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Chemistry - College, section 1, Fall 2019
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Zumdahl et al - Chemistry 10/e (Homework)

James Finch

Chemistry - College, section 1, Fall 2019

Instructor: Dr. Friendly

Current Score : 19 / 23

Due : Thursday, April 16, 2020 06:00 EDT

Last Saved : n/a Saving... ()

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Total

19/23 (82.6%)

Instructions

The tenth edition of Steve and Susan Zumdahl’s widely regarded CHEMISTRY from Cengage Learning combines a robust conceptual framework, a readable and engaging writing style, and an unparalleled selection of problems and exercises that make it one of the most trusted chemistry textbooks available today.

Question 1 displays significant figures grading for a numerical answer blank.

Question 2 adds a fill-in-the-blank answer blank to grade an element (both the symbol and the name are accepted).

Question 3 utilizes chemPad to grade a chemical formula.

Question 4 exhibits reaction grading in chemPad.

Question 5 makes use of Marvin JS to grade resonance structures.

Question 6 allows students to rank compounds using pulldown multiple-choice answer blanks.

Also available to adopters is an additional collection of almost 1,400 questions that feature feedback, tutorials, and Deep Help. This collection is organized to match the table of contents of Zumdahl's CHEMISTRY, 10th edition, and can be added from "Free Additional Content" when creating your WebAssign course at no additional cost. This demo assignment allows many submissions and allows you to try another version of the same question for practice wherever the problem has randomized values.

The answer key and solutions will display after the first submission for demonstration purposes. Instructors can configure these to display after the due date or after a specified number of submissions.

Assignment Submission

For this assignment, you submit answers by question parts. The number of submissions remaining for each question part only changes if you submit or change the answer.

Assignment Scoring

Your last submission is used for your score.

1. –/1 points ZumChem10 3.E.018. My Notes

Consider the equation below.

2 A + B → A₂B

If you mix 3.0 mol of A with 3.0 mol of B, what amount (moles) of A₂B can be produced?

WebAssign will check your answer for the correct number of significant figures.

(No Response)

1.5

moles

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2. –/2 points ZumChem10 3.E.040. My Notes

An element "X" has five major isotopes, which are listed below along with their abundances.

Isotope	Percent Natural Abundance	Mass (amu)
⁵⁸X	68.08%	57.935343
⁶⁰X	26.23%	59.930786
⁶¹X	1.14%	60.931056
⁶²X	3.63%	61.928345
⁶⁴X	0.93%	63.927966

Calculate the average atomic mass.

(No Response)

58.70

amu
What is the element?
(No Response)

Nickel -or- nickel -or- Ni

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3. –/1 points ZumChem10 3.E.088. My Notes

A sample of urea contains 1.233 g N, 0.177 g H, 0.528 g C, and 0.704 g O. What is the empirical formula of urea?

chemPad

Help

CH₄N₂O

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4. –/3 points ZumChem10 3.E.097. My Notes

Give the balanced equation for each of the following chemical reactions. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

(a) Glucose (C₆H₁₂O₆) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor.

chemPad

Help

C₆H₁₂O₆(s) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O(g)

(b) Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas.

chemPad

Help

Fe₂S₃(s) + 6 HCl(g) → 2 FeCl₃(s) + 3 H₂S(g)

(c) Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate (NH₄SCN).

chemPad

Help

CS₂(l) + 2 NH₃(g) → H₂S(g) + NH₄SCN(s)

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5. –/1 points ZumChem10 8.E.095. My Notes

Benzene (C₆H₆) consists of a six-membered ring of carbon atoms with one hydrogen bonded to each carbon. Draw the correct Lewis structures for benzene, including resonance structures. (Copy and paste the given template as many times as necessary. Assign lone pairs, radical electrons, and atomic charges where appropriate.)
(No Response)

Marvin JS

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6. –/3 points ZumChem10 3.E.078. My Notes

Arrange the following substances in order of increasing mass percent of carbon.

caffeine, C₈H₁₀N₄O₂
sucrose, C₁₂H₂₂O₁₁
ethanol, C₂H₅OH

(No Response)

sucrose

< (No Response)

caffeine

< (No Response)

ethanol

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7. –/1 points ZumChemWA10 1.3.001. My Notes

The cell of an amoeba had an estimated volume of 1115 µm³ (cubic micrometers). Convert this volume to m³ (cubic meters).

