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Test Review Atomic Theory 25-26

Total questions: 83

Worksheet time: 1hrs 23mins

Name
Class
Date
1.

Which scientist discovered the electron?

a)

Bohr

b)

Thomson

c)

Rutherford

d)

Dalton

2.

Whose model of the atom is pictured?

a)

Rutherford

b)

Thomson

c)

Dalton

d)

Bohr

3.

What did Rutheford discover about atoms?

a)

An atom is mostly empty space, but has a dense positively charged center (nucleus)

b)

An atom is always negatively charged

c)

An atom is always positively charged

d)

All particles will pass straight through gold foil with no change in path

4.

Whose atomic model is shown?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

5.

What 2 particles would you find in the nucleus of an atom?

a)

Protons and Electrons

b)

Protons and Neutrons

c)

Electrons and Neutrons

d)

Neutrons and Electrons

6.

What particle has no charge?

a)

Nucleus

b)

Proton

c)

Electron

d)

Neutron

7.

Who came up with the first atomic theory?

a)

Thomson

b)

Rutherford

c)

Dalton

d)

Schrodinger

8.

All of Dalton's theories are correct EXCEPT -

a)

All atoms of the same element are identical

b)

All matter is made of atoms

c)

Compounds contain different atoms

d)

Atoms of different atoms can combine in whole number ratios

9.

Rutherford did experiments to show -

a)

Neutrons are located in the nucleus

b)

Atoms are mostly empty space

c)

Atoms contain negative particles, now known as electrons

d)

Matter cannot be lost or gained

10.

The scientist credited for discovering the nucleus is -

a)

Dalton

b)

Chadwick

c)

Bohr

d)

Rutherford

11.

What did Bohr's atomic model look like?

a)

A ring with gold foil in the middle

b)

Electrons orbiting the nucleus like the planets around the sun

c)

A scoop of chocolate chip ice cream. It had electrons scattered within a ball of positive charge

d)

A cloud of electrons floating around the nucleus

12.

Who first came up with the idea of an atom, calling it "atomos" which means indivisible?

a)

Dalton

b)

Chadwick

c)

Democritus

d)

Thomson

13.

Which 2 subatomic particles have a mass?

a)

Protons and Neutrons

b)

Protons and Electrons

c)

Electrons and Neutrons

d)

Electrons and Quarks

14.

Which scientist used the Cathode Ray to discover the negatively charged particles in an atom?

a)

Bohr

b)

Rutherford

c)

Dalton

d)

Thomson

15.

Which answer lists the scientist in chronological order according to their disoveries?

a)

Dalton, Democritus, Thomson, Rutherford, Bohr

b)

Thomson, Democritus, Dalton, Rutherford, Bohr

c)

Democritus, Dalton, Thomson, Rutherford, Bohr

d)

Bohr, Dalton, Democritus, Thomson, Rutherford

16.

For an atom to be electrically neutral, what 2 subatomic particles must be the same?

a)

Protons and Electrons

b)

Protons and Neutrons

c)

Electrons and Neutrons

d)

They can never be neutral

17.

How many neutrons does this isotope have?

a)

63

b)

29

c)

92

d)

34

18.

How many electrons does Uranium-235 have?

a)

235

b)

143

c)

92

d)

327

19.

Which part of an atom identifies the element?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Mass

20.

An element has an atomic number of 52 and has 78 neutrons. What is it's isotope notation?

(a)  

21.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
22.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
23.
An ______________ is the same element, with the same number of protons, but different numbers of neutrons
a)
Atom
b)
Isotope
c)
Atomic Number
d)
Mass Number
24.
The smallest particle into which an element can be divided and still be the same substance
a)
neutron
b)
atom
c)
electron
25.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
26.
Niels Bohr suggested that electrons.......
a)
are found in specific orbits
b)
electrons are scattered throughout the atom
c)
electrons move according to their energy level
d)
electrons are positive
27.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
28.
The three main subatomic particles are electrons, protons and ____________.
a)
photons
b)
neurons
c)
neutrons
d)
quarks
29.
What are the two main parts of the atom?
a)
nucleus and cytoplasm
b)
nucleus and electron cloud
c)
core and electron cloud
d)
protons and neutrons
30.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
31.

