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chemistry UNIT 2

Total questions: 140

Worksheet time: 2hrs 58mins

Name
Class
Date
1.

Which alkali metal has the electron configuration 2.8.1

a)

Sodium

b)

Potassium

c)

Lithium

d)

Rubidium

2.

Which alkali metal is most reactive out of the following

a)

rubidium

b)

potassium

c)

sodium

d)

lithium

3.

How many electrons do the alkali metals have in their outer shell?

a)

1

b)

2

c)

8

d)

7

4.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

5.

Group IA has 7 elements member, but for Alkali only has 6 elements member

a)

Incorrect

b)

Correct

6.

Which alkali metal is most reactive out of the following

a)

rubidium

b)

potassium

c)

sodium

d)

lithium

7.

How many electrons do the alkali metals have in their outer shell?

a)

1

b)

2

c)

8

d)

7

8.

What happens to the atomic radius of the alkali metals as you move down the group?

a)

increase

b)

decrease

9.

Which alkali metal has the symbol Cs

a)

Caesium

b)

Ceasium

c)

Calcium

d)

Sodium

10.

Is hydrogen an alkali metal?

a)

no

b)

yes

c)

maybe

11.

What happens to the melting point of the alkali metals as you move down the group?

a)

decreases

b)

increases

12.

Which gas is released when the alkali metals react with water?

a)

hydrogen

b)

oxygen

c)

hydroxide

d)

carbon dioxide

13.

How does a group 1 metal atom form an ion?

a)

lose 1 electron

b)

lose 2 electrons

c)

gain 1 electron

d)

gain 2 electrons

14.

What is the charge of a group 1 metal ion?

a)

1+

b)

2+

c)

1-

d)

2-

15.

Which of the following is NOT a property of group 1 metals?

a)

More dense than water

b)

less dense than water

c)

low melting point

d)

soft

16.
Which is not a Alkali Metal?
a)
Lithium
b)
Sodium
c)
Gold
d)
Potassium
17.
Which group are the Alkali Metals found? 
a)
Group 1
b)
Group 6
c)
Group 18
d)
Group 13
18.
Alkali are so reactive to air they are generally stored in what?
a)
Water
b)
Oil
c)
Vaults
d)
Cotton
19.

All of the following elements are alkali metals, except

a)

copper

b)

sodium

c)

potassium

d)

francium

e)

caesium

20.

What is the chemical symbol for potassium?

a)

P

b)

Po

c)

K

d)

Na

e)

Ca

21.

Why are the alkali metals so reactive?

a)

They are metals.

b)

They have 1 valence electron

c)

They are monatomic

d)

They are diatomic

e)

They have equal numbers of protons and electrons

22.

Which of these is the least electronegative?

a)

Lithium

b)

Rubidium

c)

Potassium

d)

Sodium

e)

Caesium

23.
WHICH GROUP ELEMENTS IN THE PERIODIC TABLE IS KNOWN AS ALKALI METALS?
a)
Group 3
b)
Group 2
c)
Group 1
d)
group 7
24.
Among the followings which one is not an alkali metal?
a)
Sodium
b)
Potassium
c)
Lithium
d)
hydrogen
25.
The least reactive alkali metal
a)
Ceasium
b)
Potassium
c)
Lithium
d)
Rubidium
26.
All alkali metals have ---------------  electrons in their outermost shell.
a)
1
b)
2
c)
3
d)
4
27.
All alkali metals have ---------------  electrons in their outermost shell.
a)
1
b)
2
c)
3
d)
4
28.
--------------------- is released when alkali metal react with water
a)
Hydrogen
b)
Oxygen
c)
Metahne
d)
Carbon di oxide
29.

Chlorine compounds show oxidation states ranging from –1 to +7. What are the reagent(s) and conditions necessary for the oxidation of elemental chlorine into a compound containing chlorine in the +5 oxidation state?

a)

AgNO3(aq) followed by NH3(aq) at room temperature

b)

concentrated H2SO4 at room temperature

c)

cold dilute NaOH(aq)

d)

hot concentrated NaOH(aq)

30.

which statement is true about halogens?

a)

form covalent compounds with other non-metallic elements

b)

A less reactive halogen will displace a more reactive element form its ionic salt

c)

Form ionic compound with hydrogen

d)

form negative ion of charge -2

31.

which one is used in the manufacture of bleaches

a)

Hydrochloric caid

b)

sodium hydroxide

c)

silver iodide

d)

hydrogen

32.

