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Worksheets

25-26 Periodic Table Test Review

Total questions: 152

Worksheet time: 4hrs 45mins

Name
Class
Date
1.

Which two characteristics are associated with metals?

a)

low first ionization energy and low electronegativity

b)

low first ionization energy and high electronegativity

c)

high first ionization energy and low electronegativity

d)

high first ionization energy and high electronegativity

2.

Which element has the most similar chemical properties to oxygen?

a)

Fr

b)

Ar

c)

F

d)

S

3.

Which grouping of circles, when considered in order from the top to the bottom, best represents the relative size of the atoms of Li, Na, K, and Rb, respectively? Select the diagram that shows the circles increasing in size from the first to the fourth circle.

a)

b)

c)

d)

4.

At STP, which element is brittle and not a conductor of electricity?

a)

S

b)

K

c)

Na

d)

Ar

5.

The elements in the modern Periodic Table are arranged according to their

a)

atomic number

b)

oxidation number

c)

atomic mass

d)

nuclear mass

6.

Which element is classified as a nonmetal?

a)

Be

b)

Al

c)

Si

d)

Cl

7.

Lithium and potassium have similar chemical properties because the atoms of both elements have the same

a)

mass number

b)

atomic number

c)

number of electron shells

d)

number of valence electrons

8.

At STP, O2(g) and O3(g) are two forms of the same element that have

a)

the same molecular structure and the same properties

b)

the same molecular structure and different properties

c)

different molecular structures and the same properties

d)

different molecular structures and different properties

9.

Which Period 4 element has the most metallic properties?

a)

As

b)

Br

c)

Ge

d)

Sc

10.

Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element X be found?

a)

1

b)

2

c)

15

d)

16

11.

Which element has chemical properties that are NOT most similar to calcium?

a)

Sr

b)

Se

c)

Mg

d)

Be

12.

Which element is malleable and can conduct electricity in the solid phase?

a)

iodine

b)

phosphorus

c)

sulfur

d)

tin

13.

Which element has atoms with the greatest attraction for electrons in a chemical bond?

a)

beryllium

b)

fluorine

c)

lithium

d)

oxygen

14.

Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom?

a)

Their metallic properties decrease and their atomic radii decrease.

b)

Their metallic properties decrease and their atomic radii increase.

c)

Their metallic properties increase and their atomic radii decrease.

d)

Their metallic properties increase and their atomic radii increase.

15.

The element in Group 14, Period 3 on the Periodic Table is classified as a

a)

metal

b)

noble gas

c)

metalloid

d)

nonmetal

16.

A horizontal row of elements in the periodic table is known as a(n)

a)

series

b)

period

c)

octet

d)

group

17.

The highly mobile electrons in the valence shell of metals results in metals being

a)

dull

b)

brittle

c)

good conductors

d)

poor conductors

18.

Which substance contains particles held together by metallic bonds?

a)

Ne

b)

Ni

c)

N

d)

I

19.

An atom in the ground state contains a total of 5 electrons, 5 protons, and 5 neutrons.

The electron configuration of this atom is 2-3.

Which Lewis electron-dot diagram represents this atom?

a)

b)

c)

d)

20.

Which Lewis electron-dot diagram is correct for a S2− ion?

a)

b)

c)

d)

21.

Graphite and diamond are both solid forms of the element carbon. Which statement explains the different properties of these two forms of carbon?

a)

Diamond has ionic bonding and graphite has metallic bonding.

b)

Diamond has metallic bonding and graphite has ionic bonding.

c)

Diamond has a different crystal structure from graphite.

d)

Diamond has carbon atoms with more valence electrons than graphite.

22.

Which atom, in the ground state, has a stable valence electron configuration?

a)

Bi

b)

Cs

c)

Pb

d)

Rn

23.

Which list of elements includes a metal, a metalloid, and a noble gas?

a)

Rb, Cl, Ne

b)

Sr, Si, Rn

c)

Rn, Cl, Ne

d)

Si, Rb, Sr

24.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
25.

