Free Printable Honors Fall Semester Review 25-26

1.

How can mixtures be separated?

a)

Through chemical reactions

b)

By heating to high temperatures

c)

Through physical means

d)

By adding more substances

2.

What is a homogeneous mixture?

a)

A mixture with varying composition

b)

A mixture with uniform structure throughout

c)

A mixture with visibly different parts

d)

A mixture that separates over time

3.

Instant coffee is made by dissolving a powder in hot water. Instant coffee is a ___________________.

a)

pure substance

b)

mixture

4.

Cake batter is a substance that may contain flour, eggs, and sugar mixed by hand or with an electric mixer. Cake batter is a ___________________ .

a)

pure substance

b)

mixture

5.

What is an element?

a)

A substance that can't be broken down into other substances

b)

The trio: Fire, Water, Ice

c)

Who knows?

d)

A mixture of two substances

6.

Chalk is a mineral found in rocks. It contains carbon, oxygen, and calcium atoms. Chalk is a ___________________ .

a)

element

b)

compound

7.

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

8.

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

9.

How many protons are in a sodium atom (Na)? (Tap to enlarge the periodic table.)

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons.

10.

What is a characteristic property of alkali metals?

a)

Non-reactivity with halogens.

b)

Formation of acidic oxides when reacting with oxygen.

c)

High reactivity with water and formation of alkaline hydroxides.

d)

Low melting points compared to other metals.

11.

How does the atomic radius change as you move down the alkali metal group?

a)

The atomic radius decreases as you move down the alkali metal group.

b)

The atomic radius increases as you move down the alkali metal group.

c)

The atomic radius remains constant as you move down the alkali metal group.

d)

The atomic radius first decreases and then increases as you move down the alkali metal group.

12.

Which alkali metal is the most reactive?

a)

Cesium

b)

Potassium

c)

Sodium

d)

Lithium

13.

What are the common uses of noble gases?

a)

Common uses of noble gases include lighting, welding, cryogenics, and lasers.

b)

Batteries and power storage

c)

Air purification systems

d)

Water treatment processes

14.

How do noble gases differ from other groups in terms of reactivity?

a)

Noble gases tend to lose electrons easily.

b)

Noble gases readily form compounds with other elements.

c)

Noble gases are much less reactive than other groups due to their full valence electron shells.

d)

Noble gases are highly reactive due to their incomplete electron shells.

15.

What is a key property of transition metals?

a)

They can form different ions

b)

They cannot form complex ions.

c)

They have a fixed oxidation state.

d)

They are all nonmetals.

16.

What is the trend of ionization energy across a period?

a)

Ionization energy fluctuates randomly across a period.

b)

Ionization energy increases across a period.

c)

Ionization energy remains constant across a period.

d)

Ionization energy decreases across a period.

17.

How does electronegativity change as you move from left to right across a period?

a)

Electronegativity decreases from left to right across a period.

b)

Electronegativity remains constant across a period.

c)

Electronegativity fluctuates randomly across a period.

d)

Electronegativity increases from left to right across a period.

18.

Which element is the most electronegative on the periodic table?

a)

Oxygen

b)

Fluorine

c)

Nitrogen

d)

Chlorine

19.

How does the atomic radius change across a period?

a)

The atomic radius increases across a period.

b)

The atomic radius fluctuates randomly across a period.

c)

The atomic radius remains constant across a period.

d)

The atomic radius decreases across a period.

20.

Which group of elements has a full valence shell?

a)

Transition metals

b)

Noble gases

c)

Halogens

d)

Alkali metals

21.

What is the general trend of atomic radius as you move down a group?

a)

The atomic radius first increases and then decreases as you move down a group.

b)

The atomic radius decreases as you move down a group.

c)

The atomic radius increases as you move down a group.

d)

The atomic radius remains constant as you move down a group.

22.

Which of the following elements is a transition element?

a)

Zinc (Zn)

b)

Argon (Ar)

c)

Silicon (Si)

d)

Phosphorus (P)

23.

