(Chemistry H) Benchmarks & Finals: Quarter 3 Benchmark

"Inter" → __________ "Intra" → __________

"Inter" → *Across* "Intra" → *Between*

S & P Block Elements

"Main group elements" Representative elements show clear trends Groups 1-2, 13-18

Which sublevel is associated with a higher amount of energy, 4s or 3d?

3d. In Aufbau's diagonal rule, 3d comes after 4s

How many significant figures & round to 2 significant figures: 8201

4 8200

How many significant figures & round to 2 significant figures: 900.0

4 9.0 x 10^2

How many significant figures & round to 2 significant figures: 2.100

4 2.1

Quantum Numbers: Electron Spin Quantum Number

Indicates the spin of the electron (clockwise or counterclockwise) Values of m'sub s = 1/2, -1/2 (depiction are the arrows)

Rare Earth Metals

Inner transition metals Top group is Lanthanides (+3 oxidation state) Bottom series is Actinides (very dense, radioactive) All very chemically similar Used in lamps & lasers Tarnish readily in air

Extensive vs Intensive

Intensive: does not depend amount or size sample Extensive: depends on amount or size of sample

Interference

Interaction of 2 waves Waves can interact to combine with each other, resulting into 1 composite form Reinforcing interaction = constructive interference Cancelling interaction = destructive interference Ex: light produces an interference pattern when paired through a double slit Ex: Crest & crest combine Ex: Crest & trough cancel out

Ionic Compounds: Metals

Ionic compounds result when metals react with nonmetals Metals LOSE electrons to match the number of valence electrons of their nearest noble gas Cations (positive ions) form when the number of electrons are less than the number of protons Group 1 Metals → ion ^1+ Group 2 Metals → ion ^2+ Group 13 Metals → ion ^3+ Examples: NaCl, CaCl2, K2O (cation is first)

Types of Chemical Bonds

Ionic, covalent, metallic

What does bonding achieve?

It lowers the potential energy of atoms, stabilizing them & giving them electron configurations similar to that of a noble gas (-)Potential energy = (+)stability Gives each atom an electron configuration similar to noble gases (Group 18: He, Ne, Ar)

Half-Life

The time for half of a radioactive nuclei in a given sample to undergo decay After 1 half life = 1/2 of original sample left Determines how unstable it is Helps find its age

Line-Emission Spectrum

The specific wavelengths of visible light produced when shining a light through a prism (violet, indigo, blue, green, red)

Formula/Relationship: Frequency & Wavelength

c = λν Speed of light 3.00 x 10^8 m/s = Wavelength x Frequency

Alpha Decay

Radioactive decay by emission of an alpha particle Mass Number - 4 Atomic Number - 2

Forces That Act on an Atom: Nuclear Force

"Strong Force" Keeps protons & neutrons bound in the nucleus Gets stronger as nucleons get closer Keeps nucleus of atoms together if protons have an electromagnetic repulsion

Convert: .00093 g/mL = g/L

(.00093g / 1mL) x (1000mL x 1L) .93 g/L

Dmitri Mendeleev

(1869) Created the first widely accepted version of the periodic table that had about 63 elements Grouped elements by increasing atomic mass & aligned them by similar chemical & physical properties with spaces in between uncommon ones Left blank spaces to add new elements After the discovery of Scandium (Sc), Gallium (Ga) & Germanium (Ge), it was noticed that Mendeleev's predictions are very close to their actual value & his table became generally accepted

Henry Moseley

(1913) By working with X-rays, he determined the actual nuclear charge (atomic number) of the elements Rearranged the elements in order of increasing atomic number (1887-1915) Died in WWI, 27 years old

Glenn T. Seaborg

(1944) After co-discovering 10 new elements, he moved 14 elements out of the main body of the periodic table to their current location below the Lanthanide series. This became the Actinide Series Got a Nobel Prize even though people didn't want him to change the table & is the only person alive to have an element named after him while still alive (Seaborgium, 106)

Convert: 23.4 dm = ? mm

(23.4dm / 1) x (100 mm / 1 dm) 2340 mm

Convert: 30 days = ? min

(30days / 1) x (24 hrs / 1 day) x (60min / 1hr) 43200 min

Precision & Scientific Notation: (6.0 x 10^-4) (7.345 x 10^8) / (5.23 x 10^6)

(44.07 x 10^4) / 5.23 x 10^6

Convert: 45 L = ? dm^3

(45L / 1) x (1dm^3 / 1L) 0.45 dm^3

Convert: 8.4 ft = ? mm (1in = 2.54cm)

(8.4ft / 1) x (12in / 1 ft) x (2.54cm / 1 in) x (10mm / 1cm) 2560.3 mm

Orbits

(Like planets) allowed paths in which the electron can circle the atom (2D Bohr Model)

Percent Error Formula

(Vtrue - Vexperiment) / Vtrue x 100

Arrangement of Electrons in Atoms: Valence Electrons

* VE = 1 - 8 * (I don't remember what I wrote this for) Groups 1-2: group # = VE Groups 13-18: group # - 10 = VE 8 is the max valence electrons from s & p (octet)

Sequence: Atomic Theory to Quantum Theory

*Bohr improved Rutherford's incomplete atomic model* (Rutherford only explained the nucleus & did not explain the electron) - *Bohr discovered "orbits"* (2D paths for hydrogen, but did not have other elements) - *Quantum model* (de Broglie, Heisenberg, Schrodinger) - *Explanation of "orbitals"* (3D regions where electrons may be found) - *Quantum numbers*

Chemical Property Examples?

*Flammability:* ability to catch on fire *Toxicity:* ability to be poisonous *Heat of Combustion:* amount of heat released when substance is completely burned *Reactivity:* what happens when a substance reacts to an x value *Oxidation:* combination of a substance with oxygen (In terms of vs rust, an ex: apple turning brown) *Rust:* corrosion of iron and iron alloys *Corrosion:* a corrosive substance that will destroy or irreversibly damage another surface

Why are intensive properties more useful to scientists than extensive properties?

*Intensive Properties:* do not depend on amount of matter present or amount of sample & do not change according to conditions (Ex: boiling point, density, state of matter, color, melting point, odor, temperature, refractive index, luster, hardness, ductility, malleability) *Extensive Properties:* depend amount of matter present, & can change according to sample size or conditions (Ex: volume, mass, size, weight, length)

Physical Property Examples?

