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Chemistry bumper quiz

Total questions: 62

Worksheet time: 4hrs 48mins

Name
Class
Date
1.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
2.

Potassium and Sulfur create...

a)

KS

b)

KS2

c)

K2S

d)

K2S2

3.

The chemical formula of Iron (III) and bromine is

a)

FeBr

b)

Fe(III)Br

c)

FeBr₃

d)

Fe₂Br₃

4.
A phosphorus atom needs to gain ___ electrons to achieve a full octet.
a)
3
b)
4
c)
6
d)
5
5.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
6.
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)
7.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
8.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
9.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
10.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
11.
Electrons that are free to move in a metal are referred to as...
a)
localized electrons
b)
delocalized electrons
c)
electrostatic electrons
d)
cations
12.
Ionic bonds are between _______ and ________. 
a)
nonmetals and nonmetals 
b)
metals and metals 
c)
metals and nonmetals
d)
none
13.
Outer shell electrons are called
a)
outer electrons
b)
valence electrons
c)
negatives
14.
The compound formed between lithium and chlorine is _________.
a)
ionic
b)
covalent
15.
Elements such as  Silicon, diamond and graphite.  Compounds include  SiO2
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
16.
Melting points are very high – a large amount of energy is needed to break all the covalent bonds
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
17.
Melting points are generally high – lots of energy is needed to overcome the attractions between positive ions and delocalised electrons.  
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
18.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
19.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
20.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
21.

Why are alloyed metals usually stronger?

a)

They have atoms of different metals in them, which makes it easier for the layer to move past each other...less likely to break

b)

They have atoms of different metals in them, which makes it harder for the layer to move past each other...less likely to break

22.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

23.

One mole of carbon dioxide (CO2) contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

24.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

25.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

26.

One mole of carbon dioxide (CO2) contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

27.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

28.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

29.

A mole is:

a)

The SI unit for mass

b)

The SI unit for the amount of a substance

c)

The SI unit for volume

d)

The SI unit for area

30.

What is the conversion factor that should be used to determine how many molecules are there in 4.00 moles of glucose, C6H12O6?

a)
b)
c)
d)
31.

What converting from moles to the number of particles, moles is multiplied by:

a)

an equivalent value

b)

a conversion factor

c)

the number of atoms in the formula

d)

the mass of the substance

32.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

33.

How many atoms are in 1 mole of Iodine (I)?

a)

6.022 x 1023

b)

4.022 x 1023

c)

6.022 x 1025

d)

4.022 x 1025

34.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

35.

SELECT ALL CORRECT ANSWERS - The mole can be used to measure:

a)

The amount of atoms in an element

b)

The amount of molecules in a covalent substance

c)

The amount of formula units in an ionic compound

d)

The amount of mass an object has

36.

How many moles there are in 5.68 x 1024 formula units of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

37.

What is correct equation that should be used to determine how many molecules there are in 0.75 moles of (NH4)3PO4?

a)
b)
c)
d)
38.

How many moles are in 4.5 x 1024 atoms of lithium?

a)

2.71 x 1048 particles

b)

7.47 moles

c)

7.47 x 1024 atoms

d)

2.71 moles

39.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

40.

What is the correct equation to determine how many calcium ions (Ca2+) in 2 moles?

a)
b)
c)
d)

This cannot be determined as calcium is not bonded.

41.

How many moles of Na contain 1.45 x 1021 atoms of Na?

a)

8.73 x 1044 moles

b)

8.73 moles

c)

0.00241 moles

d)

2.41 x 1044 moles

42.

What is the correct equation to calculate the number of moles in 3.13 x 1026 molecules of H2O2?

a)
b)
c)
d)
43.

What are the units for Avogadro's number?

a)

meters

b)

particles

c)

grams

d)

liters

44.
What is the molar mass NaCl?
a)
58 grams
b)
22.95 grams
c)
162 grams
d)
6.02 x 1023
45.
How many moles are in 20 grams of Ca (Calcium)?
a)
0.5 
b)
1
c)
3
d)
20
46.
For the Balanced Reaction:
3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe;
What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
47.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
48.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
49.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
a)
6 mol
b)
2 mol
c)
3 mol
d)
15 mol
50.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

a)

Bromine atoms in lead(II) bromide are converted to ions when it is melted

b)

Electrons flow through the lead(II) bromide when it is melted

c)

The ions in lead(II) bromide are mobile charge carriers in the molten state.

d)

There are no ions in solid lead(II) bromide

51.

Positive ions (cations) move towards the cathode (-) where they will discharge by....

a)

Breaking apart

b)

Losing electrons

c)

Clumping together.

d)

Gaining electrons

52.
What is the name given to the solution that is being electrolysed?
a)
Salt solution
b)
Electric solution
c)
Mineral solution
d)
Electrolyte
53.

___________ electrode is an inert electrode.

a)

Copper

b)

Iron

c)

Carbon

d)

Zinc

54.
What particle carries the charge in the wire?
a)
electron
b)
proton
c)
ion
d)
atom
55.

What are the products at the electrodes when dilute sulfuric acid is electrolysed using inert electrodes?

a)

A

b)

B

c)

C

d)

D

56.

Which row describes the electrolysis of molten potassium bromide?

a)

A

b)

B

c)

C

d)

D

57.

The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous

sodium chloride using carbon electrodes.

At which electrode(s) is hydrogen produced?

a)

electrode 1 only

b)

electrodes 1 and 3

c)

electrode 2 only

d)

electrodes 2 and 4

58.

Reduction is the ___________ of electrons.

a)

loss

b)

gain

c)

transfer

d)

share

59.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
60.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
61.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
62.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
6
c)
8
d)
24

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