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atomic structures

Total questions: 109

Worksheet time: 2hrs 46mins

Name
Class
Date
1.

Which of the choices below has the correct order of scientists' discoveries of the structure of an atom?

a)

Bohr, Democritus, Dalton, Thomson, Rutherford, Schrodinger

b)

Democritus, Dalton, Thomson, Schrodinger, Bohr, Rutherford

c)

Democritus, Dalton, Thomson, Rutherford, Bohr, Schrodinger

d)

Schrodinger, Bohr, Rutherford, Thomson, Dalton, Deomcritus

2.

Rutherford discovered his concept of an atom before Schrodinger discovered his.

a)

True

b)

False

3.

This image is an example of ...

a)

A Bohr model

b)

A Dalton model

c)

A Rutherford model

d)

A Thomson Model

4.

Described atoms of water as roundballs

a)

Rutherford

b)

Democritus

c)

Bohr

d)

Dalton

5.

Used raisins in rice pudding to describe how electrons are distributed in the sphere.

a)

Thomson

b)

Rutherford

c)

Bohr

d)

Dalton

6.

Found that there is a higher probability to find electrons within a space surrounding the nucleus.

a)

Democritus

b)

Dalton

c)

Thomson

d)

Schrodinger

7.

Found that positive charged particles are in the nucleus and negative charged particles surround the nucleus.

a)

Rutherford

b)

Democritus

c)

Schrodinger

d)

Bohr

8.

Found that atoms are tiny, hard, and uncuttable.

a)

Schrodinger

b)

Rutherford

c)

Democritus

d)

Thomson

9.

Found that electrons in atoms orbit around the nucleus similar to the way planets around the Sun.

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

10.

Believed atoms were solid, indivisible spheres.

a)

Dalton

b)

Rutherford

c)

Bohr

d)

Democritus

11.
An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a)
13
b)
14
c)
27
d)
40
12.
Which subatomic particle has a relative charge of -1?
a)
the proton
b)
the neutron
c)
the electron
d)
the photon
13.
The nucleus contains _____
a)
only protons
b)
protons and neutrons
c)
protons and electrons
d)
electrons and neutrons
14.
number of neutrons =  _____
a)
atomic number - mass number
b)
isotope number - atomic weight
c)
mass number - atomic weight
d)
mass number - atomic number
15.
For an atom to be electrically neutral, it must contain the same number of _____
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
nucleons and electrons
16.
If you want to know which atom an element is, then count the _____
a)
protons
b)
neutrons
c)
electrons
d)
nucleons
17.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
18.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
19.
If an atom of nickel has a charge of +3, how many electrons does the atom have?
a)
28
b)
25
c)
26
d)
31
20.
If an atom of oxygen has a charge of -2, how many electrons does the atom have?
a)
18
b)
6
c)
8
d)
10
21.
When an atom gains a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
22.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
23.
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
24.
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
25.
Iron-60 (atomic number 26) is an isotope that is often used to study meteorites.  How many neutrons does iron-60 have?
a)
26
b)
60
c)
34
d)
86
26.
Isotopes of the same element have the same number of 
a)
protons
b)
neutrons
c)
electrons
d)
not enough information
27.
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
28.
Which of the following statements regarding subatomic particles is incorrect?
a)
Protons are positively charged particles and neutrons have no charge.
b)
The relative mass of the proton, electron and neutron the same.
c)
In a neutral atom the number of protons equals the number of electrons.
d)
Isotopes of an element have the same number of protons but a different number of neutrons.
29.
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
30.
How is the number of protons calculated from the periodic table?
a)
Atomic number
b)
Atomic mass
c)
Atomic mass - Atomic number
d)
Atomic Symbol
31.
How is the number of neutrons calculated from the periodic table?
a)
atomic number
b)
atomic mass
c)
atomic mass - atomic number
d)
chemical symbol
32.
Which subatomic particles are important in the formation of bonds?
a)
electrons
b)
protons
c)
neutrons
33.
If an atom loses an electron, does the atom become more positive or more negative?
a)
more positive
b)
more negative
c)
both
d)
neither
34.
If an atom gains a new electrons, does the atom become more positive or more negative?
a)
more positive
b)
more negative
c)
both
d)
neither
35.
What is the overall charge of this atom?
a)
+3
b)
-3
c)
0
d)
+1
36.
What is the overall charge of this atom?
a)
+4
b)
-3
c)
+1
d)
-1
37.
How does the size of an electron compare to the size of a proton?
a)
larger
b)
smaller
c)
equal
38.
How does the size of a proton compare to the size of a neutron?
a)
larger
b)
smaller
c)
equal
39.
Where are neutrons located in the atom?
a)
shells/orbitals
b)
rings
c)
center
d)
nucleus
40.
Where are electrons located in the atom?
a)
Nucleus
b)
Shells/orbitals
c)
rings
d)
center
41.
Where are protons located in the atom?
a)
orbitals
b)
nucleus
c)
rings
d)
positive
42.
What charge does a neutron have?
a)
positive
b)
negative
c)
no charge
d)
neutral
43.
What charge does an electron have?
a)
positive
b)
negative
c)
neutral
d)
no charge
44.
What charge does a proton have?
a)
positive
b)
negative
c)
no charge
d)
neutral
45.
What is the atomic mass of Carbon?
a)
5
b)
6
c)
7
d)
12.01
46.
What is the atomic number of Barium?
a)
20
b)
38
c)
56
d)
88
47.

