AP Chemistry Course and Exam Description
Appendix B: AP Chemistry
Equations and Constants
Throughout the test the following symbols have the definitions specified unless otherwise noted.
L,mL
liter(s), milliliter(s)
gram(s)
nanometer( s)
atmosphere(s)
g
nm
atm
mmHg
J, kJ
v
mo!
millimeters of mercury
joule(s), kilojoule(s)
volt(s)
mole(s)
ATOMIC STRUCTURE
E =energy
v = frequency
/l = wavelength
E= hv
c = llv
Planck's constant, h = 6.6l6 x 10-34 J s
Speed of light, c = 2.998 x 108 m s- 1
Avogadro's number= 6.022 x 1023 mo!- 1
Electron charge, e = -1.602 x 10- 19 coulomb
EQUILIBRIUM
[Cf[Dld
Kc = - ·- - b , where a A+ b B p c C + d D
·
[Ar[B]
Kc
KP
Ka
Kb
Kw
K = (Pcf (Po)d
(PA)a(Ps)b
P
Ka=
[H+][A-]
[HA]
K _ [OW][HB+]
b -
Kw
Equilibrium Constants
(molar concentrations)
(gas pressures)
(weak acid)
(weak base)
(water)
[B]
= [W][OW] = 1.0 x 10- 14 at 25°C
= K0 x Kb
pH = - log [W], pOH = - log [OW]
14 = pH+pOH
_
[A-1
pH - pKa +log [HA]
pKa =-logKa, pKb = -logKb
KINETICS
ln[AJi- ln[A] 0 =-kt
- 1- - -1- =kt
[A], [A] 0
t
k = rate constant
t =time
t Vi = half-life
0.693
Vi= - k -
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© 2013 1bc College Board.
AppendixB
GASES, LIQUIDS, AND SOLUTIONS
PV
= nRT
moles A
PA= Ptotal x XA, whereXA = tota1 mo1es
m
n= M
K = °C +273
D= !!!:.
v
KE per molecule=
tmv
P
V
T
n
m
=pressure
=volume
= temperature
= number of moles
=mass
M = molar mass
D =density
KE = kinetic energy
v =velocity
A = absorbance
a= molarabsorptivity
b = path length
c = concentration
2
Molarity, M = moles of solute per liter of solution
A= abc
Gas constant, R = 8.314 J mo1- 1 K- 1
= 0.08206 L atm mo1- 1 K- 1
= 62.36 L torr mor 1 K- 1
1 atm = 760 mm Hg
= 760 torr
STP = 0.00°C and 1.000 atm
THERMOCHEMISTRY/ ELECTROCHEMISTRY
q = mct!..T
!1.S0 = L, S0 products - I, S 0 reactants
m
0
=
1m; products -'i,mJ reactants
!1.G 0 = L, t!..GJ products - '£ t!..GJ reactants
!1.G 0 =
m
0
-
q =heat
m =mass
T !1.S0
= -RTlnK
= -nFE 0
I= g_
t
c = specific heat capacity
T = temperature
S0 = standard entropy
H 0 = standard enthalpy
G 0 = standard free energy
n = number of moles
E 0 = standard reduction potential
I =current (amperes)
q =charge (coulombs)
t =time (seconds)
Faraday's constant, F = 96,485 coulombs per mole
of electrons
1volt =
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© 2013 'lbc College Board.
1 joule
!coulomb
I
>
'ti
[ ~Q~Qr:.~~:ii~Ii~~Q~!_i_QQ_~. ~ml
He
!,008
4.0(}
4
Li
~·-·re
12
Na
Mg
I
22.99
24.30
I
19
20
21
22
23
24
25
26
27
28
29
30
K
Ca
Sc
Ti
v
Cr
Mn
Fe
Co
Ni
Cu
Zn
44.96 I 47.90 I 50.94 I 52.00 I 54.94
85.47
87.62
88.9i
55
56
57
72
Cs
Ba
*La
Hf
37
39
Y
I 40 l
Zr
>-3
"'
92.91
95.94
(98) I IOU
73
74
75
Ta
w
Re
Ru
! 76
I Os
46
Rh
Pd
102.91 : !06.42
77
78
Ir
Pt
i
i
Pl
n o<1Jr+.
ii" 0
0
5&
*Lanthanide Series
1: .
Ce
I
59
I Pr
60
Nd
140.l 2 I 140.9 l 144.24
0
::J
rt
<1J
~
m
7
8
9
10
B
c
N
0
F
Ne
J
90
t Actinide Series
i Th
!
91
92
Pa
U
232.04 23L04 238.03
61
!
Pm
jsm
63
(J4.5)
! J50.4
!51.97
Np
Ga! Ge
49
50
Ag
In
Sn
l 07.8'7 I 1
114.82 [ 1HL71
81
Au
33
I
As
I Se
34
35.45 I 39.95
35
Br
72.59 I 74.92 ! 78.96 I 79.90
69.72
47
I 79
3C.97 ! 32.06
I s2
Tl I Pb
I 51
Sb
I 52
I Te
121.75 127.60
83
84
Bi
Po
204.38 I 2!>7 .2 I 208.98
I 53
I 94
i
Pu
{237) ! (244)
I 64
Eu 1Gd
95
I 157.25
!I
96
Am I Cm
(243)
I (247>
65
66
Tb
Dy
Bk
1 (247)
68
69
Ho
Er
Tm
!64.93 '167.26 163.93
15&.93
97
67
98
99
Cf
Es
(251)
12s2)
1100
Fm
I (257)
101
I
36
Kr
83.80
54
I
Xe
126.91
BL29
ss
86
At
Rn
r21m I (222)
111
62
93
3l
! 28.09
I 32
63.55
196.97
~ilil: I 106 I 1~
"
~
Tc
45
132.91 i l37.33 I 138.91 1178.49 1ll\0.95 I !83.85 I 186.21
;l Q:
~
Mo
I
272
<1J
0""
44
Rg
N
"
Nb
58.69
55.85 I 58.93
I 42 I 43
rt
p-'
::::
""
41
0
rt
©
38
6
26. 98
I
Rb Sr
39.IO ! 40.08
5
::~-%!t1:
, 6.94
9
"'
2
H
3
2:
[
PERIODIC TABLE OF THE ELEIVIENTS
l
~
C'l
I 10
1 Yb
I173.1)4
I 102
Md
INo
(258)
(259)
11
Lu
174.97
103
Lr
c2621
~
C'l
g
01
ID
~
!lo
l".I
~
Ill
8
tj
ID
"'
n
~g