Physical Science Test Questions - 2075 Verified Questions

Physical Science

Test Questions

Course Introduction

Physical Science is an interdisciplinary course that provides an introduction to the fundamental concepts of physics and chemistry. Students explore the structure and properties of matter, energy, forces, motion, and the basic principles governing physical and chemical changes in the natural world. Emphasis is placed on scientific inquiry, observation, and experimentation, allowing students to develop critical thinking and problem-solving skills while understanding the relevance of physical science in everyday life and technological advancements.

Recommended Textbook Chemistry and Chemical Reactivity 9th Edition by John C. Kotz\New folder

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Chapter 1: Basic Concepts of Chemistry

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Sample Questions

Q1) Which of the following observations is/are examples of chemical change?

1)Iron (Fe)rusts,forming Fe₂O₃.

2)The density of water increases when it changes from a solid to a liquid.

3)Sodium chloride melts at 801\(^{\circ}\)C.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 2 and 3

Answer: A

Q2) Properties,such as color and density,which can be observed or measured without changing the composition of a substance are called ________ properties.

Answer: physical

Q3) What is the symbol for the element \(\underline{\text{ potassium?}}\)

A) K

B) Po

C) Pt

D) Kr

E) P

Answer: A

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Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry

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Q1) Calcium carbonate,or limestone,is relatively insoluble in water.At 25\(^{\circ}\)C,only 5.8 mg will dissolve in 1.0 liter of water.What volume of water is needed to dissolve 5.0 g of calcium carbonate?

A) 4.6 \(\times\) 10^-3 L

B) 3.0 \(\times\) 10^-2 L

C) 1.4 \(\times\) 10² L

D) 3.4 \(\times\) 10² L

E) 8.6 \(\times\) 10² L

Answer: E

Q2) Which is the largest volume?

A) 10 dL

B) 10 pL

C) 10 cL

D) 10 mL

E) 10 nL

Answer: A

Q3) Assuming the density of water is 1.00 g/cm³,the mass of 1.0 cubic meter (m³) of water is ________ grams.

Answer: 1.0 \(\times\) 10⁶

Page 4

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Chapter 3: Atoms, molecules, and Ions

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Q1) What is the mass of 8.04 \(\times\) 10^-3 mol O₂?

A) 2.51 \(\times\) 10^-4 g

B) 5.03 \(\times\) 10^-4 g

C) 0.129 g

D) 3.89 g

E) 0.257 g

Answer: E

Q2) In reactions,metals generally lose electrons to become ________,and nonmetals gain electrons to become anions.

Answer: cations

Q3) What is the correct name for Cl₂O₇?

A) dichlorine heptoxide.

B) chlorine oxide.

C) dichloride heptoxide.

D) dichlorine heptaoxygen.

E) chlorine heptaoxygen.

Answer: A

Q4) What are the names of four metalloids?

Answer: boron,silicon,germanium,arsenic,(antimony,and tellurium)

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Chapter 4: Chemical Reactions

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Q1) Which of the following are classified as precipitation reactions?

1)AgNO₃(aq)+ HCl(aq)\(\to\) AgCl(s)+ HNO₃(aq)

2)2Mg(s)+ O₂(g)\(\to\) 2MgO(s)

3)Zn(s)+ 2Ag⁺(aq)\(\to\) 2Ag(s)+ Zn²⁺(aq)

A) 1 only

B) 2 only

C) 3 only

D) 2 and 3

E) 1,2,and 3

Q2) Which of the following chemical equations is an acid-base reaction?

A) Ba(OH)₂(aq)+ K₂SO₄(aq)\(\to\) BaSO₄(s)+ 2 KOH(aq)

B) 3 NaOH(aq)+ AlCl₃(aq)\(\to\) Al(OH)₃(s)+ 3 NaCl(aq)

C) 2 H⁺(aq)+ Zn(s)\(\to\) H₂(g)+ Zn²⁺(aq)

D) 2 HCl(aq)+ Pb(NO₃)₂(aq)\(\to\) PbCl₂(s)+ 2 HNO₃(aq)

E) H₃PO₄(aq)+ NH₃(aq)\(\to\) NH₄⁺(aq)+ H₂PO₄^-(aq)

Q3) _____-oxides produce acids when reacted with water.

