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End of Year Review

Total questions: 150

Worksheet time: 4hrs 42mins

Name
Class
Date
1.

What theory explains how chemical reactions occur and why rates differ for different reactions?

a)

Thermochemical equation

b)

Collision Theory

c)

Gibbs Free Energy

d)

Entropy

2.

What is the energy transferred between objects due to a temperature difference?

a)

Internal energy

b)

Heat

c)

Entropy

d)

Enthalpy

3.

The First Law of Thermodynamics states...

a)

energy can't be created or destroyed.

b)

energy is always created.

c)

energy is always destroyed.

4.

The Second Law of Thermodynamics states...

a)

whenever there is an opportunity for energy dispersal, the energy spreads out.

b)

the energy disappears.

c)

the energy stays in place.

5.

Entropy is....

a)

a measure of energy dispersal, "chaos".

b)

when the energy disappears.

c)

when the energy is created.

6.

Three substances are added to a mug to make coffee: the coffee, which is 65°C65\degree C , the milk, which is 65°C65\degree C , and the sugar, which is in thermal equilibrium with the coffee. Describe the thermal state of the sugar.

a)

Heat will be transferred from the sugar to the coffee to reach equilibrium.

b)

Heat will be transferred from the coffee to the sugar to reach equilibrium.

c)

The sugar is 65°C65\degree C , based on the second law of thermodynamics

d)

The sugar is in equilibrium with the milk, based on the zeroth law of thermodynamics.

7.

The _____ Law of Thermodynamics says that heat always flows from an object with a higher temperature to an object of lower temperature naturally

a)

1st law of thermodynamics

b)

2nd law of thermodynamics

c)

3rd law of thermodynamics

d)

Zeroth Law

8.

The _____ Law of Thermodynamics says that heat always flows from an object with a higher temperature to an object of lower temperature naturally

a)

1st law of thermodynamics

b)

2nd law of thermodynamics

c)

3rd law of thermodynamics

d)

Zeroth Law

9.

the law of conservation of energy is the bases of...

a)

1st law of thermodynamics

b)

2nd law of thermodynamics

c)

3rd law of thermodynamics

d)

Zeroth Law

10.

What do we call the relationship between thermal energy, heat and work?

4 lines
11.

states that if the mechanical energy of a system is constant, the increase in the thermal energy of the system equal the sum of the thermal energy transferred into the system and the work done on the system

a)

1st Law of Thermodynamics

b)

2nd law of thermodynamics

c)

thermodynamics

d)

thermal insulator

e)

law of heat

12.

energy that is transferred between objects due to  temperature difference between those objects.

a)

temperature

b)

thermal energy

c)

heat

d)

solar collector

e)

convection

13.

states that energy spontaneously spreads from higher concentrations to regions of lower concentrations.

a)

1st Law of Thermodynamics

b)

2nd law of thermodynamics

c)

themal insulator

d)

heat engine

e)

thermodynamics

14.

device that converts some thermal energy into mechanical energy.

a)

thermal insulator

b)

heat engine

c)

enegine

d)

internal combustion engine

e)

solar collector

15.

A steady force pushes in the piston
of a well-insulated cylinder. In this
process, the temperature of the gas

a)

Increases

b)

Stays the same

c)

Decreases

d)

Not enough info

16.

The temperature of a glass of cold water will eventually...

a)

Match the temperature of the surrounding environment.

b)

Always be colder than the surrounding environment.

c)

Become warmer than the surrounding environment.

d)

Never change temperature.

17.

Which law of thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another?

a)

1st Law of Thermodynamics

b)

2nd Law of Thermodynamics

c)

3rd Law of Thermodynamics

d)

Zeroth Law of Thermodynamics

18.

What is the primary implication of the second law of thermodynamics in terms of entropy?

a)

Entropy of an isolated system always decreases

b)

Entropy of an isolated system always increases

c)

Entropy remains constant

d)

Entropy is irrelevant

19.

