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 |