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Chemistry: Material Properties

Total questions: 215

Worksheet time: 7hrs 29mins

Name
Class
Date
1.

Based on the diagram, the ship's bodies had covered with rust as it was always exposed to air and oxygen. Which of the following can be done to cover the rusting process?

a)

Use a nitrogen to slow down the chemical reaction

b)

Coat the bodies with zinc in a process called zinc plating

c)

Change the bodies by using zinc that does not corrode in the air

d)

Coat with sulfur as it does not dissolve in water

2.

Why is copper particularly useful in electrical circuits?

a)

does not corrode in air

b)

very reactive metal

c)

a very good conductor of heat

d)

support burning

3.

Which gases can burn in air?

a)

oxygen

b)

hydrogen

c)

nitrogen

d)

helium

4.

Which of the following happens when sodium reacts with chlorine?

[more than one answer]

a)

sodium chloride produced

b)

sodium sulfide produced

c)

bright light and white solid compound

d)

bright light and black solid compound

5.

calcium + oxygen ---> _____________

a)

calcium dioxide

b)

calcium oxygen

c)

calcium oxide

d)

calcium carbonate

6.

What happens when sulfur is heated?

a)

combine with oxygen and produces sulfuric acid

b)

combine with oxygen and produce sulfur dioxide

c)

combine with oxygen and produce sulfur oxide

7.

Brittle

a)

Metal

b)

Non metal

c)

None of them

d)

Both metal and non-metals

8.

Iron is a good conductor, malleable and magnetic. What type of element is Iron?

a)

Metal

b)

Non-metal

c)

Metalloid

d)

None of the above

9.

Name the metal which is in liquid state.

a)

Iron

b)

Mercury

c)

Zinc

d)

Aluminium

10.

Able to be beaten or hammered into shapes

a)

lustre

b)

malleable

c)

brittle

d)

insulator

11.
Good conductor of heat
a)
Metal
b)
Nonmetal
12.
Which of the following is a metal?
a)
chlorine
b)
sodium
c)
Oxygen
13.
What is NOT a property of metals
a)
brittle
b)
ductile
c)
malleable
d)
conductor
14.
What property of metals means that heat and electricity can move easily through?
a)
luster
b)
conductor
c)
malleable
d)
ductile
15.

Which words best describe NON-METALS?

a)

ductile, shiny, brittle

b)

malleable, dull, brittle, ductile

c)

brittle, dull, insulators

16.

Are metals good insulators?

a)

No

b)

Yes

17.

During the chemical reaction, METALS _____ electrons, while NON-METALS____ electrons

a)

lose

gain

b)

gain

lose

c)

both lose

d)

lose

stay the same

18.

Flourine is a metal

a)

True

b)

False

19.

Lithium can be used to make

a)

Chocolate

b)

Battery

c)

Wires

d)

Medicines

20.

Able to be drawn into wire is

a)

malleable

b)

insulator

c)

lustre

d)

ductile

21.
Which element is a metalloid?
a)
Titanium
b)
Selenium
c)
Potassium
d)
Polonium
22.
All of the following would classify an element as a metal except?
a)
Dull
b)
Luster
c)
Malleable
d)
Hard
23.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
24.

1.       Materials that produces a ringing sound when hit against a hard surface is:

 

a)

Sound sensitive

b)

Sonorous

c)

Soundorous

25.

2.      Which of the following pairs of materials are sonorous?

 

a)

Iron  & aluminum

b)

Iron & plastic

c)

Ceramic & glass

26.

Silver

a)

S

b)

Ag

c)

Au

d)

Sn

27.

Carbon

a)

C

b)

Ca

c)

Cu

d)

Cr

28.

Neon

a)

No

b)

Na

c)

Ne

d)

Ni

29.

Sodium

a)

Ne

b)

S

c)

Na

d)

Mg

30.

Plutonium

a)

Pu

b)

Pt

c)

P

d)

Po

31.

Sulfur

a)

S

b)

Sn

c)

Na

d)

Sr

32.

Fluorine

a)

Fl

b)

Ra

c)

Fr

d)

F

33.

