The electrons form a sea of electrons surrounding the positive metal ions. Delocalised electrons can carry electrical charge through the structure. Paper 1: 4.2 Bonding structure and the properties of matter: 4.2.1 Chemical bonds, ionic, covalent and metallic, an electron that is able to move freely throughout a structure, Metal atoms that have lost their outer electrons, Strong forces of attraction between oppositely charged particles, A lattice of positive metal ions surrounded by delocalised outer electrons, held together by strong electrostatic forces of attraction, Melting and boiling points of metallic substances, Reason for metals high melting and boiling points, Strong electrostatic forces between positive metal ions and negative delocalised electrons, Layers of metal ions can slide over each other, Reason alloys are harder than pure metals, Different sized atoms disrupt the layers of ions, preventing layers from sliding. The extra electrons on the outer shell leave the atom, making the metal a positive ion. Metallic structure and bonding In metals, the electrons leave the outer shells of metal atoms, forming positive metal ions and a ‘sea’ of delocalised electrons. Quizlet will be unavailable from 4-5 PM PT. ... GCSE (9-1): Chemistry: AQA: Ionic bonding. A lattice of positive metal ions surrounded by delocalised outer electrons, held together by strong electrostatic forces of attraction. Delocalised electrons can transfer heat energy quickly. On Saturday, October 10th, we'll be doing some maintenance on Quizlet to keep things running smoothly. Metallic bonding Metallic bonding is the attraction between the positive ions in a regular lattice and the delocalised electrons. Metallic bonding forms between metals and metals. Metallic bonding. Chemistry-Content-TD. 17 terms. Melting and boiling points of metallic substances.

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