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Understanding Covalent and Metallic Bonds: A Comprehensive Overview

Learn about covalent bonds formed when atoms share electrons, properties of covalent compounds, metallic bonds with metal ions and electrons, and properties of metals like electrical conductivity and malleability. Dive into electron-dot diagrams and molecules.

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Understanding Covalent and Metallic Bonds: A Comprehensive Overview

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  1. Chemical BondingChapter 8 Covalent and Metallic Bonds Section 3

  2. Covalent Bonds • A covalent bondforms when atoms share one or more electrons. • Atoms with almost a full set of electrons in their outer energy levels enter into covalent bonds with each other. • Substances that have covalent bonds tend to have low melting points and boiling pointsand are brittlein the solid state.

  3. Covalent Bonds and Molecules • Substances that have covalent bonds make up particles calledmolecules. • A molecule is usually made of two or more atoms joined in a definite ratio.

  4. Electron-Dot Diagrams • An electron-dot diagram is a way to represent the valence (outer energy level) electrons of an atom or molecule. • Place the first four dots alone on each side, then pair up any remaining dots.

  5. Covalent Compounds and Molecules • The molecule is the smallest particle of a covalently bonded compound can be divided into and still be the same compound. • The simplest molecules are composed of at least two covalently bonded atoms. • They are calleddiatomic • molecules. • e.g. H2, O2, N2, F2,Cl2, Br2, I2 • Other molecules are more • complex.

  6. Metallic Bonds • A metallic bond is a bond formed by the attraction between positively charged metal ions and the electrons surrounding these ions. • Positively chargedmetal ions form when metal atoms lose electrons.

  7. Properties of Metals • Electrical Conductivity – The free valence electrons allow metals to conduct electricity (current is the flow of electrons). • Malleability and Ductility– because the electrons move freely around the metal ions, the atoms in metals can be rearranged. • Bending without Breaking – The moving electrons maintain the metallic bonds no matter how the shape of the metal changes.

  8. It’s lab time! Covalent Bonds

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