6.3 Notes Periodic Table Trends – ATOMIC RADIUS Nuclear Charge the positive charge of the nucleus due to protons. nuclear charge increases L to R across a period because more protons are added. As nuclear charge increases electrons are pulled closer to nucleus so atomic radius decreases Trend for Atomic Radius Atomic radius decreases going left to right across a period Atomic radius increases going down a group Octet Rule The octet rule states that elements gain or lose electrons to attain an electron configuration of the nearest noble gas with 8 valence electrons. 2 will do but 8 is great!” Trend for Ionic Radius An ion is an atom that has gained or lost an electron Cations lose e- and have a positive (+) charge, become smaller than neutral atom Anions gain e- and have a negative charge, become larger than neutral atom Periodic Table Trends- Ionization Energy Ionization energy is the energy required to remove an electron from an atom in the gaseous state Electrons closest to the nucleus have high ionization energies because they are strongly attracted to the nucleus. Electrons farthest from the nucleus have low ionization energies because they are weakly attracted to the nucleus Trend for Electronegativity Electronegativity describes the tendency of an to attract a shared pair of towards itself. An atom's electronegativity is affected by both its and the distance at which its reside from the charged nucleus. The higher the associated electronegativity value, the more an element or compound attracts electrons towards it.
6.3 Notes – Periodic Table Trends ATOMIC RADIUS Nuclear Charge the positive charge of the nucleus due to protons. nuclear charge increases L to R across a period because more protons are added. As nuclear charge increases electrons are pulled closer to nucleus so atomic radius decreases Trend for Atomic Radius Atomic radius decreases going left to right across a period Atomic radius increases going down a group Octet Rule The octet rule states that elements gain or lose electrons to attain an electron configuration of the nearest noble gas with 8 valence electrons. 2 will do but 8 is great!” Trend for Ionic Radius An ion is an atom that has gained or lost an electron Cations lose e- and have a positive (+) charge, become smaller than neutral atom Anions gain e- and have a negative charge, become larger than neutral atom Periodic Table Trends- Ionization Energy Ionization energy is the energy required to remove an electron from an atom in the gaseous state Electrons closest to the nucleus have high ionization energies because they are strongly attracted to the nucleus. Electrons farthest from the nucleus have low ionization energies because they are weakly attracted to the nucleus Trend for Electronegativity Electronegativity describes the tendency of an to attract a shared pair of towards itself. An atom's electronegativity is affected by both its and the distance at which its reside from the charged nucleus. The higher the associated electronegativity value, the more an element or compound attracts electrons towards it.
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