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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions

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Sample Questions

Q1) The pH of a vinegar solution is 4.15.What is the H₃O⁺ concentration of the solution?

A) 7.1 \(\times\) 10^-5 M

B) 1.6 \(\times\) 10^-2 M

C) 0.62 M

D) 1.4 M

E) 1.4 \(\times\) 10⁴ M

Q2) What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO?

Fe₂O₃(s)+ 3 CO(g)\(\to\) 2 Fe(s)+ 3 CO₂(g)

A) 2.19 kg

B) 30.6 kg

C) 61.2 kg

D) 122 kg

E) 512 kg

Q3) The reaction of 5.07 g N₂ with 0.722 g H₂ produces 1.27 g NH₃.The percent yield of this reaction is ________.

Q4) The pH of purified water (or of a neutral solution)is _____.

Page 7

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Chapter 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

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Sample Questions

Q1) Which of these physical changes would require the release of energy?

A) condensing a gas

B) boiling a liquid

C) melting a solid

D) all of these

E) none of these

Q2) Commercial cold packs consist of solid ammonium nitrate and water.NH₄NO₃ absorbs 25.69 kJ of heat per mole dissolved in water.In a coffee-cup calorimeter,5.60 g NH₄NO₃ is dissolved in 100.0 g of water at 22.0 S1U1P1\(\circ\)S1S1P0C.What is the final temperature of the solution? Assume that the solution has a specific heat capacity of 4.18 J/g.K.

A) 0.0 S1U1P1\(\circ\)S1S1P0C

B) 17.9 S1U1P1\(\circ\)S1S1P0C

C) 11.6 S1U1P1\(\circ\)S1S1P0C

D) -54.8 S1U1P1\(\circ\)S1S1P0C

E) 26.1 S1U1P1\(\circ\)S1S1P0C

Q3) The heat required to convert a solid at its melting point to a liquid is called the heat of ________.

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Chapter 7: The Structure of Atoms

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Sample Questions

Q1) The n = ____ shell is the lowest that may contain s-orbitals.

A) 1

B) 2

C) 3

D) 4

E) 5

Q2) If a hydrogen atom in the excited n = 4 state relaxes to the ground state,what is the maximum number of possible emission lines?

A) 1

B) 3

C) 6

D) 8

E) infinite

Q3) For which of the following transitions would a hydrogen atom emit the lowest energy photon?

A) n = 4 to n = 5

B) n = 5 to n = 2

C) n = 4 to n = 3

D) n = 3 to n = 1

E) n = 3 to n = 2

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Chapter 8: The Structure of Atoms and Periodic Trends

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Q1) What is the ground state electron configuration for Cr³⁺?

A) [Ar]

B) [Ar]3d⁷4s²

C) [Ar]3d¹4s²

D) [Ar]3d²4s¹

E) [Ar]3d³

Q2) Which of the following ions have the same ground state electron configuration: S^2-,N^3-,Mg²⁺,and Br^-?

A) N^3- and Mg²⁺

B) S^2-,N^3-,and Br^-

C) S^2- and Br^-

D) Mg²⁺ and Br^-

E) S^2-,N^3-,Mg²⁺,and Br^-

Q3) Explain the difference between paramagnetic and ferromagnetic.

Q4) Place the following atoms in order of increasing atomic radii: Se,Sb,Br,and Te.

A) Br < Se < Te < Sb

B) Se < Br < Sb < Te

C) Se < Br < Te < As

D) Sb < Te < Se < Br

E) Te < Sb < Se < Br

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Chapter 9: Bonding and Molecular Structure

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Q1) When you draw the Lewis structure for PF₂Cl₃,how many single bonds,double bonds,and lone pair electrons reside on the central phosphorus atom?

