Physical Science Textbook Exam Questions - 4358 Verified Questions

Physical Science

Textbook Exam Questions

Course Introduction

Physical Science is an interdisciplinary course that provides an introduction to the fundamental principles governing the physical world. Covering topics from physics, chemistry, astronomy, and earth science, the course explores the nature of matter, energy, motion, and the forces that shape our universe. Students develop problem-solving skills as they investigate scientific concepts such as atomic structure, chemical reactions, the laws of motion, waves, electricity, magnetism, and the properties of solids, liquids, and gases. The course emphasizes the scientific method, real-world applications, and hands-on experiments to enhance understanding of the basic laws that underpin both the natural environment and modern technology.

Recommended Textbook Chemistry 7th Edition by John E. McMurry

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Chapter 1: Chemical Tools: Experimentation and Measurement

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Q1) A gold ingot weighs 5.50 lbs.If the density of gold is 19.31 g/cm³,and the length and width of the ingot are 12.0 cm and 3.00 cm respectively,what is the height of the ingot?

A)6.50 × 10^-3 cm

B)3.59 cm

C)10.2 cm

D)1.34 × 10³ cm

Answer: B

Q2) How many significant figures are there in the answer for the following problem? 23.1 + 0.5588 + 17 = ?

A)one

B)two

C)three

D)four

Answer: B

Q3) The meter is closest in length to the English system unit the ________.

Answer: yard

Q4) Chemistry is the study of the composition,properties,and transformations of

Answer: matter

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Chapter 2: Atoms, molecules, and Ions

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Q1) Which element has the chemical symbol,P?

A)lead

B)phosphorus

C)platinum

D)potassium

Answer: B

Q2) Which group of elements reacts violently with water?

A)halogens

B)noble gases

C)alkali metals

D)alkaline earth metals

Answer: C

Q3) The subatomic particles contained in the nucleus of an atom are ________ and

Answer: protons,neutrons

Q4) The number of electrons in the ion Ca²⁺ is ________.

Answer: 18

Q5) The bonding in NaI is ________,whereas the bonding in NH₃ is

Answer: ionic,covalent

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) How many anions are there in 4.50 g of MgBr₂?

A)1.47 × 10²² anions

B)2.94 × 10²² anions

C)2.46 × 10²⁵ anions

D)4.93 × 10²⁵ anions

Answer: B

Q2) When 1.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g)+ 3 O₂(g) 2 N₂(g)+ 6 H₂O(g)

A)0.232 g

B)2.17 g

C)0.464 g

D)1.86 g

Answer: A

Q3) The fundamental SI unit for measuring matter is the ________.

Answer: mole

Q4) The number of grams in 0.250mol of urea, (NH₂)₂CO,is ________.

Answer: 15.0 g

Page 5

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Chapter 4: Reactions in Aqueous Solutions

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Q1) The concentration of an aqueous solution of NaOCl can be determined by a redox titration with iodide ion in acidic solution: OCl^- (aq)+ 2 I^- (aq)+ 2 H (aq) Cl (aq)+ I₂ (aq)+ H₂O (l)

Assume that the black spheres in the buret represent I ions,the gray spheres in the flask represent OCl ions,the concentration of the I ions in the buret is 0.120 M,and the volumes in the buret and the flask are identical.What is the concentration of the NaOCl in the flask,and what fraction of the I solution in the buret must be added to the flask to react with all the OCl ions?

A)0.0400 M NaOCl;1/3 of the I must be added.

B)0.0400 M NaOCl;2/3 of the I must be added.

C)0.0600 M NaOCl;1/3 of the I must be added.

D)0.0600 M NaOCl;2/3 of the I must be added.

Q2) When 220.mL of 1.50 × 10^-4M hydrochloric acid is added to 125 mL of 1.75 × 10^-4 M Mg(OH)₂,the resulting solution will be A)acidic.

B)basic

C)neutral.

D)It is impossible to tell from the information given.

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Chapter 5: Periodicity and the Electronic Structure of Atoms

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Q1) How many subshells are there in the shell with n = 6?

