wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

6.5 Periodic Trends

Total questions: 130

Worksheet time: 2hrs 45mins

Name
Class
Date
1.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
2.
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.
3.
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
4.
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. 
5.
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.
6.
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.
7.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
8.
Which has the greater EN: 
N or C?
a)
C
b)
N
9.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
10.

Which of the following is NOT a trend that varies periodically in the periodic table?

a)

Electronegativity

b)

Ionization energy

c)

Symbols of elements

d)

Atomic radius

11.

ability of atom to attract electrons in bond

a)

Electronegativity

b)

Atomic radius

c)

Atomic number

d)

electron affinity

12.

The atomic radius across period

a)

decrease from left to right

b)

Increase from left to right

c)

decrease from right to left

d)

stay the same

13.

As you move down a Group on the periodic table, what happens to the size of the atoms?

a)

they stay the same

b)

they get larger

c)

they get smaller

14.

As you move across a row on the periodic table, what generally happens to the atomic radius?

a)

it decreases

b)

it increases

c)

it stays the same

15.

What property is being measured in this diagram?

a)

Density

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

16.

Which of the following atoms has the greatest atomic radius?

a)

nitrogen

b)

phosphorus

c)

potassium

d)

cesium

17.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
18.
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
19.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
20.
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
21.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
22.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

23.

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)

24.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

25.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

26.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

27.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

28.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

29.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

30.

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

a)

atom

b)

ion

c)

cation

d)

anion

31.

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

a)

cation

b)

anion

c)

electron

d)

ion

32.

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

a)

group or family

b)

period

c)

periodic law

d)

octet rule

33.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
34.

In the process of ionization, what is the relationship between the second ionization energy (I2) and the third ionization energy (I3)?

a)

I2 > I3

b)

I2 < I3

c)

I2 = I3

d)

There is no way to predict this relationship.

35.

Looking across period 4 of the periodic table, potassium (atomic number 19) is followed by calcium (atomic number 20), which is followed by scandium (atomic number 21). Which element should have the largest atomic radius?

a)

potassium

b)

calcium

c)

scandium

d)

All three have the same atomic radius.

36.

Consider the group 1A elements sodium (period 3), potassium (period 4), and rubidium (period 5). What would you predict about the ionization energies of these elements?

a)

Na < K < Rb

b)

Na > K > Rb

c)

Rb < Na < K

d)

Na = K = Rb

37.

Which of these elements in group 1A has the largest atomic radius?

a)

cesium

b)

rubidium

c)

potassium

d)

sodium

38.

Which element in period 4 has the highest electronegativity?

a)

potassium

b)

calcium

c)

copper

d)

bromine

39.

Which group 4A element has the highest ionization energy?

a)

carbon

b)

tin

c)

silicon

d)

lead

40.

Consider the group 1A element sodium (atomic number 11), the group 3A element aluminum (atomic number 13), and the group 7A element chlorine (atomic number 17). These elements are in period 3. How are the first ionization energies of these elements related?

a)

sodium > aluminum > chlorine

b)

sodium < aluminum < chlorine

c)

sodium < chlorine < aluminum

d)

sodium > chlorine > aluminum

41.

The sodium atom loses an electron to form a sodium ion (Na+). Which statement is correct with respect to its atomic radius?

a)

The sodium ion has a larger radius than the atom.

b)

The sodium ion has a smaller radius than the atom.

c)

The sodium ion and the sodium atom radii are the same size.

d)

The sodium ion has twice the radius of the sodium atom.

42.

Which property determines an atom's ability to attract electrons shared in a chemical bond?

a)

ionization energy

b)

atomic radius

c)

electronegativity

d)

ionic radius

43.

Which group 2A element has the largest ionic radius?

a)

magnesium

b)

calcium

c)

barium

d)

radium

44.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
45.
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
46.
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
47.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
48.
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
49.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
50.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
51.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
52.
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. 
53.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

54.

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)

55.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

56.
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.
57.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

58.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

59.

It is the measure of the mean distance from the center of nucleus to the boundary of the surrounding cloud where the electron revolves.

a)

Electronegativity

b)

Atomic radius

c)

Electron affinity

d)

Metallic property

60.

