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166 Cards in this Set
- Front
- Back
Addition Reaction
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two reactants add to form one product with no atoms left over
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Elimination Reaction
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single reactant splits into two products
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Substitution Reaction
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two reactants exchange parts to yield two new products
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Rearrangement
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single product undergoes a rearrangement of bonds to yield a single isomeric product
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Reaction Mechanism
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describes the bonds broken and formed in a chemical reaction and accounts for all reactants and products
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Bond breaking is symmetrical...
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if one electron remains with each fragment
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Bond breaking is unsymmetrical...
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if both electrons remain with one fragment and the other fragment has a vacant orbital
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Bond formation is symmetrical...
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if one electron in a covalent bond comes from each reactant
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Bond formation is unsymmetrical...
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if both electrons in a covalent bond come from one reactant
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Radical Reactions
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involve symmetrical bond breaking and symmetrical bond formation
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Polar Reactions
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involve unsymmetrical bond breaking and unsymmetrical bond formation
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Why are radicals highly reactive?
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Because they contain an atom with an unpaired electron
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A substitution reaction occurs...
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when a radical abstracts an electron from another molecule
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An addition reaction occurs...
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when a radical adds to a double bond
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In radical reactions...
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all bonds are broken and formed by reactions with species with odd numbers of electrons
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Steps in a Radical Reaction
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initiation - produces radical by symmetrical cleavage
propagation - radical abstracts an atom to produce a new radical and a stable molecule termination - occurs when two radicals combine |
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Nucleophile
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compound with an electron rich atom
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Electrophile
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compound with an electron poor atom
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The bond dissociation energy describes...
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the heat needed to break a bond
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In exothermic reactions, the bonds formed...
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are stronger than the bonds broken
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Functional Group
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group of atoms within a molecule that has a characteristic chemical behavior
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Alcohol
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carbon singly bonded to the oxygen of a hydroxyl group
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Ether
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two carbons singly bonded to one oxygen
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Alkyl Halide
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aka haloalkane, carbon singly bonded to a halogen
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Amine
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carbon atom bonded to a nitrogen
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Thiol
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carbon atom bonded to an -SH (sulfhydryl) group
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Disulfide
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carbon atom bonded to two sulfurs that are joined together
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Sulfide
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two carbons joined to the same sulfur
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Amide
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nitrogen bonded to the C=O
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Ester
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oxygen bonded to the C=O
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Carboxylic Acid
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-OH group bonded to the C=O
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Ketone
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two carbons bonded to the C=O
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Aldehyde
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@ least one hydrogen bonded to the C=O
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Orbital Filling
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1s>2s>2p>3s>3p>4s>3d>4p>5s>4d>5p>4f
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∆EN > 2.0
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ionic bond
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∆EN < 0.5
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nonpolar covalent
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∆EN between 0.5 and 2.0
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polar covalent
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Prefixes 1-10
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meth
eth prop but pent hex hept oct non dec |
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Inductive Effect
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an atom's ability to polarize a bond
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Three Categories of Functional Groups
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those with carbon-carbon multiple bonds
those with carbon singly bonded to an electronegative atom groups with a carbon-oxygen double bond |
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Alkanes are saturated...
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because they contain only single bonds
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Constitutional Isomers
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are always different compounds with different chemical properties but with the same molecular formula
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Alkyl Group
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the partial structure that remains following the removal of a hydrogen from an alkane
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4 Degrees of Alkyl Substitution for Carbon
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A primary carbon is bonded to one other carbon
A secondary carbon is bonded to two other carbons A tertiary carbon is bonded to three other carbons A quaternary carbon is bonded to four other carbons |
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Prim, Sec, and Tert Hydrogens
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primary hydrogens are bonded to primary carbons
secondary hydrogens are bonded to secondary carbons tertiary hydrogens are bonded to tertiary carbons |
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Atoms consist of...
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a dense positively charged nucleus surrounded by negatively charged electrons
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The nucleus is made up of...
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positively charged protons and uncharged neutrons. Most of the mass of the atom is found in the nucleus
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Z number
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number of protons in the nucleus
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A number
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total number of protons and neutrons
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Atoms of the same element with different values of (A)...
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are called isotopes
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Wave Equation
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describes the distribution of electrons in an atom
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Psi
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represents an orbital and is the solution to a wave equation
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The two lowest energy electrons...
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are in the 1s orbital
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The ground state electron configuration of an atom...
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is a listing of the orbitals occupied by the electrons of the atom
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Rules for Predicting GSEC
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lowest energy orbitals are filled first
only two electrons in a single orbital with spins paired if two or more orbitals of equal energy exist, all are half filled first and then electrons are paired all the electrons in a half filled shell have the same spin |
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Wedged Line (solid)
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represents a bond point toward you
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Wedged Line (dashed)
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represents a bond pointing away from you
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Solid Line
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represents a bond which lies in the plane of the page
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Atoms bond together because...