Copper

a)

Cu

b)

C

c)

Cr

d)

Co

34.

W

a)

Tungsten

b)

Mercury

c)

Gold

d)

Copper

35.

Pb

a)

Plutonium

b)

Lead

c)

Platinum

d)

Radon

36.

Mo

a)

Mercury

b)

Molybdemum

c)

Magnesium

d)

Manganese

37.

Zn

a)

Magnesium

b)

Silver

c)

Zerconium

d)

Zinc

38.

Ar

a)

Aluminum

b)

Argon

c)

Radon

d)

Oxygen

39.

O

a)

Oxygen

b)

Carbon

c)

Boron

d)

Silicon

40.

K

a)

Tungsten

b)

Fluoride

c)

Krypton

d)

Potassium

41.
H is the chemical symbol for which element?
a)
Helium
b)
Hydrogen
c)
Mercury
42.
Na is the chemical symbol for which element? 
a)
Sodium
b)
Nitrogen
c)
Neon
43.
K is the chemical symbol for which element? 
a)
Krypton
b)
Potassium
c)
Knox
44.
Ca is the chemical symbol for which element? 
a)
Carbon
b)
Chlorine
c)
Calcium
45.
Fe is the chemical symbol for which element? 
a)
Freon
b)
Iron
c)
Flourine
46.
C is the chemical symbol for which element? 
a)
Calcium
b)
Chlorine
c)
Carbon
47.
N is the chemical symbol for which element? 
a)
Sodium
b)
Nitrogen
c)
Nickel
48.
O is the chemical symbol for which element? 
a)
Osmium
b)
Odell
c)
Oxygen
49.
Si is the chemical symbol for which element? 
a)
Silicon
b)
Sodium
c)
Sulfur
50.
He is the chemical symbol for which element? 
a)
Heehaw
b)
Helfion
c)
Helium
51.
The chemical symbol for hydrogen is
a)
Hy
b)
He
c)
H
52.
The chemical symbol for sodium is
a)
S
b)
So
c)
Na
53.
The chemical symbol for potassium is
a)
Po
b)
K
c)
Ko
54.

The chemical symbol for calcium is

a)

C

b)

Ca

c)

Na

55.
The chemical symbol for iron is
a)
I
b)
Fi
c)
Fe
56.
The chemical symbol for carbon is
a)
C
b)
Ca
c)
Na
57.
The chemical symbol for nitrogen is
a)
N
b)
Ni
c)
Na
58.
The chemical symbol for oxygen is
a)
Ox
b)
Pa
c)
O
59.
The chemical symbol for silicon is
a)
S
b)
Sa
c)
Si
60.
The chemical symbol for helium is
a)
H
b)
He
c)
Ha
61.

Which correctly shows the molecule we breathe out?

a)

CO2(l)

b)

CO2(aq)

c)

CO2(g)

d)

CO2(s)

62.

What is a precipitate?

a)

A solid formed in a liquid

b)

A liquid

c)

A gas

d)

A gas formed in a liquid

63.

What happens to salt when it is stirred in hot water?

a)

it solidifies

b)

it disrupts

c)

it melts

d)

it dissolves

64.

What is the name of this compound:

NaCl?

Na = sodium

Cl = chlorine

a)

chloride sodium

b)

sodium chlorine

c)

sodium chloride

d)

chlorine sodiumide

65.

Which of the following is the correct chemical formula for iron sulfide?

a)

fes

b)

FES

c)

FeS

d)

fEs

66.

What compound is formed when aluminium reacts with iodine?

a)

Aluminium iodide

b)

Iodine aluminiumide

c)

Iodine aluminium

d)

Aluminium iodinide

67.

The smallest part of any element. Made up of protons, neutrons and electrons.

a)

Atom

b)

AMU

c)

Ion

d)

Isotope

68.

The atomic mass is the

a)

number of protons and neutrons inside the nucleus

b)

number or electrons or protons

c)

number of protons, neutrons and electrons

69.

All matter is made of _________.

a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
70.

