Chapter 5

Question 1

What are shells regarded as?

Answer 1

Energy levels

Question 2

What happens to energy as the shells increase

Answer 2

Energy increases

Question 3

What is shell number (n) also known as?

Answer 3

Principle quantum number

Question 4

How do you work out the number of electrons in each shell?

Answer 4

2(n^2)

Question 5

What are orbitals? Definition?

Answer 5

Make up the sub shells which make up the shells
Region of space around nucleus that can hold up to 2 paired electrons with opposite spins

Question 6

How many electrons can each orbital hold? What are the different types of orbitals?

Answer 6

2 electron s
s, p, d, f

Question 7

What shapes are the s and p orbitals?

Answer 7

s = sphere (greater the shell number the larger the radius)
p = dumbbell ( greater the shell number the farther the orbital from the nucleus)

Question 8

Which orbitals are in each shell?

Answer 8

n = 1: 1s
n = 2: 2s + 3 x 2p
n = 3: 3s + 3 x 3p + 5 x 3d
n = 4: 4s + 3 x 4p + 5 x 4d + 7 x 4f

Question 9

Which shell and orbitals have the highest energy?

Answer 9

fourth = highest energy
f orbital = highest energy

Question 10

What are the 3 rules of filling the orbitals?

Answer 10

RULE 1:
- orbitals fill in order of increasing energy
- EXCEPT 4s fills before 3d
RULE 2:
- electrons pair with opposite spins (up and down)
- represented by arrows
- to minimise repulsion
RULE 3:
- orbitals with the same energy (subshell orbitals) are occupied singularly first
- prevents repulsion until no other orbitals are available

Question 11

What is the shorthand notation for electron configuration?

Answer 11

Previous noble gas plus the outer electron sub shells
Na: [Ne] 3s1

Question 12

How do we write the electron configuration of ions?

Answer 12

Once filled, 4s becomes higher in energy than 3d orbital so the electrons in 4s are lost before 3d even though it fills first
Write 3d before 4s for ions

Question 13

What is the electrostatic force of attraction between in ionic bonding?

Answer 13

The oppositely charge ions in all directions

Question 14

What is the definition of ionic bonding?

Answer 14

The electrostatic force of attraction between oppositely charged ions in all directions to form a giant ionic lattice

Question 15

What affects the MP/BP of ionic compounds?

Answer 15

Ionic charge - greater charge means stronger electrostatic forces so a higher MP/BP
Ionic radius - smaller the ionic radius means the stronger the electrostatic force so higher MP/BP

Question 16

What is the pattern for size of ionic radii?

Answer 16

Increases in size down the group

Question 17

Which isoelectronic ions have smaller ionic radii?

Answer 17

Ones with the most protons as the nucleus would have stronger electrostatic forces of attraction with the electrons pulling the ionic structure closer together

Question 18

How do ionic compounds dissolve in water? Pattern for solubility?

Answer 18

The water molecules break down the lattice and surround each ion in the solution
Greater ion chargers = reduced solubility

Question 19

Definition of a molecule?

Answer 19

Smallest part of a covalent compound that can exist while retaining the chemical properties of the compound

Question 20

How do you know how many covalent bonds an atom can form?

Answer 20

Number of electrons it needs to have a full outer shell

Question 21

What are dative covalent bonds? Another name for them?

Answer 21

A covalent bond where the shared pair of electrons have been supplied by one of the bonding atoms only
They were originally a lone pair of electrons
Coordinate bonds

Question 22

How are dative covalent bonds represented in a displayed formula?

Answer 22

By an arrow from the one supplying to the bonded one

Question 23

What is 1 unusual case for covalent bonding?

Answer 23

Expanding the octet -> more electrons in the outer shell as they’re are more orbitals available

Question 24

What are reasons why some have full outer shells of 18 electrons?

Answer 24

• Limited by size of the atom
• number of electrons available from atom

Question 25

What is the second unusual case for covalent bonding?

Answer 25

Boron only has 6 electrons in the outer shell when bonded to BF3 as it only has 3 electrons to give
Unless it does dative bonding

Question 26

What is a metallic structure?

Answer 26

Positive metal ions with electrostatic forces of attraction between a sea of delocalised electrons in a regular arrangement to form a giant metallic structure.

Question 27

What are the properties of metallic structures?

Answer 27

Conductors
Malleable
Ductile
High melting point/BP
Insoluble

Question 28

What affects the strength of metals?

Answer 28

1) charge of ion - greater the charge, greater the number of delocalised electrons = stronger electrostatic forces of attraction between positive cations and delocalised electrons
2) size of ion -smaller ion means electrons are closer to nucleus so strength of electrostatic forces are stronger

Question 29

Definition of periodicity?

Answer 29

Trends across a period

Question 30

Period 2 trends in MP/BP?

Answer 30

Li, Be:
- giant metallic
- high MP/BP
B, C:
- giant covalent
- very high MP/BP
N, O, F:
- simple molecules
- low MP/BP
Ne:
- monatomic
- single atoms
- very low MP/BP

Question 31

Period 3 trend in MP/BP?

Answer 31

do it urself