Metals

Question 1

What two components are there of a metal structure?

Answer 1

a lattice of positive metal ions

a ‘sea’ of delocalised electrons

Question 2

what is metallic bonding?

Answer 2

The electrostatic attraction between the positive metal ions and the negative delocalised electrons.

Question 3

Metals are malleable because…

Answer 3

the layers of metal ions can slide over each other

Question 4

What is thermal decomposition?

Answer 4

This is when a substance breaks down into simpler substances when heated.

Question 5

metal carbonate -heat->

Answer 5

metal oxide + carbon dioxide

Question 6

uses of carbon dioxide

Answer 6

fire extinguisher
carbonated drinks
decaffeination
theatre dry ice

Question 7

metal + water —>

Answer 7

metal hydroxide + hydrogen

Question 8

group 1 metal properties

Answer 8

stored ‘under oil’ to prevent reaction with oxygen

they are soft and can be cut with a knife

Question 9

name for group 1

Answer 9

alkali metals

Question 10

what is the trend in melting points in group 1?

Answer 10

They have low melting points that decrease down the group

Question 11

When Group 1 metals react, what happens to the Group 1 metal atoms in
terms of electrons?

Answer 11

They lose their outer electron which is transferred to the other element

Question 12

When a metal reacts it loses its outer electron. Going down the group, this can happen more easily
This is because…

Answer 12

The atoms get bigger and have more shells
the outer electron is further from the nucleus
the attraction between outer electrons and the nucleus is weaker
so less energy is needed to remove the outer electron and so the metal reacts more easily

Question 13

lithium reaction with water

Answer 13

metal floats on surface of water and fizzes around, then solid disappears

Question 14

sodium reaction with water

Answer 14

metal melts into a ball, fizzes, may catch fire

Question 15

potassium reaction with water

Answer 15

lilac flame produced

Question 16

What is a displacement reaction?

Answer 16

when a more reactive metal takes the place (displaces) of a less reactive metal

Question 17

metal reactivity series

Answer 17

K, Na, Li, Ca, Mg, Al, C, Zn, Fe, Pb, H, Cu, Ag, Au, Pt

Question 18

how to remember reactivity series

Answer 18

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Question 19

oxidation

Answer 19

gain of oxygen

Question 20

reduction

Answer 20

loss of oxygen

Question 21

Redox Reaction

Answer 21

Where reduction and oxidation both take place

Question 22

oxidising agent

Answer 22

causes something else to be oxidised

Question 23

an oxidising agent is itself

Answer 23

reduced

Question 24

a reducing agent

Answer 24

causes something else to be reduced

Question 25

a reducing agent is itself

Answer 25

oxidised

Question 26

rust forms when iron is..

Answer 26

oxidised

Question 27

to rust iron we need:

Answer 27

oxygen | water

Question 28

show iron becoming hydrated by water in an equation

Answer 28

Fe2O3 (s) + xH2O (l) —> Fe2O3 •xH2O (s)

Question 29

preventing rusting | barrier method

Answer 29

use grease/oil (on moving parts) paint, and plastic (for big and small objects) prevents iron from coming in contact with water as long as coating is intact

Question 30

preventing rust | sacrificial protection

Answer 30

attach a block of a more reactive metal to the iron. this displaces the iron from rust. the block has to be replaced after some time

Question 31

preventing rust | galvanising

Answer 31

coating the iron in zinc prevents O2 and H2O from coming in contact with the iron if a crack appears zinc is more reactive so acts as a sacrificial protection as well