS) f=-3 - 3

how electrons behave...

-actions of light

amplitude

-how high crest and trough are from middle line)

32. Acids must be handled with extreme care. You will be shown the proper method for diluting strong acids.....

. Always add acid to water, swirl or stir the solution and be careful of the heat produced, particularly with sulfuric acid.

Traditional System of Nomenclature

...used historically (and still some today) to name compounds w/multiple-charge cations (To use: 1. Use Latin root of cation. 2. Use -ic ending for higher charge; -ous ending for lower charge. 3. Then say name of anion, as usual.)

• 1 p = 1.007276 amu

1 n = 1.008665 amu 1 e- = 0.0005486 amu

1. What are the 4 signs of a chemical change?

1. Evolution of a gas; formation of a precipitate; heat/light/energy given off; unexpected color change

Finding an Empirical Formula from Experimental Data

1. Find # of g of each element. (If %, assume 100g) 2. Convert each g to mol. 3. Divide each "# of mol" by the smallest "# of mol." 4. Use ratio to find formula. A compound is 45.5% yttrium and 54.5% chlorine. Find its empirical formula.

what are the 4 steps of the Quantum Numbers?

1. Principal Q# (n) → 2. Angular Momentum Q# (l) → 3. Magnetic Q# (ml) → 4. Spin # (ms) →

1. Explain the concept of mole ratio as used in the reaction-stoichiometry questions.

1. The coefficient in the balanced equation represents the mole ratios of reactants to products. These ratios are used in all stoichiometry problems to convert from moles of one substance to mole of another substance.

1. State the Periodic Law.

1. The physical and chemical properties of the elements are periodic functions of their atomic numbers.

Rules for Parentheses Parentheses are used only when the following two condition are met:

1. There is a polyatomic ion present and... 2. There are two or more of that ion in the formula.

1. How do each of the following Sl prefixes compare to the base unit? a. kilo-

1. a. 1000 (103)

1. Use the periodic table to determine whether each of the following bonds would be IONIC, POLAR COVALENT, or NONPOLAR COVALENT: a. Co-Br

1. a. Ionic

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. a. sodium and iodine

1. a. Ionic; NaI

• 1 amu =....

1/12 the mass of a 12C atom

10. Compare and contrast accuracy and precision, and then classify the examples below. a. Lab data: Trial 1 = 152.35 oC, Trial 2 = 151.98 oC, Trial 3 = 152.54 oC b. Experimental result = 47.5% H2O, Theoretical value = 48.0% H2O

10. Accuracy is the closeness of a measurement to the true value of what is being measured. Precision describes the closeness, or reproducibility, of a set of measurements taken under the same conditions. Precision is repeatability of measurements, A Accuracy is closeness to the accepted value, B

10. Which would have the larger ELECTRON AFFINITY? a. Vanadium or nickel b. Silicon or germanium

10. a. Nickel b. Silicon

3. The atoms in a pure compound are the same atoms repeated over and over again, with...

100% of the material made from the same formula.

Centi;exponential factor

10^-2 1/100; 1 centimeter (cm)=0.01 m

Milli;exponential factor

10^-3 1/1000 1 millimeter (mm)=0.001 m

Micro;exponential factor

10^-6 1/1,000,000 1 micrometer (special u m)=1*10^-6m

Nano;exponential factor

10^-9 1/1,000,000,000 1 nanometer (nm)=1*1-^-9 m

Meter;exponential factor

10^0; 1 meter (m)

Kilo;exponential factor

10^3; 1,000 1 kilometer (km)=1000m

Mega;exponential factor

10^6; 1,000,000 1 megameter (Mm)=1*10^6m

11. Identify the most and the least electronegative elements on the periodic table.

11. The most electronegative elements are near the top right (excluding the noble gases) . The least electronegative elements are near the bottom left on the periodic table.

XII

12. What is the maximum electron capacity of each of the first 5 energy levels?

12. Use 2n2 (n = energy level) 2, 8, 18, 32, 50

13. How are the actual electron configurations of chromium and copper not as predicted? Why are they exceptions?

13. Cr = 1s22s2sp63s23p64s13d5 Cu = 1s22s2sp63s23p64s13d10 Chromium has a half-filled 4s sublevel and half-filled 3d sublevel instead of a full 4s sublevel and less than half-full 3d sublevel. This is because it is better to have two half-filled sublevels than one full and the other not full or half-full. Copper has a half-full 4s sublevel and a full 3d sublevel instead of a full 4s sublevel and almost full 3d sublevel. This is because it is better to have one half-filled sublevel and one full sublevel than one not full or half-full.

14. Classify each of the following as a DIRECT PROPORTION: a. As one value increases, the other also increases b. Density c. Graph is a hyperbola d. Product is a constant e. Frequency vs wavelength f. Graph is a straight line through (0,0)

14. Direct= A, B, F

1s^1

1: energy level s: shape ^1: electron number

In September of 1860, what happened?

1st International Congress of Chemist met in Germany • Settled on method for determining atomic mass (Stanislao Cannizzaro, Italy) Italian's method ◦Provided consistenay

Pauli Exclusion Principle

2 electrons in the same orbital must have opposite spins

2. Name the 7 diatomic molecules.

2. Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, Hydrogen (Br2 I2 N2 Cl2 H2 O2 F2)

2. How do the electron configurations within the same group of elements compare?

2. Generally, the configurations of the outermost electron shells of elements within the same group are the same.

2. Round each of the following measurements to the number of significant figures indicated. a. 67.029 g to three sig. figs.

2. a. 67.0

III

3. BALANCE the following equations: a. __NaOH + __ H2S __ Na2S + __HOH

3. a. 2 NaOH + H2S Na2S + 2 HOH

3. Identify the location of the: s-block; p-block; d-block; f-block

3. s-block consists of groups 1 & 2; p-block consists of groups 13-18; d-block consists of groups 3-12; f-block consists of the bottom 2 rows (the lanthanide and actinide series) of the periodic table

1.) Matter 2.) Pure Substances; seperated by chemical changes

3.) Elements; 1 capital letter, on the PT Compound; 2 or more capital letters, not on the PT

Quantum Numbers • Pauli Exclusion Principle also says - No two electrons in an atom can have the same..... - Each electron has a unique "address":

4 quantum numbers.

5. Define intermolecular forces. What kind of substance has these forces?

5. Intermolecular forces are bonds that form between atoms on different molecules. They are weaker than intramolecular forces, which are the forces that hold molecules together.

5. Which of the following changes are PHYSICAL: a. Melting an ice cube b. Burning paper c. Sharpening a pencil d. Dissolving sugar in water e. Wood is sawed in halfe f. Milk turns sour g. Decomposing hydrogen peroxide h. Melted butter solidifies in the refrigerator

5. Physical = A, C, D, E, H

5. Use the periodic table to identify the group numbers and period numbers of the following elements. a. carbon

5. a. 14, 2

5/9(F-32)

6. Which of the following properties are EXTENSIVE: a. mass. b. boiling point c. density d. color

6. Extensive= A

6. Identify which element from each pair would be MORE REACTIVE: a. S or Ba

6. a. Ba

Carbon (C): 12.0 g....

6.02 x 1023 C atoms

CaCO3 (antacid) 100.1 g:

6.02 x 1023 CaCO3 formula units

Iron (Fe): 55.9 g....

6.02 x 1023 Fe atoms

Sodium (Na): 23.0 g...

6.02 x 1023 Na atoms

NaF (preventative for dental cavities): 42.0 g

6.02 x 1023 NaF formula units

C8H10N4O2 (caffeine) 194.0 g:

6.02 x 1023 caffeine molecules

C6H12O6 (glucose) 180.0 g:

6.02 x 1023 glucose molecules

VII

7. Which of the following substances are HOMOGENOUS MIXTUREs: a. Coke b. iron (II) nitrate c. silver d. milk e. Lucky Charms f. fruit filled jello

7. Homogenous Mixture= A, D

7. Distinguish between the ground state and an excited state of an atom.

7. The ground state occurs when all of the electrons are in the lowest possible energy state. The excited state is an unstable, momentary condition that occurs if the "right" amount of energy is absorbed by an electron then it can "jump" to a higher energy level.

7. Which would have the smaller IONIZATION ENERGY? a. Scandium or zinc b. Aluminum or indium

7. a. Scandium b. Indium

VIII

Noble gases have how many valence electrons?

8 (stable, unreactive, low-energy)

8. What is an energy level? a sublevel? an orbital?

8. An energy level is how far away from the nucleus the electron has traveled. The sublevels contain the orbitals. Orbitals are regions around the nucleus where electrons are likely to be found.

8. Which would have the smaller ELECTRONEGATIVITY? a. Potassium or cesium b. Sulfur or tellurium

8. a. Cesium b. Tellurium

9. Which would have the larger ATOMIC RADIUS? a. Magnesium or strontium b. Yttrium or silver

9. a. Strontium b. Yttrium

9. List the 4 types of sublevels, the number of orbitals in each and the maximum number of electrons in each sublevel type.

9. s 1 orbital, 2 max. electrons p 3 orbitals, 6 max. electrons d 5 orbitals, 10 max. electrons f 7 orbitals, 14 max. electrons

F=1.8c+32

9/5c+32

Atomic Number

= Number of Protons

E = h = v=

= energy (Joules or J) = Planck's constant (6.626 x10-34 Js) = frequency (s-1) (E = hv)

% of element

= g element/molar mass of compound x 100 part over whole

law of definite proportions

A chemical compound contains the same elements in exactly the same proportions by mass reagardless of the size of the sample or source of the compound.

In a flame test, what are you testing?

A flame test is an analytical procedure used in chemistry to detect the presence of certain elements, primarily metal ions, based on each element's characteristic emission spectrum. The color of flames in general also depends on temperature; see flame color.

Mass Spectrophotometer

A gaseous sample is ionized by bombarding it with electrons in the lower part of the apparatus (not shown), producing positive ions.

alloy

A homogeneous mixture of metals

Bohr Model

A model resembling planets revolving around the sun in orbits, useful in visualizing the structure of atoms. orbits, set paths Increasing energy of orbits- farhter away from nucleus, the more powerful

Anion

A negatively charged ion, gained electrons

Cation

A positively charged ion, lost electrons

Energy level

A region of set energy around the nucleus where electrons are likely to be found moving.

Electron Dot Diagrams

A representation of the number of valence electrons in an atom, using dots placed around the symbol of an element

Block

A set of elements located in adjacent element groups. Designated s, p, d, f, according to the way electrons orbit in these groups

Orbital

A three-dimensional region around the nucleus that indicates the probable location of an electron, can hold 2 electrons each.

Theory:

A well-tested explanation for a broad set of observations Can not be proven! May be changed in the future to better explain new observations or experimnetal results

To find molecular formula...

A. Find empirical formula. B. Find molar mass of empirical formula. C. Find n = mm molecular mm empirical D. Multiply all parts of empirical formula by n. (How many empiricals "fit into" the molecular?)

19. phosphorous acid A. H3PO3 B. H3PO4 C. H3P D. H3PO2

A. H3PO3 Acids- polyatomic ion ending in ite

Stock System of nomenclature

A. To name, given the formula: 1.Figure out charge on cation. 2. Write name of cation. 3. Write Roman numerals in ( ) to show cation's charge. 4. Write name of anion.

4. Classify each of the following elements as a ACTINIDE: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

ACTINIDE 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

•A compound was found to have a molecular weight = 144g/mol. It contained 37.4% Al, 50.0% C, 12.6% H. Find E.F. and M.F.

