CHM 1030 General Chemistry I

Unit I Assessment

• Question 1

5 out of 5 points

	Gases and liquids share the property of __________.
	Selected Answer:  indefinite shape Correct Answer: indefinite shape

• Question 2

5 out of 5 points

	Homogeneous mixtures are also known as __________.
	Selected Answer:  solutions Correct Answer: solutions

• Question 3

5 out of 5 points

	Which one of the following is NOT an intensive property?
	Selected Answer:  Mass Correct Answer: Mass

• Question 4

5 out of 5 points

	Identify which of the following are chemical processes: (i) reaction of copper with nitric acid (ii) freezing of water (iii) decomposition of water into hydrogen and oxygen gases (iv) compression of oxygen gas into liquid oxygen
	Selected Answer:  i, iii  Correct Answer: i, iii

• Question 5

5 out of 5 points

	A small amount of salt dissolved in water is an example of a __________.
	Selected Answer:  homogeneous mixture Correct Answer: homogeneous mixture

• Question 6

5 out of 5 points

	Of the following, only __________ is an extensive property.
	Selected Answer:  mass Correct Answer: mass

• Question 7

5 out of 5 points

	For which of the following can the composition vary?
	Selected Answer:  Both homogeneous and heterogeneous mixtures Correct Answer: Both homogeneous and heterogeneous mixtures

• Question 8

5 out of 5 points

	Which of the following equations clearly shows a conversion between temperature in degrees Celsius, t(°C), and temperature in Kelvins, T(K)?
	Selected Answer:  T(K) = t(°C) + 273.15 Correct Answer: T(K) = t(°C) + 273.15

• Question 9

5 out of 5 points

	Which one of the following is a pure substance?
	Selected Answer:  Water Correct Answer: Water

• Question 10

5 out of 5 points

	In the following list, only __________ is (are) NOT an example of matter.
	Selected Answer:  light Correct Answer: light

• Question 11

5 out of 5 points

	Which one of the following is the highest temperature?
	Selected Answer:  220°F Correct Answer: 220°F

• Question 12

5 out of 5 points

	A wooden object has a mass of 10.782 g and occupies a volume of 13.72 mL. What is the density of the object, determined to an appropriate number of significant figures?
	Selected Answer:  7.859 × 10-1 g/mL  Correct Answer: 7.859 × 10-1 g/mL

• Question 13

5 out of 5 points

	One angstrom, symbolized Å, is 10 to power of ((-10)) m. 1 cm to power of ((3)) = __________ Å to power of ((3)).
	Selected Answer:  10 to power of ((24)) Correct Answer: 10 to power of ((24))

• Question 14

5 out of 5 points

	Accuracy refers to __________.
	Selected Answer:  how close a measured number is to the true value Correct Answer: how close a measured number is to the true value

• Question 15

5 out of 5 points

	Which one of the following is TRUE about the liter?
	Selected Answer:  It is equivalent to a cubic decimeter.  Correct Answer: It is equivalent to a cubic decimeter.

• Question 16

5 out of 5 points

	The law of constant composition says that __________.
	Selected Answer:  the composition of a compound is always the same Correct Answer: the composition of a compound is always the same

• Question 17

5 out of 5 points

	The law of constant composition (also called the law of definite proportions) applies to __________.
	Selected Answer:  compounds Correct Answer: compounds

• Question 18

5 out of 5 points

	Which of the following liquids has the greatest density?
	Selected Answer:  0.022 cm3 with a mass of 0.10 g  Correct Answer: 0.022 cm3 with a mass of 0.10 g

• Question 19

5 out of 5 points

	Which state(s) of matter are significantly compressible?
	Selected Answer:  Gases only Correct Answer: Gases only

• Question 20

5 out of 5 points

	How many significant figures are in the number 0.0034050?
	Selected Answer:  5 Correct Answer: 5

Unit II Assessment

• Question 1

5 out of 5 points

	There are __________ electrons, __________ protons, and __________ neutrons in an atom of the element below.
	Selected Answer:  54, 54, 78 Correct Answer: 54, 54, 78

• Question 2

5 out of 5 points

	Which of the following atoms has the smallest number of neutrons?
	Selected Answer:  Nitrogen-14 Correct Answer: Nitrogen-14

• Question 3

5 out of 5 points

	Elements in the same group of the periodic table typically have similar __________.
	Selected Answer:  physical and chemical properties Correct Answer: physical and chemical properties

