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Atoms & Elements Unit Review

Total questions: 100

Worksheet time: 3hrs 1mins

Name
Class
Date
1.
John Dalton stated:
a)
elements are made of atoms
b)
atoms of a given element are identical
c)
atoms cannot be subdivided, created, nor destroyed
d)
all of the above
2.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
3.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
4.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
5.
Electron cloud is based on
a)
Quantum Mechanics
b)
Gold Foil Experiment
c)
Matter is made up of small particles called atoms
d)
Nuclear Theory
6.
James Chadwick discovered the ________.
a)
proton
b)
neutron
c)
electron
d)
nucleus
7.
What did Thomson discover?
a)
electron
b)
proton
c)
neutron
d)
electron cloud
8.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
9.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
10.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
11.
Atoms of the same element with a different number of neutrons
a)
Ion
b)
Gluons
c)
Isotope
d)
Quarks
12.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
13.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
14.
Proposed the Modern Electron Cloud Model of the atom
a)
Schrodinger & Heisenberg
b)
Dalton
c)
Chadwick
d)
Rutherford
15.
Believed that atoms of the same element are identical to each other
a)
Bohr
b)
Rutherford
c)
Dalton
d)
Thomson
16.
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
17.
The only element with no neutrons in its nucleus.
a)
Oxygen
b)
Helium 
c)
Hydrogen
d)
Lithium
18.

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

a)

1

b)

2

c)

3

d)

4

19.

An element with 12 protons in each atom has an atomic number of:

a)

12

b)

21

c)

2

d)

24

20.

True or false: If the number of protons changes in an atom, it becomes a different element.

a)

True

b)

False

21.

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.

22.

The mass # tells us the mass of the atom. Which two subatomic particles make up the mass of the atom?

a)

protons and electrons

b)

neutrons and electrons

c)

Kyrontrons and Kytrons

d)

protons and neutrons

23.

How many electrons can "live" on the first electron shell?

a)

2

b)

8

c)

16

d)

infinite

24.

How many electrons can "live" on the 2nd electron shell?

a)

2

b)

8

c)

16

d)

infinite

25.

What is the atomic mass of Neon?

a)

10

b)

20.18

c)

10.18

d)

20

26.
How many protons are in Beryllium?
a)
4
b)
9
c)
5
d)
2
27.
How many neutrons are in a Gold atom?
a)
79
b)
196
c)
118
d)
275
28.

Which value is most likely the number of protons for saturntonium?

a)

388

b)

219

c)

169

d)

171

29.

What information from the table could help the student identify the element?

a)

Protons

b)

Neutrons

c)

Atomic mass

d)

Valence electrons

30.

Which model represents the most reactive atom?

a)
b)
c)
d)
31.

What element contains 7 protons and 5 valence electrons?

a)

Boron

b)

Vanadium

c)

Nitrogen

d)

Lithium

32.

Where are valence electrons located on the model?

a)

Near the nucleus

b)

In the middle of the atom

c)

At the innermost level

d)

At the outermost level

33.

Based on the information, what is the identity of this atom?

a)

Fluorine (F)

b)

Cobalt (Co)

c)

Germanium (Ge)

d)

Nickel (Ni)

34.

Which student's claim about valence electrons in a sulfur atom is correct?

a)

Student 1

b)

Student 2

c)

Both Student 1 and Student 2

d)

Neither Student 1 nor Student 2

35.

Which statement best explains why protons are used to identify an element?

a)

Protons are the most easily identified subatomic particles

b)

Positive charges are more easily detected during an investigation than negative and neutral charges

c)

The number of protons is unique to each element and remains constant

d)

Protons alone cannot be used to identify an element. The number of electrons and neutrons must also be known.

36.

A group of students examines a Bohr model of an atom with 8 valence electrons. What conclusion can the students make about the chemical reactivity of the element?

a)

The element is extremely reactive because the outer energy level is full

b)

The element is nonreactive because the outer energy level is full

c)

The element is somewhat reactive because the outer energy level is full

d)

Additional information is necessary to determine reactivity

37.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
38.
A neutral atom of the isotope 2612Mg would consist of
a)
12 protons, 26 neutrons, 26 electrons
b)
26 protons, 12 neutrons, 26 electrons
c)
26 protons, 14 neutrons, 14 electrons
d)
12 protons, 14 neutrons, 12 electrons
39.

