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AP Chem [Exam] > Basic Review > Flashcards

Basic Review Flashcards

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1
Q

Scientific Method

A

a method of investigation involving observation and theory to test scientific hypotheses

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2
Q

Law of Conservation of Mass

A

matter can’t be created nor destroyed

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3
Q

Mass

A

a measure of resistance of an object to a change in its state of motion

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4
Q

Weight

A

amount of gravitational force exerted on an object

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5
Q

Celsius to Kelvin

A

Tk=Tc+273

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6
Q

Matter

A

anything occupying space and with mass

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7
Q

Law of Definite Proportion

A

a given compound always has exactly the same proportion of elements by mass

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8
Q

Law of Multiple Proportions

A

when two elements form a series of compounds, the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers

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9
Q

Radioactivity

A

Spontaneous emission of radiation

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10
Q

Types of Radiation

A

Alpha Particles- 2+ charge Beta Particles- high-speed electrons

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11
Q

Isotopes

A

atoms with the same number of protons but a different number of neutrons Gamma Ray- high-energy light

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12
Q

Chemical Bonds

A

Force that holds atoms together

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13
Q

Naming Binary Ionic Compounds

A

1.Cation first, anion second

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14
Q

Naming Polyatomic Ions

A

1.The ion with the smaller number of O2 ends in -ite

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15
Q

Finding Empirical Formulas

A

1.Calculate moles of each atom in molecule

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16
Q

Percent Yield

A

Actual Yield/Theoretical Yield*100%

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17
Q

Net Ionic Equation

A

only contains ions that change in reaction

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18
Q

Acids

A

substances that form H+ when dissolved in water; proton donors

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19
Q

Bases

A

Substances that form OH- when dissolved in water; proton acceptors

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20
Q

Molarity

A

moles of solute/volume of soln(L)

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21
Q

1atm=?mmHg/Torr

A

760mmHg/Torr

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22
Q

1atm=?Pa

A

101,325 Pa

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23
Q

Ideal Gas Law

A 
PV=nRT P=atm
V=L
n=mol
R=.0826Latm/Kmol
T=K
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24
Q

STP

A

0°C and 1 atm

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25
Q

Dalton’s Law of Partial Pressures

A

Ptotal=P1+P2+P3+…

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26
Q

Kinetic Molecular Theory

A

-FOR IDEAL GASES!!!

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27
Q

Decrease Volume and Increase Temperature

A

Increase Pressure

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28
Q

Increase Temperature

A

Increase Volume

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29
Q

Root Mean Square Velocity

A

u(rms)=(3RT/M)^1/2 R=8.31J/Kmol

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30
Q

Joule

A

SI unit of energy; Kg*m^2/s^2

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31
Q

Molality

A

mol of solute/kg of solvent

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32
Q

Normality

A

(N) number of equivalents per liter of solution

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33
Q

Enthalpy of Solution

A

▲Hsoln=▲H1+▲H2+▲H3+…

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34
Q

Chemical Kinetics

A

studies the rate at which a chemical process occurs and sheds light on its reaction mechanism

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35
Q

Zero-Order Rate Law

A

r=k

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36
Q

First-Order Rate Law

A

r=k[A]

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37
Q

Second-Order Rate Law

A

r=k[A]^2

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38
Q

Zero-Order Half Life

A

[A]0/2k

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39
Q

First-Order Half Life

A

.69/k

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40
Q

Second-Order Half Life

A

1/([A]0*k)

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41
Q

Integrated Rate Law

A

expresses how the concentrations depend on time

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42
Q

Overall Reaction Order

A

n+m (these are orders of reactants)

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43
Q

Integrated First-Order Rate Law

A

ln[A]=-kt + ln[A]0 -linear form

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44
Q

Integrated Second-Order Rate Law

A

1/[A]=kt + 1/[A]0

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45
Q

Integrated Zero-Order Rate Law

A

[A]=-kt + [A]0

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46
Q

c=

A

λv

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47
Q

Speed of light

A

c=2.9979*10^8 m/s

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48
Q

Theory of Relativity

A

E=mc^2

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49
Q

Quantum Model

A

electrons in a hydrogen atom move around the nucleus only in circular orbits

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50
Q

Quantum Mechanical Model

A

involves quantum numbers

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51
Q

Quantum Numbers

A

describe various properties of one orbital

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52
Q

Principal Quantum Number

A

(n) has values 1,2,3,…; tells energy levels

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53
Q

Angular Momentum Quantum Number

A

(ℓ), has values from 0 to (n-1); tells shape of atomic orbitals

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54
Q

ℓ=0

A

s orbital

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55
Q

ℓ=1

A

p orbital

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56
Q

ℓ=2

A

d orbital

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57
Q

ℓ=3

A

f orbital

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58
Q

ℓ=4

A

g orbital

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59
Q

Magnetic Quantum Number

A

(mℓ) has values from -ℓ to ℓ, including zero; tells orientation of the orbital relative to other orbitals

