chapter 4 atoms and chemical bonding chapter 7 ionic and metallic bonding
TRANSCRIPT
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Chapter 4
Atoms and Chemical Bonding
Chapter 7Ionic and Metallic Bonding
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Valence Electrons
• Highest energy level
• Determine chemical properties
• [Ne]4s2 3d10 4p5 - Bromine
7 valence e-
Representative elements = group #
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Valence ElectronsLewis (1916)
Valence electrons are the electrons in the atom’s highest numbered energy level.
1 2 3 4 5 6 7 8
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Electron dot Structures
• Lewis dot
• Show electrons as dots •
• Ca• •B•
• Fill in each side with one dot before you double up
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Octet Rule
In forming compounds atoms gain, lose, or sharein such a way that they achieve the electron configuration of the
nearest noble gas in the periodic table.Noble gases are stable
have eight electrons in the outermost level
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Ionic Bonding Atoms lose or gain electrons to form ions
Cations are positive ions metals generally form cations
Anions are negative ions non-metals generally form anions
Ionic compounds are held together by electrostatics- the positive charge of the cation attracting the negative charge of the anion.
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Ionic Bonding Continued
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Ionic Compound METAL + NONMETAL Important metal ions
group 1A - loose 1 electron (+1) group 2A - loose 2 electrons (+2) group 3A - loose 3 electrons (+3)
Important non-metal ions group 7A (-1), group 6A (-2), group 5A (-3)
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Properties of Ionic bonds
• Most are crystalline solids at Room temp
Stable structures with all of the (+) and (-) attractions
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Properties cont.
Stable structures with all of the (+) and (-) attractions
• High melting points
• Conduct electricity – Ions move freely so e- can travel toward (+)– When dissolved in water
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Ionic Bonds
• One cation and one anion
• Electrically neutral
• Cation gives e-
• Anion takes e-– Example Aluminum and bromine
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Common Ions and Their Position in the Periodic Table
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Lewis Structures
• Al • •Cl•
Cl
Cl
[Al] [Cl]3
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Names of Common Nonmetallic Ions
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Polyatomic IonsPolyatomic means “many-atom” ion
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Metallic bonds
• Closely packed cations
• Valence e- are free and can drift from one metal to another
• Meallic bonds consist of the attraction of ther free-floating valence e- for the positively charged metal ions
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Metallic bonds (e-)
• they do not "belong" to any one atom • are part of the whole metal crystal • *Metallic bonds are best characterized by the
phrase "a sea of electrons"*
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Metallic properties
• electrons flow explains characteristics of metals:• - Metals are good conductors of heat and electricity.
– mobility of the electrons.• - The "cement" effect of the electrons determines the
hardness Some• - Metals are lustrous.
– due to the uniform way that the valence electrons absorb and re-emit light energy.
• - Metals are malleable (can be flattened) and ductile (can be drawn into wires) – because the metal cations and electrons can "flow" around each
other, without breaking the crystal structure.
http://www.ithacasciencezone.com/chemzone/lessons/03bonding/mleebonding/metallicbonding.htm
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Alloys
• Mixture of two or more elements, at least one is a metal
• Example: brass = copper and zinc• Properies are better than those of the single
elements• Sterling silver = siler and copper
– Durable /no tarnishSteel is a very important alloy
iron, carbon, boron, chromium, manganese, and more