Unstable

1. Chlorine – 35 (neutral) Argon – 40 (neutral) Chlorine – 35 (Charge = 1-) e-= _18-_ e-= _17-_ e-= _18-_ Cl Cl Ar 2 8 8 8 2 8 7 8 2 P+ = _18+__ N0 = _22__ P+ = _17+__ N0 = _18__ P+ = _17+__ N0 = _18__ 1 1 1 2 2 2 3 3 3 Atomic # _18_ Mass # _40_ Atomic # _17_ Mass # _35_ Atomic # _17_ Mass # _35_ Octet Rule - Atoms bond together so that each atom attains a full valence shell (8 Ve-) or (2 Ve-) ***Atoms react so as to acquire the STABLE electron structure of a noble gas.– (Full Valence =Stable) Review Cl1- Review Unstable Stable Stable

2. Formation of Cations Na1+ + Na  e- Lose 1 e- Mg2+ + Mg  e- e- Lose 2 e- Metals willlosevalence electrons to form positive cations.

3. Metals will lose electrons to form cations (+) 1+ 2+ Be – 2, 2 Mg – 2, 8, 2 Ca – 2, 8, 8, 2 Sr – 2, 8, 18, 8, 2 Ba- 2, 8, 18, 18, 8, 2 Ra-2,8,18,32,18,8,2 Cations of Group 1A elements always have a charge of 1+ Group2A = 2+ Group 3A = 3+ (Metals)

4. 3+ 3- 2- 1- 1+ 2+ Naming Metals - 1A, 2A, 3A Name of the Atom = Name of Cation Lithium ( Li ) = ( Li1+ ) Lithium Ion Magnesium ( Mg ) = ( Mg2+ ) Magnesium Ion Aluminum ( Al ) = ( Al3+ ) Aluminum Ion Transition Metals

5. Non-Metals gain electrons to form anions (-) 3- 2- 1- Formation of Anions F – 2, 7 Cl – 2, 8, 7 Br – 2, 8, 18, 7 I – 2, 8, 18, 18, 7 Anions of Group 5A = charge of 3- Group 6A = 2- Group 7A = 1- (Non-Metals) (Metalloids)

6. 3+ 3- 2- 1- 1+ 2+ • All anions end in -ide Nonmetals - 5A, 6A, 7A) Name of the Atom = Name of Anion w/ - ide ending • Metals in Group 4A and 5A will always LOSE electrons to form cations (+) • Sn2+,Sn4+,Pb2+, Pb4+, Bi3+ Nitrogen ( N ) = ( N3- ) Nitride Oxygen ( O ) = ( O2- ) Oxide Chlorine ( Cl ) = ( Cl1- ) Chloride Transition Metals

7. 3+ 3- 2- 1- 1+ 2+ Naming Ionic Compounds • All anions (non-metals) end in -ide Transition Metals

8. 3+ 3- 2- 1- 1+ 2+ Transition Metals – Ions can have more than one charge Charge of Cation = Roman Numeral in Name Fe2+ = Iron (II) Fe3+ = Iron (III) Cu1+ = Copper (I) Cu2+ = Copper (II) Pb2+ = Lead (II) Pb4+ = Lead (IV) Transition Metals

9. 3+ 3- 2- 1- 1+ 2+ Naming Ionic Compounds Transition Metals

10. NO3- Sulfide 1- • nitrate 2- • NOTE: I have made changes to your copy

11. Cl Al S P K Ar Ca QUESTION – If metals lose electrons & non-metalsgain electrons, Where do these electrons come from or go to? P 3- Ar Al3+ K 1+ Cl1- S 2- Ca2+ QUESTION – What makes an atom stable? ANSWER – Having a completely filled outer energy level of electrons –Full Octet (2 e- H, He, Li, Be)

12. O Mg Cl O Ionic Bonding = Transfer of electrons (Gaining or Losing e-) (Forming IONS) Lose 1 e- Gain 1 e- Lose 2 e- Gain 2 e- Ionic Bonding typically occurs between a metal cation (+) and a nonmetal anion (-) due to a transfer of electrons --- has a net charge of ZERO Cl Na Na Mg Mg 2+ O2- Cl- Na+ ( MagnesiumOxide - MgO) ( SodiumChloride - NaCl) ( Metal + Nonmetal ) ( Metal + Nonmetal ) Ionic Bonding typically occurs between a metal cation (+) and anonmetal anion (-) due to a transfer of electrons --- has a net charge of ZERO

13. S S K K Ca Lose 2 e- Lose 1 e- Gain 2 e- Gain 2 e- S2- Ca 2+ S2- 2K1+ ( PotassiumSulfide – K2S ) ( CalciumSulfide – CaS ) ( Metal + Nonmetal ) ( Metal + Nonmetal ) 2(1+) + (2-) = zero (2+) + (2-) = zero (2+) + (2-) = zero Ionic Compounds have a net charge of zero

14. Ionic Compounds have a net charge of zero NaBr Li2O 2Li1+ Na+ O2- Br - 2(1+) + (2-) = zero (1+) + (1-) = zero MgBr2 Al2S3 2Al3+ Mg2+ 3S2- 2Br - 2(3+) + 3(2-) = zero (2+) + 2(1-) = zero (6+) + (6-) = zero

15. Subscripts2 = more than one MONOATOMIC ion No subscript= only ONE atom/ion

16. The “4” is part of the ion NH41+ The “3” is part of the ion CO32- NH4 = One polyatomic ion - no subscript (NH4 )2 = Two polyatomic ions - subscript (parenthesis)2 are used when there is more than one POLYATOMIC ION

17. - - - + + + Ionic Bonding - the electrostatic attraction (Force) that binds oppositely chargedions (cations (+) &anions (-))together Electrostatic FORCE between the charges causes the attraction & repulsion

18. Ionic Bonding - the electrostatic FORCE that holds cations and anions together Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Crystal Lattice – Orderly, repeating, three dimensional pattern of ions (cations/anions) *NOTE: All ionic solids form a crystal lattice -- Atoms, ions, and molecules can form a crystal (crystal lattice)

19. Sodium - 23 (neutral) Chlorine – 35 (neutral) e-= _11-_ e-= _17-_ 8 8 7 1 2 2 P+ = _17+__ N0 = _18__ P+ = _11+__ N0 = _12__ 1 1 2 2 3 3 Atomic # _11_ Mass # _23_ Atomic # _17_ Mass # _35_ Chlorine, Cl2 Sodium Chloride, NaCl Table Salt + = = + Chlorine Gas is poisonous - The German Army first used chlorine gas cylinders in April 1915 against the French Army. French soldiers reported seeing yellow-green clouds drifting slowly towards the Allied trenches. They also noticed its distinctive smell which was like a mixture of pineapple and pepper. When the gas arrived at the Allied front-trenches soldiers began to complain about pains in the chests and a burning sensation in their throats. Chlorine gas destroyed the respiratory organs of its victims and this led to a slow DEATH by asphyxiation

20. 1. How many valence electrons are there in an atom of oxygen? a) 2 b) 4 c) 6 d) 8

21. 7.1 Section Quiz. 2. Atoms that tend to gain a noble gas configuration by losing valence electrons are a) metals. b) nonmetals. c) noble gases. d) representative elements.

22. 3. When a magnesium atom forms a cation, it does so by a) losing two electrons. b) gaining two electrons. c) losing one electron. d) gaining one electron.

23. 4. When a bromine atom forms an anion, it does so by a) losing two electrons. b) gaining two electrons. c) losing one electron. d) gaining one electron