Draw the electron dot structure for:

• (A) Ethanoic acid
• (B) Hydrogen sulphide
• (C) Propanone
• (D) Dichlorine

Electron dot structures, also known as Lewis structures, visually represent the bonding between atoms in a molecule and the lone pairs of electrons. Here’s how to draw the electron dot structures for the given compounds:

A. Ethanoic Acid (C2H4O2)

Ethanoic acid, commonly known as acetic acid, has the following structure:

• Carbon atoms (C) are central, bonded to each other.
• Each carbon is bonded to hydrogen (H) atoms and one carbon is also bonded to a hydroxyl group (–OH).

The structure can be represented as:

H3C-C(=O)-OH

B. Hydrogen Sulphide (H2S)

This molecule consists of one sulfur atom bonded to two hydrogen atoms:

• The sulfur atom has two lone pairs of electrons.

The structure looks like:

H-S-H

With two pairs of dots around the sulfur to represent the lone pairs.

C. Propanone (C3H6O)

Propanone, also known as acetone, features a carbonyl group:

• It has three carbon atoms, with one carbon double-bonded to an oxygen atom.
• The other two carbons are bonded to hydrogen atoms.

The structure can be depicted as:

H3C-C(=O)-CH3

D. Dichlorine (Cl2)

Dichlorine consists of two chlorine atoms bonded together:

• Each chlorine atom has three lone pairs of electrons.

The simple structure is:

Cl-Cl

With three pairs of dots around each chlorine to show the lone pairs.

These structures help in understanding the arrangement of electrons and the nature of bonds in each molecule.