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Atoms & Periodic Table

Total questions: 146

Worksheet time: 3hrs 41mins

Name
Class
Date
1.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
2.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
3.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

4.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

5.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
6.
Something that takes up space and has mass.
a)
volume
b)
matter
c)
mass
d)
density
7.

Thought that you would eventually end up with a particle that could not be cut

a)

Aristotles

b)

Democritus

8.

He did not believe that such a particle could make up all substances found in nature

a)

Aristotles

b)

Democritus

c)

Zeus

d)

John Dalton

9.

A greek philosopher who used the word atomos to describe these particles.

a)

Democratus

b)

Aristotles

c)

JJ Thompson

d)

John Delton

10.

Which is smaller

a)

a cell

b)

a vein

c)

an atom

11.

Who said matter is made up of atoms

a)

Dalton

b)

Aristotle

c)

Democratus

d)

Niels Bohr

12.

Atoms cannot be created, divided or destroyed

a)

Aristotles

b)

Dalton

c)

Democratus

d)

Rutherford

13.

All atoms of a certain item are identical

a)

Niels Bohr

b)

Rutherford

c)

Dalton

d)

Aristotle

14.

Every substance is made up atoms combined in certain ways

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

15.

Who developed the atomic theory

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

16.

Who developed the atomic theory

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

17.

He found particles within the atom that have a negative charge

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

18.

He found particles within the atom that have a negative charge

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

19.

Provided evidence that atoms are made up of even smaller particles

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

20.

Atoms have a nucleus

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

21.

Small dense center that has a positive charge and is surrounded by moving electrons

a)

atoms

b)

nucleus

c)

protons

22.

The positivity charged particles in the nucleus is called

a)

atoms

b)

nucleus

c)

protons

23.

Found out that the nucleus is made out of smaller particles

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

24.

His model helped scientist predict the chemical properties of elements

a)

Dalton

b)

Thompson

c)

Bohr

d)

Rutherford

25.
Who first proposed that everything in the world was made up of tiny particles?
a)
Aristotle
b)
Democritus
c)
Plato
d)
Socrates
26.
Which philosopher stated that matter was made of four elements: earth, wind, water and fire?
a)
Aristotle
b)
Democritus
c)
Plato
d)
Socrates
27.
The electron was discovered in 1897.  Who discovered it?
a)
Ernest Rutherford
b)
John Dalton
c)
J. J. Thomson
d)
Niels Bohr
28.
Whose model showed atoms as uniformly packed spheres of positive matter filled with negatively charged electrons?
a)
J. J. Thomson
b)
John Dalton
c)
Ernest Rutherford
d)
Niels Bohr
29.
Which scientist became known as "the father of the nuclear age"?
a)
J. J. Thomson
b)
John Dalton
c)
Ernest Rutherford
d)
Niels Bohr
30.
Who stipulated that electrons orbit the nucleus at fixed energies and distances?
a)
Albert Einstein
b)
Max Planck
c)
Ernest Rutherford
d)
Niels Bohr
31.

Modern atomic theory is based on the work of many scientists. It keeps _______ideas that atoms are the basic unit of matter and that the atoms of each element are unique.

a)

Dalton

b)

Bohr

c)

Hamilton

d)

Thompson

32.

Atoms are made of electrons and protons

a)

Bohr

b)

Thompson

c)

Rutherford

d)

Hamilton

33.

The nucleus contains uncharged particles called...

a)

electrons

b)

protons

c)

neutrons

d)

atoms

34.

What is the charge of a proton?

a)

positive

b)

negative

c)

neutral

35.

Where are the protons located?

a)

Electron Cloud

b)

Nucleus

36.

What is the charge of an electron?

a)

positive

b)

negative

c)

neutral

37.

What is the charge of a proton?

a)

positive

b)

negative

c)

neutral

38.

What is the charge of a neutron?

a)

positive

b)

negative

c)

neutral

39.

Where are the electrons located?

a)

Electron Cloud

b)

Nucleus

40.

