For a Sc atom in ground electronic state:
1. how many electrons are there in 4s orbitals?
2. how many electrons are there in 3d orbitals?
3. how many electrons are there in 4p orbitals?
4. how many unpaired electrons are there?
5. to what block does Sc belong to in the periodic table (s, p, d, f)?
Why are you having trouble with this. You can look up the answers is many places, including your text/notes. Sc is #21.
1s2 2s2 2p6 3s2 3p6 3d1 4s2
To answer these questions, we need to understand the electron configuration of a neutral Sc (Scandium) atom in its ground electronic state.
1. To determine the number of electrons in the 4s orbital, we first need to know the electron configuration. The electron configuration for Sc is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1. From this configuration, we can see that there are 2 electrons in the 4s orbital.
2. To determine the number of electrons in the 3d orbitals, we look at the electron configuration again. We see that there is only 1 electron in the 3d orbital.
3. To determine the number of electrons in the 4p orbitals, we need to know the electron configuration. However, Sc does not have any electrons in the 4p orbitals in its ground state. Thus, there are no electrons in the 4p orbitals.
4. To determine the number of unpaired electrons, we look at the electron configuration again. We can see that there is only 1 unpaired electron in the 3d orbital.
5. Finally, to determine the block to which Sc belongs in the periodic table, we look at the last electron that enters the atom. In the case of Sc, the last electron enters the 3d orbital. The 3d orbital is located in the d-block of the periodic table, so Sc belongs to the d-block.