AP Chemistry Exam Study

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what is te equation for second order reaction

(1/[A]t)=kt + (1/[A]₀)

molarity

(symbol M) expresses the concentration of a solution as the numbers of moles of solute in a liter of solution

parts per volume

(volume of solute/volume of solution) x multiplication factor

Cation

+ lost e-

1 lb

16 oz

Di-

2

What is a physical property?

A characteristic that can be observed or measured without changing the identity of the substance

What is an element?

A pure substance made of only one kind of atom

Quantum

A small unit/package/amount of energy & amount of energy determines how electrons behave.

Aluminum

Al³⁺

CO

Carbon Monoxide

D

Carbon dioxide, CO2(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

CO3 2-

Carbonate

CO₃²⁻

Carbonate

Calcium

Ca²⁺

chlorite

ClO2-

Cr2O7 2-

Dichromate

KJ/mol

Electron affinity is measured in...

Argon

First noble discovered

F

Fluorine

Au

Gold

Hydrogen

H⁺

49. Indium

In

potassium

K⁺

Element

Made up of atoms with the same number of protons. Can not be broken down.

C

Methane, CH4(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

12. Magnesium

Mg

Magnesium

Mg

Magnesium

Mg²⁺

Hydroxide

OH⁻

Niels Bohr

Proposed dual nature of electrons

Tin

Sn

Sulfide

S²⁻

SCN⁻

Thiocyanate

What statement is not correct about Torr

Torr was named for the Italian scientist Torricelli

Vacuum

Used in combination reactions to ensure that only the two substances will react (that there is no air or oxygen present to interfere with the reaction).

B

When a hydrate of Na2CO3 is heated until all the water is removed, it loses 54.3 percent of its mass. The formula of the hydrate is (A) Na2CO3 . 10 H2O (B) Na2CO3 . 7 H2O (C) Na2CO3 . 5 H2O (D) Na2CO3 . 3 H2O (E) Na2CO3 . H2O

Paramagnetic

When the last e- placed spin the same direction

Au

gold

If increase reactants will also _____ proucts

increase

from arrhenius equation, catalysts _____k by _____A or _____ activation NRG

increase; increase (increase frequency of collisions with correct orientation

2 electron domains equals...

linear

Rb

rubidium

molecular equation

when the complete chemical formulas of all reactants and products are used

dynamic equilibrium

when the rates of dissolution is equal to the rate of recrystallization

Schrodinger's equation requires 3 quantum numbers which tell about....

where are electron is located

electron domain looks at....

where the electrons are, not the atoms (includes lone pairs)

if the graph represents the behavior of a gas under ideal conditions, which properties are represented on each axis?

x= V , y=P

Xe

xenon

Zn

zinc

"ites" (SO₃²⁻, NO₂⁻)

"ates" (SO₄²⁻, NO³⁻)

Subscript

# after an element in a compound. Used to balance the charge in a compound.

Coefficient

# in front of the substances in a chemical reaction. Created to balance # and types of atoms on both sides of equation.

Frequency

# of waves that pass through a given point in 1 second.

energy of an electron

(-k*z^2)/n^2

give rate in terms of each product: 2NO2----->2NO + O2

(1/2)(change in NO)/(change in time) = (change in O2)/(change in time) = -(1/2)(change in NO2)/(change in time)

mega

(M) million

Solution

(all do) solute+ solvent, homogeneous mixture, dilute

percent by mass

(mass of solute/mass of solution) x 100%

parts per million (ppm)

(mass of solute/mass of solution) x 10⁶

parts per billion (ppb)

(mass of solute/mass of solution) x 10⁹

parts by mass

(mass of solute/mass of solution) x multiplication factor

Δ E =

(q + w) or (q - PΔV) or (ΔH - PΔV)

Group 1 ox #

+1

Hydrogen ox #

+1

Group 2 ox #

+2

The charge of an alpha particle

+2

Hydrogen in a metal hydride ox #

-1

Halide ions ox #

-1 except when combined with a more electronegative element

Electrons

-1 charge, shared between atoms through chemical bonds.

Peroxide ox #

-1 for each O

Oxide ion ox #

-2

Equation for calculating the change in energy of an electron making a transition from one energy level to another

-2.18⋅10⁻¹⁸J (1/n²final - 1/n²initial)

slope of zero order line?

-k

ΔE =

-k*z^2*(1/n^2f - 1/n^2i) = hv = hc/λ

Micro

.000001 10 to the -6th power

Milli

.001 10 to the -3rd power

Centi

.01 10 to the -2nd power

Deci

.1 10 to the -1st power

ΔQ1 + ΔQ2 + ΔQ3 + ... =

0

what are the values of l?

0 to n-1

What is the highest NRG possible for an orbital?

0 when n=∞

What are the letters of l?

0-s; 1-p, 2-d, 3-f

a sample of gas has a volume of 250 ml at 2.10 atm and 227* C. What volume will the gas have at standard temperature and pressure?

0.287 liters

A tank contains both nitrogen and hydrogen gas. If the partial pressures are 190 mmHg and 303 mmHg respectively, what is the mole fraction of nitrogen?

0.385

Mono-

1

hypo____ite

1 Oxygen Atom

Ion

1 elem has to have a charge

4 qts

1 gal

paramagnetic...

1 or more electron not paired, attraction to magnetic field

Decimeter

1 x 10^-1

Picometer

1 x 10^-12

Femtometer

1 x 10^-15

Centimeter

1 x 10^-2

Millimeter

1 x 10^-3

Micrometer

1 x 10^-6

Nanometer

1 x 10^-9

Kilometer

1 x 10^3

Megameter

1 x 10^6

Gigameter

1 x 10^9

Kilo

1,000 10 to the 3rd power

Mega

1,000,000 10 to the 6th power

What are the levels for n on a series diagram?

1,2,3,4,5,6,7, ∞

Naming rules for acid without oxygen

1. Find element in the acid 2. Add prefix hydro- 3. Change element ending to -ic 4. Put "acid" at end

Naming rules for acids with oxygen

1. Find polyatomic's name 2. -ate goes to -ic -ite goes to -ous 3. Put "acid" at end

Naming Rules for Nonmetal-only Compound

1. Greek prefix for number of atoms *No mono- on 1st element 2. Name 1st element 3. 2nd element ends with -ide (NO polyatomic ions)

Naming rules for column 1, 2, and Al, Zn, and Ag

1. Name 1st element 2. 2nd element ends with -ide (polyatomic ion stays the same)

Naming rules for transition elements

1. Name 1st element 2. Roman #s for charge of first element 3. 2nd element ends with -ide (polyatomic ions stay the same)

Kinetic Molecular Theory

1. The size of a particle is negligibly small 2. The average kinetic energy of a particle is proportional to the temperature in k 3. The collision of one particle with another (or with the walls of its container) is completely elastic

Kinetic Molecular Theory of Gases

1. particles are small compared with distances btw them (move fast) 2.Part in a gas- always in motion because they have kinetic energy 3. part are assumed to exert no forces on each other 4. if you increase the temperature, you will increase the speed

1 L

1.06 qts

Rydberg's constant

1.097⋅10⁷ m⁻¹

1 mi

1.61 km

Deca-

10

Deka

10 10 to the 1st power

Hecto

100 10 to the 2nd power

1 L* atm=

101.3 J

1 standard atmosphere =____________pascals

101.325

trigonal pyramidal

107

tetrahedral

109.5

deci

10^-1

pico

10^-12

centi

10^-2

mili

10^-3

micro

10^-6

nano

10^-9

deka

10^1

hecta

10^2

kilo

10^3

mega

10^6

1 ft

12 in

trigonal planar

120

trigonal bipyramidal

120 and 90

trigonal planar bent

120 bond angle

1 atm=_______psi (lb/in2)

14.69

How many grams are in 5 moles of NH₃?

15.5 g

linear

180

trigonal bipyramidal linear

180 bond angles

John Newlands

1864 Arranged elements by mass # Finds repeating properties of elements. Doesn't account for transition metals Breaks down after ca

Demitri Mendleév

1869 Russian Ordered elements by mass # Accounts for transition metals and leaves blank spaces where nothing fits

how many p orbitals are used in sp hybridization and what happens to the others?

1; other two are left unhybridized

Spin = 1/2

1st electron

How many electrons are in an orbital?

2

D

2 K + 2 H2O ---> 2 K+ + 2 OH¯ + H2 When 0.400 mole of potassium reacts with excess water at standard temperature and pressure as shown in the equation above, the volume of hydrogen gas produced is (A) 1.12 liters (B) 2.24 liters (C) 3.36 liters (D) 4.48 liters (E) 6.72 liters

_____ite

2 Oxygen Atoms

Linear

2 e- domains (2 bonding, 0 nonbonding)

What are sp hybrid orbitals?

2 equivalent hybrid orbitals resulted from mixing an s and a p orbital

k =

2.179 * 10^-18 J

1 kg

2.2 lbs

Convert 0.302 atmospheres to torr

230 torr

STP

273 K and 1.00 atm

1 ft^3

28.32 L

electron capacity of an energy level =

2n^2

Spin = -1/2

2nd electron

Tri-

3

p orbitals have ___ orbitals

3

_____ate

3 Oxygen Atoms

Trigonal Bent

3 e- domains (2 bonding, 1 nonbonding)

Trigonal Planar

3 e- domains (3 bonding, 0 nonbonding)

1 yard

3 ft

Angular momentum quantum #

3-D region around nucleus electrons - orbits - orbital

Speed of light

3.00⋅10⁸ m/s

KEavg =

3/2 *R*T

Tetra-

4

Per____ate

4 Oxygen Atoms

Tetrahedral Bent

4 e- domains (2 bonding, 2 nonbonding)

Trigonal Pyramid

4 e- domains (3 bonding, 1 nonbonding)

Tetrahedral

4 e- domains (4 bonding, 0 nonbonding)

What are the shapes of d orbitals?

4 fat clovers and one donut with a dumbbell

1 lb

453.6 g

Penta-

5

d orbitals have ___ orbitals

5

Hexa-

6

E

6 I¯ + 2 MnO4¯ + 4 H2O(l) ---> 3 I2(s) + 2 MnO2(s) + OH¯ Which of the following statements regarding the reaction represented by the equation above is correct? (A) Iodide ion is oxidized by hydroxide ion. (B) MnO4¯ is oxidized by iodide ion. (C) The oxidation number of manganese changes from +7 to +2. (D) The oxidation number of manganese remains the same. (E) The oxidation number of iodine changes from -1 to 0.

What is the hybridization of octahedron and how many are formed?

6 sp³d²

Chemical Mole

6.022x10²³ particles=mass in grams on PT

Planck's constant

6.626⋅10⁻³⁴ J⋅s (h)

Hepta-

7

How many f orbitals are there?

7

1 standard atm=____________mmHg and_______torr

760 mmHg and 760 torr

Pressure units equal to 1 ATM

760 torr = 760 mm Hg = 14.7 psi = 101.325 kPa = 29.9 in Hg

Octa-

8

Nona-

9

octahedral

90

equation for work

=p* change in V

Single replacement

A + BX --> AX + B

C

A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl¯ as AgCl(s) ? (Assume that AgCl is insoluble.) (A) 0.10 mol (B) 0.20 mol (C) 0.30 mol (D) 0.40 mol (E) 0.60 mol

C

A 2.00-liter sample of nitrogen gas at 27 °C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is (A) 68 °C (B) 120 °C (C) 477 °C (D) 677 °C (E) 950. °C

C

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen? (A) 0.13 atm (B) 0.27 atm (C) 0.63 atm (D) 0.90 atm (E) 6.3 atm

E

A hot-air balloon rises. Which of the following is the best explanation for this observation? (A) The pressure on the walls of the balloon increases with increasing tempearature. (B) The difference in temperature between the air inside and outside the ballon produces convection currents. (C) The cooler air outside the balloon pushes in on the walls of the ballon. (D) The rate of diffusion of cooler air is less than that of warmer air. (E) The air density inside the ballon is less than that of the surrounding air.

