Free Printable Periodic Table Unit Review

1.

How are elements arranged in the periodic table?

a)

in alphabetical order

b)

in the order in which they were discovered

c)

in order of increasing atomic number

d)

in order of increasing melting points

2.

The vertical columns in the periodic table are known as:

a)

groups

b)

periods

c)

valences

d)

isotopes

3.

Group 18 of the periodic table contains nonreactive elements like helium, neon, and argon. The elements in this group are called:

a)

alkali metsls

b)

transition metals

c)

halogens

d)

noble gases

4.

Why is the periodic table so useful to scientists?

a)

it reminds them what the elements look like

b)

it can be used to predict how they react

c)

it lists the chemical formulas for all of the different compounds

d)

it contains the recipes for a variety of different kinds of mixtures

5.

Every element in the period table:

a)

combines easily with other elements

b)

is a solid at room temperature

c)

has atoms that are the same size

d)

has a unique set of properties

6.

The horizontal rows of the periodic table are known as:

a)

periods

b)

groups

c)

columns

d)

isotopes

7.

Use the periodic table to answer the question.
Out of all the lists below, which list contains the three elements that are most alike in their chemical properties?

a)

O, F, Ne

b)

Li, Mg, Sc

c)

Li, Na, K

d)

H, He, Li

8.

The atoms along the staircase are called

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

9.

Elements which are shiny, conduct electricity and heat are called

a)

metal

b)

nonmetal

c)

metalloid

d)

nonexistent

10.

In what section would Transition Metals be found?

a)

orange

b)

light blue

c)

blue

d)

white

11.

What period and group is Silver (Ag)?

a)

Period 2, Group 1

b)

Period 3, Group 16

c)

Period 5, Group 11

d)

Period 2, 14

12.

Fluorine, chlorine, bromine, iodine, and astatine make up Group 17, the halogens. Why are these elements grouped together?

a)

They all have the same atomic number.

b)

They are all nonreactive gases with similar physical properties.

c)

Their atoms all have eight electrons in their outer energy levels.

d)

They are all very reactive nonmetals with similar chemical properties.

13.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

14.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

15.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

16.

Which of the following statements is true about the 3s and the 4s sublevels?

a)

These sublevels have the same energy

b)

These sublevels are the same distance from the nucleus

c)

These sublevels hold different amounts of electrons

d)

These sublevels have the same shape

17.

Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

18.

Hund’s rule states…

a)

Atomic orbitals have opposite spins and 2 electrons each

b)

Electrons occupy orbitals of highest energy first and energy level changes as you go up

c)

Electrons occupy orbitals of lowest energy first, starting with 1s

d)

Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.

19.

What is the Pauli Exclusion Principle?

a)

An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins

b)

An atomic orbital can hold a minimum of 6 electrons, each with opposite spins

c)

An atomic orbital can hold a maximum of 6 electrons, each with the same spin

d)

An atomic orbital can hold a minimum of 2 electrons, each with opposite spins

20.

How many electrons can a d sublevel hold?

a)

14

b)

10

c)

2

d)

6

21.

The maximum number of electrons that can fit into the 2nd energy level is

a)

2

b)

8

c)

18

d)

32

22.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

23.

The electrons that are on the outer most region of the atom

a)

Shell Electrons

b)

Violent Electrons

c)

Valence Electrons

24.

The different energy levels of electrons as they orbit the nucleus

a)

Electron Cloud

b)

Orbitals (Energy Levels)

c)

2, 8, 18, 32

25.

Alkali metals are located where on the periodic table?

a)

Group 1

b)

Group 8 and Period 4

c)

Period 7

26.

Alkaline Earth Metals...

a)

are semiconductors

b)

are the most reactive type of elements

c)

have two valence electrons

27.

What atom matches this electron configuration?
1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

28.

What electron configuration matches an oxygen atom?

a)

1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶4s²3d¹

29.

The electron configuration of an atom is 1s²2s²2p⁶. The number of electrons in the atom is

a)

3

b)

6

c)

8

d)

10

30.

What do you start electron configuration with?

a)

1s²

b)

1d¹⁰

c)

1f¹⁴

d)

1p⁶

31.

There are 4 different types of subshells s,p,d,f

a)

true

b)

false

32.

Identify the Electron Configuration for Aluminum (Al)

a)

1s²2s²2p⁶3s²3p¹

b)

1s²2s²2p⁶3s²3p³

c)

1s²2s²2p⁶3s²4p¹

33.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

34.

How many valence electrons are represented here?

a)

7

b)

5

c)

2

d)

8

35.

How many p orbitals are there in a sublevel?

a)

2

b)

1

c)

4

d)

3

36.

Which element is pictured?

a)

neon

b)

fluorine

c)

magnesium

d)

argon

37.

Electron arrangement that uses arrows

a)

Electron configuration

b)

Shorthand configuration

c)

Lewis dot structure

d)

Orbital diagram

38.

This orbital diagram represents:

a)

C

b)

B

c)

N

d)

O

39.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up.

40.

Which orbital shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

41.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

42.

Which element is depicted from this orbital diagram

a)

Fluorine

b)

Neon

c)

Chlorine

d)

Argon

43.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

44.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

45.

Which element is depicted from this atomic orbital diagram?

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Phosphorus

46.

True or False: The reactivity of metals tends to decrease as you move from left to right across the periodic table.

a)

True

b)

False

47.

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

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

48.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

49.

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)

50.

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

51.

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 neutrons

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.

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

54.

