Bonding VSEPR IMF

Draw the Lewis Dot structure for ICl₂^- and determine its predicted molecular geometry.

• see-saw

• trigonal bipyramidal

• linear

• bent

Draw the Lewis Dot structure for PCl₅ and determine the predicted molecular geometry

• octahedral

• trigonal pyramidal

• seesaw

• trigonal bipyramidal

Identify the hybridization and IMF of the given structure.

• sp³d; LDF

• sp³d; LDF and Dipole-Dipole

• sp³d²; LDF

• sp³d²; LDF and Dipole-Dipole

The effect of lone pairs of electrons on molecular geometry is

• to push other atoms closer together because lone pairs are

  localized on only one nucleus, so they spread out more.

• to allow the other atoms to be further apart because lone pairs

  take up less space than bonding pairs.

• to create an aysmmetical distribution of the electrons within

  the atom, thus creating a polar molecule by creating dipoles.

• to help to create resonance structures through the formation of

  pi bonds.

Why can a molecule with the structure of NBr₅ not exist?

• Nitrogen only has two energy levels and is thus unable to expand its octet.

• Bromine is much larger than nitrogen and cannot be a terminal atom in this molecule

• It is impossible to complete the octets for all six atoms using only valence electrons.

• Nitrogen does not have a low enough electronegativity to be the central atom of this molecule.

Tags

NGSS.HS-PS1-3

Which of the following molecules has hydrogen bonding?

• HCl

• HI

• HF

• HBr

This structure is called...

• tetrahedral

• Trigonal pyramidal

• Seesaw

• Bent/Angular

Choose the correct shape for this molecule:

• Trigonal planar

• Trigonal pyramidal

• Tetrahedral

• Linear

• Bent

What is the molecular geometry/shape of this molecule

• Linear

• Trigonal Planar

• Trigonal Pyramidal

• Tetrahedral

• Bent

Which molecule would have this shape?

• BF₃

• CH₄

• PCl₅

• CO₂