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Atomic Theory and Moles

Total questions: 55

Worksheet time: 2hrs 35mins

Name
Class
Date
1.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
2.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
3.
He discovered the electron using cathode ray tube experiment.
a)
Joseph Thomson
b)
John Dalton
c)
Ernest Rutherford
d)
Robert Millikan
4.
How did each model of the atom help to develop the atomic theory? 
a)
Each model provided opinions that were added.
b)
Each model showed different properties of the same structure. 
c)
Each model showed new particles that had been discovered.
d)
Each model built upon the other to show new particles or properties of previously discovered particles. 
5.
This particle is found in the nucleus and has no charge
a)
Neutron
b)
Proton
c)
Electron
d)
Orbital
6.
This particle is found in the nucleus and has a positive charge
a)
Electron
b)
Proton
c)
Neutron
d)
Neutral
7.
This is a negatively charged particle found outside the nucleus
a)
Electron
b)
Proton
c)
Neutron
d)
Orbital
8.
The first person to propose a theory about an atom was
a)
Democritus
b)
Rutherford
c)
Dalton
d)
Aristotle
9.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom.  
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
10.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
11.
All matter is made of what?
a)
Energy 
b)
Atoms 
c)
Electrons 
d)
Compounds 
12.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
13.
James Chadwick discovered the ________.
a)
proton
b)
neutron
c)
electron
d)
nucleus
14.

He claimed that matter was made of small, hard particles that he called “atomos.”

a)

Democritis

b)

Dalton

c)

Moseley

d)

Einstein

15.

John Dalton stated:

a)

Atoms are tiny, invisible particles.

b)

Atoms of one element are all the same.

c)

Atoms of different elements are different.

d)

Compounds form by combining atoms.

e)

All of the statements listed.

16.
An atom's overall charge is ________.
a)
positive 
b)
depends
c)
neutral 
d)
negative 
17.
The weighted average of the masses of all naturally occurring isotopes of an element is
a)
Atomic number
b)
Atomic Mass
c)
Atomic weight
d)
Protons
18.
If two atoms have the same atomic number but different numbers of neutrons, they are
a)
Ions of that element
b)
Different elements
c)
Isotopes of the same atom
d)
Isotopes of different elements
19.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
20.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
21.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
22.

The atomic weight represents the weighted average of the

a)

electrons

b)

isotopes

c)

protons

23.

The Law of Conservation of Mass means that...

a)

The Mass of the reactants & products are equal.

b)

The Atoms of the reactants & products are equal.

c)

No mass or atoms is gained or lost during a chemical reaction.

d)

All the states are correct.

24.

states that, regardless of the amount, a compound is always composed of the same elements in the same proportion by mass

a)

law of definite proportions

b)

law of conservation of mass

c)

law of multiple proportions

d)

periodic table

25.

The percentage of copper and oxygen in samples of “CuO” obtained by different methods were found to be the same. This illustrates the law of:

a)

Definite proportions

b)

Conservation of mass

c)

Multiple proportions

d)

Reciprocal proportions

26.

What is the mass number of an atom?

a)

The mass number of an atom is the number of electrons in the nucleus of the atom.

b)

The mass number of an atom is the sum of the number of protons and neutrons in the nucleus of the atom.

c)

The mass number of an atom is the number of neutrons in the nucleus of the atom.

d)

The mass number of an atom is the sum of the number of electrons and protons in the nucleus of the atom.

27.

Which of the following pairs of compounds can serve to illustrate the Law of Multiple Proportions?

a)

CO and CaO

b)

CuS and CuSO4

c)

CH4 and C2H6

d)

PbO2 and P2O5

28.

Lavoisier found that when he reacted oxygen and hydrogen in a closed container, that the mass did not change. This result confirms the law of

a)

Definite Proportions

b)

Multiple Proportions

c)

Conservation of Matter

d)

Diminishing Returns

29.

If two or more compounds are composed of the same two elements, then the ratio of the masses of the second element that is combined with a certain mass of the first element is always a ratio of small whole numbers. This statement is called the law of

a)

definite proportions.

b)

conservation of mass.

c)

atomic theory.

d)

multiple proportions.

30.

Determined law of Conservation of Mass

a)

Democritus

b)

Goldstein

c)

Lavoisier

d)

Becquerel

31.

