Chem 1 – Chemistry Test Questions – Flashcards
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pKa |
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pKa = -log KaKa is the acid dissociation constant.Ka is the equilibrium constant for the dissociation of a weak acid.Acid dissolves producing Hydronium ions and conjugate baseHA H+ + A- Ka = [H+][A-] / [HA]pKa = -log Ka |
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Bronsted acid |
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H+ donorproton(H) donorhas an H+ that can be easily ripped off by a base |
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Bronsted Base |
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H+ acceptorproton (H) acceptorable to pull off H+ from an acid |
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Lewis Acid |
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Electron pair acceptor |
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Lewis Base |
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electron pair donor |
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Strength of an acid is based on... |
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...the stability of it's conjugate base |
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strong acids have ___________ conjugate bases |
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strong acids have stable conjugate bases |
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A weak acid has a less/more stable conjugate base than a strong acid |
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A weak acid has a LESS stable conjugate base than a strong acid |
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conjugate base |
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the acid once it has been deprotonated |
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Features that determine the stability of a negative charge: |
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Which is more acidic?H2 OR NH3water ammonia |
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Water |
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Which is more electronegative? oxygen or nitrogen |
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Oxygen |
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Negative charges prefer to rest on larger atoms because... |
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The charge can be spread over a much larger region of space. This makes it more stable. |
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Which is more acidic? HI or HF |
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HIF- is more electronegative than I-, but, I- is significantly larger than F-SIZE TRUMPS ELECTRONEGATIVTY |
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Why is phenol a million times stronger acid than cyclohexanol?[image] |
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Because the conjugate base of phenol is more stable than the conjugate base of cyclohexanol.Phenol's conj base has a resonance structure. The anion can delocalize the negative charge throughout the ring through resonance. Thus stabilizing it. Cyclohexanol's conj base has no resonance structure.cyclohexane is a weaker acid!![image] |
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Acetic acid |
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ethanoic acidCH3COOHa carboxylic acid |
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CH3COOH |
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[image] |
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Acetic Acid |
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[image] |
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Why is [image] the Chlorine substitued acetic acid more acidic than the hydrogen containing acetic acid? |
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The electronegative Chlorine atom is pulling some of the electron density away from the oxygens, making the oxygens not having to bear all of the negative charge by themselves. |
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Alkanes |
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Have the formula:CnH2n+2Hydrogen saturated since they have the maximum number of hydrogens possible |
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Hydrocarbons that contain a single alkene or a single ring... |
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...contain a single degree of unsaturationbecause adding either a ring or a double bond requires the loss of two hydrogens.CnH2n |
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Calculate the Degrees of Unsaturation |
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Degrees of Unsaturation = [(Number of Carbons x 2) + 2 - Number of Hydrogens] / 2Halides(F, Cl, Br, I) count as hydrogensNitrogen counts as a 1/2 |
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Double bonds add _____ degree(s) of unsaturation Rings add _____ degree(s) of unsaturation. Triple bonds add _____ degree(s) of unsaturation. |
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Double bonds add ONERings add ONETriple bonds add TWO degree(s) of unsaturation. |
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alkyne |
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need a definition for alkyne |
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Methane |
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CH4 |
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Ethane |
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CH3CH3 |
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Propane |
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CH3CH2CH3 |
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Propyl |
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three carbon alkyl substituent-C3H7 |
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Isopropyl Alcohol |
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also isopropanolpropan-2-ol[image]isomer of propanol |
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Isopropyl Alcohol |
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also isopropanolpropan-2-ol[image]isomer of propanol |
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propylene |
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propeneC3H6 |
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first and second simplest alkene |
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ethylene (ethene)C2H4propeneC3H6[image] |
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trans cis (high/low priority) |
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trans: opposite sides "E" cis: same sides "Z" |
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bp of butane vs. bp of isobutane |
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butane bp: -.5oisobutane bp: -11.7o |
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carbocation |
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positively charged carbon atom |
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styrene |
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[image]C6H5CH=CH2 |
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vinyl |
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also called ethanyl-CH=CH2a derivative of ethylene[image] |
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ethyl |
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-C2H5Abbreviated -Et[image] |
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alkyl |
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formula:CnH2n+1ex:methylethylbutyletc.very reactive when by itself. it is a free radical |
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[image] |
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tert-butyl |
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[image] |
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sec- 1-methylpropyl |
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constitutional isomer |
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same formula different connectivity |
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conformational isomer |
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same connectivity, same formula just rotated around a bond |
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nucleophile |
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electron rich nucleus loving |
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electrophile |
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electron loving electron deficient |
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What removes the mercury in an oxymercuration reaction? |
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Sodium Boro-hydrateNaBH4 |
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di-ethyl ether |
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CH3-CH2-O-CH2-CH3[image] |
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effect of halogens and other electronegative groups |
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electron withdrawing polar effect they will PULL electrons toward themselves and away from the carbon |
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electron donating polar effect |
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some groups will raise the pKa or reduce the acidity of nearby carboxylic acid groups. |
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what are 2 structural effects that affect Bronsted acidity? |
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Element effect polar effect element effect is dominated by the change in bond dissociation energies with a column and by the change in electron effiniies within a row polar effect: caused by the interactions of charges formed in the acid-base reaction with polar bonds or other charged groups in the acid or base molecule |
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if you have more substituents, then it is More/less stable |
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MORE stable because of the hyperconjugation |
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donates a proton |
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bronsted acid |
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accepts a proton |
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bronsted base |
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katilin |
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put this word in bold |