A) 5 single bonds,0 double bonds,0 lone pairs

B) 4 single bonds,1 double bond,0 lone pairs

C) 5 single bonds,0 double bonds,1 lone pair

D) 4 single bonds,1 double bond,1 lone pair

E) 3 single bonds,2 double bonds,0 lone pairs

Q2) Which of the following statements is/are CORRECT?

1)Ionic bonds form when one or more valence electrons are transferred from one atom to another.

2)Covalent bonds involve sharing of electrons between atoms.

3)In most covalently bonded compounds,electrons are NOT shared equally between the atoms.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

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Chapter 10: Bonding and Molecular Structure: Orbital

Hybridization and Molecular Orbitals

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Q1) What is the hybridization of the sulfur atom in SO₄^2-?

A) sp

B) sp²

C) sp³

D) none

Q2) What is the molecular geometry around a central atom that is sp² hybridized,has three sigma bonds,and one pi bond?

A) trigonal-planar

B) trigonal-pyramidal

C) bent

D) T-shaped

E) tetrahedral

Q3) In HF₂^- the hydrogen is shared between the two fluorine atoms.Which theory,valence bond or molecule orbital,correctly accounts for this three-center bonding?

Q4) The hybridization of the carbon atom in CF₃⁺ is ________.

Q5) Which theory,valence bond or molecule orbital,correctly predicts the existence of paramagnetic molecules?

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Chapter 11: Gases and Their Properties

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Q1) Which of the following samples contains the fewest moles of gas?

A) 1.00 L of CH₄ at STP

B) 1.00 L of Ar at -10.0°C and 1.00 atm

C) 1.00 L of NH₃ at 10°C and 1.00 atm

D) 1.00 L of H₂ at 0.0°C and 1.76 atm

E) 1.00 L of HCl at 20°C and 1.00 atm

Q2) Absolute zero is the point at which

A) a straight-line graph of V versus T (S1U1P1\(\circ\)S1S1P0C)intersects the origin.

B) a straight-line graph of 1/V versus P at constant T intersects the origin.

C) gaseous helium liquefies.

D) a straight-line graph of V versus 1/P at constant T intersects the origin.

E) a straight-line graph of V versus T (K)intersects the origin.

Q3) Which of the following gases has the greatest density at 35 S1U1P1\(\circ\)S1S1P0C and 450 mm Hg?

A) CH₄

B) Ar

C) N₂

D) Cl₂

E) C₃H₈

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Chapter 12: Intermolecular Forces and Liquids

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Q1) At 75.0 S1U1P1\(\circ\)S1S1P0C,water has an equilibrium vapor pressure of 289.1 mm Hg.If 4.22 g H₂O is sealed in an evacuated 5.00 L flask and heated to 75.0 S1U1P1\(\circ\)S1S1P0C,what mass of H₂O will be found in the gas phase when liquid-vapor equilibrium is established? Assume any liquid remaining in the flask has a negligible volume.(R = 0.08206 L.atm/mol.K,1 atm = 760 mm Hg)

A) 0.834 g

B) 1.20 g

C) 1.92 g

D) 3.02 g

E) 4.22 g

Q2) For a particular liquid,raising its temperature from 321 K to 352 K causes its vapor pressure to double.What is the enthalpy of vaporization of this liquid? (R = 8.314 J/K · mol)

A) 21.0 kJ/mol

B) 186 kJ/mol

C) 3.29 kJ/mol

D) 383 kJ/mol

E) 179 kJ/mol

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Chapter 13: The Chemistry of Solids

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Q1) Gold crystallizes in a face-centered cubic lattice with an edge length of 407.8 pm.What is the density of gold?

A) 1.21 g/cm³

B) 4.82 g/cm³

C) 2.41 g/cm³

D) 9.65 g/cm³

E) 19.3 g/cm³

Q2) Which of the following statements concerning a metal crystallized in a face-centered cubic cell is/are CORRECT?

1)One metal atom is located on each face of the unit cell,where it is shared equally between four unit cells.

2)One metal atom is located at the center of the unit cell.

