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C02 Trends of the Periodic Table

Total questions: 145

Worksheet time: 4hrs 1mins

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 have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

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.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
9.
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
10.

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

a)

the atoms have more mass, which increases the gravitational pull

b)

it doesn't, atoms get bigger going from left to right because of the additional protons and electrons that are being added.

c)

effective nuclear charge tends to increase

d)

atoms lose energy levels make them smaller

11.
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.
12.
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. 
13.
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
14.
Metals are good conductors of heat and electricity.
a)
true
b)
false
15.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
16.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
17.
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.
18.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
19.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

S

d)

Mg

20.
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
21.

According to the periodic trend, which periodic group has the smallest atomic radius?

a)

Alkali metals

b)

Halogens

c)

Noble Gases

d)

Transition metals

22.

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

23.
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 
24.
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
25.

If the distance between the two nuclei is 100pm, what is the atomic radius?

a)

200 pm

b)

100 pm

c)

50 pm

d)

25 pm

26.

Silicon has an atomic number of 14, what is it's effective nuclear charge?

a)

14

b)

4

c)

10

d)

7

27.

What is the effective nuclear charge for sodium?

a)

1

b)

11

c)

10

d)

2

28.

When looking at elements in the same period, why does increasing the effective nuclear charge make the atoms smaller?

a)

It increases the force of attraction between the protons thus pulling the protons closer together and making the atom smaller

b)

It increases the force of attraction on the valence electrons thus pulling the electrons closer to the nucleus and making the atom smaller

c)

If reduces the number of main energy levels or shells thus making the atom smaller

d)

It increases the force of repulsion the electrons have on each other thus causing the electrons to spread out and making the atom smaller

29.

Which of the following is the smallest?

a)

Na+

b)

K+

c)

Rb+

d)

Fr+

30.

Which of the following is the smallest?

a)

Na+

b)

Mg2+

c)

Al3+

31.

Which of the following is smallest?

a)

Cl-

b)

S2−

c)

P3−

32.

Which of the following is smaller?

a)

the anion (negative ion)

b)

parent atom

33.

Which of the following is smaller?

a)

the cation (positive ion)

b)

parent atom

34.

Which of the following is smaller?

a)

Sr2+

b)

Sr

35.

Which of the following is smaller?

a)

O

b)

O2−

36.

Why are cations smaller than their parent atoms?

a)

when cations form they gain protons which increases the effective nuclear charge which increases the force of attraction of the nucleus on the electrons causing the electron cloud to shrink

b)

when cations form they lose electrons which reduces the repulsion force between the electrons allowing the electron cloud to shrink.

37.

Why are anions larger than their parent atoms?

a)

when anions form they gain an additional outer shell thus making them larger

b)

when anions form they gain electrons which increases the repulsion force between the electrons causing the electron cloud to expand.

38.

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)

39.

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

40.

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

41.

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

42.

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

43.

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

44.

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

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

45.

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

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

46.

Which two groups are the most reactive?

a)

Group 1

b)

Group 2

c)

Group 16

d)

Group 17

e)

Group 18

47.

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

48.

Which of the given atoms has the lowest electron affinity?

a)

Sr

b)

Be

c)

Ca

d)

Ra

49.

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

50.

Put in order from biggest to smallest (decreasing size)

a)

Calcium

b)

Iron

c)

Zinc

d)

Bromine

e)

Krypton

1)
2)
3)
4)
5)
51.

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

Increases or decreases?

52.

This element has the lowest electron affinity

a)

magnesium

b)

sodium

c)

silicon

d)

sulfur

53.

What non-metal is the most reactive

a)

iodine

b)

sulfur

c)

oxygen

d)

fluorine

54.

What metal is most reactive

a)

lithium

b)

sodium

c)

potassium

d)

francium

55.

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

56.

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

57.

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

58.

Atomic radii trends is . . . .

a)

generally decrease along each period of the table, from the alkali metals to the noble gases; and increase down each group.

b)

generally increase along each period of the table, from the alkali metals to the noble gases; and increase down each group.

c)

generally increase along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

d)

generally decrease along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

59.

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.

60.

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.

61.

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.

62.

Which element has higher electron affinity?

a)

Bromine is higher than Calsium

b)

Chlorine is higher than Fluorine

c)

Magnesium is higher than Beryllium

d)

Sodium is higher than Aluminium

63.

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

64.

Put these in order of decreasing size (largest to smallest) (Left to Right)

a)

B

b)

C

c)

N

d)

O

e)

F

1)
2)
3)
4)
5)
65.

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)
66.

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)
67.

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)
68.

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

Increases or decreases?

69.

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

Increases or decreases?

