Free Printable Physical Science — Exam 1 (Worksheet Extraction)

1.

What is the mass number of an atom with 6 protons and 7 neutrons?

a)

6

b)

7

c)

13

d)

14

2.

Which subatomic particle determines the identity of an element?

a)

Proton

b)

Electron

c)

Neutron

d)

Nucleus

3.

Isotopes of an element differ in the number of what?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Orbitals

4.

What is the maximum number of electrons in the second energy level?

a)

2

b)

4

c)

6

d)

8

5.

Atomic radius generally increases in which direction on the periodic table?

a)

Left to right

b)

Top to bottom

c)

Diagonally

d)

Right to left

6.

What happens to electronegativity across a period?

a)

Increases

b)

Decreases

c)

Stays the same

d)

Oscillates

7.

Which of these compounds has ionic bonding?

a)

H2O

b)

CO2

c)

NaCl

d)

CH4

8.

A molecule with a bent shape is likely to be:

a)

Nonpolar

b)

Ionic

c)

Linear

d)

Polar

9.

What type of bond is formed when electrons are shared?

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

10.

In metallic bonding, electrons are:

a)

Shared between atoms

b)

Transferred

c)

Delocalized

d)

Repelled

11.

How many particles are in 1 mole of a substance?

a)

$3.14\times10^4$

b)

$6.02\times10^{23}$

c)

$1.00\times10^{20}$

d)

$9.81\times10^5$

12.

What is the molar mass of CO2?

a)

28 g/mol

b)

32 g/mol

c)

44 g/mol

d)

52 g/mol

13.

Convert 18 grams of H2O to moles (molar mass = 18 g/mol).

a)

1

b)

2

c)

0.5

d)

18

14.

What is the limiting reactant?

a)

The one in excess

b)

The one that forms the most product

c)

The one that runs out first

d)

The one with the highest molar mass

15.

If theoretical yield is 10 g and actual is 8 g, percent yield is:

a)

80%

b)

90%

c)

10%

d)

100%

16.

Which state of matter has a definite shape and volume?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

17.

What is a hypothesis in scientific research?

a)

A conclusion based on data

b)

A testable prediction

c)

A detailed experiment

d)

A proven fact

18.

What is the purpose of a control group in an experiment?

a)

To test the hypothesis

b)

To provide a comparison against the experimental group

c)

To ensure the experiment has a variable

d)

To manipulate the independent variable

19.

Which step comes first in the scientific method?

a)

Analysis

b)

Experimentation

c)

Observation

d)

Conclusion

20.

Which of the following is considered a scientific theory?

a)

A well-substantiated explanation of an aspect of the natural world

b)

An untested guess

c)

A law that describes a natural phenomenon

d)

A personal belief

21.

What is the main difference between a scientific law and a scientific theory?

a)

A law explains why phenomena occur, and a theory only describes what happens

b)

A law describes a consistent relationship or pattern in nature, and a theory provides a tested explanation for why that pattern occurs

c)

A law and a theory mean the same thing in science

d)

A law is untested while a theory is proven

22.

Which element has the smallest atomic radius?

a)

Li

b)

C

c)

F

d)

Ne

23.

Ionization energy generally trends on the periodic table to (think Fr & F):

a)

Increases down a group

b)

Decreases across a period

c)

Increases across a period

d)

Remains unchanged

24.

Which of the following is most reactive with water?

a)

Be

b)

Mg

c)

Na

d)

Al

25.

Which period contains the most elements?

a)

1

b)

2

c)

3

d)

6

26.

A compound formed from a metal and a nonmetal usually has:

a)

Covalent bonds

b)

Ionic bonds

c)

Metallic bonds

d)

Hydrogen bonds

27.

Polar molecules have:

a)

Unequal sharing of electrons

b)

Equal sharing of electrons

c)

No bonds

d)

Delocalized electrons

28.

Which of these is the best example of a polar covalent bond?

a)

O2

b)

Cl2

c)

HCl

d)

NaCl

29.

What is the first step of the scientific method?

a)

Forming a hypothesis

b)

Making observations

c)

Conducting an experiment

d)

Drawing conclusions

30.

