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Periodic Table Practice

Total questions: 140

Worksheet time: 4hrs 17mins

Name
Class
Date
1.
A ___________ is an arrangement of elements in columns
a)
columns
b)
rows
c)
periodic table
d)
electron shell
2.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
3.
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.
4.
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
5.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
6.
Which element is not a metal?
a)
H
b)
Re
c)
Al
d)
B
7.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
8.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
9.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
10.
A horizontal row of elements in the periodic table.
a)
column
b)
group
c)
period
11.
The simplest substance is..?
a)
Carbon
b)
An element
c)
Water
d)
A simple compound 
12.
A proton is....
a)
A negatively charged subatomic particle
b)
A positively charged subatomic particle
c)
A neutrally charged subatomic particle
d)
The only subatomic particle located in the nucleus
13.
A neutron has a charge of
a)
+2
b)
No charge
c)
-1
d)
+1
14.

As you move up group 16, electronegativity of each successive element _________.

a)

Decreases

b)

Increases

c)

Stays the same

15.

Which scientist developed the first published periodic table where elements were placed in order of increasing atomic mass?

a)

Henry Moseley

b)

Johann Dobereiner

c)

John Dalton

d)

Dmitri Mendeleev

16.

Which periodic trend has to do with the width of a given atom?

a)

Ionic Radius

b)

Atomic Radius

c)

Electronegativity

d)

Reactivity

17.

Elements in the same group have similar _______.

a)

Atomic Mass

b)

Symbol

c)

Chemical Properties

d)

Atomic Number

18.

As you move up group 16, reactivity of successive elements _______.

a)

Decreases

b)

Increases

c)

Stays the same

19.

Which of the following elements will have a lower ionization energy (IE) than Selenium?

a)

Sulfur

b)

Tellurium

c)

Oxygen

20.

Which of the following element(s) have higher atomic radii than Selenium?

a)

Oxygen

b)

Sulfur

c)

Tellurium

21.

Which of the following elements have the smallest ionic Radius?

a)

Oxygen

b)

Selenium

c)

Sulfur

d)

Tellurium

22.

The element with the highest electronegativity in the halogen group?

a)

At

b)

F

c)

Cl

d)

Br

23.

Which periodic group has the smallest atomic radius?

a)

Alkali metals

b)

Halogens

c)

Noble Gases

d)

Transition metals

24.

The minimum energy required to remove an electron from the ground state of an atom

a)

electron configuration

b)

energy levels

c)

ionization energy

d)

ionic bond

25.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
26.

Which of the following is in the correct order of size?

a)

Anion > Atom > Cation

b)

Atom > Cation > Anion

c)

Cation > Atom > Anion

d)

Anion > Cation > Atom

27.
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 neutrons
28.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
29.
The outermost energy level of an electron is called its...
a)
valence energy level
b)
outer energy level
c)
group
d)
period
30.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
31.
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.
32.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
33.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
34.

What are the elements in group 1 (the far left) of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

35.

What are the elements in group 2 of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

36.

What are the elements in group 18 (the far right) of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

37.

What are the elements in group 17 of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

38.

What are the elements in groups 3-12 of the periodic table called?

a)

Transition metals

b)

Non-metals

c)

Metalloids

d)

Metals

39.

What are the elements found along the "staircase" called? They have properties of both metals and non-metals.

a)

Metalloids

b)

Non-metals

c)

Transition metals

d)

Metals

40.

Hydrogen is a:

a)

Alkali metal

b)

Metalloid

c)

Non-metal

d)

Noble gas

41.

The positively charged particle in the nucleus of an atom is a:

a)

Proton

b)

Neutron

c)

Electron

d)

Shell

42.

The neutral particle in the nucleus of an atom is a:

a)

Proton

b)

Neutron

c)

Electron

d)

Shell

43.

A tiny, negatively charged particle that moves around the nucleus of an atom in clouds/shells is called:

a)

An electron

b)

A proton

c)

A neutron

d)

A shell

44.

The number of protons in the nucleus of an atom is equal to the:

a)

Atomic number

b)

Atomic mass

c)

Number of neutrons

d)

Number of valence electrons

45.

The total number of protons and neutrons in an atom's nucleus is equal to the:

a)

Atomic number

b)

Atomic mass

c)

Number of valence electrons

d)

Number of electron shells

46.

The Russian scientist who created one of the first periodic tables by using atomic mass was:

a)

Bohr

b)

Rutherford

c)

Mendeleev

d)

Thomson

47.

The subatomic particles that are located the farthest from the nucleus are:

a)

Valence electrons

b)

Valence protons

c)

Periodic electrons

d)

Periodic protons

48.

The number of electron shells an atom has is equal to the element's:

a)

Period number

b)

Group number

c)

Valence number

d)

Atomic number

49.

The number of valence electrons an element has is equal to its:

a)

Period number

b)

Group number

c)

Valence number

d)

Atomic number

50.

The model of an atom that shows electrons in circular orbits around the nucleus is called the:

a)

Bohr Model

b)

Lewis Dot Structure

c)

Rutherford Model

d)

Thomson Model

51.

