Question

match the noble - gas notations with their correct elements.
kr5s²4d¹⁰5p³
xe6s²4f¹⁴5d⁶
rn7s²5f¹¹
kr5s²4d¹⁰5p⁵
antimony osmium einsteinium iodine

Explanation:

1. For the electron - configuration $[Kr]5s^{2}4d^{10}5p^{3}$, the number of electrons beyond the noble - gas core $Kr$ is $2 + 10+3=15$. The element in the 15th group (Group 15) and 5th period is Antimony ($Sb$).
2. For the electron - configuration $[Xe]6s^{2}4f^{14}5d^{6}$, the number of electrons beyond the noble - gas core $Xe$ is $2 + 14+6 = 22$. The element in the 8th group (Group 8) and 6th period is Osmium ($Os$).
3. For the electron - configuration $[Rn]7s^{2}5f^{11}$, the number of electrons beyond the noble - gas core $Rn$ is $2+11 = 13$. The element in the actinide series with this electron - configuration is Einsteinium ($Es$).
4. For the electron - configuration $[Kr]5s^{2}4d^{10}5p^{5}$, the number of electrons beyond the noble - gas core $Kr$ is $2 + 10+5 = 17$. The element in the 17th group (Group 17) and 5th period is Iodine ($I$).

Answer:

$[Kr]5s^{2}4d^{10}5p^{3}$ - Antimony
$[Xe]6s^{2}4f^{14}5d^{6}$ - Osmium
$[Rn]7s^{2}5f^{11}$ - Einsteinium
$[Kr]5s^{2}4d^{10}5p^{5}$ - Iodine