C

A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0 °C and 1.00 atmosphere. A possible formula for the hydrocarbon is (A) CH2 (B) C2H4 (C) C3H6 (D) C4H8 (E) C5H10

D

A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. The following measurements were made. Mass of metal = 19.611 grams Volume of water before addition of metal = 12.4 milliliters Volume of water after addition of metal = 14.9 milliliters The density of the metal should be reported as (A) 7.8444 grams per mL (B) 7.844 grams per mL (C) 7.84 grams per mL (D) 7.8 grams per mL (E) 8 grams per mL

C

A sample of 0.0100 mole of oxygen gas is confined at 37° C and 0.216 atmosphere. What would be the pressure of this sample at 15° C and the same volume? (A) 0.0876 atm (B) 0.175 atm (C) 0.201 atm (D) 0.233 atm (E) 0.533 atm

D

A sample of 3.30 grams of an ideal gas at 150.0 °C and 1.25 atmospheres pressure has a volume of 2.00 liters. What is the molar mass of the gas? The gas constant, R, is 0.0821 L atm mol¯1 K¯1). (A) 0.0218 gram/mole (B) 16.2 grams/mole (C) 37.0 grams/mole (D) 45.8 grams/mole (E) 71.6 grams/mole

C

A sample of 61.8 g of H3BO3, a weak acid is dissolved in 1,000 g of water to make a 1.0-molal solution. Which of the following would be the best procedure to determine to molarity of the solution? (Assume no additional information is available.) (A) Titration of the solution with standard acid (B) Measurement of the pH with a pH meter (C) Determination of the boiling point of the solution (D) Measurement of the total volume of the solution (E) Measurement of the specific heat of the solution

C

A sample of an ideal gas is cooled from 50.0 °C to 25.0 °C in a sealed container of constant volume. Which of the following values for the gas will decrease? I. The average molecular mass of the gas II. The average distance between the molecules III. The average speed of the molecules (A) I only (B) II only (C) III only (D) I and III (E) II and III

E

A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt of (A) Cu (B) Mn (C) Fe (D) Ni (E) Zn

What is a compound?

A substance that is made from atoms of two or more elements that are chemically bonded (H20)

electrolyte

A substance whose aqueous solutions contains ions

A

A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following compounds could the solid be? (A) CaCO3 (B) BaSO4 (C) Pb(NO3)2 (D) AgCl (E) Zn(OH)2

A

A yellow precipitate forms when 0.5 M NaI(aq) is added to a 0.5 M solution of which of the following ions? A) Pb2+(aq) B) Zn2+(aq) C) CrO42¯(aq) D) SO42¯(aq) E) OH¯(aq)

Which of the following combinations of elements in a compound would be ionic? A) B and F B) N and O C) S and O D) P and O E) All of these

A) Barium and Fluorine

Based on common charges, which formula for an ionic compound is incorrect? A) CaCl B) NaF C) SrO D) MgS E) K₃P

A) CaCl

Synthesis

A+B --> AB

Double replacement

AB + CD --> AD + CB

Decomposition

AB --> A + B

atoms that have expanded octets follow this patters..

AB₅ or AB₆

C2H3O2 - or CH3COO -

Acetate

C₂H₃O₂⁻

Acetate

Ac

Actinium

A

Adding water to some chemicals can be dangerous because large amounts of heat are liberated. Which of the following does NOT liberate heat when water is added to it? (A) KNO3 (B) NaOH (C) CaO (D) H2SO4 (E) Na

B

After completing an experiment to determine gravimetrically the percentage of water in a hydrate, a student reported a value of 38 percent. The correct value for the percentage of water in the hydrate is 51 percent. Which of the following is the most likely explanation for this difference? A) Strong initial heating caused some of the hydrate sample to spatter out of the crucible. B) The dehydrated sample absorbed moisture after heating. C) The amount of the hydrate sample used was too small. D) The crucible was not heated to constant mass before use. E) Excess heating caused the dehydrated sample to decompose.

47. Silver

Ag

Silver

Ag

Elements with similar configurations like Cu

Ag, Au

Silver

Ag⁺

silver

Ag⁺

13. Aluminum

Al

Aluminum

Al

Two protons and two neutrons bound together and emitted from the nucleus during some kinds of radioactive decay.

Alpha Particle

Al

Aluminum

Al 3+

Aluminum

What would be the products of the beta decay of Magnesium-24?

Aluminum-24 and a beta particle

aluminum

Al³⁺

Am

Americium

NH₃

Ammonia

NH4 +

Ammonium

NH4 -

Ammonium

NH₄⁺

Ammonium

C

An impossible electronic configuration (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

Sb

Antimony

18. Argon (ng)

Ar

Argon

Ar

Ar

Argon

What would be the products of the positron decay of Potassium-38?

Argon -38 and a positron

As

Arsenic

As 5+

Arsenic (V)

AS 3+

Arsenic(III)

33. Arsenic

As

Arsenic

As

C

As the temperature is raised from 20 ° C to 40 ° C, the average kinetic energy of neon atoms changes by a factor of (A) 1/2 (B) [square root of](313/293) (C) 313/293 (D) 2 (E) 4

Arsenate Ion

AsO4 3-

Arsenate

AsO₄³⁻

Arsenide

As^3-

At

Astatine

Arsenic (V)

As⁵⁺

Arsenic(III)

As⁺³

D

At 25 °C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate? (A) O2 (molar mass 32 grams) (B) He2 (molar mass 4.0 grams) (C) CO2 (molar mass 44 grams) (D) Cl2 (molar mass 71 grams) (E) CH4 (molar mass 16 grams)

Isotopes

Atoms of the same element but different mass numbers. Electrons and protons are the same, but different number of neutrons.

Isotope

Atoms of the same element with different number of neutrons

79. Gold

Au

Gold

Au

Auric

Au³⁺

Aurous

Au¹⁺

Which scientist is known for studying the relationship between moles and volumes of gases?

Avogadro

2p

B

5. Boron

B

Boron

B

A reaction which has two elements are reactants and one compound as a product: A) a decomposition reaction B) A synthesis reaction C) A single-displacement reaction D) A double-displacement reaction E) combustion reaction

B) a synthesis reaction

borate

BO₃³⁻

56. Barium

Ba

Barium

Ba

Ba

Barium

Ba 2+

Barium

Barium

Ba²⁺

barium

Ba²⁺

4. Beryllium

Be

Beryllium

Be

Be

Beryllium

An electron emitted from the nucleus during some kinds of radioactive decay.

Beta Particle

Beryllium

Be²⁺

Bismuth*

Bi*

HCO₃⁻

Bicarbonate

Bi

Bismuth

Bi 3+

Bismuth (III)

Bi 5+

Bismuth (V)

HSO₄⁻

Bisulfate

HS⁻

Bisulfide

HSO₃⁻

Bisulfite

Bismuth (III)

Bi³⁺

Bismuth(III)

Bi³⁺

Bismuth (V)

Bi⁵⁺

Bismuth(V)

Bi⁵⁺

Higher frequency and lower wavelength gives what color?

Blue

B

Boron

consider the reaction below. Which of the following is true? H2 (g) +1/2 O2 (g) ---> H2O (I) N CHANGE H= -286kJ

Both a and c are true A) the reaction is exothermic C) the energy of the projects is less than that of the reactants

35. Bromine

Br

Bromine

Br

bromide

Br -

hypobromite

BrO -

bromite

BrO2 -

bromate

BrO3 -

perbromate

BrO4 -

perbromate

BrO⁴⁻

Bromate(I) (Hypobromite)

BrO⁻

hypobromite

BrO⁻

Bromate(III) (Bromite)

BrO₂⁻

bromite

BrO₂⁻

Bromate(V)

BrO₃-

bromate

BrO₃⁻

Bromate(VII) (Perbromate)

BrO₄-

Higher amplitude gives off what kind of light?

Brighter

BrO₃⁻

Bromate

Br

Bromine

Bromide

Br⁻

bromide

Br⁻

Hund's Rule

Bus seat rule. All arrows go up before down (^)

6. Carbon

C

Carbon

C

Fahrenheit --> Celsius

C = (5/9)(F - 32)

Based on common charges, which formula for an ionic compound is incorrect? A) Ba(NO₃)₂ B) Ca(OH)₂ C) MgCl₃ D) Al₂O₃ KBr

C) MgCl₃

Which of the following combinations of elements in a compound would be molecular? A) Sodium and Nitrogen B) Calcium and Oxygen C) Nitrogen and Oxygen D) Potassium and Chlorine E) Sodium and Sulfur

C) Nitrogen and Oxygen

Acetate

C2H3O2 -

acetate

C2H3O2 -

Acetate

C2H3O2-

Oxylate

C2O4 2-

oxalate

C2O4 2-

Oxlate

C2O4^2-

C

CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the molecules above? (A) Linear (B) Octahedral (C) Square planar (D) Tetrahedral (E) Trigonal pyramidal

D

CH3CH2OH boils at 78 °C and CH3OCH3 boils at - 24 °C, although both compounds have the same composition. This difference in boiling points may be attributed to a difference in (A) molecular mass (B) density (C) specific heat (D) hydrogen bonding (E) heat of combustion

Acetate

CH3COO^-

Cyanide

CN -

cyanide

CN -

Cyanide

CN-

Cyanide

CN^-

Cyanide

CN⁻

cyanide

CN⁻

Arrange the following gases in order of increasing average velocity at 25*C. He, O2, CO2, N2

CO2, O2, N2, He

Carbonate

CO3 2-

carbonate

CO3 2-

carbonate

CO3-2

Carbonate

CO3^2-

H₂CO₃

CO₂(g) + H₂O

Carbonate

CO₃²⁻

carbonate

CO₃²⁻

Carbide

C^4-

20. Calcium

Ca

Calcium

Ca

Cd

Cadmium

Cd 2+

Cadmium

Cs

Caesium

Ca

Calcium

Ca 2+

Calcium

CaIO₄

Calcium iodate

Calcium chloride and Silver nitrate react to form ___?

Calcium nitrate and silver chloride

CaC₂O₄

Calcium oxalate

Nooooo!!!

Can 2 atoms of different elements be Isoelectronic with each other?

C

Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

C

Carbon

Ionic radius

Cation - lost e- - ir is smaller than neutral atom Anion - gain e- - ir is bigger than neutral atom

calcium

Ca²⁺

48. Cadmium

Cd

Cadmium*

Cd*

Cadmium

Cd²⁺

Cs

Cesium

Cs₂CO₃

Cesium carbonate

A

Cesium chloride, CsCl (s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

For a particular process q= 20kJ and w=15kJ. What statement is true?

Change E= 35 kJ

Chemical Change

Change when one or more substances are converted into different substances with different properties

Physical change

Changes among state/form of matter

the statement "the volume of a fixed amount of gas maintained at constant pressure is directly proportional to absolute pressure" refers to whose laws

Charles

ClO3 -

Chlorate

ClO₃⁻

Chlorate

Cl

Chlorine

ClO₂

Chlorine Dioxide

ClF₃

Chlorine triflouride

ClO2 -

Chlorite

ClO₂⁻

Chlorite

CrO4 2-

Chromate

CrO₄²⁻

Chromate

Cr

Chromium

Cr 2+

Chromium (II)

Cr 3+

Chromium (III)

17. Chlorine

Cl

Chlorine

Cl

chloride

Cl -

Hypochlorite Ion

ClO -

hypochlorite

ClO -

hypochlorite

ClO-

Chlorite Ion

ClO2 -

chlorite

ClO2 -

Chlorite

ClO2^-

Chlorate Ion

ClO3 -

chlorate

ClO3 -

chlorate

ClO3-

Chlorate

ClO3^-

Perchlorate Ion

ClO4 -

perchlorate

ClO4 -

perchlorate

ClO4-

Perchlorate

ClO4^-

perchlorate

ClO⁴⁻

Chlorate(I) (Hypochlorite)

ClO⁻

Hypochlorite

ClO⁻

hypochlorite

ClO⁻

Chlorate(III) (Chlorite)

ClO₂⁻

Chlorite

ClO₂⁻

chlorite

ClO₂⁻

Chlorate

ClO₃⁻

Chlorate(V)

ClO₃⁻

chlorate

ClO₃⁻

Chlorate(VII) (Perchlorate)

ClO₄ ⁻

Perchlorate

ClO₄⁻

perchlorate

ClO₄⁻

Chloride

Cl⁻

chloride

Cl⁻

HClO₄

Cl⁻ + H₂O

27. Cobalt

Co

Cobalt

Co

Co

Cobalt

Co 2+

Cobalt (II)

Co 3+

Cobalt (III)

Visual Evidence of Chemical Reaction

Color change, gas produced, precipitate produced, and light produced

Mixture

Combination of 2 or more types of matter, each maintaining its own properties

Mixture

Combination of substances that doesn't change the individual substances chemically.

Fusion

Combining two light nuclei to form a heavier, more stable nucleus

C

Contains 1 sigma (s) and 2 pi (p) bonds (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2

Cu

Copper

Cuprous

Copper (I)

Cu +

Copper (I) or Cuprous

Cupric

Copper (II)

CuF₂

Copper (II) flouride

Cu 2+

Copper (II) or Cupric

Cobalt (II)

Co²⁺

Cobalt(II)

Co²⁺

Cobalt (III)

Co³⁺

Cobalt(III)

Co³⁺

24. Chromium

Cr

Chromium

Cr

Dichromate

Cr2O7 2-

dichromate

Cr2O7 2-

Dichromate

Cr2O7^2-

What are the two exceptions in the e- configuration rule?

