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C02 Trends Atomic/Ionic Radii

Total questions: 96

Worksheet time: 2hrs 43mins

Name
Class
Date
1.

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.

2.

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

a)

electrons are added only to the valence shell

b)

the number of energy levels increase

c)

the number of energy levels decrease

d)

shielding electrons are added to inner shells.

3.

What is true when moving down a group?

a)

electrons are added only to the valence shell

b)

the number of energy levels increase

c)

the number of energy levels decrease

d)

electrons are added to different electron shells

4.

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.

5.

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.

6.

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

7.

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

8.

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

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

9.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
10.
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
11.

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

12.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
13.
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.
14.

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

a)

Alkali metals

b)

Halogens

c)

Noble Gases

d)

Transition metals

15.
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 
16.

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

17.

If the distance between the two nuclei is 50pm, what is the atomic radius?

a)

200 pm

b)

100 pm

c)

50 pm

d)

25 pm

18.

If the distance between the two nuclei is 200pm, what is the atomic radius?

a)

200 pm

b)

100 pm

c)

50 pm

d)

25 pm

19.

How many shielding electrons does sulfur have?

(a)  

20.

How many protons does sulfur have?

(a)  

21.

What is sulfur's effective nuclear charge (Zeff)

(a)  

22.

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

a)

+14

b)

+4

c)

+10

d)

+7

23.

What is the effective nuclear charge for sodium?

a)

+1

b)

+11

c)

+10

d)

+2

24.

How many shielding electrons does sodium (Na) have?

a)

1

b)

2

c)

10

d)

11

e)

8

25.

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

26.

Which of the following is the smallest?

a)

Na+

b)

K+

c)

Rb+

d)

Fr+

27.

Which of the following is the smallest?

a)

Na+

b)

Mg2+

c)

Al3+

28.

Which of the following is smallest?

a)

Cl-

b)

S2−

c)

P3−

29.

Which of the following is smaller?

a)

the anion (negative ion)

b)

parent atom

30.

Which of the following is smaller?

a)

the cation (positive ion)

b)

parent atom

31.

Which of the following is smaller?

a)

Sr2+

b)

Sr

32.

Which of the following is smaller?

a)

O

b)

O2−

33.

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 all of the valence electrons which leaves the valence shell empty. The next lower shell (which is smaller) becomes the new outer shell.

34.

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.

35.

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)

36.

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

37.

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

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

38.

Put in order from biggest to smallest (decreasing size)

a)

Calcium

b)

Iron

c)

Zinc

d)

Bromine

e)

Krypton

1)
2)
3)
4)
5)
39.

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.

40.

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)
41.

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

Increases or decreases?

42.

Atomic radii (a)   as you go DOWN a group

Increases or decreases?

43.

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)
44.

Which one is predicted to be bigger,

O, S, Se or Te?

(a)  

45.

Which one is predicted to be smallest,

O, S, Se or Te?

(a)  

46.

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

47.

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

48.
How many valence electrons does carbon have?
a)
3
b)
4
c)
5
d)
6
49.

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

50.

Which of these represents a group?

A
B
51.

Which of these represents a period?

A
B
52.

Using the periodic trends.

Which element is bigger?

a)

sodium, Na

b)

sulfur, S

c)

can't tell using just the trends

53.

Using the periodic trends.

Which element is bigger?

a)

carbon, C

b)

fluorine, F

c)

can't tell using just the trends

54.

Using the periodic trends.

Which element is bigger?

a)

sodium, Na

b)

potassium, K

c)

can't tell using just the trends

55.

Using the periodic trends.

Which element is bigger?

a)

magnesium, Mg

b)

potassium, K

c)

can't tell using just the trends

56.

Using the periodic trends.

Which element is bigger?

a)

magnesium, Mg

b)

lithium, Li

c)

can't tell using just the trends

57.

According to periodic trends which part of the periodic table contains the BIGGEST atoms (largest radius)?

A
B
C
D
58.

According to periodic trends which part of the periodic table contains the SMALLEST atoms (smallest radius)?

A
B
C
D
59.

Select all of the shielding electrons.