What is the mass number of the element shown?

a)

15

b)

7

c)

8

d)

0

40.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
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.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
43.
An element with 4.35% have a mass of 49.9461 amu, 83.79% have amass of 51.9405 amu, 9.50% have a mass of 52.9407 amu, and 2.36% have a mass of 53.9389amu.
a)
51.99 amu
b)
52.19 amu
c)
53.45 amu
d)
17.33 amu
44.
What is the name of the atom pictured here?
a)
Nitrogen
b)
Nitrogen-15
c)
Nitrogen-7
d)
Nitrogen-8
45.
Which of the following could have 82 neutrons?
a)
W-182
b)
Ta-181
c)
Cs-132
d)
Ba-138
46.
How many total electrons does O-2 (an oxide ion) have?
a)
8
b)
10
c)
6
d)
18
47.
How many total electrons does Mg+2 (a magnesium ion) have?
a)
10
b)
12
c)
14
d)
22
48.
Cations are
a)
positive
b)
negative
c)
on the right side of the periodic table.
d)
nonmetals
49.
Negative ions (anions) form when neutral atoms _________ valence electrons.
a)
lose
b)
gain
c)
share
50.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
51.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
52.
Will a neutral phosphorus atom gain or lose electrons to become stable?
a)
gain
b)
lose
c)
neither
53.
How many electrons will a neutral sulfur atom gain to become stable?
a)
2
b)
6
c)
8
d)
3
54.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
55.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
56.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
57.
Refer to the periodic table.  What element is in period 5 and has 7 valence electrons?
a)
Technetium (Tc)
b)
Iodine (I)
c)
Tin (Sn)
d)
Chlorine (Cl)
58.
How many total atoms does CaCO3 Have?
a)
3
b)
4
c)
5
d)
6
59.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
60.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
61.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
62.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
63.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
64.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
65.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
66.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
67.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
68.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
69.
a)
2
b)
3
c)
5
70.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
71.
Which element could be lustrous and brittle?
a)
A
b)
B
c)
G
d)
L
72.
Which elements are in the same period?
a)
A & F
b)
F, B & D
c)
E & D
d)
F & B
73.

To which group does this atom belong?

a)

1

b)

3

c)

13

d)

11

74.
Is this a metal, nonmetal or metalloid?
a)
Metal
b)
Nonmetal
c)
Metalloid
75.
Is silicon a metal, nonmetal or metalloid?
a)
Metal
b)
NonMetal
c)
Metalloid
76.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
77.

Calculate the molar mass of NH4NO2

a)

50 g/mol

b)

60 g/mol

c)

64 g/mol

d)

78 g/mol

78.

The lines in the emission spectrum for hydrogen are formed from ___.

a)

energy given off when the electron moves from higher energy levels to lower energy levels

b)

electrons given off as hydrogen burns

c)

protons given off when protons move from higher energy levels to lower energy levels

d)

electrons given off as hydrogen cools

79.

Which color has the longest waves?

a)

red

b)

orange

c)

yellow

d)

green

80.

Which color has the highest energy per photon quanta?

a)

green

b)

blue

c)

red

d)

yellow

81.

The portion of the electromagnetic spectrum that humans can see is called:

a)

radio waves

b)

visible light

c)

gamma rays

d)

x-rays

82.

the distance between peaks of electromagnetic waves is called:

a)

wavelength

b)

frequency

c)

energy

d)

Planck's Constant

83.

Which type of electromagnetic energy carries the least energy?

a)

X-Rays

b)

Visible Light

c)

Ultraviolet

d)

Microwaves

84.

The formula for the radiative energy (E) carried by a photon of light is:

a)

E = h x c

b)

E = c/λ

c)

E = h x f

d)

E = mMG/d

85.

What is the speed of light?

a)

it depends on the type of electromagnetic radiation

b)

3 x 108 m/s

c)

3 x 10-34 m/s

d)

500 km/s

86.

the LOWEST point in a transverse wave is called the...

a)

crest

b)

trough

c)

wavelength

d)

frequency

87.
What element has the following electron configuration? [Ar] 3d104s24p3
a)
As
b)
P
c)
Se
d)
Ga
88.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
89.
How many orbitals are in the f sublevel
a)
1
b)
3
c)
5
d)
7
90.
What is the correct electron configuration for Selenium
a)
1s22s22p63s23p64s24d104p4
b)
1s22s22p63s23p64s23d104p4
c)
1s22s22p63s23p64s23d104p3
d)
1s22s22p63s23p64s24d104p43
91.
C=𝝺𝝂 (speed of light = wavelength x frequency in meters)
a)
EM wave equation 
b)
Quantum equation 
c)
Energy of a photon 
92.
Which is a particle of electromagnetic radiation with no mass that carries a quantum of energy?
a)
electron 
b)
neutron 
c)
microwave
d)
photon 
93.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
94.
Bromine is found in which block?
a)
s
b)
p
c)
d
d)
f
95.

Light is:

a)

a star and a galaxy

b)

a wave and a particle

c)

sound and energy

d)

unable to be measured

96.
What happens when the electrons fall back to lower energy levels?
a)
They release protons and neutrons
b)
They lose energy in the form of light
c)
They gain energy bounce back
d)
They lose energy and go completely dark
97.
This is the _____ for helium.
a)
emission spectrum
b)
absorption spectrum
c)
continuous spectrum
d)
black body spectrum
98.

Who is this woman, known for her work on radioactivity and treatment for cancer?

a)

Jane Goodall

b)

Rosalind Franklin

c)

Marie Curie

d)

Mary Anning

99.
Which model is this?
a)
Planetary
b)
Plum Pudding
c)
Nuclear
d)
Quantum Mechanical
100.
What did Planck work on?
a)
quantum theory
b)
nuclear chemistry
c)
uncertainty principle
d)
wave theory

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