A)5

B)6

C)15

D)36

Q2) The element Bh has how many valence electrons?

A)2

B)5

C)7

D)1

Q3) How many unpaired electrons are in an atom of Mt in its ground state?

A)1

B)2

C)3

D)5

Q4) The highest note on a piano has a frequency of 4186 Hz.In a vacuum 4186 Hz has a corresponding wavelength of ________ m.

Q5) Using shorthand notation,the electron configuration of Ni is ________.

Q6) What is the deBroglie wavelength in meters of a 1-ton (907 kg)vehicle having a velocity of 95 km/hr?

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Chapter 6: Ionic Compounds: Periodic Trends and Bonding

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Q1) Which chemical process is associated with the lattice energy for sodium chloride?

A)NaCl(s) Na⁺(g)+ Cl^-(g)

B)NaCl(g) Na⁺(g)+ Cl^-(g)

C)Na(s)+ 1/2 Cl₂(g) NaCl(s)

D)NaCl(s)+ H₂O(l) Na⁺(aq)+ Cl^-(aq)

Q2) Which ionic compound would be expected to have the highest lattice energy?

A)Li₂Se

B)MgS

C)Al₂O₃

D)CO₂

Q3) Atoms of which element,indicated by letter on the periodic table above,would be expected to have the highest first ionization energy,E_i1?

A)A

B)B

C)C

D)D

Q4) The group 4A element that always obeys the octet rule in its stable compounds is ________.

Q5) The ion that has 28 protons and 26 electrons is ________.

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Chapter 7: Covalent Bonding and Electron-Dot Structures

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Q1) In the most acceptable electron-dot structure for carbonyl fluoride,COF₂ the central atom is

A)C,which is singly-bonded to O.

B)C,which is doubly-bonded to O.

C)O,which is singly-bonded to C

D)O,which is doubly-bonded to C.

Q2) Of the following elements,which has the highest electronegativity?

A)As

B)Se

C)Y

D)Sb

Q3) Element A has an electronegativity of 0.8 and element B has an electronegativity of 3.0.Which statement best describes the bonding in A₃B?

A)The AB bond is largely covalent with a - on A.

B)The AB bond is largely covalent with a + on A.

C)The compound is largely ionic with A as the cation.

D)The compound is largely ionic with A as the anion.

Q4) Based on formal charges,the best Lewis electron-dot structure of BF₃ has a B-F bond order equal to ________.

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Chapter 8: Covalent Compounds: Bonding Theories and

Molecular Structure

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Q1) The number of sp² hybrid orbitals on the carbon atom in CO₃^2- is A)one.

B)two.

C)three.

D)four.

Q2) The bonds in the polyatomic ion CO₃^2- are classified as A)ionic.

B)metallic.

C)nonpolar covalent.

D)polar covalent.

Q3) What is the molecular geometry of SbCl₃?

A)T-shaped

B)tetrahedral

C)trigonal planar

D)trigonal pyramidal

Q4) The molecular geometry of OCCl₂ is ________.

Q5) Are the -bonds in CH₃CO₂^- delocalized or localized?

Page 10

Q6) The polarity of CCl₄ is ________.

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Chapter 9: Thermochemistry: Chemical Energy

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Q1) The reaction 4 Ag(s)+ O₂(g) 2 Ag₂O(s)favors Ag₂O at low temperature,but it favors Ag and O₂ at high temperatures.How can this be explained in terms of H and S?

A) H is negative and S is negative.

B) H is negative and S is positive.

C) H is positive and S is negative.

D) H is positive and S is positive.

Q2) Ethyl alcohol is produced by the fermentation of glucose,C₆H₁₂O₆.

C₆H₁₂O₆(s) 2 C₂H₅OH(l)+ 2 CO₂(g) H° = -69.1 kJ

Given that the enthalpy of formation is -277.7 kJ/mol for C₂H₅OH(l)and -393.5 kJ/mol for CO₂(g),find the enthalpy of formation for C₆H₁₂O₆.