(No Response)

1.115e-15

m³

Tutorial

Solution or Explanation

Step 1 of 3

Consult a table of units. Write the conversion factor that equates two SI or metric units of interest.
1 m = 1 ×
10⁶
µm

Step 2 of 3

Carry out any mathematical processes needed for converting the SI or metric units to another form required to solve the problem.

This problem deals with volume in cubic meters and cubic micrometers. Therefore, the equation in Step 1 must be cubed on both sides to yield the desired units.

(1 m)³	=	(10⁶ µm)³
1 m³	=	10⁶ µm × 10⁶ µm × 10⁶ µm
1 m³	=	1e+18 µm³

Step 3 of 3

Use the conversion factor from Step 2 and dimensional analysis to convert the volume of the cell from the given units to the desired units. Express the result with the proper number of significant figures.

The volume of the cell in cubic meters is:

1115 µm³ ×
1 m³
1 × 10¹⁸ µm³
= 1.115e-15 m³.

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8. –/2 points ZumChemWA10 3.CM.010. My Notes

Complete the following combination/synthesis reactions and balance the equations if necessary.

(a) Li(s) + F₂(g) →

chemPad

Help

2 Li(s) + F₂(g) → 2 LiF(s)

(b) CaO(s) + SO₂(g) →

chemPad

Help

CaO(s) + SO₂(g) → CaSO₃(s)

Tutorial

Solution or Explanation

Step 1 of 10

Define a combination/synthesis reaction and write its general form. A combination reaction, also known as a synthesis reaction, is a reaction in which two or more substances combine to form a single product. Select the general form of the reaction.

A + B → AB
Step 2 of 10

(a) Li(s) + F₂(g) →

Given that the first reaction is a combination reaction, predict its product. In the first reaction, the reactants are: Li (lithium) and F₂ (fluorine).
Here we have a metal (Li) combining with a nonmetal (F₂).
We can predict that the product formed will be an ionic compound.

Since Li belongs to group IA, it normally forms the ion Li⁺.
Since F₂ belongs to group VIIA, it normally forms the ion F⁻.
Therefore, we can predict that they will combine to form the following. (Omit states-of-matter from your answer.)
LiF
Step 3 of 10

Using the information in Step 2, write the complete reaction, showing the reactants and products without their coefficients. The first combination reaction can be written (unbalanced) as the following. (Include states-of-matter under the given conditions in your answer.)
Li(s) + F₂(g) → LiF(s)

Step 4 of 10

Determine whether the equation in Step 3 is balanced by counting the number of atoms of each element on the reactant side and the product side. For the equation in Step 3:

Li atoms:	one on the reactant side, one on the product side.
F atoms:	two on the reactant side, one on the product side.

The F atoms are not balanced. Therefore, the equation is not balanced.

Step 5 of 10

Balance the equation in Step 3. To balance the F atoms, multiply LiF on the product side by 2. The equation then becomes the following. (Include states-of-matter under the given conditions in your answer.)
Li(s) + F₂(g) → 2 LiF(s)

Now we have 1 Li atom on the reactant side and 2 Li atoms on the product side.

To balance the Li atoms, multiply Li on the reactant side by 2. The equation then becomes the following. (Include states-of-matter under the given conditions in your answer.)
2 Li(s) + F₂(g) → 2 LiF(s)

Step 6 of 10

Verify that the final equation in Step 5 is balanced by counting the number of atoms of each element on the reactant side and the product side. For the final equation in Step 5:

Li atoms:	two on the reactant side, two on the product side.
F atoms:	two on the reactant side, two on the product side.

The equation is now balanced.

