wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

C02 Trends IE EA EN Reactivity

Total questions: 120

Worksheet time: 3hrs 34mins

Name
Class
Date
1.

Base on the trend, which has the greater electronegativity,

Cl or Al?

a)

Cl

b)

Al

2.

Base on the trend, which has the greater electronegativity,

N or C?

a)

C

b)

N

3.

Based on the trend, which has the greater electronegativity,

H or F?

a)

H

b)

F

4.

Which of the following will definitely have a larger radius than Zinc?

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

5.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

e)

Chlorine (Cl)

6.
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)
7.

For elements in Group 16, how does the electronegativity change as you go down the group?

a)

decreases

b)

increases

c)

remains the same

d)

none of the above

8.
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.
9.
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. 
10.
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
11.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
12.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

S

d)

Mg

13.
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
14.

Based on electronegativity trends in the periodic table, which of the following is the most likely value for the electronegativity of silicon?

a)

2.44

b)

1.23

c)

2.22

d)

2.03

15.
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
16.

The electron cloud is ... (pick all that apply)

a)

mostly empty space

b)

mostly electrons with little empty space

c)

free to expand and contract

d)

static (does NOT change its size)

17.

Which one of the following deals with atoms losing electrons and forming positive ions?

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

18.

Which of the following increases across a row from left to right? (Mark all that apply)

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

e)

electron affinity

19.

Which of the following DECREASES across a row from left to right? (Mark all that apply)

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

e)

electron affinity

20.

Which of the following increases across a row from left to right but does NOT include the Noble Gases? (Mark all that apply)

a)

atomic radii

b)

electronegativity

c)

ionization energy

21.

Which of the following increases across a row from left to right and INCLUDES the Noble Gases? (Mark all that apply)

a)

atomic radii

b)

electronegativity

c)

ionization energy

22.

Which of the following decreases down a group? (Mark all that apply)

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

e)

electron affinity

23.

Which of the following increases down a group? (Mark all that apply)

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

e)

electron affinity

24.

Which two groups are the most reactive?

a)

Group 1

b)

Group 2

c)

Group 16

d)

Group 17

e)

Group 18

25.

Base on the Reactivity Trend, which two groups would be the second most reactive?

a)

Group 1

b)

Group 2

c)

Group 16

d)

Group 17

e)

Group 18

26.

Which of the given atoms has the lowest electron affinity?

a)

Sr

b)

Be

c)

Ca

d)

Ra

27.

Which element would experience the greatest energy loss when a neutral atom in the gaseous phase gains one additional electron?

a)

Lithium

b)

Fluorine

c)

Chlorine

d)

Krypton

28.

Electron affinity (a)   as you go from left to right.

Increases or decreases?

29.

This element has the lowest electron affinity

a)

magnesium

b)

sodium

c)

silicon

d)

sulfur

30.

What non-metal is the most reactive

a)

iodine

b)

sulfur

c)

oxygen

d)

fluorine

31.

What metal is most reactive

a)

lithium

b)

sodium

c)

potassium

d)

francium

32.

The energy it takes to remove one electron from an atom

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

33.

The tendency of an atom to attract a shared pair of electrons

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

34.

The amount of energy released when an electron is added to a neutral atom to form a negative ion

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

35.

Ionization energy trend . . . .

a)

becomes greater up and to the right of the periodic table.

b)

becomes greater down and to the right of the periodic table.

c)

becomes greater up and to the left of the periodic table.

d)

becomes greater down and to the left of the periodic table.

36.

Electronegativity trends is . . . .

a)

increases on passing from left to right along a period, and decreases on descending a group.

b)

increases on passing from left to right along a period, and increases on descending a group.

c)

decreases on passing from left to right along a period, and decreases on descending a group.

d)

decreases on passing from left to right along a period, and increases on descending a group.

37.

Electron affinity trends is . . . .

a)

generally increases across a period, and a trend of decreasing electron affinity going down groups would be expected.

b)

generally decreases across a period, and a trend of decreasing electron affinity going down groups would be expected.

c)

generally increases across a period, and a trend of increasing electron affinity going down groups would be expected.

d)

generally decreases across a period, and a trend of increasing electron affinity going down groups would be expected.

