Chem 1 – Chemistry Test Questions – Flashcards
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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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|
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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 |
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