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Y10 end of year

Total questions: 100

Worksheet time: 1hrs 14mins

Name
Class
Date
1.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
2.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
3.
All matter is made of .....
a)
energy 
b)
atoms 
c)
air
d)
chemistry
4.
The atomic number of an element tells the number of _____ in the nucleus of an atom of that element.
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
5.
Most of the mass of an atom is found it its _____.
a)
electron cloud
b)
nucleus
c)
atomic number
d)
empty space
6.
Each is an example of matter except _____.
a)
a cloud
b)
air
c)
a dust particle
d)
a beam of light
7.
An element is made up of only one kind of _____.
a)
isotope
b)
plastic
c)
atom
d)
metal
8.
Rutherford's experiment showed that most of an atom is made up of _____.
a)
a nucleus
b)
an electron cloud
c)
empty space
d)
alpha particles
9.
An element is made up of only one kind of _____.
a)
isotope
b)
plastic
c)
atom
d)
metal
10.
What subatomic particles are located in the electron cloud?
a)
quarks
b)
protons
c)
electrons
d)
neutrons
11.
Which subatomic particle has a negative charge in the atom?
a)
proton
b)
neutron
c)
electron
d)
quark
12.
Which is an electron?
a)
A
b)
B
c)
C
13.
Which is a proton?
a)
A
b)
B
c)
C
14.
Which is a neutron?
a)
A
b)
B
c)
C
15.
Which item on this element square represents the atomic number?
a)
13
b)
Al
c)
Aluminum
d)
26.981538
16.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
17.

What are valence electrons?

a)

Any of an atom's electrons

b)

Electrons located on the first energy level

c)

Electrons not attached to any atom

d)

electrons located on the outer energy level

18.

What period is Lead (Pb) in?

a)

6

b)

4

c)

Metals

d)

4A

19.

What category is silicon (Si) a part of?

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Halogens

20.

What Element is in period 4, group 5A?

a)

Antimony

b)

Arsenic

c)

Tin

d)

Germanium

21.

How many electrons does Barium (Ba) have?

a)

13

b)

2

c)

71

d)

56

22.

What is the ionic charge of Phosphorus (P)?

a)

+5

b)

-3

c)

+3

d)

-5

23.

How many electrons does a Strontium (Sr) ION have?

a)

38

b)

10

c)

8

d)

36

24.

How many neutrons does Bromine (Br) have?

a)

35

b)

80

c)

45

d)

7

25.

What period contains the element Plutonium (Pu)?

a)

8

b)

6

c)

7

d)

Plutonium doesn't exist

26.

How many electrons does a Radon (Rn) ION have?

a)

86

b)

8

c)

33

d)

Radon does not form an ion

27.

What group or family is Mercury (Hg) in?

a)

2B

b)

2A

c)

Metals

d)

Alkali metals

28.

What is group name of the most reactive metals?

a)

Noble gases

b)

Halogens

c)

Alkali metals

d)

Alkaline earth metals

29.

Why are halogens so reactive?

a)

They want to get rid of their only valance electron

b)

They only need one more electron

c)

They are non reactive, they have a full shell

30.

How many valence electrons does a carbon atom have?

a)

8

b)

4

c)

2

d)

6

31.

Which element conducts electricity the best?

a)

Silicon

b)

Fluorine

c)

silver

d)

Arsenic

32.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

33.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

34.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

35.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
36.
What does NOT happen when the temperature is increased?
a)
Particles collide more often
b)
Particles collide with more energy
c)
Particles move faster
d)
More particles collide in the correct orientation
37.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
38.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

39.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

40.

