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MCAT General Chemistry > Chapter 1 - Atomic Structure > Flashcards

Chapter 1 - Atomic Structure Flashcards

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1
Q

Where are protons and neutrons found?

A

In the nucleus

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2
Q

Each proton has an amount of charge equal to what?

A

The fundamental unit of charge
e = 1.6 x 10^-19 Coulombs

Simplified as “+1e” or even “+1”

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3
Q

Protons have a mass of approximately what?

A

One atomic mass unit (amu)

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4
Q

What are elements defined by?

A

The number of protons they contain

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5
Q

All atoms of a given element have the same atomic number but may not contain the same mass, why is this?

A

Because they can have varying number of neutrons

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6
Q

The atomic number is what sign in chemistry?

A

Z

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7
Q

How much more does a neutron weight than a proton?

A

Not much at all, slightly greater in weight

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8
Q

Why do protons and neutrons in the nucleus make up almost all the mass of an atom?

A

Because the electron is of negligible weight

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9
Q

Mass number is given what sign in chemistry

A

A

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10
Q

What is the mass number (A)

A

It is the sum of protons and neutrons in the atoms nucleus

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11
Q

What are isotopes?

A

Atoms that share the same atomic number hence are the same element but have different mass numbers due to varying number of neutrons

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12
Q

In a written equation where is the atomic number (Z), mass number(A), and atom (X)?

A

The atom is after the atomic number and mass number, the atomic number being below the mass number which is on top

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13
Q

How does an electrons charge compare to a proton?

A

Their charge is equal in magnitude but in opposition of each other 1:1

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14
Q

The mass of an electron is approximately how much of a proton?

A

1/2000

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15
Q

Since masses of subatomic particles are so small, what does this mean for electrostatic force and gravitational force?

A

The electrostatic force of attraction between the unlike charges of the proton and electron is far greater than the gravitational force of attraction based on their respective masses

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16
Q

Why do electrons have varying levels of electrical potential?

A

Because they move around the nucleus at varying distances

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17
Q

Which electrons have lower and higher levels of energy?

A

Electrons closer to the nucleus are at lower levels of energy, those further have higher levels of energy

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18
Q

What electrons have the strongest interactions with the surrounding environment and the weakest interactions with the nucleus?

A

The electrons that are furthest from the nucleus, these electrons are called valence electrons

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19
Q

What electrons are much more likely to become involved in bonds with other atoms and why?

A

Valence electrons, because they have the least electrostatic pull from their own nucleus

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20
Q

Generally speaking What determines the reactivity of an atom?

A

Valence electrons

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21
Q

How do valence electrons play a role in increasing stability?

A

They can share or transfer valence electrons in bonds allowing elements to fill their highest energy levels to increase the stability

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22
Q

What is a positive and negative charged atom called?

A

Positively charged - cation
Negatively charged - anion

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23
Q

Atomic mass unit (amu) is equal to what?

A

1.66 x 10^-24g

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24
Q

What is the difference between Atomic weight and atomic mass

A

Atomic weight is the average mass of all isotopes of an element
Atomic mass refers to the mass of an individual atom of a specific isotope of that element

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25
Q

Is the atomic weight or atomic mass on the periodic table?

A

Atomic weight

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26
Q

What is a mole?

A

A mole is a unit of measurement used to quantify the amount of a substance

It represents 6.02 x 10^23 (Avogadro’s number)

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27
Q

What did Ernest Rutherford provide experimental evidence of in 1910?

A

That an atom has a dense, positively charged nucleus that accounts for only a small portion of the atoms volume

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28
Q

What did max Planck do in 1900?

A

He developed the first quantum theory, proposing that energy emitted a electromagnetic radiation from matter comes in discrete bundles called quanta, energy of quantum, given by the Planck relation

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29
Q

What is the Planck relation formula?

A

E = hf

E - energy of a photon
h - plancks constant = 6.626 x 10^-34 J•s
f - frequency of radiation

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30
Q

In 1913, danish physicist Neil’s Bohr used the work of Rutherford and Planck to develop his model of the electronic structure of the hydrogen atom called what?