Which of the following elements is an alkaline earth metal?

a)

Potassium (K)

b)

Strontium (Sr)

c)

Iron (Fe)

d)

Copper (Cu)

24.

Identify the element located in Group 16 and Period 3 of the periodic table.

a)

Oxygen (O)

b)

Sulfur (S)

c)

Selenium (Se)

d)

Tellurium (Te)

25.

Identify the element located in Group 2, Period 4 of the periodic table.

a)

Calcium (Ca)

b)

Magnesium (Mg)

c)

Beryllium (Be)

d)

Strontium (Sr)

26.

Elements that belong to the same group have the same number of

a)

valence electrons

b)

neutral electrons

c)

inner electrons

d)

total electrons

27.

An atom has 10 protons, 15 neutrons, and 10 electrons. What is its mass number?

a)

20

b)

10

c)

35

d)

25

28.

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is

a)

13

b)

14

c)

27

d)

40

29.

How many neutrons does an atom of Au (gold) have?

a)

79 neutrons

b)

118 neutrons

c)

196 neutrons

d)

197 neutrons

30.

Is this the correct Bohr model for carbon (C), given that carbon has 6 protons?

a)

Yes

b)

No

31.

According to the Bohr model, what is the maximum number of electrons that the FIRST shell can hold?

a)

2

b)

6

c)

16

d)

8

32.

What is the name of this element?

a)

Helium

b)

Hydrogen

c)

Argon

d)

Silver

33.

Which element is represented in this Bohr model?

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Lithium

34.

Which element is represented in this Bohr model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

35.

Which of the following statements is true about nuclear reactions?

a)

The identity of the atom does not change.

b)

Only the arrangement of molecules changes.

c)

The nucleus is affected, and the identity of the atom changes.

d)

The atoms remain unchanged.

36.

Why do chemical reactions not result in the formation of new elements?

a)

Because only the nucleus is affected.

b)

Because the atoms maintain their identity and only molecules are rearranged.

c)

Because atoms are destroyed.

d)

Because protons are added to the nucleus.

37.

If an atom is written as Radium-228, what does the number 228 represent?

a)

Atomic number

b)

Number of protons

c)

Mass number

d)

Number of electrons

38.

Given the nuclide notation for Radium-228, how do you determine the number of neutrons in the nucleus?

a)

Subtract the atomic number from the mass number

b)

Add the atomic number and mass number

c)

Subtract the mass number from the atomic number

d)

Multiply the atomic number by the mass number

39.

What type of force holds protons and neutrons together in the nucleus of an atom?

a)

Gravitational force

b)

Nuclear force

c)

Magnetic force

d)

Frictional force

40.

Why do protons in the nucleus not fly apart, despite their electric repulsion?

a)

Because of gravity

b)

Because of the strong nuclear force

c)

Because of magnetic attraction

d)

Because of chemical bonds

41.

What is an alpha particle (α) in terms of its composition?

a)

A hydrogen nucleus

b)

A helium nucleus

c)

A neutron

d)

An electron

42.

Why do alpha particles have weak penetrating ability?

a)

They are very small

b)

They are electrically neutral

c)

They are relatively large and interact easily with matter

d)

They move at the speed of light

43.

What is a beta particle (β) in the context of nuclear reactions?

a)

A proton emitted from a nuclear reaction

b)

A neutron emitted from a nuclear reaction

c)

An electron emitted from a nuclear reaction

d)

A photon emitted from a nuclear reaction

44.

Which material can stop beta particles from passing through?

a)

Paper

b)

Water

c)

Foil

d)

Plastic

45.

Which of the following correctly represents the symbol for a beta particle?

a)

$^{4}_{2}\alpha$

b)

$^{1}_{1}p$

c)

$^{0}_{-1}e$

d)

$^{0}_{0}\gamma$

46.

Which of the following statements is true about gamma emission?

a)

It changes the identity of the atom.

b)

It does not change the identity of the atom.

c)

It always produces a new element.

d)

It only occurs in living organisms.

