First Year Chemistry Solved Exam Questions - 3326 Verified Questions

First Year Chemistry Solved

Exam Questions

Course Introduction

First Year Chemistry provides a foundational introduction to chemical principles and laboratory techniques essential for further studies in the sciences. Topics include the structure of atoms and molecules, chemical bonding, stoichiometry, states of matter, thermochemistry, chemical equilibria, and basic concepts of acids and bases. Hands-on laboratory sessions complement theoretical knowledge, emphasizing safe practices, experimental design, accurate measurements, and critical data analysis. This course develops problem-solving skills and scientific literacy, equipping students with the tools needed to approach complex chemical phenomena in advanced coursework and real-world applications.

Recommended Textbook Chemistry A Molecular Approach 1st Canadian Ediiton by Nivaldo J. Tro

Available Study Resources on Quizplus

25 Chapters

3326 Verified Questions

3326 Flashcards

Source URL: https://quizplus.com/study-set/2476 Page 2

Chapter 1: Units of Measurement for Physical and Chemical Change

Available Study Resources on Quizplus for this Chatper

179 Verified Questions

179 Flashcards

Source URL: https://quizplus.com/quiz/49191

Sample Questions

Q1) Convert 1.34 km² to m².

A)1340000 m²

B)134000 m²

C)1.34 × 10⁷ m²

D)1.34 × 10⁴ m²

E)1340 m²

Answer: A

Q2) If the outside air temperature is 30 °F, what is the temperature in kelvin?

A)303 K

B)307 K

C)274 K

D)272 K

Answer: D

Q3) A person is 64.00 inches tall. How tall is she in cm?

A)162.6 cm

B)25.20 cm

C)25.60 cm

D)192.0 cm

E)128.0 cm

Answer: A

Page 3

To view all questions and flashcards with answers, click on the resource link above.

Chapter 2: Atoms and Elements

Available Study Resources on Quizplus for this Chatper

167 Verified Questions

167 Flashcards

Source URL: https://quizplus.com/quiz/49192

Sample Questions

Q1) How many moles of potassium are contained in 449 g of potassium?

A)11.5 moles

B)17.6 moles

C)69.2 moles

D)23.9 moles

E)41.5 moles

Answer: A

Q2) Which element has the chemical symbol S?

A)selenium

B)silicon

C)sulfur

D)scandium

Answer: C

Q3) How many xenon atoms are contained in 2.36 moles of xenon?

A)3.92 × 10²⁴xenon atoms

B)2.55 × 10²³xenon atoms

C)1.42 × 10²⁴xenon atoms

D)7.91 × 10²⁵xenon atoms

E)1.87 × 10²⁶xenon atoms

Answer: C

To view all questions and flashcards with answers, click on the resource link above. Page 4

Chapter 3: Molecules, Compounds, and Nomenclature

Available Study Resources on Quizplus for this Chatper

178 Verified Questions

178 Flashcards

Source URL: https://quizplus.com/quiz/49193

Sample Questions

Q1) Identify the formula for barium nitrite.

A)Ba₃N₂

B)BaNO₃

C)BN

D)Ba(NO₂)₂

E)B(NO₂)₃

Answer: D

Q2) Calculate the mass percent composition of lithium in Li₃PO₄.

A)26.75%

B)17.98%

C)30.72%

D)55.27%

E)20.82%

Answer: B

Q3) Calculate the mass percent composition of oxygen in Al₂(SO₄)₃.

Answer: 56.11%

Q4) Give the name for HNO₂.

Answer: nitrous acid

To view all questions and flashcards with answers, click on the resource link above. Page 5

Chapter 4: Chemical Reactions and Stoichiometry

Available Study Resources on Quizplus for this Chatper

230 Verified Questions

230 Flashcards

Source URL: https://quizplus.com/quiz/49194

Sample Questions

Q1) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ H₂O(l) Ca(OH)₂(s)

A 4.50 g sample of CaO is reacted with 4.34 g of H₂O. How many grams of water remain after the reaction is complete?

A)0.00

B)0.00892

C)2.90

D)1.04

E)0.161

Q2) Which one of the following compounds behaves as an acid when dissolved in water?

A)RaO

B)C₄H₁₀

C)HI

D)RbOH

Q3) What is the concentration (M)of CH₃OH in a solution prepared by dissolving 16.8 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

Q4) How many grams of NaOH (MW = 40.0)are there in 250.0 mL of a 0.275 mol L^-1 NaOH solution?

Page 6

To view all questions and flashcards with answers, click on the resource link above.

