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Chem 1 Semester 1 Review

Total questions: 120

Worksheet time: 2hrs 21mins

Name
Class
Date
1.
How many elements are represented in the compound, Na2CO3 ?
a)
1
b)
2
c)
3
d)
4
2.
Which of the following are examples of elements?
a)
NaCl, O, CO2
b)
C, Au, Ag, Al
c)
Hg, Al, LiF
d)
Salt, Water, Steel
3.
How many protons does this element have?
a)
40
b)
21
c)
20
d)
41
4.

Which of the following has 5 valance electrons?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

e)

fluorine

5.

What is the formula for the ionic compound formed between magnesium and iodine?

a)

MgI2

b)

MgI

c)

Mg2I

d)

Mg2I2

6.

What is the charge of a calcium ion?

a)

+1

b)

+2

c)

+/-4

d)

-1

7.

What is the formula for the ionic compound formed between potassium and sulfur?

a)

K2S

b)

KS

c)

KS2

d)

K2S2

8.

The periodic table is mostly made up of

a)

Metalloids

b)

Nonmetals

c)

Metals

d)

Liquids

9.

Which of the following has two valence electrons in its outer shell?

a)

Na

b)

Mg

c)

Al

d)

P

10.

In the modern periodic table, how are the elements ordered?

a)

Based on when they were discovered

b)

According to decreasing atomic mass

c)

According to increasing atomic number

d)

According to Mendeleev's original design

11.

What element is in period 5 group 12

a)

Cd

b)

Zn

c)

Hg

d)

Au

12.

Which type of element is malleable, can be molded into thin wires, and is a good conductor of electricity?

a)

Nonmetal

b)

Metal

c)

Metalloid

d)

Plasma

13.

An example of a chemical change is the:

a)

Crushing of stone

b)

Burning of gasoline

c)

Formation of clouds

d)

Separation of cream from milk

14.

Which state of matter has fixed (definite) volume but not fixed (indefinite) shape?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

15.

The melting of copper is classified as a physical change because it:

a)

Produced no new substances

b)

Absorbs heat

c)

Transfers energy

d)

Changes the chemical properties of copper

16.

Sugar dissolves completely in water to form a solution. This solution is a(n):

a)

A heterogeneous compound

b)

A heterogeneous mixture

c)

A homogeneous compound

d)

A homogeneous mixture

17.

What happens when an atom forms an ion?

a)

Protons have been gained or lost

b)

Neutrons have been gained or lost

c)

Electrons have been gained or lost

d)

The nucleus changes its composition

18.

What is the subatomic particle called that has about the same mass as a proton, but has no electrical charge?

a)

Ion

b)

Isotope

c)

Neutron

d)

Electron

19.

The chemical bond formed when two atoms share one or more pairs of electrons is a(n)…

a)

Covalent Bond

b)

Ionic Bond

c)

Orbital Bond

d)

Polar Bond

20.

The correct Lewis sctructure for the oxygen atom has…

a)

4 valence electrons

b)

5 valence electrons

c)

6 valence electrons

d)

7 valence electrons

21.
Data that describes the physical characteristics of a substance is
a)
Qualitative data
b)
Quantitative data
22.
Matter is:
a)
Something that has mass
b)
Something that has a definite composition
c)
A chemical
d)
A substance
23.
Convert 20.14 into scientific notation.
a)
2.014 x 101
b)
20.14 x 100
c)
2.014 x 10-1
d)
201.4 x 10-1
24.
Made of nonmetals that are covalently bonded
a)
Compound
b)
Molecule
c)
Mixture
d)
Alloy
25.
Has a fixed volume and shape; is rigid
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
26.
Has no fixed volume or shape, fills entire container uniformly
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
27.
How many neutrons does a Carbon-13 atom have?
a)
7
b)
6
c)
5
d)
4
28.
[Ar]4s23d8
a)
Ni
b)
Cu
c)
Pd
d)
Does not exist
29.
Which of the following is a Noble gas?
a)
Rn
b)
Cd
c)
Sr
d)
Lu
30.
Cobalt (Co) and silver (Ag) are _________ based on their locations in the periodic table.
a)
Inner transition elements
b)
Transition elements
c)
Alkali metals
d)
Alkaline earth metals
31.
Energy needed to remove an  electron from an atom is called 
a)
Electronegativity
b)
Shielding Effect
c)
Ionization Energy
d)
Atomic Radius
32.
All of the elements in group 17 have _____.
a)
the same number of valence electrons
b)
a different number of valence electrons
c)
varied numbers of valence electrons
d)
no valence electrons
33.
The scientist that first developed the basic pattern of the periodic table was _____.
a)
Lavoisier
b)
Davy
c)
Mendeleev
d)
Moseley
34.