3)A metal atom is located at each of the eight lattice points,where it is shared equally between eight unit cells.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 1,2 and 3

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Page 15

Chapter 14: Solutions and Their Behavior

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Q1) A surfactant used for cleaning is called a(n)________.

Q2) What is the freezing point of an aqueous 1.36 m NaCl solution? (K_fp for water is 1.858°C/m.)Assume no ion pairing occurs.

A) 5.1°C

B) 2.5°C

C) -5.1°C

D) 0.0°C

E) -2.5°C

Q3) Which action(s)will decrease the equilibrium concentration of an inert gas (such as N₂)in water?

1)decreasing the temperature of the water

2)increasing the volume of water

3)decreasing the pressure of the gas above the liquid

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 1,2,and 3

Q4) ________ are colloidal dispersions of one liquid in another liquid.

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Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions

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Q1) The reaction kinetics for a certain reaction are studied over several temperatures.Which of the following is/are \(\underline{\text{not }}\) effected by a change in reaction temperature?

A) the reaction rate

B) the rate constant,k

C) the energy of activation,E_a

D) a and b

E) a,b,and c

Q2) Calculate the activation energy,E_a,for N₂O₅(g)\(\to\) 2 NO₂(g)+ 1/2 O₂(g)

Given k (at 45.0 S1U1P1\(\circ\)S1S1P0C)= 5.79 \(\times\) 10^-4 s^-1 and k (at 60.0 S1U1P1\(\circ\)S1S1P0C)= 3.83 \(\times\) 10^-3 s^-1.(R = 8.314 J/K.mol)

A) 0.256 kJ/mol

B) 2.83 kJ/mol

C) 31.1 kJ/mol

D) 111 kJ/mol

E) 389 kJ/mol

Q3) Radioactive isotopes decay by ________-order kinetics.

Q4) Termolecular elementary steps are rare.Why?

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Chapter 16: Principles of Reactivity: Chemical Equilibria

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Q1) In 1913,the Haber-Bosch process was patented.The product of the Haber-Bosch process is ________.

Q2) The symbol Q is called the ________.

Q3) If the reaction quotient,Q,is greater than K in a gas phase reaction,then

A) the chemical system has reached equilibrium.

B) the temperature must be increased for the reaction to proceed in the forward direction.

C) the reaction will proceed in the forward direction until equilibrium is established.

D) the reaction will proceed in the backward direction until equilibrium is established.

E) the reaction will proceed in the direction that increases the number of gas phase particles.

Q4) If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.

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Chapter 17: The Chemistry of Acids and Bases

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Q1) All of the following species behave as Lewis acids EXCEPT ____.

A) BH₃

B) Al³⁺

C) SO₂

D) Al(OH)₃

E) NH₃

Q2) Which of the following statements is INCORRECT?

A) H₃PO₄ is a stronger acid than H₂PO₄^-.

B) HClO₃ is a stronger acid than HClO₂.

C) HNO₃ is a stronger acid than HNO₂.

D) [Fe(H₂O)₆]²⁺ is a stronger acid than [Fe(H₂O)₆]³⁺.

E) HOCl is stronger acid than HOBr.

Q3) Which is NOT an amphiprotic species in water?

A) HClO₃

B) HSO₃^-

C) H₃O⁺

D) HS^-

E) HCO₃^-

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Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria

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Q1) A 1.0-liter solution contains 0.25 M HF and 0.32 M NaF (K_afor HF is 7.2 \(\times\) 10^-4).If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the \(\underline{\text{ change }}\) in pH?

A) 0.02

B) 3.27

C) 0.13

D) -0.11

E) -0.28

Q2) Two important biological buffer systems control pH in the range between 6.9 and 7.4.These buffer systems are H₂CO₃/HCO₃^- and ________.

Q3) When a weak base is titrated with a strong acid,the pH at the equivalence point is ___.

A) equal to 7

B) greater than 7.

C) less than 7.

D) equal to the acid pK_a.

E) equal to the base pK_b.

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Chapter 19: Entropy and Free Energy

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Q1) \(\Delta\)GS1U1P1\(\circ\)S1S1P0< 0 for a reaction indicates that

A) the reaction favors formation of reactants.

