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Chemical Bonding And Molecular Structure

Question
CBSEENCH11005780
Wired Faculty App

Why the bond orders of He2+ and H2– are identical?

Solution

Molecular ion                    Molecular orbital configuration
space He subscript 2 superscript plus                                       open parentheses straight sigma subscript 1 straight s end subscript close parentheses squared space left parenthesis straight sigma subscript 1 straight s end subscript right parenthesis to the power of 1
He subscript 2 superscript minus                                         left parenthesis straight sigma subscript 1 straight s end subscript right parenthesis squared space left parenthesis straight sigma subscript 1 straight s end subscript right parenthesis to the power of 1
Since both He2+ and H2– have equal number of bonding (Nb) and antibonding (Na) electrons because of identical molecular orbital configuration, their bond order is given by   equals 1 half open square brackets straight N subscript straight b space minus space straight N subscript straight a close square brackets equals space 1 half open square brackets 2 minus 1 close square brackets equals space 1 half space are space identical.

Some More Questions From Chemical Bonding and Molecular Structure Chapter

What are valence electrons?

Why do atoms combine?

Can ionic bond be formed between similar atoms?

Why two helium atoms do not combine to form He2?

What are 'Lewis structures'?

Name the conditions for the formation of an ionic bond between two atoms.

What is crystal lattice?

What is electrovalency?

What bond is present in MgCl2 molecules?

Write Lewis dot symbols for atoms of the elements Mg, Na, B, O, N, Br.

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