Given: Na, Cl, Ba, and Al.

Which has the greatest tendency to accept electrons to form negative ions?

a)

Na

b)

Cl

c)

Ba

d)

Al

61.

Given: Al, O, Cl, and N.

Which has the greatest tendency to lose electrons to form positive ions?

a)

Al

b)

Cl

c)

O

d)

N

62.

Which of the following are the characteristics of the most active nonmetals?

a)

Small radii and high ionization energies

b)

Large atomic radii and low ionization energies

c)

Small radii, low ionization energies

d)

Large atomic radii, high ionization energies

63.

The element with the lowest ionization energy in Period 3 is __________________.

a)

Sodium

b)

Chlorine

c)

Magnesium

d)

Argon

64.

Which periodic group has the smallest atomic radius?

a)

Alkali metals

b)

Halogens

c)

Noble gases

d)

Transition metals

65.

The element with the highest electronegativity in the halogens is ________________.

a)

Astatine

b)

Fluorine

c)

Chlorine

d)

Bromine

66.

Which element is the most metallic?

a)

Na

b)

Mg

c)

Cs

d)

Fr

67.

The change of energy accompanies the addition of an electron to a gaseous atom.

a)

Electronegativity

b)

Atomic radius

c)

Electron affinity

d)

Metallic property

68.

Given: At, F, Cl and Br.

Which sets correctly arranged the given elements in order of increasing electron affinity?

a)

At, Br, Cl, F

b)

F, Cl, Br, At

c)

Cl, Br, At, F

d)

Br, At, Cl, F

69.
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
70.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
71.
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
72.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
73.
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
74.
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)
75.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
76.
What term is used to describe "an atom's tendency to attract electrons to itself when is is chemically combined with another element"
a)
electronation
b)
electron affinity
c)
electronegativity
d)
electrolysis
77.
The electronegativity of Cl is the highest in Period 2.  Why?
a)
Cl is the largest and has the greatest effective nuclear charge
b)
Cl is the smallest and has the lowest effective nuclear charge
c)
Cl is the largest and has the lowest effective nuclear charge
d)
Cl is the smallest and has the greatest effective nuclear charge
78.
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
79.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
80.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
81.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
82.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
83.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

84.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
85.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
86.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
87.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
88.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
89.

Which among the elements has the highest electron affinity?

a)

Chlorine

b)

Tellurium

c)

Germanium

d)

Rhodium

90.

Which among the elements has the greatest electronegativity?

a)

Carbon

b)

Oxygen

c)

Neon

d)

Fluorine

91.

Which group of elements below follows an increasing trend?

a)

V, Ti, Sc, Ca

b)

Tl, In, Ga, Al

c)

Fr, Cs, Rb, K

d)

Ra, Ba, Sr, Ca

92.

Which among the elements has the smallest atomic radius?

a)

Chlorine

b)

Francium

c)

Yttrium

d)

Cobalt

93.

Which among the elements has the lowest metallic property?

a)

Cobalt

b)

Nickel

c)

Copper

d)

Iron

94.

Which element is commonly used for creating can of sardines?

a)

Mercury

b)

Helium

c)

Aluminum

d)

Tin

95.

Which element is commonly used for creating toothpaste?

a)

Mercury

b)

Helium

c)

Aluminum

d)

Fluorine

96.

Which element is commonly used for creating kitchenware?

a)

Mercury

b)

Helium

c)

Aluminum

d)

Chlorine

97.

Which element is commonly used for creating old thermometers?

a)

Mercury

b)

Helium

c)

Aluminum

d)

Fluorine

98.

Which element is commonly used for creating inflated balloons?

a)

Tin

b)

Helium

c)

Chlorine

d)

Fluorine

99.

TRUE or FALSE: Metallic Property increases from right to left across a period.

a)

TRUE

b)

FALSE

100.

TRUE or FALSE: Elements increase in size from left to right across a period.

a)

TRUE

b)

FALSE

101.

TRUE or FALSE: Ionization Energy decreases from left to right across a period.

a)

TRUE

b)

FALSE

102.

TRUE or FALSE: Electron Affinity increases from left to right across a period.

a)

TRUE

b)

FALSE

103.

