There are three different dichloroethylenes (molecular for- mula C,H,Cl,), which we can designate X, Y, and Z. Compound X has no dipole moment, but compound Z does. Compounds X and Z each combine with hydrogen to give the same product: C,H,Cl, (X or Z) + H, → CICH,-CH,CI What are the structures of X, Y, and Z? Would you expect com- pound Y to have a dipole moment?

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

1. Complete the following table. Molecular Formula Atom a b C C₂H4O 2. Use the Lewis structure below to complete the following table. d H b Lewis Structure H a H H-C-C C-H H-C-O: H Electron Geometry Line-Angle Structure H H :O: H C ||||-- H H C CC H d Hybridization to 3. Identify the functional groups in the Lewis structure from question #2. Approx. Bond Angle

Dichloroethylene (C2H2Cl2) has three forms (isomers), eachof which is a different substance. (a) Draw Lewis structures ofthe three isomers, all of which have a carbon–carbon doublebond. (b) Which of these isomers has a zero dipole moment?(c) How many isomeric forms can chloroethylene, C2H3Cl,have? Would they be expected to have dipole moments?

Just need the last two, Bond angle and 3D structure and polarity

Create 3 different lewis structures that are not resonance structures for a compound. Note that the compound much have 4 carbon atoms, 1 oxygen atom, 1 nitrogen atom, 6-10 hydrogen atoms. The formula for the 3 compounds do not need to be exactly the same. Consider also: 1st compound: There must be 1 carbon atom with tetrahedral geometry around it. 2nd compound: There must be 1 carbon with trigonal planar geometry 3rd compound: There must be 1 carbon with linear geometry around it. Encircle those carbons mentioned. Make sure that lone pairs are visible.

Number of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance HSO4 S: S: Select one . S: Select one .. Select one XeTe4 Хе: Xe: Select one ... Xe: Select one .. Select one PHO P: P: Select one ... P: Select one .. Select one ... v PCIO P: P: Select one ... P: Select one .. Select one ..

Please explain

Use the Lewis dot structure (make sure you show all electron pairs) to predict the electronic geometry_(EG) and the shape of the molecule H2O. O EG - bent; shape - bent O EG - trigonal planar; shape lincar O EG- tetrahedral; shape - bent O EG - tetrahcdral; shape trigonal pyramidal O EG - trigonal bipyramidal; shape - tetrahedral

Please fill in the blank ! In part B, the difference is that the molecules have more than one atom with two or more attached neighbors. As molecules become larger and more complex, VSEPR theory does not attempt to create names for the overall geometries that result. Instead, we continue to consider the geometry about one central atom at a time. By giving the arrangement about each such atom in the larger structure, we can generate enough information to develop an overall picture. Thus, in your report for part B, you should determine which atoms have more than one bound neighbor, then repeat the procedure for part A. When deciding whether the molecules in part B are polar or nonpolar, focus on the molecule as a whole, not the geometry about a single atom. If the molecule is polar, draw a dipole arrow on your sketch indicating polarity.