Multiple Choice
How many electrons can occupy the first energy level (n = 1) of an atom?
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10. Periodic Properties of the Elements
The Electron Configuration
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In which of the following orbitals would an electron, on average, be closest to the nucleus?
A
3s
B
1s
C
2s
D
2p
Verified step by step guidance1
Recall that the average distance of an electron from the nucleus depends primarily on the principal quantum number $n$. The smaller the value of $n$, the closer the electron is to the nucleus on average.
Identify the principal quantum number $n$ for each orbital: for 1s, $n=1$; for 2s and 2p, $n=2$; for 3s, $n=3$.
Understand that within the same principal quantum number, s orbitals have electron density closer to the nucleus than p orbitals, but the principal quantum number has a greater effect on average distance than the type of orbital.
Compare the orbitals given: since 1s has the smallest $n$ value, electrons in the 1s orbital are, on average, closest to the nucleus compared to 2s, 2p, or 3s orbitals.
Conclude that the electron in the 1s orbital is closest to the nucleus on average because it has the lowest principal quantum number, which dominates the average distance factor.
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