Cr: [Ar]4s¹3d⁵ and Cu: [Ar]4s¹3d¹⁰

Chromate

CrO4 2-

chromate

CrO4 2-

Chromate

CrO4-2

Chromate

CrO4^2-

Cr₂O₇²⁻ in base

CrO4₂⁻ + H₂O

CrO₄²⁻ in a base

CrO₂⁻ + H₂O

Chromate

CrO₄²⁻

chromate

CrO₄²⁻

John Dalton

Created atomic theory

Ernest Rutherford

Created nuclear model with gold foil experiment

Chromium (II)

Cr²⁺

Chromium(II)

Cr²⁺

Chromium (III)

Cr³⁺

Chromium(III)

Cr³⁺

chromium

Cr³⁺

Cr₂O₇²⁻ in acid

Cr³⁺ + H₂O

Dichromate

Cr₂O₇²⁻

dichromate

Cr₂O₇²⁻

55. Cesium

Cs

Cesium

Cs

Cesium

Cs⁺

29. Copper

Cu

Copper

Cu

Copper(I)

Cu+

Copper (II)

Cu²⁺

Copper(II)

Cu²⁺

Cupric

Cu²⁺

cupric

Cu²⁺

Cuprous

Cu¹⁺

cuprous

Cu¹⁺

Copper (I)

Cu⁺

CN -

Cyanide

CN⁻

Cyanide

Carbide

C⁴⁻

Acetate

C₂H₃O₂⁻

Ethanoate (Acetate)

C₂H₃O₂⁻

acetate

C₂H₃O₂⁻

Oxalate

C₂O₄²⁻

oxalate

C₂O₄²⁻

Tartrate

C₄H₄O₆²⁻

L=2

D orbital

A reaction which has two compounds as reactants and two compounds as products: A) decomposition reaction B) synthesis reaction C) single-displacement reaction D) double-displacement reaction E) combustion reaction

D) double-displacement reaction

Amplitude

Deals with the intensity of the wave

Robert Boyle

Defined element

Gas to solid

Deposition

Gas

Describes something in the gaseous phase that is usually found as a gas at normal room conditions.

Vapor

Describes something in the gaseous phase this is usually found in a phase other than gas at normal room conditions.

Cr₂O₇²⁻

Dichromate

Lower amplitude gives off what kind of light?

Dimmer

What is the weakest Van der Waals force?

Dispersion

Wavelength

Distance from crest to crest or trough to trough

Atomic radius

Distance from nucleus to valence e- Relates properties like DENSITY

Principle Quantum #

Distance from nucleus — shell

Solid

Do NOT break the compound apart into its ions; it is NOT in solution when it reacts. If it is going into solution of water is a product, follow solubility rules for products.

Equation for calculating the energy associated with the electron in a hydrogen atom

E = -2.18⋅10⁻¹⁸J (z²/n²)

Equation for energy of a photon

E = hν; E = hc/λ

What did planck theorize?

E can only be absorbed or released from atoms in certain amounts

kinetic energy

E due to motion of an object

potential energy

E due to position or composition

Which of the following pairs is incorrect? A) CO carbon monoxide B) CaO Calcuim oxide C) MgCl₂ Magnesium chloride D) AlP Aluminium phosphide E) Li₂SO₃ Dilithium sulfite

E) Li₂SO₃ Dilithium sulfite

What is the equation to calculate the energy of ONE quantum?

E=hv

Eka aluminum and Eka silicon

Eka Means under

Occurs when an inner orbital electron is captured by the nucleus of its own atom.

Electron Capture

Aufbau principle

Electrons will automatically occupy the lowest energy sublevel

Ga/Ge

Elements that first were discovered

Quantum Theory

Energy and Matter are particulate, massive, and wavelike

Atomic line spectra

Energy of atoms is quantized. photon emitted when electron changes orbit (Bohr)

Ionization energy

Energy required to remove an e- from an atom in its ground state

Electron Affinity

Energy that is released when an e- is accepted/gained(negative sign)

A

Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining in the vessel after some of the gas mixture has effused? A) PHe < PNe < PAr B) PHe < PAr < PNe C) PNe < PAr < PHe D) PAr < PHe < PNe E) PHe = PAr = PNe

Reaction is in solution

Equation must be written in NET IONIC FORM; spectator ions must be left out and all ions must be shown in ionic form.

mass-protons

Equation to find electrons

CH3-CH2-CH2-CH3 and CH (with 3 CH3 attached w/ a single bond)

Examples of isomers

E

Explains the experimental phenomenon of electron diffraction (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

9. Fluorine

F

Fluorine

F

fluoride

F -

Celsius --> Fahrenheit

F = (9/5)C + 32

L=3

F orbital

Hypofluorite Ion

FO -

Flourite Ion

FO2 -

Fluorate Ion

FO3 -

Perfluorate Ion

FO4 -

The larger the sample of a given substance, the more dense it is. True or false

False

True or False: 1mole of methane (CH₄) and 1 mole of oxygen (O₂) would have the same number of atoms.

False

Water is considered a mixture because it consists of hydrogen and oxygen. True or false

False

26. Iron

Fe

Iron

Fe

Ferrate ion

FeO4 2-

Ferrous

Fe²⁺

Iron (II)

Fe²⁺

Iron(II)

Fe²⁺

ferrous

Fe²⁺

Ferric

Fe³⁺

Iron (III)

Fe³⁺

Iron(III)

Fe³⁺

ferric

Fe³⁺

D

For the substance represented in the diagram, which of the phases is most dense and which is least dense at - 15 °C. Most Dense Least Dense (A) Solid Gas (B) Solid Liquid (C) Liquid Solid (D) Liquid Gas (E) The diagram gives no information about densities.

Ionic bonds

Form when electrons are transferred. Metals and non-metals

JJ Thomson

Found particles called electron and that an atom has a neutral charge Also helped plum pudding model.

87. Francium

Fr

Fr

Francium

Halide ions (Cl⁻, Br⁻, etc.)

Free Halogens (Cl₂, Br₂, etc.)

Liquid to solid

Freezing

DECREASES

From left to right AR...

increases

From left to right EA...

INCREASES

From left to right IE..

INCREASES

From top to bottom AR..

DECREASES

From top to bottom EA...

DECREASES

From top to bottom IE.

Francium

Fr⁺

Fluoride

F⁻

fluoride

F⁻

31. Gallium

Ga

Gallium

Ga

Ga

Gallium

High-energy electromagnetic waves emitted from a nucleus as it changes from an excited state to a ground energy state.

Gamma Rays

Gallium

Ga³⁺

32. Germanium

Ge

Germanium

Ge

Ge

Germanium

Germanium

Ge⁴⁺

B

Gold, Au(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

Alkali metals

Group 1 - have 1 valence electron +1 oxidation state

Halogens

Group 17 - have 7 valence electrons -1 is preferred oxidation state

Noble gases

Group 18 - full orbitals Non-reactive

Alkaline Earth metals

Group 2 - have 2 valence electrons +2 oxidation state

Transition metals

Groups 3-12 - electrons in the d-orbitals Can have a variety of oxidation states

Polyatomic ions

Groups of covalently bonded atoms with an overall charge

1. Hydrogen

H

1s

H

Hydrogen

H

hydride

H -

change in H=

H products- H reactions

D

H2(g) + (1/2) O2(g) ---> H2O(l) DH° = - 286 kJ 2 Na(s) + (1/2) O2(g) ---> Na2O(s) DH° = - 414 kJ Na(s) + (1/2) O2(g) + (1/2) H2(g) ---> NaOH(s) DH° = - 425 kJ Based on the information above, what is the standard enthalpy change for the following reaction? Na2O(s) + H2O(l) ---> 2 NaOH(s) (A) -1,125 kJ (B) -978 kJ (C) -722 kJ (D) -150 kJ (E) +275 kJ

Dihydrogen Phosphite Ion

H2PO3 -

Dihydrogen Phosphate Ion

H2PO4 -

dihydrogen phosphate

H2PO4 -

Dihydrogen Phosphate

H2PO4^-

Hydronium

H3O+

hydrogen oxalate

HC2O4 -

Hydrogen Carbonate (Bicarbonate Ion)

HCO3 -

hydrogen carbonate

HCO3 -

Bicarbonate

HCO3-

Bicarbonate or Hydrogen carbonate

HCO3-

Hydrogen Carbonate

HCO3^-

formate

HCO₂⁻

Hydrogen Carbonate

HCO₃⁻

Hydrogen carbonate

HCO₃⁻

Hydrogen carbonate/Bicarbonate

HCO₃⁻

bicarbonate

HCO₃⁻

Strong Acids:

HCl H2SO4 HNO3 HBr HI HClO4

What are the strong acids?

HCl, HBr, HI, H2SO4, HNO3,l HClO4, HClO3

Strong Acids

HCl, HBr, HI, HClO₄, HNO₃, HIO₄, H₂SO₄, HClO₃

Weak Acids

HC₂H₃O₂, HF, etc.

Hydrogen Oxalate

HC₂O₄⁻

Hydrogen Phosphite Ion

HPO3 2-

Hydrogen Phosphate Ion

HPO4 2-

hydrogen phosphate

HPO4 2-

Monohydrogen Phosphate

HPO4^2-

Hydrogen Phosphate

HPO₄²⁻

Hydrogen phosphate

HPO₄²⁻

hydrogen sulfide

HS -

Hydrogen Sulfite

HSO3 -

hydrogen sulfite

HSO3 -

Hydrogen Sulfite

HSO3^-

Hydrogen Sulfate

HSO4 -

hydrogen sulfate

HSO4 -

Hydrogen Sulfate

HSO4^-

Hydrogen Sulfite

HSO₃⁻

Hydrogen sulfite

HSO₃⁻

bisulfite

HSO₃⁻

Hydrogen Sulfate

HSO₄⁻

Hydrogen sulfate

HSO₄⁻

Hyrdogen Sulfate

HSO₄⁻

bisulfate

HSO₄⁻

Hydrogen Sulfide

HS⁻

bisulfide

HS⁻

Free Halogens (Cl₂, etc.)

Halide ions (Cl⁻)

D

Has a bond order of 2 (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2

C

Has the largest bond-dissociation energy (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2

Non-polar bonds

Have no partially charged regions, so the electrons are equally shared in bonds

2. Helium (ng)

He

Helium

He

He

Helium

What would be the products of the alpha decay of Uranium-233?

Helium-4 and Thorium-229

80. Mercury

Hg

Mercury

Hg

Mercury (II)

Hg²⁺

Mercury(II)

Hg²⁺

mercuric

Hg²⁺

Mercury (I)

Hg₂²⁺

Mercury(I)

Hg₂²⁺

mercurous

Hg₂²⁺

E

How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms? (A) 164 grams (B) 96 grams (C) 62 grams (D) 50. grams (E) 41 grams

C

How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl? (A) 3.9 mL (B) 35 mL (C) 260 mL (D) 1,000 mL (E) 3,900 mL

A

How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the concentration of the NO3¯ ion to 1.0-molar? (Assume that the volume of the solution remains constant.) (A) 0.060 mole (B) 0.12 mole (C) 0.24 mole (D) 0.30 mole (E) 0.40 mole

-ide

Hydro_____ic acid

H

Hydrogen

H +

Hydrogen

HCO3 -

Hydrogen Carbonate

HI

Hydrogen Iodide

HSO4 -

Hydrogen Sulfate

B

Hydrogen gas is collected over water at 24 °C. The total pressure of the sample is 755 millimeters of mercury. At 24 °C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas? (A) 22 mm Hg (B) 733 mm Hg (C) 755 mm Hg (D) 760 mm Hg (E) 777 mm Hg

H3O +

Hydronium

OH -

Hydroxide

OH⁻

Hydroxide

ClO⁻

HypoChlorite

ClO -

Hypochlorite

hydrogen

H⁺

Hydride

H⁻

H₂O (reduction)

H₂ + OH⁻

acetate

H₂C₃O₂⁻

H₂O₂ in acid

H₂O

H₂O₂ decomp.