A molecule of carbon monoxide, CO, has one atom of oxygen while a molecule of carbon dioxide, CO2, has two. In a sample of CO containing 1 g of carbon, 1.33 g of oxygen will combine with the carbon to form the molecule. What is the mass of oxygen in a sample of CO2 containing 1 g of carbon?

a)

1.33 g

b)

3.0 g

c)

2.66 g

d)

0.0 g

32.

In an experiment, Alex and Rachel discover that their sample of table salt, also known as sodium chloride, NaCl, consists of 39.34% by mass sodium, Na, and 60.66 % by mass chlorine, Cl. Later, Alex wonders what the percentage of Na might be in the table salt in his saltshaker at home. Rachel tells him, correctly, that it is

a)

39.34%

b)

60.66%

c)

90%

d)

impossible to tell without analyzing the salt.

33.

An atom of potassium has 19 protons and 20 neutrons. Its mass number is

a)

9

b)

19

c)

20

d)

39

34.

Which of the following is not equal to 1.00 mol of carbon-12?

a)

6.022×10236.022\times10^{23} carbon atoms

b)

12.0 g of carbon

c)

6.0 g of carbon

d)

6.022×10236.022\times10^{23}  & 6.0 g of carbon

35.

The molar mass of an element is numerically equal to

a)

The element’s average atomic mass.

b)

The element’s average atomic number.

c)

The number of electrons possessed by an element.

d)

The percentage composition of the element by mass.

36.

To calculate the number of atoms present in 2.0 mol of an element, you would

a)

Add Avogadro’s number of atoms per mole to 2.0 mole.

b)

Subtract Avogadro’s number of atoms per mole from 2.0 mole.

c)

Multiply Avogadro’s number of atoms per mole by 2.0 mole.

d)

Divide Avogadro’s number of atoms per mole by 2.0 mole.

37.

The units of molar mass are

a)

g/mol

b)

mol/g

c)

amu/mol

d)

amu/g

38.

The molecular mass of CO2 is 44.01 u. What is the mass of 2.0 mol of CO2?

a)

44.01 mol

b)

44.01 g

c)

88.02 mol

d)

88.02 g

39.

How many moles of sodium hydroxide, NaOH, are in a 35.65 g sample of NaOH? (The molar mass of NaOH is 40.01 g/mol.)

a)

0.8910 mol

b)

1.122 mol

c)

1426 mol

d)

5.366×10235.366\times10^{23} mol

40.
What is the atomic mass of the pictured isotope?
a)
2
b)
4
c)
6
d)
Hehehehe
41.
A carbon isotope consists of 6 protons, 6 electrons and 8 neutrons.  What is the mass number for this isotope?
a)
12
b)
14
c)
6
d)
8
42.

What particles are found in an oxygen-18 nucleus?

a)

9 protons, 9 neutrons

b)

10 protons, 8 neutrons

c)

8 protons, 10 neutrons

d)

18 protons, 18 neutrons

43.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
44.

Calculate the average atomic mass of the element iron (Fe) using the following data:

[Isotope / % abundance]

[Iron 54 / 6% ] [Iron 56 / 92% ] [ Iron 57 / 2% ]

a)

53.7 amu

b)

54.9 amu

c)

5592.0 amu

d)

55.9 amu

45.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
46.

A mole of any substance is how many particles?

a)

6.02 x 1023

b)

6.02 x 10-23

c)

602 million

d)

602

47.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
48.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
49.

How many molecules would be in 8.4 moles of Octane (C8H18)?

a)

5.77 x 1023

b)

5.04 x 1024

c)

5.77 x 1026

d)

5.04 x 1023

50.

How many molecules are in 32.4 grams of phosphorous pentoxide P2O5?

a)

1.37 x 1023 molecules

b)
0.29 moles
c)

1.73 x 1022 molecules

d)
0.29 molecules
51.
How many molecules are present in 25 g of NaBr?
a)
102.96 molecules
b)
0.24 molecules
c)
1.45x1023 molecules
d)
2.34 x 1020molecules
52.
What is the mass of 54.3x1045molecules of BeO?
a)
3.27x1070 g
b)
9.01 x1022g
c)
2.25 x1024 g
d)
1.31 x1069g
53.
How many moles are in 4.5x1024 particles?
a)

7.47 particles

b)

7.47mol

c)
2.71x1047 mol
d)
2.71x1047 particles
54.
How many grams is 1.2 moles of Neon?
a)
0.05 grams
b)
16.6 grams
c)
21.2 grams
d)
24 grams
55.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol

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