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Timberlake Chemistry Semester 1 Exam review

Total questions: 204

Worksheet time: 6hrs 46mins

Name
Class
Date
1.

A pure substance is matter that consists of matter with a composition that

a)

is fixed in a definite proportion at all time.

b)

varies according to the amount of water present

c)

depends on the temperature

d)

always contains two or more substances

2.

Compounds are pure substances that by definition consist of

a)

a single element

b)

oxygen and hydrogen

c)

two or more elements in combination

d)

solids

3.

Using the diagram on the left, identify which circle contains molecules of an element.

a)

A

b)

B

c)

C

d)

D

4.

Using the diagram on the left, identify which circle contains atoms of an element.

a)

A

b)

B

c)

C

d)

D

5.

Using the diagram on the left, identify which circle contains a mixture of two elements and a compound.

a)

A

b)

B

c)

C

d)

D

6.

Using the diagram on the left, identify which circle contains molecules of a compound.

a)

A

b)

B

c)

C

d)

D

7.

What is a physical property?

a)

can be observed or measured without changing the composition of matter

b)

characteristic of a substance that may be observed when it participates in a chemical reaction

c)

flammability, toxicity, chemical stability, and heat of combustion

d)

a chemical reaction

8.

What is a chemical property?

a)

characteristic of a substance that may be observed when it participates in a chemical reaction

b)

can be observed or measured without changing the composition of matter

c)

States of matter include liquid, solid, and gaseous states.

d)

odor, boiling point, ability to conduct heat, ability to conduct electricity, ability to dissolve in other substances

9.

Which is an example of a physical change?

a)

A chemical going from solid to liquid

b)

Formation of bubbles when two chemicals are put together

c)

A piece of copper grows a coat of silver when put into a solution

d)

A substance catching fire

10.

Which is an example of a chemical change?

a)

A chemical going form a liquid to a solid

b)

A chemical going from a solid to a gas

c)

Bending a piece of wire until it breaks

d)

The formation of bubbles when two chemicals are put together.

11.

Which state of matter has both a definite volume and definite shape?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

12.

Which state of matter has a definite volume and no definite shape?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

13.

Which state of matter has no definite volume and no definite shape?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

14.

Which state of matter is made of high energy ions and electrons?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

15.

Which of the following does NOT describe a pure substance?

a)

has a fixed composition

b)

distinct properties

c)

contain only one type of matter

d)

each substance retains its own properties

16.

Which two describes an element?

a)

Cannot be broken down into simpler substances

b)

Composed of only one type of atom

c)

Does not have same composition throughout

d)

Can be seperate by physical means

17.

The difference between a compound and an element is? Pick two

a)

Contain two or more kinds of atoms

b)

Can be separated into simpler particles

c)

Can be separated by physical means

d)

The components of it retain their unique properties

18.

A mixture that does not have same composition throughout the mixture.

a)

Heterogeneous

b)

Homogeneous

c)

Elements

d)

Compounds

19.

A mixture that does have uniform composition throughout the mixture.

a)

Heterogeneous

b)

Homogeneous

c)

Elements

d)

Compounds

20.

Which mixture type can also be called a solution?

a)

Heterogeneous

b)

Homogeneous

c)

Elements

d)

Compounds

21.

Which of these are physical ways to separate components of a mixture?

a)

Filtration

b)

Distillation

c)

Magnetism

d)

Chromatography

22.

The first letter of an element symbol is always.....

a)

lower case

b)

capitalized

c)

small

d)

starts with a vowel

23.

Water is a compound and not an element or mixture because....

a)

Can be decomposed into the elements and it has its own unique properties

b)

Because it can be separated by physical means

c)

Because all the components keep their own properties and do not change

d)

Because it is heterogeneous

24.

When a firecracker explodes, giving off light and heat, and breaking the wrapper into many pieces, ____.

a)

a physical change takes place

b)

a chemical change takes place

c)

both a physical and chemical change are taking place

d)

the wrapper evaporates into a gas

e)

the fuse undergoes a physical change only

25.

The temperature of liquid nitrogen is -196 degrees Celsius. What is the corresponding reading on the Kelvin scale?

a)

77 K

b)

-127 K

c)

-91 K

d)

48 K

e)

146 K

26.

A patient has a temperature of 38.5 degrees Celsius. What is the temperature in degrees Fahrenheit?

a)

70.5 degrees F

b)

311.0 degrees F

c)

126.95 degrees F

d)

101.3 degrees F

e)

11.7 degrees F

27.