The total number of protons and neutrons in the nucleus of an atom is its

a)

atomic number

b)

Avogadro's number

c)

mass number

32.

The atomic mass of an element listed in the periodic table is the

a)

average atomic mass

b)

relative atomic mass of the most abundant isotope

c)

relative atomic mass of the most abundant radioactive isotope

d)

mass number of hte least abundant isotope

33.

An aluminum isotope consists of 13 protons, 13 electrons and 14 neutrons. Its mass number is

a)

13

b)

14

c)

27

d)

40

34.

A line spectrum is produced...

a)

when an electron goes from its ground state to its excited state

b)

when an electron moves from its excited state to its ground state

c)

when an electron moves into the nucleus

d)

when an electron moves to another position in the same sublevel

35.

If electrons in an atom have the lowest possible energies, the atom is in the

a)

ground state

b)

inert state

c)

excited state

d)

radiation - emitting state

36.

Atoms of the same element can differ in

a)

chemical properties

b)

mass number

c)

atomic number

d)

number of protons

37.

Three isotopes of argon occur in nature—36Ar, 38Ar, and 40Ar. Calculate the average atomic mass of argon to two decimal places, given the following relative atomic masses and abundances of each of the isotopes: argon-36 0.337%, argon-38 0.063%, and argon-40 99.600%

a)

54.37

b)

40.00

c)

39.99

d)

3998

38.
The first person to ever talk about an atom was
a)
Democritus
b)
Rutherford
c)
Dalton
39.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
40.
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. 
41.
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.
42.
Who came up with this model of an atom?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
43.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
44.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)
Proton
b)
Neutron
c)
Electron
d)
Orbitals
45.
His atomic model was depicted similar to a planetary/solar system
a)
Niels Bohr
b)
Joseph Thomson
c)
Ernest Rutherford
46.

Isotopes of the same element must have a different number of

a)

neutrons

b)

protons

c)

both neutrons and protons

47.

An atom of Chlorine-37 has

a)

37 protons, 37 neutrons and 37 electrons

b)

17 protons, 37 neutrons and 17 electrons

c)

17 protons, 20 neutrons and 37 electrons

d)

17 protons, 20 neutrons and 17 electrons

48.

How many neutrons does the isotope of Lithium have?

a)

8

b)

4

c)

3

d)

5

49.

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

50.

Two isotopes of carbon are carbon-12 and carbon-14. These isotopes differ from one another by two protons.

a)

true

b)

false

51.

Copper has two isotopes, Cu-63 and Cu-65. If the average atomic mass of copper is 63.5 g, what is the % of each isotope?

a)

50% Cu-63 and 50% Cu-65

b)

25% Cu-63 and 75% Cu-65

c)

75% Cu-63 and 25% Cu-65

52.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
53.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
54.

What is the atomic mass of the pictured isotope?

a)

17

b)

35

c)

18

55.
How many neutrons does a Sulfur-32 isotope have?
a)
15
b)
16
c)
32
d)
12
56.
What is the name of the pictured isotope?
a)
Chlorine-Schmorine
b)
Chlorine-17
c)
Chlorine-35
d)
Chlorine-18
57.

What is the name of the pictured isotope?

a)

Copper-29

b)

Copper-63

c)

Copper-34

58.

Nitrogen has two isotopes. One isotope has a mass of 14.003 amu and a relative abundance of 99.63%, while the other has a mass of 15.000 amu and a relative abundance of 0.37%. What is the average atomic mass for nitrogen?

a)

14.993 amu

b)

14.456 amu

c)

14.778 amu

d)

14.007 amu

59.