*Melting Point:* temp. at which solid melts to liquid *Boiling Point:* temp. at which the vapor pressure is large enough that bubbles form inside the body of the liquid *Freezing Point:* temp. below at which liquid turns into solid *Conductivity:* transmission of heat/electricity/sound *Solubility:* ability to be dissolved/mixed into another *Viscosity:* resistance to flow/stickiness *Density:* measure of the relative "heaviness" of objects with a constant volume *Ductility:* easily pulled or stretched into thin wire *Color:* vividness of visual appearance *Luster:* shine or glow *Hardness:* rigid & resistant to pressure *Odor:* distinctive smell

Properties: Metal

*Melting/Boiling Point:* (Cu) Wide Range - most transition metals are high *Conductivity:* Very good *Ductility/Malleability:* Very good

Properties: Covalent

*Melting/Boiling Point:* (H20, CO2) Low *Conductivity:* Always poor *Ductility/Malleability:* Good

Properties: Ionic

*Melting/Boiling Point:* (NaCl) High *Conductivity:* 1. Solid = poor 2. Liquid = good 3. Solution = very good *Ductility/Malleability:* Poor/brittle

Ionic Compounds

*Nonmetals & metals*

Polar Compounds

*Nonmetals & nonmetals* or Metalloids & semiconductors

Physical property vs chemical property?

*Physical Properties:* properties that do not change the chemical nature of matter & can be seen without changing *Chemical Properties:* properties that do change the chemical nature of matter & can be seen with changing

A silver dollar has a mass of 26.73 grams. Convert this to kilograms, centigrams & milligrams 1 ounce = 28.35 grams

.02673 kg 2673 cg ? mg

Reasons For Metallic Properties

1. *Valence electrons are mobile,* as they are held very weakly by their nuclei (low ionization energy) 2. *D orbitals* have a lot of room to move around in It's a sea of freely flowing electrons held loosely by their nuclei

Dalton's Atomic Theory

1. All matter is composed of atoms 2. All atoms of the same element are identical; atoms of different elements have different properties 3. Atoms cannot be subdivided, created, or destroyed *disproven by subatomic particles: proton, neutron & electron* 4. Atoms of different elements combined with simple whole number ratios to form chemical compounds *disproven by isotopes, which vary in neutrons* 5. In chemical reactions, atoms cannot be created or destroyed (Law of Conservation of Mass)

You are to set up an experiment that will allow you to separate the following mixture: sand, iron filings, salt, & sawdust. Explain each separation technique & the property that allowed the substance to be separated

1. Because of magnetism, you should get a magnet to take away the *iron filings* 2. Dissolve *salt* into water so it is only water (would know it is there) 3. *Sawdust* would flow because of water & density 4. Strain/filter out *sand* 5. Boil & evaporate the water out of the *salt*

Atomic Theory: Pioneers

1. Dalton: introduced Dalton's atomic theory 2. Thompson: discovered electron by experimenting with cathode ray 3. Rutherford: discovered proton with gold foil experiment 4. Chadwick: discovered neutron, the particle with no charge 5. Millikan: determined charge to mass ratio of electron with oil drop experiment

2 Types of Attraction in Molecules

1. Int*ra*molecular Bonds: Ionic, non polar, covalent, polar covalent, metallic 2. Int*er*molecular Forces (IMF): Have to do with the attraction between molecules versus the attraction between atoms in a molecule, metal or compound (In order of decreasing strength, 3 IMFs are: H-bonding, Dipole-dipole & London Forces)

Scientists: Quantum Model

1. Werner Heisenberg: Uncertainty Principle (it is impossible to determine simultaneously both the position & velocity of an electron) 2. Louis de Broglie: Wave Properties of Matter (matter can exhibit wavelike behavior) 3. Erwin Schrödinger: 4 quantum numbers & came up with mathematical equations

Covalent Bonds: 2 Types

1. Nonpolar: Bonded atoms that share electrons equally. The same atoms are bonded (or very similar) Example: Cl—Cl = Cl2 2. Polar: Bonded atoms that don't share electrons equally. Different atoms bond Example: H—N—H (pretend there is another H atom bonded to N, underneath) = NH3

Quantum Numbers: 4 Types

1. Principal Quantum Number (n = 1, 2, 3... infinite) (distance from the nucleus) 2. Orbital/Angular Momentum Quantum Number (l = n-1 all integers below) (shape) 3. Magnetic Quantum Number (m*sub l = -l to +l, all the numbers in between) (orientation) 4. Spin Quantum Number (m*sub s = 1/2, -1/2) (spin direction)

Effective Nuclear Charge: 2 Factors

1. The distance the nucleus is from the valence electrons 2. Shielding: inner electrons that shield the nucleus from pull on valence electrons *Little shielding + little distances = decreases pull

Scientific Notation: 1.23

1.23 x 10^0

How many significant figures & round to 2 significant figures: 540000

2 5000

Diatomic Molecule

2 atoms of the same type of element forming a molecule 7 elements that form diatomic molecule (HOFNBriCl = "peanut brittle"): H, O, F, N, Br, I, Cl (H2, 02, F2, Br2, I2, Cl2)

Compound

2(+) different atoms chemically bonded together Form a different molecule/compound Chemical reaction occurs

Mixture

2(+) substances (elements, lattices, molecules, compounds) that are not chemically bonded together Each substance keeps its own properties & can be easily separated No chemical reaction occurs

Scientific Notation: 32000000

3.2 x 10^7

Precision & Scientific Notation: (4.26 x 10^12) x (5.4 x 10^-8)

23.004 x 10^4 2.3 x 10^5

The Eiffel Tower is 299.314 meters high. express this height in decameters, kilometers, centimeters & millimeters

2993 dm .2993 hm 29931.4 cm 299314 mm

How many significant figures & round to 2 significant figures: 0.000346

3 .00035

Precision & Scientific Notation: (9.31 x 10^13) / (3.1 x 10^6)

3.003 x 10^7 3.0 x 10^7

When a nurse says that a patient needs 400 cc's of fluid, what is she referring to?

400 mL of cm^3

Scientific Notation: 0.0000052

5.2 x 10^-6

Mendeleev's Table to Modern Table: Mendeleev Table

63 elements Left space for Scandium (Sc), Gallium (Ga) & Germanium (Ge)

A sample of aluminum has a mass of 8.4 grams. If it displaces 3.1 mL of water, what is its density? If the sample was cut exactly in half, what would the density be for half of this sample?