The atomic number of oxygen, 8, indicates that there are eight

a)

protons in the nucleus of an oxygen atom.

b)

oxygen nuclides.

c)

neutrons outside the oxygen atom's nucleus.

d)

energy levels in the oxygen atom's nucleus.

35.

The total number of protons and neutrons in the nucleus of an atom is its

a)

atomic number.

b)

Avogadro number.

c)

mass number.

d)

average atomic mass.

36.

The atomic mass of an element listed in the periodic table is the

a)

average atomic mass.

b)

relative atomic mass of the most abundant isotope.

c)

relative atomic mass of the most abundant radioactive isotope.

d)

mass number of the least abundant isotope.

37.

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is

a)

13.

b)

14.

c)

27.

d)

40.

38.

Which 2 subatomic particles are found in the nucleus of an atom?

a)

Proton and electron

b)

Proton and neutron

39.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
40.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
41.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
42.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
43.

What is the correct Lewis structure for NH3?

a)
b)
c)
d)
44.

Which is the correct Lewis structure for carbon dioxide?

a)
b)
c)
d)
45.

Metals make _____ ions.

a)

positive

b)

negative

c)

neutral

46.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
47.

Nonmetals will make _____ions.

a)

positive

b)

negative

c)

neutral

48.

Why is this Lewis Structure incorrect? Select all that apply.

a)

There should be a single bond between H and C.

b)

There should be a triple bond between C and N.

c)

Carbon has too many bonds around it.

d)

Hydrogen needs more electrons.

49.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

50.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
51.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

52.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
53.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
54.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

55.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

56.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

57.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

58.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

59.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
60.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

61.

Elements with the electron configuration ending in p4 are in which group on the periodic table?

a)

4

b)

14

c)

16

d)

18

62.

According to the Law of Conservation of Mass, in any chemical change

a)

the mass of reactants is less than the mass of products

b)

the mass of reactants is greater than the mass of products

c)

the masses of products and reactants have no predictable relationship

d)

the mass of reactants is equal to the mass of products

63.

Which scientist used the gold foil experiment?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Chadwick

64.

What is the formula for the ionic compound formed between aluminum and chlorine?

a)

AlCl3

b)

Al2Cl3

c)

Al3Cl

d)

AlCl

65.

What is the independent variable in the Alka Seltzer experiment?

a)

Temperature

b)

Room Pressure

c)

Volume of Vinegar

d)

Number of Alka Seltzer Tablets

66.

What is the dependent variable in the Alka-Seltzer experiment?

a)

final temperature

b)

room pressure

c)

volume of vinegar

d)

number of Alka Seltzer tablets

67.

The mass of a 5.00 cm3 sample of gold is 96.5g. Calculate its density.

a)

0.0518 g/cm3

b)

19.3 g/cm3

c)

101.5 g/cm3

d)

483 g/cm3

68.

A chemical change occurs when

a)

dissolved minerals solidify to form a crystal.

b)

ethanol is purified through distillation.

c)

salt deposits form from evaporated seawater.

d)

a steel bridge rusts.

69.

Argon, krypton, and xenon are

a)

alkaline earth metals

b)

noble gases

c)

actinides

d)

lanthanides

70.

According to Dalton’s atomic theory,

a)

Different elements combine in simple whole-number ratios to form compounds.

b)

atoms are mostly empty space

c)

​an electron carries a negative change

d)

can be destroyed in chemical reactions.

71.

How do you measure the volume using a graduated cylinder?

a)

Measurements must be taken from the top of the meniscus and at eye level

b)

Measurements must be taken by looking from above the cylinder

c)

Measurements must be taken by looking from below the cylinder

d)

Measurements must be taken from the bottom of the meniscus and at eye level

72.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
73.
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
74.

How do we solve for mass if we know density and volume?

a)

Mass = Density / Volume

b)

Mass = Volume / Density

c)

Mass = Density x Volume

d)

Cannot solve for mass

75.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
76.

Accuracy means

a)

the measurements are close to each other

b)

the measurement is close to the true value

c)

the measurements are close to each other

d)

the measurements are close to each other and the true value.

77.

