Complete the following table based on the structure of the given molecules or ions. (Note: Lewis structure will not be graded) Molecule/lon Electron Pair Geometry Molecular Geometry Hybridization of the Central Atom Resonance Structures (Yes/No) |(a) Chlorine trifluoride (CIF3) |(b) Nitrite ion (NO2')

In consideration of the overall resonance hybrid OCN(^-), which is the proposed resonance structure that's most important? In lewis Dot Form*

b) What is the electron geometry and the molecular shape of CBR2O respectively? (Hint: Refer to your work on worksheet 8)

Draw a Lewis structure for (a) PH₄⁺; (b) C₂F₄; (c) SbH₃.

Draw a Lewis structure for (a) CH₄S; (b) S₂Cl₂; (c) CHCl₃.

A 0.167-g sample of an unknown compound contains 0.00278 mol of the compound. Elemental analysis of the compound gives the following percentages by mass: 40.00% C; 6.71% H; 53.29% O. Determine the molecular formula, molar mass, and Lewis structure of the unknown compound.

What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom?

Draw Lewis structures for Hydronium ion, H3O+ Number of electron sets (groups):  ? Electronic Geometry:  ? Number of bonding electron sets (groups):  ? Number of non-bonding electron sets (groups) or lone pairs:  ? Molecular Geometry:  ? How many bonds have a dipole:  ? If present, do the dipole cancel each other:  ? Is the molecule polar:  ?

Draw the Lewis Structures for boron trifluoride (BF3), phosphorous trichloride (PCI3), oxygen difluroide (OF2), nitrogen trichloride (NCI3) and meth (CH4). Which do you expect to be the most polar? (Hint: which will have the greatest molecular dipole?) O boron trifluoride O phosphorous trichloride O methane O oxygen difluroide O nitrogen trichloride

Suppose that a molecule has four bonding groups and one lone pair on the central atom. Suppose further that the molecule is confined to two dimensions (this is a purely hypothetical assumption for the sake of understanding the principles behind VSEPR theory). Make a sketch of the molecule and estimate the bond angles.