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60
Q

Nodes

A

where there are no electrons

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61
Q

Electron Spin Quantum Number

A

(msubs) can only be +1/2 or -1/2

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62
Q

Pauli Exclusion Principle

A

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

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63
Q

Aufbau Principle

A

as protons are added to the nucleus, electrons are similarly added

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64
Q

Hund’s Rule

A

the lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals

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65
Q

Equilibrium Expression

A

K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don’t count

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66
Q

Equilibrium constant

A

K

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67
Q

Reaction Quotient

A

(Q) does the same as equilibrium expression, except it uses initial concentrations

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68
Q

Q=K

A

at equilibrium (Q?K)

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69
Q

Q>K

A

shift to left (Q?K)

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70
Q

Q

A

shift to right (Q?K)

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71
Q

Le Chatelier’s Principle

A

if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change

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72
Q

Acid Dissociation Constant

A

Ka=[products]^m/[reactants]^n

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73
Q

pH=

A

Err:509

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74
Q

Buffered Solution

A

a solution that resists a change in its pH

75
Q

Solubility Product

A

(Ksp) an equilibrium expression

76
Q

Law of Conservation of Energy

A

energy can’t be created nor destroyed

77
Q

Heat

A

the transfer of energy between two objects due to temperature difference

78
Q

Work

A

force acting over distance

79
Q

▲E

A

q+w

80
Q

Specific Heat Capacity

A

J/°Cg or J/Kg

81
Q

Molar Heat Capacity

A

J/°Cmol or J/Kmol

82
Q

Hess’s Law

A

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

83
Q

▲H°reaction

A

Σn▲H°(products)-Σn▲H°(reactants)

84
Q

Entropy

A

(S) the driving force for a spontaneous is an increase in entropy of the universe

85
Q

▲Suniv

A

▲Ssys+▲Ssurr

86
Q

▲Ssurr

A

-▲H/T

87
Q

▲G

A

▲H-T▲S

88
Q

▲G°

A

▲H°-T▲S°

89
Q

G

A

G°+RTln(Q) R=8.31

90
Q

w(max)

A

Err:501

91
Q

Galvanic Cell

A

a device in which chemical energy is changed to electrical energy

92
Q

Anode

A

where oxidation occurs

93
Q

Cathode

A

where reduction occurs

94
Q

Cell Potential

A

(Ecell) driving force of the electrons

95
Q

Volt

A

unit of electrical potential; J/C

96
Q

Faraday

A

96,485 C/mol e-

97
Q

▲G

A

-nFE E=cell potential

98
Q

Ampere

A

(A), C/s

99
Q

Bond Energy

A

energy required to break a bond

100
Q

Polar Covalent Bond

A

bond in which atoms aren’t so different that electrons are completely transferred but are different enough that unequal sharing occurs

101
Q

Electronegativity

A

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

102
Q

Dipole Moment

A

a molecule having a center of positive charge and a center of negative charge

103
Q

▲H

A

Σ(bonds broken)-Σ(bonds formed)

104
Q

Lone Pair

A

pairs of electrons localized on an atom

105
Q

Bonding Pairs

A

electron pairs found in the space between the atoms

106
Q

Resonance

A

when more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows

107
Q

Formal Charge

A

(# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)

108
Q

Valence Electrons(assigned)

A

(# of lone pair e-)+1/2(# of shared e-)

109
Q

Steps to VSEPR Model

A
  1. Draw the Lewis Structure
110
Q

Linear

A

180°, sp

111
Q

Trigonal Planar

A

120°, sp^2

112
Q

Tetrahedral

A

109.5°, sp^3

113
Q

Trigonal Bipyramidal

A

90°&120°, dsp^3

114
Q

Octahedral

A

90°, d^2sp^3

115
Q

Hybridization

A

the mixing of native atomic orbitals to form special orbitals for bonding

116
Q

Sigma Bond

A

the line running between the atoms

117
Q

Pi Bond

A

occupies the space above and below a sigma bond

118
Q

Molecular Orbitals (MOs)

A

similar to atomic orbitals, except between molecules

119
Q

Antibonding Molecular Orbital

A

higher in energy than the atomic orbitals of which it is composed

120
Q

Bond Order

A

bonding e- - # antibonding e-/2

121
Q

Coordination Compound

A

consists of a complex ion, a transition metal with attached ligands, and counterions

122
Q

Counterions

A

anions or cations as needed to produce a compound with non net charge

123
Q

Ligand

A

a neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion

124
Q

London Dispersion Forces

A

the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

125
Q

+ Delta G

A

Thermodynamically unfavorable (non-spontaneous)

126
Q
  • Delta G
A

Thermodynamically favorable (spontaneous)

127
Q
  • Delta H
A

Exothermic, more energy released by bonds forming than absorbed by bonds breaking

128
Q

+ Delta H

A

Endothermic, more energy absorbed by bonds breaking than released by bonds forming

129
Q

+ Delta S

A

Increase in entropy, more disorder on right side than left side

130
Q
  • Delta S
A

decrease in entropy, more disorder on left side than right side

131
Q

Large eq. constant K

A

Forward reaction favored, greater rt. side than left side concentration/pressures, - delta G

132
Q

Small eq. constant K

A

backward reaction favored, greater left side than right side concentration/pressure, + delta G

133
Q

Acids with a large Ka

A

Stronger (more ionizing, more hydrogens free to roam)

134
Q

Bases with small Kb

A

Weaker (less ionizing, more hydroxides “stuck” to cation)

135
Q

Coefficients ARE exponents for..

