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Ionic bonding occurs between a metal and a non-metal. Electrons are transferred from the metal to the non-metal to achieve full outer shells. When the electrons are transferred, it creates charged particles called ions. Oppositely charged ions attract through electrostatic forces to form a giant ionic lattice. Example:
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Chapter 2: Atomic Structure and Chemical Bonding. Materials → Molecules → Atoms. Atoms = protons (p) + neutrons (n) + electrons (e) Protons and neutrons are made of quarks. Quantitative measurements need units: metric or S.I. (Systeme International) or mks (meter-kilogram-second) units.
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In metals, positive metal ions (cations) are fixed in a lattice and surrounded by mobile delocalised electrons. The strong electrostatic attraction between the positive metal ions and the sea of negative delocalised electrons hold the metal together.
Chapter 14 – Intermolecular Forces 14.1 Types of Intermolecular Forces What is the difference between a bond and an intermolecular force? • Bonds: between atoms. This is the force that holds atoms together within a molecule aka intramolecular force. Polar and Nonpolar covalent bonds are examples of bonds.
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Simple bonding models assume that the total bonding results from the sum of two forces: an attractive force (FA ) and a repulsive (FR). the net force. • The repulsive force dominates at small distances, and the attractive force dominates at larger distances. At equilibrium they are just equal.
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Chemical Bonds are the attractive forces that hold atoms together in more complex units. An understanding of how and why atoms attach together in the manner they do is central to chemistry.
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Goal. To understand why atoms form molecules. Objectives. After this chapter, you should be able to. interpret the properties of elements that are important for life from the periodic table. understand why and how atoms form bonds. draw Lewis dot and line structures to represent chemical bonds. What is life?