AI2CI6H18

4. Classify each of the following elements as a ALKALINE EARTH METAL: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

ALKALINE EARTH METAL 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

4. Classify each of the following elements as a ALKALI METAL: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

ALKALINE METAL 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

16. HI A. iodic acid B. iodine acid C. hydrogen monoidide D. hydroiodic acid

Acids- binary D. hydroiodic acid

silver sulfide

Ag1+ S2- ◦Ag2S

2. aluminum hydroxide

Al(OH)3 Ionic- Single Charge Cation & Polyatomic Anion

27. aluminum oxalate

Al2(C2O4)3 Ionic- Single Charge Cation & Polyatomic Anion

** Warning: Reduce to lowest terms. Al3+ and O2- Ba2+ and S2- In3+ and Br1-

Al2O3 Ba2S2=BaS In1Br3=InBr3 ◦The "1" is redundant

Flame Tests for Certain Metals BORAX BEAD TESTS FOR CERTAIN METALS

All beads formed in the oxidizing flame

How are electrons behaving as particles?

All wavelengths of visible light are blurred together (rainbow) Gas sample gives only certain lines. This is like a fingerprint and can be used to ID a gas sample

38. Inserting and removing glass tubing from stoppers can be dangerous. Always lubricate glassware (tubing, thistle tubes, thermometers, etc.) before attempting to insert it in a stopper....

Always protect your hands with towels or cotton gloves when inserting glass tubing into, or removing it from, a rubber stopper. If a piece of glassware becomes "frozen" in a stopper, take it to your instructor for removal.

46. Never leave a lit burner unattended. Never leave anything that is being heated or is visibly reacting unattended....

Always turn the burner or hot plate off when not in use.

Ion

An atom or group of atoms that has a positive or negative charge.

Who was J.A.R. Newlands (1864)?

Arranged the 62 known elements into groups of seven according to increasing atomic mass. He proposed that an eighth element would then repeat the properties of the first element in the previous group. Law of Octaves ◦Repetivie pattern of seven

Electron configuration

Arrangement of electrons in the orbitals of an atom.

Intro to the Periodic Table

Arranges the elements in order according to their properties.

Average Atomic Mass ►weighted average of all nautrally occuring isotopes ►on the Periodic Table ►round to 2 decimal places

Avg. Atomic Mass = (mass)(%) + (mass)(%)/100

18. vanadium (V) sulfide A. V5S B. V2S5 C. V5SO4 D. V2(SO5)5

B. V2S5 Ionic- Multi Charge Cation & Elemental Anion

13. HClO2 A. chloric acid B. chlorous acid C. hypochlorous acid D. hydrochlorous acid

B. chlorous acid Acids- polyatomic ion ends in ite

11. FeI2 A. iron diiodide B. iron (II) iodide C. iron (I) iodide D. iron iodide

B. iron (II) iodide Ionic- Multi Charge Cation & Elemental Anions

Albert Einstein Saves the Day! • Electromagnetic radiation can be...

BOTH wave and particle.

BaF2

Barium Fluoride

BaO

Barium Oxide

What Rutherford Expected... ► The alpha particles to pass through without changing direction ► The positive charges were spread out evenly. Alone there was not enough to stop the alpha particles from passing straight through the material

Because, he thought the mass was evenly distributed in the atom.

Who reacts most like who? ⭘ Fluorine and Br or Ne?

C+273

► 12C atom = 1.992 × 10-23 g

C-12 chosen as arbitrary standard

17. cerium (I) perchlorate A. CsClO4 B. CsClO C. CeClO4 D. CeClO

C. CeClO4 Ionic- Multi Charge Cation & Polyatomic Anion

12. NH4NO3 A. ammonium nitride B. nitrogen nitrite C. ammonium nitrate D. diammonium nitrogenoxide

C. ammonium nitrate Ionic- Polyatomic Cation & Polyatomic Anion

14. Ag3PO4 A. silver (II) phosphate B. silver (II) phosphite C. silver phosphate D. silver phosphite

C. silver phosphate Ionic- Single Charge Cation & Polyatomic Anion

sucrose C12H22O11; emp. form-

C12H22O11

butane C4H10; emp. form-

C2H5

propane C3H8; emp. form-

C3H8

octane C8H18; emp. form-

C4H9

naphthalene C10H8; emp. form-

C5H4

1. A carbon/hydrogen compound is 7.7% H and has a molar mass of 78 g. Find its molecular formula.

C6H6

carbon tetrachloride

CCI4

glucose C6H12O6; emp. form-

CH2O

Cyanide

CN⁻

carbon dioxide

CO2

Al2(CO3)3

CO3 2- is a ion and there are three of them.

Carbonate

CO₃ ²⁻

Carbon Monoxide

cadmium iodide

Cd2+ I1- ◦CdI2

⭘What are some chem/physical prop?

Chem: flammability, acidity/basicity, corrosion, reactivity, toxicity Phys: color, mpt, bpt, shape, texture, density, mass, brittleness, tensile strength

5. Which of the following changes are CHEMICAL: a. Melting an ice cube b. Burning paper c. Sharpening a pencil d. Dissolving sugar in water e. Wood is sawed in halfe f. Milk turns sour g. Decomposing hydrogen peroxide h. Melted butter solidifies in the refrigerator

Chemical = B, F, G

•HClO2

Chlorous acid

Chlorite

ClO₂ ⁻

Chlorate

ClO₃ ⁻

Perchlorate

ClO₄ ⁻

cobalt (III) chloride

Co3+ CI1- -> CoCI3

7. Which of the following substances are PURE COMPOUNDs: a. Coke b. iron (II) nitrate c. silver d. milk e. Lucky Charms f. fruit filled jello

Compound= B

Chemical Changes

Convert one substance into a NEW substance with completely NEW properties (through a chem REACTION). Describe a substance's ability to REACT with other substances. For example...? • For Example: ◦a) Hydrogen and oxygen react to produce water ◦H2 and O2 are called the reactants ◦H2O is called the product ◦b) iron and oxygen react to produce rust

CuBr

Copper bromide? -> Copper(I) Bromide • Cu? Br-1 ◦Cu+1

CuBr2

Copper bromide? -> Copper(II) Bromide • Cu? Br2- ◦Cu2+

15. SeI6 A. selenium (VI) iodide B. selenium iodide C. selenium iodine D. selenium hexaiodide

Covalent- both Nonmetals D. selenium hexaiodide

cesium fluoride

CsF

Who reacts most like who? ⭘ Iron and Cu or sulfur?

copper

Acetate

C₂H₃O₂ ⁻

Physical Changes

DOES NOT involve a change in the identity of the substance. For example...? Basically a change in any phys prop... BUT BE CAREFUL! Sometimes easily reversible... BUT NOT ALWAYS! ‣ Crushing chalk, bending wire, melthing ice, cutting paper Can be observed or measured WITHOUT changing the chemical composition of the substance. For example...?

22. Dress properly for working in the laboratory. Long hair, dangling jewelry, and loose or baggy clothing are hazardous. Long hair must be tied back....

Dangling jewelry and loose clothing must be secured. Shoes must completely cover the foot. No sandals allowed.

10 -

Deca

anhydrous salt Uses:

Desiccants: in leather goods, electronics, vitamins ◦Soaks up a lot of water

48. Heated metals and glass remain very hot for a long time. They should be set aside to cool and picked up with caution. Use tongs or heat- protective gloves if necessary....

Determine if an object is hot by bringing the back of your hand close to it prior to touching it.

n2=# of orbitals per level • 2n2 rule: ....

Determine to total number of electrons at each level

2 -

N2O5

Dinitrogen pentaoxide

Ionic Radius

Distance from the center of an ion's nucleus to its outermost electron

_________________________________________________observed that elements listed in order of atomic mass showed regularly (or periodically) repeating properties. He announced his Periodic Law in 1869 and published a list of known elements in a tabular form. He had the courage to leave gaps where the Periodic Law did not seen to fit, predicting that new elements would be discovered to fill them."

Dmitri Mendeleyev (1834-1907)

47. You will be instructed in the proper method of heating and boiling liquids in test tubes...

Do not point the open end of a test tube being heated at yourself or anyone else.

45. Exercise extreme caution when using a gas burner. Take care that hair, clothing, and hands are at a safe distance from the flame at all times....

Do not put any substance into the flame unless specifically instructed to do so. Never reach over an exposed flame. Ignite gas (or alcohol) burners only as instructed by the teacher.

5. Do not eat food, drink beverages, or chew gum in the laboratory...

Do not use laboratory glassware as containers for food or beverages.

Pure Substances Include...

ELEMENTS ◦Fe, N2, S8, U COMPOUNDS ◦H2O, NaCI, HNO3

Particles in the Atom Subatomic particles

Electron: -e -1 1/1840 = 0 9.11*10^-28

Atom (no charge) : Protons =

Electrons

Aufbau Principle

Electrons fill an atom in order of increasing energy level, starting at the lowest level.

Valence electron

Electrons in the outermost energy level of an atom. They are involved in bonding and affect the reactivity of an atom.

valence electrons

Electrons on the outermost energy level of an atom important during chemical bonding

7. Which of the following substances are PURE ELEMENTs: a. Coke b. iron (II) nitrate c. silver d. milk e. Lucky Charms f. fruit filled jello

Element= C

famous people...

Es, Fm, Md, No, Lr, Rf, Bh

hydrate examples:

Examples: CuSO4 . 5 H2O BaCl2 . 2 H2O Na2CO3 . 10 H2O FeCl3 . 6 H2O

covalent compounds=

FORGET CHARGES!

Noble gas atoms have..... They are stable, low-energy, and unreactive.

FULL valence shells. 8 e=stability

describe Dutch Periodic Table

Families/blocks, circular order to different elements

Who reacts most like who? ⭘ Sodium and Fr or Mg?

place names...

Fr, Po, Ge, Ga, Eu, Am, Cf, Sc

4. Classify each of the following elements as a GENERAL NONMETAL: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

GENERAL NONMETAL 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

Condensation

Gas to liquid

diatomic elements

H2, O2, Br2, F2, I2, N2, CI2

water

H2O

25. hydrosulfuric acid

H2S Acid- binary

4. Classify each of the following elements as a HALOGEN: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

HALOGEN 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

1. acetic acid

HC2H3O2 Acid- polyatomic ion ending in -ate

NO2 -1 ion = nitrite Becomes

HNO2 = nitr ous acid

NO3 -1 ion = nitrate Becomes

HNO3 = nitr ic acid

28. nitric acid

HNO3 Acid- Polyatomic ion ending in -ate

Atomic radius

Half the distance between the nuclei of two like atoms

40. When removing an electrical plug from its socket, grasp the plug, not the cord....

Hands must be completely dry before touching an electrical switch, plug, or outlet.

7 -

Hepta

frequency,v, units?....

Hertz (Hz or 1/S)

7. Which of the following substances are HETEROGENOUS MIXTUREs: a. Coke b. iron (II) nitrate c. silver d. milk e. Lucky Charms f. fruit filled jello

Heterogeneous Mixture= E, F

6 -

Hexa

names related to element properties... Latin Descriptions

Hg, Xe

crest

Highest point of a wave

35. Take great care when transferring acids and other chemicals from one part of the laboratory to another....

Hold them securely and walk carefully.

