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General Chemistry- Atomic Structure Flashcards

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MCAT flashcards
1
Q

What are the three subatomic particles?

A

Protons
Neutrons
Electrons

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2
Q

What is the fundamental unit of charge?

A

+1e

e=1.6x10^-19C

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3
Q

What’s the mass of a proton?

A

1 Atomic Mass Unit (amu)

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4
Q

What is the atomic number?

A

(Z) or the number of protons found in an atom, of that element.

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5
Q

What charge do neutrons have?

A

None, they are neutral

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6
Q

What makes up almost the entire mass of an atom?

A

Sum of the protons and neutrons in the nucleus

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7
Q

What is an isotope?

A

Atoms that share an atomic number, but have different mass numbers

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8
Q

What is the charge of an electron?

A

-1e

e=1.6x10^-19C

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9
Q

What is the mass of an electron?

A

1/2000 of a proton

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10
Q

What occurs due to the small masses of protons and electrons?

A

The electrostatic force of attraction is far greater than the gravitational force of attraction

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11
Q

Varying distance from the nucleus, causes what?

A

Varying levels of electrical potential energy.

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12
Q

Which have higher energy, electrons closer to the nucleus or further from the nucleus?

A

Further from the nucleus

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13
Q

What are the valence electrons?

A

Electrons furthest from the nucleus because they have the strongest interactions with the surrounding environment and weakest interactions with the nucleus

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14
Q

Valence electrons are much more likely to be involved in what?

A

Bonds with other atoms

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15
Q

Why are valence electrons more likely to bond with other atoms?

A

They experience the least electrostatic pull from their own nucleus

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16
Q

What do valence electrons determine?

A

The reactivity of an atom

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17
Q

What does the transferring of valence electrons allow?

A

Elements to fill their highest level to increase stability

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18
Q

What is the name of a positively charged atom?

A

Cation

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19
Q

What is the name of a negatively charged atom?

A

Anion

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20
Q

What are the symbols of protons, neutrons and electrons?

A

Protons: p, p+, 1/1H
Neutron: N^0, 1/0n
Electron: e-, or 0/-1e
See table 1.1

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21
Q

Where are electrons found?

A

Orbitals

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22
Q

Which subatomic particle is the most important for determining each of the following properties:
Charge:
Atomic Number:
Isotopes:

A

Charge: Electrons
Atomic Number: Protons
Isotopes: Neutrons

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23
Q

What’s the difference between atomic mass and mass #?

A

Nothing, they are synonymous

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24
Q

What is the difference between atomic weight and atomic mass?

A

Atomic weight is constant for a given element, while mass changes from isotope to isotope

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25
Q

What is the definition of atomic mass unit?

A

1/12 mass of the carbon-12 atom about 1.66x10^-24g.

AMU=Mass of proton or neutron

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26
Q

Where might mass be loss in regards to the mass number?

A

Binding energy

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27
Q

What is the greek meaning of isotopes?

A

Same place

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28
Q

How do you refer to an isotope?

A

The element name followed by the mass number.

Ex: carbon-12

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29
Q

What are the three isotopes of hydrogen?

A

Protium (greek: first) 1 proton + 1AMU
Deuterium (second) 1 proton, 1 neutron, 2AMU
Tritium (third) 1 proton, 2 neutrons, 3 amu

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30
Q

In nature almost all elements exist as what?

A

Two or more isotopes

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31
Q

What is the atomic weight?

A

The weighted average of all the naturally occuring isotopes of an element.

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32
Q

What do half-lives correspond with?

A

Stability

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33
Q

What do half-lives help determine?

A

The relative proportions of the different isotopes in nature.

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34
Q

What is a mole?

A

A number of “things” based on Avogadro’s number

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35
Q

What is avogadro’s number?

A

NA= 6.02x10^23

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36
Q

What are the definitions of atomic mass and atomic weight?