Which one does NOT represent a possible reaction?

a)

fluorine + sodium chloride ==> sodium fluoride + chlorine

b)

chlorine + sodium iodide ==> sodium chloride + iodine

c)

chlorine + potassium bromide ==> potassium chloride + bromine

d)

bromine + sodium chloride ==> sodium bromide + chlorine

33.

Which four numbers a, b, c and d are required to balance the equation?

a Cl2(aq) + b KI(aq) ==> c KCl(aq) + d I2(aq)

a)

2 1 1 2

b)

1 2 2 1

c)

2 1 2 1

d)

1 2 1 2

34.

which property of halogens increases from fluorine to iodine

a)

electronegativity of elements

b)

oxidizing power of elements

c)

bond length in the halogen molecule

d)

First ionization energy

35.

The given table shows the results obtained when the halogens X2, Y2 and Z2 were added to separate aqueous solutions containing X-, Y- and Z-. which set correctly shows the strength (strongest first) of the ions X-, Y- and Z- as reducing agents?

a)

X- Y- , Z-

b)

X-, Z-, Y-

c)

Y-, Z-, X-

d)

Z-, X-, Y-,

36.

silver nitrate is added to an aqueous solution containing Br- to give a precipitate X, which is then tested for its solubility in concentrated ammonia. which of the following correctly describes the the colour of X and its solubility in ammonia.

a)

white insoluble

b)

cream slightly soluble

c)

white slightly soluble

d)

yellow insoluble

37.

An excess of aqueous solution of silver nitrate is added to an aqueous solution containing both potassium chloride and potassium bromide. the precipitate formed is the filtered off and washed with distilled water. The precipitate is then shaken with aqueous ammonia and filtered off again.which ion does the final filtrate contain?

a)

chloride

b)

silver

c)

iodide

d)

potassium

38.

Which property of halogen decreases down the group?

a)

Bond energy of the hydrogen halogen bond

b)

Thermal stability

c)

Boiling point

d)

Reducing ability of halides

39.

Which property of halogen decreases down the group?

a)

Bond energy of the hydrogen halogen bond

b)

Thermal stability

c)

Boiling point

d)

Reducing ability of halides

40.

In their elemental state, halogens exist as monoatomic molecules.

a)

True

b)

False

41.

The reactivity of halogens increases down the group.

a)

True

b)

False

42.

Halogens form negative ions.

a)

True

b)

False

43.

All halogens are gases.

a)

True

b)

False

44.

Halogens become darker in colour down the group.

a)

True

b)

False

45.

Halogens have 6 electrons in their outer shell.

a)

True

b)

False

46.

All noble gases have 8 electrons in their outer shell.

a)

True

b)

False

47.

The properties of noble gases made them difficult to discover.

a)

True

b)

False

48.
Cl
a)
chlorido
b)
Chlorine
49.
Bromine
a)
Bm
b)
Br
50.
Which is true about kinetic theory of gases?
a)
temperature determines the kinetic energy of particles
b)
particles lose energy when they collide with one another
c)
molar mass determines the kinetic energy of particles
d)
container size determines kinetic energy of the particle
51.
Particles in a gas 
a)
move in straight paths and random directions
b)
move in straight paths but always left to right
c)
move more slowly as heat is added to the container
d)
attract one another
52.
The energy of an object as it is in motion is defined as
a)
Kinetic Theory
b)
Kinetic energy
c)
Potential energy
d)
Electric energy
53.
Compressing a gas makes the pressure _______.
a)
increase
b)
decrease
c)
stay the same
d)
I don't know
54.
When you heat a gas, the particles' energy ________ . This causes the particles to _______________.
a)
increases, have fewer collisions
b)
increases, have more collisions
c)
decreases, have more collisions
d)
remain the same, have more collisions
55.
If I have a gas in a container, and I reduce the volume of the container, what happens to the pressure ?
a)
pressure increases as particles collide less
b)
pressure decreases as particles collide more
c)
pressure increases as particles collide more
d)
pressure will remain the same
56.
What pressure in mmHg is equal to 1.43 kPa?
a)
1.43 mmHg
b)
10.7 mmHg
c)
101.325 mmHg
d)
760 mmHg
57.
What pressure in kPa is equal to 2.65 atm?
a)
268 kPa
b)
0.0261 kPa
c)
39.0 kPa
d)
265 kPa
58.