A)-1411.5 kJ/mol

B)-1273.3 kJ/mol

C)-740.3 kJ/mol

D)-602.1 kJ/mol

Q3) The law of conservation of energy is also known as the ________ law of thermodynamics.

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Chapter 10: Gases: Their Properties and Behavior

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Q1) Historical records of greenhouse gases can be found in A)polar ice caps.

B)oil from the ground.

C)the Alps.

D)the Dead Sea Scrolls.

Q2) Refrigeration and air conditioning are a source of greenhouse gases such as A)CHClF₂. B)Ne.

C)HBr.

D)H₂.

Q3) A carbon dioxide monitoring product provides a reading of 202 ppm.Calculate the percent carbon dioxide by volume.

A)2.02

B)0.0202

C)0.202

D)20.2

Q4) According to Graham's law,the rate of effusion of a gas is inversely proportional to the ________.

Q5) The region of the atmosphere that is closest to the earth's surface is the ________.

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Chapter 11: Liquids, solids, and Phase Changes

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Sample Questions

Q1) Which of the following forms a molecular solid?

A)CaCl₂ 

B)C₉H₈O₄

C)C,graphite

D)palladium

Q2) For the process: HNO₃(g) HNO₃(l), H° is -39.04 kJ/mol and S° is -111.74 J/(mol K).What is the normal boiling point of pure HNO₃?

A)2.86°C

B)76.2°C

C)270.3°C

D)349.4°C

Q3) The property of a liquid that is a measure of the liquid's resistance to increase its surface area is ________.

Q4) Which is classified as an amorphous solid?

A)palladium(II)bromide

B)phosphorus tetrachloride

C)plastic

D)potassium iodide

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Chapter 12: Solutions and Their Properties

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Q1) A solution is prepared by dissolving 17.75 g sulfuric acid,H₂SO₄,in enough water to make 100.0 mL of solution.If the density of the solution is 1.1094 g/mL,what is the mole fraction H₂SO₄ in the solution?

A)0.0181

B)0.0338

C)0.0350

D)19.0

Q2) Assume that the vapor at point c is condensed and reboiled.What is the vapor composition during reboiling?

A)100% decane

B)composition at point b

C)composition at point c

D)composition at point e

Q3) What volume of 0.716 M KBr solution is needed to provide 13.0 g of KBr?

A)6.55 mL

B)9.31 mL

C)18.5 mL

D)153 mL

Q4) Molarity is defined as ________,whereas molality is defined as ________.

Page 15

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) Which of the elementary reactions shown above has a molecularity of three?

A)elementary reaction (a)

B)elementary reaction (b)

C)elementary reaction (c)

D)elementary reactions (a), (b),and (c)

Q2) The aquation of tris(1,10-phenanthroline)iron(II)in acid solution takes place according to the equation: Fe(phen)₃²⁺ + 3 H₃O⁺ + 3 H₂O Fe(H₂O)₆²⁺ + 3 phenH⁺

If the activation energy is 126 kJ/mol and frequency factor is 8.62 × 10¹⁷ s^-1,at what temperature is the rate constant equal to 3.63 × 10^-3 s^-1 for the first-order reaction?

A)0°C

B)36°C

C)50°C

D)94°C

Q3) An aqueous reaction occurs by a two-step mechanism,shown below.

Step 1: A₂X₂ + Y A₂X + XY

Step 2: A₂X₂ + XY A₂X + X₂ + Y In this reaction the intermediate is ________,and the catalyst is ________.

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Chapter 14: Chemical Equilibrium

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Q1) The reaction CaCO₃(s) CaO(s)+ O₂(g)is endothermic 298 K.The effect of increasing the partial pressure of O₂ in the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO₃ once equilibrium is reestablished.

Q2) If K_c is the equilibrium constant for a forward reaction what is K_c' for the reverse reaction?

