Metals

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Periodic table

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Horizontal rows are called PERIODS

Hello. My name’s Dimitri Mendeleev. In the 19th century I arranged all the known elements into a pattern according to their properties. This pattern is called “The Periodic Table”

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What does the periodic table tell you?

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The SYMBOL of the element

The NAME of the element

The PROTON NUMBER of the element

The MASS of the element

Elements and symbols that you should know:

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Part 1 – The obvious ones:

1. Hydrogen
2. Helium
3. Lithium
4. Beryllium
5. Boron
6. Carbon
7. Nitrogen

8. Oxygen
9. Fluorine
10. Neon
11. Magnesium
12. Aluminium
13. Silicon
14. Phosphorus

H

He

Li

Be

B

C

N

O

F

Ne

Mg

Al

Si

P

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Some more obvious ones:

15. Sulphur
16. Chlorine
17. Argon

18) Calcium

19) Zinc

The less obvious ones:

1. Sodium
2. Potassium
3. Iron
4. Copper
5. Silver

6) Tin

7) Gold

8) Mercury

9) Lead

S

Cl

Ar

Ca

Zn

Na

K

Fe

Cu

Ag

Sn

Au

Hg

Pb

Group 1 – The alkali metals

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Group 1 – The alkali metals

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1) These metals all have to be stored under ____ because they react with _______

Some facts…

2) Reactivity increases as you go _______ the group.

5) They all react with water to form an alkali (hence their name) and __________, e.g:

Words – down, oil, cut, hydrogen, water, salt

3. They are all soft and easily ____

4) They form white soluble solids, like sodium chloride (___)

The Transition Metals

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1) This section includes metals like gold, mercury, iron, copper

Some facts…

2) They are all ______ and solid (except _________)

3) They are ____ reactive than the alkali metals

Words – hard, coloured, mercury, less, catalyst, insoluble

4) They can form __________ compounds, usually _______

5) They can be used as a ______ (a chemical that speeds up a reaction)

Reactions of metals with oxygen

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When a metal reacts with oxygen it will form a METAL OXIDE. This is what happens when a metal rusts. We can make this reaction happen quicker by burning the metal.

Reactions of metals with water

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When a metal reacts with water hydrogen is always given off. The other product will be either a metal hydroxide or a metal oxide.

Reactions of metals with acids

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When a metal reacts with an acid it gives off hydrogen (which can be “popped” using a lit splint). The other product is a salt.

Complete the following reactions:

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1. Lithium + water
2. Lithium + hydrochloric acid
3. Silver + oxygen
4. Magnesium + sulphuric acid
5. Potassium + oxygen
6. Aluminium + oxygen
7. Manganese + water
8. Sodium + sulphuric acid
9. Lithium + oxygen
10. Nickel + hydrochloric acid

Lithium hydroxide + hydrogen

Lithium chloride + hydrogen

Silver oxide

Magnesium sulphate + hydrogen

Potassium oxide

Aluminium oxide

Manganese oxide + hydrogen

Sodium sulphate + hydrogen

Lithium oxide

Nickel chloride + hydrogen

Reactivity Practical

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Task: to place six metals in order of reactivity

Equipment: hydrochloric acid, calcium, copper, iron, aluminium, magnesium, zinc

Conclusion: I think the order of reactivity is…

The actual order of reactivity is:

Calcium

Magnesium

Aluminium

Zinc

Iron

Copper

The Reactivity Series

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The Reactivity Series lists metals in order of reactivity:

Potassium

Sodium

Calcium

Magnesium

Aluminium

Carbon

Zinc

Iron

Lead

Copper

Silver

Gold

An example question on reactivity

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Displacement reactions

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A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound.

Displacement reactions

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A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound.

Some example reactions…

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Extension work – write down the equations for these reactions

Reaction

No Reaction

Reaction

Reaction

No Reaction

No Reaction

Extracting Metals

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A METAL ORE is a mineral or mixture of minerals from which it is “economically viable” to extract some metal.