A well-tested explanation that unifies a broad range of observations is a:

a)

Hypothesis

b)

Theory

c)

Guess

d)

Procedure

31.

Which of the following is a qualitative observation?

a)

The liquid has a pH of 3

b)

The sample weighs 4.5 grams

c)

The solution is blue

d)

The temperature is 22°C

32.

A variable that is changed during an experiment is called the:

a)

Control variable

b)

Independent variable

c)

Dependent variable

d)

Experimental constant

33.

What is the purpose of a control group in an experiment?

a)

To test the hypothesis

b)

To provide a baseline for comparison

c)

To eliminate human error

d)

To speed up data collection

34.

Which of the following is a physical change?

a)

Burning wood

b)

Rusting iron

c)

Melting ice

d)

Baking a cake

35.

Which is not a state of matter?

a)

Solid

b)

Liquid

c)

Gas

d)

Energy

36.

Which is an example of a homogeneous mixture?

a)

Salad

b)

Sand and water

c)

Salt water

d)

Oil and vinegar

37.

What defines a chemical property?

a)

Shape and color

b)

Ability to undergo a change in composition

c)

Mass and volume

d)

Freezing point

38.

Which of these is a chemical change?

a)

Dissolving sugar in water

b)

Boiling water

c)

Cutting paper

d)

Digesting food

39.

What is the unit of measurement for amount of substance in the SI system?

a)

Gram

b)

Liter

c)

Mole

d)

Kelvin

40.

The number of significant figures in the measurement 0.00340 is:

a)

2

b)

3

c)

4

d)

5

41.

Which instrument is best for measuring the volume of a liquid accurately?

a)

Beaker

b)

Erlenmeyer flask

42.

What does the Law of Conservation of Mass state?

a)

Mass can be created and destroyed

b)

Mass is always increasing

c)

Mass is conserved in physical but not chemical changes

d)

Mass cannot be created or destroyed in a chemical reaction

43.

In a chemical equation, what do the coefficients represent?

a)

Volume of the substances

b)

Number of atoms in a molecule

c)

Relative number of moles of each substance

d)

Energy levels of the electrons

44.

Which subatomic particle has the smallest mass?

a)

Proton

b)

Neutron

c)

Electron

d)

Ion

45.

The atomic number of an element is equal to its number of:

a)

Neutrons

b)

Electrons

c)

Protons

d)

Orbitals

46.

What kind of ion forms when an atom loses electrons?

a)

Cation

b)

Anion

c)

Neutral

d)

Isotope

47.

What is the correct symbol for the element potassium?

a)

K

b)

P

c)

Po

d)

Pt

48.

What is Avogadro’s number used to calculate?

a)

Gravitational force

b)

Particles per mole

c)

Mass to energy conversion

d)

Solution color

49.

Which of the following best describes a covalent bond?

a)

Sharing of electrons

b)

Transfer of protons

c)

Electron transfer

d)

Nucleus merging

50.

Which element is a halogen?

a)

Oxygen

b)

Fluorine

c)

Calcium

d)

Nitrogen

51.

Which type of reaction is: 2H2 + O2 → 2H2O

a)

Double Replacement

b)

Decomposition

c)

Synthesis

d)

Single replacement

52.

Which part of the atom is most involved in bonding?

a)

Neutrons

b)

Electrons

c)

Protons

d)

Nucleus

53.

Which of the following is a noble gas?

a)

Nitrogen

b)

Argon

c)

Hydrogen

d)

Chlorine

54.

Which compound is organic?

a)

H2O

b)

C6H12O6

c)

NaCl

d)

PO4

55.

What kind of bond holds NaCl together?

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

56.

Which particle has a negative charge?

a)

Proton

b)

Neutron

c)

Electron

d)

Atom

57.

What is the total number of valence electrons in CH4?

a)

6

b)

8

c)

10

d)

12

58.

What is the mass of 1 mole of NaCl?

a)

58.44 g

b)

23 g

c)

35.5 g

d)

50.0 g

59.

Which of the following is a physical property?

a)

Flammability

b)

Reactivity with acid

c)

Density

d)

Combustion

60.

