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2024 Midterm Study Guide

Total questions: 203

Worksheet time: 51hrs 45mins

Name
Class
Date
1.
A testable prediction about a scientific investigation is a(n)
a)
Question
b)
Observation
c)
Hypothesis
d)
Experiment
2.
A series of steps used by scientists to solve a problem or answer a question. 
a)
scientific method
b)
recipe
c)
data collection
d)
metric system
3.

The information you collect while doing your experiment is called

a)

conclusions

b)

data

c)

hypotheses

d)

procedures

4.

The process of obtaining information by using the senses is called a/an

a)

Conclusion

b)

Observation

c)

Inquiry

d)

Scientific method

5.

Data gathered using the senses are referred to ___________.

a)

quantitative data

b)

logical data

c)

measured data

d)

qualitative data

6.

An explanation based on many repeated observations during experiments.

a)

conclusion

b)

scientific law

c)

theory

d)

hypothesis

7.

To make observations you use your _______.

a)

Feet

b)

Experience

c)

Senses

d)

Smile

8.

Performing a test or experiment allows you to test your ___________.

a)

Conclusions

b)

Hypothesis

c)

Data

d)

Question

9.
What is the first step in the scientific method?
a)
Ask a question
b)
Conclusion
c)
No Horse Play
d)
Observe
10.

Which of the following shows the correct sequence for the scientific method inquiry?

a)

Conclusion, Experimentation, Hypothesis, Observation

b)

Observation, Experimentation, Hypothesis, Conclusion

c)

Observation, Hypothesis, Experimentation, Conclusion

d)

Experimentation, Conclusion, Observation, Hypothesis

11.

Name this piece of equipment that is used to measure (but not precise), heat, and mix large amounts of liquids?

a)

beaker

b)

flask

c)

test tube

d)

graduated cylinder

12.

Name this piece of equipment that allows you to measure liquid's volume and measures in milliliters?

a)

test tube

b)

beaker

c)

flask

d)

graduated cylinder

13.

Name this piece of equipment that measures temperature in liquid or gas, and measures in degrees Celsius?

a)

hot plate

b)

beaker

c)

thermometer

d)

bunsen burner

14.

Name this piece of equipment that holds liquids and allows reactions in a small space?

a)

test tube

b)

hot plate

c)

dropper

d)

beaker

15.

Name this piece of equipment that heats objects with an open flame?

a)

hot plate

b)

thermometer

c)

bunsen burner

d)

beaker

16.

What is used to protect your eyes from chemicals, broken glass, and fire?

a)

Fire blanket

b)

Eye wash

c)

Goggles/Protective eye wear

d)

Flask

17.
What is used to hold test tubes?
a)
Test tube rack
b)
Magnifying glass
c)
Petri dish
d)
Funnel
18.

What is used to pick up items?

a)

Clamps

b)

Tongs

c)

Hand lens

d)

Pipette

19.

This is used to pour lab materials into an object with a small opening

a)

scoop

b)

funnel

c)

bunsen burner

d)

goggles

20.

This is used to hold test tubes

a)

test tube holder

b)

eye wash

c)

eye dropper

d)

lab apron

21.

This is used to protect your body and clothes during an experiment.

a)

test tube holder

b)

eye wash

c)

eye dropper

d)

lab apron

22.

This is used to put out a fire

a)

fire extinguisher

b)

thermometer

c)

beaker

d)

tongs

23.
Identify the equipment shown here:
a)
concave glass
b)
convex glass
c)
watch glass
d)
glass plate
24.

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

25.
Fooling around in the lab, throwing things, and doing unauthorized experiments are all:
a)
Not dangerous
b)
Great if you have time
c)
Always against the rules
d)
Ok every other Tuesday
26.

What is the volume?

a)

42 mL

b)

43 mL

c)

44 mL

d)

45 mL

27.

What is the volume?

a)

23 mL

b)

28 mL

c)

36 mL

d)

38 mL

28.

