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.
There are a number of differences:-
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.
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.
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.
the 2s orbital is at a higher energy level
The 2s orbital and 3s orbital both have the same spherical shape and can hold a maximum of two electrons of opposite spin. They only differ because the 3s orbital is further out from the nucleus than the 2s orbital, thus the 3s orbital has a higher energy value.
Two per level (that is, 2 1s, 2 2s, 2 3s, etc.)
Carbon has 6 total electrons: 2 located in the 1s orbital, 2 located in the 2s orbital, and 2 in 2p orbitals. 2+2+2=6.
The energy level closest to the nucleus is the 1s orbital and can hold 2 electrons as do all s orbitals. Every electron orbital has a distinct shape and number. The 1s orbital has the same shape the 2s orbital and the 3s orbital and so forth. There are other orbital shapes such as p, d, and f. Regardless of the number or level of the orbital, all p orbitals are the same shape and all d orbitals are the same shape. Orbitals differ in distance from the nucleus and the distance is indicated by the number before the orbital shape.
The 2s orbital is larger than the 1s orbital and is higher in energy.
the 2s orbital is at a higher energy level
The electron configuration of nitrogen is 1s^2 2s^2 2p^3. Nitrogen has a total of seven electrons, with two in the 1s orbital, two in the 2s orbital, and three in the 2p orbital.
The 2s orbital and 3s orbital both have the same spherical shape and can hold a maximum of two electrons of opposite spin. They only differ because the 3s orbital is further out from the nucleus than the 2s orbital, thus the 3s orbital has a higher energy value.
The 1S orbital will hold the innermost pair of electrons.
The 2s orbital looks much like the 1s orbital except that the electron is more likely to be found further from the nucleus. The bonds that are formed are called the Sp3 bond and the Sp2 bond.
Two per level (that is, 2 1s, 2 2s, 2 3s, etc.)
⬆⬇1s ⬆⬇2s ⬆2p 2p should look like _ _ _ 2p
1s + 1s + 1 = 2s + 1
There are 2 energy levels in a Carbon atom. The first energy level consists of '1s' orbital, and the second energy level consists of the '2s' orbital and the '2p' orbital.
Carbon has 6 total electrons: 2 located in the 1s orbital, 2 located in the 2s orbital, and 2 in 2p orbitals. 2+2+2=6.
4 electrons. First orbital is the 1s which has 2 electrons. Second orbital is the 2s which has 2 electrons.