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Unit 4- The Periodic Table

Total questions: 106

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

Who created the Periodic Table?

a)

Albert Einstein

b)

Dmitri Mendeleev

c)

Isaac Newton

d)

Marie Curie

2.

What is the purpose of the Periodic Table?

a)

To list all known planets

b)

To arrange all known elements by trends and groups of similar characteristics

c)

To display all known animals

d)

To organize all known languages

3.

What does the number 43 represent in the element box for Technetium?

a)

Atomic Number

b)

Atomic Mass

c)

Element Name

d)

Symbol

4.

What is the symbol for the element Technetium?

a)

Tc

b)

Tm

c)

Te

d)

Th

5.

What is the atomic mass of Technetium as shown in the element box?

a)

98.907

b)

43.000

c)

99.000

d)

97.907

6.

Which part of the element box indicates the name of the element?

a)

Technetium

b)

Tc

c)

43

d)

98.907

7.

What does the Periodic Table organize elements by?

a)

Atomic mass

b)

Atomic number

c)

Element symbol

d)

Chemical properties

8.

What does the Atomic Mass represent in an element box?

a)

The number of protons

b)

The number of electrons

c)

The weighted average of all isotopes

d)

The chemical symbol

9.

What is the name of the first group in the periodic table?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Alkaline Earth Metals

10.

Which group in the periodic table contains the noble gases?

a)

Group 1

b)

Group 2

c)

Group 8

d)

Group 4

11.

Which element is located in Period 2 and Group 1 of the periodic table?

a)

Sodium

b)

Lithium

c)

Potassium

d)

Rubidium

12.

How many periods are there in the periodic table?

a)

5

b)

6

c)

7

d)

8

13.

Which element is found in Period 4 and Group 2?

a)

Calcium

b)

Magnesium

c)

Strontium

d)

Barium

14.

Which of the following is a family of elements in the periodic table?

a)

Noble Gases

b)

Noble Metals

c)

Rare Earth Elements

d)

Heavy Metals

15.

What is the family name for elements like sodium and potassium?

a)

Alkaline Earth Metals

b)

Transition Metals

c)

Alkali Metals

d)

Halogen Gases

16.

Which family of elements is known for being very unreactive?

a)

Halogen Gases

b)

Noble Gases

c)

Alkali Metals

d)

Transition Metals

17.

What are the columns in a Periodic Table called?

a)

Periods

b)

Groups

c)

Families

d)

Rows

18.

What are the rows in a Periodic Table called?

a)

Groups

b)

Families

c)

Periods

d)

Columns

19.

What term is used for elements that are grouped together by their similarities in chemical properties?

a)

Periods

b)

Groups

c)

Families

d)

Rows

20.

Which element is located in Period 3 and Group 16 of the periodic table?

a)

Tellurium

b)

Selenium

c)

Sulfur

d)

Oxygen

21.

What is the family name for elements like fluorine and chlorine?

a)

Halogens

b)

Alkali Metals

c)

Noble Gases

d)

Transition Metals

22.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

23.

In a neutrally charged atom, which two subatomic particles are equal in number?

a)

protons and neutrons

b)

all subatomic particles are equal in number

c)

neutrons and electrons

d)

protons and electrons

24.

Which subatomic particle is counted to determine the type of element the atom represents?

a)

proton

b)

neutron

c)

electron

d)

boron

25.

Particles in an atom that have no charge are 

a)

negatrons 

b)

electrons 

c)

neutrons 

d)

protons 

26.

How many neutrons are in an atom of "K"?

a)

29

b)

19

c)

58

d)

20

27.

Adding or subtracting neutrons from an atom means it is now a(n)...

a)

ion

b)

mixture

c)

isotope

d)

neutral atom

28.

Adding or subtracting electrons from an atom means it is now a(n)...

a)

ion

b)

mixture

c)

isotope

d)

neutral atom

29.

Can the mass number of an atom change?

a)

yes, if its number of protons changes

b)

yes, if its number of neutrons changes

c)

yes, if its number of electrons changes

d)

no, it always stays the same

30.

