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Atoms, Moles, & The Periodic Table

Total questions: 53

Worksheet time: 1hrs 26mins

Name
Class
Date
1.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

2.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

3.

Shivani measures out 6.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

340 g

4.

How many grams are in 1.2 moles of neon?

a)

0.059 grams

b)

7.2 x 1023 grams

c)

2.0 x 10-24 grams

d)

24 grams

5.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
6.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
7.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of neutrons in the nucleus

c)

the number of protons and neutrons in the nucleus

d)

the number of protons in the energy levels

8.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of neutrons in the nucleus

c)

the number of protons and neutrons in the nucleus

d)

the number of protons and electrons in the atom

9.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

10.

How is the number of neutrons in the nucleus of an atom calculated?

a)

Add the number of e- and p+ together

b)

Subtract the number of p+ from the mass number

c)

Subtract the number of e- from p+

d)

Add the mass number to the number of e-

11.

What subatomic particles would you find in the nucleus of an atom?

a)

Protons only

b)

Neutrons and Electrons

c)

Protons and Neutrons

d)

Protons and Electrons

12.

If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?

a)

12 neutrons

b)

12 protons

c)

12 electrons

d)

24 protons and neutrons

13.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

10

b)

20

c)

25

d)

35

14.

Which of the following determines the identity of an element?

a)

number of protons

b)

number of neutrons

c)

atomic mass

d)

number of shells

15.

Elements which are shiny, conduct electricity and heat are called

a)

metal

b)

metalloid

c)

nonmetal

d)

nonexistent

16.

Atoms with similar properties are most likely located...

a)

in the same period.

b)

in different periods.

c)

in the same group.

d)

to the right and left of each other.

17.

Which elements have the most similar chemical properties?

(use your periodic table)

a)

K and Na

b)

K and Cl

c)

K and Ca

d)

K and S

18.

How are elements ordered on the Periodic Table?

a)

Alphabetical Order

b)

By their atomic mass.

c)

By their color.

d)

By their atomic number.

19.

Rows on the period table are called _____ while columns are called _____.

a)

groups, families

b)

periods, groups

c)

groups, periods

d)

families, groups

20.

Used empirical evidence to develop atomic theory...

a)

Dalton

b)

Rutherford

c)

Bohr

d)

Thomson

21.

Which statement is true.

a)

Atoms are a theory

b)

Atoms are a law

22.

This scientists thought that we cold predict the location of electrons in electron energy levels/shells...

a)

Schrodinger / Heisenberg

b)

Bohr

c)

Rutherford

d)

Dalton

23.

Who conducted the "Gold Foil" experiment?

a)

Rutherford

b)

Bohr

c)

Dalton

d)

Thomson

24.

Who discovered the electron?

a)

Rutherford

b)

Bohr

c)

Dalton

d)

Thomson

25.
Which scientist developed the atomic theory?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
James Chadwick
26.
Who discovered the proton?
a)
Thomson
b)
Dalton
c)
Bohr
d)
Rutherford
27.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
28.
James Chadwick discovered the ________.
a)
proton
b)
neutron
c)
electron
d)
nucleus
29.
This scientist believed that electrons orbit the nucleus.
a)
Dalton
b)
Bohr
c)
Rutherford
d)
Chadwick
30.
The Gold Foil experiment was done by __________.
a)
Chadwick
b)
Bohr
c)
Rutherford
d)
Thomson
31.
Where are the most nonmetals located on the periodic table?
a)
In the bottom row
b)
On the left side and in the middle
c)
On the right side
d)
In the top row
32.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
33.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

34.

Match the following

a)

lithium

1.

2 energy levels

b)

helium

2.

1 energy level

c)

aluminum

3.

3 energy levels

d)

bromine

4.

4 energy levels

e)

strontium

5.

5 energy levels

35.

The metals tend to _____________ electrons and become positive ions.

a)

lose

b)

gain

36.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
37.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
38.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
39.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
40.

Magnesium(Mg) is in Group 2A on the periodic Table, it becomes an ion after ...................

a)

it loses 2 electrons

b)

it gains 2 electrons

41.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

42.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
43.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
44.
If an atom loses two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
45.
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.
46.

Covalent bonds are formed when_____________.

a)

electrons are transferred

b)

electrons are shared

c)

electrons vanish

d)

protons absorb electrons

47.
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.
48.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
49.

What type of bond is the strongest?

a)

single

b)

Double

c)

James

d)

triple

50.

Which of the following is a pure substance that contains two or more elements? (Sodium chloride is an example of this.)

a)

compound

b)

ion

c)

molecule

d)

solution

51.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

52.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

53.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

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