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1st Semester Chemistry Practice Test

Total questions: 150

Worksheet time: 5hrs 0mins

Name
Class
Date
1.

Which type of flask is this?

a)

Beaker

b)

Volumetric

c)

Erlenmeyer

d)

Graduated Cylinder

2.

There are ___ meters in 25 kilometers (km).

a)

250m

b)

2500m

c)

25000m

d)

.025m

3.

Chemists use this unit of measure for volume?

a)

meter

b)

liter

c)

gram

d)

wavelength

4.

How many kilograms are in 774,000 grams?

a)

.0774 Kg

b)

7,740 Kg

c)

774 Kg

d)

774,000,000 Kg

5.

When using descriptive words like boiling, blue and bubbles as you carry out a chemical experiment, you are recording and collecting.......

a)

Quantitative Data

b)

Qualitative Data

c)

Verified Data

d)

Estimated Data

6.

What is the element name for the symbol, P ?

a)

Platinum

b)

Potassium

c)

Palladium

d)

Phosphorus

7.

Most of the mass of the atom is located....

a)

in the empty space.

b)

in the orbital energy levels (orbitals).

c)

in the nucleus.

d)

in the valence shells.

8.

Which of the following experiment demonstrated that there must be some positive charge in the nucleus?

a)

Neils Bohr Model of the Atom

b)

Rutherford's Gold Foil

c)

J.J. Thompson's Plum Pudding Model

d)

John Dalton's Atomic Theory

9.

If you subtract the atomic number from the atomic mass, the number remaining is the same as.....

a)

the number of neutrons in the atom.

b)

the number of electrons in the atom.

c)

the number of protons in the atom.

d)

the nuclear mass of the atom.

10.

This subatomic particle defines the element.

a)

Neutron

b)

Proton

c)

Electron

d)

Nucleus

11.

Which one is the electron configuration for an oxygen atom?

a)

1s22s22p63s23p64s2

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p6

12.

What is the abbreviated electron configuration for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

13.

When a metal bonds with a non-metal, the bond that forms is called___?

a)

Metallic

b)

Covalent

c)

Ionic

d)

Shared

14.

What kind of bond forms between two nonmetals?

a)

ionic

b)

covalent

c)

metallic

d)

symbiotic

15.

What are valence electrons?

a)

sum of the protons and neutrons

b)

protons minus electrons

c)

electrons in the innermost shell (orbital)

d)

electrons in the outermost shell (orbital)

16.

What is the correct formula for Sodium Oxide?

a)

NaO

b)

NaO2

c)

Na2O

d)

Na2O2

17.

Name the following compound: K2O

a)

Potassium Dioxide

b)

Potassium oxide

c)

Potassium II oxide

d)

Dipotassium oxide

18.

How would you name MgCl2?

a)

Magnesium chlorine

b)

Magnesium chloride

c)

Magnesium dichloride

d)

Magensium II chloride

19.

An -ate or -ite at the end of a compound name usually indicates that the compound contains _____________.

a)

fewer electrons than protons

b)

neutral molecules

c)

only two elements

d)

a polyatomic ion

20.

What is the name of H2SO4?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

21.

Which of the following shows both the correct formula and correct name of an acid?

a)

HClO2, chloric acid

b)

HNO2, hydronitrous acid

c)

H3PO4, phosphoric acid

d)

HI, iodic acid

22.

A process that absorbs heat is a(n) _________.

a)

Exothermic process

b)

Polythermic process

c)

Endothermic process

d)

Ectothermic process

23.

A metallic bond is between

a)

metal and metal

b)

metal and nonmetal

c)

nonmetal and nonmetal

24.

The periodic table is organized by the

a)

atomic numbers

b)

alphabetical order

c)

densities

d)

melting points

25.

What is the oxidation number for Carbon?

a)

+4 and -4

b)

-3

c)

+1

26.

What is the oxidation number for Nitrogen?

a)

+4 and -4

b)

-3

c)

+1

27.

Is this the correct lewis dot for Sodium?

a)

yes

b)

no

28.

Which Lewis dot matched the configuration:

1s21s^2   2s22s^2   2p22p^2  

a)
b)
c)
29.

Which Lewis dot matched the configuration:

1s21s^2   2s22s^2   2p22p^2   2p62p^6   3s13s^1  

a)
b)
c)
30.

What is the correct Lewis Dot diagram for a molecule of Nitrogen trihydride (NH3)?

a)
b)
c)
31.

Which name represents the formula Fe2O3Fe_2O_3  ?

a)

Iron (III) oxide

b)

Iron (II) oxide

32.

