# Ion formation

##### Intros
###### Lessons
1. Introduction to ions
2. Recall particles and charge.
3. Why atoms form ions.
4. How atoms form ions.
5. Predicting common ions.
##### Examples
###### Lessons
1. Use information in the Periodic Table to find the number of sub-atomic particles in elements.
How many electrons are in an atom of the following species?
i) P
ii) Ru
iii) Rb
1. Identify atoms and their charge when given the number of sub-atomic particles.
Identify the element and the charge on the particle described below.
1. i) A particle with 50 protons and 52 electrons.
ii) A particle with 13 protons and 10 electrons.
2. i) A particle with 16 protons and 18 electrons.
ii) A particle with 3 protons and 2 electrons.
2. Find out the number of sub-atomic particles when given ions and their charge.
Find the number of protons and electrons in the following species:
1. i) Cr$^{3+}$
ii) F$^-$
2. i) Sb$^{3+}$
ii) Zn$^+$
###### Topic Notes
In this lesson, we will learn:
• To understand the reason chemical atoms form ions and the particle that causes ionization.
• To calculate the charge of ions from electron and proton numbers
• To apply knowledge of ion charges to find number of electrons in ions
• To predict an element's stable ions based on the Periodic table

Notes:

• Atoms are comprised of protons, neutrons and electrons. In a neutral atom, the number of electrons is equal to the number of protons.

• Many elements and substances engage in chemical reactions to obtain a full outer shell of electrons, which involves metal atoms losing electrons to empty their outer shell ('dropping down a shell' in the process) and non-metal atoms gaining electrons to complete a full outer shell.

• These changes in number of electrons changes the overall charge of an atom, if the number of protons and electrons isn't equal in an atom then it becomes a charged atom.

CHARGED ATOMS ARE CALLED IONS.

• Chemical reactions only involve outer-shell electrons. They virtually never change the nucleus of an atom.

• To find the charge of an atom or ion, subtract the number of electrons from the number of protons in the particle.

• The electron shell configuration (and therefore its position in the Periodic Table) of an element is strongly related to the stable ions it is able to form – atoms gain or lose a number of electrons to fill their outer shell, which dictates their charge!

Ion formation normally occurs when electrons are transferred from one atom, usually a metal, and donated to another atom, usually a non-metal – this is how ionic compounds are formed.