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Worksheets

Erhama - Chemistry

Total questions: 205

Worksheet time: 5hrs 13mins

Name
Class
Date
1.

Name the type of bonding in which the electrons are shared.

a)

Ionic bonding

b)

Covalent bonding

c)

Metallic bonding

2.

The covalent bond forms between

a)

a metal and nonmetal

b)

a nonmetal and nonmetal

c)

a metal and metal

3.

Number of covalent bonds can form in group 16

a)

three

b)

two

c)

four

4.

As bond length increase the strength...

a)

increases

b)

decreases

c)

no change

5.

The energy required to break the bonds between two covalently bonded atoms

a)

bond dissociation energy

b)

activation energy

c)

none of these

6.

The reaction in which the energy released.

a)

endothermic

b)

exothermic

c)

none of these

7.

The number of covalent bonds form in group 17

a)

One

b)

Two

c)

Three

8.

The number of pairs of electrons shared in triple covalent bond

a)

Two

b)

Three

c)

One

9.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
10.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
11.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
12.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
13.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
14.
The chemical bond formed when two atoms share electrons  is called a(an) IONIC bond. 
a)
True
b)
False
15.
The forces between molecules are much STRONGER than the forces between ions. 
a)
True
b)
False
16.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
17.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
18.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
19.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
20.

Ionic or covalent?

NaCl

a)

Ionic

b)

Covalent

21.
Ionic or covalent?
H2O
a)
Ionic
b)
Covalent
22.
what type of bond is the strongest
a)
single
b)
Double
c)
coordination
d)
triple
23.
How many valence electrons does oxygen have?
a)
2
b)
3
c)
6
d)
4
24.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
25.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
26.
How many bonds does carbon have to create in order to satisfy the octet rule
a)
1
b)
2
c)
3
d)
4
27.
How many valence electrons does hydrogen have?
a)
4
b)
3
c)
2
d)
1
28.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
29.
Is this image an example of covalent bonding?
a)
Yes
b)
No
30.
Outer shell electrons are called
a)
outer electrons
b)
valence electrons
c)
negatives
31.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

nothing

b)

gain 7

c)

lose 1

32.

How many valence electrons does Boron have?

a)

1

b)

2

c)

3

d)

4

33.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

34.

Ionic bonds are between

a)

metals and nonmetals

b)

2 metals

c)

2 nonmetals

35.

How are ionic bonds formed?

a)

transfer of electrons

b)

sharing of electrons

36.

Group numbers on the periodic table help us determine

a)

number of valence electrons

b)

state of the element (solid, liquid, gas)

37.

Electrons are involved in chemical reactions, not protons or neutrons.

a)

true

b)

false

38.

Water is an example of what?

a)

molecular compound (covalent compound)

b)

ionic compound

39.

Salt is an example of what?

a)

ionic compound

b)

covalent compound

40.

Atoms involved in a covalent bond are not charged, while atoms involved in an ionic bond are charged (negative or positive)

a)

true

b)

false

41.

Which of the following is the correct Lewis Structure for the molecule fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

42.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
43.

What is the correct Lewis Structure for ammonia (NH3)

a)
b)
c)
d)
44.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
45.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
46.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
47.
How many pi bonds does this have? 
a)
1
b)
2
c)
3
d)
4
48.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
49.
Pi bonds are formed by 
a)
side to side overlap of s orbitals
b)
end to end overlap of s orbitals
c)
side to side overlap of p orbitals
d)
end to end overlap of p orbitals
50.
How many pi bonds are there in a double bond? 
a)
0
b)
1
c)
2
d)
3
51.
How many pi bonds are there in a single bond? 
a)
0
b)
1
c)
2
d)
3
52.
How many sigma bonds are there in a triple bond? 
a)
0
b)
1
c)
2
d)
3
53.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
54.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
55.
An electron has what kind of charge?
a)
no charge
b)
positive 
c)
negative
d)
it depends
56.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
57.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

58.
When the number of electrons equals the number of protons the atom has what charge?
a)
sponge bob
b)
positive charge
c)
negative charge
d)
neutral charge
59.

Ionic bonds are formed from a combination of metal elements and __________________ elements.

a)

non-metal

b)

receive

c)

metal

d)

donate

60.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

61.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

62.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

63.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

64.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

65.

Magnesium Hydroxide is an ionic compound made up from Mg2+ and OH- ions. Which is its correct formula?

a)

MgOH

b)

MgOH2

c)

Mg(OH)2

d)

MgO

66.

negatively charged ions are called what?

a)

anion

b)

cation

c)

ionic bond

d)

dogion

67.

A positively charged ion is called what?

a)

anion

b)

onion

c)

cation

d)

dogion

68.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

69.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
70.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

71.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

72.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

73.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds.

d)

They have many weak bonds.