38.

Which element has higher electron affinity?

a)

Bromine is higher than Calcium

b)

Chlorine is higher than Fluorine

c)

Magnesium is higher than Beryllium

d)

Sodium is higher than Aluminium

39.

Which element has lower electron affinity?

a)

Bromine is lower than Calsium

b)

Chlorine is lower than Fluorine

c)

Berylliumis lower than Magnesium

d)

Aluminium is lower than Sodium

40.

Put these in order of predicted increasing electron affinity (smallest to largest) (Left to Right)

a)

B

b)

C

c)

N

d)

O

e)

F

1)
2)
3)
4)
5)
41.

Put these in order of predicted increasing ionization energy (smallest to largest) (Left to Right)

a)

Al

b)

Si

c)

P

d)

S

e)

Cl

1)
2)
3)
4)
5)
42.

Put these in order of predicted increasing electronegativity (smallest to largest) (Left to Right)

a)

Al

b)

Si

c)

P

d)

S

e)

Cl

1)
2)
3)
4)
5)
43.

Electronegativity (a)   as you go from left to right.

Increases or decreases?

44.

Ionization Energy (a)   as you go from left to right.

Increases or decreases?

45.

Electronegativity (a)   as you go UP a group

Increases or decreases?

46.

Ionization Energy (a)   as you go UP a group

Increases or decreases?

47.

Electron Affinity (a)   as you go UP a group

Increases or decreases?

48.

Electron Affinity (a)   as you go DOWN a group

Increases or decreases?

49.

Ionization Energy (a)   as you go DOWN a group

Increases or decreases?

50.

Electronegativity (a)   as you go DOWN a group

Increases or decreases?

51.

Put these in order of predicted INCREASING electronegativity (smallest to largest) (Left to Right)

a)

I

b)

Br

c)

Cl

d)

F

1)
2)
3)
4)
52.

Put these in order of predicted INCREASING ionization energy (smallest to largest) (Left to Right)

a)

Cs

b)

Rb

c)

K

d)

Na

e)

Li

1)
2)
3)
4)
5)
53.

Put these in order of predicted INCREASING electron affinity (smallest to largest) (Left to Right)

a)

I

b)

Br

c)

Cl

d)

F

1)
2)
3)
4)
54.

Which one is predicted to have the HIGHEST Electronegativity?

O, S, Se or Te?

(a)  

55.

Which one is predicted to be smallest,

O, S, Se or Te?

(a)  

56.

Which one is predicted to be bigger,

O, S, Se or Te?

(a)  

57.

Which one is predicted to have the LOWEST Electronegativity?

O, S, Se or Te?

(a)  

58.

Which one is predicted to have the HIGHEST Ionization Energy?

O, S, Se or Te?

(a)  

59.

Which one is predicted to have the LOWEST Ionization Energy?

O, S, Se or Te?

(a)  

60.

Which one is predicted to have the LOWEST Electron Affinity?

O, S, Se or Te?

(a)  

61.

Which one is predicted to have the LOWEST Electron Affinity?

B, C, N, or O

(a)  

62.

Which one is predicted to have the LOWEST Ionization Energy?

B, C, N, or O

(a)  

63.

What is effective nuclear charge?

a)

The charge that effects the mass of the atom.

b)

The charge that the protons feel from the rest of the atom.

c)

The charge felt by the valence electrons.

d)

The charge felt by the core electrons.

64.

As you move down a group, the effective nuclear charge

a)

increase

b)

decreases

c)

stays the same

65.

Effective nuclear charge ________ across a period.

a)

increases

b)

decreases

c)

stays the same

66.

Which of the following elements has the most "shielding" electrons?

a)

nitrogen

b)

phosphorus

c)

arsenic

d)

bismuth

67.

What periodic trend do you notice about valence electrons?

(Mark all that apply.)

a)

Valence electrons increase across a row

b)

Valence electrons increase down a group

c)

Valence electrons decrease across a row

d)

Valence electrons decrease down a row

e)

Valence electrons stay constant down a group.

