Organic Chemistry Terms

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Hund's Rule Cation Radius of an Atom: 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 Anion Electron Configuration: As we progress from H(atomic #1) up higher atomic # lowest orbitals are filled first

Atom that gains electrons becomes a negative ion

Description of election structure for an element
Bond Length Noble-gas Confoguration Covalent Radii: Determines distance between nuclei

ex [Ne] perfect 8 electrons, octet rule

Symmetircal covalent compound ex. Cl-Cl or H-H and dividing by two.
Complete Structural Formulas Acid Condensed Structural Formulas: Formulas in general

Substance that can denote a H ion to a base

Bonds are not always shown and atoms of the same type bonded to one other atom are grouped together
Conjugate Acid Basicity constant Equilibrium 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 Bond Polygon 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 atom

Cyclic compounds a represented by these
Degenerate Molecular Orbitals Magnetic Moment: Orbitals that have the same energy

Shared electrons result from merging of atomic orbitals into shared orbitals

Spin of a charged particles gives rise to a small magnetic field
Double Bonds Atomic Orbitals Single Bonds: Two atoms can share two pairs of electrons

Regions in space with finding electron with specific energy

Sharing of one pair of electrons between two atoms
Electron Density Lewis formulas or Lewis structures Node: Probability of finding an electron in a particular spot

dot formulas

zero point, probability of fiding an electron is very small
Electronegativity Pauling Scale Electropositive: Measure of an atom's attraction for its own bonding electrons, especially in covalently bonded compounds

Numerical scale of electonegativity

Element with a very low negativity
Empirical Formula Strong Acid Molecular Formula: Type of atom and numerical ratio in a molecule

Acid undergoes essentially complete ionization in water

Actual number of each atom in a molecule
Equilibrium Constant: Reflects how far the reaction proceeds toward completion [K]
Free Radical Weak Acid Bond Dissocation Energy: Unpaired electron

Small proportion of its molecules broken into ions in water

value, delta H
Heterolytic Cleavage Amines Homolytic 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 electrons

Each 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 Constant Lewis 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 radius van der Waals forces: Nonpolar molecules that are attracted to one another by weak dipole-dipole interactions

distance at which the attraction is greatest

The 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 Bond First Energy Level: The chemistry of the compounds of carbon

Covalent bonds which exert equal or nearly equal attractions for the bonding electron

Lowest energy level of an electron
Partial Charges Carboxyl Group Bond Angle: Distrubution of electron density in a polar bond

-CO2H weak acid. Compounds that contain carboxyl groups are carboxylic acids

More than two atoms in a molecule bonds form angle 60-180*
Polar Covalent Bond Conjugate Base Ionic 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 ion

Continusam increases with nonpolar equivlent bonds to ionic bonds
Second Energy Level Formal Charge Third Energy Level: Electrons in second energy level, higher energy

To some of the elements in these structures

Electrons in third shell the higher in energy
Size Henderson-Hasselbalch Equation Electronegativity: 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 Base Line-bond Formulas: Show struture of molecules or order of attachment

Substance that accepts a H ion from an acid

Dashes for bonds, electrons not written
Valence-Bond Theory Standing Waves Amplitude: Line-bond formulas are used to describe cobalent bonds and their interactions

Wave that has a fixed point at both ends

The height of a standing wave

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Created By harichar