74.

True or false? Ionic compounds have high melting points.

a)

true

b)

false

75.

True or false? Ionic compounds have low boiling points.

a)

true

b)

false

76.

True or false? Ionic compounds conduct electricity when they are in their solid state.

a)

true

b)

false

77.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

78.

Why do ionic compounds conduct electricity when they are molten or dissolved?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

79.

Magnesium oxide is insoluble in water. Can magnesium oxide conduct electricity?

Select yes or no and a reason.

a)

Yes

b)

No

c)

Magnesium oxide can be heated so that it melts and conducts electricity.

d)

Magnesium oxide doesn't dissolve, so it stays in its solid state and doesn't conduct electricity.

80.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

81.

Which of the following is NOT TRUE about covalent compounds?

a)

They have low melting and boiling points.

b)

They are formed from 2 nonmetals.

c)

They can conduct electricity when dissolved in water (aqueous).

82.

Which element is most likely to form 2 bonds?

a)

Carbon

b)

Sulfur

c)

Nitrogen

d)

Fluorine

83.

Which element is most likely to form 4 bonds?

a)

Carbon

b)

Fluorine

c)

Sulfur

d)

Nitrogen

84.

A single covalent bond is made up of _____ electrons.

a)

one

b)

two

c)

three

d)

four

85.

True or False: Ionic compounds are usually liquids at room temperature.

a)

True

b)

False

86.
In which state does matter completely fill its closed container?
a)
Gas
b)
Liquid
c)
Solid
d)
Ice
87.
Which state of matter has a fixed shape and volume and it's molecules move very slowly?
a)
Liquid
b)
Gas
c)
Solid
d)
Plasma
88.

flammability of a substance

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

89.

size of an object

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

90.

freezing point

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

91.

drawing copper into a wire

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

92.

corrosion of a bicycle frame

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

93.

formation of water when hydrogen burns

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

94.

boiling water

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

95.

a characteristic that can be observed without changing the substance

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

96.

Color is what type of property?

a)

Physical

b)

Chemical

97.

Reactivity is what type of property?

a)

Physical

b)

Chemical

98.

What happens to the atoms of a substance in a physical change?

a)

Atoms get bigger

b)

Atoms change their arrangement and motion

c)

Atoms get smaller

d)

Atoms bond together differently

99.

What happens to the atoms of a substance in a chemical change?

a)

Atoms get bigger

b)

Atoms change their arrangement and motion

c)

Atoms get smaller

d)

Atoms bond together differently

100.

All of the following phases of matter may flow EXCEPT:

a)

plasma.

b)

solid.

c)

liquid.

d)

gas.

101.

List the phases of water in order, from the phase with the slowest molecular movement to the phase with the fastest molecular movement.

a)

Gas-Liquid-Solid

b)

Liquid-Solid-Gas

c)

Solid-Liquid-Gas

d)

Gas-Solid-Liquid

102.

This picture shows an example of

a)

gas

b)

plasma

c)

liquid

d)

solid

103.

The picture shows an example of

a)

gas

b)

plasma

c)

liquid

d)

solid

104.

The picture shows an example of

a)

gas

b)

plasma

c)

liquid

d)

solid

105.
What is a kind of matter that cannot be broken down into any other kind of substance?
a)
Elements
b)
Mixtures
c)
Compounds
d)
Density
106.
Which property is extensive?
a)
density
b)
mass
c)
color
d)
none of the above
107.
Luster (how shiny something is) is considered a
a)
Physical property
b)
Chemical Property
108.
Basic building block of physical matter: cannot be broke down to a simpler structure.
a)
Molecule 
b)
Element 
c)
Solution 
d)
Atom
109.
The Smallest unit of an element 
a)
Atom
b)
Element 
c)
Cell 
d)
Compound
110.
A chemical reaction involving the rearrangement of the atoms of one or more substances
a)
Physical Change
b)
Chemical Change 
c)
Physical Science
d)
Conservation of Matter
111.

The temperature at which a substance boils.

a)

Melting point

b)

Boiling point

c)

Thermal conductivity

d)

Electrical conductivity

112.

An object's melting point is_____________________.

a)

the temperature at which a substance boils

b)

the temperature at which a substance goes from a solid to a liquid

c)

a physical characteristic

d)

a chemical charateristic

113.

An object or substance always has both physical and chemical properties.

a)

True

b)

False

114.

Which is the best definition of an intensive property?

a)

A property that changes as the amount of a substance increases or decreases

b)

A property that is so extreme it can only be described as intense

c)

A property that does not depend on the amount of a substance present

d)

A property that is only found on the inside of a material

115.
Which is most accurate?
a)
Gasses have the greatest kinetic energy
b)
Liquids have the greatest kinetic energy
c)
Solids have the greatest kinetic energy
d)
None have the greatest kinetic energy
116.

