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Chemistry Semester 1 Study Guide

Total questions: 100

Worksheet time: 50mins

Name
Class
Date
1.

What element has the electron configuration 1s2 2s2 2p6 3s2 3p21s^2\,2s^2\,2p^6\,3s^2\,3p^2 ?

a)

silicon

b)

silver

c)

nitrogen

d)

selenium

2.

After developing a plan, effective problem solving always involves doing what with that plan?

a)

Evaluating it.

b)

Implementing it.

c)

Analyzing it.

d)

Doing the calculation.

3.

How do the energy differences between the higher energy levels of an atom compare with the energy differences between the lower energy levels of the atom?

a)

They are smaller in magnitude than those between lower energy levels.

b)

They are greater in magnitude than those between lower energy levels.

c)

There is no significant difference in the magnitudes of these differences.

d)

No answer can be determined from the information given.

4.

How is the number of neutrons in the nucleus of an atom calculated?

a)

Subtract the number of electrons from the number of protons.

b)

Add the mass number to the number of electrons.

c)

Add the number of electrons and protons together.

d)

Subtract the number of protons from the mass number.

5.

What is the temperature of absolute zero measured in °C?

a)

-73°C

b)

-273°C

c)

-173°C

d)

-373°C

6.

Which of these steps should always be followed for effective problem solving?

a)

using a trial-and-error approach and then evaluating

b)

developing a plan and then implementing the plan

c)

performing metric conversions

d)

buying a larger quantity of material than estimated

7.

The range in size of most atomic radii is approximately

a)

5×10−21 m5\times10^{-21}\ \text{m} to 2×10−20 m2\times10^{-20}\ \text{m}

b)

2 to 5 nm

c)

5×10−11 m5\times10^{-11}\ \text{m} to 2×10−10 m2\times10^{-10}\ \text{m}

d)

2 to 5 cm

8.

When a measurement is multiplied by a conversion factor, the numerical value

a)

remains the same, but the actual size of the quantity measured is generally changed.

b)

and the actual size of the quantity measured are generally changed.

c)

is generally changed, but the actual size of the quantity measured remains the same.

d)

and the actual size of the quantity measured remain the same.

9.

What is the measurement 111.009 mm rounded off to four significant digits?

a)

110 mm

b)

111.0 mm

c)

111 mm

d)

111.01 mm

10.

What is the relative mass of an electron?

a)

11840\tfrac{1}{1840} the mass of a C-12 atom

b)

11840\tfrac{1}{1840} the mass of a hydrogen atom

c)

11840\tfrac{1}{1840} the mass of a neutron + proton

d)

11840\tfrac{1}{1840} the mass of an alpha particle

11.

Which of the following was a major contribution to chemistry by Antoine Lavoisier?

a)

He encouraged scientists to form explanations based on philosophical arguments.

b)

He developed the science of alchemy.

c)

He showed that oxygen is required for material to burn.

d)

He demonstrated the presence of phlogiston in air.

12.

Which subatomic particle plays the greatest part in determining the properties of an element?

a)

electron

b)

proton

c)

neutron

d)

nucleus

13.

Which field of science studies the composition and structure of matter?

a)

geology

b)

chemistry

c)

physics

d)

biology

14.

Isotopes of the same element have different

a)

numbers of electrons.

b)

atomic numbers.

c)

numbers of neutrons.

d)

numbers of protons.

15.

Dalton's atomic theory included which idea?

a)

All atoms of all elements are the same size.

b)

Atoms of different elements always combine in one-to-one ratios.

c)

Individual atoms can be seen with a microscope.

d)

Atoms of the same element are always identical.

16.

If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? 1. 1020E^{20}_{10}\text{E} 2. 1120E^{20}_{11}\text{E} 3. 921E^{21}_{9}\text{E} 4. 1021E^{21}_{10}\text{E}

a)

1 and 4

b)

2 and 3

c)

3 and 4

d)

1 and 2

17.

