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Unit 2 practice Exam

Total questions: 48

Worksheet time: 1hrs 13mins

Name
Class
Date
1.

Isotopes are atoms of the same element with different numbers of

a)

electrons

b)

neutrons

c)

protons

d)

nuclei

2.

Elements on the Periodic Table are ordered according to their

a)

element name

b)

element symbol

c)

number of atoms

d)

atomic number

3.

Protons have a ____________ charge, neutrons have a ____________ charge, and electrons have a ____________ charge.

a)

positive; negative, neutral

b)

positive, neutral, negative

c)

neutral, negative, positive

d)

negative, neutral, positive

4.

The number of neutrons in an atom can be found by

a)

adding the number of neutrons and protons together.

b)

adding the atomic mass and the atomic number.

c)

subtratcting the atomic number from the atomic mass.

d)

subtracting the atomic mass from the atomic number.

5.

The smallest particle of an element that has the same chemical properties of the element is

a)

a molecule of that element.

b)

an atom of that element.

c)

a proton of that element.

d)

the nucleus of the element.

6.

The history of the Atomic Theory involves many changes from its early form. Theories change because

a)

people decide to no longer agree with them.

b)

all theories must be changed after a certain time.

c)

new evidence is found that allows the theory to be changed.

d)

when scientists die, their theories are always changed.

7.

Whose model suggested that negative particles were mixed in with positively charged material - like seeds in a watermelon?

a)

J.J. Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Albert Einstein

8.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

9.
What can you conclude from the fact that scientists continue to update the atomic model?
a)
New information about atoms continues to be discovered
b)
Old information about atoms is completely useless
c)
Scientists did not have any information about atoms until a few years ago
d)
Scientists still have no idea what atoms look like
10.

Which scientist first suggested that atoms could join?

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

11.
Moseley discovered that the ________ was the most fundamental property needed for organization.                                                 
a)
atomic mass
b)
mass number
c)
atomic number
d)
number of protons
12.
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
13.
Different isotopes have...
a)
different masses
b)
different atomic numbers
c)
different electrons
d)
different protons
14.
How many neutrons does a Sodium 24 isotope have?
a)
12
b)
13
c)
14
d)
15
15.
What is the name of the pictured isotope?
a)
Carbon-12
b)
Carbon-13
c)
Carbon-14
d)
Carbon-15
16.

In an element box, the number at top is the

a)

atomic number

b)

atomic name

c)

atomic mass

d)

atomic symbol

17.

___________________ are positively charged particles located in the nucleus of an atom.

a)

Electrons

b)

Neutrons

c)

Protons

d)

Isotopes

18.

Isotopes are atoms of the same element with different numbers of

a)

electrons

b)

neutrons

c)

protons

d)

nuclei

19.

Elements on the Periodic Table are ordered according to their

a)

element name

b)

element symbol

c)

number of atoms

d)

atomic number

20.

A scientist creates a hypothesis, but the data she collects fail to support that hypothesis. The scientist should then

a)

change the data to support the hypothesis.

b)

change the hypothesis to match the results.

c)

forget the whole idea and walk away.

d)

use the data to develop and test a new hypothesis.

21.

Protons have a ____________ charge, neutrons have a ____________ charge, and electrons have a ____________ charge.

a)

positive; negative, neutral

b)

positive, neutral, negative

c)

neutral, negative, positive

d)

negative, neutral, positive

22.

The chemical symbol in this element box is

a)

26

b)

Fe

c)

Iron

d)

55.845

23.

The variable that is changed in an experiment is the

a)

independent variable.

b)

the dependent variable.

c)

the controlled variable.

d)

the data variable

24.

The number of neutrons in an atom can be found by

a)

adding the number of neutrons and protons together.

b)

adding the atomic mass and the atomic number.

c)

subtratcting the atomic number from the atomic mass.

d)

subtracting the atomic mass from the atomic number.

25.

The nucleus of an atom is located in its

a)

electron cloud

b)

center

c)

proton

d)

backpack

26.

The smallest particle of an element that has the same chemical properties of the element is

a)

a molecule of that element.

b)

an atom of that element.

c)

a proton of that element.

d)

the nucleus of the element.

27.

The history of the Atomic Theory involves many changes from its early form. Theories change because

a)

people decide to no longer agree with them.

b)

all theories must be changed after a certain time.

c)

new evidence is found that allows the theory to be changed.

d)

when scientists die, their theories are always changed.

28.

Models are used to study atoms because atoms are very

a)

dangerous

b)

sneaky

c)

rare

d)

small

29.

All matter is made of

a)

electrons

b)

protons

c)

neutrons

d)

atoms

30.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
31.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
32.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
33.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
34.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
35.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
36.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1
37.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
38.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
39.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
40.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
41.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
42.

Name the ionic compound, LiCl

a)

lithium chlorine

b)

lithium chloride

c)

lithium chlorate

d)

lithium monochloride

43.

Name the ionic compound, CaCO3

a)

calcium carbide

b)

calcium carbon trioxide

c)

calcium carbon oxide

d)

calcium carbonate

44.

Name the ionic compound, FeBr3

a)

Iron (II) bromide

b)

Iron (III) bromide

45.
K20 - name?
a)
potassium dioxide
b)
potassium oxide
c)
potassium oxygen
d)
dipotassium dioxide
46.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

Po2O5

47.

What is the name for SiCl4?

a)

silicon tetrachloride

b)

silicon quadchloride

c)

monosilicon tetrachloride

d)

silicon chloride

48.

What is the chemical formula of sulfur hexabromide?

a)

SBr₆

b)

S₆Br

c)

S(VI)Br

d)

SBr4

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