In a heat engine, which law of thermodynamics is primarily applied to determine the efficiency of the engine?

a)

1st Law of Thermodynamics

b)

2nd Law of Thermodynamics

c)

3rd Law of Thermodynamics

d)

Zeroth Law of Thermodynamics

20.

Which law of thermodynamics is often associated with the concept of absolute zero temperature?

a)

1st Law of Thermodynamics

b)

2nd Law of Thermodynamics

c)

3rd Law of Thermodynamics

d)

Zeroth Law of Thermodynamics

21.

The zeroth law of thermodynamics is fundamental in defining which of the following concepts?

a)

Temperature

b)

Heat

c)

Work

d)

Energy

22.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
23.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

24.

A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true?

a)

It is an exothermic reaction

b)

It is an endothermic reaction

25.
Have you ever eaten sherbet sweets candy? They fizz in your mouth and your tongue feels cold. Why do you think that is?
a)
It is an exothermic reaction
b)
It is an endothermic reaction
c)
It is made of ice
d)
It is dissolving your mouth
26.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Kinetic

d)

Potential

27.

When a substance changes from a solid to a liquid, the particles move

a)

Faster

b)

Slower

28.

When a substance changes from a solid to a liquid, it is an

a)

Exothermic Change

b)

Endothermic Change

29.

Organize these options into the correct types of energy use.

Categorize the following

absorbs energy

releases energy

splitting a molecule

forming a molecule

melting ice

NH4NO3 (s) + H2O(l) + 23.8 kJ → NH4OH(aq) + HNO3NH_4NO_3\ \left(s\right)\ +\ H_2O\left(l\right)\ +\ 23.8\ kJ\ \rightarrow\ NH_4OH\left(aq\right)\ +\ HNO_3  

6SOCl2 + CoCl2⋅6H2O → CoCl2 + 6SO2 + 12HCl    ΔH=+6SOCl_2\ +\ CoCl_2\cdot6H_2O\ \rightarrow\ CoCl_2\ +\ 6SO_2\ +\ 12HCl\ \ \ \ \Delta H=+  

H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + H2O (l)   ΔH = −H_2SO_4\ \left(aq\right)\ +\ 2NaOH\ \left(aq\right)\ \rightarrow\ Na_2SO_4\ \left(aq\right)\ +\ H_2O\ \left(l\right)\ \ \ \Delta H\ =\ -  

Endothermic
Exothermic
30.
A molecule is made up of ____ or more atoms.
a)
1
b)
2
c)
3
d)
4
31.

Match the following

a)

a molecule made of at least two different elements in a fixed ratio

1.

compound

b)

a group of two or more atoms bonded together

2.

molecule

c)

simplest form of matter

3.

element

d)

elements and compounds

4.

pure substances

e)

two or more substances NOT chemically combined

5.

mixture

32.

As you move across the periodic table, from left to right, the metallic character of the elements________

a)

increases

b)

decreases

c)

stays the same

33.

Which of the following has a larger radius than Zinc

a)

Gallium

b)

Magnesium

c)

Strontium

d)

Aluminum

34.

Which has a lower ionization energy: Lithium or Potassium?

a)

Lithium

b)

Potassium

35.

Which atom has the most valence electrons

a)

Ca

b)

C

c)

Cl

d)

Si

36.

As you move across the periodic table, from left to right, ionization energy is __________________.

a)

decreasing

b)

increasing

37.

As you move across a period, do the atoms get smaller or larger?

a)

smaller

b)

larger

38.

How many valence electrons does a neutral atom of nitrogen have?

a)

2

b)

4

c)

5

d)

6

39.

Which atom is more electronegative?

a)

K

b)

Rb

c)

Cl

d)

B

40.

As atoms in Group 15 are considered in order from top to bottom, the electronegativity of each successive element....

a)

increases

b)

decreases

c)

remains the same

d)

none of the above

41.

As you move down the periodic table, atoms tend to get bigger because...

a)

They have more mass

b)

They have more protons

c)

They have more energy levels

d)

They have more mass

42.