Negatively charged particle

a)

proton

b)

neutron

c)

electron

48.

What do protons, electrons and neutrons make?

a)

element

b)

compound

c)

atom

49.

Which of the following type of bond occurs when one atom gives one or more electrons to another atom?

a)

Covalent bonding

b)

Both ionic and covalent bonding

c)

Compound bonding

d)

Ionic bonding

50.

What kind of substances tend to form covalent bonds?

a)

Two metals bonding together

b)

None of the answers are correct.

c)

Metals bonding with nonmetals

d)

Two nonmetals bonding together

51.

Which of the following is NOT a subatomic particle found inside the atom?

a)

Electrons

b)

Protons

c)

Ions

d)

Neutrons

52.

Beryllium has an atomic number of 4 and an atomic mass of 9. What can we conclude from this?

a)

There are 4 protons

b)

There are 5 neutrons

c)

A neutral beryllium atom will have 4 electrons

d)

All of these

53.

If you know the atomic number and the atomic mass of an atom then you should be able to figure out...

a)

the number of neutrons

b)

the name of the element

c)

the number of protons

d)

all of these

54.

Which of the following are NOT found in the atomic nucleus?

a)

electrons

b)

Nuclear Force

c)

Neutrons

d)

Protons

55.

A __________ is a subatomic particle with a neutral charge.

a)

proton

b)

neutron

c)

electron

d)

nucleus

56.

If you create a mixture by putting two substances together, what kind of bonding occurs?

a)

Covalent bonding

b)

Compound bonding

c)

Ionic bonding

d)

None of the answers are correct

57.

An element is defined by the number of:

a)

Electrons

b)

Protons

c)

Ions

d)

Neutrons

e)

Chemical Bonds

58.

What is true about all of the atoms of a single element?

a)

They have the same number of protons.

b)

They have the same number of protons, neutrons, and electrons.

c)

They have the same number of protons and neutrons.

d)

They have the same number of neutrons.

59.

What is the atomic number of this element?

a)

17

b)

18

c)

35

d)

35.453

60.

What is the average atomic mass of Magnesium?

a)

12.011

b)

14.007

c)

22.990

d)

24.305

61.

A __________ is a subatomic particle with a negative charge.

a)

proton

b)

neutron

c)

electron

d)

nucleus

62.

A __________ is a subatomic particle with a positive charge.

a)

proton

b)

neutron

c)

electron

d)

nucleus

63.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
64.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
65.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
66.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
67.

What is a valence electron?

a)

Electrons in the first energy shell

b)

Electrons in the second energy shell

c)

Electrons in the outer shell

d)

Total number of electrons

68.

What is a valence electron?

a)

Electrons in the first energy shell

b)

Electrons in the second energy shell

c)

Electrons in the outer shell

d)

Total number of electrons

69.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
70.
What is the name of this element?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
71.

A __________ is a subatomic particle with a negative charge.

a)

proton

b)

neutron

c)

electron

d)

nucleus

72.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
73.

Found that electrons in atoms orbit around the nucleus similar to the way planets around the Sun.

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

74.

How many electrons does sulfur have

a)

16

b)

32

c)

48

d)

12

75.

Believed atoms were solid, indivisible spheres.

a)

Dalton

b)

Rutherford

c)

Bohr

d)

Democritus

76.

When trying to identify an unknown element, a scientist determines what other elements the unknown element reacts which chemically. Which property of the unknown element determines the other elements in reacts with?

a)

the total number of neutrons in the unknown element

b)

the total number of particles in the nucleus of the unknown element

c)

the number of protons in the nucleus of the unknown element

d)

the number of valence electrons in the unknown element

77.

A model of an atom is shown in the image. An atom of which element is represented by this model?

a)

Boron (B)

b)

Carbon (C)

c)

Neon (Ne)

d)

Sodium (Na)

78.

The table in the image below lists three characteristics of an atom of an element. An atom of which element is described by the data in the table?

a)

Radon (Rn)

b)

Cadmium (Cd)

c)

Rubidium (Rb)

d)

Astatine (At)

79.

