Yesterday in class, we talked about Zeop (Z*) increasing in the following systems: = 738 KJ/mol = 1450 KJ/mol Today, we will see if this is true by using a set of rules called Slater's Rules. Mg (g) ------> Mg (8) + Mg(8) -------> Mg² 2+ (8) + e e- IE IE Slater's rules to calculate a shielding constant (S): ZEF= = Z - S 1. Write out the electronic configurations of the element or ion in the following order and groupings: (1s) (2s, 2p) (3s, 3p) (3d) (48,4p) (4d) (4f) (5s,5p) 2. All of the electrons in the (ns, np) group shield the valence e to an extent of 0.35 each.*** The ns, np group is the same group as the valence e. 3. All e's in the n-1 level shield to an extent of 0.85. 4. All e's in the n-2 level, or lower, shield completely (i.e. 1.00 each).
Yesterday in class, we talked about Zeop (Z*) increasing in the following systems: = 738 KJ/mol = 1450 KJ/mol Today, we will see if this is true by using a set of rules called Slater's Rules. Mg (g) ------> Mg (8) + Mg(8) -------> Mg² 2+ (8) + e e- IE IE Slater's rules to calculate a shielding constant (S): ZEF= = Z - S 1. Write out the electronic configurations of the element or ion in the following order and groupings: (1s) (2s, 2p) (3s, 3p) (3d) (48,4p) (4d) (4f) (5s,5p) 2. All of the electrons in the (ns, np) group shield the valence e to an extent of 0.35 each.*** The ns, np group is the same group as the valence e. 3. All e's in the n-1 level shield to an extent of 0.85. 4. All e's in the n-2 level, or lower, shield completely (i.e. 1.00 each).
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter18: The Nucleus: A Chemist's View
Section: Chapter Questions
Problem 78CWP
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Transcribed Image Text:Chem 1 Workshop
Effective Nuclear Charges
following systems:
Yesterday in class, we talked about Zep (Z*) increasing in the
Mg (g) ------> Mg* (g) + e-
+
Mg (g). -------> Mg
--> Mg ²+ (8)
= 738 KJ/mol
IE
IE = 1450 KJ/mol
Today, we will see if this is true by using a set of rules
called Slater's Rules.
Slater's rules to calculate a shielding constant (S):
Zere = Z - S
EFF
1. Write out the electronic configurations of the element or
ion in the following order and groupings:
(18) (2s, 2p) (3s, 3p) (3d) (48,4p) (4d) (4f) (5s,5p)
Ex. Nitrogen
2. All of the electrons in the (ns, np) group shield the
valence e to an extent of 0.35 each. ***
The ns,np group is the same group as the valence e.
3. All e's in the n-1 level shield to an extent of 0.85.
4. All e's in the n-2 level, or lower, shield completely
(i.e. 1.00 each).
ne
Grouping
ZEFF
ZEFP
Ex. Zinc. 30
Zn
2
7 N
(15)² (25, 2p)
S = (2x 0.85)
Z
e
2
15 ² 25² ap3
4
Dr. Ogar
Z-S
(.
+
7-3.10
3
3.90
(4 x 0.35 ) = 3.10
(15) ² (25, 2p) (35, zp) (3 d) ⁰ (4S, 4p)
= 2*
=Z-25.65 =
40-25.65 = 4.35
(1 x 0.35) + (18 x 0.85) + (10 × 1.00 ) = 25.65
ZEFP
**except is where 0.30 works better
22
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Transcribed Image Text:Additional
questions page 22
1. Does Zeff explain why the I.E.
for Mst is greater than
Mg? Explain
2. Does 2 eff explain the trend in
atomic sizes as you go
to C? Explain.
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