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Fall Practice Final

Total questions: 101

Worksheet time: 25hrs 15mins

Name
Class
Date
1.
If reaction starts with 20g of reactants it should produce 
a)

a total of 40g of products

b)

a total of 10g of products

c)

a total of 80 g of products

d)

a total of 20g of products

2.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

3.
Particles in an atom that are neutral and have no charge are 
a)

negatrons 

b)

electrons 

c)

neutrons 

d)

protons 

4.
The atomic number is equal to _.
a)

the number of protons only

b)

the number of neutrons only

c)

the total number of protons and neutrons

d)

the number of protons neutrons and electrons

5.
An atom becomes _________ when it gains electrons.
a)

Positive

b)

Negative

c)

Neutral

d)

Invinsible

6.
An atom that has gained or lost electrons is called ...
a)

a quantum

b)

an isotope

c)

an ion

d)

an multivalent

7.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

8.

Protons are

a)

Negative

b)

Positive

c)

No charge

9.

Neutrons have

a)

Negative

b)

Positive

c)

No charge

10.

Electrons are are

a)

Negative

b)

Positive

c)

No charge

11.

What is true about the isotope nitrogen-15? (check all that are true)

a)

It has 7 protons

b)

It has 7 electrons

c)

It has 7 neutrons

d)

It has a mass number of 15

e)

It is the most common isotope of N.

12.

A negative ion is called a(an) _______. It is the result of an atom ______ electrons.

(a)  

13.

The ion Sr2+ has:

a)

88 neutrons

b)

36 electrons

c)

40 electrons

d)

38 electrons

14.
In a correctly written symbol what would be located in the "A" position?
a)

number of neutrons

b)

atomic number

c)

number of electrons 

d)

mass number

15.

In a correctly written symbol what would be located in the "Z" position?

a)

number of neutrons

b)

atomic number

c)

number of electrons

d)

mass number

16.
How many protons does this isotope of titanium have?
a)

48

b)

22

c)

26

d)

70

17.
How many neutrons does the isotope of lithium have?
a)

8

b)

3

c)

4

d)

5

18.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

19.
What atom matches this electron configuration?
1s22s22p63s2
a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

20.
What is the shorthand electron configuration for Sulfur atom?
a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

21.

What atom matches this electron configuration?

[Xe] 6s24f145d9

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

22.
According to the octet rule most elements need _______ valence electrons.
a)

2

b)

8

c)

6

d)

18

23.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)

4

b)

6

c)

8

d)

2

24.
This is a correct dot diagram for neon (Ne)
a)

true

b)

false

25.
This could be the dot diagram of
a)

Mg

b)

Cl

c)

C

d)

O

26.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

27.

What group is the most reactive non metals?

a)

1

b)

17

c)

2

d)

1

28.

What group is the most reactive metals?

a)

2

b)

18

c)

1

d)

16

29.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)

Sodium is less electronegative than potassium. 

b)

Sodium has fewer energy levels than potassium. 

c)

Sodium has a larger ionic radius than potassium. 

d)

Sodium has lower ionization energy than potassium. 

30.
Which of these elements has the greatest atomic radius? 
a)

H

b)

N

c)

Cl

d)

Cs

31.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)

Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.

b)

Atomic radii increase from left to right across a period and increase from top to bottom in a group.

c)

Atomic radii decrease from left to right across a period and increase from top to bottom in a group.

d)

Atomic radii increase from left to right across a period and decrease from top to bottom in a group.

32.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)

fluorine

b)

chlorine 

c)

bromine 

d)

iodine 

33.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)

beryllium, Be

b)

potassium, K

c)

titanium, Ti

d)

yttrium, Y

34.
What is the family name of this group of elements? 
a)

Alkali metals 

b)

Halogens 

c)

Noble Gases 

d)

Alkali Earth Metals 

35.

