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Worksheets

2.4 Chemistry NCEA

Total questions: 135

Worksheet time: 2hrs 59mins

Name
Class
Date
1.

What type of particle(s) makes up HCl?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

2.

What type of particle(s) makes up HCl?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

3.

What type of attractive forces exist between HCl particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

4.

What type of particle(s) makes up SiO2?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

5.

What type of attractive forces exist between SiO2 particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

6.

What type of particle(s) makes up diamond (C)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

7.

What type of attractive forces exist between diamond (C) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

8.

What type of particle(s) makes up graphite (C)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

9.

What type of attractive forces exist between copper (Cu) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

10.

What type of particle(s) makes up copper (Cu)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

11.

What type of particle(s) makes up sodium (Na)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

12.

What type of attractive forces exist between sodium (Na) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

13.

What type of particle(s) makes up gold (Au)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

14.

What type of attractive forces exist between gold (Au) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

15.

What type of attractive forces exist between graphite (C) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds & weak intermolecular forces

16.

What type of attractive forces exist between methane (CH4) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

17.

What type of particle(s) makes up methane (CH4)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

18.

What type of particle(s) makes up water (H2O)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

19.

What type of attractive forces exist between water (H2O) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

20.

What type of attractive forces exist between iodine (I2) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

21.

What type of particle(s) makes up iodine (I2)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

22.

What type of particle(s) makes up carbon dioxide (CO2)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

23.

What type of attractive forces exist between carbon dioxide (CO2) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

24.

What type of attractive forces exist between calcium oxide (CaO) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

25.

What type of particle(s) makes up calcium oxide (CaO)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

26.

What type of attractive forces exist between lithium sulfate (Li2SO4) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

27.

What type of particle(s) makes up lithium sulfate (Li2SO4)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

28.

What type of particle(s) makes up ammonium nitrate (NH4NO3)?

a)

Molecules

b)

Metal cations & delocalised electrons

c)

Cations & anions

d)

Atoms

29.

What type of attractive forces exist between ammonium nitrate (NH4NO3) particles?

a)

Weak intermolecular forces

b)

Metallic bonds

c)

Ionic bonds

d)

Covalent bonds

30.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
31.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
32.
What is the maximum number of electrons in the second energy level?
a)
18
b)
8
c)
32
d)
2
33.
What are Valence electrons defined as ?
a)
as electrons in the atom's outermost orbitals. 
b)
as electrons in the atom's innermost orbitals.
34.

X atom has 12 protons. what is the electron arrangement of atom X?

a)

2.8

b)

2.8.8

c)

2.8.2

d)

2.10

35.

An atom has 10 protons in its nucleus. how many electrons does the atom have?

a)

10

b)

11

c)

12

d)

13

36.

Y atom has 13 protons in its nucleus. How many valence electrons does Y atom have?

a)

13

b)

3

c)

10

d)

8

37.

E2+ has an electron arrangement of 2.8. how many proton does E2+ have?

a)

10

b)

8

c)

12

d)

2

38.

F3- has an electron arrangement of 2.8.8. How many protons does F3- have?

a)

15

b)

18

c)

8

d)

10

39.

what is the electron arrangement of atom N?

a)

2.

b)

2.8

c)

2.5

d)

2.8.8

40.

What is the formula for Sodium Nitrate?

a)

NaN

b)

NaN2

c)

Na(NO3)2

d)

NaNO3

e)

SN

41.
What is the name of NH4Cl?
a)
nitrogen tetrahydrogen chloride
b)
ammonium chlorine
c)
ammonium chloride
d)
ammonium chlorate
42.

Identify Gallium(III) Sulfate

a)

GaSO4

b)

Ga2(SO4)3

c)

Ga3(SO4)2

d)

Ga2SO4

43.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
44.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
45.

What is the name of AgNO3?

a)

Silver(III) Nitrate

b)

Silver Mononitrate

c)

Silver(I) Nitrate

d)

Monosilver Nitrate

46.
What's the name of the compound NH4NO3 ?
a)
nitrogen hydrogen oxygen
b)
ammonium nitrite
c)
nitrogenous water
d)
ammonium nitrate
47.

If copper(II) and phosphate bond together, the formula would be:

a)

Cu2(PO4)3

b)

CuPO4

c)

Cu3(PO4)2

d)

Cu3PO4

48.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
49.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
50.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
51.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
52.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
53.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
54.
A cation is a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
55.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
56.
Ionic bonds happen because of the ____ of valence electrons.
a)
sharing
b)
transfer
57.
What type of bond is this? Lithium with Fluorine?
a)
ionic
b)
covalent
58.
What type of elements will form an ionic bond?
a)
Metals + Metals
b)
Nonmetals + Nonmetals
c)
Metals + Nonmetals
d)
None of the above
59.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

60.
What will be the compound name of the following chemical formula?
NaCl
a)
Potassium Chloride
b)
Sodium Chloride
c)
Calcium Chloride
d)
Sodium Chlorine
61.
Metals tend to 
a)
gain electrons
b)
lose electrons
62.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
63.

Ionic compounds can conduct when molten or dissolved because ...

a)

There are strong electrostatic attractions present

b)

The ions are free to move and conduct

c)

Ions can vibrate

d)

There is a metal present

64.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

65.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

66.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

67.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

68.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

69.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

70.

Which of these is incorrect?

a)
b)
71.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

72.
This is a correct dot diagram for magnesium (Mg)
a)
true
b)
false
73.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
74.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
75.

