Free Printable Chem A Study Guide

1.

What particle view below is a mixture?

a)

b)

c)

d)

2.

What is the best classification for this substance?

a)

An element

b)

A compound

c)

A mixture

3.

Is this a pure substance?

a)

Yes

b)

No

4.

What is an example of a physical property?

a)

Silver is shiny

b)

Alcohols are flammable

c)

Alkali metals are reactive with water

d)

Acids are sometimes corrosive

5.

What is an example of a chemical change?

a)

Tearing paper

b)

Dissolving salt in water

c)

Melting ice

d)

Burning wood

6.

Is this image showing a homogeneous or a heterogeneous mixture? Image: Cesar salad

a)

homogeneous

b)

heterogeneous

7.

Does this image represent a chemical or a physical change?

a)

Chemical change

b)

Physical change

8.

Which below shows a CHEMICAL change?

a)

b)

c)

9.

What is a pure substance that cannot be broken down into any other substance by physical or chemical means. Ex: Gold, Silver, Oxygen, & Nitrogen

a)

element

b)

compound

c)

mixture

d)

salad

10.

What is an atom which has gained or last electrons called?

a)

isotope

b)

atom

c)

ion

d)

balanced

11.

What type of property can only be observed by changing the substance into a new substance. Ex: Flammability, oxidation

a)

chemical

b)

physical

12.

Air is an example of a(n)

a)

element

b)

compound

c)

heterogenous mixture

d)

homogenous mixture

13.

Phase changes (going from a solid to a liquid to a gas) are what types of changes?

a)

chemical

b)

physical

14.

On the Periodic Table each element increases by one _________

a)

electron

b)

proton

c)

neutron

d)

letter

15.

A row across the Periodic Table where each element has the same number of energy shells

a)

column

b)

family

c)

period

16.

In a family or column, the elements have similar properties because they all have the same number of

a)

protons

b)

neutrons

c)

valence electrons

d)

electrons

17.

What is the octet rule? How many valence electrons can the first three periods hold?

a)

8

b)

2

c)

2 8 8

d)

2 8 16

18.

Whether or not bonds form is due to the ?????

a)

valence electron configurations

b)

protons

c)

atomic mass

d)

chance

19.

When heat is added to matter, the molecules tend to

a)

move faster and farther apart

b)

slow down

c)

nothing, heat has no impact on the state of matter

d)

freeze

20.

What is the volume in this graduated cylinder?

a)

5.8 mL

b)

50.8 mL

c)

53.0 mL

d)

58.0 mL

21.

What is a unit that could be used to measure the MASS of an object?

a)

milliliter (mL)

b)

centigram (cg)

c)

kilometer (km)

d)

centimeter cubed (cm³)

22.

The formula for density is $D\ =\ \frac{m}{V}$ , what is this equation rearranged for $m$ ?

a)

$m\ =\ \frac{D}{V}$

b)

$m\ =\ \frac{V}{D}$

c)

$m\ =\ V\times D$

d)

$m\ =\ D+V$

23.

Volume is....

a)

The amount of matter in an object.

b)

measured with a balance or scale.

c)

The same as mass.

d)

How much space an object takes up.

24.

Find the density of an object that has a mass of 40.5 g and a volume of 2.8 mL

$D\ =\ \frac{m}{V}$

a)

14.5 g/mL

b)

0.07 g/mL

c)

113.4 g/mL

d)

37.7 g/mL

25.

What is the volume of a block of aluminum (density = 2.7 g/cm³) if it has a mass of 93.4 g?

a)

90.7 cm³

b)

34.6 cm³

c)

0.03 cm³

d)

252.2 cm³

26.

Use the image below to find the volume of the object. A is before the rock is added, B is after the rock is added.

a)

30 mL

b)

60 mL

c)

90 mL

d)

150 mL

27.

What is the volume of liquid in this graduated cylinder?

a)

30.7 mL

b)

31.7 mL

c)

32.0 mL

d)

37.0 mL

28.

