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Ionisation Energy

Ionisation Energy. Based on the position of calcium & copper in the periodic table, make comparisons with respect to their: Atomic radius ionisation energy Metallic character Order in the Activity Series (more likely to oxidize) Extraction method for each

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Ionisation Energy

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  1. Ionisation Energy

  2. Based on the position of calcium & copper in the periodic table, make comparisons with respect to their: • Atomic radius • ionisation energy • Metallic character • Order in the Activity Series (more likely to oxidize) • Extraction method for each • Possible experiment(s) that will help to compare their reactivity

  3. Problem #1 • Avoid personification “…because he has a larger nucleus….”

  4. Problem #2 • Stating the obvious “…both elements differ in their radius and number of protons….”

  5. Problem #3 • Positions don’t mean anything! “…because it is above, it is more reactive….” The apple must be more reactive, it is found above. I am found below, therefore, I must be less reactive

  6. Problem #4 • Cause and Effect “…because it is on the ‘left’, it is more reactive” versus “…because it is more reactive, it is on the left”

  7. Problem #5 • Extraction with Carbon or CO Used for metals that are slightly more reactive than copper.

  8. Problem #6 • Froth floatation & electrolysis of Cu These are not methods of extraction; these points are irrelevant (floatation is to mechanically separate Cu; electrolysis is to purify it in the very end)

  9. Atomic Radius • Atomic radii decrease across a period as each subsequent element gains an additional proton, creating a greater attraction to its valence shell. • Ca, having less protons than copper, has a weaker attraction for its outer electrons. • This results in Ca having a weaker nuclear attraction and a larger radius than that of Cu

  10. Ionisation Energy • Ionisation energy is the energy required to remove an electron from an atom • Since Ca has a larger radius, it requires less energy to remove the valence electron as it is further away from the oppositely charged nucleus • Cu, having a smaller radius, exerts a greater attraction for is electrons that are closer to the nucleus. This makes it difficult to remove the attracted electron which makes the I.E. greater for Cu

  11. Metallic Character • Metals in Group 2 will readily lose their valence electrons to achieve noble gas configurations due to its larger atomic radii and lower ionisation energies • The ease to which is loses electrons makes Ca more metallic in character in comparison to Cu which doesn’t readily lose its electron

  12. Activity Series • When comparing the reactivity series of metals, Ca, with the lower ionisation energy, will readily lose its electron making it more reactive compared to Cu • Therefore, Ca will readily oxidize to form an ion compared to Cu

  13. Experiments React each metal with each other’s metal ion, as follows: Ca (s) + Cu+2 (aq)  Ca+2 (aq) + Cu (s) Cu (s) + Ca+2 (aq)  No REACTION (copper is not reactive enough to displace Calcium ions in solution)

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