To “extract” a metal from a metal oxide we need to REDUCE the oxygen. This is called a REDUCTION reaction. To put it simply:

Most ores contain METAL OXIDES (e.g. rust = iron oxide).

Some definitions:

Iron ore

“Reduce” the oxygen to make iron

How do we do it?

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Potassium

Sodium

Calcium

Magnesium

Aluminium

Carbon

Zinc

Iron

Tin

Lead

Copper

Silver

Gold

Platinum

Extracting metals

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1. What is an ore?
2. In what form are metals usually found in the Earth?
3. How do you get a metal out of a metal oxide?
4. What is this type of reaction called?

The Blast Furnace

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Electrolysis

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Electrolysis

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Electrolysis

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Electrolysis is used to extract a HIGHLY REACTIVE metal.

When we electrolysed copper chloride the negative chloride ions moved to the positive electrode and the positive copper ions moved to the negative electrode – OPPOSITES ATTRACT!!!

Redox reactions

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These happen during electrolysis:

These two processes are called REDOX REACTIONS

OILRIG – Oxidation Is Loss of electrons

Reduction Is Gain of electrons

Purifying Aluminium

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Aluminium has to be extracted from its ore (called ________) by electrolysis. This is because aluminium is very ___________. The ore is mixed with cryolite to lower its ________ ________. The ore is then melted so that the ions can ______. The positively charged aluminium ions gather at the ___________ electrode. Oxygen forms at the positive electrode and causes it to wear away, which means that they have to be __________ frequently.

Words – melting point, replaced, negative, bauxite, reactive, move

Purifying Copper

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Solution containing copper ions

Rusting Experiment

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RUST

NO RUST – no water

NO RUST – no oxygen

Rusting

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Rust is formed when iron reacts with water AND _____. It’s an example of an oxidation reaction which can be sped up using _____. There are several ways of dealing with rust:

1. Regular _______ or oiling
2. Galvanising – this is when iron objects are coated with ______
3. Making objects out of a non-rusting metal, such as ________ _______
4. Attaching zinc bars to ships – the water will react with the zinc before it reacts with the iron, because zinc is more ______

Words – stainless steel, reactive, painting, oxygen, salt, zinc

Quiz on acids and alkalis

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1. This a pH of less than 7
2. This could kill cells
3. A metal hydroxide (e.g. sodium hydroxide) would be an _____
4. When this reacts with a metal hydrogen is released
5. A metal carbonate (e.g. calcium carbonate) would be an _____
6. This would feel soapy on your skin
7. This could be a corrosive
8. This will turn universal indicator purple
9. This would taste sour
10. This means “a base that can be dissolved”

Acid, alkali or both???

Universal Indicator and the pH scale

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Universal Indicator is a mixture of liquids that will produce a range of colours to show how strong the acid or alkali is:

Stomach acid

Lemon juice

Water

Soap

Oven cleaner

Baking powder

An acid contains hydrogen ions, H⁺

An alkali contains hydroxide ions, OH^-

Neutralisation reactions

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When acids and alkalis react together they will NEUTRALISE each other:

OH

Sodium hydroxide

Cl

Hydrochloric acid

Neutralisation experiment

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In this experiment we mixed sodium hydroxide (an _____) and hydrochloric acid together and they ________ each other. The equation for this reaction is…

Words – nitrate, neutralised, alkali, sulphate, salt, evaporating

A ____ was formed during the reaction, and we could have separated this by __________ the solution. The salt that we formed depended on the acid:

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• Hydrochloric acid will make a CHLORIDE
• Nitric acid will make a _________
• Sulphuric acid will make a _________

Making salts

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Whenever an acid and alkali neutralise each other we are left with a salt, like a chloride or a sulphate. Complete the following table:

Salts of transition metals

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These are the TRANSITION METALS – if we make a salt using a base made from one of these metals the procedure is different…

1) Drop the base into the acid…

2) Filter it to remove any leftover base

3) Evaporate it to get the salt