What is the volume of liquid in this graduated cylinder?

a)

4.7 mL

b)

5.7 mL

c)

5.4 mL

d)

4.2 mL

29.

The type of bond formed when electrons are shared between atoms is a

a)

ionic bond

b)

covalent bond

c)

hydrogen bond

d)

peptide bond

30.

The electrons in the outermost energy level are called

a)

valence

b)

ions

c)

covalent

d)

farthest out

31.

This reaction is showing energy being _____________

a)

Absorbed

b)

Released

c)

There is no change in energy shown

32.

Chemical reactions start with _____________ and end with _______________

a)

Reactants, Products

b)

Products, Reactants

c)

Substances, Chemicals

d)

Chemicals, Compounds

33.

If an atom has 2 valence electrons, what kind of bond will it most likely form

a)

ionic

b)

covalent

c)

hydrogen

d)

peptide

34.

A molecule with an uneven distribution of charge over the molecule is called

a)

lopsided

b)

bonded

c)

negative

d)

polar

35.

What is a property you would expect a metal to have?

a)

It will not conduct electricity.

b)

It is dull.

c)

It is brittle.

d)

It is malleable.

36.

What pair of elements are in the same PERIOD?

a)

Scandium (21) and Bromine (35)

b)

Scandium (21) and Yttrium (39)

c)

Helium (2) and Neon (10)

d)

Iodine (53) and Astatine (85)

37.

What element below is in the same GROUP as Aluminum (13)

a)

Sodium (11)

b)

Thallium (81)

c)

Silicon (14)

d)

Argon (18)

38.

What statement below is true about the periodic table?

a)

The heavier the element, the more likely it is to be a gas.

b)

Elements in the same PERIOD share similar properties.

c)

Elements in the same GROUP share similar properties.

d)

Elements are arranged by date of discovery, from earliest to most recent.

39.

Selenium has atomic number of 34, what does this tell us?

a)

It has a mass of 34.

b)

It has 34 protons.

c)

It has 34 neutrons.

d)

It was the 34th element discovered.

40.

How many electrons are in a NEUTRAL atom of boron?

a)

5

b)

6

c)

10

d)

11

41.

What particles are found in the nucleus of an atom?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

d)

Protons, neutrons and electrons

42.

Carbon and Sulfur are examples of...

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Gases

43.

In the atom diagram shown, A is pointing to the darker particles, these are known as

a)

electrons

b)

protons

c)

neutrons

d)

the nucleus

44.

In the atom diagram shown, E is pointing to

a)

An electron

b)

a proton

c)

a neutron

d)

the nucleus

45.

B and C are found in the ______ of an atom.

a)

electron cloud

b)

Space

c)

Nucleus

d)

Outside

46.

What charge does an electron have?

a)

Negative

b)

Positive

c)

Neutral

d)

Contrated

47.

What is the atomic mass of this atom?

a)

1

b)

3

c)

4

d)

7

48.

What is the atomic number of this atom?

a)

4

b)

5

c)

9

d)

none of the above

49.

What is a valence electron?

a)

an electron that is found in the outermost orbital of an atom.

b)

an electron found in the innermost orbital of an atom.

c)

an electron found in the middle orbital.

50.

Using the information provided, determine how many electrons the a Boron atom contains.

a)

2.5

b)

5

c)

6

d)

10.81

51.

The atomic number of an element is determined by the _________ of ________ in the nucleus.

a)

protons, neutrons

b)

number, electrons

c)

electrons, protons

d)

number, protons

52.

Elements are _________ 1 type of atom.

a)

Made of

b)

Tiny

c)

chemical formula

53.

How many Carbon atoms are in this compound

a)

6

b)

7

c)

3

54.

How many significant figures: 216 m

a)

1

b)

2

c)

3

d)

0

55.

How many significant figures: 153.0 mL

a)

1

b)

2

c)

3

d)

4

56.

Round 1047.78 to three sig figs

a)

104

b)

105

c)

1050

d)

1050.00

57.

