Download N4 - whitburnscience

National 4 & 5 Chemistry
NATIONAL 4 AND NATIONAL 5 CHEMISTRY
Unit 1: Chemical Changes and Structure
WRITING CHEMICAL
FORMULAE
(INCLUDING – IONIC FORMULAE)
PRACTICE EXAMPLES BOOKLET
Page 1 of 17
National 4 & 5 Chemistry
N4
ELEMENT FORMULAE
N4
In your jotter, write the formulae of the following elements. Present the information in a table
with the headings “ELEMENT” and “FORMULA.”
carbon
aluminium
lithium
oxygen
chromium
tungsten
hydrogen
germanium xenon
nitrogen
silicon
radon
chlorine
arsenic
bromine
cobalt
titanium
zirconium
silver
N4
radium
- IDE COMPOUNDS 1
N4
In your jotter, name the elements in the following compounds. Present the information in a
table with the headings “COMPOUND NAME” and “ELEMENTS PRESENT.”
N4
potassium oxide
sodium chloride
magnesium sulphide
aluminium bromide
calcium carbide
hydrogen iodide
silicon oxide
lithium phosphide
copper fluoride
magnesium nitride
mercury oxide
sodium silicide
- IDE COMPOUNDS 2
In your jotter, name the following compounds. Present the information in a table with the
headings “FORMULA” and “COMPOUND NAME.”
MgCl2
CaF2
CuO
Al2O3
K2O
K3N
NH3
H2S
PI3
PbBr4
Na2O
LiI
Fe2S3
MnO2
AuCl3
SiBr4
Page 2 of 17
N4
National 4 & 5 Chemistry
N4
-ATE & -ITE COMPOUNDS
N4
In your jotter, name the elements in following compounds. Present the information in a table
with the headings “COMPOUND NAME” and “ELEMENTS PRESENT.”
sodium sulphate
aluminium nitrate
calcium carbonate
cobalt phosphate
tin sulphite
lead chlorate
silver nitrite
mercury bromate
aluminium silicate
copper carbonate
nickel chromate
barium iodate
N4
1.
VALENCY DIAGRAMS
Draw the valency picture of the following atoms.
potassium
2.
N4
N4
carbon
fluorine
oxygen
barium
Draw the valency diagram and write the formula of the following compounds.
potassium oxide
sodium chloride
magnesium oxide
aluminium bromide
calcium carbide
aluminium sulphide
silicon oxide
lithium phosphide
nitrogen fluoride
hydrogen oxide
carbon hydride
sodium silicide
FORMULAE OF -IDE COMPOUNDS
Use the short cut method to write the formulae of the following compounds.
lithium fluoride
beryllium sulphide
aluminium nitride
rubidium oxide
sulphur chloride
boron oxide
phosphorus hydride
carbon oxide
aluminium sulphide
nitrogen iodide
silicon nitride
magnesium carbide
sodium hydride
barium chloride
germanium bromide
Page 3 of 17
N4
National 4 & 5 Chemistry
N4
RULE BREAKING FORMULAE
N4
Write the formulae of the following compounds.
nitrogen dioxide
phosphorus tribromide
chlorine trifluoride
manganese dioxide
dinitrogen oxide
sulphur dioxide
phosphorus pentachloride
silicon tetrabromide
nitrogen triiodide
N5
FORMULAE WITH GROUPS 1
N5
Draw the valency diagram and write the formula of the following compounds.
ammonium fluoride
calcium sulphate
aluminium phosphate
lithium carbonate
potassium hydroxide
sodium sulphate
ammonium hydroxide
potassium nitrate
rubidium phosphate
N5
FORMULAE WITH GROUPS 2
N5
Use the table of “Formulae Of Selected Ions Containing More Than One Atom” to write the
formulae of the following compounds.
ammonium nitrate
calcium chromate
potassium permanganate
sodium hydrogencarbonate
lithium dichromate
