Organic Chemistry Terms
Terms
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Hund's RuleCationRadius of an Atom
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Filling atomic orbitals, pairing of two electrons in degenerate orbitals doesn't occur until each orbital contain one electrons.Atom that loses elctrons becomes a positive ion.Distance from the center of nulceus to out
- Aufbau Principle
AnionElectron Configuration- As we progress from H(atomic #1) up higher atomic # lowest orbitals are filled first
Atom that gains electrons becomes a negative ionDescription of election structure for an element- Bond Length
Noble-gas ConfogurationCovalent Radii- Determines distance between nuclei
ex [Ne] perfect 8 electrons, octet ruleSymmetircal covalent compound ex. Cl-Cl or H-H and dividing by two.- Complete Structural Formulas
AcidCondensed Structural Formulas- Formulas in general
Substance that can denote a H ion to a baseBonds are not always shown and atoms of the same type bonded to one other atom are grouped together- Conjugate Acid
Basicity constantEquilibrium Control- Of a base is the product of this reaction of the base and H ion
base opposite of Ka[thermodynamic control] Reversible reactions- Cyclic Compounds
Hydrogen BondPolygon Formulas- Compound that contains one or more rings
A partially positive H-atom of are molecule is attracted to the unshared pair of electrons of the electronegative atomCyclic compounds a represented by these- Degenerate
Molecular OrbitalsMagnetic Moment- Orbitals that have the same energy
Shared electrons result from merging of atomic orbitals into shared orbitalsSpin of a charged particles gives rise to a small magnetic field- Double Bonds
Atomic OrbitalsSingle Bonds- Two atoms can share two pairs of electrons
Regions in space with finding electron with specific energySharing of one pair of electrons between two atoms- Electron Density
Lewis formulas or Lewis structuresNode- Probability of finding an electron in a particular spot
dot formulaszero point, probability of fiding an electron is very small- Electronegativity
Pauling ScaleElectropositive- Measure of an atom's attraction for its own bonding electrons, especially in covalently bonded compounds
Numerical scale of electonegativityElement with a very low negativity- Empirical Formula
Strong AcidMolecular Formula- Type of atom and numerical ratio in a molecule
Acid undergoes essentially complete ionization in waterActual number of each atom in a molecule- Equilibrium Constant
- Reflects how far the reaction proceeds toward completion [K]
- Free Radical
Weak AcidBond Dissocation Energy- Unpaired electron
Small proportion of its molecules broken into ions in watervalue, delta H- Heterolytic Cleavage
AminesHomolytic Cleavage- Both bonding electrons are retained by one of the atoms
Similar to ammonia; amine contains N atom bonded covalently to one or more C atoms and has unshared pair of electronsEach atom recieves one electron f- Ionic Bond
Covalent Bond- Results from transfer of electrons from one atom to another
Results from sharing of a pair of ele trons by two atoms- Lewis Acid
Acidity ConstantLewis Base- Substance that can accept a pair of electrons
Ionization of an acid in water [Ka]Substance that cen donate a pair of electrons- London Forces
van der Waals radiusvan der Waals forces- Nonpolar molecules that are attracted to one another by weak dipole-dipole interactions
distance at which the attraction is greatestThe various dipole-dipole interactions- Molecular Orbitak (MO) Theory
Valence-Shell Electron-Pair Repulsion (VSEPR) Theory- provides mathematical descriptions of orbitals, their energies, and their interactions
Valence electrons or electron pairs repel each other. These repulsions are used to explain bons angles and molecular geometry- Organic Chemistry
Nonpolar BondFirst Energy Level- The chemistry of the compounds of carbon
Covalent bonds which exert equal or nearly equal attractions for the bonding electronLowest energy level of an electron- Partial Charges
Carboxyl GroupBond Angle- Distrubution of electron density in a polar bond
-CO2H weak acid. Compounds that contain carboxyl groups are carboxylic acidsMore than two atoms in a molecule bonds form angle 60-180*- Polar Covalent Bond
Conjugate BaseIonic Character- Bond with an uneven distirbution of electron density
An acid is the ion or molecule that is formed when an acid loses its H ionContinusam increases with nonpolar equivlent bonds to ionic bonds- Second Energy Level
Formal ChargeThird Energy Level- Electrons in second energy level, higher energy
To some of the elements in these structuresElectrons in third shell the higher in energy- Size
Henderson-Hasselbalch EquationElectronegativity- Strength increases when size increases
pH= pKa + log [A]/[HA]If more electronegative atom can carry a negative charge more readily than a less electronegative atom- Structural Formula
BaseLine-bond Formulas- Show struture of molecules or order of attachment
Substance that accepts a H ion from an acidDashes for bonds, electrons not written- Valence-Bond Theory
Standing WavesAmplitude- Line-bond formulas are used to describe cobalent bonds and their interactions
Wave that has a fixed point at both endsThe height of a standing wave - Aufbau Principle