H₂O + O₂

Dihydrogen Phosphate

H₂PO₄⁻

Dihydrogen phosphate

H₂PO₄⁻

Hydronium

H₃O⁺

hydronium

H₃O⁺

53. Iodine

I

Iodine

I

iodide

I -

B

I2(g) + 3 Cl2(g) ---> 2 ICl3(g) According to the data in the table below, what is the value of DH° for the reaction represented above? Bond Average Bond Energy (KJ/mole) I---I 149 Cl---Cl 239 I---Cl 208 (A) - 860 kJ (B) - 382 kJ (C) + 180 kJ (D) + 450 kJ (E) + 1,248 kJ

Triiodide Ion

I3 -

Hypoiodite Ion

IO -

hypoiodite

IO -

Iodite Ion

IO2 -

iodite

IO2 -

Iodate Ion

IO3 -

iodate

IO3 -

Iodate

IO3^-

Periodate Ion

IO4 -

periodate

IO4 -

periodate

IO⁴⁻

Iodate(I) (Hypoiodite)

IO⁻

hypoiodite

IO⁻

Iodate(III) (Iodite)

IO₂⁻

iodite

IO₂⁻

Iodate(V) (Iodate)

IO₃⁻

iodate

IO₃⁻

Iodate(VII) (Periodate)

IO₄⁻

E

If 87 grams of K2 SO4 (molar mass 174 grams) is dissolved in enough water to make 250 milliliters of solution, what are the concentrations of the potassium and the sulfate ions? [K+] [SO42¯] (A) 0.020 M 0.020 M (B) 1.0 M 2.0 M (C) 2.0 M 1.0 M (D) 2.0 M 2.0 M (E) 4.0 M 2.0 M

E

In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of (A) a tetrahedron (B) a square-based pyramid (C) a trigonal bipyramid (D) a square (E) an octahedron

B

In a qualitative ananlysis for the presence of Pb2+, Fe2+, and Cu2+ ions in a aqueous solution, which of the following will allow the separation of Pb2+ from the other ions at room temperature? A) Adding dilute Na2S(aq) solution B) Adding dilute HCl(aq) solution C) Adding dilute NaOH(aq) solution D) Adding dilute NH3(aq) solution E) Adding dilute HNO3(aq) solution

Proton

In the nucleus. +1 charge Determines what element an atom will be.

Neutrons

In the nucleus. No charge, but hold the protons together with strong nuclear force

D

In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? (A) It remains constant. (B) It increases only. (C) It increases, then decreases. (D) It decreases only. (E) It decreases, then increases.

B

In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00 ? (A) CrO3 (B) CrO2 (C) CrO (D) Cr2O (E) Cr2O3

Weak electrolytes

Includes weak acids/bases. They must be written together.

B

Indicates that an atomic orbital can hold no more than two electrons (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

IO₃⁻

Iodate

I

Iodine

KJ/mol

Ionization energy measured in..

Strong acids and bases

Ionize 100%. They must be written as separate ions.

Fe

Iron

Ferrous

Iron (II)

Fe 2+

Iron (II) or Ferrous

FeO

Iron (II) oxide

Ferric

Iron (III)

Fe 3+

Iron (III) or Ferric

Fe₂S₃

Iron (III) sulfide

D

Is added to silicon to enhance its properties as a semiconductor (A) Pb (B) Ca (C) Zn (D) As (E) Na

Passed over

Is used simply to tell you that the reactants come into contact with one another meaning they can react.

D

Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

B

Is used to explain the fact that the four bonds in methane are equivalent (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

E

Is used to explain why iodine molecules are held together in the solid state (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

A

Is used to explain why the boiling point of HF is greater than the boiling point of HBr (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

Bubbled

It deescribed the method needed to get a gas to react with either a liquid or a substance in solution.

Shaken

It described the method needed to get two liquids with different densities (or polarities) to react together.

Iodide

I⁻

iodide

I⁻

Specific heat units

J / (g * °C) or cal / (g * °C)

units of specific heat capacity

J/ g degrees C; E required to raise temp of one gram of substance by 1 degree Celsius

19. Potassium

K

Potassium

K

Kelvin <--> Celsius

K = C + 273.15

kinetic energy

KE = 1/2 mv² energy due to the motion of an object; dependent on the mass of the object and the square of its velocity.

ΔH units

KJ / mol

36. Krypton (ng)

Kr

Krypton

Kr

Kr

Krypton

Potassium

K⁺

4f

La

La

Lanthanum

Pb

Lead

Plumbous

Lead (II)

Pb 2+

Lead (II) or Plumbous

Plumbic

Lead (IV)

Pb 4+

Lead (IV) or Plumbic

The largest element that has stable isotopes.

Lead - 82 (Bismuth acceptable)

3. Lithium

Li

Lithium

Li

Photoelectric effect

Light has particulate behavior (Einstein)

Li

Lithium

Li +

Lithium

Lithium

Li⁺

lithium

Li⁺

Always Soluble Alkali Metals

Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺

More stable

Lowers energy of an orbital

Dz2

M=-1

Dx2y2

M=-2

Dxy

M=0

S suborbital

M=0 (s)

Dxz

M=1

Dyz

M=2

Atom

MEANS NEUTRAL

Ionic compound

Made up of oppositely charged ions (cation, then anion)

Mg

Magnesium

Mg 2+

Magnesium

Mg(ClO₃)₂

Magnesium chlorate

Mn

Manganese

Mn 2+

Manganese (II)

Mn 4+

Manganese (IV)

Density

Mass divided by volume

Law of Conservation of Mass

Mass is neither created nor destroyed during a chemical reaction. It is conserved.

D

Mass of an empty container = 3.0 grams Mass of the container plus the solid sample = 25.0 grams Volume of the solid sample = 11.0 cubic centimeters The data above were gathered in order to determinethe density of an unknown solid. The density of the sample should be reported as (A) 0.5 g/cm3 (B) 0.50 g/cm3 (C) 2.0 g/cm3 (D) 2.00 g/cm3 (E) 2.27 g/cm3

Molar mass

Mass of one mole=periodic table mass in grams

Pure Substance

Matter that has constant composition and a specific formula (element OR compound)

One one

Matter travels in ___ direction(s) at ___ time

Solid to liquid

Melting

Hg

Mercury

Hg2 2+

Mercury (I)

Mercurous

Mercury (I)

Hg2 2+

Mercury (I) or Mercurous

Mercuric

Mercury (II)

Hg₃N₂

Mercury (II) nitride

Hg 2+

Mercury (II) or Mercuric

Ionic

Metal & Non-metal Transfer

Free metals

Metal Ions

Metallous ions (Sn²⁺, Fe²⁺)

Metallic Ions (Sn⁴⁺, Fe³)

Metallic ions (Sn⁴⁺, Fe³⁺, etc.)

Metallous ions (Sn²⁺, Fe²⁺, etc.)

CH₄

Methane

magnesium

Mg²⁺

Homogeneous

Mixed to a constant composition (aka solutions-solid, liquid or gas)

Solution

Mixture that looks uniform throughout. AKA homogenous mixture. ex) coffee, air, etc.

25. Manganese

Mn

Manganese

Mn

Permanganate

MnO4 -

permanganate

MnO4 -

Permanganate

MnO4-

Permanganate

MnO4^-

permanganate

MnO⁴⁻

MnO₄ in base

MnO₂

Manganate

MnO₄²⁻

manganate

MnO₄²⁻

Manganate(VII)

MnO₄⁻

Permanganate

MnO₄⁻

permanganate

MnO₄⁻

Manganese (II)

Mn²⁺

Manganese(II)

Mn²⁺

manganese

Mn²⁺

MnO₂ in acid

Mn²⁺ + H₂O

MnO₄ in acid

Mn²⁺ + H₂O

Manganese (III)

Mn³⁺

Manganese(IV)

Mn⁴⁺

42. Molybdenum

Mo

Elements with similar configurations like Cr

Mo

A

Molecules that have planar configurations include which of the following? I. BCl3 II. CHCl3 III. NCl3 (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

Mo

Molybdenum

C

Most common hybrid

Solids and pure liquids

Must be written together.

7. Nitrogen

N

Nitrogen

N

nitride

N 3-

Azide Ion

N3 -

Ammonium

NH4 +

Ammonium

NH4+

amide

NH₂⁻

NH₄OH

NH₃(aq gas) + H₂O

Ammonium

NH₄⁺

ammonium

NH₄⁺

Always Soluble Polyatomic Ions

NH₄⁺, NO₃⁻

HNO₃, dilute (approx. 6M)

NO + H₂O

2HNO₂

NO(g) + NO₂(g) + H₂O

Nitrite

NO2 -

nitrite

NO2 -

Nitrite

NO2-

Nitrite

NO2^-

Nitrate

NO3 -

nitrate

NO3 -

Nitrate

NO3-

Nitrate

NO3^-

HNO₃, conc. (10-12M)

NO₂ + H₂O

Nitrite

NO₂⁻

nitrite

NO₂⁻

Nitrate

NO₃⁻

nitrate

NO₃⁻

The farther away from the nucleus, the higher the ____

NRG

11. Sodium

Na

Sodium

Na

Na₂O₂

NaOH

Sodium

Na⁺

sodium

Na⁺

41. Niobium

Nb

10. Neon (ng)

Ne

Neon

Ne

Anion

Negative ion. Forms when an atom gains electrons

Anion

Negative ion; gained one or more electrons

Ne

Neon

Ground state

Neutral

28. Nickel

Ni

Nickel

Ni

Ni

Nickel

Ni 2+

Nickel (II)

Ni

Nickle

NO3 -

Nitrate

NO₃⁻

Nitrate

NO2 -

Nitrite

NO₂⁻

Nitrite

N

Nitrogen

Nickel

Ni²⁺

Nickel (II)

Ni²⁺

Nickel(II)

Ni²⁺

nickel

Ni²⁺

Nickel (III)

Ni³⁺

Medeleév's pt problems

Nobles not discovered Missing elements Pt arranged by mass #

Molecular

Non-metal & Non-metal Covalent Sharing

Heterogeneous

Not blended smoothly throughout, individual parts; distinct

mass defect

Nuclear changes occur with small but measurable losses of mass

Thermodynamic quantities consist of two parts:

Number gives the magnitude of the change. Sign indicates the direction of the flow.

Atomic number

Number of protons in the element.

Nitric

N²⁺

Nitride

N³⁻

nitride

N³⁻

Nitrous

N¹⁺

The correct formula for dinitrogen pentoxide

N₂O₅

8. Oxygen

O

Oxygen

O

E

O || CH3-C-CH2-CH3 The organic compound represented above is an example of (A) an organic acid (B) an alcohol (C) an ether (D) an aldehyde (E) a ketone

oxide

O 2-

Superoxide Ion

O2 -

Peroxide

O2 2-

peroxide

O2 2-

Peroxide

O2-2

Peroxide

O2^2-

cyanate

OCN⁻

Hypochlorite

OCl^-

Hydroxide

OH -

hydroxide

OH -

Hydroxide

OH-

Hydroxide

OH^-

hydroxide

OH⁻

Dipole-dipole

Occur between molecules with permanent opposite charges

D

Of the following molecules, which has the largest dipole moment? (A) CO (B) CO2 (C) O2 (D) HF (E) F2

C

On a mountaintop, it is observed that water boils at 90°C, not at 100°C as at sea level. This phenomenon occurs because on the mountaintop the A) equilibrium water vapor pressure is higher due to the higher atmospheric pressure B) equilibrium water vapor pressure is lower due to the higher atmospheric pressure C) equilibrium water vapor pressure equals the atmospheric pressure at a lower temperature D) water molecules have a higher average kinetic energy due to the lower atmospheric pressure E) water contains a greater concentration of dissolved gases

Dmitri Mendeleev

Organized elements by atomic # (periodic table)

Valence electrons

Outermost shell/orbitals

C2O4 2-

Oxalate

C₂O₄²⁻

Oxalate

O

Oxygen

Oxide

O²⁻

oxide

O²⁻

H₂O (oxidation)

O₂ + H⁺

Peroxide

O₂²⁻

peroxide

O₂²⁻

15. Phosphorous

P

Phosphorus

P

density =

P * (molar mass) / (R*T)

phosphide

P 3-

Momentum (equation)

P = h/λ

L=1

P orbital

Combined gas laws

P1 * V1/ n1 * T1 = P2 * V2 / n2 * T2

P(tot) =

P1 + P2 + ...

Hypophosphite Ion

PO2 3-

phosphite

PO3 3-

Phosphite

PO3^3-

Phosphate

PO4 3-

phosphate

PO4 3-

phosphate

PO4-3

Phosphate

PO4^3-

Phosphite

PO₃³⁻

phosphite

PO₃³⁻

Phosphate

PO₄³⁻

phosphate

PO₄³⁻

Ideal Gas Law

PV=nRT

Pd

Palladium

Hydrogen bonding

Particularly strong from of dipole-dipole formed by the interaction of H on one molecule with O, F, or N atoms on another.

82. Lead

Pb

Lead

Pb

Plumbate Ion

PbO3 2-

Lead (II)

Pb²⁺

Lead(II)

Pb²⁺

Plumbous

Pb²⁺

lead

Pb²⁺

Lead (IV)

Pb⁴⁺

Lead(IV)

Pb⁴⁺

Plumbic

Pb⁴⁺

46. Palladium

Pd

ClO4 -

Perchlorate

ClO₄⁻

Perchlorate

Period and Groups/Families

Periods are rows, Groups/Families are columns

MnO4 -

Permanganate

MnO₄⁻

Permanganate

O2 2-

Peroxide

O₂²⁻

Peroxide

PO4 3-

Phosphate

PO₄³⁻

Phosphate

PO₃³⁻

Phosphite

P

Phosphorus

Pt

Platinum

Lord Kelvin

Plum pudding model

Pu

Plutonium

Po

Polonium

-ate and -ite endings are what type of ions?