The ______________is required to break the bonds of the reactants.

a)

Carbonic energy

b)

Activation energy

c)

Plutonic energy

d)

Energi Gaib

41.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
42.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
43.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
44.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

45.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
46.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

47.
Compounds with these kinds of bonds have low melting and boiling points.
a)
Metallic
b)
Ionic
c)
Covalent
d)
None of the above
48.
Occurs when electrons float in a "sea;" this type of bond can be found in alloys.
a)
Metallic
b)
Ionic
c)
Covalent
d)
None of the above
49.
Occurs when valence electrons are shared between two or more atoms.
a)
Metallic
b)
Ionic
c)
Covalent
d)
None of the above
50.
Carbon tetrachloride has a ______ bond, and its formula is ______.
a)
covalent, CCl
b)
ionic, CCl4
c)
covalent, CCl4
d)
ionic, CCl
51.
Which of the following compounds has a tetrahedral molecular shape?
a)
Br2
b)
CO2
c)
NF3
d)
CH4
52.
The molecular geometry of H2O (a very special molecule) is...
a)
Tetrahedral
b)
Bent
c)
Linear
d)
Trigonal planar
53.
A covalent compound is non-polar when...
a)
the electrons are shared equally.
b)
the electrons are shared unequally.
c)
the electrons are lost to another atom.
d)
the electrons are gained from another atom. 
54.
Warning: Tricky!!
What is the correct name for Cu2O3 ?
a)
Copper (II) Oxide
b)
Copper (III) Oxide
c)
Copper (III) dioxide
d)
dicopper trioxide
55.
What is the correct formula for Beryllium hydroxide?
a)
Be(OH)2
b)
Be(OH)
c)
Be2+(OH)1-
d)
BeOH2
56.
What molecular shape is this?
a)
Tetrahedral
b)
Trigonal Planar
c)
Linear
d)
Bent
57.

Carbon is able to bond with atoms of other elements in many different ways because it has

a)

six protons.

b)

four electrons.

c)

six valence electrons.

d)

four valence electrons.

58.

An element whose atoms can make straight chains, branched chains, and rings is

a)

carbon.

b)

hydrogen.

c)

nitrogen.

d)

oxygen.

59.

How many chemical bonds can each carbon atom form?

a)

one

b)

two

c)

three

d)

four

60.

Which form of pure carbon is so hard that it can be used in cutting tools?

a)

diamond

b)

graphite

c)

nanotube

d)

fullerene

61.

Which form of pure carbon is formed of layers that slide past one another?

a)

diamond

b)

graphite

c)

fullerene

d)

nanotube

62.

What is the shape of pure carbon fullerenes?

a)

hollow tube

b)

hollow ball with a pattern like a geodesic dome

c)

flat layers

d)

hard, solid crystal shaped like a ball

63.
Giant lattice structure held together by attraction between  positive and negatively charged ions 
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
64.
Elements such as  Silicon, diamond and graphite.  Compounds include  SiO2
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
65.
Low melting and boiling points which increase with increasing molecule size due to increased intermolecular forces.
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
66.
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 
67.
Lattice structure in which all atoms are joined to others by covalent bonds
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
68.
Conductors due to delocalised electrons
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
69.
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 
70.
Formulae of these might include H2O
each molecule contains 1 O and 2H atoms 
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
71.
Compounds containing a metal and non-metal.
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
72.
Conductors due to delocalised electrons
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
73.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
74.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
75.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
76.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
77.
Which elements tend to lose electrons?
a)
metals
b)
nonmetals
78.
Which of the following is relevant for copper?
a)
Ion
b)
Ionic bonding
c)
Metallic bonding
d)
Covalent bonding
79.
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
80.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
81.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
82.
Atoms form ions in order to become
a)
isotopes
b)
stable
c)
metals
d)
nonmetals
83.
An anion in aqueous solution produces: 
1. Effervescence when hydrochloric acid is added
2. Gas given off form a white precipitate with lime water. 
What is the ion?
a)
Carbonate ion , CO32-
b)
Nitrate ion, NO3-
c)
Sulfate ion, SO42-
d)
Chloride ion, Cl-
84.
An anion in aqueous solution produces: 
1. Effervescence when sodium hydroxide and aluminium foil is added to the solution and warm.
2. Moist red litmus paper turn blue
What is the ion?
a)
Carbonate ion , CO32-
b)
Nitrate ion, NO3-
c)
Sulfate ion, SO42-
d)
Chloride ion, Cl-
85.

An anion in aqueous solution produces:

1. white precipitate when dilute hydrochloric acid followed by barium chloride solution is added.

What is the ion?

a)

Carbonate ion , CO32-

b)

Nitrate ion, NO3-

c)

Sulfate ion, SO42-

d)

Chloride ion, Cl-

86.