70.

Atomic radii (a)   as you go from left to right.

Increases or decreases?

71.

Ionic radii (a)   as you go across a period from left to right.

Increases or decreases?

72.

Atomic radii (a)   as you go UP a group

Increases or decreases?

73.

Atomic radii (a)   as you go DOWN a group

Increases or decreases?

74.

Electronegativity (a)   as you go UP a group

Increases or decreases?

75.

Ionization Energy (a)   as you go UP a group

Increases or decreases?

76.

Electron Affinity (a)   as you go UP a group

Increases or decreases?

77.

Electron Affinity (a)   as you go DOWN a group

Increases or decreases?

78.

Ionization Energy (a)   as you go DOWN a group

Increases or decreases?

79.

Electronegativity (a)   as you go DOWN a group

Increases or decreases?

80.

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)
81.

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)
82.

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)
83.

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

a)

Cs

b)

Rb

c)

K

d)

Na

e)

Li

1)
2)
3)
4)
5)
84.

Which one is predicted to be bigger,

O, S, Se or Te?

(a)  

85.

Which one is predicted to be smallest,

O, S, Se or Te?

(a)  

86.

Which one is predicted to have the HIGHEST Electronegativity?

O, S, Se or Te?

(a)  

87.

Which one is predicted to have the HIGHEST Electron Affinity?

O, S, Se or Te?

(a)  

88.

Which one is predicted to have the HIGHEST Ionization Energy?

O, S, Se or Te?

(a)  

89.

Which one is predicted to have the LOWEST Electronegativity?

O, S, Se or Te?

(a)  

90.

Which one is predicted to have the LOWEST Ionization Energy?

O, S, Se or Te?

(a)  

91.

Which one is predicted to have the LOWEST Electron Affinity?

O, S, Se or Te?

(a)  

92.

Which one is predicted to have the LOWEST Electron Affinity?

B, C, N, or O

(a)  

93.

Which one is predicted to have the LOWEST Ionization Energy?

B, C, N, or O

(a)  

94.

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.

95.

As you move down a group, the effective nuclear charge

a)

increase

b)

decreases

c)

stays the same

96.

Effective nuclear charge ________ across a period.

a)

increases

b)

decreases

c)

stays the same

97.

Why does Cs have a larger radius than Na?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a less effective nuclear charge

98.

Why does Ca have a larger radius than Se?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a lower effective nuclear charge

99.

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

a)

nitrogen

b)

phosphorus

c)

arsenic

d)

bismuth

100.

In the following configuration, which electrons are the core electrons?

1s2 2s2 2p6 3s2 3p4

Hint: 1s = 1st shell, 2s & 2p = 2nd shell, 3s & 3p = 3rd shell

a)

1s2 2s2 2p6

b)

3s2 3p4

c)

1s2 2s2

d)

2s2 2p6 3s2 3p4

101.

In the following configuration, which electrons are the valence electrons?

1s2 2s2 2p6 3s2 3p4

Hint: 1s = 1st shell, 2s & 2p = 2nd shell, 3s & 3p = 3rd shell

a)

1s2

b)

3s2 3p4

c)

1s2 2s23s2

d)

2s2 2p6 3s2 3p4

e)

2s2 2p6

102.

How many shielding electrons does carbon have? (hint: find the total number of electrons and subtract the valence electrons)

a)
1
b)
2
c)
3
d)
4
e)

6

103.
How many valence electrons does carbon have?
a)
3
b)
4
c)
5
d)
6
104.
Which of the following elements has the most "shielding" electrons?
a)
Neon
b)
flourine
c)
oxygen
d)
They have the same
105.

Which of these represents a group?

A
B
106.

Which of these represents a period?

A
B
107.
Which of the following elements has the highest effective nuclear charge?
a)
Indium
b)
Antimony
c)
tellerium
d)
Tin
108.
Which of the following elements has a greater effective nuclear charge?
a)

lithium

b)

calcium

c)

phosphorus

d)

aluminum

109.

What is the effective nuclear charge of sodium?

(a)  

110.

What is the effective nuclear charge of calcium?

(a)  

111.

What is the effective nuclear charge of aluminum?

(a)  

112.

What is the effective nuclear charge of carbon?

(a)  

113.

What is the effective nuclear charge of nitrogen?

(a)  

114.

What is the effective nuclear charge of sulfur?

(a)  

115.

What is the effective nuclear charge of chlorine?

(a)  

116.

What is the effective nuclear charge of neon?

(a)  

117.

What is the effective nuclear charge of neon?

(a)  

118.