Mixtures: there are 2 types -______________________ -_______________________

Homogeneous Heterogeneous

•HBr

Hydrobromic acid

• HCl • Chlorine is the second element • Chlorine becomes "chloric"

Hydrochloric acid

• HF • fluorine is the second element • fluorine becomes "fluoric"

Hydrofluoric acid

Have No Fear Of Ice Cold Beer

Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, Bromine (hydrogen, nitrogen, fluorite, oxygen, iodine, chlorine, and bromine)

•H2S

Hydrosulfuric acid

Hydronium

H₃O⁺

3. Classify each of the following as a property of IONIC bonding: a. Network of particles b. Sea of electrons c. Soluble in water d. brittle e. Poor conductors when solid f. malleable g. Good conductors when molten or aqueous h. Reflect light

IONIC 3. a. Ionic b. Metallic c. Ionic d. Ionic e. Ionic f. Metallic g. Ionic h. Metallic

21. Contact lenses should not be worn in the laboratory. If you choose to wear contact lenses while working in the lab, you do so at your own risk. Acrylic nails are extremely flammable....

If you choose to wear acrylic nails during a lab activity, you do so at your own risk.

Evidence of a Chemical Change

If it's hard to reverse, this is also a sign that it can be a chemical change During any physical or chemical change, mass is neither created or destroyed! This is the law of conservation of mass. Example? • transfer of energy (heat, light, sound) • unexpected color change • generation of a gas (foaming, bubbles, odor) • unexpected formation of a solid (called a "precipitate")

2. Follow all written and verbal instructions carefully.....

If you do not understand a direction or part of a procedure, ask your instructor before proceeding.

lanthanides:

In f-block elements 58-71

actinides

In f-block elements 90-103

Electronegativity

Indicates the relative ability of an atom to attract the bonding electrons of another atom

6. Which of the following properties are INTENSIVE: a. mass. b. boiling point c. density d. color

Intensive= B, C, D

14. Classify each of the following as an INVERSE PROPORTION: a. As one value increases, the other also increases b. Density c. Graph is a hyperbola d. Product is a constant e. Frequency vs wavelength f. Graph is a straight line through (0,0)

Inverse= C, D, E

Single-Charge Cations

Ionic Compounds (cation/anion combos)

20. calcium cyanide A. CaCN B. Ca2CN C. CaCN2 D. Ca(CN)2

Ionic- Single Charge Cation & Polyatomic Anion D. Ca(CN)2

FeO

Iron oxide? -> Iron(II) Oxide ◦Fe? O2- ‣ Fe2+

Fe2O3

Iron oxide? -> Iron(III) Oxide • Fe? Fe? O2- O2- O2- ◦Fe+3 Fe+3

Scientific Method

It involves collecting evidence (data), interpreting it (analysis) and using it to draw logical conclusions about reality.

K-273

Explain the Cathode Ray Tube Experiment Thomson Model of the Atom

Key points. J.J. Thomson's experiments with cathode ray tubes showed that all atoms contain tiny negatively charged subatomic particles or electrons vacuum tube - all the air has been pumped out. Passing an electric current makes a beam appear to move from the negative to the positive end.

units:

L, dm^3, mL, cm^3

4. Classify each of the following elements as a LANTHANIDE: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

LANTHANIDE 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

23. Protect your clothes....

Lab aprons should be worn during laboratory activities.

Noble gases were not known at the time. Newland's referred to his arrangement as the __________________.

Law of Octaves

Electronegativity=

Linus Pauling 1901 - 1994

Vaporization

Liquid to gas

long wavelength(you should know the symbol)=

Low frequency

trough

Lowest point of a wave

Mega; unit abbreviation

3. Classify each of the following as a property of METALLIC bonding: a. Network of particles b. Sea of electrons c. Soluble in water d. brittle e. Poor conductors when solid f. malleable g. Good conductors when molten or aqueous h. Reflect light

METALLIC 3. a. Ionic b. Metallic c. Ionic d. Ionic e. Ionic f. Metallic g. Ionic h. Metallic

4. Classify each of the following elements as a METALLOID: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

METALLOID 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

MgI2

Magnesium Iodide

1. Principal Quantum Number

Major energy levels Size of the orbital

Island Diagram

Mass (g) Mole (mol) Particle (molecule, formula unit, etc.) Atoms (At.)

____________ are combinations of two or more kinds of matter each of which retains its own _______________ and ____________________ ; can be separated into its components by physical means.

Mixtures composition, properties

1 -

Mono

dinitrogen trioxide

N2O3

30. dinitrogen trioxide

N2O3 Covalent

2. A compound has 26.33 g nitrogen, 60.20 g oxygen, and molar mass 92 g. Find molecular formula.

N2O4

7. Be prepared for your work in the laboratory. Read all procedures thoroughly before entering the laboratory......

NEVER FOOL AROUND in the LABORATORY. HORSEPLAY, PRACTICAL JOKES, AND PRANKS ARE DANGEROUS AND PROHIBITED.

(NH4)2SO4

NH4 1+ is a ion and there are two of them; SO4 2- is a ion but there is only one of it.

Ammonium

NH₄+

26. nitrogen triiodide

NI3 Covalent

Covalent start with

NMs contain two types of nonmetals

Co(NO3)2

NO3 1- is a ion and there are two of them

NaNO3

NO31- is a ion, but there is only one of it.

4. Classify each of the following elements as a NOBLE GAS: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

NOBLE GAS 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

Any-old-value of energy to be absorbed or released is _______ ______. This explains the lines of color in an emission spectrum.

NOT OK. (certain sizes)

Nitrite

NO₂ ⁻

Nitrate

NO₃ ⁻

To write an ionic compound's formula, we need: 1. the two types of ions 2. the charge on each ion Na1+ and F1- Ba2+ and O2- Na1+ and O2- Ba2+ and F1-

NaF BaO Na2O BaF2

11. Always work in a well-ventilated area. Use the fume hood when working with volatile substances or poisonous compounds....

Never place your head in the fume hood.

33. Handle flammable hazardous liquids over a pan to contain spills....

Never dispense flammable liquids anywhere near an open flame or source of heat.

6. Perform only those experiments authorized by the instructor.....

Never do anything in the laboratory that is not called for in the laboratory procedure or by your instructor. Carefully follow all instructions, both written and oral. Unauthorized experiments are prohibited.

19. When using sharp instruments, always carry with tips and points pointing down and away. Always cut away from your body.....

Never try to catch falling sharp instruments. Grasp sharp instruments only by the handles.

41. Examine glassware before each use; never use chipped or cracked glassware....

Never use dirty glassware.

29. Never use mouth suction to fill a pipet. Use a rubber bulb or pipet pump...

Never use pipets for uses other than those intended.

4. nickel (II) hypochlorite

Ni(ClO)2 Ionic- Multi Charge Cation & Polyatomic Anion

NI3

Nitrogen Triiodide

Pauli's Exclusion Principle

No more than two electrons (with opposite spin) can occupy any given orbital.

3. Never work alone......

No student may work in the laboratory without an instructor present.

9 -

Nona

12. Be alert and proceed with caution at all times in the laboratory...

Notify the instructor immediately of any UNSAFE conditions that you observe.

•P& N in...

Nucleus (more protected)

Atomic Mass=

Number of Protons + Number of Neutrons

Co(OH)2

OH1- is a ion and there are two of it.

NaOH

OH1- is a ion but there is only one of it.

Hydroxide

OH⁻

The Scientific Method Steps do not have to occur in a specific order ; some steps may occur more than once!

Observations: example: you pull a chain on a lamp, but the light does not go on Hypothesis: a proposed explanation for the observations Example? Experiments: a procedure used to test the hypothesis Example? A model: (perhaps computerized) can be used if the experiment would be difficult or impossible-example: atoms or molecules Theory: A well-tested explanation for a broad set of observations Can not be proven! May be changed in the future to better explain new observations or experimnetal results Scientific Law: a concise statement summarizing the results of many observations and experiments Only states a relationship; does not try to prove an explanation (theory)!

8 -

Octa

Newlands Law of _____________

Octaves (1863)

S orbital EVERY energy level

Only 1 on each level

Hund's Rule

Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin

Peroxide

O₂ ²⁻

3. phosphorus trifluoride

PF3 Covalent

Phosphite

PO₃ ³⁻

Phosphate

PO₄ ³⁻

homogeneous: (or solution) (type of mixture)

Particles are microscopic; sample has same composition and properties throughout: evenly mixed

The multiple-charge cations are: (Colored red; essentially the majority of the D block)

Pb, Sn, and the transition elements (but - of course! - not Ag, Cd, or Zn) In some cases, 1+...in others 2+

5 -

Penta

•HClO4

Perchloric acid

H3PO4

Phosphoric acid

•H3PO4

Phosphoric acid

37. Never handle broken glass with your bare hands. Use a brush and dustpan to clean up broken glass.....

Place broken glass in the designated glass disposal container.

Thomson's Model

Plum pudding model

KCI

Potassium Chloride

Max Planck (1900):

Proposed that amounts of energy are quantized (certain quantities allowed)

Oil Drop Experiment

Robert Millikan, suspended oil drops between charged plates, shot x-rays that put an electron on them, determined the smallest increment of charge difference needed to suspend the drops, and determined the charge on one electron A drop of oil was placed in a cylinder with negative and positive plates, the drops were charged using an x-ray. Different waves of xrays let the drops fall at different rates. Determined that the mass of the electron is 9.10 x 10^-28 by Robert Milikan

2. A ruthenium/sulfur compound is 67.7% Ru. Find its empirical formula.

Ru2S3

Rutherford's Apparatus

Rutherford received the 1908 Nobel Prize in Chemistry for his pioneering work in nuclear chemistry.

elements known to the ancients...

S, Sn, C, Cu Sulfur/Tin; stuff you can dig out of the ground

Sulfite

SO₃ ²⁻

Sulfate

SO₄ ²⁻

Chemistry by Accident! Just because an experiment doesn't go as expected, doesn't mean it's a failure...

Saccharin Sticky Notes Polytetra-fluoroethylene Vulcanized Rubber

Quantum Model (#5) • Used calculations to devise and solve math equations describing behavior of electron • Like Bohr, quantum model restricts energy of electrons to certain values • Unlike Bohr, quantum model does not specify the path who did?^

Schrodinger (1887-1961)

Purpose

Science is a hands-on laboratory class. You will be doing many laboratory activities which require the use of hazardous chemicals. Safety in the science classroom is the #1 priority for students, teachers, and parents. To ensure a safe science classroom, you must, at ALL times, follow the list of rules in this contract. You must agree to follow this contract and both you and a parent, or guardian, must sign one copy of the contract before you can participate in the laboratory. Another copy is to be kept in your science notebook.

-James Randi

Science is best defined as a careful, disciplined, logical search for any and all aspects of knowledge about the universe, obtained by examination of the best available evidence and always subject to correction and improvement upon discovery of better evidence. -James Randi

describe the periodic pyramid

Seperates elements into the blocks; cut it out and make a three demensional pyramid

14. Labels and equipment instructions must be read carefully before use...

Set up and use the prescribed apparatus as directed in the laboratory instructions or by your instructor.

Molecular Formula

Shows the true number and type of atoms in a molecule

tin (II) oxide

Sn2+ O2- -> SnO

tin (IV) oxide

Sn4+ O2- -> Sn2-O4+ -> SnO2

NaF

Sodium Fluoride

Na2O

Sodium Oxide

13. Dispose of all chemicals properly. Never mix chemicals in sink drains. Sinks are to be used only for water and those solutions designated by the instructor...