A student is studying calcium, a highly reactive element that humans need for strong bones. Which characteristic of calcium is most closely related to its chemical reactivity?

a)

the 20 protons in each atom of calcium

b)

the density of calcium, which is 1.54 g/cm3

c)

the atomic mass of calcium, which is 40.078 amu

d)

the 2 valence electrons in each atom of calcium

80.

A chemist is identifying the elements present in a sample of seawater. What characteristics of an element's atoms always determines the element's identity?

a)

the number of protons

b)

the number of neutrons

c)

the location of valence electrons

d)

the number of valence electrons

81.

The atoms of a certain element each contain 11 protons and 1 valence electron. Which statement correctly identifies this element and describes its chemical reactivity?

a)

The element is sodium and it is highly reactive

b)

The element is fluorine and is not very reactive

c)

The element is sodium and is not very reactive

d)

The element is fluorine and it is highly reactive

82.

Tin, Sn, is a soft white metal. It has a low melting point compared with other metals. Tin is widely used as a coating for cans of food. Which statement accurately describes atoms of tin?

a)

Tin atoms have 50 protons

b)

Tin atoms have five valence electrons

c)

Tin atoms have 119 neutrons

d)

Tin atoms have 68 electrons

83.

The diagram shows a model of an atom. The model has four different symbols on it. Each symbol represents a different role for one of the particles within the atom. In this model, which particle determines the reactivity of this atom?

a)

Particle W

b)

Particle X

c)

Particle Y

d)

Particle Z

84.

overall charge =

a)

# of (+protons) plus # of (-electrons) = ____

b)

# of (+protons) minus

85.

Atoms of which two elements have a combined total of 23 protons?

a)

Sodium, Na, and magnesium, Mg

b)

Boron, B, and carbon, C

c)

Copper, Cu, and zinc, Zn

d)

None of these

86.

an atom or group of atoms with a positive or negative charge

a)

ion

b)

isotope

c)

metals

d)

protons and electrons

87.

the atomic number represents this

a)

protons

b)

neutrons

c)

mass number

d)

isotope

88.

this group of elements tend to loose electrons

a)

metals

b)

nonmetals

c)

protons

89.

when electrons are lost a ____ charge is obtained

a)

positive

b)

negative

c)

gained

d)

ion

90.

protons + neutrons

a)

mass number

b)

atomic mass

c)

isotope

d)

ion

91.

protons neutrons and electrons are called this

a)

subatomic particles

b)

atomic mass

c)

ion

d)

isotope

92.

A chemist is identifying the elements present in a sample of seawater. What characteristics of an element's atoms always determines the element's identity?

a)

the number of protons

b)

the number of neutrons

c)

the location of valence electrons

d)

the number of valence electrons

93.

this group of elements tend to gain electrons

a)

nonmetals

b)

metals

c)

atomic mass

d)

ion

94.

for a neutral atom, the charge on these particles balance out the charge on protons

a)

electrons

b)

isotopes

c)

nonmetals

d)

mass number

95.

in order for a neutal atom to obtain a negative charge, electrons must be _____

a)

gained

b)

positive

c)

negative

d)

protons

96.

The atoms of a certain element each contain 11 protons and 1 valence electron. Which statement correctly identifies this element and describes its chemical reactivity?

a)

The element is sodium and it is highly reactive

b)

The element is fluorine and is not very reactive

c)

The element is sodium and is not very reactive

d)

The element is fluorine and it is highly reactive

97.

an average of masses of different isotopes

a)

atomic mass

b)

subatomic particles

c)

ion

d)

metals

98.
Valence Electrons determine an element's _____________.
a)
Reactivity
b)
Location
c)
Identity
d)
Color
99.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
100.

different numbers of neutrons create these different "versions"

a)

isotopes

b)

metals

c)

electrons

d)

atomic mass

101.

The identity of the atom is determined by the ______.

a)

protons

b)

neutrons

c)

electrons

102.

Neutrons have a ________ charge.

a)

positive

b)

negative

c)

neutral

103.

The atomic mass of an atom is equal to

a)

number of protons plus number of neutrons

b)

number of protons plus number of electrons

c)

number of electrons plus the number of neutrons

104.

What charge does an electron have?

a)

positive

b)

neutral

c)

negative

105.

Which parts of the atom move around the nucleus?

a)

electrons

b)

protons

c)

electrode particles

d)

neutrons

106.

In what part of an atom can the protons and neutrons be found?

a)

nucleus

b)

neutrine

c)

electron cloud

d)

proton cloud

107.

Subatomic particle that has a positive charge

a)

electron

b)

poitron

c)

neutron

d)

proton

108.

How many electrons does sulfur have

a)

16

b)

32

c)

48

d)

12

109.
Which particle has a positive charge?
a)
electron
b)
orbital
c)
proton
d)
neutron

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