• Question 4

5 out of 5 points

	Which isotope has 45 neutrons?
	Selected Answer:  Correct Answer:

• Question 5

5 out of 5 points

	Isotopes are atoms that have the same number of __________ but a different number of __________.
	Selected Answer:  Protons; neutrons Correct Answer: Protons; neutrons

• Question 6

5 out of 5 points

	What is the molecular formula for 1-propanol?
	Selected Answer:  C3H7OH  Correct Answer: C3H7OH

• Question 7

5 out of 5 points

	All atoms of a given element have the same __________.
	Selected Answer:  number of protons Correct Answer: number of protons

• Question 8

5 out of 5 points

	The gold foil experiment performed in Rutherford's lab __________.
	Selected Answer:  led to the discovery of the atomic nucleus Correct Answer: led to the discovery of the atomic nucleus

• Question 9

5 out of 5 points

	Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?
	Selected Answer:  Ca, Sr Correct Answer: Ca, Sr

• Question 10

5 out of 5 points

	In the symbol below, X represents __________.
	Selected Answer:  C Correct Answer: C

• Question 11

5 out of 5 points

	Which statement below correctly describes how alpha, beta, and gamma radiation are affected by an electric field?
	Selected Answer: Alpha and beta are deflected in opposite directions, while gamma shows no response. Correct Answer: Alpha and beta are deflected in opposite directions, while gamma shows no response.

• Question 12

5 out of 5 points

	A molecular formula always indicates __________.
	Selected Answer:  how many of each atom are in a molecule Correct Answer: how many of each atom are in a molecule

• Question 13

5 out of 5 points

	The charge on an electron was determined __________.
	Selected Answer:  during the Millikan oil drop experiment Correct Answer: during the Millikan oil drop experiment

• Question 14

5 out of 5 points

	Barium reacts with a polyatomic ion to form a compound with the general formula Ba3(X)2. What would be the most likely formula for the compound formed between sodium and the polyatomic ion   X?
	Selected Answer:  Na3X  Correct Answer: Na3X

• Question 15

0 out of 5 points

	The element X, in the table below, has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu.
	Selected Answer:  219.7 Correct Answer: 220.4

• Question 16

5 out of 5 points

	Of the following, the smallest and lightest subatomic particle is the __________.
	Selected Answer:  electron Correct Answer: electron

• Question 17

5 out of 5 points

	Cathode rays are __________.
	Selected Answer:  electrons Correct Answer: electrons

• Question 18

5 out of 5 points

	Which one of the following molecular formulas is also an empirical formula?
	Selected Answer:  H2O  Correct Answer: H2O

• Question 19

5 out of 5 points

	There are __________ protons, __________ neutrons, and __________ electrons in 238U+5.
	Selected Answer:  92, 146, and 87  Correct Answer: 92, 146, and 87

• Question 20

5 out of 5 points

	Which one of the following compounds is chromium (III) oxide?
	Selected Answer:  Cr2O3  Correct Answer: Cr2O3

Unit III Assessment

• Question 1

5 out of 5 points

	The formula weight of magnesium fluoride (MgF2), rounded to one decimal place, is __________ amu.
	Selected Answer:  62.3  Correct Answer: 62.3

• Question 2

5 out of 5 points

	How many carbon atoms are there in 52.06 g of carbon dioxide?
	Selected Answer:  7.122 × 1023  Correct Answer: 7.122 × 1023

• Question 3

5 out of 5 points

	Which one of the following substances is the product of the combination reaction Al (s) + I2 (s) → __________?
	Selected Answer:  AlI3  Correct Answer: AlI3

• Question 4

5 out of 5 points

	The mass % of H in methane (CH4) is __________.
	Selected Answer:  25.13  Correct Answer: 25.13

• Question 5

5 out of 5 points

	The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2. The mass of 1.00 mol of allicin, rounded to the nearest integer, is __________ g.
	Selected Answer:  162  Correct Answer: 162

• Question 6

5 out of 5 points

	One mole of __________ contains the smallest number of atoms.
	Selected Answer:  NaCl  Correct Answer: NaCl

• Question 7

5 out of 5 points

	A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O.
	Selected Answer:  6.02 × 1023  Correct Answer: 6.02 × 1023

• Question 8

5 out of 5 points

	The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is __________ amu.
	Selected Answer:  123.11  Correct Answer: 123.11

