CHEMISTRY        UNITS 3 and 4
PRETEST    DATA PAGE
Use the data tables below and the periodic table over the page to help you answer the pre-test questions.
Table 1: Formulae and charge of selected ions:
Cations
Anions
Na+  sodium
OH   hydroxide
NH4+ ammonium
Cl   chloride
Ag+  silver
NO3   nitrate
Mg2+  magnesium
O2   oxide
Zn2+  zinc
SO42   sulfate
Cu2+  copper
CO32   carbonate
Pb2+  lead
PO43   phosphate
Table 2: Solubility of ions in water:
Ions that are soluble in water
Compounds with the following ions are always soluble in water
Ammonium NH4+ 
Sodium  Na+ 
Potassium K+ 
Nitrate  NO3
Compounds with the following ions are mostly soluble in water
Chloride Cl   except with silver, Ag+, or lead, Pb2+
Sulfate SOreaction mass42   except with silver, Ag+, or lead, Pb2+
Ions that are not soluble in water
Compounds with the following ions are mostly not soluble in water
Hydroxide OH
Sulfide S2  
Carbonate CO32  
Phosphate PO43  
except with
Ammonium NH4+  Sodium  Na+ 
Potassium K+ 
Table 3: Molar mass of selected elements:
Element
H
C
O
Ne
Na
Cl
Pb
Molar mass (g per mol)
1.0
12.0
16.0
20.1
23.0
35.5
207.2
Table 4: Molar mass of gases
STP standard temperature and pressure
temperature 0°C, pressure 101.3 kPa
SLC standard laboratory conditions
  temperature 25°C, pressure 101.3 kPa
One mol of any gas occupies 22.4 litres at STP
One mol of any gas occupies 24.5 litres at SLC
CHEMISTRY        UNITS 3 and 4
PRETEST QUESTIONS
1.
Use the Periodic Table given on the previous page to help you answer the following questions.
(a)
What is the atomic number of the following elements
(i)    silver
(ii)    radon
(iii)    radium
½ + ½ + ½ = 1½ marks
(b)
What is the chemical symbol of the following elements
(i)    gold
(ii)    silicon
(iii)    sodium
(iv)    antimony
½ + ½ + ½ + ½ = 2 marks
(c)
Identify the element with 13 protons and 13 neutrons.
1 mark
2.
Butane, C4H10 is commonly used in LPG and lighter fluid. It’s melting and boiling points are shown below.
melting point/ freezing (solidification) point
138 ºC
boiling (evaporation) point/ condensation point
0.5 ºC
Circle the physical state of butane
at room temperature, 25 C
  solid          liquid      gas
at fridge temperature, 4 C
  solid          liquid      gas
at 5 C
  solid          liquid      gas
½ + ½ + ½ = 1½  marks
Use the table of ions (Table 1) on the data page to help you answer questions 3 and 4.
3.
Identify the ions present in the following ionic compounds and name the compound.
(a)    MgCl2
(b)    Na3PO4
(c)    Ag2S
3 marks
4.
Work out the chemical formula of the following compounds.
(a)  Silver hydroxide
(b)  Magnesium carbonate
(c)  Zinc nitrate
3 marks
5.
Balance the following chemical equations.
(a)    Mg(s)  +  N2(g)    Mg3N2(s)
(b)    Ca(S)  +  O2(g)    CaO(s)
(c)    H2(g)  +  O2(g) H2O(l)
(d)    Al (s) +  I2 (l)  Al2I6(s)
4 marks
Pre-test questions continued…
6.
Use the solubility table (Table 2) on the data page to determine which of the following ionic compound are soluble.
(a)    lead sulfate
(b)    silver chloride
(c)    ammonium chloride
(d)    zinc carbonate
½ + ½ + ½ + ½ = 2 marks
7.
The compound Cu(NO3)2 dissolves in water by dissociation  of ions
(a)
Identify the ions in the compound.
(b)
Write the ionic equation of the dissociation reaction. Show the state of each compound or ion.
1 + 2 = 3 marks
Refer to the molar mass of elements (Table 3) on the data page to help you answer questions 8, 9 and 10.
8.
Find the molar mass of the following compounds
(a)    H2O
(b)    NaCl
2 marks
9.
Find the mass of 1.3 mol of CH4
1 mark
10.
Calculate the number of mol contained in the following samples, rounded to three decimal places.
(a)    50 g of lead
(b)    62 g of NaCl
2 marks
Refer to the molar volume of gases (Table 4) on the data page to help you answer the follo
wing question.
11.
(a)
Work out the volume of 1.4 mol of chlorine (Cl2) at STP
(b)
Work out the mass of 2.8 L of neon (Ne) gas at SLC
1 + 1 = 2 marks
The table below summarises the different types of acid reactions:
Reactions of acids
The chemical formulae of selected compounds.
1. acid + metal   salt + hydrogen
  This reaction does not occur with Cu, Hg, or Ag.
2. acid + metal carbonate
      salt + water + carbon dioxide
3. acid + metal oxide   salt + water
4. acid + metal hydroxide   salt + water
HCl (aq)
Na2CO3 (aq)
NaCl (aq)
H2O (l)
CO2 (g)
CuO (s)
CuCl2 (aq)
H2O (l)
H2SO4 (aq)
NaOH (aq)
Na2SO4 (aq)
    Carbonates contain the CO32 ion

Pre-test questions continued…
12.
Use the summary of acid reactions shown above to predict the products of the following reactions:
(a)
HCl (aq) + Mg (s)   
(b)
HCl (aq) + Na2CO3 (aq) 
(c)
HCl (aq) + CuO (s) 
(d)
H2SO4 (aq) + NaOH (aq) 
1 + 1 + 1 + 1 = 4 marks
13.
Are the following reactions oxidation or reduction reactions?
(a)
Cl2(g)  +  2e     2Cl (aq)
(b)
Pb (s)    Pb2+ (aq) +  2e    
½ + ½ = 1 mark
14.
The reaction Zn(s)  + S(s)    ZnS (aq) can be written as two half reactions:
        Zn(s)    Zn2+(aq)  +  2e   and S(s)  +  2e     S2  (aq)
(a)
Identify the oxidant in this redox reaction   
(d)
Identify the reductant in this redox reaction   
½ + ½ = 1 mark
15.
Iron reacts with hydrochloric acid according to the ionic equation
Fe(s)  +  2H+(aq)  Fe2+(aq) + H2(g)
(a)
What has been oxidised in this reaction?
(b)
Write a half equation for the oxidation reaction.
(d)
What has been reduced in this reaction?
(e)
Write a half equation for the reduction reaction.
½ + 1 + ½ + 1 = 3 marks

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