8.4g / 3.1mL = 2.7096774 2.7 g/mL Density would remain the same

Mendeleev's Table to Modern Table: Modern Table

90 elements 2 Groups of Later Additions: 14 Lanthanides & 3 Actinides (Rare Earth Elements) + Noble Gases = ("brings us to") 90 elements

Electron Sea

A "sea" of delocalized, mobile electrons which move freely about the metals network of empty atomic orbitals

Polyatomic Ion

A *group* of *covalently bonded* atoms that *has a charge*

Orbital

A 3D region around the nucleus that indicates the probable location of an electron

Electromagnetic Radiation

A form of energy that exhibits wavelike behavior as it travels through space

Molecule

A group of neutral (no charge), covalently bonded atoms Examples: H2O, CO2, CH4, SO2 Nonpolar or polar Covalently bonded Covalent bonds form between nonmetals & nonmetals

Alpha Particle

A helium nucleus Has a charge of +2 Contains 2 protons & 2 neutrons Nucleus is stable Results in a decrease in mass number by 4 and a decrease in atomic number by 2 Stopped by paper Emission is the most massive (heaviest)

A molecule is __________ bonded

A molecule is *covalently* bonded Nonmetal & nonmetal

Heterogeneous Mixture

A non-uniform mixture of smaller constituent parts Can be separated from one another Consists of visibly different substances

Photon

A particle of electromagnetic radiation with no mass that carries a quantum of energy

Monatomic Ion

A single atom that forms from a charged particle Example: F^-1, Ca^+2, O^-2, Li^+1

Excited State

A state in which an atom has a higher potential energy than it has in its ground state

VSEPR

A theory that tells us that electron pairs align themselves as far away from each other as possible *V*alence *S*hell *E*lectron *P*air *R*epulsion

Intermolecular Forces: Hydrogen Bonding

A very strong type of dipole Dipole attraction is created when *F, O, or N are bonded to H (Because it bonds between strongest. All have highest/strongest electronegativities) They are given this special name (H-bonding) because compounds containing these forces are important in biological systems

Generic Formula

A, B, E *A*: Represents any central atom *B*: Represents the number of bonds around the central (double & triple bonds count as 1) *E*: Represents unshared pairs of electrons around the central atom Example: H2O would be AB2E2

Problem Solving: How do you find an element's group number using its noble gas notation?

Add all the electrons outside of the brackets

Problem Solving: Number of Valence Electrons

Add the number of electrons in the highest number energy levels VE = 1 - 8 (I don't remember what I wrote this for) Groups 1-2: group # = VE Groups 13-18: group # - 10 = VE 8 is the max valence electrons from s & p (octet)

If you had a mixture of cork & sand & they were both the same size particles, how would you separate these substances? What property would allow this?

Add water because density allows it to float. Then, filter out the sand

Boron Group (Group 13)

All have 3 valence electrons Change in properties (what)

Carbon Group (Group 14)

All have 4 valence electrons All living things have carbon in them

Nitrogen Group (Group 15)

All have 5 valence electrons Family includes nonmetals, metalloids & metals

Oxygen Group (Group 16)

All have 6 valence electrons

Electromagnetic Spectrum

All of the frequencies or wavelengths of electromagnetic radiation All electromagnetic radiation moves at speed of light

Enthalapy of Vaporization

Amount of heat required to convert one mole of a metal to its vapor (+)Heat of vaporization = (+)strength of metallic bond

Chemical Bond

An attractive the force that holds atoms or ions together 3 types: ionic, covalent, metallic Bonds determine structure of the compound Structure affects properties (boiling point, conductivity)

Principles: Aufbau Principle

An electron occupies the lowest-energy orbital that can receive it Diagonal Rule: chart including 1s, 2s, 2p, 3s, 3p... (inside out: left = lower, right = higher)

Stable Ion

An ion with a full energy sublevel When they want to get to its octet Example: Ca^+2

Black Body Radiation

An object heated & giving off light doesn't do it in a continuous way but in small packets of energy called photons (light is made of photons) This is where Ephoton = h x v comes from

Homogenous Mixture

Any combination of substances that has uniform composition and properties; a mixture that is uniform throughout One would not see different things

List the derived measurements with their respective units

Area - m^2 Volume - m^3 Density - kg/m^3

Electron Cloud

Area around nucleus of an atom where the atom's electrons are most likely to be found

Switches Between Mendeleev's & Moseley's Periodic Tables

Argon & Potassium (Ar & K) Cobalt & Nickel (Co & Ni) Tellurium & Iodine (Te & I) Thorium & Protactinium (Th & Pa)

Shielding

As more inner energy levels are added to atoms, the inner layers of electrons shield the outer electrons form the nucleus Effective nuclear charge (ENC) on outermost electrons (valence electrons) is less = outer electrons are less tightly held

1 amu

Atomic Mass Unit Exactly 1/12 the mass of a Carbon-12 atom

The first & most important elemental property is __________

Atomic radius

Isotope

Atoms of the same element that have different numbers of neutrons

What rule uses the chart with arrows?

Aufbau Principle's Diagonal Rule

Explain how basic units & derived are different & how they are alike

Base Measurements: Length, mass, time, amount/count of substance & temperature Derived Measurements: Area, density & volume Relationship: Need basic unit to measure derived Basic: get by 1 significant measure Derived: get by 2 or more basic measurements

What were the shortcomings of Bohr's model?

Bohr only experimented with hydrogen & he did not explore other elements

Bohr's Atomic Model vs Quantum Mechanical Model

Bohr's Atomic Model: (partially disproved) 1. Only accurate for hydrogen 2. Uses "orbit," says that electrons move in specific paths with different specific amounts of energy 3. 2 dimensional, only uses n=1, n=2, n=3 - Quantum Mechanical Model: 1. Applies to every element 2. Uses "orbitals," a 3 dimensional region of electrons 3. Includes 4 quantum numbers

How would you separate salt from the water in a sample of sea water?

Boil water first. They are only physically mixed & not chemically combined so this method is acceptable. Boil until it evaporates

Ionic Bond

Bond formed by the attraction between oppositely charged ions Cation: Positive, lost electrons Anion: Negative, gained electrons Oppositely charged ions attract each other & form ionic bond Example: Na^+ + Cl^- = NaCl Electrons are transferred from one atom to another Negative ions attract more positive ions & a network is formed Ionic compounds result when metals react with nonmetals

Semiconductors

Boron, silicon, germanium, arsenic, antimony, tellurium

Criteria that determines if a substance is considered a pure substance?

