Basic Review Flashcards
(183 cards)
1
Q
Scientific Method
A
a method of investigation involving observation and theory to test scientific hypotheses
2
Q
Law of Conservation of Mass
A
matter can’t be created nor destroyed
3
Q
Mass
A
a measure of resistance of an object to a change in its state of motion
4
Q
Weight
A
amount of gravitational force exerted on an object
5
Q
Celsius to Kelvin
A
Tk=Tc+273
6
Q
Matter
A
anything occupying space and with mass
7
Q
Law of Definite Proportion
A
a given compound always has exactly the same proportion of elements by mass
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
9
Q
Radioactivity
A
Spontaneous emission of radiation
10
Q
Types of Radiation
A
Alpha Particles- 2+ charge Beta Particles- high-speed electrons
11
Q
Isotopes
A
atoms with the same number of protons but a different number of neutrons Gamma Ray- high-energy light
12
Q
Chemical Bonds
A
Force that holds atoms together
13
Q
Naming Binary Ionic Compounds
A
1.Cation first, anion second
14
Q
Naming Polyatomic Ions
A
1.The ion with the smaller number of O2 ends in -ite
15
Q
Finding Empirical Formulas
A
1.Calculate moles of each atom in molecule
16
Q
Percent Yield
A
Actual Yield/Theoretical Yield*100%
17
Q
Net Ionic Equation
A
only contains ions that change in reaction
18
Q
Acids
A
substances that form H+ when dissolved in water; proton donors
19
Q
Bases
A
Substances that form OH- when dissolved in water; proton acceptors
20
Q
Molarity
A
moles of solute/volume of soln(L)
21
Q
1atm=?mmHg/Torr
A
760mmHg/Torr
22
Q
1atm=?Pa
A
101,325 Pa
23
Q
Ideal Gas Law
A
PV=nRT P=atm V=L n=mol R=.0826Latm/Kmol T=K
24
Q
STP
A
0°C and 1 atm
25
Dalton's Law of Partial Pressures
Ptotal=P1+P2+P3+...
26
Kinetic Molecular Theory
-FOR IDEAL GASES!!!
27
Decrease Volume and Increase Temperature
Increase Pressure
28
Increase Temperature
Increase Volume
29
Root Mean Square Velocity
u(rms)=(3RT/M)^1/2 R=8.31J/Kmol
30
Joule
SI unit of energy; Kg*m^2/s^2
31
Molality
mol of solute/kg of solvent
32
Normality
(N) number of equivalents per liter of solution
33
Enthalpy of Solution
▲Hsoln=▲H1+▲H2+▲H3+...
34
Chemical Kinetics
studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
35
Zero-Order Rate Law
r=k
36
First-Order Rate Law
r=k[A]
37
Second-Order Rate Law
r=k[A]^2
38
Zero-Order Half Life
[A]0/2k
39
First-Order Half Life
.69/k
40
Second-Order Half Life
1/([A]0*k)
41
Integrated Rate Law
expresses how the concentrations depend on time
42
Overall Reaction Order
n+m (these are orders of reactants)
43
Integrated First-Order Rate Law
ln[A]=-kt + ln[A]0 -linear form
44
Integrated Second-Order Rate Law
1/[A]=kt + 1/[A]0
45
Integrated Zero-Order Rate Law
[A]=-kt + [A]0
46
c=
λv
47
Speed of light
c=2.9979*10^8 m/s
48
Theory of Relativity
E=mc^2
49
Quantum Model
electrons in a hydrogen atom move around the nucleus only in circular orbits
50
Quantum Mechanical Model
involves quantum numbers
51
Quantum Numbers
describe various properties of one orbital
52
Principal Quantum Number
(n) has values 1,2,3,...; tells energy levels
53
Angular Momentum Quantum Number
(ℓ), has values from 0 to (n-1); tells shape of atomic orbitals
54
ℓ=0
s orbital
55
ℓ=1
p orbital
56
ℓ=2
d orbital
57
ℓ=3
f orbital
58
ℓ=4
g orbital
59
Magnetic Quantum Number
(mℓ) has values from -ℓ to ℓ, including zero; tells orientation of the orbital relative to other orbitals
60
Nodes
where there are no electrons
61
Electron Spin Quantum Number
(msubs) can only be +1/2 or -1/2
62
Pauli Exclusion Principle
in a given atom no two electrons can have the same set of four quantum numbers
63
Aufbau Principle
as protons are added to the nucleus, electrons are similarly added
64
Hund's Rule
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
65
Equilibrium Expression
K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
66
Equilibrium constant
K
67
Reaction Quotient
(Q) does the same as equilibrium expression, except it uses initial concentrations
