periodicity

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8 Terms

1
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atomic radius trends

  • increase going from TOP to BOTTOM and RIGHT to LEFT

  • more shielding, less protons (Zeff) to “tighten” the radius.

2
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ionic radius trends

  • within the same period, anions are always larger than cations.

  • increase from TOP to BOTTOM (more shielding) and from RIGHT to LEFT (protons)

3
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what is the trend for the isoelectronic series?

  • as a positive nuclear charge INCREASES, the ionic radius DECREASES.

    • greater positive charge pull electrons closer to the nucleus.

  • as negative charge DECREASES, the ionic radius INCREASES.

    • more negative ions experience electron repulsion, increasing radius.

4
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ionization energy trend (energy required to remove an electron)

  • increases going from LEFT to RIGHT and from BOTTOM to TOP.

5
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electron affinity trend (energy of gaining an electron)

  • increases from BOTTOM to TOP (less shielding) and LEFT to RIGHT (closer to the octet)

  • more exothermic = more energy being released when an electron is added.

6
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electronegativity trends (the ability of an atom to attract shared electrons in a covalent bond)

  • increases from BOTTOM to TOP (less shielding) and LEFT to RIGHT (higher Zeff/more protons)

7
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what are the reactivity trends for Group 1 alkali metals?

  • high reactivity (increases going DOWN)

    • this trend can be explained with ionization: lower ionization (less attraction & stability) = easier electron loss = losing single electron = forms a positive ion = more reactivity.

8
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what are the reactivity trends for