Page 1

E1 1. a. Good electrical conductor, good thermal conductor, can be made into wires b. Breaks easily brital, melts above 25째C 2. a. Copper is used in electrical wiring because it conducts electricity very well b. Mercury is used in thermometers because it expands a lot when it is heated c. Gold is used for jewelry because it look attractive and does not tarnish d. Aluminum is used for drink cans because it can be easily pressed in shape 3.

a. b. Steel, zinc would work. 4. a.

All atoms in a tin have the same number of protons: if 50 atoms are neutral then they have 50 electrons. Due to the difference in the isotopes they don't have the same number of neutrons.

b.

2

5. a. i. Mercury ii. Tungsten b. Ability to withstand high temperatures and it does not melt even when it is glowing. c. Mercury is a liquid form when exposed at room temperatures, Lead is a solid at room temperature. d. i.

Tungsten


ii. E2

It has the highest boiling point

1. a. Acid + base  salt+ water b. Sulphuric acid+ magnesium oxide--> magnesium sulphate + water 2. a. i. True ii. False iii. False iv. True b.

Neutralization is a chemical reaction

3. a.

b.

i.

Zinc oxide+ sulphuric acid  zinc sulphate

ii.

Potassium hydroxide+ hydrochloric acid  potassium chloride

iii.

Iron hydroxide+ sulphuric acid  iron sulfate

water

c. i.

Sulphuric acid+ potassium hydroxide  potassium sulphate + water

ii.

7

iii.

neturlization

4. a. i.

6

ii.

3

i.

Copper oxide or

b.

ii. Copper oxide+ sulphuric acid  copper sulphate +water c.


E3 1. a.

Cloudiness in the tube and bubbles

b. i.

The squeaky pop test

ii. The solution would turn cloudy iii. Hydrogen is a gas which creates the cloudy effect as the bubbles rise towards the surface.

c. Magnesium+ hydrochloric acid  P. 46 – 47; 54. This is the experiment that you had done in the lab (p. 54) !!!!!!!!! d.

T would probably not react (Why not?)

a.

Chromium

2.

b. i. Chromium sulphate and water will be produced. ii.

Chromium oxide + sulphuric acid  Chromium sulphate + water

i.

Hydrochloric acid

ii.

hydrogen

iii.

Hydrogen is explosive

c.

d. i.

Acids react with chromium (metal + acid  salt +hydrogen)

ii.

corrosion

3. a.

Aluminium reacts with oxygen in the air forming a layer of aluminum oxide. This layer protects the alunium from corrosion by acid.

b. i.

The mecury chloride solution removes the aluminum oxide layer therefore unprotecting the alunium underneath.

ii.

It would beome alumin sulphate.


iii.

Alunium +sulphuric acid  aluminum sulphate +hydrogen

4. a. 8 b. 2

E4 1. a. Hydrogen gas b.

Metal carbonates produce carbon dioxide which does not make a pop sound when a splint is lighted nearby.

c. i.

By using an Indicator or PH meter.

ii.

Carbon dioxide would be produced.

d. Zinc carbonate + sulphuric acid  zinc sulphate + carbon dioxide + water e. Heat + color change 2. a.

i.

Water, carbon dioxide and sodium citrate

ii. Citric Acid + Sodium Hydrogencarbonate> Sodium Citrate + Water + Carbon Dioxide

b.

Because it is dry inside the sweet!

c.

Because carbon dioxide is not an appropriate fuel for the fire. For a fire you would need oxygen instead.

a.

Stomach acid is caused by stimulation of the parietal cells.

b.

It helps neutralize the acids by using calcium carbonate.

c.

Hydrochloric acid + calcium carbonate  calcium chloride + water + carbon dioxide

3.

4. a. because it neturlize the acid therefore reducing the acidity. b.


i. calcium carbonate + sulphuric acid  calcium suplate + water + carbon dioxide ii. sodium carbonate + sulphuric acid  sodium sulphate + water + carbon dioxide c. i. Too much would lead to an excess of alkaline. ii.

