How does 2s orbital differ from a 1s orbital?

Answer 1

1s and 2s orbitals differ in that 2s orbitals lie farther away from the nucleus in the next principle energy level. Other than that, they occupy the same shape of orbital, spherical, as indicated by the s.

Answer 2

There are a number of differences:-

• The energy of the "s is higher than the 1S
• The 1s orbital has no radial nodes, whereas the 2s has 1. (A radial node is a spherical surface where the probability of finding the the electron is zero)
• The 2s orbital is "bigger" than the 1s , the electron density of the 2s is higher further out from the nucleus.

Answer 3

There are three loops making up the 2p orbital. They simply are oriented differently, at 90 degrees to one another. Each has two electrons at most, each orbiting in reversed directions. They can only be distinguished as different atomic pathways, but not differentiated by properties.

Answer 4

The orbital occupied by the hydrogen electron is called a 1s orbital. The "1" represents the fact that the orbital is in the energy level closest to the nucleus. The "s" tells you about the shape of the orbital. s orbitals are spherically symmetric around the nucleus

a 2s orbital - This is similar to a 1s orbital in terms of its shape, except the electron occupying the 2s orbital will, usually, be further away from the nucleus than an electron in the 1s orbital.

- this is an orbital at the second energy level.

Answer 5

The 2s orbital is the same as the 1s orbital except that it is at a higher engery level. Like the 1s orbital it is spherical in shape and can hold up to 2 electrons. Because the 2s orbital is the next highest orbital to the 1s orbital it gets 'filled' with electrons only after the 1s orbital is filled with its two.

Answer 6

The 2s orbital is larger and has a higher energy level than the 1s orbital. The 2s orbital also contains nodes (regions with zero probability of finding an electron) while the 1s orbital does not.