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Y10 U1-4 Test Revision

Total questions: 223

Worksheet time: 3hrs 4mins

Name
Class
Date
1.

In the diagram, where will the white ring of ammonium chloride form?

a)

A

b)

B

c)

C

d)

D

2.

Why does the ring of ammonium chloride form closer to the hydrochloric acid end?

a)

HCl diffuses faster than NH₃

b)

NH₃ diffuses faster than HCl

c)

NH₃ is heavier than HCl

d)

The gases always react in the centre

3.

Which two of the following explain why it takes time for ammonium chloride to form? Select TWO

a)

Gas particles move in random directions

b)

Gas particles collide with each other

c)

Gas particles have very weak bonds

d)

Gas particles dissolve in the glass tube

4.

In which state of matter are particles arranged in a regular, fixed pattern?

(a)  

5.

Which state of matter has particles that move freely and spread far apart?

(a)  

6.

Which state of matter has particles with the least energy?

(a)  

7.

In which state of matter can particles flow past one another but still remain close together?

(a)  

8.

Which state of matter has a definite volume but no definite shape?


(a)  

9.

In which state of matter do particles move by only vibrating around fixed points?


(a)  

10.

Which state of matter has particles that are furthest apart?


(a)  

11.

Why can gases be compressed but solids cannot?

a)

Gas particles are heavier than solid particles

b)

Gas particles have large spaces between them

c)

Gas particles are arranged in a fixed pattern

d)

Solids have weak forces of attraction

12.

Which state of matter has the strongest forces of attraction between particles?


(a)  

13.

Which statement best describes the arrangement of particles in a liquid?

a)

Regular, tightly packed, only vibrating

b)

Random arrangement, close together, sliding past one another

c)

Random arrangement, very far apart, moving freely

d)

Fixed arrangement, widely spaced

14.

What state of matter is represented in this picture?

a)

solid

b)

liquid

c)

gas

15.

What state of matter is represented in the picture above?

a)

solid

b)

liquid

c)

gas

16.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
17.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
18.

Freezing

a)

Solid to gas

b)

Liquid to solid

c)

Gas to solid

19.

Boiling

a)

liquid to gas

b)

gas to solid

c)

gas to liquid

20.

What is happening when my ice cream changes from a solid to a liquid?

a)

freezing

b)

melting

c)

burning

21.

Particles of a liquid

a)

are tightly packed together and stay in a fixed position.

b)

are free to move around one another but still touch.

22.

Solid to Gas

a)

Deposition

b)

Sublimation

c)

Evaporation

23.

What is condensation?

a)

gas to solid

b)

gas to liquid

c)

liquid to solid

24.

The slower the particles in a substance move,

a)

the colder it is.

b)

the warmer it is.

c)

the more energy it has.

25.

Liquid to Gas

a)

Condensation

b)

Evaporation

c)

Sublimation

26.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

27.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

28.

A gas typically consists of:

a)

low energy particles that experience high attractive forces between them.

b)

low energy particles that experience no attractive forces between them.

c)

high energy particles that experience high attractive forces between them.

d)

high energy particles that experience little attractive force between them

29.

Which of the following statements is true regarding the particle structure of liquids? Particles of a liquid are:

a)

very close together, so the liquid cannot easily change its shape.

b)

fast-moving, so they fill the volume of their container.

c)

relatively close together, so they cannot be easily compressed.

d)

very far apart, so they have plenty of room to move around.

30.

Which process could cause a material to change state from gas to liquid?

a)

Adding heat

b)

Adding energy

c)

Removing particles

d)

Removing energy

31.

If I add heat to a solid, how will the motion of the particles be affected?

a)

They will move slower

b)

They will stop moving

c)

They will move faster

d)

They will move to a different container

32.

How can you stop the movement of particles?

a)

Increase the temperature

b)

Decrease the temperature

c)

You can't.

d)

Hold them still with your hands.

33.
Which diagram best shows the end result of diffusion?
a)
F
b)
G
c)
H
d)
J
34.
The picture  is an example of _________________.
a)
isotonic
b)
diffusion
c)
osmosis
d)
active transport
35.
In diffusion, particles move down a _______ ________
a)
Concentrate gradient
b)
Conceited gradient
c)
Concentration gradient 
d)
Concentrated orange juice
36.
Diffusion stops when the concentration is evenly spread out - true or false?
a)
100% definitely true.
b)
Could be false though.
37.
An increase in temperature does what to diffusion?
a)
Speeds it up
b)
Slows it down
c)
Has no effect
d)
I wish i knew. Really I do.
38.