rubidium hydrogensulphate
ammonium ethanoate
potassium sulphite
hydrogen phosphate
caesium hydroxide
magnesium carbonate
barium dichromate
Page 4 of 17
National 4 & 5 Chemistry
N5
ROMAN NUMERAL FORMULAE 1
N5
Write the formulae of the following transition metal compounds.
You will need to use the “Formulae Of Selected Ions Containing More Than One Atom” to
write the formula of some of the compounds.
copper(II) oxide
nickel(II) chloride
gold(I) nitrate
iron(II) carbonate
silver(I) hydroxide
mercury(I) sulphate
zinc(II) sulphide
platinum(II) fluoride
cobalt(III) phosphate
manganese(IV) oxide
chromium(III) bromide
vanadium(V) oxide
titanium(II) sulphite
iron(III) phosphate
scandium(III) chloride
N5
ROMAN NUMERAL FORMULAE 2
Write the formulae of the following compounds.
zinc chloride
lead(II) sulphate
tin(IV) chloride
lead(II) sulphide
zinc carbonate
silver nitrate
ammonium bromide
nickel(III) fluoride
tin(IV) oxide
lead(II) chromate
mercury(II) iodide
magnesium sulphite
zinc dichromate
silver permanganate
tin(II) phosphide
sodium ethanoate
ammonium hydroxide
zinc sulphite
lead(IV) oxide
titanium(IV) chloride
vanadium(V) iodide
Page 5 of 17
N5
National 4 & 5 Chemistry
N5
REMOVING BRACKETS
N5
Write the formulae of the following compounds.
copper(II) carbonate
potassium ethanoate
sodium permanganate
mercury(II) dichromate
silver hydroxide
ammonium fluoride
lithium phosphate
barium sulphate
caesium hydrogencarbonate
nickel(II) chromate
cobalt(III) phosphate
gold(II) carbonate
N5
FORMULAE WITH GROUPS 3
N5
Write the formulae of the following compounds.
calcium nitrate
ammonium carbonate
aluminium sulphate
zinc hydroxide
iron(III) sulphite
copper(II) hydroxide
ammonium phosphate
lead(II) nitrate
gold(III) hydrogensulphate
silver chromate
tin(II) phosphate
barium permanganate
magnesium hydroxide
cobalt(II) phosphate
ammonium dichromate
tin(IV) hydrogencarbonate
manganese(IV) carbonate
nickel(II) hydroxide
lithium chromate
lead(IV) sulphite
ammonium phosphate
N5
IONIC FORMULAE 1
Write the ionic formulae of the following compounds.
sodium chloride
calcium oxide
aluminium bromide
potassium sulphide
nickel(II) chloride
iron(III) oxide
sodium phosphide
aluminium oxide
silver oxide
barium sulphide
copper(II) iodide
lead(II) chloride
tin(II) chloride
cobalt(III) sulphide
manganese(IV) oxide
calcium nitride
zinc chloride
magnesium carbide
Page 6 of 17
N5
National 4 & 5 Chemistry
N5
IONIC FORMULAE 2
Write the ionic formulae of the following compounds.
iron(II) carbonate
aluminium sulphate
sodium phosphate
barium hydroxide
copper(II) sulphite
potassium permanganate
calcium ethanoate
ammonium dichromate
zinc hydrogencarbonate
lead(II) hydroxide
silver chromate
ammonium chloride
tin(IV) phosphate
mercury(II) nitrate
ammonium phosphate
Page 7 of 17
N5
National 4 & 5 Chemistry
NATIONAL 4 AND NATIONAL 5 CHEMISTRY
Unit 1: Chemical Changes and Structure
BALANCING
EQUATIONS
PRACTICE EXAMPLES BOOKLET
Rules
1. Can’t change
formula
2. Can change
quantity.
Page 8 of 17
National 4 & 5 Chemistry
N5
BALANCING EQUATIONS 1
N5
In your Jotter balance the following chemical equations using the ‘check table to help you’:
1) Zn +
HCl
Left

