Download presentation
Presentation is loading. Please wait.
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 Compounds
1+ 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
Similar presentations
© 2024 SlidePlayer.com Inc.
All rights reserved.