l = 1
The second quantum number (l) for the electrons in the 4 p energy sublevel of bromine would be 1.
M1 = -1
The quantum number relating to the size and energy of an orbital
The level of energy possessed by all electrons in one type of orbital. -APEX
The hydrogen atom only has one energy level (shell). The first energy level also contains only one sublevel, 1s sublevel (subshell), which can only hold two electrons. When you get to the second energy level in the second period on the periodic table, it has two sublevels, the 2s and the 2p sublevels. Both of the electrons in the 2s sublevel have the same energy. The 2p sublevel can hold 6 electrons. All of the electrons in the 2p sublevel have the same energy, which is higher than the energy in the 2s sublevel. So, as we move down the periods on the periodic table, we move from the first energy level to the seventh energy level. Each energy level contains specific numbers of sublevels, and all of the atoms within a particular sublevel have equal energy.
The second quantum number (l) for the electrons in the 4 p energy sublevel of bromine would be 1.
ms -1/2
M1 = -1
ms -1/2
ms=-1/2
ms -1/2
M1 = -1
The quantum number relating to the size and energy of an orbital
The 3d sublevel is not filled until after the 4s sublevel, because the 3d sublevel has more energy than the 4s sublevel, and less energy than the 4p sublevel.
The level of energy possessed by all electrons in one type of orbital
It is a surface of constant probability i.e. an electron is just as likely to be found in a small volume anywhere around this surface. Energy sublevel
The level of energy possessed by all electrons in one type of orbital. -APEX