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CPET Quiz - 8-9

Total questions: 111

Worksheet time: 2hrs 5mins

Name
Class
Date
1.

Why can't we observe hydrogen atoms directly?

a)

They are too large

b)

They are too small

c)

They are too far away

d)

They are too bright

2.

Who proposed the idea that matter is discontinuous and atoms are indivisible?

a)

Plato

b)

Aristotle

c)

Democritus

d)

Socrates

3.

What are electrons?

a)

Positively charged particles

b)

Neutrally charged particles

c)

Negatively charged particles

d)

Particles with no charge

4.

What discovery showed that atoms are divisible?

a)

Discovery of protons

b)

Discovery of neutrons

c)

Discovery of electrons

d)

Discovery of photons

5.

Who discovered electrons?

a)

Albert Einstein

b)

Niels Bohr

c)

J.J. Thompson

d)

Ernest Rutherford

6.

Who discovered protons?

a)

Niels Bohr

b)

J.J. Thomson

c)

Ernest Rutherford

d)

Albert Einstein

7.

What surrounds the tiny, massive, positively charged nucleus according to Rutherford?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Photons

8.

How far do electrons circle from the nucleus according to Rutherford's model?

a)

10 times the radius of the nucleus

b)

1,000 times the radius of the nucleus

c)

10,000 times the radius of the nucleus

d)

100,000 times the radius of the nucleus

9.

Who is credited with the discovery of neutrons?

a)

Albert Einstein

b)

Niels Bohr

c)

James Chadwick

d)

Ernest Rutherford

10.

According to Planck, how does matter emit and absorb energy?

a)

In continuous waves

b)

In discrete units called quanta

c)

In random bursts

d)

In constant streams

11.

What does the nucleus in the Bohr model consist of?

a)

Electrons and protons

b)

Protons and neutrons

c)

Neutrons and electrons

d)

Electrons only

12.

In the Bohr model, where are electrons located?

a)

In the nucleus

b)

In distinct orbits (levels)

c)

Randomly around the atom

d)

In a single orbit

13.

What term describes the allowed transitions of electrons between energy levels in the Bohr model?

a)

Radiationless orbits

b)

Quantum leaps

c)

Random jumps

d)

Continuous transitions

14.

Who proposed the concept of matter waves?

a)

Einstein

b)

De Broglie

c)

Newton

d)

Planck

15.

Where do electrons exist according to the orbital model?

a)

In fixed orbits

b)

In probability clouds or orbitals

c)

In a vacuum

d)

In solid matter

16.

What principle states that you cannot measure the exact position of a wave?

a)

Pauli exclusion principle

b)

Heisenberg uncertainty principle

c)

Bohr's model

d)

Rutherford's theory

17.

Which subatomic particle has a positive charge?

a)

Neutrons

b)

Electrons

c)

Protons

d)

Photons

18.

Where are electrons found in an atom?

a)

In the nucleus

b)

Orbiting the nucleus

c)

In the proton cloud

d)

In the neutron field

19.

Which subatomic particle is found in the nucleus and has no charge?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Positrons

20.

What is the atomic number of Neon?

a)

8

b)

9

c)

10

d)

11

21.

What is the charge of a proton?

a)

-1

b)

0

c)

+1

d)

+2

22.

What is the mass of a proton equivalent to?

a)

One electron mass

b)

One neutron mass

c)

One atomic mass unit (AMU)

d)

One gram

23.

Together with neutrons, what do protons determine?

a)

The atomic number of an element

b)

The chemical properties of an element

c)

The atomic mass of an element

d)

The isotopic abundance of an element

24.

Which subatomic particle is not found in the nucleus of an atom?

a)

Proton

b)

Neutron

c)

Electron

d)

All of the above are found in the nucleus

25.

Which of the following is true about isotopes?

a)

They have different atomic numbers but the same mass number

b)

They have the same atomic number but different mass numbers

c)

They have different numbers of electrons but the same number of protons

d)

They are always ions

26.

