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MCAT Gen. Chem Ch. 3
Term | Definition |
---|---|
Octet Rule | Elements will be most stable with eight valence electrons. |
Elements With An Incomplete Octet And Are Stable: | H, He, Li, Be, and B |
Elements With An Expanded Octet And Are Stable: | Elements in Period 3 or greater |
Compounds With An Odd Number Of Electrons Cannot Have: | Eight electrons on each element |
Ionic Bond | Formed via the transfer of one or more electrons form an element with a relatively-low ionization energy to an element with a relatively high electron affinity |
Ionic Bonds Occur Between Elements With: | Large electronegativity (Delta EN > 1.7). This occurs usually between metals and nonmetals. |
Cation | Positively charged ion |
Anion | Negatively charged ion. |
Crystalline Lattices | Formed by ionic compounds. These are large, organized arrays of ions. |
Ionic Compounds Have Unique: | Physical and chemical properties. |
Ionic Compounds Tend To: | Dissociate in water and other polar solvents. |
Ionic Solids Tend To: | Have high melting points. |
Covalent Bond | Formed via the sharing of electrons between two elements of similar electronegativities. |
Bond Order | Refers to whether a covalent bond is a single bond, double bond, or triple bond. |
As Bond Order Increases: | Bond strength increases, bond energy increases, and bond length decreases. |
Covalent Bonds Can Be Categorized As: | Nonpolar or polar depending on the nature of the elements involved |
Nonpolar Bonds | Result in molecules in which both atoms have exactly the same electronegativity. |
Some Bonds Are Considered Nonpolar When: | There is a small difference in electronegativity between the atoms (Delta EN < 0.5) |
Polar Bonds | Form when there is a sig. difference in electronegativities (Delta EN = 0.5 to 1.7) but not enough to transfer electrons and form an ionic bond. |
In A Polar Bond, The More Electronegative Element Takes On: | A partial negative charge |
In A Polar Bond, The Less Electronegative Element Takes On: | A partial positive charge |
Coordinate Covalent Bonds | Result when a single atom provides both bonding electrons while the other atom does not contribute any |
Coordinate Covalent Bonds Are Most Often Found In: | Lewis acid-base chemistry. |
Lewis Dot Symbols | Chemical representation of an atom's valence electrons |
Formal Charges | Exist when an atom is surrounded by more or fewer valence electrons than it has in its neutral state |
Resonant Structures | Represent all of the possible configurations of electrons (stable and unstable) that contribute to the overall structure |
Valence Shell Electron Pair Repulsion (VSEPR) Theory | Predicts the 3-D molecular geometry of covalently bonded molecules |
Nonbonding Electrons Exert More Repulsion Than Bonding Electrons Because: | They reside closer to the nucleus. |
Electronic Geometry | Position of all electrons in a molecule, whether bonding or nonbonding. |
Molecular Geometry | Refers to the position of only the bonding pairs of electrons in a molecule. |
Polarity Of Molecules | Dependent on the dipole moment of each bond and the sum of the dipole moments in a molecular structure. |
Nonpolar Molecules May Contain: | Nonpolar bonds, or polar bonds with dipole moments that cancel each other |
Sigma Bonds | Result of head-to-head bond overlap. |
Pi Bonds | Result of the overlap of two parallel electron cloud densities. |
Intermolecular Forces | Electrostatic attractions between molecules. They are significantly weaker than covalent bonds. |
London Dispersion Forces | Weakest interactions but are present in all atoms. |
As The Size Of An Atom Or Structure Increases: | London dispersion force increases |
Dipole-dipole Interactions | Occur between the oppositely charged ends of polar molecules, and are stronger than London forces. |
Dipole-dipole Interactions Are Evident In: | Solid and liquid phases but are negligible in the gas phase due to the distance between particles |
Hydrogen Bonds | Specialized subset of dipole-dipole interactions involved in intra- and intermolecular attraction |
Hydrogen Bonding Occurs When Hydrogen Is Bonded To: | One of three very electronegative atoms, NOF: Nitrogen, Fluorine, Oxygen |
Eq. 3.1: Dipole Moment | p = qd. p = dipole moment. q = mag. of charge. d = displacement vector between two partial charges. |
Eq. 3.2: Formal Charge | Formal Charge = V - N nonbonding - 1/2 N bonding. V = normal number of electrons in the atom's valence shell. N = number of electrons. |
Created by:
SamB91
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