Bonding A bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals. + p-orbital p-orbital atom1 atom2 π bond If an atom has sp³ hybridization in a molecule: The maximum number of o bonds that the atom can form is The maximum number of p-p bonds that the atom can form is

MOLECULE NAME LEWIS STRUCTURE SHAPE NAME HYBRIDIZATION BOND ANGLE POLAR/NONPOLAR # SIGMA & PI BONDS H2O               CH4               N2H4               SO3               C2H4               HNO2               HCN

Electron group Molecular Polarity (or ion) Formula Lewis structure АХЕ Bond Notation geometry geometry angle BrF3 XeF2 IOF5 TeF5-

Use VSEPR theory to complete the following table for KrCl₂ Lewis Structure #electron groups #lone pairs hybridization type VSEPR formula bond angle(s) Geometric arrangement Name and draw 3D molecular shape Polar or Non-polar? Explain why.

For each, draw the lewis structure, a 3D Structure including Angles, Electron Pair Geometry, Molecular Geometry, and whether it is "Polar or Non/Polar" A)   SF6 B)   CH2O

Number of nonbonding pairs: CH2O (C is central atom) Number of bonding groups: Total number of electron groups: Electron Geometry Molecular shape HCN (C is central atom) Number of nonbonding pairs: Number of bonding groups: Total number of electron groups: Electron Geometry Molecular shape Number of nonbonding pairs: CO,2 Number of bonding groups: Total number of electron groups: Electron Geometry Molecular shape PC13 Number of nonbonding pairs: Number of bonding groups: Total number of electron groups: Electron Geometry Molecular shape

What is the molecular structure of a molecule that has a trigonal planar electron-pair geometry and one lone pair on the central atom?