Solid chemicals, metals, filter paper, and all other insoluble materials are to be disposed of in the proper waste containers, not in the sink. Check the label of all waste containers twice before adding your chemical to the container.

strontium fluoride

SrF2

p orbital NOT 1st energy level

Starts at 2nd energy level 3 on each level

d orbital NOT 1st or 2nd energy level

Starts at 3rd energy level 5 on each level

f orbital NOT 1st 2nd or 3rd energy level

Starts at 4th energy level 7 on each level

Octet Rule:

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

describe Stowe's Periodic Table

Stowe's PT is weird, the s block makes this pseduo backbone while all the others stack on top of each other (P,d,f surround it)

H2SO3

Sulfurous acid

4. Classify each of the following elements as a TRANSITION METAL: a. Potassium b. Phosphorus c. Arsenic d. Einsteinium e. Europium f. Xenon g . Zirconium h. Palladium i. Bromine j . Polonium k. Beryllium l. Rubidium

TRANSITION METAL 4. a. Alkali Metal b. General Nonmetal c. Metalloid d. Actinide e. Lanthanide f. Noble Gas g . Transition Metal h. Transition Metal i. Halogen j . Metalloid k. Alkaline Earth Metal l. Alkali Metal

27. Check the label on chemical bottles twice before removing any of the contents....

Take only as much chemical as you need.

3. A 17.40 g sample of a technetium/oxygen compound contains 11.07 g of Tc. Find the empirical formula.

Tc2O7

4 -

Tetra

mythology-related names...

Th, Pm, Ta, Ti, P

Niels Bohr 4th Model Atom Electrons as particles

The Planetary Model of the Atom

Electronegativity (unit less)

The ability of an atom in a molecule to attract shared electrons to itself.

Ionization energy

The amount of energy required to remove an electron from each of one mole of gaseous atoms.

Group

The columns of the periodic table. There are 18 groups in total on the periodic table

molar mass:

The mass of one mole of a substance

Visible Spectrum of Light

The part of the electromagnetic spectrum that can be seen. Visible light makes up only 35 percent of natural sunlight. violet(short frequency) is bent most and red least

HNO3

The polyatomic ion is nitrate Nitric acid

HNO2

The polyatomic ion is nitrite Nitrous acid

Periodic law

The principle that states that chemical properties of the elements are periodic functions of their atomic numbers

26. All chemicals in the laboratory are to be considered dangerous. Do not touch, taste, or smell any chemicals unless specifically instructed to do so...

The proper technique for smelling chemical vapors will be demonstrated to you.

Periods

The rows of the periodic table. Corresponds to the energy level of the s and p blocks.

Periodic trend

ThePeriodic trend gradual change of any property in the elements across a period or down a group.

20. Any time chemicals, heat, or glassware are used, students must wear laboratory goggles.....

There are no exceptions to this rule.

Sub-level

There are four possible sublevels: s, p, d, f

3 -

Tri

covalent

Use Greek prefixes to indicate how many atoms of each element, but don't use "mono" on first element.

Iron Ring

Used to support funnels and wire gauze/beakers

29. vanadium (V) oxide

V2O5 Ionic- Multi Charge Cation & Elemental Anion

foreign languages... Latin-Based

W, Fe, Au, Ag, Pb, Sb, Cu, Na, K

15. Keep hands away from face, eyes, mouth, and body while using chemicals or preserved specimens....

Wash your hands with soap and water after performing all experiments. Clean (with soap), rinse, and wipe dry all work surfaces and apparatus at the end of the experiment. Return all equipment clean and in working order to the proper storage area.

Law of Multiple Proportions

When two different compounds have same two elements, equal mass of one element results in integer multiple of mass of other. (if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers)

8. Observe good housekeeping practices....

Work areas should be kept clean and tidy at all times. Bring only your laboratory instructions, worksheets, and/or reports into the work area. Other materials should be stored in the classroom.

Contributions of alchemists: Information about elements: - the elements mercury, sulfur, and antimony were discovered - XXX Develop lab apparatus /.... - alchemists learned... - developed... - new...

XXX XXX XXX XXX - properties of some elements procedures / experimental techniques how to prepare acids several alloys glassware

The Greeks History of the Atom ► Not the history of atom, but.... ► In 400 B.C the Greeks tried... (chemicals) and broke them.... ► Democritus and Leucippus....

XXX XXX the idea of the atom to understand matter down into earth, water, fire, and air. Greek philosphores

Calculating Molar Mass X Add together the molar mass from each... X If there are subscripts in the compound, there are more than 1 of that atom, and so the molar... X The total answer is how many grams one...

XXX individual atom in the compound mass for that atom should be multiplied by the subscript number mole of the compound weighs

•A compound is 53.5%Xe and 46.5 % F what is the E.F. and the M.F.? •Given the Molecular Formula molar mass = 245 g

XeF6

16. Experiments must be personally monitored at all times....

You are assigned a laboratory station at which to work. Do not wander around the room, distract other students, or interfere with the laboratory experiments of others.

zinc phosphide

Zn2+ P3- ◦ Zn3P2

‣ Atom:

a basic builder block of matter • 118 different kinds

Scientific Law:

a concise statement summarizing the results of many observations and experiments Only states a relationship; does not try to prove an explanation (theory)!

to get back to ground state, excited electrons decay and emit....

a photon

Experiments:

a procedure used to test the hypothesis Example?

Hypothesis:

a proposed explanation for the observations Example?

Abbreviated Electron Configuration

a way of writing the electron configuration of an atom that uses a nearby, prior noble gas (with a full octet) as a starting point

Consequences for inadequate lab preparation will be:

a) For the 1st occurrence: a 50% point deduction for the lab report. Students will complete the lab quiz for the experiment. Students receive a Lab Safety Referral and must return the Lab Safety Referral with a parent signature. b) For the 2nd and 3rd occurrences: no credit for the lab report but student will take the lab quiz. Students receive a Lab Safety Referral and must return it with a parent signature. c) For the 4th occurrence: no credit for either the lab report or lab quiz. Students will be referred to the Dean's office during class time. Students receive a Lab Safety Referral and must return it with a parent signature. d) For the 5th occurrence and additional occurrences: no credit for either the lab report or lab quiz. Students will be referred to the Principal's office during class time. Students receive a Lab Safety Referral and must return it with a parent signature.

Students must adequately prepare for all experiments by:

a) Reading the entire experiment procedure before the scheduled lab period, b) Completing the theoretical background or prelab questions with correct citations, and c) Preparing any data collection tables described.

For each of the following sets of atoms, list them in order of increasing atomic radius: a. Sr, Mg, Ba, Be

a. Be, Mg, Sr, Ba

Rank the IONS in order of increasing ionic radius. a. Sr, Mg, Ba, Be

a. Sr +2, Mg +2, Ba +2, Be +2

Electromagnetic radiation is...

absorbed by matter only in whole #'s of photons.

• starts with H-

acid

Students will not receive credit for either the lab report or lab quiz for the experiment....

after receiving a Lab Safety Referral, in either situation above.

Chemistry affects all aspects of life and most natural events because...

all living and nonliving things are made of matter

2. Mass is the...

amount of matter in an object, and its typical unit is the gram.

hydrate:

an anhydrous salt with the water attached

The science lab is NOT...

an athletic field or a shopping mall.

Electronegativity-• if there is a bond where atoms are sharing electrons ◦How much is each atom is going to pull________________________________ ‣ Are they going to share evenly, or unevenly

an electron towards itself

anhydrous salt:

an ionic compound (i.e., a salt) that attracts water molecules and forms loose chemical bonds with them; symbolized by MN

anhydrous salt

anion:________ cation:_______

anion: a (-) ion cation: a (+) ion

3. There is NO elevator. 4. All equal rooms must have one e- before....

any doubling up.

• salt:

any ionic compound

• matter:

anything having mass and volume

INTENSIVE PROPERTIES

are INdependent of the amount of matter present ◦For Example: ‣ Bp, mp, density, malleability, ductility, color

"Hotel Atom" Analogy Rules 1. Max. of two e- per room (i.e., orbital). 2. Not all rooms..... The best rooms fill up first!!! s orbital (suite) p orbital (party) d orbital (dorms) 3. There is NO elevator. 4. All equal rooms must have one e- before any doubling up. f orbital (frat)

are equal.

•Electrons are in regions (exposed/absorby clouds)...

around nucleus (•This makes electrons able to absorb energy)

25. If a chemical should splash in your eye(s) or on your skin, immediately flush with running water from the eyewash station, sink, or safety shower (for a significant chemical spill) for....

at least 20 minutes. Notify the instructor immediately.

What Rutherford got... richocheting alpha particles Explanation of Alpha-Scattering Results

atom wasn't as it appeared

number of protons # of protons determines kind of atom= number of electrons in a neutral atom= the number of protons + neutrons=

atomic number atomic number mass number

which would be larger, the original atom or hte ion.

atoms=smaller ions-larger

1. How do each of the following Sl prefixes compare to the base unit? b. centi-

b. 0.01 (10-2)

2. Round each of the following measurements to the number of significant figures indicated. b. 0.15 L to one sig fig.

b. 0.2 L

5. Use the periodic table to identify the group numbers and period numbers of the following elements. b. argon

b. 18, 3

3. BALANCE the following equations: b. __Al + __Fe(NO3)2 ___Al(NO3)3 + ___Fe

b. 2 Al + 3 Fe(NO3)2 2 Al(NO3)3 + 3 Fe

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. b. NaCl

b. Ionic; Sodium chloride

Rank the IONS in order of increasing ionic radius. b. Cs, Po, Rn, Pb

b. K+1, Se2-, Kr

1. Use the periodic table to determine whether each of the following bonds would be IONIC, POLAR COVALENT, or NONPOLAR COVALENT: b. S-O

b. Polar Covalent

6. Identify which element from each pair would be MORE REACTIVE: b. Rb or Y

b. Rb

For each of the following sets of atoms, list them in order of increasing atomic radius: b. Cs, Po, Rn, Pb

b. Rn, Po, Pb, Cs

Students must bring the Lab Safety Referral to parents for a signature. Students will not...

be allowed to remain in the lab if they engage in unsafe behavior.

and I mITE

be nauseOUS

• When light travels thru space, it...

behaves like waves.

• When light interacts with matter, it....

behaves more like a stream of particles. (dual nature of light)

• More layers of electrons=___________________________________________________________________ ◦The electrons that are outer, or hte valence electrons are easier to reomive, comapred ot hte ones closer to thenucleus that will make when we think about our trends, how it harder to be removed • does the layers of our eelctrons influecne the trends were talking about? ◦Size-makes them bigger ‣ Fluffer, more layers • Attraction, attraciton is weaken b/c of that shileding.

bigger shield that detracts from the connection between the electrons and the nucleus

check slides 57-66

bleeop bloop

Structure of the Atom There are two regions The nucleus Electron cloud With protons and neutrons Positive charge Almost all the mass maths helpstick • The region where the electron can be found • Negative charge • Almost all the volume of an atom

bleep bloop

https://classroom.google.com/c/MTI3OTUzNDIzOTE1/m/MjM3NjM5NzQ0NDYx/details

bleep bloop

ur mum

bleep bloop

Atoms-individual building...

blocks of matter pieces of elements from table

hello

bloop bleep

distillation

boiling off one substance while a second substance with a higher bp stays behind

Chemical properties can only be observed

by performing a chemical reaction or otherwise changing the chemical composition of the substance.

