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MCAT > Chimica (Italia) > Flashcards

Chimica (Italia) Flashcards

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
why is the electrostatic force of attraction between subatomic particles greater than the gravitational force?
because their masses are so small
26
the electrons closer to the nucleus are at lower or higher energy levels?
closer, lower farther, higher
27
what are valence electrons?
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
a positively charged atom is called a ______ and a negatively charged atom is an _______
cation; anion
29
what is the size/definition of the atomic mass unit
1/12 the mass of the carbon-12 atom approximately 1.66 x 10^-24 g
30
do isotopes exhibit similar chemical properties?
yes, because they have the same number of protons and electroons
31
the atomic mass of an atom (in amu) is nearly equal to its _______
mass number (has to do with sum of protons and neutrons for that particular atom)
32
what is the atomic weight
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
how are half-life, stability, and proportions of isotopes related?
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
what are the two main naturally occurring isotopes of chlorine
chlorine-35 and chlorine-37 chlorine-35 is about three times more abundant than chlorine-37
35
what is Avogadro's number
6.02 x 10^23 the number of 'things' (atoms, molecules, ions) in a mole
36
what is the Planck relation
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
what is Bohr's equation for the angular momentum of an electron
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
what is Bohr's equation for the energy of an electron
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
what is the ground versus excited state of an atom
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
(mnemonic) as electrons go from a lower energy level to a higher energy level, they get _______
AHED Absorb light Higher potential Excited Distant (from nucleus)
41
when electrons go from higher to lower energy levels, what is emitted?
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
what is the speed of light in a vacuum
c = 3.00 x 10^8 m/s
43
T or F: the wavelengths in an element's absorption and emission spectra are the same
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
What is the key takeaway from atomic and emission spectra?
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
what is the Pauli exclusion principle
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
what is the Heisenberg uncertainty principle?
it is impossible to simultaneously determine the momentum and the position of an electron
47
what is an electron's energy state
its position and energy as described by its quantum numbers
48
what is the principal quantum number?
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
what is the equation for maximum number of electrons within a shell
2n^2
50
the difference in energy between two shells _________ as distance from the nucleus increases
decreases
51
what is the azimuthal quantum number
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
what is the spectroscopic notation of each subshell
l = 0 subshell is s l = 1 subshell is p l = 2 subshell is d l = 3 subshell is f
53
what is the equation for maximum number of electrons within a subshell
4l + 2
54
what is the magnetic quantum number
m(l) specifies the particular orbital within a subshell where an electron is most likely to be found
55
each orbital can hold a maximum of ______ electrons
2
56
what are the possible values of m(l)
-l to l, including 0
57
how many orbitals in each subshell?
s = 1 p = 3 d = 5 f = 7
58
what is the spin quantum number
m(s) - there are two spin orientations for electrons (+1/2, -1/2)
59
what are paired vs parallel electrons
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
what is the Aufbau principle
electrons fill from lower to higher energy subshells and each subshell will fill completely before electrons enter the next one
61
what is the n + l rule
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
how do you write the electron configurations of ions
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
what is Hund's rule
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
what are the two notable exceptions to standard electron configuration
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
what are paramagnetic vs diamagnetic materials
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
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MCAT (13 decks)

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