Calculate 12.34 + 1.234 + 0.1234 and give your answer with the correct number of significant figures.

a)

13.6974

b)

13.697

c)

13.70

d)

13.7

58.

What is the volume of liquid in this graduated cylinder?

a)

43.0 mL

b)

43 mL

c)

43.05 mL

d)

44.5 mL

59.

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

60.

This bullseye demonstrates...

a)

High Accuracy & High Precision

b)

High Accuracy & Low Precision

c)

Low Accuracy & High Precision

d)

Low Accuracy & Low Precision

61.

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

62.

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

63.

Change from standard form to scientific notation: 12,000,000

a)

12.0 x 10⁷

b)

0.12 x 10⁷

c)

1.2 x 10⁶

d)

1.2 x 10⁷

64.

Change from standard form to scientific notation: 0.004078

a)

4.078 x 10^-3

b)

4.078 x 10³

c)

40.78 x 10^-4

d)

.4078 x 10^-2

65.

Try to change the number back to standard form: 6.79 x 10⁴

a)

679,000

b)

6,790

c)

67,900

d)

6,790,000

66.

Multiply:
(9.4 x 10⁶)(3.2 x 10⁵)

a)

30.08 x 10¹¹

b)

3.8 x 10¹

c)

3.008 x 10¹²

d)

2.9375 x 10¹

67.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

68.

Which of the following would increase the (gas) pressure of a system?

a)

Increase the Temperature

b)

Pump in more gas

c)

Decrease the volume

d)

All of these

69.

In order to convert to Kelvin, you add ______ to the Celsius measurement.

a)

372

b)

273

c)

237

d)

732

70.

What is 50 °C in Kelvin?

a)

223

b)

323

c)

100

d)

50

71.

Charles' Law States...

a)

As Pressure goes up volume goes down

b)

As Pressure goes up temperature goes up

c)

As Volume goes up temperature goes up

d)

As Pressure goes down volume goes down

72.

Which container is higher in temperature?

a)

left

b)

right

c)

both have the same temperature

d)

I don't know

73.

What three variables are in the Ideal Gas Law?

a)

Pressure, Temperature, Volume

b)

Pressure, Kelvin, # of moles

c)

# of moles, Temperature, Volume

d)

Volume, Heat, and Greenhouse Gases

74.

Decreasing the pressure of a gas causes

a)

increased volume

b)

decreased volume

75.

In which state are the particles least able to move? (Which is the solid?)

a)

State A

b)

State B

c)

State C

d)

None

76.

Which container will have higher pressure?

a)

First container

b)

second container

77.

The change of one state of matter to another is called

a)

Osmosis

b)

Phase Change

c)

Matter

d)

Energy

78.

Transition from a liquid to a gas

a)

Condensation

b)

Freezing

c)

Evaporation

d)

Melting

79.

Three containers with the same amount of the same material are shown below. Which container has the substance with the highest amount of energy?

a)

The container on the left

b)

The middle container

c)

The container on the right

d)

All have an equal amount of energy

80.

Three containers with the same amount of the same material are shown below. Which container has the substance with the lowest amount of energy?

a)

The container on the left

b)

The middle container

c)

The container on the right

d)

All have an equal amount of energy

81.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma!!!

82.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

83.

Based on this photo, when liquid turning to gas is which of the following down below?

a)

Consensation

b)

Freezing

c)

Evaporation

d)

Melting

84.

What is the freezing temperature of the material?

a)

0oC

b)

100oC

c)

-25oC

d)

225oC

85.

What is the boiling temperature of the material?

a)

0oC

b)

100oC

c)

-25oC

d)

225oC

86.

At what TIME does the material enter the phase change from solid to liquid

a)

~5min

b)

~10 MIN

c)

~15min

d)

~25min

87.

At what TIME does the material enter the phase change from liquid to gas

a)

~5min

b)

~15 min

c)

~25min

d)

~35min

88.

As time increases, what is happening to the motion of molecules in the material?

a)

increasing

b)

decreasing

89.

In region B, identify the state(s) of matter

a)

gas

b)

liquid

c)

solid

90.