In chemical compounds, covalent bonds form when

a)

both atoms already have full valence shells.

b)

electrons are completely transferred between two metals.

c)

pairs of electrons are shared between two non-metal atoms.

d)

two non-metal atoms are attracted to each other by opposite charges.

76.

What is the name of this shape?

a)

Tetrahedral

b)

Trigonal Pyramidal

c)

Angular or Bent

d)

Linear

77.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
78.

A mystery substance has a low melting point, does not dissolve in water, does not conduct electricity, and is made of non-metals. Which type of bonding is most likely to be present?

a)

Metallic

b)

Ionic

c)

Covalent Network

d)

Covalent Molecular

79.

A mystery substance has a very high melting point, does not dissolve in water, does not conduct electricity, and is made of non-metals. This substance is very hard. Which type of bonding is most likely to be present?

a)

Metallic

b)

Ionic

c)

Covalent Network

d)

Covalent Molecular

80.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

81.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

82.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

83.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

84.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

85.

What kind of bond does this show?

a)

Ionic

b)

Covalent

86.

What happens when you put an ionic compound in water?

a)

The ions separate

b)

The ions pack more closely together

c)

Nothing happens

87.

In nonpolar covalent bonds....

a)

Electrons are more attracted to one atom than the other

b)

Electrons are equally shared between atoms

88.

In polar covalent bonds...

a)

Electrons are more attracted to one atom than the other

b)

Electrons are equally shared between atoms

89.

Which of these atoms will electrons be most attracted to in a covalent bond?

a)

Na

b)

H

c)

Be

d)

F

90.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

91.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

92.
What does this image represent?
a)
Atom
b)
Element
c)
Molecule
d)
Marshmallows
93.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
94.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
95.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
96.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
97.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
98.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
99.

What is the bond angle for a trigonal pyramidal molecule?

a)

90

b)

107

c)

109.5

d)

120

100.
How many unshared pairs of electrons will a pyramidal molecule have? 
a)
1
b)
2
c)
3
d)
4
101.
What is the bond angle for this molecule?
a)
109.5
b)
120
c)
107
d)
90
102.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
103.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

104.

A molecular geometry with 3 bonding pairs is

a)

Trigonal pyramidal

b)

Trigonal planar

c)

Trigonal bipyramidal

d)

T-shaped

105.

A molecular geometry with 2 lone pairs and 2 bonding pairs is

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Linear

106.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
107.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
108.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Linear

c)

Bent

d)

Tetrahedral

109.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
110.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
111.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
112.

Which best describes a triple bond?

a)

3 shared pairs of electrons

b)

3 shared electrons

c)

a central electron with 3 atoms bonded around it

113.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
114.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

115.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
116.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
117.
Is respiration an Endothermic or an Exothermic reaction?
a)
Endothermic
b)
Exothermic
118.
Baking bread and cooking an egg are examples of....?
a)
Endothermic processes
b)
Exothermic processess
c)
None of these 
119.
Is photosenthysis an Exothermic or an Endothermic reaction?
a)
Endothermic
b)
Exothermic
120.
What type of reaction is shown in the photo?
a)
Exothermic
b)
Isothermic
c)
Endothermic
d)
None of the  above
121.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
bubbles of gas appear
d)
dissolving
122.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
123.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
124.

What is the Heat of Reaction  ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

125.

How much activation energy is needed for this reaction?

a)

300 KJ

b)

500 KJ

c)

400 KJ

d)

100 KJ

126.

Are the products or reactants of this reaction storing more energy in their chemical bonds?

a)

Both storing the same

b)

No way to tell

c)

Products

d)

Reactants

127.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

128.

What kind of equation is this: 2KI + MgCl2 + 200KJ ----> 2KCl + MgI2

a)

Endothermic

b)

Exothermic

129.

In this equation, is more energy stored in the bonds of the reactants or products: NaCl + AgF +100KJ -----> NaF + AgCl

a)

Products

b)

Reactants

130.
Some average bond enthalpies, in kJ/mol, are as follows:
H-H = 436
Cl-Cl = 242
H-Cl = 431
What is the enthalpy change for the decomposition of hydrogen chloride?
2 HCl --> H2 + Cl2
a)
-184 kJ
b)
+ 184 kJ
c)
- 247 kJ
d)
+ 247 kJ
131.

The average bond enthalpies for O-O and O=O are 146kJ/mol and 496kJ/mol respectively. Calculate the enthalpy change for the reaction shown.

a)

-102kJ

b)

+102kJ

c)

+146kJ

d)

-248 kJ

132.

Calculate the enthalpy change, in kJ/mol for the reaction

H2 (g) + ½O2 (g) → H2O (g)


Data of bond energy:

H−H = +436 kJ/mol

O=O = +498 kJ/mol

H−O = +464 kJ/mol

a)

−243 kJ/mol

b)

−6 kJ/mol

c)

+6 kJ/mol

d)

+221 kJ/mol

133.

The enthalpy change for the reaction between hydrochloric acid and sodium hydroxide is −56 kJ/mol. Therefore ...

a)

the reaction is exothermic and the temperature rises

b)

the reaction is exothermic and the temperature falls

c)

the reaction is endothermic and the temperature rises

d)

the reaction is endothermic and the temperature falls

134.

Which of these diagram correctly represent an endothermic reaction?

a)
b)
c)
d)
135.

In an endothermic reaction in aqueous solution, which of the following is correct?

a)

temperature increases, sign of enthalpy change is positive

b)

temperature increases, sign of enthalpy change is negative

c)

temperature decreases, sign of enthalpy change is positive

d)

temperature decreases, sign of enthalpy change is negative

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