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OAT - Chem
Chapter 3 - Bonding and Chemical Interactions
| Term | Definition |
|---|---|
| these bind together to make molecules | atoms |
| chemical bonds | intramolecular strong bond |
| intermolecular forces | weaker force |
| Octet Rule | atoms tend to bond with other atoms until it has 8 electrons in outermost shell to become stable like Nobles |
| What the octet rule doesn't apply to | Hydrogen |
| Ionic Bonding | e- transferred from atom with low IE to atom with high electron affinity; electrostatic forces |
| Covalent Bonding | electrons are shared btwn 2 atoms; can be single double or triple |
| Polar Covalent Bonding | partially covalent and partially ionic bonding |
| Cation | loses e- and becomes |
| Anion | gains e- and becomes |
| Bond Order | number of shared electrons between atoms (1,2,3 for single double triple) |
| Bond Length | avg distance btwn the 2 nuclei of atoms involved; the more e- shared, the shorter the BL |
| Bond E | E required to separate 2 atoms |
| bonding electrons | shared e- of covalent bond |
| nonbonding electrons | e- not involved in covalent bond |
| lone e- pairs | unshared e- pairs |
| Lewis Structure | chemical symbol of an element surrounded by dots, each representing a valence e- |
| Steps to Lewis Structure | 1. draw skeletal structure, least electronegative in middle, halogens and hydrogen on ends 2. Count up the valence electrons 3. complete octets 4. Shared e- are lines, lone pairs are dots |
| Formal Charges | V-1/2bonding-nonbonding; or if it is missing a valence e- then +1 and vice versa |
| Resonance | two or more nonidentical Lewis structures for a molecule |
| Resonance Hybrid | the actual molecule is a mix of the resonance structures |
| Polar Covalent Bond | like HCL and H2O, partially ionic character |
| NonPolar Covalent Bond | H2, Cl2, O2 |
| Lewis Acid | can accept electrons to form covalent bond |
| Lewis Base | can donate lone pair of electrons to form covalent bond |
| VSEPR determines | geometry of molecules |
| Linear | 2 regions of electron density, 180 degrees |
| Trigonal Planar | 3 regions of electron density, 120 degrees |
| Tetrahedral | 4 regions of electron density, 109.5 degrees |
| Trigonal Bipyramidal | 5 regions of electron density, 180-120-90 degrees |
| Octahedral | 6 regions of electron density, 180-90 degrees |
| Axial | elements up and down |
| Equitorial | elements on "equator" of molecules surrounding central atom |
| 1 lone pair on a trigonal planar molecule | bent shape |
| 1 lone pair on tetrahedral molecule | trigonal pyramid |
| 2 lone pairs on tetrahedral molecule | bent shape |
| 1 lone pair on trigonal bipyramid | Seesaw shape |
| 2 lone pairs on trigonal bipyramid | T-shape |
| 3 lone pairs on trigonal bipyramid | linear |
| 1 lone pair on octahedral | square pyramid |
| 2 lone pairs on octahedral | square planar |
| 3 lone pairs on octahedral | T-shape |
| 4 lone pairs on octahedral | linear |
| A polar bonding molecule must have what to be polar | net dipole moment or else it is nonpolar |
| l = 0, 1, 2, 3 | s, p, d, f |
| m | +l to -l |
| s | sphere shape |
| p | peanut shape |
| when orbitals have same sign | bonding orbitals |
| when orbitals have opposite signs | nonbonding orbitals |
| when orbitals overlap head to head | sigma bond |
| when orbitals overlap parallel | pi bond |
| Dipole-Dipole Interaction | when 2 polar molecules come into close contact with each other; pos of one close to neg of other |
| H-Bonding | F O N; strongest |
| Dispersion Forces | short-lived dipoles; large molecules have greater forces, also London Force |
Created by:
JaeBae4444
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