Question

c) if the bond is covalent identify it as polar or non - polar. (hint: use the electronegativity)t1 - 2
non - polar

1. draw the electron dot diagrams for: t1 - 4

a) hydronium ion (h₃o⁺)
b) so₃

Explanation:

a) Hydronium ion ($H_3O^+$): Oxygen (central atom) has 6 valence electrons, each H has 1. Total valence electrons: $6 + 3(1) - 1$ (positive charge) = 8. O forms 3 bonds (2 single, 1 coordinate covalent) and has 1 lone pair.
b) Sulfur trioxide ($SO_3$): Sulfur (central atom) has 6 valence electrons, each O has 6. Total valence electrons: $6 + 3(6) = 24$. S forms 3 double bonds with O (resonance structures), no lone pairs.

Answer:

a) H:O:H (with one more H attached to O via a coordinate bond, O has one lone pair)
..
H
b) O=S=O (with a third double-bonded O, trigonal planar, resonance)
||
O

(Note: Electron dot diagrams use dots for lone pairs; for simplicity, bonds are represented as lines here, with lone pairs implied on O atoms: each O in $SO_3$ has 2 lone pairs, O in $H_3O^+$ has 1 lone pair.)