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Formal charge

AP Chemistry Zumdahl 7E Chapter 8 Notes

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Chemistry
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Chemical bonding
Chemical bond
Octet rule
Lewis structure
Ionic bonding
Covalent bond
Resonance
Chemistry
Valence electron
Valence
Formal charge
VSEPR theory

AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy (greater stability) than separated ions B. Coulomb's Law 1. ? ? ? ? ? ? ? ? ?= - r QQ E nmJx 21191031.2 a. E = energy in joules b. Q1 and Q2 are numerical ion charges c. r = distance between ion center in nanometers d. negative sign indicates an attractive force C. Bond Length (covalent) 1. Distance at which the system energy is at a minimum 2. Forces at work a. Attractive forces (proton - electron) b. Repulsive forces (electron - electron, proton - proton) 3. Energy is given off (bond energy) when two atoms achieve greater stability together than apart

Chapter 8

Subject: 
Chemistry
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Chemistry
Chemical bonding
Chemical bond
Valence electron
Lewis structure
Octet rule
Covalent bond
Ionic bond
Hydrogen bond
Lone pair
Formal charge
electron
Technology

Claire Rafson Chapter 8 Notes 8.1- Bond Energy- The strength of a bonding interaction. The energy required to break the bond. Why do bonds occur? So the system can achieve the lowest possible energy by behaving in this way. Ionic bonding- electrostatic attractions of the closely packed, oppositiyly charged ions. Ionic compound- Metal reacts with a nonmetal Coulombs law- interaction between pair of ions. E= (2.31X 10^-19 J* nm) (Q1Q2/r) A bond will form if the energy of the aggregate is lower than that of the separated atoms. Covalent bonds- type of bonding in which electrons are shared by nuclei. (i.e Hydrogen bonding) Polar Covalent Bond- Atoms are different enough that they have unequal sharing results. 8.2-
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