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secondary
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A compound containing a functional group bonded to a carbon atom bonded to two other carbon atoms and one hydrogen atom
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ionic interaction
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Attraction between oppositely charged ions
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ground-state electron configuration
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The lowest-energy electron configuration for an atom or molecule
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polar covalent bonds
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A covalent bond between atoms whose difference in electronegativity is between approximately .5 and 1.9
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primary
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A compound containing a functional group bonded to a carbon atom bonded to only one other carbon atom and two hydrogens
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potential energy
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The energy that can be released if given an opportunity
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tetrahedral
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A bonding arrangement in which an atom is bonded to four atoms located at the corners of a tetrahedron
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alcohol
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A compound containing an --OH (hydroxyl) group bonded to a tetrahedral carbon atom
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bonding electrons
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Valence electrons involved in forming a covalent bond
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organic chemistry
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The study of the compounds of carbon
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sigma bonding molecular orbital
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A molecular orbital in which electron density is concentrated between two nuclei, along the axis joining them, and is cylindrically symmetric
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covalent bond
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A chemical bond formed between two atoms by sharing one or more pairs of electrons
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electron affinity
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Energy added or released when an electron is added to an atom or molecule
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anion
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An atom or group of atoms bearing a negative charge
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carbonyl group
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A C=O group
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excited state
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A state of a system at higher energy than the ground state
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bond length
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The distance between nuclei in a covalent bond in picometers
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tertiary
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A compound containing a functional group bonded to a carbon atom bonded to three other carbon atoms
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secondary amine
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An amine in which nitrogen is bonded to two carbons and one hydrogen
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functional groups
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An atom or group of atoms within a molecule that shows a characteristic set of physical and chemical properties
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ketone
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A compound containing a carbonyl group bonded to two carbons
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pyramidal
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A bonding arrangement in which an atom is bonded to three atoms in a triangular pyramid
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bond dipole moment
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A measure of the polarity of a covalent bond. it is the product of the charge on either atom of a polar covalent bond times the distance between the nuclei
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hybrid orbital
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An atomic orbital formed by the combination of two or more atomic orbitals
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carboxylic acid
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A compound containing a carboxyl, --COOH, group
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contributing structures
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Representation of a molecule or ion that diffes only in the distribution of valence electrons
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bonding molecular orbital
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A molecular orbital in which electrons have a lower energy than they would in isolated atomic orbitals
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hybridization
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The combination of atomic orbitals of different types
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carboxylic amide
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A derivative of a carboxylic acid in which the --OH is replaced by an amine
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resonance
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A theory that many molecules are best described as a hybrid of several Lewis structures
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valence electrons
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Electrons in the valence (outer most) shell of an atom
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amino group
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A compound containing a nitrogen atom bonded to one, two, or three carbon atoms by single bonds
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valence bond theory
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A model of bonding that places electron pairs between adjacent atoms to create bonds
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orthogonal
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Having no net overlap
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shells
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A region of space around a nucleus that can be occupied by electrons, corresponding to a principal quantum number
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VSEPR
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A method for predicting bond angles based on the idea that electron pairs repel each other and keep as far apart as possible
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formal charge
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The charge on an atom in a polyatomic ion or molecule
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orbital
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A region of space that can hold two electrons
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carboxylic ester
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A derivative of a carboxylic acid in which H of the carboxyl group is replaced by a carbon
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antibonding molecular orbital
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A molecule orbital in which electrons have a higher energy than they would in isolated atomic orbitals
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ground state
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The lowest energy state of a system
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energy
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The ability to do work
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aldehyde
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A compound containing a --CHO group
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quantization
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Having discrete values for energy and momentum
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delocalization
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The spreading of electron density over a larger volume of space
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primary amine
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An amine in which nitrogen is bonded to one carbon and two hydrogens
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phasing
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Sign of the wavefunction at particular coordinates in space, either plus or minus. Phasing is often represented as different colors, such as red and blue used in this text
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sp3 hybrid orbital
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A hybrid atomic orbital formed by the combination of one s atomic orbital and three p atomic orbitals
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double-eaded arrows
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A symbol used to show that structures oneither side are resonance contributing structures
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orbital
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A region of space that can hold two electrons
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ionization potential
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The energy needed to romove the most loosely held electron from an atom or molecule
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sp2 hybrid orbital
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A hybrid atomic orbital formed by the combination of one s atomic orbital and two p atomic orbitals
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resonance hybrid
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A molecule, ion, or radical described as a composite of a number of contributing structures
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octet rule
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Group 1A-7A elements react to achieve an outer shell of eight valence electrons
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valence shell
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The outermost occupied elctron shell of an atom
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node
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A point in space where the value of a wave function is zero
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electronegativity
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A measure of the force of an atom's attraction for electrons
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nonpolar covalent
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A covalent bond between atoms whose difference in electronegativity is ess than approximately .5
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Lewis dot structure
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The symbol of an element surrounded by a number of dots equal to the number of electrons in the valence shell of the atom
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bond dissociation enthalpy
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The amount of energy required to break a bond into two radicals in the gas phase at 25 degrees C
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isomers
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Different compounds with the same molecular formula
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Molecular orbital theory
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A theory of chemical bonding in which electrons in molecules occupy molecular orbitals that extend over the entire molecule and are formed by the combination of the atomic orbitals that make up the molecule
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molecular dipole moment
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The vector sum of individual bond dipoles
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wave functions
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A solution to a set of equations that defines the energy of an electron in an atome and the region of space it may occupy
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lone pair or nonbonding electrons
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Valence electrons not involved in forming covalent bonds. Also called unshaired pairs
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tertiary amine
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An amine in which nitrogen is bonded to three carbons
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cation
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An atom or group of atoms bearing a positive charge
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sp hybrid orbital
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A hybrid atomic orbital formed by the combination of one s atomic orbital and one p atomic orbital
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conjugation
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Lack of atoms between pi bonds or between pi bonds and lone-pair electrons
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quantum mechanics (wave mechanics)
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The branch of science that studies particles and their wavelike properties
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