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Chapter 5 Test Review

Total questions: 111

Worksheet time: 2hrs 59mins

Name
Class
Date
1.
In the modern periodic table, elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
2.
What is another name for the elements in group 1A?
a)
Alkaline Earth Metals
b)
Noble gases
c)
Transition Metals
d)
Alkali Metals
3.
Alkaline Earth Metals are found in which group of the periodic table?
a)
Group 1
b)
Group 2
c)
Group 3
d)
group 4
4.
Elements in the same ________ are chemically similar.
a)
group
b)
period
c)
octave
d)
table
5.
In the picture, the elements located on either side of the red line are called...
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
6.
Lithium (Li) is part of the _ family.
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
Noble gases
7.
Chromium (Cr) is part of the _ family.
a)
Alkali Metals
b)
Alkaline Earth Metals
c)
Transition Metals
d)
Precious Metals
8.
Alkaline Earth metals each have ___ valence electrons.
a)
2
b)
1
c)
5
d)
1 or 2
9.
Which elements are the most similar regarding their chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
10.
Which family of metals would be the most reactive?
a)
Noble Metals
b)
Transition Metals
c)
Alkaline Earth Metals
d)
Alkali Metals
11.

Shiny, good conductors, malleable and ductile

a)

metals

b)

nonmetals

12.

dull, brittle solids or gases

a)

metals

b)

nonmetals

13.

right side of the periodic table

a)

metals

b)

nonmetals

14.

left side of the periodic table

a)

metals

b)

nonmetals

15.

tend to lose electrons

a)

metals

b)

nonmetals

16.

tend to gain electrons

a)

metals

b)

nonmetals

17.

tend to form anions

a)

metals

b)

nonmetals

18.

tend to form cations

a)

metals

b)

nonmetals

19.

tend to undergo oxidation

a)

metals

b)

nonmetals

20.

tend to undergo reduction

a)

metals

b)

nonmetals

21.

Barium, Ba is an example of a

a)

Alkali metal

b)

Alkaline earth metal

c)

Halogen

d)

Noble gas

e)

Transition metal

22.

Chromium, Cr is an example of a

a)

Alkali metal

b)

Alkaline earth metal

c)

Halogen

d)

Noble gas

e)

Transition metal

23.

Iodine, I is an example of a

a)

Alkali metal

b)

Alkaline earth metal

c)

Halogen

d)

Noble gas

e)

Transition metal

24.

Rubidium, Rb is an example of a

a)

Alkali metal

b)

Alkaline earth metal

c)

Halogen

d)

Noble gas

e)

Transition metal

25.

This chemical family of elements tends to form more than one ion and tends to form colored compounds.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

26.

This chemical family of elements are colorful diatomic elements.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

27.

This chemical family of elements is the most reactive nonmetal group.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

28.

This chemical family of elements is the most reactive metal group.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

29.

This chemical family of elements is very reactive and forms ions with a +2 charge.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

30.

This chemical family of elements is very reactive and forms ionic compounds that are always soluble in water.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

31.

This chemical family of elements is inert or nonreactive.

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

32.

Which element would most likely have the same bonding characteristics as sodium, Na?

a)

Li

b)

Ba

c)

O

d)

F

e)

Ar

33.

Which element would most likely have chemical properties that are very similar to the chemical properties of magnesium, Mg?

a)

Li

b)

Ba

c)

O

d)

F

e)

Ar

34.

Chlorine, Cl and Iodine, I are known disinfectants used to kill bacteria, which of the following would most likely also have the same disinfectant properties?

a)

Li

b)

Ba

c)

O

d)

Br

e)

Ar

35.

Which chemical family typically uses Roman numerals to indicate the charge of the ion?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

e)

Transition metals

36.

How many valance electrons does helium, He have?

a)

1

b)

2

c)

3

d)

4

e)

5

37.

How many valance electrons does oxygen, O have?

a)

3

b)

4

c)

5

d)

6

e)

7

38.

What charge do ions of oxygen, O have?

a)

+1

b)

+2

c)

+3

d)

-2

e)

-1

39.

What charge do ions of chlorine, Cl have?

a)

+1

b)

+2

c)

+3

d)

-2

e)

-1

40.

What charge do ions of aluminum, Al have?

a)

+1

b)

+2

c)

+3

d)

-2

e)

-1

41.

This chemical family of elements tends to be very radioactive.

a)

Alkali metals

b)

Lanthanides

c)

Halogens

d)

Actinides

e)

Transition metals

42.

What charge do ions of potassium, K have?

a)

+1

b)

+2

c)

+3

d)

-2

e)

-1

43.

What charge do ions of calcium, Ca have?

a)

+1

b)

+2

c)

+3

d)

-2

e)

-1

44.

What is another name for the elements in group 7A/17?

a)

Alkaline Earth Metals

b)

Noble gases

c)

Transition Metals

d)

Alkali Metals

e)

Halogens

45.

