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Science Quiz on Matter and Energy

Total questions: 137

Worksheet time: 1hrs 9mins

Name
Class
Date
1.

The ability of a metal to be drawn out into thin wires is a ______________.

a)

physical property

b)

physical change.

c)

chemical property

d)

chemical change

2.

The proportions of substances in a mixture ___________________ .

a)

are always equal for each substance in the mixture

b)

can vary among the substances.

c)

never can be determined accurately.

d)

are always the same for each substance

3.

A mixture in which particles are so small they cannot be seen with a microscope is a _____________________.

a)

heterogeneous mixture

b)

suspension

c)

element

d)

solution

4.

A(n) ________ is a substance in which all the atoms in it are alike.

a)

compound

b)

solution

c)

element

d)

mixture

5.

Which of the following is a compound?

a)

oxygen

b)

silicon

c)

vinegar

d)

milk

6.

Which of the following is a substance?

a)

cheese

b)

milk

c)

tea

d)

water

7.

A change in size, shape, or state of matter is a _________________ .

a)

physical property

b)

physical change

c)

chemical property

d)

chemical change

8.

Which of the following is an example of physical weathering?

a)

acid rain corroding a statue.

b)

Formation of stalactites in a cave

c)

Formation of a canyon by a flowing stream.

d)

Change of calcium carbonate in limestone to calcium hydrogen carbonate.

9.

If using a microscope allows you to see substances in a mixture, that mixture is ____ .

a)

heterogeneous

b)

homogeneous

c)

solution

d)

microgeneous

10.

Scientists have broken down protons and neutrons into smaller particles called ___ .

a)

quarks

b)

nuclei

c)

vacuoles

d)

isotopes

11.

The number of which type of particle determines the identity of an element?

a)

neutrons

b)

electrons

c)

photons

d)

protons

12.

Vertical columns of elements are called ___________ .

a)

Periods

b)

Lines

c)

Rows

d)

Groups

13.

The atomic number of manganese is 25; its mass number is 55. How many neutrons does an atom of manganese have in its nucleus?

a)

30

b)

25

c)

55

d)

60

14.

The _________________of an atom is the number of neutrons plus protons.

a)

atomic number

b)

half-life

c)

mass number

d)

nucleus number

15.

Which of the following atomic particles is positively charged?

a)

neutrons

b)

electron

c)

Proton

d)

positron

16.

The illustration shows the upper right section of the periodic table. Which section of the table represents the metalloids?

a)

light orange shaded.

b)

dark shaded section in middle

c)

medium shaded section to the left

d)

lightly shaded section to the right

17.

Which of these elements belong to the third period of the periodic table?

a)

chlorine only

b)

carbon, oxygen and neon

c)

sodium and chlorine

d)

all of the elements

18.

Which of the following element would you expect to be least reactive?

a)

Chlorine

b)

neon

c)

carbon

d)

sodium

19.

Which of the following is a state of matter?

a)

Plasma

b)

particle

c)

thermal

d)

diffuse

20.

What is the most common state of matter in the universe?

a)

liquid

b)

solid

c)

gas

d)

Plasma

21.

On which points on the graph is water increasing in temperature?

a)

F & H

b)

F & G

c)

G & K

d)

F, G, H & K

22.

The gaseous atoms start to lose their electrons and become positively charged ions. The lost electrons are then able to float freely. This process is called ___________.

a)

Deposition

b)

De-ionization

c)

Ionization

d)

Condensation

23.

The change of a substance from solid directly to gaseous state upon heating is called __________.

a)

Sublimation

b)

Deposition

c)

Condensation

d)

De-ionization

24.

The change of a substance from gaseous state to liquid on cooling is called __________________.

a)

Deposition

b)

Sublimation

c)

De-ionization

d)

Condensation

25.

The amount of energy needed to change a substance from solid to liquid phase is the substance's ______________________ .

a)

heat of vaporization

b)

heat of transformation

c)

melting point

d)

heat of fusion

26.

