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General Chemistry Flashcards

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1
Q

SF6 hybridization

A

sp3d2

  • angles are 90 degrees
  • octahedral
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2
Q

PCl5

A

sp3d

  • angles are 90, 120 degrees
  • trigonal bipyramidal
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3
Q

Enantiomers rotate plane-polarized light in what way?

A

To the same degree but in opposite directions

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4
Q

Chiral compounds are optically _____

A

Active

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5
Q

Plane-polarized light = _____

A

Photons oriented with electric field in same direction

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6
Q

Meso compound

A

Multiple chiral centers but is optically inactive

  • Plane of symmetry through center
  • Achiral
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7
Q

Epimers

A

Diastereomers that differ in configuration at only one chiral carbon

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8
Q

Chiral carbon of an anomer

A

Anomeric carbon

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9
Q

E (entogegen)

A

Higher priority substituents of double bond are on opposite sides

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10
Q

Z form for alkenes

A

Higher priority substituents of double bond are on zee zame zide

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11
Q

What molecules can form hydrogen bonds?

A

Any H attached to N, O, or F

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12
Q

What kinds of bonds are in noble gases?

A

London dispersion forces (induced dipole)

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13
Q

Are larger atoms more or less polarizable? Why?

A

Larger atoms = more polarizable b/c electrons can get farther from the nucleus and create a larger dipole moment

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14
Q

What does a decrease in enthalpy mean?

A

More stable product

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15
Q

As temperature increases, rate ______, and reaction time _______

A

Increases; decreases

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16
Q

How are the molarities of ideal gases related at the same temperature and pressure?

A

They are all the same

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17
Q

What is the relationship between mL and cm?

A

1 mL = 1 cm^3

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18
Q

Which are more stable: trans or cis?

A

Trans b/c less steric hindrance

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19
Q

Dissolving a solid in a liquid ______ boiling point and _______ freezing point

A

Increases boiling point, decreases freezing point

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20
Q

Break of two carbon chunks from saturated fatty acids and inject them into TCA as acetyl CoA is ______

A

Beta oxidation

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21
Q

Smaller percentage of oxygen in a molecule = _____ energy of substrate

A

More energy

  • C must be oxidized
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22
Q

Molecular geometry of molecule with three bonds and one lone pair

A

Trigonal pyramidal

  • Bond angles = 109.5˚
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23
Q

What is the enthalpy of formation of a pure element in its natural state?

A

Zero

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24
Q

Diastereomers and enantiomers differ because diastereomers can be _____

A

Separated by physical means (crystallization)

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25
Q

Naturally occurring products have what stereochemistry?

A

S

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26
Q

In a Fischer projection, the lower priority group is in what direction?

A

To the side

27
Q

How do you resolve enantiomers in a racemic mixture?

A

Enantiomers only react w/ chiral compounds => must use chiral molecule to resolve

28
Q

Stereospecificity

A

Different isomers => different products

29
Q

Stereoselective

A

Certain stereoisomer product dominates

30
Q

Relation b/w stereospecific and stereoselective

A

Any reaction that is stereospecific is also stereoselective

Stereoselective is not always stereospecific

31
Q

Oxidized OH = ______

A

Ketone or aldehyde

32
Q

How do enantiomers differ?

A
  • They have opposite observed rotations
  • They react differently with chiral molecules
  • Everything else is the same
33
Q

What is an enol?

A

Both an alkene and an alcohol attached to the same carbon

  • Can be tautomerized from a ketone
34
Q

Meso compounds

A
  • Achiral, but do contain chiral carbons
  • Line of symmetry
  • Due to being achiral => do not rotate plane-polarized light (not optically active)
35
Q

Chiral molecules

A

Non-superimposable mirror images

36
Q

Most stable conformation isomer = _____

A

Anti

37
Q

What type of molecules do H bonds form b/w?

A

Partially positive H (bound to N, O, F) and partially negative electronegative atom (N, O, F)

38
Q

Heat of formation

A

Change in energy from elemental form to experimental form

39
Q

Formula for heat of formation for a reaction

A

(∆Hf˚ of products) - (∆Hf˚ of reactants)

  • Must multiply each ∆Hf˚ by they number of moles for that product
40
Q

What is the effect of adding solute on the freezing point?

A

Freezing point depression

  • Solute makes it harder for liquid to form crystalline structure
41
Q

What is the effect of adding solute on the boiling point?

A

Boiling point elevation

  • Makes it more difficult for molecules to escape as vapor => need higher temperature
  • Decreases vapor pressure
42
Q

Strongest solid structure

A

Covalent network

  • Covalent bonds are the strongest
  • Very high melting point
43
Q

What type of bonds are hydrogen bonds?

A

Non-covalent bonds

44
Q

Are ammonium and Group 1 salts water soluble?

A

Yes

45
Q

Are salts with NO3 and acetate (CH3COO-) water soluble?

A

Yes

46
Q

Are halides soluble?

A

Yes, except for fluorides or unless formed with Ag, Pb, or Hg2

47
Q

Are salts with sulfate (SO42-) water soluble?

A

Yes, except for those formed with Ca, Sr, Ba, and Pb

  • Bapbcasr
48
Q

Are metal oxides soluble?

A

No, unless formed w/ alkali metals, ammonium, and CaO, SrO, and BaO

49
Q

Are hydroxides soluble?

A

No, unless formed w/ alkali metals, ammonium, Ca, Sr, or Ba

50
Q

Are carbonates (CO3), phosphates, sulfides, and sulfites soluble?

A

No, unless formed w/ alkali metals or ammonium

51
Q

In an electrochemical cell, where does oxidation take place? What about reduction?

A 
Oxidation = anode
Reduction = cathode

An Ox
Red Cat

52
Q

What is the difference between Galvanic and Electrolytic cells?

A
  • Galvanic house spontaneous reactions w/ positive electromotive force
  • Electrolytic house nonspontaneous reactions w/ negative emf
53
Q

Standard electromotive force

A

Difference in standard reduction potential b/w two half-cells

  • Positive for galvanic cells
  • Negative for electrolytic cells
54
Q

Relation b/w E˚ and ∆G˚

A
  • When E is positive, ∆G is negative (galvanic)
  • When E is negative, ∆G is positive (electrolytic)
  • When E is 0, ∆G is 0 (concentration cells)
55
Q

Most stable conformation for cyclic molecules have heavier groups in _____ position

A

Heavier = equatorial

56
Q

Torsional strain

A

Repulsion b/w electrons in bonds that do not share an atom

  • Occurs in eclipsed bonds
57
Q

Steric strain

A

How close molecules are to each other

58
Q

Isoprene

A

5 carbons

59
Q

For establishing stereoconfiguration, where should the lowest priority group be pointing?

A

Away (dash)

  • If it’s pointing towards you, configuration will be the opposite of what it looks like
    (if it looks R when lowest priority is towards you, it will actually be S)
60
Q

Formula for number of stereoisomers

A

2^n

  • n = number of chirality centers
61
Q

Enantiomers have _____ configurations at which chirality centers?

A

Opposite configurations at all chirality centers

62
Q

Diastereomers have _____ configurations at which chirality centers?

A

Opposite configurations at some chirality centers

63
Q

What should you look for to determine cis or trans?

A

Two identical groups on opposite sides of the double bond

Chemistry (4 decks)

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