Final answer:
The full electron configurations for the requested atoms and ions are N: 1s2 2s2 2p3, O: 1s2 2s2 2p4, Sr2+: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6, and I−: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6.
Step-by-step explanation:
To write the full electron configurations for the atoms and ions N, O, Sr2+, and I−, we start by referencing their positions on the periodic table. The configuration is built by adding electrons to atomic orbitals following the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Here are the full electron configurations:
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- N (Nitrogen): 1s22s22p3
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- O (Oxygen): 1s22s22p4
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- Sr2+ (Strontium ion): Sr has an atomic number of 38, meaning its neutral atom configuration is 1s22s22p63s23p63d104s24p65s2. As Sr2+, it loses two electrons, which come from the outermost shell, resulting in 1s22s22p63s23p63d104s24p6.
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- I− (Iodide ion): Iodine's atomic number is 53, so its neutral atom configuration is 1s22s22p63s23p63d104s24p64d105s25p5. The I− ion has gained an extra electron, completing the 5p subshell, resulting in 1s22s22p63s23p63d104s24p64d105s25p6.