Convert

100oC100^oC  to Kelvin

a)

373 K373\ K  

b)

273 K273\ K  

c)

212 K212\ K  

d)

0 K0\ K  

28.

Convert

450 K450\ K  to Celsius

a)

723oC723^oC  

b)

277oC277^oC  

c)

177 oC177\ ^oC  

d)

623oC623^oC  

29.

Convert

300 K300\ K  to Celsius

a)

573oC573^oC  

b)

37oC37^oC  

c)

27oC27^oC  

d)

600oC600^oC  

30.

Convert

0oC0^oC  to Kelvin

a)

−273 K-273\ K  

b)

273 K273\ K  

c)

32 K32\ K  

d)

−32 K-32\ K  

31.

Convert

0 K0\ K  to Celsius

a)

273oC273^oC  

b)

−273oC-273^oC  

c)

32oC32^oC  

d)

−32oC-32^oC  

32.

What is the boiling point of water on the Celsius scale?

a)

0oC0^oC

b)

373oC373^oC

c)

100oC100^oC

d)

212oC212^oC

33.

What is the boiling point of water on the Fahrenheit scale?

a)

0oF0^oF

b)

373oF373^oF

c)

100oF100^oF

d)

212oF212^oF

34.

What is the boiling point of water on the Kelvin scale?

a)

0K0^{ }K

b)

373K373^{ }K

c)

100K100^{ }K

d)

212K212^{ }K

35.

What is the freezing/melting point of water of the Fahrenheit scale?

a)

−273oF-273^oF

b)

0oF0^oF

c)

32oF32^oF

d)

273oF273^oF

36.

What is the freezing/melting point of water of the Celsius scale?

a)

−273oC-273^oC

b)

0oC0^oC

c)

32oC32^oC

d)

273oC273^oC

37.

Which of the following is an example of potential energy?

a)

chewing food

b)

water stored in a reservoir

c)

burning wood

d)

a fan blade turning

e)

riding an exercise bike

38.

The phrase "ability to do work" is a definition of ____

a)

specific heat

b)

energy

c)

calorie

d)

heating

e)

cooling

39.

The specific heat of a substance is the amount of heat needed to ____

a)

change 1 g of the substance from the solid to the liquid state

b)

raise the temperature of 1 g of the substance by 1 degree Celsius

c)

change 1 g of the substance from the liquid to the solid state

d)

convert 1 g of a liquid to a gas

e)

convert 1 g of a solid to a gas

40.

How many joules are required to raise the temperature of a 35.0 g sample of iron from 25 degrees Celsius to 35 degrees Celsius. Iron has a specific heat of 0.450 J/g degrees C.

a)

10 J

b)

16 J

c)

35 J

d)

160 J

e)

350 J

41.
How many Joules of energy are required to make 100 grams of ice at 0 C completely melt?
a)
200 J
b)
400 J
c)
30,000 J
d)
2,000,000 J
42.
What is the change in temperature when 50,000 Joules of energy is added to 200 grams of water at 25 C?
a)
0.016 C
b)
1,500 C
c)
63 C
d)
0.4 C
43.
How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?
a)
1400 J
b)
2800 J
c)
210,000 J
d)
1,400,000 J
44.
How much liquid water can you change 20 C if you apply 20,000 J?
a)
500 g
b)
100,000 g
c)
250 g
d)
350 g
45.
What is the change in temperature when 40,000 Joules of energy is added to 50 grams of ice at -4 C?
a)
200 C
b)
Solve
c)
Solve
d)
Solve
46.
How many Joules of energy are required to change 10 gram of ice at -2 C to water at 20 C?
a)
440 J
b)
880 J
c)
10,140 J
d)
66,000 J
47.

The dietary calorie (Cal) is equal to __

a)

1000 kcal

b)

100 kcal

c)

100 calories

d)

10 calories

e)

1 kcal

48.

A glazed doughnut contains 22 g of carbohydrate, 12 g of fat, and 2 g of protein. How many kilojoules of energy does the doughnut contain? (The accepted caloric values for foods are 17 kJ/g for carbohydrate, 38 kJ/g for fat and 17kJ/g for protein.)

a)

860 kJ

b)

660 kJ

c)

280 kJ

d)

200 kJ

e)

70 kJ

49.