A

The Bohr model

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31
Q

What is the equation for angular momentum when the object is moving in a circle around a fixed axis like an electron is?

A

L=mvr

L=angular momentum
m=mass
v=linear velocity of object
r=distance between object and the axis of rotation

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32
Q

What is the equation for kinetic energy?

A

K=1/2mv^2

K = kinetic energy
m = mass
v = velocity

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33
Q

Bohr placed restrictions on the possible values of the angular momentum, predicting that the possible values for the angular momentum of an electron orbiting a hydrogen nucleus could be given by what formula?

A

L=nh/2pie

L = angular momentum of electron
n = principal quantum number
h = Planck’s constant

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34
Q

What is quantization and it’s relation to chemistry?

A

Quantization is the process of restricting continuous values to specific discrete values meaning certain properties of particles can only have distinct quantized values

This challenges classical continuous behavior, now a fundamental principal in quantum theory, revolutionizing our understanding of the atomic and subatomic world

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35
Q

What does “rh” in chemistry stand for?

A

Rydberg constant
equal to 2.18 x 10^-18 joules

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36
Q

Energy of an electron has what relationship with principal quantum number (n)?

A

They are directly proportional, as (n) increases, the energy of the electron also increases, thus the electron is found further from the nucleus

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37
Q

What is the principal quantum number (n)?

A

It represents the energy level or shell of an electron in an atom

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38
Q

The orbit with the smallest, lowest energy radius is defined as what?

A

The ground state (n=1)

When atoms are considered in a ground state it is in the state of lowest energy, in which all electrons are in the lowest possible orbitals

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39
Q

If an electron was promoted to an orbit with a larger radius (higher energy) the atom was said to be in…

A

An excited state

An atom is in this state when at least one electron has moved to a subshell of higher than normal energy

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40
Q

Electrons can be excited to higher energy level (excited state) how?

A

By heat or other energy forms to yield excited states

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41
Q

How long is the lifetime of an excited state?

A

It is brief, electrons will return rapidly to the ground state

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42
Q

When an electron goes from a excited state back to a ground state what results?

A

Emission of discrete amounts of energy in the form of photons

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43
Q

What is the formula for electromagnetic energy of photons?

(If frequency is not used)

A

E = hc/wavelength (lambda)

E = electromagnetic energy of photons
h = plancks constant
c = speed of light in a vacuum (3.00 x 10^8 m/s)

Combination of E = hf and
f = c/lambda

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44
Q

MNEMONIC

as electrons go from lower energy level to a higher energy level, they get AHED, what does AHED stand for?

A

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

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45
Q

Energy translations do not form a continuum but rather…

A

Are Quantized to certain values

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46
Q

What is the line spectrum?

A

The line spectrum is composed of light at specific frequencies, each line on the emission spectrum corresponds to a specific electron transition

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47
Q

Explain what the Lyman series, Balmer series, and Paschen series is?

A

These series’s are groups of hydrogen emission lines corresponding to transitions from energy levels:

N ≥ 2 to n = 1 -Lyman series

N ≥ 3 to n = 2 -Balmer series

N ≥ 4 to n = 3 -Paschen series

48
Q

How are higher energy translations related to photon wavelengths

A

They are in opposition, higher energy translations equals shorter photon wavelengths

49
Q

The energy of an emitted photon corresponds to the difference in energy between what?

A

The higher energy initial state and the lower energy final state

E_photon = E_initial - E_final

50
Q

When an electron goes from a lower state to a higher state of energy then back to a lower state of energy, what is happening in these energy changes?

A

When electrons move from a lower state to a higher state of energy they undergo absorption and must absorb the right amount of energy to do so, they absorb this energy in the form of light, when electrons move from high back to low energy they undergo emission, emitting the same amount of energy in the form of light (photon)

51
Q

What is the formula for energy of electron in atoms with only one electron, such as hydrogen?