What periodic trend do you notice between the atomic mass and the atomic number?

a)

Atomic mass usually increases as the atomic number increases

b)

Atomic mass does not change across a row but does increase down a group

c)

There is no relationship between atomic number and atomic mass.

d)

Atomic mass usually decreases as the atomic number increases

e)

Atomic mass is double the atomic number

119.

What periodic trend do you notice about atomic mass?

(Mark all that apply.)

a)

Atomic mass usually increases across a row

b)

Atomic mass increases down a group

c)

Atomic mass usually decreases across a row

d)

Atomic mass usually decreases down a row

e)

Atomic mass increases then decreases across a row

120.

What periodic trend do you notice about atomic number?

(Mark all that apply.)

a)

Atomic number usually increases across a row

b)

Atomic number increases down a group

c)

Atomic number usually decreases across a row

d)

Atomic number usually decreases down a row

e)

Atomic number stays constant down a group.

121.

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.

122.

What is true when moving from left to right across a row in the first 3 periods?

a)

electrons are added to the same electron shell

b)

the number of energy levels increase

c)

the number of energy levels decrease

d)

electrons are added to different electron shells

123.

What is true when moving down a group?

a)

electrons are added to the same electron shell

b)

the number of energy levels increase

c)

the number of energy levels decrease

d)

electrons are added to different electron shells

124.

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

125.

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.

126.

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.

127.

Which of the following correctly describes the GROUP trend for atomic radius?

a)

Atomic radius increases as new electrons are added within the same electron shell

b)

Atomic radius decreases with increasing number of energy levels.

c)

Atomic radius decreases as new electrons are added within the same electron shell

d)

Atomic radius increases with increasing number of energy levels.

128.

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

a)

Atomic radius increases as new electrons are added within the same electron shell

b)

Atomic radius decreases with increasing number of energy levels.

c)

Atomic radius decreases as new electrons are added within the same electron shell

d)

Atomic radius increases with increasing number of energy levels.

129.

Which of the following correctly describes the PERIOD (L to R) 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.

130.

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.

131.

Why does ionization energy increase across a period (L to R)?

a)

increasing effective nuclear charge

b)

increasing valence electrons

c)

increasing number of electron shells

d)

decreasing number of electron shells

e)

decreasing effective nuclear charge

132.

Why does ionization energy decrease down a group?

a)

increasing effective nuclear charge

b)

increasing valence electrons

c)

increasing number of electron shells

d)

decreasing number of electron shells

e)

decreasing effective nuclear charge

133.

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

134.

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

135.

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

136.

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

137.

What trend do you notice for the atomic radii shown in the picture?

Select a correct answer

a)

atomic radius decreases as atomic numbers increase

b)

atomic radius decreases from lithium to potassium

c)

atomic radius decreases from lithium to neon

d)

Ionization energy decreases helium to calcium

138.

What trend do you notice for the atomic radii shown in the picture?

Select a correct answer

a)

atomic radius increases as atomic numbers increase

b)

atomic radius increases from lithium to potassium

c)

atomic radius increases from lithium to neon

d)

Ionization energy increases from sodium to zinc

139.

How much energy is need to remove the first electron from aluminum?

a)

578 kJ/mol

b)

1817 kJ/mol

c)

2745 kJ/mol

d)

11575 kJ/mol

e)

14830 kJ/mol

140.

How much energy is need to remove the second electron from aluminum?

a)

578 kJ/mol

b)

1817 kJ/mol

c)

2745 kJ/mol

d)

11575 kJ/mol

e)

14830 kJ/mol

141.

How much energy is need to remove the third electron from aluminum?

a)

578 kJ/mol

b)

1817 kJ/mol

c)

2745 kJ/mol

d)

11575 kJ/mol

e)

14830 kJ/mol

142.

How much energy is need to remove the fourth electron from aluminum?

a)

578 kJ/mol

b)

1817 kJ/mol

c)

2745 kJ/mol

d)

11575 kJ/mol

e)

14830 kJ/mol

143.

How much energy is need to remove the fifth electron from aluminum?

a)

578 kJ/mol

b)

1817 kJ/mol

c)

2745 kJ/mol

d)

11575 kJ/mol

e)

14830 kJ/mol

144.

match the Periodic Trends

a)

increase across a period and increases down a group

1.

atomic mass

b)

increases across a period and decreases down a group, does NOT include the Noble gases

2.

electronegativity

c)

increases across a period and decrease down a group, does include the Noble Gases

3.

Ionization energy

d)

decreases across a period and increases down a group

4.

atomic radius

145.

Which Trends include the noble gases?

Categorize the following

ionization energy

atomic mass

atomic radius

electronegativity

ionic radius

Includes the Noble Gases
Does NOT include the Noble Gase

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