Phosphorous is a nonmetal in Group 5A of the Periodic Table. How will the phosphorus atom shown below achieve an octet if it takes part in an ionic bond? Remember that atoms bond to achieve a full outer level of 8 valence electrons, which is considered an octet.
To achieve an octet in an ionic bond, phosphorus (P) will typically lose 3 electrons to form a 3+ ion. This is because phosphorus has 5 valence electrons and needs 8 valence electrons to achieve an octet.
The phosphorus atom shown below would lose its 3 valence electrons to become an ion with a positive charge of 3+:
Phosphorus atom (before bonding): 1s² 2s² 2p⁶ 3s² 3p³
Phosphorus ion (after losing 3 electrons): 1s² 2s² 2p⁶
By losing 3 electrons, the phosphorus ion becomes isoelectronic with the noble gas neon (Ne), which has a full outer level of 8 valence electrons. This allows the phosphorus atom to achieve an octet and become more stable.
a
Phosphorus will lose 5 electrons.
b
Phosphorus will gain 5 electrons.
c
Phosphorus will lose 3 electrons.
d
Phosphorus will gain 8 electrons.
e
Phosphorus will lose 8 electrons.
f
Phosphorus will gain 15 electrons.
g
Phosphorus will gain 3 electrons.
h
Phosphorus will lose 15 electrons.