In the picture the red dots represent...

a)

solvent

b)

solute

c)

solution

d)

diffusion

39.
Which factor can affect gas pressure?
a)
Temperature 
b)
Volume
c)
The Amount of Gas
d)
All of the answers are correct
40.

(6A) States of matter are determined by their:

a)

ONLY the amount of energy contained by their molecules

b)

ONLY the arrangement of their molecules

c)

The arrangement AND energy contained by their molecules

d)

Viscosity

41.

(6A) In the image above, which of those phases has the most energy?

a)

Solid

b)

Liquid

c)

Gas

d)

All of the above

42.

Gases are easily compressed because of .......................................

a)

the size of its particles.

b)

the space between the particles in a gas.

c)

the mass of the particles.

43.

Match the following

a)
1.

solid

b)
2.

liquid

c)
3.

gas

44.

Which of the following is a correct description for solids?

a)

closely arranged and in fixed positions

b)

closely arranged and vibrate in fixed positions

c)

closely arranged and can move around

45.
a)

A

b)

B

c)

C

d)

D

46.

a)

A

b)

B

c)

C

d)

D

47.

a)

A

b)

B

c)

C

d)

D

48.
a)

A

b)

B

c)

C

d)

D

49.

a)

A

b)

B

c)

C

d)

D

50.

a)

A

b)

B

c)

C

d)

D

51.

An ice cube is gently warmed as shown. Which process is taking place?

a)

Decomposition

b)

Dissolving

c)

Boiling

d)

Melting

52.

A man spills ink on his polyester shirt. The table shows the solubility of ink and of polyester in four solvents. Which solvent should be used to remove the ink?

a)

A

b)

B

c)

C

d)

D

53.

A measure of how much solute will dissolve in a solvent

a)

Solubility

b)

Solution

c)

Solvent

d)

Solute

54.

Solubility (g per 100g of solvent) =

a)

(mass of solid/mass of water removed) x 100

b)

(mass of solution/mass of solid removed) x 100

c)

mass of water removed/mass of solution

d)

mass of water removed/mass of solid

55.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

56.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

57.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

58.

At what temperature can you fully dissolve 60g of KNO3?

a)

27

b)

30

c)

37

d)

You cannot determine this

59.

At what temperature can you fully dissolve 120g of NaBr?

a)

70

b)

20

c)

100

d)

You cannot determine this

60.
What is able to dissolve other substances?
a)
Solute
b)
Salt
c)
Suspension
d)
Solvent
61.
If I dissolve carbon dioxide in water, what is my solvent?
a)
Carbon Dioxide
b)
There is no solvent
c)
Oxygen
d)
Water
62.

Define the term soluble.

a)

Can dissolve in water

b)

Cannot dissolve in water

c)

Partially dissolves in water

63.

Define the term insoluble.

a)

Can dissolve in water.

b)

Cannot dissolve in water.

c)

Partially dissolves in water.

64.

A crystal of purple potassium manganate(VII) was added to each of the beakers shown in the diagram.

One beaker contained hot water and the other beaker contained cold water. In both beakers the purple colour of the potassium manganate(VII) spreads out. Which result and explanation are correct?

a)

result - colour spreads faster in cold water

explanation - particles move faster at a higher temperature

b)

result - colour spreads faster in cold water

explanation - particles move slower at a higher temperature

c)

result - colour spreads faster in hot water

explanation - particles move faster at a higher temperature

d)

result - colour spreads faster in hot water

explanation - particles move slower at a higher temperature

65.

A student uses the apparatus shown to find out how many different pigments are in leaves.


What is this separation method called?

a)

Chromatography

b)

Distillation

c)

Filtration

d)

Evaporation

66.

A plant colour X is a mixture. Chromatography is used to compare X with three other coloured mixtures, P, Q and R. The results are shown in the diagram.


Which other mixtures contain the plant colour X?

a)

P only

b)

P and Q only

c)

R only

d)

P, Q and R

67.

