4 Bonding

Question 1

Attractive Force is proportional to ((+q)(-q))/r²

Answer 1

+q= magnitude of positive charge

-q = magnitude of negative charge

r = distance between charges

Question 2

If the central atom has 2 electron pairs, then it has

Answer 2

sp hybridization and its basic shape is linear

Question 3

If the central atom has 3 electron pairs, then it has

Answer 3

sp² hybridization and its basic shape is trigonal planar; its bond angles are about 120º.

With one non-binding pair the shape is bent

Question 4

If the central atom has 4 electrons pairs, then it has

Answer 4

sp³ hybridiation and its basic shape is tetrahydral; its bond angles are about 109.5º

o lone pairs = tetrahydral

1 non-binding pair = trigonal pyramidal

2 non-binding pair = bent

Question 5

If the central atom has 5 electron pairs, then it has

Answer 5

sp³d hybridization and its basic shape is trigonal bipyramidal.

o lone pairs of electrons = trigonal bipyramidal

1 non-binding pairs of electrons = folded square, see-saw, distorted tetrahedron

2 non-binding pairs of electrons = T-shaped

3 non-binding pairs of electrons = linear

Question 6

If the central atom has 6 electron pairs, then it has

Answer 6

sp3d2 hybridization and its basic shape is octahedral.

0 lone pairs = octahydral

1 lone pair = square pyramidal

2 lone pair= square planar

Question 7

Van der Waals Forces

Answer 7

Dipole - dipole (strong)

positive end of one polar molecule attracted to the negative end of another.

London Dispersion Forces(weak)

Due to random motions of electrons one side of an atom may be temporarily charged

Hydrogen(strongest)

Strong bond between hydrogen and an extremely electronegative element (flourine, oxygen, or nitrogen)