What is another name for the elements in group 8A/18?

a)

Alkaline Earth Metals

b)

Noble gases

c)

Transition Metals

d)

Alkali Metals

e)

Halogens

46.

Who is credited with the discovery of the periodic table?

a)

Mendeleev

b)

Moseley

c)

Seaborg

d)

Bohr

e)

Nelands

47.

Who is credited with the discovery of the periodic law?

a)

Mendeleev

b)

Moseley

c)

Seaborg

d)

Bohr

e)

Nelands

48.

Who is credited with modifying the periodic law so that it uses the atomic number of the elements?

a)

Mendeleev

b)

Moseley

c)

Seaborg

d)

Bohr

e)

Nelands

49.

Who is credited with modifying the periodic table so that it is in order by atomic number?

a)

Mendeleev

b)

Moseley

c)

Seaborg

d)

Bohr

e)

Nelands

50.

Whose periodic table was in order by atomic mass?

a)

Mendeleev

b)

Moseley

c)

Seaborg

d)

Bohr

e)

Nelands

51.

Base on the trend, which has the greater electronegativity,

Cl or Al?

a)

Cl

b)

Al

52.

Base on the trend, which has the greater electronegativity,

N or C?

a)

C

b)

N

53.

Based on the trend, which has the greater electronegativity,

H or F?

a)

H

b)

F

54.

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

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

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.
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)
57.
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
58.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
59.
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
60.

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

61.
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.
62.
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. 
63.
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
64.
Metals are good conductors of heat and electricity.
a)
true
b)
false
65.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
66.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
67.
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.
68.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
69.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
70.
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
71.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
72.

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

73.
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 
74.
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
75.

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

76.

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

a)

14

b)

4

c)

10

d)

7

77.

What is the effective nuclear charge for sodium?

a)

1

b)

11

c)

10

d)

2

78.

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

79.

Which of the following is smallest?

a)

Na+

b)

K+

c)

Rb+

d)

Fr+

80.

Which of the following is smallest?

a)

Na+

b)

Mg2+

c)

Al3+

81.

Which of the following is smallest?

a)

Cl-

b)

S2−

c)

P3−

82.

Which of the following is smaller?

a)

the anion (negative ion)

b)

parent atom

83.

Which of the following is smaller?

a)

the cation (positive ion)

b)

parent atom

84.

Which of the following is smaller?

a)

Sr2+

b)

Sr

85.

Which of the following is smaller?

a)

O

b)

O2−

86.

Why are cations smaller than their parent atoms?

a)

when cations form they lose their outer shell thus making them smaller

b)

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

87.

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.

88.

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)

89.

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

90.

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

91.

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

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

92.

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

a)

ionic radii

b)

atomic radii

c)

electronegativity

d)

ionization energy

93.

Who discovered a way to determine the number of protons in an atom of each element?

a)

Mendeleev

b)

Moseley

c)

Seaborg

d)

Bohr

e)

Nelands

94.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

95.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
96.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
97.

In a Lewis structure (electron dot structure) the dots represent

a)

all the electrons in the atom

b)

the valence electrons

c)

the number of protons in the nucleus

d)

the number of protons and neutrons in the nucleus

e)

the inner shell electrons

98.

Elements in main group 1A have _____ valence electron(s).

a)

1

b)

2

c)

3

d)

4

e)

5

99.

Elements in main group 2A have _____ valence electron(s).

a)

1

b)

2

c)

3

d)

4

e)

5

100.

Elements in main group 3A have _____ valence electron(s).

a)

1

b)

2

c)

3

d)

4

e)

5

101.

Elements in main group 4A have _____ valence electron(s).

a)

6

b)

2

c)

3

d)

4

e)

5

102.

Elements in main group 5A have _____ valence electron(s).

a)

6

b)

2

c)

3

d)

4

e)

5

103.

Elements in main group 6A have _____ valence electron(s).

a)

6

b)

2

c)

3

d)

4

e)

5

104.

Elements in main group 7A have _____ valence electron(s).

a)

6

b)

2

c)

7

d)

8

e)

5

105.

Most Elements in main group 8A have _____ valence electron(s) but He has ______ valence electrons. (Select both answers.)

a)

6

b)

2

c)

7

d)

8

e)

5

106.

Elements in main group 1 tend to form ions with a ______ charge.

a)

+1

b)

-1

c)

+2

d)

-2

e)

+3

107.

Elements in main group 2 tend to form ions with a ______ charge.

a)

+1

b)

-1

c)

+2

d)

-2

e)

+3

108.

Elements in main group 13 tend to form ions with a ______ charge.

a)

+1

b)

-1

c)

+2

d)

-2

e)

+3

109.

Elements in main group 17 tend to form ions with a ______ charge.

a)

+1

b)

-1

c)

+2

d)

-2

e)

+3

110.

Elements in main group 16 tend to form ions with a ______ charge.

a)

+1

b)

-1

c)

+2

d)

-2

e)

+3

111.

Elements in main group 15 tend to form ions with a ______ charge.

a)

+1

b)

-1

c)

+2

d)

-2

e)

-3

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