When water is heated to 100°C, it changes to steam. The steam has a larger volume than the water.

Which change on heating explains this increase in volume?

a)

The bonds between hydrogen and oxygen break.

b)

The molecules become lighter.

c)

The spacing between the molecules increases.

d)

The water molecules expand.

68.

Two gas jars are set up as shown.

The lid is removed and the gas jars are left to stand. After some time the contents of both gas jars are brown. Which process causes this to happen?

a)

condensation

b)

diffusion

c)

evaporation

d)

filtration

69.

Kuku just made himself a cup of hot tea.

Which row describes the water particles in the air above the cup compared with the water particles in the cup?

a)

A

b)

B

c)

C

d)

D

70.

Hydrogen chloride gas, HCl, reacts with ammonia gas, NH3, to form solid ammonium chloride. The apparatus is set up as shown. After a few minutes, solid ammonium chloride forms where the two gases meet.

a)

A

b)

B

c)

C

d)

D

71.

The colours in an ink can be separated by chromatography.


Which diagram shows the correct way to set up the apparatus?

a)

A

b)

B

c)

C

d)

D

72.

Which statement about paper chromatography is correct?

a)

A solvent is needed to dissolve the paper.

b)

Paper chromatography separates mixtures of solvents.

c)

The solvent should cover the baseline.

d)

The baseline should be drawn in pencil.

73.

Which of the following best defines solubility?

a)

The mass of solvent that dissolves in 100 g of solute

b)

The mass of solute that dissolves in 100 g of solvent

c)

The time taken for a solute to dissolve in water

d)

The mass of solution after evaporation

74.

A student adds excess salt to water and stirs. Why must excess solid be used?

a)

To speed up the experiment

b)

To make the solution saturated

c)

To keep the temperature constant

d)

To stop evaporation

75.

A student records:

  • Mass of evaporating dish = 50.0 g

  • Mass of dish + dry solid after heating = 54.2 g
    What is the mass of the solid in grams?



(a)  

76.

In a solubility experiment, a student calculates:
Mass of solute = 12.0 g
Mass of water = 20.0 g

What is the solubility in g per 100 g of water?

a)

12.0 g/100 g

b)

20.0 g/100 g

c)

60.0 g/100 g

d)

240.0 g/100 g

77.

If water is not completely evaporated, how will the calculated solubility be affected?

a)

Too high

b)

Too low

c)

No effect

d)

Cannot be measured

78.

If the solid decomposes on heating, how will this affect the result?

a)

The calculated solubility will be too high

b)

The calculated solubility will be too low

c)

No change

d)

It depends on the solvent used

79.

Why must the solution be stirred before pouring into the basin?

a)

To help the solid dissolve evenly

b)

To cool it down

c)

To make the water evaporate faster

d)

To remove impurities

80.

A student forgets to weigh the empty evaporating dish. Which calculation will they NOT be able to do?

a)

Mass of solute

b)

Mass of solution

c)

Mass of water

d)

Solubility in g/100 g

81.

Which experimental error would make the calculated solubility appear higher?

a)

Water not fully evaporated

b)

Heating too strongly so solid decomposes

c)

Using too little solute at the start

d)

Forgetting to stir

82.

Why is solubility usually given at a stated temperature?

a)

Temperature has no effect on solubility

b)

Solubility always decreases with temperature

c)

Solubility depends on temperature

d)

Solubility is constant for all substances

83.

Mass of evaporating dish = 62.5 g
Mass of dish + dry solid after heating = 68.4 g
What is the mass of the solid in grams

(a)  

84.

Mass of dish = 41.0 g
Mass of dish + dry solid = 48.6 g
What is the mass of the solid in grams?

(a)  

85.

Mass of dish = 55.5 g
Mass of dish + solid = 59.0 g
What is the mass of the solid?

(a)  

86.

Mass of solute = 8.0 g
Mass of water = 16.0 g
What is the solubility in g per 100 g water?

a)

25.0 g/100 g

b)

50.0 g/100 g

c)

200.0 g/100 g

d)

12.5 g/100 g

87.

Mass of solute = 15.0 g
Mass of water = 25.0 g
What is the solubility?

a)

15.0 g/100 g

b)

25.0 g/100 g

c)

60.0 g/100 g

d)

150.0 g/100 g

88.

