1. Describe the relationship between: a. the radius of a cation and that of the

Question

1. Describe the relationship between:

a. the radius of a cation and that of the atom from which it is formed.

b. the radius of an anion and that of the atom from which it is formed

2.

Examination of the first few successive ionization energies for a given element

usually reveals a large jump between two ionization energies. For example, the

successive ionization energies of magnesium show a large jump between IE 2 and IE 3.

The successive ionization energies of aluminum show a large jump between IE 3 and IE

Explain why these jumps occur and how you might predict the jumps

Explanation / Answer

1.
a. The radius of cation is smaller than its parent atom.Because by the loss of elecron there may be decrease of no of shells or increases effective nuclear charge
Na+< Na

b. The radius of anion is larger than its parent atom.Because by accepting elecron there may be increase of no of electrons in a particular shells. net effective nuclear charge decreases.
Cl->Cl

2. Mg = 12 = 1s2 2s2 2p6 3s2
Removal of 2e- from 3s orbitals requires less ammount of energy.But removal of 3rd electron from 2p orbital requires larger amount of energy because it is completely filled orbital.

Al = 13 = 1s2 2s2 2p6 3s2 3p1
Removal of 1e- require less ammount of energy than 3rd electron. Because 3s orbital is completely filled.

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