Which of the following is used to speed up a chemical reaction?

a)

Solvent

b)

Inhibitor

c)

Catalyst

d)

Reactant

61.

Which type of bond results from electrostatic attraction between ions?

a)

Metallic

b)

Covalent

c)

Ionic

d)

Hydrogen

62.

Balance the following equation and use it to determine the oxygen requirement: NH3 + O2 → NO2 + H2O. According to the balanced equation, 1.00 mole of NH3 requires how many moles of O2?

a)

0.57

b)

1.25

c)

1.33

d)

1.75

e)

3.5

63.

What is the definition of combustion?

a)

Combining with O2

b)

Combining with H2O

c)

O2 and C6H12O6

d)

Combining with H2

64.

What is the total mass of products formed when 16 grams of CH4 is burned with excess oxygen?

a)

16 g

b)

32 g

c)

64 g

d)

80 g

65.

Which of the following elements exists as a diatomic molecule?

a)

neon

b)

nitrogen

c)

lithium

d)

sulfur

66.

Avogadro's number of representative particles is equal to one ____.

a)

kilogram

b)

kelvin

c)

gram

d)

mole

67.

Avogadro's number of representative particles is equal to one ____.

a)

kilogram

b)

kelvin

c)

gram

d)

mole

68.

All of the following are equal to Avogadro's number EXCEPT ____.

a)

the number of atoms of bromine in 1 mol Br2

b)

the number of atoms of gold in 1 mol Au

c)

the number of molecules of nitrogen in 1 mol N2

d)

the number of molecules of carbon monoxide in 1 mol CO

69.

How many moles of tungsten atoms are in $4.8\times10^{25}$ atoms of tungsten?

a)

$8.0\times10^{2}$ moles

b)

$8.0\times10^{1}$ moles

c)

$1.3\times10^{1}$ moles

d)

$1.3\times10^{2}$ moles

70.

How many moles of silver atoms are in $1.8\times10^{20}$ atoms of silver?

a)

$3.0\times10^{-4}$

b)

$3.3\times10^{-3}$

c)

$3.0\times10^{-2}$

d)

$1.1\times10^{-4}$

71.

How many atoms are in 0.075 mol of titanium?

a)

$1.2\times10^{-35}$

b)

$2.2\times10^{4}$

c)

$6.4\times10^{2}$

d)

$4.5\times10^{22}$

72.

How many molecules are in 2.10 mol CO2?

a)

$2.53\times10^{24}$ molecules

b)

$3.79\times10^{24}$ molecules

c)

$3.49\times10^{24}$ molecules

d)

$1.26\times10^{24}$ molecules

73.

How many atoms are in 3.5 moles of arsenic atoms?

a)

$5.8\times10^{24}$ atoms

b)

$7.5\times10^{1}$ atoms

c)

$2.1\times10^{24}$ atoms

d)

$1.7\times10^{23}$ atoms

74.

The atomic masses of any two elements contain the same number of ____.

a)

atoms

b)

grams

c)

ions

d)

milliliters

75.

What is true about the molar mass of chlorine gas?

a)

The molar mass is 35.5 g.

b)

The molar mass is 71.0 g.

c)

The molar mass is equal to the mass of one mole of chlorine atoms.

d)

none of the above

76.

The mass of a mole of NaCl is the ____.

a)

molar mass

b)

atomic mass

c)

molecular mass

d)

gram atomic mass

77.

What is the molar mass of Gold (III) chloride?

a)

96 g

b)

130 g

c)

232.5 g

d)

303.6 g

78.

What is the molar mass of ammonium carbonate?

a)

144 g

b)

138 g

c)

96 g

d)

78 g

79.

What is the mass in grams of 5.90 mol C8H18?

a)

0.0512 g

b)

19.4 g

c)

389 g

d)

673 g

80.

How many moles of CaBr2 are in 5.0 grams of CaBr2?

a)

$2.5\times10^{-2}$ mol

b)

$4.2\times10^{-2}$ mol

c)

$4.0\times10^{-1}$ mol

d)

$1.0\times10^{-3}$ mol

Physical Science — Exam 1 (Worksheet Extraction)

Total questions: 80

Worksheet time: 40mins

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