68.

Which of the following correctly describes the trend for electronegativity?

a)

Electronegativity increases with increasing number of energy levels. Electronegativity increases as new electrons are added within the same electron shell

b)

Electronegativity decreases with increasing number of energy levels. Electronegativity increases as new electrons are added within the same electron shell

c)

Electronegativity increases with increasing number of energy levels. Electronegativity decreases as new electrons are added within the same electron shell

d)

Electronegativity decreases with increasing number of energy levels. Electronegativity decreases as new electrons are added within the same electron shell

69.

Which of the following correctly describes the PERIOD (L to R) trend for electronegativity?

a)

Electronegativity increases as new electrons are added within the same electron shell

b)

Electronegativity decreases with increasing number of energy levels.

c)

Electronegativity decreases as new electrons are added within the same electron shell

d)

Electronegativity increases with increasing number of energy levels.

70.

Which of the following correctly describes the GROUP trend for electronegativity?

a)

Electronegativity increases as new electrons are added within the same electron shell

b)

Electronegativity decreases with increasing number of energy levels.

c)

Electronegativity decreases as new electrons are added within the same electron shell

d)

Electronegativity increases with increasing number of energy levels.

71.

Which of the following correctly describes the PERIOD (L to R) trend for Ionization Energy?

a)

Ionization Energy increases as new electrons are added to the valence electron shell

b)

Ionization Energy decreases with increasing number of energy levels.

c)

Ionization Energy decreases as new electrons are added to the valence electron shell

d)

Ionization Energy increases with increasing number of energy levels.

72.

Which of the following correctly describes the GROUP trend for Ionization Energy?

a)

Ionization Energy increases as new electrons are added within the same electron shell

b)

Ionization Energy decreases with increasing number of energy levels.

c)

Ionization Energy decreases as new electrons are added within the same electron shell

d)

Ionization Energy increases with increasing number of energy levels.

73.

On the graph what does Na to Ar represent?

a)

a group

b)

a period

c)

an electron orbital

d)

a radom collection of elements

74.

On the graph what does Li to Fr represent?

a)

a group

b)

a period

c)

an electron orbital

d)

a radom collection of elements

75.

What trend do you notice for the ionization energies shown in the picture?

Select a correct answer

a)

Ionization energy decreases as atomic numbers increase

b)

Ionization energy decreases from hydrogen to helium

c)

Ionization energy decreases from helium to argon

d)

Ionization energy decreases lithium to oxygen

76.

What trend do you notice for the ionization energies shown in the picture?

Select a correct answer

a)

Ionization energy increases as atomic numbers increase

b)

Ionization energy increases from neon to sodium

c)

Ionization energy increases from lithium to neon

d)

Ionization energy increases helium to oxygen

77.

  • Weak electrostatic attractions make it easy to ​ (a)   electrons, but harder to ​ (b)   electrons

  • Strong electrostatic attractions make it easier to ​ (c)   electrons, but harder to ​ (d)   electrons.

Choose from the below words
lose
gain
78.

Categorize the following as related to an increasing force or decreasing force of attraction between the NUCLEUS and the VALENCE ELECTRONS

Categorize the following

decreasing atomic radius

increasing ionization energy

increasing electronegativity

caused by higher effective nuclear charge

increasing atomic radius

decreasing ionization energy

decreasing electronegativity

caused by more shielding

increasing electron affinity

decreaing electron affinity

Increasing Force of Attraction
Deceasing Force of Attraction
79.

Which of the following correctly describes why electronegativity increases across a row? pick 2

a)

a decrease in the strength of attraction between the nucleus and valence electrons occurs

b)

atoms get smaller bringing the charges closer

c)

an increase in the strength of attraction between the nucleus and valence electrons occurs

d)

atoms get bigger creating more separation between the charges

80.