What did Dmitri Mendeleev invent?

a)

Chemistry

b)

Periodic Table

c)

Atoms

d)

Calculator

71.
What is at the center of every atom?
a)
An electron
b)
A compound
c)
A molecule
d)
A nucleus
72.
If an atom has 3 electrons, how many protons does it have?
a)
1
b)
2
c)
4
d)
3
73.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
74.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
75.
The positively charged particles of an atom are the ________.
a)
electrons
b)
protons
c)
neutrons
d)
protons & neutrons
76.
The particles with no charge in an atom are the _______.
a)
electrons
b)
neutrons
c)
protons
d)
protons and neutrons
77.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
78.

How many atoms of hydrogen are in this compound?

a)

1

b)

2

c)

3

d)

4

79.

How man atoms of carbon are there?

a)

1

b)

2

c)

3

d)

4

80.

How many atoms of Iron are in this compound?

a)

1

b)

2

c)

3

d)

4

81.

How many atoms of hydrogen are in

C6H12O6

a)

6

b)

12

c)

18

d)

2

82.

How many atoms of oxygen are in

3Fe2O3

a)

6

b)

9

c)

18

d)

2

83.

Select the chemical formula for this molecule?

a)

B1F3

b)

BF

c)

BF3

d)

FB

84.

What is the chemical formula for this molecule?

a)

H1F2

b)

H1F1

c)

HF

d)

HeF

85.

What is the chemical formula for this molecule?

a)

H1O2

b)

H1O1

c)

HO

d)

H2O2

86.

What is the chemical formula for this molecule?

a)

C1I4

b)

C1I1

c)

CI4

d)

C2I2

87.

What is the chemical formula for this molecule?

a)

N2He4

b)

NeH3

c)

N2H4

d)

N2H2

88.

A substance made up of atoms of two or more different elements joined by chemical bonds

a)

Molecule

b)

compound

c)

polar covalent bond

d)

nonpolar covalent bond

89.

How many atoms of oxygen are in this compound?

2Ca(OH)2

a)

1

b)

2

c)

3

d)

4

90.
K20 - name?
a)
potassium dioxide
b)
potassium oxide
c)
potassium oxygen
d)
dipotassium dioxide
91.

CaF2- name?

a)

calcium fluorate

b)

calcium fluoride

c)

fluoride calcite

d)

fluorine calciumate

92.

Na2SO4- name?

a)

sulfur sulfate

b)

sodium sulfide

c)

sodium sulfate

d)

sodium oxygenate

93.

LiNO3- name?

a)

lithium oxygenate

b)

nitrogen lithate

c)

lithium nitride

d)

lithium nitrate

94.

MgO- name?

a)

oxygen magnesium

b)

magnesium oxide

c)

magnesium oxate

d)

magnesium oxygenate

95.

LiOH- name?

a)

hydrogen lithium

b)

lithium oxyhydride

c)

lithium oxide

d)

lithium hydroxide

96.

KOH

a)

Carbon oxide

b)

potassium oxide

c)

potassium hydride

d)

potassium hydroxide

97.
What is the correct name of the compound with the formula MgO?
a)
magnesium oxygen
b)
magnesium oxide
c)
manganese oxygen
d)
manganese oxide
98.
What is the correct name of the compound with the formula KH?
a)
potassium hydrogen
b)
potassium peroxide
c)
potassium hydride
d)
potassium monohydride
99.
What is the correct name of the compound with the formula CaO?
a)
calcium oxide
b)
calcium oxygen
c)
calcium monoxide
d)
monocalcium monoxide
100.

The name for the ionic compound NaF is

a)

Sodium fluoride

b)

Nappium fluoride

c)

Sodium fluorine

d)

Fluorine sodiumide

101.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

102.

__ is a pure substance containing two or more kinds of atoms.

a)

Element

b)

compound

c)

mixture

d)

solution

103.

What is the name of the compound LiCl?

a)

Lithium Chlorine

b)

Lithiide Chloride

c)

Lithiide Chlorine

d)

Lithium Chloride

104.