What is the approximate frequency of a photon having an energy 5×10−24 J5\times10^{-24}\ \text{J} ( h=6.6×10−34 J⋅sh=6.6\times10^{-34}\ \text{J}\cdot\text{s} )?

a)

3×10−57 Hz3\times10^{-57}\ \text{Hz}

b)

3×10−58 Hz3\times10^{-58}\ \text{Hz}

c)

1×10−10 Hz1\times10^{-10}\ \text{Hz}

d)

8×109 Hz8\times10^{9}\ \text{Hz}

18.

The metals in Groups 1A, 2A, and 3A

a)

all have ions with a 1+1^+ charge.

b)

gain electrons when they form ions.

c)

all form ions with a negative charge.

d)

lose electrons when they form ions.

19.

What is another name for the transition metals?

a)

noble gases

b)

Group A elements

c)

Group C elements

d)

Group B elements

20.

How are the frequency and wavelength of light related?

a)

They are directly proportional to each other.

b)

Frequency equals wavelength divided by the speed of light.

c)

They are inversely proportional to each other.

d)

Wavelength is determined by dividing frequency by the speed of light.

21.

What is the electron configuration of potassium?

a)

1s2 2s2 2p6 3s2 4s11s^2\,2s^2\,2p^6\,3s^2\,4s^1

b)

1s2 2s2 2p6 3s2 3p6 4s11s^2\,2s^2\,2p^6\,3s^2\,3p^6\,4s^1

c)

1s2 2s2 2p10 3s2 3p31s^2\,2s^2\,2p^{10}\,3s^2\,3p^3

d)

1s2 2s2 3s2 3p6 3d11s^2\,2s^2\,3s^2\,3p^6\,3d^1

22.

What unit is used to measure weighted average atomic mass?

a)

amu

b)

nanogram

c)

angstrom

d)

gram

23.

If a liter of water is heated from 20°C to 50°C, what happens to its volume?

a)

The volume first increases, then decreases.

b)

The volume decreases.

c)

The volume increases.

d)

The volume first decreases, then increases.

24.

Which of the following is a mixture?

a)

table salt

b)

mayonnaise

c)

sucrose

d)

baking soda

25.

Which of the following was one of Dalton’s improvements over Democritus’s ideas?

a)

Atoms retain their identity in a chemical reaction.

b)

Atoms are indivisible.

c)

Matter consists of tiny particles called atoms.

d)

Atoms are indestructible.

26.

What causes the shielding effect to remain constant across a period?

a)

Electrons are added to the same principal energy level.

b)

The atomic radius increases.

c)

The charge on the nucleus is constant.

d)

Electrons are added to different principal energy levels.

27.

What element in the second period has the largest atomic radius?

a)

neon

b)

potassium

c)

carbon

d)

lithium

28.

According to the Heisenberg uncertainty principle, if the position of a tiny moving particle is known, the

a)

spin of the particle cannot be exactly determined.

b)

velocity of the particle cannot be exactly determined.

c)

charge of the particle cannot be exactly determined.

d)

mass of the particle cannot be exactly determined.

29.

Which of the following statements is true?

a)

The nucleus of an atom is positively charged and never has a mass of 1 amu.

b)

Protons are positively charged and have a mass of 1 amu.

c)

Electrons are negatively charged and have a mass of 1 amu.

d)

Neutrons are negatively charged and have a mass of 1 amu.

30.

Which of the following is a physical property?

a)

ability to rust

b)

melting point

c)

explosive

d)

combustible

31.

How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum?

a)

The speed of visible light is greater.

b)

No answer can be determined from the information given.

c)

The speeds are the same.

d)

The speed of gamma rays is greater.

32.

What is one difference between a mixture and a compound?

a)

A mixture can only be separated into its components by chemical means.

b)

A compound consists of more than one phase.

c)

A mixture must be uniform in composition.

d)

A compound can only be separated into its components by chemical means.

33.

In an s orbital, the probability of finding an electron a particular distance from the nucleus can best be determined by the

a)

deBroglie equation.

b)

direction of the electron with respect to the nucleus.

c)

quantum mechanical model.

d)

boundary of the electron cloud.

