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Chemistry Unit 5

Total questions: 78

Worksheet time: 1hrs 5mins

Name
Class
Date
1.
A physical property that describes how tightly packed molecules are in a substance
a)
Density
b)
Conductivity
c)
Solubility
d)
Magnetistm
2.
Density is measured in ___________
a)
g
b)
g/mL
c)
mL
d)
N
3.
Which is dependent on the amount of a sample?
a)
mass
b)
density
c)
melting point
d)
electrical conductivity
4.
Which is an example of a physical property?
a)
ability to react with acid
b)
 color
c)
flammability
d)
ability to react with oxygen
5.
Physical properties are
a)
properties that can be observed without changing the identity of the substance
b)
properties that describe how a substance changes into a completely different substance
c)
properties that we can only observe with our eyes
d)
properties that we need special tools to observe
6.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
c)
liquid properties
d)
real properties
7.
What is burning an example of?
a)
physical change
b)
physical property
c)
chemical change
d)
chemical property
8.

Look at this picture of Argon off the periodic table. Which of the following is true for this element?

a)

18 protons

b)

40 protons

c)

22 protons

d)

21.9 protons

9.

Look at this picture of Argon off the periodic table. Which of the following is true for this element?

a)

18 neutrons

b)

40 neutrons

c)

22 neutrons

d)

21.9 neutrons

10.

Look at this picture of Argon off the periodic table. Which of the following is true for this element when it is neutral?

a)

18 electrons

b)

40 electrons

c)

22 electrons

d)

21.9 electrons

11.

Which part of an atom is used to identify it?

a)

number of protons

b)

number of neutrons

c)

number of electrons

12.

When you two atoms with different masses, Carbon-12 and Carbon-13 for example, what type of atom do you have?

a)

Neutral atom

b)

Ion

c)

Isotope

13.

When you two isotopes of an atom, Carbon-12 and Carbon-13 for example, what has changed in the atomic structure?

a)

Number of protons

b)

Number of neutrons

c)

Number of electrons

14.

When you have an ion of an atom, O-2 for example, what has changed in the atomic structure?

a)

Number of protons

b)

Number of neutrons

c)

Number of electrons

15.

When you have a positive ion of an atom, Na+1 for example, do you have a higher number of protons or electrons?

a)

Number of protons

b)

Number of electrons

16.

Which of the following is correct?

a)

Protons are positive, electrons are negative, neutrons are neutral.

b)

Protons are neutral, electrons are negative, neutrons are positive

c)

Protons are negative, electrons are positive, neutrons are neutral

d)

Protons are positive, electrons are neutral, neutrons are negative

17.

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

18.

What two subatomic particles must be equal for an atom to have no charge (neutral).

a)

protons and neutrons

b)

protons and electrons

c)

electrons and neutrons

19.

Found in the nucleus of an atom. This particle has a positive charge.

a)

Neutron

b)

Proton

c)

Electron

d)

Decepticon

20.

Found orbiting outside the nucleus, this subatomic particle has a negative charge.

a)

Neutron

b)

Proton

c)

Electron

d)

Idontknowatron

21.

Found in the nucleus of an atom, this subatomic particle has a neutral (or no ) charge

a)

Neutron

b)

Proton

c)

Electron

d)

Whattheheckatron

22.

The periodic table is in order by the

a)

Mass number

b)

Neutron number

c)

Atomic number

d)

APE MAN Number

23.

Name the element

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Oxygen

24.

Identify #4

a)

proton

b)

neutron

c)

electron

d)

nucleus

25.

Identify #3

a)

proton

b)

neutron

c)

electron

d)

nucleus

26.

Identify #2

a)

proton

b)

neutron

c)

electron

d)

nucleus

27.
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
28.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
29.
What is the atomic mass equal to?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
30.
Contains only one kind of atom.
a)
Element
b)
Compund
c)
Mixture
31.
Contains two or more atoms combined
a)
Elements
b)
Compounds
c)
Mixtures
32.
The air is a _________. 
a)
element 
b)
mixture 
c)
compound 
d)
energy 
33.
Elements can be broken down into simpler substances. 
a)
false 
b)
true 
c)
sometimes 
34.

Examples are diamonds (C) and Uranium (U)

a)

elements

b)

mixtures

c)

compounds

35.
Is sugar (C12H22O11) an element or a compound?
a)
Element
b)
Compound
36.
An element is made up of only one kind of _____.
a)
isotope
b)
plastic
c)
atom
d)
metal
37.
What is salad?
a)
element
b)
compound
c)
mixture
38.
Classify the picture with the correct label.
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
39.
Which of the following is an element?
a)
Sugar
b)
Salt
c)
Water
d)
Oxygen
40.
The building block of matter is
a)
Mixture
b)
Atom
c)
Element
d)
Substance
41.
Water is an element
a)
true
b)
false
42.

Which example is a compound?

a)

N2

b)

O2

c)

Cu

d)

H2O2

43.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
44.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
45.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
46.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1
47.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
48.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
49.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
50.
A bond that forms when electrons are transferred is called a/an
a)
ionic bond
b)
covalent bond
c)
hydrogen bond
51.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
52.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
53.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
54.
What charge does a potassium (K) ion have?
a)
+1
b)
-1
c)
+2 
d)
-2
55.
The compound formed between lithium and chlorine is _________.
a)
ionic
b)
covalent
56.
What type of bond is this?
a)
ionic
b)
covalent
57.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

58.

How many total atoms are in C6H1206

a)

3

b)

6

c)

12

d)

24

59.

After a chemical reaction occurs, atoms are not created nor destroyed,

a)

just rearranged into a new substance

b)

just changed into different elements

c)

just turned into unstable elements

60.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
61.
When an atom loses an electron, it is called a..
a)
crystal
b)
formula
c)
ion
62.

16. What is the number of valence electrons for Calcium (Group 2)?

a)

1

b)

2

c)

3

d)

4

63.
What would you name this molecule?
a)
SNa3
b)
H3O
c)
NaCl
d)
H2O
64.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
65.

What is the correct formula for this molecule?

a)

CH

b)

C1H4

c)

CH4

d)

C4H

66.

What is the Law of Conservation of Mass?

a)

It states that matter cannot be created or destroyed.

b)

It states that energy cannot be created or destroyed.

c)

It states that matter can be created or destroyed.

d)

It states that sound can be created or destroyed.

67.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number in front of a chemical formula.
c)
The number in between the chemical symbols.
d)
The number behind a chemical formula.
68.
What is the part of the chemical equation in green called? 
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
69.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
70.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
71.
Which problem is balanced?
(Check ALL answers)
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
72.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
73.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
74.
Element or compound?
H2O
a)
element
b)
compound
75.
Is this balanced?
Al + O2 → 2Al2O3
a)
Yes
b)
No
76.

Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe

a)

yes

b)

no

77.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
78.
Is the following reaction balanced?
2CH3OH + 3O2 --> 2CO2 + 4H2O
a)
yes
b)
no

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