Chem/Phys 1 Flashcards by Danielle Kapustin

formula for degrees of unsaturation

(2C+2)-H / 2

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Bronsted-Lowry acid vs base

acid gives H+, base receives H+

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Lewis acid vs base

acid=electron pair acceptor, base= electron pair donor

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epimers

a type of diastereomer that differs at exactly 1 chiral center

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meso compounds

achiral, must contain at least 1 chiral center, have an internal plane of symmetry

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speed of light (in a vacuum)

3 x 10^8 m/s

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electric charge of a proton/electron

1.6 x 10^-19

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density of water

1000 kg/m^3

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3 kinematic formulas

Vf=Vi + at, Vf^2=Vi^2 t +2ad, d=Vi t +1/2at^2

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Newton’s first law

F=ma

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Friction formula

mu x normal force

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1 cm^3= ___ L?

1 mL= .001 L

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ionization energy trend

Ionization energy is the amount of energy required to remove an electron. As radius decreases and number of protons increases, its harder to remove an electron. So ionization energy increases towards the direction of NY where there is the most energy.

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Electron affinity

Energy change (energy required/released) to add an additional electron. If energy is released, the energy change is negative and electron affinity is negative. If energy is required to add an electron, electron affinity is positive

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relationship between visible light, energy, wavelength, frequency and which colors are highest/lowest energy

red has the longest wavelength and lowest energy, violet has the shortest wavelength and highest energy (E = hν = hc/λ where v=frequency and gamma is the wavelength)

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diamagnetic vs paramagnetic

diamagnetic=all electrons are paired and atom is REPELLED by an external magnetic field. Paramagnetic=unpaired electrons and atom is ATTRACTED to an external magnetic field

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alpha decay

alpha particle (2 protons and 2 neutrons) is emitted in order to become more stable, reducing the atomic number by 2 and teh mass number by 4

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beta decay

conversion of a neutron to a proton, and an electron is emitted. Atomic number increases by one but mass number remain the same

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electron capture

capture an electron from the n=1 shell and use it to convert a proton into a neutron. Atomic number is decreased by one and mass number remains the same

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Gamma decay

photon is emitted which changes neither mass number nor atomic number

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how many moles per liter of pure water

55 moles of water in 1 L

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solubility rules

NAG SAG: Nitrates, acetates, Group 1, Sulfates, Ammonium, Group 17. Exceptions are PMS: Pb, Mercury (Hg), Silver

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Mixing solutions formula

CV+CV=CV final

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polar bonds are shorter/equal/longer than non-polar bonds

shorter because polar bonds are stronger than nonpolar bonds

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what does anhydrous mean

anhydrous means in the absence of water

visible light region wavelengths

400 nm (violet) to 700 nm (red).

formal charge

formal charge = valence e for that element – ½(bonding electrons) – lone electrons (FC=V- B/2 - L)

which atoms form only 3 bonds? (6 valence electrons)

B and Al (and some other group 3 atoms)

which atoms can make 5 bonds?

Si, P, S, Cl

fusion vs vaporization vs crystallization vs condensation vs sublimation vs deposition

fusion=melting, vaporization=boiling, condensation=gas to liquid, crystallization=liquid to solid, sublimation=solid to gas, deposition=gas to solid

relationship between heat capacity/specific heat and temperature change

high specific heat=smaller change in temp

1 calorie = ___ Joules

4.2

specific heat equation

q=mc(delta t)

effect of pressure on water melting

increased pressure on ice results in increased melting. Increased pressure=decreased melting point, decreased pressure=increased melting point

volatile

easily evaporated, weakest IMFs

which gasses behave most ideally?

weakest IMFs and smallest molecular weights/volumes

structure of diamond

all carbon- only covalent bonds

Standard temperature and pressure

1 atm and 0 degrees C

volume of an ideal gas (per mole)