A(n) ______________________ is that type of a process that gains thermal energy.

a)

exothermic reaction

b)

reactive reaction

c)

endothermic reaction

d)

Chain reaction

27.

Which of the following combination can be represented as exothermic reactions?

a)

Condensation, De-ionization & Freezing

b)

Melting, Freezing & Condensation

c)

Vaporization, Condensation and sublimation

d)

Melting, Vaporization and sublimation

28.

Which of the following combination can be represented as endothermic reactions?

a)

Vaporization, Condensation and sublimation

b)

Condensation, De-ionization & Freezing

c)

Melting, Vaporization and sublimation

d)

Melting, Freezing & Condensation

29.

A complex ion is _____.

a)

only found in compounds

b)

an ion with more than one atom

c)

a single atom that has formed an ion

d)

an ion made from large atoms

30.

Compounds that are hydrates contain which of the following?

a)

water

b)

nitrogen

c)

hydrogen chloride

d)

chlorine

31.

The name of the given compound "Na2CO3.10H2O" is _________.

a)

Watery Sodium carbonate

b)

Sodium carbonate with 10 water molecules

c)

Sodium Carbonate Decahydrate

d)

sodium carbonate

32.

_______Mn + ________HI ________H2 + __________MnI3

a)

2, 6, 3, 2

b)

2, 3, 6, 2

c)

6, 2, 3, 2

d)

6, 2, 2, 3

33.

____CoBr3 + ____CaSO4 ______CaBr2 + _______Co2(SO4)3

a)

1, 3, 3, 2

b)

3, 3, 2, 1

c)

2, 3, 3, 1

d)

3, 2, 3, 1

34.

2, 3, 6, 1 is the correct balancing of which of the following equations?

a)

Na3P + CaF2 NaF + Ca3P2

b)

LiNO3+ CaBr2 Ca(NO3)2 + LiBr

c)

HBr + Mg(OH)2 MgBr2 + H2O

d)

LiCl + Br2 LiBr +Cl2

35.

_________ turns blue litmus red.

a)

Acids

b)

Salts

c)

Bases

d)

Water

36.

__________ have sour taste.

a)

Acids

b)

Bases

c)

Salts

d)

Water

37.

Which of these acids could be hydrogen chloride?

a)

X only

b)

Y only

c)

X or Z

d)

X, Y and Z

38.

Aluminum hydroxide is used as ___________.

a)

Antacid

b)

Fertilizer

c)

Cleaner

d)

Digesting Liquid

39.

Gastric juice in stomach is a solution of ________ and water.

a)

H2SO4

b)

H2CO3

c)

HCl

d)

HNO3

40.

The pH of a concentrated solution of sodium chloride in pure water at 25ºC is .

a)

7

b)

10

c)

2

d)

8

41.

A chemical reaction between an acid and a base to form water and salt is called ___.

a)

Saltation

b)

Neutralization

c)

Basification

d)

Acidification

42.

__________ have slippery touch.

a)

Bases

b)

Acids

c)

Salts

d)

Water

43.

_______ is the rate at which energy is converted.

a)

Power

b)

Force

c)

Efficiency

d)

Effort

44.

Energy stored in chemical bonds is _______________________.

a)

chemical potential energy

b)

Gravitational potential energy

c)

Elastic potential energy

d)

kinetic energy

45.

A car engine changes chemical potential energy into the ____________ energy of the moving car.

a)

potential energy

b)

metallic energy

c)

kinetic energy

d)

photo energy

46.

Roger Federer's tennis ball has a mass of 0.3 kg. If he holds the ball above the ground at a height of 2.0 m to serve, what is its gravitational potential energy (GPE)?

a)

6J

b)

6V

c)

6W

d)

6N

47.

A baseball with a mass of 0.15 kg is moving at a speed of 40.0 m/s. Find baseball's kinetic energy.

a)

120V

b)

120J

c)

120W

d)

120N

48.

When an athlete eats a bowl of pasta, then rides in a bicycle race, energy transformation taking place is _____________________.

a)

chemical potential energy to kinetic energy

b)

kinetic potential energy to potential energy

c)

potential energy to material energy

d)

no energy transformation takes place.