Which of the following correctly describes why ionization energy increases across a row? pick 2

a)

a decrease in the strength of attraction between the nucleus and valence electrons occurs

b)

atoms get smaller bringing the charges closer

c)

an increase in the strength of attraction between the nucleus and valence electrons occurs

d)

atoms get bigger creating more separation between the charges

81.

Which of the following correctly describes why ionization energy decreases down a group? pick 2

a)

a decrease in the strength of attraction between the nucleus and valence electrons occurs

b)

atoms get smaller bringing the charges closer

c)

an increase in the strength of attraction between the nucleus and valence electrons occurs

d)

atoms get bigger creating more separation between the charges

82.

Which of the following correctly describes why electron affinity decreases down a group? pick 2

a)

a decrease in the strength of attraction between the nucleus and valence electrons occurs

b)

atoms get smaller bringing the charges closer

c)

an increase in the strength of attraction between the nucleus and valence electrons occurs

d)

atoms get bigger creating more separation between the charges

83.

Which of the following correctly describes why electron affinity increases across a row? pick 2

a)

a decrease in the strength of attraction between the nucleus and valence electrons occurs

b)

atoms get smaller bringing the charges closer

c)

an increase in the strength of attraction between the nucleus and valence electrons occurs

d)

atoms get bigger creating more separation between the charges

84.

Which of the following correctly describes why electronegativity decreases down a group? pick 2

a)

a decrease in the strength of attraction between the nucleus and valence electrons occurs

b)

atoms get smaller bringing the charges closer

c)

an increase in the strength of attraction between the nucleus and valence electrons occurs

d)

atoms get bigger creating more separation between the charges

85.

Which element is MOST Likely to lose an electron?

a)

Element Q

b)

Element R

c)

Element S

d)

Element T

e)

Element U

86.

Which element is LEAST Likely to lose an electron?

a)

Element Q

b)

Element R

c)

Element S

d)

Element T

e)

Element U

87.

Which element has the STRONGEST Force of Attraction between the nucleus and the valence electrons?

a)

Element Q

b)

Element R

c)

Element S

d)

Element T

e)

Element U

88.

Which element has the WEAKEST Force of Attraction between the nucleus and the valence electrons?

a)

Element Q

b)

Element R

c)

Element S

d)

Element T

e)

Element U

89.

Element R is...

a)

most likely to lose an electron

b)

least likely to lose an electron

c)

most likely to gain an electron

d)

least likely to gain an electron

90.

Element S is...

a)

most likely to lose an electron

b)

least likely to lose an electron

c)

most likely to gain an electron

d)

least likely to gain an electron

91.

Element D is...

a)

most likely to lose an electron

b)

least likely to lose an electron

c)

most likely to gain an electron

d)

least likely to gain an electron

92.

Element C is...

a)

most likely to lose an electron

b)

least likely to lose an electron

c)

most likely to gain an electron

d)

least likely to gain an electron

93.

Which element has the STRONGEST Force of Attraction between the nucleus and the valence electrons?

a)

Element A

b)

Element B

c)

Element C

d)

Element D

e)

Element E

94.

From the elements listed

Element D has the...

a)

strongest force of attraction between the nucleus and valence electrons

b)

weakest force of attraction between the nucleus and valence electrons

95.

Which element has the WEAKEST Force of Attraction between the nucleus and the valence electrons?

a)

Element A

b)

Element B

c)

Element C

d)

Element D

e)

Element E

96.

Which element is MOST LIKELY to gain an electron?

a)

Element A

b)

Element B

c)

Element C

d)

Element D

e)

Element E

97.

Which element is LEAST LIKELY to gain an electron?

a)

Element A

b)

Element B

c)

Element C

d)

Element D

e)

Element E

98.

According to Coulomb's Law what happens to the electrostatic force if the atom gets bigger and the valence electrons are moved further AWAY from the nucleus?

a)

force of ATTRACTION between the valence electrons and the nucleus INCREASES

b)

force of ATTRACTION between the valence electrons and the nucleus DECREASES

c)

force of REPULSION between the valence electrons and the nucleus INCREASES

d)

force of REPULSION between the valence electrons and the nucleus DECREASES

99.