B) the reaction is spontaneous.

C) the reaction is nonspontaneous.

D) the reaction is at equilibrium.

E) the reaction cannot reach equilibrium.

Q2) A 100-mL sample of water is placed in a coffee cup calorimeter.When 1.0 g of an ionic solid is added,the temperature decreases from 21.5°C to 20.8°C as the solid dissolves.For the dissolving of the solid

A) (\(\Delta\)H) < 0

B) (\(\Delta\)S)(universe)> 0

C) (\(\Delta\)S)(system)< 0

D) (\(\Delta\)S)(surroundings)> 0

E) none of these

Q3) For the process Br₂(l)\(\to\) 2Br(g),

A) (\(\Delta\)H) is + and \(\Delta\)S is + for the reaction.

B) (\(\Delta\)H) is + and \(\Delta\)S = 0 for the reaction.

C) (\(\Delta\)H) is - and \(\Delta\)S is - for the reaction.

D) (\(\Delta\)H) is - and \(\Delta\)S is + for the reaction.

E) (\(\Delta\)H) is + and \(\Delta\)S is - for the reaction.

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Chapter 20: Principles of Reactivity: Electron Transfer Reactions

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Q1) Assuming the following reaction proceeds in the forward direction, 3 Sn⁴⁺(aq)+ 2 Cr(s)\(\to\) 3 Sn²⁺(aq)+ 2 Cr³⁺(aq)

A) Sn⁴⁺(aq)is the reducing agent and Cr(s)is the oxidizing agent.

B) Cr(s)is the reducing agent and Sn²⁺(aq)is the oxidizing agent.

C) Sn⁴⁺(aq)is the reducing agent and Sn²⁺(aq)is the oxidizing agent.

D) Cr(s)is the reducing agent and Cr³⁺(aq)is the oxidizing agent.

E) Cr(s)is the reducing agent and Sn⁴⁺(aq)is the oxidizing agent.

Q2) The following electrochemical cell has a potential of +0.326 V at 25 S1U1P1\(\circ\)S1S1P0C.Pt | H₂(g,1.00 atm)| H⁺(aq,1.00 M)|| Cl^-(aq)| AgCl(s)| Ag

The standard reduction potential,ES1U1P1\(\circ\)S1S1P0,of AgCl(s)= +0.222 V.What is the Cl^-(aq)concentration?

A) 1.9 \(\times\) 10^-19 M

B) 5.5 \(\times\) 10^-10 M

C) 0.018 M

D) 1.03 M

E) 1.8 \(\times\) 10⁹ M

Q3) Explain the function of a salt bridge in a voltaic cell.

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Chapter 21: Environmental Chemistry Earths

Environment,energy,and Sustainability

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Q1) The majority of crude oil ends up being used

A) to make synthetic fibers.

B) to make fine chemicals.

C) to make plastics.

D) as fuel.

E) to make rubber.

Q2) The minimum wavelength of light required to decompose a single ozone molecule is 320.nm.Calculate the minimum energy required to decompose 1.00 mole of ozone.(h = 6.626 \(\times\) 10^-34 J.s; c = 3.00 \(\times\) 10⁸ m/s; 1 nm = 10^-9 m; 1mol = 6.022 \(\times\) 10²³)

A) 6.21 \(\times\) 10^-19 kJ/mol

B) 120 kJ/mol

C) 0.374 kJ/mol

D) 374 kJ/mol

E) 0.00267 kJ/mol

Q3) Explain why fossil fuels,hydrocarbons produced by natural processes,are considered a nonrenewable energy resource.

Q4) Explain why the melting of Arctic sea ice will not raise the sea level.

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Chapter 22: The Chemistry of the Main Group Elements

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Q1) Quartz is the pure crystalline form of

A) silica,SiO₂.

B) sodium silicate,NaSiO₄.

C) calcium orthosilicate,Ca₂SiO₄.

D) silicon tetrachloride,SiCl₄.

E) silicon carbide,SiC.

Q2) The only acid that decomposes silicon dioxide is ____.