• Question 9

5 out of 5 points

	Which of the following are combustion reactions? (i) CH4(g) + O2(g) → CO2(g) + H2O(l) (ii) CaO(s) + CO2(g) → CaCO3(s) (iii) PbCO3(s) → PbO(s) + CO2(g) (iv) CH3OH(l) + O2(g) → CO2(g) + H2O(l)
	Selected Answer:  i and iv  Correct Answer: i and iv

• Question 10

5 out of 5 points

	The mass % of Al in aluminum sulfate (Al2(SO4)3) is __________.
	Selected Answer:  15.77  Correct Answer: 15.77

• Question 11

5 out of 5 points

	What is the mass in grams of 9.76 × 1012 atoms of naturally occurring sodium?
	Selected Answer:  3.73 × 10-10  Correct Answer: 3.73 × 10-10

• Question 12

5 out of 5 points

	When the equation CH4 + O2 → CO2 + H2O is balanced, what are the coefficients?
	Selected Answer:  1, 2, 1, 2  Correct Answer: 1, 2, 1, 2

• Question 13

5 out of 5 points

	Of the reactions below, which one is a decomposition reaction?
	Selected Answer:  NH4Cl → NH3 + HCl  Correct Answer: NH4Cl → NH3 + HCl

• Question 14

5 out of 5 points

	One mole of __________ contains the largest number of atoms.
	Selected Answer:  C10H8  Correct Answer: C10H8

• Question 15

5 out of 5 points

	Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of 5.0 grams of O2 with 6.0 grams of S. What is the % yield of SO3 in this experiment?            S (s) + O2 (g) → SO3 (g) (not balanced)
	Selected Answer:  95  Correct Answer: 95

• Question 16

5 out of 5 points

	Propane (C3H8) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of 22.05 grams of propane with excess oxygen. What is the % yield in this reaction?
	Selected Answer:  57.6  Correct Answer: 57.6

• Question 17

5 out of 5 points

	How many moles of pyridine (C5H5N) are contained in 3.13 g of pyridine?
	Selected Answer:  0.0396  Correct Answer: 0.0396

• Question 18

5 out of 5 points

	A sample of CH2F2 with a mass of 19 g contains __________ atoms of F.
	Selected Answer:  4.4 × 1023  Correct Answer: 4.4 × 1023

• Question 19

5 out of 5 points

	A 30.5 gram sample of glucose (C6H12O6) contains __________ moles of glucose.
	Selected Answer:  0.169  Correct Answer: 0.169

• Question 20

5 out of 5 points

	The molecular weight of the ethanol (C2H5OH), rounded to the nearest integer, is __________ amu.
	Selected Answer:  46  Correct Answer: 46

Unit IV Assessment

• Question 1

5 out of 5 points

	A __________ ΔH corresponds to an __________ process.
	Selected Answer:  negative; exothermic  Correct Answer: negative; exothermic

• Question 2

5 out of 5 points

	The units of specific heat capacity are __________.
	Selected Answer:  J/g-K or J/g-°C Correct Answer: J/g-K or J/g-°C

• Question 3

5 out of 5 points

	A sample of calcium carbonate [CaCO3 (s)] absorbs 45.5 J of heat, at which time the temperature of the sample increases from 21.1°C to 28.5°C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams) of the sample?
	Selected Answer:  7.5  Correct Answer: 7.5

• Question 4

5 out of 5 points

	The value of ΔE for a system that performs 13 kJ of work on its surroundings and loses 9 kJ of heat is __________ kJ.
	Selected Answer:  -22  Correct Answer: -22

• Question 5

5 out of 5 points

	For which one of the following reactions is the value of ΔH°rxn equal to ΔHf° for the product?
	Selected Answer:  2 C (s, graphite) + 2 H2 (g) → C2H4 (g)  Correct Answer: 2 C (s, graphite) + 2 H2 (g) → C2H4 (g)

• Question 6

5 out of 5 points

	The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydroiodic acid is __________.
	Selected Answer:  NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq)  Correct Answer: NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq)

• Question 7

5 out of 5 points

	Which one of the following is a diprotic acid?
	Selected Answer:  Sulfuric acid Correct Answer: Sulfuric acid

• Question 8

5 out of 5 points

	What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to 350. mL to make a 2.75 M solution of magnesium chloride?
	Selected Answer:  107 Correct Answer: 107

• Question 9

5 out of 5 points

	An ammonium ion will form an insoluble salt with __________.
	Selected Answer:  None of the above Correct Answer: None of the above