As you move across the periodic table, atoms tend to get smaller. This is because...

a)

The atoms have more mass

b)

The atoms have more neutrons

c)

The atoms have less mass

d)

They have more protons

43.

Electronegativity is

a)

the ability of an atom to accept/ attract electrons

b)

the energy required to remove an electron from an atom in a gaseous or ion state

c)

a life philosophy (the glass is half empty)

d)

the ability of an atom to lose electrons

44.

Ionization energy is ....

a)

the energy required to add an electron to an atom

b)

the energy required to shield the outer electrons from the nucleus

c)

a measure of the ability of an atom to attract electrons

d)

how much energy it takes to remove an electron from an atom

45.

The atom with the largest atomic radius in Group 18 is....

a)

He

b)

Xe

c)

Ne

d)

Rn

46.

Metals have the largest...

a)

atomic radius and electronegativity

b)

electronegativity and ionization energy

c)

ionization and atomic radius

d)

atomic radius only

47.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period, and increases down a group

b)

Electronegativity decreases across a period and decreases down a group

c)

Ionization energy increases across a period and increases down a group

48.

What metalloid is in the fourth period and in the same group as carbon?

a)

boron

b)

tin

c)

silicon

d)

germanium

49.

An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than krypton but less than iodine. Use the periodic table to identify the element

a)

selenium

b)

polonium

c)

tellurium

d)

sulfur

50.

Vertical columns of elements (families) on the periodic table with similar properties

a)

period

b)

row

c)

groups

d)

quadrants

51.

Which atom has the largest radius

a)

Mg

b)

B

c)

S

d)

Br

52.

How are anhydrous compounds different from hydrates?

a)

Anhydrous compounds contain more water molecules than hydrates

b)

Anhydrous compounds and hydrates are the same

c)

Anhydrous compounds do not contain water molecules, unlike hydrates

d)

Anhydrous compounds use Greek letters to indicate the number of water molecules present

53.

What is a hydrate?

a)

A compound without water

b)

A compound that contains water molecules in its structure

c)

A gas at room temperature

d)

A liquid that does not mix with water

54.

Which of the following is an example of a hydrate?

a)

NaCl

b)

CuSO₄·5H₂O

c)

H₂O

d)

CO₂

55.

What happens to a hydrate when it is heated?

a)

It gains water

b)

It loses water of hydration

c)

It melts

d)

It becomes a gas

56.

What is a non-polar covalent bond?

a)

transfer of electrons

b)

is a bond where electrons are shifted to the more electronegative atom

c)

Sea of electrons

d)

is a bond where electrons are shared equally

57.

Ionic Bonds involve the….

a)

Sharing of Valence Electrons

b)

Sea of Valence Electrons

c)

Transfer of Valence Electrons

d)

no valence electrons

58.

Metallic bonds involve…..

a)

Sharing of Valence Electrons

b)

Mobile Sea of Valence Electrons

c)

Transfer of Valence Electrons

d)

no valence electrons

59.

What type of bond is formed between nitrogen and oxygen?

a)

Metallic

b)

No bond will form

c)

Ionic

d)

Covalent

60.

What type of bond is formed between sodium and bromine?

a)

Metallic

b)

No bond will form

c)

Ionic

d)

Covalent

61.
Metals and nonmetals form which kind of bond?
a)
Polar covalent
b)
Ionic
c)
Non-polar covalent
d)
Metallic
62.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
63.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

64.

What is happening to the electrons during a covalent bond?

a)

The electrons are being shared

b)

One element is taking electrons, another is giving away electrons

c)

The electrons don't move

d)

Both atoms give away electrons

65.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
66.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
67.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

68.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
69.

A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory is known as

a)

real gas

b)

ideal gas

c)

imaginary gas

d)

perfect gas

70.