When reading the volume in a graduated cylinder, look at the ___ of the meniscus.

a)

top

b)

bottom

c)

It doesn't matter.

d)

What is a meniscus?

29.

This is used to safely mix chemicals

a)

Glass Stirring Rod

b)

Baseball Bat

c)

Test Tube

d)

Stir thingy

30.
Are made from a combination of 2 or more elements in a constant ratio...
a)
Atome
b)
Mixture
c)
Compounds
d)
Elements
31.
A combination that can be separated by physical processes is a .....
a)
Atom
b)
Compound
c)
Element
d)
Mixture
32.
What is a homogeneous mixture?
a)
a mixture that is the same throughout.
b)
a mixture that is made up of one type of atom.
c)
a mixture that is made up of one type of compound
d)
a mixture that cannot be separated through physical changes
33.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
34.
What type of mixture is this?
a)
homogenous mixture
b)
chemical
c)
heterogeneous mixture 
d)
solid mix
35.
Italian Salad Dressing is a . . .
a)
heterogeneous mixture
b)
homogeneous mixture
c)
Pure Substance
d)
Compound
36.
Chicken soup is an example of what kind of substance?
a)
homogenous mixture
b)
solution
c)
heterogeneous mixture
d)
compound
37.
Kool-Aid
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
38.
Carbon
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
39.
Aluminum
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
40.
Co
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
41.
O2
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
42.
NaCl
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
43.
This picture represents: 
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
44.

The ability to burn is known as---

a)

Flammability

b)

Combustion

c)

Density

d)

Exploding

45.

Mass divided by volume is the formula for calculating----

a)

Mass

b)

Volume

c)

Density

d)

Matter

46.

Reactivity (bubbling, fizzing) is a --- property.

a)

Chemical

b)

Physical

47.
Ice melting is an example of a
a)
physical change
b)
chemical change
c)
physical property
d)
chemical property
48.
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
49.
Which is an example of a chemical change?
a)
melting ice to make water
b)
baking cake batter to make a cake
c)
putting cheese on bread to make a cheese sandwich
d)
cutting an orange into slices for a snack
50.
Hammering wood together to build a playhouse
a)
Chemical change
b)
Physical change
51.
a copper penny turning greenish after a few years.
a)
Chemical Change
b)
Physical Change
52.
Burning a marshmallow over a campfire
a)
Physical
b)
Chemical
53.

______________________ can only be recognized when substances react or do not react chemically with one another.

a)

Physical properties

b)

Chemical properties

c)

Flammable properties

d)

Colorful properties

54.
Which is an example of a physical property?
a)
ability to react with acid
b)
 state of matter
c)
flammability
d)
ability to react with oxygen
55.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
rust
56.
How would you write 4.3756 x 104 in standard form?
a)
437,560,000
b)
0.00043756
c)
43,756
d)
4,3756
57.
How would you write 0.0005 in scientific notation?
a)

50 E5

b)

5 E-4

c)

5 E3

d)

.5 E-3

58.
How would you write -5.6 x 10-3 in standard form?
a)
0.0056
b)
-5,600
c)
0.00056
d)
-0.0056
59.
Scientific Notation is made up of two number parts. The first part should be a number between 1 and 100.
a)
True
b)
False
60.
Scientific Notation is made up of two number parts. The second part is a power of base 10.
a)
True
b)
False
61.
When writing a number in scientific notation, the first number must be greater than 1, but less than 10.
a)
False
b)
True
62.
The rule of scientific notation is to write all exponents with a base of ____.
a)
50
b)
5
c)
100
d)
10
63.
How do you write
1001
in scientific notation?
a)
1.0001 x 104
b)
1.01 x 105
c)
1.001 x 103
d)
10.1 x 103
64.
How do you write
8.317 x 106
in standard form?
a)
8, 371, 000
b)
83, 170, 000
c)
837, 100
d)
8, 317, 000
65.
Which of the following is correct scientific notation?
a)
20.35 x 104
b)
.2035 x 104
c)
2035 4
d)
2.035 x104
66.
Express the following in scientific notation:
.000457
a)
457 x 106
b)
457 x 10-6
c)
4.57 x104
d)
4.57 x 10-4
67.
Express the following in standard notation:
8.025 x 10-8
a)
.00000008025
b)
.000000008025
c)
802,500,000,000
d)
80,250,000,000
68.
Express the following in scientific notation:
10,030,400,000
a)
1.00304 x 109
b)
1.00304 x 1010
c)
1.00403 x 1010
d)
1.00304 x10-10
69.