• Question 10

0 out of 5 points

	The internal energy of a system is always increased by __________.
	Selected Answer:  having the system do work on the surroundings Correct Answer: adding heat to the system

• Question 11

5 out of 5 points

	Which of the following is insoluble in water at 25°C?
	Selected Answer:  Mg3(PO4)2  Correct Answer: Mg3(PO4)2

• Question 12

5 out of 5 points

	Of the species below, only __________ is NOT an electrolyte.
	Selected Answer:  C12H22O11(aq)      Correct Answer: C12H22O11(aq)

• Question 13

5 out of 5 points

	ΔH for an endothermic process is __________ while ΔH for an exothermic process is __________.
	Selected Answer:  positive; negative  Correct Answer: positive; negative

• Question 14

5 out of 5 points

	For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product?
	Selected Answer:  (1/2) N2 (g) + O2 (g) → NO2 (g) Correct Answer: (1/2) N2 (g) + O2 (g) → NO2 (g)

• Question 15

5 out of 5 points

	Which one of the following is a weak acid?
	Selected Answer:  HF  Correct Answer: HF

• Question 16

5 out of 5 points

	Which of the following combinations will produce a precipitate?
	Selected Answer:  KOH (aq) and Mg(NO3)2 (aq)  Correct Answer: KOH (aq) and Mg(NO3)2 (aq)

• Question 17

5 out of 5 points

	Which of the following is a correct expression for molarity?
	Selected Answer:  mol solute/L solution Correct Answer: mol solute/L solution

• Question 18

5 out of 5 points

	The neutralization reaction between aqueous potassium hydroxide and aqueous acetic acid would be written as which of the following?
	Selected Answer:  KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 ( aq)  Correct Answer: KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 ( aq)

• Question 19

5 out of 5 points

	Consider the following two reactions: A → 2B ΔH°rxn = 456.7 kJ/mol A → C ΔH°rxn = -22.1kJ/mol Determine the enthalpy change for the process: 2B → C
	Selected Answer:  -478.8 kJ/mol Correct Answer: -478.8 kJ/mol

• Question 20

5 out of 5 points

	Which one of the following is not a monoprotic acid?
	Selected Answer:  Sulfuric acid Correct Answer: Sulfuric acid

Unit V Assessment

• Question 1

5 out of 5 points

	Atomic radius generally increases as we move __________.
	Selected Answer:  down a group and from right to left across a period Correct Answer: down a group and from right to left across a period

• Question 2

5 out of 5 points

	Which one of the following atoms has the largest radius?
	Selected Answer:  Te Correct Answer: Te

• Question 3

5 out of 5 points

	The ground state configuration of fluorine is __________.
	Selected Answer:  [He]2s22p5  Correct Answer: [He]2s22p5

• Question 4

5 out of 5 points

	The wavelength of light emitted from a traffic light having a frequency of 5.75 × 1014 Hz is __________.
	Selected Answer:  522 nm  Correct Answer: 522 nm

• Question 5

5 out of 5 points

	Of the elements below, __________ is the least metallic.
	Selected Answer:  Ar Correct Answer: Ar

• Question 6

5 out of 5 points

	The photoelectric effect is __________.
	Selected Answer:  the emission of electrons by a metal when struck with light of sufficient energy Correct Answer: the emission of electrons by a metal when struck with light of sufficient energy

• Question 7

5 out of 5 points

	Which equation correctly represents the first ionization of sodium?
	Selected Answer:  Na(g) → Na+(g) + e-  Correct Answer: Na(g) → Na+(g) + e-

• Question 8

5 out of 5 points

	According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the __________ of an electron.
	Selected Answer:  momentum Correct Answer: momentum

• Question 9

5 out of 5 points

	Which equation correctly represents the electron affinity of calcium?
	Selected Answer:  Ca(g)+ e- → Ca-(g)  Correct Answer: Ca(g)+ e- → Ca-(g)

• Question 10

5 out of 5 points

	Of the choices below, which correctly orders the successive values for first ionization energies in a range from largest to smallest?
	Selected Answer:  Ar > Cl > S > Si > Al Correct Answer: Ar > Cl > S > Si > Al

• Question 11

5 out of 5 points

	The ground state configuration of tungsten is __________.
	Selected Answer:  [Xe]6s24f145d4      Correct Answer: [Xe]6s24f145d4