Can't be separated Can't be decomposed by ordinary means

What is used as the standard to determine relative atomic mass? What are the units used when talking about a single atom or molecule?

Carbon-12 is standard Atomic mass units (amu)

Name at least 2 isotopes that are useful to us & why

Carbon-12: standard for finding atomic mass Carbon-14: carbon dating

Atomic Nucleus

Center of atom Central part of atom that contains both protons & neutrons

Physical change or chemical change? A tree is chopped down

Chemical Alive tree will begin to decompose

Physical change or chemical change? Leaves changing color in the fall

Chemical Chemicals change in leaves, as nutrients drain into tree's branches, trunk, & roots for winter storage, causing the leaves to stop producing the green pigment in chlorophyll

Physical change or chemical change? Gasoline is burned in a car engine

Chemical Combustion of gasoline makes water and carbon dioxide Chemical bonds are being broken

Physical change or chemical change? Iron nail rusts in water

Chemical Iron is oxidized (iron oxide) Turns into a compound

If you leave an apple slice on the counter, it reacts with the air & turns brown. Is this a physical change or a chemical change? Why?

Chemical The apple reacts with oxygen due to oxidation & reactivity

Plants use carbon dioxide, water, & sunlight to produce their food. Is this a physical or chemical change? Why? What is the process called?

Chemical Change Photosynthesis Water + carbon dioxide = glucose & oxygen (new chemical species are formed)

Gold coins have been known to lie on the bottom of the ocean unchanged by the environment for hundreds of years after a shipwreck. Would this be a physical or chemical property? Why?

Chemical Property In terms of reactivity, it does not react

Covalent Bond

Chemical bond where 2 atoms share a pair of valence electrons Can be single, double, or triple bond (Single: 2 electrons, double: 4 electrons, triple: 6 electrons) Molecules are always covalently bonded *Always formed between nonmetals* Lower melting points 2 Types: 1. Nonpolar: Bonded atoms that share electrons equally. The same atoms are bonded (or very similar) Example: Cl—Cl = Cl2 2. Polar: Bonded atoms that don't share electrons equally. Different atoms bond Example: H—N—H (pretend there is another H atom bonded to N, underneath)= NH3

Aristotle's Theory

Classical elements were air, water, fire & earth ("the elements alone or combined make up everything") There are very few elements that don't combine

Octet Rule

Completely filled s & p orbital (valence electrons) = 8VE. Very stable & unreactive Exception is helium (1s) because there is no p - its s is filled & it is stable with 2 (full!) (helium is most stable & unreactive)

Element, compound, heterogenous mixture, or homogenous mixture? CH4

Compound

Element, compound, heterogenous mixture, or homogenous mixture? Ethyl Alcohol

Compound

Element, compound, heterogenous mixture, or homogenous mixture? Water

Compound

________ (compounds/mixtures) can be broken down into simpler substances only by chemical change

Compounds

Compounds & mixtures can both be broken down into simpler substances. Explain how this happens for each type of matter

Compounds decompose (chemical change) with the use of heat & mixtures can be separated using filtration (separation by particle size), vaporization (separation by boiling/etc), floatation (separation of solids by different densities), magnetism (separation by magnetic field attractions, "pulled" out of mixture), mechanical separation (separation by hand or tool if large enough), paper chromatography (for mixtures that have components that "stick" to materials in different ways, separation by inner molecular attractions)

Wave

Continuous & has a form or pattern Described by a few properties with dimensions: wavelength (length of 1 cycle), frequency (how often wave crest passes) & amplitude (height above "rest position" Light is a part of electromagnetic spectrum

Molecules are __________

Covalent

Polyatom

Covalently bonded large share atoms

If a block of stainless steel has a mass of 400g & measures 4cm by 4cm by 3cm, what would its density be? If the block was cut exactly in half, what would be the density of each piece?

Density = mass / volume D = 400 / 4 x 4 x 3 D = 400g / 48 D = 8.3g / mL If you cut a block of stainless steel in half, you would have two bars with half the mass of the original bar The density of stainless steel does not change

Calculate the density of a piece of wood if it has a mass of 750 grams & dimensions of 12cm x 0.6cm x 1.8cm

Density = mass / volume D = 750g / 12.96cm 57.87g / mL or 60 g/mL Same

Why is density such an important measurement in chemistry? When the density of a substance is compared to water what can that tell us?

Density is an intensive property It tells whether an object will float or sink

Quantum Theory

Describes mathematically the wave properties of electrons & other very small particles

Stanislao Cannizzaro

Developed a method that led to the determination of standard relative atomic masses

Periodic Table: Blocks

Diagram

Electron Dot Diagram

Diagram that uses the element symbol to represent the nucleus & inner electrons. Dots surrounding the symbol represent the valence electrons

Lewis Structure

Diagram using electron dot notation for molecules. Element symbol represents the nucleus & all inner electrons. Dots between atoms (or dash) are shared by each other. Electrons not shared are shown as dots Center element should be the one that needs to gain the most valence electrons to fulfill octet Single Bond: 1 shared pair of electrons (dash = 2 electrons) Double Bond: 2 shared pairs of electrons Triple Bond: 3 shared pairs of electrons Dashes in the center = 2 electrons Outside dashes = 1 electron Example: H2O

Helium

Does not have 8 valence electrons In Group 18 (noble gas) because it's extremely stable

Filtration is a separation technique often used. Give a minimum of 3 ways it's used every day life

Drinking Water: every day water is filtered out from lead & other wastes Pasta: boiled in water until water is filtered out using a drain Sunglasses: the light from the sun is limited in ways that the glasses protect you/filter out UV rays

Quantum Mechanical Model

Electrons are located in specific energy levels No exact path around the nucleus Region = orbital The model estimates the probability of finding an electron in a certain position

Valence Electrons

Electrons that are lost, gained, or shared in chemical bonding (Location) Electrons in the highest principle quantum number (highest energy level) Create bonds

Element, compound, heterogenous mixture, or homogenous mixture? Gold

Element

Element, compound, heterogenous mixture, or homogenous mixture? Mercury

Element

Anion Names

Element - last 3-4 letters + ide Flouride, Oxide, Nitride What does this even mean

Isotope Notation: Hyphen-Method

Element-(fill in element's mass number here)

________ (elements/compounds) are pure substances that cannot be broken down further

Elements

Is a mixture a pure substance? Why/why not?

Elements & compounds are always the same but not in a mixture. Mixtures are physically mixed & are not chemically combined Can be chemically separated

When is a sample of matter considered a pure substance?