Where are the neutrons located?

a)

Electron Cloud

b)

Nucleus

41.

How can you tell how many neutrons are in an atom?

a)

Atomic Number

b)

Atomic Mass

c)

Atomic Number - Atomic Mass

d)

Atomic Mass - Atomic Number

42.

Where is most of the mass of the atom located?

a)

Electron Cloud

b)

Nucleus

43.

How many neutrons in this atom?

Atomic number = 6

Atomic mass - 12

a)

12

b)

4

c)

6

d)

8

44.

How many protons in Phosphorus?

Atomic # = 15, Atomic Mass = 31

a)

31

b)

15

c)

16

d)

8

45.

How many electrons in one atom of Iron?

a)

56

b)

30

c)

26

d)

36

46.

How can you tell how many protons an atom has?

a)

Atomic number

b)

Atomic Mass

c)

Atomic Number - Atomic Mass

d)

Atomic Mass - Atomic Number

47.

What is the overall charge of an atom?

a)

positive

b)

negative

c)

neutral

d)

orange

48.

How many ELECTRONS in one atom of Lithium?

a)

3

b)

4

c)

7

d)

5

49.

What is the atomic mass of aluminum?

a)

13

b)

27

c)

26

d)

14

50.
Where is the proton located?
a)
In the very dense nucleus
b)
Floating around in the negative electron cloud
c)
the loose nucleus
d)
the positive electron cloud
51.
Which description about the proton is accurate?
a)
Positively charged particle with a mass less than 0 amu
b)
A neutrally charged particle with a mass less than 0 amu
c)
Positively charged particle with a mass of 1 amu
d)
A neutrally charge particle with a mass of 1 amu
52.
What is the charge of the neutron?
a)
Negative
b)
Positive
c)
electrical charge
d)
Neutral (no charge)
53.
What is the mass of a neutron?
a)
1 amu
b)
0 amu
c)
same as electron
d)
doesn't have any mass
54.

Atoms have as many neutrons as they have protons

a)

True

b)

False

55.
Describe an Electron Cloud?
a)
the mist outside of an atom
b)
home of the protons
c)
where electrons are located
d)
nucleus
56.

Why is an object, like a table, solid?

a)

The atoms are touching

b)

The nuclei are so close

c)

There are so many atoms

d)

The electrons are moving so fast they are everywhere at once.

57.

It takes more than 1,800 electrons to equal the mass of one proton

a)

False

b)

True

58.

The charge of a single electron is represented as 1

a)

True

b)

False

59.

Fill in the blanks

a)

Proton-nucleus

b)

Electron cloud

c)

Almost 0 u

d)

Neutral = 0

60.

Which of these statements is INCORRECT?

a)

The number of protons determines the atomic number.

b)

The atomic number and number of protons are the same.

c)

An atomic number of 5 means there are 5 protons.

d)

The number of neutrons is always the same as the number of protons.

61.

An element with 3 protons in each atom has an atomic number of:

a)

1

b)

2

c)

3

d)

4

62.

Which of these statements is INCORRECT?

a)

The number of protons determines the atomic number.

b)

The atomic number and number of protons are the same.

c)

An atomic number of 5 means there are 5 protons.

d)

The number of neutrons is always the same as the number of protons.

63.

Which of these statements is CORRECT?

a)

The number of protons determines the nucleus.

b)

Atoms may not always have the same number of neutrons.

c)

An atomic number of 8 means there are 5 protons.

d)

The atoms of a certain element always have the same number of protons.

64.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

65.
Isotopes are atoms of the same element that have the same number of __________ but different number of __________ . Therefore, isotopes of the same element have different masses. 
a)
protons, neutrons
b)
protons, electrons
c)
neutrons, protons
d)
electrons, protons
66.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
67.