47.

Which material is required to effectively stop gamma radiation?

a)

Tissue

b)

Aluminum

c)

Concrete wall or lead

d)

Plastic

48.

What happens to the atomic number during positron emission?

a)

It increases by 1.

b)

It stays the same.

c)

It decreases by 2.

d)

It decreases by 1.

49.

Which of the following best describes the charge of a positron?

a)

Negative

b)

Neutral

c)

Positive

d)

Double positive

50.

Which of the following best describes electron capture?

a)

An inner orbital electron is captured by its own atom.

b)

An atom emits an alpha particle.

c)

An atom loses a neutron.

d)

An atom gains a proton from another atom.

51.

What type of nuclear reaction is this?

a)

alpha

b)

beta

c)

gamma

d)

hot

52.

Which type of nuclear radiation is being emitted here?

a)

Alpha

b)

Beta

c)

Gamma

d)

none

53.

What type of reaction is this?

a)

alpha

b)

beta

c)

gamma

d)

quiet

54.

What type of reaction is this?

a)

Alpha

b)

Beta

c)

Gamma

55.

If the half-life of uranium-232 is 70 years, how many half-lives will it take for 10 g of it to be reduced to 1.25 g?

a)

1 half-life

b)

2 half-lives

c)

3 half-lives

d)

4 half-lives

56.

What is the half-life of iodine-131?

a)

32 days

b)

8 days

c)

16 days

d)

24 days

57.

The maximum distance from the equilibrium/origin line to the top of the crest or the bottom of the trough is called the __________ of the wave.

a)

amplitude

b)

wavelength

c)

frequency

d)

speed

58.

The distance from one point to the next identical point(from crest to crest) on a wave is called the ________________.

a)

waveform

b)

peak

c)

amplitude

d)

wavelength

59.

Which letter(s) represent the crest of the wave?

a)

A

b)

B & D

c)

B & F

d)

F

60.

A wave with a large wavelength will have a ______ frequency and _____ energy

a)

high, low

b)

high, high

c)

low, high

d)

low, low

61.

Low frequency waves have _________ wavelengths.

a)

varying

b)

long

c)

the same

d)

short

62.

High frequency waves have _________ wavelength.

a)

varying

b)

long

c)

the same

d)

short

63.

The number of waves that occur in one second is...

a)

frequency

b)

wave speed

c)

amplitude

d)

wavelength

64.

Which wave in the diagram has the longest wavelength?

a)

1

b)

2

c)

3

d)

4

65.

The greater the frequency, the ________ energy carried by the wave.

a)

more

b)

less

66.

A high-frequency wave has ___________ than a low-frequency wave

a)

a longer wavelength

b)

a shorter wavelength

c)

the same wavelength

d)

a stronger source

67.

Which letter(s) represent the trough of the wave?

a)

A

b)

B & D

c)

D

d)

C & G

68.

Which vocabulary term is used to identify the distance between points C & G?

a)

Amplitude

b)

Crest

c)

Frequency

d)

Wavelength

69.

The unit of frequency is ___.

a)

meters

b)

nanometers (nm)

c)

m/s

d)

Hertz

70.

Which wave has a longer wavelength?

a)

wave C

b)

wave D

71.

Which wave has a greater frequency?

a)

A

b)

B

72.

Which property of these waves differs?

a)

Frequency

b)

Wavelength

c)

Amplitude

d)

Pitch

73.

These waves have the same

a)

amplitude

b)

frequency

c)

period

d)

wavelength

74.

What atom matches this electron configuration?

1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

75.

What is the energy of a photon of blue light that has a frequency of 6.31 x 10¹⁴ Hz? (h=6.626x10^-34 J sec)

a)

4.75 x 10^-7 J

b)

4.18 x 10^-19 J

c)

6.31 x 10¹⁴ J

d)

9.44 x 10^-32 J

e)

2.39 x 10^-32 J

76.