Centi; unit abbreviation

c =v(symbol for wavelength)

c = speed of light (3 x 10^8 m/s) v = frequency (s^-1) (symbol for wavelength) = wavelength (m)

For each of the following atoms, determine the ion each atom will form: c. F, S, Al

c. -1,-2,+3

1. How do each of the following Sl prefixes compare to the base unit? c. mega-

c. 1000000 (106)

5. Use the periodic table to identify the group numbers and period numbers of the following elements. c. barium

c. 2, 6

2. Round each of the following measurements to the number of significant figures indicated. c. 52.8005 mg to five sig figs.

c. 52.801

For each of the following sets of atoms, list them in order of increasing atomic radius: c. Rb, F, Ca, Si

c. F, Si, Ca, and Rb

Rank the IONS in order of increasing ionic radius. c. Rb, F, Ca, Si

c. F-1, S2-, Al3+

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. c. Cu3(PO4)2

c. Ionic; Copper (II) phosphate

1. Use the periodic table to determine whether each of the following bonds would be IONIC, POLAR COVALENT, or NONPOLAR COVALENT: c. H-H

c. Nonpolar Covalent

6. Identify which element from each pair would be MORE REACTIVE: c. N or O

c. O

example of a Photoelectric Generator

calculator

Ion (________) : Protons > Electrons Ion (________) : Electrons > Protons

cation anion

criss-cross rule:

charge on cation / anion "becomes" subscript of anion / cation

The arrangement of the periodic table gives us insight into many of the expected ________________________________________________________________________.

chemical and physical properties of the elements

• Pure substances have a ____________ ____________.

chemical formula

Pure Substances can only be _______________ seperated (elements and compounds)

chemically

Because isotopes are chemically identical (same electronic structure), they cannot be separated by.............

chemistry. So Physics separates them by diffusion or centrifuge (mass spectrograph is too slow)

9. Keep aisles...

clear.

23. CoBr2

cobalt (II) bromide Ionic- Multi Charge Cation & Polyatomic Anion

falling from different levels....

color

Carbon dioxide

compound

18. Know what to do if there is a fire drill during your laboratory period;....

containers must be closed, gas valves turned off, fume hoods turned off, and any electrical equipment turned off.

white light=

continuum spectrum

• Starts with nm-

covalent

1. How do each of the following Sl prefixes compare to the base unit? d. micro-

d. 0.000001 ( 10-6)

2. Round each of the following measurements to the number of significant figures indicated. d. 3.17497 mol to three sig figs.

d. 3.17 mol

5. Use the periodic table to identify the group numbers and period numbers of the following elements. d. chromium

d. 6, 4

6. Identify which element from each pair would be MORE REACTIVE: d. S or Br

d. Br

1. Use the periodic table to determine whether each of the following bonds would be IONIC, POLAR COVALENT, or NONPOLAR COVALENT: d. Na-I

d. Ionic

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. d. calcium and sulfur

d. Ionic; CaS

Electronegativity ⭘Down a group-

decreases.

◦Properties:

describe the matter ‣ What it looks like, smells like; its mass, temp., etc. ‣ how it behaves

electron configuration:

descrption of where electrons are located

• Valence Electrons ◦What are valence electrons? ‣ Outer shell electrons which consist of the s and p electrons • In total, you can have 8 ◦2s electrons and 6 p electrons ‣ Valence electrons _______________________________________________________________ • Valence electrons are bonding electrons • Why is group 18 so unreactive? ◦Stability results ___________________________________________________________________________________________________ ‣ It is filled with 2s and 6 p electrons • Stable octet

determine chemcial properoties from the speal electron configuration of outer shell.

Energy of photon depends on the.... • Bohr's calculated energies matched the IR, visible, and UV lines for......

difference in energy levels the H atom

heterogeneous

different composition and properties in the same sample; unevenly mixed

Allotropes

different forms of the same element in the same state of matter exs: oxygen gas and ozone

Isotopes ► Atoms of the same element with different mass numbers. ► Some are naturally occurring and some man made

different nubmer of neutrons

Historical Models (model #5) ► Electron Cloud Model Ernst Schrodinger revised Bohr's model by having the e- occupy orbitals with....

different shapes and energies. The orbitals surround the + nucleus in a "cloud-like" pattern.

A model:

difficult or (perhaps computerized) can be used if the experiment would be impossible-example: atoms or molecules

5. P2O5

diphosphorus pentoxide Covalent

energy and frequency=

directly proportional

frequency and energy=

directly related

• Amplitude (A)...

distance from the origin to the trough or crest

- The principal quantum number tells the average relative distance of the electron from the nucleus - n = 1, 2, 3, 4, 5, 6, 7 - As n increases for a given atom, so does the average.... - Electrons with higher values of n are easier to remove from an atom. 74 S orbitals shown as "onion layers"- A series of concentric spherical shells

distance of the electrons from the nucleus.

Niels Bohr (1913):

e- can possess only certain amounts of energy, and can therefore be only certain distances from nucleus. (less energy=closer)

1. How do each of the following Sl prefixes compare to the base unit? e. milli-

e. 0.001 (10-3)

5. Use the periodic table to identify the group numbers and period numbers of the following elements. e. phosphorus

e. 15, 3

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. e. Tin (IV) oxide

e. Ionic; SnO2

1. Use the periodic table to determine whether each of the following bonds would be IONIC, POLAR COVALENT, or NONPOLAR COVALENT: e. C-Br

e. Polar Covalent

• Four Quantum Numbers: - Specify the "address" of....

each electron in an atom

Quantum Numbers 4. Spin # (ms) →

electron 1/2 or -1/2 (an orbital can hold two electrons with opposite-direction spins) (up arrow means positive, down arorw means negatvie)

• A magnetic moment is called....

electron spin.

Quantum Mechanical Model Modern atomic theory describes the electronic structure of the atom as the probability of finding electrons within certain regions of space (orbitals).

electrons as waves

The angular momentum quantum number (l) Second quantum number l - Value of l describes the shape of the region of space occupied by the electron - Allowed values of l depend on the type of orbital s=0, p=1, d=2, f=3 - Regions of space occupied by....

electrons in the same subshell have the same shape but are oriented differently in space

Aufbau Principle

electrons will take lowest energy orbital avaiable path of least residence

Gold (Au)

element

Oxygen (O2)

element

Can be either the same...

element or different elements

Polyatomic

elements consist of several "like" atoms bonded together

Monatomic

elements consist of unbounded, "like" atoms examples: Fe, Al, Cu, He

electrons abosrb...

energy

Quantum Numbers 1. Principal Q# (n) →

energy levels 1-7

Bohr's model of the atom accounted mathematically for the.......

energy of each of the transitions.

Einstein's photons of light were individual packets of....

energy that had many characteristics of particles.

43. If you do not understand how to use a piece of....

equipment, ask the instructor for help.

Observations:

example: you pull a chain on a lamp, but the light does not go on

If "right" amount of energy is absorbed by an e-, it can "jump" to a higher energy level. This is an unstable, momentary condition called the ____________.

excited state

Chemical and physical changes are accompanied by energy changes that may be __________________ or __________________.

exothermic endothermic

10. Know the locations and operating procedures of all safety equipment including the....

eyewash station, safety shower, fire extinguisher, and fire blanket. Know where the fire alarm and the exits are located.

5. Use the periodic table to identify the group numbers and period numbers of the following elements. f. potassium

f. 1, 4

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. f. zinc and chlorine

f. Ionic; ZnCl2

• Dmitri Mendeleyev was the - ____________________ periodic table • Observed that elements listed in order of atomic mass showed regular/perodically repeating properties Publicshed preiodc table in 1869 ◦Publshed known elements ‣ Arranged elements ________________________________

father of by atomic mass

Red diamond determines ________________ of substance.

flammability

look within families _______________________________________________________________

for comparisons

Hund's Rule:

for equal energy orbitals, each must have one electron before any take a second

Later we will differentiate molecules from formula units-....

for now, they are both words for groups

shielding effect: kernel e- "shield" valence e- from attractive__________________________________________________

force of the nucleus -- caused by kernel and valence e- repelling each other

Careers in Chemistry:

forensics research (cures and treatments) development (new products) production (quality control) chemical sales software engineering teaching law

• An electron has two possible orientations in an external magnetic field, which are described by a....

fourth quantum number ms .

Sections of Periodic Table to Know

from left to right, s-block, d-block, p-block....lonesome section, the island, f-block (number down paper from 1-7; ,diagonally) d-block; n-1 f-block; n-2

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. g. Co(NO3)2

g. Ionic; Cobalt (II) nitrate

Shorthand Electron Configuration (S.E.C.) To write S.E.C. for an element: 1. Put symbol of noble..... 2. Continue writing e- config. from that point.

gas that precedes element in brackets.

Deposition

gas to solid (energy removed from the system)

Students must comply with safe behavior. Approved...

goggles MUST be covering their eyes AT ALL TIMES during the lab.

When all e- are in lowest possible energy state, an atom is in the ____________ .

ground state

What is ground state & excited state?

ground state is normal state for electron, excited is the higher level electrons jump to when they get energy • See color when electron relaxes back down to ground

Is the ground or excited state more stable?

ground state is stable (Can use color to ID elements.-Why is copper green? • Difference in energy of ground state and excited state is unique to each element)

alkali metals:

group 1 (except H); 1+ charge; very reactive Hydrogen; s prop like alkali, but not rly

coinage metals:

group 11 • metals have low melting point ◦Molten metal ‣ They don't tarnish and are very shiny

halogens:

group 17; 1- charge; very reactive • form a 1- ion when they become an ion • Most aggrisve, alkali metal and halogen=stable compound ◦Ex: table salt

noble gases:

group 18; no charge; unreactive

alkaline earth metals:

group 2; 2+ charge; less reactive than alkalis

___________ - contain elements with very similar chemical properties.

groups (vertical columns; numbered 1-18 across the top)

main block (representative) elements:

groups 1, 2, 13-18 all the s and all the p

The single-charge cations are: (metals have one particular charge)

groups 1, 2, 13, and (Ag1+, Cd2+, and Zn2+ save these 3) Will match with negative anions-blue parts

transition elements:

groups 3-12; variable charges from different groups

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. h. Ammonium phosphate

h. Ionic; (NH4)3PO4

Max Planck-

h=6.626*10^-34j*s E=hv (German physicist who developed quantum theory and was awarded the Nobel Prize for physics in 1918.)

Writing Formulas of Ionic Compounds chemical formula:

has neutral charge, shows types of atoms and how many of each

•Energy Level- how far away from the nucleus the electron....

has travelled 1st energy level is closest to nucleus

• Exothermic:

heat is coming out of chemicals ◦Chemical change that is producing heat (any combustion reaction. a neutralization reaction. rusting of iron (rust steel wool with vinegar) the thermite reaction. reaction between water and calcium chloride. reaction between sodium sulfite and bleach (dilute sodium hypochlorite) reaction between potassium permanganate and glycerol.)

Chicken soup

heterogeneous mixture

Pizza

heterogeneous mixture

Sand

heterogeneous mixture

short wavelength(you should know the symbol)=

high frequency

Salt water

homogeneous mixture

Alloys

homogeneous mixture of metals

inverse proportion

hyperblodo ([pressure/volume relationship) k=xy

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. i. HgSO4

i. Ionic; Mercury (II) sulfate

Dalton Model (#1)of the Atom Late 1700's - John Dalton- England Teacher- summarized results of his experiments and those of others Combined...

ideas of elements with that of atoms in Dalton's Atomic Theory

42. Report damaged electrical equipment...

immediately. Look for things such as frayed cords, exposed wires, and loose connections.

Each element has a unique bright-line emission spectrum. i.e. "Atomic Fingerprint" Helium Bohr's calculations only worked for hydrogen! Attempts were made to adapt to include elliptical orbits, still no good./ Bohr historically very...

important because it showed the quantized energy.

