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1. A Review of General Chemistry

Electronegativity

1. A Review of General Chemistry

Electronegativity

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Differences between ionic, polar and covalent bonds

Differences between ionic, polar and covalent bonds

Johnny Betancourt

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Multiple Choice

Which molecule/s contain/s net dipoles?

Multiple Choice

Which molecule/s contain/s net dipoles?

Multiple Choice

Which molecule/s contain/s net dipoles?

Multiple Choice

Which of the solvents are apolar and polar?

Multiple Choice

Indicate the correct partial charge distribution for a C–N bond.

Multiple Choice

Which bond is most likely to be ionic?

Textbook Question

For each compound, state whether its bonding is covalent, ionic, or a mixture of covalent and ionic. a. NaCl b. NaOH c. CH3Li d. CH2Cl2 e. NaOCH3 f. HCO2Na g. CF4

Textbook Question

Use electronegativities to predict the direction of the dipole moments of the following bonds. N—Cl N—O N—S N—B B—Cl

Textbook Question

Use the symbols δ+ and δ− to show the direction of the polarity of the indicated bond in each of the following compounds: g. I—Cl h. H2N—OH

Textbook Question

Use the symbols δ+ and δ− to show the direction of the polarity of the indicated bond in each of the following compounds: c. H3C—NH2 d. H3C—Cl

Textbook Question

There are three isomers with molecular formula C2H2Cl2. Draw their structures. Which one does not have a dipole moment?

Textbook Question

Explain why CH3Cl has a greater dipole moment than CH3F even though F is more electronegative than Cl.

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero? a. CH3CH3 b. H2C═O c. CH2Cl2

Textbook Question

B. Draw a structure for each of the species that shows approximate bond angles. C. Which species have no dipole moment?

Textbook Question

Show the direction of the dipole moment in each of the following bonds (use the electronegativities given in [Table 1.3] ): a. H3C—Br b. H3C—Li

Textbook Question

b. Which of the following has a bond closest to the ionic end of the bond spectrum? CH3NH2 CH3CH3 CH3F CH3OH

Textbook Question

a. Which of the following has a polar covalent bond? CH3NH2 CH3CH3 CH3F CH3OH

Textbook Question

Explain why HCl has a smaller dipole moment than HF, even though the H—Cl bond is longer than the H—F bond.

Textbook Question

Which of the following has a. the most polar bond? b. the least polar bond? NaI LiBr Cl2 KCl

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero? g. BeCl2 h. BF3

Textbook Question

If the dipole moment of CH3F is 1.847 D and the dipole moment of CD3F is 1.858 D, which is more electronegative: hydrogen or deuterium?

Textbook Question

Account for the difference in the shape and color of the potential maps for ammonia and the ammonium ion in [Section 1.11]

Textbook Question

Rank the bonds from most polar to least polar. d. C—H, C—C, C—N

Textbook Question

Rank the bonds from most polar to least polar. c. H—O, H—N, H—C

Textbook Question

Rank the bonds from most polar to least polar. b. C—Cl, C—I, C—Br

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero? d. NH3 e. H2C═CH2 f. H2C═CHBr

Textbook Question

According to the potential map

for the ammonium ion, which atom has the greatest electron density?

Textbook Question

Two isomers of 1,2-dichloroethene are known. One has a dipole moment of 2.4 D; the other has zero dipole moment. Draw the two isomers, and explain why one has zero dipole moment. CHCl=CHCl 1,2-dichloroethene

Textbook Question

1. Draw the Lewis structure. 2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment. 3. Estimate whether the compound will have a large, small, or zero dipole moment. h. HCN i. CH3CHO j. H2C=NH

Textbook Question

1. Draw the Lewis structure. 2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment. 3. Estimate whether the compound will have a large, small, or zero dipole moment. e. CH3F f. CF4 g. CH3OH

Textbook Question

Sulfur dioxide has a dipole moment of 1.60 D. Carbon dioxide has a dipole moment of zero, even though C―O bonds are more polar than S―O bonds. Explain this apparent contradiction.

Textbook Question

A single bond between two carbons with different hybridizations has a small dipole. What is the direction of the dipole in the indicated bonds? a. CH3—↓CH═CH2 b. CH3—↓C≡CH

Textbook Question

For each of the following compounds, 1. draw the Lewis structure. 2. show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment. 3. estimate whether the compound will have a large, small, or zero dipole moment. a. CH3CH=NCH3

Textbook Question

The C=O double bond has a dipole moment of about 2.4 D and a bond length of about 1.23 Å. b. Use this information to evaluate the relative importance of the following two resonance contributors:

Textbook Question

The C≡N triple bond in acetonitrile has a dipole moment of about 3.6 D and a bond length of about 1.16 Å. Calculate the amount of charge separation in this bond. How important is the charge-separated resonance form in the structure of acetonitrile?

Textbook Question

For the molecules shown, indicate the direction of the dipole moment. (b)

Textbook Question

For the molecules shown, indicate the direction of the dipole moment. (a)

Textbook Question

(•••) Given the Lewis structures, indicate the direction of the dipole moment, if there is one. [See Assessment 2.63.] (a)

Textbook Question

(•••) Given the Lewis structures, indicate the direction of the dipole moment, if there is one. [See Assessment 2.63.] (b)

Textbook Question

(••••) Carbon dioxide (CO₂) has no dipole moment (μ = 0 D). The related molecule sulfur dioxide (SO₂) does have a dipole moment (μ = 1.6 D) Explain this observation. [See Assessments 2.62 and 2.69.]