TRUE or FALSE: Electronegativity decreases from left to right across a period.

a)

TRUE

b)

FALSE

104.

The _____ do not have defined values for electronegativity.

a)

alkaline earth metals

b)

alkali metals

c)

noble gases

d)

halogens

105.

The elements in group 3-12 are the

a)

alkaline earth metals

b)

alkali metals

c)

transition metals

d)

halogens

106.

When electrons that are blocked from the full force of the nucleus' positive charge

a)

shielding

b)

inner transition metals

c)

valence

d)

electronegativity

107.

Tendency for an atom to attract electrons when chemically bonded to another atom.

a)

shielding

b)

valence

c)

ionization

d)

electronegativity

108.

The energy required to remove the 2nd most loosely held electron.

a)

2nd Ionization Energy

b)

1st Ionization Energy

c)

2nd Electonegativity

d)

1st Electronegativity

109.

The anion form of an atom is always ______ than its neutral form.

a)

smaller

b)

larger

c)

the same

d)

unable to tell

110.

The cation form of an atom is always ____ than its neutral form.

a)

smaller

b)

larger

c)

the same

d)

unable to tell

111.

The ___ of an atom is found by measuring the distance between the nuclei of two like atoms and halving the distance.

a)

electronegativity

b)

atomic size

c)

ionic size

d)

ionization energy

112.

Which atom has the smaller atomic size?

a)

As

b)

Br

113.

Which atom has the larger electronegativity?

a)

B

b)

In

114.

Which atom has the larger electronegativity?

a)

Rb

b)

Cs

115.

Which atom has the larger first ionization energy?

a)

Si

b)

Sn

116.

Which atom has the larger first ionization energy?

a)

Ti

b)

Mn

117.

Which atom or ion is larger?

a)

Fe2+

b)

Fe3+

118.

Which atom or ion is larger?

a)

N3-

b)

N

119.

Which atom or ion is larger?

a)

Ca2+

b)

Ca

120.

Which atom or ion is larger?

a)

P2-

b)

P1-

121.

Which atom or ion is larger?

a)

Br1-

b)

Br

122.

Which atom or ion is larger?

a)

Ca2+

b)

Ca

123.

Which atom or ion is larger?

a)

S

b)

S2-

124.

As you move from left to right across the periodic table the size of the atom will

a)

increase

b)

decrease

c)

not change

125.

Within a period the elements will have the same number of occupied _______

a)

orbitals

b)

sublevels

c)

Energy levels

126.

The ionization energy of the elements will _____ as you move down a group on the Periodic table.

a)

increase

b)

decrease

c)

no change

127.

As you move across a period from left to right the electronegativity of an element will _______.

a)

increase

b)

decrease

c)

stay the same

128.

As you move down a group, the electronegativity of an element will ______.

a)

increase

b)

decrease

c)

stay the same

129.

As the negative charge on an ion increases, the size of the atom will ______.

a)

increase

b)

decrease

c)

stay the same

130.

The highest possible value for electronegativity is

a)

4.0

b)

7.0

c)

5.0

d)

8

Similar Resources on Wayground

Simple Machines and

135 questions

Simple Machines and

quiz

Worksheet

•

12th Grade

Chemistry Final Practice

132 questions

Chemistry Final Practice

quiz

Worksheet

•

10th - 12th Grade

Chemistry Midterm Review 2

130 questions

Chemistry Midterm Review 2

quiz

Worksheet

•

10th - 12th Grade

Review: Chemistry Final Exam for 1st Semester 2023-24

127 questions

Review: Chemistry Final Exam for 1st Semester 2023-24

quiz

Worksheet

•

10th Grade

Midterm Review (Chemistry)

132 questions

Midterm Review (Chemistry)

quiz

Worksheet

•

9th - 12th Grade

CFE Review Standard

127 questions

CFE Review Standard

quiz

Worksheet

•

8th Grade - University

Unit 2 Review Quiz

133 questions

Unit 2 Review Quiz

quiz

Worksheet

•

9th Grade - University

Chem Semester 2 Final

130 questions

Chem Semester 2 Final

quiz

Worksheet

•

10th - 12th Grade