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Chapter 19 Molecules and Compounds

This section delves into the two primary types of chemical bonds: ionic and covalent. Ionic bonds form when atoms gain or lose electrons to achieve stability, exemplified by sodium and chlorine's interactions. Covalent bonds, on the other hand, occur when atoms share electrons, often resulting in diatomic molecules like H2 and O2. The concept of electronegativity is also vital, as it describes the attraction an atom has for electron pairs in covalent bonds. This guide clarifies how to distinguish between ionic and covalent bonding based on the types of elements involved.

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Chapter 19 Molecules and Compounds

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  1. Chapter 19 Molecules and Compounds Section 19.1 Bonding and Molecules – Part 2

  2. Types of Chemical Bonds • Recall that atoms gain, lose, or share e- to gain 8 valence e-. • so that they become stable.

  3. IonicBonds-formed when atoms gain or lose electrons. • Ex: Na has 1 valence e- =

  4. When Na loses that electron, its 2nd E.L. becomes full and stable with 8 e-. sodium atom sodium ion Atoms with an electrical charge are called ions.

  5. Chlorine has 7 valence electrons. • If Cl gains 1 electron, its valence shell will be full and stable. chlorine atom chlorine ion

  6. Opposites attract, so… • Are these two ions likely to bond?

  7. Covalent Bonds • Most atoms share electrons to gain an octet. • Covalentbonds are formed when e- are shared.

  8. Covalent Bonds, cont. • Covalent bonds can form between 2 different types of atoms or between 2 or more atoms of the same type.

  9. Diatomicmolecules: • – covalently bonded atoms of the same type. • Exs: H2 Cl2 F2 I2 O2 Br2 N2

  10. How can you tell whether a bond is ionic or covalent? In GENERAL: • Ionic – metal / nonmetal • Covalent – 2 nonmetals

  11. Electronegativity • Sometimes e- are shared unequally in covalent bonds. • Electronegativity – attraction atom has for shared pair of e-.

  12. Electronegativity • Elements in Group 17 have highest electronegativity. • Elements in Groups 1 and 2 have lowest electronegativity.

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