49.

A material that works against the flow of electricity is _____________.

a)

a conductor

b)

resistance

c)

metal

d)

an insulator

50.

Electrons flow from areas of _________voltage to areas of ____________voltage.

a)

higher, lower

b)

lower, higher

c)

lower, lower

d)

higher to higher

51.

What is voltage?

a)

the flow of electric charge

b)

a flow of electrons that is always changing directions

c)

the difference in electrical potential between two places along an electrical circuit

d)

a flow of electrons along a circuit in one direction

52.

We measure current in a standard unit called _______________.

a)

Amperes

b)

Coloumbs

c)

Voltage

d)

Ohm

53.

In which type of circuit are there two or more branches for charge to move through?

a)

series

b)

open

c)

parallel

d)

Uniform

54.

When one lightbulb in a string of bulbs wired as a series circuit burns out, _____.

a)

all the lights go out

b)

the remaining lights are unaffected

c)

the remaining lights glow dimmer

d)

the remaining lights glow brighter

55.

According to Ohm's law, as the resistance in a circuit _______, the current _______.

a)

increases, increases

b)

increases, decreases

c)

decreases, decreases

d)

increases, remains constant

56.

What is the current through this circuit?

a)

0.80 A

b)

1.25 A

c)

30 A

d)

120 A

57.

The purpose of fuses and circuit breakers is to _____.

a)

prevent breaks in the circuit

b)

allow circuits to be overloaded

c)

prevent circuits from overheating

d)

decrease the resistance

58.

The area around the magnet's poles are the areas where the magnetic field is the ___________.

a)

strongest

b)

weakest

c)

medium

d)

normal

59.

A/An ___________________________ never loses its magnetism.

a)

Electromagnet

b)

permanent magnet

c)

compass needle

d)

North pole

60.

The south pole of a magnet will ______ the south pole of another magnet.

a)

attract

b)

first attract and then repel

c)

repel

d)

first repel and then attract

61.

Which of the following combination of elements are all magnetic materials.

a)

sulphur, carbon and hydrogen

b)

iron, carbon and sodium

c)

nickel, iron and nitrogen.

d)

iron, cobalt and nickel

62.

Magnetic lines are moving from_____________________.

a)

south to north pole inside a magnet

b)

east to south pole outside a magnet

c)

north to west pole inside a magnet

d)

north to south pole inside a magnet

63.

Which of the following best describes an electromagnet?

a)

temporary magnet

b)

unchanging magnetic properties

c)

insensitive to electric currents

d)

permanent magnet

64.

The magnetic field of an electromagnet can be increased by __________.

a)

decreasing the number of coils

b)

increasing the number of coils

c)

decreasing the current

d)

changing the direction of the current

65.

What effect does increasing the current in the wire have on an electromagnet?

a)

It decreases the strength of the magnetic field.

b)

It increases the strength of the magnetic field

c)

It has no effect on the electromagnet.

d)

It causes it to become a permanent magnet.

66.

All compasses contain a magnetized needle which points __________.

a)

east-west

b)

south-east

c)

north-south

d)

west-north

67.

Quantitative observations are recorded in the form of _______________________.

a)

detailed descriptions.

b)

precise predictions.

c)

numerical data.

d)

step-by-step procedures.

68.

The measurement 0.0254 g, rounded off to two significant figures, would be _____.

a)

2.5 x 102 g

b)

0.02g

c)

0.026g

d)

0.025g

69.

Written in scientific notation, the measurement 0.000065 cm is ________.

a)

6.5 x 10−5 cm

b)

6.5 x 10−4 cm

c)

6.5 x 10−6 cm

d)

6.5 x 10−3 cm

70.

Write the value of the given operations using scientific notation.

a)

4 x 10-2

b)

4 x 10-3

c)

4 x 10-4

d)

4 x 10-5

71.