Select all that is true: We cannot change an atom's number of protons because...

a)

protons = atomic number and we can't change an element into another element

b)

changing the number of protons an atom has would mean it has changed into another element

c)

because protons have no mass

d)

we can change the number of neutrons, not protons

31.

Which subatomic particle contains "no" mass?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Atoms

32.

How many groups are in the North American Periodic Table (the one we study)?

a)

8

b)

18

c)

10

d)

20

33.

Select all that apply: The atomic mass on the Periodic Table...

a)

is a decimal

b)

is protons + neutrons of a specific atom

c)

is larger than the atomic number

d)

takes into account the abundance of each isotope of an element

34.

Atomic mass is a decimal because...

a)

It is the weighted average of all isotopes of an element

b)

Atomic mass is protons + neutrons, and there can be 0.5 of a neutron

c)

It needs to be rounded to find the number of neutrons

d)

Making it a fraction would be too hard

35.
What side of the periodic table are metals on?
a)
left
b)
right
c)
top
d)
bottom
36.
What side of the periodic table are nonmetals on?
a)
left
b)
right 
c)
top
d)
bottom
37.
Is oxygen metal or nonmetal?
a)
metal
b)
nonmetal
38.
All of these properties describe metals EXCEPT...
a)
malleable
b)
conductors
c)
brittle 
d)
luster
39.
How would this element be classified?
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Metamorphic
40.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
41.
Luster is ___________
a)
A.  the way light is reflected off a surface.
b)
A.  how well a piece of matter conducts electricity. 
c)
A.  the capability of being drawn out into thin wires or threads.
d)
A.  the capability of being hammered out thin.
42.

Elements that are mostly dull, brittle, not malleable or ductile, and poor conductors of heat and electricity are referred to as _______________.

a)

Metals

b)

Nonmetals

c)

Metalloids

43.

When a metal can allow heat or electricity to flow through it, we say it is ___________.

a)

lustrous

b)

malleable

c)

ductile

d)

conductive

44.
If you have a material that can conduct electricity well it is probably a...
a)
Metalloid
b)
Matter
c)
Non-metal
d)
Metal
45.
What physical properties are used to classify elements as metals, non-metals, or metalloids?
a)
Color, smell, physical state
b)
Reactivity, streak, hardness
c)
Ability to burn, mass, density
d)
Luster, conductivity, malleability
46.

Most metals are ....

a)

Cations

b)

Anions

47.

Most non-metals are...

a)

Anions

b)

Cations

48.

Metals normally form

a)

negative ions

b)

positive ions

49.

non metals normally form ...

a)

negative ions

b)

positive ions

50.

Metals like to

a)

give away electrons

b)

gain electrons

51.

non metals like to

a)

gain electrons

b)

give away electrons

52.

Group 2 elements form what type of ion charge?

a)

2+

b)

2-

c)

1+

d)

1-

53.

Group 7 elements form

a)

1- cations

b)

1- anions

c)

2- anions

d)

2+ cations

54.

How can you tell isotopes of the same element apart?

a)

By their color

b)

By their mass number

c)

By their chemical symbol

d)

By their atomic number

55.

What is an isotope?

a)

A different element with the same number of protons

b)

Versions of the same element with the same number of protons but a different number of neutrons

c)

Elements with the same number of neutrons and protons

d)

A molecule with a different number of electrons

56.

What does the number next to the isotope mean? (e.g., "Carbon-14")

a)

The number of electrons in the isotope

b)

The atomic number of the isotope

c)

The mass number of the isotope

d)

The number of protons in the isotope

57.

How can you tell isotopes of the same element apart?

a)

They have a different number of protons

b)

They have a different number of electrons

c)

They have a different number of neutrons

d)

They have a different atomic number

58.

Why is atomic mass considered to be the "weighted average"?

a)

A) It considers the most common isotope only.

b)

B) It averages the mass of all isotopes equally.

c)

C) It takes into account the abundance of each isotope.

d)

D) It is the sum of protons and neutrons.

