Understand Atomic Size and Ionization Energy Trends in the Periodic Table
Explore the periodic trends in atomic size and ionization energy, learning how atomic radius and electron removal energy change across periods and groups. Discover the concepts of shielding and how these trends relate to the placement of elements in the periodic table.
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Presentation Transcript
Periodic Trends Periodic Trends
Atomic Size Scientists use the distance from the center of the nucleus to the boundary of the surrounding electron cloud as the atomic radius. Cause of trends Period: As you go across a row the atomic number(# of protons) increases but no increase in Shielding Ex) A Na atom is larger than an Ar atom because 18 protons can pull on energy levels 1 through 3 with greater strength than 11 protons can.
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Atomic Size Scientists use the distance from the center of the nucleus to the boundary of the surrounding electron cloud as the atomic radius. Group: As you go down a group the number of energy levels increases and shielding occurs. (the # protons increase but the energy levels also increase). Ex) A Na atom is smaller than an Fr atom because energy level #3 is closer to the nucleus than energy level # 7
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Ionization Energy: the amount of energy required to remove an electron from an atom. Period Trend Cause of trends Period: Closer to 8 closer to being happy
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Ionization Energy: the amount of energy required to remove an electron from an atom. Group Trend Cause of trends Group: Ex) A Na atom has a higher I.E. than a Fr atom, because Fr's electron is further from the nucleus...less proton pulling power...AND already has more Energy.
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Electronegativity (electron affinity): a measure of how well an atom can attract and hold an electron from another atom.
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This results in the formation of an ion and it is the ionic radius that will dominate how well the atom can retain the electron. Cause of trends Row proton strength increases across row but size of atom decreases Period
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Ionic Size Gain electron size increase Anion negative ion is larger than its neutral atom Lose electron size decrease Cation positive ion, are smaller than their neutral atom
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