ZnCl2 + H2
3) CaO
 CaCl2 + H2O
Right
Ca
O
H
Cl
2) Na + H2SO4  Na2SO4 + H2
4) Al
+
Fe2O3
 Al2O3 + Fe
Right
Na
H
S
O
N5
HCl
Left
Right
Zn
H
Cl
Left
+
Left
Right
Al
Fe
O
BALANCING EQUATIONS 2
In your jotter balance the following chemical equations:
Page 9 of 17
N5
National 4 & 5 Chemistry
NATIONAL 4 AND NATIONAL 5 CHEMISTRY
Unit 1: Chemical Changes and Structure
FORMULA MASS
PRACTICE EXAMPLES BOOKLET
RELATIVE ATOMIC MASS
The average mass of an atom is called the RELATIVE ATOMIC MASS. The relative atomic
mass of selected elements is listed in the chemistry data booklet.
ATOM
RELATIVE
ATOMIC MASS
H
1
hydrogen
O
16
oxygen
Cl
35.5
chlorine
MASS OF A FORMULA
The total mass of all the atoms in a formula is called the FORMULA MASS.
oxygen gas
(O2)
O
O
1
32
Cl
35.5
16
1
O
H
H
FORMULA
MASS
12
water
(H2O)
16
R A M 16
carbon chloride
(CCl4) 35.5
Cl
C
Cl
Cl
35.5
Page 10 of 17
18
35.5
154
National 4 & 5 Chemistry
N4
FORMULA MASS
N4
Calculate the formula mass of each of the following :
1.
chlorine [Cl2]
2. hexane [C6H14]
3.
magnesium hydroxide [Mg(OH)2]
4.
5.
aluminium carbonate [Al2(CO3)3]
6. Calcium Carbonate [CaCO3]
ammonium phosphate [(NH4)3PO4]
Calculate the formula and then the formula mass of each of the following :
7.
Oxygen
8. Hydrogen
9.
Lithium Nitride
10. Sodium hydride
11. lithium carbonate
N5
12. Copper (ii) sulphate
GRAM FORMULA MASS
N5
1.
oxygen [O2]
2. sucrose [C12H22O11]
3.
calcium carbonate [CaCO3]
4. iron(III) sulphate [Fe2(SO4)3]
5.
ammonium nitrate [NH4NO3]
6. Ammonium carbonate [(NH4)2CO3]
Calculate the formula and then the gram formula mass of each of the following :
7.
Nitrogen
9.
Calcium Chloride
11. ammonium phosphate
8.
Bromine
10. Aluminium Oxide
12. Calcium nitrite
Page 11 of 17
National 4 & 5 Chemistry
NATIONAL 4 AND NATIONAL 5 CHEMISTRY
Unit 1: Chemical Changes and Structure
THE MOLE
Page 12 of 17
National 4 & 5 Chemistry
N5
GRAM FORMULA MASS IS ONE MOLE
N5
Calculate the mass of 1 mole of each of the following compounds:
1. Hydrogen
4. Sulfur dioxide
7. Calcium carbonate
N5
2. Nitrogen monoxide
5. Carbon hydride
8. Magnesium nitrate
3. Sodium chloride
6. Potassium permanganate
9. Lithium hydroxide
MOLES TO MASS CALCULATION
N5
Calculate the mass (m) of each of the following:
1.
2.
3.
4.
5.
6.
7.
N5
2 moles of iron [Fe]
0.1 mole of nitrogen [N2]
1.5 moles of sodium oxide [Na2O]
0.75 moles of zinc nitrate [Zn(NO3)2]
4.7 moles of sodium hydroxide [NaOH]
0.125 mole silver(I) nitrate [AgNO3]
4 mole of butane [C4H10].
MASS TO MOLES CALCULATION
Calculate the number of moles (n) in :
1.
2.
3.
4.
5.
6.
7.
8.
28 g of silicon [Si]
40 g of bromine [Br2]
36 g of water [H2O]
33.3 g of calcium chloride [CaCl2]
456.25 g of nickel(II) nitrate [Ni(NO3)2]
6 g of water [H2O] .
6.4g of oxygen [O2] .
693 g of ammonium sulphate [(NH4)2SO4]
Page 13 of 17
N5
National 4 & 5 Chemistry
N5
1.
THE MOLE AND REACTION QUANTITIES (MOLE RATIO)
N5
The balanced equation below shows the reaction between silicon and chlorine producing
silicon chloride.
Si
+
2Cl2
SiCl4
Calculate the number of moles of chlorine required to make 5 mole of silicon chloride.
2.
The balanced equation for the combustion of butane, C4H10, is shown below.
2 C4H10
+
13 O2
8 CO2
+
10H2O
Calculate the number of moles of oxygen required to burn 0.5 mole of butane, C4H10.
3.
The balanced equation for the reaction between zinc and silver nitrate is shown below.
Zn
+
2 AgNO3
Zn(NO3)2
+
2 Ag
Calculate the number of moles of zinc required to produce 12 mole of silver.
4.
The balanced equation for the reaction between magnesium oxide and phosphoric acid
is shown below.
3 MgO
+
2 H3PO4
Mg3(PO4)2
+
3 H2O
Calculate the number of moles of magnesium oxide, MgO, required to make 2.5 mole of
magnesium phosphate, Mg3(PO4)2.
5.
The balanced equation below shows the reaction between aluminium and iodine
producing aluminium iodide.
2 Al
+
3 I2
2 AlI3
Calculate the number of moles of iodine, which reacts with 0.25 mole of aluminium.
Page 14 of 17
National 4 & 5 Chemistry
N5
1.
MOLE RATIO & MASSES
N5
Calcium reacts with chlorine to form calcium chloride as shown by the following
balanced equation.
Ca
+