What types of property would volume be described as?

a)

Physical and extensive

b)

Physical and intensive

c)

Chemical and extensive

d)

Chemical and intensive

117.

Which is the best description of a liquid?

a)

definite shape and definite volume

b)

indefinite shape and definite volume

c)

definite shape and indefinite volume

d)

indefinite shape and indefinite volume

118.

What does H2O represent?

a)

An element

b)

A compound

c)

A homogeneous mixture

d)

A heterogeneous mixture

119.

Which is the most compressible state of matter?

a)

Solid

b)

Liquid

c)

Gas

120.
Anything that has mass and takes up space.
a)
volume
b)
matter
c)
solid
d)
temperature
121.
Carbon
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
122.
NaCl
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
123.

Why are both hydrogen and cesium s-block elements, when hydrogen has one electron and cesium has 55?

a)

All blocks contain at least one element from each period.

b)

Blocks of elements on the periodic table are based only on an element's valence electrons.

c)

The s-block includes only the most reactive elements.

d)

They have identical electron configurations.

124.

Atoms of elements in group 1 have ____________.

a)

one electron in their outermost energy level

b)

two electrons in their outermost energy level

c)

seven electrons in their outermost energy level

d)

eight electrons in their outermost energy level

125.

Which of the blocks on the periodic table contains the most elements?

a)

s block

b)

p block

c)

d block

d)

f block

126.

What makes the d block wider than either the s block or the p block?

a)

The d sub-orbital can hold ten electrons, making the d block ten elements wide.

b)

The d block is the most researched area of the periodic table.

c)

The elements in the d block are more important than the elements in the rest of the table.

d)

The elements in the d block are all metals.

127.

From the table below, determine the atomic number of the noble gas at the end of period 5.

a)

18

b)

36

c)

54

d)

52

128.

Which element has n=2 and s2 p6 configuration?

a)

He

b)

O

c)

Ne

d)

Ni

129.
How many valence electrons does an atom of sulfur (S) have?
a)
2
b)
3
c)
6
d)
16
130.

4.The arrangement of elements in the Modem Periodic Table is based on their

a)

(a) increasing atomic mass in the period

b)

(b) increasing atomic number in the horizontal rows

c)

(c) increasing atomic number in the vertical columns

d)

(d) increasing atomic mass in the group

131.

6.What is the atomic number of element of period 3 and group 17 of the Periodic Table?

a)

(a) 10

b)

(b) 4

c)

(c) 17

d)

(d) 21

132.

Name the neutral atom in the Periodic Table which has the same number of electrons as K+ and Cl-.

a)

(a) Helium

b)

(b) Argon

c)

(c) Neon

d)

(d) Krypton

133.

Carbon belongs to the second period and Group 14. Silicon belongs to the third period and Group 14. If atomic number of carbon is 6, the atomic number of silicon is

a)

(a) 7

b)

(b) 14

c)

(c) 24

d)

(d) 16

134.

On moving from left to right in a period in the Periodic table, the size of atom

a)

Increases

b)

Decreases

c)

Does not change appreciably

d)

First decreases and then increases

135.

Nitrogen and phosphorus are

a)

Non metals

b)

Metals

c)

Metalloids

d)

None of the above

136.

P-block elements are those elements in which last electron enters in

a)

P ortibal

b)

S orbital

c)

d orbital

d)

None of the above

137.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

138.

Identify the Electron Configuration for Aluminum (Al)

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

139.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

140.

What atom matches this electron configuration?

1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

141.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost orbit of an atom

142.

This is a correct dot diagram for fluorine (F)

a)

true

b)

false

143.

The elements in this group all have 5 valance electrons.

a)

Group 5

b)

Group 15

c)

Group 3

d)

Group 18

144.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
145.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
146.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
147.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
148.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
149.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
150.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
151.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
152.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

153.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
154.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

155.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
156.

How many dots would you put around carbon, a group 14 element?

a)

4

b)

6

c)

8

d)

18

157.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
158.

smallest particle of matter that retain the properties of element is ____________________

a)

atom

b)

proton

c)

cathode

d)

energy

159.

electrons are discovered by _________experiment

a)

cathode ray tube

b)

gold foil

c)

oil drop

160.

The figure shows ________________________

a)

cathode ray tube experiment

b)

gold foil experiment

c)

oil drop experiment

161.

The path of cathode ray ( shown in the figure ) proves that _____

a)

electrons have negative charge

b)

electrons have positive charge

c)

electrons have no charge

d)

electrons have both negative and positive charge

162.

The figure shows _____________experiment

a)

oil drop

b)

cathode ray tube

c)

gold foil

163.