A serving of fish contains 4.0 g of fat, and 50.0 g of protein. If the caloric value of protein is 4 kcal/g and fat is 9 kcal/g, how many kcal are in the serving? Round the answer to the tens place.

a)

240 kcal

b)

54 kcal

c)

470 kcal

d)

220 kcal

e)

490 kcal

50.
The  mass of an atom is located  in the ___________ and the volume of an atom is made of the ____________
a)
electron cloud, nucleus
b)
electron cloud, energy levels
c)
nucleus, electron cloud
d)
nucleus, neutrons
51.
Isotopes are atoms of the same element that have the same number of __________ but different number of __________ . Therefore, isotopes of the same element have different masses. 
a)
protons, neutrons
b)
protons, electrons
c)
neutrons, protons
d)
electrons, protons
52.
A neutral atom of Carbon-13 has ________ electrons and _________ neutrons
a)
13, 13
b)
6, 7
c)
7, 7
d)
6, 6
53.
A neutral atom of the isotope 2612Mg would consist of
a)
12 protons, 26 neutrons, 26 electrons
b)
26 protons, 12 neutrons, 26 electrons
c)
26 protons, 14 neutrons, 14 electrons
d)
12 protons, 14 neutrons, 12 electrons
54.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
55.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
56.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
57.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

58.

What is the atomic number of Barium, Ba?

a)

20

b)

38

c)

56

d)

88

59.

How many protons are in a sodium atom, Na?

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons.

d)

Sodium has 22 protons.

60.

An element has the mass number 12 and atomic number 6. The number of neutrons in it is:

a)

6

b)

10

c)

4

d)

8

61.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

62.

How many neutrons does C-14 [atomic #6] contain?

a)

6

b)

7

c)

14

d)

8

63.

How many neutrons does an atom of the isotope Neon-22 have?

a)

12

b)

10

c)

22

d)

20

64.

How many electrons are in an atom with an atomic number of 50?

a)

5

b)

8

c)

50

d)

2

65.

If an atom has 10 electrons, how many protons does it have?

a)

0

b)

1

c)

10

d)

5

66.

How many neutrons does an atom of Nitrogen-13 have?

a)

6

b)

7

c)

13

d)

5

67.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

68.

What elements are in fluorapatite, Ca10(PO4)6F2, a major compound in treated human teeth?

a)

carbon, potassium, oxygen, iron

b)

calcium, phosphorus, oxygen, hydrogen

c)

calcium, phosphorus, oxygen, fluorine

d)

calcium, phosphorus, oxygen, flerovium

69.

Arsenic is an example of a(n) ________.

a)

metalloid

b)

alkalai metal

c)

nonmetal

d)

nobal gas

e)

transitional element

70.

Which of the following is a characteristic of the modern periodic table?

a)

A group is a horizontal row on the periodic table.

b)

A period is a column on the periodic table.

c)

The elements in each group have similar chemical properties.

d)

The B groups contain the representative elements.

e)

The A groups contain the transition elements.

71.

Which of the following elements is a metal?

a)

nitrogen

b)

fluorine

c)

argon

d)

calcium

e)

phosphorous

72.

What is the atomic number of nickel?

a)

110

b)

28

c)

46

d)

78

73.

What is the atomic number of Cu? What element is Cu?

a)

24, chromium

b)

48, cadmium

c)

96, curium

d)

29, copper

74.

Atomic number 21 is

a)

Ca

b)

Sc

c)

Fe

d)

Co

75.

What is the atomic number of lithium?

a)

2

b)

3

c)

4

d)

5

76.

The element in this list with chemical properties similar to magnesium is _

a)

sodium

b)

carbon

c)

boron

d)

radium

e)

chlorine

77.

Which is a noble gas?

a)

xenon

b)

nitrogen

c)

sulfur

d)

gold

e)

chlorine

78.

Which of the following is a characteristic of nonmetals?

a)

shiny

b)

malleable

c)

god conductors of heat

d)

low melting point

e)

good conductor of electricity

79.

Which element would have physical and chemical properties similar to chlorine?

a)

Ar

b)

I

c)

S

d)

O

e)

P

80.

Which of the following is true about the proton?

a)

It has a charge of -1 and is in the nucleus of the atom.

b)

It has a charge of +1 and is in the nucleus of the atom.

c)

It has a charge of 0 and is in the nucleus of the atom.

d)

It has a charge of -1 and is not in the nucleus of the atom.

e)

It has a charge of +1 and is not in the nucleus of the atom.

81.

The smallest particle of an element that retains the characteristics of the element is a(n) ________.

a)

electron

b)

proton

c)

neutron

d)

atom

e)

nucleus

82.