In region D, identify the state(s) of matter

a)

gas

b)

liquid

c)

solid

91.

In region A, identify the state(s) of matter

a)

gas

b)

liquid

c)

solid

92.

In region E, identify the state(s) of matter

a)

gas

b)

liquid

c)

solid

93.

In region C, identify the state(s) of matter

a)

gas

b)

liquid

c)

solid

94.

In order to convert 25 km to miles using dimensional analysis, which conversion factor should be used?

a)

$\frac{1\ mi}{5280\ ft}$

b)

$\frac{1\ km}{0.62137\ mi}$

c)

$\frac{0.62137\ mi}{1\ km}$

95.

Which conversion factor would you use to convert from cm to inches?

a)

$\frac{1\ in}{2.54\ cm}$

b)

$\frac{2.54\ cm}{1\ in}$

c)

$\frac{2.54\ in}{1\ cm}$

96.

Which conversion factor would you use to convert 819 mL to L?

a)

$\frac{1\ L}{1000\ mL}$

b)

$\frac{1000\ L}{1\ mL}$

c)

$\frac{1000\ mL}{1\ L}$

97.

Choose the correct conversion factor and answer for this conversion:
$8,203\ mL\ \times\ \frac{1\ L}{1000\ mL}\ \times\ \ \ \ \ \ \ ?\ \ \ \ \ \ \ \ =\ \ \ \ ?$

a)

$\frac{3.7854\ gal}{1\ L}\ =\ 31.05\ gal$

b)

$\frac{3.7854\ L}{1\ gal}\ =\ 31.05\ gal$

c)

$\frac{1\ gal}{3.7854\ L}\ =\ 2.167\ gal$

98.

The molecules of a liquid vs. a solid....

a)

Move slower in a liquid.

b)

Move slower in a solid.

99.

Water has a specific heat of 4184 J/KgºC. Wood has a specific heat of 1760 J/KgºC. What material needs more energy to raise the temperature 1ºC

a)

Wood

b)

Water

c)

Both are the same

100.

A high specific heat means...

a)

It heats up quickly with energy added

b)

It requires more energy to change temperature

101.

A sample of iron receives 50.J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25 g

b)

30 g

c)

20 g

d)

50 g

102.

You have 20 g of water with specific heat of 4.18 J/g°C. The 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

103.

If the same amount of heat is added to each sample, the smallest change in temperature will occur in the

a)

Iron

b)

Dry Air

c)

Granite

d)

Water

104.

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy. What material would be the coolest after being heated?

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

105.

Energy is transferred as heat between two objects of ___________ temperatures.

a)

differing

b)

same

106.

The measure of average kinetic energy of all the particles within an object is called ____________.

a)

temperature

b)

conduction

c)

radiation

d)

heat

107.

When you measure the temperature of hot soup, you are measuring the:

a)

thermal energy given off by the bowl

b)

specific heat of the bowl

c)

average kinetic energy of the particles in the soup

d)

thermal expansion of the particles in the soup

108.

Heat is a flow of energy caused by

a)

specific heat

b)

density differences in solids

c)

temperature differences

d)

thermal expansion

109.

What is thermal equilibrium?

a)

When two objects are at rest at the same time.

b)

When two or more objects reach a common temperature.

c)

When two objects have the same specific heat.

110.

What is the formula to calculate heat energy required to raise the temperature of any substance?

a)

Q=mc∆t

b)

Q=mc

c)

Q= ½mv

d)

m=QC

111.

What does the C represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

element symbol

112.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

113.

Subatomic particles with a positive charge

a)

neutrons

b)

atomic mass

c)

protons

d)

isotopes

114.

Which two subatomic particles make up the nucleus of an atom?

a)

Protons and Electrons

b)

Neutrons and Electrons

c)

Electrons and Protons

d)

Protons and Neutrons

115.

Where are the Electrons found in the structure of an atom?

a)

In the nucleus

b)

In spaces around the nucleus

116.

