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
• 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.
Introduction to ions
Identify atoms and their charge when given the number of sub-atomic particles.
Identify the element and the charge on the particle described below.
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:
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