Chapter 5, Electrons and Bonding

Question 1

What is an atomic orbital?

Answer 1

A region around the nucleus that can hold up to two electrons, with opposite spins.

Question 2

What are the different types of orbitals?

Answer 2

s, p, d and f orbitals

Question 3

s - how many orbitals and electrons

Answer 3

one orbital so it can hold two electrons

Question 4

p - how many orbitals and electrons

Answer 4

has three orbitals so can hold 2*3= 6 electrons

Question 5

d - how many orbitals and electrons

Answer 5

has 5 orbitals so can hold 2*5= 10 electrons

Question 6

f - how many orbitals and electrons?

Answer 6

has 7 orbitals so can hold 2*7= 14 electrons

Question 7

What are ionic compounds?

Answer 7

Oppositely charged ions held together by electrostatic attraction.

Question 8

Features of giant ionic structures

Answer 8

regular structure
cubic shape
giant repeating pattern

Question 9

Why do most ionic compounds dissolve in water?

Answer 9

As water molecules are polar they can attract the positive and negative ions and break up the structure.

Question 10

Why do ionic compounds have high melting points?

Answer 10

As there are many strong electrostatic forces between oppositely charged ions. Lots of energy needed to overcome these forces.

Question 11

What is covalent bonding?

Answer 11

The sharing of outer electrons in order for the atoms to obtain a full shell.

Question 12

What is a dative covalent bond?

Answer 12

Where ONE atom donates 2 electrons to an atom or ion to form a bond.

Question 13

Why do molecules have specific shapes?

Answer 13

Since bonds repel each other equally. Bonds contain electrons so they will want to be as far apart as possible.

Question 14

What do lone pairs do in terms of shape?

Answer 14

Change the shape and bond angles. Lone pairs push bonding pairs closer together.

Question 15

Carbon dioxide

Answer 15

BP-2 LP-0 linear 180

Question 16

BCl3 (boron trichloride)

Answer 16

BP-3 LP-3 trigonal planar 120

Question 17

CH4 (methane)

Answer 17

BP-0 LP-0 Tetrahedral 109.5

Question 18

PCl5

Answer 18

BP-5 LP-0 trigonal bipyramidal 120 and 90 degrees

Question 19

SF6 sulfur hexafluoride

Answer 19

BP-6 LP-0 octahedral 90

Question 20

NH3 ammonia

Answer 20

BP-3 LP-1 trigonal pyramidal 107

Question 21

H20 water

Answer 21

BP-2 LP-2 non linear 104.5

Question 22

What is electronegativity?

Answer 22

The ability for an atom to attract electrons towards itself in a covalent bond.

Question 23

How do we quantify how electronegative an element is?

Answer 23

By using the Pauling scale.

Question 24

How can covalent bonds become polar?

Answer 24

If the atoms attached to it have a difference in electronegativity.

Question 25

What happens in an induced dipole dipole?

Answer 25

Electrons in an atom or molecule can move from one end to another

Question 26

Which crystal does an induced dipole-dipole force occur in?

Answer 26

Iodine

Question 27

Why are there weaker induced dipole-dipole forces in branched hydrocarbons?

Answer 27

As they can’t pack together as close. This lowers their boiling points.