Chapter 5: Gases

Available Study Resources on Quizplus for this Chatper

154 Verified Questions

154 Flashcards

Source URL: https://quizplus.com/quiz/49195

Sample Questions

Q1) How many moles of an ideal gas are required to produce a pressure of 3.00 bar in a 1.50 L container with a temperature of 25.0 °C?

A)0.146

B)0.0874

C)0.182

D)0.914

E)1.08

Q2) Identify the gas particle that travels the slowest.

A)H₂

B)O₂

C)Ne

D)N₂

E)CO

Q3) Which of the following gas samples would be most likely to behave ideally under the stated conditions?

A)Ne at STP

B)CO at 200 bar and 25 °C

C)SO₂ at 2 bar and 0 K

D)N₂ at 1 bar and -70 °C

E)O₂ at 400 bar and 25 °C

To view all questions and flashcards with answers, click on the resource link above. Page 7

Chapter 6: Thermochemistry

Available Study Resources on Quizplus for this Chatper

156 Verified Questions

156 Flashcards

Source URL: https://quizplus.com/quiz/49196

Sample Questions

Q1) A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, _combustionU = -15.48 kJ g^-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of C_cal?

A)24.34 kJ °C^-1

B)8.009 kJ °C^-1

C)14.18 kJ °C^-1

D)16.67 kJ °C^-1

E)9.170 kJ °C^-1

Q2) Choose the reaction that illustrates _fH° for NaHCO₃.

A)Na(s)+ H₂(g)+ C(s)+ O₂(g) NaHCO₃ (s)

B)Na⁺(aq)+ HCO₃ ^-1 (aq) NaHCO₃ (s)

C)Na⁺(aq)+ H2O (l)+ CO₂ (g) NaHCO₃(s)

D)Na(s)+ 1/2 H₂(g)+ C(s)+ 3/2 O₂(g) NaHCO₃ (s)

E)Na(s)+ 2 H(g)+ C(s)+ 3 O(g) NaHCO₃(s)

Q3) Why are the standard heats of formation for elements in their most stable form assigned a value of 0?

Q4) Give the equation with the elements in MgSO₄ in their standard state as the reactants and MgSO₄ as the product.

To view all questions and flashcards with answers, click on the resource link above. Page 8

Chapter 7: The Quantum-Mechanical Model of the Atom

Available Study Resources on Quizplus for this Chatper

173 Verified Questions

173 Flashcards

Source URL: https://quizplus.com/quiz/49197

Sample Questions

Q1) Identify the colour of a flame test for sodium.

A)violet

B)red

C)white

D)yellow

E)blue

Q2) Define diffraction.

Q3) Identify the colour that has a wavelength of 460 nm.

A)blue

B)green

C)red

D)yellow

Q4) Sketch one of the 3p orbitals below. How are they different from the 2p orbitals?

Q5) Give the value of l for a 3p sublevel.

A)1

B)0

C)-1

D)2

E)-2

To view all questions and flashcards with answers, click on the resource link above. Page 9

Chapter 8: Periodic Properties of the Elements

Available Study Resources on Quizplus for this Chatper

127 Verified Questions

127 Flashcards

Source URL: https://quizplus.com/quiz/49198

Sample Questions

Q1) Identify the element that has a ground-state electronic configuration of [Kr]5s²4d⁵.

A)Tc

B)Mn

C)Nb

D)Ru

Q2) How many unpaired electrons are present in the ground-state Ge atom?

A)0

B)3

C)1

D)2

E)4

Q3) Use the periodic table to predict the most stable oxidation state for the following element: Al

A)+1

B)+2

C)+3

D)-1

E)-2

Q4) Why do successive ionization energies increase?

To view all questions and flashcards with answers, click on the resource link above. Page 10

Chapter 9: Chemical Bonding I: Lewis Theory

Available Study Resources on Quizplus for this Chatper

143 Verified Questions

143 Flashcards

Source URL: https://quizplus.com/quiz/49199

Sample Questions

Q1) Choose the bond below that is least polar.

A)P-F

B)C-Br

C)C-F

D)C-I

E)C-Cl

Q2) Identify the compound with the lowest magnitude of lattice energy.

A)KCl

B)KBr

C)SrO

D)CaO

Q3) Using periodic trends, place the following bonds in order of increasing ionic character. S-F Se-F O-F

A)Se-F < S-F < O-F

B)S-F < Se-F < O-F

C)O-F < Se-F < S-F

D)Se-F < O-F < S-F

E)O-F < S-F < Se-F

Q4) List the least electronegative atom.

