Periodic Trends

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19 Terms

1

periodicity

  • Trends or recurring variations in element properties with increasing atomic numbers

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2
  • electronegativity

  • The tendency of an atom to attract electrons in a bond to itself

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3
  • ionization energy

  • Energy required to remove an electron from a gaseous atom or ion/remove from the 1rst electron in the valence electron’s shell

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4
  • Atomic Radius

  • One half of the distance between the nuclei of 2 identical atoms when they are joined by a covalent bond

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5
  • Nuclear Charge

  • The pull exerted on a specific electron by the nucleus (# of protons)

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6
  • sheilding

  • when another electron blocks the attraction of an additional electron to the nucleus

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7
  • effective nuclear charge

  • the regular amount of protons, or the nuclear charge (z), with sheilding taken into account; zeff=z-sheilding

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8
  • across a period, atomic radius __________ because ___________

decreases because the effective nuclear charge (zeff) increases while shielding remails constant (n is constant), and electrons are pulled closer by increasing atomic number/protons in the nucleus, causing more attraction and a smaller atomic radius

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9
  • down a group, atomic radius __________ because ___________

increases because there are more energy levels; the principal quantum number (n, vertical numbers) increases as energy levels are added, giving rise to a larger atomic radius

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10

Why Exceptions for atomic radius happen

  • a new subshell (s, p, d, f) is added to the outermost energy level; instead of decreasing, it increases

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11
  • Exceptions for atomic radius

  • Mg—>Al

    • [Ne]s2—>[Ne]3s2,3p1

  • Zn—>Ga

    • [Ar] 4s2,3d10—>[Ar] 4s2,3d10, 4p1

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12
  • across a period, ionization energy ___________ because ___________

increases because the effective nuclear charge (zeff) goes up with the increasing atomic number, causing more attraction; this makes it more difficult to remove a valence a valence electron, meaning more energy will be required

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13
  • down a group, ionization energy __________ because ____________

decreases because more energy levels are present, meaning that there are more core electrons (electrons close to the center), giving rise to more sheilding; there is therefore less attraction, making it easier to remove a valence electron and causing more blockage; this blockage makes it easier to take an electron away with less energy required

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14

why exceptions for ionization energy happe

  • when 1 orbital is full or half full, it is more stable and harder for an electron to be removed, making it decrease

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15
  • exceptions for ionization energy

  • Be—>B

  • Mg—>Al

  • N→O

  • P—>S

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16
  • Across a period, electronegativity ___________ because ___________

increases because there is more effective nuclear charge (zeff), meaning that it is more attractive to valence electrons

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17
  • down a group, electronegativity _______ because ____________

decreases because there are more energy levels, meaning that there are more core electrons and therefore more sheilding; there is more distrance between valence electrons and the nucleusl it is less attractive to the electrons

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18

why exceptions happen for electronegativity

  • electrons aren’t necessary because an atom is already stable with a full outer shell

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19

exceptions for electronegativity

  • noble gases are already stable so they have very little electronegativity

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