a SiF4, KrF4, and Sef4 molecules have similar formulas, but each has a different shape. Draw Lewis structures for these compounds, and then determine the expected hybridization of the central atom. Hybridization SiF4: Hybridization KrF4: Hybridization SeF4:

Determine a hybridization and bonding scheme for COIH. Draw its Lewis structure. Determine the hybridization, electron and molecular geometry for the central atom and the number of o and T bonds. Sketch the molecule including overlapping orbitals, label all bonds. (Make sure overlapping orbitals are the appropriate shape orbital that is ½ filled and can share an electron.). Is this molecule polar or non-polar?

In each of the groups below, all molecules except one share the same orbital hybridization of the central atom. Identify which molecule is different, and name the hybridization for that molecule and the rest of the group. a) NO3", CO32", SO;2", BCI3 b) H2S, SIF4, SeO2, PB13 c) HCN, N2O, NO2", CS2 (Hint: N is the central atom in N2O) d) ClO3", NC13, AlCl3, H3O*

Each of the structures for ClOCl, NCOH, and ClNO has atoms connected in the order given in their formulas. Identify the type of hybridization for the central atom in each compound.

Understanding the hybridization of individual atoms in a molecule. Depending on the number of single, double, or triple bonds carbon can be sp, sp2, or sp3. Please give an example of one of these. Please consider the hybridization state of all carbons in a molecule.