Subatomic particles that are neutral in charge

a)

Neutrons

b)

Protons

c)

Nucleus

d)

Electrons

117.

What does the C represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

element symbol

118.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

119.

Is this the correct Bohr model for carbon (C) if carbon has 6 protons?

a)

Yes

b)

No

120.

An atom has a full first energy level (electron shell) and 5 electrons in its second level (shell). How many electrons does this atom have?

a)

2

b)

7

c)

9

d)

Need more information

121.

Is this the correct Bohr model for helium (He) if helium has 2 electrons?

a)

Yes

b)

No

122.

How many electrons will be in the 1st shell, 2nd shell, 3rd shell, and or 4th shell? (electrons = 20)

a)

2, 8, 8, 3

b)

2, 8, 8, 0

c)

2, 8, 8, 1

d)

2, 8, 8, 2

123.

What subatomic particle determines the name of the element?

a)

Electron

b)

Proton

c)

Neutron

d)

Boson

124.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

125.

What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

none of the above

126.

What is the mass of this atom?

a)

9

b)

10

c)

19

d)

28

127.

How many electron shells does this element have

a)

7

b)

5

c)

3

d)

2

128.

If the element, Silicon, had a mass of 30.22 amu and had 16 protons,

how many neutrons would it have?

a)

15 neutrons

b)

14 neutrons

c)

16 neutrons

d)

13 neutrons

129.

If the atomic number of sodium (Na) is 11 and sodium (Na) has 10 neutrons and 11 electrons,

what is the mass of sodium (Na) ? _ amu

(a)

130.

Which of the following is true about subatomic particles?

a)

The mass of a neutron is much lighter than the mass of a proton.

b)

Electrons are negatively charged and are the lightest subatomic particle.

c)

Protons are positively charged and the lightest subatomic particle.

d)

Neutrons have no charge and are the lightest subatomic particle.

131.

What is the mass number of an atom that has 20 protons, 20 neutrons, and 20 electrons?

a)

20

b)

40

c)

60

d)

80

132.

Which scientist's model is referred to as the Plum Pudding Model?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

133.

Which scientist was the first person responsible for proposing the idea of atoms?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

134.

Which scientist's model is referred to as the Planetary model?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

135.

Which model of the atom is the most up to date model?

a)

The Billiard Ball Model

b)

The Plum Pudding Model

c)

The Planetary Model

d)

The Wave Mechanical Model

e)

The Nuclear Model

136.

In the atomic model nicknamed the "plum pudding" model, what do the plums represent?

a)

the nucleus

b)

the atom

c)

the electrons

d)

the positive material

137.

This is a correct dot diagram for fluorine (F)

a)

true

b)

false

138.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

139.

What element has this electron configuration?

a)

hydrogen

b)

helium

c)

lithium

d)

beryllium

140.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

141.

What element has this electron configuration?

a)

helium

b)

lithium

c)

beryllium

d)

boron

142.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

143.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

144.

Which element is represented by this electron configuration?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

145.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

146.

Which of the following is the electron configuration for Fluorine

a)

b)

c)

d)

147.

Which of the following is the electron configuration for neon?

a)

b)

c)

d)

148.

Which of the following is the electron configuration for silicon?

a)

b)

c)

d)

149.

Which of the following is the orbital notation for oxygen?

a)

b)

c)

d)

150.

An electron occupies the lowest energy orbital that can receive it.

a)

Hund’s rule

b)

Pauli exclusion principle

c)

Bohr model of the atom

d)

Aufbau principle

151.

All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

d)

Core Notation

152.

No two electrons in the same atom can have the same four quantum numbers.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

d)

Noble gas notation

153.

Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?

a)

Hund's

b)

Aufbau's

c)

Pauli's Exclusive

154.

Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?

a)

Aufbau's

b)

Hund's

c)

Pauli exclusive

155.

Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

156.

What is the element?

a)

Neon

b)

Chlorine

c)

Aluminum

d)

Argon

157.

What is the element?

a)

sulfur

b)

chlorine

c)

phosphorus

d)

silicon

158.