Polyatomic

Cation

Positive ion. Forms when an atom loses electrons

Cation

Positive ion; lost one or more electrons

Ion

Positively or negatively charged ion

A particle that has the same mass as an electron, but has a positive charge, and is emitted during some kinds of radioactive decay.

Positron

K

Potassium

K +

Potassium

KMnO₄

Potassium Permanganate

KClO

Potassium hypochlorite

Driving Forces in Double Replacements

Precipitate, Weak Electrolytes, & Formation of Gas

A

Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

Boyle's Law

Pressure and Volume are inversely related P1 V1= P2 V2

Nucleons

Protons and neutrons

Hot

Provides the necessary activation energy for the reaction to take place. Usually used for the single replacement reactions involving hydrogen.

78. Platinum

Pt

Platinum

Pt

Henry Mosley

Pt arranged by atomic # & e- configuration b

94. Plutonium

Pu

Phosphide

P³⁻

phosphide

P₃⁻

Correct formula for Tetraphosphorus hexasulfide

P₄S₆

energy released equation

Q= mc change in temperature

ΔErxn =

Qrxn / mol

Universal Gas Constant

R= atm*l/ mol* k

88. Radium

Ra

Radium

Ra

Ra

Radium

Rn

Radon

Graham's Law of Effusion

Rate of effusion of gas 1/ rate of effusion of gas 2 square root of M2/ square root of M2

Radium

Ra²⁺

37. Rubidium

Rb

Rubidium

Rb

Rubidium

Rb⁺

Lower frequency and higher wavelength gives what color?

Red

*

Review greek prefixes

45. Rhodium

Rh

86. Radon

Rn

Radon

Rn

44. Ruthenium

Ru

Rb

Rubidium

RbClO₄

Rubidium percholate

16. Sulfur

S

Sulfur

S

sulfide

S 2-

L=0

S orbital

Octet rule

S&P blocks like 8 valence e- & will gain/lose e-

Thiosulfate Ion

S2O3 2-

thiosulfate

S2O3 2-

Thiosulfate

S2O3^2-

Thiocyanate

SCN -

thiocyanate

SCN -

Thiocyanate

SCN^-

Thiocyanate

SCN⁻

thiocyanate

SCN⁻

Ag

SIlver

Sulfite

SO3 2-

sulfite

SO3 2-

sulfite

SO3-2

Sulfite

SO3^2-

Sulfate

SO4 2-

sulfate

SO4 2-

Sulfate

SO4-2

Sulfate

SO4^2-

H₂SO₄, hot, conc.

SO₂ + H₂O

H₂SO₃

SO₂(g) + H₂O

Sulfite

SO₃²⁻

sulfite

SO₃²⁻

Sulfate

SO₄²⁻

sulfate

SO₄²⁻

Isoelectronic

Same e- config and # of e-

51. Antimony

Sb

Antimony

Sb

Antimonate Ion

SbO4 3-

21. Scandium

Sc

3d

Sc

Sc

Scandium

34. Selenium

Se

Selenium

Se

Selenate Ion

SeO4 2-

Se

Selenium

Selenide

Se²⁻

Noble gas cores

Show only valence e- in detail

Electron Notation

Shows 2 Quantum NUMBERS

electron configuration

Shows all four quantum numbers with arrows.

14. Silicon

Si

Silicon

Si

Silicate

SiO3^2-

Silicate

SiO₃²⁻

Si

Silicon

Ag

Silver

Ag +

Silver

Ag₃P

Silver phosphide

Silicon

Si⁴⁺

Silicate Ion

SlO3 2-

50. Tin

Sn

Stannate Ion

SnO3 2-

Stannous

Sn²⁺

Tin (II)

Sn²⁺

Tin(II)

Sn²⁺

stannous

Sn²⁺

Stannic

Sn⁴⁺

Tin (IV)

Sn⁴⁺

Tin(IV)

Sn⁴⁺

stannic

Sn⁴⁺

Na

Sodium

Na +

Sodium

NaBr

Sodium Bromide

Na₂O

Sodium Oxide

NaCH₃COO

Sodium acetate

C

Sometimes called Sp3 hybrid

Dual Nature of e-

Sometimes travel like matter; sometimes like waves

Fission

Splitting a heavy nucleus into two nuclei with smaller mass numbers

Nuclear fission

Splitting of a nucleus into smaller parts

38. Strontium

Sr

Strontium

Sr

Strontium

Sr²⁺

strontium

Sr²⁺

Burned

Stated so that hydrocarbons combust.

Strongly heated

Stated so that metal carbonates will decompose, OR if the reaction takes place with nitrogen gas this term is needed to ensure the triple covalent bond of the nitrogen is broken.

What force holds the nucleus together?

Strong (or nuclear)

Sr

Strontium

Sr 2+

Strontium

Neutrons

Subatomic particle responsible for chemical behavior of an element

Solid to gas

Sublimation

SO4 2-

Sulfate

SO₄²⁻

Sulfate

SO3 2-

Sulfite

SO₃²⁻

Sulfite

S

Sulfur

SO₂

Sulfur dioxide

S

Sulphur

sulfide

S²⁻

Thiosulfate

S₂O₃²⁻

thiosulfate

S₂O₃²⁻

S₂O₃²⁻

S₄O₆²⁻

43. Technetium

Tc

52. Tellurium

Te

tellurate

TeO₄²⁻

Solution or solutions

Tell you that the compounds are in solution. You should assume the solution is aqueous. Use solubility rules.

Te

Tellurium

C

The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron? (A) Cl2 (B) N2 (C) NH3 (D) CCl4 (E) H2O2

D

The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb orbitals should be (A) sp2 (B) sp3 (C) dsp2 (D) dsp3 (E) d2sp3

C

The cooling curve for a pure substance as it changes from a liquid to a solid is shown right. The solid and the liquid coexist at (A) point Q only (B) point R only (C) all points on the curve between Q and S (D) all points on the curve between R and T (E) no point on the curve P\ R______S \Q/ \T

A

The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom? (A) H2S (B) NH3 (C) CH4 (D) HCN (E) CO2

Hess' Law

The energy change for a total process = the sum of the enthalpy change of the individual steps 1. ΔH for a forward reaction is equal in magnitude, but opposite in sign to a reverse reaction 2. ΔH is directly proportional to the moles of reactant and product

E

The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions (A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy

C

The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion (A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy

E

The ground-state configuration for the atoms of a transition element (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

B

The ground-state configuration of a common ion of an alkaline earth element (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

B

The ground-state configuration of a negative ion of a halogen (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

C

The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely to be (A) Na (B) Mg (C) Al (D) Si (E) P

Molar mass

The mass in grams of 1 mole of substance

B

The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is (A) 12.7 (B) 19.0 (C) 27.5 (D) 38.0 (E) 57.0

B

The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the following? I. Mg2+ is more positively charged than Na+ II. O2¯ is more negatively charged than F¯ III. The O2¯ ion is smaller than the F¯ ion (A) II only (B) I and II only (C) I and III only (D) II and III only (E) I, II, and III

E

The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true EXCEPT: (A) Its formula is CaH2. (B) It is ionic. (C) It is solid at room temperatur(E) (D) When added to water, it reacts to produce H2 gas. (E) When added to water, it forms an acidic solution.

B

The phase diagram above provides sufficient information for determining the (A) entropy change on vaporization (B) conditions necessary for sublimation (C) deviations from ideal gas behavior of the gas phase (D) latent heat of vaporization (E) latent heat of fusion

Reduction

The process of gaining electrons Oxidation number decreases

Oxidation

The process of losing electrons Oxidation number increases

D

The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is (A) N2O (B) NO (C) NO2 (D) N2O3 (E) N2O5

A

The structural isomers C2H5OH and CH3OCH3 would be expected to have the same values for which of the following? (Assume ideal behavior.) (A) Gaseous densities at the same temperature and pressure (B) Vapor pressures at the same temperature (C) Boiling points (D) Melting points (E) Heats of vaporization

C

The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is (A) 28 mm Hg (B) 56 mm Hg (C) 133 mm Hg (D) 161 mm Hg (E) 189 mm Hg

D

The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M HCl(aq) solution is approximately A) 50.0 mL B) 60.0 mL C) 100. mL D) 110. mL E) 120. mL

C

The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is (A) 3.10 grams (B) 12.0 grams (C) 29.4 grams (D) 294 grams (E) 300. grams

Atomic mass

The weighted average mass of one mole an element's atoms (isotopes)

SCN -

Thiocynate

S2O3 2-

Thiosulfate

S₂O₃²⁻

Thiosulfate

Th

Thorium

22. Titanium

Ti

Half life

Time it takes for half of a radioisotope to decay

Sn

Tin

Stannous

Tin (II)

Sn 2+

Tin (II) or Stannous

Stannic

Tin (IV)

Sn 4+

Tin (IV) or Stannic

Ti

Titanium

To which class does the element chromium (Cr) belong?

Transition Elements

Phase change

Transition of matter from one state to another (water-vapor-ice)

A change in the identity of a nucleus as a result of a change in the number of its protons.

Transmutation

A cation is a positively charged ion that has fewer electrons than protons. True or false

True

A glass of tea with ice cubes in it is an example of a heterogeneous mixture. True or false

True

In order for an atom of an element to be neutral, its number of electrons must equal its number of protons. True or false

True

Most molecular compounds remain as molecules when dissolved in water. True or false

True

The mass of an isotope is the sum of the number of protons and neutrons in its nucleus. True or false

True

W

Tungsten

D

Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the following? I. sp II. sp2 III. sp3 (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

92. Uranium

U

Uranium

U

U

Uranium

Root Mean Square Velocity

Urms= Square root of 3RT/ M final units are M/s

Gaseous

Usually used for covalent compounds. Do not break the compound apart, it is not ionic.

Liquid

Usually used for molecular compounds. Do not break the compound apart, it is not ionic.

C

Utilized as a coating to protect Fe from corrosion (A) Pb (B) Ca (C) Zn (D) As (E) Na

A

Utilized as a shield from sources of radiation (A) Pb (B) Ca (C) Zn (D) As (E) Na

23. Vanadium

V

Vanadate Ion

VO3 -

What electrons are on the outer shell?

Valence electrons

V

Vanadium

Liquid to gas

Vaporization/evaporation

Lewis dot structure

Visual representations of valence electrons

Charles's Law

Volume and Temperature are directly related (constant pressure and moles) V1/T1= V2/T2

Avogadro's Law

Volume and number of moles are directly related (constant temperature and pressure) V1 /n1= V2 /n2

Tungsten

W

All same

Waves travel in ____ directions at the ____ time

Weak Electrolytes

Weak Acids

Dispersion forces

Weakest of intermolecular force between two non-polar molecules

Magnetic quantum #

What axis the shape is on - suborbital

Electron spin quantum #

What direction the electron spins - e-spin

Products

What is produced in a chemical reaction. To the right of the arrow.

A

What is the most electronegative element? (A) O (B) La (C) Rb (D) Mg (E) N

Reactants

What reacts in a chemical reaction. To the left of the arrow.

Reduction Agent

Whatever species is being oxidized/losing electrons

Oxidizing Agent

Whatever species is being reduced/gaining electrons

B

When a solution of sodium chloride is vaporized in a flame, the color of the flame is (A) blue (B) yellow (C) green (D) violet (E) White

Hybrid orbitals

When an orbital steals another orbital (from s) to make it either half or full

Shielding Effect

When inner she'll e- block the charge of the nucleus from valence e-

Diamagnetic

When the last e- placed is paired and spin in opposite direction.

E

Which element exhibits the greatest number of different oxidation states? (A) O (B) La (C) Rb (D) Mg (E) N

D

Which of the elements above has the smallest ionic radius for its most commonly found ion? (A) O (B) La (C) Rb (D) Mg (E) N

E

Which of the following acids can be oxidized to form a stronger acid? (A) H3PO4 (B) HNO3 (C) H2CO3 (D) H3BO3 (E) H2SO3

C

Which of the following actions would be likely to change the boiling point of a sample of a pure liquid in an open container? I. Placing it in a smaller container II. Increasing the number of moles of the liquid in the container III. Moving the container and liquid to a higher altitude (A) I only (B) II only (C) III only (D) II and III only (E) I, II, and III

E

Which of the following compounds is ionic and contains both sigma and pi covalent bonds? (A) Fe(OH)3 (B) HClO (C) H2S (D) NO2 (E) NaCN

A

Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments? (A) Atoms contain electrons. (B) Practically all the mass of an atom is contained in its nucleus. (C) Atoms contain protons, neutrons, and electrons. (D) Atoms have a positively charged nucleus surrounded by an electron cloud. (E) No two electrons in one atom can have the same four quantum numbers.

