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MCAT > Chimica (Italia) > Flashcards

Chimica (Italia) Flashcards

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1
Q

what are the structural and condensed formulas of an alcohol

A

R - O - H
ROH

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2
Q

what are the structural and condensed formulas of an aldehyde

A

R - C(=O) - H
RCHO

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3
Q

what are the structural and condensed formulas of an amide

A

R - C(=O) - N(-H) - H
RCONH2

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4
Q

what are the structural and condensed formulas of an amine

A

R - N(-H) - H
RNH2

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5
Q

what are the structural and condensed formulas of a carboxylic acid

A

R - C(=O) - O - H
RCOOH

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6
Q

what are the structural and condensed formulas of an ester

A

R - C(=O) - O - R’
RCOOR’

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7
Q

what are the structural and condensed formulas of an ether

A

R - O - R’
ROR’

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8
Q

what are the structural and condensed formulas of a halide

A

can be -Cl, -Br, -F, or -I
RCl

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9
Q

what are the structural and condensed formulas of a ketone

A

R - C(=O) - R’
RCOR’

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10
Q

what are the standard conditions

A

25˚C or 298.15 K
1 atm (101.325 kPa)
1 M

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11
Q

how many liters are in a mole at standard conditions?

A

22.4 L

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12
Q

how do you convert between C˚ and F˚?

A

F˚ = (9/5)C˚ +32

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13
Q

how do you convert between C˚ and K

A

K = C˚ + 273.15

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14
Q

what is the freezing point of water in C˚, F˚, and K?

A

0˚C
32˚F
273.15 K

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15
Q

what is the boiling point of water in C˚, F˚, and K?

A

100˚C
212˚ F
373.1 K

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16
Q

what is the fundamental unit of charge

A

e
1.6x10^-19 C

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17
Q

what is the charge and mass of protons

A

+1 ; 1 amu

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18
Q

what is the atomic number (Z) of an element?

A

unique identifier for each element ; equal to the number of protons found in an atom of that element

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19
Q

what is the charge and mass of neutrons

A

0 (neutral) ; ~1 amu (slightly larger than protons)

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20
Q

what is the mass number (A) of an atom?

A

the sum of the protons and neutrons in an atom’s nucleus
- atoms of the same element always have the same atomic number but not always the same mass number (isotopes)

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21
Q

what are isotopes?

A

atoms that share an atomic number but have different mass numbers due to a different number of neutrons

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22
Q

how many naturally occurring isotopes does carbon have?

A

3
12/6C, 13/6C, 14/6C

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23
Q

how many naturally occurring isotopes does hydrogen have and what are their names?

A

3
1/1H (protium)
2/1H (deuterium)
3/1H (tritium)

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24
Q

what is the charge and mass of electrons

A

-1 ; 1/2000 that of a proton’s mass

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25
Q

why is the electrostatic force of attraction between subatomic particles greater than the gravitational force?

A

because their masses are so small

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26
Q

the electrons closer to the nucleus are at lower or higher energy levels?

A

closer, lower
farther, higher

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27
Q

what are valence electrons?

A

electrons that are farthest from the nucleus and thus have the strongest interactions with the surroundings and weakest with the nucleus
- generally determine the reactivity of an atom

28
Q

a positively charged atom is called a ______ and a negatively charged atom is an _______

A

cation; anion

29
Q

what is the size/definition of the atomic mass unit

A

1/12 the mass of the carbon-12 atom
approximately 1.66 x 10^-24 g

30
Q

do isotopes exhibit similar chemical properties?

A

yes, because they have the same number of protons and electroons

31
Q

the atomic mass of an atom (in amu) is nearly equal to its _______

A

mass number (has to do with sum of protons and neutrons for that particular atom)

32
Q

what is the atomic weight

A

the weighted average of the different isotopes of an element
- also represents the mass of one mole of that element in grams
- in nature, isotopes are usually present in standard proportions
- this is the number reported on the periodic table

33
Q

how are half-life, stability, and proportions of isotopes related?

A

An isotope’s half-life is directly related to its stability, meaning that a longer half-life indicates a more stable isotope. Also, more stable isotopes are generally found in greater proportions.

34
Q

what are the two main naturally occurring isotopes of chlorine

A

chlorine-35 and chlorine-37
chlorine-35 is about three times more abundant than chlorine-37

35
Q

what is Avogadro’s number

A

6.02 x 10^23
the number of ‘things’ (atoms, molecules, ions) in a mole

36
Q

what is the Planck relation

A

relation that determines the energy of a quantum (discrete bundle in which energy is emitted)
E = hf
h = Planck’s constant (6.626 x 10^ -34 J⋅s)
f = frequency of the radiation

37
Q

what is Bohr’s equation for the angular momentum of an electron

A

L = nh / 2pi

n = principle quantum number
h = Planck’s constant
shows that the angular momentum of an electron changes only in discrete amounts with respect to n