A

Equilibrium expression

136
Q

Coefficients MAY be exponents for..

A

Rate law

137
Q

Boyle’s law

A

Pressure and volume of gases are inversely related at constant temperature.

138
Q

Pb (2+) + Ni → Ni (2+) + Pb…..which is cathode?

A

Pb(2+)/Pb

139
Q

How do you solve a calorimetry problem?

A

Q (lost)= Q (gained)

140
Q

Which is anode, which is cathode?

A

More positive (as on reduction potential table) is the anode

141
Q

What is the combined gas law?

A

(P1V1/)/T1=(P2V2)/T2

142
Q

What is half life constant?

A

1st order reactions!!

143
Q

What graph represents a 1st order reaction?

A

ln[A] versus time is linear

144
Q

What is the titration equation?

A

MaVana=MbVbnb

145
Q

What is electrical force?

A

Force= (Kq1q2)/r^2

146
Q

What does Kp=Kc?

A

Kp=Kc(RT)^Δn (of gas…right compared to left)

147
Q

What is entropy?

A

amount of disorder in a system (lower number means less disorder)

148
Q

When is ΔG negative (thermodynamically favorable)?

A

ALWAYS when +ΔS and -ΔH

149
Q

How is absorbance related to % transmittance?

A

A=-log(%T/100)

150
Q

When does K=Q?

A

system is at equilibrium and reaction does not shift to left or right

151
Q

What happens to bonds in an exothermic reaction?

A

They are formed

152
Q

What happens to bonds in an endothermic reaction?

A

They are broken.

153
Q

What is vapor pressure?

A

the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system.

154
Q

When does pH=pKa?

A

half equivalence point

155
Q

When can dispersion forces in one substance be greater than hydrogen bond forces in another substance?

A

if there is a temporary dipole moment

156
Q

electronegativity

A

how much the nucleus pulls on the shared electrons

157
Q

critical point

A

When a substance has reached an irreversible state of matter

158
Q

larger k favors the…

A

right side stuff, or products

159
Q

What graph represents a zero order reaction?

A

[A] vs. time if it is linear

160
Q

What graph represents a second order reaction?

A

1/[A] vs. time if it is linear

161
Q

buffer

A

weak acid with its conjugate base or weak base with its conjugate acid

162
Q

Absorbance

A

A=(absorbativity)(path length in m)(concentration in M)

163
Q

vapor pressure

A

keeps a substance from becoming a gas, increases with pressure

164
Q

Hydrogen bonds

A

Oxygen, Nitrogen, Fluorine with

Hydrogen

165
Q

Strong IMF

A

means a higher boiling point, harder to change phases, greater the difference in electronegativity means the stronger the attraction.

166
Q

sublimation

A

change directly from solid to gas at low pressure

167
Q

temperature

A

the average kinetic energy, the speed of particles

168
Q

One of the few substances that expands in solid form

A

water

169
Q

changes directly from gas to solid

A

deposition

170
Q

weak acids

A

do not dissociate completely, does not release all its hydrogens, higher pKa, does not fully “break away”

171
Q

To change a substance from solid to liquid or liquid to gas…

A

you’d need an increase in temperature or a decrease in pressure.

172
Q

factors that affect rate

A

reaction type, temperature, pressure, surface area, & catalysts

173
Q

Titration equation with acid/base

A

(#H+) m1v1=m2v2(#OH-)

174
Q

REDOX

A

reduction: gains electrons

175
Q

Atomic Radius & Ionization Energy & Electronegativity Trends

A

Atomic Radius: Increase↓, Decrease→ Ionization Energy: Decrease↓, Increase→
Electronegativity: same as Ionization Energy

176
Q

Brønsted-Lowery Conjugate Acid/Base Pairs

A

Conjugate base = acid - one H⁺

177
Q

Slowest step in multi-step reaction

A

slow rate step = rate determining

178
Q

Beer’s Law

A

A= - log%T A=Absorbance

T=Transmittance in DECIMAL

179
Q

Kw

A

Kw=1.0x10⁻¹⁴

180
Q

What is the numerator and denominator in the K eq?

A

(right side stuff) raised to coefficients/left side stuff raised to coefficients

181
Q

Effective charge on an electron

A

Number of protons in nucleus-number of electrons in lower energy levels.

182
Q

What are the strong acids?

A

HCl, HBr, HI, HNO3, and first hydrogen ion on H2SO4

183
Q

Covalent Network Solids

A

Diamond (Carbon), Graphite (Carbon), Sand (SiO₂)

AP Chem [Exam] (5 decks)

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