The model of an atom that uses dots surrounding the atomic symbol to represent valence electrons is called the:

a)

Bohr Model

b)

Lewis Dot Structure

c)

Rutherford Model

d)

Thomson Model

52.
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.
53.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
54.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
55.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
56.
If an atom had the same properties as fluorine (F), it would probably be located in
a)
period 1.
b)
period 2.
c)
group 2.
d)
group 17.
57.
Atoms with similar properties are most likely located...
a)
in the same period.
b)
in the same group.
c)
in different periods.
d)
to the right and left of each other.
58.
What is the element symbol for boron? 
a)
B
b)
Bo
c)
Bn
d)
W
59.
Each element is unique based on its number of protons, also known as the...
a)
atomic mass
b)
valence number
c)
atomic symbol
d)
atomic number
60.
The atomic number of this pictured element is
a)
28
b)
58.6934
c)
Ni
d)
Nickel
61.
what does the 6 represent?
a)
Atomic mass
b)
atomic number
c)
chemical symbol
d)
element name
62.
Group Name and Number for Neon
a)
Alkaline Earth Metals 2 or 2A
b)
Noble Gases 18 or 8A
c)
Halogens 17 or 7A
d)
Alkali Metals 1 or 1A
63.
Group Name and Number for Flourine
a)
Transition Metals 3-12
b)
Noble Gases 18 or 8A
c)
Halogens 17 or 7A
d)
Alkali Metals 1 or 1A
64.
Group Name and Number for Magnesium
a)
Alkaline Earth Metals 2 or 2A
b)
Noble Gases 18 or 8A
c)
Halogens 17 or 7A
d)
Alkali Metals 1 or 1A
65.
A proton is....
a)
A negatively charged subatomic particle
b)
A positively charged subatomic particle
c)
A neutrally charged subatomic particle
d)
The only subatomic particle located in the nucleus
66.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
67.
What is the atomic mass of Neon?
a)
10
b)
30
c)
10.18
d)
20.18
68.
Which is a neutron?
a)
A
b)
B
c)
C
69.
What is the formula to solve for the neutron?
a)
Mass + Atomic Number= Neutrons
b)
Mass x Atomic Number = Neutrons
c)
Mass - Atomic Number = Neutrons
d)
Mass + Number of Protons = Neutron
70.

Which scientist edited the Periodic Table and arranged elements in increased atomic number?

a)

Rutherford

b)

Dalton

c)

Mendeleev

d)

Moseley

71.

Which scientist created the Periodic Table and arranged elements in increasing atomic mass?

a)

Rutherford

b)

Thomson

c)

Mendeleev

d)

Moseley

72.

Elements in the same group or family have _____________.

a)

the same number of valence electrons and different properties.

b)

the same number of valence electrons and similar properties

c)

different number of valence electrons and similar properties.

d)

different number of valence electrons and different properties.

73.

Which class of elements are malleable, ductile, shiny when clean and polished, good conductors of heat and electricity, and reacts with acids to form hydrogen gas?

a)

metals

b)

nonmetals

c)

metalloids

d)

ions

74.

What is the name of Group 1 elements?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

75.

What is the name of the elements that are unreactive and have a full octet?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Transition Metals

76.

What is an atom or bonded group of atoms that has a positive or negative charge?

a)

ion

b)

atom

c)

metal

d)

nonmetal

77.

What is the term of an atom that will lose electron(s) and have a positive change?

a)

cation

b)

anion

c)

electronegativity

d)

ionic radius

78.

Where are metalloids located on the Periodic Table?

a)

In the s block.

b)

In the f block.

c)

In the d block.

d)

The elements that touch the staircase except aluminum.

79.

What is the trend for atomic radius (radii)?

a)

It increases left to right on the Periodic Table and decreases down a group.

b)

It decreases left to right on the Periodic Table and increases down a group.

c)

It increases left to right on the Periodic Table and increases down a group.

d)

It decreases right to left on the Periodic Table and decreases down a group.

80.

Why does the atomic radius decrease across a period?

a)

There are more protons in the nucleus that pull electrons closer.

b)

There are more electrons in the nucleus that pull protons closer.

c)

There are more protons in the nucleus that pull neutrons closer.

d)

There are more neutrons in the nucleus that pull protons closer.

81.

What does the atomic radius increase down a group?

a)

There are more electrons and energy levels.

b)

There are fewer electrons and energy levels.

c)

There are more protons that need more energy levels.

d)

There are more neutrons that need more energy levels.

82.

What element has the largest atomic radius?

a)

oxygen

b)

neon

c)

carbon

d)

sodium

83.

Which element has the smallest atomic radius?

a)

magnesium

b)

chlorine

c)

bromine

d)

argon

84.

What is the trend for ionization energy?

a)

Across a period (left to right) it increases and down a group it decreases.

b)

Across a period (left to right) it decreases and down a group it increases.

c)

Across a period (left to right) it decreases and down a group it decreases.

d)

Across a period (left to right) it increases and down a group it increases.