Q5) Describe a covalent bond.

To view all questions and flashcards with answers, click on the resource link above.

Chapter 10: Chemical Bonding Ii: Molecular Shapes,

Valence Bond Theory, and Molecular Orbital Theory

Available Study Resources on Quizplus for this Chatper

168 Verified Questions

168 Flashcards

Source URL: https://quizplus.com/quiz/49200

Sample Questions

Q1) Determine the electron geometry for the molecule CS₂.

A)Linear

B)Trigonal planar

C)Tetrahedral

D)Trigonal bipyramidal

E)Octahedral

Q2) Give the approximate bond angle for a molecule with T-shape molecular geometry.

A)<90°

B)90°

C)>90°

D)<120°

E)120°

Q3) Determine the electron geometry (eg)and molecular geometry (mg)of ICl₂ .

A)eg = tetrahedral, mg = bent

B)eg = tetrahedral, mg = trigonal pyramidal

C)eg = trigonal bipyramidal, mg = linear

D)eg = trigonal bipyramidal, mg = trigonal planar

E)eg = octahedral, mg = linear

Q4) Explain why oil and water do not mix.

To view all questions and flashcards with answers, click on the resource link above. Page 12

Chapter 11: Liquids, Solids, and Intermolecular Forces

Available Study Resources on Quizplus for this Chatper

132 Verified Questions

132 Flashcards

Source URL: https://quizplus.com/quiz/49201

Sample Questions

Q1) How much energy is required to vaporize 158 g of butane (C₄H₁₀)at its boiling point if its _vapH is 24.3 kJ mol^-1?

A)15.1 kJ

B)66.1 kJ

C)89.4 kJ

D)11.2 kJ

E)38.4 kJ

Q2) Place the following compounds in order of increasing strength of intermolecular forces. CO₂ F₂ NH₂CH₃

A)NH₂CH₃ < CO₂ < F₂

B)F₂ < NH₂CH₃ < CO₂

C)NH₂CH₃ < F₂< CO₂

D)F₂ < CO₂ < NH₂CH₃

E)CO₂ < NH₂CH₃ < F₂

Q3) Which is expected to have the largest dispersion forces?

A)C₃H₈

B)C₁₂H₂₆

C)F₂

D)BeCl₂

To view all questions and flashcards with answers, click on the resource link above. Page 13

Chapter 12: Solutions

Available Study Resources on Quizplus for this Chatper

159 Verified Questions

159 Flashcards

Source URL: https://quizplus.com/quiz/49202

Sample Questions

Q1) Twice as much pentane (C₅H₁₂)is mixed with hexane (C₆H₁₄)by mass. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

A)386 Torr

B)300 Torr

C)311 Torr

D)253 Torr

E)344 Torr

Q2) Solutions having osmotic pressures less than those of body fluids are called

A)isosmotic

B)hyperosmotic

C)hyposmotic

D)neosmotic

E)magnosmotic

Q3) Explain why water does not dissolve in gasoline.

Q4) What happens to a supersaturated solution of potassium acetate once it is cooled and a small crystal of solid potassium acetate is added?

To view all questions and flashcards with answers, click on the resource link above. Page 14

Chapter 13: Chemical Kinetics

Available Study Resources on Quizplus for this Chatper

162 Verified Questions

162 Flashcards

Source URL: https://quizplus.com/quiz/49203

Sample Questions

Q1) The rate constant, k, for a first-order reaction is equal to 4.2 × 10^-4 s^-1. What is the half-life for the reaction?

A)2.9 × 10^-4 s

B)1.2 × 10³s

C)1.7 × 10³ s

D)2.4 × 10³ s

Q2) What are the units of k in a first-order reaction?

A)mol L^-1 s^-1

B)mol L^-1 s

C)L mol^-1s^-1

D)M² s^-1

E)s^-1

Q3) What are the units of k in the following rate law? Rate = k[X][Y]^1/2

A)mol L^-1 s^-1

B)L mol^-1s^-1

C)Lmol^-1/2s^-1

D)L^1/2mol^-1/2s^-1

E)L mol^-1s^-1/2

Q4) Explain what the exponential factor in the Arrhenius equation represents.

Q5) Define half-life.

To view all questions and flashcards with answers, click on the resource link above. Page 15

Chapter 14: Chemical Equilibrium

Available Study Resources on Quizplus for this Chatper

123 Verified Questions

123 Flashcards

Source URL: https://quizplus.com/quiz/49204

Sample Questions

Q1) The equilibrium constant, K_p, equals 3.40 for the isomerization reaction: cis-2-butene trans-2-butene

If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene, what is the equilibrium pressure of each gas?

