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121 Cards in this Set
- Front
- Back
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1 |
Meth |
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2 |
Eth |
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3 |
Prop |
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4 |
But |
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5 |
Pent |
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6 |
Hex |
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7 |
Hept |
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8 |
Oct |
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9 |
Non |
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10 |
Dec |
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11 |
Undec |
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12 |
Dodec |
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13 |
Tridec |
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14 |
Tetradec |
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15 |
Pentadec |
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Direction Position |
Prefix stands for? |
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# of Carbons in Main Chain |
Root stands for? |
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Type of Functional Group |
Suffix stands for? |
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sp3 |
- Single Bonds, Tetrahedral/Pyramidal/Bent - Uses s & all 3 p orbitals |
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sp2 |
- Double bonds, Trigonal Planar - Uses s & 2 p orbitals |
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sp |
- Triple bonds, Linear - Uses s and 1 p orbital |
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Saturated |
- As many hydrogens as possible - Single Bonds sp3 |
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Unsaturated |
- Compound that contains at least on multiple bond (double or triple) sp2 or sp |
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1 |
s orbital # |
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3 |
p orbital # |
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5 |
d orbital # |
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Pi Bond |
- Approach from the side for more overlap |
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Sigma Bond |
- Approach "head on" or directly - First bond made between carbon and another atom |
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180 2 |
Linear Angle/ Bonds |
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120 3 |
Trigonal Planar Angle/ Bonds |
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<120 (~116) 2 Bonds, 1 Lone Pair |
Bent Trigonal Planar Angle and Bonds |
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109.5 4 |
Tetrahedral Angle and Bond |
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<109.5 (~107) 3 Bonds 1 Lone Pair |
Trigonal Pyramid Angle and Bond |
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<109.5 (~104.5) 2 Bonds, 2 Lone Pairs |
Bent Tetrahedral Angle and Bond |
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4 4 |
Normal Number of Bonds for Carbon, Valence Electrons |
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3 Bonds, 1 Lone Pair 5 Electrons |
Normal Number of Bonds for Nitrogen, Valence Electrons |
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2 Bonds, 2 Lone Pairs 6 Electrons |
Normal Number of Bonds for Oxygen, Valence Electrons |
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Aufbau Principle Pauli Exclusion Principle |
- Lowest energy orbitals fill up first - 2 Electrons of opposite spin can occupy orbital |
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Hund's Rule |
- If 2 or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full |
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Oxygen |
Which element doesn't form triple bonds? |
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[# Total Valence Electrons] - [# of Bonds] - # of Lone Pair Electrons] |
Equation for Formal Charge |
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+1 |
Formal Charge? |
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Neutral |
Formal Charge? |
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-1 |
Formal Charge? |
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+1 |
Formal Charge? |
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Neutral |
Formal Charge? |
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-1 |
Formal Charge? |
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+1 |
Formal Charge? |
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Neutral |
Formal Charge? |
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-1 |
Formal Charge? |
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Amide (Carbonyl + Amine) |
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Alkyl Halides |
C-X |
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Acid Halides |
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3sp3, 1 Lone Pair |
Hybridization of Nitrogen |
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2sp3, 2 Lone pairs |
Hybridization of Oxygen |
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3sp3, 1 sp2 (5 Covalent Bonds) |
Hybridization of Phosphorus |
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2sp3, 2 Lone Pairs ( 4 Covalent Bonds) |
Hybridization of Sulfur |
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DOWN INCREASES |
Electronegativity decreases going (up/down) and (increases/decreases) going across. |
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Fluorine - 4 |
Which atom has the highest electronegativity and what charge? |
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Inductive Effect |
Shifting of electrons in a bond in response to the electronegativity of nearby atoms |
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-yl |
Suffix given for attachments on carbon chains? |
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Iso- |
Prefix given for attachments on carbon chains that end in a 'V' shape |
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Tert-Butyl |
T-Shape 4 Carbon Attachment called? |
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Sec |
When there is another attachment on attachment? |
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Fluoro |
Fluorine (F) attachment |
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Chloro |
Chlorine (Cl) attachment |
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Bromo |
Bromine (Br) attachment |
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Iodo |
Iodine (i) attachment |
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Cyclo |
Suffix for rings as attachments |
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Cis |
Same Side |
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Trans |
Opposite Side |
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Alkane Alkene Alkyne |
- Contain single bond between adjacent carbon atoms - Double bond - Triple bond |
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Aromatic Compounds |
- Contain benzene ring |
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Hydroxyl (Alcohol) |
-OH |
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Thiol |
-SH |
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Ether |
-C-O-C- |
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Carbonyl Aldehyde Ketone |
C=O H-C=O R1 - [C = O] - R2 |
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Carboxylic Acid (Carbonyl + Hydroxyl) |
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Ester |
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Amine |
-NH2 - R2-NH - R3-N |
