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Chemistry Quiz

Total questions: 70

Worksheet time: 35mins

Name
Class
Date
1.

Which of the following is an example of qualitative information about a substance?

a)

Color of the substance

b)

Melting temperature of the substance

c)

Mass of the substance

d)

Volume of the substance

e)

Boiling temperature of the substance

2.

Which of the following statements is true of a chemical equation?

a)

It is a representation of only a physical change rather than a chemical or molecular change.

b)

It shows that the reactants on the left side of an equation produce the products on the right side of the equation.

c)

The number of atoms found in the reactants doubles in the products.

d)

The number of atoms found in the reactants halves in the products.

e)

The identity of the substance in a chemical equation is preserved.

3.

Which of the following is NOT an example of an intensive property of matter?

a)

Color

b)

Boiling point

c)

Density

d)

Mass

e)

Thermal conductivity

4.

Which of the following is NOT a correct name–symbol combination?

a)

Phosphorus, P

b)

Iron, Fe

c)

Chlorine, Cl

d)

Potassium, K

e)

Sodium, So

5.

A hypothesis is a _____.

a)

tentative explanation or predication based upon experimental observations

b)

well-tested unifying principle that explains a body of facts

c)

set of experiments designed to test a theory

d)

set of quantitative data

e)

concise statement of behavior that is always the same under the same conditions.

6.

Which of the following statements concerning green chemistry is NOT correct?

a)

It is better to prevent waste than to treat or clean up waste after it is formed.

b)

Synthetic methods should be designed to use and generate substances that possess little or no toxicity to human health or the environment.

c)

Substances used in a chemical process should pose minimal risk for accidents.

d)

Raw materials should be renewable whenever technically and economically practical.

7.

Which one of the following is most likely to be a homogeneous mixture?

a)

plain yogurt

b)

blood

c)

gasoline

d)

milk and water

e)

hot milk and coffee powder

8.

Balancing chemical equations is an application of

a)

The law of conservation of matter

b)

The law of conservation of energy

c)

The law of multiple proportions

d)

The law of conservation of matter and energy

e)

The conversion of a hypothesis to a law

9.

Which of the following is not a base SI unit?

a)

Kilogram

b)

Ampere

c)

Calorie

d)

Second

e)

Meter

10.

The wavelength of light emitted from a particular red diode laser is 651 nm. What is the wavelength in meters?

a)

6.51 × 10¹¹ m

b)

6.51 × 10⁻² m

c)

6.51 × 10⁻⁴ m

d)

6.51 × 10⁻⁷ m

e)

6.51 × 10⁻⁹ m

11.

Atoms are made of three subatomic particles. What are these particles and their charges?

a)

proton (+1), neutron (0), and electron (−1)

b)

proton (−1), neutron (+1), and electron (0)

c)

proton (+1), neutron (−1), and electron (0)

d)

proton (0), neutron (+1), and electron (−1)

e)

proton (−1), neutron (0), and electron (+1)

12.

A neutral atom of an isotope ₈₀Hg²⁰⁰ contains _____.

a)

200 neutrons and 280 electrons

b)

80 protons and 200 neutrons

c)

200 protons and 120 electrons

d)

200 protons, 80 neutrons, and 200 electrons

13.

The masses of isotopes and their abundances are determined experimentally using _____.

a)

a mass spectrometer

b)

an analytical balance

c)

a centrifuge

d)

distillation

e)

electrolysis

14.

A sample of an element consists of two isotopes. The percent abundance of one of the isotopes is 43.0%. What is the percent abundance of the other isotope?

a)

14.5%

b)

21.5%

c)

28.5%

d)

43.0%

e)

57.0%

15.

Which of the following elements belong to the halogens?

a)

Sodium

b)

Magnesium

c)

Nitrogen

d)

Chlorine

e)

Neon

16.

How many sodium atoms are in 0.5 mol of sodium? (Avogadro number is 6.022 x 10^23).

a)

6.022 x 10^23

b)

3.011 x 10^23

c)

1.2044 x 10^24

d)

1.5055 x 10^23

e)

3.011 x 10^22

17.

