Metals

properties of metals

good conductors of electricity and heat, high melting and boiling points (solid at room temperature), hard, strong, don't shatter easily, look shiny when polished

1 of 35

properties of metal II

sonorous, high density, form positive ions when the react, react with oxygen to form oxides that are bases

2 of 35

reacting with dilute acids

metals react with dilute acids to form salts, and hydrogen gas is given off

3 of 35

reacting with oxygen

metals react with oxygen to form oxides, and these oxides are bases - they neutralise acids, forming salts and water

4 of 35

what they form when they've reacted

metals form positive ions when they react

5 of 35

reactive metals

have strong drives to give up electrons and form ions, with stable outer electron shells, so they reacts readily to form compounds

6 of 35

order of reactivity (from least to most) with water

gold (no reaction), silver (no reaction), copper (no reaction), iron (slow with steam), zinc (quite slow with steam), magnesium (very slow with cold water, but vigorous with steam), calcium (less violent with cold water)

7 of 35

order of reactivity II

sodium (violent with cold water), potassium (very violent with cold water; catches fire)

8 of 35

order of reactivity (from least to most) with hydrochloric acid

gold (no reaction), silver (no reaction), copper (no reaction even w. concentrated acid), lead (slow + only if acid is concentrated), iron (slow), zinc (quite slow), magnesium (vigorous)

9 of 35

hydrogen is displaced

when a metal reacts with water or hydrochloric acid, it drives hydrogen out, and takes its place, which shows the metal is more reactive than hydrogen, and has a stronger drive to form a compound

10 of 35

redox reaction

a type of chemical reaction that involves a transfer of electrons between two species

11 of 35

oxidation

the loss of electrons

12 of 35

reduction

gain of electrons

13 of 35

competing with carbon

carbon is more reactive than some metals, it will reduce their oxides to the metal

14 of 35

competing with other metals for oxygen

a metal will reduce the oxide of a less reactive metal, and the reduction always gives out heat - it is exothermic

15 of 35

competing to form ion in solution

a metal displaces a less reactive metal from solutions of its compounds

16 of 35

comparing the drive to form ions

the more reactive metal forms positive ions more readily

17 of 35

the reactivity series

least reactive (hydrogen displaces these metals): gold, silver, copper; increasing reactivity (carbon displaces these metals): lead, iron, zinc; most reactive (carbon can't reduce their oxides): aluminium, magnesium, calcium, sodium, potassium

18 of 35

their drive

the reactivity series is a list of the metals in order of their drive to give up electrons, and form positive ions with stable outer shells

19 of 35

reacting

a metal will react with a compound of a less reactive metal by pushing the less reactive metal out of the compound and taking its place

20 of 35

stable

the more reactive the metal, the more stable its compounds are, they don't break down easily

21 of 35

electrolysis

chemical decomposition produced by passing an electric current through a liquid or solution containing ions; used when the metal is very reactive, so its hard to extract from its ores, since they're stable compounds

22 of 35

compounds

the less reactive the metal, the less it likes to form compounds

23 of 35

thermal decomposition

the lower the reactivity of a metal, the more readily its compounds decompose when heated; carbonate, except those of Na and K, decompose to the oxide and carbon dioxide; hydroxides, except those of Na and K, decompose to the oxide and water

24 of 35

thermal decomposition II

nitrates, except those of Na and K, decompose to the oxide, nitrogen dioxide, and oxygen, and the nitrates of Na and K form nitrites and oxygen

25 of 35

uses of the reactivity series

the thermite process; making simple cells (a simple cell consists of to different metals in an electrolyte, electrons flow from the more reactive metal, so it is called the negative pole, the other metal is the positive pole)

26 of 35

uses of the reactivity series II

using other metals in simple cells (the further apart the metals are in reactivity, the higher the voltage will be); the sacrificial protection of iron (the zinc is used instead of the iron); galvanising (the iron or steel is coated with zinc)

27 of 35

metals in the earth's crust

the crust is mostly made of compounds, but also contains some elements, such as copper, silver, mercury, platinum and gold, and these occur native (uncombined) because they are unreactive

28 of 35

precious metals

include gold, silver, platinum, and palladium because they are scarce, expensive, and are often kept as a store of wealth

29 of 35

extraction of unreactive metals

these metals occur in their ores as elements, and all you need to do is separate the metal from sand and other impurities

30 of 35

ores of other metals

contain the metals as compounds, so they have to be reduced to give the metal: metal compound --> reduction --> metal

31 of 35

extraction of more reactive metals

these compounds are very stable, and need electrolysis to reduce them

32 of 35

extraction of less reactive metals

these compounds are less stable, and can be reduced to the metal by a chemical reaction

33 of 35

blast furnace

used for extracting iron from its ore

34 of 35

electrolysis tank

used for the electrolysis of aluminium

35 of 35

Get Revising

Metals

Other cards in this set

Card 2

Front

Back

Card 3

Front

Back

Card 4

Front

Back

Card 5

Front

Back

Comments

Similar Chemistry resources:

Other cards in this set

Card 2

Front

Back

Card 3

Front

Back

Card 4

Front

Back

Card 5

Front

Back

Comments

Related discussions on The Student Room

Similar Chemistry resources: