The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?

A. + 5 and + 8

B. + 3 and + 6

C. + 5 and + 6

D. + 3 and + 8

E. + 1 and + 4

Question

Jay Krueger

Chemistry

1 February, 01:45

The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?

A. + 5 and + 8

B. + 3 and + 6

C. + 5 and + 6

D. + 3 and + 8

E. + 1 and + 4

+1

Answers (1)

Know the Answer?

Kash Murray · Answer 1

Option B. + 3 and + 6

Explanation:

Zeff = z - s

where z is the atomic number, s is the number of shielding (non-valence) electrons

For Boron, electronic configuration is 1s²2s³.

z = 5, s = 2

Zeff = 5 - 2 = + 3

For Oxygen, electronic configuration is 1s²2s²2p⁴

z = 8, s = 2

Zeff = 8 - 2 = + 6

The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?A. + 5 and + 8B. + 3 and + 6C. + 5 and + 6D. + 3 and + 8E. + 1 and + 4

The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?

A. + 5 and + 8

B. + 3 and + 6

C. + 5 and + 6

D. + 3 and + 8

E. + 1 and + 4