2.2 Definitions

Question 1

Electron pair repulsion theory

Answer 1

The shape adopted by a simple molecule or ion is that which keeps repulsive forces to a minimum

Question 2

Bonding and lone pairs…

Answer 2

OF ELECTRONS!

Question 3

Non-polar bond

Answer 3

Atoms have equal electronegativity

Question 4

Polar bond

Answer 4

Different atoms with different electronegativities

Question 5

When going to the right of the periodic table, nuclear charge…

Answer 5

Increases

Question 6

When going to the right of the periodic table, electron shielding…

Answer 6

Stays the same

Question 7

When going to the right of the periodic table, distance from the nucleus…

Answer 7

Decreases

Question 8

When going up a group in the periodic table, nuclear charge…

Answer 8

Decreases

Question 9

When going up a group in the period table, electron shielding…

Answer 9

Decreases

Question 10

When going up a group in the periodic table, distance from the nucleus…

Answer 10

Decreases

Question 11

2 bonds, 0 lone pairs

Answer 11

Linear, 180°

Question 12

3 bonds, 0 lone pairs

Answer 12

Trigonal planar, 120°

Question 13

4 bonds, 0 lone pairs

Answer 13

Tetrahedral, 109.5°

Question 14

6 bonds, 0 lone pairs

Answer 14

Octahedral, 90°

Question 15

4 bonds, 1 lone pair

Answer 15

Pyramidal, 107°

Question 16

4 bonds, 2 lone pairs

Answer 16

Non-linear, 104.5°

Question 17

London dispersion forces

Answer 17

Weakest, temporary dipole induced dipole interaction, non-polar, simple covalent molecules, more electrons=stronger

Question 18

Dipole-dipole forces

Answer 18

Permanent dipole interaction, polar molecules

Question 19

Hydrogen bonds

Answer 19

Strongest, H directly bonded to N, O, or F, causes higher boiling points

Question 20

Why only N, O, and F?

Answer 20

They have high charge density because their high charges are packed into small sized atoms, making intermolecular attractions greater