The relationship between wavelength and frequency is λ=c/f. Calculate the wavelength of light that has a frequency of 5.2 x 10¹²Hz. The speed of of light is 3.0x 10⁸ m/s.

a)

5.8 x 10 ^-5 m

b)

5.8 x 10 ^-7 m

c)

5.19 x 10 ¹⁴ m

d)

1.56 x 10 ²³ m

77.

What is the wavelength (λ) of electromagnetic radiation with a frequency (ν) of 9.01 x 10¹⁵ s^-1 ?

a)

3.32 x 10^-8 m

b)

6.66 x 10^-7 m

c)

4.13 x 10^-9 m

d)

1.88 x 10¹⁵ m

78.

What is a characteristic property of alkali metals?

a)

Non-reactivity with halogens.

b)

Formation of acidic oxides when reacting with oxygen.

c)

High reactivity with water and formation of alkaline hydroxides.

d)

Low melting points compared to other metals.

79.

How does the atomic radius change as you move down the alkali metal group?

a)

The atomic radius decreases as you move down the alkali metal group.

b)

The atomic radius increases as you move down the alkali metal group.

c)

The atomic radius remains constant as you move down the alkali metal group.

d)

The atomic radius first decreases and then increases down the alkali metal group.

80.

Which alkali metal is the most reactive?

a)

Cesium

b)

Potassium

c)

Sodium

d)

Lithium

81.

What are the common uses of noble gases?

a)

Common uses of noble gases include lighting, welding, cryogenics, and lasers.

b)

Batteries and power storage

c)

Air purification systems

d)

Water treatment processes

82.

How do noble gases differ from other groups in terms of reactivity?

a)

Noble gases have a tendency to lose electrons easily.

b)

Noble gases readily form compounds with other elements.

c)

Noble gases are much less reactive than other groups due to their full valence electron shells.

d)

Noble gases are highly reactive due to their incomplete electron shells.

83.

What is a key property of transition metals?

a)

They can form different ions

b)

They cannot form complex ions.

c)

They have a fixed oxidation state.

d)

They are all nonmetals.

84.

What is the trend in ionization energy across a period?

a)

Ionization energy fluctuates randomly across a period.

b)

Ionization energy increases across a period.

c)

Ionization energy remains constant across a period.

d)

Ionization energy decreases across a period.

85.

How does electronegativity change as you move from left to right across a period?

a)

Electronegativity decreases from left to right across a period.

b)

Electronegativity remains constant across a period.

c)

Electronegativity fluctuates randomly across a period.

d)

Electronegativity increases from left to right across a period.

86.

What is the most electronegative element on the periodic table?

a)

Oxygen

b)

Fluorine

c)

Nitrogen

d)

Chlorine

87.

How does the atomic radius change across a period?

a)

The atomic radius increases across a period.

b)

The atomic radius fluctuates randomly across a period.

c)

The atomic radius remains constant across a period.

d)

The atomic radius decreases across a period.

88.

Which group of elements has a full valence shell?

a)

Transition metals

b)

Noble gases

c)

Halogens

d)

Alkali metals

89.

What is the general trend of atomic radius as you move down a group?

a)

The atomic radius first increases and then decreases as you move down a group.

b)

The atomic radius decreases as you move down a group.

c)

The atomic radius increases as you move down a group.

d)

The atomic radius remains constant as you move down a group.

90.

Which of the following elements is a transition element?

a)

Zinc (Zn)

b)

Argon (Ar)

c)

Silicon (Si)

d)

Phosphorus (P)

91.

Which of the following elements is an alkaline earth metal?

a)

Potassium (K)

b)

Strontium (Sr)

c)

Iron (Fe)

d)

Copper (Cu)

92.

Identify the element located in Group 16 and Period 3 of the periodic table.

a)

Oxygen (O)

b)

Sulfur (S)

c)

Selenium (Se)

d)

Tellurium (Te)

93.

Identify the element located in Group 2 and Period 4 of the periodic table.

a)

Calcium (Ca)

b)

Magnesium (Mg)

c)

Beryllium (Be)

d)

Strontium (Sr)

94.

