Organic Chemistry Flashcards
Locate Partial Charges and Polar Bonds in the given structure
Step 1:
Identify all polar covalent bonds.
Step 2:
Determine the direction of each dipole.
Step 3:
Indicate the location of partial charges.
Define: Node
The place in the electron cloud where there is no electron density
Define: Degenerate Orbitals
Orbitals that have the same energy level.
What geometry does sp create?
a) Trigonal Planar
b) Bent
c) Tetrahedral
d) Linear
e) Trigonal Pyramidal
d) Linear
Trigonal planar geometry with no lone pairs has a __________ arangement of atoms
Trigonal planar
Define: Hydrocarbons
Comounds that contain only carbon and hydrogen atoms
Hydrogen bonding causes a(n) ______ in boiling/melting point.
Branching causes a(n) _______ in boiling point.
increase; decrease
Ether
Amide
Define: Divalent
The atom will, generally, form 2 bonds (Example: Oxygen)
Define: Functional Group
A characteristic group of atoms/bonds that possess a predictable chemical behavior.
Define: The Aufbau Principle
The lowest-energy orbital is filled first
Amide
Steric number = 4
a) sp3
b) sp2
c) sp
a) sp3
Define: Pauli Exclusion Principle
Each orbital can accomodate a maximum of two electrons that have opposite spin
Alkyne
Define: Tetravalent
The atom will, generally, form 4 bonds (Example: Carbon)
Define: Trivalent
The atom will, generally, form 3 bonds (Example: Nitrogen)
If Ka < 1
A) Strong Base
B) Strong Acid
A)
If Ka > 1
A) Strong Base
B) Strong Acid
B)
Define: Covalent Bond
The result of two atoms sharing a pair of electrons
Alkene
Alkyne
A polar covalent bond corresponds to
a) 0.5 difference in electronegativity
b) between 0.5 and 1.7 difference in electronegativity
c) 1.7 difference in electronegativity
b)
Between 0.5 and 1.7 difference will result in a polar covalent bond
Define: Induction
The withdrawl of electrons toward oxygen.
Induction will cause partial positive and negative charges.
Carboxylic Acid
Ester
A covalent bond corresponds to
a) 0.5 difference in electronegativity
b) between 0.5 and 1.7 difference in electronegativity
c) 1.7 difference in electronegativity
a)
An 0.5 difference in electronegativity will create a coavelnt bond
What geometry does sp2 create?
a) Trigonal Planar
b) Bent
c) Tetrahedral
d) Linear
e) Trigonal Pyramidal
a) Trigonal Planar
Amine
Alkene
Amine
Define: Bronsted-Lowry Acids & Bases
Acid: Proton (H+) donor
Nase: Proton acceptor
Acids react with bases. An Acid - Base is a Proton- Transfer reacton.
An sp3-hybridized orbital forms
a) A single bond
b) A double bond
c) A tripple bond
a) A single bond
Equation: Keq = ________
Keq = [H3o+][A-]
———————-
[HA] [H2O]
Halogens
Group 7A (Florine, Chlorine, Bromine and Iodine)
Alcohol
What geometry does sp3 create?
a) Trigonal Planar
b) Bent
c) Tetrahedral
d) Linear
e) Trigonal Pyramidal
c) Tetrahedral
Tetrahedral geometry with no lone pairs has a __________ arangement of atomsm
Tetrahedral
Linear geometry has a __________ arangement of atoms
Linear
Trigonal planar geometry with one lone pairs has a __________ arangement of atoms
Bent
Equation: How to determine how many double/triple/ring bonds exist in a structure.
CNumber of - 1/2 (HNumber of) - 1/2(HalogensNumber of) + 1/2 (NNumber of) + 1
An HDI of 1 means there is 1 double bond or 1 ring. NO triple bonds.
An HDI of 2 means there is 1 double bond and 1 ring, 2 double bonds, 2 rings, or 1 triple bond.
Carboxylic Acid
Alkyl Halide
Alcohol
Tetrahedral geometry with two lone pairs has a __________ arangement of atoms
Bent
Define: Valence
Describes the number of bonds that are usually formed by each element
How to count Sigma and Pi bonds
A single bond contains 1 sigma bond.
A double bond contains 1 sigma bond and 1 pi bond.
A tripple bond contains 1 sigma bond and 2 pi bonds.