Who made the first periodic table?

a)

Dimitri Mendelev

b)

Dmitri Mendeleev

c)

Dmitri Mendelev

d)

Dimirti Mendeleev

68.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
69.
Who arranged the first periodic table.
a)
Mosely
b)
Einstein
c)
Mendeleev
d)
Bohr
70.
Mendeleev classified elements based on not only atomic mass but what else?                                                   
a)
reactivity
b)
boiling points
c)
physical properties only 
d)
 chemical & physical properties
71.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
72.
Which statement is not a difference between Mendeleev's table and the modern periodic table?
a)
there are no transition elements Mendeleev's table.
b)
Elements are arranged according to atomic no. not atomic mass.
c)
no gaps in the modern periodic table.
d)
much more than 60 elements in the modern periodic table.
73.
Which statement is not a difference between Mendeleev's table and the modern periodic table?
a)
there are no transition elements Mendeleev's table.
b)
Elements are arranged according to atomic no. not atomic mass.
c)
no gaps in the modern periodic table.
d)
much more than 60 elements in the modern periodic table.
74.

Rows on the periodic table are called ___________.

a)

Periods

b)

Sentences

c)

Fences

75.

The columns in the periodic table are called ___________.

a)

Towers

b)

Herds

c)

Groups

76.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
77.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
78.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
79.
The sum of the protons and neutrons in the nucleus of an atom
a)
Atomic Number
b)
Compound
c)
Electrons
d)
Mass Number (also called Atomic Mass)
80.
What does an atom's period tell us?
a)
Number of protons
b)
Number of electrons
c)
Number of valence electrons
d)
Number of shells
81.

About 3⁄4 of the elements on the periodic table are ________.

a)

metalloids

b)

nonmetals

c)

metals

d)

gases

82.

Elements on the periodic table are arranged in rows and columns according to their _________.

a)

properties

b)

categories

c)

atomic number

d)

boiling point

83.

Elements with properties of metals and nonmetals are ___________.

a)

metalloids

b)

metals

c)

nonmetals

d)

gases

84.

Group 1 metals that react quickly with other elements are ___________.

a)

metals

b)

alkaline earth metals

c)

alkali metals

d)

nonmetals

85.

___________ are located on the left side of the periodic table.

a)

Nonmetals

b)

Gases

c)

Metals

d)

Metalloids

86.

_________ are located on the right side of the periodic table.

a)

Nonmetals

b)

Metals

c)

Metalloids

d)

Gases

87.

A one or two letter abbreviation for the element.

a)

nickname

b)

chemical symbol

c)

initial

d)

atomic symbol

88.

The 18 columns in the periodic table are called?

a)

rows

b)

periods

c)

categories

d)

groups

89.

Elements in the same group share similar:

a)

characteristics

b)

atomic numbers

c)

mass

d)

size

90.

Which group contains the most reactive nonmetals?

a)

lanthanides

b)

alkaline earth

c)

halogens

d)

noble gases

91.

Which group contains the least reactive nonmetals?

a)

actinides

b)

halogens

c)

alkali metals

d)

noble gases

92.

Which element is the simplest, containing only one proton and one electron?

a)

hydrogen

b)

oxygen

c)

aluminum

d)

zinc

93.

Atom size increases as you move them from left to right.

a)

True

b)

False

94.

Osmium has the highest known density, and it is located a the center of the table

a)

True

b)

False

95.

As you move from left to right within a period, the atomic number of each element increases by one.

a)

True

b)

False

96.
A ____________is the force that holds atoms together in a compound.
a)
Chemical Formula
b)
Chemical Reaction
c)
Chemical Bond
d)
Synthesis Reaction
97.

Atoms that are held together by a chemical bond

a)

atom

b)

ion

c)

molecule

98.

A chemical change does create or destroy atoms

a)

True

b)

False

99.

In order for atoms to be rearranged, chemical bonds have to be formed or broken

a)

True

b)

False

100.

Protons are involved in chemical bonding

a)

True

b)

False

101.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
102.

The outer most energy level is the energy level_______from the nucleus

a)

Closest

b)

Side to Side

c)

Furthest

103.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell of an atom

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

104.