Match the name and formula:

a)

iron (II) oxide, Fe2O3

b)

potassium chloride, KCl

c)

carbon monoxide, CO2

33.

Which is the electron configuration of an atom of Period 3 element?

a)

1s22s1

b)

1s22s22p63s1

34.

Alkali metals have...

a)

1 valence electron, +1 charge

b)

2 valence electrons, +2 charge

c)

1 valence electrons, -1 charge

35.

Decomposing of an apple is an example of...

a)

chemical change

b)

physical change

36.

Which one is the least reactive group?

a)

Alkali metal

b)

Alkali earth metal

c)

Halogens

d)

Noble Gases

37.

Which of the following is the Lewis dot diagram for Bromine:

a)
b)
c)
38.

Which answer is an example of a chemical change?

a)

Boiling water

b)

rusting iron

c)

dissolving powder

d)

freezing water

39.

Which answer is an example of a physical change?

a)

freezing water

b)

burning coal

c)

rusting iron

d)

baking a cake

40.

Which answer is an example of a physical change?

a)

baking a cake

b)

burning coal

c)

rusting iron

d)

dissolving powder

41.

1s22s22p63s23p63d104s24p3

Which element does this configuration belong to?

a)

Arsenic

b)

Calcium

c)

Lithium

d)

Aluminum

42.

Which of the following substances are elements?

a)

water

b)

salt

c)

carbon dioxide

d)

hydrogen

43.

States of Matter: Melting, Freezing, Evaporating, and Sublimating are all...

a)

physical changes.

b)

chemical changes.

44.

States of Matter: Which of the following has a tightly packed structure?

a)

solid

b)

liquid

c)

gas

45.

Which of these is an example of a Homogeneous mixture:

a)

Tea with sugar

b)

oil and water

c)

NaCl

d)

H2O

46.

Which of these is an example of a Heterogeneous mixture:

a)

Tea with sugar

b)

oil and water

c)

NaCl

d)

H2O

47.

Which of these is an example of a Compound:

a)

Tea with sugar

b)

oil and water

c)

Gold

d)

H2O

48.

Which of these is an example of a Element:

a)

Tea with sugar

b)

oil and water

c)

Gold

d)

H2O

49.

Horseplay, practical jokes, or pranks in the classroom are

a)

not dangerous.

b)

okay if you are working alone.

c)

always against the rules.

d)

okay.

50.

Before you leave the science room, you should

a)

wash your hands with soap and water.

b)

return all equipmernt to the proper storage area.

c)

clean your work area and equipment.

d)

all of the above.

51.

Atoms of the same element that have different numbers of neutrons.

a)

Isotope

b)

Covalent Bond

c)

Enzymes

d)

Ionic Bonds

52.

A covalent bond is formed as a result of

a)

transferring electrons

b)

sharing electrons

c)

transferring protons

d)

sharing protons

53.
Organic compounds are compounds contain ______________.
a)
O
b)
C
c)
N
d)
S
54.
Which solution releases H+ in solution?
a)
Base
b)
Acid
c)
Buffer
d)
Water
55.

What is the number of protons that the element in this image contain?

a)

14

b)

7

c)

15

d)

18

56.
Which type of bond has one pair of electrons shared between atoms?
a)
ionic
b)
single covalent
c)
metallic
d)
double covalent
57.
Which is true of binary ionic compounds?
a)
They consist of only 2 atoms.
b)
They have bonds that share 2 valence electrons.
c)
They contain 2 different anions.
d)
They consist of atoms of only 2 element types.
58.
Which is the charge that results when oxygen becomes an ion?
a)
+3
b)
+2
c)
-2
d)
-3
59.
Which is the correct name for the compound FeS?
a)
iron (II) sulfide (II)
b)
iron (II) sulfide
c)
iron (I) sulfide
d)
iron sulfide
60.
Group 13 (3A) elements tend to most often acquire which charge when they form ions?
a)
-3
b)
+5
c)
+3
d)
-5
61.
Which category of elements have the property of being malleable and ductile?
a)
gases
b)
metals
c)
metalloids
d)
nonmetals
62.
Which is the most important characteristic in determining an element's chemical properties?
a)
the number of protons and neutrons in its nucleus
b)
which period it is found in
c)
the number of valence electrons it contains
d)
its outermost energy level
63.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
64.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
65.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
66.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
67.
If an atom has 3 electrons, how many protons does it have?
a)
1
b)
2
c)
4
d)
3
68.
Elements with similar properties
a)
Periods
b)
Groups
69.
Where are electrons?
a)
Nucleus
b)
Orbits
70.
On Periodic Table, how are elements ordered?
a)
color
b)
shape
c)
atomic number
d)
alphabetically
71.
A "group" is a ____________ on the periodic table.
a)
column
b)
row
72.
A "period" is a ____________ on the periodic table.
a)
column
b)
row
73.
How many elements are in the this compound?
H2CO4N5
a)
11
b)
4
c)
12
d)
5
74.
How many TOTAL atoms are in this compound?
H2C3O4N5
a)
5
b)
14
c)
15
d)
19
75.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
76.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
77.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
78.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
79.
What is the only substance with a neutral pH of 7?
a)
Milk
b)
Orange Juice
c)
Water
d)
Blood
80.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
81.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
82.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
83.

