Ionic bonding

High School

Definition

A type of chemical bond formed when one atom transfers one or more electrons to another, creating positively and negatively charged ions that attract each other. Ionic bonds usually form between metals and non-metals, as in sodium chloride (table salt).

Worked examples

\(\)Na\( \)→\( \)Na\(^+ + e^-\) and \(\)Cl\( + e^- \)→\( \)Cl\(^-\), then \(\)Na\(^+ + \)Cl\(^- \)→\( \)NaCl\(\)

Sodium transfers one electron to chlorine, forming opposite ions that attract to make an ionic bond.

\(\)Mg\(^{2+} + 2\)Cl\(^- \)→\( \)MgCl\(_2\)

Magnesium loses two electrons to form \(\)Mg\(^{2+}\); two chloride ions balance the charge.

Common mistakes

Both atoms share electrons equally in ionic bonding → One atom transfers electrons completely to the other Sharing electrons is covalent bonding; ionic bonding is a full transfer creating charged ions.
Ionic bonds form between two non-metals → Ionic bonds typically form between a metal and a non-metal Non-metals usually share electrons (covalent); metals readily lose electrons to non-metals.
The metal becomes negatively charged after transfer → The metal loses electrons and becomes positively charged Losing electrons means losing negative charge, so the metal ion is positive.

Where you'll use it next

You'll use ionic bonding to predict formulas of compounds, explain properties like high melting points and conductivity in solution, balance chemical equations, and understand electrolytes in chemistry and biology.

Found in 1 StudyPug lesson

Mastering Ionic and Covalent Bonding

Chemistry 11

Dive into the world of chemical bonds! Explore ionic and covalent bonding, understand their formation, and discover how they shape the properties of compounds. Build a strong foundation for advanced chemistry concepts.

11th Grade11th