34.

A substance that forms a vapor is generally in what physical state at room temperature?

a)

liquid or solid

b)

liquid

c)

gas

d)

solid

35.

A golf ball has more mass than a tennis ball because it

a)

takes up more space.

b)

contains different kinds of matter.

c)

contains more matter.

d)

has a definite composition.

36.

In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a)

Zn, 30 protons, 60 electrons

b)

Cs, 55 protons, 132.9 electrons

c)

In, 49 protons, 49 electrons

d)

F, 19 protons, 19 electrons

37.

By the early 1800’s, chemists started organizing elements into groups because

a)

there were so many new elements that had been discovered.

b)

the printing press made it possible to disseminate knowledge faster.

c)

universities had a sudden influx of students interested in chemistry.

d)

more books were being published on the topic.

38.

What is the charge of a cation?

a)

The charge depends on the size of the nucleus.

b)

a negative charge

c)

a positive charge

d)

no charge

39.

Which of the following can be classified as a mixture?

a)

pure water

b)

pure nitrogen

c)

pure gold

d)

pure air

40.

What must occur for a change to be a chemical reaction?

a)

The change must involve a change in mass.

b)

There must be a change in physical properties.

c)

The change must involve a change in volume.

d)

There must be a change in chemical properties.

41.

How do conceptual problems differ from numeric problems?

a)

Solutions to conceptual problems normally do not involve calculations.

b)

Logic is not usually involved in solving numeric problems.

c)

Solutions to conceptual problems involve analysis, while numeric solutions do not.

d)

A plan is necessary to solve numeric problems, but is not necessary for conceptual problems.

42.

Which of the following statements is true about ions?

a)

Cations form when an atom loses electrons.

b)

Cations form when an atom gains electrons.

c)

Anions form when an atom gains protons.

d)

Anions form when an atom loses protons.

43.

The principal quantum number indicates what property of an electron?

a)

energy level

b)

speed

c)

position

d)

electron cloud shape

44.

What is another name for the representative elements?

a)

transition elements

b)

Group B elements

c)

Group A elements

d)

Group C elements

45.

What are quanta of light called?

a)

charms

b)

excitons

c)

muons

d)

photons

46.

The atomic number of an element is the total number of which particles in the nucleus?

a)

protons and electrons

b)

protons

c)

neutrons

d)

electrons

47.

The atomic number of an element is the total number of which particles in the nucleus?

a)

protons

b)

neutrons

c)

protons and electrons

d)

electrons

48.

Which of the following decreases with increasing atomic number in Group 2A?

a)

ionic size

b)

ionization energy

c)

number of electrons

d)

shielding effect

49.

Which color of visible light has the shortest wavelength?

a)

violet

b)

blue

c)

yellow

d)

green

50.

What is the SI unit of mass?

a)

liter

b)

joule

c)

kilogram

d)

candela

51.

Which of the following was originally a tenet of Dalton's atomic theory, but had to be revised about a century ago?

a)

Atoms of different elements can combine with one another in simple whole number ratios.

b)

Compounds are made by combining atoms.

c)

The atoms of any one element are different from those of any other element.

d)

Atoms are tiny indivisible particles.

52.

Which of the following is an example of chemistry research in the main area of energy?

a)

specific reactions between prescription drugs and chemicals in cells

b)

developing rechargeable batteries

c)

determining the composition of extra-terrestrial soil and rocks

d)

producing bioplastics

53.

Which of the following equals one atomic mass unit?

a)

the mass of one carbon-12 atom

b)

the mass of one helium-4 atom

c)

one-twelfth the mass of one carbon-12 atom

d)

the mass of one electron

54.

Which of the following volumes is the smallest?

a)

one milliliter

b)

one liter

c)

one deciliter

d)

one microliter

55.

Which of the following represents a compound?

a)

H2O

b)

H

c)

H-3

d)

O-16

56.

Which of the following mass units is the largest?

a)

1 cg

b)

1 mg

c)

1 dg

d)

1 ng

57.

