Master Level Writing Service: General Chemistry I (CHM 1030) Columbia Southern University

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 ΔH_f° 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 ΔH_f° of KBr is equal to __________.

Selected Answer:	ΔH_f°[K (g)] + ΔH_f°[Br (g)] + I_l(K) + E(Br) - ΔH_lattice
Correct Answer:	ΔH_f°[K (g)] + ΔH_f°[Br (g)] + I_l(K) + E(Br) - ΔH_lattice

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.

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