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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  • The electronegativity of the atom with the negative charge
  • The size of the atom with the negative charge
  • Stabilization of the negative charge with resonance
  • Stabilization of the negative charge by adjacent electronegative atoms
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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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