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Chemistry Pre-assessment

Total questions: 139

Worksheet time: 3hrs 35mins

Name
Class
Date
1.

What aspect of the periodic table will tell you valence electrons?

a)

Groups

b)

Families

c)

Transitions

d)

Periods

2.

The symbol for Iron is

a)

Ir

b)

Fe

c)

I

d)

On

3.

What atom is the largest based on its location on the periodic table?

a)

H

b)

Ne

c)

As

d)

Fr

4.

What element is the most electronegative?

a)

H

b)

C

c)

Mg

d)

F

5.

All of the noble gasses do not bond because

a)

They are gasses

b)

They have 7 valence electrons

c)

They have their outer orbital filled

d)

They are ions.

6.

Iron can have more than one oxidation number. What are the two oxidation numbers Iron may have.

a)

+ 1, 2

b)

-2.-1

c)

2+, 1+

d)

0, 1+

7.

The element with a e-configuration of 1s2,2s2p6,3s1

a)

Calcium

b)

Potassium

c)

Sodium

d)

Argon

8.

Periods on the periodic table tell you.

a)

Valence Electrons

b)

Amount of Orbitals

c)

Electronegativity Only

d)

Size of the atom Only

9.

A ___________ is an arrangement of elements in columns

a)

columns

b)

rows

c)

periodic table

d)

electron shell

10.

The atomic number tells you what?

a)

number of electrons

b)

number of protons

c)

number of neutrons

d)

both electrons and protons in an atom.

11.
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
12.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
13.
Which element is not a metal?
a)
H
b)
Re
c)
Al
d)
B
14.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
15.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
16.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
17.
A horizontal row of elements in the periodic table.
a)
column
b)
group
c)
period
18.
A vertical column in the periodic table.  Elements share similar properties.
a)
row
b)
group
c)
period
19.
The simplest substance is..?
a)
Carbon
b)
An element
c)
Water
d)
A simple compound 
20.
A proton is....
a)
A negatively charged subatomic particle
b)
A positively charged subatomic particle
c)
A neutrally charged subatomic particle
d)
The only subatomic particle located in the nucleus
21.
A neutron has a charge of
a)
+2
b)
No charge
c)
-1
d)
+1
22.
Basic unit of matter - the smallest piece of matter known
a)
Element 
b)
Atom
c)
Molecule
d)
Compound
23.
Density is...
a)
the amount of mass in an object
b)
the amount of space an object takes up
c)
the amount of mass in a given space
d)
the weight of an object
24.
Negatively charged part of an atom located in levels outside the nucleus
a)
Proton
b)
Neutron
c)
Electron
d)
Neutron
25.
The density of water is 
a)
.1 g/cubic cm
b)
10g/cubic cm
c)
1.0 g/cubic cm
d)
0 g/cubic cm
26.
Burning a piece of paper 
a)
Chemical Change 
b)
Physical Change 
27.
Milk turning sour
a)
Chemical Change
b)
Physical Change 
28.
What is the symbol for the element Neon?
a)
Na
b)
Ne
c)
He
d)
N
29.
Which of the following is NOT a mixture? 
a)
NaCl + H2O
b)
C6H12O6 + H2O
c)
C6H12O6
d)
SiO2 +H2O
30.
Has properties different than the elements that make it up 
a)
Compound 
b)
Mixture 
31.
These are the two particles located inside the nucleus of an atom 
a)
Protons and Electrons 
b)
Protons and Neutrons 
c)
Electrons and Neutrons 
d)
Neutrons and Molecules 
32.

How many MOLECULES are in the following compound: CaCO3

a)

1

b)

3

c)

5

d)

0

33.

If I mix 8 grams of kool-aid powder with 82 grams of water, how much will the resulting kool-aid drink weigh?

a)

A little more than 82 grams

b)

74 grams

c)

90 grams

d)

82 grams

34.
A(n) _____ is a unique substance that forms when two or more elements combine chemically.
a)
element
b)
compound
c)
mixture
d)
all of the above
35.
If I have a block of wood with a density of 0.5 g/cm3 and I cut it in half, the density of one of the halves of wood would now be. . . 
a)
0.25 g/cm3 
b)
1.0 g/cm3
c)
0.5  g/cm3
d)
5.0  g/cm3
36.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
37.
Where are electrons of an atom found?
a)
Nucleus
b)
Electron Cloud
c)
Some are in the nucleus and some in the electron cloud.
d)
They are moving everywhere.
38.