What is the mass number of an atom with 6 protons and 8 neutrons?

a)

6

b)

8

c)

14

d)

12

27.

What structure did Rutherford discover in his model of an atom?

a)

the Nucleus

b)

the Electron Cloud

c)

the quarks

d)

the atomic mass

28.

The Greek philosopher Democritus coined what word for a tiny piece of matter that cannot be divided?

a)

Element

b)

Atom

c)

Electron

d)

Molecule

29.
In a neutral atom, the number of electrons is equal to the number of _______.
a)
Neutrons
b)
Orbits
c)
Protons
d)
subatomic particles
30.

Smallest of the 3 subatomic particles

a)

protons

b)

neutrons

c)

electrons

31.

An element

a)

contains one type of atom

b)

contains two or more different type of atoms

c)

is two or more different substances not chemically combined

d)

is the way something is put together or combined

32.

Carbon

a)

CA

b)

Ca

c)

C

d)

Cn

33.

Sulfur

a)

Sf

b)

Sr

c)

S

d)

Su

34.

Neon

a)

Nn

b)

No

c)

N

d)

Ne

35.

Calcium

a)

Ca

b)

CA

c)

Cl

d)

CL

36.

Helium

a)

H

b)

He

c)

HE

d)

Hl

37.

Hydrogen

a)

H

b)

Hy

c)

Hg

d)

h

38.

Potassium

a)

T

b)

P

c)

K

d)

Pm

39.

Aluminum

a)

A

b)

Am

c)

An

d)

Al

40.

The smallest amount you can have of a compound is called a

a)

Molecule

b)

Compound

c)

Atom

d)

Sprinkle

41.

The smallest amount you can have of one element is a(n)

a)

Molecule

b)

Compound

c)

Atom

d)

Sprinkle

42.

H2O is an example of

a)

Compound

b)

Element

43.
What is the chemical symbol for the element oxygen
a)
O
b)
Oxy
c)
ox
d)
Oy
44.
What element is represented by the Chemical symbol Mg
a)
Manganese
b)
Magnesium
c)
Molybdenum
d)
Mitrium
45.
What is the chemical symbol for the element Fluorine
a)
F
b)
Fl
c)
Flu
d)
f
46.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
47.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
48.
Calcium is most like which of the following?
a)
Barium
b)
Potassium
c)
Cesium
d)
Nitrogen
49.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
50.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
51.
What is the name of the group that never reacts--ever ever they are stable with a full outermost ring!!!
a)
noble gases
b)
transition
c)
halogens
d)
borons
52.
The number at the bottom of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element name
53.
The number at the top of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
Chemical Symbol
d)
Element Name
54.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
55.
Which element is found in group 16 period 3?
a)
Sulfur (S)
b)
Selenium (Se)
c)
Chlorine (Cl)
d)
Carbon (C)
56.
Which element is found  in group 17 period 3?
a)
Chlorine
b)
Flourine
c)
Oxygen
d)
Phosphorous
57.
Which element is found in period 3 group 2?
a)
Sodium (Na)
b)
Magnesium (Mg)
c)
Yttrium (Y)
d)
Boron (B)
58.
Which element is found in group 18 period 4?
a)
Neon (Ne)
b)
Chlorine (Cl)
c)
Krypton (Kr)
d)
Xenon (Xe)
59.
a)

137

b)

56

c)

6

d)

2

60.
a)

74

b)

108

c)

47

d)

11

61.
a)

2

b)

8

c)

16

d)

4

62.
a)

18

b)

8

c)

40

d)

3

63.
a)

12

b)

30

c)

65

d)

4

64.

What are the three main groups of the periodic table?

a)

groups

b)

metal

c)

nonmetals

d)

metalloids

e)

periods

65.

What do the vertical columns on the periodic table tell us?

a)

The number of orbitals

b)

The number of valence electrons (electrons on the outer most shell)

66.

What do the horizontal rows on the periodic table tell us?

a)

The number of orbitals

b)

The number of valence electrons (the electrons on the outer most shell)

67.