Which of the following is not true about the volume of a gas?

a)

Most of the volume is empty space.

b)

The volume is occupied by particles in continuous, rapid, random motion.

c)

The volume is about 10 times greater than that occupied by an equal number of particles in the liquid or solid state.

d)

Generally, the volume can be easily changed

71.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

72.

Which of the following is the equation needed to calculate the kinetic energy, KE, of a moving particle?

a)

KE = 1/2 mv2

b)

KE = 2mv

c)

KE = mv

d)

KE = 1/2 m2v

73.

If a gas has the same temperature throughout, which gas molecule has the highest average velocity?

a)

O2

b)

H2O

c)

H2

d)

Xe

74.

Which of the following is not a physical property of gases?

a)

absence of definite volume

b)

large density

c)

high compressibility

d)

fluidity

75.

Which states of matter are fluid?

a)

gases and liquids

b)

liquids and solids

c)

gases only

d)

liquids only

76.

For a fixed amount of gas at a constant temperature, the volume increases as the pressure...

a)

remains steady.

b)

increases.

c)

decreases.

d)

fluctuates.

77.

How is pressure explained in the kinetic molecular theory?

a)

As a result of temperature only

b)

From gravitational forces between particles

c)

As a result of volume changes

d)

From gas particles colliding with container walls

78.

What relationship does Boyle’s law describe?

a)

Pressure and volume are inversely proportional

b)

Volume and temperature are directly proportional

c)

Temperature and volume are inversely proportional

d)

Pressure and temperature are directly proportional

79.

According to Charles’s law, what happens when temperature increases?

a)

Pressure increases

b)

Pressure decreases

c)

Volume decreases

d)

Volume increases

80.

What type of collisions do gas particles have according to the kinetic molecular theory?

a)

Inelastic

b)

Elastic

c)

Partial

d)

Non-colliding

81.

How do gas molecules move?

a)

in a circular motion

b)

in straight line paths

c)

in an orderly fashion

d)

constantly and randomly

82.

The more energy that particles have, the ___ they move.

a)

faster

b)

slower

83.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
What is the mass in grams of H₂ gas when 4.0 moles of HCl is added to the reaction?
a)
0.99 g
b)
4.0 g
c)
2.0 g
d)
6.0 g
84.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g
85.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
What is the mass in grams of H₂ gas when 4.0 moles of HCl is added to the reaction?
a)
0.99 g
b)
4.0 g
c)
2.0 g
d)
6.0 g
86.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
87.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
88.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
89.
How many liters of NH3 are needed to react completely with 30.0L of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
5.0 L
b)
20.0 L
c)
7.5 L
d)
120.0 L
90.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

91.

1Mg + 2H2O --> Mg(OH)2 + H2

What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium?

a)

62.0 L

b)

0.12 L

c)

2.77 L

d)

1.15 L

92.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

93.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
94.
The first person to propose a theory about an atom was
a)
Democritus
b)
Rutherford
c)
Dalton
d)
Aristotle
95.
Rutherford's gold foil experiment provided evidence that...
a)
Negative and positive charges are spread evenly throughout the atom.
b)
Alpha particles have a positive charge.
c)
Gold is not a dense as previously thought.
d)
There is a dense positively charged nucleus at the center of an atom.
96.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom.  
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
97.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
98.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
99.
Who stated that all atoms of the same element are exactly alike?
a)
Democritus
b)
Dalton
c)
Thomson
d)
Borh
100.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)
Proton
b)
Neutron
c)
Electron
d)
Orbitals
101.
Niels Bohr suggested that electrons.......
a)
are found in specific orbits
b)
electrons are scattered throughout the atom
c)
electrons move according to their energy level
d)
electrons are positive
102.
Which is the correct sequence of the scientists who made major changes in the model of the atom?
1-JJ Thomson
2-Erwin Schrodinger
3-John Dalton
4-Niels Bohr
5-Ernest Rutherford
a)
2, 1, 4, 3, 5
b)
3, 1, 5, 4, 2
c)
5, 3, 2, 1, 4
d)
4, 3, 2, 1, 5
103.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
104.
The word atom comes from a Greek word "atomos" that means
a)
Invisible
b)
Indivisible
c)

Divided

d)

Destroyed

105.
His atomic model was depicted similar to a planetary/solar system
a)
Bohr
b)
Thomson
c)
Rutherford
d)
Dalton
106.
John Dalton stated:
a)
elements are made of atoms
b)
atoms of a given element are identical
c)
atoms cannot be subdivided, created, nor destroyed
d)
all of the above
107.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
108.