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the resulting compound is more stable than the individual atoms
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Atoms tend to achieve the electron configuration...
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of the nearest noble gas
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The number of covalent bonds formed by an atom...
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is dependent upon the number of electrons it has and the number it needs to achieve an octet
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Valence electrons not used for bonding are called?
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lone pair electrons
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Covalent bonds are formed by?
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The overlap of two atomic orbitals each of which contains one electron. The two electrons have opposite spins
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The greater the orbital overlap...
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the greater the strength of the chemical bond
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Bonds formed by the head on overlap of two atomic orbitals are called?
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Sigma bonds and they have cylindrical symmetry
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Bond Strength
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is the measure of the amount of energy needed to break a bond
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Bond Length
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is the optimum distance between two nuclei
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SP3 Bond Angle
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109.5˚
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SP2 Bond Angle
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120˚
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SP Bond Angle
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180˚
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Formal Charge
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FC = VE - (1/2BE - NBE)
VE -> valence electrons BE -> bonding electrons NBE -> nonbonding electrons |
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Resonance structures differ only in...
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placement of pi and nonbonding electrons
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Individual resonance forms...
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are imaginary, not real. The real structure of the atom is a resonance hybrid
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Any three atom grouping with a multiple bond adjacent to a nonbonding p orbital has ___ resonance forms.
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Two
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A Bronsted-Lowry acid...
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donates an proton (H+ ion)
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A Bronsted-Lowry base...
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accepts a proton (H+)
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The product that results when a base accepts a proton is?
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the conjugate acid of the base
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The product that results when the acid loses a proton is?
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the conjugate base of the acid
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Stronger acids have ____ acidity constants
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Larger
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Weaker acids have ____ acidity constants
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Smaller
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A strong acid has a ____ pKa
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small
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A weak acid has a ____ pKa
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large
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The conjugate base of a strong acid...
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is a weak base
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The conjugate base of a weak acid...
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is a strong base
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Two kinds of organic acids
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those with H bonded to O and those that have a hydrogen bonded to a carbon next to a C=O group
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The main type of organic base contains?
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a nitrogen atom with a lone electron pair
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A Lewis acid...
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accepts an electron pair
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A Lewis base...
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has a pair of non-bonding electrons
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n-Alkyl groups are formed by?
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the removal of an end carbon of a straight chain alkane
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Branched chain alkyl groups are formed by?
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the removal of a hydrogen atom from an internal carbon
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In the IUPAC system of nomenclature, a chemical system name has?
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a prefix, a parent and a suffix
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The parent shows?
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the number of carbons in the principle chain
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The suffix identifies?
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the functional group family
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The prefix shows?
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the location of functional groups
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Staggered Conformation
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is the lowest energy conformer and results when all the C-H bonds are as far from one another as possible
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Eclipsed Conformation
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is the highest energy conformer and results when all the C-H bonds are as close to each other as possible
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Lab reactions are carried out it in?
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organic solvents and take place over a wide temperature range
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Biological reactions take place in?
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aqueous medium and take place at the organism's body temperature
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An Intermediate is?
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the species that lies at an energy minimum between two transition states in a reaction of at least two steps
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The difference in energy between the reactants and the transition state is?
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the energy of activation. its value ranges from 40 to 150kJ/mol
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After reaching the transition state a molecule can?
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either go on to form products or revert to the starting material
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what is the formula to calculate ∆G˚?
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∆G˚ = ∆H - T∆S
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A reaction that produces one product molecule from two reactant molecules has _____ entropy.
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negative
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A reaction that produces two product molecules from one reactant molecule has _____ entropy?
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positive
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If ∆H is negative?
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the reaction is exothermic
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If ∆H is positive?
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the reaction is endothermic
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What is ∆H a measure of?
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the change in total bonding energy during a reaction
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∆S equals?
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entropy. the measure of freedom of motion of a reaction
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If ∆G is negative then the reaction is ______ and will be ______.
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favorable, exergonic
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If ∆G is positive then the reaction is _____ and will be _____.
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unfavorable, endergonic
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For a reaction to proceed as written...
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the energy of the products must be lower than the energy of the reactants
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If Keq is greater than one.
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[products]>[reactants]
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If Keq is less than one.
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[reactants]>[products]
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∆G˚ describes?
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the energy change that occurs during a reaction, the Gibbs free energy change.
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Electrons must move from _____ to ______.