A

Which of the following does NOT behave as an electrolyte when it is dissolved in water? (A) CH3OH (B) K2CO3 (C) NH4Br (D) HI (E) Sodium acetate, CH3COONa

A

Which of the following gases deviates most from ideal behavior? A) SO2 B) Ne C) CH4 D) N2 E) H2

D

Which of the following has the lowest conductivity? (A) 0.1 M CuS04 (B) 0.1 M KOH (C) 0.1 M BaCl2 (D) 0.1 M HF (E) 0.1 M HNO3

E

Which of the following is a correct interpretation of the results of Rutherford's experiments in which gold atoms were bombarded with alpha particles? (A) Atoms have equal numbers of positive and negative charges. (B) Electrons in atoms are agganged in shells. (C) Neutrons are at the center of an atom. (D) Neutrons and protrons in atoms have nearly equal mass. (E) The positive charge of an atom is concentrated in a small region.

C

Which of the following is lower for a 1.0-molar aqueous solution of any solute than it is for pure water? (A) pH (B) Vapor pressure (C) Freezing point (D) Electrical conductivity (E) Absorption of visible light

A

Which of the following is true at the triple point of a pure substance? (A) The vapor pressure of the solid phase always equal the vapor pressure of the liquid phase. (B) The temperature is always 0.01 K lower that the normal melting point. (C) The liquid and gas phases of the substance always have the same density and are therefore indistinguishable. (D) the solid phase always melts if the pressure increases at constant temperature. (E) The liquid phase always vaporizes if the pressure increases at constant temperature.

A

Which of the following molecules has a dipole moment of zero? (A) C6H6 (benzene) (B) NO (C) SO2 (D) NH3 (E) H2S

D

Which of the following pairs of liquids forms the solution that is most ideal (most closely follows Raoult's law)? A) C8H18(l) and H2O(l) B) CH3CH2CH2OH(l) and H2O(l) C) CH3CH2CH2OH(l) and C8H18(l) D) C6H14(l) and C8H18(l) E) H2SO4(l) and H2O(l)

C

Which of the following sets of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (atomic number 31) ? (A) 4, 0, 0, 1/2 (B) 4, 0, 1, 1/2 (C) 4, 1, 1, 1/2 (D) 4, 1, 2, 1/2 (E) 4, 2, 0, 1/2

E

Which of the following solids dissolves in water to form a colorless solution? (A) CrCl3 (B) FeCl3 (C) CoCl2 (D) CuCl2 (E) ZnCl2

Saturated solutions

Written in ionic form (not together)

Suspensions

Written together

E

X = CH3-CH2-CH2-CH2-CH3 Y = CH3-CH2-CH2-CH2-OH Z = HO-CH2-CH2-CH2-OH Based on concepts of polarity and hydrogen bonding, which of the following sequences correctly lists the compounds above in the order of their increasing solubility in water? (A) Z < Y < X (B) Y < Z < X (C) Y < X < Z (D) X < Z < Y (E) X < Y < Z

54. Xenon

Xe

Xenon

Xe

Xe

Xenon

39. Yttrium

Y

Y

Yttrium

What is equation to calculate effective nuclear charge?

Z (of eff) = Z (# of protons) - S (average number of screening electrons)

nuclide is radioactive

Z > 83

Zn

Zinc

Zn 2+

Zinc

What would be the product if Gallium-67 decays by electron capture?

Zinc-67

Zr

Zirconium

30. Zinc

Zn

Zinc

Zn

Which will not dissolve in water? NaCl ZnCO3 K3PO4 LiOH

ZnCO3

Zinc

Zn²⁺

zinc

Zn²⁺

40. Zirconium

Zr

Electron configuration of Cu

[Ar]4s¹3d¹⁰

Electron configuration of Cr

[Ar]4s¹3d⁵

Van der Waals forces equation

[Pobs = a(n/v) squared] *(v-nb)= nrt corrected pressure corrected volume

D

__ Cr2O72¯ + __ e¯ + __ H+ ---> __ Cr3+ + __ H2O(l) When the equation for the half reaction above is balanced with the lowest whole-number coefficients, the coefficient for H2O is (A) 2 (B) 4 (C) 6 (D) 7 (E) 14

-ate

_____ic acid

-ite

_____ous acid

physical change

a change in form of a substance, not in chemical composition

mixture

a combination of two or more substances in which each substance retains its own chemical identity

scientific method

a dynamic process used to answer questions about our physical world

conversion factor

a fraction whose numerator and denominator are the same quantity expressed in different units

excited state

a higher energy state than the ground state

activity series

a list of metals arranged in order of decreasing ease of oxidation

mass

a measure of the amount of material in an object

heterogeneous mixture

a mixture that does not have the same composition, properties, and appearance throughout

homogeneous mixture (solution)

a mixture that is uniform throughout ( a solution)

Beta emission converts

a neutron to a proton

Photons

a particle of electromagnetic radiation having zero mass and an energy given by Plancks law.

Nodes

a point of zero amplitude of a wave.

dilution

a process in which solutions of lower concentrations can then be obtained by adding water

titration

a process in which we combine a solution of known concentration (a standard solution) with a solution of unknown concentration to determine the unknown concentration or the quantity of solute in the unknown

distillation

a process that depends on differences in the volatility of the compounds, a mixture is heated in a device, vapor passes through a cooled tube (a condenser) where it condenses back into its liquid state

enthalpy

a property of a system equal to E + PV, whereE is the internal energy of the system, P is the pressure of the system, and V is the volume of the system. At constant pressure the change in enthalpy equals the energy flow as heat.

internal energy

a property of a system that can be changed by a flow of work, heat, or both;delta E = q + w, where delta E is the change in the internal energy of the system, q is heat, and w is work.

state function (property)

a property that is independent of the pathway.

Electron capture converts

a proton to a neutron

Positron emission converts

a proton to a neutron

oxidation-reduction or redox reactions

a reaction in which electrons are transferred between reactants

standard state

a reference state for a specific substance defined according to a set of conventional definitions.

Orbital

a region in an atom where there is a high probability of finding electrons

chemical equation

a representation of a chemical reaction showing the relative numbers of reactant and product molecules.

Paschen series

a series of emission lines having energies in the infrared region.

Lyman series

a series of emission lines having energies in the ultraviolet region.

Line spectrum

a series of fine lines of individual colors separated by colorless spaces

Balmer series

a series of spectral lines that have energies in the visible region.

Quantum number

a set of numbers with integer values that define the properties of an atomic orbital.

Standing wave

a single frequency wave having fixed points of zero amplitude.

Quantization

a situation in which only certain energies are allowed.

saturated solution

a solution in which the dissolved solute is in equilibrium with the undissolved solute

aqueous solution

a solution in which water is the dissolving medium

unsaturated solution

a solution which has less solute than the equilibrium amount; if more solute is added, it will dissolve

reactants

a starting substance in a chemical reaction. It appears to the left of the arrow in a chemical equation.

chemical equilibrium

a state in which the relative numbers of each type of ion or molecule in the reaction are constant over time

All the d orbitals together make up...

a sublevel

compound

a substance composed of two or more elements

chemical change (chemical reaction)

a substance is transformed into a chemically different substance

products

a substance resulting from a chemical reaction. It is shown to the right of the arrow in a chemical equation.

element

a substance that cannot be separated into simpler substances by chemical means; composed of only one type of atom

nonelectrolyte

a substance that does not form ions in solution

Nodal surface

a surface on which there is zero probability of finding an electron.

hypothesis

a tentative explanation that guides in planning further experiments

Photon

a tiny particle or packet of light energy

greenhouse effect

a warming effect exerted by the earths atmosphere (particularly CO₂ and H₂O) due to thermal energy retained by absorption of infrared radiation.

How can electrons move between orbitals?

absorbing and emitting E in quanta (E = hv)

C₂H₃O₂⁻ CH₃COO⁻

acetate

If you graph lnk versus (1/T) what can you find from the slope?

activation NRG( multiply by -R)

What does E(of a ) equal to?

activtion NRG; the NRG it takes to get to the transition point

diamagnetic...

all electrons are paired, weakly repelled by external magnetic field

What is the Balmer series?

all orbitals back to n=2

What is the paschen series?

all orbitals back to n=3

What is the Lyman series?

all orbitals fall back to n=1

3 Main Types of Radiation

alpha, beta, gamma

Physical Change

alters a substance w/o changing its composition [melting boiling point]

Al

aluminum

NH₄⁺

ammonium

dimensional analysis

an approach to problem solving in which we keep track of units as we carry measurements through calculations

molecule

an entity composed of two or more atoms with the atoms attached to one another in a specific way

theory

an explanation of the general causes of certain phenomena, with considerable evidence or facts to support it

electron configuration

an expression giving the population of electrons in each sublevel.

precipitate

an insoluble solid formed by a reaction in solution

mass spectrometer

an instrument used to determine the relative masses of atoms by the deflection of their ions on a magnetic field.

ϱ (rho) =

angular momentum quantum number describes the shape of an orbital possible values: 0 to n-1

filtration

another method of separation, which is used when a mixture consists of a solid and a liquid, poured onto a mesh

Positrons

anti-particle of the electron

Sb

antimony

what orbitals can a sigma bond be of?

any

property

any characteristic that gives a sample of matter its unique identity

intensive properties

are independent of the amount of matter examined; are used to identify substances

Ar

argon

As

arsenic

z = (for radius)

atomic number

z = (for energy of an electron)

atomic radius

PE decreases in a bond when...

atoms reach minimum bond length (steadily increases after)

Mean free path-

average distance between collisions

at bonding distance attractive forces between nuclei and electrons just ____ repulsive forces

balance

Ba

barium

How was the wave mechanical model developed?

based on the electron's wave properties

Be

beryllium

nano

billionth

metal and a nonmatal yield...

binary salt

Bi

bismuth

Core electrons _____ valence electrons from experiencing full charge of nucleus

block (shielding effect) (core e repel valence e from center)

B

boron

BrO₃ ⁻

bromate

Br

bromine

BrO₂ ⁻

bromite

how does an electron move to another orbit?

by absorbing or emitting a photon whose energy equals the difference in energy between the two states

Equation for finding the frequency

c/λ

Cd

cadmium

Ca

calcium

science of measuring heat

calorimetry

physical properties

can be measured without changing the identity and composition of the substance (color, odor, density, melting point, boiling point, hardness)

indicator

can be used to show the end point of the titration, which coincides closely with the equivalence point

in CO2 what do the dipoles do? What does this mean?

cancel; not polar

C

carbon

CO₃ ⁻²

carbonate

CO₃²⁻

carbonate

What does EM do?

carries NRG through space

hybridization only if its the ____ atom ( more that 2 atoms present)

central

Cs

cesium

average rate

change in concentration over change in time throughout interval

ClO₂⁻

chlorate

ClO₃ ⁻

chlorate

Cl

chlorine

ClO⁻

chlorite

ClO₂ ⁻

chlorite

CrO₄²⁻

chromate

Cr

chromium

fossil fuels

coal, petroleum, or natural gas; consists of carbonbased molecules derived from decomposition of once-living organisms.

Co

cobalt

What is an electron shell?

collection of orbitals with the same value of n

a =

constant

pure substance

constant composition, mixtures separated by physical methods

1/2 life of first order reaction is ______; it doesn't depend on ______ of ______

constant; concentration; [A]₀

Cu

copper

valence-bond theory...

covalent bond forms when orbitals from two atoms overlap

the electrons in sp hybrid orbitals form ________ with the two F atoms

covalent bonds

Dmitri Mendeleev

created the first periodic table, arranged elements by increasing atomic mass and discovered elements that had yet to be discovered

CN⁻

cyanide

ϱ = 3

d more complicated

As the wavelength increases, the frequency...

decreases

phosphorescence

delay between NRG absorbed and give off of light; lasts longer and continues after NRG source is removed

chemical properties

describe the way a substance may change, or react, to form other substances

effusion

desribes the passage of a gas through a tiny office into an evacuated chamber

Cr₂O₇²⁻

dichromate

vapor pressure lowering (ΔΡ)

difference in vapor pressure between the pure solvent and the solution

H₂PO₄ ⁻

dihydrogen phosphate

Hg₂²⁺

dimercury (l)

If two charges, equal in magnitude and opposite in sign, are separated by a distance, then a _____ is established

dipole

what is µ?

dipole

What does the nuclear charge experienced by an electron depend on?

distance from nucleus and number of electrons in the spherical volume

if rate=K[A] what expect when [A[ doubled?

double

bond order = 2

double bond

Visible/Balmer series

dropping to the first excited state (2)

Ultraviolet/Lyman series

dropping to the ground state

Infrared/Paschen series

dropping to the second excited state (3)

Hertz

e unit of frequency, cycles per second.

pi bonds...

electron density lies above and below the plane of the nuclei; double bond (also has a sigma)

sigma bonds...

electron density lies on axis between nuclei; single bonds

beta particle

electron ejected from the nucleus

Why are sigma bonds more stable?

electrons are surrounded by nucleus (positive charge)

according to Bohr's model, why do colors from exited gases arise? Why is each element different?

electrons move between E states in atom; each element has different number of electrons

What did Bohr's model exhibit?

electrons orbited around nucleus; charged particle moving in orbit should lose E by emitting EM radiation; electrons were confined to specific E states

delocalized electron

electrons that are not stationed to one place (must have resonance structures)

lanthanide

elements 57 - 71

actinide

elements 90 - 103

p-block elements

elements with an outer shell configuration of ns2npx

s-block elements

elements with the valance electron configuration of ns1 or ns2

heat flow into a system and absorb E from surroundings

endothermic reaction

capacity to do work or to produce heat--> transfer of energy from one surface to another based on temperature

energy

law of conservation of energy

energy can be converted from one form to another but can be neither created nor destroyed.