He created the Planetary Model of the atom

a)

Bohr

b)

Dalton

c)

Rutherford

d)

Thomson

84.

What will this atom do to become stable?

a)

Gain 3 e-

b)

Gain 5 e-

c)

Lose 3 e-

d)

Lose 5 e-

e)

Already stable

85.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
86.

What is the atomic mass of the atom pictured?

a)

9

b)

10

c)

18

d)

19

e)

28

87.

When there are more protons than electrons in an atom it is a...

a)

cation, positively charged

b)

dogion, positively charged

c)

anion, negatively charged

d)

uhion, negatively charged

e)

isotope, positively charged

88.

Assuming it is neutral, what element is this?

a)

Fluorine

b)

Helium

c)

Argon

d)

Oxygen

89.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
90.

What will this element do to become stable?

a)

Gain 7 e-

b)

Lose 1 e-

c)

Gain 1 e-

d)

Lose 3 e-

91.

What is this element?

a)

Helium

b)

Oxygen

c)

Sodium

d)

Phosphorous

92.

This element tends to _________________ and form a(n) ________________

a)

lose 4 e-; anion

b)

gain 4 e-; anion

c)

lose 2 e-; cation

d)

gain 2 e-; cation

e)

lose 4 e-; cation

93.
What is the volume in this buret?
a)
24.1mL
b)
24.3mL
c)
24.2L
d)
24.2mL
94.
More than two-thirds of the elements are classified as
a)
a. nonmetals
b)
b. metals
c)
c. metalloids
d)
d. noble gases
95.
The arrangement of the elements in the present Periodic Table is based on atomic
a)
a. mass
b)
b. number
c)
c. radius
d)
d. density
96.
Which list of elements contains two metalloids?
a)
a. Si, Ge, Po, Pb
b)
b. As, Bi, Br, Kr
c)
c. Si, P, S, Cl
d)
d. Po, Sb, I, Xe
97.
According to the Periodic Table, which element has more than one positive oxidation state (number)?
a)
a. cadmium
b)
b. iron
c)
c. silver
d)
d. zinc
98.
Which element has chemical properties that are most similar to the chemical properties of sodium?
a)
a. Mg
b)
b. K
c)
c. Se
d)
d. Cl
99.
What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons?
a)
a. 21
b)
b. 42
c)
c. 45
d)
d. 66
100.
Different isotopes of the same element must have a different 
a)
a. mass number
b)
b. atomic number
c)
c. number of protons
d)
d. number of electrons
101.

What does IUPAC stand for?

a)

International Union of Pure and Applied Chemistry

b)

International Union of Physical and Aphysical Chemistry

c)

International Union of Potassium and Arsenic Chemistry

d)

International Union of Your Mom

102.

Classify the following molecule.

a)

polar

b)

nonpolar

103.

Classify the following molecule.

a)

polar

b)

nonpolar

104.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

105.
F2
a)
Polar 
b)
Nonpolar 
106.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
107.

The attraction that an atom has for shared electrons in bonds is

a)

electron affinity.

b)

electronegativity.

c)

electropositivity.

d)

electromagnetism.

108.

Excluding the Noble gas family, where on the Periodic Table are the elements with the highest electronegativity located?

a)

upper right

b)

lower right

c)

upper left

d)

lower left

109.

Phosphorus has an electronegativity value of 2.1. Chlorine's electronegativity value is 3.0. What type of bond will these two elements form?

a)

ionic

b)

nonpolar covalent

c)

polar covalent

d)

metallic

110.

When two atoms of the same nonmetal element bond together, they form a(n)

a)

ionic bond.

b)

nonpolar covalent bond.

c)

polar covalent bond.

d)

James Bond.

111.

Which of the following pairs of elements is most likely to form an ionic bond? (You should refer to a Periodic table.)

a)

sulfur and oxygen

b)

sulfur and fluorine

c)

sodium and sulfur

d)

oxygen and fluorine

112.

