Giant Chemical Structures - Part 2 | Properties of Matter | Chemistry | FuseSchool

This is part 2 for our videos on giant chemical structures. Part 1 is here: Giant ionic structures also have exceptionally high melting points. This is because the electrostatic interactions between the ions are very strong. Mg2+ and O2- ions have double the number of charges on their ions than Na+ and Cl- ions which only have single charges. This means that MgO is held together by stronger ionic bonds than NaCl. Giant ionic lattices, when in the solid state, do not conduct electricity because their ions are fixed in the lattice.This lattice structure is lost when the solid is melted, freeing up ions which can then conduct electricity. Magnesium Oxide has a very high melting point, so it retains its ionic lattice structure at a high temperature. Although, eventually it will melt. This means that its ions are unable to conduct electricity, and so makes a very good insulator. Metals all share the same structure, whereby electrons in the outer shells of the metal atoms are free to move. The metallic bond is a force of attraction between these free electrons and the positively charged metal ions. Metallic bonds are strong, so metals maintain a regular structure and usually have high melting and boiling points. In addition to this, metals also have other common properties; they conduct heat and electricity because of the free electrons ability to move. Free electrons also allow the metal ions to slide past one another, and so can be hammered into shapes; this is called ‘malleability.’ The ease at which a metal can be pulled into wires depend on how ductile it is. In summary, there are three main types of giant chemical structures. These are giant covalent structures – which have high melting points and variable electrical conductivities; giant ionic lattices, which have regular arrangements of oppositely charged ions, held together by electrostatic interactions. Giant ionic lattices are very strong, so these structures have high melting points. As solids they do not conduct electricity, but when molten, will conduct. Finally, metals have a giant structure where the packed lattice have atoms that are not bonded by fixed pairs of electrons, but rather have a ‘sea’ of electrons roaming these partially filled outer shells at will.positively charged metal ions are surrounded by free electrons. Metals, because of their free electrons, generally have high melting points, conduct heat and electricity; they are also malleable and ductile. VISIT us at, where all of our videos are carefully organised into topics and specific orders, and to see what else we have on offer. Comment, like and share with other learners. You can both ask and answer questions, and teachers will get back to you. These videos can be used in a flipped classroom model or as a revision aid. Click here to see more videos: Twitter: Access a deeper Learning Experience in the FuseSchool platform and app: Friend us: This Open Educational Resource is free of charge, under a Creative Commons License: Attribution-NonCommercial CC BY-NC ( View License Deed: ). You are allowed to download the video for nonprofit, educational use. If you would like to modify the video, please contact us:

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