How many valence electrons does Oxygen have?

a)

8

b)

16

c)

6

d)

7

26.

What is the number of electrons MOST atoms want in their valence orbital?

a)

2

b)

6

c)

8

d)

16

27.

Is this the correct Lewis Dot Structure for Boron?

a)

Yes

b)

No, missing electrons

c)

No, too many electrons

d)

No, dots are in wrong place.

28.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
29.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
30.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
31.

Which two elements have properties in common?

a)

Nitrogen and Phosphorous

b)

Oxygen and Nitrogen

c)

Sulfur and Nitrogen

32.
Which element could be lustrous and brittle?
a)
A
b)
B
c)
G
d)
L
33.

Mendeleev noticed that a ​ (a)   of ​ (b)   appeared when he arranged the elements in order of increasing ​ (c)   He found that the properties ​ (d)   regularly.

Choose from the below words
pattern
properties
atomic mass.
repeated
atomic number
34.

Please choose the atom with the larger atomic radius. ​ (a)  

Choose from the below words
Lithium
Nitrogen
35.

Please choose the atom with the larger atomic radius. ​ (a)  

Choose from the below words
Cesium
Rubidium
36.

Most elements in a group have the same number of ​ (a)   in the outer energy level and tend to have similar ​ (b)  

Choose from the below words
electrons
properties
protons
mass
37.

Match the following

a)

Alkali Metals

1.

Group 1

b)

Alkaline Earth Metals

2.

Group 2

c)

Halogens

3.

Group 17

d)

Noble Gases

4.

Group 18

38.

Increasing the number of protons in an atom within a row ​ (a)   the atomic number​ and (b)   the radius of the atom.

Choose from the below words
increases
decreases
does not affect
39.

Please choose the atom with the larger atomic radius.​ (a)   L

Choose from the below words
Lead
Tin
40.

Match the following metals with their family name.

a)

Krypton (Kr)

1.

Noble Gas

b)

Oxygen

2.

Non-metal

c)

Arsenic

3.

Semi Metal

41.

Which periodic group (aka family) has the highest electronegativity? Click the spot on that group.

A
B
C
D
E
42.

As you move from down a group on the Periodic Table...

The atomic radius ​ (a)   .

Choose from the below words
increases
decreases
stays the same
43.

As you move from down a group on the Periodic Table...

The number of occupied energy levels ​​ (a)   .

Choose from the below words
increases
stays the same
decreases
44.

Which element is a good conductor of electricity and is malleable?

a)

Si

b)

Na

c)

S

d)

Cl

45.

Which element has atoms with a complete octet in their valence shell in the ground state?

a)

Si

b)

Mg

c)

Al

d)

Ne

46.

Which element is most likely to form a negative ion by gaining one electron?

a)

Mg

b)

Al

c)

F

d)

Na

47.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

48.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
49.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

50.
Which of these elements has the highest ionization energy?
a)
Lithium (Li)
b)
Potassium (K)
c)
Francium (Fr)
d)
Sodium (Na)
51.

What is Ionization energy?

a)

The energy used in a chemical reaction

b)

Potential energy

c)

The energy it takes to remove one electron from an atom or ion in its gaseous state

52.

Explain why ionization energy decreases as you go down a group.

a)

Outer electrons are further away from the nucleus you go down a group

b)

Electrons feel less pull from the nucleus as you go down a group

c)

Electrons are easier to remove as you go down a group

d)

All of the above

53.

Select all that explain the ionization energy trend within periods

a)

electrons are closer to the nucleus

b)

their is a weak pull between electrons from the nucleus, making them easily moveable

c)

feel more of a pull from nucleus, making them harder to move

d)

electrons are further from the nucleus

54.

Which of the following lists the atoms in order of increasing Ionization energy?

a)

calcium, iron, copper

b)

copper, iron, calcium

c)

calcium, copper, iron

d)

iron, copper, calcium

55.

