All p orbitals are the same - px, py, pz - 2 electrons in each, 6 in a p orbital in total.
What you say is true for a 2px prbital, i.e. where the principal quantum number n=2. Let's consider hydrogen. When l=2, as befits a p-orbital, n=2 is the smallest value for the principal quantum number n for which the radial equation has a solution. That means it is the smallest n such that there is a solution with energy -13.6/n^2. Since it is the lowest energy for which the radial equation (with l=1) has a solution, the radial part of the wave function has no node. In contrast, 3p orbitals do have radial nodes, but 3d orbitals don't, for the same reason.
6total 2 in px 2 in py and 2 in pz
Cartesian coordinates. However ... there are 3 p orbitals for each principal quantum number, but representing them as px, py, and pz is simply a human mathematical convenience; they're all equivalent and it's simply a convenient way of orthogonalizing them. The d and f orbital names and representations are even less "real".
Six in p orbital, in each sublevel of p (px, py, pz) there are two electrons at max.
The px orbital has a magnetic quantum number value of -1, and the py orbital has a magnetic quantum number value of 0.
Since they are p orbitals, 6 electrons are occupied in the 3p orbital. there are 3 types of p orbital, px, py and pz
Maximum of two in each of the p orbital. there are three p orbitals (px, py and pz)
An orbital can only occupy maximum of 2 electrons. As p orbital consist of 3 orbitals. And has 3 orientations. Px, Py, Pz. So as there are 3 orbitals so p orbital can occupy at the maximum 6 electrons regardless of principle quantum no.. In 4p 4 is principle quantum no. So it represent 4p represent the p orbital of 4th shell. So it also occupy at the maximum of 6 electrons.
All p orbitals are the same - px, py, pz - 2 electrons in each, 6 in a p orbital in total.
What you say is true for a 2px prbital, i.e. where the principal quantum number n=2. Let's consider hydrogen. When l=2, as befits a p-orbital, n=2 is the smallest value for the principal quantum number n for which the radial equation has a solution. That means it is the smallest n such that there is a solution with energy -13.6/n^2. Since it is the lowest energy for which the radial equation (with l=1) has a solution, the radial part of the wave function has no node. In contrast, 3p orbitals do have radial nodes, but 3d orbitals don't, for the same reason.
6total 2 in px 2 in py and 2 in pz
Two types,sigma bonds (bond is along the ais between the atoms, formed by pz-pz overlap.pi bonds ("above and below2 the bond axis, thers a nodal plane through te atoms) formed by overlap px-px, py-py
It hold 6 thre p orbital (Px Py Pz) and each one hold two so total is six electron can p orbital
Six in p orbital, in each sublevel of p (px, py, pz) there are two electrons at max.
Six in p orbital, in each sublevel of p (px, py, pz) there are two electrons at max.
Cartesian coordinates. However ... there are 3 p orbitals for each principal quantum number, but representing them as px, py, and pz is simply a human mathematical convenience; they're all equivalent and it's simply a convenient way of orthogonalizing them. The d and f orbital names and representations are even less "real".