Elements that belong to the same group have the same number of

a)

valence electrons

b)

neutral electrons

c)

inner electrons

d)

total electrons

95.

What is the correct name for the ionic compound with the formula $NaCl$ ?

a)

Sodium chloride

b)

Sodium chlorate

c)

Sodium(I) chloride

d)

Sodium chlorite

96.

How do you write the formula for calcium chloride?

a)

$CaCl$

b)

$CaCl_2$

c)

$Ca_2Cl$

d)

$CaCl_3$

97.

What is the correct name for $CuO$ ?

a)

Copper oxide

b)

Copper(I) oxide

c)

Copper(II) oxide

d)

Copper(III) oxide

98.

Write the formula for Iron(III) oxide.

a)

$FeO$

b)

$Fe_2O_3$

c)

$Fe_3O_4$

d)

$FeO_2$

99.

What is the correct name for $KBr$ ?

a)

Potassium bromide

b)

Potassium(I) bromide

c)

Potassium bromate

d)

Potassium(I) bromate

100.

How do you write the formula for magnesium nitrate?

a)

$Mg(NO_3)_2$

b)

$MgN$

c)

$Mg_2(NO_3)_3$

d)

$Mg(NO_2)_2$

101.

What is the correct name for $Al_2O_3$ ?

a)

Aluminum oxide

b)

Aluminum(I) oxide

c)

Aluminum(II) oxide

d)

Aluminum(III) oxide

102.

Write the formula for sodium sulfate.

a)

$NaSO_4$

b)

$Na_2SO_4$

c)

$NaS$

d)

$Na_2S_2O_3$

103.

What is the correct name for $SnCl_4$ ?

a)

Tin(IV) chloride

b)

Tin(II) chloride

c)

Tin chloride

d)

Tin chlorate

104.

How do you write the formula for copper(I) sulfide?

a)

$CuS$

b)

$Cu_2S$

c)

$CuS_2$

d)

$Cu_2S_3$

105.

What is the correct name for $CaCO_3$ ?

a)

Calcium carbonate

b)

Calcium carbide

c)

Calcium(II) carbonate

d)

Calcium carbonite

106.

Write the formula for potassium permanganate.

a)

$KMnO_4$

b)

$K_2MnO_4$

c)

$KMn_2O_7$

d)

$K_2Mn_2O_7$

107.

What is the correct name for $FeCl_3$ ?

a)

Iron(III) chloride

b)

Iron(II) chloride

c)

Iron chloride

d)

Iron chlorate

108.

How do you write the formula for calcium phosphate?

a)

$Ca_3(PO_4)_2$

b)

$CaPO_4$

c)

$Ca_2PO_4$

d)

$Ca(PO_3)_2$

109.

What is the correct name for $AgNO_3$ ?

a)

Silver nitrate

b)

Silver(I) nitrate

c)

Silver nitrite

d)

Silver(I) nitrite

110.

What is the correct name for the covalent compound $CO_2$ ?

a)

Carbon monoxide

b)

Carbon dioxide

c)

Carbon trioxide

d)

Dicarbon monoxide

111.

Which of the following is the correct name for the compound $N_2O_5$ ?

a)

Dinitrogen pentoxide

b)

Nitrogen pentoxide

c)

Nitrogen dioxide

d)

Dinitrogen dioxide

112.

Name the covalent compound $PCl_3$ .

a)

Phosphorus trichloride

b)

Phosphorus chloride

c)

Phosphorus dichloride

d)

Phosphorus tetrachloride

113.

What is the correct name for the compound $SF_6$ ?

a)

Sulfur hexafluoride

b)

Sulfur fluoride

c)

Sulfur pentafluoride

d)

Sulfur tetrafluoride

114.

Which of the following is the correct name for $CCl_4$ ?

a)

Carbon tetrachloride

b)

Carbon chloride

c)

Carbon trichloride

d)

Carbon dichloride

115.