Determine the Formal Charge of
Step 1: Determine the appropriate number of valence electrons.
Step 2: Determine the actual number of valence electrons.
Step 3: Assign a formal charge.
Because the Nitrogen exhibits 4 valence electrons the charge will be possitive.
Define: Electronegativity
A measure of the ability of an atom to attract electrons
Define: Monovalent
The atom will, generally, form 1 bond (Example: Halogens & Hydrogen)
Alkyl Halide
Define: Lone pair
A pair of unshared or nonbonding electrons
Define: Solubility
Like disolves like
Define: Steric Number
Total number of sigma bonds plus lone pairs
Steric number = 3
a) sp3
b) sp2
c) sp
b) sp2
Equation: Keq= _________
Kep = 10(pKa(larger) - pKa(smaller))
Define: Formal Charge
Associated with an atom that does not exhibit the appropriate number of valence electrons
Tetrahedral geometry with one lone pair has a __________ arangement of atoms
Trigonal pyramidal
Steric number = 2
a) sp3
b) sp2
c) sp
c) sp
Ether
The larger the pKa value, the ________ the acid.
WEAKER
Electronegativity Trend in the Periodic Table
Electronegative values increase from left to right and from bottom to the top
An sp-hybridized orbital forms
a) A single bond
b) A double bond
c) A tripple bond
c) A tripple bond
Define: Lewis Theory
Acid: Electron - Pair acceptor
Base: Electron - Pair donor
Ketone
Define: Valence Electrons
The electrons in the outermost shell of an atom
Equation: pKa = _________
pKa = - log(Ka)
Ketone
Define: Hund’s Rule
When dealing with degenerate orbitals, such as p orbitals, on electron is placed in each degenerate orbital first, before electrons are paired up.
An electronegativity difference of ____ means that the electrons are not shared at all
a) 0.5 difference in electronegativity
b) between 0.5 and 1.7 difference in electronegativity
c) 1.7 difference in electronegativity
c)
A difference in electronegativity greater then 1.7 will result in non-shared electrons
Ester
Predict the geometry for the central atom in each of the compounds below
(a) NH3 (b)H3O+ (c) BH4- (d) BCl3
(e) BCl4- (f) CCl4 (g) CHCl3 (h) CH2Cl2
Define: Conjugate Pairs
Conjugate pairs differ by an H+
An sp2-hybridized orbital forms
a) A single bond
b) A double bond
c) A tripple bond
b) A double bond
Define: Exothermic
In an exothermic process, the system gives energy to the surroundings.
Therefore ΔH is negative.
Define: Endothermic
In an endothermic process, the system receives energy from the surroundings.
Therefore ΔH is positive.
Equation: Gibb’s free Energy
ΔG = ΔH -TΔS
Equation: Rate
Rate = k [A]x[B]y
Define: Nucleophile
A nucleophile (Lewis base) is an electron-rich atom capable of donating a pair of electrons.
Define: Electrophile
An electrophile (center of the atom) is an electrion deficient atom that is capable of accepting a pair of electrons.
Define: Primary Carbon
A carbon attached to one other carbon.
(R - C - Cl)
Define: Secondary Carbon
A carbon that is attached to two other carbons.
Define: Tertiary Carbon
A carbon that is attached to three other carbons.
Equation: Substitution Reaction - Nucleophilic Attack
Nuc:- + Substrate – LG ——-> Substrate – Nuc + LG-
Equation: Substitution Reaction - Loss of a Leaving Group
Substrate – LG —-LG—> Substrate —:Nuc—> Substrate – Nuc
Define: Concerted Process
In a concerted process, nucleophilic attack and loss of the leaving group occur at the same time. Thus it is a one step process.
Define: Stepwise Process
In a stepwise process, loss of the leaving group occurs first followed by the nucleophilic attack.
SN2
A) Unimolecular
B) Bimolecular
B)
SN1
A) Unimolecular
B) Bimolecular
A)
Define: Inversion of Configuration
When a nucleophile attacks the back side of the molecule (the side opposite the leaving group), the absolute configuration of the product will be opposite the absolute configuration of the reactant.
Define: Rate-Determining Step
The slowest step of the reaction. For SN1, this will be the step that it loses the leaving group.
Define: Racemic
A molecule with a chiral carbon, when racted, will create a 50/50ish split between its enantiomers with a slight favor to the non-inverted enantiomer.
