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Class Notes : From Atom to ION

Class Notes : From Atom to ION. Essential Question :. How does the atomic structure affect chemical bonding?. Ions. Ions are atoms which have gained or lost one or more valence electrons giving the ion a net positive or negative charge . Ions occurs with a metal and a nonmetal atom.

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Class Notes : From Atom to ION

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  1. Class Notes: From Atom to ION

  2. Essential Question: How does the atomic structure affect chemical bonding?

  3. Ions • Ions are atoms which have gained or lost one or more valence electrons giving the ion a net positive or negative charge. • Ions occurs with a metal and a nonmetal atom. • The attraction between the positives and negatives brings the particles together and creates an ionic compound.

  4. Cations Let’s look at Mg Positive Ion 12 protons 10 electrons Neutral Atom 12 protons 12 electrons Metal : lose 1 or more e- to formpositive (+) ionscalled cations.

  5. Cation Positively charged ion – which means the atom has more protons than electrons

  6. Cations: (+) ions Metals form (+) ions • Na & Na+{sodium atom & sodium ion} • Atom: Na {11p+, 11 e-, 12 n} • Ion: Na+{11p+, 10e-, 12 n}

  7. Anions Ions Nonmetals:gain 1 or more e- to form negative(-) ions called anions. Neutral Atom 17 protons 17 electrons Chloride Ion 17 protons 18 electrons

  8. Anion Negatively charged ion – which means the atom has more electrons than protons

  9. Anions: (-) ions NonMetalsform(-) ions • F & F- { fluorine atom, fluorideion} • Atom: F {9p+, 9 e-, 10 n0, mass # 19} • Ion: F- {9p+, 10e-, 10 n0, mass # 19}

  10. Predicting Oxidation Charges Group 1: Lose 1 electron to form 1+ ions H+ Li+ Na+ K+

  11. Predicting OxidationCharges Group 2: Loses 2 electrons to form 2+ ions Be2+ Mg2+ Ca2+ Ba2+ Sr2+

  12. Predicting OxidationCharges Group 13: Loses 3 electrons to form 3+ ions B3+ Al3+ Ga3+

  13. Predicting OxidationCharges Group 14: Lose 4 electrons or gain 4 electrons? Neither! Group 14 elements rarely forms ions.

  14. Predicting Oxidation Charges Group 15: Gains 3 electrons to form 3- ions N3- Nitride P3- Phosphide As3- Arsenide

  15. Predicting Oxidation Charges Group 16: Gains 2 electrons to form 2- ions Oxide O2- S2- Sulfide Se2- Selenide

  16. Predicting Oxidation Charges Gains 1 electron to form 1- ions F1- Group 17: Fluoride Br1- Bromide Cl1- Chloride I1- Iodide

  17. Predicting OxidationCharges Group 18: Stable Noble gases do not form ions!

  18. Predicting Oxidation Charges Groups 3 - 12: Many transition elements have more than one possible oxidation state. Iron(II) = Fe2+ Iron(III) = Fe3+ Roman Number states the oxidation charge for the transitional metals Iron(II) = Fe2+

  19. Predicting OxidationCharges Groups 3 - 12: Some transition elements have only one possible oxidation state. Zinc = Zn2+ Silver = Ag+

  20. Ions Ion Oxidation Charges and the Periodic Table • Group 1 form 1+cations • Group 2 : form 2+ cations. • Groups 3 to 12 form 1+ or more cations (use the Roman Numerals) • Group 13: form 3 +cations • Group 15 : form anions , 3- ions • Group 16 : form anions , 2- ions • Group 17 : form anions , 1- ions • Group 18: no charges, do not form ions easily.

  21. Comprehension Check! Define an ion. Define an cation. Define an anion. Explain what metals do with their valence electrons? Explain what nonmetals do with their valence electrons? Explain what is the oxidation charges/number.

  22. Cations: (+) ions Be & Be 2+{beryllium atom & beryllium ion} • Atom: Be {4p+, 4 e-, 5 n, mass # 9} • Ion: Be 2+{4p+, 2 e-, 5 n, mass # 9} • Oxidation Number Practice: • K Mg Al BCSi + 2+ 3+ 3+ 4+ 4+

  23. Anions: (-) ions. • S & S 2-{sulfur atom, sulfideion} • Atom: S {16p+, 16 e-, 16 n0, mass # 32} • Ion: S 2- {16p+, 18e-, 16 n0, mass # 32} • Oxidation Number Practice: • P O N As Se Cl - 2- 3- 3- - 2-

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