As we go farther to the right, more coulombic attraction, no new energy level, more pull, smaller size ◦More columbic attraction b/c more portons and more electrons ◦Smae energy level ‣ More pull, therefore we tuck the electrons in closer • They snuggle______________________________ ◦Smaller size ‣ Atomic radius, via more attraciton

in closer to the necleus

44. Do not immerse hot glassware...

in cold water as it may shatter.

kernal (core) electrons

in inner energy levels closests to nucleus

Electronegativiati • Electronegativity, ionizaiotn energygt, electrion affinity all move ________________________________________________________________ ◦Increase to the right, decrease down • atomic radius is odd man out ◦B/c inversely proportional to hte pull on the electrons ‣ A very weak pull on hte electrons, means the atom is very fluffy and spread out • A strong pull means the electrons are tucked in and therefore the atom has a much smaller radius

in the same directions

if the frequency is....

increased, the ejected electrons will travel faster

Electronegativity ⭘Across a period-

increases.

graduated cylinder

instrument used to measure volume of a liquid

39. Fill wash bottles only with distilled water and use only as....

intended, e.g., rinsing glassware and equipment.

energy and wavelength

inversely related

wavelength and frequency=

inversely related

inference

involves a judgment or assumption

• Starts with metal-

ionic

10. FeSO4

iron (II) sulfate Ionic- Multi Charge Cation & Polyatomic Anion

Students cannot copy another student's work and use... If this occurs, no points will be given for the lab report and an Academic Dishonesty Report....

it as their own. will be completed by the teacher.

Heisenberg uncertainty principle

it is impossible to know exactly both the velocity and the position of a particle at the same time

Basic Flame tests are not sensitive enough to ID every element. • What happens if sample contains more than 1 metal?

it just doesn't work

In order to observe an electron, one would need to hit it with photons having a very short wavelength. • Short wavelength photons would have a high frequency and a great deal of energy. • If one were to hit an electron,......... • Lower energy photons would have a smaller effect but would not give precise information.

it would cause the motion and the speed of the electron to change.

ends in -IDE,

it's right off the table

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. j. CBr4

j. Covalent; Carbon tetrabromide

Kilo; unit abbreviation

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. k. barium and fluorine

k. Ionic; BaF2

electron shield=

kernel electrons

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. l. CaS

l. Ionic; Calcium sulfide

Wavelength(you should know the symbol)....

length of one complete wave

less photons=

less energy

Rydberg Equation 31 •In late 1900's a mathematical relationship was discovered to explain these lines • this eqn fits the wavelength of....

light to energy levels;

hot gas=

line emission spectrum

direct proportion-

linear (Density) (Y=kx) (k=y/x)

Matter and Energy are...

linked(just change form)

Ion Formation Patterns - Atoms gain or.......electrons to become more stable. - Isoelectronic with the Noble Gases.........

lose same electron configuration as noble gases

Empirical Formula

lowest-terms formula

Meter; unit abbreviation

Milli; unit abbreviation

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. m. FePO4

m. Ionic; Iron (III) phosphate n. Ionic; Li2O

Molecule-anything...

made up of at least 2 atoms

describe Benfey's Periodic Table

main block, s and p in circle ◦F block and d block on outskirts ‣ MORE SPACES • Super actanids to come

Define Law of Conservation Mass

mass is neither created nor destroyed in ordinary chemical reactions

Law of Conservation of Mass

mass is neither created nor destroyed during ordinary chemical reactions

Intensity of light is a....

measure of the number of photons.

• Ionic Compound=

metal or poly group; first part ◦Roman numerals for only red metals

______________________- have some properties of metals and some properties of nonmetals.

metalliods

_______________________-properties? Malleable, ductile, good conductors, shiny, silvery except for copper and gold, they're more yellow/orange, solid except for mercury. Located to the _____ of the staircase.

metals left

Also, pure compounds have consistent properties but...

mixtures can have varying properties based on the composition of that mixture.

shorter wavelengths=

more frequency

Nano; unit abbreviation

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. n. lithium and oxygen

n. Ionic; Li2O

wavelength is associated with....

nanometers

John Dalton's Atomic Theory (1803) 1. All matter is made of tiny indivisible particles called atoms.-XXX 2. Atoms of the same element are exactly alike; in particular, they have the same mass. Atoms of different elements are different.-XXX John Dalton's Atomic Theory (1803) 3. Atoms of different elements combine in whole-number ratios to form chemical compounds. Dalton's model of atom-XXX 4. In chemical reactions, atoms are combined, separated, or rearranged.-XXX

no no yes yes

Democritus' model of atom

no protons, no neutrons, no electrons solid and indesstructible

______________- Group 18; a special group of nonmetals. Very stable and highly UNreactive!

noble gases

______________-properties? • Gases or brittle solid, poor conductors, colorful, but dull Located to the _______ of the staircase.

nonmetals right

Rutherford's 3rd model of the atom

now has nucleus

Electrons tiny particles/waves cannot be seen • Their exact location cannot be found at any 1 time without stopping them • They move at speed light around...

nucleus in a random fashion described by waves

• Frequency(V)...

number of waves that pass a point during a certain period of time hertz-Hz (1/s)

Third quantum is ml , the magnetic quantum number Value of ml describes the orientation of the region in space occupied by the electrons with respect to an applied magnetic field - Allowed values of ml depend on the value of l - ml can range from -l to l in integral steps ml = −l, -l + l, . . . 0 . . ., l - 1, l - For a given set of quantum...

numbers, each principal shell contains a fixed number of subshells, and each subshell contains a fixed number of orbitals

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. o. KF p. Nickel (II) cyanide

o. Ionic; Potassium fluoride

4. Physical properties are properties that can be

observed or measured without changing the chemical composition of the substance.

Compounds-anything made up...

of at least 2 different elements

Photon are units or bundles...

of energy with no rest mass. e=hv

Law of multiple proportions John Dalton When two different compounds have same two elements, equal mass...

of one element results in integer multiple of mass of other.

Element names come from a variety _________________.

of sources.

robert millikan's work

oil drop experiment measured the charge of an electron electrons are smaller supports Thomson's model

• Elements have ____ capital letter while compounds have _________.

one multiple

Labs requiring after school make-up are predetermined and...

one of the four Chemistry teachers will supervise.

Other atoms "want" to be like noble gas atoms. -- doesn't apply to He, Li, Be, B (which want 2) or to H (which wants either 0 or 2) fluorine atom, F ** They give away...

or acquire e-.

4. When first entering the science room, do not touch any equipment, chemicals,....

or other materials in the laboratory area until you are instructed to do so.

17. Students are never permitted in the science storage room.....

or preparation areas unless given specific permission by the instructor.

electrons exist only in _____ with ______ amounts of energy called _____________ • Therefore... • electrons can only gain or lose certain amounts of energy • only certain ________ are produced

orbits specific energy levels photons

3. Magnetic Quantum Number ( ml )

orientation of orbital specifies the exact orbitial within each sublevel

34. Never remove chemicals or....

other materials from the laboratory area.

30. Dispose of all pipets used with any chemical....

other than water after each lab period.

Recycling plants use machines to separate:

paper, metal, glass, and plastics based on their physical properties!

electrons have both....

particle and wave properities

24. C5P6

pentacarbon hexaphosphide Covalent

Contain the symbol of the element, the mass number and the atomic number

peridoic elemental cubies

Periodic Law ⭘ The physical and chemical properties of the elements are ________________________________________________________________________.

periodic functions of their atomic numbers. • Meaning ◦Repetitive pattern based on their atomicn ubmers ‣ Determines physical and chemcail properties

______________- show trends in properties moving across the table. What about the two periods at the bottom?? horizontal rows, numbered 1-7 down the side

periods

electrons are absorbing...

photons

• Endothermic:

physical change (Melting ice cubes. Melting solid salts. Evaporating liquid water. Converting frost to water vapor (melting, boiling, and evaporation, in general, are endothermic processes.)

Mixtures can be ______________ seperated (homogenous and heterogenious)

physically

The Bohr model of the atom, like many ideas in the history of science, was at first prompted by and later partially disproved by experimentation.

plantery model

◦-ate/ite=

poly group

36. Carry glass tubing, especially long pieces, in a vertical....

position to minimize the likelihood of breakage and injury.

• When an electrically charged object spins, it....

produces a magnetic moment parallel to the axis of rotation and behaves like a magnet.

electrons=

proportionate waves

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. q. Aluminum sulfite

q. Ionic; Al2(SO3)3

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. r. SiO2

r. Covalent; Silicon dioxide

If the student continues to refuse to wear goggles, the student...

receives a Principal's office referral for noncompliance.

Students receive no credit for either the lab report or lab quiz after....

receiving a Dean's office or Principal's office referral.

If a student continues to engage in unsafe behavior after receiving a Dean's office referral, they receive a Principal's office....

referral for discussions about removing the student from the science course.

When e- falls back to a lower-energy, more stable orbital (it might be the orbital it started out in, but it might not), atom...

releases the "right" amount of energy as light. (always releases energy as light, not matter what electrons were given, b/c it's always releasing photons)

Can only explain by assuming electromagnetic radiation is quantized and frequency....

represents min E needed to remove electron from metal.

1. Conduct yourself in a...

responsible manner at all times in the laboratory.

21. RbI

rubidium iodide Ionic- Single Charge Cation & Elemental Anions

7. Ru2O7

ruthenium (VII) oxide Ionic- Multi Charge Cation & Elemental Anions

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. s. Calcium chlorate hexahydrate

s. Ionic; Ca(ClO3)2 · 6H2O

Lab preparation is not "just another homework assignment". Inadequate lab preparation results in unsafe lab behavior. After...

school make-up sessions will not be scheduled for inadequate lab preparation.

suspension

settles over time

As we go down, the__________________________________

shielding effect increases

9. SiCl5

silicon pentachloride Covalent

8. AgCl

silver chloride Ionic- Single Charge Cation & Elemental Anion

Electromagnetic Spectrum Batting Order....

small to large: x-rays ultra violet visible: Violet Blue Green Yellow Orange Red infarred (small frequency) radio 9small frequency)

If students engage in unsafe lab behavior, i.e., by "goofing off" or continuously...

socializing rather than working on the experiment, they will receive a Lab Safety Referral and will be sent to the Dean's office for unsafe lab behavior.

NaBr

sodium bromide

Sublimation

solid to gas (Energy put into system.)

• states of matter:

solid, liquid, or gas

Volume is the....

space that matter occupies, and its typical units are L or cm3

Micro; unit abbreviation

special u

Scientific Law:

states what happens ◦Doesn't change ◦Never violated ‣ Examples: law of gravity, law of conservation

Students will be reminded to put on the googles. However, if a...

student does not comply with the safety requirement, the student will receive a Lab Safety Referral and will be sent to the Dean's office for noncompliance and/or lose points on that lab.

Any behavior that puts....

students in jeopardy for injury is unacceptable.

1. Chemistry is the...

study of the composition of matter and changes that matter undergoes

6. H2SO4

sulfuric acid Acid- polyatomic ion ending in -ate

• H2SO3 The polyatomic ion is sulfite

sulfurous acid

22. H2SO3

sulfurous acid Acid- polyatomic ion ending in -ite

When light strikes a metal....

surface, electrons are ejected. (individual stream, not wave)

1. Classify the category of chemical described below using IONIC, COVALENT, OR ACIDIC. Then write the corresponding name or formula. t. P4O10

t. Covalent; Tetraphosphorus decaoxide

49. Never look into a container...

that is being heated.

Mixtures are made of more than one different material, so...

the chemical formulas are different throughout the mixture.

• Up and down results from layers of electrons and___________________________________________________________________

the shielding effect

JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel prize for describing.....

the wave-like nature of the electron.

