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Chemistry 161
Chapter 6
| Term | Definition |
|---|---|
| Octet Rule | Atoms will gain, lose or share electrons in order to achieve a noble gas electron configuration |
| Lone pair | Pair of valence electrons that are not involved in covalent bond formation |
| Single Bond | A par of electrons shared by two atoms |
| Multiple bond | A chemical bond in which two atoms share two or more pair of electrons |
| Double bond | A multiple bond in which the atoms share two pair of electrons |
| Triple bond | A multiple bond in which the atoms share three pairs of electrons |
| Enthalpy | A thermodynamic quantity closely related to energy |
| Central atom | An atom that is bonded to more than one atom |
| Polar | Electrons are shared but not shared equally |
| Polar covalent bonds | Bonds in which electrons are unequally shared |
| Electronegativity | The ability of an atom to attract an electron pair in a covalent bond to itself (increases across a period, decreases down a group)*similar to atomic radius trend |
| Low electronegativity | Formation of cations |
| High electronegativity | Formation of anions |
| Nonpolar | Having a uniform distribution of electron density. Bonds between atoms whose electronegativities differ by less than 0.5 =purely covalent/nonpolar |
| Polar covalent | Bonds between atoms whose electronegativities range of 0.5-2.0 |
| Ionic bonds | Bonds between atoms whose electronegativity differ by 2.0 or more |
| Dipole moment (μ) | Quantitative measurement of the polarity of a bond. μ= charge (Q) x distance (r) between charges |
| Formal charge | Method of electron "bookkeeping" in which shared electrons are divided equally between that atoms that share them |
| Resonance structure | Two or more equally valid Lewis structures for a single molecule that differ only in electron positions |
| Incomplete octet | Atoms with less than 4 valence electrons |
| Octet expansion | When more than eight electrons can be accommodated around the central atom. For 3rd period elements and above. (D orbitals) |
| Coordinate covalent bond/Dative bond | Bond in which one of the atoms donates both electrons |
| Molecules with ODD number of electrons | When total number of electrons is odd, not all the atoms will have complete octets, and there must be an UNPAIRED electron in the molecule |
| Free radicals | Molecules (species) with an odd number of electrons. Very reactive |
| Bond length | Distance between the nuclei of two atoms joined by a covalent bond |
| Atomic size | As atomic size increases bond length increases |
| Bond strength | The shorter the bond length the the stronger the bond strength |
Created by:
cynthiaf1021
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