Which of the following will have a lower ionization energy than Ca?

a)

Magnesium (Mg)

b)

Beryllium (Be)

c)

Strontium (Sr)

36.
Which atom has the largest atomic radius?
a)

potassium

b)

rubidium 

c)

francium

d)

cesium

37.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)

The atoms have more mass.

b)

The atoms have more protons.

c)

The atoms have more energy levels

d)

The atoms have more neutrons

38.
Which element is not in the Alkali metal family?
a)

Li

b)

Ca

c)

Fr

d)

Cs 

39.

Argon (Ar) belongs to which family?

a)

alkali metal

b)

alkaline earth metal

c)

halogen

d)

noble gas

40.
How many valence electrons does an alkaline earth metal have? 
a)

1

b)

2

c)

7

d)

8

41.
How many valence electrons does a halogen have? 
a)

1

b)

2

c)

7

d)

8

42.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

43.

Ions are formed when atoms...

a)

lose or gain electrons

b)

lose or gain protons

c)

lose or gain neutrons

d)

split in two

44.

Ionic bonds are the _____ between positive and negative ions.

a)

covalent bonds

b)

metallic bonds

c)

polar bonds

d)

electrostatic attraction

45.

Many ionic compounds are soluble in water.

a)

True

b)

False

46.

Ionic compounds conduct electricity only when molten or dissolved because...

a)

electrons are free to move

b)

water is free to move

c)

molecules are free to move

d)

ions are free to move

47.
When metals bond with non-metals they form what type of bonds
a)

covalent

b)

ionic

c)

cooperative

d)

lewis

48.

When a nonmetal gains electrons, it becomes this type of ion.

a)

Anion

b)

Cation

49.

When a metal loses electrons, it becomes this type of ion.

a)

anion

b)

cation

50.
When an ionic compound is formed, its charge is 
a)

negative

b)

neutral (no charge)

c)

positive

51.

Is this compound ionic or covalent?

a)

Ionic

b)

Covalent

52.

Is this compound ionic or covalent?

a)

ionic

b)

covalent

53.

What will this atom do to become stable?

a)

Gain 7 electrons

b)

Lose 1 electrons

c)

Nothing, it is already stable

54.

What will this atom do to become stable?

a)

Lose 2 electrons

b)

Gain 6 electrons

c)

Gain 8 electrons

d)

Lose 1 electron

e)

Nothing, it is already stable

55.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

56.
Which of the following is a property of an ionic compound?
a)

high melting point

b)

soft

c)

malleable

d)

liquid at room temperature

57.

Why do all bonds form?

a)

for atoms to become stable

b)

so an atom can be unstable

c)

so the number of protons and electrons can equal.

d)

so they can gain neutrons.

58.

How many electrons are shared in a double bond?

a)

2

b)

4 pairs

c)

6

d)

4

59.

How many electrons are shared in a single bond?

a)

2 pairs

b)

4

c)

2

d)

1

60.
What does the Law of Conservation of Mass state?
a)

Matter cannot be gained or lost in a chemical reaction.

b)

Matter can only be lost in a chemical reaction.

c)

Matter can only be gained in a chemical reaction.

d)

Matter can be gained and lost in a chemical reaction. 

61.
How many atoms of carbon (C) are in C6H12O6?
a)

3

b)

6

c)

12

d)

24

62.
How many atoms are there TOTAL in:
H2SO4
a)

6

b)

5

c)

7

d)

3

63.
The specific heat of aluminum is 0.21 cal/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)

105 J

b)

10.5 J

c)

1.05 J

64.
20 g of water. specific heat of water is 4.18 J/x°C.  temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?
a)

418 Joules

b)

209 J

c)

83 J

d)

4.18 J

65.
The specific heat is the amount of energy needed to raise the temperature one degree Celsius of a substance.
a)

True

b)

False

66.

Water has a specific heat of 4.184 J/gºC.  Wood has a specific heat of 1.760 J/gºC.  What material needs more energy to raise the temperature 1ºC

a)

Wood

b)

Water

c)

Both are the same

67.
How does heat flow?
a)

Always from cold to warm

b)

Always from warm to cold

c)

Both warm to cold & cold to warm

d)

It depends on the temperature

68.

