Basic Chemistry Pre-Test Questions - 1129 Verified Questions

Basic Chemistry

Pre-Test Questions

Course Introduction

Basic Chemistry provides an introduction to the fundamental principles of chemistry, including the structure of atoms and molecules, the periodic table, chemical bonding, stoichiometry, chemical reactions, states of matter, and basic thermodynamics. The course emphasizes both conceptual understanding and practical problem-solving skills, equipping students with a foundational knowledge essential for further studies in chemistry and related scientific fields. Through lectures, laboratory work, and interactive exercises, students gain hands-on experience in applying chemical concepts to real-world situations.

Recommended Textbook

Principles of Chemistry The Molecular Science 1st Edition by John W. Moore

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1129 Verified Questions

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Page 2

Chapter 1: The Nature of Chemistry

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Sample Questions

Q1) Which of the following represents a pair of allotropes?

A) air and oxygen

B) glucose and sucrose

C) graphite and diamond

D) sand and glass

E) carbon monoxide and carbon dioxide

Answer: C

Q2) What is a possible explanation of observations called?

A) law

B) model

C) qualitative statement

D) hypothesis

E) theory

Answer: D

Q3) How many atoms are in a diatomic molecule?.

Answer: two

Q4) Burning of hydrogen fuel is a(n) _____________ change.

Answer: chemical

Q5) Ethanol contains 2 carbons, 6 hydrogens, 1 oxygen. Write its chemical formula. Answer: C₂H₆O

Page 3

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Chapter 2: Atoms and Elements

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Sample Questions

Q1) An element containing 26 protons, 26 electrons and 30 neutrons will have the symbol:

A) (⁸²Te).

B) (⁵²Zn).

C) (⁵⁶Fe).

D) (⁵⁶Zn).

E) (⁵²Te).

Answer: C

Q2) A pond has dimensions of 24 m. by 25 m. by 3.0 m. What is the volume of the pond in liters?

A) 1.8 × 10^-3 L

B) 1.8 × 10² L

C) 1.8 × 10³ L

D) 1.8 × 10⁴ L

E) 1.8 × 10⁶ L

Answer: E

Q3) Write the atomic symbol for an atom that contains 24 protons, 24 electrons and 26 neutrons.

Answer: 11ea782d_fd70_540d_bbd5_b1588926a94a_TB5061_11

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Page 4

Chapter 3: Chemical Compounds

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Sample Questions

Q1) A compound is composed of 56.4% phosphorus and the remainder oxygen. Determine the empirical formula of the compound.

A) PO₅

B) P₂O

C) P₃O₂

D) P₂O₃

E) P₂O₅

Answer: D

Q2) An organic compound has an empirical formula of C₂H₃O and had an approximate molecular weight of 86. What is its molecular formula?

A) C₂H₃O

B) C₄H₆O₂

C) C₆H₈O₃

D) C₈H₁₂O₄

E) C₁₀H₁₄O₅

Answer: B

Q3) The molecular formula for copper (II) oxide is _____________.

Answer: CuO

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Chapter 4: Quantities of Reactants and Products

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Sample Questions

Q1) What is the maximum possible quantity of product obtained from a chemical reaction called?

A) percent yield

B) molecular weight of the product

C) stoichiometric coefficients

D) limiting reactant

E) theoretical yield

Q2) The complete reaction of 16.12 g of titanium with 23.88 g of chlorine (Cl₂) produces a compound with the formula Ti_xCl_y. What is the empirical formula of the compound?

A) TiCl

B) Ti₂Cl

C) Ti₄Cl

D) TiCl₂

E) TiCl₄

Q3) A decomposition reaction occurs when _____________ reactant(s) produces two or more products.

Q4) A combination reaction is considered the opposite of a(n) _____________ reaction.

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Chapter 5: Chemical Reactions

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Sample Questions

Q1) A solution is prepared by dissolving 20.0 g of NaI in enough water to make 300.0 mL of solution. How many moles of ions are in 25.0 mL of this solution?