How many significant figures are in the number 0.00450?

a)

2

b)

3

c)

4

d)

5

70.

Identify the number of significant figures in the measurement 123.45.

a)

3

b)

4

c)

5

d)

6

71.

What is the result of adding 12.11 and 0.034 with the correct number of significant figures?

a)

12.144

b)

12.14

c)

12.1

d)

12.145

72.

Subtract 45.6 from 123.45 and express the answer with the correct number of significant figures.

a)

77.85

b)

77.9

c)

77.8

d)

77.850

73.

Multiply 6.022 by 0.10 and express the answer with the correct number of significant figures.

a)

0.6022

b)

0.60

c)

0.6

d)

0.602

74.

Divide 123.4 by 2.0 and express the answer with the correct number of significant figures.

a)

62

b)

61.7

c)

61.70

d)

61.8

75.

Round 123.456 to four significant figures.

a)

123.4

b)

123.5

c)

123.45

d)

123.46

76.

A measurement is recorded as 0.00340 m. How many significant figures does this measurement have?

a)

2

b)

3

c)

4

d)

5

77.

If you add 1.234 and 0.0567, what is the result with the correct number of significant figures?

a)

1.2907

b)

1.291

c)

1.29

d)

1.3

78.

What is the result of multiplying 2.34 by 0.56 with the correct number of significant figures?

a)

1.3104

b)

1.31

c)

1.3

d)

1.310

79.

Round the number 987.654 to three significant figures.

a)

988

b)

987.7

c)

987.65

d)

987.6

80.

How many significant figures?

76490

a)

3

b)

4

c)

5

d)

6

81.

What is 7.555 rounded to two significant figures?

a)

7.6

b)

7.5

c)

70

d)

76

e)

7.60

82.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
83.
Round 7256.320004 to 8 significant figures.
a)
7256.3200
b)
7256.0000
c)
72563200
d)
72560000
84.

Convert 565,900 seconds into days.

a)

4.5 days

b)

5.5 days

c)

6.5 days

d)

7.5 days

85.

How many minutes are in a school year, 190 days?

a)

269,000 minutes

b)

11,400 minutes

c)

16,156 minutes

d)

273,600 minutes

86.

Convert 43 miles into feet.

a)

123,000 feet

b)

200,000 feet

c)

250,260 feet

d)

227,040 feet

87.

Convert 1,800 grams to kilograms.

a)

18 kilograms

b)

1.8 kilograms

c)

180 kilograms

d)

0.18 kilograms

88.

Convert 1.07 meters to centimeters.

a)

107 centimeters

b)

17 centimeters

c)

1070 centimeters

d)

1007 centimeters

89.

What were John Dalton two contributions to atomic history?

a)

Created the atomic theory

b)

Discovered that the atom is mostly empty space

c)

Believed that atoms cannot be rearranged during chemical reactions

d)

Hypothesized that the atom is a tiny, hard sphere

e)

Discovered the electron

90.

What subatomic particles make up the nucleus of an atom?

a)

electrons

b)

protons

c)

neutrons

d)

leptons

e)

mesons

91.
Discovered that the atom has a small, dense, positively charged nucleus.
a)
Ernest Rutherford
b)
Heisenberg
c)
Democritus
d)
JJ Thomson
92.

Who was the first to propose that matter consist of indivisible particle of matter called atoms?

a)

John Dalton

b)

Aristotle

c)

Democritus

d)

Plato

93.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)

nucleus

b)

Neutron

c)

Electron

d)

Orbitals

94.