Which is the electron configuration for beryllium?

a)

b)

c)

d)

159.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

160.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

161.

Which element is pictured?

a)

neon

b)

fluorine

c)

magnesium

d)

argon

162.

How many d orbitals are there in a given sublevel?

a)

1

b)

3

c)

5

d)

7

163.

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

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

164.

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

165.

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

a)

Ar

b)

He

c)

Kr

d)

Rn

166.

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.

167.

What is the name of family I

a)

Alkaline Earth Metals

b)

Boron Family

c)

Alkali Metals

d)

Halogen Family

168.

Families all have similar

a)

Names

b)

atomic numbers

c)

atomic masses

d)

properties

169.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

170.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

171.

The rings around the nucleus of an atom are

a)

target rings

b)

sound waves

c)

energy levels

172.

When we did the flame tests, we saw light and color in the form of fire. This happened because...

a)

The atom was absorbing energy.

b)

The atom was releasing energy.

c)

The atom was exploding.

173.

Consider the following data:

Cu - blue, green, teal

Na - yellow-orange

K - yellow, orange, pink/lavender

Li - red, light red

Sr - deep red

If the unknown color was yellow-orange, which element is most likely the unknown?

a)

Cu

b)

Na

c)

K

d)

Li

174.

Consider the following data:

Cu - blue, green, teal

Na - yellow-orange

K - yellow, orange, pink/lavender

Li - red, light red

Sr - deep red

If the unknown color was yellow,orange with some pink, which element is most likely the unknown?

a)

Cu

b)

Na

c)

K

d)

Li

175.

An atomic emission spectrum is...

a)

unique to the element

b)

a complete rainbow

c)

both of these are correct

d)

neither of these are correct

176.

The location electrons are found most of the time is called

a)

electron cloud

b)

atomic emission spectrum

c)

wavelength

d)

all of these

177.

A practical application of atomic emission spectra is ....

a)

neon lights

b)

fireworks

c)

identifying unknown substances

d)

all of these

178.

How many electrons can fit on the 1st energy level (orbital) for any Bohr Model?

a)

2

b)

6

c)

8

d)

10

179.

How many electrons can fit on the 2nd energy level (orbital) for any Bohr Model?

a)

2

b)

6

c)

8

d)

10

180.

How many electrons can fit on the 3rd energy level (orbital) for any Bohr Model?

a)

2

b)

6

c)

8

d)

10

181.

?

a)

Lithium

b)

Boron

c)

Carbon

d)

Neon

182.

What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

none of the above

183.

What is a valence electron?

a)

Electrons in the first energy shell

b)

Electrons in the second energy shell

c)

Electrons in the outer shell

d)

Total number of electrons

184.

When an electron moves away from the nucleus, it

a)

moves to the ground state

b)

moves to an excited state

c)

gives off specific frequencies of light

d)

never returns

185.

When an electron is in the ground state

a)

It has fallen into the nucleus.

b)

It is in its normal orbit.

c)

It has absorbed energy to move it away from the nucleus.

d)

It is no longer part of an atom

186.

When electrons fall from an excited state to their ground state,

a)

They absorb energy from the environment.

b)

They wobble back and forth.

c)

They emit specific frequencies of light.

d)

They spin out of orbit.

187.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

188.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

189.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

190.

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

a)

true

b)

false

191.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br^-1

b)

Br⁺¹

c)

Br⁺⁷

d)

Br^-7

192.

What is the charge of an atom that has lost one electron?

a)

-1

b)

-2

c)

+1

d)

+2

193.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

194.

This atom is considered a

a)

Cation

b)

Anion

195.

This atom is considered a

a)

Cation

b)

Anion

196.

What is the ionic charge of this atom?

a)

-2

b)

-1

c)

+1

d)

+2

197.

What is the ionic charge of this atom?

a)

-2

b)

-1

c)

+1

d)

+2

Chem A Study Guide

Total questions: 197

Worksheet time: 99hrs 30mins

Similar Resources on Wayground