A)P(cis-2-butene)= 0.0485 bar and P(trans-2-butene)= 0.165 bar

B)P(cis-2-butene)= 0.0458 bar and P(trans-2-butene)= 0.156 bar

C)P(cis-2-butene)= 0.0735 bar and P(trans-2-butene)= 0.250 bar

D)P(cis-2-butene)= 0.0943 bar and P(trans-2-butene)= 0.321 bar

Q2) Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl)_eq = 0.22 atm, P(NO)_eq = 0.10 atm, P(Cl₂)_eq = 0.081 atm. 2NOCl(g) 2NO(g)+ Cl₂(g)

A)3.7 × 10^-2atm

B)60 atm

C)27 atm

D)1.7 × 10^-2atm

E)1.8 × 10^-3atm

Q3) Can the K_p and K_c for a reaction ever have the same value? Why or why not?

To view all questions and flashcards with answers, click on the resource link above.

Page 16

Chapter 15: Acids and Bases

Available Study Resources on Quizplus for this Chatper

148 Verified Questions

148 Flashcards

Source URL: https://quizplus.com/quiz/49205

Sample Questions

Q1) Determine the pOH in a 0.235 mol L^-1 NaOH solution.

A)13.76

B)0.24

C)13.37

D)0.63

E)12

Q2) Identify the strongest acid.

A)H₂O

B)H₂S

C)H₂Se

D)H₂Te

E)CaH₂

Q3) Calculate the concentration of bicarbonate ion, HCO₃^-, in a 0.010 mol L^-1 H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

A)6.6 × 10^-5 mol L^-1

B)4.3 × 10^-7 mol L^-1

C)4.3 × 10^-9 mol L^-1

D)5.6 × 10^-11 mol L^-1

To view all questions and flashcards with answers, click on the resource link above. Page 17

Chapter 16: Aqueous Ionic Equilibrium

Available Study Resources on Quizplus for this Chatper

161 Verified Questions

161 Flashcards

Source URL: https://quizplus.com/quiz/49206

Sample Questions

Q1) Determine the molar solubility of CaSO₄ in a solution containing 0.100 mol L^-1 Na₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

A)4.9 × 10^-3 mol L^-1

B)2.4 × 10^-4 mol L^-1

C)5.8 × 10^-10mol L^-1

D)1.2 × 10^-5 mol L^-1

E)0.10 mol L^-1

Q2) Determine the molar solubility of BaF₂in pure water. K_sp for BaF₂ = 2.45 × 10^-5.

A)1.83 × 10^-2 mol L^-1

B)1.23 × 10^-5 mol L^-1

C)2.90 × 10^-2 mol L^-1

D)4.95 × 10^-3 mol L^-1

E)6.13 × 10^-6 mol L^-1

Q3) Identify the compound that forms stalactites and stalagmites.

Q4) Define a buffer.

Q5) Explain the common ion effect with respect to molar solubility.

Q6) Give the name of the compound that is in antifreeze and is toxic to pets.

Page 18

To view all questions and flashcards with answers, click on the resource link above.

Chapter 17: Gibbs Energy and Thermodynamics

Available Study Resources on Quizplus for this Chatper

111 Verified Questions

111 Flashcards

Source URL: https://quizplus.com/quiz/49207

Sample Questions

Q1) Consider a reaction that has a negative _rH and a negative _rS. Which of the following statements is TRUE?

A)This reaction will be spontaneous only at low temperatures.

B)This reaction will be spontaneous at all temperatures.

C)This reaction will be nonspontaneous at all temperatures.

D)This reaction will be nonspontaneous only at low temperatures.

E)This reaction will be spontaneous only at absolute zero (0 Kelvin).

Q2) Calculate _rS° for the following reaction. The S° for each species is shown below the reaction. 4NH₃(g)+ 5O₂(g) 4NO(g)+ 6H₂O(g)

S°(J K^-1 mol^-1)192.8 205.2 210.8 188.8

A)+287.4 J K^-1 mol^-1

B)-401.2 J K^-1 mol^-1

C)+160.0 J K^-1 mol^-1

D)-336.6 J K^-1 mol^-1

E)+178.8 J K^-1 mol^-1

Q3) Give the standard states for a gas, liquid, solid, and solution.

Q4) Why can endothermic reactions be spontaneous?

Q5) Why is heating your home with gas more efficient than heating it with electricity?