Which of the following is the best analogy for Thomson's model of the atom?

a)

marble

b)

plum pudding

c)

solar system

d)

ripple in water standing still

95.

Ultimately, Schrodinger's model had electrons in ______ around the nucleus

a)

Specific orbits

b)

Nodes

c)

Waves

d)

Clouds

96.
Ernest Rutherford discovered that atoms were mostly _________________. 
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space. 
97.

The Bohr ( Neils Bohr) model is the first atomic model to describe electron shells. What does this mean?

a)

Calcium carbonate exoskeletons to protect the electrons from predators

b)

Special places the electron can be without the nucleus interfering

c)

Levels and paths that the electrons travel around when they orbit the nucleus

d)

Quantum spin probabilities which account for electron momentum

98.

Is it possible to find the velocity and position of a moving particle at the same time

a)

no

b)

yes

c)

sometimes

d)

none of the above

99.

What are the three particles that make up the atom?

a)

protons, neutrons and isotopes

b)

protons, negatives and electrons

c)

neutrons, isotopes and electrons

d)

protons, neutrons and electrons

100.

The positive particles of an atom are

a)

electrons

b)

neutrons

c)

nucleus

d)

protons

101.

Electrons have this type of charge

a)

negative

b)

neutral (no charge)

c)

positive

102.

What does the nucleus of an atom contain?

a)

Electrons and neutrons

b)

Protons and neutrons

c)

Electrons and protons

d)

Neutrons and electrons

103.

An element with 6 electrons has:

a)

6 electron shells

b)

4 valence electrons

c)

6 valence electrons

d)

2 valence electrons

104.

One of the differences between the isotopes and regular atom is

a)

They have different number of protons

b)

They have different number of electrons

c)

They have different number of neutrons

105.
What is the atomic number of the atom pictured? 
a)
11
b)
12
c)
22
d)
23
106.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
107.
What number indicates an electron?
a)
1
b)
2
c)
3
d)
4
108.

What happens to an atom that gains an electron?

a)

It becomes a cation.

b)

It remains neutral.

c)

It becomes an anion.

d)

It loses a proton.

109.

What is a positively charged ion called?

a)

Anion

b)

Cation

c)

Neutral atom

d)

Isotope

110.

Why does an atom become a cation?

a)

It gains protons.

b)

It loses electrons.

c)

It gains electrons.

d)

It loses protons.

111.

What is an atom described as in the text?

a)

The smallest particle that can exist independently

b)

The largest unit of matter

c)

A type of molecule

d)

A compound

112.

What is the charge of a neutron?

a)

Positive

b)

Negative

c)

No charge

d)

Variable charge

113.

What can electrons do that protons and neutrons cannot?

a)

Orbit the nucleus

b)

Be shared with other atoms to form chemical bonds

c)

Exist in the nucleus

d)

Have a positive charge

114.

What does the atomic number of an element tell us?

a)

The number of neutrons in one atom of that element

b)

The number of electrons in one atom of that element

c)

The number of protons in one atom of that element

d)

The total number of subatomic particles in one atom of that element

115.

What are materials called that are composed of two or more elements?

a)

Mixtures

b)

Alloys

c)

Compounds

d)

Solutions

116.

Which of the following statements is true according to the text?

a)

Every element has a different number of electrons.

b)

No two elements have the same atomic number.

c)

All elements have been created by humans.

d)

The periodic table does not include noble gases.

117.

What is an atom with an equal number of electrons and protons called?

a)

Anion

b)

Cation

c)

Neutral atom

d)

Isotope

118.

What charge does an anion carry?

a)

Positive

b)

Negative

c)

Neutral

d)

Variable

119.

According to the law of charges, what happens when two like charges come into contact?

a)

They attract each other

b)

They repel each other

c)

They cancel each other out

d)

They create a new charge

120.