Mass of solute = 7.5 g
Mass of water = 30.0 g
What is the solubility?

a)

20.0 g/100 g

b)

25.0 g/100 g

c)

100.0 g/100 g

d)

200.0 g/100 g

89.

Mass of solution = 32.0 g
Mass of solute = 8.0 g

Step 1: Calculate mass of water.
Step 2: Calculate solubility in g per 100 g water.

a)

25.0 g/100 g

b)

33.3 g/100 g

c)

40.0 g/100 g

d)

400.0 g/100 g

90.

Mass of solution = 50.0 g
Mass of solute = 15.0 g

Step 1: Calculate mass of water.
Step 2: Calculate solubility in g per 100 g water.

a)

30.0 g/100 g

b)

35.0 g/100 g

c)

150.0 g/100 g

91.

Which method is used to separate water from a salt solution?

a)
Distillation
b)

Chromatography

c)
Filtration
d)

Crystallisation

92.

Which method would you use to obtain pure crystals of potassium nitrate from a potassium nitrate solution?

a)
Filtration
b)
Distillation
c)
Sublimation
d)

Crystallisation

93.

Which method separates sand from salty water?

a)
Evaporation
b)
Filtration
c)
Distillation
d)
Sedimentation
94.

Which method separates ethanol from water?

a)
Evaporation
b)
Distillation
c)
Filtration
d)
Centrifugation
95.

Which technique is used to check if a food colouring contains more than one dye?

a)
Filtration
b)
Microscopy
c)
Spectroscopy
d)
Chromatography
96.

A student writes: “Filtration can be used to separate salt from salt solution.”
Is this correct?

a)

No, because salt evaporates during filtration

b)

Yes. Salt can be easily filtered out of a salt solution.

c)

Yes. Filtration is the best method to separate salt from salt solution.

d)

No. Filtration cannot be used to separate salt from salt solution.

97.

A student suggests: “Distillation is the best method to separate sand from salty water.”

a)
No, distillation is not the best method to separate sand from salty water.
b)
Filtration is less effective than distillation for this separation.
c)
Distillation is the only method to separate sand from water.
d)
Yes, distillation effectively separates sand from salty water.
98.

A student claims: “Filtration can be used to separate copper sulfate crystals from copper sulfate solution.”

a)

Correct

b)

Incorrect, use crystallisation

c)

Incorrect, use chromatography

d)

Incorrect, use distillation

99.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
100.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
101.
A pure substance containing only one kind of atom.
a)
element
b)
compound
102.
A compound consists of two or more elements bound together.
a)
True
b)
False
103.

Which compound is best represented by this particle diagram?

a)

NH3

b)

H2O

c)

CH4

d)

HCl

104.

Which compound is best represented by this particle diagram?

a)

C2H6

b)

C6H12O6

c)

CO2

d)

NaCl

105.

This diagram represents a _____.

a)

Element

b)

Compound

c)

Mixture of compound and element

d)

Mixture of two elements

106.
This diagram represents a _____.
a)
pure substance that is a compound
b)
mixture of elements
c)
pure substance that is an element
d)
mixture of compounds
107.

What does this illustrate

a)

Elements

b)

Compunds

c)

Mixture of Elements and Compunds

d)

Mixture of Compounds

108.

This picture represents which of the following?

a)

A single element

b)

Mixture of molecules

c)

mixture of atoms

d)

mixture of compounds

109.
Classify the picture with the correct label.
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
110.

A beaker containing solid carbon dioxide is placed in a fume cupboard at room temperature. The

carbon dioxide becomes gaseous.

Which process describes this change of state?

a)

Boiling

b)

condensation

c)

evaporation

d)

sublimation

111.

The table below shows information about two isotopes of element X.

Calculate the relative atomic mass (Ar) of element X. Give your answer to 1 decimal place

(a)  

112.

Which diagram shows a gas?

a)

A

b)

B

c)

C

d)

D

e)

E

113.

The atomic number is the number of (a)   ?

114.

Which of these particles has a positive charge?

a)

electron

b)

proton

c)

neutron

115.

