Electronegativity - Online Tutor, Practice Problems & Exam Prep

Select all that correctly predict one compound with the higher molecular dipole moment in these pairs of compounds: Propyl chloride and propyl iodide, 1-chlorobutane and cyclobutane. Explain.

Which of the following compounds has the greatest tendency for carbonyl oxygen to donate an electron pair?

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Identify the oxygen atom that has the greater electron density and write the possible product when the given molecule reacts with H⁺.

Determine which has a larger dipole moment: CHCl₃ or CDCl₃, based on the fact that hydrogen is more electronegative than deuterium. 

True or False: We would expect Cu to be more electronegative than Fe because the former has a larger size than the latter.

Which of the following organometallic compounds reacts most strongly with an H⁺?

A) CH₃Li

B) CH₃Na

C) (CH₃)₂Mg

D) (CH₃)₂Cu

Identify which of the following compounds has the smallest dipole moment.

Show the direction of the dipole moment for the following compounds, cis-1,2-dibromoethene and trans-1,2-dibromoethene. Determine which of the two compounds has the larger dipole moment.

Determine the direction of the dipole moment of the following compound.

Which of the following compounds has the greatest tendency for nitrogen to donate an electron pair?

A carbon-carbon bond with varying hybridizations has a small dipole moment. In the specified bonds below, draw the direction of the dipole.

For each of the following molecules CH₃Cl, CCl₄ and C₂H₅OH, draw the appropriate Lewis structure, show how the bond dipole moments and dipole moments created by non-bonding pairs of electrons contribute to the molecular dipole moment, and estimate the magnitude of molecular dipole moment.

Identify which of the following compounds has the lowest dipole moment.

Determine which of the following isomers with the molecular formula C₂H₂F₂ does not have a dipole moment.

What is the direction of the dipole moment of the following compound?

Determine the direction of polarity of the indicated bond in the following compounds, using the symbols δ+ and δ−:

a. H₃C—CH₂—OH
b. H₃C—CH₂—F

Arrange the bonds in a decreasing order of polarity.

H—Cl, H—Br, H—F, H—I

Based on the electrostatic potential maps given below, explain why the potential map of pyrrole is more red in the center while the potential map of pyrrolidine is more red at the bottom.

Determine, between the atoms of chlorine (Cl) and iodine (I), which has a larger atomic radius and which is more electronegative.

Determine the direction of polarity of the indicated bond in the following compounds, using the symbols δ+ and δ−:

a. F—I
b. HO—F

Explain why boron trichloride has a dipole moment of zero, while phosphorus trichloride has a dipole moment of 0.97 D despite the fact that B-Cl bonds are more polar than P-Cl bonds.

Identify the compounds with polar covalent bonds from the list below.

H₂C=CH₂  CH₃—Cl  F—F  H—F

Determine one set in which the direction of the dipole moments of each bond is from the left to the right.

Explain why chlorobenzene has a smaller dipole moment than cyclohexyl chloride.

Determine which bond is stronger and why.

N—N or N—H

Identify which of the following compounds has the lowest dipole moment.

Identify which of the following compound has the most ionic covalent bond character.

For the given compound, draw its dipole moment's direction.

For the following compound, indicate its dipole moment's direction.

The S=O bond has a bond length of about 1.49 Å and a dipole moment of about 3.96 D. Determine the relative importance of the resonance contributors shown below using the above information.

State whether the given statement is True or False: 

H₂S is more polar than H₂O due to the fact that H-S bond is longer than H-O bond. 

Arrange the bonds in a decreasing order of polarity.

N—I, N—N, N—F

Determine which bond is stronger and why.

H₃C—F or H₃C—Cl

A) C-F bond is s stronger due to larger size and smaller electronegativity of F.

B) C-Cl bond is stronger due to smaller size and greater electronegativity of Cl.

C) C-F bond is stronger due to smaller size and greater electronegativity of F.

D) C-Cl bond is stronger due to bigger size and smaller electronegativity of Cl.

Select all sets that correctly describe the Lewis structure, the contribution of bond dipole moments and non-bonding pairs of electrons to the molecular dipole moment, and an estimation of the magnitude of the dipole moment for compounds CH₂=NCH₃, CH₃OH and CCl₄.

(1) Small molecular dipole moment.                     (2) Small molecular dipole moment.

