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MCAT > General Chemistry Ch. 1 > Flashcards

General Chemistry Ch. 1 Flashcards

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MCAT flashcards
1
Q

Atomic number =

A

of protons

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2
Q

The mass of one proton is approximately _

A

1 amu

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3
Q

Mass number =

A

of neutrons + # protons

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4
Q

Which is larger: neutron or proton mass?

A

Neutron mass

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5
Q

Define isotope

A

atoms with the same atomic number (# protons) but different mas number (# neutrons)

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6
Q

The reactivity of an atom is determined by ___

A

Valence electrons

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7
Q

Atomic mass ~~ __

A

Mass number

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8
Q

List and describe the Hydrogen isotopes:

A

1H1 (Protium)
2H1 (Deuterium)
3H1 (Tritium)

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9
Q

Define atomic weight

A

The weighted average of isotopes of that element

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10
Q

Define Avogadro’s number

A

number of units in one mole of any substance (defined as its molecular weight in grams), equal to 6.02214076 × 10^23

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11
Q

Define quanta

A

Energy emitted as electromagnetic radiation in discrete bundles

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12
Q

Define Planck’s constant

A

Relates the energy in one quantum (photon) of electromagnetic radiation to the frequency of that radiation. 6.626176 x 10-34 joule-seconds

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13
Q

The energy of an electron (decreases/increases) the farther out from the nucleus

A

Increases

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14
Q

As electrons go from a lower energy to higher energy level, they get AHED. List the meaning of the acronym.

A

Absorb light
Higher potential
Excited
Distant from nucleus

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15
Q

What is the speed of light in a vacuum?

A

3.00 x 10^8 m/s

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16
Q

List the Hydrogen emission lines

A

1) Lyman series
2) Balmer series
3) Paschen series

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17
Q

Describe the lyman series

A

Hydrogen spectral series of transitions and resulting ultraviolet emission lines of the hydrogen atom as an electron goes from n ≥ 2 to n = 1

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18
Q

The (Lyman/Balmer) series has larger energy transitions

A

Lyman

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19
Q

Describe the Balmer series

A

Series of spectral emission lines of the hydrogen atom that result from electron transitions from higher levels (n ≥ 3) down to the energy level with principal quantum number 2, resulting in four wavelengths emitted in the visible region

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20
Q

Describe the Paschen series

A

A sequence of absorption or emission lines in the near-infrared part of the spectrum, due to hydrogen. They are caused by electron jumps in levels n ≥ 4 to n = 3

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21
Q

Define the Heisenberg uncertainty principle

A

One can’t determine the exact momentum and position of an electron; either the momentum has to be stopped to determine position or the electron must be moving to determine momentum

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22
Q

List and describe the 4 quantum numbers

A

The principal quantum number (n), the orbital angular momentum quantum number (l), the magnetic quantum number (ml), and the electron spin quantum number (ms).

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23
Q

Define the Pauli exclusion principle

A

No 2 electrons in an atom can have same 4 quantum numbers

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24
Q

What do quantum numbers describe?

A

The energy state of electrons

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25
Q

A large principle quantum number (n) denotes ___

A

higher energy level and radius of electron shell

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26
Q

Each shell can hold ___ electrons

A

2n^2

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27
Q

The principle quantum number must be (positive/negative)

A

positive

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28
Q

The angular momentum quantum number (l) determines the __

A

Shape and number of subshells within an energy level

29
Q

For angular momentum quantum number: if n = 1, l = ___

A

0

30
Q

What is the spectroscopic notation if l = 0?

A

s

31
Q

For angular momentum quantum number: if n = 2, l is ___

A

0 and 1

32
Q

For angular momentum quantum number: if n = 3, l = __

A

0, 1, and 2

33
Q

For angular momentum quantum number: if n = 4, l = ___

A

0, 1, 2, and 3

34
Q

What is the spectroscopic notation if l = 1?

A

p

35
Q

What is the spectroscopic notation if l = 2?

A

d

36
Q

What is the spectroscopic notation if l = 3?

A

f

37
Q

The maximum number of electrons that can be held within a subshell is determined by:

A

4l + 2

38
Q

The magnetic quantum number (ml_ describes ___

A

the specific particular orbital within a subshell where an electron is likely to be found

39
Q

Each orbital can hold __ electrons

A

2

40
Q

List the rule to determine magnetic quantum number

A

For l, ml = 2l + 1, with values between -l and +l

41
Q

If n = 1, ml is ___

A

0

42
Q

If n = 2, ml is ___

A

-1, 0, +1

43
Q

If n = 3, ml is ___

A

-2, -1, 0, +1, +2

44
Q

If n = 4, ml is ___

A

-3, -2, -1, 0, +1, +2, +3

45
Q

List the ml values of a s subshell

A

0

46
Q

List the ml values of a p subshell

A

-1, 0, +1

47
Q

List the ml values of a d subshell

A

-2, -1, 0, +1, +2

48
Q

List the ml values of an f subshell

A

-3, -2, -1, 0, +1, +2, +3

49
Q

Paired electrons are electrons in the (same/different) orbital with the (same/opposite) spins

A

same, opposite

50
Q

Electrons in different orbitals with the same ms values have __ spins

A

Parallel

51
Q

___ orbitals are spherical

A

s

52
Q

___ orbitals are dumbbell shaped

A

p

53
Q

Define the Aufbau principle

A

Electrons fill from lower to higher energy levels

54
Q

Define the n+l principle

A

If n+l are equal for 2 atoms, the subshell with the lower n value has lower energy and will fill with electrons first

55
Q

Define Hund’s rule

A

In subshells with more than one orbital, the orbitals are filled so that there are a maximum number of half-filled orbitals with parallel spins

56
Q

For _ and _ subshells, electrons from lower energy subshells can give up electrons so that the higher energy subshells can be half-full instead of completely full

A

d and f

57
Q

Define paramagnetic

A

Materials with atoms of unpaired electrons that can orient their spins to align with magnetic field and will be weakly attracted to field

58
Q

Define diamagnetic

A

Materials where atoms have only paired electrons and will be slightly repelled by a magnetic field

59
Q

As n (the principal quantum number) increases, the radius and energy ____

A

Increase

60
Q

Protium has an atomic mass of _ and _ # of proton(s)

A

1 amu and 1 proton

61
Q

Deuterium has an atomic mass of __ and __# of protons and __ # of neutrons

A

2 amu; 1 proton, 1 neutron

62
Q

Tritium has an atomic mass of __ and __# of protons and __# of neutrons

A

3 amu; 1 proton, 2 neutrons

63
Q

__ is the weighted average of atomic isotopes

A

Atomic weight

64
Q

The energy of an electron ____ as n increases (as it goes farther from the nucleus)

A

Increases (becomes less engative)

65
Q

Define the Pauli Exclusion Principle

A

no two electrons of a given atom can have the same set of four quantum numbers

66
Q

The principal quantum number is _ and denotes _ and _

A

n; radius and energy level

67
Q

The azimuthal quantum number (angular momentum) is _ and denotes _ and _

A

l; shape and number of subshells

68
Q

The magnetic quantum number is __ and denotes __

A

ml; the particular orbital within a subshell where an electron is most likely to be found

MCAT (13 decks)

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