What is a valence electron?

a)

An electron in the innermost shell of an atom

b)

An electron that is free from the atomic structure

c)

An outer shell electron of an atom that can form a chemical bond with another atom

d)

A positively charged particle within the nucleus

121.

Where do electrons form orbits, or shells, in an atom?

a)

Around the atom's core

b)

Around the atom's nucleus

c)

Within the atom's protons

d)

Outside the atom's electron cloud

122.

99.9% of the atom's mass is located in the

a)

electrons

b)

nucleus

c)

protons

d)

neutrons

123.

Carbon atomic number is 6. This means that an carbon atom must have

a)

6 electrons

b)

6 protons

c)

6 electrons and protons

d)

6 neutrons

124.

Which element has a (rounded) atomic mass of 45?

a)

Rhodium (Rh)

b)

Scandium (Sc)

c)

Titanium (Ti)

d)

Calcium (Ca)

125.

Which element has an atomic number of 33?

a)

Arsenic (As)

b)

Sulfur (S)

c)

Chlorine (Cl)

d)

Selenium (Se)

126.

How many neutrons does Gallium (Ga) have?

a)

31

b)

70

c)

39

d)

Answer cannot be determined.

127.

How many electron shells does Krypton (Kr) have?

a)

4

b)

8

c)

2

d)

Not enough information to determine.

128.

Which element has 3 electrons shells and 2 electrons in the outermost shell?

a)

Magnesium

b)

Boron

c)

Sodium

d)

Aluminum

129.

Which of the following is MOST reactive?

a)

Nitrogen

b)

Silicon

c)

Lithium

d)

Argon

130.

To be stable, what number of electrons do most elements want in their outermost shell?

a)

2

b)

4

c)

6

d)

8

131.

To determine the atomic mass you add what two subatomic particles:

Choose the 2 that apply.

a)

Protons

b)

Electrons

c)

Neutrons

d)

Atoms

e)

Elements

132.

Which of these elements is a Alkali Metal and has 4 electrons in its outermost shell?

a)

Potassium

b)

Silicon

c)

Calcium

d)

Answer not possible.

133.

What element is a Noble Gas with 2 electron shells?

a)

Neon

b)

Argon

c)

Lithium

d)

Answer not possible.

134.

Which element has 2 electron shells and 4 electrons in the outermost shell?

a)

Carbon

b)

Calcium

c)

Nitrogen

d)

Bromine

135.

What is the atomic symbol for Sulfur?

a)

S

b)

Su

c)

Se

d)

Sl

136.

What is the symbol for potassium?

a)

P

b)

Po

c)

K

d)

Answer not given

137.

What does the group number tell you?

a)

Number of electron shells

b)

Number of electrons in the outermost shell

c)

Number of protons

d)

Number of neutrons

138.

What does the period number tell you?

a)

Number of electron shells

b)

Number of electrons in the outermost shell

c)

Number of protons

d)

Number of neutrons

139.

What do all the alkaline earth metals have in common?

a)

They all have the same amount of electron shells.

b)

They all have the same amount of electrons in their outermost shell.

c)

They all have the same atomic number

d)

None of the above

140.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
141.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
142.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
143.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
144.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
145.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
146.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
147.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
148.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
149.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
150.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
151.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
152.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
153.

When an atom becomes charged, it is referred to as __

a)

an element

b)

an ion

c)

a neutral atom

154.

Which of the following list of ions represent the correct charge for each element?

a)

Na1+ , Ca2+, Al3+

b)

O-1, F!+, Na1+

c)

He2+,Na2+,F2+

155.

Which of the following contains only nonmetals ?

a)

H, O, Na, Rb

b)

H, Cl, O, N

c)

H, C, K,, Rb

d)

none of the selections have nonmetals

156.

Which of the following list of metalloids is in period 3?

a)

Silicon

b)

Germanium

c)

Astatine

d)

Tellurium

157.

Why does ionization energy increase across a period?

a)

The increasing nuclear charge in the atom allows it to hold on more tight to its electrons so it takes more energy to remove them

b)

nuclear charge stays the same going across a period

c)

electrons gain more energy across a period

158.