Elements & compounds. When it cannot be broken down into simpler, stable substances & is made of 1 type of atom

Are elements & compounds pure substances? Why/why not?

Elements are pure substances because they are made of only one type of atom Pure substances are joined chemically. Water, a compound, is composed of two different elements, which are pure substances, an oxygen chemically bonded to two hydrogen atoms Elements & compounds are always the same

Reactive Elements

Elements that are reactive bond easily with other elements to make compounds Incomplete valence electron level All atoms want to have 8 electrons in outmost energy level (octet rule) Atoms bond until level is complete (few valence electrons lose them during bonding, 6, 7, or 8 gain)

Element vs compound?

Elements: cannot be broken down Compounds: can be broken down by chemical processes

The Law of Conservation of Energy

Energy cannot be created or destroyed; it only changes form

Lattice Energy

Energy given off when 1 mole of an ionic compound forms (+)Energy = (+)strength of bond

Bond Energy

Energy needed to break a molecular compound Shorter bond = (+)energy needed Example: Breaking a stick is harder when it's short

Ionization Energy

Energy needed to remove an electron from an atom Measured in kilojoules (KJ) A(atom) + energy → A(atom)^+ + electron The atom has been ionized or charged Represents noble gases Does not represent f & d blocks

Formula/Relationship: Energy of a Photon

Ephoton = hv Ephoton = Planck's Constant, 6.626 x 10^-34 J/s x Frequency

What groups or blocks are missing on both?

F & d blocks Rare earth metals (Lanthanides & Actinides) & transition metals

Electronegativity Difference Between Different Atoms Bonded Together (Ionic, Polar, or Nonpolar)

Find the difference between elements using their electronegativity & categorize: I, P or NP Nonpolar: 0 to 0.3 Polar: 0.3 to 1.7 Ionic: 1.7 to 3.3 Polar & ionic are covalent

Group 13-16 are named after their __________

First element Group 13: Boron Group Group 14: Carbon Group Group 15: Nitrogen Group Group 16: Oxygen Group

Molecular Formula

Formula showing the number & types of elements that are covalently bonded

Alkali Metals

Group 1 1 valence electron Never found pure in nature (always bonded with another element) Shiny, soft, very low density, very low melting point in pure state Most reactive of metals Reacts violently with water (explodes & catches on fire) Example: sodium

Halogens

Group 17 Right before noble gases 7 valence electrons To stabilize to octet, they gain 1 electron Most active nonmetals Never found alone in nature Very aggressive & reactive Reacts with alkali metals to make salts All nonmetals Bromine is the only nonmetal liquid at room temperature & mercury is the only metal at room temperature Example: Fluorine, chlorine, bromine

Noble Gases

Group 18 All colorless, odorless gases Extremely unreactive Inactive because their outermost energy level is full Do not readily combine with other elements to combine as compounds so they are called inert All are found in small amounts on earth's atmosphere Much more unreactive than transition metals Argon is used a lot, #3 in the atmosphere

Alkaline Earth Metals

Group 2 2 valence electrons Never found pure in nature Harder, denser, higher melting temperatures than Alkali Metals Example: magnesium, calcium

Transition Metals

Groups 3-12 Largest group Entire d-block 1-4 valence electrons lost in bonding Good conductors of heat & electricity (metallic properties) Some can be found pure in nature (unreactive, Au, Ag, Cu, Co) Compounds are usually brightly colored & often used in color paints Least reactive metals, greatest density, hardest & highest melting temperatures Many combine with oxygen to form compounds called oxides (corrosion = presence of water/moisture weakens metals themselves) Example: copper, zinc, gold, nickel, silver, iron (copper, gold & silver can be found alone)

Diatomic Molecule: 7 Elements

H, O, F, N, Br, I, Cl (H2, 02, F2, Br2, I2, Cl2) Think: HOFNBriCl = "peanut brittle"

Covalent Radius

Half the distance between the nuclei of 2 bonded atoms Atomic radii are usually measured in picketers (pm) 1 x 10^-12m, or angstroms (Å) 1 x 10^-10m Example: 2 Br atoms bonded together are 2.85 angstroms apart, so the radium of each atom is 1.43 Å

Element, compound, heterogenous mixture, or homogenous mixture? Carbonated Beverage

Heterogeneous

Element, compound, heterogenous mixture, or homogenous mixture? Raisin Bran

Heterogeneous

Beta Particle

High-speed electron emitted in the decay of a radioactive isotope Has a charge of -1 Results in same mass number & an increase in atomic number by 1 Stopped by aluminum foil Emission is the most charged

Element, compound, heterogenous mixture, or homogenous mixture? Air

Homogeneous

Element, compound, heterogenous mixture, or homogenous mixture? Milk

Homogeneous

Element, compound, heterogenous mixture, or homogenous mixture? Stainless Steel

Homogeneous

Periodic Table: Periods

Horizontal row Left & right

Malleability

How metals can't be broken even when molded/bent into different shapes Electrons allow atoms to slide by The ability of a metal to be hammered into shape

What rule can be described as electrons not liking each other so they spread out whenever they can?

Hund's Rule

What has to happen for visible light to be emitted from a tube of hydrogen gas?

Hydrogen gas must be excited by heat or electricity

How can you tell if a molecule is polar or nonpolar using its generic formula?

If the difference in electronegativity for the atoms in a bond is greater than 0.4 OR find its geometry/shape Is it symmetrical? If so, it is nonpolar *Linear* SYMMETRICAL - nonpolar Bent/Angular - polar *Trigonal Planar* SYMMETRICAL - nonpolar Trigonal Pyramidal - polar *Tetrahedron* SYMMETRICAL - nonpolar

Hydrogen

In Group 1, but it is not a metal Unique element Gas at room temperature Has 1 proton & 1 electron in its one & ONLY energy level Needs 1 more electron to fill its valence shell / s orbital 1 valence electron

Ionic Compounds: Nonmetals

In ionic compounds, nonmetals in 15, 16 & 17 gain electrons from metals Anions (negatively charged) → nonmetals add electrons to achieve octet Hydrogen is an exception Nonmetal ionic charge: 3-, 2-, or 1- Electrostatic Attraction: Between atoms of metals & nonmetals with very different electronegativity, formed by transfer of electron Examples: NaCl, CaCl2, K2O 1. Opposite charges 2. Electrostatic Attraction 3. Very structured arrangement