A
B
C
D
E
F
G
H
I
60.

Select all of the valence electrons.

A
B
C
D
E
61.

According to Coulomb's Law, OPPOSITE charges .....

a)

attract

b)

repel

c)

neither

62.

According to Coulomb's Law, LIKE charges .....

a)

attract

b)

repel

c)

neither

63.

According to Coulomb's Law, BIGGER charges means...

a)

stronger force

b)

weaker force

c)

no change

64.

According to Coulomb's Law, SMALLER charges means...

a)

stronger force

b)

weaker force

c)

no change

65.

According to Coulomb's Law, charges FARTHER apart means...

a)

stronger force

b)

weaker force

c)

no change

66.

According to Coulomb's Law, charges CLOSER together means...

a)

stronger force

b)

weaker force

c)

no change

67.

Click on the end of the period with the

Higher Zeff

A
B
68.

Click on the end of the period with the

Bigger Atoms

A
B
69.

Click on the end of the period with the

Smaller Atoms

A
B
70.

Click on the end of the period with the

Lower Zeff

A
B
71.

Which one has a larger radius, the atom or the ion? (Click on it.)

A
B
72.

Which one is bigger, the atom or the ion?

Click on it.

A
B
73.

How does Zeff change down a group?

a)

Zeff increases down a group

b)

Zeff decreases down a group

c)

Zeff stays relatively constant down a group

74.

Choose the element with the largest atomic radius.

A
B
C
D
E
75.

The atomic radius (a)   across a row from left to right and ​ ​ (b)   down a group. ​

Choose from the below words
decreases
increases
goes up and down
stays the same
76.
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
77.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
78.

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

a)

Oxygen

b)

Sulfur

c)

Tellurium

79.

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

a)

Oxygen

b)

Sulfur

c)

Tellurium

80.

Which would be a correct title for this diagram?

a)

Electronegativity trends

b)

Atomic Radius trends

c)

Atomic Mass trends

81.

Which of the following atoms has the largest atomic radius?

a)

nitrogen

b)

phosphorus

c)

potassium

d)

cesium

82.

What causes the shielding effect inside an atom?

a)

the electrons between the nucleus and the valence shell

b)

the extra neutrons in the nucleus

c)

the extra protons in the nucleus

d)

the valence electrons only

83.

What property is being measured in this diagram?

a)

Density

b)

Electronegativity

c)

Atomic Radius

d)

Atomic Mass

84.

Ions are formed when atoms gain or lose ___.

a)

electrons

b)

protons

c)

neutrons

d)

atomic mass

85.

How do scientists measure the size of atoms?

a)

by counting energy levels

b)

measuring the distance between 2 nuclei

c)

measuring the nucleus

d)

using the atomic number

86.

In group 2, which of these elements has the largest atomic radius?

a)

Ba

b)

Mg

c)

Ca

d)

La

87.

Which of these halogens has the largest atomic radius?

a)

fluorine, F

b)

chlorine, Cl

c)

bromine, Br

d)

iodine, I

88.

As you move across a period, what happens to the nuclear charge in the atoms?

a)

It increases because more protons are added.

b)

It decreases because protons are taken away.

c)

It stays the same.

89.

When an atom loses an electron, the size will

a)

be greater

b)

decrease then increase back to normal size

c)

have no change

d)

be smaller

90.

When atom gains an electron, the size will

a)

increase

b)

decrease

c)

have no change

d)

increase then decrease back to normal size

91.

Which end contains BIGGER atoms?

A
B
92.

Which end contains SMALLER atoms?

A
B
93.

What does Zeff stand for? (3 words)

(a)  

94.

Label the arrows for the correct trends for

Atomic Radius

a)decreases
b)increases
c)constant
d)varies
1
2
1)
2)
95.

If the force of attraction between the nucleus and valence electrons INCREASES what is the effect on the size of the atom?

a)

atomic radius decreases

b)

atomic radius increases

c)

no effect

96.

If the force of attraction between the nucleus and valence electrons DECREASES what is the effect on the size of the atom?

a)

atomic radius decreases

b)

atomic radius increases

c)

no effect

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