A

Atomic mass: Just slightly less than the sum of the masses of protons and neutrons in a given atom of an elements
Atomic weight: Average weight of the naturally occuring isotopes

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37
Q

While molar mass is typically written in grams per mole (g/mol), is the ratio moles per gram (mol/g) also acceptable?

A

The ratio is equivalent concept. It is therefore acceptable, as long as units can be cancelled in dimensional analysis.

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38
Q

What did Ernest Rutherford give evidence to? What date?

A

Evidence that an atom has a dense positively charged nucleus, which is only a small portion of the volume in 1910

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39
Q

What did Max Planck develop? What year?

A

1899-Quantum theory

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40
Q

What is quantum theory?

A

Energy emitted as electromagnetic radiation from matter comes in discrete bundles called quanta.

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41
Q

How is the energy of a quantum determined?

A

The Planck relation: E=hf

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42
Q

What do the letters represent in the Planck relation?

A

E=hf
E is energy
h is proportionality constant known as Planck’s constant= 6.626x10^-34Js
F or v=Frequency of radiation

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43
Q

What is angular momentum?

A

L=mvr

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44
Q

What is kinetic energy?

A

K=1/2mv^2

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45
Q

What did Bohr determine that went against the common knowledge of classical mechanics?

A

Bohr placed restrictions on the possible values of the angular momentum, when classical mechanics postulates that an object revolving around a circle has an infinite number of values

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46
Q

What did Bohr develop?

A

A model of the electronic structure of a hydrogen atom and an equation that could predict the values for angular moment of an electron orbiting a hydrogen nucleus.

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47
Q

What was Bohr’s equation for angular moment of an electron?

A

L=nh/2(pi)

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48
Q

What do the letters represent in Bohr’s equation for angular momentum of an electron?

A

L=nh/2(pi)

n: the principal quantum number
h: Planck’s constant

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49
Q

When was Bohr’s discovery?

A

1913

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50
Q

What did Bohr postulat?

A

The centripetal force acting on the electron as it revolved around the nucelus was created by the elecctrostatic force between the positively charged proton and the negatively charged electron

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51
Q

What is the equation for Bohr’s use of angular momentum to find the energy of an electron?

A

E=-(Rh)/n^2

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52
Q

What do the letters mean in the equation for Bohr’s equations to find the energy of an electron?

A

E=-(Rh)/n^2
(Rh): Rydberg unit of energy= 2.18x10^-18J/electron
n: principal quantum number

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53
Q

Does the energy of an electron increase or decrease the further it is from the nucleus?

A

Energy of an electron increases the farther out from the nucleus that it is located

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54
Q

Does the electron always have an attractive force towards a proton?

A

Yes, an electron in any of its quantized states in the atom will have an attractive force towards the proton

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55
Q

How does energy of an electron change?

A

In discrete amounts with respect to the quantum number.

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56
Q

How does angular moment of an electron change?

A

Only in discrete amounts with respect to the principal quantum number

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57
Q

What is an important point when looking at the energy of an electron?

A

While the magnitude of the fraction is getting smaller, the actual value it represents is getting larger (becoming less negative.)

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58
Q

How does Bohr describe the hydrogen atom?

A

The structure of the hydrogen atom as a nucleus with one proton forming a dense core, around which a single electron revolved in a defined pathway (orbit) at discrete energy value

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59
Q

According to Bohr’s theory, what could result in an electron jumping?

A

Transfer of the exact amount of energy equal to the difference between one orbit and another

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60
Q

What is ground state?

A

The orbit with the smallest, lowest-energy radius (n=1)

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61
Q

What is an excited state, in regards to an electron?

A

At least one electron has moved to a subshell of higher than normal energy

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62
Q

What do we know now, that contradicts Bohr’s model?

A

Electrons are not restricted to specific pathways, but tend to be localized in certain regions of space.

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63
Q

As electrons go from a lower energy level to a higher energy level they get what?

A 
Aborption of light
Higher potential 
Excited
Distant (from the nucleus)
(AHED)
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64
Q

How can electrons be excited to a higher energy level?