What is the name of the compound K2S?

a)

Potassium Sulfur

b)

Potassium Sulfide

c)

Krypton Sulfide

d)

Krypton Sulfur

105.

What is the name of the compound BaF2?

a)

Barium Fluorine

b)

Barium Fluoride

c)

Boron Fluoride

d)

Born Fluorine

106.

What is the formula for Potassium Iodide?

a)

PI

b)

KI

c)

PI2

d)

KI2

107.

What is the formula for Sodium Fluoride?

a)

SF

b)

SFl

c)

NaF

d)

NaFl

108.

What is the formula for Magnesium Chloride?

a)

MgCl

b)

MgCl2

c)

MnCl

d)

MnCl2

109.

What is the formula for Calcium Sulfide?

a)

CaS

b)

CaS2

c)

CaSe

d)

CaSe2

110.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
111.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
112.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
113.

A substance made by mixing other substances together

a)

Sediment

b)

Insoluble

c)

Suspension

d)

Mixture

114.

The substance in which a solute dissolves to produce a Mixture.

a)

Colloid

b)

Evaporation

c)

Decanting

d)

Solvent

115.

The substance that dissolves in a solvent to produce a mixture.

a)

Solute

b)

Immiscible Liquid

c)

Decanting

d)

Mixture

116.

The process by which water changes from a liquid to a gas or vapor.

a)

Condensation

b)

Evaporation

c)

Immiscible Liquid

d)

Solution

117.

The process of pouring away a liquid while leaving a solid behind.

a)

Insoluble

b)

Sediment

c)

Decanting

d)

Dissolving

118.

A substance (solid) that will not dissolve in a solvent even after mixing 

a)

Colloid

b)

Mixture

c)

Dissolving

d)

Insoluble

119.

 The process in which solid particles in a liquid or gaseous fluid are removed by the use of a filter medium 

a)

Mixture

b)

Decanting

c)

Filtration

d)

Evaporation

120.

The conversion of a liquid into vapor that is subsequently condensed back to liquid form.

a)

Dilute

b)

Distillation

c)

Compound

d)

Concentrate

121.

Substance made up of different elements joined together by a chemical bond

a)

Dilute

b)

Condensing

c)

Compound

d)

Concentrate

122.

Make (a liquid) thinner or weaker by adding water or another solvent to it.

a)

Dilute

b)

Distillation

c)

Compound

d)

Condensing

123.

This method is a technique used in separating a less-dense substance from a denser one.

a)

decantation

b)

evaporation

c)

distillation

d)

filtration

124.

This technique is based on the differences of the boiling point of the substance in the mixture.

a)

decantation

b)

distillation

c)

filtration

d)

chromatography

125.

This method is useful in a pharmaceutical industry in determining the amount of each chemical in each product.

a)

distillation

b)

chromatography

c)

sieving

d)

decantation

126.

This method is used in separating soluble solid from a liquid such as salt from water.

a)

evaporation

b)

distillation

c)

decantation

d)

filtration

127.
How do you separate iron filings from sand?
a)
You can use a filter.
b)
You can use a fagnet.
c)
You can use a magnet.
d)
You can use all of the methods!
128.

Which of of these mixtures could be separated by filtration?

a)

sugar and milk

b)

sand and water

c)

milk and water

d)

sugar and water

129.

You want to see what colors are all present in a solution. What method would you use?

a)

chromatography

b)

flotation

c)

mangetism

d)

sifting

130.

Which of the following best describes chromatography?

a)

A solid is stirred in a liquid to make the solid float to the top.

b)

A solution is heated until all the liquid turns to gas to leave a solid behind.

c)

A solvent moves solutes up a paper based on how well the solute dissolves in the solvent.

d)

A mixture of solids is put in a container that allows small particles to leave the container.

131.

How to separate sugar and water?

a)

Decantation

b)

Distillation

c)

Filtration

d)

Evaporation

132.

How to separate iron filings from flour?

a)

Distillation

b)

Evaporation

c)

Filtration

d)

Magnetic Attraction

133.

What are the subatomic particles?

a)

Protons, Electrons, Neutrons

b)

Molecules, and atoms

c)

Electrons, Protons, Nucleus

d)

Nucleus, and Electrons

134.

