Question

Consider the two molecules BF₃ and NF₃. Compare and contrast them in terms of the following:

(a) valence-level orbitals on the central atom that are used for bonding

Both use the _orbitals for bonding. B uses _ s and _p orbitals while N uses _s and _ p orbitals for bonding.

(b) shape of the molecule

BF₃ is _ while NF₃ is _

c) number of lone electron pairs on the central atom

BF₃ has _ lone pair(s)

NF₃has _ lone pair(s)

(Answer should be either one or no)

(d) type and number of bonds found in the molecule

BF₃ has _covalent bonds. NF₃ has _covalent bonds.

(Answer should be either very polar or polar)

Answer 1

Electronic configuration of

B : 1s22s22p1 (ground state), 1s22s12p2 (exited state)

N : 1s22s22p3

أمر ما T- Z:

a) both use hybridised orbitals for bonding. B uses 1s orbital and 2p orbitals and N uses 1s orbital and 3p orbital for bonding.

b) BF3 having sp2 hybridisation forms trigonal planar, NF3 having sp3 hybridisation forms pyramidal geometry.

c) BF3 has no lone pairs while NF3 have one lone pair.

d) because of high electronegativity differences BF3 has 3 very polar covalent bonds,

because of low electronegativity differences NF3 has 3 polar covalent bonds.