Orbitals don't contain elements. The elements each have specific orbitals based on the number of electrons it has. All of the elements have at least one s orbital. Hydrogen being the simplest element has one electron in the 1s orbital. The s orbital can contain a maximum of 2 electrons.
The elements in the s-block have their last electrons in their electron configuration in the s-orbital.
If you're talking about any s sublevel at all, then any element except hydrogen would fit that. If you're talking specifically about elements that have the s orbital as their valence (outermost) orbital, and also have that valence s orbital filled with 2 electrons, then helium and anything in the second column of the periodic table will all fit that description. (He, Be, Mg, Ca, Sr, Ba, Ra)
Two elements
hydrogen and helium
The elements which falls under the group 16 has 4 electrons in its outer p orbital...
S orbital contains only 2 electrons and not elements.
For the elements in the s-block, the valence electrons are filled in the s orbital.
The elements in the s-block have their last electrons in their electron configuration in the s-orbital.
The S orbital contains a maximum of two electrons
S block elements are named so bcozIn this elements last electron enters the outermost s orbital(i.e. ns1 or ns2).
If you're talking about any s sublevel at all, then any element except hydrogen would fit that. If you're talking specifically about elements that have the s orbital as their valence (outermost) orbital, and also have that valence s orbital filled with 2 electrons, then helium and anything in the second column of the periodic table will all fit that description. (He, Be, Mg, Ca, Sr, Ba, Ra)
Two elements
Group 1: have 1 valence electrons (half filled s orbital) Group 2: have 2 valence electrons (completely filled s orbital)
hydrogen and helium
The elements which falls under the group 16 has 4 electrons in its outer p orbital...
This is because the elements in the first period only use their s orbitals, youll notice that Hydrogen is 1S and exists as the diatomic H2 and that Helium has the configuration 2S and exists as free Helium. The reason for this is that any S orbital can only hold two electrons, the octet rule applies when there are S and P orbitals present which can hold up to 8 electrons( 2 from the S orbital and 6 from the D orbital).
Only two: hydrogen and helium. This corresponds to the fact that there can be only two s orbital electrons in any electron shell, and the first shell has only s orbital electrons.