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Chapter 15

Chapter 15. Ionic Bonding. Valence Electrons. Do the electron configuration for the following elements Li Be B O F Ne. Valence Electrons. Now look at the outermost electrons by looking at the last s and p orbital Circle and count these electrons These are the valence electrons.

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Chapter 15

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  1. Chapter 15 Ionic Bonding

  2. Valence Electrons • Do the electron configuration for the following elements • Li • Be • B • O • F • Ne

  3. Valence Electrons • Now look at the outermost electrons by looking at the last s and p orbital • Circle and count these electrons • These are the valence electrons

  4. Valence electrons • Valence electrons are in the highest energy level of an element’s atom • Valence electrons are the same as group # (roman numeral) for the group A representative elements • Valence electrons are usually the only electrons used in chemical bonds • We use valence e- to write Lewis Dot Structures

  5. Valence electrons (cont.) A. Lewis Dot Structure Ex: bromine ● ● Br ● ● ● ● ●

  6. Electron configurations for cations & anions A. Octet Rule: when forming compounds atoms want to have 8 electrons (s2p6) like the noble gases (except He)

  7. Cations(metals)tend to lose electrons,positively charged ion + lose 1 e- Na (atom) Na (cation) 1s22s22p63s1 1s22s22p6 octet Using the Dot Structure + ● lose 1 e- Na (cation) Na (neutral atom) 2+ ● Mg (cation) lose 2 e- Mg (neutral atom) ●

  8. Anions(Nonmetals) have negative charges because they gain electrons - gain 1 e- Cl (atom) Cl (chloride ion) 1s22s22p63s23p5 1s22s22p63s23p6 valence octet Using the Dot Structure - ● ● ● ● gain 1 e- Cl (chloride ion) Cl (neutral atom) ● ● ● ● ● ● ● ● ● ● ● 2- ● ● ● ● gain 2e- O (oxide ion) O (neutral atom) ● ● ● ● ● ● ● ● ● ●

  9. Practice N 3- ● ● ● ● gain 3e- N (nitride ion) ● ● ● ● ● ● ● ● ● + Lose 1 e- ● Li Li - ● ● ● ● I (iodide ion) gain 1 e- I ● ● ● ● ● ● ● ● ● ● ● +2 ● Ca Lose 2e- Ca ●

  10. Ionic Compound 1. ionic compounds form crystals 2. high melting and boiling points 3. hard and brittle 4. conduct electricity when dissolved in water or melted • Composed of a metal (cation) and nonmetal (anion) • Ionic bond – oppositely charged ions attract • Electrically neutral (+) = (-) A. Properties

  11. Ionic Bonds Na +1 -1 1. Sodium and Chlorine - ● ● ● ● donates e- Na+ Cl ● Cl ● ● ● + ● ● ● ● ● ● ● ● NaCl +1 -2 2. Potassium and Oxygen ● donates e- K K+ -2 ● ● O ● ● ● ● + O ● ● ● ● ● donates e- ● ● K+ ● ● K K2O

  12. AlBr3 +3 -1 3. Aluminum and Bromine - ● ● Br ● ● ● Br ● ● ● ● ● ● ● ● Al ● ● - ● Al+3 ● ● ● ● Br Br + ● ● ● ● ● ● ● ● ● ● ● ● ● - ● ● Br ● ● ● Br ● ● ● ● ● ● ● ● ● ● +2 -3 4. Magnesium and Nitrogen Mg+2 -3 ● ● ● Mg ● ● N N ● ● ● ● ● ● ● Mg+2 ● ● ● -3 + ● ● ● N Mg ● ● ● ● ● ● Mg+2 ● N ● ● ● ● ● Mg ● ● Mg3N2

  13. OUTPUT EXAMPLE: 1. Potassium & Fluorine +1 -1 ● ● ● - ● ● + F K F + K ● ● ● ● ● ● ● ● ● ● ● KF

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