• Question 12

5 out of 5 points

	The element that has a condensed electron configuration of [Ar]4s1 is __________.
	Selected Answer:  K  Correct Answer: K

• Question 13

5 out of 5 points

	The ground state electron configuration of Fe is __________.
	Selected Answer:  1s22s22p63s23p64s23d6      Correct Answer: 1s22s22p63s23p64s23d6

• Question 14

5 out of 5 points

	Which one of the following is NOT a valid value for the magnetic quantum number of an electron in a 4d subshell?
	Selected Answer:  3 Correct Answer: 3

• Question 15

5 out of 5 points

	Which of the following electron configurations represents a violation of the Pauli Exclusion Principle?
	Selected Answer:  Correct Answer:

• Question 16

5 out of 5 points

	Of the elements below, __________ has the highest melting point.
	Selected Answer:  Li Correct Answer: Li

• Question 17

5 out of 5 points

	Of the following, which gives the correct order to show decreasing atomic radius for Mg, Na, P, Si and Ar?
	Selected Answer:  Na > Mg > Si > P > Ar Correct Answer: Na > Mg > Si > P > Ar

• Question 18

5 out of 5 points

	Which one of the following is the correct mathematical expression for the inverse relationship between the frequency and wavelength of electromagnetic radiation?
	Selected Answer:  νλ = c  Correct Answer: νλ = c

• Question 19

5 out of 5 points

	In which set of elements would all members be expected to have very similar chemical properties?
	Selected Answer:  Ar, Ne, Kr Correct Answer: Ar, Ne, Kr

• Question 20

5 out of 5 points

	Which one of the following configurations depicts an excited oxygen atom?
	Selected Answer:  1s22s22p23s2      Correct Answer: 1s22s22p23s2

Unit VI Assessment

• Question 1

5 out of 5 points

	In the nitrate ion (NO3- ), __________.
	Selected Answer:  all bonds lengths are the same  Correct Answer: all bonds lengths are the same

• Question 2

5 out of 5 points

	Using the Born-Haber cycle, the ΔHf° of KBr is equal to __________.
	Selected Answer:  ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K) + E(Br) - ΔHlattice  Correct Answer: ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K) + E(Br) - ΔHlattice

• Question 3

5 out of 5 points

	The central atom in __________ obeys the octet rule.
	Selected Answer:  PCl3  Correct Answer: PCl3

• Question 4

5 out of 5 points

	A valid Lewis structure of __________ cannot be drawn without the central atom violating the octet rule.
	Selected Answer:  SF4  Correct Answer: SF4

• Question 5

5 out of 5 points

	Lattice energy is __________.
	Selected Answer: the energy required to convert a mole of ionic solid into its constituent ions in the gas phase Correct Answer: the energy required to convert a mole of ionic solid into its constituent ions in the gas phase

• Question 6

5 out of 5 points

	A valid Lewis structure of __________ cannot be drawn without the central atom violating the octet rule.
	Selected Answer:  PF5  Correct Answer: PF5

• Question 7

5 out of 5 points

	Of the molecules below, the bond in __________ is the most polar.
	Selected Answer:  HF  Correct Answer: HF

• Question 8

5 out of 5 points

	Of the bonds C-N, C=N, and C≡N, the C-N bond is __________.
	Selected Answer:  weakest/longest  Correct Answer: weakest/longest

• Question 9

5 out of 5 points

	Of the ions below, ONLY __________ has a noble gas electron configuration.
	Selected Answer:  Cl-  Correct Answer: Cl-

• Question 10

5 out of 5 points

	There are __________ valence electrons in the Lewis structure of PCl3.
	Selected Answer:  26  Correct Answer: 26

• Question 11

5 out of 5 points

	Resonance structures differ by __________.
	Selected Answer:  placement of electrons only Correct Answer: placement of electrons only

• Question 12

5 out of 5 points

	Of the bonds C-C, C=C, and C≡C, the C-C bond is __________.
	Selected Answer:  weakest/longest  Correct Answer: weakest/longest

• Question 13

5 out of 5 points

	As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________.
	Selected Answer:  decreases, increases Correct Answer: decreases, increases

• Question 14

5 out of 5 points

	Which ion below has a noble gas electron configuration?
	Selected Answer:  Na1+  Correct Answer: Na1+

• Question 15

5 out of 5 points

	In which of the molecules below is the carbon-carbon distance the shortest?
	Selected Answer:  H-C≡C-H Correct Answer: H-C≡C-H