What is this subatomic particle that has positive charge?

a)

Electron

b)

Neutron

c)

Proton

d)

Megatron

135.

What is this subatomic particle that has negative charge?

a)

Electron

b)

Neutron

c)

Proton

d)

Megatron

136.

What is this subatomic particle that has no charge?

a)

Electron

b)

Neutron

c)

Proton

d)

Megatron

137.

What is the smallest particle of an ELEMENT, and it has also all the properties of it?

a)

Molecules

b)

Nucleus

c)

Subatomic particle

d)

Atoms

138.

What is the small, DENSE REGION consisting of protons and neutrons at the CENTER of an atom?

a)

Molecules

b)

Nucleus

c)

Subatomic particle

d)

Atoms

139.

It is consisting of two or more atoms combined together in a specific arrangement. It is the smallest particle of compound that can exist independently. What is this?

a)

Molecules

b)

Nucleus

c)

Subatomic particle

d)

Atoms

140.

Where can we find the location of the Atomic Nucleus?

a)

Center

b)

Left Side

c)

Right Side

d)

Above

141.

What is the atomic model proposed by J.J Thompson, and suggest that negatively-charged electrons were embedded in a kind of cloud or soup of positive charge?

a)

Asia's Next Top Model

b)

Quantum Atomic Model

c)

Plum Pudding Model

d)

Nuclear Model

142.

How many elements are in this compound formula [H2O2 ]?

a)

2

b)

4

c)

8

d)

1

143.

How many atoms total are there in this compound Na3(OH)?

a)

3

b)

2

c)

4

d)

5

144.

How many protons does an O2 atom have?

a)

7

b)

8

c)

16

d)

24

145.

An atom is said to be neutral if it has same number of electrons and...…..

a)

electrons

b)

protons

c)

neutrons

d)

ions

146.

The subatomic particle has almost no mass is.....................

a)

proton

b)

electron

c)

neutron

d)

no correct answer

147.

This is how you find the number of neutrons in an atom.

a)

Subtract atomic number from atomic mass

b)

Divide atomic mass by the atomic number.

c)

Subtract the atomic mass from the atomic number.

d)

Add atomic mass to the atomic number.

148.

The atomic mass is the number of .................+ ........................

a)

protons , electrons

b)

electrons, neutrons

c)

protons , neutrons

d)

positive ion , negative ion

149.

The Atomic number is known as the _______

a)

Number of electrons in an atom

b)

Number of Protons in an atom

c)

Number of neutrons in an atom

d)

Number of Protons and electrons in an atom

150.
In this picture, the Electrons are found in which color?
a)
Blue
b)
Red
c)
Green
151.
The subatomic particles in green are...
a)
Protons
b)
Neutrons
c)
Electrons
152.
Where are the Electrons found in the structure of an atom?
a)
In the nucleus
b)
In spaces around the nucleus
153.
Where is the nucleus located in an atom?
a)
Near the electron shells/levels
b)
Near the center of an atom
154.
Niels Bohr suggested that electrons.......
a)
are found in specific orbits
b)
electrons are scattered throughout the atom
c)
electrons move according to their energy level
d)
electrons are positive
155.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
156.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
157.

Choose the correct description of J. J. Thomson's Model of an Atom.

a)

The model is a indivisible and indestructible sphere

b)

The model is a semi-solid sphere in which negatively charged particles with very little mass - electrons- float freely in a positively-charged "pudding" of greater mass.

c)

The model is a sphere in which negatively charged particles - electrons- move around the center of an atom creating an electron cloud

d)

The model is a sphere in which negatively charged particles - electrons - move around the nucleus of an atom in a defined passes, called orbits, like planets around the sun

158.

Why did Ernest Rutherford and his colleagues perform the Gold-Foil Experiment?

a)

They wanted to test and confirm the Plum-Pudding model

b)

They wanted to test John Dalton's Model

c)

They were looking for electrons

d)

They wanted to come up with their own Atomic Model

159.

