Organic Chemistry 1 ACS Exam
Atomic number number of protons in the nucleus of an atom
Mass number atomic weight
Protons don't equal Neutrons Isotopes
Electrons Used for bonding, determining structure of molecules, located in orbital shells
Electron Density the probability that an electron will be found in a particular region of an atom
Quantum numbers (n) n1 = lowest energy, n=2 eight electrons,
Pauli Exclusion Principle Each orbital can hold max. 2 electrons with spins paired
Alfoau Principle Start with the lowest energy and fill until we have correct number of electrons
Hund's Rule Two or more electrons of the same energy will go into different orbitals rather
than pair
Valence electrons Electrons on the outermost energy level of an atom
Bond formation Octet Rule - want 8 electrons in the outter most shell
Ionic bonding metal + nonmetal, transfer of electrons
Covalent bonding sharing of electrons
single bond 1 sigma bond
double bond 1 sig 1 pi
triple bond 1 sig 2 pi
Common Bonding Patterns Carbon: VE - 4// LP - 0// bonds: 4
Nitrogen: VE- 5// LP - 1 // bonds: 3
Oxygen: VE- 6// LP - 2 // bonds: 2
Hydrogen: VE - 1 // LP - 0 // bonds: 1
Halogens: VE - 7// LP: 3 // bonds: 1
, Organic Chemistry 1 ACS Exam
Formal Charge (group #) - (nonbonding electrons) - (number of bonds)
Condensed Structures bonds aren't shown
Expanded shows all bonds (lewis structure)
Line Angle don't write C or H to C bonds
Constitutional Isomers same molecular formula, different connectivity
Geometric Isomers have the same covalent arrangements but differ in spatial arrangements (has
cis/trans)
Resonance Different ways of drawing the same compound
Resonance Structure rules 1. Can't break single bonds
2. Overall charge must be the same
3. Valid lewis structures
Hybrid Orbitals sigma bonds + lone pairs around a certain atom
Hybrids sp3/ 109.5 / tetrahedral
4 sp / trigonal
3 sp / 180 / linea
2
Dipole-Dipole has electron lone pairs
hydrogen bonding strongest bonding, has O,N,F
London Dispersion has no electron pairs
Inductive force when electrons are shifted towards more electronegative atoms
Arehenius acid a substance that forms H3O+ from water
Arehenius base substance that forms -OH in water
Atomic number number of protons in the nucleus of an atom
Mass number atomic weight
Protons don't equal Neutrons Isotopes
Electrons Used for bonding, determining structure of molecules, located in orbital shells
Electron Density the probability that an electron will be found in a particular region of an atom
Quantum numbers (n) n1 = lowest energy, n=2 eight electrons,
Pauli Exclusion Principle Each orbital can hold max. 2 electrons with spins paired
Alfoau Principle Start with the lowest energy and fill until we have correct number of electrons
Hund's Rule Two or more electrons of the same energy will go into different orbitals rather
than pair
Valence electrons Electrons on the outermost energy level of an atom
Bond formation Octet Rule - want 8 electrons in the outter most shell
Ionic bonding metal + nonmetal, transfer of electrons
Covalent bonding sharing of electrons
single bond 1 sigma bond
double bond 1 sig 1 pi
triple bond 1 sig 2 pi
Common Bonding Patterns Carbon: VE - 4// LP - 0// bonds: 4
Nitrogen: VE- 5// LP - 1 // bonds: 3
Oxygen: VE- 6// LP - 2 // bonds: 2
Hydrogen: VE - 1 // LP - 0 // bonds: 1
Halogens: VE - 7// LP: 3 // bonds: 1
, Organic Chemistry 1 ACS Exam
Formal Charge (group #) - (nonbonding electrons) - (number of bonds)
Condensed Structures bonds aren't shown
Expanded shows all bonds (lewis structure)
Line Angle don't write C or H to C bonds
Constitutional Isomers same molecular formula, different connectivity
Geometric Isomers have the same covalent arrangements but differ in spatial arrangements (has
cis/trans)
Resonance Different ways of drawing the same compound
Resonance Structure rules 1. Can't break single bonds
2. Overall charge must be the same
3. Valid lewis structures
Hybrid Orbitals sigma bonds + lone pairs around a certain atom
Hybrids sp3/ 109.5 / tetrahedral
4 sp / trigonal
3 sp / 180 / linea
2
Dipole-Dipole has electron lone pairs
hydrogen bonding strongest bonding, has O,N,F
London Dispersion has no electron pairs
Inductive force when electrons are shifted towards more electronegative atoms
Arehenius acid a substance that forms H3O+ from water
Arehenius base substance that forms -OH in water
