Draw the Lewis structure for SO₂ (by following the octet rule on all atoms) and then determine the number of nonbonding electron pairs on the central atom.

Without drawing the Lewis structures, predict which of the species below will have an expanded octet. SF6, XeF4, PO4 3−

Below is the Lewis structure of the nitrogen N2 molecule.  Count the number of bonding pairs and the number of lone pairs around the right nitrogen atom in this molecule.

For which one or ones of the following molecules or ions would we expect to use resonance forms in writing the Lewis structures? SO3,  SO32-,  CO32-, ClO3-

Answer the questions in the table below about the shape of the chlorine trifluoride (ClF,) molecule. How many electron groups are around the central chlorine atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central chlorine atom? (You may need to use the scrollbar to see all the choices.) |(choose one)

Select which of the following compounds violate the octet rule. more than one answer,  SF4 H2O SF5

Predicting deviations from ideal bond angles Consider the nitrogen trifluoride (NF3) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the nitrogen-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the nitrogen-fluorine bonds to be ... 0 口。 (choose one) (choose one) about the same bigger smaller

Write the Lewis structure for H2S.

is it acceptable to have more than an octet of electrons on elements C, N, O, and F? true or false

Below is the Lewis structure of the peroxide (O2−2) ion.  Count the number of bonding pairs and the number of lone pairs around the right oxygen atom