Periodic Trends. Oct 10 9:43 AM WHAT IS A TREND? A change that is predictable and repeats. ex: seasons, months, days of the week, school day

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1 Periodic Trends Oct 10 9:43 AM WHAT IS A TREND? A change that is predictable and repeats ex: seasons, months, days of the week, school day ATOMIC RADIUS: The distance from the center of the nucleus of an atom to the end of the electron cloud. TREND ACROSS a period (left to right): DECREASES Across a period, protons are added to the nucleus. Electrons are also added, but to the same energy level (i.e. same distance from the nucleus). As the number of protons increases, the positive "pull" on the negative electrons increases pulling the electrons in closer. TREND DOWN a group: INCREASES Ionic Radius: As electrons are added to more energy levels, the inner electrons shield the outer electrons from the pull of the nucleus. The outer electrons have less attraction to the nucleus due to this shielding effect, increasing the atom s size Positive ions are smaller than their neutral atom. Why? Negative ions are larger than their neutral atom. Why? Sep 24 7:50 AM 1

2 Sep 24 8:43 AM Other Trends... Ionization Energy Electronegativity Reactivity All can be explained in terms of the atomic radius trend. Sep 23 6:26 PM 2

3 IONIZATION ENERGY: TREND ACROSS a period: INCREASES the energy needed to remove the outermost electron from an atom as the atom s radius decreases, the valence electrons are held tighter by the nucleus, requiring more energy to remove one NOTE: non-metals have such HIGH ionization energy that it becomes impossible to remove an electron...they cannot form positive ions Pull TREND DOWN a family: DECREASES as the atom s radius increases, the valence electrons are held less tightly by the nucleus, requiring less energy to remove one Sep 24 9:24 AM Successive Ionization Energies 1st ionization energy: 2nd ionization energy: 3rd ionization energy: the energy needed to remove the 1st electron the energy needed to remove the 2nd electron the energy needed to remove the 3rd electron and so on... Sep 23 6:35 PM 3

4 Successive Ionization Energies Cont... each additional electron that is removed requires more energy once a metal ion achieves a noble gas electron configuration there is a LARGE jump in ionization energy the ionization energy increases so much that it becomes impossible to remove another electron this is why alkali metals, alkaline earth metals and aluminum all have specific positive charges Sep 23 6:45 PM Successive Ionization Energies Cont... For example... Mg 1s 2 2s 2 2p 6 3s 2 1st ionization energy = 737 kj Mg +1 1s 2 2s 2 2p 6 3s 1 Mg +2 2nd ionization energy = 1450 kj BIG JUMP 3rd ionization energy = 7731 kj 1s 2 2s 2 2p 6 same configuration as Ne Sep 23 7:16 PM 4

5 Ionization Energies in KJ/mol H 1312 He Li Be B C N O F Ne Na Mg Sep 24 9:17 PM ELECTRONEGATIVITY: the ability of an atom to attract an additional electron when bonded to another atom TREND ACROSS a period(left to right): INCREASES as the atom s radius decreases, the nucleus has a stronger attraction for an extra electron NOTE: Metals have such low electronegativity that they cannot attract an additional electron...they do not form negative ions. TREND DOWN a group: DECREASES ** the atom s radius increases, the nucleus has a weaker hold on an extra electron Noble gases have no electronegativity. Noble gases already have a filled valence shell so they do not need to attract any additional electrons. ** Sep 24 9:31 AM 5

6 Trends Summarized Atomic Radius Ionization Energy Electronegativity decreases increases increases increases decreases decreases Oct 10 9:21 AM Reactivity Trends Metals lose electrons - low ionization energy Nonmetals gain electrons - high electronegativity nonmetal 7 gain Metal Reactivity: TREND ACROSS a period (left to right): DECREASES as the radius decreases, electrons move closer to the nucleus feeling more attraction making it harder to remove an electron TREND DOWN a group: INCREASES metal 1 lose as the radius increases, electrons move farther from the nucleus feeling less attraction making it easier to remove an electron Non-Metal Reactivity: TREND ACROSS a period: INCREASES as the radius decreases, easier for an extra electron to feel the pull from the nucleus TREND DOWN a group: DECREASES as the radius increases, harder for an additional electron to be added (less attraction felt from the nucleus) Oct 13 3:21 PM 6

7 Practice Examples... Choose from the following answers; K, Ca, Rb, Sr 1. Which element has the largest atomic radius? Rb 2. Which element has the largest ionization energy? Ca 3. Which element has the lowest electronegativity? Rb 4. Which metal of the group would be the least reactive? Ca Sep 21 1:06 PM 7

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