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MED 102- GENERAL CHEMISTRY > 5. ATOMIC AND ELECTRONIC STRUCTURE (PART 3) > Flashcards

5. ATOMIC AND ELECTRONIC STRUCTURE (PART 3) Flashcards

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1
Q
  1. Provide names for the following labels?
A
  1. Element
  2. Total Electrons
  3. Box Orbital Diagram
  4. Electron Configuration
  5. Number of Electrons
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2
Q
  1. What does Hund’s Rule state?
A
  • we should maximise the number of unpaired spin-up electrons
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3
Q
  1. What happens when we pair up electrons in the same orbital?
A
  • we force them to share the same space
  • both electrons are negative
  • both electrons have the same charge
  • these two electrons repel each other
  • the increase in repulsion causes an increase in the energy of the atom
  • the atom is less stable

NB: this is why we keep electrons unpaired

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4
Q
  1. How and why do we keep electrons unpaired?
A
  • we keep them unpaired by placing them in adjacent orbitals
  • they have a lower repulsive energy when they are unpaired
  • there is no electromagnetic resistance
  • the orbital is much more stable
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5
Q
  1. Do we place the unpaired electrons as spin-up or spin-down electrons?
    WHY?
A
  • spin up electrons
  • they have a lower energy as they are working in the same direction of the magnetic field
  • the atom is more stable
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6
Q
  1. Which of these Carbon atoms is the most stable?
A
  • Option D
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7
Q
  1. What does a violation of Hund’s Rule lead to?
A
  • it leads to excited electronic states
  • these have a higher energy than the lowest ground state
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8
Q
  1. Provide names for the following labels?
A
  1. Ground state
    (the lowest energy state)
  2. Excited State
    (higher energy)
  3. Excited State
    (higher energy)
  4. Excited State
    (higher energy)
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9
Q
  1. What is Pauli’s Exclusion Principle?
A
  • no two electrons in a given atom can have the same set of 4 quantum numbers
  • at least one of the quantum numbers has to be different
  • the quantum numbers are: n, L, mL, mS
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10
Q
  1. Which of these are the two best examples of Pauli’s Exclusion Principle?
A

B and C

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11
Q
  1. What type of Electronic Configuration is this?
A

Full Electronic Configurations

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12
Q
  1. What type of Electronic Configuration this is?
A

Noble Gas Electron Configurations

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13
Q
  1. What type of Electronic Configuration is this?
A

Condensed Electronic Configurations

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14
Q
  1. Provide names for the following labels?
A
  1. Full Electronic Configuration
  2. Condensed Electronic Configuration
  3. Box Orbital Diagram
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15
Q
  1. What kind of Electronic Configuration is this?
A
  • it is an Anomalous Electronic Configuration
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16
Q
  1. What happens in an Anomalous Electron Configuration?
A
  • one electron is promoted from the 4s to the 3d sub shell
  • this is to achieve a d5 (half full d sub shell) or a d 10 (full d sub shell) configuration
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17
Q
  1. Why is a d5 or a d10 sub shell desirable?
A
  • they have a special degree of stability
18
Q
  1. Can you change a d3 or a d8 sub shell to a d5 or a d10 sub shell?
A
  • NO
  • you can only change a d4 or a d9 sub shell
19
Q
  1. Elements in which other groups will have anomalous electronic configurations?
A
  • Group 6
  • Group 11
20
Q
  1. Electrons from which orbital are likely to leave first when there is a transfer of electrons (ionic/covalent bonding)?
A
  • electrons from the s orbital
  • this is the outermost electron configuration
  • these electrons are found in the outermost shell of the atom
21
Q
  1. What is another name for the electrons found in the outermost shell, and what do they do?
A
  • they are called Valence electrons
  • they are exchanged between other atoms
22
Q
  1. What is shielding?
A
  • it is when we cannot see the nucleus of the atom as something is blocking us from seeing it
  • an electron cloud or a higher density of electrons in the shells is what causes this shielding
23
Q
  1. What is the value and the symbol of the valence electrons of Group 1 (Alkali Metal) elements?
A
  • s1
  • they have an extra electron to freely give away to reach an octet (most stable state)
24
Q
  1. What is the value and the symbol of the valence electrons of Group 7 (halogens) elements?
A
  • p6
  • they are seeking an extra electron to reach an octet (most stable state)
25
Q
  1. What is atomic radius?
A
  • the distance from the centre of the atom to its circumference
  • it can also be seen to be the size of the atom
26
Q
  1. How does the atomic radius react with regard to groups and periods?
A
  • it increases as we move down the group
  • it decreases as we move right along the period
27
Q
  1. Why does the atomic radius increase as we move down the group?
A
  • this is due to the addition of extra shells as we move down the group
  • the extra shells have an increasing Principle Quantum Number (n)
  • this makes them larger in size
28
Q
  1. Why does the atomic radius decrease as you go along the period?
A
  • electrons are being placed in the same shell as we move along the period
  • these shells are still at the same distance from the nucleus as they were before the addition of the other electrons
  • the nuclear charge increases by one unit each time we move to the right
  • the increasing nuclear (positive) charge attracts the electrons in the shells
  • this pulls the shells closer to the nucleus
  • this decreases the size of the atom
29
Q
  1. What is the Ionisation energy?
A
  • the energy required to remove one electron from a neutral atom
  • it is the energy we have to use up in order to remove the electron from the attractive force of the nucleus
30
Q
  1. Which law is proven through the fact that electrons are attracted to the nucleus?
A
  • Coulomb’s law
31
Q
  1. What is the formula to work out the ionisation energy?
A
32
Q
  1. What does Q1 represent?
A
  • the effective nuclear charge
    (the number of protons-the number of intermediate electrons)
33
Q
  1. What are intermediate electrons?
A
  • electrons that shield the nucleus
  • this ensures that the valence electron does not feel the full positive charge
34
Q
  1. What does Q2 represent?
A
  • it is equal to the value of one electron
    (Q2 = -1)
35
Q
  1. What happens the atomic number increases?
A
  • Q1 increases
  • the energy of attraction to the electron also increases
  • this makes it much more difficult to separate an electron from it’s attractive force to the nucleus
36
Q
  1. What does R represent?
A
  • the distance of the electron from the nucleus
37
Q
  1. What happens when R increases?
A
  • the energy of attraction decreases
38
Q
  1. What happens when the number of atomic shells increases?
A
  • R increases
  • energy of attraction decreases
39
Q
  1. What has exactly the opposite trend than the atomic radius?
A
  • the ionisation energy
40
Q
  1. Read through the summary.
    Does everything make sense?
A
  • yes

MED 102- GENERAL CHEMISTRY (27 decks)

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