how do i find the number of lone pairs and e-pairs in the lewis structure?

Answer 1

You write out the Lewis structure according to the rules. Then whatever electrons are left over, arrange them into the lone pairs. You just have to be careful that the Lewis theory breaks down very soon and produces many anomalies. Examples are BF3, SF6, and any oxide of nitrogen with just one N.

With H2O, draw 2 H's next to the O. Put an x for an H-electron between each H and the O. Put a * for an O-electron between them too. O has 6 valence electrons, so that leaves 4 *'s left over. Put these 4 *'s in two pairs on the other sides of the O. Two lone pairs.

Answer 2

one million. Electronegativity has no longer something to do with predicting sp hybridization. If carbon has sp hybridization it relatively is as a results of fact it relatively is in a linear molecule like CO2. 2. The molecule it relatively is maximum polar relies upon as a lot on the geometry as on the electronegativity. CH3Cl is polar, yet CH3CHO is extra polar. 3. C2H6 has no lone pairs. CH3CHO has 2 lone pairs on oxygen. CH3Cl has 3 lone pairs on Cl. CO2 has 4 lone pairs on 2 oxygen atoms. ============ follow up ============= Ryan has basically responded the 1st question properly. Acetaldehyde has a dipole 2nd of two.7 D, and is amazingly polar. extra polar than chloromethane. Ryan says CO2 has no lone pairs. no longer so. CO2 has 4 pairs. 2 pairs on each and every of two oxygen atoms.