CHEM 333: Study Guide
90 Cards in this Set
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s,p,d,f
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Shells are broken into subshells:
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Orbital
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Is the region of space that holds 2 electrons
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Electron configuration
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Is a description of electrons in orbitals (number and where)
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Ground state configuration
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Is the lowest energy configuration you can have.
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Aufbau Principle
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GSC rule that you fill the orbital from lowest energy to the highest energy
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Pauli Exclusion Principle
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GSC rule that there are only 2 electrons per orbital. The spins are paired opposite.
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Hund's rule
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GSC rule that you add 1 electron to each orbital equal in energy. (Minimized electrostatic repulsion)
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Valence electrons
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The outer/last shell of electrons.
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Octet rule
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The 2nd row of elements want 8 electrons (noble gas status)
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Anion
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Gain 1 electron
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Cation
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Lose 1 electron
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Ionic
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Chemical bond to lose or gain an electron is to become ______.
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Covalent
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A chemical bond formed between atoms by sharing electron pairs.
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Ionic or Covalent
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2 bond ways to complete an octet:
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Lone pairs
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nonbonding pairs of electrons
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Polar
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A characteristic where atoms do not share electrons equally.
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Electronegativity
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Use _________ to predict polar or nonpolar.
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Formal charge
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Is determined by = the (# of valence es)-(# of e lone pairs)- 1/2 (shared)
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Multiple bonds
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Atoms sharing more than just 2 electrons.
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Double bonds
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2 atoms share 4 electrons.
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Triple bonds
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2 atoms share 6 electrons.
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VSEPR
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We predict bond angle by "valence shell electron pair repulsion"
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Tetrahedral 109.5
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4 regions of electron densities gives a ________ shape with a bond angle of ______
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Pyramidal
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A tetrahedral with 1 lone pair gives the ______ shape.
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Bent
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A tetrahedral with 2 lone pairs gives the _______ shape.
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Trigonal planar 120
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3 regions of electron densities gives a ___________ shape with a bond angle of _______
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Linear 180
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2 regions of electron densities gives a _________ shape with a bond angle of _____
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Major contributers
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Of resonance Include 1). filled octets, 2). least separation of unlike charges (or neutral), 3). maximum number of covalent bonds, and 4). negative charge is the more electronegative atom.
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Electron density
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Is the probability of where you will find electrons.
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Quantum mechanics
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Is the idea that the properties of electrons are best explained by treating electrons as waves not particles.
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Traveling and standing
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The 2 types of waves:
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Wave function
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Is math that describes waves.
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Mixing
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Constructive and destructive wave functions are called ______
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Constructive
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Add orbitals
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Destructive
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Subtract orbitals
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Add
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Orbitals "in phase.."
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Subtract
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Orbitals "out of phase.."
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Pi* Pi
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____ is higher in energy than __.
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4sp^3
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(Tetrahedral) 1s + 3p =
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3sp^2
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(Trigonal planar) 1s + 2p =
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2sp
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(Linear) 1s + 1p =
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S character
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The greater the percent of ________, the shorter the bond.
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Homolytic cleavage
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Bond breaking in which the bonding electron pair is split evenly between the products
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Heterolytic
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Bond breaking in which both electrons remain with only one part
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Hydrocarbon
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Naming where there the molecule only contains carbon and hydrogen
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Alkanes
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A type of hydrocarbon where it is saturated. Every carbon has the max number of Hs (and no double bonds)
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-ane
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Suffix of alkanes
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Alkenes
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A type of hydrocarbon, where it is unsaturated. Also has one or more double bond
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-ene
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Suffix of alkenes
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Alkynes
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A type of hydrocarbon where there is one or more triple bond
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-yne
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Suffix of alkynes
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Aromatic
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A type of hydrocarbon that has rings and stuff
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Functional Groups
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A naming for carbon and other atoms.
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Alkylhalides
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Is an alkane but in replace of a H there is a F, Cl, Br, or I.
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C that halide
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Classifying of a Alkylhalide is based on ________ is attached to.
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primary, secondary, tertiary
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Classifying sections: 1, 2, 3 (for alkylhalides, alcohols, amines, esters,
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Alcohols
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Naming of OH hydroxyl group bonded to an sp3 carbon.
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Ethers
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Naming of oxygen bonded to 2 different alkyl groups
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Amines
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Naming of an amino group? Nitrogen is bonded to 1, 2, or 3 carbons by a single bond.
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Ammonia
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The exception to amines. Nitrogen is attached to 3 Hs not Cs
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Aldenhydes and Ketones
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Naming, both contain a carbonyl group.
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Aldenhyde
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Naming with a carbonyl bonded to 1 H and 1 C
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Formaldehyde
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Exception to the Aldenhydes. CH2O - not 1 H and 1 C but 2 Hs
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Ketone
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Naming with carbonyl bonded to 2 Cs
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Carboxylic Acid
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Naming where molecule contains COOH. This is acetic acid
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Acetic acid
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COOH
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Formic acid
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A carboxylic acid that has H, it is CO2H2
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Esters
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Naming of a derivative of carboxylic acid. Replace OH with amine compound
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Nitriles
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Naming of a simple carbon to nitrogen
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Reaction Mechanism
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Is a description of molecular events as reactants become products
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Bronstead base
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A substance that accepts a proton, H+ acceptor
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Bronstead acid
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A substance that gives up a proton, H+ donor
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Source
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The arrow in "arrow pushing" starts where the electron is found:
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Sink
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The arrow in "arrow pushing" points to where the electron ends up:
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products/reactants
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Keq or the equilibrium constant is:
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Weaker
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A larger pka ---> ______ acid (strength)
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Stronger
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A smaller pka ---> _____ acid (strength)
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Stronger
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Weak acid (made into conjugate base) ---> _______ conjugate base (strength)
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Weak
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Strong acid (made into a conjugate base) ---> _______ conjugate base (strength)
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Equilibrium
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_______ lies toward the weakest acid
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Stability conjugate base
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The _______ of the _______ determines acidity
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More
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The more stable the conjugate base is the ___ acidic
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Increase
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Increase in the elctronegativity is an ______ in acidity
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Increase
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Larger the atom, the ______ in acidity
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Increase
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An increase in s character (by hybridization) is an _____ in acidity
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Ion-ion force
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A strong electrostatic force between positive and negative atoms
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Van der waals
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Forces (or interactions) between molecules
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Dipole-dipole
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A type of van der waals reaction when molecules are polar
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Hydrogen bonding
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A type of van der waals interaction where H bonds with N, O, and F. it is weaker than covalent bonds.
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London dispersion
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A type of van der waals interaction where it is non-polar. Attraction results from interaction between temporary, induced dipoles. Very weak.
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CHEM 333: Exam 2