In order to determine if a molecule is polar, you must consider the

a)

polarity of bonds and symmetry of the molecule.

b)

number of electrons and number of bonds.

c)

polarity of bonds only.

d)

total charge of each ion and number of multiple bonds.

113.

Why is it difficult to wash oil from your hands with plain water?

a)

Both substances are polar. Like polarities repel.

b)

Both substances are nonpolar. Like polarities repel.

c)

Water is nonpolar, and oil is polar, so they will not combine.

d)

Water is polar, and oil is nonpolar, so they will not combine.

114.

Which element has 5 electrons in its Lewis dot structure?

a)

Boron

b)

Carbon

c)

Phosphorus

d)

Sulfur

115.

When is a molecule polar?

a)

when it is asymmetrical with at least one polar bond

b)

it is asymmetrical

c)

it is symmetrical

d)

it is symmetrical with at least one polar bond

116.

This molecule has ______ bond and is a ______ molecule.

a)

polar, nonpolar

b)

nonpolar, nonpolar

c)

nonpolar, polar

d)

polar, polar

117.

This molecule has _____ bonds and is a _______ molecule.

a)

polar, nonpolar

b)

nonpolar, nonpolar

c)

nonpolar, polar

d)

polar, polar

118.

Carbon dioxide has polar bonds but is considered a nonpolar molecule. Why?

a)

it has an asymmetrical shape

b)

net dipole moment exists between the atoms of the molecule

c)

the bond polarity between C and O cancel

d)

C is considered slightly positive while O is slightly negative

119.

This is an example of a ____ bond.

a)

nonpolar covalent

b)

ionic

c)

polar covalent

d)

metallic

120.

Is H2S a polar or nonpolar molecule?

a)

polar

b)

nonpolar

121.

Why is the molecule nonpolar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

122.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

123.

KCl, potassium chloride, is used to stop the heart during open-heart surgery. What type of compound is it?

a)

ionic

b)

polar covalent

c)

nonpolar covalent

d)

metallic

124.

Bronze is an alloy of copper (Cu) with primarily tin (Sn) as the second most prevalent element. What type of bonding occurs in a sample of bronze?

a)

ionic

b)

polar covalent

c)

nonpolar covalent

d)

metallic

125.

Water is a polar covalent molecule. Which represents the correct assignment of dipoles for H2O? Remember: the tip of the arrow is the partial negative end and the bottom of the arrow (which looks like a plus sign) is the partial positive end.

a)
b)
c)
d)
126.

How many TOTAL resonance structures can exist for this molecule?

a)

1 total structures

b)

2 total structures

c)

3 total structures

d)

4 total structures

127.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
128.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
129.

Type of bond between Br & Br

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

130.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
131.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
132.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
133.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
134.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
135.

Binary acids start with "____________"

a)

acid

b)

nitric

c)

hydraulic

d)

hydro

136.

Always add the word "________" to the end when naming acids

a)

base

b)

hydro

c)

acid

d)

Baumstark

137.

When naming binary acids, the ending always changes to:

a)

-ate

b)

-ite

c)

-ic

d)

-ous

138.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

139.

When naming oxyacids, change "-ate" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

140.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
141.
Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide
142.

The cation in an acid is always

a)

a metal

b)

hydrogen

c)

hydroxide

d)

negatively charged

143.
Which has a pH below 7?
a)
Acid
b)
Base
144.

Who developed the modern periodic table?

a)

Bohr

b)

Einstein

c)

Newton

d)

Mendeleev

145.

The properties of element X are: MALLEABLE, DUCTILE, SHINY, CONDUCTS HEAT AND ELECTRICITY. Which represents the identity of element X?

a)

Carbon (C)

b)

Sulfur (S)

c)

Copper (Cu)

d)

Iodine (I)

146.

Which of these elements is most reactive?

a)

Sodium (Na)

b)

Carbon (C)

c)

Magnesium (Mg)

d)

Neon (Ne)

147.

A student finds that an unknown element readily reacts with alkali metals. Which is the best conclusion about the unknown element?

a)

it is an alkaline earth metal

b)

it is a noble gas

c)

it is in group 16

d)

it is in group 17

148.

The metals and nonmetals are divided by a "stair step." What are the elements called that are attached to the stair step?

a)

gases

b)

metals

c)

nonmetals

d)

metalloids

149.

Which explains why the alkali metals are the most reactive group in the periodic table?

a)

They are radioactive

b)

They have only one electron in their outer energy level

c)

They have complete outer energy levels

d)

They have the highest atomic masses of any elements

150.

A student created a table listing the properties of a sample of matter. Based on the table, the student collected data on a sample of which of the following types of matter?

a)

Vinegar

b)

Salt

c)

Iron Fillings

d)

Sand

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