Which of the following sets of ions is present in sodium sulfate, Na2SO4?

a)

Na+, S2-, and O2-

b)

Na+, S2+, and O2-

c)

Na+ and SO4^2-

d)

Na+, S2-, and O2+

e)

Na+ and SO4^-

18.

The reaction of chlorine molecule with potassium iodide yields iodine molecule and potassium chloride. Write a balanced chemical equation for this reaction.

a)

Cl2(g) + KI(s) → I(s) + KCl2(s)

b)

Cl2(g) + 2 KI(s) → I2(s) + 2 KCl(s)

c)

Cl2(g) + KI2(s) → I2(s) + KCl2(s)

d)

Cl(g) + KI(s) → I(s) + KCl(s)

e)

Cl2(g) + 2 K2I(s) → I2(s) + 2 K2Cl(s)

19.

How much energy is gained by copper when 48.7 g of copper is warmed from 10.2 °C to 67.0 °C? The specific heat capacity of copper is 0.385 J/(g·°C).

a)

1.91 × 10² J

b)

25.79 J

c)

21.86 J

d)

1.06 × 10³ J

e)

1.26 × 10³ J

20.

What is the enthalpy change for the reaction below? 4 CO₂(g) + 5 H₂O(ℓ) → C₄H₁₀(g) + 13/2 O₂(g)

a)

+1439 kJ/mol-rxn

b)

+2877 kJ/mol-rxn

c)

-5754 kJ/mol-rxn

d)

-2877 kJ/mol-rxn

e)

+5754 kJ/mol-rxn

21.

Which of the following techniques is used to measure the energy evolved or absorbed as heat in a chemical or physical process?

a)

Calorimetry

b)

Polarimetry

c)

Coulometry

d)

Spectrometry

e)

Colorimetry

22.

Which one of the following substances is classified as a chemical compound?

a)

Na

b)

Mg

c)

O₂

d)

NO

e)

N₂

23.

All of the following are examples of intensive properties of matter except _____.

a)

thermal conductivity

b)

color

c)

malleability

d)

weight

e)

boiling point

24.

How many s orbitals are in the n = 3 shell?

a)

0

b)

6

c)

5

d)

3

e)

1

25.

Boron, carbon, nitrogen, oxygen and fluorine are in the same period of the periodic table. Which of the following bonds is most polar?

a)

B-H

b)

C-H

c)

N-H

d)

O-H

e)

F-H

26.

Which of the following molecules is polar?

a)

CS₂

b)

SO₂

c)

XeF₂

d)

XeF₄

e)

SO₃

27.

Electronegativity is a measure of _____.

a)

atomic size

b)

electron affinity

c)

ionization energy

d)

the ability of an atom to attract electrons

e)

nuclear charge

28.

What is the bond angle in a linear molecule or ion?

a)

120°

b)

109°

c)

90°

d)

72°

e)

180°

29.

What is the shape of the water molecule (H₂O) where the central O-atom is surrounded by two lone pairs of electrons and two single bonds?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

linear

e)

trigonal planar

30.

Which of the following molecules has a Lewis dot structure that does not obey the octet rule where the central atom has more than eight electrons in the outermost shells?

a)

NO

b)

SO₃

c)

CO₂

d)

SF₆

e)

NH₃

31.

If two or more species have the same number of electrons, resulting in similar Lewis structures, they are said to be ____.

a)

isoelectronic

b)

resonant structures

c)

ionic

d)

neutral

e)

covalent

32.

What is the total number of valence electrons in the sulfate ion, SO₄²⁻? Both S and O are in group 6 of the periodic table.

a)

30

b)

12

c)

14

d)

24

e)

32

33.

Which of the following equations corresponds to the second ionization of magnesium?

a)

Mg(g) → Mg⁺(g) + e⁻

b)

Mg(s) → Mg⁺(g) + e⁻

c)

Mg⁺(g) → Mg²⁺(g) + e⁻

d)

Mg(g) → Mg²⁺(g) + 2e⁻

e)

Mg(g) + e⁻ → Mg⁻(g)

34.