A) 0.0111 mol

B) 0.0222 mol

C) 0.0445 mol

D) 0.111 mol

E) 0.445 mol

Q2) Which compound will not dissolve in water in large amounts?

A) KNO₃

B) NH₄Cl

C) Ca(OH)₂

D) AgCl

E) Ag₂SO₄

Q3) Which of the following represents oxidation?

A) 2 H⁺ + 2 e^- H₂

B) F₂ + 2 e^- 2 F^-

C) Mg²⁺ + 2 e^- Mg

D) Na Na⁺ + e^-

E) Ni²⁺ + 2 e^- Ni

Q4) Give an example of a strong base.

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Chapter 6: Energy and Chemical Reactions

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Sample Questions

Q1) How much energy in kilojoules is required to raise the temperature of 20.0 g of water from 22.0°C to 37.0°C? The specific heat of water = 4.184 J g^-1 °C^-1.

Q2) In an endothermic reaction, heat is transferred from the _____________ to the

Q3) What is the molar heat capacity of aluminum (specific heat = 0.902 J g^-1 °C^-1)?

A) 0.034 J mol^-1 °C^-1

B) 24.8 J mol^-1 °C^-1

C) 29.3 J mol^-1 °C^-1

D) 120 J mol^-1 °C^-1

E) 1.5 × 10²⁵ J mol^-1 °C^-1

Q4) Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g^-1 °C^-1).

A) 490 J

B) 979 J

C) 1.47 × 10³ J

D) 7.65 × 10³ J

E) 5.98 × 10⁴ J

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Chapter 7: Electron Configurations and the Periodic Table

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Sample Questions

Q1) The time span between wave peaks is called a(n) _____________.

Q2) What is the electron configuration of Br^-?

A) 1s²2s²2p⁴

B) 1s²2s²2p⁶

C)

1s²2s²2p⁶3s²3p⁶3d<sup >10</sup>4s²4p⁶

D)

1s²2s²2p⁶3s²3p⁶3d<sup >10</sup>4s²4p⁵

E)

1s²2s²2p⁶3s²3p⁶3d<sup >10</sup>4s²4p⁴

Q3) What is the correct electron configuration for beryllium (Be)?

A) 1s²2s²

B) 1s²2s²2p¹

C) 1s²2s²2p²

D) 1s²2s²2p⁴

E) 1s²2s²2p⁶

Q4) Atomic radii _____________ going from left to right across a row of the periodic table.

Q5) In a vacuum, all light travels with the same _____________

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Chapter 8: Covalent Bonding

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Sample Questions

Q1) The ____________ of an element is its ability to pull electrons towards itself when participating in a covalent bond.

Q2) Which bond is shortest?

A) carbon-oxygen double bond

B) carbon-oxygen single bond

C) carbon-nitrogen single bond

D) carbon-carbon double bond

E) carbon-nitrogen double bond

Q3) What is the formal charge on carbon in HCN?

A) -2

B) -1

C) 0

D) +1

E) +2

Q4) Which element is the most electronegative?

A) phosphorus

B) silicon

C) carbon

D) nitrogen

E) oxygen

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Chapter 9: Molecular Structure

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Sample Questions

Q1) The VSEPR model attempts to ____ electron-pair ____.

A) eliminate; repulsions

B) minimize; collisions

C) minimize; repulsions

D) maximize; attractions

E) maximize; repulsions

Q2) Which molecule is nonpolar?

A) NCl₃

B) SO₂

C) PH₃

D) IF

E) CF₄

Q3) Use the VSEPR model to predict the electron-pair geometry and the O-C-O bond angles for CO₃^2-.

