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(prefix) Deca: (# of atoms) 10
(Prefix) Di: (# of atoms) 2
(prefix) Hepta: (# of atoms) 7
(prefix) Hexa: (# of atoms) 6
(prefix) Nona: (# of atoms) 9
(prefix) Octa: (# of atoms) 8
(prefix) Penta: (# of atoms) 5
(prefix) Tetra: (# of atoms) 4
(prefix) Tri: (# of atoms) 3
Angular <120*: 2 bonded atoms and 1 non bonded e- pair
Angular roughly 104.5*: 2 bonded atoms and 2 non bonded e- pairs
C2H5OH: Ethanol (formula)
C6H12O6: Glucose (formula)
Covalent Bonding: Shared electrons to complete an octet. Tend to bond between atoms of similar tendencies.
Dipole: One pole is more negative the other more positive. They are separated and aligned with the field.
Electrolytes: Soluble will will form positive and negative ions in solution by dissociation. Electrical Conductors.
Electronegativity: A measure of the ability of an atom to attract e- in a chemical bond. Higher En has more of a chance to attract than Low En. Higher is at top right of table, lower bottom left.
Exceptions to the octet rule: 1. Some molecules don't have 8 e- 2. Some molecules have an expanded octet.
Features of Ionic Bonds: 1. Atoms of elements with low Ionization energy and low electron affinity form positive ions. 2. Atoms of elements with high ion ionization energies and high e- affinities form negative ions. 3. Ion formation takes place by e- transfer. 4. The positive and negative are held together by the electrostatic force between ions of opposite charge in an ionic bond. 5.Reactions between metals and nonmetals tend to result in an ionic bond.
H20: Water (formula)
High e- Affinity: Readily accepts an e-
High Ionization Energy: Won't easily give up an e-
Inter Molecular Forces: Forces between molecules determine the solubility, freezing and boiling point.
Intra molecular Forces: Attractive forces within the molecules and are chemical vonds that determine the shape and polarity of individual molecules.
Ionic Bond: The transfer of electrons from ions of opposite charges that are attracted to each other.
Ions: Atoms with charges (negative-anion) (positive-cation)
Linear 180*: 2 bonded atoms, and 0 non bonded e- pairs
Low e- Affinity: Doesn't want anymore e-
Low Ionization Energy: Readily loses an e-
Molecular structure: The geometry of a molecule is affected by the number of non bonded e- pairs around the central atom and by the number of bonded pairs.
Molecular structures: 1. Linear 2. Trigonal Planar 3. Angular 4. Tetrahedral 5. Trigonal Pyramidal 6. Angular
Monatomic ions: ions consisting of a single atom
Negative ion Characteristics: 1. Located on the right of table 2. Nonmetals 3. Have high ionization energies and high e- affinities
NH3: ammonia (formula)
Nonelectrolytes: Dissolve in solution usually retain their neutral character. Not electrical conductors.
Polar Covalent Bond: A bond made up of unequally shared e- because of; partial e- transfer, the bond having both ionic and covalent properties, and unequally e- density.
Polar molecule: If it's center of positive and negative charges don't coincide. No dipoles exist and their charges are the same.
Polyatomic ions: Composed of two or more atoms bonded together
Positive ion Characteristics: 1. located on the left of the table 2. Metals 3. Low ionization energy and low e- affinity.
Resonance: When a compound has two or more Lewis structures that contribute to the real structure it displays the property.
Solubility: The maximum amount of solute that disolves in a given amount of solvent at a specified temperature. "likes dissolve likes""
Tetrahedral Roughly 109*: 4 bonded atoms and 0 non bonded e- pairs
Trigonal Planar 120*: 3 bonded atoms and 0 non bonded e- pairs
Trigonal Pyramidal roughly 107*: 3 bonded atoms and 1 non bonded e- pair
Writing names of compounds: First the cation, followed by the anion with the suffix of ide