Which element would you expect to have a higher ionization energy, sulfur (S) or chlorine (Cl), and why?

a)

Sulfur, because it has a larger atomic radius

b)

Chlorine, because it has a higher nuclear charge

c)

Sulfur, because it has a lower nuclear charge

d)

Chlorine, because it has a smaller atomic radius

56.

What is the primary reason for the increase in ionization energy across a period?

a)

Increase in atomic radius

b)

Increase in nuclear charge

c)

Decrease in electron shielding

d)

Decrease in atomic mass

57.

Why does ionization energy decrease as atomic radius increases?

a)

Because electrons are closer to the nucleus

b)

Because electrons are further from the nucleus

c)

Because nuclear charge decreases

d)

Because electron shielding decreases

58.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

59.

Electronegativity (a)   as you go down a group.

60.

Electronegativity trends are the same as:

a)

Atomic radius trends

b)

Ionization energy trends

c)

Both of these

d)

None of these

61.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

62.

As you move across a period, the outer electrons are ________ to the nucleus, so the nucleus of the atom is ________ to attract electrons in a bond.

a)

closer, more able

b)

closer, less able

c)

further, less able

d)

further, more able

63.

Why does electronegativity decrease as you go down a group?

a)

As you go down a group, the outer electrons are further away from the nucleus

b)

As you go down a group, the nucleus is less able to attract electrons in a bond

c)

Both of these

d)

None of these

64.

Electronegativity is the ability of an atom to attract electrons in a physical bond.

a)

false

b)

true

65.

Match the following

a)
1.

Group

b)
2.

Period

c)

1969 Periodic Table was organized by:

3.

Atomic Mass

d)

Modern Periodic Table is organized by:

4.

Atomic Number

66.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size
67.

Which is larger

a)

Na

b)

Na+

68.

Which is larger

a)

I

b)

I-

69.

Which ion is larger

a)

Cu+

b)

Cu2+

70.
Why are cations larger and anions smaller than their respective atoms?
a)
Cations are larger than their respective atoms because of decreased electron repulsion
b)
Cations are larger than their respective atoms because of increased electron repulsion
c)
Anions are smaller than their respective atoms because of increased effective nuclear charge
71.
Which has the greater EN: 
H or F?
a)
H
b)
F
72.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
73.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
74.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

75.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

76.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

77.

Identify the number of valence electrons in each group

Know the valence electron trend

a)1
b)2
c)3
d)4
e)5
f)6
g)7
h)8
1
2
3
4
5
6
7
8
1)
2)
3)
4)
5)
6)
7)
8)
78.

Why are certain elements not chemically active?

a)

They have incomplete energy levels

b)

They have complete energy levels

c)

They are too heavy

d)

They are too light

79.

The main reason noble gases are found in nature as single atoms is because they (a)   .

Choose from the below words
They are too reactive
They have complete valence shells
They are too heavy
They are metallic
80.

What is a key property of inert gases like helium?

a)

Highly reactive

b)

Non-reactive

c)

Very dense

d)

Very colorful

81.

Which one of these is not a property of noble gases?

a)

Colorless

b)

Odorless

c)

Flammable

d)

Gas at room temperature

82.

Name group 18 on the periodic table.

a)

alkali metals

b)

transition metals

c)

alkaline earth metals

d)

noble gases

83.

The majority of elements on the periodic table are

a)

man made

b)

nonmetals

c)

metals

d)

gases

84.

Which group have properties similar to both metals and nonmetals?

a)

Halogens

b)

Metalloids

c)

Alkaline Earth Metals

d)

Noble Gases

85.

What is the name of this group?

a)

Nonmetals

b)

Alkali Metals

c)

Transition Melals

d)

Halogens

86.

Match the following

a)

1.

Period 6

Group 6

b)

2.

Period 5

Group 3

c)

3.

Period 7

Group 8

d)

4.

Period 1

Group 18

e)

5.

Period 4

Group 3

87.