A) tetrahedral, 90^\(\circ\)

B) triangular planar, 120^\(\circ\)

C) bent, 120^\(\circ\)

D) linear, 180^\(\circ\)

E) bent, 180^\(\circ\)

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Page 11

Chapter 10: Gases and the Atmosphere

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Sample Questions

Q1) How are the pressure and the absolute temperature of a gas related for a given number of moles at constant volume?

A) They are exactly opposites.

B) They are not related.

C) They are directly proportional.

D) They are indirectly proportional.

E) Not enough information is given to determine the relationship.

Q2) What is the density of oxygen gas (O₂) at STP? R = 0.0821 L atm mol^-1 K^-1.

A) 1.43 g/L

B) 0.714 g/L

C) 1.31 g/L

D) 1090 g/L

E) 716 g/L

Q3) What is the correct name for the atmospheric layer in which commercial jets fly?

A) ionosphere

B) thermosphere

C) mesosphere

D) stratosphere

E) troposphere

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Chapter 11: Liquids, Solids, and Materials

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Sample Questions

Q1) In face-centered cubic unit cells, ____ of the atom on each face of the unit cell is counted as part of that unit cell.

A) all

B) none

C) 1/2

D) 1/4

E) 1/8

Q2) Which property of a liquid is paired with an incorrect explanation for that property?

A) fluid, because the molecules retain some mobility

B) transmit pressure equally in all directions, because their molecules can move in all directions

C) capillary action, because the molecules are less attracted to each other than to the walls of the container

D) incompressible, because the molecules are relatively far apart

E) viscous, because the molecules can become entangled as they move past each other

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13

Chapter 12: Chemical Kinetics: Rates of Reactions

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Sample Questions

Q1) At a given temperature, the kinetics parameters for a new chemical reaction are determined in the following sequence from first to last

A) orders of reaction, k, rate law

B) k, orders of reaction, rate law

C) orders of reaction, rate law, k

D) k, rate law, orders of reaction

E) rate law, k, orders of reaction

Q2) Which statement is true about a catalyst?

A) It increases the activation energy involved in a reaction.

B) It can be the same phase as the reactants (heterogeneous) or a different phase (homogeneous).

C) It is formed during an early step in the reaction and consumed in a later step.

D) It does not participate in the reaction.

E) It does not appear in the overall equation for the reaction.

Q3) When studying kinetics, it is more accurate to measure instantaneous reaction rates at particular times rather than the average rates of reaction over time intervals. Explain why.

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Chapter 13: Chemical Equilibrium

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Sample Questions

Q1) Consider the statement, "At equilibrium, a reaction has proceeded as far as it will go, and no further reaction will be observed."

a. From a macroscopic viewpoint, is this statement correct ? Explain your answer.

b. From a nanoscale viewpoint, is this statement correct? Explain your answer.

Q2) The concentration equilibrium constant, K_c, and the pressure equilibrium constant, K_p, are related by the expression

A) K_c = K_p(RT)^Dn

B) K_c = K_p(Dn)^RT

C) K_p = K_c(RT)^Dn

D) K_p = K_c(R)^TDn

E) K_p = K_c(Dn)^RT

Q3) A chemical equilibrium may involve

A) reactants and products exhibiting different states of matter

B) molecular rearrangements

C) a chemical change of one compound into another

D) reaction of elements to produce one or more compounds

E) any of these

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Chapter 14: The Chemistry of Solutes and Solutions

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Sample Questions

Q1) Starting with a saturated solution of sodium chloride in water at room temperature, adding solid sodium chloride will

A) increase the concentration of the solution

B) decrease the concentration of the solution

C) increase the anion concentration and decrease the cation concentration of the solution

D) decrease the anion concentration and increase the cation concentration of the solution

E) have no effect on the concentration of the solution

Q2) Which unit of concentration is dependent on temperature?

A) mole%

B) ppm

C) molality

D) molarity

E) mass%

Q3) The solubility in water of magnesium fluoride, MgF₂, is 7.3 mg/100 mL. Is a solution containing 33 mg MgF₂ in 475 mL water unsaturated, saturated, or supersaturated? Show a calculation to support your answer.