Step 7 of 10

(b) CaO(s) + SO₂(g) →

Given that the second reaction is a combination reaction, predict its product. In the second reaction, the reactants are: CaO (calcium oxide) and SO₂ (sulfur dioxide).
Here we have a metal oxide (CaO) combining with sulfur dioxide (SO₂).
We can predict that the product formed will be a sulfate.

Since Ca belongs to group IIA, it normally forms the ion Ca²⁺.
Sulfate is a polyatomic ion with the chemical formula SO₃²⁻.
Therefore, we can predict that they will combine to form the following. (Omit states-of-matter from your answer.)
CaSO₃
Step 8 of 10

Using the information in Step 7, write the complete reaction, showing the reactants and products without their coefficients. The second combination reaction can be written (unbalanced) as the following. (Include states-of-matter under the given conditions in your answer.)
CaO(s) + SO₂(g) → CaSO₃(s)

Step 9 of 10

Verify that the equation in Step 8 is balanced by counting the number of atoms of each element on the reactant side and the product side. For the equation in Step 8:

Ca atoms:	one on the reactant side, one on the product side.
O atoms:	three on the reactant side, three on the product side.
S atoms:	one on the reactant side, one on the product side.

The equation is balanced.

Step 10 of 10

Write the complete, balanced equations from Steps 5 and 8. The balanced equations for the two reactions are the following. (Include states-of-matter under the given conditions in your answer.)
(a) Li(s) + F₂(g) →
2 Li(s) + F₂(g) → 2 LiF(s)

(b) CaO(s) + SO₂(g) →
CaO(s) + SO₂(g) → CaSO₃(s)

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9. –/8 points ZumChemWA10 9.EX.008. My Notes

(a) Write an orbital diagram depicting the valence electrons of a carbon atom. (Complete each energy level from left to right. Enter __ for an unoccupied orbital, ↑_ for a singly occupied orbital, and ↑↓ for a doubly occupied orbital.)

(No Response)

↑↓

(No Response)

↑_

(No Response)

↑_

(No Response)

(b) Write an orbital diagram depicting the hybridized carbon orbitals present in the compound, CH₂O. (Complete each energy level from left to right. Enter __ for an unoccupied orbital, ↑_ for a singly occupied orbital, and ↑↓ for a doubly occupied orbital.)

(No Response)

↑_

(No Response)

↑_

sp²

(No Response)

↑_

(No Response)

↑_

Tutorial

Solution or Explanation

Step 1 of 6

(a) Write an orbital diagram depicting the valence electrons of a carbon atom.

Determine the electron configuration of the carbon atom. The atomic number of carbon is 6. Therefore, the carbon atom possesses 6 electron(s).

Recalling the order and capacity of each orbital, it is clear that carbon's 6 electron(s) will only fill up to the 2p orbital. Therefore, the full electron configuration of the C atom is the following.
1s² 2s² 2p²

Step 2 of 6

Draw an orbital diagram showing the distribution of valence electrons in the carbon atom. Carbon is in group IVA of the periodic table and therefore has 4 valence electron(s). According to the electron configuration in Step 1, 4 valence electron(s) will be located in the outermost orbitals: 2s and 2p. Create an orbital diagram for the 2s and 2p levels. Then fill in the electrons, remembering to follow Hund's rule. (Complete each energy level from left to right. Enter __ for an unoccupied orbital, ↑_ for a singly occupied orbital, and ↑↓ for a doubly occupied orbital.)

↑↓
2s

↑_

↑_
2p

Step 3 of 6

(b) Write an orbital diagram depicting the hybridized carbon orbitals present in the compound, CH₂O.

Draw the Lewis structure for CH₂O to determine its number of electron domains. (Assign lone pairs, radical electrons, and atomic charges where appropriate.)

In CH₂O, the central carbon has 3 bonding electron domain(s) (The double bond counts as 1 bonding domain.) and 0 nonbonding electron domain(s). The total number of electron domains on the central atom of CH₂O is 3.
Step 4 of 6

Determine the electron-domain geometry of CH₂O, using the VSEPR model. According to the VSEPR model, a molecule having a central atom with 3 bonding domains and 0 nonbonding domains has a trigonal planar electron-domain geometry.