59.

How is atomic mass calculated?

a)

Add the mass of each isotope.

b)

Multiply the mass of each isotope by its abundance, and add them together.

c)

Subtract the mass of each isotope from its abundance.

d)

Divide the mass of each isotope by its abundance.

60.

What is the difference between atomic mass and mass number?

a)

Atomic mass is the total number of protons and neutrons, while mass number is the average mass of all isotopes.

b)

Atomic mass is the average mass of all isotopes, while mass number is the total number of protons and neutrons.

c)

Atomic mass and mass number are the same.

d)

Atomic mass is the number of electrons, while mass number is the number of protons.

61.

What is the isotope notation for carbon with 8 neutrons?

a)

12C^{12}C or carbon-12

b)

14C^{14}C or carbon-14

c)

13C^{13}C or carbon-13

d)

15C^{15}C or carbon-15

62.

How many neutrons does a regular atom of carbon have?

a)

8

b)

7

c)

6

d)

5

63.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
64.

What does a Lewis-Dot Structure depict?

a)

The number of protons in an element

b)

The number of valence electrons in an element

c)

The atomic mass of an element

d)

The number of neutrons in an element

65.

What are valence electrons important for in an atom?

a)

Determining the color of the atom

b)

Determining how the atom might bond with other atoms

c)

Determining the size of the atom

d)

Determining the weight of the atom

66.

Where are valence electrons located?

a)

Innermost ring/energy level

b)

Outermost ring/enery level

c)

Inside the nucleus

67.

What does the group number of an element in the periodic table represent?

a)

The number of protons in the element

b)

The number of valence electrons in the element

c)

The atomic mass of the element

d)

The number of neutrons in the element

68.

How many valence electrons do elements in Group 1 have?

a)

1

b)

2

c)

8

d)

4

69.

Which group has elements with 8 valence electrons, except for Helium?

a)

Group 8

b)

Group 1

c)

Group 2

d)

Group 3

70.

What is unique about Helium's valence electrons compared to other elements in Group 8?

a)

It has 2 electrons

b)

It has 8 electrons

c)

It has 1 electron

d)

It has 4 electrons

71.

What do all elements in a group have in common regarding valence electrons?

a)

They have the same number of valence electrons

b)

They have different numbers of valence electrons

c)

They have no valence electrons

d)

They have twice the number of valence electrons

72.

What rule governs the behavior of atoms in bonding?

a)

The Duet Rule

b)

The Octet Rule

c)

The Triple Rule

d)

The Double Rule

73.

Why does Na bond with Cl to make NaCl?

a)

Because Na has 7 valence electrons and Cl has 1.

b)

Because Na has 1 valence electron and Cl has 7.

c)

Because both Na and Cl have 8 valence electrons.

d)

Because Na and Cl do not share electrons.

74.

Which group on the Periodic Table contains elements with a full valence shell, thus making them inert (unreactive)?

a)

Alkali Metals

b)

Halogens

c)

Noble Gases

d)

Transition Metals

75.

What do you draw along with the element symbol in a Lewis-Dot Structure?

a)

Atomic number

b)

Number of protons

c)

Correct number of valence electrons

d)

Number of neutrons

76.

How should you draw the valence electrons around the element symbol in a Lewis structure?

a)

Clockwise

b)

Randomly

c)

Counter-clockwise

d)

In a straight line

77.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

78.

What is an ion?

a)

An atom with a neutral charge

b)

An atom that has lost or gained electrons

c)

An atom with more protons than electrons

d)

An atom with more electrons than protons

79.

What happens to the charges in an ion?

a)

They cancel each other out

b)

They become neutral

c)

They do not cancel each other out

d)

They become positive

80.

What is a cation?

a)

An atom that has gained an electron and is negative in charge

b)

An atom that has lost an electron and is positive in charge

c)

An atom that has gained a proton and is positive in charge

d)

An atom that has lost a proton and is negative in charge

81.