Elements that are shiny and conduct heat and electricity well and are the most of the periodic table

a)

Metal

b)

Nonmetal

c)

Metalloid

105.

Are poor conductors of heat and electricity. The elements to the right of the zigzag line are _______.

a)

Metal

b)

Nonmetal

c)

Metalloid

106.

Are elements that have some properties of metals and some of nonmetals. They border the zigzag line on the periodic table (6 elements)

a)

Metal

b)

Nonmetal

c)

Metalloid

107.

An______is a charged particle that forms when an atom loses or gains an electron.

a)

metal

b)

proton

c)

ion

d)

atom

108.

A particle with a positive or negative charge. It forms when an atom gains or losses electrons from it's outer most energy level.

a)

Electron

b)

Ion

c)

Molecule

d)

Atom

109.

1808

a)

John Dalton

b)

JJ. Thompson

c)

Ernest Rutherford

d)

Niels Bohr

110.

1897

a)

John Dalton

b)

JJ. Thompson

c)

Ernest Rutherford

d)

Niels Bohr

111.

1909

a)

John Dalton

b)

JJ. Thompson

c)

Ernest Rutherford

d)

Niels Bohr

112.

1913

a)

John Dalton

b)

JJ. Thompson

c)

Ernest Rutherford

d)

Niels Bohr

113.
How are ionic bonds formed?
a)

Transfer of electrons from a metal to non metal

b)

Sharing of electrons from a metal to nonmetal

114.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
115.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
116.
When the number of electrons equals the number of protons the atom has what charge?
a)
sponge bob
b)
positive charge
c)
negative charge
d)
neutral charge
117.
What are ionic bonds?
a)
valence electrons transferred between atoms
b)
Inner most electrons transferred between atoms
118.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
119.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
120.
Same repel, opposites
a)
avoid
b)
attract
c)
push
d)
pull
121.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
122.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
123.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
124.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
125.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
126.
An electron has what kind of charge?
a)
no charge
b)
positive 
c)
negative
d)
it depends
127.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
128.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

129.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
130.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
131.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
132.

When ions bond, they form a repeating three-dimensional pattern called

a)

Brittleness

b)

Crystal Lattice Structure

c)

Electrical Conductivity

d)

Solubility in Water

133.

Solid ionic compound does not conduct electricity

a)

True

b)

False

134.

Melted ionic compounds can conduct electric current. (Electrical Conductivity)

a)

True

b)

False

135.

Properties ionic Compounds

a)

Crystal Lattice Structure

b)

Solubility in Water

c)

Electrical Conductivity

d)

Brittleness

e)

Fluffyness

136.
Is salt (NaCI) a compound or a element
a)
Compound
b)
element
137.

Name the type of bonding in which the electrons are shared.

a)

Ionic bonding

b)

Covalent bonding

c)

Metallic bonding

138.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
139.

Forms when atoms share one or more pairs of electrons.

a)

True

b)

False

140.

Molecules that contain atoms of more than one element are called

a)

covalent bond

b)

covalent compound

141.

Properties of covalent compounds

a)

Low Solubility in Water

b)

Low Melting and Boiling Points

c)

Poor Electrical Conductivity

d)

Brittlness

142.

Forms between metal atoms when their outermost energy level overlap

a)

Electrical Conductor

b)

Ionic Compound

c)

Ionic Bond

d)

Metallic Bond

143.

What is the basis of a metallic bond?

a)

the attraction of neutral metal atoms.

b)

the attraction between protons and neutrons.

c)

the attraction between positive metal ions and interlocking electrons.

d)

the attraction between positive metal ions and free moving electrons.

144.

What do electrons do in a metallic bond?

a)

They stay on the metal atom.

b)

They are transferred from atom to atom.

c)

They form a covalent bond with another atom.

d)

They float around freely.

145.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

146.

Properties of most metallic compounds

a)

Good Electrical Conductors

b)

Malleable and ductile

c)

Solubility in Water

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