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1. Check for longest chain 2. Name & Number substituents 3. List attachments alphabetically (Except halogens go first) |
3 Steps of Naming |
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1. Imaginary 2. pi 3. Non-bonding 4. Stable 5. sp3 (Single) 6. Equivalent |
Resonance Rules - Individual resonance forms are ___1___ - Forms differ only in the placement of their__2__ or ___3___ electrons - The more forms, the more __4__ than any individual resonance - Cannot jump a __5__ bond - Different forms do not have to be __6__ - Obey normal rules of valency |
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Planar |
Amide bonds have a ___ form |
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charge |
Typically you do not see a carbon with a double bond AND a _____ |
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Inductive Effects |
- Groups donate or withdraw electrons through sigma bonds |
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Resonance Effects |
Donate or withdraw electrons through pi bonds |
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Electron Donating Group |
- When attachment has lone pair of electrons - "Activates the ring" |
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Electron withdrawing group |
- When attachment has partial positive or even full positive charge - "Deactivates ring" |
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An ionic bond is between ions (which fully support a charge). The polar covalent bond is shared between two atoms with a difference in electronegativity over 0.5 but less than 1.9 |
main difference between a polar covalent bond and an ionic bond? |
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Cn H2n+2 |
How to calculate hydrogens and carbons for saturated hydrocarbons? |
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Propyl Isopropyl |
2 Types of 3-Carbon Alkyl Groups |
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Butyl Sec-Butyl Isobutyl Tert-butyl |
4 Types of 4 Carbon Alkyl Groups |
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1. Primary 2. Secondary 3. Tertiary 4. Quaternary |
__1__ carbon is bonded to one other carbon __2__ carbon is bonded to two other carbons __3__ carbon is bonded to three other carbons __4__ carbon is bonded to four other carbons |
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1. Iso 4. Substituent Di/Tri/Tetra 5. Halogens |
Select all those that order alphabetically 1. Iso 2. Sec/Tert "T" 3. Di/Tri/Tetra 4. Substituent Di/Tri/Tetera 5. Halogens |
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Acid Base |
Bronsted Lowry Definition - Proton donor - Proton acceptor |
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Acid Base |
Lewis Definition - Accepts e- pair - Donates e- pair |
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- Conjugate base - Conjugate acid |
Product that results from acid losing proton Product that results from base accepting proton |
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H-A [Acid]+ B:[Base] <=> A:[C. Base]- + H-B+[C. Acid] |
General Equation for Acid-Base Reaction |
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Ka = 10^(-pKa) |
How to solve for the acidity constant, Ka given pKa |
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1. Strong 2. Weaker 3. Weaker 4. Stronger |
The ___1___ the acid, the more its equilibrium shifts to the right, and has a ___2___ conjugate base. An acid shifting to the left of equilibrium is __3__ and has a ___4___ conjugate base. |
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1. ortho 2. para 3. double |
Charges (+,-) are always on ___1___ and ___2__ carbons for resonance. There never is a carbon in the ring with both a charge and __3__ bond. |
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greater 1. 25 2. 33 3. 50 |
the (weaker/greater) the percents character of the bond, the more acidic the compound is. sp3 is __1___ %, sp2 is __2__% and sp is __3__% |
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pKA |
- pH at which hydrogen can be removed ( the lower it is, the more acidic) |
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a. more stable A- c: loses hydrogen faster e: lower pKa |
Choose all statements in regards to more acidity a: More stable A- b: Less stable A- c: Loses hydrogen faster d: Loses hydrogen slower e: Lower pKa f: Higher pKa |
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1. Size of anion 2. Electronegativity 3. Resonance 4. Inductive Effects (EDG vs. EWG) |
4 Things that help stabilize A- |
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Iodine > Bromine > Chlorine > Fluorine Larger the anion, the more stable |
List the 4 halogens based on more stable to least stable. Explain why. |
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1. EWG 2. EDG |
Inductive Effects: ___1___ make compound more acidic by lowering pKa by stabilizing the anion (spreading out charge). ___2____ makes compound less acidic by raising pKa because they destabilize the anion (concentrate charge in one area) |
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1. Melting 2. Boiling 3. inert 4. parrafins 5. phobic |
Alkane properties: As molecular weight increases, so do __1__ and __2__ points. Typically ___3___; they have low affinity. Also called __4__. They are hydro__5__ and flammable. |
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Gaseous Liquid Solid |
@ Room Temperature, what is its state? 1-4 Carbons 5-8 Carbons 10+ Carbons |
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1. Resonance forms are imaginary. True form lies somewhere in between the structures called a "hybrid." 2. Involve change in placement of electrons in p-orbitals. Double bond changes places with lone pair, radical, or a positive charge. 3. Follows all valence rules & formal charge rules. 4. The more resonance a structure has, the more stable. 5. Resonance structures do not have to be equivalent. |
5 Main Rules of Resonance |
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I > Br > Cl > F
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Rank from best acid to worst acid. Iodine Chlorine Fluorine Bromine |
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F > Cl > Br > I
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Rank from most electronegative to least electronegative. Iodine Chlorine Fluorine Bromine |
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Ethylene |
Common name for ethene |
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Propylene
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Common name for propylene |
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Vinyl
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Common name for Ethene attachment |
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Allyl
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Common name for Propene attachment |
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1. Hydrophobic 2. Melting/Boiling Point a little higher than alkanes 3. Reactive because of extra electron between carbons of double bond (pi orbitals) |
3 Physical Properties of Alkenes |
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n = # of Carbons
X = Halogens [(2n+2) - (#H -#N + #X)] /2 |
Degrees of Unsaturation Equation |
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- Halogens, Oxygen, Nitrogen
- Metals |
List 3 Examples of Atoms with negative partial charge relative to Carbon. List 1 type of Atom with positive partial charge relative to carbon. |
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1. MCPBA (Metachlorobenzoic acid)
2. Peracids |
Epoxides are formed by these 2 main reagents |
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Carboxylic acids with extra oxygen |
What are peracids? |