Textbook Question

Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.] Now, look at Figure 2.20 to check your answers. (a) C―C (b) C―O (c) C―H (d) C―F (e) C―Cl (f) C―S

Textbook Question

Rank the following elements from least electronegative to most electronegative. Na Si F Mg C O N

Textbook Question

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why? (b) N vs. O

Textbook Question

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why? (d) B vs. Si

Textbook Question

In each pair of atoms, which has the larger atomic radius? Which is more electronegative? (c) O vs. S

Textbook Question

In each pair of atoms, which has the larger atomic radius? Which is more electronegative? (b) C vs. O

Textbook Question

Which bond is stronger? Briefly explain why. b.

Textbook Question

Which bond is stronger? Briefly explain why. a.

Textbook Question

For each pair of compounds, predict which one has the higher molecular dipole moment, and explain your reasoning. a. ethyl chloride or ethyl iodide b. 1-bromopropane or cyclopropane

Textbook Question

For each alkene, indicate the direction of the dipole moment. For each pair, determine which compound has the larger dipole moment. a. cis-1,2-difluoroethene or trans-1,2-difluoroethene

Textbook Question

c. Which compound has the greater electron density on its oxygen atom?

Textbook Question

b. Which compound has the greater electron density on its nitrogen atom?

Textbook Question

a. Which oxygen atom has the greater electron density?

Textbook Question

Refer to the electrostatic potential maps

to answer the following questions: c. Why is the center of the electrostatic potential map of benzene more red than the center of the electrostatic potential map of pyridine?

Textbook Question

Which is more reactive, an organolithium compound or an organosodium compound? Explain your answer

Textbook Question

(a) Rank the following bonds in terms of the strength of their bond dipole (1 = weakest, 6 = strongest). (b) Which carbon has the largest δ⁺ ? C―F C―Br C―I C―H C―C C―Cl

Textbook Question

A mixture of seven amino acids (glycine, glutamate, leucine, lysine, alanine, isoleucine, and aspartate) is separated by chromatography. Explain why only six spots show up when the chromatographic plate is coated with ninhydrin and heated.

Textbook Question

Based on your answer to Assessment 2.22, would you expect a larger atom to be more or less electronegative than a smaller atom?

Textbook Question

(•••) Given the Lewis structures, indicate the direction of the dipole moment, if there is one. [See Assessment 2.63.]

(e) <IMAGE>

Textbook Question

Use the symbols δ+ and δ− to show the direction of the polarity of the indicated bond in each of the following compounds:

e. HO—Br

f. H3C—Li

Textbook Question

After examining the potential maps for LiH, HF, and H2, answer the following questions: <IMAGE>

a. Which compounds are polar?

b. Why does LiH have the largest hydrogen?

c. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?

Textbook Question

Rank the following compounds from highest dipole moment to lowest dipole moment:

<IMAGE> <IMAGE> <IMAGE> <IMAGE>

Textbook Question

Which of the following compounds have a dipole moment of zero?

<IMAGE>

Textbook Question

b. In what direction is the dipole moment in calicene? Explain.

<IMAGE>

Textbook Question

The C=O double bond has a dipole moment of about 2.4 D and a bond length of about 1.23 Å.

a. Calculate the amount of charge separation in this bond.

Textbook Question

From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.

In each case, predict whether the dipole moment is relatively large (electronegativity difference >0.5) or small.

a. C—Cl

b. C—H

c. C—Li

d. C—N

e. C—O

Textbook Question

For each alkene, indicate the direction of the dipole moment.

For each pair, determine which compound has the larger dipole moment.

b. cis-1,2-dibromoethene or trans-2,3-dibromobut-2-ene

Textbook Question

For each alkene, indicate the direction of the dipole moment.

For each pair, determine which compound has the larger dipole moment.

c. cis-1,2-dibromo-1,2-dichloroethene or cis-1,2-dichloroethene

Textbook Question

The N—F bond is more polar than the N—H bond, but NF3 has a smaller dipole moment than NH3. Explain this curious result.

NF3

μ= 0.2 D

NH3

μ = 1.5 D

Textbook Question

For each of the following compounds,

1. draw the Lewis structure.

2. show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. estimate whether the compound will have a large, small, or zero dipole moment.

d. <IMAGE>

Textbook Question

For each of the following compounds,

1. draw the Lewis structure.

2. show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. estimate whether the compound will have a large, small, or zero dipole moment.

e. <IMAGE>

Textbook Question

The electrostatic potential maps for ammonia and water are shown here. The structure of ammonia is shown within its EPM. Note how the lone pair creates a region of high electron potential (red), and the hydrogens are in regions of low electron potential (blue). Show how your three-dimensional structure of water corresponds with its EPM. <IMAGE>

Textbook Question

Why are Na+ and K+ unable to form covalent bonds?

Textbook Question

Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.

(b) Mg and Br

Textbook Question

Give the charge most likely to result from ionization of the following metals. (b) Aluminum

Textbook Question

Without looking at Figure 2.20, use your intuition to estimate whether a bond is ionic, polar covalent, or covalent. [Really, don't look until you've done all the problems.] Now, look at Figure 2.20 to check your answers.

(a) Na―Cl

Textbook Question

Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species. (a) Al and F

Textbook Question

A. Draw a Lewis structure for each of the following: 2. HNO3 B. Draw a structure for each of the species that shows approximate bond angles. C. Which species have no dipole moment?

Textbook Question

A. Draw a Lewis structure for each of the following:

3. N3−

B. Draw a structure for each of the species that shows approximate bond angles.

C. Which species have no dipole moment?

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