Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
If alkali metals loses one electron, they achieve the electronic configuration of the nearest noble gases.
All halogens have 7 valence electrons. They gain one electron and achieve noble gas electronic configuration
The stable ions of all the elements except the Transition metals, Actinide, and Lanthanide series (that is the d and f block elements) form stable ions that are isoelectronic to a nobel gas by gaining or losing electrons in order to achieve an s2 p6 stable octet. For example, sodium will lose one electron to have the same electron configuration as neon, while nitrogen will gain three electrons to become isoelectronic to neon.
It accepts one electron.
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
If alkali metals loses one electron, they achieve the electronic configuration of the nearest noble gases.
All halogens have 7 valence electrons. They gain one electron and achieve noble gas electronic configuration
The "Noble gas electron configuration," or the condensed electron configuration, for F is [He] 2s2 3p5.
It accepts one electron.
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
The stable ions of all the elements except the Transition metals, Actinide, and Lanthanide series (that is the d and f block elements) form stable ions that are isoelectronic to a nobel gas by gaining or losing electrons in order to achieve an s2 p6 stable octet. For example, sodium will lose one electron to have the same electron configuration as neon, while nitrogen will gain three electrons to become isoelectronic to neon.
It accepts one electron.
It accepts one electron.
atoms in stable compounds almost always have a noble gas electron configuration or when representative metals and nonmetals react, thay transferelectrons in such a way that both th cation and the anion have noble gas electron configuration.
Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
The noble gas electron configuration of radon is [Xe]4f145d106s26p6.