What is an anion?

a)

An atom that has lost an electron and is positive in charge

b)

An atom that has gained an electron and is negative in charge

c)

An atom that has lost a proton and is positive in charge

d)

An atom that has gained a proton and is negative in charge

82.

How can you remember the charge of a cation?

a)

Cations are negative

b)

Cations are neutral

c)

Cations are PAWsitive

d)

Cations are negative and positive

83.

Are most elements on the Periodic Table metals or nonmetals?

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Gases

84.

How many electrons do atoms want in their valence shell to be stable?

a)

2

b)

4

c)

6

d)

8

85.

Atoms are compared to humans because they always want to take the path of:

a)

Most resistance

b)

Least resistance

c)

No resistance

d)

Maximum resistance

86.

What does an atom with 3 valence electrons prefer to do?

a)

Gain 5 more electrons

b)

Lose 3 electrons

c)

Gain 3 electrons

d)

Lose 5 electrons

87.

What is the first step in finding ion notation?

a)

Determine ionic charge

b)

Find out how many valence electrons your atom has

c)

Figure out the path of least resistance

d)

Look at the atomic mass

88.

What happens when an atom loses an electron?

a)

It becomes more negative

b)

It becomes more positive

c)

It stays the same

d)

It becomes neutral

89.

What is the purpose of figuring out the path of least resistance for an atom?

a)

To determine its atomic mass

b)

To find out if it should gain or lose electrons to achieve an octet

c)

To calculate its density

d)

To measure its temperature

90.

What must be considered regarding electrons when drawing Lewis-Dot Structures for ions?

a)

The number of protons

b)

Electrons that have been transferred (gained or lost)

c)

The atomic mass

d)

The number of neutrons

91.

Where should the ionic charge be placed in a Lewis-Dot Structure?

a)

Inside the brackets

b)

Next to the element symbol

c)

Outside the brackets

d)

Above the element symbol

92.

Why are ions formed?

a)

To make our lives difficult

b)

Because atoms want to be stable

c)

Because atoms have the same number of protons and electrons

d)

Because atoms gained neutrons

93.
Who was the first person to study atomic theory?
a)
Dalton
b)
Democritus
c)
Chadwick
d)
Miller
94.
What was the name of J.J Thomsons' model of atomic structure. 
a)
Electron Cloud Model 
b)
Electron Sea Model
c)
Plum Pudding Model 
d)
Bohr Model
95.
What does the Bohr model suggest?
a)
Atoms are small, hard, indivisible objects. 
b)
That protons in the nucleus are attracted to electrons in the electron clouds. 
c)
That electrons travel around the nucleus of an atom in orbits or definite paths.
96.

Which Scientist created this model?

a)

Democritus

b)

Chadwick

c)

Bohr

d)

Rutherford

97.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
98.

What experiment led Thomson to his discovery?

a)

gold foil experiment

b)

cathode ray tube experiment

c)

none, he had a thought experiment

d)

bombarding of alpha particles

99.

Which scientist used the gold foil experiment in his discovery?

a)

Bohr

b)

Thomson

c)

Rutherford

d)

Chadwick

100.

What model of the atom came about first.

a)
b)
c)
d)
e)
101.

The idea of atomos (uncuttable or indivisible bits of matter) was first stated by:

a)
Democritis
b)
Dalton
c)
Moseley
d)
Einstein
102.

Which scientist theorized, but incorrectly stated, that all atoms of an element were identical and were indivisible?

a)
Democritus
b)
Dalton
c)
Thomson
d)
Borh
103.

What atomic theory is considered the planetary model?

a)

Dalton

b)

Bohr

c)

J. J. Thomson

d)

Quantum model

104.

Who founded the electron?

a)

Thomson

b)

Rutherford

c)

Bohr

d)

Chadwick

105.

Who founded the proton?

a)

Thomson

b)

Rutherford

c)

Bohr

d)

Chadwick

106.

Who founded the neutron?

a)

Thomson

b)

Rutherford

c)

Bohr

d)

Chadwick

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