Episode 8 of the Shedding Light on Atoms series explains how ionic bonds are formed in 3D lattice structures. Spiro Liacos, a science teacher, examines how atoms can gain or lose electrons, and how the number of electrons gained or lost depends on an atom's electron configuration. The program concludes by comparing ionic compounds with covalent compounds, explaining the difference at the atomic level.

Originally released by Liacos Educational Media, 2015. Streaming video file encoded with permission for digital streaming by Infobase on February 17, 2016. Link to website with Teacher's notes and Question Sheet for students available under Additional info tag.

Characteristics of an Atom --(1:38) -- Sodium Chloride Structure -- (2:40) -- Ionic Bonds -- (2:59) -- Ionic Compounds -- (3:44) -- Periodic Trends -- (4:20) -- Periodic Patterns -- (1:26) -- Chemical Formulas -- (4:22) -- Ionic Compound Formulas -- (3:11) -- Transition-Metal Compounds -- (2:03) -- Chemical Reaction -- (2:10) -- Polyatomic Ions -- (4:04) -- Ionic vs. Covalent -- (3:59) -- Strong Ionic Bonds -- (2:30) -- Credits: Covalent Bonding: Shedding Light on Atoms, Episode 8 -- (0:22). Part A: Introduction: Atoms are made of protons, neutrons, and electrons. Protons have a positive charge and electrons have a negative charge. In a pure sample of lithium metal, every atom has three protons and three electrons. Part B: Table Salt and the Ionic Bond: Ionic bonds form between the atoms of metals and of non-metals. Ionic bonding involves the transfer of electrons from metal atoms to non-metal atoms which results in the atoms becoming charged. The charged atoms, called ions, attract each other and bond together, thus forming an ionic compound. Part C: Periodic Trends: Atoms gain or lose electrons depending on their electron configurations. Part D: Working out Chemical Formulas: In NaCl, there is one Cl atom for every one Na atom, but in MgCl2, there are 2 Cl atoms for every one Mg atom. Why is this? Part E: Transition-Metal Compounds: Some metals only ever lose a specific number of electrons (Na atoms, for example, can only ever form Na+ ions), while others can form a range of ions (Fe atoms can form Fe2+ ions and Fe3+ ions). Part F: Polyatomic Ions: Some ions are made of more than one atom. Part G: Ionic vs Covalent: Ionic compounds have really high melting points, and you’ll rarely see them in their liquid state. Covalent compounds, though, are very commonly found as liquids and gases at room temperature. Why? And what is the difference, at the atomic level, between a solid, a liquid, and a gas anyway?.