How many unpaired electrons are present in each of these species?
(a) 1s22s23p1
1
ground-state= __________
(b) 1s2 2s2 2p6
0
ground-state=______________
I Cant get the ground state config i think there might be somethign wrong...
In a there is 1 unpaired electron in the ground state. In b unpaired electrons = 0.
i know. i need help with the ground state config
Oh, don't worry! I'll help you figure it out with a little clownish flair. Let's go step by step.
(a) 1s22s23p1
To find the ground-state electron configuration, we can represent it as:
1s^2 2s^2 2p^1
Now, let's count the unpaired electrons. We have one unpaired electron in the 2p orbital. So the answer is 1 unpaired electron! Ta-da!
(b) 1s2 2s2 2p6
For this one, the ground-state electron configuration is:
1s^2 2s^2 2p^6
In this configuration, all the electrons are happily paired up, which means we have no unpaired electrons. Zero, zilch, none at all! So the answer is 0 unpaired electrons! Voila!
Hope that clears things up for you. If you have any more questions, I'm here to clown around with answers!
It seems that the ground-state electron configurations provided are incomplete or contain errors. In order to determine the number of unpaired electrons, we need to have the correct ground-state electron configuration for each species.
Please provide the correct and complete ground-state electron configurations for both (a) and (b), and I will be happy to help you determine the number of unpaired electrons.
To determine the number of unpaired electrons in each species, we first need to write out the ground state electron configuration for each species.
(a) The electron configuration given is 1s²2s²3p¹. To determine the ground state electron configuration, we start from the lowest energy level, which is the 1s orbital. The 1s² means that there are two electrons in the 1s orbital. Moving on to the 2s orbital, we also have two electrons in the 2s². Finally, the 3p¹ indicates that there is one electron in the 3p orbital.
Therefore, the ground state electron configuration for species (a) is 1s²2s²2p¹.
Now, to determine the number of unpaired electrons, we look at the electron distribution in the orbitals. In the ground state electron configuration, we can see that there is one electron in the 2p orbital. Since the 2p orbital has three available slots for electrons (2px, 2py, 2pz), and only one electron is present, one of the slots remains unoccupied. Therefore, there is 1 unpaired electron in species (a).
(b) The electron configuration given is 1s²2s²2p⁶. Similar to before, we begin with the 1s orbital, which contains two electrons, and move on to the 2s orbital, which also contains two electrons. Next, we fill the 2p orbital with six electrons.
Therefore, the ground state electron configuration for species (b) is 1s²2s²2p⁶.
In this configuration, all the orbitals in the 2p sublevel are fully occupied. Since each orbital can hold a maximum of 2 electrons, and all 6 slots are filled, there are no unpaired electrons in species (b).