A

Heat

Other energy forms

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65
Q

Once the electrons are no longer being excited, what occurs?

A

Electrons will rapidly return to ground state

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66
Q

What is a result of electrons returning to ground state?

A

Emission of discrete amounts of energy in the form of photons

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67
Q

What equation demonstrates photon emission?

A

E=hf (a photon is emitted with energy)

68
Q

What is the equation for electromagnetic energy of a photon?

A

E= hc/(/) (p.12)

69
Q

What do the letters represent in the equation for electromagnetic energy of a photon?

A

E= hc/(/)
h: Planck’s constant
c: speed of light in a vacuum (3.00X10^8m/s)
(/): wavelength of the radiation

70
Q

What is the speed of light in a vacuum?

A

3.00x10^8m/s

71
Q

What happens when an electron returns to ground state?

A

Electrons will each emit a photon with a wavelength characteristic of the specific energy transition it undergoes.

72
Q

Do energy transitions of electron form a continum?

A

No, they are quantized to certain values

73
Q

What is a line spectrum?

A

Lines which corresponds to specific electron transition

74
Q

Each element has a unique what?

A

Atomic emission spectrum which can be used as a fingerprint for the element

75
Q

How can elements be determined on other planets/stars?

A

The light from a star can be resolved into its component wavelengths which then match to the known line spectra of the elements

76
Q

What is the Lyman series?

A

The group of hydrogen emission lines corresponding to transitions from energy n>2 to n=1

77
Q

Which element does the Bohr model explain in regards to the emission spectrum?

A

The atomic emission spectrum of hydrogen

78
Q

What is the Balmer series?

A

The corresponding transitions from energy levels n>3 to n=2

79
Q

What is the Paschen series?

A

Transitions from n>4 to n=3

80
Q

Which has larger energy transitions, Lyman or Balmer series?

A

Lyman series compared to Balmer series

81
Q

Which series has wavelengths in the visible region?

A

Balmer series with four wavelengths in the visible region

82
Q

Which series has shorter photon wavelengths in the UV region?

A

Lyman series

83
Q

Energy is inversely proportional to what?

A

wavelength

84
Q

What is the equation for energy and wavelength?

A

E=hf=hc/(/)

85
Q

What is the combined equation of Bohr and Planck’s calculations?

A

E=hc/(/)=-R [(1/(ni)^2)-(1/(nf)^2]

86
Q

What is the equation explaining that combines Bohr’s and Planck’s calculations?

A

The energy of the emitted photon corresponds to the difference in energy between the higher-energy initial state and the lower-energy final state.

87
Q

What occurs when an electron is excited and is moving to a higher energy level?

A

It must absorb exactly the right amount of energy to make that transition. Electron transition results in energy absorption at specific wavelengths

88
Q

What are the two spectrums given off by an electron?

A

Emission spectrum

absorption spectrum.

89
Q

What can the two spectrums show?

A

Unique elements and which element is present in a given area. Absorption and emission wavelengths of an element are what? The exact same

90
Q

Why are absorption and emission wavelengths the same?

A

The difference in energy between levels remains unchanged so emission and absorption will be the same.

91
Q

What is required to identify elements in the gas phase?

A

Absorption spectra

92
Q

Each element has what in regards to identification spectras?

A

Each element has a characteristic set of energy levels.

93
Q

What was the flaw of Bohr’s model?

A

Inadequate to explain the structure and behavior of atoms containing more than one electron

94
Q

What didn’t Bohr’s model take into account?

A

The repulsion between multiple electrons surround the nucleus

95
Q

What is the important difference between Bohr’s model and the modern quantum model?

A

Bohr postulated that electrons follow a clearly defined circular pathway or orbit at a fixed distance from the nucleus, wherreas modern quantum mechanics has shown that this is not the case.

96
Q

What are orbitals?

A

Localized regions of space around the nucleus where electrons move rapidly

97
Q

Orbitals are part of which atomic model?