22.4 L per 1 mole sample of gas

Avogadro's number (# of particles in a mole) approximated

6x10^23

1 atm = ___ torr

760

760 torr= ___mmHG

760

1 atm=___kPa

101

celcius to kelvin

C+273=K

2 factors relevant to gas behavior

IMFs and molecular weight

where on a heating curve can you get the specific heat (c)

the slope

prefix for 4 carbons

but-

prefix for 2 carbons

eth-

Rf value

distance traveled by individual component / distance traveled by solvent

IR stretch of carbonyls (C=O)

1700 cm-1, very strong and intense "v" shape

IR stretch of alkenes (C=C)

1650 cm-1

IR stretch of triple bond (C≡C)

2260-2100 cm-1

IR stretch of alcohols (O-H)

2600-3200 cm-1 very strong and very broad "U" shape (broadness is due to H bonding)

IR stretch of N-H bond

3150-2500

which base only deprotonates carboxylic acids?

weak base solvents like NaHCO3 (sodium bicarbonate)

which base deprotonates phenols AND carboxylic acids?

strong base solvents like NaOH

which acid protonates amines?

strong acids (HCl)

are amines nucleophiles or electrophiles?

nucleophiles because they have a lone pair to donate

isochoric process

constant volume so deltaE=Q

units of Pa

J/m^3

in a closed system, if internal energy increases, what happens to temperature?

temperature increases

L amino acid vs D amino acid

amino group on the left=L, amino group on the right=D

acidic amino acids

D (aspartate) and E (glutamate)

basic amino acids

lysine (K), arginine (R), histidine (H)

amino acids with aromatic side chains

Tryptophan (W), Phenylalanine (F), Tyrosine (Y)

Strecker synthesis of amino acids

aldehyde becomes an immine, then H is replaced with CN, then acid workup to become COOH

Gabriel Malonic ester synthesis

phthalimide + KOH is deprotonated, then attacks alkyl halide via SN2, decarboxylation

Zwitterion

amino acid ion where net charge is 0, at pI

determining L or D of carbohydrates

look at second to last (penultimate) carbon with an OH. OH groups attacks the anomeric carbon to form a ring.

Anomeric carbon of a carbohydrate

the carbon attached to 2 oxygens in a ring which was initially a COOH group on the end.

Benedict's test

Cu2+ reagent reduces aldehyde of a sugar into a COO- group and Cu precipitate

a vs b glycosidic linkages

a is when oxygen group is down, b is when oxygen group is up. look at carbon attached to 2 oxygens

Size exclusion chromatography

used to separate proteins, small proteins get stuck in beads, large proteins eluded

Thin-Layer chromatography and column chromatography

used to separate based on polarity, stationary phase is polar, mobile phase is nonpolar

reverse phase HPLC (reverse phase High performance liquid chromatography)

nonpolar stationary phase and polar mobile phase, polar eludes first

Ion Exchange Chromatography

used to separate proteins based on charges

Affinity Chromatography

lock and key interactions drive separation. Used to separate proteins from a biochemical mixture

ELISA

used to determine the presence of antigens or antibodies

Blotting (South, North, West)

South=DNA, North=RNA, West/East=proteins (SNOW DRoP)

Gas chromatography and distillation

separation based on volatility/boiling point, low boiling point substances get stuck and are eluded as liquids

extraction (solvents)

separation based on solubility on polar/nonpolar solvents

Resolution of enantiomers techniques

convert enantiomers to diasteriomeric salts, separate salts, then revert salts to their original enantiomers

Mass spectroscopy

used to determine molecular weight and elemental/isotopic composition

UV/Vis spectroscopy

indicates the presence of a conjugated pi system. As conjugation increases, wavelength absorbed increases (appears more green)

IR spectroscopy

used to distinguish between molecules with different functional groups

H-NMR

measures nonequivalent hydrogens. Splitting pattern=n+1=number of nonequivalent neighboring hydrogens. Area under signal (integration)=# of Hs represented by the signal

isochoric

volume is constant, no work being done

isobaric

pressure is constant, expansion. Work done is the area under the curve of pressure and volume.

isothermal

temperature is constant, work is done as volume increases

Chem/Phys 1 Flashcards

(89 cards)