• mass:

the amount of matter in an object

31. When transferring reagents from one container to another, hold...

the containers away from your body.

Halogens

the elements in group 7A on the periodic table (-1charge)

Noble gases

the elements in group 8A on the periodic table

Transition metals

the elements in groups 1B-8B on the periodic table, also the d-block

Lanthanides and Actinides

the elements in period 6 and 7 with atomic numbers from 57-70 and 89-102. Part of the f-block

ionization energy:

the energy required to remove an e- from an atom

1. Lab Safety. I have read the "Student Safety Contract" and I understand...

the importance of safety in a chemistry lab. Students have been taken through a safety instruction program to prevent any misunderstandings.

24. Report any accident (spill, breakage, etc.) or injury (cut, burn, etc.) to....

the instructor immediately, no matter how trivial it may appear.

• H2SO4

the polyatomic ion is sulfate HClO3 Sulfuric acid

The Types of Study

the production and use of products

• weight:

the pull of gravity on an object

pure science

the search for knowledge; facts Examples: What happens when these chemicals are mixed together? How many moons are there around this new planet?

• volume:

the space an object occupies

Organic Chemistry:

the study of chemicals containing carbon Examples: glucose and ethanol

Inorganic Chemistry:

the study of chemicals that generally do not contain carbon Examples: salt, water, rust This is the type of chemistry we will be learning this year!

Physical Chemistry:

the study of energy transfers that occur when matter undergoes a change Example: factors that affect the rate of photosynthesis in trees

Biochemistry:

the study of processes that take place in living organisms Examples: muscle, contraction, digestion

Analytical Chemistry:

the study of the composition of matter Example: testing the air for pollutants

Chemistry is...

the study of the composition of MATTER and the changes that MATTER undergoes.

⭘ The physical and Periodic Law chemical properties of the elements are periodic functions of _____________________________________________

their atomic numbers

Periodicity

there are trends in properties of elements • 2 reaons -- left-right AND up-down trends

A Scientific Experiment Experiments must be controlled:

they must have two set-ups where only one variable is different and the other variables are the same • variable: any factor that could influence the result • conclusion: must be based on the data

• Coulombic attraction depends on the amount of charge you have ◦Bigger nuclei are going to attract more than smaller nuclei ‣ Bigger magnet will stick longer and stronger to the fridge, opposed to smaller ones ‣ Secondly, the distance between those two charges • When subsatnces are closer together,_______________________________________________________________________________________________________ ◦Has to have that proximatity

they're able to have a stronger attraction than farther away

Your teacher will supply the mock data for....

those labs not requiring after school make-up.

Just like light, the electron also has a dual wave-particle nature. • Einstein's Wave Particle Duality applies...

to both electrons and light.

28. Never return used, or unused, chemicals...

to their original containers.

4. Lab Make-Up. I understand that ALL labs must be completed. For those that need....

to be done in the lab, the ONLY make-up time will be an announced day after school promptly at 3:05 PM.

Antoine-Laurent Lavoisier, late 1700's...

transformed chemistry from a science of observation to a science of measurement Designed a balance that could mass a substance to the nearest 0.0005 gram Proved that substances require oxygen to burn, thus disproving the theory that substances release the material "phlogiston" when burned

• theory:

tries to explain why or how something happens ◦Based on current evidence ‣ Examples: Theory of Gravity, Atomic Theory

• For any electron, ms can have only two possible values, designated +1/2 (up) and - 1/2 (down), indicating that the...

two orientations are opposite and the subscript s is for spin.

Compounds • contain ___ or _____ different types of atoms • have __________ that are different from those of their _______________________ ____________.

two, more properties constituent elements

Quantum Numbers 2. Angular Momentum Q# (l) →

type of orbital S=0 p=1 d=2 f=3

2. Lab Expectations. I have read the attached "Lab Safety Policy and Procedures" and I....

understand that for the safety of everyone involved in the lab, rules will be strictly enforced. Not following the rules will result in "Lab Safety Referrals" and loss of points. Students who repeatedly misbehave will not be allowed to return to the lab.

Missed labs will either need to be made....

up after school or mock data will be issued.

ask about visible liht chart m thign

ur mum mate

50. Do not place hot apparatus directly on the laboratory desk. Always...

use an insulating pad. Allow plenty of time for hot apparatus to cool before touching it.

observation

uses the five senses

applied science

using knowledge to solve a problem Example: new refrigerants

difference between valence electrons and core electrons

valence electrons: in outer energy level core electrons: inner energy levels; closer to nucleus

• Left to right results from coulombic attraction-attraction between (+) protons and (-) electrons ◦Left to right through a period ‣ Attraction________________________________________

varies on stregth

Nuclear Forces: very strong, short range proton-proton, proton- neutron, neutron-neutron attractions. These are forces which hold the nucleus together.

very strong, short range proton-proton, proton- neutron, neutron-neutron attractions. These are forces which hold the nucleus together.

I ATE an acid and it

was ICk

Dalton's model of the atom

was a solid sphere of matter that was uniform throughout

light can be both a....

wave and a particle

• composition:

what the matter is made of

Experiments were done that could not be explained....

with wave theory of light

Students must return the Lab Safety Referral....

with a parent's signature.

Benet Academy requires that all students always comply..... Your signature demonstrates that you have read and understood...

with established safety policies and procedures outlined below. the safety policy.

Anhydrous:

without water

3. Absences. I understand that it is the student's responsibility to obtain any missed work and complete the...

work as necessary. The missed notes should be obtained from classmates, not from a private lecture after school.

An unsatisfactory model for the hydrogen atom According to classical physics, light should be emitted as the electron circles the nucleus. A loss of energy would cause the electron to be drawn closer to the nucleus and eventually spiral into it.

work based on Thomson and Rutherford

1s^2; explain

x^2: 2 electrons s=shape 1=ring closest to nucleus

NH41+ and N3-

• (NH4)3N

Separate Island- Do not associate with the rest! Covalent Bonding

• 2 Non-Metals • NO CHARGES!!!! • Sharing Electrons Naming: Use the Prefixes

State of the Periodic Table in the 1860's

• 60 elements discovered ◦Scientists work to learn each elements properties and compounds they form ‣ No reliable method to determine atomic mass • Everyone did it their own way-NO comparable way ◦Calculated from diff methods

Isoelectronic Species

• All species have the same number of electrons ◦All of these ions, have the samen nujmber electrons as their closests nuble gas ‣ Lay it out, protons and neutrons counts are differnet, but the electron counts are consistant

1.Homogeneous

• Also called solution • Composition and properties are uniform throughout

⭘If steel (a Metal) and granite (a NM) are both hard, why aren't car engines made of granite?

• Although both are hard, other properties aren't the same. For example, the low heat conditions of rock makes them explode under high temperatures, they are also brittle making them poor for constructing engines.

• What is a spectroscope? • How does it work?

• Any gaseous mass of atoms can be made to emit light by sending a spark • Optical instrument used to ID material • Measures properties of light over a specific portion of Espec • Used to produce spectral lines, measure wave length, intensities

Ba2+ and SO42-

• BaSO4

Ba(OH)2

• Barium hydroxide

⭘What's the difference between a chemical and physical property (rev CH1/2)?

• Chemical property must be tested. Physical property can be observed without changing ID of material. ◦Determine flammability ‣ Either it does or does not • If it does, end product is not hte smae, not hte same what you were left with ◦Change identitiy of the material ◦if you want to know the color of something

2.Heterogeneous

• Composition and properties vary from point to point in the mixture

1894's John William Strut (English) & William Ramsey (Scottish)

• Discoverd all Noble gases but Radon ◦Proposed the Noble Gases group ‣ Fit right in • Co-discoverd plutonium (#94) and all elements thru #102- actinide series

Fe3+ and Cr2O72-

• Fe2(Cr2O7)3

iron (III) nitrite

• Fe3+ NO2-1 ◦Fe(NO2)3

Döbereiner's Triads (1817)

• First person to really put the idea of organizing the elements in play ◦Found these elements considered triads ‣ Found them via taking the average atomic mass of two of those elements it would be very similar to hte third member of the traid • In addition to them having this pattern with their atomic masses ◦They also had similar properties ‣ These triads ended up becoming columns that are families ‣ Dobereiner discovered groups of three related elements which he termed a triad

Chemical Properties

• For Example: ◦Does it burn? ◦Rust? ◦Explode in water? ◦React with acid?

Acids- Named based on negative part

• Have (H) as positive • Binary o H attached to single Naming: Hydro ____ ic Acid • Oxyacids- Polyatomic Ion o Polys ends ATE Naming: ______ic acid o Polys end ITE Naming: ______ous acid

Acid Nomenclature

• Identifying the compound as an acid. • Acids begin with "H" • Binary Acids have only 2 elements. • Identify the other element. (Not Hydrogen) • Change the ending of the element's name to "-ic" • Put a "hydro-" in front

Acid Nomenclature • Oxyacids have a polyatomic ion. • Identify the polyatomic ion.

• If the polyatomic ion ends with "-ate" it will be an "-ic acid"

Who was Lothar Meyer (1830 - 1895)?

• Invented peridoic table independetly of Mendeleev ◦Not given much credit ‣ To little to late • Same principle though his work was not published until 1870 - one year after Mendeleev's

‣ Wavelength is directly or inversely related to frequency?

• Inversely related

Lithium Hydroxide

• LiOH

⭘Give 4 properties of Metals

• Malleable, ductile, conduct electricity, shiny, react w acides/oygen

Mg2+ and NO21-

• Mg(NO2)2

ammonium chlorate

• NH4+ CIO3-1 ◦NH4CIO3

ammonium phosphide

• NH4+ P3- ◦(NH4)3P

NH41+ and ClO31-

• NH4CIO3

Elemental Anions

• Negative Non Metal with only 1 option for charge • Groups 15, 16, 17 Naming: Root + ide

Polyatomic Ions

• Negative ion groups staying together • Some will be given and some need to be memorized • CN-1 OH-1 O2 -2 CO3 -2 ClO3 -1 PO4 -3 NO3 -1 SO4 -2 ClO4 -1 PO3 -3 NO2 -1 SO3 - ClO2 -1 C2H3O2 -1 Naming: Names from handout to be memorized

The Octet Rule and Common Ions

• Neon is perfectly happy ◦Not doing anything • Oxygen ◦When it becomes an ion, it's going to gain 2 electrons ‣ Still has 8 protons, now it has 10 electrons around the outside • Charges will becomes negative via a surplus of electrons

• Where on that energy level?

• Orbitals are regions around the nucleus where electrons are likely to be found.

Lead (II)Hydroxide

• Pb(OH)2

lead (II) permanganate

• Pb2 MnO4-1 ◦Pb(MnO4)2

Single Charge Cation

• Positive Metal with one option for charge • Groups 1,2, and 13 • Ag1+ , Zn+2, Cd+2 Naming: Name from the Table directly

Multiple Charge Cation

• Positive Metals with multiple options for charges • Found in the Transition Metals • Pb, Sn Naming: Name from Table + Parenthesis with Roman numeral (Charge of Metal)

Polyatomic Ions

• Positive groups staying together • NH4 + , H3O+ Naming: Names from handout to be memorized

Sn4+ and SO42-

• Sn(SO4)2

NaOH

• Sodium hydroxide

Atomic Radius (picometer)

• The atomic radius is 1/2 the distance between nuclei of 2 identical atoms ◦The reason they define it this why is that it is hard to see the edge of a atom is ‣ But atoms won't stack on top of each other • So by putting 2 atoms right next to each other ◦If they measrue from one nuclei to the other ‣ Then they divide it in half=radius of one cirlce ‣ Down a group-increases ‣ across a period-decreases

⭘ What was the reason for chemical periodicity? ⭘ (section 6.3)

• The reason for periodicity is explained by the arrangment of the electrons abobut the nucleus!