In a famous experiment conducted by Ernest Rutherford, positively charged alpha particles were scattered by a thin gold foil. Which of the following is a conclusion that resulted from this experiment?

a)

The nucleus is negatively charged

b)

The atom is a dense solid and is indivisible

c)

The mass is conserved when atoms react chemically

d)

The nucleus is very small and the atom is mostly empty space

109.

What subatomic particle was discovered in the cathode ray tube experiment?

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

110.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
111.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
112.

This helped prove the existence of:

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

113.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
114.
Atoms of the same element with a different number of neutrons
a)
Ion
b)
Gluons
c)
Isotope
d)
Quarks
115.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
116.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
117.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
118.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
119.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

120.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
121.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
122.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
123.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
124.
Which of these has a linear molecular shape?
a)
SCl2
b)
SiH4
c)
NH3
d)
O2
125.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
126.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
127.

Elements in the same group or family have _____________.

a)

the same number of valence electrons and different properties.

b)

the same number of valence electrons and similar properties

c)

different number of valence electrons and similar properties.

d)

different number of valence electrons and different properties.

128.

Which class of elements are malleable, ductile, shiny when clean and polished, good conductors of heat and electricity, and reacts with acids to form hydrogen gas?

a)

metals

b)

nonmetals

c)

metalloids

d)

ions

129.

What is the name of the elements that are unreactive and have a full octet?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Transition Metals

130.

The Halogen group has an oxidation number of -1. Why?

a)

The Halogen group will gain one electron, therefore have an oxidation number of -1.

b)

The Halogen group will lose one electron, therefore have an oxidation number of -1.

c)

The Halogen group will lose seven electrons, therefore have an oxidation number of -1.

131.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

132.
What element is this?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
133.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
134.
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
135.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
136.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
137.
?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
138.
?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
139.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

140.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

141.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
142.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
143.

Why do carbon, silicon, and tin all react similarly?

a)

They are located in the same period

b)

They have an even atomic number

c)

They have the same number of energy levels

d)

They are located in the same group

144.
What do the numbers down the side tell us about the atoms in each row?
a)
number of protons
b)
number of electrons
c)
number of energy levels
d)
absolutely nothing
145.

Match the correct term with its definition

a)
Arrhenius Acid
1.

Produce H+ as the only positive ion

b)
Arrhenius Base
2.

Produce Oh- as the only negative ion

c)
Bronsted-Lowry Acid
3.

Proton donor

d)
Bronsted-Lowry Base
4.

Proton Acceptor

e)

Electrolyte

5.

Conducts electricity when dissolved

146.

Bases, also known as ​ (a)   will turn litmus paper ​ (b)   . This is because they have a pH ​ (c)   . They taste ​ (d)   .

Choose from the below words
alkali and OH-
blue
above 7
bitter
below 7
H+
red
sour
147.

​ Acid formulas start with ​ (a)   , while base formulas end with ​ (b)   . Salts contain ​ (c)   .

Choose from the below words
hydrogen
hydroxide
neither hydrogen nor hydroxide
148.

Organize these options into the right categories.

Categorize the following

sour taste

bitter taste

pH = 8.2

pH = 1.8

turns blue litmus paper red

turns red litmus paper blue

slippery

increase hydroxide ions

increase hydrogen ions

pH = 5.4

Acid
Base
149.

What is pH based on?

a)

The pOH.

b)

The dissociation of water.

c)

The concentration of hydroxide ions.

d)

The formation of water.

150.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

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