Suppose you dissolve 0.435 g of KMnO4 in enough water to give 250. mL of solution. What is the concentration (M)?

a)

0.0110 M

b)

0.002753 M

c)

158 M

d)

1.74 M

e)

0.0000112

59.

If 0.10 mol of Copper (II) chloride is dissolved in enough water to make 2.0 L of solution, what is the Molarity and the number of grams of Copper (II) chloride dissolved in the solution?

a)

0.05 M, 13.45 g

b)

0.2 M, 1625 g

c)

0.05 M, 9.9 g

d)

0.2 M, 13.45 g

60.

What is the concentration of Sodium Carbonate when 25.3 g is dissolved to produce a 250. mL solution?

a)

0.955 M

b)

0.239 M

c)

1.91 M

d)

1.22 M

61.

If ammonium carbonate is reacted with copper (II) nitrate, which of the following would be the correct net ionic equation? (Carbonates are not very soluble)

a)

2NH4+ (aq) + CO32- (aq) --> (NH4)2CO3 (s)

b)

2NH4+ (aq) + 2NO3- (aq) --> 2NH4NO3 (s)

c)

CO32- (aq) + Cu2+ (aq) --> CuCO3 (s)

d)

Cu2+ (aq) + 2NO3- --> Cu(NO3)2 (s)

62.

If ammonium carbonate is reacted with copper (II) nitrate, which of the following would be the correct net ionic equation? (Carbonates are not very soluble)

a)

2NH4+ (aq) + CO32- (aq) --> (NH4)2CO3 (s)

b)

2NH4+ (aq) + 2NO3- (aq) --> 2NH4NO3 (s)

c)

CO32- (aq) + Cu2+ (aq) --> CuCO3 (s)

d)

Cu2+ (aq) + 2NO3- --> Cu(NO3)2 (s)

63.

If ammonium carbonate is reacted with copper (II) nitrate, which of the following would be the correct spectator ions (Carbonates are not very soluble)

a)

ammonium and carbonate

b)

ammonium and copper

c)

copper and nitrate

d)

ammonium and nitrate

e)

copper and carbonate

64.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
65.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
66.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
67.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
68.
NH4NO3
a)
soluble
b)
insoluble
69.
AgCl
a)
soluble
b)
insoluble
70.
K2SO4
a)
soluble
b)
insoluble
71.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
72.
Which of these lists contains only soluble substances?
a)
sodium nitrate, potassium chloride, calcium carbonate
b)
lead nitrate, lead chloride, lead sulfate
c)
calcium nitrate, copper chloride, ammonium phosphate
d)
silver nitrate, barium sulfate, copper carbonate
73.
What is the precipitate formed between potassium bromide and ammonium sulfide
a)
potassium sulfide
b)
ammonium bromide
c)
potassium ammonium
d)
no ppt is formed
74.
What is the name of the precipitate formed in the reaction of calcium sulfide and aluminum nitrate
a)
calcium nitrate
b)
aluminum sulfide
c)
no ppt is formed
d)
aluminum nitrate
75.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
76.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
77.

Will magnesium displace zinc sulfate?

a)

Yes

b)

No

78.

Fluorine is part of the reactivity series.

a)

True

b)

False

79.

Does copper react with dilute acid?

a)

No

b)

Yes

80.

Copper + Oxygen -->

a)

Copper Oxide

b)

Copper Oxate

c)

Oxygen Copperate

d)

Oxygen Coppide

81.

Which does NOT react with oxygen?

a)

Magnesium

b)

Calcium

c)

Potassium

d)

Lead

82.

Fe + HCl -->

a)

FeCl2 + H2

b)

2FeCl2 + H2

c)

FeCl2 +2H2

d)

FeHCl

83.