A) CF₃CO₂H

B) H₂SO₄

C) HBr

D) HF

E) HClO₄

Q3) What mass of MgO would be produced by heating a 300.-kg sample that is 59.0% Mg(OH)₂? Assume complete reaction and no other source of magnesium.

A) 122 kg

B) 256 kg

C) 3.03 kg

D) 434 kg

E) 207 kg

Q4) Give two examples of the allotropes of elemental oxygen.

Page 24

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Chapter 23: The Chemistry of the Transition Elements

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Q1) Which of the following d-block ion electron configurations may be high spin \(\underline{\text{ or }}\) low spin when placed in an \(\underline{\text{ octahedral ligand}}\) field?

A) [Ar]3d⁸

B) [Ar]3d³

C) [Ar]3d⁹

D) [Ar]3d⁴

E) [Ar]3d²

Q2) The spectrochemical series is an arrangement of

A) ligands in order of their tendency to split the d orbitals of a transition metal ion. B) coordination compounds in order of increasing octahedral ligand field splitting. C) complex ions in order of the wavelength of light absorbed. D) ligands in the order of electronegativity. E) ligands in order of Lewis basicity.

Q3) The complex ion [NiCl₄]^2- is paramagnetic,but the complex ion [Ni(NH₃)₄]²⁺ is diamagnetic.Why do the magnetic properties of these two nickel complexes differ?

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25

Chapter 24: Carbon: Not Just Another Element

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Q1) What is the monomer of Teflon?

A) CH₂CH₂

B) CF₂CF₂

C) CH₂C(CN)₂

D) CH₂CHCN

E) CH₂CHCH₃

Q2) The process by which long chain hydrocarbons in petroleum are shortened is called ________.

Q3) Identify the product(s)of the hydrogenation of cis-2-hexene.

A) 2-hydroxyhexane

B) 2,3-dihydroxyhexane

C) trans-2-hexane

D) carbon dioxide and water

E) hexane

Q4) What is the product of the addition of excess F₂ to acetylene?

A) 1,2-difluoroethane

B) ethylene

C) 1,1,2,2-tetrafluoroethane

D) ethane

E) 1,1-difluoroethylene

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Chapter 25: Biochemistry

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54 Verified Questions

54 Flashcards

Source URL: https://quizplus.com/quiz/72720

Sample Questions

Q1) Which of the following functional groups is not found in carbohydrates (sugars)?

A) carboxylic acid

B) alcohol

C) ketone

D) aldehyde

E) ether

Q2) Which of the following units is \(\underline{\text{ not }}\) found in a DNA molecule?

A) a phosphate group

B) a peptide bond

C) an organic base

D) a five-membered ring

E) a ribose sugar

Q3) If you start with a single duplex DNA molecule,how many duplex DNA molecules will you have after 10 amplification cycles by the polymerase chain reaction?

Q4) What is the role of tRNA in protein synthesis?

Q5) The amide linkages in a protein and also called ___ bonds.

Q6) A compound which contains both a positive and negative charge is called a ____.

Q7) The oxygen that bridges two sugars in a disaccharide is known as a ___ bond.

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Chapter 26: Nuclear Chemistry

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Source URL: https://quizplus.com/quiz/72721

Sample Questions

Q1) Which of the following statements is/are CORRECT?

1)The transuranium elements are created in a nuclear reaction sequence that begins with bombardment of a lighter nucleus with low energy helium nuclei.

2)A low energy neutron may be captured by a nucleus,giving a product in which the mass number is increased by one unit.

3)Nuclear reactions involving neutron capture followed by gamma ray emission are referred to as (n,\(\gamma\))reactions.

A) 1 only

B) 2 only

C) 3 only

D) 2 and 3

E) 1,2,and 3

Q2) By what (single step)process does americium-241 decay to neptunium-237?

A) (\(\alpha\)) particle emission

B) (\(\beta\)) particle emission

C) positron emission

D) electron capture

E) neutron capture

Q3) Explain the treatment named boron neutron capture therapy (BNCT).

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