A pot of 2400g of water at a temperature of 25˚C is heated on a stove until the water boils (100˚C).  The specific heat of water is 4.184 J/(g˚C). Determine the heat energy needed to heat the water in the pot to boiling.

a)

133.76J

b)

43,062.2J

c)

753,120J

d)

1,003,200J

69.
Energy due to motion is ____________ energy. 
a)

Potential 

b)

Energy

c)

Kinetic

d)

Friction

70.
The faster an object moves, the ________ kinetic energy it has. 
a)

more

b)

less

c)

none of the above

d)

all of the above 

71.
__________ is stored energy. 
a)

Potential

b)

Kinetic

c)

None of the above 

d)

All of the above 

72.
What kind of energy is in a moving skateboard?
a)

Potential

b)

Kinetic

c)

Both potential and kinetic energy

d)

none of the above

73.
What kind of energy is in a rock at the edge of a cliff?
a)

Potential

b)

Kinetic

c)

Both potential and kinetic energy

d)

none of the above

74.
Which point has the most potential energy?
a)

G

b)

f

c)

b

d)

a

75.

Which best describes temperature?

a)

It is equal to the heat difference between two objects

b)

It is proportional to the total energy in an object

c)

It is the measurement of the average kinetic energy of particles in an object

d)

It is equal to an object's specific heat capacity

76.

What type of heat transfer?


Water that is boiling

a)

Conduction

b)

Convection

c)

Radiation

77.

What type of heat transfer?


A pan heating on a stove

a)

Conduction

b)

Convection

c)

Radiation

78.

What type of heat transfer?


Moves as a current

a)

Conduction

b)

Convection

c)

Radiation

79.

What type of heat transfer?


Sun rays reaching earth

a)

Conduction

b)

Convection

c)

Radiation

80.

What type of heat transfer?


Heat transfer through a solid

a)

Conduction

b)

Convection

c)

Radiation

81.

What units are used to measure heat and energy?

a)

meters or kilometers

b)

joules or calories

c)

kelvin or celsius

d)

liters or kiloliters

82.

What does heat do when convection currents are moving?

a)

Sinks

b)

Rises

c)

Stays in place

83.
In convection, COOL air
a)

Rises

b)

Sinks

c)

stays in the same place

84.

Convection currents occur when ______________________ energy transfers between a fluid.

a)

potential

b)

kinetic

c)

thermal/heat

d)

electric

85.

Convection currents in the Earth's mantle are caused by:

a)

Less dense hot magma moving downward

b)

Less dense hot magma moving upward

c)

Tectonic plate movement

d)

More dense cooler magma moving upward

86.

Earth's MANTLE is solid, but also fluid.

a)

True

b)

False

87.

The OUTER CORE is the only truly liquid layer inside the Earth.

a)

True

b)

False

88.

Where do convection cycles happen?

a)

inner core

b)

mantle

c)

crust

89.
What is the correct order (starting from the surface) of Earth's layers?
a)

crust, outer core, inner core, mantle

b)

mantle, outer core, inner core, crust

c)

crust, mantle, outer core, inner core

d)

outer core, inner core, crust, mantle

90.

Which is a stronger bond?

a)

Ionic

b)

Covalent

91.

What is the cause of the various periodic table trends (ionization energy, electronegativity & atomic radius)

a)

The atomic mass

b)

the positive/negative attraction between protons and electrons

c)

the number of neutrons of an atom

d)

the type of element/atom

92.
In an exothermic reaction, heat is ...
a)

taken in

b)

given out

93.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

94.

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

95.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Kinetic

d)

Potential

96.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)

g /J C

b)

°C/g J

c)

kJ/g

d)

J/g°C

97.
What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)
a)

0.111 J/g°C

b)

1.29 J/g°C

c)

0.129 J/g°C

d)

22225.85 J

98.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

99.

Emission spectra (bright line spectra) are created when electrons relax from ___.

a)

higher to lower energy levels.

b)

lower to higher energy levels.

c)

s orbitals to p orbitals.

d)

one atom to a different atom.

100.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

101.

What drives convection currents?

a)

thermal energy & density

b)

radiation energy

c)

conduction energy

d)

wind patterns and radiation

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