Metal + Hydrochloric acid -->

a)

Metal Chloride + Hydrogen

b)

Chlorine + Metal Hydrogen

c)

Chlorine Hydrogen + Metal

84.

Sulfate

a)

SO

b)

SO2

c)

SO3

d)

SO4

85.

Nitrate

a)

NO

b)

NO2

c)

NO3

d)

NO4

86.
Which metal is more reactive than calcium?
a)
magnesium
b)
potassium
c)
silver
d)
aluminum
87.

Which of the following is MOST reactive?

a)

Magnesium

b)

Lead

c)

Tin

d)

Copper

e)

Zinc

88.
Which of the following substances contain acid?
a)
An orange
b)
Bleach
c)
Distilled water
d)
Washing powder
89.
Which of the following substances contain an alkali?
a)
Baking powder
b)
Coca cola
c)
Distilled water
d)
Vinegar
90.
Which of the following pH numbers indicates a neutral substance?
a)
1
b)
5
c)
7
d)
14
91.
Which of the following pH numbers indicates a strong acid?
a)
1
b)
5
c)
7
d)
14
92.
Which of the following pH numbers indicate a strong alkali?
a)
1
b)
5
c)
7
d)
14
93.
Which of the following acids do we have in our stomach?
a)
Ethanoic acid
b)
Hydrochloric acid
c)
Nitric acid
d)
Sulphuric acid
94.
What colour is universal indicator in strong acid?
a)
Green
b)
Orange
c)
Purple
d)
Red
95.
What colour is universal indicator in a neutral solution?
a)
Green
b)
Orange
c)
Purple
d)
Red
96.
What colour is universal indicator in a strong alkali?
a)
Green
b)
Orange
c)
Purple
d)
Red
97.
Strong acids and strong alkalis are.......
a)
Able to turn blue litmus paper red
b)
Corrosive and/or caustic
c)
Sour
d)
Sweet
98.

Are common sodium and potassium salts soluble or insoluble in water?

a)

Soluble

b)

Insoluble

99.

Are nitrates soluble or insoluble in water?

a)

Soluble

b)

Insoluble

100.

Which of these form a precipitate when mixed?

a)

Ammonium nitrate and copper sulfate

b)

Potassium chloride and Sodium carbonate

c)

Copper sulfate and potassium chloride

d)

Ammonium nitrate and Sodium carbonate

e)

Copper sulfate and Sodium carbonate

101.

When copper oxide is added to hydrochloric acid, what happens to the copper atoms?

a)

They gain electrons

b)

Nothing

c)

They lose electrons

102.

Use the information in the table to explain why phenolphthalein is the same colour in a solution of hydrochloric acid as it is in pure water.

a)

HCl has pH greater than 7 so is the same as water (with neutral pH) in phenolphthalein

b)

HCl has pH neutral so is the same as water (with neutral pH) in phenolphthalein

c)

HCl has pH less than 7 so is the same as water (with neutral pH) in phenolphthalein

103.

Which indicator would be best to do a titration forming ammonium chloride? (ammonium chloride is acidic in solution)

a)

phenol red

b)

methyl orange

c)

phenolpthalein

d)

bromothymol blue

104.

Which of the following is the correct balanced ionic equation for the reaction between an acid and tin metal forming tin(IV) ions and hydrogen gas?

a)

Sn(s) + H+(aq) -> Sn4+(aq) + H2(g)

b)

Sn(s) + 2H+(aq) -> Sn4+(aq) + H2(g)

c)

Sn(s) + 4H+(aq) -> Sn4+(aq) + 2H2(g)

d)

2Sn(s) + 2H+(aq) -> 2Sn4+(aq) + H2(g)

105.

How many times greater is the concentration of acid ions in acid rain with a pH of 2 compared to the concentration of acid ions in natural rainwater with a pH of 5?

a)

3 times

b)

100 times

c)

10 times

d)

1000 times

106.

A group of students were asked to investigate a green solid and a clear solution. They were told that the solid contains a single metal compound, and the solution conducts electricity due to the presence of ions.

After some tests they noted the following:

● The green solid had a high melting point and was insoluble in water.

● The clear solution conducted electricity and formed chlorine gas during electrolysis.

