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Atomic Structure Flashcards

1
Q

Protons have a mass of…

A

1 amu (atomic mass unit)

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2
Q

Z stands for

A

atomic number, the number of protons in an atom of an element

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3
Q

While all atoms of an element have the same atomic number, they do not necessarily have the same…

A

atomic mass due to isotopes!

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4
Q

A stands for

A

mass number, the sum of all protons and neutrons within an atom

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5
Q

Isotopes

A

atoms that have the same atomic number, but different mass numbers

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6
Q

Because subatomic masses are so small, electrostatic force of attraction between protons and electron is….

A

far greater than the gravitational force of attraction based on mass

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7
Q

Electrons close to the nucleus have..

A

lower energy levels and strongest interaction with nucleus

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8
Q

Electrons further away from the nucleus…

A

have higher energy levels and strongest interaction with the surrounding environment

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9
Q

Valence Electrons

A

electrons in the outer most shell of an atom, they determine the reactivity of an atom

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10
Q

Increase stability

A

having a full valence electron shell

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11
Q

Cation vs Anion

A

positively charged atom vs negatively charged atom

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12
Q

Atomic Mass/Mass Number

A

are synonymous! It varies from one isotope to another

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13
Q

Atomic Weight

A

Is constant for a given element; the weighted average of all isotope weights

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14
Q

Isotopes

A

when an element differs in the number of neutrons

but because protons and electrons are constant, they exhibit similar chemical principles

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15
Q

Half life corresponds with and helpd determine…

A

stability and helps determine proportions of isotopes

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16
Q

Avogadros Number

A
  1. 02*10^23 atoms/molecules /ions/things in 1 mole
    ex: 12 amu atomic weight of carbon means
  2. 02*10^23 atoms of carbon = 12 amu
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17
Q

Calculating Atomic Weight of an Unknown Element

A

(% Isotope 1)(atomic mass Isotope 1) + ….. = Atomic Weight

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18
Q

Ernest Rutherford

A

gave evidence that an atom has a dense, positively charged nucleus that is a small portion of atoms volume

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19
Q

Max Planck

A

developed first quantum thoery, energy emitted as electromagnetic radiation from matter comes from quanta

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20
Q

Planck Relation

A

E = hF

E = energy

h = plancks constant

f = frequency of radiation

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21
Q

Bohr Model Postulate

A

that centripetal force causing electrons to be in orbit is caused due to the electrostatic force between the positively charged protons and negatively charged electrons

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22
Q

Angular Momentums of an Electron Equation

A

L = nh/2pi

n = quantum number
h = plancks constant

angular momentum only changes with respect to the quantum number

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23
Q

Energy of an Electron

A

E = - Rh / n^2

Rh = rydberg unit of energy

Energy changes with respect to the quantum number like angular momentum

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24
Q

a value of 0 energy states that a proton and electron are…

A

not attracted at all, not close

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25
Energy of an electron increases...
the farther from the nucleus it is (as quantum number increases)... think energy of an electron equation
26
Ground State
lowest electron energy
27
Excited State
highest electron energy as electron moves above to another shell further out
28
How can electrons be excited?
via heat/energy forms
29
Emission of photons
when excited form electrons drop back down to ground state, they emit energy in the form of photons the photon emitted has a wavelength associated with it depending on the specific energy transmission
30
Electromagnetic Energy of Photons
E = hc/ lambda lamba = wavelength h = Planck's constant
31
Atomic Emission Spectrum
each element can have its electrons excited to a different set of distinct energy levels giving them a unique atomic emission spectrum
32
Lyman Series
group of hydrogen emission lines corresponding energy levels n greater than or equal to 2 to n = 1
33
Balmer Series
group of hydrogen emission lines corresponding energy levels n greater than or equal to 3 to n = 2
34
Paschen Series
group of hydrogen emission lines corresponding energy levels n greater than or equal to 4 to n = 3
35
Lyman Series has larger energy transitions than Balmer series therefore it...
has shorter photon wavelengths
36
Combining Planck's and Bohr's Theories states
The energy emitted photon corresponds to the difference in energy between the higher energy initial state and the lower energy final state
37
Absorption spectrum
in addition to each element having a unique emission spectrum, they also each have a unique absorption spectrum
38
Emission and Absorption Spectrum
uniques for each element, wavelength for each corresponds with one another because difference in energy levels is unchanged
39
Quantum Mechanical Model
electrons move rapidly and are localized in regions of space around nucelus known as orbitals
40
Heisenberg Uncertainty Principle
its impossible to determine perfectly the momentum and position of an electron
41
Pauli Exclusion Principle
no two electrons in a given atom can possess the same set of 4 quantum numbers
42
Principle quantum Number (n)
the larger the integer value of n (electron shell), the higher the energy level and radius of the electons shell
43
Maximum number of Electrons Within a Shell
2n^2
44
The difference in energy between two shells DECREASES as the distance from the nuclues ___
INCREASES n=3 to n=4 is lower than n= 2 to n=3
45
Azimuthal (Angular Momentum) Quantum Number (l)
refers to the shape and number of subshells within a principle energy level l = all numbers less than n -1 ex: n=2 ; l = 1 or 0 this means there are 2 subshells (1 and 0) within the second principal energy level
46
``` l = 0 l = 1 l = 2 l = 3 ```
s, p, d, f orbitals respectively
47
Maximum Number of Electrons within a subshell =
4l + 2
48
Magnetic Quantum Number (ml)
specifies the particular orbital within a subshell where an electron is most likely to be found at a given time - l , 0 , l
49
s subshell orbital shape | p subshell orbital shape
s subshell have spherical orbitals | p subshell has 3 dumbell type orbitals
50
As atomic number increases, so too does the number of....
electrons
51
Spin Quantum Number (ms)
spin orientation +1/2 or -1/2
52
Parallel Spins
Electrons in different orbitals with the same ms values
53
Example: 2p^4
Indicates that 4 electrons in the second p subshell of second principal energy level is filled, also that all energy levels below 2p are filled
54
Aufbau Principle
each subshell will fill completely before electrons enter the next one
55
n + l rule
ranks subshells by increasing energy the lower the sum of n+l,, the lower the energy of the subshell. IF n+l are equal, then the subshell with the lower n has the lower energy and will fill first **pg 21
56
***Subshells for cations
start with neutral element and then remove electrons from subshells with the highest n value
57
Ex: electron configuration of Fe 3+
Neutral: [Ar] 4s^2 3d^6 Cation: [Ar]3d^5
58
Hunds RUle
within a given subshell, orbitals are filled so maximum number of half-filled orbitals with parallel spins (each orbital has an electron before one is completely filled)
59
Notable exceptions to Electron Config
Chromium and ELements in its group [Ar]4s13d4 Copper and elements in its group [Ar]4s13d10
60
The presense of paired or unpaired electrons affects the....
chemical and magnetic properties of an atom or molecule
61
Paramagnetic
unpaired electrons will orient their spins in alignment with a magnetic field and material will be attracted to the field
62
Diamagnetic
materials with paired electrons will be slightly repelled y a magnetic field
63
Valence ELectrons for Groups 13-18
highest s and p subshell electrons are the valence electrons
64
Valence Electrons for Transition Elements
highest s and d subshell electrons
65
All elements in period three (startng with sodium) and below may accept electrons into....
their d subshell and hold more than 8 electrons in the valence shell

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