A

Quantum Mechanical Model of Atoms

98
Q

What is impossible to pinpoint int he modern quantum model?

A

Exact whereabouts of an electron at a given moment in time

99
Q

What is the best that can be done to determine the location of an electron in the quantum mechanical model?

A

Describe the probability of finding an electron within a given region

100
Q

What is the Heisenberg Uncertainty Principle?

A

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

101
Q

What are the four quantum number that can describe an atom?

A

n, l, (ml), (ms)

102
Q

What is the Pauli exclusion principle?

A

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

103
Q

What is an electron’s energy state?

A

The position and energy of an electron described by its quantum numbers

104
Q

What does the values of n limit?

A

The value of n limits the values of l, which limits the values of (ml)

105
Q

What do the values of the quantum numbers five info about?

A

Size
Shape
Orientation of the orbitals

106
Q

What is the pricipal quantum number?

A

First quantum number, denoted by the letter “n.”

107
Q

What quantum number is used in Bohr’s model?

A

First quantum number which takes on any positive integer value

108
Q

What is the meaning of principal quantum number n?

A

The larger the integer value of n, the higher the energy level and radius of the electron’s shell.

109
Q

Each shell has the capacity to what?

A

hold a certain number of electrons

110
Q

What is the equation for the maximum number of electrons within a shell?

A

2n^2

111
Q

What is the 2nd quantum number?

A

Azimuthal quantum number (angular momentum) designated by the letter “l”

112
Q

What does the second quantum number refer to?

A

The shape and number of subshells within a given principal energy level (shell).

113
Q

What is important about the 2nd quantum number?

A

It has important implications for chemical bonding and bond angles

114
Q

What is the equation to determine the range of possible values for ‘l”?

A

l=(n-1)

115
Q

Wjat os spectroscopic notation?

A

The shorthand representation of the principal and azimuthal quantum number.

116
Q

What letters are designated by which subshells?

A

l=0 subshell: s
l=1 subshell: p
l=2 subshell: d
l=3 subshell: f

117
Q

Looking at the periodic table, which groups are in which subshells?

A

Alkali: s-block plus helium
Halogen: p-block
transition: d block
Lanthanide/Acinide: f-block

118
Q

What is the equation for the maximum number of electrons within a subshell?

A

4”l”+2

119
Q

What increases with “l” value?

A

Energies of the subshell

120
Q

What is the third quantum number?

A

Magnetic quatnum number desginated by the letter (ml)

121
Q

What does the third quantum number specify?

A

The particular orbital within a shubshell where an electron is mostlikely to be found at a given moment in time.

122
Q

Each given orbital can hold a max of how many electrons?

A

Two electrons

123
Q

What are are the possible values of (ml)?

A

The possible values are the integers between -1 and +1 including 0

124
Q

The four different orbitals have how many orbitals each?

A

s subshell: 1 (0)
p subshell: 3 (-1, 0, +1)
d subshell: 5 (-2, -1, 0, 1, 2)
f subshell: 7 (-3, -2, -1, 0, 1, 2, 3)

125
Q

The shape of the orbitals is dependent of what?

A

Dependent on the subshell

126
Q

What shape is the s subshell?

A

Spherical

127
Q

What shape is the p subshell?

A

Dumbell shaped

128
Q

How is the p subshell orbitals aligned?

A

Along the x, y, and z axes

129
Q

What are the p subshell orbitals referred to as?

A

px, py, pz

130
Q

How are the d and f subshells shapes defined?

A

By the concept probability density

131
Q

How many elements are contained in each subshell block on the periodic table?

A

s block: 2 groups of elements
p block: 6 groups of elements
d block: 10 groups of elements
f block: 14 groups of elements

132
Q

What is the 4th quantum number?

A

Spin quantum number or (ms)

133
Q

How many spin orientations does an electron have?

A

Two spin orientations

+1/2) and (-1/2

134
Q

When two electrons are in the same orbital, what happens?

