AP Chemistry Exam Study
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
