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Periodic Properties
electron configurations properties
hydrogen atom 1 electron
to remove e- nf = ∞
E = x 6.022 x 1023 atomsatom mol
= 1311 kJmol
Z = 1
from ground state ni = 1
2.178 x 10-18 J
E =1
nf2
-1
ni2
- RH Z2
nuclear charge
1s1
Ionization Energy, I
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He+ Z = +2
E =1
nf2
-1
ni2
- RH Z2 = 5250 kJ/mol
1s1 E = 5250 kJ/mol
systems with more than 1 electron
studied experimentally ionization reactions
higher nuclear charge lowers orbital energy
-
+
-
2+
stabilizes system
H 1s1 Z = +1 E = 1311 kJ/mol
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1. Effect of 2 electrons in same orbital
He 1s2
Z = +2
E = 2372 kJ/mol
same nuclear charge
-
2+
-
2+ -
orbital energy higher
e- e- repulsion
less stable
easier to remove e-
He+ 1s1 E = 5250 kJ/mol
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2. Effect of electrons in different orbital
Li
Li2+
1s2
2s1
Z = +3
E = 2954 kJ/mol
E = 520 kJ/mol
same nuclear charge
3+3+
ground state 2s1
excited state
1s 1s
2s 2s
-
-
-
-
inner electrons shielding chargeZeff < Z
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3. Effect of orbital shape
Li
Li
1s2
1s2
Z = +3
E = 341 kJ/mol
E = 520 kJ/mol
same nuclear charge
ground state 2s1
excited state 2p1
3+
1s
2s
3+
1s
2p
-
-
--
-
-
s orbitals penetrating lower energy
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determine orbital energiesElectrostatic interactions
1. Greater nuclear charge (Z) lowers energy
2. Electron-electron repulsion raise energy
electrons more difficult to remove
electrons easier to removeelectrons shield Z
inner electrons shield better
3. Orbitals with more penetration lower energy
electrons more difficult to remove
s < p < d < f
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Ionization Energy
energy required to remove an e- from gas phase atoms
X+ (g) X2+(g) + e-
first ionization energy I1X (g) X+(g) + e-
second ionization energy I2
lowest I1 Csn = 6
highest I1 Hen = 1
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I1 decrease Zeff decreases more shielding e-
I1 increase Z increases shielding stays same
core e-
adding valence e-
core e- unchanged
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5+
1s
2s
2p
10+
-
1s
2s
2p
-
-
-
-
-
-
-
-
-
B Ne
-
-
-
-
-
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4+
1s
2s
Be B
5+
1s
2s
2p
-
-
N O
-
-
-
-
-
-
-
e- e- repulsion
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Second Ionization Energy I2
Na
I1 I2 I3 I4 I5 I6 I7
Mg
AlSi
P
S
Cl
Ar
495
735
580
780
1060
1005
1255
1527
4560
1445
1815
1575
1890
2260
2295
2665
7730
11,600
16,100
21,200
27,000very difficult to removecore electrons
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Atomic Radius
metallic radius Al 143 pm
covalent radiusCl 100 pm
C-Cl 177 pm
Cl 100 pm
C 77 pm
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Atomic Radiusincrease in size n dominates
decrease in size
Zeff dominates
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Ionic sizes
e-
+ -
isoelectronic series
46 e-
+49 +50 +51 ions get smaller
same # electrons