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Chapter 6

Chapter 6. Chemical Bonding: Ionic Bonds. Why and How Atoms Bond. ALLOTROPES. Why do chemical bonds form?.

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Chapter 6

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  1. Chapter 6 Chemical Bonding: Ionic Bonds

  2. Why and How Atoms Bond ALLOTROPES

  3. Why do chemical bonds form? Chemical bonds form to lower the energy of the system, the components of the system become more stable through the formation of bonds. Everything wants to be more stable - its easy to lie down than stand up, bonding is Nature's way of allowing the elements to lie down. There are several types of chemical bond. Initially we will concern ourselves with three basic types, ionic bonding, which involves the transfer of electron(s), covalent bonding, which involves sharing of electrons and metallic bonding, which in some ways can be considered as a combination of both.

  4. ELECTRON DOT DIAGRAM Is a shorthand method to illustrate the # of valence electrons You will use dot structures when illustrating ionic compounds SKETCH THIS IN YOUR NOTEBOOK

  5. Electronegativity The affinity for electrons. Wants to gain e- Open this link, and read the description of electronegativity

  6. Chemical Formulas • A notation that shows what elements a compound contains. • It shows the ratio of atoms or ions of the elements in the compound. • Example: NaCl, C6H12O6

  7. Stable Electron Configurations • All atoms that do not have a complete set of valence electrons tend to react. • This will satisfy the “Octet Rule”….the achieving of electron configurations similar to those of “Noble Gases” • Some elements achieve stable electron configurations thru TRANSFER of electrons and some thru SHARING of electrons

  8. Ionic Compounds • This compound only occurs when a metal combines with a non-metal. • This compounds tend to be very brittle….shatter when struck!!! • The metal(low electron affinity) will always transfer an electron to the non-metal(high electron affinity) • This will cause the formation of “IONS” which is when the charge of the atom is NOT BALANCED!!!!!! • Ions are either positively charged or negatively charged. • The metal will become a positive ion called a “CATION.” • The non-metal will become a negative ion called a “ANION.” • The “CATION” or metal is always written first in the compound followed by the “ANION.”

  9. Ionic Bonds Form Crystal Lattices The crystal structure of NaCl In NaCl, each chloride ion is surrounded by six sodium ions and each sodium ion is surrounded by six chloride ions!!!

  10. Formation of Ionic Bonds • Remember….opposites attract!! • When a cation and anion are close together, a chemical bond forms between them. • This bond is called: An “IONIC BOND”

  11. Naming Ionic Compounds • Write the name of the “Cation” (+) first • Then, write the name of the “Anion” (-) • Add an “ide” suffix to the end of the anion • Ex: sodium chloride, potassium chloride, magnesium oxide

  12. Type I Ionic Compounds The metal present forms one “1” type of cation Type II Ionic Compounds The metal present can form “2” or more cations that have different charges!!!! ION SYSTEMATIC NAME ION SYSTEMATIC NAME Fe3+ Iron (III) Sn4+ Tin (IV) Sn2+ Tin (II) Fe2+ Iron (II) Cu2+ Copper (II) Pb4+ Lead (IV) Cu+ Copper (I) Pb2+ Lead (II) Co3+ Cobalt (III) Co2+ Cobalt (II)

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