Law of Conservation of Energy

energy can be converted from one to another, but it cannot be created or destroyed; the total energy of the universe is constant

potential energy

energy due to position or composition.

enthalpy of solution ΔΗ

energy of solution

Ionization energy

energy required to remove one electron from a neutral atom

heat

energy transferred between two objects due to a temperature difference between them.

to minimize electorn repulsions, nonbonding pairs are always in _____ positions

equatorial

trigonal bypyramidal: 3 electron pairs in the _______ position and the other 2 are in the ______ position

equatorial; axial

surroundings

everything in the universe surrounding a thermodynamic system.

E flows out of the system; E gained by surroundings must be equal to E lost by system

exothermic reaction

ϱ = 4

f more complicated

What is Hund's rule?

fill each orbital singly before and orbital gets another electron

What is aufbau principle?

fill orbitals in order of increasing E

paper chromatography

filter paper for the stationary phase, biochemists, travels up paper as if it were a wick

F

flourine

Dalton's Law of Partial Pressures

for a mixture of gases in a container Ptot= p1 + p2 + p3

work

force acting over a distance.

pressure=

force/area

Fr

francium

v =

frequency

What is A

frequency factor; related to frequency of collisions and probability that collision will have favorable orientation

melting and freezing

fusion ΔHfus

states of matter

gas, liquid, and solid

scientific laws

general rules that summarize how nature behaves

fluorescence

gives off EM but not after NRG source is removed

what tells us its second order?

graph 1/[A]t versus time and get straight line

what tells us is first order?

graph ln[A](subscript t) versus time and get straight line

Phase diagram

graphs of the phases of matter for a substance vs temperature and pressure

free halogens in concentrated base

halogen-ate ions (ClO₃⁻, etc.)

solid

has a definite shape and volume; molecules are held tightly together in definite arrangements and wiggle slightly

liquid

has a distinct volume independent of its container but had no specific shape; assumes the shape of the portion of the container it occupies; molecules are packed more closely together but move rapidly and slide

gas

has no fixed volume or shape; conforms to the volume and shape of its container; molecules are far apart and move at high speeds

heat capacity t

he amount of energy required to raise the temperature of an object by one degree Celsius.

Alpha decay is limited to

heavy, radioactive nuclei

He

helium

alpha particle

helium nucleus

transition state

high NRG species where ground is flipping around (progress of breaking and forming bonds so high NRG)

Gamma rays

high energy photons produced in association with other forms of decay.

Best for ideal gas behavior

high pressure, low temperature

centi

hundredth

H

hydrogen

HCO₃⁻

hydrogen carbonate

HCO₃ ⁻

hydrogen carbonate (bicarbonate)

HPO₄ ⁻²

hydrogen phosphate

HSO₄⁻

hydrogen sulfate

H₃O⁺

hydronium

OH⁻

hydroxide

BrO ⁻

hypobromite

ClO ⁻

hypochlorite

free halogens in dilute base

hypohalite (ClO⁻, etc.)

What is R equal to?

ideal-gas constant : 8.314 J/K-mol

How does the physical state of reactants affect the rate?

if more readly combine then react more rapidly (gas faster than solidor liquid)

what does enthalpy tell you?

if the reaction will go

significant figures

in a measured quantity, they include one estimated digit (the last digit of the measurement)

Hess's law

in going from a particular set of reactants to a particular set of products, the enthalpy change is the same whether the reaction takes place in one step or in a series of steps; in summary, enthalpy is a state function.

catalysts ______ reaction rates by...

increase; lowering activation energy or increasing number of effective collisions

As the wavelength decreases, the frequency...

increases

precision

indicates how closely different measurements of a quantity agree with one another

accuracy

indicates how well a measurement agrees with the accepted or "true" value

Spin quantum number

indicates the two spin states of an electron in an orbital (ms = 1/2 or -1/2

half life depends on ___ and therefore...

initial concentration; 1/2 life changes as concentration decreases

Electron capture

inner-orbital electron is captured by the nucleus

above the threshold frequency the # of electrons ejected depends on the _____ of the light

intensity

Why can there be a dip in a reaction graph

intermediate present (mcs, come stability but willing to react)

rate law depends on concentration of _______

intermediate species

What kind of relation ship does each have: energy and wavelength; wavelength and frequency; energy and frequency?

inverse, direct, inverse

I

iodine

spectator ions

ions that appear in identical forms among both the reactants and products of a complete ionic equation

Fe

iron

Surface density plot

is a plot of 4(pie)r2 ¥2vs. r.

What does it mean to day that NRG is quantized?

it is not continuous (released/absorbed in steps)

A reaction will always form a gas if...

it produces H₂S and/or HCN.

for a half life equation, what it k equal to?

k= 0.693/t

What is the Arrhenius equation?

k=Ae^(-Activation NRG/RT)

oxidation numbers

keep track of electrons during chemical reactions and are assigned to atoms using specific rules

base unit for thermodynamic temperature...

kelvin

any time Joules in equation, what is the mass in?

kg

Kr

krypton

E or an orbital increases with increasing values of ___

l and n

what is the azimuthal quantum number?

l, defines shape of orbital

S

l=0; sharp

P

l=1; principal

D

l=2; diffuse

F

l=3; fundamental

*

label sections on periodic table (alkali metals, alkaline earth, halogens, noble gases, transition metals)

What do sp orbitals look like?

large lobes of dumbbell

concentrated solution

large quantities of solute relative to solvent

Pb

lead

What is the threshold frequency?

least amount of NRG required to eject electors in photoelectric effect

Intermediates are ___ stable than reactants and they are ____ in quantity but have ______ concentration

less; small; constant

What is the photoelectric effect?

light shining on surface of a metal can cause electrons to be ejected from the metal

solvent

likes dissolve likes, water is universal because it is polar covalent

according to the valence-bond model, a linear arrangement of electron domains implies ____ hybridization

linear; sp

Li

lithium

what is the equation for first order?

ln[A]t= -kt + ln[A]₀

what is the equation for arrhenius equation of a line?

lnk= -activation NRG/RT + lnA

What does molecular geometry ignore?

lone pairs

Hydrates when heated...

lose water of hydration

Intermediates usually unstable with ____concentrations

low

To be labeled as ideal, a gas must satisfy which of the below conditions?

low pressure, high temperature

the _______the number of heat capacity the better conductor, the _________ the number the better insulator

lower, higher

ΔQ = (for temp change)

m*c*ΔT

ΔQ = (for state change)

m*ΔHvap or m*ΔHfus

Mg

magnesium

mϱ =

magnetic quantum number describes the orientation of an orbital possible values: -ϱ to 0 to ϱ

what is the dipole moment?

magnitude of the dipole

balancing a chemical equation

making sure that all atoms present in the reactants are accounted for among the products

Mn

manganese

Density

mass/volume

Wave-particle duality

matter and energy have wave and particle properties

physical change

matter does not change its composition (ex. changes of states)

pure substance

matter that has distinct properties and a composition that doesn't vary from sample to sample (elements and compounds)

amplitude....

max displacement from zero

Electronegativity

measure of the ability of an atom to attract electrons closer to it in a chemical bond

Manometer

measures the pressure of a gas sample

A barometer

measures the pressure of the atmosphere

Hg

mercury

Most metallic oxies are stable, but some decompose to...

metal and oxygen gas

Metal hydrogen carbonates, when heated, decompose to...

metal carbonate and water and carbon dioxide

Metal chlorates when heated decompose to...

metal chloride and oxygen gas

Metallic carbonates when heated decompose to...

metal oxide and carbon dioxide

Metallic hydroxides when heated decompose to...

metal oxide and water

metric system

metric units are used for scientific measurements

micro

millionth

diffusion

mixing of gases

colloidal dispersion (colloid)

mixture in which a dispersed substance is dispersed in a dispersing agent

Dumas Law

mm= DRT/P

mole percent (mol %)

mole fraction x 100%

isoelectronic

molecules or ions that have the same number of valance electrons and comparable lewis structures

van't Hoff factor (i)

moles of particles in solution/moles of formula units dissolved

molarity (M)

moles of solute per 1 L of solution

mole fraction (χ)

moles of solute/(moles of solute + moles of solvent)

molality (m)

moles of the solute per 1 kg of solvent

CO3-2 and PO4-3

most are insoluble except: Group 1 metals and NH4+

OH-

most are insoluble except: Group 1 metals, NH4+, Ba+2, Sr+2 Ca is slightly soluble

S-2

most are insoluble except: Group 1, 2, and NH4+

NO3- and C2H3O2-

most are soluble

SO4-2

most are soluble except: Ca, Ba, Sr, Pb, Ag2

what three factors did arrhenius discover most reaction-rate data obeyed?

must have enough collisions with proper orientation and enough NRG

what is the principle quantum number?

n

for s orbitals # of nodes =

n-1

n(tot) =

n1 + n2 + ...

What is the lowest and most stable orbital?

n=1

PV =

nRT

r = radius =

n^2a/z

Ne

neon

effective nuclear charge...

net positive charge experienced by an electron in many electron atom (Z of eff)

Ni

nickel

NO₃⁻

nitrate

NO₂⁻

nitrite

N

nitrogen

Ground state function has ____ nodes

no

What is the Pauli exclusion principle?

no 2 electrons can have same set of 4 QN

paulo's exclusion principal =

no 2 electrons in the same atom can have the same set of quantum numbers

Pauli exclusion principle

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

Pauli exclusion principle

no two electrons in the same atom can have the same four quantum numbers. there are two electrons with opposite spin in each orbital.

for the rxn 2NO----->2NO + O2, would NO and O2 be produced at the same time?

no, NO produced 2x faster

do pi bonds have hybridization? why or why not?

no; only p orbitals involved

why are reactions likely not one step?

not very likely all species hit each other at one time with correct orientation

6 electron domains equals...

octahedral

atomic size (radius)

one half of the distance of closest approach between two nuclei in the ordinary form of an element

chemical change

one in which a given substance becomes a new substance with different properties and different composition

semipermeable membrane

openings are for size specific and smaller particles

2 electrons of _____ spin in orbital overlap

opposite

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

C₂O₄²⁻

oxalate

O

oxygen

ϱ = 2

p bilobed

momentum, mv, is a ____ property

particle

BrO₄ ⁻

perbromate

ClO₄ ⁻

perchlorate

ClO₄⁻

perchlorate

MnO₄⁻

permanganate

O₂²⁻

peroxide

PO₄ ⁻³

phosphate

PO₄³⁻

phosphate

P

phosphorus

What is the emission spectrum?

photons emitted from excited state systems as they drop to lower NRG states

boiling and freezing

physical changes

what are the four factors that affect rate?

physical state of reactants, temp of reaction; catalyst; concentration of reactants

h =

planck's constant = 6.626 * 10^-34 J*s

Pt

platinum

It is possible for a molecules with polar bonds to be ______ or _______

polar nonpolar

Endothermic =_____process Exothermic=_______ process

positive negative

K

potassium

Rydberg's equation (definition)

predicts the position and wavelength of any line in a given series

SI units

preferred units used in scientific measurement (length=meter (m), mass=kilogram (kg), time=second (s), temperature=Kelvin (K))

if the volume of a sample of gas in a piston is decreased to 1/3 of its original value at a constant temperature, which of the following will increase?

pressure

n =

principal quantum # - "Energy level" describes size of an orbital possible values: 1,2,3...

Absorption spectrum

produced when atoms absorb photons of certain wavelengths and become excited

Emission spectrum

produced when atoms in an excited state emit photons as they return to lower energy states

colligative property

property which depends on the number of solute particles dissolved in solution

bases

proton acceptors; they increase the concentration of OH-(aq) in aqueous solutions

recrystallization

purification of a solid involves dissolving the solid and letting it precipitate out of solution and reform

if rate=k[A]² what expect when A doubled

quadrupled

e- spin is ___ so can only have 1 spin OR other spin (no in between

quantized

Electromagnetic radiation

radiation that consists wave like electric and magnetic fields, including light, microwaves, radio signals, and x-rays.