Which of the following statements describes why Fluorine is the most electronegative element on the periodic table?

a)

The small Fluorine atom with its strong nuclear easily attracts 1 more electron to its nucleus

b)

Fluorine's valence electrons sit far away from the nucleus thus making it a large strong atom

c)

Fluorine gives up all 7 valence electrons with ease

159.

Helium, atomic #2, has how many energy levels?

a)

two

b)

one

c)

an infinite number

160.

As electrons are added around the nucleus of an atom the nuclear charge becomes less effective, thus making the amount of energy it takes to remove electrons from an atom decrease down a group. This is known as _____

a)

electronegativity

b)

the shielding effect

c)

electron affinity

161.

In terms of electron configurations and shielding, why do atoms get smaller as you move across a period?

a)

The electrons become smaller

b)

the protons become smaller

c)

the nuclear charge increases as protons are added but electron energy stays the same as they accumulate in the same energy level.

162.

Which of the following statements represent ion formation?

a)

metals form positive ions as they lose valence electrons and nonmetals form negative ions as they gain electrons to their valence shell

b)

metals form positive ions as they gain valence electrons and nonmetals form negative ions as they lose electrons to their valence shell

c)

an ion has the same number of electrons as protons

163.

Elements in the same Group share similar properties because_______

a)

they have the same atomic number

b)

they have the same energy shells

c)

they have the same number of valence electrons

d)

they are the same color

164.

Noble gases share this property.

a)

are solid at room temperature

b)

very reactive

c)

not reactive

165.

The ability of an atom to attract electrons toward their nucleus is referred to as___

a)

ionization energy

b)

electronegativity

c)

periodicity

166.

The electron configuration of an atom is 1s22s22p6.  The total number of electrons in the atom is 

a)
3
b)
6
c)
8
d)
10
167.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
d)

1s2 2s2 2p6 3s2 3p2

168.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
169.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
170.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)

1s22s22p4

c)
1s22s22p6
d)
1s22s22p63s23p6
171.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
172.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
173.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
174.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
175.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
176.

Typically, atoms are more stable when they are

a)

bonded together

b)

apart from each other

177.

Why do atoms bond?

a)

They typically don't bond

b)

To add or take away energy levels

c)

To have a full valance shell.

d)

To have a full inner shell

178.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

179.

Covalent bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

It depends on the situation

180.

Which bond does this picture best represent?

a)

Metallic bond

b)

ionic bond

c)

covalent bond

d)

James Bond

181.

What do positive ions tend to do?

a)

lose electrons

b)

gain electrons

c)

lose protons

d)

gain protons

182.

What happens when magnesium loses 2 electrons?

a)

It stabilizes to a net charge of 0

b)

It turns into an atom

c)

It becomes negatively charged

d)

It becomes positively charged

183.

Predict the bond between Mg and Cl

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

184.

Which is the correct Lewis Structure for oxygen?

a)
b)
c)
d)
185.

What is the correct Lewis structure for BF3?

a)
b)
c)
d)

BF3 (The formula is the Lewis Structure)

186.

What category of element usually forms a positive ion?

a)

Metals

b)

Nonmetals

c)

metalloids

d)

Noble gases

187.

Which category of elements usually form negative ions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

188.

CaCl2 is an example of what type of bond?

a)

Covalent

b)

Metallic

c)

Ionic

189.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
190.
If a you saw the following, K+; what does it tell you about the  the ion.
a)
it has lost one electron 
b)
it has lost one proton 
c)
it has lost two electrons 
d)
it is a negative ion 
191.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
192.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
193.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
194.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
195.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
196.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
197.

Is this the correct structure for CH2O?

a)

Yes

b)

No

198.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
199.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
200.
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
201.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
202.

By replacing the element symbol, this could be a diagram of which element?

a)

Li

b)

Al

c)

C

d)

Be

203.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

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