To view all questions and flashcards with answers, click on the resource link above. Page 19

Chapter 18: Electrochemistry

Available Study Resources on Quizplus for this Chatper

126 Verified Questions

126 Flashcards

Source URL: https://quizplus.com/quiz/49208

Sample Questions

Q1) Which of the following is the strongest reducing agent?

A)Al(s)

B)Zn(s)

C)Mg(s)

D)Al³⁺(aq)

E)Mg²⁺(aq)

Q2) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) 2K(s)+ I₂(s) 2K (aq)+ 2I (aq)

K⁺(aq)+ e K (s) E° = -2.93 V

I₂(s)+ 2 e 2 I (aq) E° = +0.54 V

A)+6.40 V

B)+1.85 V

C)-5.32 V

D)+3.47 V

E)+5.32 V

Q3) Why are iron nails coated with zinc?

Q4) Explain the significance of the standard hydrogen electrode (SHE)in the tabulation of standard reduction potentials of other species.

To view all questions and flashcards with answers, click on the resource link above. Page 20

Chapter 19: Radioactivity and Nuclear Chemistry

Available Study Resources on Quizplus for this Chatper

115 Verified Questions

115 Flashcards

Source URL: https://quizplus.com/quiz/49209

Sample Questions

Q1) Describe what changes occur in the atomic nucleus during alpha decay.

A)The mass number and atomic number decrease.

B)The mass number and atomic number increase.

C)The mass number is unchanged and the atomic number decreases.

D)The mass number is unchanged and the atomic number increases.

E)The mass number and atomic number do not change.

Q2) Nuclides below the valley of stability can become more stable through which of the following processes?

A)gamma emission

B)beta emission

C)positron emission

D)neutron emission

E)neutron bombardment

Q3) Find a correct technique used in radiometric dating.

A)uranium-238 to bismuth-206

B)potassium-40 to argon-40

C)carbon-14 to nitrogen-11

D)lead-206 to uranium-238

E)calcium-41 to argon-42

Q4) How does a dosimeter measure exposure to radioactivity?

Page 21

To view all questions and flashcards with answers, click on the resource link above.

Chapter 20: Organic Chemistry I: Structures

Available Study Resources on Quizplus for this Chatper

109 Verified Questions

109 Flashcards

Source URL: https://quizplus.com/quiz/49210

Sample Questions

Q1) Explain the concept of bond polarization and inductive effect using organic halides as an example.

Q2) Which of the following is TRUE regarding index of hydrogen deficiency (IHD)?

A)When calculating IHD, oxygen does not change the number of H atoms in the parent formula, halogens are considered equal to hydrogen, and nitrogen requires one additional hydrogen atom in the parent formula.

B)When calculating IHD, oxygen requires one additional hydrogen atom in the parent formula, halogens are considered equal to hydrogen, and nitrogen does not change the number of H atoms in the parent formula.

C)When calculating IHD, oxygen is treated like hydrogen, halogens require one additional hydrogen atom in the parent formula, and nitrogen does not change the number of H atoms in the parent formula.

D)When calculating IHD, oxygen does not change the number of H atoms in the parent formula, halogens are considered equal to hydrogen, and nitrogen requires two additional hydrogen atoms in the parent formula.

E)When calculating IHD, oxygen and halogens do not change the number of H atoms in the parent formula, and nitrogen requires two additional hydrogen atoms in the parent formula.

To view all questions and flashcards with answers, click on the resource link above. Page 22

Chapter 21: Organic Chemistry II: Reactions

Available Study Resources on Quizplus for this Chatper

96 Verified Questions

96 Flashcards

Source URL: https://quizplus.com/quiz/49211

Sample Questions

Q1) Which part of HCN, the hydrogen or the cyano group, adds to the O in a C=O bond and why?

Q2) Write a balanced chemical reaction to represent the combustion of 2,2-dimethylpropane.

A)C₅H₁₂ + 8O₂ 5CO₂ + 6H₂O

B)C₃H₈ + 5O₂ 3CO₂ + 4H₂O

C)C₅H₁₂ + H₂ CH₄ + 2C₂H₆

D)C₃H₈ + H₂ CH₄ + C₂H₆

E)2 C₃H₈ + O₂ 3CH₄ + 2H₂O

Q3) What are primary alcohols oxidized to?