Who predicted that all matter can behave as waves as well as particles?

a)

Albert Einstein

b)

Erwin Schrodinger

c)

Louis de Broglie

d)

Max Planck

58.

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

a)

8

b)

32

c)

18

d)

2

59.

As you move from left to right across the second period of the periodic table

a)

atomic radii increase.

b)

electronegativity decreases.

c)

ionization energy increases.

d)

atomic mass decreases.

60.

Which of the following equalities is correct?

a)

1 cm^3 = 1 mL

b)

10 kg = 1 g

c)

100 cg = 10 g

d)

1000 mm = 100 m

61.

Which of the following is a physical property of a substance in the liquid state?

a)

indefinite mass

b)

definite volume

c)

not easily compressed

d)

definite shape

62.

Which of the following elements is a transition metal?

a)

copper

b)

tin

c)

tellurium

d)

cesium

63.

What is the maximum number of f orbitals in any single energy level in an atom?

a)

1

b)

5

c)

7

d)

3

64.

Express the sum of 7.68 m and 5.0 m using the correct number of significant digits.

a)

13 m

b)

10 m

c)

12.68 m

d)

12.7 m

65.

Which of the following is true about compounds?

a)

They have properties similar to those of their component elements.

b)

They have compositions that vary.

c)

They can be physically separated into their component elements.

d)

They are substances.

66.

Which of the following electron configurations is most likely to result in an element that is relatively inactive?

a)

a filled energy sublevel

b)

a filled highest occupied principal energy level

c)

a half-filled energy sublevel

d)

one empty and one filled energy sublevel

67.

An example of a homogeneous mixture is

a)

distilled water.

b)

noodle soup.

c)

stainless steel.

d)

oxygen.

68.

Which of the following statements is true about ions?

a)

Cations are common among nonmetals.

b)

Charges for ions are always written as numbers followed by a plus or minus sign.

c)

Anions are positively charged ions.

69.

Which of the following isotopes has the same number of neutrons as phosphorus-31?

a)

1632S^{32}_{16}\mathrm{S}

b)

1429Si^{29}_{14}\mathrm{Si}

c)

1428Si^{28}_{14}\mathrm{Si}

d)

1532P^{32}_{15}\mathrm{P}

70.

Which of the following statements is false?

a)

Chemistry explains many aspects of nature.

b)

Knowledge of chemistry helps prepare people for careers in soil science.

c)

Studying chemistry ensures that officials make correct choices in funding technology.

d)

Knowledge of chemistry allows the public to make informed decisions.

71.

Which substance has a chemical symbol that is derived from a Latin name?

a)

hydrogen

b)

oxygen

c)

potassium

d)

calcium

72.

How many energy sublevels are in the second principal energy level?

a)

2

b)

3

c)

4

d)

1

73.

The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific notation?

a)

1.54×10−10 m1.54 \times 10^{-10}\text{ m}

b)

1.54×1012 m1.54 \times 10^{12}\text{ m}

c)

1.54×10−12 m1.54 \times 10^{-12}\text{ m}

d)

1.54×1010 m1.54 \times 10^{10}\text{ m}

74.

Which scientist developed the quantum mechanical model of the atom?

a)

Niels Bohr

b)

Ernest Rutherford

c)

Albert Einstein

d)

Erwin Schrodinger

75.

Which state of matter has a definite volume and takes the shape of its container?

a)

solid

b)

liquid only

c)

gas only

d)

both b and c

76.

Which variable is directly proportional to frequency?

a)

position

b)

energy

c)

wavelength

d)

velocity

77.

Which state of matter is characterized by having an indefinite shape, but a definite volume?

a)

gas

b)

liquid only

c)

solid only

d)

both b and c

78.

The comparison of the number of atoms in a copper coin the size of a penny with the number of people on Earth is used to illustrate which of the following?

a)

that atoms are very large

b)

that atoms are indivisible

c)

that atoms are very small

d)

that in a copper penny, there is one atom for every person on Earth

79.

