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Chapter 12 Exam 5
| Question | Answer |
|---|---|
| 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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