We're asked to write the electron configuration for the following ions, and determine which have noble-gas configurations.
Recall that when an atom forms an ion it either gains or loses electrons:
The valence electrons are found in the highest numbered orbital or higher energy orbital in a subshell.
For this problem, we need to do these steps:
Step 1: Determine # of electrons from atomic number using Periodic Table
Step 2: Write ground-state electron configuration
Ground-state means that the element is in its lowest energy form (not in excited state).
Step 3: Write electron configuration of each ion
Step 4: Compare with nearest noble gas to determine whether it has a noble gas configuration
Recall that electron configurations are written from lower energy to higher energy orbital.
The following periodic table shows the orbitals in order of increasing energy levels: s < p < d < f:
Recall that the distribution of electrons for each atomic orbital are:
s _ 1 orbital → can hold a maximum of 2 electrons
p _ _ _ 3 orbitals → can hold a maximum of 6 electrons
d _ _ _ _ _ 5 orbitals → can hold a maximum of 10 electrons
f _ _ _ _ _ _ _ 7 orbitals → can hold a maximum of 14 electrons
Write the electron configuration for the following ions, and determine which have noble-gas configurations:
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Electron Configuration concept. You can view video lessons to learn Electron Configuration. Or if you need more Electron Configuration practice, you can also practice Electron Configuration practice problems.
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Based on our data, we think this problem is relevant for Professor Stewart's class at Sacramento City College.