Which of these particles does not have an electrical charge?

a)

electron

b)

proton

c)

neutron

116.
What is the relative charge of a neutron?
a)
0
b)
+2
c)
+1
d)
-1
117.
What is the relative charge of a proton?
a)
0
b)
+2
c)
+1
d)
-1
118.

What is the relative mass of a proton?

a)

0.0001

b)

0.001

c)

2

d)

1

119.

What is found in the nucleus?

a)

protons and electrons

b)

neutrons and electrons

c)

neutrons and protons

d)

protons, neutrons and electrons

120.
Complete the missing label on the diagram.
a)
Neutron
b)
Centre
c)
Nucleus
d)
Sub atomic particle
121.
Where are the Electrons found in the structure of an atom?
a)
In the nucleus
b)
In spaces around the nucleus
122.

In a neutral atom,

a)

protons = electrons

b)

protons = neutrons

c)

neutrons = electrons

d)

protons = neutrons = electrons

123.
What is the mass number?
a)
Number of protons plus neutrons
b)
Number of protons plus electrons
c)
Number of neutrons plus electrons
124.
An isotope is an atom with the same number of....
a)
protons and neutrons but a different number of electrons.
b)
neutrons and electrons but a different number of protons.
c)
protons and electrons but a different number of neutrons.
125.
In what order are elements on the modern periodic table?
a)
Mass number
b)
Atomic Mass
c)
Atomic number
d)
Relative Atomic Mass
126.

How many protons does Nitrogen have?

a)

7

b)

8

c)

14

d)

14.01

127.

If an element has an atomic number of 11 and a mass number of 23, how many neutrons does it have?

a)

11

b)

12

c)

23

d)

34

128.

An element has 17 protons and 18 neutrons in the nucleus. What is the element's mass number?

a)

17

b)

18

c)

1

d)

35

129.

Which of the labeled structures is an electron?

a)

a

b)

b

c)

c

130.

Which of the labeled structures is a neutron?

a)

a

b)

b

c)

c

131.

How many electrons can the first shell hold?

a)

4

b)

8

c)

2

d)

18

132.

What is an element?

a)

A combination of two or more substances that are chemically combined

b)

A pure substance made of two or more elements chemically combined

c)

A substance made of atoms with different numbers of protons

d)

A substance made of atoms that all contain the same number of protons

133.

What is a compound?

a)

A mixture of elements that can be separated by physical means

b)

A pure substance made of two or more elements chemically combined

c)

A combination of two or more substances that are not chemically combined

d)

A substance made of atoms that all contain the same number of protons

134.

What is the charge of a neutron?

a)

1+

b)

1-

c)

2+

d)

Neutral

135.

What does the atomic number represent?

a)

The number of neutrons in an atom

b)

The mass of an atom

c)

The total number of protons and neutrons in the nucleus

d)

The number of protons in the nucleus of an atom

136.

How many electrons can the first shell hold?

a)

4

b)

8

c)

2

d)

18

137.

What is the electronic configuration of sodium?

a)

2,8,1

b)

2,8

c)

2,1

d)

2,8,2

138.

What are isotopes?

a)

Atoms of different elements with the same number of protons

b)

Different atoms of the same element with different numbers of neutrons

c)

Atoms that have the same mass number

d)

Atoms that are chemically combined

139.

What is the relative atomic mass unit based on?

a)

The mass of a nitrogen atom

b)

The mass of a hydrogen atom

c)

The mass of a carbon-12 atom

d)

The mass of an oxygen atom

140.

Which of the following is a characteristic of noble gases?

a)

They have full outer shells of electrons

b)

They are highly reactive

c)

They have no electrons

d)

They are found in Group I

141.

What is the mass number of an atom?

a)

The total number of protons and electrons

b)

The total number of protons and neutrons

c)

The number of neutrons only

d)

The number of protons only

142.

75% of naturally occurring chlorine is Cl-35. The remaining chlorine is Cl-37. Which of the below equations shows how to calculate the relative atomic mass of chlorine?

a)

(75x37) + (25x35) / 100 = 35.5

b)

(75x35) + (25x37) / 100 = 35.5

c)

(75x37) + (25x35) / 100 = 35

d)

(75x35) + (25x37) / 100 = 37

143.

A solution containing the maximum amount of dissolved solute is referred to as...

a)

Unsaturated

b)

Insaturated

c)

Asaturated

d)

Saturated

144.