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a nucleophilic source, an electrophilic sink
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A nucleophile can be either ______ charged or ______.
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negatively charged, neutral
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An electrophile can be either _____ charged or ______.
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positively charged, neutral
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If two substituents are on the same side of the ring?
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it is cis disubstituted
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If two substituents are on opposing sides of the ring?
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it is trans disubstituted
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Factors accounting for Ring Strain
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torsional strain - due to eclipsing of bonds
steric strain - results when atom approach too closely angle strain - occurs when bond angles are distorted from their normal values |
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Polar reactions occur as a result of?
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positive and negative charges within molecules due to differences in electronegativity between atoms
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Biological reactions take place in _________ each of which has a _________.
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several small steps, small activation energy
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The equilibrium constant (Keq) shows what?
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the ratio of product concentration to reactant concentration
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-RT(lnKeq) = ?
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∆G˚
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In radical reactions all bonds are broken and formed by reactions of species with ____________.
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odd numbers of electrons
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Steroids have ______ fused rings.
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four
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Bicyclic ring systems have rings that are _____________.
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connected by bridges
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In cis 1,2-dimethylcyclohexane, one methyl group is ______ and one is _______ in both chair conformations which are of ______ energy
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axial, equatorial, equal
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In trans 1,2-dimethylcyclohexane, both methyl groups are either _____________.
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both axial or both equatorial
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After a ring flip...
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an axial bond becomes an equatorial bond and vice versa
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Two kinds of bonding positions on a cyclohexane ring?
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axial - perpendicular to the plane of the ring
equatorial - hydrogens roughly in the plane of the ring |
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Each carbon in a cyclohexane has?
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one axial hydrogen and one equatorial hydrogen
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Each side of a cyclohexane ring has?
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alternating axial and equatorial hydrogens
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The chair conformation of cyclohexane is __________.
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strain free
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The twist boat conformation of cyclohexane little ______ strain but experiences both ________ strain and ________ strain.
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angle, steric, torsional
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In a standard drawing of cyclohexane the ________ bond is in the front.
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lower
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Cyclopentane has little ______ strain but considerable ________ strain.
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angle, torsional
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In an effort to relieve strain, cyclopentane adopts a puckered conformation. In this conformation one carbon is ________ and the hydrogens are _________.
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bent out of plane, nearly staggered
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Cyclopropane has _____ bonds
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bent
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Because of bent bonds, cyclopropane is ____________ than other cycloalkanes.
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more reactive
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Cyclobutane has less _______ strain than cyclopropane but more _______ strain.
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angle, torsional
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Cyclobutane has almost the same total strain as _________.
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cyclopropane
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The more strained the compound the _______ the heat of combustion.
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higher
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The most favored conformation for any straight chain alkane has carbon-carbon in _________ arrangements and large substituents ______ to each other.
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staggered, anti
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Steric Strain
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the repulsive interaction that results from forcing atoms to be closer together than their atomic radii allow
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Anti Conformation
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one of the staggered conformers of butane. positions the methyl groups as far apart as possible (lowest energy)
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Gauche Conformation
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one of the staggered conformations of cyclobutane. positions the methyl groups 60˚ apart (second lowest energy)
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The boiling and melting points of an alkane increase with _________________.
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increasing molecular weight
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Increased branching _________ an alkane's boiling point.
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lowers
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If the carbons are in a row the alkane is?
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a straight chain alkane
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If the carbon chain has a branch then the alkane is?
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a branched chain alkane
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Isomers whose atoms are connected differently are?
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constitutional isomers
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The chemistry of every organic molecule is determined by?
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its functional group
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Hydrophilic substances dissolve in water because?
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they are able to form hydrogen bonds
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The products of an acid-base reaction are _____________ than the reactants
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more stable
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What is dipole moment?
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a measure of a molecule's overall polarity
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A crossed arrow is used to indicate?
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bond polarity. the tail of the arrow is electron poor, the tip electron rich.
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Carbon has an EN of?
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2.5
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Elements on the right side of the periodic table are ________ electronegative than elements on the left side.
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more
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2 ways two 1s orbitals can combine.
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additive combination - bonding MO, lower in energy than the two hydrogen 1s orbitals
subtractive combination - antibonding MO, higher in energy than the two hydrogen 1s orbitals |
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Torsional Strain
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is due to eclipsing of bonds
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Angular Strain
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is due to distortion of bonding angles from their normal values
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Additive Combination
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bonding MO, lower in energy than the two 1s orbitals
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Subtractive Combination
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antibonding MO, higher in energy than the two 1s orbitals
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Axial bonds lie...
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perpendicular to the plane of the ring
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Equatorial bonds lie...
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roughly in the plane of the ring
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