The experiment ( shown in the figure ) lead to determine __________

a)

mass and charge of the electron

b)

the size of the electron

c)

the mass of the atom

d)

the charge of the atom

164.

The name of the model of the atom ( shown in the figure) is _______________

a)

plum pudding model

b)

nuclear model

c)

energy levels model

d)

quantum model

165.

the part ( labeled by the question mark in the figure ) is _______________

a)

atom

b)

nucleus

c)

proton

d)

electron

166.

Ag47108Ag_{47}^{108}  contains ________ protons, ________ neutrons and ________ electrons

a)

47, 61, 47

b)

108, 61, 108

c)

47, 108, 47

d)

60, 47, 60

167.

All atoms of the same element have the same _____________.

a)

number of protons

b)

number of neutrons

c)

Mass number

d)

Mass

168.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
169.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
170.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
171.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
172.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
173.

Which of these has the smallest atomic radius?

a)

K

b)

Rb

c)

Fr

d)

Cs

174.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
175.

As you move to the right across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have more neutrons

c)

the atoms have more protons.

d)

the atoms have more electrons.

176.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
177.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
178.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
179.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
180.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
181.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

182.
A group of elements that includes the most active of the elements is the -
a)
halogens.
b)
noble gases.
c)
nitrogen group.
d)
alkaline earth metals.
183.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size
184.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

185.

When atom gains an electron, the size will

a)

increase

b)

decrease

c)

have no change

d)

smaller

186.

When atom loses an electron, the size will

a)

be greater

b)

increase

c)

have no change

d)

be smaller

187.

A metallic bond is a bond between ________.

a)

nonmetals

b)

metals

c)

transition metals

d)

metalloids

188.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

189.

What do electrons do in a metallic bond?

a)

They stay on the metal atom.

b)

They are transferred from atom to atom.

c)

They form a covalent bond with another atom.

d)

They float around freely.

190.

What is meant by the term "sea of electrons"?

a)

It's what we call all the free floating electrons in a metal.

b)

It's what we call electrons that are floating in a liquid.

c)

It's the total number of electrons in a metal atom.

d)

It's the total number of electrons in the ocean.

191.

Why are metals good conductors of electricity?

a)

The electric current can easily travel along the surface of the metal because it is smooth.

b)

A negative charge can easily push the sea of electrons in one direction, making a current.

c)

Metals attract electricity.

d)

Metals are malleable.

192.

Why are metals malleable? (They can bend without breaking.)

a)

Metals are very smooth.

b)

Metals have a sea of electrons.

c)

The sea of electrons form a strong metallic bond.

d)

Even though the metal ions repel each other, the electron sea holds all the atoms in place.

193.

What property of metals is the image describing?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

194.

What property of metals is being shown in figure 1(b) in the image?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

195.

What is the one thing responsible for a metal being malleable, ductile, and conductive?

a)

metal atoms

b)

its covalent bonds

c)

its valence electrons

d)

its sea of free-floating electrons

196.

Which of the following lists of elements contain only metals?

a)

Li, Al, Te

b)

Ni, Pb, H

c)

Na, Os, Ga

d)

Ca, Zn, I

197.

What could be a charge on aluminum?

a)

1+

b)

2+

c)

3+

d)

4+

198.

Alloys are important because

a)

their properties are often superior to the component elements

b)

their properties are a blend of the component elements

c)

they never corrode

d)

they are less expensive than their component elements.

199.

Why are metals good conductors?

a)

they have mobile electrons

b)

they have mobile atoms

c)

they have crystal structures that can rearrange

d)

they have mobile protons

200.

Malleability means

a)

the ability to be drawn into a wire

b)

the electrons of metals are mobile

c)

the ability to be hammered into a shape

d)

the ability to be a conductor of electricity

201.

Metals are ductile because metallic bonds

a)

hold the layers of ions in rigid positions

b)

maximizes the repulsive force in a metal

c)

allows planes of protons and electrons to slide past one another

d)

are easily broken

202.

Metals are hard because metals have a

a)

sea of electrons that tightly hold the nuclei together

b)

they form triple bonds

c)

low melting point

d)

high luster

203.

The melting point of magnesium is higher than that of sodium because

a)

the relative atomic mass of sodium is less than that of magnesium

b)

the metallic bonding in magnesium is stronger than that in sodium

c)

the atoms in magnesium are packed more closely than the atoms in sodium

d)

the atomic size of magnesium is larger than that of sodium

204.

Metals are shiny because ______________.

a)

The protons glow

b)

The valence electrons at the surface of the metal interact with the light

c)

The electrons are excited to a higher energy state

d)

The neutrons react with the free electrons

205.
Metals...
a)
all have similar physical properties
b)
some have similar physical properties
c)
don't similar physica properties
d)
very few have similar physical properties

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5th - 12th Grade