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nordsb [41]
3 years ago
10

Consider the perchlorateanion.

Chemistry
1 answer:
Agata [3.3K]3 years ago
6 0

Answer:

(a) Chlorine atom

(b) 0

(c) 109.5°

(d) about the same

Explanation:

Perchlorate is a negatively charged molecule that is composed of one carbon atom and four oxygen atoms. In this molecule, the <em>central chlorine atom</em> that is present in +7 oxidation state, is covalently bonded to four oxygen atoms.

Thus the number of <u>bond pairs is 4</u> and the number of <u>lone pairs on the central chlorine atom is 0</u>.

So according to the VSEPR theory, perchlorate ion has a <em>tetrahedral geometry</em>. Therefore, the<em> </em><u>ideal bond angle for the perchlorate ion is 109.5°</u>.

<u>The actual bond angle of perchlorate is about the same as ideal bond angle.</u> This is because the perchlorate is <em>resonance stabilized</em> and thus all the chlorine-oxygen bonds are equivalent.

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Answer:

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