Question

State whether each of these statements is true or false. (a) a carbon–carbon triple bond is shorter than a carbon–carbon single bond. (b) there are exactly six bonding electrons in the o2 molecule. (c) the c—o bond in carbon monoxide is longer than the c—o bond in carbon dioxide. (d) the o—o bond in ozone is shorter than the o—o bond in o2. (e) the more electronegative the atom, the more bonds it makes to other atoms.

Answer 1

Answer:

(a) a carbon–carbon triple bond is shorter than a carbon–carbon single bond.

The given statement is true.This because bond order in of (C-C) bond in triple bond is 3 whereas the bond order of (C-C) bond in single bond is 1. Higher the bond order shorter will be the bond length.

(b) There are exactly six bonding electrons in the oxygen molecule.

The given statement is false. This is because bond order present in oxygen molecule is 2 which means there are 4 bonding electrons in the oxygen molecule.

(c) the (C-O) bond in carbon monoxide is longer than the (C-O) bond in carbon dioxide.

The given statement is false.This because bond order in of (C-O) bond in CO is 3 whereas in $CO_2$ the bond order of (C-O) bond is 2. Higher the bond order shorter will be the bond length.

(d) The (O-O) bond in ozone is shorter than the (O-O) bond in oxygen.

The given statement is false. This is because bond order in of (O-O) bond in ozone molecule is 1.5 whereas in $O_2$ the bond order of (O-O) bond is 2. Higher the bond order shorter will be the bond length.

(e) The more electro-negative the atom, the more bonds it makes to other atoms.

The given statement is false. This is because atom with more electro-negative character. Since, they are highly electron rich atoms so they will tend to form less number of bonds with other atom.