68
Q=K
at equilibrium (Q?K)
69
Q>K
shift to left (Q?K)
70
Q
shift to right (Q?K)
71
Le Chatelier's Principle
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
72
Acid Dissociation Constant
Ka=[products]^m/[reactants]^n
73
pH=
Err:509
74
Buffered Solution
a solution that resists a change in its pH
75
Solubility Product
(Ksp) an equilibrium expression
76
Law of Conservation of Energy
energy can't be created nor destroyed
77
Heat
the transfer of energy between two objects due to temperature difference
78
Work
force acting over distance
79
▲E
q+w
80
Specific Heat Capacity
J/°C*g or J/K*g
81
Molar Heat Capacity
J/°C*mol or J/K*mol
82
Hess's Law
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
▲H°reaction
Σn▲H°(products)-Σn▲H°(reactants)
84
Entropy
(S) the driving force for a spontaneous is an increase in entropy of the universe
85
▲Suniv
▲Ssys+▲Ssurr
86
▲Ssurr
-▲H/T
87
▲G
▲H-T▲S
88
▲G°
▲H°-T▲S°
89
G
G°+RTln(Q) R=8.31
90
w(max)
Err:501
91
Galvanic Cell
a device in which chemical energy is changed to electrical energy
92
Anode
where oxidation occurs
93
Cathode
where reduction occurs
94
Cell Potential
(Ecell) driving force of the electrons
95
Volt
unit of electrical potential; J/C
96
Faraday
96,485 C/mol e-
97
▲G
-nFE E=cell potential
98
Ampere
(A), C/s
99
Bond Energy
energy required to break a bond
100
Polar Covalent Bond
bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
101
Electronegativity
ability of an atom in a molecule to attract shared electrons to itself
102
Dipole Moment
a molecule having a center of positive charge and a center of negative charge
103
▲H
Σ(bonds broken)-Σ(bonds formed)
104
Lone Pair
pairs of electrons localized on an atom
105
Bonding Pairs
electron pairs found in the space between the atoms
106
Resonance
when more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
107
Formal Charge
(# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
108
Valence Electrons(assigned)
(# of lone pair e-)+1/2(# of shared e-)
109
Steps to VSEPR Model
1. Draw the Lewis Structure
110
Linear
180°, sp
111
Trigonal Planar
120°, sp^2
112
Tetrahedral
109.5°, sp^3
113
Trigonal Bipyramidal
90°&120°, dsp^3
114
Octahedral
90°, d^2sp^3
115
Hybridization
the mixing of native atomic orbitals to form special orbitals for bonding
116
Sigma Bond
the line running between the atoms
117
Pi Bond
occupies the space above and below a sigma bond
118
Molecular Orbitals (MOs)
similar to atomic orbitals, except between molecules
119
Antibonding Molecular Orbital
higher in energy than the atomic orbitals of which it is composed
120
Bond Order
bonding e- - # antibonding e-/2
121
Coordination Compound
consists of a complex ion, a transition metal with attached ligands, and counterions
122
Counterions
anions or cations as needed to produce a compound with non net charge
123
Ligand
a neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
124
London Dispersion Forces
the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
125
+ Delta G
Thermodynamically unfavorable (non-spontaneous)
126
- Delta G
Thermodynamically favorable (spontaneous)
127
- Delta H
Exothermic, more energy released by bonds forming than absorbed by bonds breaking
128
+ Delta H
Endothermic, more energy absorbed by bonds breaking than released by bonds forming
129
+ Delta S
Increase in entropy, more disorder on right side than left side
130
- Delta S
decrease in entropy, more disorder on left side than right side
131
Large eq. constant K
Forward reaction favored, greater rt. side than left side concentration/pressures, - delta G
132
Small eq. constant K
backward reaction favored, greater left side than right side concentration/pressure, + delta G
133
Acids with a large Ka
Stronger (more ionizing, more hydrogens free to roam)
134
Bases with small Kb
Weaker (less ionizing, more hydroxides "stuck" to cation)
135
Coefficients ARE exponents for..