Name the covalent compound $NO_2$ .

a)

Nitrogen dioxide

b)

Nitrogen oxide

c)

Dinitrogen oxide

d)

Nitrogen trioxide

116.

What is the correct name for the compound $H_2O_2$ ?

a)

Dihydrogen dioxide

b)

Hydrogen pentoxide

c)

Hydrogen dioxide

d)

Dihydrogen oxide

117.

Which of the following is the correct name for $P_4O_{10}$ ?

a)

Tetraphosphorus decoxide

b)

Phosphorus oxide

c)

Phosphorus pentoxide

d)

Tetraphosphorus pentoxide

118.

Name the covalent compound $SO_3$ .

a)

Sulfur trioxide

b)

Sulfur dioxide

c)

Sulfur oxide

d)

Sulfur tetroxide

119.

What is the correct name for the compound $N_2H_4$ ?

a)

Dinitrogen tetrahydride

b)

Nitrogen hydride

c)

Dinitrogen hydride

d)

Nitrogen tetrahydride

120.

Draw the Lewis structure for $H_2O$ . Which of the following correctly represents the number of lone pairs on the oxygen atom?

a)

0 lone pairs

b)

1 lone pair

c)

2 lone pairs

d)

3 lone pairs

121.

For the molecule $CH_4$ , how many total valence electrons are present in the Lewis structure?

a)

6

b)

8

c)

10

d)

12

122.

Draw the Lewis structure for $NH_3$ . How many bonding pairs and lone pairs are present in the structure?

a)

3 bonding pairs, 1 lone pair

b)

2 bonding pairs, 2 lone pairs

c)

4 bonding pairs, 0 lone pairs

d)

3 bonding pairs, 0 lone pairs

123.

Which of the following molecules has a double bond in its Lewis structure?

a)

$O_2$

b)

$H_2$

c)

$F_2$

d)

$N_2$

124.

Draw the Lewis structure for $CO_2$ . How many double bonds are present in the structure?

a)

0

b)

1

c)

2

d)

3

125.

The chemical formula of tetraphosphorus heptaoxide is

a)

F₄O₁₀

b)

P₄O₇

c)

PO

d)

P₁₀O₄

126.

Covalent compounds

a)

Share electrons

b)

transfer electrons

c)

contain a sea of electrons

d)

conduct electricity

127.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

128.

VSEPR theory is to

a)

determine the number of bonding and lone pairs electrons

b)

determine the number of ECC

c)

determine the shape and geometry of molecule

d)

determine the lewis structure of molecule

129.

What is the VSEPR theory used to predict?

a)

Bond Strength

b)

Polarity

c)

Molecular Shape

d)

Electronegativity

130.

Which of the following shapes has unshared pairs of electrons on the central atom?

a)

Bipyramidal

b)

Bent

c)

Trigonal Planar

d)

Tetrahedral

131.

Which molecule would have this shape?

a)

BF₃

b)

CH₄

c)

PCl₅

d)

CO₂

132.

What molecule could this be?

a)

BF₃

b)

CH₄

c)

H₂O

d)

CO₂

133.

Who could this molecule be?

a)

CH₄

b)

CO₂

c)

PCl₅

d)

BF₃

134.

Who could this be?

a)

CO₂

b)

NH₃

c)

H₂S

d)

CH₄

135.

What molecular shape is the structure shown here? (BCl₃)

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

136.

What molecular shape is the structure shown here? (H₂O)

a)

tetrahedral

b)

trigonal planar

c)

bent

d)

trigonal pyramidal

137.

Determine the molecular shape of carbon tetrafluoride.

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

138.

This is a correct dot diagram for fluorine (F)

a)

true

b)

false

139.

What is the correct Lewis Dot Structure for ammonia NH₃

a)

b)

c)

d)

140.

Which is the correct Lewis structure for carbon dioxide?

a)

b)

c)

d)

141.

Valid Lewis dot diagram?

a)

True

b)

False

142.

Which of the following is the correct Lewis dot structure for a molecule of fluorine, F₂?

a)

b)

c)

d)

143.