A chemical reaction was carried out three times. The mass of the product was 8.93 g for the first trial, 8.94 g for the second trial, and 8.92 g for the third trial. The reaction is known to yield 8.60 g of product. The three mass values measured are __________.

a)

Accurate

b)

precise

c)

both accurate and precise.

d)

neither accurate nor precise.

72.

The number of significant figures in the measurement 0.000 305 kg is ___________.

a)

two

b)

six

c)

seven

d)

three

73.

Aluminum has a density of 2.70 g/cm3. What would be the mass of a sample whose Volume is 10.0 cm3?

a)

2.7g

b)

0.27g

c)

28g

d)

27g

74.

One cubic centimeter is equivalent to ____________

a)

1 gram.

b)

1 liter.

c)

1 milliliter.

d)

1 kilogram.

75.

A proposed explanation that is based on observations & that can be tested is known as a(n) ___________________.

a)

hypothesis.

b)

law.

c)

experiment.

d)

principle.

76.

A chemical bond that results from the electrostatic attraction between positive & negative ions is called a(n) __________.

a)

Covalent bond

b)

polar bond

c)

non-polar bond

d)

Ionic bond

77.

LiCl has an Electronegativity difference of 2.18, what is the type of bond?

a)

metallic bond

b)

polar covalent bond

c)

non-polar covalent bond

d)

Ionic bond

78.

In a crystal of an ionic compound, each cation is surrounded by a number of __________.

a)

negative ions.

b)

dipoles.

c)

positive ions.

d)

molecules.

79.

Use table below to choose pair of elements that will most likely have the least ionic character.

a)

O and Cl

b)

Na and Cl

c)

H and O

d)

Na and O

80.

The structure given below represents which compound?

a)

Ammonium ion

b)

Ammonium hydride

c)

Ammonium hydroxide

d)

Ammonia

81.

Compared with solid ionic compounds, solid molecular compounds generally are more brittle.

a)

true

b)

false

82.

The measure of an atom's ability to attract bonded electrons is its ______________.

a)

electronegativity

b)

polarization.

c)

ionization

d)

electron affinity

83.

In a double covalent bond, _______ are shared between the two atoms.

a)

2 electrons

b)

4 electron pairs

c)

2 electron pairs

d)

6 electron pairs

84.

In Lewis electron dot formula, _______________ electrons are represented by dots around the symbol.

a)

only valance shell

b)

total

c)

only K-shell

d)

K and L shell

85.

Actual yield are always _________ theoretical yields.

a)

greater than

b)

smaller than

c)

the same as

d)

zero as compared to

86.

A balanced chemical equation explicitly provides you with the __________.

a)

conditions under which the reaction occurs

b)

molar masses of the reactants and products.

c)

mole ratios needed to solve a stoichiometry problem

d)

conversion factors needed to solve a stoichiometry problem.

87.

The number of significant figures in an answer to a stoichiometry problem is determined only by ________.

a)

the number of significant figures of any measured quantities in the problem.

b)

the number of decimal places in the molar masses of substances in the chemical equation.

c)

the number of significant figures in the mole ratio used to solve the problem.

d)

the number of significant figures in the molar masses of substances in the chemical equation.

88.

The type of stoichiometry problem that involves the most steps is a____________.

a)

mass-to-mole conversion.

b)

mole-to-mass conversion

c)

mass-to-mass conversion.

d)

mole-to-mole conversion.

89.

Which information is not needed to solve a mass-to-mass stoichiometric calculation?

a)

the mass ratio

b)

the mole ratio

c)

molar mass of the unknown substance

d)

molar mass of a given substance

90.

Avogadro's number = ________________

a)

9.11 x 1019

b)

6.022 x 10-19

c)

6.022 x 1023

d)

6.022 x 10-23

91.

Which of the following is a colloid?

a)

water

b)

soil

c)

milk

d)

concrete

92.

When particles size in a solution & colloid are compared, the particle size in solution is _____.

a)

smaller.

b)

larger.

c)

the same size as in the colloid.

d)

either smaller or larger, depending on the colloid and the solution

93.

Which of the solution in given figure shows a Non-electrolyte?

a)

A

b)

B

c)

C

d)

all of them

94.

