Some REVIEW SLIDES
(these are not comprehensive)
–Nota&on for atoms: A X
Z
•X = element symbol •A = atomic mass number = # of protons + # of neutrons •Z = atomic number = # of protons = # of electrons in a neutral atom Know which experiments were used to determine the nature of the atom Mass Spectra
Relative Intensity
0.6
0.5
0.4
0.3
0.2
0.1
0.0
69
70
71
72
73
Mass Number
74
75
Know the difference between amu of an isotope and the
average atomic mass of an element
Be able to calculate average atomic masses of element from
the percent abundance of the isotopes, and vice versa
Be able to name Simple Compounds Be familiar with the following calculations:
Empirical and molecular formulae from mass % or mole % of
elements in a compound.
Stoichiometric Calculations: Amounts of Reactants and
Products.
Acid-base titrations
Calculations involving a limiting reagent
• chemical reactions:
– most common reactions may be classified into
3 classes:
• ..
• ..
• ..
precipita(on reac(ons acid-­‐base reac(ons Know Solubility rules Perform Stoichiometric Calcula&ons oxida(on-­‐reduc(on reac(ons Calculate Oxida&on Numbers; Balance Redox Reac&ons using the half-­‐reac&on method in acidic and alkaline media • Ideal gas:
– Know the difference between :
• Boyle’s law:
• Charle’s law:
• Avogadro’s law:
k
V=
P
V = bT
PV = nRT
V = an
R = 0.08206 L atm/(K mol) Be able to interchange units, know the meaning of, and be
able to use partial pressures, mole fractions, and the density
of gases. Know STP.
Kine&c Molecular Theory of Gases: KEavg
L
⎛ 1
⎞
= N A ⎜ mu 2 ⎟
⎝ 2
⎠
PV 2
= KEavg = RT
n
3
• can use the ra&o of any of the following to compare with urms
3RT
=
M
Be careful with units (M
is kg/mol!);
R is 8.314 J/K.mol
–
–
–
–
–
M12 M 21
molecular speeds rates of effusion effusion &mes distance traveled by molecules amount of gas effused Real Gases •Know how to use the van der Waals equa(on, and why: 2
⎡
⎛ n ⎞ ⎤
⎢ Pobs + a ⎜ ⎟ ⎥ ( V − nb ) = nRT
⎝ V ⎠ ⎥⎦
⎢⎣
corrected pressure
corrected VOLUME
Energy, Enthalpy, and Thermochemistry ΔE = heat + work ΔH = ΔE + Δ(PV) Understand the concepts of
heat flow and work. Get your
signs right! Think from the
system’s perspective.
|w| = |PΔV| = |nRΔT| w = -­‐P ΔV Thermodynamics of ideal gases (know and be
able to use in calculations):
• molar heat capacity = Cv = (3/2)R
• Cp = = Cv + R = (5/2)R
– for a monoatomic gas at constant volume
Cv > 3/2R and Cp > (5/2)R for polyatomic gases
• heating a gas: energy and enthalpy
ΔE = nCvΔT
ΔH = nCpΔT
You need to know how to
calculate ΔH ΔE, q, and w
for given situations.
ΔE = qv
ΔH = qp
• Calorimetry (use in calculations):
– the science of measuring heat
specific heat capacity =
molar heat capacity =
J
g oC
or
J
g
o
K
J
J
or
mol o C
mol K
• constant-pressure ΔE =qp + w = ΔH + w
Heat Evolved by reaction = heat absorbed by solution
=Specific heat capacity x mass of solution x increase in temperature
• constant-volume ΔE = qV
Energy released by reaction
= heat capacity of calorimeter x increase in temperature
Indirect determina&ons of ΔH: a)Hess’s Law (remember H is a state func&on: path independent) b) Standard enthalpies of forma&on ΔHoreaction = ∑ ΔHof (prod.) − ∑ ΔHof (react.)
Atomic theory.