A

They must have opposite spins

135
Q

What are electrons refered to as when they are in the same orbital?

A

Paired

136
Q

What does electrons having parallel spins mean?

A

Electrons in different orbitals with the same (ms) values have parallel spins

137
Q

What is electron onfiguration?

A

The pattern by which subshells are filled and the number eletrons within each principal energy level and subshell

138
Q

How do you read spectroscopic notation?

A

The first number denotes the principal energy level, the letter designates the subshell and the superscript give the number of electrons in that subshell.

139
Q

What is the electron subshell flow diagram?

A

See figure 1.12 page 20. The tree

140
Q

What is the Aufbau Principle?

A

Electrons fill from lower to higher energy subshells. Each subshell will fill completely before electrons begin to enter the next one

141
Q

What is the building-up principle?

A

The Aufbau principle

142
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 subshell

143
Q

For the n+l rule, what do you do if two subshells has the same n+l value?

A

The subshell with the lower n values has a lower energy.

144
Q

What are the two ways to not memerize the subshell flow?

A

The n+l rule

Reading the periodic table

145
Q

How can electron configuration be abbreviated?

A

By placing the noble gas that precedes the element in brackets

146
Q

How do you write the electron configuration for Anions?

A

Because Anions have additionally charged electrons you fill them up the same way as above.

147
Q

How do you write electron configuration for Cations?

A

Start with the neutral atom, and remove electrons from the subshells with the highest value for n first.

148
Q

What happens if multiple subhsells are tied for highest n vlaue when removing electrons from Cations?

A

Electrons are removed from the subshell with the highest l value

149
Q

What is Hund’s rule?

A

Within a given subhsell, orbitals are filled such that there are a maximum number of half-filled orbitals with parallel spins.

150
Q

When do electrons fill according to Hund’s rule?

A

When subhsells contain more than one orbital, the orbitals will fill according to Hund’s rule.

151
Q

What is the basis for Hund’s rule?

A

Electron repulsion: electrons in the same orbital tend to be closer to each other and thus repel each other more than electrons placed in different orbitals.

152
Q

Which orbitals have lower energies?

A

Half-filled and Fully filled

153
Q

What does lower energies in an orbital mean?

A

Higher stability

154
Q

What groups are the notable exceptions to electron configuration?

A

Chromium and Copper groups

155
Q

What is the exception for Chromium and copper in regards to its configuration?

A

Instead of filling up the s subshell it fills up a larger subshell first because the electrons can fill up half or full in that other subshell.

156
Q

Can similar exceptions to the configuration of electrons be seen in the f subshell?

A

Yes

157
Q

Can similar exceptions to the configuration of electrons be seen in the p subshell?

A

Never! the extra stability doesn’t outweight the cost

158
Q

What is affected by the presence of paired or unpaired electrons?

A

The chemical and magnetic properties of an atom or molecule.

159
Q

What materials are paramagnetic?

A

Atoms with unpaired electrons will orient their spins in alignment with a magnetic field and be weakly attracted to the magnetic field.

160
Q

What causes materials to be diagmagnetic?

A

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

161
Q

What are the valence electrons?

A

Electrons that are in its outermost energy shell
Are most easily removed
Are available for bonding

162
Q

What are the the characteristics of valence electrons?

A

Are most easily removed
Are available for bonding
Dominate chemical behavior

163
Q

For groups IA and IIA (1 and 2), which subshells have valence electrons?

A

The highest s subshell electrons are valence electrons

164
Q

For group IIIA-VIIIA (13-18), which subshells have valence electrons?

A

The highest s and p subshells electronns are valence electrons

165
Q

For transition elements, which subshells have valence electrons?

A

Highest s and d subshell electrons

166
Q

For lanthanide and actinide series elements, which subshells have valence electrons?

A

Highest s and f subhsells

167
Q

Which period of elements violates the octet rule?

A

Elements in period three (starting with sodium) and below may accept electrons into their d subshell which allows them to hold more than eight electrons in their valence shell.

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