Which of the following solutions does not contain an electrolyte?

a)

potassium bromide-water solution

b)

hydrochloric acid solution

c)

sugar-water solution

d)

sodium chloride-water solution

95.

The formula of ammonium hydroxide is ____________________.

a)

NH2OH

b)

NH4

c)

NH4OH

d)

NH3

96.

A highly polar molecule that contains a weak bond between a hydrogen atom and another element would be ______.

a)

a strong acid.

b)

a nonelectrolyte.

c)

unable to ionize completely.

d)

a weak acid.

97.

In the following reaction, which substance acts as a Brønsted-Lowry acid?

a)

NH3

b)

NH4+

c)

HCl

d)

Cl-1

98.

pHs of 8 - 14 indicate ____________.

a)

basic

b)

Acidic

c)

Neutral

d)

Salty

99.

pH + pOH = __________.

a)

7

b)

10

c)

12

d)

14

100.

Which of the following substances is both a Brønsted-Lowry base and an Arrhenius base?

a)

NH4+

b)

HCl(g)

c)

NH3

d)

HCl(aq)

101.

What is the [OH-] in a sample of lime juice with a pH of 2.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-7 M

c)

1.0 x 10-2 M

d)

1.0 x 10-12 M

102.

The pH of a solution is 5.9. Calculate the pOH.

a)

8.1

b)

8%

c)

8.10 g

d)

8.10 moles

103.

At pH 4.4 (acidic medium), Methyl Red appear _______ in the solution.

a)

yellow

b)

green

c)

orange

d)

red

104.

A chemical reaction in which products can react to re-form reactants is called _____.

a)

stoichiometric reaction.

b)

buffered reaction.

c)

reversible reaction

d)

reforming reaction.

105.

Forward reaction goes from ______________.

a)

left to right

b)

right to left.

c)

top to bottom

d)

bottom to top.

106.

When the backward reaction is favored, there are ________ products than reactants.

a)

more

b)

equal

c)

balanced

d)

less

107.

For any reaction at chemical equilibrium, the concentrations of products & reactants ____.

a)

remain unchanged.

b)

decrease

c)

change

d)

are equal

108.

Consider the given equilibrium equation energy. At equilibrium, which reaction will be favored when extra CO gas is introduced?

a)

Forward

b)

Reverse

c)

both reverse and forward

d)

the reaction will stop

109.

What is the equilibrium expression for the following equation?

a)

A.

b)

B.

c)

C.

d)

D.

110.

If the value for 'K(eq)' is very large, then the equilibrium favors the _________ reaction.

a)

Backward

b)

forward

c)

firsst forward then backward

d)

first backward and then forward

111.

Consider the following equation: Which statement is correct?

a)

The equilibrium lies to the right.

b)

This is an example of static equilibrium.

c)

The equilibrium lies to the left.

d)

This is not an equilbrium

112.

Consider the reaction: 2HI(g) H2(g) + I2(g). At a temperature of 520°C, the equilibrium concentration of HI is 0.80 M, H2 is 0.010 M & I2 is 0.010 M. What is the K for reaction?

a)

1.3 x 10-3

b)

6.3 x 101

c)

8.0 x 103

d)

1.6 x 10-4

113.

If oxidation is taking place, what also must be occurring?

a)

Reduction

b)

Corrosion

c)

Electrolysis

d)

electroplating

114.

Another name for an oxidation-reduction reaction is _________________.

a)

Oxidizing agent

b)

Half reaction

c)

Redox reaction

d)

Reducing agent

115.

H2S is the compound primarily responsible for the odor in skunk spray. When H2S is oxidized, the odor _______.

a)

increases.

b)

decreases.

c)

remains same

d)

first increase and then decrease

116.

Sodium hypochlorite, NaOCl, is household bleach. It removes stains from clothing through a redox reaction in which the stain molecules are oxidized. Sodium hypochlorite acts as a(n) ________.

a)

oxidizing agent.

b)

reducing agent

c)

neutralizing agent.

d)

ionizing agent.

117.