The atom with the largest atomic radius in Group 18 is -

a)

Ar

b)

He

c)

Kr

d)

Rn

55.

Which of the following elements is a noble gas?

a)

Carbon

b)

Helium

c)

Oxygen

d)

Nitrogen

56.

What is the maximum number of electrons that can occupy a p sublevel?

a)

2

b)

6

c)

14

d)

10

57.

Which element has the electron configuration 1s²2s²2p⁶3s²3p⁵?

a)

Neon

b)

Chlorine

c)

Argon

d)

Fluorine

58.

What is the electron configuration for an atom with 12 electrons?

a)

1s² 2s² 2p⁶ 3s²

b)

1s² 2s² 2p⁶ 3p²

c)

1s² 2s² 2p⁶ 3s¹

d)

1s² 2s² 2p⁶ 3d²

59.

Which of the following is correct about calcium?

a)

group 6, period 3

b)

group 4, period 5

c)

group 2, period 4

d)

group 3, period 6

60.

This halogen is liquid at room temp.

a)

Ba

b)

Br

c)

Bh

d)

Bi

61.

Which of the following is correct about magnesium?

a)

group 6, period 3

b)

group 4, period 5

c)

group 2, period 3

d)

group 3, period 6

62.

This noble gas has 2 electrons.

a)

H

b)

Ne

c)

He

d)

Li

63.

This element is in group 14, carbon family, period 4.

a)

C

b)

Ge

c)

Sn

d)

Ga

64.

This element is in the halogen family, period 4

a)

Ba

b)

Br

c)

Bh

d)

Bi

65.

This noble element is a gas! It can be found in period 6.

a)

Rn

b)

Rh

c)

Re

d)

Ru

66.

This alkaline earth metal has 5 electron shells.

a)

Mg

b)

Y

c)

Sr

d)

Ba

67.

This noble element has three full valence shells.

a)

Li

b)

B

c)

Ar

d)

Ne

68.

Which of the following elements is classified as a metalloid?

a)

Iron (Fe)

b)

Aluminum (Al)

c)

Tellurium (Te)

d)

Carbon (C)

69.

Which of the following elements is classified as a Nonmetal?

a)

Fluorine (F)

b)

Magnesium (Mg)

c)

Aluminum (Al)

d)

Germanium (Ge)

70.

Which of the following elements is classified as a metal?

a)

Sodium (Na)

b)

Fluorine (F)

c)

Boron (B)

d)

Radon (Rn)

71.

Determine which group of the periodic table is being described in the following: Group 7A of the periodic table, which are highly reactive nonmetals, with fluorine being the most reactive of the group.

a)

Alkali Metals

b)

Oxygen Group

c)

Halogens

d)

Noble Gases

72.

Using the periodic table, which CLASS of elements does Silicon (Si) belong?

a)

Metals

b)

Nonmetals

c)

Metalloids

73.

Determine which of the following groups of the periodic table would be the MOST reactive group?

a)

Alkali Metals

b)

Alkali Earth Metals

c)

Boron Group

74.

Alkali Earth Metals have how many valence electrons?

a)

1

b)

2

c)

4

d)

8

75.

Group 1A elements are are called...

a)

Alkali Metals

b)

Alkali Earth Metals

c)

Halogens

d)

Noble Gases

76.

Elements in a group have similar properties because they have the same...

a)

Number of neutrons

b)

Number of elements

c)

Number of protons

d)

Number of valence electrons

77.

Across a period from left to right, elements become _____________ metallic and ___________nonmetallic in their properties.

a)

More....Less

b)

less....more

c)

Less....The same

78.

The atomic number tells you what?

a)

protons + neutrons

b)

number of protons

c)

number of neutrons

79.

Group 18 elements are known as the _____ _____ and have full valence shells.

a)

royal gases.

b)

supreme solids.

c)

noble gases.

d)

legit liquids.

80.

Which elements have the most similar chemical properties?

a)

K and Na

b)

K and Ca

c)

K and Cl

d)

K and S

81.

In what section would Transition Metals be found?

a)

orange

b)

light blue

c)

blue

d)

white

82.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

83.

What's a valence electron?

a)

electrons in the second energy level

b)

electrons in the outermost energy level

c)

the atomic number

d)

electrons in the first level

84.

How many valence electrons does N have?

a)

5

b)

6

c)

7

d)

8

85.

How many valence electrons does Al have?

a)

1

b)

2

c)

3

d)

4

86.

Which of the following is an example of a transition metal?

a)

Ca

b)

Cl

c)

C

d)

Cu

87.

Which of the following is an example of a nonmetal?

a)

Ca

b)

Cu

c)

Cl

d)

Cs

88.

Which element is least reactive?

a)

I (iodine)

b)

Br

c)

Cl

d)

F

89.

Which element is the most reactive?

a)

Be

b)

Ca

c)

Mg

d)

Ba

90.

Which element has the lowest ionization energy?

a)

Li

b)

B

c)

N

d)

F

91.

Which element is the most electronegative?

a)

Li

b)

B

c)

N

d)

F

92.

Which element is the smallest?

a)

Li

b)

B

c)

N

d)

F

93.

Which element is has the highest ionization energy?

a)

H

b)

Li

c)

Na

d)

K

94.

Which element is most electronegative?

a)

H

b)

Li

c)

Na

d)

K

95.

Which element is larger?

a)

H

b)

Li

c)

Na

d)

K

Periodic Table Unit Review

Total questions: 95

Worksheet time: 3hrs 10mins

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