λν = c hc
Ephoton = hν =
λ
h
m=
λv
2
⎛
⎞
Z
−18
⎜
E = −2.178x10 J⎜ 2 ⎟⎟
⎝ n ⎠
2
2
⎛
⎞
Z
Z
−18
ΔE = −2.178 x 10 J⎜⎜ 2 − 2 ⎟⎟
⎝ n final n initial ⎠
ĤΨ = EΨ
Radial probability (4πρ2R2)
ΔxΔp ≥ h/4π
07_104
Distance from nucleus (r)
(a)
(b)
Nodes
07_105
07_106B
Node
1s
2s
(a)
z
3s
z
z
y
y
y
1s
2s
(b)
3s
x
x
x
2px
2py
2pz
(b)
07_109
07_108B
z
z
y
y
x
x
x
dyz
z
z
x
y
fz3 - 3 zr 2
x
y
z
z
y
fx 3 - 3 xr 2
z
fy 3 - 3 yr 2
5
z
z
y
x
x
dx2 - y2
x
5
5
dxy
y
(b)
z
z
y
dxz
z
x
x
x
x
dz2
y
y
fxyz
y
fy(x2 - z2)
y
fx(z2 - y2)
fz(x2 - y2)
15
ℓ= 0
→ s
1
→ p
–ℓ = integer (0, 1, 2, 3…n-1)
2
→ d
mℓ
3
→ f
4
→ g
= 2ℓ+1
n ℓ
1 0
2 0
1
3 0
1
2
4 0
1
2
3
designation mℓ
1s
2s
2p
3s
3p
3d
4s
4p
4d
4f
# of orbitals
0
0
-1,0,1
0
-1,0,1
-2,-1,0,1,2
0
-1,0,1
-2,-1,0,1,2
-3,-2,-1,0,1,2,3
1
1
3
1
3
5
1
3
5
7
07_118
1s
2s
2p
3s
3p
3d
4s
4p
4d
4f
5s
5p
5d
5f
6s
6p
6d
7s
7p
1s 2s 2p 3s 3p 4s 3d 4p 5s # e’s
2
4
10
12
18
20
30
36
38
Period number, highest occupied electron level
Representative
07_116
Elements
1A Group
ns1
numbers
d - Transition Elements
Noble
gases
8A
ns2np6
1
1
H
1s1
2
Li
2s1
3
11
12
Na
3s1
Mg
3s2
2
3A
4A
5A
6A
7A
2
1
2
2
2
3
2
4
ns np ns np ns np ns np ns2np5
2A
ns2
3
19
4
Be
2s2
20
21
22
23
24
25
26
27
39
40
41
42
43
44
45
5
37
38
Rb
5s1
Sr
5s2
6
55
56
57
72
Cs
6s1
Ba
6s2
La*
6s25d1
Hf
4f146s25d2
89
104
87
88
Fr
7s1
Ra
7s2
5
6
7
8
9
10
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
3s23p1 3s23p2 3s23p3 3s23p4 3s23p5 3s23p6
K
4s1
Ca
4s2
He
1s2
B
C
N
O
F
Ne
2
1
2
2
2
3
2
4
2
5
2s 2p 2s 2p 2s 2p 2s 2p 2s 2p 2s22p6
4
7
Representative Elements
28
29
30
31
32
33
34
35
36
46
47
48
49
50
51
52
53
54
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
4s23d1 4s23d2 4s23d3 4s13d5 4s23d5 4s23d6 4s23d7 4s23d8 4s13d10 4s23d10 4s24p1 4s24p2 4s24p3 4s24p4 4s24p5 4s24p6
Y
Zr
Nb
Mo
Tc
Ru
Rh
2
1
2
2
1
4
1
5
1
6
1
7
5s 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s14d8
73
74
75
76
77
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
25p1 5s25p2 5s25p3 5s25p4 5s25p5 5s25p6
10
1
10
2
10
5s
4d
5s 4d 5s 4d
78
79
80
81
82
83
84
85
86
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
6s25d3 6s25d4 6s25d5 6s25d6 6s25d7 6s15d9 6s15d10 6s25d10 6s26p1 6s26p2 6s26p3 6s26p4 6s26p5 6s26p6
105
106
107
108
Ac** Unq Unp Unh Uns Uno
7s26d1 7s26d2 7s26d3 7s26d4 7s26d5
109
110
Une Uun
7s26d7
111
Uuu
f - Transition Elements
58
Lanthanides*
Actinides**
Ce
59
Pr
60
Nd
61
Pm
62
Sm
63
Eu
64
Gd
65
Tb
66
Dy
67
Ho
68
Er
69
Tm
70
Yb
71
Lu
6s24f15d1 6s24f35d0 6s24f45d0 6s24f55d0 6s24f55d0 6s24f75d0 6s24f75d1 6s24f95d0 6s24f105d0 6s24f115d0 6s24f125d0 6s24f135d0 6s24f145d0 6s24f145d1
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
7s2f06d2
Fig. 12.29
7s25f26d1 7s25f36d1 7s25f46d1 7s25f66d0 7s25f76d0 7s25f76d1 7s25f96d0 7s25f106d0 7s25f116d0 7s25f126d0 7s25f136d0 7s25f146d0 7s25f146d1
07_127
Atomic radius increases
1A
2A
Atomic radius decreases
3A
4A
5A
6A
7A
8A
H
He
37
31
Li
Be
152
112
B
C
N
O
F
Ne
85
77
75
73
72
71
Al
Si
P
S
Cl
Ar
Mg
Na
186
160
143
118
110
103
100
98
K
Ca
Ga
Ge
As
Se
Br
Kr
227
197
135
122
120
119
114
112
Rb
Sr
In
Sn
Sb
Te
I
Xe
248
215
167
140
140
142
133
131
Cs
Ba
Tl
Pb
Bi
Po
At
Rn
265
222
170
146
150
168
140
140
• Ionization energy:
– increases increases from left to right in a period and from
bottom to top in a group:
• Electron affinity:
–increases increases from left to right in a period and from
bottom to top in a group
• Atomic radius:
– increases increases from right to left in a period and from
top to bottom in a group
Good Luck !