Identify the type of bond or the type of orbital the indicated electrons occupy in the diatomic molecule, I, shown below A A) A = 1 sigma bond; B = sigma bond B) A = 1 sigma bond; B = s nonbonding orbital C) A = 1 sigma bond; B - sp nonbonding orbital D) A = 1 pi bond; B = sp' nonbonding orbital E) A = 1 pi bond; B = p nonbonding orbital В

VSEPR HOMEWORK Molecule Lewis Structure #e groups #lone-pair e Hybridization type VSEPR Formula (i.e Molecular Type) Geometric arrangement Molecular Shape Bond Angle Is the molecule Polar? Justify 3d Drawing PCI₂F₁

Molecule or Polyatomic CHzCl 2- Co₂² CH4 CS₂ H₂O Lewis structure H-C-CI: H H H-C-H H s=c=s H–O–H 2- Hybrid- ization AXE 3 sp³ AX4 2 sp² AX3 3 sp³ AX4 sp AX2 3 sp³ AX₂E2 Electron pair geometry Molecular shape tetrahedral tetrahedral trigonal planar trigonal planar tetrahedral tetrahedral linear linear tetrahedral bent Bond angles all ~109.5° all 120° all ~109.5° 180° ~109.5° Bond Polarity H C 2.5 2.1 Cl 2.5 3.0 CO 2.5 3.5 C-H 2.5 2.1 Molecular Polarity if the molecule is polar, add a dipole arrow if not polar, state so and why H H H i no molecular polarity because of shape CI H H HC H no polar bonds, so no molecular polarity H S=C=S H

Select the items below that are properties of sigma bonds  options:   sidewise overlap of atomic orbitals   stronger bonds   head-on overlap of atomic orbitals   double or triple covalent bonds   weaker bonds   single covalent bond Select the items below that describe pi bonds options:   single covalent bond   stronger bonds   sidewise overlap of atomic orbitals   weaker bonds   head on overlap of atomic orbitals   double or triple covalent bond

please don't provide hand writtin solution....

What are the angles a and b in the actual molecule of which this is a Lewis structure? H H H C H a a = C b = ⁰ C H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. H X

Examine the model structures for PCl5and BrF5. Both molecules have five atoms attached to the central atom but different bond angles. Explain this difference.

How can we predict the ideal bonds ?