● When the two substances were added together, the green solid disappeared, a colourless gas was formed and the solution turned bright blue. The gas formed in the reaction was found to extinguish a flame.


Suggest a name for the green solid.

a)

Copper Sulfate

b)

Iron Sulfate

c)

Copper Carbonate

d)

Iron Oxide

107.

The recommended quantity of calcium oxide required to cure most acidic soils is 280 g per square metre.


If a farmer has a field of acidic soil measuring 120 metres by 65 metres, calculate the mass of calcium oxide required for this field in kilograms. (1 kg = 1000 g.)

a)

2184

b)

2184000

c)

2.184

d)

21.84

108.

How does calcium carbonate neutralise hydrochloric acid?

a)

Calcium reacts with hydrogen ions

b)

Carbonate reacts with hydrogen ions

c)

Carbonate forms water with chloride ions

d)

Calcium neutralises the hydrogen ions

109.

The pH of pure water

a)

5.6

b)

7.0

c)

8.1

d)

0.0

110.

What is the meaning of the above hazard warning symbol?

a)

Corrosive

b)

Explosive

c)

Toxic

d)

Radioactive

111.

Acid in our stomach:

a)

Hydrochloric acid

b)

Sulfuric acid

c)

Acetic acid

d)

Carbonic acid

112.

Acid in soft drink:

a)

Hydrochloric acid

b)

Sulfuric acid

c)

Acetic acid

d)

Carbonic acid

113.
What happens when a solution of an acid is mixed with a solution of a base in a test tube?(i) The temperature of the solution increases(ii) The temperature of the solution decreases(iii) The temperature of the solution remains the same(iv) Salt formation takes place
a)
(a) (i) only
b)
(b) (i) and (iii)
c)
(c) (ii) and (iii)
d)
(d) (i) and (iv)
114.
2. An aqueous solution turns red litmus solution blue. Excessaddition of which of the following solution would reverse the change?
a)
(a) Baking powder
b)
(b) Lime
c)
(c) Ammonium hydroxide solution
d)
(d) Hydrochloric acid
115.
3. During the preparation of hydrogen chloride gas on a humid day, the gas is usually passed through the guard tube containing calcium chloride. The role of calcium chloride taken in the guard tube is to
a)
(a) absorb the evolved gas
b)
(b) moisten the gas
c)
(c) absorb moisture from the gas
d)
(d) absorb Cl– ions from the evolved gas
116.
4. Which of the following salts does not contain water of crystallisation?
a)
(a) Blue vitriol
b)
(b) Baking soda
c)
(c) Washing soda
d)
(d) Gypsum
117.
Sodium carbonate is a basic salt because it is a salt of
a)
(a) strong acid and strong base
b)
(b) weak acid and weak base
c)
(c) strong acid and weak base
d)
(d) weak acid and strong base
118.
. Calcium phosphate is present in tooth enamel. Its nature is
a)
(a) basic
b)
(b) acidic
c)
(c) neutral
d)
(d) amphoteric
119.
7. A sample of soil is mixed with water and allowed to settle. The clear supernatant solution turns the pH paper yellowish-orange. Which of the following would change the colour of this pH paper to greenish-blue?
a)
(a) Lemon juice
b)
(b) Vinegar
c)
(c) Common salt
d)
(d) An antacid
120.
what happens when a solution of  an acid is mixed with a solution of a base in a test tube?a
a)
temperature of the solution increases 
b)
temperature of the solution decreases
c)
temperature remains constant
d)
no reaction
121.
an aqueous soln turns red lithmus blue . excess addition of which of the following would reverse the change
a)
baking powder
b)
lime
c)
ammonium hydroxide solution
d)
HCL
122.
during preparation of HCL gas on a humid day the gas is usually passed through the guardtube containing calcium chloride .The role of calcium chloride is 
a)
absorb the evolved gas
b)
moisten the gas
c)
absorb moisture from the gas
d)
absorb CL ions from the evolved gas
123.
calcium phosphate is present in tooth enamel its nature is
a)
basic
b)
acidic 
c)
neutral
d)
amphoteric
124.
What is a strong acid?
a)
A substance that completely disintegrates to produce OH- ions in a solution.
b)
A substance that disintegrates partially to produce H+ ions in a solution.
c)
A substance that completely disintegrates to produce H+ ions in a solution.
d)
A substance that disintegrates partially to produce OH- ions in a solution.
125.
What is an Acid?
a)
Substance that produces hydrogen ions in aqueous solutions. Also known as proton donor.
b)
Substance that produces hydroxide ions in aqueous solutions. Also known as electron donor.
c)
Substance that produces hydrogen ions in aqueous solutions. Also known as proton receiver.
d)
Substance that produces hydrogen ions in aqueous solutions. Also known as electron donor.
126.
What is a base?
a)
Substance that donates hydrogen ions in solution
b)
Substance that donates hydroxide ions in solution
c)
Substance that receives hydroxide ions in solution
d)
Substance that donates phosphorus ions in solution
127.
What is a strong base?
a)
A substance that disintegrates completely to produce OH- ions in a solution.
b)
A substance that forms when there is OH- ions in a solution.
c)
A substance that replaces it's Hydrogen ions for Hydroxide.
d)
A solution in which there are more Hydroxide ions than Hydrogen ions.
128.
What is a salt?
a)
An element on the periodic table
b)
A mixture
c)
A condiment for food.
d)
An ionic compound.
129.
What is an oxidation reduction reaction?
a)
A reaction in which a solution changes color.
b)
A reaction that involves the transfer of protons.
c)
A chemical reaction that involves the transfer of electrons.
d)
A reaction that reduces the oxidation in a metal.
130.
What is the name for the following formula: H3PO4?
a)
Phosphide acid
b)
Phosphorous acid
c)
Hydrophosphic acid
d)
Phosphoric acid
131.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