A)secondary alcohols

B)ethers

C)esters

D)aldehydes

E)ketones

To view all questions and flashcards with answers, click on the resource link above. Page 23

Chapter 22: Biochemistry

Available Study Resources on Quizplus for this Chatper

55 Verified Questions

55 Flashcards

Source URL: https://quizplus.com/quiz/49212

Sample Questions

Q1) Which of the following statements is TRUE?

A)Monosaccharides are the building blocks of polypeptides.

B)Nucleotides are the building blocks of saccharides.

C)Fatty acids are responsible for DNA replication.

D)Peptides are the building blocks of amino acids.

E)Carbohydrates are water soluble and responsible for short-term energy storage.

Q2) Which of the following link together into amino acid units?

A)glycosidic linkages

B)disulfide linkages

C)peptide bonds

D)hydrogen bonds

E)ester linkages

Q3) Which of the following shows all of the tripeptides that can be formed from one molecule each of alanine (Ala), methionine (Met), and proline (Pro)?

A)AlaMetPro

B)AlaMetPro and AlaProMet

C)AlaMetPro, AlaProMet, ProMetAla, ProAlaMet, MetProAla, MetAlaPro

D)AlaMetPro, AlaProMet, ProAlaMet

E)AlaMetPro, AlaProMet, ProAlaMet, MetProAla

Q4) How do cis- and trans-fats differ?

To view all questions and flashcards with answers, click on the resource link above. Page 24

Chapter 23: Chemistry of the Nonmetals

Available Study Resources on Quizplus for this Chatper

50 Verified Questions

50 Flashcards

Source URL: https://quizplus.com/quiz/49213

Sample Questions

Q1) Write the balanced reaction that shows the formation of ICl₃ from its elements.

Q2) Which of the following statements is TRUE?

A)Ionic carbides form between carbon and another highly electronegative element.

B)Carbides are soft materials with low melting points.

C)Metallic carbides are more malleable than the pure metal.

D)Covalent carbides are formed between carbon and a nonmetal with low electronegativity.

E)Carbides can be cationic, anionic, and covalent.

Q3) pyrosilicate

A)Si₂O₅^2-

B)SiO₄^4-

C)Si₄O₁₁^6-

D)SiO₃^2-

E)Si₂O₇^6-

Q4) Why are the chemical properties of nitrogen and phosphorus so different when they are in the same family?

Q5) Draw the Lewis structure for IF₄ and determine the geometry of the ion.

Q6) Describe the major production method for obtaining oxygen.

Page 25

To view all questions and flashcards with answers, click on the resource link above.

Chapter 24: Metals and Metallury

Available Study Resources on Quizplus for this Chatper

49 Verified Questions

49 Flashcards

Source URL: https://quizplus.com/quiz/49214

Sample Questions

Q1) Which of the following is TRUE concerning substitutional alloys?

A)The metals involved must have similar radii.

B)One type of metal atom is inserted in between the metal atoms in the initial crystal structure of the other metal.

C)The two metals must be miscible over the entire composition range.

D)Titanium carbide is an example of a substitutional alloy.

E)The metals forming a substitutional alloy must have very different electronegativities.

Q2) Which of the following is a general property of a metal?

A)high resistivity

B)good conductor of heat

C)low boiling point

D)low melting point

E)high electronegativity

Q3) What are the components of bronze?

A)copper and tin

B)lead and aluminum

C)nickel and zinc

D)copper and zinc

E)zinc and lead

To view all questions and flashcards with answers, click on the resource link above. Page 26

Chapter 25: Transition Metals and Coordination Compounds

Available Study Resources on Quizplus for this Chatper

55 Verified Questions

55 Flashcards

Source URL: https://quizplus.com/quiz/49215

Sample Questions

Q1) What is the ground-state electron configuration for Cr³⁺ (Z = 24)?

A)[Ar] 4s²3d⁷

B)[Ar] 4s²3d¹

C)[Ar] 3d³

D)[Ar] 4s¹3d²

Q2) coordination

A)[Zn(NH₃)₂Cl₂]Br_{2 and}[Zn(NH₃)₂Br₂]Cl₂

B)[Cr(en)₃]³⁺

C)[Ni(CN)₂(OH)₂]^2-

D)[Cu(SCN)₄]^3-and[Cu(NCS)₄]^3-

E)[Cr(NH₃)₃(CO)₃]³⁺

Q3) Which of the following can function as a bidentate ligand?

A)CN^-

B)SH^-

C)HO

D)H₂NCH₂

Q4) What is the difference between a weak-field complex and a strong-field complex?

Q5) Explain how EDTA is used to treat lead poisoning.

To view all questions and flashcards with answers, click on the resource link above. Page 27