If you were using simple evaporation, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

145.

If you were using distillation, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

146.

What is the electron configuration of the ion this atom would form?

a)

2,6

b)

2,7

c)

2

d)

2,8

147.

Why are the noble gases so unreactive?

a)

They made a group decision not to react

b)

They have a large number of electrons

c)

They don't like to give up electrons

d)

They have a full outer shell of electrons

148.

What is the correct description of this atom?

a)

It has an atomic number of 3, and an atomic mass of 5

b)

It has an atomic mass of 6, and an atomic number of 6

c)

It has an atomic number of 3, and an atomic mass of 6

d)

It has an atomic mass of 6, and an atomic number of 9

149.

Which of the following is the Bohr Model of Nitrogen?

a)

b)

c)

d)

150.

What is wrong with this Bohr Model of Oxygen?

a)

The nucleus needs should have electrons.

b)

There are not enough electrons in the first orbital.

c)

This is actually correct.

d)

The electron pairing is incorrect.

e)

This is the Bohr Model of Sulfur.

151.

Which of the following is the Bohr Model of Silicon?

a)

b)

c)

d)

152.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
153.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
154.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
155.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
156.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
157.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
158.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
159.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
160.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
161.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
162.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
163.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
164.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
165.
The electrons of an atom are found...
a)
in the outer "cloud" surrounding the atom.
b)
in the nucleus of the atom.
c)
in the cloud and in the nucleus.
166.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
167.
How are elements on the periodic table arranged by?
a)
in alphabetic order
b)
simular physical & chemical properties
c)
their symbols
d)
Just simular physical properties
168.
Two elements chemically bonded form
a)
element
b)
compound
c)
mixture
d)
solutions
169.
What element is will have the most similar physical and chemical properties to the element Sulfur (S)?
a)
Carbon (C)
b)
Phosphorous (P)
c)
Oxygen (O)
d)
Neon (Ne
170.
What element is will have the most similar physical and chemical properties to the element Lithium (Li)?
a)
Sodium (Na)
b)
Magnesium (Mg)
c)
Beryllium (Be)
d)
Calcium (Ca)
171.
What element is will have the most similar physical and chemical properties to the element Bromine (Br)?
a)
Fluorine (F)
b)
Carbon (C)
c)
Krypton (Kr)
d)
Selenium (Se)
172.
What element is will have the most similar physical and chemical properties to the element Nitrogen (N)?
a)
Phosphorous (P)
b)
Carbon (C)
c)
Oxygen (O)
d)
Sulfur (S)
173.
Elements that are arranged in __________ have the most similar physical and chemical properties to each other.
a)
periods
b)
groups
174.
All matter is composed of (contains) at least one element on the periodic table
a)
True
b)
False
175.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
176.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
177.

What are the three main groups of the periodic table?

a)

groups

b)

metal

c)

nonmetals

d)

metalloids

e)

periods

178.

What do the vertical columns on the periodic table tell us?

a)

The number of orbitals

b)

The number of valence electrons (electrons on the outer most shell)

179.

What do the horizontal rows on the periodic table tell us?

a)

The number of orbitals

b)

The number of valence electrons (the electrons on the outer most shell)

180.
What is the symbol for Potassium?
a)
P
b)
K
c)
Pb
d)
Pd
181.
What is the symbol for Carbon?
a)
C
b)
Ca
c)
Cl
d)
H
182.
What family is Sodium a part of?
a)
Transition Metals
b)
Halogens
c)
Alkali Metals
d)
Alkaline Earth Metals
183.
What family is silver a part of?
a)
Transition Metals
b)
Noble Gases
c)
Alkali Metals
d)
Alkaline Earth Metals
184.
What family is Cadmium a part of?
a)
Noble Gases
b)
Metalloids
c)
Transition Metals
d)
Actinoids
185.
Silicon is a 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Halogen
186.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
187.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
188.
Who first developed the Periodic Table?
a)
Mendeleev
b)
Mosely
c)
Mendella
d)
Murphy
189.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
190.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
191.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
192.

Who created the first Periodic Table

a)

Dmitri Mendeleev

b)

Albert Einstein

c)

Planck

d)

Heisenberg

193.