An anion in aqueous solution produces:

1. white precipitate when dilute hydrochloric acid follow by barium chloride solution is added.

What is the White precipitate?

a)

BaCl

b)

BaNO3

c)

BaSO4

87.
An anion in aqueous solution produces: 
1. white precipitate when dilute nitric acid follow by silver nitrate solution is added.
What is the ion?
a)
Carbonate ion , CO32-
b)
Nitrate ion, NO3-
c)
Sulfate ion, SO42-
d)
Chloride ion, Cl-
88.
An anion in aqueous solution produces: 
1. white precipitate when dilute nitric acid follow by silver nitrate solution is added.
What is the white precipitate?
a)
AgCl
b)
AgNO3
c)
Ag2SO4
89.
A metallic ion in aqueous solution produces 
1. a white precipitate with aqueous ammonia, soluble in excess;
2. a white precipitate with aqueous sodium hydroxide, soluble in excess.
What is the ion?
a)
Al3+
b)
Ca2+
c)
K+
d)
Zn2+
90.
A metallic ion in aqueous solution produces 
1. no precipitate with aqueous ammonia;
2. a white precipitate with aqueous sodium hydroxide, insoluble in excess.
What is the ion?
a)
Al3+
b)
Ca2+
c)
Pb2+
d)
Zn2+
91.
A metallic ion in aqueous solution produces 
1. no precipitate with aqueous ammonia;
2. a white precipitate with aqueous sodium hydroxide, insoluble in excess.
What is the ion?
a)
Al3+
b)
Ca2+
c)
Pb2+
d)
Zn2+
92.
A metallic ion in aqueous solution produces 
1. light blue precipitate with aqueous ammonia, soluble in excess to form deep blue solution;
2. light blue precipitate with aqueous sodium hydroxide, insoluble in excess.
What is the ion?
a)
Al3+
b)
Ca2+
c)
Cu2+
d)
Zn2+
93.
A metallic ion in aqueous solution produces 
1. a green precipitate with aqueous ammonia, insoluble in excess;
2. a green precipitate with aqueous sodium hydroxide, insoluble in excess.
What is the ion?
a)
Al3+
b)
Fe2+
c)
Pb2+
d)
Zn2+
94.
A metallic ion in aqueous solution produces 
1. a reddish-brown precipitate with aqueous ammonia, insoluble in excess;
2. a reddish-brown precipitate with aqueous sodium hydroxide, insoluble in excess.
What is the ion?
a)
Fe3+
b)
Fe2+
c)
Pb2+
d)
Zn2+
95.
Which of the following is the correct description on a positive result observation for test on ammonia gas?
a)
The lighted splint is extinguish with a 'pop' sound.
b)
The glowing splint is rekindled. 
c)
A white precipitate is formed. The white precipitate dissolves upon further bubbling
d)
The moist blue red litmus paper turn blue. 
96.

Which of the following is the correct description on a positive result observation for test on carbon dioxide gas?

a)

The lighted splint is extinguish with a 'pop' sound.

b)

The glowing splint is rekindled.

c)

A white precipitate is formed in limewater. The white precipitate dissolves upon further bubbling

d)

The moist blue red litmus paper turn blue.

97.

An anion in aqueous solution produces:

1. cream precipitate when dilute nitric acid follow by silver nitrate solution is added.

What is the ion?

a)

Bromide ion, Br-

b)

Nitrate ion, NO3-

c)

Sulfate ion, SO42-

d)

Chloride ion, Cl-

98.

An anion in aqueous solution produces:

1. yellow precipitate when dilute nitric acid follow by silver nitrate solution is added.

What is the ion?

a)

Bromide ion, Br-

b)

Nitrate ion, NO3-

c)

Iodide ion, I-

d)

Chloride ion, Cl-

99.

Which of the following determine the properties of a polymer?

a)

chemical nature of the monomer

b)

length of the polymer chain

c)

how the monomers are joined together

d)

All of the above

100.

Once formed, it can be heated and reformed over and over again

a)

thermoset

b)

thermoplastic

c)

elastomer

d)

kevlar

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