Isotopes are atoms of the same element that have ________.

a)

different atomic numbers

b)

the same atomic numbers but different numbers of protons

c)

the same atomic numbers but different numbers of electrons

d)

the same atomic number but different numbers of neutrons

e)

the same atomic mass but different numbers of protons

83.

The symbol of the element in Period 3 and Group 2A(2) is ________.

a)

B

b)

Be

c)

Mg

d)

Ca

e)

Al

84.

The symbol of the element in Period 4 and Group 7A(17) is ________.

a)

B

b)

Be

c)

Mg

d)

Fl

e)

Br

85.

If an element's atomic mass is 137, and the element's atomic number is 56, then that particular element has....

a)

137 protons, 137 neutrons, and 137 electron

b)

56 protons, 81 neutrons, and 56 electrons

c)

137 protons, 56 neutrons, and 137 electrons

d)

56 protons, 56 neutrons, and 56 electrons

e)

56 protons, 81 neutrons, and 137 electrons

86.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
87.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
88.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
89.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
90.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
91.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
92.
Identify the element in Period 5 that has 1 valence electron?
a)
Rb
b)
Nb
c)
Ag
d)
Sb
93.
What element in Period 4 has 5 valence electrons?
a)
Zr
b)
As
c)
V
d)
Sb
94.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
95.
How are elements arranged in the periodic table?
a)
in alphabetical order
b)
in the order in which they were discovered
c)
 in order of increasing atomic number
d)
 in order of increasing melting points
96.
The vertical columns in the periodic table are known as:
a)
groups
b)
periods
c)
valences
d)
isotopes
97.
Group 18 of the periodic table contains nonreactive elements like helium, neon, and argon. The elements in this group are called:
a)
alkali metsls
b)
transition metals
c)
halogens
d)
noble gases
98.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

99.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

100.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
101.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
102.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
103.

The maximum number of electrons that can fit into the 2nd energy level is

a)

2

b)

8

c)

18

d)

32

104.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

105.
The electrons that are on the outer most region of the atom
a)
Shell Electrons
b)
Violent Electrons
c)
Valence Electrons
106.
The different energy levels of electrons as they orbit the nucleus
a)
Electron Cloud
b)
Orbitals (Energy Levels)
c)
2, 8, 18, 32
107.
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
108.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
109.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
110.
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 2p box 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.
111.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
112.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
113.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
114.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
115.

True or False: The reactivity of metals tends to decrease as you move from left to right across the periodic table.

a)

True

b)

False

116.
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. 
117.
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
118.
How many sig figs are there?
100.00
a)
1
b)
3
c)
4
d)
5
119.
How many sig figs are there?
100000000
a)
1
b)
9
c)
10
120.
How many sig figs are there?
4004
a)
1
b)
2
c)
3
d)
4
121.
How many sig figs are there?
0.000008
a)
1
b)
2
c)
6
d)
7
122.
How many sig figs are there?
0.00400
a)
1
b)
3
c)
5
d)
6
123.
How many sig figs are there?
9009.00
a)
2
b)
4
c)
5
d)
6
124.
How many sig figs are there?
4000.
a)
1
b)
3
c)
4
125.
How many sig figs are there?
27000000
a)
2
b)
5
c)
8
126.
How many sig figs are there?
5.00000008
a)
2
b)
6
c)
9
127.
Which of the following numbers has three significant figures?
a)
1014 miles
b)
101 feet
c)
1000 yards
d)
all of the choices
128.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
129.
How many significant figures does the following number have: 0.998005
a)
9
b)
10
c)
6
d)
5
130.
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
131.
Calculate 1.23 m x 0.89 m and give your answer with the correct number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.095 m2
132.
Calculate 923 g ÷ 20312 cm3 and give your answer with the correct number of significant figures.
a)
0.04 g/cm3
b)
0.045 g/cm3
c)
0.0454 g/cm3
d)
0.05 g/cm3
133.
Calculate 12.47 m ÷ 3.2 s and give your answer with the correct number of significant figures.
a)
4 m/s
b)
3.9 m/s
c)
3.90 m/s
d)
3.897 m/s
134.
Calculate 0.020 cm x 50 cm x 11.1 cm and give your answer with the correct number of significant figures.
a)
10 cm3
b)
11.1 cm3
c)
11 cm3
d)
11. cm3
135.
Which of the following numbers have four significant figures?
a)
56.75 g
b)
40.01 g
c)
0.6000 g
d)
all of the choices
136.
All of the following have one significant figure except:
a)
100 cm
b)
0.0001 cm
c)
2 cm
d)
2.00 cm
137.