E5 1. a. When a metal oxide react with an acid it creates water. When a metal oxide react with an acid it creates salt. b. A salt appered, colour change c. i.

Zinc nitrate+ water

ii.

Hydrochloric acid + water

iii.

Zinc oxide + water

2. Calcium sulphate  setting broken bones Copper sulphate controlling diesies on grapevines Sodium chloride  flavoring or preserving food (also P. 44) Espom salts as a laxative Sodium chloride  clearing snow and ice from roads

3. a.

Color change to pink

b. i.

It would neutralize

ii.

Because it contains an acid and a base so it become neutralized.

c. Cobalt sulphate 4. a.

Iron Oxide + sulfuric acid.-->Iron sulphate + water

b.

Feo+H2SO4FEso4+H2O

c.

It comes from the iron oxide and sulphuric acid


d. i.

7

ii.

4

e. Hydrochloric acid

F1 1. a. Form change and color change b. oxygen c. magnesium oxide d. magnesium + oxygenďƒ magnesium oxide e. It is not as reactive f.

Potassium.

2. a. i.

Iron is more reactive

ii.

It does not tarnish that easily

iii. Iron b.

sodium

c.

Silver is more reactive

d. Iron + oxygen ďƒ haematite e. i.

Sodium is kept under oil in a tightly sealed container because it will not tarnish that way.

ii.

Platinum used for jewelry does not tarnish because it is not as reactive

3. a.

She poured water on the magnesium

b.

It generates a lot of energy

c. i. It would not have exploded if she had poured water on it


ii. Because it has less energy d.

There was a lot of energy in the magnesium

e.

It cut out the oxygen

4. a.

P. 52-53

b.

P. 52 (a)

a.

When potassium reacts with water

b.

When calcium reacts with hydrochloric acid

c.

It is dangerous to react potassium with acid because

d.

Acids can be used to mark decorations onto glass because

F2 1.

Calcium chloridie and hydrogen are formed. Acids are corrosive. It forms hydrogen gas, which contacts fire. Acids give stronger reactions with metals than water.

2. a.

Na + H2O

b.

Magnesium + sulphuric acid → ___________ _______________________ + Hydrogen (P. 54,)

3. a. i.

P. 52

ii.

P. 52

i.

P. 46; 47

ii.

P. 46, 47

b.

c.

P. 46, 47

d. i.

P. 56, 58

ii.

P. 56, 58


e.

P. 54

f.

P. 54

4. a. i.

P. 58

ii.

P. 54

iii.

P. 51

iv.

P. 51

i.

P. 46

ii.

P. 46

iii.

P. 46

b.

F3 1. a.

P. 56

b.

P. 56

a.

P. 56

b.

P. 56

a.

P. 57

b.

P. 57

c.

P. 57

2.

3.

d. i.

P. 56, 57

ii.

P. 56, 57

i.

P. 56, 57

4. a.


ii.

P. 56, 57

b.

P. 56, 57

c.

P. 56, 57

a.

P. 56, 57

b.

P. 56, 57

c.

P. 56, 57

d.

P. 56, 57

a.

P. 58-59

b.

P. 58-59

c.

P. 58-59

d.

P. 58-59

5.

F4 1.

2. a. i.

P. 58-59

ii. P. 58-59 b. 3. a. i. P. 58-59 ii.

P. 58-59

i.

P. 58-59

ii.

P. 58-59

i.

P. 58-59

ii.

P. 58-59

b.

c. d.


4. a.

P. 58-59

b.

P. 58-59

c.

P. 58-59 i. P. 58-59 ii.

P. 58-59

iii.

P. 58-59

F5 p. 60 – 61 1. a. i. ii. b. i. ii. c. i. ii. 2. a. b. c. d. e. i. ii. f. i. ii.


3. a. i. ii. iii. iv. v. b. i. ii. iii.

E1 (dec 25 13)