Organic chemistry
is the branch of chemistry that deals with the chemistry of living “organic” substances (e.g. substances from animals and plant)s
Inorganic Chemistry
INORG OR ORG?
It is the general study of chemicals / elements.
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Organic chemistry
is the branch of chemistry that deals with the chemistry of living “organic” substances (e.g. substances from animals and plant)s
Inorganic Chemistry
INORG OR ORG?
It is the general study of chemicals / elements.
Inorganic Chemistry
INORG OR ORG?
Minerals
Inorganic Chemistry
INORG OR ORG?
All elements in the periodic table
Organic Chemistry
INORG OR ORG?
It is specific to the study of CARBON and to all substances containing it.
Organic Chemistry
INORG OR ORG?
Biological species (animals, plants)
Organic Chemistry
INORG OR ORG?
C, H, O, N, S, P, X (halogens)
hydrocarbons
composed entirely of C and H atoms
hydrocarbon derivatives
composed of C, H, and one or more element.
4
Carbon atoms based on their atomic configuration will have _ valence electron and must form _ bonds to achieve its Octet rule.
Atomic number
gives the # of protons / electrons
Mass number
the total # of protons and neutrons in the nucleus.
Atomic Orbitals
Also known as wave function.
It is the solution to a wave equation — the mathematical expression used to describe the distribution of electrons in an atom.
spherical
shape of s orbital
dumbbell shape
shape of p orbital
ORBITAL
a region of space around a nucleus where electrons are most likely to be found.
electron shells
Atomic orbitals are arranged around the nucleus in different layers known as “__” based on their sizes and energy levels.
Hund’s principle
states that every orbital in a subshell is singly occupied before other orbitals are completely filled and that electrons in a singly occupied orbital will have the same spin
Aufbau’s principle
states that electrons will fill the lowest available energy level before filling the higher levels
Pauli’s Exclusion principle
states that no two electrons will have identical quantum numbers (spin is opposite)
Octet rule
states that the valence shell (outermost shell) must be filled completely and must achieve a noble gas configuration (8 valence electron).
Ionic Bond
IONIC OR COVALENT
Electrons are transferred.
Ionic Bond
IONIC OR COVALENT
Between atoms of different eletronegativity (cations and anions)
Ionic Bond
IONIC OR COVALENT
Metals and Non-metals
Covalent Bond
IONIC OR COVALENT
Electrons are shared.
Covalent Bond
IONIC OR COVALENT
Between similar atoms and atoms of nearly equal electronegativity.
Covalent Bond
IONIC OR COVALENT
Non-metals
Lewis dot structure
shows the kernel or nucleus represented by the symbol of the atom surrounded by its valence electrons represented by dots.
Kekule structure
also known as line-bond structures; shows 2- electron covalent bonds as a line and the lone-pair electrons (non-bonding electrons) as dots.
Electronegativity
a measure of the relative attraction an atoms has for the shared electron in a bond.
Bond polarity
a measure of the degree of inequality in the sharing of electrons between two atoms in a chemical bond.
Non-polar covalent bond
a covalent bond in which there is a equal sharing of electrons between two atoms.
Polar covalent bond
a covalent bond in which there is an unequal sharing of electrons between two atoms.
2 and above
Electronegative difference of Ionic bonds
1.5-2
Electronegative difference of ionic or polar covalent
1.5-0.4
Electronegative difference of polar covalent
0.4 and below
Electronegative difference of nonpolar covalent
Formal Charge
the no. of valence electrons in the neutral atom minus the number of covalent bonds to the atom and the number of unshared electrons on the atom.
Formal Charge
these charges will have an impact on chemical reactions and product formation.
Orbital hybridization
is a concept of combining orbitals to form hybrid orbitals that are suitable for pairing electrons to form covalent bonds.
Tetrahedral,
the geometric shape of carbon with 4 hybridize orbitals with a specific bond angle.
sigma bonds
head-on overlap
stronger
hybrid
sp3
single bond
pi bond
sideway overlap
weaker (reactive)
unhybrid
sp2 and sp
found in double or triple bond (BELOW in double; top and bottom in triple)
sp3 carbon
forms when 2s orbital hybridize with 3 2p orbitals forming four (4) sp3 hybrid orbitals.
sp2 carbon
forms when 2s orbital hybridize with 2 2p orbitals forming three (3) sp2 hybrid orbitals and one (1) unhybridized p-orbital.
sp carbon
forms when 2s orbital hybridize with 1 2p orbital forming two (2) sp hybrid orbitals and two (2) unhybridized p-orbitals.
Functional Group
a group of atom within a molecule that possess a characteristic behavior.
Functional Group
is a structural feature of a molecule which determine its reactivity and can therefore be used for molecule classification.
moiety or portion of the structure that undergoes specific reactions.
Linear
a straight-chain molecule with no branching substituents.
Branched
a straight chain of atoms, usually carbon, with any number of secondary, straight-chain branches.
Cyclic
a compound in which a series of atoms are connected to form a ring.
Saturated organic molecule
is composed of all sp3 hybridized carbons.
All carbons form only single bonds with each other (e.g. Alkane)
Unsaturated organic molecule
possesses a number of pi-bond (1 or 2)
which allows further addition of new atoms into the chain (e.g. alkene / alkyne).
Addition
the combination of two or more molecules to form a bigger molecule.
Elimination
a reaction wherein two substituents are removed from a molecule either in one-step or two-step mechanism.
Substitution
a reaction wherein one functional group in a compound is replaced by another functional group.
Rearrangement
a reaction wherein the carbon skeleton of an organic molecule is rearranged to yield a structural isomer of the original molecule (mostly for stability purposes).
Organic REDOX
oxidation or reduction reactions of some functional groups in an organic molecule.
Addition
halogenation,
Addition
hydrogenation,
Addition
hydrohalogenation
Addition
acetal formation
Addition
hydrate formation
Elimination
dehydration
Elimination
Unimolecular or Bimolecular elimination (E1/E2)
Substitution
Types: Aromatic Electrophilic (SE), Radical
(SR), Unimolecular or Bimolecular Nucleophilic (SN1/SN2),
Substitution
Nucleophilic aliphatic/acyl
Substitution
Friedel-Craft’s Acylation and Alkylation
Rearrangement
tautomerization,
Rearrangement
hydride/methide shift
bonding electrons
number of electrons - number of valence electrons