An element with the electron configuration [Xe] 6s^2 4f^14 5d^7 would belong to

Question

An element with the electron configuration [Xe] 6s^2 4f^14 5d^7 would belong to which table? A) transition elements B) alkaline earth elements C) halogens D) rare earth elements E) none of the above 10. Which of the following electron configurations is correct? A) Ga: [Kr] 4s^2 3d^10 4p^1 B) Mo: [Kr]5s^2 4d^5 C) Ca: [Ar] 4s^1 4s^1 3d^10 D) Br: [Kr] 4s^2 3d^10 4p^7 E) Bi: [Xe] 6s^2 4f^14 5d^10 6p^3 11 .Order the elements S, Cl, and F in terms of increasing atomic radii. A) S, Cl, F B) Cl, F, S C) F, S, Cl D) F, Cl, S E) S, F, Cl 12. Which of the following atoms would have the largest second ionization A) Mg B) Cl C) S D) Ca E) Na 13.Consider the following orderings. I. Na^+

Explanation / Answer

9) An element with electronic configuration [Xe] 6s2 4f14   5d7 is Iridium is a transition element.

10) The electron configuration of Bi (Bismuth is correct)

11)               F<Cl<S.
F and Cl is the group-17 halogen, S is in group-16.
along a group, atomic radii decreases as effective nuclear charge increases
Cl is just below F, periodwise. along a period, atomic radii increases, as an extra shell is added

12) The highest second ionization energy would have to be an ion with 1 valence electron, as once it is ionized the first time, it will require much more energy to ionize again since it needs to destroy the energetically favorable full valence orbital.Therefore, since the only element which is in group 1 of the periodic table is Na, or sodium, it has to be answer E.

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