Ionic Compounds (cognito)

What is the charge of ions formed by metals and non-metals, and why are ions attracted to each other?

Metals normally form ions which have a positive charge, while non-metals form ions with a negative charge.

Ions are attracted to other ions with the opposite charge, due to electrostatic forces. 

Describe an ionic structure

Ionic structures involve many ions bonded together via ionic bonds.

The solid arranges itself into a regular 3D structure known as a lattice.

3 properties that ionic compounds have

1. High melting and boiling points

2. conduct electricity when liquid

3. high strength bonds

Why can ionic compounds only conduct electricity when in liquid/molten, or aqueous form?

The ions are free to move and carry charge.

In order for a material to conduct electricity, it must have charged particles (like electrons or ions), that are free to flow through the structure.

Why do ionic compounds have high melting and boiling points?

Ionic compounds have relatively high melting and boiling points.

This is because ionic bonds are very strong, and a high amount of energy is required to break the bonds.

Correct formula for the ionic compound, potassium chloride

KCl

How do ionic compounds maintain a neutral overall charge?

ionic compounds arrange their ions in a way that creates a neutral overall charge.

For example, magnesium ions have a 2+ charge, while chloride ions have a 1- charge.

Therefore, for every magnesium ion, two chloride ions will be attracted to it, resulting in an overall neutral charge.

Correct formula for a nitrate ion

NO₃^-

describe when Potassium ions and carbonate ions forming an ionic compound

Potassium ions and carbonate ions can form an ionic compound.

Potassium ions have a 1+ charge, while carbonate ions have a 2- charge.

This means every carbonate ion will ionically bond with 2 potassium ions.

What is the chemical formula for the compound calcium sulfate?

CaSO4

Formula for following ions:

Hydroxide:

Sulphate:

Nitrate:

Carbonate:

Ammonium:

Hydroxide: OH-

Sulphate: SO42-

Nitrate: NO3-

Carbonate: CO32-

Ammonium: NH4+