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MCAT: General Chemistry > Chapter 1: Atomic Structure > Flashcards

Chapter 1: Atomic Structure Flashcards

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1
Q

Do electrons closer to the nucleus have higher energy, or farther?

A

Farther electrons have higher energies

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2
Q

What is the atomic number?

A
  • Z
  • Number of protons
  • Bottom number
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3
Q

What is the mass number?

A
  • A
  • Sum of an element’s protons and neutrons
  • Top number
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4
Q

What is the atomic mass?

A

Essentially equal (slightly less) to the mass number

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5
Q

What is atomic weight?

A
  • Weighted average of the naturally occurring isotopes in an element
  • Periodic table lists atomic weight
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6
Q

How does n influence the energy of an electron?

A

As n increases, the energy values approach zero from a more negative value

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7
Q

“As electrons go from a lower energy level to a higher energy level, they get AHED”: what does this mean?

A
  • Absorb light
  • Higher potential
  • Excited
  • Distant (from the nucleus)
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8
Q

According to Planck’s equation, what is a positive E? What is a negative E?

A
  • Positive: Emission (jumping to a lower energy level)

- Negative: Absorption (jumping to a higher energy level)

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9
Q

What is an orbital?

A

Region of space around a nucleus defined by the probability of finding an electron in that region of space

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10
Q

What is the Heisenberg uncertainty principle?

A

It is impossible to know both an electron’s position and its momentum exactly at the same time.

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11
Q

What is the principle quantum number?

A
  • n

- Describes the average energy of the shell

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12
Q

What is the azimuthal quantum number?

A
  • l
  • Describes the subshell within a given principle energy level
  • Shape of the orbital
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13
Q

For any given value of n, what is the range of possible values of l?

A

0 to (n-1)

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14
Q

What is the maximum number of electrons within a subshell?

A

4l + 2

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15
Q

What is the l value of the s, p, d, and f orbitals?

A
  • s: 0
  • p: 1
  • d: 2
  • f: 3
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16
Q

What is the magnetic quantum number?

A
  • Specifies the particular orbital within a subshell where an electron is likely to be found at a given moment in time
  • Orientation
17
Q

For any given value of l, what are the possible values of ml?

A
  • l to + l
18
Q

What is the maximum number of electrons within a shell?

A

2n^2

19
Q

What is the number of orbitals?

A

n^2

20
Q

What is the spin quantum number?

A
  • Indicates the spin orientation of an electron in an orbital
  • +1/2 = up
  • -1/2 = down
21
Q

What does the Pauli exclusion principle state?

A

No two electrons in a given atom can possess the same set of four quantum numbers.

22
Q

What is the 4f subshell?

A
  • Lanthanide series

- 14 elements

23
Q

What happens when you are in the d subshell in the periodic table?

A
  • You must subtract n-1, which becomes the number preceding d
  • Example: when n = 4, it is 3d, and not 4d
24
Q

What is Hund’s rule?

A

Subshells with multiple orbitals (p, d, and f) fill electrons so that every orbital in a subshell gets one electron before any of them get a second.

25
Q

What does paramagnetic mean?

A
  • Unpaired electrons that align with magnetic fields

- Attracting the material to a magnet.

26
Q

What dos diamagnetic mean?

A
  • All paired electrons

- Cannot easily be realigned; they are repelled by magnets.

27
Q

What is the actual configuration of chromium?

A

(Ar)4s1 3d5

28
Q

What is the actual configuration of copper?

A

(Ar) 4s1 3d10

29
Q

Where are valence electrons found for representative elements?

A

s and/or p-orbitals

30
Q

Where are valence electrons found for transition elements?

A

s and either d- or f-orbitals

31
Q

What is the Aufbau principle?

A

Electrons fill from lower- to higher-energy subshells, and each subshell will fill completely before electrons begin to enter the next one.

32
Q

Which equation allows you to tell which subshell would fill first?

A

o The lower the sum of the values of n + l, the lower the energy of the subshell, which would fill first.
o If two subshells possess the same n + l value, the subshell with the lower n value fills first.

MCAT: General Chemistry (4 decks)

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