The ions in most ionic compounds are organized into a

a)

molecule

b)

crystal lattice

c)

Lewis Structure

d)

polyatomic ion

39.

Ionic compounds are formed by ionic bonds between

a)

metals and metals

b)

transition metals

c)

nonmetals and nonmetals

d)

metals and nonmetals

40.

metals and nonmetals

a)

metallic bonds

b)

ionic bonds

c)

covalent bonds

d)

polyatomic ions

41.

Which of the following atom’s Lewis dot notation shows six valence electrons?

a)

nitrogen

b)

magnesium

c)

sulfur

d)

iodine

42.

How many electrons do strontium atoms generally lose?

a)

0

b)

1

c)

2

d)

3

43.

Cesium has an electronegativity value of 0.7 and fluorine has and electronegativity value of 4.0. Which of the following statements is true?

a)

Cesium has less of a tendency to attract electrons than fluorine.

b)

Fluorine repels electrons more than cesium.

c)

Cesium attracts electrons easier than fluorine.

d)

Fluorine has less of a tendency to attract electrons than cesium.

44.

If atoms that share electrons, have an unequal attraction for the electrons, the bond is called

a)

ionic

b)

polar

c)

nonpolar

d)

metallic

45.

The melting points of ionic compounds are higher than the melting points of molecular compounds because

a)

ionic compounds are brittle.

b)

attractive forces between ions are stronger than the attractive forces between molecules.

c)

Ionic substances are all flammable.

d)

none of the above

46.

Which of these compounds would have the highest melting point?

a)

NH3NH_3  

b)

OF2OF_2  

c)

H2OH_2O  

d)

NaCl

47.

The VSEPR theory is a model for predicting...

a)

the strength of metallic bonds.

b)

the shape of molecules.

c)

lattice energy.

d)

ionization energy.

48.

The chemical formula for water is H2O. This formula is an example of a(n)

a)

Lewis Structure

b)

formula unit

c)

molecular formula

d)

ionic formula

49.

Which of the following molecules has a single covalent bond?

a)

F2F_2  

b)

CO2CO_2  

c)

N2N_2  

d)

NO

50.

Which of the following molecules has a single lone pair of electrons?

a)

HClHCl  

b)

CH4CH_4  

c)

H2OH_2O  

d)

NH3NH_3  

51.

What is the molecular shape for carbon tetrachloride, CCl4.

a)

square

b)

tetrahedral

c)

trigonal planar

d)

trigonal pyramidal

52.

Which of the properties listed below is NOT a property of ionic compounds?

a)

hardness

b)

brittle

c)

low melting point

d)

high melting point

53.

A covalent bond between two different atoms in which the bonding electrons are not shared equally is a

a)

polar bond

b)

nonpolar bond

c)

ionic bond

d)

hydrogen bond

54.

Which of the following is the correct Lewis structure for hydrogen chloride, HCl?

a)

b)

55.

Determine the Lewis Structure for the nitrate ion, NO3−NO_3^-  

, Then, predict its molecular geometry.

a)

tetrahedral

b)

trigonal planar

c)

bent

d)

linear

56.

The electrons involved in the formation of a chemical bond are called

a)

dipoles.

b)

s block electrons.

c)

Lewis electrons.

d)

valence electrons.

57.

When drawing a Lewis Structure, the central atom is generally the

a)

atom with the fewest electrons.

b)

atom with the least electronegativity.

c)

atom with the highest atomic number.

d)

atom with the most electrons.

