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1. Rb, Mg, P, Cl
2. Ba, Ca, Fe, Al, O
3. IE is the energy needed to remove valence electron from the atom (atom is in gas phase).
Down a group, the IE decreases (less CF so less tightly held)
Across a period, the IE increases (more CF so more tightly held)
4. Be to B, decrease CF so decrease IE due to valence electron added to B is in the p block as opposed to Be valence electron are in s block so p block valence electron is slightly further from the nucleus so less CF and lower IE.
5. Fr
6. Noble Gases, they have highest CF (highest IE) and they have completely filled outer energy level (energy shell).
7. Cs, Ca, Ni, C, O
8. Will discuss definition. Going across a period, since the nuclear charge is increasing (while added valence electron are added to same energy level), the CF is increasing causing valence electron (shared or unshared) to be more tightly held (closer) increasing EN value of element. As you go down a Group, the valence electrons are being found in higher and higher energy level so electron are held less tightly (lower CF) and EN decreases.
9. Nuclear charge (addition of protons in nucleus) and what energy level valence electron are being placed (found).
10. As you go across a period, the nuclear charge increase ( valence electron are being placed in the same energy level) so the CF increases. Going down a Group, the valence electrons are being placed in higher and higher energy levels causing them to be farther from nucleus causing the CF to decrease.
11. For metals, atom will lose its valence electron(s) (has a lower CF thereby low Ionization Energy), the Atomic radii is always greater than Ionic radii. For non-metals, atom gains electrons valence electrons (has a high CF) and due to electron - electron repulsion, the Ionic radii is always lager than the Atomic radii.