Which of the following is the best evidence that the particles that make up a cathode ray had a negative charge?

a)

The particles were produced by many different metals.

b)

The ray was attracted toward a positive electric field.

c)

Line emission spectra for an element are always the same.

d)

The ray caused a phosphorescent screen to glow.

160.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
161.

JJ Thomson's experiment that he used to discover electrons

a)

gold foil experiment

b)

cathode ray experiment

c)

neither of these is correct

d)

hydrogen atom emission spectra

162.

Choose one of the conclusions that Ernest Rutherford made based on the experimental results of his Gold-Foil experiment

a)

He concluded that the atom is indivisible

b)

He concluded that the atom is mostly empty space

c)

He concluded that the atom has neutrons

d)

He concluded that the atom is tightly packed with subatomic particles all mixed together

163.

Based on Rutherford's model of the atom, electrons in the atom are located

a)

inside of the nucleus of the atom

b)

outside and around the nucleus of the atom

c)

outside and inside of the nucleus of the atom

d)

flowing freely around the positive "pudding"

164.

Who discovered the neutron?

a)

JOSEPH JOHN THOMSON

b)

ERNEST RUTHERFORD

c)

NEILS BOHR

d)

JAMES CHADWICK

165.

Who discovered the proton?

a)

JOSEPH JOHN THOMSON

b)

ERNEST RUTHERFORD

c)

NEILS BOHR

d)

JAMES CHADWICK

166.

Who discovered the electron?

a)

JOSEPH JOHN THOMSON

b)

ERNEST RUTHERFORD

c)

NEILS BOHR

d)

DEMOCRITUS

167.
Who's model is this?
a)

Thompson

b)
Rutherford
c)
Democritus
d)
Bohr
168.
Who came up with this model?
a)
Dalton
b)

Thompson

c)
Rutherford
d)
Bohr
169.

Where are the electrons found?

a)

In the nucleus

b)

The same place as the protons

c)

In shells

d)

The same place as neutrons

170.

The first electron shell can old how many electrons?

a)

8

b)

2

c)

6

d)

4

171.

The second electron shell can old how many electrons?

a)

8

b)

2

c)

6

d)

4

172.

The correct electron configuration for sodium is....

a)

2, 8, 2

b)

2

c)

2, 8

d)

2, 8, 1

173.

Elements in group 1 have how many electrons in the outer shell?

a)

4

b)

1

c)

6

d)

8

174.

Elements in group 5 have how many electrons in the outer shell?

a)

1

b)

4

c)

6

d)

5

175.

The noble gases are ____ as a result of having a full outer shell.

a)

Volatile

b)

Reactive

c)

Stable

d)

Electronegative

176.

Which of the following is an electron configuration of an element from period 3? (you can pick more than one answer)

a)

2,5

b)

2,8

c)

2,8,1

d)

2,1

177.

What is the capacity of the second electron shell?

a)

2

b)

4

c)

6

d)

8

178.

The number of electrons is the same as the number of neutrons.

a)

True

b)

False

179.

Which statement best describes the arrangement of elements in the periodic table?

a)

Elements are arranged in decreasing atomic mass from left to right.

b)

Elements are arranged in decreasing atomic number from left to right.

c)

Elements are arranged in increasing atomic number from left to right

d)

Elements are arranged in increasing number of neutrons from left to right.

180.

He, Ne, and Ar are all noble gases. What is common among these gases?

a)

They are flammable.

b)

They are highly reactive.

c)

They are metals.

d)

They are unreactive.

181.

Which metal explodes when exposed to water

a)

Alkali

b)

Alkali Earth

c)

Transition

182.

Group 2 on the periodic table are the

a)

Alkali metals

b)

Alkali Earth Metals

c)

Transition Metals

183.

Group 1

a)

Alkali Metals

b)

Alkali Earth Metals

c)

Transition Metals

184.
Which of the following is the most reactive in water?
a)
Lithium
b)
Sodium
c)
Potassium
185.

Alkali are so reactive to air they are generally stored in what?

a)

Water

b)

Oil

c)

Vaults

d)

Cotton

e)

a vacuum

186.
As Alkali Metals atomic number increases their melting point?
a)
Increases
b)
Decreases 
c)
Stays the same
187.
--------------------- is released when alkali metal react with water
a)
Hydrogen
b)
Oxygen
c)
Metahne
d)
Carbon di oxide
188.