3 Intermolecular Forces

In order of DECREASING strength 1. H-Bonding (Hydrogen Bonding) 2. Dipole-Dipole 3. London Forces

In the Lewis Structure, dashes in the center equal __________ & outside dashes equal __________

In the Lewis Structure, dashes in the *center equal 2 electrons* & *outside dashes equal 1 electron*

Formula/Relationship: l, Sublevel & Shape

In the order of l, sublevel & shape 0, s, sphere 1, p, dumbell 2, d, flower 3, f, complex 4, g

Quantum Numbers: Principle Quantum Number

Indicates main energy level n = 1, 2, 3... infinite Describes how large a region is & proximity to nucleus Each main energy level has sublevels

Quantum Numbers: Orbital/Angular Momentum Quantum Number

Indicates shape of orbital sublevels l = n - 1 is directly connected to principal quantum

Quantum Numbers: Magnetic Quantum Number

Indicates the orientation of the orbital in space Values of m'sub l integers from -l to l Number of values = number of orbitals Ex: for l = 2, m'sub l is m'sub l = -2, -1, 0, 1, 2

Crystal Lattice Structure

Lattice Structure/Crystal Lattice A rigid framework of ions Caused by strong attraction between each other (ions) Example: cubes, hexagons, tetrahedrons

Period Trends: Atomic Radii, Ionization Energy & Electronegativity

Left to right → (-)Atomic radii (AR) (+)Ionization energy (IE) (+)Electronegativity (EN)

Bond Length

Length of the covalent bond formed between atoms Shorter bond = (+)energy needed Example: Breaking a stick is harder when it's short

Structural Formula

Lewis Structure that only shows the bonds Example: C3H8 Isomer: The same element, but rearranged

Forces That Act on an Atom: Electrostatic Force

Like charges repel & opposite charges attract Holds electrons from flying out in atom Effect is decreased by nuclear force in the nucleus

Problem Solving: How do you find an element's block using its noble gas notation?

Look for the letter of the highest energy level (highest energy level will always be the last level in the notation)

Problem Solving: How do you find an element's period number using its noble gas notation?

Look for the number of the highest energy level (highest energy level will always be the last level in the notation)

Metallic Properties

Malleability Ductility Luster Good conductors of heat & electricity in both solids & liquids

The Law of Conservation of Mass

Mass is neither created nor destroyed during ordinary chemical reactions or physical changes

Problem Solving: How do you find the number of neutrons?

Mass number - atomic number = number of neutrons

Isotope Notation: Nuclear Symbol

Mass number at the top, atomic number at the bottom & element on the right side

Mass Number vs Average Atomic Mass

Mass number is the number of protons & neutrons Average atomic mass is the average mass of all the isotopes of a certain type (weighted average that takes into account the abundances of all of the different isotopes) Weighted average uses the relative abundance ( out of 1, not 100) Out of 100 is a %

Compare & contrast mass & weight

Mass: measure of how much matter is in a substance & never changes Weight: measure of gravitational pull & can change depending on pull

Electronegativity

Measure of the tendency of an atom to attract a bonding pair of electrons Fluorine (F) is highest (king of the hill) Cesium is lowest (Cs) Does not represent noble gases or f & d blocks

If the nucleus was the size of a marble, how big would the outside edge of the atom be? What does most of an atom consist of?

Met stadium parking lot Empty space (absolutely nothing)

Give the 5 basic unites of measurements used in chemistry in the SI system, what quantity is being measured, the symbol & what is used to measure each

Meter - (m) - Length Kilogram - (kg) - Mass Second - (s) - Time Mole - (mol) - Amount/Count Kelvin - (°K) - Temperature

Intermolecular Forces: Dipole-Dipole Attractions

Molecules have a separation of charge Happens in BOTH ionic & polar bonds (+)Electronegativity = (+)strength of dipole *Molecules are attracted to each other in a compound by these positive & negative forces. If not, all molecules would be gases* Molecules add up * stick together when negative attracts to positive

Ionic Radii: Anion

Negative, gains 1 or more electrons Anion is always LARGER than parent atom

Electron

Negatively charged subatomic particle

Neutron

Neutrally charged subatomic particle Inside nucleus of an atom

Principles: Pauli Exclusion Principle

No two electrons in the same atom can have the same set of four quantum numbers

The sodium atom has 11 electrons. If the outermost electron is in the 4s orbital, would this atom be considered in the ground state?

No, the outermost should have been 3s^1 (lowest state), but because it continued to move up to 4s^1, the atom is in the excited state

What group is represented on ionization energy but not on electronegativity?

Noble gases are not in electronegativity

Why are the noble gases used for shortcut notation?

Noble gases are stable & nonreactive (helium is the most stable & unreactive) Each one completes an energy level

__________ is the only nonmetal liquid at room temperature __________ is the only metal liquid at room temperature

Nonmetal: bromine Metal: mercury (cohesion = sticks to itself)

Nonmetals __________ to achieve octet Metals __________ to achieve octet

Nonmetals *gain* to achieve octet Metals *lose* to achieve octet

Gamma Rays

Not charged particles like alpha & beta Electromagnetic radiation with high frequency

Why are some isotopes unstable?

Nucleus is too big, as there are too many protons & neutrons Increasing distance between proton (+)nuclear force increases = (-)electrostatic = (-)stability & strength Typically heavier isotopes

Mass Number

Number of protons & neutrons combined

Nuclear Charge

Number of protons = atomic number in the nucleus Size of nucleus What holds electrons from zipping out (electrostatic force)

Atomic Number

Number of protons in an element

Arrangement of Electrons in Atoms: Electron Configuration Notation (ECN)

Orbital notation but replaces arrows with superscripts

Sublevels

Orbitals of different shapes

Principles: Hund's Rule

Orbitals of equal energy are each occupied by one electron before any pairing occurs Electrons will spread out if they can without going to a higher energy orbital (Electrons will have the same spin direction in each of the orbitals they occupy individually)

Problem Solving: How do you find the amount of a radioisotope remaining after decay if the number of half-lives is given?

Original amount of radioisotope * (0.5^# of half-lives)

Problem Solving: How do you find the amount of a radioisotope remaining after decay if the number of half-lives is not given?

Original amount of radioisotope x 0.5^(time passed / half-life length)

Elements in the same column have the same __________

Outer shell electron configuration (valence electrons) Picture: periodic table energy levels (Aufbau)

Wave-Particle Duality: Characteristics

Particle: 1. Photoelectric Effect 2. Black Body Radiation - Wave: 1. Diffraction 2. Interference of matter waves 3. Continuous 4. Wavelength & frequency

What rule can be compared to no 2 people having the same fingerprints?