What is the name of J.J. Thomson's Model of an Atom?

a)

Jimmy Neutron Model

b)

Solar System Model

c)

Plum-Pudding Model

d)

Quantum mechanical Model

78.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
79.

what part of the atom tells you what element it is?

a)

Protons

b)

nuetrons

c)

electrons

d)

electron cloud

80.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

81.

How many electrons can the p sublevel hold?

a)
8
b)

6

c)
2
d)
4
82.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
83.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
84.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
85.

What is a cation's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element

86.

What is an anion's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element's charge

87.

If an atom gains electrons, the charge will be positive.

a)

true

b)

false

88.

Which of the following colors of light have the highest energy

a)

red

b)

orange

c)

green

d)

violet

89.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
90.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
91.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There are too many electrons in the 1s orbital

c)

In the 2p boxes, there should only be 1 electron in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up

92.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
93.

____________ is the tendency for an atom of an element to attract the electrons of another element when they are chemically combined.

a)

Electronegativity

b)

Atomic Radius

c)

Ionization Energy

94.
Carbon dioxide (CO2) contains how many atoms of oxygen?
a)
0
b)
1
c)
2
d)
3
95.

A substance that is made up of only one kind of atom is a(n)

a)

compound

b)

homogeneous mixtures

c)

element

d)

solution

96.

Convert 2.5 centimeters ot kilometers

a)

2.5 x 105 km

b)

2500 km

c)

2.5 x 10-5 km

d)

250 km

97.

Vertical columns on the periodic table are called...

a)

periods

b)

groups/famiilies

c)

classes

d)

there is no name for vertical columns

98.

Which element has 16 protons?

a)

oxygen

b)

sulfur

c)

nitrogen

d)

potassium

99.

Identify the correct scientific notation for 0.00061

a)

6.1 x 104

b)

.61 x 10-3

c)

6.1 x 10-4

d)

6.1 x 10-5

100.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
101.
How many significant figures does the following number have: 100.3
a)
4
b)
3
c)
5
d)
2
102.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
103.
Calculate 7.987 m - 0.54 m and give your answer with the correct number of significant figures.
a)
7.45 m
b)
7.447 m
c)
7.4 m
d)
7.5 m
104.
Solve and give your answer with the correct number of significant figures
(12.470)(271)
a)
3366.9
b)
3.37x103
c)
3400
d)
3370
105.

What equipment allows you to measure liquid's volume and measures in milliliters?

a)

test tube

b)

beaker

c)

flask

d)

graduated cylinder

106.

Which equipment heats objects with an open flame?

a)

hot plate

b)

thermometer

c)

bunsen burner

d)

beaker

107.

When is it OK to eat or drink at the lab tables?

a)

Always

b)

Only during group work, not during labs

c)

Never

d)

Whenever I'm hungry

108.

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.

109.

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.

110.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
111.

If you shake oil and water until little oil droplets are mixed throughout, what will happen if you let it sit for a while?

a)

The oil and water will be separated again.

b)

The oil and water will continue to bond.

c)

The oil and water will not move.

112.

Molecules that stick to the same type of molecules.

a)

cohesion

b)

adhesion

c)

hydrophilic

d)

hydrophobic

113.

Oil and water don't mix because oil is

a)

hydrophilic

b)

hydrophobic

c)

an emulsifier

d)

a buffer

114.
The tightness across the surface of water that enables paper clips to float is ____________.
a)
adhesion
b)
capillary action
c)
surface tension
d)
polarity
115.
Which statement explains why water molecules stick together?
a)
both sides are negative
b)
one side has a positive charge and the other side has a negative charge
c)
one side has a negative charge adn the other side has a neutral charge
d)
both sides are positive
116.

Which property of water allows water to climb up a tree's root system to the leaves?

a)

Cohesion

b)

Adhesion

c)

Polarity

d)

Capillary Action

117.
You know that 12 inches = 1 foot.  Convert 60 inches to feet.
a)
720 feet
b)
5 feet
c)
5 inches
d)
72 feet
118.

If a person weighs 125.0 lbs, how many milligrams do they weigh?

a)

56,700,000 mg

b)

56,818,181 mg

c)

56, 820 mg

d)

56, 818 mg

119.

How do you calculate the number of neutrons? *

a)

Mass = Atomic number - Neutrons

b)

Mass - Atomic number = Neutrons

c)

Atomic number = Neutrons

120.
Group  15 elements form what type of charge?
a)
-1
b)
-3
c)
+3
d)
15

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