A)- K_c

B)K_c

C)(K_c)^-1

D)none of these

Q3) A 1.50 L vessel contains an equilibrium mixture of 0.100 mol of NO,0.150 mol of Br₂,and 0.250 mol of NOBr at 25°C.What is the value of K_p for the reaction below? 2 NO(g)+ Br₂(g) 2 NOBr(g)

A)2.56

B)62.5

C)1.28 × 10²

D)1.53 × 10³

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Chapter 15: Aqueous Equilibria: Acids and Bases

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Q1) What is the hydronium ion concentration of a 0.100 M acetic acid solution with a K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is:

CH₃CO₂H(aq)+ H₂O(l) H₃O⁺(aq)+

CH₃CO₂^-(aq).

A)1.3 × 10^-2 M

B)4.2 × 10^-2 M

C)1.3 × 10^-3 M

D)4.2 × 10^-3 M

Q2) Which one of the following salts,when dissolved in water,produces the solution with the lowest pH?

A)NaI

B)KI

C)MgI₂

D)AlI₃

Q3) Identify the Br nsted-Lowry bases.

A)(1)and (3)

B)(1)and (4)

C)(2)and (3)

D)(2)and (4)

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Chapter 16: Applications of Aqueous Equilibria

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Q1) Which point a-d represents the first equivalence point?

A)point a

B)point b

C)point c

D)point d

Q2) Which of the following titrations result in a basic solution at the equivalence point?

A)HCl titrated with LiCH₃CO₂

B)HOCl titrated with KOH

C)HI titrated with LiOH

D)Pb(NO₃)₂ titrated with NaI

Q3) Which is a net ionic equation for the neutralization of a strong acid with a strong base?

A)HI(aq)+ NaOH(aq) H₂O(l)+ NaI(aq)

B)H₃O⁺(aq)+ OH^-(aq) 2 H₂O(l)

C)HF(aq)+ NaOH(aq) H₂O(l)+ NaF(aq)

D)HCl(aq)+ OH^-(aq) H₂O(l)+Cl^-(aq)

Q4) What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

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Chapter 17: Thermodynamics: Entropy, free Energy, and Equilibrium

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Q1) At high temperatures,boron carbide vaporizes according to B₄C(s) 4 B(g)+ C(s)

At 2500 K,the equilibrium pressure of B(g)is 0.0342 mm Hg over a mixture of 0.300 mol B₄C(s)and 0.500 mol C(s).Calculate G° for this process.

A)832 kJ

B)799 kJ

C)281 kJ

D)247 kJ

Q2) The brown color associated with photochemical smog is due to NO₂(g),which is involved in an equilibrium with N₂O₄(g)in the atmosphere. 2 NO₂(g) N₂O₄(g)

Predict the signs of the enthalpy and entropy change for the forward reaction.

A)The enthalpy change is negative and the entropy change is negative.

B)The enthalpy change is negative and the entropy change is positive.

C)The enthalpy change is positive and the entropy change is negative.

D)The enthalpy change is positive and the entropy change is positive.

Q3) A reaction has G° = + 21.5 kJ/mol, H° = + 25.0 kJ/mol,and S° = + 15.0 J/molK can become spontaneous at a temperature of ________ K.

Page 20

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Chapter 18: Electrochemistry

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Q1) Consider the galvanic cell,Pb(s) Pb²⁺(aq) Cu²⁺(aq)

Cu(s).Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive)?

A)increase the [Pb²⁺] concentration

B)increase the [Cu²⁺] concentration

C)increase the mass of Pb(s)

D)decrease the mass of Pb(s)

Q2) If the cell reaction involves ions in solution,as the cell reaction in a galvanic cell continues,

A)E for the cell increases.

B)E for the cell decreases.

C)E° for the cell increases.

D)E° for the cell decreases.

Q3) According to Table 17.1,which aqueous metal ion will reduce Ag⁺,but not Cu²⁺?

A)Fe²⁺

B)Fe³⁺

C)Mn²⁺

D)Sn²⁺

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Chapter 19: Nuclear Chemistry

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Q1) Elements with ________ atomic mass are best possible candidates for a fusion reaction.