58.
How many independent variables can be tested in a controlled experiment?
a)
one
b)
two
c)
three
d)
as many as possible
59.
What is the group in an experiment that receives treatment with the independent variable?
a)
control group
b)
experimental group
c)
constant group
d)
variation group
60.
Which type of graph shows the differences between groups?
a)
Bar
b)
Pie
61.
When writing your hypothesis, what information follows IF?
a)
dependent variable
b)
how you know it will happen
c)
independent variable
d)
anything 
62.
This variable in an experiment is the one being deliberately changed by the scientist. 
a)
dependent variable
b)
independent variable
c)
data
d)
control group
63.
What step does every scientific experiment begin with?
a)
hypothesis
b)
question/problem
c)
procedures
d)
conclusion
64.
Type of graph that shows changes in quantities over time and distance.
a)
line graph
b)
pie graph
c)
bar graph
65.
What are compounds?
a)
Substances made of one or more types of elements.
b)
Substances made of one or more types of neutrons.
c)
Substances made of one or more types of nuclei.
d)
Substances made of one or more type of electron. 
66.
What is a pure substance?
a)
Protons Neutrons and Electrons. 
b)
Particles that collide. 
c)
Substance that can be separated by physical means.
d)
Substance that cannot be separated by physical means. 
67.
What is an atom made of? 
a)
Subatomic elements 
b)
Protons Neutrons and Electrons 
c)
Microscopic Particles 
d)
Positive Negative Neutral 
68.
What is the charge of a neutron?
a)
Positive
b)
Negative
c)
Neutral
69.
What is the atomic number of Carbon? 
a)
6
b)
12.0107
c)
C
d)
Carbon
70.
Which of the follow are NOT physical properties?
a)
Color
b)
Flammability
c)
State of Matter
d)
Taste 
71.
Solubility is
a)
an items ability to dissolve
b)
an items ability to melt
c)
an items ability to freeze
d)
an items ability to boil 
72.
The States of Matter are: 
a)
Solid Liquid Grass
b)
Solid Liquid Gasp
c)
Solid Liquid Gap
d)
Solid Liquid Gas 
73.
Chemical properties are the way a substance 
a)
restarts 
b)
reacts
c)
renews
d)
reviews 
74.
What is the smallest unit of matter? 
a)
Element 
b)
Atom
c)
Molecule 
d)
Compound 
75.
Which one is NOT a compound? 
a)
H2O
b)
CO2
c)
NaCl
d)
Ne
76.
I am anything that has mass and takes up space!
a)
energy
b)
matter
c)
molecules
d)
atoms
77.
A change in the form of a substance that does not change its identity?
a)
Physical Change
b)
Malleability
c)
Soluability
d)
Density
78.
The relationship between mass and volume?
a)
Volume
b)
Density
c)
weight
79.
Characteristic that can be observed or measure such as color, state, or hardness?
a)
Physical Change
b)
Physical Property
c)
Solubility 
80.
Which of the following is not an example of physical Change?
a)
Shaping of a gold bar
b)
explosion of fireworks
c)
sanding a piece of wood
d)
melting of popsicle
81.
What is the best way to tell if a chemical change has taken place?
a)
The matter changes color
b)
The change is reversible
c)
The mixture separates into layers
d)
The composition changes
82.
The tool used to measure the mass of a substance or object is a ______________.
a)
balance
b)
graduated cylinder
c)
ruler
d)
thermometer
83.
Jack has a rock. The rock has a mass of 14g and a volume of 2cm3. What is the density of the rock?
a)
7 mL
b)
7 g/cm3
c)
28 g/cm3
d)
1/7 g/cm3
84.
What is the volume of Object X?
a)
10.0 cm3
b)
15.0 cm3
c)
20.0 cm3
d)
25.0 cm3
85.
Put the liquids in order from most dense to least dense?
a)
4, 3, 2, 1
b)
1, 2, 3, 4
c)
3, 4, 2, 1, 
d)
4, 3, 1, 2
86.
Which box has a higher density?  
a)
Box A
b)
Box B
c)
cannot be determined
d)
they are the same
87.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
88.
How many protons does an atom of Nitrogen have?
a)
14
b)
7
c)
15
d)
18
89.
Which of the following is a negatively charged subatomic particle?
a)
Electron
b)
Proton
c)
Neutron
d)
Quark
90.
How many neutrons are in an atom of Beryllium?
a)
4
b)
9
c)
9.01
d)
5
91.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
92.
Which is the correct formula for:
 three hydrogen (H)
one sulfur (S)
four oxygen (O)
a)
H3SO4
b)
HSO4
c)
H4S3O
d)
H2O
93.
How many total atoms are in 2Cu(SO4)2?
a)
12
b)
16
c)
20
d)
22
94.
How many atoms of Oxygen (O) are in 2Cu(SO4)2?
a)
8
b)
12
c)
16
d)
20
95.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
96.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
97.
A mole of Neon contains
6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
98.
Calculating percent composition determines the ___________ of each atom in a compound
a)
percent by mass
b)
percent by volume
c)
percent by number
99.
In this image, what are the information in red is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
100.
In this image, what are the information to the right of the arrow (in black) is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
101.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
102.
What is the empirical formula for the following molecular formula: C5H12
a)
C5H12
b)
CH3
c)
CH2
d)
C2.5H6
103.
The law of conservation of mass states that....
a)
Matter can be made
b)
Matter can be destroyed
c)
Matter can neither be made or destroyed
104.
You mix lemon juice and baking soda. The temperature drops on the thermometer. This is a ______reaction.
a)
Exothermic
b)
Endothermic
c)
Ionic
105.
Is this balanced?...
Al + O2 --> 2Al2O3
a)
Yes!
b)
NO!
106.
Balance this equation...
HgO --> 2Hg + O2
a)
It is balanced 
b)
2HgO --> Hg + O2
c)
2HgO --> 2Hg + O2
107.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
108.
Which of these substances is acidic?
a)
tap water
b)
lemon
c)
ammonia
d)
baking soda
109.
How is a standard hydrogen atom different from a hydrogen ion?
a)
a hydrogen ion has an extra electron.
b)
a hydrogen ion is missing an electron.
c)
a hydrogen ion has an extra proton.
d)
a hydrogen ion is missing a proton.
110.
What might happen if you mixed a strong acid with an equally strong base?
a)
You would see an explosive chemical reaction.
b)
The acid would destroy the base.
c)
The base would destroy the acid.
d)
You'd wind up with a pH-neutral substance.
111.
An extremely strong base would have a pH of:
a)
1
b)
7
c)
9
d)
14
112.
Healthy environments for life have a pH closest to:
a)
1
b)
3
c)
7
d)
10
113.
A beaker contains a mixture of a sand and small pebbles. What kind of mixture is this?
a)
Homogeneous  
b)
Solution
c)
Heterogeneous  
d)
Compound    
114.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
115.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
116.
Which substance is reduced in the following reaction? 
NaOH + Li --> LiOH + Na
a)
Li
b)
Na
c)
O
d)
H
117.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
118.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
119.
True or False - Elements in  the same group have similar chemical properties.
a)
True
b)
False
120.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
121.
Ionic Bonds form between two ions that have
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
122.
Ions that are made of more than one atom bonded covalently are called
a)
ionic compounds
b)
crystals
c)
polyatomic atoms
d)
ionic bonds
123.
Nonmetals are most likely to _____________ valence electrons in order to have a stable arrangement.
a)
lose
b)
gain
c)
gain or share
d)
share
124.
Which of the following is NOT a polyatomic ion?
a)
NH4+
b)
HCO3-
c)
Ca2+
d)
SO42-
125.
How many are shared in a double bond?
a)
2
b)
4 pairs
c)
6
d)
4
126.
When a metal reacts with a nonmental, it makes
a)
an ionic compound
b)
a covalent compound
c)
a low melting point
d)
water molecules
127.

