Question

Write Lewis structures for the following molecules: (a) ICl, (b) PH3, (c) P4 (each P is bonded to three other P atoms), (d) H2S, (e) N2H4, (f ) HClO3, (g) COBr2 (C is bonded to O and Br atoms).

Answer 1

Lewis structures for (a) ICl: I-Cl, (b) PH3: P-H, (c) P4: P-P-P-P, (d) H2S: H-S, (e) N2H4: N-N-H-H, (f) HClO3: H-Cl-O, (g) COBr2: C=O and C-Br.

Step-by-step explanation:

(a) Lewis structure for ICl:

I: 7 valence electrons
Cl: 7 valence electrons

ICl is a polar molecule with a single bond. The Lewis structure would show I as the central atom bonded to Cl with a single bond. The I atom would have three lone pairs around it, and the Cl atom would have one lone pair.

(b) Lewis structure for PH3:

P: 5 valence electrons
H: 1 valence electron

The central P atom would be bonded to three H atoms and have one lone pair. Each H atom would have one lone pair around it.

(c) Lewis structure for P4:

P4 consists of four P atoms, each bonded to three other P atoms. The Lewis structure would show the P atoms forming a ring with single bonds between each of them.

(d) Lewis structure for H2S:

H: 1 valence electron
S: 6 valence electrons

The Lewis structure would show the H atoms bonded to the S atom with single bonds. The S atom would have two lone pairs around it, and each H atom would have one lone pair.

(e) Lewis structure for N2H4:

N: 5 valence electrons
H: 1 valence electron

The Lewis structure would show two N atoms connected by a single bond and each N atom bonded to two H atoms. Each N atom would have two lone pairs around it, and each H atom would have one lone pair.

(f) Lewis structure for HClO3:

H: 1 valence electron
Cl: 7 valence electrons
O: 6 valence electrons

The Lewis structure would show the Cl atom bonded to an O atom with a single bond and the O atom bonded to the H atom with a single bond. The Cl atom would have three lone pairs, and the O atom would have one lone pair.

(g) Lewis structure for COBr2:

C: 4 valence electrons
O: 6 valence electrons
Br: 7 valence electrons

The Lewis structure would show the C atom bonded to two O atoms and one Br atom, with double bonds between the C and O atoms and a single bond between the C and Br atoms. The C atom would have no lone pairs, the O atoms would each have two lone pairs, and the Br atom would have three lone pairs.

Answer 2

Answer : The Lewis-dot structure for the following molecules are shown below.

Explanation :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

In the Lewis-dot structure the valance electrons are shown by 'dot'.

Now we have to determine the Lewis-dot structure for the following molecules.

(a) The given molecule is,
`ICl`

As we know that iodine and chlorine have '7' valence electrons.

Therefore, the total number of valence electrons in
`ICl` = 7 + 7 = 14

According to Lewis-dot structure, there are 2 number of bonding electrons and 12 number of non-bonding electrons.

(b) The given molecule is,
`PH_3`

As we know that phosphorous has '5' valence electrons and hydrogen has '1' valence electrons.

Therefore, the total number of valence electrons in
`PH_3` = 5 + 3(1) = 8

According to Lewis-dot structure, there are 6 number of bonding electrons and 2 number of non-bonding electrons.

(c) The given molecule is,
`P_4`

As we know that phosphorous has '5' valence electrons.

Therefore, the total number of valence electrons in
`P_4` = 4(5) = 20

According to Lewis-dot structure, there are 6 number of bonding electrons and 14 number of non-bonding electrons.

(d) The given molecule is,
`H_2S`

As we know that sulfur has '6' valence electrons and hydrogen has '1' valence electrons.

Therefore, the total number of valence electrons in
`H_2S` = 6 + 2(1) = 8

According to Lewis-dot structure, there are 4 number of bonding electrons and 4 number of non-bonding electrons.

(e) The given molecule is,
`N_2H_4`

As we know that nitrogen has '5' valence electrons and hydrogen has '1' valence electrons.

Therefore, the total number of valence electrons in
`N_2H_4` = 2(5) + 4(1) = 14

According to Lewis-dot structure, there are 10 number of bonding electrons and 4 number of non-bonding electrons.

(f) The given molecule is,
`HClO_3`

As we know that chlorine has '7' valence electrons, oxygen has '6' valence electrons and hydrogen has '1' valence electrons.

Therefore, the total number of valence electrons in
`HClO_3` = 1 + 7 + 3(6) = 26

According to Lewis-dot structure, there are 12 number of bonding electrons and 14 number of non-bonding electrons.

(g) The given molecule is,
`COBr_2`

As we know that bromine has '7' valence electrons, oxygen has '6' valence electrons and carbon has '4' valence electrons.

Therefore, the total number of valence electrons in
`COBr_2` = 4 + 6 + 2(7) = 24

According to Lewis-dot structure, there are 8 number of bonding electrons and 16 number of non-bonding electrons.