The oxidation number of uncombined iodine(I2) is ______________.

a)

-1.

b)

-2.

c)

0

d)

+1

118.

The element sulfur can exist in all of the following oxidation states except _______.

a)

+5

b)

+4

c)

+6

d)

-2.

119.

The sum of the oxidation numbers for all atoms in a polyatomic ion is equal to _____________.

a)

-2.

b)

the charge of the products.

c)

the charge on that ion.

d)

0

120.

Which of the given equations is showing a non-redox reaction?

a)

Ca(OH)2(aq) + 2HCl(aq) CaCl2(aq) + 2H2O(l)

b)

CH4(g) + 2O2(g) CO2(g) + 2H2O(g)

c)

2Al(s) + 3CuCl2(aq) 2AlCl3(aq) + 3Cu(s)

d)

C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(l)

121.

Consider the given reaction: In this reaction, _________________.

a)

S(s) + O2(g) SO2(g)

b)

the oxygen is oxidized and the sulfur is oxidized.

c)

the oxygen is oxidized and the sulfur is reduced.

d)

the oxygen is reduced and the sulfur is reduced.

122.

If the particles that make up an object have more kinetic energy, then that object ___________.

a)

feels cold

b)

feels neither hot not cold

c)

feels sometime hot and sometime cold

d)

feels hotter

123.

Thermal energy is __________________to the temperature and average kinetic energy of an object.

a)

directly proportional

b)

inversely proportional

c)

not related

d)

not proportional

124.

On Fahrenheit scale, the normal body temperature is ________________oF.

a)

100

b)

310

c)

98

d)

37

125.

Why is the temperature of hot tea higher than the temperature of iced tea?

a)

The particles in hot tea are moving faster.

b)

The particles in hot tea are moving slower.

c)

The particles in both teas have same speed

d)

The particles in both teas have no speed.

126.

Specific heat is measured in the unit of ______________.

a)

°C /Kg • J

b)

Kg/J• °C

c)

J/kg • °C

d)

JKg°C

127.

1000.0 mL of 4.00°C water is heated until its temperature is 37.0°C. If the specific heat of water is 4.18 J/Kg°C, calculate the amount of heat energy needed to cause this rise in temperature.

a)

13800J

b)

13800J/Kg. °C

c)

13800Kg/J. °C

d)

13800°C/Kg.J

128.

___________is the transfer of thermal energy in a fluid by moving particles from one place to another

a)

Conduction

b)

Radiation

c)

Temperature

d)

Convection

129.

Conduction is faster in _____________________.

a)

solids & liquids than in gases.

b)

gases & liquids than in solids

c)

solids & gases than in liquids

d)

all the states of matter.

130.

The transfer of energy by radiation occurs in all states of matter but it works best with ___________.

a)

liquids

b)

solids

c)

gases

d)

plasma

131.

The give diagram is representing __________ wave.

a)

longitudinal

b)

transverse

c)

electromagnetic

d)

matter wave

132.

In ________________________, the particles of a medium vibrate up and down.

a)

transverse waves

b)

longitudinal waves

c)

electromagnetic waves

d)

matter wave

133.

________________ can travel through vacuum.

a)

matter waves

b)

mechanical waves

c)

electromagnetic waves

d)

all of the waves

134.

The correct relation between frequency, wavelength and speed is ___________.

a)

υ = ƒ x λ

b)

ƒ = υ x λ

c)

λ = ƒ x υ

d)

υ = ƒ / λ

135.

Frequency is the ____________________________.

a)

no. of waves / time in minutes

b)

time in seconds / no. of waves

c)

no. of waves / time in seconds

d)

time in minutes / no. of waves

136.

The __________the compressions, the larger the amplitude is, and the more energy the wave carries.

a)

thinner

b)

less denser

c)

weak

d)

denser

137.

Calculate the wavelength of a radiation with a frequency of 8.0 x 1014Hz.

a)

3.8 x 10-7m

b)

3.8 x 10-17m

c)

3.8 x 10-14m

d)

3.8 x 10-27m

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