(3) Large molecular dipole moment.                 (4)  Small molecular dipole moment.

(5) Zero molecular dipole moment.

Which atom in methyl chloride has the highest electron density, based on the given potential map?

Arrange the bonds in a decreasing order of polarity.

C—O, C—F, C—S

Draw the direction of the net dipole moment in the structure below.

Determine the compound with the most polar bond and the compound with the least polar bond among the compounds below:

CsF LiCl  H₂  NaCl

Explain the difference in the potential maps for methyl chloride and methyl lithium in terms of color.

Using the electronegativities of the atoms, determine the direction of the dipole moment in the indicated bonds.

a. H₃C—Cl
b. H₃C—Mg

Thin-layer chromatography was used to separate a mixture of alanine, phenylalanine, tyrosine, and serine. Rank the order of amino acid spots formed from top (1) to bottom (4) when the chromatographic plate was coated with ninhydrin solution and heated.

For each compound KCl, KOH, CH₃CH₂Li, CHCl₃, LiOCH₃, HCO₂K, and CH₄, classify the bonding as covalent, ionic, or a mixture of covalent and ionic.

Determine the degree of charge separation in the C=O bond of acetone if the bond length and the dipole moment are about 2.4 D and 1.23 Å respectively. How significant is the charged-separated resonance form in the structure of acetone?

Draw the structure for the following molecule that shows the approximate bond angle around the N atom and describe the polarity of the molecule.

CH₃CH₂CONHCH₃

Illustrate the direction of the dipole moment of the following indicated bonds. Use the symbols δ+ and δ−.

(i) HO—I

(ii) H₃CH₂C—Na

Arrange the following molecules in decreasing net dipole moment.

Select the molecule with a zero dipole moment.

The potential maps for BeH₂, H₂, and HCl are shown below.

(i) Identify the polar compound/s.

(ii) Justify why BeH₂ has the largest hydrogen.

(iii) Identify the compound with the hydrogen that will have the most attraction to a negative charge.

Determine the direction of the dipole moment in sesquifulvalene. Why is it pointing in that direction?

If the C≡N triple bond has a length of 1.16 Å and a dipole moment of 3.6 D, what is its charge separation?

Explain why OF₂ has a smaller dipole moment than H₂O when the O—F bond is more polar than the O—H bond.

μ(OF₂) = 0.3 D, μ(H₂O) = 1.8 D.

Using the concept of electronegativity, predict if a dipole (electronegativity difference ≥ 0.5) is present for each bond. If yes, show the direction of the dipole moment.

(i) C—F

(ii) C=O

(iii) C≡N

(iv) C—Mg

Show the direction of the dipole moment for each of the compounds below (If applicable). Predict which will have the smaller/no dipole moment.

Show the direction of the dipole moment for each of the compounds below (if applicable). Predict which will have a larger dipole moment.

For the given molecule:

Draw the Lewis structure, indicate the dipole moments, and show how they together with nonbonding pairs of electrons contribute to the molecule's net dipole moment. Approximate whether the dipole moment would be large, small, or zero.

Draw the Lewis structure of the given molecule, indicate the dipole moments, and show how they together with nonbonding pairs of electrons contribute to the molecule's net dipole moment. Approximate whether the dipole moment would be large, small, or zero.

The electrostatic potential maps for PH₃ and H₂S are shown below. The red region represents high electron potential and the blue region represents low electron potential. Draw the three-dimensional structure of H₂S and explain how it corresponds with its electrostatic potential map.

Provide a reason why alkali metals can not form covalent bonds.

Give the ionic compound (with charges) that will be forming from the following metal and non-metal.

Ca and Cl

Identify the charge of the ion that results from the ionization of Ga (from group 3A).

Without referring to electronegativity values, estimate whether the bond shown below is ionic, polar covalent, or covalent.

K―Br

Draw the ionic compound that most likely forms between the metal magnesium and the nonmetal iodine.

For the species given below:
(i) Draw an appropriate Lewis structure.
(ii) Draw a structure that shows approximate bond angles.
(iii) State if it has a net zero dipole moment.

HClO₃

i) Provide the Lewis structure of CO₂.

ii) Show approximate bond angles in the structure.

iii) Does CO₂ have a net dipole moment?