1 describe how the atomic radius(size) and the ionization energy changes\n1. within a group(same column)\n2…

1 describe how the atomic radius(size) and the ionization energy changes\n1. within a group(same column)\n2. within a period(same row)\nsentence starters\nfrom this activity, the models show that as we go down a group, the atomic radius....\nfor example,...\nas we go from left to right in the same period, the atomic radius...\none the other hand, as we go down a group, the ionization energy...\nfinally, as we move from left to right, the ionization energy...\nfor example,...\nin conclusion, the atomic radius influences the ionization energy. in general, the larger atoms....

1 describe how the atomic radius(size) and the ionization energy changes\n1. within a group(same column)\n2. within a period(same row)\nsentence starters\nfrom this activity, the models show that as we go down a group, the atomic radius....\nfor example,...\nas we go from left to right in the same period, the atomic radius...\none the other hand, as we go down a group, the ionization energy...\nfinally, as we move from left to right, the ionization energy...\nfor example,...\nin conclusion, the atomic radius influences the ionization energy. in general, the larger atoms....

Answer

Brief Explanations:

  • Within a group:
    • Atomic radius: As we go down a group, new electron shells are added. For example, in Group 1 (alkali metals), from lithium ((Li)) to francium ((Fr)), the number of electron shells increases. This causes the atomic radius to increase.
    • Ionization energy: Ionization energy is the energy required to remove an electron from an atom. As the atomic radius increases down a group, the outermost electrons are farther from the nucleus and are less strongly attracted. So, ionization energy decreases down a group.
  • Within a period:
    • Atomic radius: As we move from left to right in a period, the number of protons in the nucleus increases (nuclear charge increases). The electrons are added to the same shell. The increased nuclear charge pulls the electrons closer. For example, in period 3, from sodium ((Na)) to chlorine ((Cl)), the atomic radius decreases.
    • Ionization energy: With the decreasing atomic radius from left to right in a period, the electrons are more tightly bound to the nucleus. So, ionization energy generally increases from left to right in a period.

Answer:

  • Within a group:
    • Atomic radius increases (e.g., in Group 1, from (Li) to (Fr) new shells are added).
    • Ionization energy decreases (outer electrons are less tightly bound as radius increases).
  • Within a period:
    • Atomic radius decreases (e.g., period 3, (Na) to (Cl), nuclear charge pulls electrons closer).
    • Ionization energy increases (electrons more tightly bound as radius decreases).