hydrogen
It is simple: 1s^1 Note: The "^" symbol means the the following number is in the form of a superscript.
scandium
1s1...it is simply an isotope so the number of neutrons changes but the number of electrons remains the same
Valence electron configuration in group 1A: ns1 in which n=1, 2, 3, 4, 5, ... etc. Starting with Hydrogen, H, electron configuration: 1s1 followed by Lithium, Li, electron configuration: (1s2), 2s1 (non valence electrons in () brackets)
These elements are B, Al Br.
Hydrogen electron configuration will be 1s1.
Electron configurations are only made for pure elements. The electron configuration for Hydrogen is 1s1. The electron configuration for Oxygen is 1s2 2s2 2p4
They both have only ONE, the smallest, electron orbital occupied: H: 1s1 and He: 1s2
It is simple: 1s^1 Note: The "^" symbol means the the following number is in the form of a superscript.
1s1 2p2 3d3 4f1
In the ground state - only 1 1s1
The ground state electron configuration of hydrogen is 1s1.
The elements hydrogen and helium are exempted from the octet rule. The octet rule, as you might recall, states that elements prefer to have eight electrons in their valence shells. Hydrogen has a lone electron in its valence shell, and cannot begin to "borrow" electrons to create a shell with eight electrons in it. Remember that its electron, a 1s1 electron, is in the 1s shell. Helium has a full 1s shell with its two electrons (1s1, 1s2). It has no interest in any other electron configuration because its valence shell is full. The first two elements on the periodic table are the exceptions to the octet rule. A link can be found below.
Hydrogen's electron configuration is 1s1. It has only one electron. It is located in the first energy level.
scandium
For hydrogen atoms, it is 1s1. For hydrogen positive ions (protons), it is 1s0. For hydride ions, it is 1s2 or [He]-.
The ground state electron configuration of the hydrogen atom is 1s1, and for helium it is 1s2.