• Question 16

5 out of 5 points

	In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons.
	Selected Answer:  4; 2 Correct Answer: 4; 2

• Question 17

5 out of 5 points

	There are __________ valence electrons in the Lewis structure of HCN.
	Selected Answer:  10 Correct Answer: 10

• Question 18

5 out of 5 points

	Of the atoms below, __________ is the most electronegative.
	Selected Answer:  Cl Correct Answer: Cl

• Question 19

5 out of 5 points

	The central atom's number of valence electrons in __________ makes it an exception to the octet rule.
	Selected Answer:  BF3  Correct Answer: BF3

• Question 20

5 out of 5 points

	Which of the following has the bonds correctly arranged in order of increasing polarity?
	Selected Answer:  O−F, N−F, Be−F, Mg−F  Correct Answer: O−F, N−F, Be−F, Mg−F

Unit VII Assessment

• Question 1

5 out of 5 points

	Of the following species, __________ will have bond angles of 120°.
	Selected Answer:  SO3 Correct Answer: SO3

• Question 2

5 out of 5 points

	The carbon-carbon α bond in ethylene, H2C=CH2, results from the overlap of __________.
	Selected Answer:  sp2 hybrid orbitals  Correct Answer: sp2 hybrid orbitals

• Question 3

5 out of 5 points

	A typical double bond consists of __________.
	Selected Answer:  one sigma and one pi bond Correct Answer: one sigma and one pi bond

• Question 4

5 out of 5 points

	According to valence bond theory, which orbitals overlap in the formation of the bond in HCl?
	Selected Answer:  1s on H and 3p on Cl Correct Answer: 1s on H and 3p on Cl

• Question 5

5 out of 5 points

	The molecular geometry of the left-most (methyl group) carbon atom in the molecule below is __________.
	Selected Answer:  tetrahedral Correct Answer: tetrahedral

• Question 6

5 out of 5 points

	The electron-domain geometry of a carbon-centered compound is tetrahedral. The hybridization of the central carbon atom is __________.
	Selected Answer:  sp3  Correct Answer: sp3

• Question 7

5 out of 5 points

	When four atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed?
	Selected Answer:  Four Correct Answer: Four

• Question 8

0 out of 5 points

	A typical triple bond __________.
	Selected Answer:  consists of three shared electrons Correct Answer: consists of one α bond and two π bonds

• Question 9

5 out of 5 points

	Based on molecular orbital theory, there are __________ unpaired electrons in the B2.
	Selected Answer:  2  Correct Answer: 2

• Question 10

5 out of 5 points

	Based on molecular orbital theory, the only molecule in the list below that has unpaired electrons is __________.
	Selected Answer:  O2  Correct Answer: O2

• Question 11

5 out of 5 points

	The molecular geometry of the right-most (C=O) carbon atom in the molecule below is __________.
	Selected Answer:  trigonal planar Correct Answer: trigonal planar

• Question 12

5 out of 5 points

	Of the molecules below, only __________ is nonpolar.
	Selected Answer:  BF3  Correct Answer: BF3

• Question 13

5 out of 5 points

	The central C atom in the CH4 molecule has __________ unbonded electron pairs and __________ bonded electron pairs in its valence shell.
	Selected Answer:  0; 4  Correct Answer: 0; 4

• Question 14

0 out of 5 points

	Of the following, only __________ has sp2 hybridization of the central atom.
	Selected Answer:  ICl3  Correct Answer: BF3

• Question 15

5 out of 5 points

	The hybridization scheme for BeF2 is __________.
	Selected Answer:  sp  Correct Answer: sp

• Question 16

5 out of 5 points

	Of the molecules below, only __________ is polar.
	Selected Answer:  CH3Cl  Correct Answer: CH3Cl

• Question 17

5 out of 5 points

	The electron-domain geometry of __________ is tetrahedral.
	Selected Answer:  SnCl3-  Correct Answer: SnCl3-

• Question 18

5 out of 5 points

	The molecular geometry of the NF3 is __________.
	Selected Answer:  trigonal pyramidal  Correct Answer: trigonal pyramidal

• Question 19

5 out of 5 points

	Of the molecules below, only __________ is polar.
	Selected Answer:  NH3  Correct Answer: NH3

• Question 20

5 out of 5 points

	ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule.
	Selected Answer:  2  Correct Answer: 2

Unit Assignments

Unit I Problem Solving

Find the answers to the following problems by providing line-by-line (step-by-step) solutions for each applicable question. You must show your work for questions 1-4 to get full credit for each question. Each question is worth 20 points. Please be sure to include the appropriate units as part of your final answer.