Calculate the atomic mass of silicon. The three silicon isotopes have atomic masses and relative abundances of 27.9 amu (92.2%), 28.9 amu (4.7%) and 29.9 amu (3.1%). Round your answer to 3 sig figs and only type a #.

(a)  

60.

Calculate the average atomic mass of the following element:

25Y (11%), 32Y (39%), 29Y (22%), 30Y (28%)

a)

32.0

b)

30.0

c)

29.0

61.

Calculate the average atomic mass of the following element:

25Y (11%), 32Y (39%), 29Y (22%), 30Y (28%)

a)

32.0

b)

30.0

c)

29.0

62.

What do all isotopes of hydrogen have in common?

a)

1 proton

b)

1 electron

c)

Mass of 1

d)

1 neutron

63.

What do the mass numbers on the periodic table represent?

a)

The mass of the most abundant isotope

b)

The mass of the least abundant isotope

c)

The average mass of the two most abundant isotopes

d)

The average mass of all the isotopes

64.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

excited state

d)

ground state

65.

With each higher energy level, the electrons are

a)

lower in energy

b)

more stable

c)

weaker

d)

farther from the nucleus

66.
A line spectrum is produced when an electron moves from one energy level
a)
into the nucleus.
b)
to another position in the same sublevel.
c)
to a higher energy level.
d)
to a lower energy level.
67.
Light is emitted when electrons ...
a)
jump from high to low 
b)
jump from low to high 
c)
either of these
d)
none of these
68.

How can scientists use the color spectrum of individual elements to help determine the composition of stars in our galaxy?

a)

Since each element has its own unique line spectra, it is possible to use a spectrometer to examine the light being emitted by the stars to determine what elements are present?

b)

Since each element does not have its own unique color spectrum, it is impossible to determine what elements make up our starts.

c)

Since the stars are so far away, the light we would be studying can not be trusted to determine their composition.

69.

The bright-line spectrum of an element in the gaseous phase is produced as

a)

protons move from lower energy states to higher energy states

b)

protons move from higher energy states to lower energy states

c)

electrons move from lower energy states to higher energy states

d)

electrons move from higher energy states to lower energy states

70.

The diagram represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of three of these elements. Which element is not present in the mixture?

a)

A

b)

D

c)

X

d)

Z

71.

Based on the bright-line spectra shown in the image, which two gases are present in the mixture?

Según los espectros de líneas brillantes que se muestran en la imagen, ¿qué dos gases están presentes en la mezcla?

a)

A and C

b)

B and D

c)

B and C

d)

A and D

72.

The unknown emission spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

73.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.

Using the bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”). Select all that apply

a)

Lithium

b)

Strontium

c)

Cadmium

74.

What gases are in the unknown mixture?

Select all that apply

a)

Gas A

b)

Gas B

c)

Gas C

d)

Gas D

75.

Which element(s) is/are found in the star's spectra below?

a)

Hydrogen only

b)

Hydrogen & Helium

c)

Calcium only

d)

Hydrogen & Calcium

76.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
77.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

78.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
79.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
80.

What happens when an electron absorbs a photon?

a)

The electron loses energy and moves to a lower energy level or orbital.

b)

The electron remains in the same energy level or orbital.

c)

The electron is destroyed and ceases to exist.

d)

The electron gains energy and moves to a higher energy level or orbital.

81.

What happens when an electron emits a photon?

a)

The electron transitions from a higher energy state to a lower energy state and emits a photon.

b)

The electron absorbs a photon and transitions to a higher energy state.

c)

The electron emits multiple photons simultaneously.

d)

The electron remains in the same energy state and emits a photon.

82.

According to Bohr, the energy absorbed by an electron upon excitation comes in a fixed amount called

a)

exact energy

b)

fixed energy

c)

quantized energy

d)

None of the above

83.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

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