According to Coulomb's Law what happens to the electrostatic force if the atom gets smaller and the valence electrons are moved CLOSER TO the nucleus?

a)

force of ATTRACTION between the valence electrons and the nucleus INCREASES

b)

force of ATTRACTION between the valence electrons and the nucleus DECREASES

c)

force of REPULSION between the valence electrons and the nucleus INCREASES

d)

force of REPULSION between the valence electrons and the nucleus DECREASES

100.

According to periodic trends, which element has a HIGHER ionization energy,

Li or B?

A
B
101.

According to periodic trends, which element is more likely to LOSE an electron,

Li or B?

A
B
102.

According to the periodic trend, which element has a HIGHER ionization energy,

B or O?

A
B
103.

According to the periodic trend, which element is MORE likely to LOSE an electron

B or O?

A
B
104.

According to the periodic trend, which element has a HIGHER ionization energy,

Li or O?

A
B
105.

According to the periodic trend, which element is MORE likely to LOSE an electron,

Li or O?

A
B
106.

According to the periodic trend, which element is MORE likely to LOSE an electron,

Li or Cs?

A
B
107.

According to the periodic trend, which element is MORE likely to LOSE an electron,

N or As?

A
B
108.

According to the periodic trend, which element has a HIGHER ionization energy,

N or As?

A
B
109.

According to the periodic trend, which element has a HIGHER ionization energy,

Ca or Ba?

A
B
110.

According to the periodic trend, which element has a HIGHER electron affinity,

rubidium or iodine?

A
B
111.

According to the periodic trend, which element has a HIGHER electron affinity,

fluorine or iodine?

A
B
112.

According to the periodic trend, which element has a HIGHER electron affinity,

lithium or carbon?

A
B
113.

According to the periodic trend, which element has a HIGHER electron affinity,

aluminum or indium?

A
B
114.

According to the periodic trend, which element is MORE likely to GAIN an electron

rubidium or iodine?

A
B
115.

According to the periodic trend, which element is MORE likely to GAIN an electron

fluorine or iodine?

A
B
116.

According to the periodic trend, which element is MORE likely to GAIN an electron

potassium or boron?

A
B
117.

According to the periodic trend, which element is MORE likely to GAIN an electron aluminum or indium?

A
B
118.

According to the periodic trend, which element is LESS likely to GAIN an electron

rubidium or iodine?

A
B
119.

Using the Blank Periodic Table:

Which elements would be highly reactive?

​ ​ (a)   ​ (b)   ​ (c)   ​

Choose from the below words
J
H
E
A
F
G
B
C
D
120.

Categorize these properties

Categorize the following

smaller atomic radius

bigger ionization energy

bigger electron affinity

bigger atomic radius

smaller ionization energy

smaller electron affinity

weaker force of attraction on the valence electrons

stronger force of attraction on the valence electrons

Smaller Atoms
Larger Atoms

Similar Resources on Wayground

Periodic Law Review

120 questions

Periodic Law Review

quiz

Worksheet

•

11th Grade

IIT-JEE & NEET LEVEL-7 (9-O)

120 questions

IIT-JEE & NEET LEVEL-7 (9-O)

quiz

Worksheet

•

9th Grade

Ionic Compounds (Chapter 8)

115 questions

Ionic Compounds (Chapter 8)

quiz

Worksheet

•

9th - 12th Grade

LATIHAN KIMIA

118 questions

LATIHAN KIMIA

quiz

Worksheet

•

10th Grade

Metric Conversion Practice

123 questions

Metric Conversion Practice

quiz

Worksheet

•

9th - 12th Grade

U2 Quiz Review

120 questions

U2 Quiz Review

quiz

Worksheet

•

11th Grade

Ôn tập cuối học kì 1-Cơ bản

117 questions

Ôn tập cuối học kì 1-Cơ bản

quiz

Worksheet

•

10th Grade

Unit 8 and 9 Test. Physical Science (Atoms and Compounds)

120 questions

Unit 8 and 9 Test. Physical Science (Atoms and Compounds)

quiz

Worksheet

•

9th - 12th Grade