38
Q

what is Bohr’s equation for the energy of an electron

A

E = - RH / n^2

RH = Rydberg unit of energy (2.18 x 10^-18 J/electron)

  • a value of 0 energy is assigned to a state in which the proton and electron are so far that there is no attractive force
  • the negative sign shows that the energy of an electron increases (becomes less negative) the farther out from the nucleus it is (increasing n)
  • the magnitude of the fraction is getting smaller, but the actual value it represents is getting larger (less negative)
39
Q

what is the ground versus excited state of an atom

A

ground state - state of lowest energy where all electrons are in the lowest possible orbitals

excited state - at least one electron has moved to a subshell of higher than normal energy

40
Q

(mnemonic)
as electrons go from a lower energy level to a higher energy level, they get _______

A

AHED
Absorb light
Higher potential
Excited
Distant (from nucleus)

41
Q

when electrons go from higher to lower energy levels, what is emitted?

A

discrete amounts of energy (E = hf) in the form of photons

E = hf = hc / λ = RH [1/ni^2 - 1/nf^2]
c = speed of light
λ = wavelength

42
Q

what is the speed of light in a vacuum

A

c = 3.00 x 10^8 m/s

43
Q

T or F: the wavelengths in an element’s absorption and emission spectra are the same

A

True
- the difference in energy between levels remains unchanged so whether you’re absorbing (going up) or emitting (going down) it’s the same change in energy

44
Q

What is the key takeaway from atomic and emission spectra?

A

unique for each element as each element has a characteristic set of energy levels
- for electrons to move between levels they must absorb or emit the right amount of energy to do so in the form of light

45
Q

what is the Pauli exclusion principle

A

no two electrons in a given atom can possess the same set of 4 quantum numbers
- no more than 2 electrons can occupy the same orbital
- 2 electrons in the same orbital must have opposite spins

46
Q

what is the Heisenberg uncertainty principle?

A

it is impossible to simultaneously determine the momentum and the position of an electron

47
Q

what is an electron’s energy state

A

its position and energy as described by its quantum numbers

48
Q

what is the principal quantum number?

A

n ; can theoretically take on any positive integer value
the larger the integer, the higher the energy level and radius of the electron’s shell

49
Q

what is the equation for maximum number of electrons within a shell

A

2n^2

50
Q

the difference in energy between two shells _________ as distance from the nucleus increases

A

decreases

51
Q

what is the azimuthal quantum number

A

l (angular momentum)
- refers to the shape and number of subshells within a given principal energy level/shell
- has implications about chemical bonding and bond angles
- limited from values 0 to (n - 1)
- energies of subshells increase with increasing l value (but there will be overlap if different n, for example 4s has lower energy than 3d)

52
Q

what is the spectroscopic notation of each subshell

A

l = 0 subshell is s
l = 1 subshell is p
l = 2 subshell is d
l = 3 subshell is f

53
Q

what is the equation for maximum number of electrons within a subshell

A

4l + 2

54
Q

what is the magnetic quantum number

A

m(l)
specifies the particular orbital within a subshell where an electron is most likely to be found

55
Q

each orbital can hold a maximum of ______ electrons

A

2

56
Q

what are the possible values of m(l)

A

-l to l, including 0

57
Q

how many orbitals in each subshell?

A

s = 1
p = 3
d = 5
f = 7

58
Q

what is the spin quantum number

A

m(s)
- there are two spin orientations for electrons (+1/2, -1/2)

59
Q

what are paired vs parallel electrons

A

paired electrons - two electrons in the same orbital and thus with opposite spins

parallel electrons - electrons in different orbitals with the same m(s) values

60
Q

what is the Aufbau principle

A

electrons fill from lower to higher energy subshells and each subshell will fill completely before electrons enter the next one

61
Q

what is the n + l rule

A

can be used to rank subshells by increasing energy
- the lower the sum of n + l, the lower the energy
- if you have two with the same n + l value, the lower n value is lower energy

62
Q

how do you write the electron configurations of ions

A

for anions, add electrons
for cations, subtract electrons (subtract from the highest value for n first, if there is a tie use highest l value)

63
Q

what is Hund’s rule

A

within a given subshelll, orbitals are filled such that there is a maximum number of half-filled orbitals with parallel spins (basis for this is electron repulsion)

64
Q

what are the two notable exceptions to standard electron configuration

A

chromium and copper (and their groups)
- will take one electron from 4s subshell and add it to 3d because half-filled (chromium) and filled (copper) orbitals have lower energy (and thus higher stability) than other states
- this sometimes happens in f blocks but never in p

65
Q

what are paramagnetic vs diamagnetic materials

A

paramagnetic - materials that are made up of atoms with unpaired electrons that will orient their spins in alignment with a magnetic field (attracted)

diamagnetic - materials consisting of atoms made of only paired electrons that are slightly repelled by magnetic field

66
Q
A
67
Q
A

MCAT (10 decks)

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