Atoms used to be thought to look like little solar systems. Now they are thought to be nesting shells of probability density functions known as orbitals. The S1 and P1 orbitals are the first two filled with other S and P orbitals following along with the various D and F orbitals. The S orbitals are essentially spheres with the P orbitals looking like infinity signs.
Aside: A probability density function maps out where the electron is most likely to be in relation to the nucleus of the atom - not that it is there, just likely to be.
s and p relate to the orbit where the electron most likely is. s orbitals tend to be spherically symmetric around the nucleus, whereas p orbitals would look like two identical balloons tethered at the nucleus.
The s and p orbitals are further classified by the addition of a number, so for example the 1s orbital is closer to the nucleus then the 3s and so on
An s-orbital is spherically symmetric. There are three p orbitals which are at right angles to one another and are called the px, py and pz .
Each orbital can ONLY hold a maximum of two electrons ( Pauli's exclusion principle), these two electrons have opposite spins.
For each principal quantum number n (sometimes called the shell) there is just one
s-orbital (eg 1s, 2s, 3s etc) and for principal quantum numbers 2 and above three p orbitals.,(2px, 2py, 2pz, 3px, 3py, 3pz etc)
The energy sequence low to high is
1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f etc.
The S orbital is spherical (s for sphere). The p orbital looks like an infinity sign (or an 8), with the crossover, being the nucleus). The p orbital is often described as dumbbell shaped.
the s orbital is lower in energy than the p orbital
s orbitals are spherical, so there cannot be any angle 'between' an s orbital and a p orbital. However, each lobe of a p orbital is perpendicular (90 degrees in all directions) to the surface of an s orbital.
Electron in s-orbital is closer to nucleus than electron in p-orbital and electron in p-orbital is closer to nucleus than electron in d-orbital and so on. So,more energy is requried to remove electron from s-orbital than electron in p-orbital in spite of both having same principal quantum number. Similarly, p orbital will require more energy than d-orbital. this is called penetrating effect. it decreases in order s>p>d>f>... Note that Orbital should have same "n"
The s orbital is lower in energy than the porbital.
An s orbital
the s orbital is lower in energy than the p orbital
The s orbital fills before the p orbital because it has lower energy, and is more stable.
s-orbital more affinity to electrons than p when 'empty'
The s orbital is lower in energy than the porbital.
s orbitals are spherical, so there cannot be any angle 'between' an s orbital and a p orbital. However, each lobe of a p orbital is perpendicular (90 degrees in all directions) to the surface of an s orbital.
Electron in s-orbital is closer to nucleus than electron in p-orbital and electron in p-orbital is closer to nucleus than electron in d-orbital and so on. So,more energy is requried to remove electron from s-orbital than electron in p-orbital in spite of both having same principal quantum number. Similarly, p orbital will require more energy than d-orbital. this is called penetrating effect. it decreases in order s>p>d>f>... Note that Orbital should have same "n"
It has a lower energy level. All else being equal, electrons tend to go into the lowest energy orbital with space available.
The s orbital is lower in energy than the porbital.
The orbital names s, p, d, and fstand for names given to groups of lines in the spectra of the alkali metals. These line groups are called sharp, principal, diffuse, and fundamental.
An s orbital
No. Helium is the only noble gas to have an empty p-orbital, and has one full s-orbital. The rest all have at least one of each orbital full.
120 degrees