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

a)

increases

b)

decreases

189.

Which alkali metal is the least reactive?

a)

lithium

b)

sodium

c)

potassium

d)

rubidium

190.

Which of the following is not an alkali metal

a)

Sodium

b)

Caesium

c)

Francium

d)

Calcium

e)

Potassium

191.

What is produced when an alkali metal reacts with water?

a)

Metal oxide + Oxygen

b)

Metal oxide + Hydrogen

c)

Metal hydroxide + Oxygen

d)

Metal hydroxide + Hydrogen

192.

What are the products of the reaction between an alkali metal and oxygen?

a)

Metal oxide + Hydrogen

b)

Metal oxide

c)

Metal hydroxide + hydrogen

d)

Metal hydroxide

193.

Which of the following does NOT describe alkali metals?

a)

Shiny

b)

Soft

c)

High density

d)

Good conductivity

194.

What is the trend for the reactivity of alkali metals?

a)

Reactivity decreases down the group.

b)

Reactivity increases down the group.

c)

Reactivity increases up the group.

d)

There is no change in reactivity.

195.

When added to water, which alkali metal burns with a lilac flame and whizzes across the surface of the water?

a)

Lithium

b)

Sodium

c)

Potassium

d)

Rubidium

196.

How many valence electrons do Alkaline Earth Metals have?

a)

1

b)

2

c)

3

d)

7

197.

Which metal is NOT an Alkaline Earth Metal?

a)

Calcium

b)

Radon

c)

Strontium

d)

Radium

198.

Alkali Metals are brittle

a)

True

b)

False

199.

Alkaline Earth metals conduct heat and electricity

a)

True

b)

False

200.

Compounds of Alkaline Earth Metals form _____ solutions

a)

Basic (Bases)

b)

Acidic (Acids)

201.

The letter(s) used to represent an element, instead of its full name.

a)

Atomic branding

b)

Chemical symbol

c)

Elemental letters

d)

Element mark

202.

A combination of chemical symbols that show which elements a substance is made up of.

a)

Chemical formula

b)

Substance recipe

c)

Periodic formula

d)

Composition symbol

203.

When a more reactive element replaces a less reactive element in a compound.

a)

Combustion

b)

Replacement reaction

c)

Displacement reaction

d)

Knock-out reaction

204.

Which of these elements are Halogens?

a)

Fluorine

b)

Helium

c)

Zinc

d)

Bromine

205.

Halogens are the elements of group:

a)

1

b)

2

c)

7

d)

8

206.

Fluorine and Chlorine are ____________at room temperature.

a)

gases

b)

liquids

c)

solids

d)

amorphous

207.

Bromine is _____________ at room temperature.

a)

gas

b)

liquid

c)

solid

d)

none

208.

The melting and boiling points of halogens:

a)

decrease down the group

b)

increase down the group

c)

remain constant

d)

none

209.

The atomic number and atomic mass of halogens:

a)

increase down the group

b)

decrease down the group

c)

remains constant

d)

none

210.

Halogens exist in the:

a)

monoatomic state

b)

diatomic state

c)

triatomic state

d)

none

211.

______________is commonly used as an antiseptic and is used to make drinking water safe and to treat swimming pools.

a)

Fluorine

b)

Chlorine

c)

Bromine

d)

Iodine

212.

The atomic number of chlorine is 17, how many electrons does it contain?

a)

8

b)

17

c)

35

d)

none

213.

What is the mean of the "halogens"?

a)

acid former

b)

salt former

c)

alkali former

d)

non metal former

214.

Which of the "Halogens" has yellowish green color?

a)

Chlorine

b)

Bromine

c)

Flourine

d)

Iodine

215.

The melting and boiling points of halogens:

a)

decrease down the group

b)

increase down the group

c)

remain constant

d)

none

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