A)very low

B)moderate

C)moderate to heavy

D)very heavy

Q2) Relative to the amount of energy released in a typical chemical reaction,the amount of energy released in a typical fission reaction is about A)the same.

B)1/2 times greater.

C)10⁸ times greater

D)10⁷times greater

Q3) ²⁰¹Tl is used in myocardial perfusion imaging.It undergoes beta decay with a half-life of 73 hours generating 80 keV X-rays.A typical dose is 2.5 mCi which is equal to ________ Bq.

Q4) An average person receives 40 mrem of radiation from medical procedures annually.If a dose as low as 25 rem can lead to a decrease in white blood cell count,what is the maximum number of medical procedures that involve radiation allowable before white blood cell count decrease occurs?

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Chapter 20: Transition Elements and Coordination Chemistry

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Q1) What is the name of the complex [Ni(H₂O)₄(NH₂CH₂CH₂N H₂)]SO₄ 5H₂O?

A)aquaethylenediaminenickel(II)sulfate hydrate

B)tetraaquaethylenediaminenickel(II)sulfate pentahydrate

C)tetraaquabis(ethylenediamine)nickel(II)sulfate pentahydrate

D)tetraaquabis(ethylenediamine)nickel(III)sulfate pentahydrate

Q2) Which of the Co(III)complexes above are enantiomers of each other?

A)(A)and (B)

B)(C)and (D)

C)(A), (B),and (C)

D)(A), (B), (C),and (D)

Q3) Using the above schematic of an artist's color wheel,determine the color absorbed if a substance is seen as being green in color.

A)blue

B)orange

C)red

D)violet

Q4) Cr²⁺ has ________ d electrons.

Q5) The formula for tetraamminediiodochromium(III)bromide is ________.

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Chapter 21: Metals and Solid-State Materials

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Q1) What structural features appear necessary for superconductivity in the 1-2-3 YBa₂Cu₃O₇ superconductor?

A)high metallic character

B)infinite extended layers of Cu and O atoms and a fractional oxidation state for Cu

C)presence of an inner transition element

D)All of these are necessary.

Q2) Which one of the following is an electrical insulator?

A)alumina

B)germanium doped with antimony

C)gold

D)tellurium

Q3) In this picture the valence band is given by letter(s)

A)a.

B)b.

C)c.

D)a and b.

Q4) One source of titanium is pyrophanite,MnTiO₃.The oxidation states of manganese and titanium in pyrophanite are ________ and ________,respectively.

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Chapter 22: The Main-Group Elements

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Q1) Which statement is most inconsistent with the chemistry of silicon?

A)In nature,it is generally found combined with oxygen in SiO₂ and in various silicate minerals.

B)It crystallizes in a diamond-like structure and does not form the graphite-like allotrope.

C)It is a hard,gray,semiconducting solid that melts at 1410°C.

D)It is obtained by oxidation of silica sand with coke.

Q2) Which of the following is a peroxide?

A)Li₂O

B)K₂O₂

C)CaO

D)CsO₂

Q3) Covalent hydrides of the type MH₃ are likely to form with elements of what group?

A)3A

B)4A

C)5A

D)6A

Q4) Carbon combines with some metals and semimetals to form carbides.What is the formula of aluminum carbide?

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Chapter 23: Connections to Organic and Biological Chemistry

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Q1) Which compound will exhibit cis-trans isomerism?

A)1,2-dichloroethane

B)1,2-dichloroethene

C)dichloroethyne

D)ethylene

Q2) Monosaccharides are classified as either ________ or ________.

Q3) None of the listed compounds contains a ring.Which could have one carbon-carbon triple bond?

A)C₃H₈

B)C₂H₂

C)C₁₀H₂₀

D)All of these

Q4) What is an example of the proper number of bonds to carbon?

A)two double bonds

B)one double bond + one triple bond

C)three single bonds

D)five single bonds

Q5) The four cyclic amine bases that occur in DNA are ________,________,________,and ________.

Page 26

Q6) Linoleic acid,a fatty acid,contains ________ carbons and ________ double bonds.

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