Question

Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.

(a)$P{H}_3$.

(b)$P{H}_4+$.

(c)$P_2{H}_4$.

(d)$P{O_4}^3-$

(e)$P{F}_5$

Short answer

(a) The lewis structure of PH₃ is

(b) The lewis structure of $P{H}_4^{+}$

(c) The lewis structure of P₂H₄

(d) The lewis structure of $P{O}_4^{3-}$

(e) The lewis structure of PF₅

Step-by-step solution

Determine the formula for active power and apparent power

• Lewis structures, also known as Lewis dot formulas, Lewis dot structures, electron dot structures.
• Lewis electron dot structures, are diagrams that depict the bonding between atoms in a molecule as well as any lone pairs of electrons that may be present.

Determine the Lewis structure of PH3

(a)The lewis structure of PH₃

In phosphine$P{H}_3,$Phosphorus (P) is attached to$3H$atoms. The valence electron configurations of the elements are as follows:

$\begin{array}{l}P=3s^{2}3p^3\\ H=1s^1\end{array}$

As a result, the total number of valence electrons involved is: 8. The centre P atom has a lone pair of electrons in addition to the three bond pairs.

Determine the Lewis structure of $P{H}_4^{+}$

(b)The lewis structure of $P{H}_4^{+}$

In$P{H}_4^{+}$, Phosphorus (P) is attached to 4 H atoms. The valence electron configurations of the elements are as follows:

$\begin{array}{l}P=3s^{2}3p^3\\ H=1s^1\end{array}$

As a result, the total number of valence electrons involved is: 9. Furthermore, because the molecule has a net charge of +1, the actual electrons involved in bonding are 9-1=8.

Determine the Lewis structure of P2H4

(c)The lewis structure of $In{P}_2{H}_4$

$In{P}_2{H}_4$, Each Patom has a link with another Patom 2 H atoms. A covalent bond also exists between the two P atoms.

The valence electron configurations of the elements are as follows:

$\begin{array}{l}P=3s^{2}3p^3\\ H=1s^1\end{array}$

As a result, the total number of valence electrons involved is: 14. Each P atom has one lone pair of electrons in addition to the two bond pairs.

Determine the Lewis structure of $P{O}_4^{3-}$

(d)The lewis structure of $P{O}_4^{3-}$

In$P{O}_4^{3-}$, The P atom is surrounded by 40 other atoms. The valence electron configurations of the elements are as follows:

$\begin{array}{l}P=3s^{2}3p^3\\ O=2s^{2}2p^4\end{array}$

As a result, the number of valence electrons involved is: 29. Furthermore, there is a -3 net charge. As a result, the molecular ion's total electrons are 29+3=32. For example, the Lewis structure for $P{O}_4^{3-}$ is essentially a resonance hybrid with a partial double bond character on each P-O bond.

Determine the Lewis structure of PF5

(e)The lewis structure of $P{F}_5$

In$P{F}_5$, Phosphorus (P) is attached to$5F$atoms. The valence electron configurations of the elements are as follows:

$\begin{array}{l}P=3s^{2}3p^3\\ F=2s^{2}2p^5\end{array}$

As a result, the total number of valence electrons involved is 40. Each F atom is surrounded by 5 bond pairs and 3 lone pairs.