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Atomic Theory and Periodicity Review

Total questions: 92

Worksheet time: 2hrs 20mins

Name
Class
Date
1.
This particle is found in the nucleus and has no charge
a)
Neutron
b)
Proton
c)
Electron
d)
Orbital
2.
This particle is found in the nucleus and has a positive charge
a)
Electron
b)
Proton
c)
Neutron
d)
Neutral
3.
This is a negatively charged particle found outside the nucleus
a)
Electron
b)
Proton
c)
Neutron
d)
Orbital
4.
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.
5.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively and positively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
6.
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. 
7.
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
8.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)
Proton
b)
Neutron
c)
Electron
d)
Orbitals
9.
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
10.
His atomic model was depicted similar to a planetary/solar system
a)
Bohr
b)
Thomson
c)
Rutherford
d)
Dalton
11.
Place the following scientists in order, from earliest to latest: 
A) Ernest Rutherford
B) J.J. Thomson
C) John Dalton
a)
B,C,A
b)
C,A,B
c)
A,C,B
d)
C,B,A
12.

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.

13.

John Dalton wrote postulates to make the idea of the atom useful. Which postulate below was proven wrong?

a)

All elements are made up of tiny indivisible particles called atoms.

b)

The atoms of one element are different from the atoms of another element.

c)

Atoms of different elements chemically combine to form chemical compounds.

d)

During chemical reactions, atoms are rearranged.

14.

What evidence did Rutherford use to support the idea that the atom was mostly empty space?

a)

the vast majority of the alpha particles went through the foil unaffected.

b)

the vast majority of the alpha particles were deflected at 90 degrees.

c)

one alpha particle was deflected by the gold foil.

d)

beams of alpha particles were deflected by magnets.

15.

What did Rutherford expect to happen to the alpha particles bombarding the gold foil?

a)

they would be absorbed by the gold.

b)

they would be deflected by the gold.

c)

they would go completely through the gold foil.

d)

the would be changed into beta radiation by the gold foil.

16.

Protium, Deuterium and Tritium are isotopes of the element Hydrogen.


Why does Tritium have a greater mass number than both Protium and Deuterium?

a)

It has more protons

b)

It has more neutrons

c)

It is electrically neutral

d)

It has more electrons

17.

What is the mass number of a nitrogen atom that has 8 neutrons?

a)

15

b)

14

c)

22

d)

8

18.

What is the mass number of an atom that contains 9 protons, 10 neutrons, and 9 electrons?

a)

9

b)

10

c)

18

d)

19

19.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
20.
How many neutrons does an Oxygen-19 isotope have?
a)
19
b)
8
c)
11
d)
10
21.
What is the name of the pictured isotope?
a)
Carbon-12
b)
Carbon-13
c)
Carbon-14
d)
Carbon-15
22.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
23.
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
24.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
25.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

26.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

27.

What are the elements (Be, Mg, Ca,...) in Group 2 called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble Gases

28.

Elements that have atoms with full valence shells in the ground state are in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

29.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
30.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
31.
How do positive ions form?
a)
by gaining electrons
b)
getting compliments
c)
by losing electrons
d)
gaining more protons
32.

Which of these is correct?

a)
b)
c)
33.

Which has the longest wavelength?

a)

Gamma Rays

b)

Visible Light

c)

Microwaves

d)

Radiowaves

34.

Which has the highest frequency?

a)

Gamma Rays

b)

Visible Light

c)

Microwaves

d)

Radiowaves

35.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
36.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
37.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
38.
Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy
a)
Radio waves
b)
Ultraviolet Rays
c)
Gamma Rays
d)
X-rays
39.

Which electromagnetic waves carry more energy?

a)

If it has a long wavelength

b)

If it has a short wavelength

c)

If it has a low frequency

d)

They all carry the same amount of energy

40.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.25x1023m

d)

2.25x1023 Hz

41.
Violet light has a wavelength of
4.10 x 10-12  m. What is the frequency?
a)
1.23 x 10^ -3 Hz
b)
7.31 x 10^ 19 Hz
c)
1.37 x 10^12 Hz
d)
3.0 x 10^ 8 Hz
42.

Red light has a wavelength of 675 x 10-9 m. What is its frequency?

a)

2.03x1011 m

b)

4.44x1014 Hz

c)

4.44x1014 nm

d)

2.03x1011 Hz

43.
What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 
a)
2.32 x 109 Hz
b)
3.60 x 1015 Hz
c)
1.58 x 10-51 Hz
d)
3 x 108  m/s
44.
What is the energy of an X-ray with a frequency of 1.0 x 1017 Hz?
a)
6.63 x 10-34 J
b)
6.63 x 10-17 J
c)
1.51 x 1016 J
d)
1.51 x 10-16 J
45.
What is the energy of light whose wavelength is 4.06 x 10-11 m? 
a)
2.69 x 10-44 J
b)
1.63 x 10-23 J
c)
4.90 x 10-15 J
d)
8.97 x 10-53 J
46.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

47.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

48.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

49.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

50.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

51.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
52.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

53.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

54.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

55.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
56.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
57.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
58.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
59.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
60.

Which has the smaller Electronegativity?

a)

Cl

b)

Al

61.

Which has the larger Electronegativity?

a)

Carbon

b)

Nitrogen

62.

Which of the following will have a larger radius than Gallium (Ga)?

a)

Ge

b)

Al

c)

Mg

d)

Sr

63.

Which of these has the smallest atomic radius?

a)

K

b)

Rb

c)

Fr

d)

Cs

64.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
65.

Which would be the easiest to take an electron from?

a)

He

b)

F

c)

Ba

d)

Fr

66.

As you move to the right across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have more neutrons

c)

the atoms have more protons.

d)

the atoms have more electrons.

67.

What is meant by isolectronic?

a)

Group of atoms or ions that have the same electronic configuration

b)

Group of atoms or ions that have the same protonic configuration

c)

Group of atoms or ions that have the same charges

d)

Group of atoms or ions that have different electronic configuration

68.

What is the example of species that are isolectronic species?

a)

Na+ and Mg2+

b)

Na+ and Na

c)

Na+ and Na2+

69.

Which species has the larger radius?

a)

Na

b)

Na+

70.

Which species has the larger radius?

a)

Cl

b)

Cl-

71.

Which is larger... P or P3- ? … and why?

a)

P3- because it gains an energy level

b)

P3- due to extra electron repulsion

c)

P because it loses an energy level

d)

P because of extra electron repulsion

72.

Na+ (Zeff=+9) and Al3+(Zeff=+11) are isoelectronic species (1s2 2s2 2p6). Which of these ion is smaller?

a)

Na+

b)

Al3+

c)

They have the same size

73.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
74.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
75.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
76.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
77.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
78.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
79.

Which block (s, p, d, or f) contains the non-metals?

a)

s block

b)

p block

c)

d block

d)

f block

e)

both d and f

80.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
81.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
82.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
83.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
84.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
85.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
86.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
87.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
88.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
89.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
90.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
91.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
92.
What is the formula to solve for the neutron?
a)
Mass + Atomic Number= Neutrons
b)
Mass x Atomic Number = Neutrons
c)
Mass - Atomic Number = Neutrons
d)
Mass + Number of Protons = Neutron

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