How many moles are 98.3 grams of aluminum hydroxide, Al(OH)3? (Ar Al=27, H=1, O=16)

a)

1.26 moles

b)

0.8 moles

c)

7,673.4 moles

d)

150 moles

128.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.0500 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
129.
How many molecules are in 2.00 moles of H2O?
a)
124x1024 molecules of H2O
b)
1.20x1023 molecules of H2O
c)
1.20x1024 molecules H2O
d)
124
130.
How many atoms are in 1.50 moles of Hg?
a)
9.03x1023 atoms Hg
b)
9.03x1024 atoms Hg
c)
903 atoms of Hg
d)
9.03 atoms of Hg
131.

How many grams are in 1.2 x 1024 molecules of CO? (molar mass of CO = 28 g/mol)

a)

28.2 g

b)

55.8 g

c)

6.02 g

d)

1.2 g

132.

How many grams of silicon (atomic mass = 28.1 amu) would there be in a sample that contained 9.99 x 1022 atoms?

a)

1.69 g

b)

4.66 g

c)

1.66 g

d)

1.79 g

133.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
134.

Why is the mole used to measure the atom?

a)

Atoms are extremely tiny particles, and their size varies from element to element

b)

Atoms are all the same size for every element

c)

Some atoms cannot be counted using the mole

d)

For count my dog`s hairs.

135.

The mole can be used to measure (SELECT ALL CORRECT ANSWERS)

a)

The amount of atoms

b)

The amount of molecules or compounds in a substance

c)

The amount of particles

d)

The amount of fission or fusion decay over time

136.

Calculate the number of moles copper (II) sulfate in 320g of CuSO4.

Cu =63 , S =32 ,O=16

a)

2

b)

4

c)

6

d)

8

137.

88.0 grams of CO2 is about _____________. [Select 2 answers.]

a)

1 mole of CO2

b)

2 moles of CO2

c)

6.02 x 1023 molecules of CO2

d)

two times 6.02 x 1023 molecules of CO2

138.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
139.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 3 moles of Fe2O3?
a)
6 moles Fe
b)
4 moles Fe
c)
2 moles Fe
d)
1 moles Fe

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