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Chemical Bonding Chapter 8

Chemical Bonding Chapter 8. Covalent and Metallic Bonds Section 3. Covalent Bonds. A covalent bond forms 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.

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Chemical Bonding Chapter 8

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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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