85.

What is ionization energy?

a)

The energy required to remove an electron from a neutral atom of an element.

b)

The energy change that occurs when an electron is acquired by a neutral atom.

c)

The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

d)

How close an atom is to its neighboring atom.

86.

Which element has the highest ionization energy?

a)

oxygen

b)

sulfur

c)

silicon

d)

potassium

87.

What is the ability of an atom in a chemical compound to attract electrons from another atom in the compound?

a)

ionization energy

b)

electronegativity

c)

atomic radius

d)

electron affinity

88.

Which element has the largest electronegativity?

a)

barium

b)

oxygen

c)

iron

d)

lithium

89.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
90.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
91.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
92.
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
93.
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 neutrons
94.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
95.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
96.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
97.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
98.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
99.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
100.
Vertical columns of elements (families) on the periodic table with similar  properties
a)
groups
b)
periods
c)
quadrants
d)
rows
101.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)
Sodium is less electronegative than potassium. 
b)
Sodium has fewer energy levels than potassium. 
c)
Sodium has a larger ionic radius than potassium. 
d)
Sodium has lower ionization energy than potassium. 
102.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
103.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
104.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
105.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
106.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
107.
All elements found on the left side of the Periodic Table of the Elements have what properties in common?
a)
They conduct heat and electricity 
b)
They are all gases 
c)
They are brittle and dull
d)
They are radioactive
108.
Which of these elements has an electron structure most similar to that of element X?
a)
1
b)
2
c)
3
d)
4
109.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
110.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
111.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
112.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
113.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
114.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
115.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
116.
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 neutrons
117.
How many "valance electrons" are in chlorine?
a)
7
b)
2
c)
17
d)
8
118.
Carbon-12, Carbon-13, and Carbon-14 are...
a)
ions
b)
isotopes
c)
electronegative
d)
radioactive
119.
How many Protons does Bromine have?
a)
45
b)
79.904
c)
80
d)
35
120.
How many Neutrons does Bromine have?
a)
35
b)
80
c)
45
d)
79.905
121.
Does this carbon have the correct amount of electrons?
a)
Yes
b)
No, it needs one more
c)
No, it needs two more
d)
No, it needs three more
122.
Nitrogen has 5 valence electrons
a)
True
b)
False, it has 7
c)
False, it has 14
d)
False, it has 7.01
123.
An isotope has...
a)
the same number of protons but different number of electrons
b)
same number of protons but different number of neutrons
c)
same number of electrons and neutrons
d)
same number of electrons, protons, and neutrons
124.
Elements that are gases, brittle, and not conductive are
a)
Metals
b)
Metalloids
c)
Transition Metals
d)
Non-metals
125.
Not non-metals or metals but somewhere in between
a)
noble gases
b)
isotopes
c)
metalloids
d)
ions
126.
Is this Lewis Dot Structure correct
a)
Yes
b)
No, chlorine has 6 valence
c)
No, chlorine has 8 valence
d)
No, chlorine has 17 electrons
127.
How many electrons are in the following chlorine atom?
a)
7
b)
8
c)
17
d)
13
128.
What is titanium's atomic mass?
a)
47.867
b)
22
c)
26
d)
49
129.
The atomic mass of Boron is 10.81, which means Boron has..
a)
5 electrons and 6 protons, each weigh 1 amu
b)
5 neutrons and 6 electrons, each weigh 1 amu
c)
6 neutrons and 5 protons, each weigh 1 amu
d)
10.81 protons each weighing around 1 amu
130.

I am usually a good conductor and shiny/lustrous

a)

Metal

b)

Metalloid

c)

Non-metal

131.

I am usually a gas, and at the very right side of the periodic table of elements

a)

Metal

b)

Metalloid

c)

Non-metal

132.

I am Chlorine many electrons to I need to be complete?

a)

8

b)

7

c)

1

d)

0

133.

Potassium has 1 valence electron, would it rather gain 7 electrons or lose its one valence electron to complete its energy level?

a)

lose 1 electron

b)

gain 1 electron

c)

lose 7 electrons

d)

gain 7 electrons

134.

Lewis Dot Structure shows us the..

a)

Energy Levels of electrons

b)

Valence electrons

c)

number of protons

d)

total number of electrons

135.
 Which of the following statements are FALSE?
a)
metals are located to the LEFT of the zig-zag line
b)
metals are less reactive than nonmetals
c)
nonmetals are located to the RIGHT of the zig-zag line
d)
metalloids have properties of both metals and nonmetals
136.

Mendeleev arranged the elements by their ________________

a)

alphabetical

b)

density

c)

melting point

d)

atomic mass

137.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
138.

Elements in the same group or family have the same number of

a)

neutrons

b)

valence electrons

c)

electrons

d)

energy levels

139.

Electrons...

a)

are found in the nucleus

b)

give us the atomic number of an element

c)

are how we identify each elements

d)

have a negative charge

140.

Elements in the same period have the same number of

a)

neutrons

b)

valence electrons

c)

electrons

d)

energy levels

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