A

E = -RH/n^2

E - energy of electron
RH - Rydburg constant
n - principal quantum number

52
Q

Electrons move rapidly and are localized within regions of space around the nucleus called what

A

Orbitals

53
Q

What is the Heisenberg uncertainty principal?

A

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

54
Q

What are the four quantum numbers

A

N, l, Ml, Ms

55
Q

Any electron in an atom can be completely described by what?

A

It’s quantum numbers

56
Q

What is the Pauli exclusion principal?

A

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

57
Q

Any position and energy of an electron described by its quantum numbers are known as it’s what?

A

Energy state

58
Q

How does the values of the quantum numbers limit others?

A

The value of n limits the values of l, which limits the values of Ml

This is because it gets more localized as you go through the quantum numbers

59
Q

Values of the quantum numbers qualitatively gives information about what?

A

Size, shape, and orientation of the orbitals

60
Q

What is the first quantum number also known as?

A

The principal quantum number denoted as (n)

61
Q

The larger (n) is the greater…

A

The energy, and radius of electrons shell

62
Q

Maximum number of electrons in a shell is what formula

A

Max capacity of electrons in a shell = 2n^2

63
Q

Energy difference is a function of

1/ni- 1/nf

ni = principal quantum number initial
nf = principal quantum number final

What does this mean as distance from nucleus increases?

A

Difference in energy between the 2 shells decreases as the distance from the nucleus increases

64
Q

NEVER forget that electrons DO NOT travel in…

A

defined orbits

65
Q

What is the second quantum number called

A

The azimuthal (angular momentum) quantum number

Denoted as “l”

66
Q

The azimuthal quantum number represents what

A

Shape and number of sub shells within a given principal energy level

67
Q

For any given value of n how do you find l?

A

l is 0 to (n-1)

Example: n=4 l = 0,1,2,3

68
Q

N value also tells you the number of what within a shell?

A

Number of possible subshells

Example: n = 2 (l = 0,1) - 2 subshells

n = 4 (l = 0,1,2,3) - 4 subshells

69
Q

What is spectroscopic notation?

A

The shorthand representation of the principal and azimuthal quantum numbers

n is given it’s same number

l follows the number in a letter corresponding to its value

70
Q

What are the letters for “l” being
0,1,2, and 3

A

0 - s
1 - p
2 - d
3 - f

71
Q

What is the max capacity of electrons within a subshell?

A

4l + 2

72
Q

What happens to the energies of the subshells as l value increases

A

Energies of the subshells will increase, however the energies of subshells from different principal energy levels may overlap

Example: 4s subshell will have a lower energy level than 3d

73
Q

What is the third quantum number?

A

The magnetic quantum number denoted as “ml”

74
Q

What does the magnetic quantum number specify?

A

The particular orbit within a subshell where an electron is most likely to be found at a given moment in time

75
Q

Each orbital can hold a max of how many electrons?

A

2

76
Q

What are the possible values for ml?

A

The integers between -l and +l including 0

Example: l = 3 then ml has 7 orbitals (-3 to 3)

77
Q

Shape of orbitals are dependent on what?

A

The subshell in which they are found

78
Q

Orbitals in s subshell and p subshell are what shapes

A

s subshell - spherical
p subshell - dumbell shape

79
Q

What are the 3 p orbitals often denoted as

A

px, py, pz

80
Q

Shapes of orbitals are defined in terms of a concept called probability density, what does this mean?

A

Probability density refers to the likelihood that an electron will be found in a particular region of space

81
Q

What is the fourth quantum number called?

A

The spin quantum number denoted as “ms”

82
Q

An electron has how many spin orientations?

A

2, spin up (+1/2) and spin down (-1/2)

83
Q

Whenever electrons are in the same orbital they must have what?

A

Opposite spins

Referred to as being paired in this case

84
Q

Electrons in different orbitals with the same ms values are said to have…

A

Parallel spins

85
Q

What is the electron configuration?

A

Representation of the arrangement of electrons in the atomic orbitals, following the order of filing based on energy levels and subshells

86
Q

What notation does electron configuration use?