Equilibrium expression
136
Coefficients MAY be exponents for..
Rate law
137
Boyle's law
Pressure and volume of gases are inversely related at constant temperature.
138
Pb (2+) + Ni → Ni (2+) + Pb.....which is cathode?
Pb(2+)/Pb
139
How do you solve a calorimetry problem?
Q (lost)= Q (gained)
140
Which is anode, which is cathode?
More positive (as on reduction potential table) is the anode
141
What is the combined gas law?
(P1V1/)/T1=(P2V2)/T2
142
What is half life constant?
1st order reactions!!
143
What graph represents a 1st order reaction?
ln[A] versus time is linear
144
What is the titration equation?
MaVana=MbVbnb
145
What is electrical force?
Force= (Kq1q2)/r^2
146
What does Kp=Kc?
Kp=Kc(RT)^Δn (of gas...right compared to left)
147
What is entropy?
amount of disorder in a system (lower number means less disorder)
148
When is ΔG negative (thermodynamically favorable)?
ALWAYS when +ΔS and -ΔH
149
How is absorbance related to % transmittance?
A=-log(%T/100)
150
When does K=Q?
system is at equilibrium and reaction does not shift to left or right
151
What happens to bonds in an exothermic reaction?
They are formed
152
What happens to bonds in an endothermic reaction?
They are broken.
153
What is vapor pressure?
the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system.
154
When does pH=pKa?
half equivalence point
155
When can dispersion forces in one substance be greater than hydrogen bond forces in another substance?
if there is a temporary dipole moment
156
electronegativity
how much the nucleus pulls on the shared electrons
157
critical point
When a substance has reached an irreversible state of matter
158
larger k favors the...
right side stuff, or products
159
What graph represents a zero order reaction?
[A] vs. time if it is linear
160
What graph represents a second order reaction?
1/[A] vs. time if it is linear
161
buffer
weak acid with its conjugate base or weak base with its conjugate acid
162
Absorbance
A=(absorbativity)(path length in m)(concentration in M)
163
vapor pressure
keeps a substance from becoming a gas, increases with pressure
164
Hydrogen bonds
Oxygen, Nitrogen, Fluorine with
| Hydrogen
165
Strong IMF
means a higher boiling point, harder to change phases, greater the difference in electronegativity means the stronger the attraction.
166
sublimation
change directly from solid to gas at low pressure
167
temperature
the average kinetic energy, the speed of particles
168
One of the few substances that expands in solid form
water
169
changes directly from gas to solid
deposition
170
weak acids
do not dissociate completely, does not release all its hydrogens, higher pKa, does not fully "break away"
171
To change a substance from solid to liquid or liquid to gas...
you'd need an increase in temperature or a decrease in pressure.
172
factors that affect rate
reaction type, temperature, pressure, surface area, & catalysts
173
Titration equation with acid/base
(#H+) m1v1=m2v2(#OH-)
174
REDOX
reduction: gains electrons
175
Atomic Radius & Ionization Energy & Electronegativity Trends
Atomic Radius: Increase↓, Decrease→ Ionization Energy: Decrease↓, Increase→
Electronegativity: same as Ionization Energy
176
Brønsted-Lowery Conjugate Acid/Base Pairs
Conjugate base = acid - one H⁺
177
Slowest step in multi-step reaction
slow rate step = rate determining
178
Beer's Law
A= - log%T A=Absorbance
| T=Transmittance in DECIMAL
179
Kw
Kw=1.0x10⁻¹⁴
180
What is the numerator and denominator in the K eq?
(right side stuff) raised to coefficients/left side stuff raised to coefficients
181
Effective charge on an electron
Number of protons in nucleus-number of electrons in lower energy levels.
182
What are the strong acids?
HCl, HBr, HI, HNO3, and first hydrogen ion on H2SO4
183
Covalent Network Solids
Diamond (Carbon), Graphite (Carbon), Sand (SiO₂)