How many significant figures: 450 m

a)

3

b)

2

c)

1

d)

0

138.
What is 78.5 rounded to one significant figure?
a)
79
b)
78.5
c)
70
d)
80
139.
How many significant figures does the following number have: 100.00210
a)
7
b)
5
c)
10
d)
8
140.
Round 0.010229 to four sig figs
a)
1022
b)
1023
c)
0.01023
d)
0.01022
141.
Calculate 923 g ÷ 20312 cm3 and give your answer with the appropriate number of significant figures.
a)
0.04 g/cm3
b)
0.045 g/cm3
c)
0.0454 g/cm3
d)
4 x 10-2 g/cm3
142.
How many Significant Figures in the number below?
4.56 x 103
a)
5
b)
4
c)
6
d)
3
143.
How many significant figures does the following number have: 1740200
a)
2
b)
1
c)
3
d)
5
144.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
145.
Calculate 1.23 m x 0.89 m and give your answer with the correct number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.095 m2
146.
Calculate 0.020 cm x 50 cm x 11.1 cm and give your answer with the correct number of significant figures.
a)
10 cm3
b)
11.1 cm3
c)
11 cm3
d)
11. cm3
147.
Round off 509.96 to 4 significant figures.
a)
509.9
b)
509.0
c)
510.0
d)
510
148.
Solve. Round using SigFig math rules.
1.3562-mL / 14.32 g
a)
0.09-mL/g
b)
0.097-mL/g
c)
0.0973-mL/g
d)
0.09471-mL/g
149.
What is 78.5 rounded to one significant figure?
a)
79
b)
78.5
c)
70
d)
80
150.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
151.
How many significant figures does the following number have: 100.00210
a)
7
b)
5
c)
10
d)
8
152.

Solve. Round using SigFig math rules.

98.7°C - 97.25°C

a)

1°C

b)

1.5°C

c)

1.45°C

d)

1.450°C

153.

Solve. Round using SigFig math rules.

103 cm x 11 cm

a)

11 cm2

b)

1100 cm2

c)

1130 cm2

d)

1133 cm2

154.

Solve. Round using SigFig math rules.

12.5 mL + 20.05 mL + 2.69 mL

a)

35 mL

b)

35.2 mL

c)

35.24 mL

d)

35.240 mL

155.

Determine the number of Significant Figures in 10 Liters

a)

4

b)

3

c)

2

d)

1

156.

Determine the number of Significant Figures in 10.0 grams

a)

5

b)

4

c)

3

d)

2

157.

Solve. Round using SigFig math rules.

1.3562 mL / 14.32 g

a)

0.094 mL/g

b)

0.0947 mL/g

c)

0.094706 mL/g

d)

0.09471 mL/g

158.
Which number is correctly written in scientific notation?
a)
8.2 x 102
b)
82 x 107
c)
3.45 x 94
159.
Which number is correctly written in scientific notation?
a)
3.2867 x 10-7
b)
21.8689 x 10-4
c)
0.1537 x 105
160.
Which number is correctly written in scientific notation?
a)
10.4 x 103
b)
9.99 x 106
c)
143.002 x 10-4
161.
Write in standard form: 
8 x 104
a)
8,000
b)
80,000
c)
.00008
162.
Write in standard form: 
6.254 x 106
a)
6,254,000
b)
6,254,000,000
c)
625,400
163.
Write in standard form: 
7.3003 x 10-5
a)
.000073003
b)
.0000073003
c)
730,030
164.
Write in standard form: 
2.12 x 10-3
a)
.00212
b)
.000212
c)
2,120
165.
Write in scientific notation: 
241 million
a)
2.41 x 108
b)
2.41 x 107
c)
24.1 x 108
166.
Write in scientific notation: 
0.0000378 
a)
3.78 x 10-5
b)
3.78 x 10-6
c)
0.378 x 10-5
167.
Write in scientific notation: 
540,020,000
a)
5.4002 x 108
b)
5.4 x 108
c)
5.4002 x 104
168.
Write in scientific notation: 
0.0079245
a)
7.9245 x 10-3
b)
7.9245 x 10-2
c)
7.9245 x 103
169.
Which number is correctly written in scientific notation?
a)
5.67 x 105
b)
56.7 x 103
c)
0.567 x 106
170.
Add. 
(4.5 x 108) + (2.67 x 108)
a)
7.17 x 101
b)
7.17 x 108
c)
1.83 x 108
171.
Subtract.
(7 x 104) - (4.2 x 102)
a)
6.958 x 104
b)
6.58 x 104
c)
6.958 x 102
172.
Add.
(8.31 x 107) + (1.01 x 104)
a)
8.30899 x 107
b)
8.31101 x 103
c)
8.31101 x 107
173.
Subtract.
(5.6 x 109) - (2.4 x 106)
a)
5.5976 x 109
b)
55.976 x 109
c)
5.5976 x 106
174.

