Write the difference between 1 S and 2 S orbitals
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Answer:
1s and 2s sub-orbitals are nearest to the nucleus. The main difference between 1s and 2s orbitals is the difference of their energy level, which is, 2s orbital is a higher energy level than 1s orbital.
What is 1s Orbital?
1s orbital is the orbital that is closest to the nucleus. It has the lowest energy among other orbitals. It is also the smallest spherical shape. Therefore, the radius of s orbital is small. There can be only 2 electrons in the s orbital. The electron configuration can be written as 1s1, if there is only one electron in the s orbital. But if there is a pair of electrons, it can be written as 1s2. Then the two electrons in the s orbital move to the opposite directions because of the repulsion that occurs due to the same electrical charges of the two electrons. When there is an unpaired electron, it is called paramagnetic. That is because it can be attracted by a magnet. But if the orbital is filled and a pair of electrons are present, the electrons cannot be attracted by a magnet; this is known as diamagnetic.
What is 2s Orbital?
The 2s orbital is larger than 1s orbital. Hence, its radius is larger than that of the 1s orbital. It is the next closet orbital to the nucleus after 1s orbital. Its energy is higher than 1s orbital but is lower than other orbitals in an atom. 2s orbital also can be filled only with one or two electrons. But 2s orbital is filled with electrons only after the completion of 1s orbital. This is called Aufbau principle, which indicates the order of electron filling into sub-orbitals.
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