Please don't provide handwritten solution .... \table [[\table [[molecule or], [polyatomic ion]], \table [[polar or], [nonpolar? ]], \table [[atomclosest to], [negative side]]], [H₂S, \table[[polar], [nonpolar]], ], [HCl, \table[[polar], [nonpolar]]],[CH \table[[polar], [nonpolar]], ]]molecule orpolyatomic ionH₂SHClCHApolar ornonpolar?polarnonpolarpolarnonpolarpolarnonpolar×atom closest tonegative sideS

if individual bond dipoles cancel out each other molecule is said to be non-polar.If individual bond…

Answered: molecule or polyatomic ion H₂S HCl CHA…

molecule or polyatomic ion H₂S HCl CHA polar or nonpolar? polar nonpolar O polar nonpolar polar nonpolar X atom closest to negative side 0

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter20: Organic Chemistry

Section: Chapter Questions

Problem 2A

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For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name hydrogen fluoride acetic acid compound hydrogen iodide formula or Lewis structure HF H :0: |_|| H- C-C-O-H H HI Between molecules of the compound? ОО ОО yes no yes no hydrogen-bonding force yes no Between molecules of the compound and molecules of water? ОО ОО yes no yes no yes no X Ś
Complete Table 3 (Remember that the values pertain to the Central atoms only. In this table, you will have more than one central atom so report more than one value, ie. 3 / 3) Table 3 Molecules with Multiple Central Atoms Molecule C2H4 H2O2. CH3OH. CH3NH2 Number of Bond Pairs / / / / Number of Lone Pairs / / / / Number of Electron Domains / / / / Molecular Geometry (Shape) / / / / Bond Angle / / / / Polar or Non-Polar Nonpolar Polar Polar Polar
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< Complete the following structural formula for a neutral molecule by adding H atoms to complete the valence of each atom. Do not introduce any double or triple bonds. Then complete the Lewis diagram by adding any unshared electron pairs needed, so that each atom except H has a complete octet. [Review Topics] [References] Use the References to access important values if needed for this question. Br Br C—C— Write the molecular formula in the order CHX, where X stands for Cl or Br. Submit Answer The number of unshared pairs in the Lewis diagram unshared pair(s). Retry Entire Group 9 more group attempts remaining Previous Email Instructor Next Save and E
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. A hydrogen bond is a(n) sharing of a pair of electrons between a hydrogen and an oxygen atom sharing of a pair of electrons between a hydrogen and a nitrogen atom an attraction between a hydrogen atom and an oxygen or nitrogen atom that are either in two different molecules or within the same molecule an attraction between oppositely charged ions to form a molecule
- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity. Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Types nonpolar covalent polar covalent nonpolar & polar covalent ionic ionic & covalent Type of molecule Nonpolar Polar Ionic 5. C2Cl2 valence e-1 = shape= type of bonds = type of molecule = 6. AICI3 valence e-1 for one Cl-1 = shape= type of bonds = type of molecule = 7. K3PO3 valence e-1 = shape= type of bonds = type of molecule = 8. KH2PO3 valence e-1 = shape at the P= type of bonds = type of molecule = dicarbon dichloride aluminum chloride potassium phosphite potassium dihydrogen phosphite
- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity. Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Types nonpolar covalent polar covalent nonpolar & polar covalent ionic ionic & covalent Type of molecule Nonpolar Polar lonic 1. HCC13 valence e-1 = shape= type of bonds = type of molecule = 2. SCI2 valence e-1 = shape= type of bonds = type of molecule = 3. P204 valence e-1 = shape= type of bonds = type of molecule = 4. N2O4 valence e-1 = shape= type of bonds = type of molecule = hydrogen carbon trichloride sulfur dichloride diphosphorus tetroxide dinitrogen tetroxide
Lewis Structure Electronic geometry Molecular (name & drawing) geometry Molecule Total # Polar or Valence e Non- (name & drawing) polar CH, (methane) NH, (ammonia) H,0 (water) co, (carbon dioxide) |CH,0 |(formaldehyde)
For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. name dimethyl ether iodomethane acetic acid compound formula or Lewis structure H T H-C-Ö-C-H I H HILIA CH₂I | H H :O: | || H-C-C-O-H Between molecules of the compound? O yes O no O yes O no hydrogen-bonding force O yes O no Between molecules of the compound and molecules of water? O yes Ono O yes O no O yes O no X S