Phosphide Ion and Lewis Structures

The video tutorial explains how to draw the Lewis structure for the phosphide ion (P3-). It begins by illustrating the Lewis structure for neutral phosphorus, which has five valence electrons. The tutorial then adds three extra electrons to account for the negative charge of the phosphide ion, resulting in a stable octet. The final structure is enclosed in brackets to indicate the ion's charge.

What is the initial step in drawing the Lewis structure for the phosphide ion?

• Find phosphorus on the periodic table

• Add extra electrons to phosphorus

• Draw the Lewis structure for phosphorus as a neutral element

• Identify the charge of the ion

In which group is phosphorus found on the periodic table?

• Group 15

• Group 16

• Group 17

• Group 14

How many valence electrons does neutral phosphorus have?

• Eight

• Five

• Seven

• Three

What change is made to phosphorus to form the phosphide ion?

• Remove one electron

• Remove three electrons

• Add three electrons

• Add one electron

Why does phosphorus have a minus three charge in the phosphide ion?

• It gains three protons

• It gains three electrons

• It loses three protons

• It loses three electrons

What is the term used to describe the eight valence electrons around the phosphide ion?

• Quartet

• Sextet

• Octet

• Duet

What is the significance of having an octet in the phosphide ion?

• It makes the ion unstable

• It makes the ion neutral

• It makes the ion stable

• It makes the ion positively charged

What additional notation is used to correctly represent the phosphide ion's Lewis structure?

• Brackets

• Parentheses

• Quotation marks

• Curly braces