A

Spectroscopic notation

87
Q

What does the superscript in electronic configuration represent

A

The number of electrons in the subshell

88
Q

If the electron configuration is 2p^4 what does that imply about the energy levels before 2p?

A

They have already been filled (1s, 2s)

89
Q

In what order do electrons fill their subshells?

A

According to the Aufbau Principal (building up principal) electrons will fill from lower-to higher-energy subshells

90
Q

What is the n+l rule?

A

The lower the sum of the values of the first and second quantum numbers (n+l) the lower the energy of the shell

91
Q

If 2 subshells posses the same n+l value what subshell fills first?

A

The lower n value has a lower energy level and will fill electrons first

92
Q

What will fill first with electrons 5d vs 6s

A

6s because it has 6 n+l value while 5d has 7 n+l value

93
Q

What is the lowest s subshell, p subshell, d subshell, and f subshell

A

s subshell - 1s
p subshell - 2p
d subshell - 3d
f subshell - 4f

94
Q

What series is pulled out and placed below the rest of the periodic table in most tables?

A

The lanthanide and actinide series (f block)

95
Q

In terms of spectroscopic notation on electronic configuration where is the lanthanide and actinide series placed between?

A

Lanthanide series is between 6s and 5d

Actinide series is between 7s and 6d

96
Q

Electron configurations for elements can be abbreviated by placing what that precedes the element of interest in brackets?

A

The preceding noble gas

97
Q

When dealing with an anion in electron configuration using noble gases what do you do?

A

You simply just add the needed amount of electrons

98
Q

For the element “F” and “F-“ what is the electron configuration

A

F is [HE] 2s^2 2p^5
Then F- is [HE] 2s^2 2p^6

99
Q

When dealing with cations in electronic configuration for elements what electrons do you remove first?

A

When dealing with a cation remove electrons from the subshells with the highest value for n first, if multiple subshells are tied for the highest n value, then electrons are removed from the subshell with the highest “l” value

100
Q

Fe and Fe3+ electron configuration using noble gases

A

Fe is [Ar] 4s^2 3d^6

Then Fe+3 is [Ar] 3d^5

101
Q

What does Hunds rule state?

A

That within a given subshell, orbitals are filled such that there are a maximum number of half filled orbitals with parellel spins

102
Q

Electrons in the same orbital tend to be closer to each other and thus tend to…

A

Repel each other more than electrons placed in different orbits

103
Q

Lower energies equals what referring to stability?

A

Higher stability

104
Q

Half filled and fully filled orbitals tend to have what types of energy levels compared to other states

A

Lower energies

105
Q

There are some exceptions to the Aufbau principal, why does this happen and what is it known as?

A

Instead of energy levels filling low to high they deviate to achieve a more stable configuration, known as the “half filled and fully filled subshell stability rule”

106
Q

What are paramagnetic materials and how do they orient themselves?

A

Materials composed of atoms with unpaired electrons

This will orient their spins in alignment with a magnetic field, and thus the material will be weakly attracted to the magnetic field

107
Q

What does paramagnetic cause in a magnetic field?

A

It will cause parallel spins in unpaired electrons and therefore cause an attraction (weak)

108
Q

What are diamagnetic materials? How do they orient themselves in a magnetic field?

A

Materials consisting of atoms that have only paired electrons

will be slightly repelled by a magnetic field

109
Q

In each row of periodic table how many elements are in the s-block,
d-block, and f-block

A

s-block - 2 elements
d-block - 10 elements
f-block - 14 elements

110
Q

What are valence electrons?

A

Electrons of an atom that are in the outermost energy shell, most easily removed, and available for bonding

111
Q

What subshell are the valence electrons in Elements in group 1 and 2

A

Only the highest s subshell

112
Q

Group 13-18 has valence electrons in what subshell?

A

Highest s and p subshell

113
Q

Transition elements are what groups?

A

Groups 3-12

114
Q

Transition elements (groups 3-12) have valence electrons in what subshell?

A

Highest s and d subshells

115
Q

Lanthanide and actinide series have valence electrons in what subshells?

A

Highest s and f subshells

MCAT General Chemistry (2 decks)

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