Geology Reference
In-Depth Information
Therefore
6.4
(a) Rewrite Moseley's Law in the linear form:
aa a
⋅
=
×
K
HCO
+
−
H CO
2
3
3
−
506
.
−
6 4
.
=
10
×
10
1
2
(
)
=−
1
2
1
2
kZ k
σ
i..
ymxc
1
/λ
−
11 46
.
=
10
=+
10
5.
Therefore pH = 5.73
This is the pH value for pre-industrial rainwater.
The values for 1960 and 2012 are 5.71 and 5.66, a
pH change of - 0.05.
a
H CO
=
=
−
/
( )
and plot against
Z.
Points fall on a straight line if the equation
holds.
1
2
For each point calculate 1
+
−
3
=
(
)
−
(
1
2
)
1
2
1561 1830
47 39
/. /.
k
2
=
gradient
−
1
2
=
0 00297
.
pm
Chapter 5
1
2
(
)
1
2
/k /λ
For yttrium (Y), for example, σ= −
σ= −
Z
11
0 1098
0 00296
.
5.1
2p, 3 s, 4f, 5d
5.2
39
.
6
C
1s
2
2s
2
2p
2
.
(b) Read off graph at
Z
= 43:
= 2 022
11
Na
1s
2
2s
2
2p
6
3s
1
or [Ne]3 s
1
13
Al
[Ne]3s
2
3p
1
17
Cl
[Ne]3s
2
3p
5
1
2
(
)
−
1
2
(
)
=
−
.
Therefore
λ
= 67.6 pm = 0.676 × 10
−10
m
1
/
λ
0 1216
pm
18
Ar
[Ne]3s
2
3p
6
= [Ar]
26
Fe
[Ar]4s
2
3d
6
E v c
q
==
λ
4 135 10 2 997 10
0 676 10
/
(
)
(
)
.
×
−
15
.
×
8
−
1
eV sms
m
Chapter 6
=
−
10
.
×
=
183
30
eV
=
18 33
.
keV
6.1
The Pauli principle dictates that each orbital can
hold no more than two electrons:
Chapter 7
Z
Name
Configuration
Block
Group
Valency
Core
Valence
3
Li
1 s
2
2 s
1
s
I
1
7.1
Ionic radii in Box 7.2 lead to following radius
ratios:
Si
+
: 0.26. Al
3+
: 0.36 (tet)/0.46 (oct). Ti
4+
: 0.52. Fe
3+
:
0.55. Fe
2+
: 0.65. Mg
2+
: 0.61. Ca
2+
: 0.91. Na
+
: 0.94
(8-fold). K
+
: 1.20.
Co-ordination numbers: 4: Si
4+
, A1
3+
. 6: A1
3+
, Ti
4+
,
Fe
3+
, Mg
2+
. 8: Ca
2+
, Na
+
. 12: K
+
.
7.2
In the higher oxidation state (Fe
3+
, Eu
3+
), the ion
has fewer valence electrons and there is less mutual
repulsion between them, so ions are smaller than
2+ ions. Ionic potentials: Fe
2+
: 23. Fe
3+
: 41. Eu
2+
: 16.
Eu
3+
: 28. The 3+ ion has a higher polarizing power
than the 2+ ion, and therefore forms a more cova-
lent bond.
7.3
He-He: van der Waals interaction; very weak, so
He is a monatomic gas at room temperature.
Ho-Ho: electronegativity of Ho is between 1.1
and 1.3, therefore metallic bond. Crystalline metal
at room temperature.
Ge-Ge: metallic/covalent bond. Electronegativity
similar to Si in Figure 7.8b. Semiconductor at room
temperature.
5
B
1 s
2
2s
2
2p
1
p
III
3
8
O
1 s
2
2s
2
2p
4
p
VI
−2
9
F
1 s
2
2s
2
2p
5
p
VII
−1
14
Si
1s
2
2s
2
2p
6
3s
2
3p
2
P
IV
4
6.2
Ti [Ar] 4s
2
3d
2
: block d
Ni [Ar] 4s
2
3d
8
: block d
As [Ar] 4s
2
3d
10
4p
3
: block p
U [Rn] 7s
2
6d
1
5f
3
: block f
6.3
Na valency = 1. Oxygen = −2, therefore there are
2 atoms of sodium per atom of oxygen:
Na
2
O
x =
2
y =
1
Similarly
SiO
2
x =
1
y =
2
x =
1
y =
4
MgCl
2
x =
1
y =
2
Valency of scandium is 3, valency of oxygen = −2.
Each Sc combines with 3/2 atoms of oxygen, or 2
Sc atoms combine with 3 oxygen atoms:
SiF
4
Sc
2
O
3
x =
2
y =
3
Similarly
P
2
O
5
x =
2
y =
5
BN
x =
1
y =
1
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