In the trigonal planar electron-domain geometry of CH₂O, the C atom is at the center and the H and O atoms each occupy a corner of an equilateral triangle.
Step 5 of 6

Determine the type of orbital hybridization that can explain the electron-domain geometry of CH₂O. A trigonal planar electron-domain geometry implies that the orbital hybridization of the central (C) atom is the following.

sp²-hybridization

Note how this hybridization produces the 3 hybrid orbital(s) required for a molecule to assume trigonal planar electron-domain geometry.

Step 6 of 6

Draw orbital diagrams to show how the atomic orbitals of carbon (from Step 1) hybridize to form bonding orbitals in CH₂O. As noted in Step 4, the orbital hybridization of the C atom in CH₂O is sp². The sp² designation implies that 1 s orbital and 2 p orbitals hybridize to produce 3 sp² hybrid orbitals.

Only valence electrons of the C atom are involved with bonding. Therefore, we know that carbon's 2s orbital and 2 of its 2p orbitals will hybridize in forming CH₂O.

To create the hybrid orbitals in the orbital diagram, first "promote" 1 of the 2s electrons to the empty 2p orbital. Then, replace the 2s and 2 of the 2p orbitals with 3 sp² hybrid orbitals. (Complete each energy level from left to right. Enter __ for an unoccupied orbital, ↑_ for a singly occupied orbital, and ↑↓ for a doubly occupied orbital.)

atomic orbitals of carbon

↑_
2s

↑_
2p_z

↑_
2p_x

↑_
2p_y

bonding orbitals(after hybridization)

↑_

↑_
sp²

↑_

↑_
2p

Therefore, after hybridization, there is/are 3 sp² hybrid orbital(s) along with 1 unhybridized 2p orbital(s).

Note that the sp² hybrid orbitals each contain 1 electron(s). 2 of these electrons will pair with those of the 2 hydrogen atoms while the third electron, as well as the electron in the 2p orbital, will pair with the oxygen atom, forming a double bond.

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10. –/1 points ZumChemWA10 22.1.001. My Notes

Draw the structural formula for hexane, a straight-chain alkane.(No Response)

Marvin JS

Tutorial

Solution or Explanation

Step 1 of 4

Recall the definition of a structural formula. The structural formula for a molecular compound can be defined as a graphical representation showing the:

arrangement of atoms in a molecule, as well as the chemical bonding between them.

The atoms are represented by their chemical symbols, and each bond between a pair of atoms is shown as a line connecting the atoms in the molecule.
Step 2 of 4

Recall the definition of a straight-chain alkane and write its general formula. A straight-chain alkane is an open-chain hydrocarbon in which the carbon atoms are linked to one another to form a single chain, without any branches. All of the carbon-carbon bonds and carbon-hydrogen bonds are single bonds, and each carbon atom has 4 single bonds.

The general formula for a straight-chain alkane where n is the number of carbon atoms in each molecule is the following.

C_nH_{2n + 2}
Step 3 of 4

From the name of the compound and the general formula for a straight-chain alkane, write the molecular formula for the compound. The name hexane is given to a straight-chain alkane that has 6 carbon atoms.

Knowing the general formula for a straight-chain alkane (given in Step 2), we can write the molecular formula of hexane as the following. (Omit states-of-matter from your answer.)
C₆H₁₄
Step 4 of 4

Draw the structural formula for the given compound. Since the molecular formula of hexane is C₆H₁₄ (given in Step 3), the structural formula needs to have 6 C atoms and 14 H atoms.

We can start drawing the structural formula by linking the 6 C atoms together with a single bond. We can then place 3 H atoms around each terminal C atom and 2 H atoms around each internal C atom, linking them with single bonds.

The structural formula for hexane is the following.

Note that each carbon atom has a total of four single bonds linking it to four other atoms.

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Zumdahl et al - Chemistry 10/e (Homework)

Current Score : 19 / 23

Due : Thursday, April 16, 2020 06:00 EDT

Last Saved : n/a Saving... ()

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