132.

Which of the following is a strong acid?

a)

NaOH

b)

HCl

c)

HF

d)

H2O

133.
The Acid-Base classification system that defined acids as those that release H+ and bases as release OH- is known as ________.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
134.

A few drops of sodium hydroxide solution was added to a metal salt solution.

A dark green gelatinous precipitate was formed.

Which metal ion (cation) was present in the salt solution?

a)

iron(III) ion, Fe3+

b)

iron(II) ion, Fe2+

c)

copper(II) ion, Cu2+

d)

zinc ion, Zn2+

135.

A sample of a salt was dissolved in hydrochloric acid. A platinum wire was dipped into the solution and then placed in a roaring bunsen flame. A blue flame colour was produced.


From this 'flame test' observation, what was the identity of the metal ion in the salt?

a)

calcium ion, Ca2+

b)

sodium ion, Na+

c)

potassium ion, K+

d)

copper(II) ion, Cu2+

136.

Colourless crystals of substance X were dissolved in water and a few drops of dilute nitric acid, followed by a few drops of silver nitrate solution were added. A white precipitate formed. A few crystals of X were mixed with a few drops of concentrated hydrochloric acid. When a platinum wire was dipped in this mixture, and then placed in a roaring bunsen flame, a red flame colour was seen. From these observations deduce the identity of substance X.

a)

copper(II) chloride, CuCl2

b)

potassium sulphate, K2SO4

c)

sodium sulfate, Na2SO4

d)

calcium chloride, CaCl2

137.

A sample of a salt was dissolved in hydrochloric acid. A platinum wire was dipped into the solution and then placed in a roaring bunsen flame. A lilac/violet flame colour was produced.


From this 'flame test' observation, what was the identity of the metal ion in the salt?

a)

sodium ion, Na+

b)

potassium ion, K+

c)

copper(II) ion, Cu2+

d)

calcium ion, Ca2+

138.

A gas turns damp orange potassium dichromate(VI) paper green.


The gas is?

a)

oxygen, O2

b)

sulfur dioxide, SO2

c)

carbon dioxide, CO2

d)

ammonia, NH3

139.

A brown solution of a substance turns dark blue when a drop of starch solution was added.


The substance is most likely to be?

a)

sulfur dioxide, SO2

b)

chlorine, SO2 ?

c)

iodine, I2

d)

bromine, Br2

140.
Which of the following vocabulary terms matches the following definition:
*  when a solid mixes with a liquid and you can't see it anymore
a)
liquid
b)
suspension
c)
crystal
d)
dissolve

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