The ground state electronic configuration of an element with atomic number 12 is 1s² 2s² 2p⁶ 3s². What is the typical charge on the monatomic ion of the element?

a)

+1

b)

+2

c)

+3

d)

-1

e)

-2

35.

Which of the following statements is true of atomic radii?

a)

They decrease down a group and remain constant across a period.

b)

They decrease down a group and increase across a period.

c)

They increase down a group and increase across a period.

d)

They increase down a group and remain constant across a period.

e)

They increase down a group and decrease across a period.

36.

Which of the following elements is found in the s-block of the periodic table?

a)

Calcium (Ca)

b)

Neon (Ne)

c)

Aluminum (Al)

d)

Silicon (Si)

e)

Bromine (Br)

37.

The small, but important, energy differences between 3s, 3p, and 3d electrons is a consequence of

a)

the number of electrons they can hold

b)

their principal quantum number

c)

the Heisenberg uncertainty principle

d)

their effective nuclear charge

e)

Hund's rule

38.

Which of the following statements is true?

a)

Outer electrons efficiently shield one another from nuclear charge.

b)

Core electrons effectively shield outer electrons from nuclear charge.

c)

Valence electrons are the most difficult of all electrons to remove.

d)

Core electrons have the lowest ionization energies of all electrons.

e)

Valence electrons in the outermost shell of all elements have the highest ionization energy.

39.

The procedure by which electrons are assigned to (or built up into) orbitals is known as the ____ principle.

a)

Aufbau

b)

Bohr

c)

Planck

d)

Hund

e)

Pauli

40.

Which of the following electron configurations is not allowed?

a)

1s²2s²2p⁵

b)

1s²2s²2p⁶

c)

1s²2s⁴

d)

1s²2s²2p⁶3s²

e)

1s²2s²2p⁴

41.

What is the maximum number of electrons that can occupy a p orbital?

a)

1

b)

2

c)

6

d)

10

e)

14

42.

How many electrons can be described by the following quantum numbers: n = 4, ℓ = 2, mℓ = 2, ms = -1/2?

a)

1

b)

2

c)

6

d)

10

e)

18

43.

It is impossible to simultaneously measure the exact location and energy of an electron. This is called

a)

Aufbau exclusion principle

b)

Line emission spectrum theory

c)

Heisenberg’s uncertainty principle

d)

The photoelectric effect

e)

The Pauli exclusion principle

44.

An electron with the quantum number n = 2, ℓ = 0 is in which orbital?

a)

1s

b)

2s

c)

2p

d)

3s

e)

3p

45.

In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus,

a)

energy is absorbed.

b)

light is emitted.

c)

energy is emitted.

d)

no change in energy occurs.

e)

none of these

46.

Which type of experiment demonstrates that an electron has the properties of a wave?

a)

nuclear fission

b)

electron diffraction

c)

light emission from atomic gases

d)

mass spectroscopy

e)

photoelectric effect

47.

Which type of experiment demonstrates that light has the properties of a particle?

a)

nuclear fission

b)

electron diffraction

c)

light emission from atomic gases

d)

mass spectroscopy

e)

photoelectric effect

48.

Which of the following is the correct series of lines that have energies in the visible region of the hydrogen spectrum?

a)

Balmer series

b)

Lyman series

c)

Brackett series

d)

Pfund series

e)

Humphreys series

49.

Which species in the reaction below undergoes oxidation? H₂O(g) + CO(g) → H₂(g) + CO₂(g)

a)

H₂O

b)

CO

c)

H₂

d)

CO₂

e)

None

50.

What mass of Na₂CO₃ is present in 0.650 L of a 0.230 M Na₂CO₃ solution? (molar mass Na₂CO₃ = 106.0 g/mol)

a)

15.8 g

b)

68.8 g

c)

24.3 g

d)

299 g

e)

37.5 g

51.

What is the pH of 2.9 × 10⁻³ M HCl(aq)?

a)

3

b)

2.5

c)

-2.5

d)

2.9

e)

1.5

52.