Pauli Exclusion Principle

Physical change or chemical change? Paper is cut into small pieces

Physical It is still paper, at different sizes & shapes

Physical change or chemical change? You sharpen your pencil

Physical Pencil stays the same

Physical change or chemical change? Gaseous CO2 is made a solid

Physical Phase change, not composition change

Physical change or chemical change? Water boiling

Physical Phase change, the water is changing forms & becomes water vapor but it is still water

You drop a glass on the floor & it breaks into tiny pieces. Is this a physical change or a chemical change? Why? Name physical properties & chemical properties of the glass

Physical The glass did not change into new substance, it just changed shape & broke apart, nonetheless still glass Physical Properties: hardness, texture, transparency Chemical Property: brittle, not reactive to most substances

Physical change or chemical change? Dissolving sugar in water

Physical They do not chemically combine to form a new substance

Ionic Radii: Cation

Positive, lose 1 or more electrons Cation is always SMALLER than parent atom

Proton

Positively charged subatomic particle Inside nucleus of atom

Explain the difference between precise measurements and accurate measurements. Give an example of each

Precise: how close values are together Ex: three arrows hitting a similar area on a target consecutively, though may not be bulls-eye Accurate: how close value is to accepted value Ex: arrow hitting bulls-eye on target

Radioactive Decay

Process in which an unstable atomic nucleus loses energy by emitting radiation in the form of a particles or electromagnetic waves Elements that undergo this process are called radio types or radioactive nuclides

Why is the proton used to identify an atom & not the other subatomic particles? What is this identifier called?

Proton, because it directly connects to its atomic number. When you change the number of protons, you also change the element completely Identifier: Atomic number

Why don't atoms have a charge?

Protons & electrons have equal but opposite charges. Therefore, they cancel out

In a ________ (pure substance/mixture) all samples of matter have the same properties

Pure substance

Compare qualitative and quantitative measurements. Give an example of each & an advantage of each

Qualitative: describe without numbers Ex: "the sky is blue" (+)used by senses = quick & easy to use Quantitative: describe with numerical values Ex: the amount of mass is a single grape (+)numerical value = exact & reliable

Intermolecular Forces: London Dispersion

Question: Nonpolar molecules do not have dipoles like polar molecules. How then, can non polar compounds form solids or liquids? London forces (Van der Waals forces) are due to small dipoles that exist in nonpolar molecules Because electrons are moving around in atoms, there will be instances when the change around an atom is not symmetrical; The resulting *tiny, temporary dipoles cause attractions between atoms/molecules* (+)MASS = (+)LONDON FORCES (+)Intermolecular forces = (+)melting & boiling point (the more energy it takes to overcome them)

Beta Decay

Radioactive decay in which a beta particle is emitted Occurs when neutron changes into a proton & electron As a result, the nucleus has one less neutron, but one extra proton Mass number stays the same Atomic number increases by 1

Gamma Decay

Radioactive decay where atom releases gamma rays

Visible Spectrum

Red, orange, yellow, green, blue, indigo, violet (ROYGBIV)

Problem Solving: How do you find the number of electrons?

Refer to the number of protons. The number of protons is equivalent to the number of electrons

Network

Repeating pattern of multiple ions Example: NaCl Every Na ion is next to 6 Cl ions

What were the shortcomings of Rutherford's model?

Rutherford only explained the nucleus & did not explain the electron

Formula/Relationship: Diagonal Rule Key (Orientations)

S = 1 orientation P = 3 orientations D = 5 orientations F = 7 orientations

Explain why a beaker containing sand & water is a mixture although sand itself is a pure substance

Sand & water do not mix smoothly enough to form a new substance. They just stay in the beaker together (They retain their own identities & properties, & are not chemically combined)

Mendeleev's Predicted Elements

Scandium (Sc), Gallium (Ga) & Germanium (Ge)

Scientists: Packet of Energy Called a Quantum

Schrödinger

Number of Elements Today

Scientists have identified 90 natural naturally occurring elements & made 28 synthetic

Relationships: Bond Energy & Bond Length

Shorter bond = (+)energy needed Example: Breaking a stick is harder when it's short Inversely proportional

Formula Unit

Simplest whole number ratio of cations to anions in an ionic compound Example: NaCl, CaF2

Ionic Radii

Size of an ion Cation: Positive, lose 1 or more electrons Anion: Negative, gains 1 or more electrons

Electron Shell

Specific area where electrons of the same energy level are found

Quantum Numbers: Overview

Specify the properties of atomic orbitals & the properties of electrons in orbitals Describe atomic orbitals & electrons in atoms Similar to an address (n, l, m'subscript l, m'subscript s)

Formula/Relationship: Shape Orientations

Sphere = 1 orientation Dumbell = 3 orientations Flower = 5 orientations Complex = 7 orientations

Why are standards important in measurement? What are the standards of each of the SI measurements?

Standard units are forever: they will be used thousands of years from now & are therefore reliable & greatly agreed upon Length - Meter Mass - Kilogram Time - Second Amount/Count - Mole Temperature - Kelvin

__________ determine the amount of periods

Sublevels (s = 2, p = 6, d = 10, f = 14) *THIS IS SUPER COOL, CHECK THE BLOCKS*

Element

Substance that cannot be broken down into simpler substances by chemical means Composed of atoms that have the same atomic number (each atom has the same number of protons in its nucleus as all other atoms of that element)

Speed of Light

Symbol: (c) 3.00 x 10^8 m/s All electromagnetic radiation moves at speed of light

Planck's Constant

Symbol: (h) 6.626 x 10^-34 J/s

Wavelength

Symbol: (λ) The distance between corresponding points on adjacent waves Inverse relationship with frequency

Frequency

Symbol: (ν= Greek letter Nu) The number of complete wavelengths that pass a point in a given time Inverse relationship with wavelength

The __________ intermolecular forms are, the __________ the melting & boiling point

The *stronger* intermolecular forms are, the *higher* the melting & boiling point (the more energy it takes to overcome them)

Ductility

The ability of a metal to be drawn into wire

Mendeleev's Table to Modern Table: In Between

The addition of 27 elements (Duh) (63 + 27 = 90)

Electron Configuration

The arrangement of electrons in an atom

Refraction/Diffraction (?)