Is this a valid Lewis structure for CH₂O?

a)

Yes

b)

No

144.

This is a correct dot diagram for magnesium (Mg)

a)

true

b)

false

145.

Which Lewis Dot Model drawing correctly shows an O₂ molecule?

a)

b)

c)

d)

146.

Convert $45000$ to scientific notation.

a)

$4.5 \times 10^3$

b)

$4.5 \times 10^4$

c)

$4.5 \times 10^5$

d)

$45 \times 10^3$

147.

Convert $3.2 \times 10^{-3}$ to standard notation.

a)

$0.0032$

b)

$0.032$

c)

$0.00032$

d)

$32$

148.

How many significant figures are in the number $0.004560$ ?

a)

3

b)

4

c)

5

d)

6

149.

Convert $7.89 \times 10^2$ to standard notation.

a)

$0.789$

b)

$7.89$

c)

$78.9$

d)

$789$

150.

Convert $0.00052$ to scientific notation.

a)

$5.2 \times 10^{-4}$

b)

$5.2 \times 10^{-5}$

c)

$5.2 \times 10^{-6}$

d)

$5.2 \times 10^{-3}$

151.

Convert $5.67 \times 10^3$ to standard notation.

a)

$0.567$

b)

$5.67$

c)

$56.7$

d)

$5670$

152.

Convert $2.5 \times 10^{-2}$ to standard notation.

a)

$0.025$

b)

$0.25$

c)

$2.5$

d)

$25$

153.

What is a pure substance?

a)

A mixture of different elements

b)

A sample of matter that can be broken into simpler substances

c)

A sample of matter that cannot be broken into simpler substances

d)

A combination of gases

154.

What kind of properties do pure substances have?

a)

Variable chemical and physical properties

b)

Definite chemical and physical properties

c)

Only chemical properties

d)

Only physical properties

155.

Which of the following is a pure substance?

a)

Saltwater

b)

Copper wire

c)

Soil

d)

Air

156.

Which element has the symbol 'Na'?

a)

Nitrogen

b)

Neon

c)

Sodium

d)

Nickel

157.

Which element has the symbol 'Pb'?

a)

Palladium

b)

Platinum

c)

Lead

d)

Lithium

158.

Which of the following is a pure substance?

a)

Air

b)

Saltwater

c)

H2O

d)

Sand

159.

Which of the following is NOT a characteristic of compounds?

a)

Composed of more than one kind of atom

b)

Can be separated into simpler substances

c)

Have a fixed composition

d)

Composed of only one kind of atom

160.

How can mixtures be separated?

a)

Through chemical reactions

b)

By heating to high temperatures

c)

Through physical means

d)

By adding more substances

161.

Which type of mixture is represented by a non-uniform composition?

a)

Homogeneous

b)

Heterogeneous

c)

Solution

d)

Colloidal

162.

What is a homogeneous mixture?

a)

A mixture with varying composition

b)

A mixture with uniform structure throughout

c)

A mixture with visible different parts

d)

A mixture that separates over time

163.

Which of the following best describes a homogeneous mixture?

a)

A mixture with different phases

b)

A mixture with uniform composition

c)

A mixture with visible particles

d)

A mixture that settles over time

164.

Instant coffee is made by dissolving a powder in hot water. Instant coffee is a ___________________ .

a)

pure substance

b)

mixture

165.

Cake batter is a substance that may contain flour, eggs and sugars mixed by hand or with an electric mixer. Cake batter is a ___________________ .

a)

pure substance

b)

mixture

166.

What is an Element?

a)

A substance that can't be broken down into other substances

b)

The trio: Fire, Water, Ice

c)

Who knows?

d)

A mixture of two substances

167.

Chalk is a mineral found in rocks. It contains carbon, oxygen and calcium atoms. Chalk is a ___________________ .

a)

element

b)

compound

Honors Fall Semester Review 25-26

Total questions: 167

Worksheet time: 13hrs 24mins

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