For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) C-C(B) C?C (A, B)(C) C?O(D) C-O (C, D)bondlengthtitle. gifThe length of a covalent bond depends upon the size of the atoms and the bond order. For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) P-Cl(B) Si-Cl (A, B)(C) P-I(D) H-I (C, D)bondlengthtitle. gifThe length of a covalent bond depends upon the size of the atoms and the bond order. For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) Cl-I(B) I-I (A, B)(C) P-Br(D) P-Cl (C, D)

See explanation

Explanation:

In the section A,B

C triple bond O has a higher bond energy. A triple bond is shorter and more difficult to break hence they have a higher bond energy.

For the same reason in the C,D section; C triple bond N has a higher bond energy.

In the next section, the higher the bond order the shorter the bond. Hence C triple bond C is the shortest in the A,B section while C triple bond O is the shortest in the C,D section. Both have a bond order of 3.

In the A,B section; I is larger than Br hence H-Br has the shortest bond length.

In the C,D section; Br is larger than Cl hence P-Cl has the shortest bond length.

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