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O chem chpt.1 and 3
| Term | Definition |
|---|---|
| how many bonds can hydrogen have; how many valance electrons; how many lone pairs | 1;1;0 |
| how many bonds can carbon have; how many valance electrons; how many lone pairs | 4;4;0 |
| how many bonds can nitrogen have; how many valance electrons; how many lone pairs | 3;5;1 |
| how many bonds can phosphorus have; how many valance electrons;how many lone pairs | 3;5;1 |
| how many bonds can sulfur have; how many valance electrons; how many lone pairs | 2;6;2 |
| how many bonds can oxygen have; how many valance electrons; how many lone pairs | 2;6;2 |
| how many bonds can chlorine, flourine, bromine, and iodine have; how many valance electrons; how many lone pairs | 1;7;3 |
| why can phosphorus and sulfur (anything past 2 row) form more bonds than they normally have | they can expand their octet so as to "use up" lone pairs |
| what atoms cannot "use up" lone pairs/expand octet to form more bonds | halogens, oxygen, boron, carbon, nitrogen (atoms in the second row) |
| which bond is more important in organic chemistry: covalent or ionic | covalent- between 2 nonmetals |
| triple bonds are hybridized as | sp |
| double bonds are hybridized as | sp^2 |
| single bonds are hybridized as | sp^3 |
| sigma bonds | front to front- formed from 2 s orbitals, 1 s orbital and 1 p orbital, or 2 p orbitals |
| pi bonds | the second line in a double bond and the second and third line in a triple bond- side to side- formed from 2 p orbitals, 1 p orbital and 1 d orbital, or 2 d orbitals |
| organic compounds are defined as | any compound that contains carbon (some exceptions) |
| carbocation | a molecule that gives carbon a positive charge, that carbon given this name |
| carboanion | a molecule that gives carbon a negative charge, the carbon is given this name |
| hydride | a hydrogen atom that has a lone pair |
| formal charge | represents the difference between the number of valence electrons in a neutral atom and the number of electrons assigned to that atom in the lewis structure |
| partial charge | forms when electrons are shared unevely in covalent bond giving one end a partially negative cahrge and the other a partially positive charge (usually polar) |
| resonance structures | a compound that can be represented in different lewis structures that share the same connectivity but differ in the arrangement of electrons |
| major contributors | the resonance structures of a certain compound that have greater stability; the more atoms that a structure has to delocalize electrons over the more stable |
| minor contributors | a resonance structure of a compound that has charge separations is higher in energy and is less stable |
| rules to draw resonance structures 1-2 | 1.all resonance structures must be valid lewis structures for the compound 2.only electrons- whether lone pairs, radicals, or bonding electrons- can be shifted between structures; the position of atoms must remain uchanged |
| bronsted-lowery acid | a molecule that can transfer a proton |
| bronsted-lowery base | a molecule that accepts a proton |
| lewis acid | a molecule or ion that transfers a pair of electrons |
| lewis base | a molecule or ion that accepts a pair of electrons |
| Ka | related to equillibrium values,-large values mean that the equillibrium shifts to the right favoring products; small values indicate an equillibrium shifting to the left in favor of reactants |
| pKa | -log (Ka)- when products are favored can be negative,; high=weak acid, low=strong acid |
| is pKb used in organic chemistry | no- can gain what we need from pKa and base acid-base strength off of that |
| the stronger the acid the stronger the base | the weaker the base the weaker the acid |
| how does bond strength affect acidity | the strength of the bond from which a proton is lost is crucial; the weaker the bond the easier it is to lose the proton, resulting in a stronger acid |
| how does electronegativity affect acidity | the electronegativity of the atom bonded to the proton also influences acidity; a more electronegative atom stabalizes the negative charge left after proton loss, making the acid stonger |
| how does the inductive effect affect acidity | even when electronegative atoms are not directly bonded to the ptoton they can influence acidity through the inductive effect;transmitting their electron;withdrawing effects through sigma bonds; this effect diminishes rapidly with distance from the proton |
| how does the resonance effect affect acidity | the ablility of the conjugate base to delocalize charge via resonance significantly increases acidity |
| electrophile | an electron pair acceptor |
| nucleophile | an electron pair donor |
| adduct | the product of a lewis acid-base reaction |
| leaving group | the group that accepts electrons from the breaking/broken bond |
| acid-base equilibria | products are favored when the conjugate acid is weaker than the original acid (drives equillibrium towards products); if conjugate acid is stronger than the original acid the equillibrium will shift to the left (favoring reactants) |
| only _______ move not ____________ | electrons; atoms |
| rules to draw resonance structures 3-4 | 3.the number of unpaired electrons (if any) must remain consistent across all resonance structures 4.the major resonance contributor is the structure whith the lowest energy; greatest stability |
| rules to draw resonance structures 5 | 5.the more delocalized a charge is over 2 or more atoms, the more stable the resonance structure |
| nirtic acid is a strong acid becasue of the presencce of __________ and the _____________ | (+) formal charge; resonance |
| sp is (high acidity/low acidity) | high |
| sp^2 is (higher acidity/lower acidity) | higher |
| sp^3 is (high acidity/low acidity) | low |
| when acids have a big difference in pKa does the reaction occur slowly/slightly or quickly/totally | quickly/totally |
| when acids have little differences in pKa does the reaction occur slowly/slightly or quickly/totally | slowly/slightly |
| when the pKa of a conjugate acid is lower than the acid in the reaction what does that mean and which way do we shift | the conjugate acid is more acidic and we will shift to the reactants (left) |
| when the pKa of a conjugate acid is higher than the acid in the reaction what does that mean and which way do we shift | the conjugate acid is less acidic and we will shift towards products (right) |
| any hydrogen has the potential to be | acidic |
| linear has a bond angle of | 180(no lone pairs); 180 (three lone pairs) |
| trigonal planar has a bond angle of | 120 |
| bent has a bond angle of | <120 (one lone pair); <109.5 (~105)(two lone pairs) |
| tetrahedral has a bond angle of | 109.5 |
| trigonal pyramidal has a bond angle of | <109.5 (~107) |
| trigonal bypyramidal has a bond angle of | 90;120 |
| see-saw has a bond angle of | <90;<120 |
| T-structure has a bond angle of | <90 |
| octehedral has a bond angle of | 90;90 |
| square pyramidal has a bond angle of | 90;<90 |
| square planar has a bond angle of | 90 |
Created by:
allijeli
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