Cl2
CaCl2
Calculate the mass of chlorine, which will react, with 10 g of calcium.
2.
Sodium reacts with water to form sodium hydroxide and hydrogen gas. The balanced
equation for the reaction is shown below.
2 Na
+

2 H2O
2 NaOH
+
H2
Calculate the mass of sodium hydroxide produced when 9.2 g of sodium is reacted with
water.
3.
Zinc reacts with nitric acid to produce zinc(II) nitrate and hydrogen gas. . The balanced
equation for the reaction is shown below.
Zn
+

2 HNO3
Zn(NO3)2
+
H2
Calculate the mass of zinc required to produce 75.6 g of zinc(II) nitrate when zinc is
reacted with nitric acid.
4.
Copper(II) oxide reacts with hydrochloric acid to produce copper(II) chloride and water .
The equation for the reaction is shown below.
CuO
(a)
+

HCl
CuCl2
+
H2O
Copy and balance the equation.
(b) Calculate the mass of copper(II) chloride produced when 201.25 kg of copper(II)
oxide is reacted with hydrochloric acid.
Page 15 of 17
National 4 & 5 Chemistry
5.
The alcohol called methanol (CH3OH) is produced in industry by reacting hydrogen with
carbon monoxide. The equation for the reaction is shown below.
CO
+
H2

CH3OH
The manufacturer has an order for 800 tonnes of methanol (CH3OH).
(a)
Copy and balance the equation.
(b) Calculate the mass of carbon monoxide required to make 800 tonnes of methanol.
(c)
Calculate the mass of hydrogen required to make 800 tonnes of methanol.
Page 16 of 17
National 4 & 5 Chemistry
N5
MOLE CALCULATIONS INVOLVING SOLUTIONS
N5
Calculate the concentration of the following solutions.
1.
2.
3.
4.
5.
0.5 mole of sodium chloride in 500 cm3 of solution.
2 mole of nitric acid in 4000 cm3 of solution.
0.25 mole of potassium carbonate in 200 cm3 of solution.
1.5 mole of nickel(II) sulphate in 3 litres of solution.
0.05 mole of lithium bromide in 50 cm3 of solution.
Calculate the number of moles of solute in the following solutions.
1.
2.
3.
4.
5.
N5
200 cm3 of a 2 mol l -1 solution of potassium hydroxide.
1800 cm3 of a 0.25 mol l -1 solution of cobalt(II) chloride.
75 cm3 of a 0.5 mol l -1 solution of phosphoric acid.
2 litres of a 0.4 mol l -1 solution of zinc nitrate.
750 cm3 of a 3 mol l -1 solution of copper(II) chloride.
MOLE CALCULATIONS INVOLVING SOLUTIONS & MASSES
Calculate the mass of compound in the following solutions.
1.
2.
3.
4.
5.
500 cm3 of a 2 mol l -1 solution of potassium carbonate (K2CO3).
2500 cm3 of a 0.2 mol l -1 solution of copper(II) chloride (CuCl2).
100 cm3 of a 0.5 mol l -1 solution of sulphuric acid (H2SO4).
2 litres of a 0.4 mol l -1 solution of potassium nitrate (KNO3).
250 cm3 of a 1.5 mol l -1 solution of tin(II) sulphate (SnSO4).
Calculate the concentration of the following solutions.
1.
2.
3.
4.
5.
7.975 g of copper(II) sulphate [CuSO4] in 100 cm3 of solution.
5 g of sodium hydroxide [NaOH] in 500 cm3 of solution.
273 g of zinc chloride [ZnCl2] in 1500 cm3 of solution.
37.125 g of magnesium nitrate [Mg(NO3)2] in 400 cm3 of solution.
59.6 g of ammonium phosphate [(NH4)3PO4] in 2 litres of solution.
Page 17 of 17
N5