1997 AP Exam

Explain each of the following observations using principles of atomic structure and/or bonding

b) The ionic radius of N^3– is larger than that of O^2–.

N^3–(1s²)(2s²,2p⁶) Z^* = 7 – (2 · 0.85 + 7 · 0.35) = 2.85

O^2–(1s²)(2s²,2p⁶) Z^* = 8 – (2 · 0.85 + 7 · 0.35) = 3.85

The electrons in N^3– experience a smaller effective nuclear charge and are less bound to the nucleus compared to the electrons in oxygen. The result is the electrons in nitrogen will take up a occupy volume.

Explain each of the following observations using principles of atomic structure and/or bonding

b) The ionic radius of N3– is larger than that of O2–.

N3– (1s2)(2s2,2p6) Z* = 7 – (2 · 0.85 + 7 · 0.35) = 2.85

O2– (1s2)(2s2,2p6) Z* = 8 – (2 · 0.85 + 7 · 0.35) = 3.85

The electrons in N3– experience a smaller effective nuclear charge and are less bound to the nucleus compared to the electrons in oxygen. The result is the electrons in nitrogen will take up a occupy volume.

b) The ionic radius of N^3– is larger than that of O^2–.

N^3–(1s²)(2s²,2p⁶) Z^* = 7 – (2 · 0.85 + 7 · 0.35) = 2.85

O^2–(1s²)(2s²,2p⁶) Z^* = 8 – (2 · 0.85 + 7 · 0.35) = 3.85

The electrons in N^3– experience a smaller effective nuclear charge and are less bound to the nucleus compared to the electrons in oxygen. The result is the electrons in nitrogen will take up a occupy volume.