Which of the following elements has the lowest electronegativity?

a)

carbon

b)

bromine

c)

fluorine

d)

lithium

80.

How many significant figures are in the measurement 811.40 grams?

a)

five

b)

three

c)

two

d)

four

81.

The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be

a)

the same.

b)

the same as each other only in the ultraviolet range.

c)

the same as those of several other elements.

d)

different from each other.

82.

If the temperature of a piece of steel decreases, what happens to its density?

a)

The density increases.

b)

The density decreases.

c)

The density first increases, then decreases.

d)

The density does not change.

83.

How does atomic radius change from left to right across a period in the periodic table?

a)

It first increases, then decreases.

b)

It tends to decrease.

c)

It first decreases, then increases.

d)

It tends to increase.

84.

Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?

a)

more shielding of the electrons in the highest occupied energy level

b)

an increase in size of the nucleus

c)

an increase in number of protons

d)

fewer electrons in the highest occupied energy level

85.

Three different people weigh a standard mass of 2.00 g on the same balance. Each person obtains a reading of 7.32 g for the mass of the standard. These results imply that the balance that was used is

a)

accurate and precise

b)

precise

c)

neither accurate nor precise

d)

accurate

86.

Which of the following involves a chemical change?

a)

grinding

b)

melting

c)

decomposing

d)

mixing

87.

What distinguishes a substance from a mixture?

a)

The composition of substances cannot vary, while the composition of mixtures can.

b)

Samples of the same substance can have different intensive properties.

c)

Substances are compounds, and mixtures are not.

d)

Mixtures are groupings of elements, and compounds are not.

88.

As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit

a)

cannot be determined.

b)

increase.

c)

remain the same.

d)

decrease.

89.

What must be done to be certain that a chemical change has taken place?

a)

Demonstrate that energy was absorbed by the reactants after the change.

b)

Check the composition of the sample before and after the change.

c)

Demonstrate that a release of energy occurred after the change.

d)

Check for the production of bubbles before and after the change.

90.

Which of the following elements has the smallest first ionization energy?

a)

magnesium

b)

sodium

c)

calcium

d)

potassium

91.

Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?

a)

increase in number of protons

b)

fewer electrons in the highest occupied energy level

c)

increase in atomic size

d)

increase in size of the nucleus

92.

Of the following elements, which one has the smallest first ionization energy?

a)

aluminum

b)

boron

c)

silicon

d)

carbon

93.

A cubic meter is about the same as the volume occupied by a ____.

a)

basketball arena

b)

washing machine

c)

cup of milk

d)

kilogram of water

94.

How do the isotopes hydrogen-1 and hydrogen-2 differ?

a)

Hydrogen-2 has two protons; hydrogen-1 has one.

b)

Hydrogen-2 has one proton; hydrogen-1 has none.

c)

Hydrogen-2 has one more electron than hydrogen-1.

d)

Hydrogen-2 has one neutron; hydrogen-1 has none.

95.

Which of the following factors contributes to the increase in ionization energy from left to right across a period?

a)

an increase in the shielding effect

b)

fewer electrons in the highest occupied energy level

c)

an increase in the number of protons

d)

an increase in the size of the nucleus

96.

Which of the following changes to a metal is a chemical change?

a)

melting

b)

bending

c)

rusting

d)

polishing

97.

Which of the following is a physical property of water?

a)

It is composed of hydrogen and oxygen.

b)

It reacts with calcium metal to produce a basic solution.

c)

It can be decomposed by electrolysis.

d)

It melts below room temperature.

98.

How does atomic radius change from top to bottom in a group in the periodic table?

a)

It first increases, then decreases.

b)

It tends to decrease.

c)

It tends to increase.

d)

It first decreases, then increases.

99.

Emission of light from an atom occurs when an electron

a)

jumps from a lower to a higher energy level.

b)

falls into the nucleus.

c)

drops from a higher to a lower energy level.

d)

moves within its atomic orbital.

100.

Which temperature scale has no negative temperatures?

a)

Joule

b)

Celsius

c)

Fahrenheit

d)

Kelvin

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