Guided course 03:49How to use Organic Chemistry to make Lewis Structures easier.Johnny Betancourt2565views23rank7comments
Multiple Choice How many valence electrons does a nitrogen atom have, and how many bonds does a neutral nitrogen atom typically make?7840views
Multiple Choice How many lone pairs of electrons does the nitrogen atom have in the following structure (assume all formal charges are already drawn in). 431views
Textbook QuestionDraw Lewis structures for the following compounds and ions, showing appropriate formal charges. (CH3)2O—BF3 [HONH3]+ KOC(CH3)3 [H2C=OH]+1168views
Textbook QuestionDraw Lewis structures for the following compounds and ions, showing appropriate formal charges. +CH3 -CH3 NaBH4 NaBH3CN1029views
Textbook QuestionWrite Lewis structures for the following molecular formulas. Circle any lone pairs (pairs of nonbonding electrons) in the structures. C3H6 (one double bond) C3H4 (two double bonds) C3H4 (one triple bond)1308views
Textbook QuestionDimethyl sulfoxide (DMSO) has been used as an anti-inflammatory rub for race horses. DMSO and acetone appear to have similar structures, but the C=O carbon atom in acetone is planar, while the S=O sulfur atom in DMSO is pyramidal. Draw Lewis structures for DMSO and acetone , predict the hybridizations, and explain these observations.1546views
Textbook QuestionFor each of the given species: a. Draw its Lewis structure. b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles. 1. H2CO2631views
Textbook QuestionFor each of the given species: a. Draw its Lewis structure. b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles. 2. HCN362views1rank
Textbook Question(•) Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet. (a) 8 electrons367views
Textbook Question(•) How many valence electrons does each of the following contribute to a Lewis structure? (j) Al357views
Textbook Question(•) How many valence electrons does each of the following contribute to a Lewis structure? (c) B370views
Textbook Question(•) How many valence electrons does each of the following contribute to a Lewis structure? (g) S508views
Textbook Question(•) How many valence electrons does each of the following contribute to a Lewis structure? (i) Cl370views
Textbook Question(•) How many valence electrons does each of the following contribute to a Lewis structure? (l) ―1 charge479views
Textbook Question(•) Show how the Lewis dot structure for each of the following atoms would overlap to form a single bond. (b) C and O919views
Textbook Question(•) Which atom in each pair would you expect to be the central atom in a Lewis structure? (b) C vs. O344views
Textbook Question(•) Which atom in each pair would you expect to be the central atom in a Lewis structure? (d) C vs. N367views
Textbook Question(•) Which atom in each pair would you expect to be the central atom in a Lewis structure? (f) C vs. F400views
Textbook Question(•) Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet. (d) 12 electrons504views
Textbook Question(•) Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet. (e) 6 electrons445views
Textbook Question(••) Draw the Lewis structure for the following molecular formulas. (l) SO²/₄⁻595views
Textbook QuestionDraw Lewis structures for the following free radicals. a. The ethyl radical, CH3—CH2 b. The tert-butyl radical, (CH3)3C•1416views1comments
Textbook Question(••••) In addition to radicals, anions, and cations, a fourth class of reactive intermediates is carbenes. A neutral species, the simplest carbene has a molecular formula of CH₂ . (a) Draw the Lewis structure of CH₂ .461views
Textbook Question(••) Draw the Lewis structure for the following molecular formulas.(j) H₂SO₄302views
Textbook QuestionDraw complete Lewis structures, including lone pairs, for the following compounds.g. <IMAGE>h. <IMAGE>485views
Textbook QuestionDraw complete Lewis structures, including lone pairs, for the following compounds.a. Pyridine <IMAGE>b. Pyrrolidine <IMAGE>c. Furan <IMAGE>267views
Textbook Questiona. Both PCl3 and PCl5 are stable compounds. Draw Lewis structures for these two compounds.288views
Textbook QuestionGive Lewis structures corresponding to the following line–angle structures. Give the molecular formula for each structure. E. <IMAGE>F. <IMAGE> 336views1rank
Textbook QuestionGive Lewis structures corresponding to the following line–angle structures. Give the molecular formula for each structure. G. <IMAGE>H. <IMAGE> 268views
Textbook QuestionDraw Lewis structures for the following compounds.dimethylamine, CH3NHCH3diethyl ether, CH3CH2OCH2CH31-chloropropane,CH3CH2CH2Cl241views
Textbook QuestionDraw Lewis structures fora. two compounds of formula C4H10b. two compounds of formula C2H6O333views
Textbook QuestionCyclopropane (C3H6, a three-membered ring) is more reactive than most other cycloalkanes.a. Draw a Lewis structure for cyclopropane.b. Compare the bond angles of the carbon atoms in cyclopropane with those in an acyclic (noncyclic) alkane.311views
Textbook QuestionFor each of the following compounds and ions,1. Draw a Lewis structure.2. Show the kinds of orbitals that overlap to form each bond.3. Give approximate bond angles around each atom except hydrogen.g. <IMAGE>203views
Textbook QuestionFor each of the following compounds and ions,1. Draw a Lewis structure.2. Show the kinds of orbitals that overlap to form each bond.3. Give approximate bond angles around each atom except hydrogen.h. <IMAGE>204views
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