What is the name of the element? (Periodic table will be needed)

a)

sodium

b)

magnesium

c)

vanadium

68.

What group and period does this element belong in? *

a)

period 1 and group 3

b)

period 3 and group 1

c)

period 2 and group 3

d)

period 3 and group 2

69.

How many valence electrons does the element have?

a)

1

b)

2

c)

3

d)

4

70.

How many orbitals does Nickel have?

a)

3

b)

4

c)

5

d)

10

71.

Who discovered the nucleus?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

72.

Who proposed a model with electrons moving in specific layers?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

73.

Who discovered the electrons?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

74.

This element has two valence electrons and two energy levels?

a)

Beryllium (Be)

b)

Lithium (Li)

c)

Zinc (Zn)

75.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
76.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
77.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
78.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
79.
What element is this?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
80.
?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
81.
?
a)
Helium
b)
Oxygen
c)
Sodium
d)
Phosphorous
82.

Mendeleev's genius was his ability to

a)

predict elements that were not discovered yet

b)

organize elements by their mass

c)

had an element named after himself

d)

organize elements by properties

83.

The first energy shell can hold ______ electrons.

a)

2

b)

8

c)

18

84.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

85.

Elements in the same group have __________

a)

Similar Properties

b)

Same number of shells

c)

Similar Mass

86.

What do all elements in the same period have?

a)

same number of shells

b)

same number of electrons

c)

belong in the same family

87.

When an atom gives away an electron it becomes

a)

an isotope

b)

a negative ion.

c)

a positive ion.

d)

sad.

88.

An atom that has the same number of protons but different numbers of neutrons is an _______________.

a)

isotope

b)

ion

c)

molecule

d)

awesome atom

89.

What are the red elements (those on the left)?

a)

metals

b)

nonmetals

c)

metalloids

90.

What are the blue elements (those on the right)?

a)

metals

b)

nonmetals

c)

metalloids

91.

The diagram shows a model of an atom of a particular element. Which element is represented by the model?

a)
b)
c)
d)
92.

The diagram shows a model of an atom of a particular element. Which element is represented by the model?

a)
b)
c)
d)
93.

Using the periodic table as a reference, which group of elements has similar chemical properties?

a)

C, N, O, F

b)

Mg, Ca, Sr, Ba

c)

B, Si, As, Te

d)

He, Ne, Ar, Xe

94.

Where are most metals on the periodic table?

a)

On the left side of the periodic table

b)

On the right side of the periodic table

95.

Most element on the periodic table are _______?

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Gases

96.

Found in group two of the periodic table; highly reactive

a)

period

b)

Alkali Earth Metals (Group 2)

c)

metalloids (semimetals)

d)

alkali metals (group 1)

97.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
98.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
99.

Ionic bonds happen because of the ____ of valence electrons.

a)

sharing

b)

transfer

c)

keeping

d)

covering

100.

How do covalent bonds form?

a)

Donating & receiving valence electrons between atoms

b)

Oppositely charged ions attract each other & form bonds

c)

Scientists are still not sure how they form

d)

Sharing valence electrons between atoms

101.

The formation of a covalent bond relies on the interaction or bonding of...

a)

2 Nonmetals

b)

1 Nonmetal & 1 Metal

c)

2 Metals

d)

2 Noble Gases

102.

Which of these atoms is stable?

a)
b)
c)
d)
103.
How many electrons should Boron have around its Lewis dot model?
a)
1
b)
3
c)
5
d)
7
104.
How many electrons should Hydrogen have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
105.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
106.
How many electrons should Flourine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
107.

This type of bonding can be described as "I give, I get"

a)

ionic

b)

covalent

c)

metallic

108.

This type of bonding can be described as a "cooperation"

a)

ionic

b)

covalent

c)

metallic

109.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
110.

How many electrons are delocalised in a metal?

a)

1

b)

2

c)

as many as are in the valence shell

d)

as many as are in the first energy level

111.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions

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