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Chapter 12 Exam 5

QuestionAnswer
Bond Force that holds groups of 2 or more atoms together. They work as an unit
Bond Energy Energy needed to break the bond
* Ionic Bonding Attraction of opposites (anions and cations)
Ionic Compound Metal attracted to non metal
* Covalent Bonding Electrons are shared by nuclei to form molecules. Ex H molecule
* Polar Covalent Bond Electrons are not shared equally Atoms are not so different that e- are completely transferred but are different enough to share unequaly. Ex HF
* Electronegativity Ability of an atom in a molecule to attract electrons in a chemical bond.
Dipole moment Molecule that has a center of + & a center of - charge
Principle All atoms of stable chemical compounds of rep elements achieve a noble gas electron configuration.
* Lewis Structure shows the bonds between atoms. 1. Add all valence e- 2. Divide by 2 (pairs) 3. Surround central atom with 4 e- pair 4. Remaining e- complete the octet 5. Two exceptions H (only needs 2 e-/ B only needs 6 e-)
Duet Rule Sharing of 2 e-
* Octec Rule (one 2s & three 2p orbitals) e- are needed to fill the orbitals
* Bonding electrons Electron pairs are shared by atoms
* Non bonding electrons The 3 other pairs of e- that are not shared
* Single Bond 2 atoms share 1 e- pair
Double Bond 2 atoms share 2 e- pairs
Triple Bond 2 atoms share 3 e- pairs
* Resonance More than one Lewis structure can be drawn for a molecule.
* Molecular Structure 3D arrangement of atoms around a central atom due to electron repulsion
* Linear Structure All atoms in a line. Ex CO2 180 bond angles
* Triagonal Planar Structure 120 bond angles
* Tetrahedral Structure Four identical triangular faces (4 bonding pairs and the atoms are repelled to the 4 corners)
* Valence shell electron pair repulsion (VSEPR)model Electron pairs surrounding an atom repel each other
* Trigonal Pyramid One side is different from the other 3 (3 bonding pairs and 1 nonbonding pair)
* Cation Positively charged (loses e-)
* Anion Negatively charged (gains e-)
* Non Polar Covalent Bond Bond is not polarized. Difference is less than 0.5 (electronegative difference)
* Delta notation Used to state the charge on polar bonds
* Coordinate Covalent Bond One atom gives a lone pair of e- to another atom
* Hydrogen Bond Intermolecular attraction. Like H attracted to O in a water molecule
* Electron dot formula Symbol of an element surrounded by its valence e-
* Electron pair geometry Shows the arrangement of bonding and nonbonding e- pairs around the central atom
* Bond Lenght The distance bt the 2 atoms is smaller than the sum of ther atomic radii
* Bond energy Energy needed to break a covalent bond
* Structural Formula Uses dashes to show bonding
Created by: lesliemelissa19
 

 



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