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Question 4

a)

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Rank the following atoms in order of effective nuclear charge, from lowest to highest: Na, Cl, Si, Al, S. Do not use Slater's rules to solve.

b)

Rank the following pairs of elements in terms of their electron affinities compared against each other.

Note that larger (more positive) electron affinities refer to more exothermic electron affinities, as defined in the Tro textbook.

All pairs must be correctly ranked for full credit.

S vs. Al

K vs. Na

P vs. S

O vs. F

Answer 1

Solution:

A) Na, Cl, Si, Al,S

The effective nuclear charge without slater rule only depends upon the number of protons in the nucleus. High atomic number element shows maximum nuclear charge.

Hence, order will be: Cl > S > Al > Si > Na

B) The electron affinity of an element is defined as the enery required to add electron to a gaseous element.

In a periodic table, when we move from left to right in periods, the electron affinity increases, while in a group it decreases with radius.

The electron affinity for the given pairs of elements are:

1) S vs Al

S > Al

2) K vs Na

Na > K

3) P vs S

S > P

4) O Vs F

F > O