Which of the following elements is in the same period as Phosphorus?

a)

Sodium

b)

Oxygen

c)

Neon

d)

Gold

194.

Most of the elements are in the________________ category.

a)

Noble gases

b)

Metals

c)

Non-metals

d)

metalloids

195.

Which of the following is an alkali metal?

a)

Tin

b)

Carbon

c)

Nitrogen 

d)

Lithium

196.

 Which of the following elements is a metal?

a)

H

b)

Ar

c)

Zn

d)

B

197.

Li, Cs, and Na belong to

a)

Transition metals

b)

Halogens

c)

Alkali metals

d)

Alkaline Earth metal

198.

Hydrogen can be classified as 

a)

Metal

b)

Nonmetal

c)

Alkali metal

d)

Transition metal

199.

As the atomic number increase, ______________ contributes to the increase in atomic size within a group in the periodic table.

a)

a. Electron repulsion 

b)

b. More shielding of the nucleus by electrons from inner to outer energy levels

c)

c. The proton number 

d)

d. The ionic energy

200.

Elements in the same group of the periodic table always have the same number of _______ as one another.

a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
201.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
202.

What type of elements are poor conductors of heat and electricity?

a)

transition metals

b)

inner transition metals

c)

metals

d)

nonmetals

203.

Neutron are a sub-atomic particle that

a)

Is found in the nucleus

b)

flying around the nucleus

c)

have a positive charge

d)

have a negative charge

204.

What property is the same for every atom of an element?

a)

energy

b)

mass number

c)

atomic number

d)

number of neutrons

205.

Rubidium is in Group I of the Periodic Table and bromine is in Group VII. Rubidium reacts with bromine to form an ionic compound. Which row shows the electron change taking place for rubidium and the correct formula of the rubidium ion?

a)

A

b)

B

c)

C

d)

D

206.

The relative atomic mass of chlorine is 35.5. When calculating relative atomic mass, which particle is the mass of a chlorine atom compared to?

a)

a neutron

b)

a proton

c)

An atom of carbon - 12

d)

an atom of hydrogen - 1

207.
What section is the least reactive? 
a)
yellow
b)
red
c)
dark blue
d)
orange
208.

Neon is colorless, a poor conductor of heat and is not able to be stretched. How would it be classified?

a)

Nonmetal

b)

Metalloid

c)

Metal

d)

None of the above

209.

Which group of the periodic table is composed of inert (not reactive) gases?

answer choices

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

210.

Which is a halogen?

a)

Helium

b)

Chlorine

c)

Oxygen

d)

Neptune

211.

Elements in a .................. have similar chemical properties.

a)

period

b)

group

c)

row

212.

I am a nonmetal

I am in period 2

I am in group 16

a)

Ba

b)

Si

c)

O

d)

S

213.

These two elements have similar chemical properties to Barium (Ba).

a)

Ca and Ra, because they are in the same group.

b)

Cs and La, because they are in the same period number.

c)

Ca and Y, because they are 90 degree angle.

214.
Flammability (burns): Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
215.
Boiling Point: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
216.
Ability to rust is this type of property:
a)
Physical property
b)
Chemical property
217.
What is the electronic configuration of Calcium?
a)
2,8,8,1
b)
2,8,8,3
c)
2,8,8,4
d)
2,8,8,2
218.
State the electronic configuration for Fluorine
a)
2,7
b)
2,6
c)
2,8
d)
2,8,1
219.
How many electrons are in the outer shell of halogens?
a)
110
b)
2
c)
7
d)
5
220.

What type of oxide do metals typically form?

a)

Amphoteric oxides

b)

Neutral oxides

c)

Basic oxides

d)

Acidic oxides

221.

What type of oxide do metals typically form?

a)

Amphoteric oxides

b)

Neutral oxides

c)

Basic oxides

d)

Acidic oxides

222.

What is an element?

a)

A combination of two or more substances that are chemically combined

b)

A pure substance made of two or more elements chemically combined

c)

A substance made of atoms with different numbers of protons

d)

A substance made of atoms that all contain the same number of protons

223.

What is a compound?

a)

A mixture of elements that can be separated by physical means

b)

A pure substance made of two or more elements chemically combined

c)

A combination of two or more substances that are not chemically combined

d)

A substance made of atoms that all contain the same number of protons

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