Question

Why is the valence shell electron pair repulsion model used to predict molecular geometry? Lone pair...

Why is the valence shell electron pair repulsion model used to predict molecular geometry?

Lone pair repulsion is stronger than bonding pair repulsion.

Valence electrons are constantly moving.

Lewis structures of molecules can tell the bond strength between atoms.

Lone pair electrons of the central atom are attracted to the bonding pair electrons.
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

A)Lone pair repulsion is stronger than bonding pair repulsion.

Lone pair-lone pair > lone pair - bond pair >bond pair - Bond pair

The bonding electron pair shared in a sigma bond with an adjacent atom lies further from the central atom than a nonbonding (lone) pair of that atom, which is held close to its positively charged nucleus. VSEPR theory therefore views repulsion by the lone pair to be greater than the repulsion by a bonding pair. As such, when a molecule has 2 interactions with different degrees of repulsion, VSEPR theory predicts the structure where lone pairs occupy positions that allow them to experience less repulsion. Lone pair-lone pair (lp-lp) repulsions are considered stronger than lone pair-bonding pair (lp-bp) repulsions, which in turn are considered stronger than bonding pair-bonding pair (bp-bp) repulsions.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. When determining the molecular geometry of a molecule, which of the following needs to be...
1. When determining the molecular geometry of a molecule, which of the following needs to be considered? Choose all that apply A. Number of bonding domains on the central atom. B. Number of non-bonding electron pairs on the central atom. C. Number of core electrons on the central atom. D. Number of unpaired valence electrons in the central atom. 2. A central atom is found to have one double bond, one single bond, and one non-bonding pair of electrons. How...
Identify the electron pair geometry and the molecular structure of each of the following molecules: (a)...
Identify the electron pair geometry and the molecular structure of each of the following molecules: (a) ClNO (N is the central atom) (b) CS2 (c) Cl2CO (C is the central atom) (d) Cl2SO (S is the central atom) (e) SO2F2 (S is the central atom) (f) XeO2F2 (Xe is the central atom) (g) ClOF2 + (Cl is the central atom)
Hydrogen peroxide is a syrupy, viscous water-soluble compound. This is expected based on the structure. The...
Hydrogen peroxide is a syrupy, viscous water-soluble compound. This is expected based on the structure. The Lewis structure has _______ total valence electrons. There are _______ bonding pairs and _______ non-bonding pairs. The electron pair geometry around each oxygen atom is _______ giving a _______ shape at each oxygen atom. The central bond is _______ (polar/nonpolar) and the peripheral bonds are _______ (polar/nonpolar) with the dipole vectors pointing _______ (away from/towards) the oxygen atoms. Overall the bond dipoles _______ (add...
1. What is the formal charge on each of the Oxygen atoms in the chlorate ion,...
1. What is the formal charge on each of the Oxygen atoms in the chlorate ion, ClO3-1? a. -1 b. 0 c. +1 d. +2 2. Draw the Lewis structure and predict the geometry for SO4-2. a. Bent b. Linear c. Tetrahedral d. Trigonal Bipyramidal 3. Which of the following is not planar? a. SO3 b. NO3- c. BCl3 d. ClO3- 4. Draw the Lewis structure and predict the geometry for SF4. a. Trigonal Pyramidal b. Linear c. Seesaw d....
Learning Outcomes (Unit 2) Perform quantitative calculations based on the relationship between wavelength, energy, and the...
Learning Outcomes (Unit 2) Perform quantitative calculations based on the relationship between wavelength, energy, and the speed of light. Identify and rank the different types of radiation which comprise the electromagnetic spectrum. Explain why classical mechanics doesn't describe electromagnetic radiation. Describe the photoelectric effect and relate the energy and/or intensity of the photons to the work function and kinetic energy of the ejected electrons. Explain the origin of atomic and emission spectra and relate these spectra to discrete energy levels....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT