1s2 2s2 2p6 3s1
Sodium has an electronic structure of 2, 8, 1 with one electron in its outermost shell, while chlorine has an electronic structure of 2, 8, 7 with seven electrons in its outermost shell. This difference in electron configuration determines their chemical properties, with sodium being a reactive metal and chlorine being a reactive nonmetal.
Atoms of the element sodium (atomic number 11) have the electron configuration 1s22s22p63s1 with the noble gas form [Ne] 3s1
The ground state electronic configuration for sodium is 1s^2 2s^2 2p^6 3s^1. This means that sodium has two electrons in the 1s orbital, two electrons in the 2s orbital, six electrons in the 2p orbital, and one electron in the 3s orbital.
There are three electronic shells in sodium while four in iron so Iron is larger in size. other words to make it shorter it would be the iron
The most likely electron configuration for a sodium ion (Na+) in its ground state is 1s2 2s2 2p6. This configuration represents the electronic structure of a sodium atom that has lost one electron to become a sodium ion, achieving a stable octet configuration similar to that of a noble gas.
Atomic number for sodium is 11. 2-8-1 is the electronic configuration of sodium.
The electronic configuration of a sodium atom is 1s2 2s2 2p6 3s1. This means that sodium has 11 electrons distributed across its energy levels.
Sodium has an electronic structure of 2, 8, 1 with one electron in its outermost shell, while chlorine has an electronic structure of 2, 8, 7 with seven electrons in its outermost shell. This difference in electron configuration determines their chemical properties, with sodium being a reactive metal and chlorine being a reactive nonmetal.
There is no particular similarity between the electronic structure of the elements sodium and fluorine. Their electronic structures are similar only to the extent that all elements have certain features in common. The electrons form shells around the nucleus. This is true of sodium and fluorine as well as all other elements.
Atoms of the element sodium (atomic number 11) have the electron configuration 1s22s22p63s1 with the noble gas form [Ne] 3s1
Electronic configuration means the arrangement of electrons in shells in atoms. Eg:Electronic configuration of Sodium is 1s2,2s2,2p6,3s1.
The electronic configuration of sodium is [Ne]3s1. Sodium has one valence electron. And it belongs to group 1. The valence electron is in 3s orbitals and it tells that sodium is a s-block element and is in period 3.
Sodium is atomic number 11 so it has 11 electrons. The electronic configuration would be 1s2 2s2 2p6 3s1.
1s2, 2s2, 2p6, 3s1
The ion formed when sodium achieves a noble-gas electronic configuration is Na+. This means that sodium has lost one electron to achieve the same electron configuration as neon, a noble gas, which has a stable electron configuration.
No, sodium iodine is not a correct term. Sodium iodide is an ionic compound composed of sodium cations (Na+) and iodide anions (I-). This compound forms when a metal (sodium) reacts with a non-metal (iodine) to transfer electrons and achieve a stable electronic configuration.
The ground state electronic configuration for sodium is 1s^2 2s^2 2p^6 3s^1. This means that sodium has two electrons in the 1s orbital, two electrons in the 2s orbital, six electrons in the 2p orbital, and one electron in the 3s orbital.