For which of the following transitions would an electron require the absorption of the highest amount of energy?

a)

n = 1 to n = 2

b)

n = 4 to n = 6

c)

n = 5 to n = 4

d)

n = 7 to n = 6

e)

n = 6 to n = 7

53.

Which of the following ranks the regions of the electromagnetic spectrum from shortest to longest wavelength?

a)

A. microwaves > x-rays > gamma rays > visible > infrared

b)

B. gamma rays > x-rays > visible > infrared > microwaves

c)

C. infrared > gamma rays > x-rays > visible > microwaves

d)

D. x-rays > gamma rays > infrared > visible > microwaves

e)

E. visible > infrared > microwaves > x-rays > gamma rays

54.

Which of the following observations is/are examples of chemical change?

a)

A. 1 only

b)

B. 2 only

c)

C. 3 only

d)

D. 1 and 2

e)

E. 2 and 3

55.

Which of the following statements is/are correct?

a)

A. 1 only

b)

B. 2 only

c)

C. 3 only

d)

D. 1 and 2

e)

E. 1, 2, and 3

56.

Which of the following statements concerning the kinetic-molecular theory of matter is/are correct?

a)

A. 1 only

b)

B. 2 only

c)

C. 3 only

d)

D. 1 and 2

e)

E. 1, 2, and 3

57.

Which of the following statements concerning atomic structure is/are correct?

a)

A. 1 only

b)

B. 2 only

c)

C. 3 only

d)

D. 2 and 3

e)

E. 1, 2, and 3

58.

Which of the following statements concerning the reaction of nitroglycerin is/are CORRECT?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

59.

Which of the following statements is/are CORRECT about solutions?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1 and 3

60.

Which of the following statements concerning electrolytes and nonelectrolytes is/are true?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 3

e)

2 and 3 only

61.

Which of the following are classified as precipitation reactions?

a)

1 only

b)

2 only

c)

3 only

d)

2 and 3

e)

1, 2, and 3

62.

Which of the following statements is/are CORRECT about ionic and covalent bonds?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

63.

Which of the following statements is/are CORRECT about ionization energy?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

64.

Which of the following statements is/are CORRECT for an oxygen atom? 1. The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s electron. 2. The effective nuclear charges felt by 2s and 2p electrons are identical. 3. The effective nuclear charge felt by a 2p electron is less than that felt by a 2s electron.

a)

1 only

b)

2 only

c)

3 only

d)

1 and 3

e)

1, 2, and 3

65.

Which of the following statements is/are true about the atomic line spectra? 1. An atom is said to be in ground state when its electrons are present in the lowest possible energy levels. 2. States for the H atom with higher energies (n > 1) are called excited states. 3. An electron has the lowest energy when it is present in the n = 2 level.

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

66.

Which of the following is/are correct postulates of Bohr’s theory of the hydrogen atom? 1. The energy of an electron in an atom is quantized (i.e. only specific energy values are possible). 2. The principal quantum number (n), specifies each unique energy level. 3. An electron transition from a lower energy level to a higher energy level results in an emission of a photon of light.

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

67.

Which of the following statements is/are CORRECT? 1. The conduction of electricity through copper wire is a chemical change. 2. The rusting of iron is a chemical change. 3. The evaporation of ammonia at -33.3 °C is a chemical change.

a)

1 only

b)

2 only

c)

3 only

d)

2 and 3

e)

1, 2, and 3

68.

Which of the following statements is/are CORRECT? 1. A system is defined as an object or collection of objects being studied. 2. Surroundings are defined as the entire universe, including the system. 3. In an endothermic reaction, heat is transferred from the system to the surroundings.

a)

1 only

b)

2 only

c)

3 only

d)

1 and 3

e)

1, 2, and 3

69.

A hot piece of iron is dropped into a beaker containing colder water. Which of the following statements is/are CORRECT?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

70.

Which of the following statements concerning the Pauli exclusion principle is/are CORRECT?

a)

1 only

b)

2 only

c)

3 only

d)

1 and 2

e)

1, 2, and 3

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