b) Using the templates provided, draw the sigma bonding (o) and antibonding (o*) orbitals for the C2-C3 bond in hexane. Be sure to include proper shading of lobes. H H H H H H H σ bonding orbital o* anti-bonding orbital

The actual structure of SF4 places the lone pair in only one of two possible sites. To discuss the stability of the observed structures, we need only consider bond angles LP/LP ii. BP/BP >> LP/BP > LP/LP LP/BP > BP/BP >> LP/LP LP/LP >>> LP/BP > BP/BP LP/LP = LP/BP = BP/BP ii. iv. V.

Pls help ASAP.

a) Draw Lewis structures for each of the compounds below. Be sure to show all bonding and non-bonding valence electrons. Also, clearly indicate any formal charges on atoms. b) Consider the molecular geometry information given for each compound below: based on this information, specify the orbitals that each atom could use in σ- and à-bonding (sp², sp³, p, etc.) and for holding non-bonding electron pairs. Explain how your orbital assignments are consistent with the observed geometries. H₂CO (formaldehyde) HCO-angle 120⁰ CH3CO₂ (acetate anion) HCC-angle ≈ 109⁰ CCO-angle OCO≈ 120° DCH=CHBr(1-bromo-2-deuterioethylene) (two isomers) (all atoms are coplanar) (CH3)2SO (dimethylsulfoxide, DMSO) HCS-angle CSO CSC≈ 109⁰ ≈