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- Explain why boron (B) has a higher ionization energy than fluorine (F).
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- Explain why the first innization energy of Ca is greater than that of K, whereas the second ionization energy of Ca is lower than the second ionization energy of K.(a) Briefly describe how the atomic radii and ionization energies of group 1A(1) elements compared with those of group 8A(18). Also, explain why the values of these properties are so different between these two groups. 2.Cesium has 1 valence electron. How many possible bonds can be formed and why?
- Why fluorin has low electron affinity as compared to chlorine?Rank lithium, fluorine, and nitrogen in order of decreasing ionization energyAll of the following statements concerning the characteristics of the halogens are true except which: a) The first ionization energies decrease as the atomic numbers of the halogens increase. b) Fluorine is the best oxidizing agent. c) Fluorine atoms have the smallest radii. d) Iodine liberates free bromine from a solution of bromide ion. e) Fluorine is the most electronegative of the halogens.
- 1. Which halogen has the highest ionization energy? Explain why. 2. Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.3. Does the reaction of a main-group metal oxide in water produce an acidic or a basic solution? Write a balanced equation for the reaction of a Group 2A(2) oxide with water.What causes the changes in ionisation energy across period 2 elements?