**Molecule G: PF₅** - **Lewis structure:** [Space left blank for drawing] - **Hybridization:** - **Number of σ and π bonds:** - σ: [Space left blank] - π: [Space left blank] - **Molecular shape:** [Space left blank] - **Number of valence electrons:** [Space left blank] - **Number of bonded atoms on central atom:** [Space left blank] - **Number of lone pairs on central atom:** [Space left blank] - **Bonded-atom lone-pair arrangement:** [Space left blank] - **Polarity:** [Space left blank] - **Central atom steric number:** [Space left blank] - **Bond angles:** [Space left blank] - **Bond order (P-F):** [Space left blank] --- **Molecule H: TeF₆** - **Lewis structure:** [Space left blank for drawing] - **Hybridization:** - **Number of σ and π bonds:** - σ: [Space left blank] - π: [Space left blank] - **Molecular shape:** [Space left blank] - **Number of valence electrons:** [Space left blank] - **Number of bonded atoms on central atom:** [Space left blank] - **Number of lone pairs on central atom:** [Space left blank] - **Bonded-atom lone-pair arrangement:** [Space left blank] - **Polarity:** [Space left blank] - **Central atom steric number:** [Space left blank] - **Bond angles:** [Space left blank] - **Bond order (Te-F):** [Space left blank]

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 atom 1 atom 2 π bond If an atom has sp³d hybridization in a molecule: If an atom has sp 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 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

HCN?

CF2H2?

Hybridization around central Molecular Number of Lewis Structure Sketch 3D Molecular Electron shape of electron Formula Valence Geometry Geometry Electrons atom domains around central atom (include all atoms in the sketch) CO2 SbCls NH3

Which of the following molecules exhibit bond angles of 120 degrees CH_2O CO_2 N_2O ONCI

For each of the following molecules, write the Lewis structures, predict the electron geometry, molecular geometry, bond angles, expected hybrid orbitals on central atoms and predict the overall polarity. BRF3 ICI4

Describe the hybrid orbitals used by the carbon atom inN=C-Cl. Predict the geometry of the molecule.

Hybridi- Molecular Polarity Formula Lewis structure Total # of Electron group Molecular Valence geometry geometry zation Electrons BRF3 XeF2 ICI5 ICI2-

Consider the skeletal structure shown below: N-C-C-N Draw the Lewis structure and: 1- indicate the hybridization for each atom 2- indicate each sigma bond and each pi bond 3- show the lone electron pairs