1. Review Review Cl1- Unstable Stable Stable
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- Cl Cl Ar
Review
Atomic # _17_ Mass # _35_
Chlorine – (neutral)
P+ = _17+__
N0 = _18__ 1 2 3
e- = _17-_ 8 7
Atomic # _17_ Mass # _35_
Chlorine – (Charge = 1-)
P+ = _17+__
N0 = _18__ 1 2 3
e- = _18-_ 8
Atomic # _18_ Mass # _40_
Argon – (neutral)
P+ = _18+__
N0 = _22__ 1 2 3
e- = _18-_ 8
Unstable
Stable
Stable

2. Formation of Cations Na  Na
Lose 1 e- Mg  Mg
Lose 2 e-

3. Metals lose electrons to form cations (+)
New Notes
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+
Group 2A = 2+
Group 3A = 3+
Cations of Group 1A elements have a charge of 1+. Cations of Group 2A elements have a charge of 2+.
(Metals)

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

5. Non-Metals gain electrons to form anions (-)
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-
Atoms of nonmetals and metalloids form anions by gaining enough valence electrons to attain the electron configuration of the nearest noble gas. Interpreting Diagrams In which group of the periodic table do the elements bromine and iodine belong?
(Non-Metals)
(Metalloids)

6. Nonmetals - 5A, 6A, 7A)
All anions end in -ide
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 1+ 2+ 3+ 3- 2- 1-
Transition Metals

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

8. Transition Metals Charge of Cation = Roman Numeral in Name
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) 1+ 2+ 3+ 3- 2- 1-
Transition Metals

9. Naming Ionic Compounds1+ 2+ 3+ 3- 2- 1-
Transition Metals

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

11. QUESTION – What makes an atom stable?
QUESTION – If metals lose electrons and non-metals gain electrons, Where do these electrons come from or go to? P Ar Al K Cl S Ca
P 3- Ar
Al 3+
K 1+
Cl 1-
S 2-
Ca 2+
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. Ionic Bonding = Transfer of electrons
(Gaining or Losing e-)
(Forming IONS)
Ionic Bonding typically occurs between a metal cation (+) and a nonmetal anion (-) due to a transfer of electrons --- has a net charge of ZERO
Lose 1 e-
Gain 1 e-
Lose 2 e-
Gain 2 e- Na Cl Mg O Na Cl Mg O
Na+
Cl-
Mg 2+
O 2-
( Sodium Chloride - NaCl )
( Magnesium Oxide - MgO )
( Metal + Nonmetal )
( Metal + Nonmetal )
Ionic Bonding typically occurs between a metal cation (+) and a nonmetal anion (-) due to a transfer of electrons --- has a net charge of ZERO

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

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

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

16. NH4 = One polyatomic ion - no subscript
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 charged ions (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-
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)
Cl-
Cl-
Na+
Na+
Cl-
Cl-
Na+
Na+
Cl-
Cl-
Na+
Na+

19. + = = + Chlorine, Cl2 Sodium Chloride, NaCl 8 8 7
Table Salt + =
Atomic # _11_ Mass # _23_
Sodium (neutral)
P+ = _11+__
N0 = _12__ 1 2 3
e- = _11-_ 8
Atomic # _17_ Mass # _35_
Chlorine – (neutral)
P+ = _17+__
N0 = _18__ 1 2 3
e- = _17-_ 8 7 = +
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?
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