Write 5cm as a percentage of 20cm

a)

25%

b)

40%

c)

10%

d)

20%

175.

Write 7 days as a percentage of 10 days

a)

35%

b)

7%

c)

70%

d)

7/10

176.

Write 27 as a percentage of 50

a)

54%

b)

27%

c)

46%

d)

18.5%

177.

Write 3g as a percentage of 20g

a)

15%

b)

12%

c)

3%

d)

60%

178.

Write 4m as a percentage of 5m

a)

75%

b)

40%

c)

20%

d)

80%

179.

Write 164 as a percentage of 200

a)

82%

b)

16.4%

c)

32.8%

d)

80%

180.

Write 130ml as a percentage of 1000ml

a)

13%

b)

1.3%

c)

130%

d)

26%

181.

Write 60 marks out of 80 marks as a percentage

a)

60%

b)

75%

c)

80%

d)

20%

182.

Gertrude receives £5 from her grandmother. She gives £1.50 to her sister. What percentage did Gertrude keep?

a)

30%

b)

15%

c)

70%

d)

35%

183.

Hannah scored 60 out of 90 in a French test, 50 out of 80 in a drama test, 85 out of 130 in an art test and 13 out of 20 in a maths test.


In which subject did she score the highest percentage?

a)

French

b)

Drama

c)

Art

d)

Maths

184.

Write 164 as a percentage of 200

a)

82%

b)

16.4%

c)

32.8%

d)

80%

185.

Sodium and Bromine will make a _____ bond

a)

Ionic

b)

Hydrogen

c)

Covalent

d)

Exploding

186.

the mutual sharing of one or more pairs of electrons between two atoms.

a)

Covalent

b)

Ionic

187.

type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound.

a)

Ionic

b)

Covalent

188.

 

This type of bonding can be described as "I give, I get"

a)

Covalent

b)

my mom

c)

Ionic

d)

Friendship

189.

Why do all bonds form?

a)

filling the outermost energy level

b)

to win

c)

to make other atoms unstable

d)

to be famous

190.

What two types of atoms make a covalent bond?

a)

2 Metal

b)

2 Ionic

c)

1 nonmetal 1 metal

d)

2 Nonmetal

191.

 

NaCl

a)

metallic

b)

covalent

c)

Ionic

192.

Hydrogen and Chlorine will from a ____ bond

a)

Unique

b)

bestie

c)

Covalent

d)

Ionic

193.

Conducts electricity well when melted or dissolved

a)

Conductor

b)

Ionic

c)

Covalent

194.

Beryllium and sulfur will form a ____ bond

a)

Covalent

b)

Metallic

c)

Ionic

d)

Unique

195.

Poor electrical conductivity

a)

Ionic

b)

Covalent

c)

among us

196.

In ionic bonds, metals tend to?

a)

Keep their electrons

b)

Gain valence electrons

c)

Lose valence electrons

d)

None of these answers are correct

197.

MgO

a)

Ionic

b)

Metallic

c)

Covalent

198.

What type of bond involves the sharing of electrons between atoms?

a)

James Bond

b)

Covalent Bond

c)

Ionic Bond

d)

Both Covalent and Ionic bonds

199.

Why don't noble gases form bonds?

a)

They all have a full octet

b)

Noble gases do form bonds

c)

They only bond when with eachother

d)

none of these answers are correct

200.

 

This type of bonding can be described as a "cooperation"

a)

Diverse

b)

Ionic

c)

Covalent

201.

Water, H2O, forms what type of bond?

a)

Ionic

b)

Covalent

c)

Water

d)

James

202.

When metals bond with non-metals they form what type of bonds

a)

Ionic

b)

Covalent

203.

An ionic compound forms between a?

a)

2 nonmetals

b)

metal and nonmetal

c)

2 metals

d)

noble gasses

204.

 

Some are solids, some are liquids, and some are gases at room temperature.

a)

Ionic

b)

Covalent

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