Match the following

a)

1.

Group 1

b)

2.

Group 2

c)

3.

Group 13

d)

4.

Group 14

e)

5.

Group 15

88.

Which is not a property of metals?

a)

malleable

b)

shiny

c)

good conductors

d)

brittle

89.

Which is a chemical property

a)

melting point

b)

reactivity

c)

boiling point

d)

malleability

90.

Which is a property of metals?

a)

gas at room temperature

b)

good conductors of electricity

c)

brittle

91.

Which particle is responsible for the reactivity of an element?

a)

proton

b)

neutron

c)

electron

92.

Which is true of the noble gases?

a)

They do not react with other elements.

b)

They are solid at room temperature.

c)

They are reactive.

d)

They are all heavy.

93.

Which element has 2 valence electrons in its 2nd energy level?

a)

beryllium

b)

helium

c)

magnesium

d)

calcium

e)

carbon

94.

Which of the following elements has the 3rd energy level as its outermost level of electrons?

a)

magnesium

b)

lithium

c)

potassium

d)

neon

e)

oxygen

95.

Which of the following elements has 5 valence electrons?

a)

boron

b)

phosphorus

c)

magnesium

d)

chlorine

96.

How are elements grouped on the periodic table?

a)

Physical appearance

b)

Number of protons

c)

Number of valence electrons

d)

Number of valence neutrons

97.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

98.

Which 3 elements have 3 valence electrons?​ (a)   ​ (b)   ​ (c)   ​

a)

B

b)

Al

c)

Ga

d)

Be

e)

Ge

99.

Elements that have atoms with full valence shells in the ground state are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

100.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
101.

Which elements have the most similar chemical properties?

a)

boron and carbon

b)

oxygen and sulfur

c)

aluminum and bromine

d)

argon and silicon

102.

A chemist is looking for an element that reacts similarly to the element

lithium (Li). Which would be the best choice?

a)

gold (Au)

b)

neon (Ne)

c)

fluorine (F)

d)

sodium (Na)

103.

Which best describes elements found in a column of the periodic table?

a)

The elements have the same-size atoms.

b)

The elements have the same atomic number.

c)

The elements have similar chemical properties.

d)

The elements are all found naturally in the same physical state.

104.

Which best describes how the current periodic table is arranged?

a)

by atomic mass

b)

by atomic number

c)

in alphabetical order by element symbol

d)

in numerical order by number of neutrons in the nucleus

105.

Which best describes the reactivity of metals when moving from left to

right on the periodic table?

a)

They become less reactive.

b)

They become more reactive.

c)

The reactivity remains the same.

d)

The reactivity decreases, then increases.

106.

Which property would be most useful in placing a newly discovered

element in Group 18 (VIIIA) on the periodic table?

a)

reactivity

b)

malleability

c)

conductivity

d)

nonreactivity

107.

Where would a new highly reactive metal most likely be placed on the

periodic table?

a)

right side

b)

left side

c)

middle

d)

top

108.

Nonmetals break easily. They are ....

a)

brittle

b)

semiconductors

c)

shiny

109.

Which one is a semiconductor?

a)

metals

b)

nonmetals

c)

metalloids

110.

What are some general properties of nonmetals?

a)

Shiny, good conductors of heat and electricity

b)

Dull, poor conductors of heat and electricity

c)

Malleable and ductile

d)

High density and high melting points

111.

What is the most reactive nonmetal?

a)

Fluorine

b)

Iodine

c)

Chlorine

d)

Bromine

112.
Luster is ___________
a)
A.  the way light is reflected off a surface.
b)
A.  how well a piece of matter conducts electricity. 
c)
A.  the capability of being drawn out into thin wires or threads.
d)
A.  the capability of being hammered out thin.
113.
What physical properties are used to classify elements as metals, non-metals, or metalloids?
a)
Color, smell, physical state
b)
Reactivity, streak, hardness
c)
Ability to burn, mass, density
d)
Luster, conductivity, malleability
114.
If you have a material that can conduct electricity well it is probably a...
a)
Metalloid
b)
Matter
c)
Non-metal
d)
Metal
115.
I have an object that is dull, brittle, and an insulator, what is it?
a)
metalloid
b)
non-metal
c)
metal
d)
matter
116.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
117.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
118.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
119.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

120.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
121.
In general, what can be said of the melting points of metals?
a)
They are low.
b)
They are high.
c)
They are lower than nonmetals.
d)
They do not have melting points.
122.