The bending of a wave as it moves around an obstacle or passes through a narrow opening due to change of speed Example: bending spoon illusion, white light

Radius

The distance from the center of the nucleus to the edge of the electron cloud Since a cloud's edge is difficult to define, scientists use covalent radius

Continuous Spectrum

The emission of a continuous range of frequencies of electromagnetic radiation

The Photoelectric Effect

The emission of electrons from a metal when light shines on the metal Einstein

Ground State

The lowest energy state of an atom

Why is the mass number an integer & average atomic mass a decimal?

The mass number is the number of protons & neutrons, which come in whole numbers & average atomic mass is the weighted average of all the different isotopes

Quantum

The minimum amount of energy that can be gained or lost by an atom

Periodic Law

The properties of the elements are periodic functions of their atomic numbers When elements are arranged in order of increasing atomic number (mass during Mendeleev's time), their physical & chemical properties show a predictable periodic pattern The properties of yet undiscovered elements can be predicted based on their apparent location on the periodic table (columns) The recurring pattern of trends in the periodic table makes the periodic table periodic. As you go through a column, you'll see that there is a recurring pattern in their physical & chemical properties. You can also predict what other elements the element can chemically react with

The Law of Definite Proportions

The proportion of elements in any compound is always the same

Effective Nuclear Charge

The pull that an electron feels from the nucleus How the pull is acting (-)Distance to nucleus (closer) = (+)pull it feels (+)Effective nuclear charge = (+)tighter the electron cloud is pulled Effective nuclear charge (ENC) on outermost electrons (valence electrons) is less = outer electrons are less tightly held 2 Factors: 1. The distance the nucleus is from the valence electrons 2. Shielding: inner electrons that shield the nucleus from pull on valence electrons *Little shielding + little distances = decreases pull

Why makes the periodic table periodic?

The recurring pattern of trends in the periodic table makes the periodic table periodic. As you go through a column, you'll see that there is a recurring pattern in their physical & chemical properties. You can also predict what other elements the element can chemically react with by just its location

Isomer

The same element, but rearranged Structural formula

Arrangement of Electrons in Atoms: Exceptions in Notations

These elements will want to become as stable as possible, so it possible for an extra arrow to shift into the next energy level; arrow shifts to the next energy sublevel because shells want to be either half filled or completely full Exceptions: Cr(24), Cu(29) & Ag(47)

Why do atoms bond?

To form a full octet, or fill the outermost energy level through gaining, losing, or sharing electrons Exception: Helium has 1 electron & will want 2 = duet Noble gases don't bond because they already have octet

Hertz (Hz)

Unit of frequency, = waves/second

Group Trends: Atomic Radii, Ionization Energy & Electronegativity

Up to down ↓ (+)Atomic radii (AR) (-)Ionization energy (IE) (-)Electronegativity (EN)

How do you know which element to put in the center of the Lewis Structure?

Use the element that needs to gain the most valence electrons to fulfill octet

Arrangement of Electrons in Atoms: Noble Gas Notation

Uses a noble gas in brackets to show the inner electrons & then the remaining electrons are shown in regular ECN notation Choice of noble gas must be the nearest atomic number to the element & should be slightly smaller than it

Arrangement of Electrons in Atoms: Orbital Notation

Uses blanks to represent orbitals & arrows to represent electrons

Periodic Table: Groups

Vertical columns (families) Up & down

Metallic Bonding

Very few metals can be found in nature alone (gold, silver, copper) Occurs between like atoms of a metal in the free state (not in compound, pure) Example: zinc atoms, silver atoms Reasons For Their Properties: 1. *Valence electrons are mobile,* as they are held very weakly by their nuclei (low ionization energy) 2. *D orbitals* have a lot of room to move around in It's a sea of freely flowing electrons held loosely by their nuclei

Water & gasoline are mixed together. How would you separate these 2 liquids? What property/properties make this possible?

Water is less dense so it would rise. Gas & water do not mix, so you can boil the mixture & wait for the water to vaporize

If a person was standing at sea level then traveled to top of Mt. Everest, what would change: the person's mass or weight? Why?

Weight Gravitational pull is not always the same Mass is not affected

Emission

When an electron falls from a higher energy level to a lower energy level & a photon is emitted Energy of each absorbed or emitted photon corresponds to a particular frequency, which is where we get Ephoton = h x v (used for particles) Electrons move down = emit Opposite: absorption

Why is it better to organize the periodic table by atomic number & not atomic mass?

When changing an atomic number (number of protons/electrons), you completely change the element. Because the atomic number never changes, it is more useful in regards to organization. In addition, the different isotopes of an element create overlaps when based on atomic mass

Absorption

When energy is added & an electron moves from a lower energy level to a higher energy level Energy of each absorbed or emitted photon corresponds to a particular frequency, which is where we get Ephoton = h x v Electrons move up = absorb Opposite: emission

What is the photoelectric effect & how does it help support the particle characteristics of light?

When light hits metal, electrons are released, showing it takes a certain amount of energy to excite electrons, which is done using photons that each have a quantum of energy

S Block

Who has the time to read this

2nd Ionization Energy

Will take an ion & add energy to remove a second electron A^+ + energy → A^+2 + electron This process can continue until the ion reaches stability (+)Larger atom = (+)Ease for electrons to move

If x-rays have shorter waves compared to microwaves, why are we more concerned with the former than the latter?

X-rays have shorter waves, but higher frequency, which means that they have a high amount of energy Microwaves have longer waves, but have lower frequency, which means that they have a lower amount of energy (Wavelength & frequency have an inverse relationship = high energy is bad)

Problem Solving: Determine Group, Period & Block of [Ar(18)]4s^2-3d^10-4p^5

[Ar(18)]*4*s^2-3d^10-*4*p^5 Group 17 (add all electrons outside of brackets) Period *4* (highest energy level number) P block (highest energy level letter)

Problem Solving: Determine Group, Period & Block of [Kr(36)]5s^2-4d^10

[Kr(36)]*5*s^2-4d^10 Group 12 (add all electrons outside of brackets) Period *5* (highest energy level number) D block (highest energy level letter)

Problem Solving: Determine Group, Period & Block of [Xe(54)]6s^1

[Xe(54)]*6*s^1 Group 1 (add all electrons outside of brackets) Period *6* (highest energy level number) S block (highest energy level letter)

Formula/Relationship: n & l

l = n - 1

Formula/Relationship: Total Number of Orbitals

n^2

Formula/Relationship: Total Number of Electrons In Energy Level

n^2 x 2