Question

what is the lewis structure, molecular shape, polarity, and bond angle of N2, HF, and P4?

Answer 1

Solution - Lewis structure ! No - It has 5 external electron In which = 3 e of each N is used in making 3 bonds and de remains as lone pair. 2 (N! Ni) (3 bond pair t2 lone pate) moleculars, geometry of this molecule is binear :( NEN Bond angle = 180° 180°

Polarity in In No both Nitrogen atom has same electronegativity, So It is non polar Note! of the same atom A molecule made up of 2 is always non polar, (1) HA Lewis structure & 8o here hydrogen has one e, and - Fluorine has 7 valence elections, so they make a single bond with each other and 3 one pain remains on fluorine. I bond paint 3 Lone fair PCA Molecular shape ! It has sp3 hybridisation in it, is orbitals T and 3 poubital, Thus Hf is simply a linear s omolecule, 'It is simply a linear diatomic molecule, so - there is no bond angle. in Polarity Hydrogen has Electronegativity of Q1 and fluorine and electronegativity of 40, So here must be muity between two atoms, 80 Hf is polar two atome come polarity between

Lewis structure in p has 5 Valence election, so each . Phasphorous makes 3 bond with other p, and one tone pair will be there care ip (s bond paint I lone pair) Sp3 hybridisation Molecular shape i molealar shape of Pu is tetrahedral - because of sp3 hybridization and has bond angle of 109°981 - - Polarity - In I same be zero y all of the atom bonding so Electronegative difference 40 there is no palarity ause are would in Py. -