1.       Mercury, the only metal that exists as a liquid at room temperature, melts at 234.3 K. Convert this melting point to degrees Celsius.

2.      Mercury has a boiling point of 356.58°C. Convert this temperature to degrees Fahrenheit.

3.      Mercury metal is poured into a graduated cylinder that holds exactly 22.5 mL. The mercury used to fill the cylinder weighs 306.0 g. From this information, calculate the density of mercury, in grams per cubic centimeter.

4.      What is the density of mercury in pounds per cubic inch (lb/in³)? a. 1 lb = 454g, 1 in= 2.54 cm.

5.      What are some of the physical and chemical properties of Mercury? Mention at least two of each.

Information about accessing the Blackboard Grading Rubric for this assignment is provided below.

Unit V Problem Solving

In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 2.01 Å (Li–        F), 2.82 Å (Na-Cl), 3.30 Å (K–Br), and 3.67 Å (Rb–I), respectively.

1.        Predict the cation-anion distance of each ionic compound above using the values of ionic radii given in Figure 7.7 on page 257 in the textbook. To receive full credit, you must show how you predicted the distance for each molecule by providing a step-by-step solution for each molecule. The solution for each molecule is worth 8 points; thus, a total of 32 total points is possible for this question.

2.       Calculate the difference between the experimentally measured ion-ion distances provided at the beginning of this assignment and the ones you have predicted in problem 1. You must show how you calculated the difference for each molecule by providing a step-by-step solution for each molecule to get full credit (6 points for each molecule; total possible points for this section is 24 points). Assuming that we have an accuracy of 0.04Å in the measurement, please indicate for each molecule if your predicted ion-ion distances are accurate or not accurate with respect to their experimental ion-ion distances (2 points for each molecule; total possible points for this section is 12 points). A total of 32 total points is possible for this question.

3.       What estimates of the cation-anion distance would you obtain for these four compounds using their bonding atomic radii? (Note: these values are also in Figure 7.7 but are different from the ionic radii.) For each of the four compounds, calculate the difference between the predicted ionic bond distance, which you calculated in problem 1, and predicted atomic bond distances you calculated in this problem. To receive full credit, you must show how you calculated the difference for each molecule by providing a step-by step solution for each molecule (6 points for each molecule; total possible points for this section is 24 points). Again, assuming that we have an accuracy of 0.04Å in the measurement, indicate for each molecule if your predictions are less or more accurate using the atomic radii prediction method; explain your answer (2 points for each molecule; total points possible for this section is 8 points). Using your knowledge of atomic and ionic radii trends in the periodic table, why might one prediction method be more appropriate to use than the other in certain molecules (worth 4 points)? A total of 36 points is possible for this set of questions.

Information about accessing the Blackboard Grading Rubric for this assignment is provided below.

Unit VIII Problem Solving

Your book presents all of the formulas you will need to complete this assignment, except for the average molecular speed, shown below. μavg = ^√  _· 

Let's show the formula for molecular speed at work. Provide a line-by-line solution for the molecular speed of each of the following five gases at 300K: CO, SF6, H2S, Cl2, HBr. You must show your work for each gas to get full credit (6 points for each gas). Finally, use these speeds to help place the five gases in order of increasing average molecular speed i.e. lowest to highest speeds (3 points).

1.       Now let's calculate the rms speeds of CO and Cl2 gas by providing line-by-line solutions for each molecule. You must show your work for each gas to get full credit (16 points for each gas). Compare your calculated rms speeds of the CO and Cl2 molecules at 300 K by explaining any potential fundamental differences between the molecules (1 point).

2.      The most probable speed formula behaves similarly to the molecular speed formula. Calculate the most probable speeds of the CO and Cl2 molecules by providing line-by-line solutions for each molecule. You must show your work for each gas to get full credit (16 points for each gas). Compare the molecular speeds of the CO and Cl2 molecules at 300 K by explaining any potential fundamental differences between the molecules (1 point). Finally, from your calculations what is the trend in similarities between rms speeds for CO and Cl2 and the most probable speeds for CO and Cl2 (1 point)?

Information about accessing the Blackboard Grading Rubric for this assignment is provided below.