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MCAT C/P > Electronic Structure (PHY, GC) > Flashcards

Electronic Structure (PHY, GC) Flashcards

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MCAT flashcards
1
Q

The electrons closer to the nucleus are at ___ energy levels, while those that are further out (in higher electron shells) have ____ energy.

A

lower, higher

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2
Q

Valence electrons have the ___ interactions with the surrounding environment and the ____ interactions with the nucleus.

A

strongest, weakest

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3
Q

Valence electrons are much more likely to become involved in bonds with other atoms because they experience the ___ electrostatic pull from their own ____.

A

least, nucleus

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4
Q

A positively charged ion

A

cation

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5
Q

A negatively charged ion

A

anion

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6
Q

The atomic mass of an atom (in amu) is nearly equal to the _____, which is the sum of the protons and neutrons

A

mass number

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7
Q

Atoms of the same element with varying mass numbers are called

A

isotopes

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8
Q

Isotopes differ in their number of ___

A

neutrons

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9
Q

Atomic weight

A

The weighted average of the different isotopes and is the number reported on the periodic table

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10
Q

Avogadro’s number

A

6.02 x 10 ^ 23

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11
Q

What does Avagadro’s Number represent?

A

The number of “things” (atoms, ions, molecules) in 1 mole

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12
Q

As electrons go from a lower energy level to a higher energy level, they get AHED

A

A: absorb light
H: higher potential
E: excited
D: distant (from nucleus)

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13
Q

When an electron returns to ground state,

A

it emits a photon with wavelength of energy it undergoes

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14
Q

The electromagnetic energy of photons equation

A 
E = hc/λ 
where 
h = Planck's constant
c = speed of light (3.0 x 10^8 m/s)
λ = wavelength of radiation
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15
Q

The energy of the emitted photon corresponds to the difference in energy between the _____-energy ___ state and the ___-energy ___ state

A

higher-energy initial state, lower-energy final state

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16
Q

a positive E corresponds to ___ and a negative E corresponds to ____

A

(+) E = emission

(-) E = absorption

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17
Q

According to the Pauli Exclusion Principle,

A

no 2 electrons in a given atom can possess the same set of 4 quantum numbers

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18
Q

Heisenberg Uncertainty Principle

A

It is impossible to simultaneously determine, with perfect accuracy, the momentum and the position of an electron

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19
Q

The principle quantum number, n: the larger the integer value of n, the ____ the energy level and radius of the electron’s shell

A

higher

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20
Q

Maximum number of electrons within a shell (equation)

A

2n^2

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21
Q

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

A

decreases

22
Q

angular momentum, l

A

refers to the shape and number of subshells

value of l ranges from 0 to (n-1)

23
Q 
l = 0 subshell is _
l = 1 subshell is _ 
l = 2 subshell is _
l = 3 subshell is _
A

s, p, d, f

24
Q

Maximum number of electrons within a subshell (equation)

A

4l +2

25
Q

magnetic quantum number, ml

A

specifies the particular orbital within a subshell where an electron is most likely to be found at a given moment in time.

26
Q

each orbital can hold a maximum of ___ electrons

A

two

27
Q

The possible values of ml are the integers between ___ and ___, including 0

A

-l and +l

28
Q

spin quantum number, ms

A

two spin orientations designated by +1/2 and -1/2

29
Q

Whenever two electrons are in the same orbital, they must have ____ spins

A

opposite

30
Q

Every element has a ____ atomic absorption and emission line spectrum

A

unique

31
Q

An _______ is the pattern of line formed when a light passes through a prism to separate it into the different frequencies of light it contains

  • each of these spectral lines corresponds to a different electron transition from a ___ energy state to a ___ energy state
A

atomic emission spectrum

  • higher, lower
32
Q

The n+l rule, used to rank subshells by ____ energy.

A

increasing

This rule states that the lower the sum of the values of the first and second quantum numbers, n + l, the lower the energy of the subshell.

–> if 2 subshells possess the same n+l value, the subshell with the lower n value has a lower energy and will fill with electrons first.

33
Q

The n+l rule in action,

Which will fill first, the 5d subshell or the 6s subshell?

A

The 6s will fill first

5d: n=5 + l=2 = 7
6s: n=6 + l=0 = 6

34
Q

The lowest s subshell is __, the lowest p subshell is __, the lowest d subshell is ___, and the lowest f subshell is ___

A

1s, 2p, 3d, 4f

35
Q

What is the electron configuration of osmium (Z = 76)?

*use noble gas abbreviation

A

[Xe]6s24f145d6

36
Q

What is the electron configuration of Fe3+?

A

[Ar]3d5

37
Q

Hund’s rule tells us that ___ and ___ orbitals have ___ energies (___ stability) than other states

A

half-filled, fully filled, lower energies, higher stability

38
Q

Hund’s rule creates 2 notable exceptions to electron configuration, chromium (and the other elements in its group) and copper (and the other elements in its group). What are the electron configurations of Chromium (Z=24) and Copper (Z=29)?

A

Chromium: [Ar]4s13d5

Copper: [Ar]4s13d10

39
Q

Paramagnetic of diamagnetic?
Materials composed of atoms with unpaired electrons will orient their spins in alignment with a magnetic field, thus be weakly attracted to the magnetic field

A

paramagnetic

–> mnemonic:
PARAmagnetic means that a magnetic field with cause PARAllel spins in unpaired electrons and thus cause an attraction

40
Q

Paramagnetic or diamagnetic?

Materials consisting of atoms that have only paired electrons will be slightly repelled by a magnetic field

A

diamagnetic

41
Q

The ____ ____ of an atom are those electrons that are in its _____ energy shell, are ____ ____ removed, and are available for _____.

A

valence electrons, outermost, most easily, bonding

42
Q

All elements in period ____ (starting with ___) and below may accept electrons into their d subshell, which allows them to hold more than eight electrons in their valence shell –> this allows them to violate the ___ ____.

A

three, sodium, octet rule

43
Q

The ____ is the net positive charge experienced by an electron in a multi-electron atom.

A

effective nuclear charge (Zeff)

44
Q

The _____ describes the ___ in the attraction between an electron and the nucleus in any atom with more than 1 electron shell.

A

shielding effect, decrease

45
Q

The more electron shells there are, the __ the shielding effect experienced by the outermost electrons.

A

greater

46
Q

The effective nuclear charge on an electron is given by the following equation:

A

Zeff = Z-S
Z is the number of protons in the nucleus (atomic #)
S is the number of electron between the nucleus and the electron in question (the number of non-valence electrons)

47
Q

The shielding effect explains why ____ electrons are ______ removed from the atom

A

valence-shell, more easily

48
Q

When light strikes materials, it can ____ electrons from them. This is called the ____ _____.

A

eject. photoelectric effect

49
Q

In the photoelectric effect, electrons are ____ from matter as a consequence of their _____ from electromagnetic radiation of high frequency (_____ wavelength), such as UV radiation.

A

emitted, absorption of energy, short

50
Q

If the energy of the light is such that the electron is ___ above ____ associated with the atom, the electron can break free from the atom leading to ____ of the atom. These escaping electrons are called ___.

A

excited, energy levels, ionization, photons

51
Q

Energy of a photon equation:

A

E = hf
h is Planck’s constant
f is the frequency of EM wave

52
Q

The energy required to knock off an electron is called the _____.

A

Ionization energy

MCAT C/P (6 decks)

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