Want this question answered?
Aluminum has 13 electrons. Use aufbau principle or periodic table to put these electrons into orbitals. 1s2 2s2 2p6 3s2 3p1 Because there is a lone electron in the p orbital that is not paired, aluminum in its ground state has 1 unpaired electron.
Arsenic is paramagnetic because the electron configuration is {Ar}4s^2,3d^10,4p^3. Due to the unpaired electron at the end (4p^*3*) the atom in ground state is paramagnetic. **OR Arsenic would be paramagnetic since the 4 p orbitals each contain one electron with parallel spin. These three unpaired electrons give arsenic its paramagnetic property.
Add the electrons in accordance with the aufbau principle and then count the unpaired ones.
Two
When an electron returns to its ground state it emits energy in the form of light.
These elements are B, Al Br.
1 unpaired electron
1 number of unpaired electron.
Exactly 0.
There are 0 unpaired electrons which would make it diamagnetic
Aluminum has 13 electrons. Use aufbau principle or periodic table to put these electrons into orbitals. 1s2 2s2 2p6 3s2 3p1 Because there is a lone electron in the p orbital that is not paired, aluminum in its ground state has 1 unpaired electron.
mg
Mn is configured: [Ar] 4s2 3d5 , soMn2+ has an electron configuration of: [Ar] 4s0 3d5It looks like that 5 or 3 or (at least) 1 (one) electrons are to be unpaired.
There are 4 unpaired electrons in the ground state electron configuration of an Fe atom. These 4 unpaired electrons are in the 3d subshell.
Arsenic is paramagnetic because the electron configuration is {Ar}4s^2,3d^10,4p^3. Due to the unpaired electron at the end (4p^*3*) the atom in ground state is paramagnetic. **OR Arsenic would be paramagnetic since the 4 p orbitals each contain one electron with parallel spin. These three unpaired electrons give arsenic its paramagnetic property.
there is only one unpaired electron in copper
3 unpaired electrons