EL 8 Spectacular Metals

Question 1

Physical Properties of Metals (9)

Answer 1

• Malleable
• Sonorous
• High Density
• Shiny
• Ductile
• Good Thermal Conductor
• Good Electrical Conductor
• High Melting Point
• High Boiling Point

Question 2

Explain bonding in metals [3 marks]

Answer 2

• Metallic Bonding
• The outer electrons of metals become delocalised and are free to move in a sea of electrons
• Positively charged metallic cations are attracted to the delocalised negatively charged electrons

Question 3

Group 1 and 2 Metal Properties (3)

Answer 3

• Soft = Easy to cut
• Weak = Breaks easily
• Low melting point

Question 4

Group 1 and 2 Metal Origins (What are they found as)

Answer 4

• Highly reactive = Found as cations (Positively charged ions)

Question 5

Define “salt”

Answer 5

A chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions

Question 6

Group 1 and 2 Metals react with water to form…?

Answer 6

Metal + Water —> Metal Hydroxide and Hydrogen

Question 7

Group 1 Metals are known as…?

Answer 7

Alkaline Metals

Question 8

Group 2 Metals are known as…?

Answer 8

Alkaline Earth Metals

Question 9

Hydroxide Ion

Answer 9

OH 1-

Question 10

Nitrate Ion

Answer 10

NO3 1-

Question 11

Sulphate Ion

Answer 11

SO4 2-

Question 12

Carbonate Ion

Answer 12

CO3 2-

Question 13

Hydrogen Carbonate Ion

Answer 13

HCO3 1-

Question 14

Group 1 and 2 Metals react with oxygen to form…?

Answer 14

Metal + Oxygen —> Metal Oxide

Question 15

Group 1 and 2 Metals react with halogens to form…?

Answer 15

Metal + Halogen —> Metal Halide

Question 16

Why are Group 1 and 2 Metals more reactive as you go down? (3)

Answer 16

i) Greater Number of Shells

ii) Electron Shielding

iii) Greater Nuclear Charge

Question 17

Why are Group 1 Metals more reactive than Group 2 Metals?

Answer 17

Group 1 = 1 electron to be removed

Group 2 = 2 electrons to be removed

Therefore, Group 2 requires more energy = less reactive

Question 18

Group 2 Metal Oxides react with water to form…?

Answer 18

Metal Oxide + Water —> Metal Hydroxide

Question 19

Group 2 Metal Oxides react with acid to form…?

Answer 19

Metal Oxide + Acid —> Salt + Water

Question 20

Group 2 Metal Hydroxides react with acid to form…?

Answer 20

Metal Hydroxide + Acid —> Salt + Water

Question 21

Group 2 Metal Hydroxides dissolve in water to form…?

Answer 21

Metal Hydroxide —-> Metal Ions + Hydroxide Ions

Question 22

Factors affecting Charge Density (2)

Answer 22

• Ions with a smaller radius = higher charge density
  —> i.e. found at the top of groups in the periodic table
• Ions with a greater charge = higher charge density
  —> Al3+ > K+

Question 23

Group 2 Carbonates Thermal Stability Trend

Answer 23

As you go down Group 2, thermal stability increases (requires more heat) since there is less distortion

Question 24

Group 2 Hydroxides Solubility Trend

Answer 24

As you go down Group 2, solubility increases

Question 25

Group 2 Sulphates & Carbonates Solubility Trend

Answer 25

As you go down Group 2, solubility decreases

Question 26

Define First Ionisation Enthalpy

Answer 26

The energy requires to remove one electron from every atom in one mole of isolated gaseous atoms

Question 27

First Ionisation Enthalpy Equation

Answer 27

X(g) —> X+(g) + e-

Question 28

Shape of a s subshell

Answer 28

Spherical

Question 29

Number of orbitals in a s subshell

Answer 29

One Orbital

Question 30

Shape of a p subshell

Answer 30

Dummbell

Question 31

Number of orbitals in a p subshell

Answer 31

Three Orbitals

Question 32

Shape of a d subshell

Answer 32

Double Dummbell

Question 33

Number of orbitals in a d subshell

Answer 33

Five Orbitals

Question 34

How many electrons can fit in a single orbital?

Answer 34

2e-

Question 35

Factors which affect Ionisation Enthalpy (3)

Answer 35

i) Atomic Radius Larger radius = Less energy required ii) Electron Shielding More shields lead to more shielding = Less energy required iii) Nuclear Charge The number of protons in the nucleus influences the Ionisation Energy

Question 36

Why is there a drop in Ionisation Energy between Group 2 and 3?

Answer 36

The addition of a p subshell

Question 37

Why is there a drop in Ionisation Energy between Group 5 and 6?

Answer 37

The electron repulsion when the 4th electron occupies its position in the orbital

Question 38

Thermal Decomposition of a Metal Carbonate

Answer 38

MCO3(s) —> MO(s) + CO2(g)

Question 39

Group 2 Hydroxide’s pH in Water Trend

Answer 39

As you go down Group 2, pH increases

Question 40

As you go across a Period, what happens to the Ionisation Energy and why is this?

Answer 40

Number of Shells and Shields stay the same = These factors have no effect on the Ionisation Energy Nuclear Charge Increases = Ionisation Energy generally increases

Question 41

Example : Why is AlCl3 more distorted than NaCl?

Answer 41

The cation Al 3+ has a greater charge than that of the cation Na +, therefore Al 3+ has a higher charge density than Na +

Question 42

Example : Why is AlF3 less distorted than AlBr3?

Answer 42

The anion F- has a smaller radius than that of the anion Br-, therefore Br- has a lower charge density and is more readily distorted