Guided course 11:33Differences between ionic, polar and covalent bondsJohnny Betancourt1864views31rank9comments
Textbook QuestionFor 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. CF41058views1rank
Textbook QuestionUse electronegativities to predict the direction of the dipole moments of the following bonds. N—Cl N—O N—S N—B B—Cl1229views
Textbook QuestionUse 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—OH752views
Textbook QuestionUse 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—Cl1277views
Textbook QuestionThere are three isomers with molecular formula C2H2Cl2. Draw their structures. Which one does not have a dipole moment?3473views
Textbook QuestionExplain why CH3Cl has a greater dipole moment than CH3F even though F is more electronegative than Cl.974views
Textbook QuestionWhich of the following molecules would you expect to have a dipole moment of zero? a. CH3CH3 b. H2C═O c. CH2Cl2688views
Textbook QuestionB. Draw a structure for each of the species that shows approximate bond angles. C. Which species have no dipole moment?399views
Textbook QuestionShow 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—Li963views
Textbook Questionb. Which of the following has a bond closest to the ionic end of the bond spectrum? CH3NH2 CH3CH3 CH3F CH3OH686views
Textbook Questiona. Which of the following has a polar covalent bond? CH3NH2 CH3CH3 CH3F CH3OH801views
Textbook QuestionExplain why HCl has a smaller dipole moment than HF, even though the H—Cl bond is longer than the H—F bond.939views
Textbook QuestionWhich of the following has a. the most polar bond? b. the least polar bond? NaI LiBr Cl2 KCl1446views3rank
Textbook QuestionWhich of the following molecules would you expect to have a dipole moment of zero? g. BeCl2 h. BF3408views
Textbook QuestionIf 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?821views
Textbook QuestionAccount for the difference in the shape and color of the potential maps for ammonia and the ammonium ion in [Section 1.11] 562views
Textbook QuestionWhich of the following molecules would you expect to have a dipole moment of zero? d. NH3 e. H2C═CH2 f. H2C═CHBr521views
Textbook QuestionAccording to the potential map for the ammonium ion, which atom has the greatest electron density?639views
Textbook QuestionTwo 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-dichloroethene1179views1rank
Textbook Question1. 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=NH1258views
Textbook Question1. 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. CH3OH1804views
Textbook QuestionSulfur 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.3394views
Textbook QuestionA 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≡CH825views
Textbook QuestionFor 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 b. CH3CH2OH c. CBr41185views
Textbook QuestionThe 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: 1642views
Textbook QuestionThe 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? 1482views
Textbook Question(•••) Given the Lewis structures, indicate the direction of the dipole moment, if there is one. [See Assessment 2.63.] (a)422views
Textbook Question(•••) Given the Lewis structures, indicate the direction of the dipole moment, if there is one. [See Assessment 2.63.] (b)447views
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.]1343views1rank
Textbook QuestionUsing 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―S386views
Textbook QuestionRank the following elements from least electronegative to most electronegative. Na Si F Mg C O N429views
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. O336views
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. Si333views
Textbook QuestionIn each pair of atoms, which has the larger atomic radius? Which is more electronegative? (c) O vs. S358views
Textbook QuestionIn each pair of atoms, which has the larger atomic radius? Which is more electronegative? (b) C vs. O391views
Textbook QuestionFor 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 cyclopropane753views
Textbook QuestionFor 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-difluoroethene925views
Textbook QuestionRefer 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?669views
Textbook QuestionWhich is more reactive, an organolithium compound or an organosodium compound? Explain your answer433views
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―Cl415views
Textbook QuestionA 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.627views
Textbook QuestionBased on your answer to Assessment 2.22, would you expect a larger atom to be more or less electronegative than a smaller atom?322views
Textbook Question(•••) Given the Lewis structures, indicate the direction of the dipole moment, if there is one. [See Assessment 2.63.](e) <IMAGE>310views
Textbook QuestionUse the symbols δ+ and δ− to show the direction of the polarity of the indicated bond in each of the following compounds:e. HO—Brf. H3C—Li299views
Textbook QuestionAfter 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?271views
Textbook QuestionRank the following compounds from highest dipole moment to lowest dipole moment:<IMAGE> <IMAGE> <IMAGE> <IMAGE>333views
Textbook QuestionThe 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.315views
Textbook QuestionFrom 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 302views
Textbook QuestionFor 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-ene319views
Textbook QuestionFor 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-dichloroethene243views
Textbook QuestionThe N—F bond is more polar than the N—H bond, but NF3 has a smaller dipole moment than NH3. Explain this curious result.NF3μ= 0.2 DNH3 μ = 1.5 D374views
Textbook QuestionFor 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>208views
Textbook QuestionFor 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>225views
Textbook QuestionThe 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>329views
Textbook QuestionShow the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.(b) Mg and Br324views
Textbook QuestionGive the charge most likely to result from ionization of the following metals. (b) Aluminum410views
Textbook QuestionWithout 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―Cl313views
Textbook QuestionShow the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species. (a) Al and F371views
Textbook QuestionA. 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?432views
Textbook QuestionA. 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?325views