4. ATOMIC AND ELECTRONIC STRUCTURE (PART 2) Flashcards

1
Q
  1. What is Quantum Mechanics?
A
  • it is a branch of science that deals with matter on the sub-microscopic level

Sub-Microscopic= atomic

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2
Q
  1. What does Quantum Mechanics give us?
A
  • it gives us an accurate description of how atoms and molecules behave
  • it can also give an accurate description of how electrons in an atom behave and how they are are arranged around the nucleus
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3
Q
  1. What are electrons responsible for?
A
  • the chemical properties of an element
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4
Q
  1. What is the Quantum Mechanical Picture?
A
  • it is a statistical theory
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5
Q
  1. Which space do electrons occupy?
A
  • the space around the nucleus
  • this space resembles orbits (like how the moon orbits around the Earth)
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6
Q
  1. What Theory must be applied to determine the true picture?
A
  • the Quantum Theory
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7
Q
  1. In which forms can electrons be perceived as?
A
  • waves
  • particles
  • this is determined by the observer and the tests run by the observer
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8
Q
  1. Which equation is this?
    What does it solve for?
A
  • the Schrodinger Equation
  • also known as the wave equation
  • it solves for the motion of the electron
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9
Q
  1. What is the explicit form of the Schrodinger Equation?
A
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10
Q
  1. What kind of energy does this part of the equation represent?
A
  • Kinetic Energy
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11
Q
  1. What kind of energy does this part of the equation represent?
A
  • Potential Energy
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12
Q
  1. Label the following parts of the equation?

12.1: Pink Part
12.2: Blue Part
12.3: Yellow Part

A

12.1: The Hamiltonian

12.2: Energies of the system

12.3: Wave Functions

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13
Q
  1. What is the Hamiltonian Operator?
A
  • it is the sum of the kinetic and potential energies of the system
  • the system is the atom and specifically the electrons distribution in the atom
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14
Q
  1. What are the Energies of the system (E)?
A
  • when looking at the electron distribution in the atom, the E are the energies of the individual orbitals
  • Orbitals are the homes of the electrons
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15
Q
  1. What are the Wave Functions
A
  • they are functions that contain all the possible information of the system
  • the square of the wave function gives the probability of finding the electron in a specific region of space around the nucleus
  • this corresponds with the shape of the specific orbital
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16
Q
  1. What are Orbitals?
A
  • they are the regions around the nucleus where electrons exist and can be found
  • they are the mathematical solutions
  • they are specific electron cloud fomations
17
Q
  1. What are the electrons attracted to?
A
  • the positive nucleus
  • this is according to Coulomb’s Law
  • the electron stays near to the nucleus because of this charge
18
Q
  1. What kind of shape is an “s” orbital?
A
  • it is circularly shaped
19
Q
  1. What kind of shape is a “p” orbital?
A
  • it is dumbbell/infinity sign shaped
20
Q
  1. What happens to the probability of finding an electron the further away from the nucleus you move?
A
  • the probabilities drop
  • you are less likely to find an electron the further away you move from the central nucleus
  • the distribution of electron density thins out the further away from the nucleus we move
21
Q
  1. What is needed to move the electron further from the nucleus?
A
  • energy
  • this is because the electron is attracted to the positive nucleus
22
Q
  1. What 3 attributes are specific to each orbital?
A
  1. Shape
  2. Size
  3. Three- Dimensional Orientations

NB: there is a specific quantum number for each of these

23
Q
  1. What is a quantum number?
A
  • it is a numerical index that provides a specific description for a given orbital
24
Q
  1. What shape does a “d” orbital have?
A
  • it is clover shaped
  • this is also known as a double dumbbell shape
25
Q
  1. What shape does an “f” orbital have?
A
  • it has no definite shape due to its complexity
26
Q
  1. What is “L” in orbital terms?
A
  • it is the Orbital Angular Momentum (Azimuthal) Quantum Number
  • it defines the shape of the Orbital
27
Q
  1. What is the numerical value of the following letters representing sub-shells?

27.1: s
27.2: p
27.3: d
27.4: f

A

27.1: 0
27.2: 1
27.3: 2
27.4: 3

28
Q
  1. What is the Principle Quantum number (n)?
A

-is the number in front of the letter

  • as the principle quantum number increases, so does the overall size of the orbital
29
Q
  1. 2s and 3s Orbitals are not solid throughout. There is empty space in certain places. What is this empty space called?
A
  • nodes
30
Q
  1. What is a node?
A
  • it is a region where the probability of finding an electron is exactly zero
  • this only happens with “s” type orbitals
31
Q
  1. How do you work out how many nodes an orbital has?
A
  • you use the formula: n-1
  • FOR EXAMPLE: a 2s orbital has 1 node
    BECAUSE: 2-1=1
32
Q
  1. What happens to the size of the Orbital as the value of “n” increases?
A
  • the “p” and the “s” orbitals will grow in size
33
Q
  1. What is the 3D- Orientation of the Orbital established by?
A
  • it is established by the Magnetic Quantum Number (mL)
34
Q
  1. What are the three ways that the Orbitals can be oriented?
A
  • along the Z Axis (Pz)
  • along the X Axis (Px)
  • along the Y Axis (Py)
35
Q
  1. Read through this summary.
    Do you understand everything?
A
  • yes