Ra

radium

Rn

radon

instantaneous rate

rate at that exact time; must graph concentration vs time and get slope of curve at time of exact interest

Bar

reactant is solid

Crystals

reactant is solid

Filings

reactant is solid

Pellet

reactant is solid

Powdered

reactant is solid

Ribbon

reactant is solid

Turnings

reactant is solid

exchange reactions or metathesis

reactions such as precipitation reactions, in which cations and anions appear to exchange partners

precipitation reactions

reactions that result in the formation of an insoluble product

endothermic

refers to a reaction where energy (as heat) flows into the system.

exothermic

refers to a reaction where energy (as heat) flows out of the system.

What is a node?

region in space where probability of finding electrons is zero

extensive properties

relate to the amount of substance present

electrons in multiple bonds _____ more than electrons in single bonds

repel

What is absorption spectrum?

result form the absorption of electromagnetic radiation (ES to GS)

in theory all reactions are ____

reversible

aufbau principle

rule stating that sublevels are filled in order of increasing energy

ϱ = 1

s spherical

For a particular substance, λ emitted in EM spectra are ________ as λ absorbed in absorption spectra

same

degenerate...

same energy (same l and n)

Sc

scandium

Tyndall effect

scattering of light by a colloid

chain reaction

self-sustaining fission process

What is a sub-shell?

set of orbitals with the same n and l

What things are required in the FR answers?

shape name, number of bonded or unboded pairs, angle, and hybridization

orbital overlap...

shared region of space between orbitals

Higher NRG EMs should have ____ wavelengths and _____ frequencies

short; large

complete ionic equation

shows all dissolved strong electrolytes as their component ions

Si

silicon

Ag

silver

bond order =1

single bond

dilute solution

small quantities of solute relative to solvent

What is quanta?

smallest amount of E that can be emitted or absorbed as electromagnetic radiation

Na

sodium

Cl- and most other halides

soluble except: Ag, Pb, Hg2

What are the strong bases?

soluble hydroxides (alkali hydroxides and Ba2+), slightly soluble hydroxides (Ca2+ and Sr2+)

solution

solute dissolved in a solvent

strong electrolytes

solutes that exist in solution completely or nearly completely as ions

weak electrolytes

solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions

homogenous mixture

solution

supersaturated solution

solution contains more than the equilibrium amount

endothermic reaction-

solution gets cooler

exothermic reaction-

solution gets warmer

aqueous solution

solution in which water is the solvent

osmosis

solvent travels through a semi-permeable membrane in order to dilute a more concentrated solution

transition elements

some elements that lie in rows 4 to 7 of the periodic table, comprising scandium through zinc, yttrium through cadmium and lanthanum through mercury

c =

speed of light = λ*v

ms =

spin quantum number possible values: ± 1/2

When electrons are close to proton/nucleus, the atom is more ____ and has ____ NRG

stable; lower

Uncertainty principle (definition)

stated that it is impossible to know the exact position and momentum of a particle simultaneously

Heisenberg's Uncertainty principle

states it is impossible to determine both the position and the momentum of an electron in an atom simultaneously with great certainty.

ferromagnetism

stronger, permanent magnetism, unpaired electrons are influenced by orientations of their neighboring electrons

Sr

strontium

compound

substance with a constant composition that can be broken down into elements by chemical processes

elements

substances that cannot be decomposed into simpler substances by chemical or physical means

acids

substances that ionize in aqueous solutions to form hydrogen ions, thereby increasing the concentration of H+ (aq) ions. Also known as proton donors

SO₄²⁻

sulfate

SO₃²⁻

sulfite

S

sulfur

include everything else in the universe

surroundings

syngas

synthetic gas, a mixture of carbon monoxide and hydrogen, obtained by coal gasification.

part of the universe on which we wish to focus attention

system

What is the equation for half life?

t(of 1/2) = (1/k[A]₀)

reaction order..

tell how concentration changes affect rate

deci

tenth

4 electron domains equals...

tetrahedral

system

that part of the universe on which attention is to be focused.

Kelvin scale

the SI temperature scale

percent yield

the actual yield of a product as a percentage of the theoretical yield.

concentration

the amount of solute dissolved in a given quantity of solvent or quantity of solution

solubility

the amount of solute which will dissolve in a solvent at a certain temperature

solubility

the amount of the substance that can be dissolved in a given quantity of solvent at the given tenperature

chemical stoichiometry

the calculation of the quantities of material consumed and produced in chemical reactions.

energy

the capacity to do work or to cause heat flow.

All p orbitals have node in ....

the center

what is delta E equal to?

the change in energy from the products to the reactants

Z (in equations)

the charge of the nucleus

quantitative analysis

the determination of the amount of a given substance that is present in a sample

qualitative analysis

the determination of the presence or absence of a particular substance in a mixture

entropy

the disorder of the universe is increasing

Wavelength

the distance between successive crests in a wave.

Wavelength

the distance the wave travels during one cycle (λ)

volatile

the ease with which a substance can be changed to its vapor

Aufbau process

the electrons are arranged in an atom in order of increasing energy

core electrons

the electrons in an atom's completed set of shells

law of constant composition (law of definite proportions)

the elemental composition of a pure compound is always the same

Blackbody radiation

the emission of light from hot objects. showed that energy is quantized and only certain values allowed (Planck)

electron affinity

the energy change occuring when an atom of the lement in the gas phase gains an electron

heat of hydration ΔΗ

the energy it takes to dissolve a solute in water

first law of thermodynamics

the energy of the universe is constant; same as the law of conservation of energy.

specific heat capacity

the energy required to raise the temperature of one gram of a substance by one degree Celsius.

molar heat capacity

the energy required to raise the temperature of one mole of a substance by one degree Celsius.

ionization energy

the energy required to remove an electron from an atom or ion in the gas phase

standard enthalpy of formation

the enthalpy change that accompanies the formation of one mole of a compound at 25°C from its elements, with all substances in their standard states at that temperature

Celsius scale

the everyday temperature scale of most countries

molecular formula

the exact formula of a molecule, giving the types of atoms and the number of each type.

Momentum (definition)

the force or speed with which something moves

reduction

the gain of electrons by a substance

Amplitude

the height of a crest of each wave (the intensity of the radiation)

Wave-particle duality

the idea that the electron has properties of both a wave and a particle.

inner transition elements

the lanthanides and actinides series

oxidation

the loss of electrons by a substance

ground state

the lowest energy state of an atom

Principal quantum number

the main energy level occupied by the electron (n = 1, 2, 3, etc)

molar mass

the mass in grams of one mole of molecules or formula units of a substance; also called molecular weight.

Orbitals

the matter wave for an allowed energy state of an electron in an atom or molecule.

theoretical yield

the maximum amount of a given product that can be formed when the limiting reactant is completely consumed.

temperature

the measure of the hotness or coldness of an object; determines the direction of heat flow

Hund's rule

the most stable arrangement of electrons is that with the maximum number of unpaired electrons, all with the same spin direction

salt

the neutralization reaction between an acid and a metal hydroxide produces water and salt or any ionic compound whose cation comes from a base and whose anion comes from an acid

effective nuclear charge

the nuclear charge experiences by an electron in a multielectron atom, as modified by the other electrons

Quantum number

the number assigned to each orbit of an electron

mole (mol)

the number equal to the number of carbon atoms in exactly 12 grams of pure ¹²C : Avogadro's number. One mole represents 6.02 x 10²³ units.

Avogadro's number

the number of atoms in exactly of pure ¹²C , equal to 6.02 x 10²³

Frequency

the number of complete waves passing a point in a given amount of time.

Frequency

the number of cycles the wave undergoes per second (ν)

Magnetic quantum number

the orientation of an orbital around the nucleus (ml = -l to l)

valance electrons

the outermost and most reactive electrons of an atom

mass percent

the percent by mass of a component of a mixture or of a given element in a compound.

Paramagnetic

the physical property of being attracted by a magnetic field.

Diamagnetic

the physical property of being repelled by a magnetic field, resulting from having all electrons paired.

equivalence point

the point in the titration at which stoichiometry equivalent quantities of reactants are brought together

osmotic pressure

the pressure required to stop the osmotic flow

Electron density

the probability of finding an atomic electron within a given region of space.

Speed of a wave

the product of the frequency and wavelength (m/s)

Principle quantum number

the quantum number n that is a positive unitless integer and represents the energy level.

Angular momentum quantum number

the quantum number that indicates the shape of the orbital (l = 0 to n-1)

mole ratio

the ratio of moles of one substance to moles of another substance in a balanced chemical equation.

limiting reactant

the reactant that is completely consumed when a reaction is run to completion.

displacement reactions

the redox reactions between metals and acids and between metals and salts

calorimetry

the science of measuring heat flow.

actinides

the series of elements between actinium and rutherfordium in the periodic table

lanthanides

the series of elements between lanthanum and hafnium in the periodic table

empirical formula

the simplest whole-number ratio of atoms in a compound.

atom

the smallest representative particle of an element

Henry's Law

the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid

boiling point elevation

the solution has a boiling point that is higher that the original pure solvent's b.p. - colligative

freezing point depression

the solution has a freezing point that is lower than the original pure solvent's f.p. - colligative

Line emission spectrum

the spectrum of light emitted by excited atoms in the gas phase, consisting of discrete wavelengths.

what does the rate of effusion measure?

the speed at which the gas is transferred into the chamber

Excited state

the state of an atom in which at least one electron is not in the lowest possible energy level.

Ground state

the state of an atomic which all electrons are in the lowest possible energy levels.

thermodynamics

the study of energy and its interconversions.

chemistry

the study of the composition, structure, properties, and changes of matter

components

the substances that make up a mixture

Internal energy E of a system is

the sum of the kinetic and potential energies of all the "particles" in the system.

Boundary surface

the surface of an orbital that makes the orbital easier to draw

average atomic mass

the weighted average mass of the atoms in a naturally occurring element; also known as atomic weight

Some compounds can be decomposed by electricity into...

their elements

study of energy and its inter conversions

thermodyamics

NCS⁻

thiocyanate

SCN⁻

thiocyanate

S₂O₃²⁻

thiosulfate

chromatoraphy

third method of separation, stationary phase a solid, mobile phase is either liquid or gas. High affinity for mobile phase moves quickly, high affinity for solid phase moves slowly

strong acids

those acids that are strong electrolytes

strong bases

those bases that are strong electrolytes

net ionic equation

those ions that go through the reaction unchanged (spectator ions) are omitted

kilo

thousand

milli

thousandth

if rate=k[A]³ what expect when [A] double?

time eight

What is half life?

time for [A]t to reach 1/2[A]₀

Sn

tin

Ti

titanium

5 electron domains equals...

trigonal bypyramidal

3 electron domains equals...

trigonal planar

pico

trillionth (0.000 000 000 001)

bond order = 3

triple bond

W

tungsten

Why are two spots for line spectrum of a many electron atom found?

two different spins

miscible

two liquids are soluble in each other at any amount

photons...

type of quanta, deal with radiant NRG and light NRG

Atomic Mass

unit=amu Average mass of all the naturally occurring isotopes of an element

U

uranium

What is the magnetic quantum number?

values between -l and +l; gives 3D orientation of each orbital

V

vanadium

Raoult's law

vapor pressure of the solution equals mole fraction of the solution x the vapor pressure of the pure solvent

evaporating and condensing

vaporization ΔHvap

mixture

variable composition

bond dipoles and dipole moments are ______ qualities

vector (have direction and size)

Some oxyacids when heated decompose to...

water and nonmetal oxide

de Broglie decided matter can act like a _____

wave

λ is a _____ property

wave

λ =

wavelength

What to properties does light exhibit?

wavelike and particle-like

weak acids

weak electrolytes

weak bases

weak electrolytes

law

what happened, observations

Refraction

when a light wave passes from one medium into another and the speed of the wave changes.

Diffraction

when a wave strikes the edge of an object and bends around it or breaks apart.

ideal solution

when both the solute and the solvent are volatile and follows Raoult's law at all concentrations

when can zero order reactions sometimes occur?

when enzymes act as catalysts

what tells us its zero order?

when graph concentration versus time and get straight line

When does a zero order graph show a horizontal line?

when graphed rate versus concentration (not affected by concentration)

When electrons move between orbitals, when is energy emitted (negative)?

when n of initial is greater than n of final

neutralization reaction

when solutions and of acids and bases are mixed this reaction occurs

can bond orders be fractions?

yes

if molecular geomotry linear and B atoms are different, is it polar?

yes

Heisenberg's uncertainty principle

ΔX * mΔv

ΔH° =

Σ(np*ΔH°fp) - Σ(nr*ΔH°fr)

de Broglie's wavelength

λ = h/(mv) m = mass in kg v = velocity in m/s

What equation did de Broglie derive?

λ = h/mv (must have mass in kg!)

de Broglie wavelength (equation)

λ = h/mν

Equation for calculating the wavelength of a photon

λ = hν/∆E

Anion

— lost e-

μrms =

√(3*R*T/(molar mass))

(Rate of Effusion of Gas A) / (Rate of Effusion of Gas B) =

√(Molar mass of gas B) / √(Molar mass of gas A)

To completely remove electrons n = ___ and E= ___

∞ ; 0


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