⭘What are metalloids used for?

• They are used in the fabrication of computer chips. Because they conduct electricity only under some conditions, they are good for making electrical switches.

Isoelectronic Species

• They're not the same size ◦But all five ions are not the same size, who has the largest diameter? ‣ Same number of electrons, but we must think about how many layers of electeons, but cahrge on the nucleus ‣ Oxygen is going to the largest, so its only have 8 portons to pull those electorns in,, looseest • Magnesium has 12 protons to pull those elctrons in, snuggles in a lot mroe ◦If your looking at 2 ions, think about hwo many electrons and how many layers, but also, what's the strenght of their nucleus and how will htat influecne the diameter

zinc phosphate

• Zn2+ PO4-3 ◦Zn3(PO4)2

Physical Properties

• can be observed or measured WITHOUT changing the chemical composition of the substance ◦For Example: ‣ mass, volume, density, mp, bp, color, odor, size, shape, texture, state of matter, malleability, ductility, conductivity, luster

1)A hamburger is cooked

• chemical change

4) Old ham goes bad in the refrigerator

• chemical change

Solid

• definite shape, definite volume • Particles tightly packed, very orderly

8. Density= Mass/Volume Less consistent pattern • Nonmetals generally lower density • Lower period metals generallly higher density

• density and melting point do share simialries in that which elemnts share high and low values low density elements at hte top highest density eleemnts are at the bottom osmium has densitt of 22.6 g/ml

James Chadwick (1932) • discovered particles with similar mass to proton but zero charge

• discovered neutrons • Neutrons critical for the stability of the nucleus

quantitative data

• example: 55 L or 83 degrees C measurements

qualitative data

• example: clear liquid descriptions

Trends in Atomic and Ionic Size

• for our metals, in general, they want tog ive away electrons ◦Form positive ions ‣ When they do that they end up smaller than their orignal parent • Cations are smaller than their parent atoms ◦If they have less electrons, these are going to be electrons where they're losing a whole layer ‣ They should get smaller

In the Law of Octaves, what happened?

• missing noble gas columns • They didn't know as much about the valence electrons at that time, so the pattern was more based on physical properties and how it reacted chemically with other substances. ◦The Nobles Gases they found had no properties related to their octaves

Liquid

• non definite shape, definite volume • Particles still packed together, but not orderly-free to "flow"

Gas

• non definite shape, non definite volume • Particles very far apart, mostly empty space!

Trends in Atomic and Ionic Size

• nonmetals tend to gain electrons ◦If we gain electrons, our atom gets larger ‣ We haven't changed the layers of electrons for the nonmetals ‣ Filled in layer, more elections • Each proton has to divivde hte attraciton with more electrons ◦By doing that, your weakening each individual attraction, ans so the atom gets fluffer then it was orginially

5. Electron affinity (kJ/mol) ⭘ The energy change given off when an electron is gained by a neutral atom. ⭘ An anion is formed. ⭘ Down group- Decrease ⭘ Across a period- Increase

• opposite reaciton ◦Electron is gained by an antom and energy is given off

2)Thousand Island dressing and mayonnaise are mixed to make "secret sauce" for hamburgers

• physical change

3)Water is boiled in preparation for making pasta

• physical change

5) A rock star gets a tattoo on his forehead

• physical change

Properties of Some Elements Predicited by Mendeleev

• pretty darn accurate ◦Understood in great detail that if this particular compound was a member of a curtain family, it would acct in the same way as other faimily memebers ‣ Considered father b/c not ddi he create it, but also had the wisdom to leaves spaces

What was the Law of Octaves?

• repetitive pattern after a certain number of elements ◦7 before repeated ‣ No noble gases

Shielding Effect

• rly is looking at how the electrons in between hte valence electrions and the nucleus interfer ◦About shielding ‣ Kernel electrons interfer with the outer vlanece electrons • Kernel electrons block the attractive forec of the nucleus from the valence electrons

percentage composition:

• the mass of each element in a compound • We will round to 2 decimal places

Relative Size of Atoms

• this trend is also a diaganol ◦But it's opposite diagnol of electronegativity ‣ The biggest is hte bottom left • The smallest is upper right

Who was Henry G.J. Moseley?

• was a Rutherford student ◦Able to figure out the atomic numbers of elements ‣ Did arrange the PT by atomic number • Couple spots were pattern was imporved ◦Killed in WWI, age 28 ‣ Battle of Gallipoli in Turkey 1887 - 1915

‣ What is the equation that relates these values?

•C=v(symbol for wavelength)

◦Speed of Light-c

‣ 3.0*10^8 m/s

EXTENSIVE PROPERTIES

‣ Change depending on the amount of matter present • For Example: ◦mass, volume, length

◦Energy is directly or inversely related to frequency?

‣ Directly related

◦Frequency-v

‣ Hertz (Hz_ which is per second)

◦Wavelength-(symbol for wavelength)

‣ M or nm (if visible light)---FIND OUT MORE

electronegativity • lower left hand corner ◦Atoms that have al ot of layers of electrons ‣ They don't really want hte elctrons they have • They want to form postivie iosn ◦They don't share them, just give it away ‣ Little bit higher electronegativity in the middle of the road

‣ Upper right hand corenre, high electronegativity valeus

Greek Model Democritus (400 BC) ► Idea of 'democracy' ► Idea of 'atomos'

► Atomos = invisible ► 'Atom' is derived ► No experiments to support idea so a philosopher rather than a scientist "To understand the very large, we must understand the very small."

Subatomic Particles- top quark last discovered in 1995 at fermilab

► Quarks ► component of protons & neutrons ► 6 types ► 3 quarks = 1 proton or 1 neutron

Thomson Model of the Atom 1897 ► J.J. Thomson discovered the electron and knew that electrons could be emitted from matter. ► William Thomson (Lord Kelvin) proposed that atoms consist of small, negative electrons embedded in a massive, positive sphere.

► The electrons were like currants in a plum pudding. ► This is called the 'plum pudding' model of the atom. (Many textbooks now use the names " raisin bun" or "chocolate chip cookies" when referring to Thompson's model of the atom. Although it was other scientist that actually gave Thompson's model of the nickname "plum pudding.")

Mass Number

► mass # = protons + neutrons • always a whole number • NOT on the Periodic Table!

Density and the Atom ►Since most of the particles went through, the atom was mostly empty space.

►Because the alpha rays were deflected so much, the positive pieces it was striking were heavy. ►Small volume and big mass = big density ►This small dense positive area is the nucleus

Modern View ►The atom is mostly empty space ►Two regions ►Nucleus ►protons and neutrons ►Electron cloud ►region where you might find an electron no predetermined

►Electron cloud ►region where you might find an electron no predetermined no predetermined path

Law of Definite Proportions Joseph Louis Proust ►Each compound has a specific ratio of elements

►It is a ratio by mass ►Water is always 8 grams of oxygen for every 1 gram of hydrogen

Ernest Rutherford 3rd atomic model ►Learned physics in J.J. Thomson' lab.

►Noticed that 'alpha' particles were sometime deflected by something in the air. Gold-Foil Experiment

Size of an atom ►Atoms are incredibly tiny. ►Measured in picometers (10-12 meters) ►Hydrogen atom, 32 pm radius

►Nucleus tiny compared to atom ►Radius of the nucleus near 10-15 m. ►Density near 1014 g/cm3 ►IF the atom was the size of a stadium, the nucleus would be the size of a marble.

1897 Thomson discovers the electron 1911 Rutherford discovers the nucleus 1932 Chadwick discovers the neutron

►Somewhere between Thomson and Chadwick, physicists realized that there are positively charged constituents of the nucleus, which we call 'protons'. The way this happened was a gradual process, and that is why it is hard to say exactly who discovered the proton, although if you had put a name against it, it would be Rutherford, sort of... Controversy

• Circel the bigger atomic raduis of the following elements • I/Ag

◦Ag

Hydroxide

◦Always 1-

• Formula Units

◦Anything made up of a cation and an anion

• Compounds

◦Anything made up of at least 2 different elements • Both Formula Unit and Compound are types of particles

• Molecules

◦Anything made up of at least 2 non-metal atoms ‣ Note that if the compound formula begins with NH4 then it is a formula unit and NOT a molecule • Can be either the same element or different elements • Remember that diatomic molecules are made up of the same element

• Circel the bigger atomic raduis of the following elements • Ba/F

◦Ba

1940's Glenn Theodore Seaborg

◦Discovered 100+ isotpoes ‣ Authored the Actinide Series Concept ‣ 1951 Noble Prize • only Living person to have element named after them ◦Have element named his name while he was alive ‣ Honor bestowed upon him ‣ Bottom row of the f-block, actinide series ‣ Worked on Manhattan series ‣ Most well known and most intellegent chemist in the 1940s • Worked at UC Berkley ◦Calfornium, Berklium, and Americanium

Energy

◦E j or kj (e=hv)

Describe what is happening when...

◦Electron goes from ground to excited state ‣ Electron absorbs energy from light, heat, electricity ‣ Electron goes farther away from nucleus ‣ Electron goes up in energy, and moves away from nucleus • Temporary ‣ Farthest away from nucleus has the most energy ◦Electron goes from excited state to ground state ‣ Electron releases extra energy as light • photons? ‣ electron goes down in energy, and moves closer to nucleus • Long term until electron gets new energy

• Planck's constant

◦H=6.626*10^-34js

• Pure Substances

◦Have a fixed composition ◦Have fixed properties

• Atoms

◦Individual building blocks of matter ‣ pieces of elements from table

Who was J.W. Döbereiner (1829)?

◦Law of Triads Elements could be classified into groups of three, or triads. Trends and physical properties such as density, melting point, and atomic mass were observed. • groups of three element with similar properties

• Circel the bigger atomic raduis of the following elements • Mg/sr

◦Mg

• Circel the bigger atomic raduis of the following elements • Mg/p

◦P

• Circel the bigger atomic raduis of the following elements • Pb/sb

◦Sb

• Frequency

◦V Hertz (Hz) which is /sec

Ionic Radii

◦When they're ion, the positive ion volumns gets smaller, whether thats' the +1 +2 +3 ◦the negative colums get bigger

• Acid

◦if the word "acid" is in the written name, it's a acid

• Ionic

◦roman numerals, metals ◦polyatomic group

Stuff about Dmitri Mendeleyev papaer?

◦section of paper he published ‣ Dashes-no elements yet discovered • 100 piece puzzles with 50 pieces

• Covalent

◦tri and hexa

What are the 9 Periodic Trends?

⭘Electronegativity ⭘Atomic Radius ⭘Ionic Radii ⭘Ionization Energy ⭘Electron Affinity ⭘Shielding Effect ⭘Reactivity ⭘Density ⭘Melting Point

Who is credited for the majoirt of the Modern Periodic Table?

⭘Henry G.J. Moseley, English ⭘Determined the atomic numbers of elements from their X-ray spectra (1914) ⭘Arranged elements by increasing atomic number ⭘Elements fit into better pattern when arranged by increasing atomic number

Who was Dmitri Mendeleyev (1834-1907)?

⭘Russian ⭘Invented periodic table ⭘Organized elements by properties ⭘Predicted existence of several unknown elements ⭘Element 101 named after him

Chem; Semester 1 Review-M2

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