incorrect\nyour answer is incorrect.\nlist these electron subshells in order of increasing energy.\n6s, 5p…

incorrect\nyour answer is incorrect.\nlist these electron subshells in order of increasing energy.\n6s, 5p, 4f, 6p\nnote for advanced students: you may assume these subshells are all in an atom with many electrons, not a hydrogen atom.\nyour answer

incorrect\nyour answer is incorrect.\nlist these electron subshells in order of increasing energy.\n6s, 5p, 4f, 6p\nnote for advanced students: you may assume these subshells are all in an atom with many electrons, not a hydrogen atom.\nyour answer

Answer

Explanation:

Step1: Recall the (n + l) rule

The energy of an electron sub - shell is determined by the sum of the principal quantum number (n) and the angular momentum quantum number (l). For s sub - shell, l = 0; for p sub - shell, l = 1; for f sub - shell, l = 3.

Step2: Calculate (n + l) for each sub - shell

For 6s: n = 6, l = 0, so n + l=6 + 0 = 6. For 5p: n = 5, l = 1, so n + l=5 + 1 = 6. For 4f: n = 4, l = 3, so n + l=4 + 3 = 7. For 6p: n = 6, l = 1, so n + l=6 + 1 = 7. When (n + l) values are the same, the sub - shell with lower n has lower energy.

Step3: Order the sub - shells

Since 5p and 6s have (n + l)=6 and 5 < 6, 5p has lower energy than 6s. Also, 4f and 6p have (n + l)=7 and 4 < 6, 4f has lower energy than 6p.

Answer:

5p, 6s, 4f, 6p