Name one chemical property of nonmetals.

a)

Tendency to gain electrons

b)

Shiny appearance

c)

Tendency to lose electrons

d)

High thermal conductivity

123.

Metalloids have the same properties as

a)

metals.

b)

nonmetals.

c)

neither, they are a combination of both.

124.

Classify the elements

Categorize the following

Cu

N

Ge

B

Si

As

Sb

Na

Al

I

P

Se

H

Sn

Ni

Te

He

Ga

Metal
Nonmetal
Metalloid
125.

What are diatomic elements?

a)

Elements that form two-atom molecules when not combined in a compound.

b)

Two elements that combine with one atom from each element.

c)

Elements that are always in pairs no matter what.

126.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

127.

H

a)

Diatomic

b)

Monatomic

128.

I

a)

Diatomic

b)

Monatomic

129.

N

a)

Diatomic

b)

Monatomic

130.

F

a)

Diatomic

b)

Monatomic

131.

O

a)

Diatomic

b)

Monatomic

132.

Cl

a)

Diatomic

b)

Monatomic

133.

Br

a)

Diatomic

b)

Monatomic

134.

B

a)

Diatomic

b)

Monatomic

135.

Be

a)

Diatomic

b)

Monatomic

136.

C

a)

Diatomic

b)

Monatomic

137.

Ca

a)

Diatomic

b)

Monatomic

138.

Na

a)

Diatomic

b)

Monatomic

139.

Ne

a)

Diatomic

b)

Monatomic

140.

Fe

a)

Diatomic

b)

Monatomic

141.

P

a)

Diatomic

b)

Monatomic

142.

Which element has the most metallic character in the Periodic table?

a)

SODIUM

b)

POTASSIUM

c)

CEASIUM

d)

RUBIDIUM

143.

If an element has a low ionization energy, then it is likely to be …………….

a)

NON-METALLIC

b)

METALLIC

c)

METALLOID

d)

NOTA

144.

As you move down a group in the periodic table, metallic character:

a)

Decreases

b)

Stays the same

c)

First increases, then decreases

d)

Increases

145.

As you move across a period from left to right, nonmetallic character:

a)

Increases

b)

Stays the same

c)

First decreases, then increases

d)

Decreases

146.

Why does metallic character increase down a group?

a)

Atomic size decreases

b)

Outer electrons are closer to the nucleus

c)

Outer electrons are farther from the nucleus and easily lost

d)

Nuclear charge increases

147.

Across a period, metallic character:

a)

Increases

b)

Decreases

c)

Varies randomly

148.

Explain, in terms of atomic structure and coulombic attraction, why argon has a greater first

ionization energy than sulfur.

4 lines
149.

Explain, in terms of atomic structure and coulombic attraction, why barium has a lower first ionization energy than magnesium.

4 lines
150.

Explain why atomic radius increases down a group but decreases across a period.

4 lines
151.


Down a group electronegativity (a)  

Because the atomic radius​ (b)   which​ (c)   the distance between the electrons and nucleus.

Leading to ​ (d)   attraction between the nucleus and the electrons.

Choose from the below words
decreases
increases
stays the same
weaker
stronger
152.

Across a period electronegativity​ (a)  

Because the atomic radius​ (b)   which​ (c)   the distance between the electrons and nucleus.

Leading to ​ (d)   attraction between the nucleus and the electrons.

Choose from the below words
increases
decreases
stronger
stays the same
weaker

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