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16

Chapter 15: Acids and Bases

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Sample Questions

Q1) Which compound is the most acidic?

A) GeH₄

B) H₂Se

C) HBr

D) AsH₃

E) H₂O

Q2) Which substance can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry acid?

A) HPO₄^2-

B) H₂O

C) NH₄⁺

D) PO₄^3-

E) HSO₄^-

Q3) Which of the following salts forms an acidic solution when dissolved in water?

A) LiF

B) K₃PO₄

C) NH₄ClO₄

D) NaOCl

E) NaNO₃

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Page 17

Chapter 16: Additional Aqueous Equilibria

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Sample Questions

Q1) A buffer solution is 0.500 M in ascorbic acid and 0.500 M in sodium ascorbate. Its pH is 4.10. After addition of 10 mL of 1 M NaOH to 1.00 L of this buffer, the most likely value of the pH is

A) 4.08.

B) 4.10.

C) 4.12.

D) 5.95.

E) 10.15.

Q2) In which aqueous solution would the smallest amount of barium sulfate dissolve?

A) 0.1 M Mg(OH)₂

B) 0.1 M Na₂SO₄

C) 0.1 M Al₂(SO₄)₃

D) 0.1 M Ba(NO₃)₂

E) 0.1 M HCl

Q3) In which liquid or solution would CuI(s) have the greatest solubility?

A) 0.1 M aqueous ammonia

B) distilled water

C) 0.1 M aqueous copper(I) nitrate

D) saturated aqueous calcium hydroxide

E) 0.1 M aqueous sodium iodide

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Chapter 17: Thermodynamics: Directionality of Chemical Reactions

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Sample Questions

Q1) The boiling point of tin is 232^\(\circ\)C. The heat of vaporization of tin at its boiling point is 247 kJ. The entropy of vaporization is

A) 2045 J/K.

B) 1065 J/K.

C) 939 J/K.

D) 489 J/K.

E) 2.04 J/K.

Q2) Which has the highest entropy?

A) H₂O(g) at 150^\(\circ\)C

B) H₂O(g) at 100^\(\circ\)C

C) H₂O(l) at 100^\(\circ\)C

D) H₂O(l) at 4^\(\circ\)C (the temperature of maximum density)

E) H₂O(s) at -50^\(\circ\)C

Q3) Which has the highest entropy at a given temperature?

A) SO₂(s)

B) S(s)

C) O₂(g)

D) SO₂(l)

E) SO₂(g)

Page 19

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Chapter 18: Electrochemistry and Its Applications

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Sample Questions

Q1) Which compound contains the atom with the highest oxidation number?

A) FeCl₃

B) SnH₄

C) NaClO₄

D) CrO₃

E) H₂O₂

Q2) Which change describes an oxidation half-reaction?

A) decrease in oxidation number

B) loss of electrons

C) electrons as reactants

D) reactant acting as an oxidizing agent

E) pure oxygen becoming oxide ion

Q3) Galvanizing a metal (coating its surface with zinc) to prevent corrosion works because

A) the coating limits access of oxygen to the metal surface

B) the coating reacts to give an impermeable layer of zinc hydroxide

C) the zinc coating provides cathodic protection

D) of reasons a and b.

E) of reasons a, b, and c.

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Page 20

Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) Which element has only radioactive isotopes?

A) Al

B) La

C) Li

D) Lr

E) Ir

Q2) A radioactive isotope that decomposes by K-electron capture emission

A) combines one of its electrons with one of its protons creating an additional neutron

B) gains an electron from its environment

C) gains a helium nucleus

D) gains a particle similar to an electron, but positively charged

E) gains a negatively-charged neutron

Q3) A radioactive isotope that decomposes by beta particle emission loses

A) a positron

B) an electron

C) a neutron

D) a proton

E) a helium nucleus

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