What relationship exists between the electron structure of Group IA ion and the electron structure of the nearest Noble Gas?
It compares to those of the nearest noble gases by adding electrons to those groups.
Hope it`s useful :)
Fluorine attains the electron configuration of neon (the nearest noble gas).
They have one valence electron. If this electron is lost, the atoms form cations with the electronic configuration of the nearest noble gas.
[He] 2s1
"Noble gas configuration" means that in writing out an electron configuration for an atom, rather than writing out the occupation of each and every orbital specifically, you instead lump all of the core electrons together and designate it with the symbol of the corresponding noble gas on the periodic table (in brackets). For example, the noble gas configuration of phosphorus will be [Ne]3s23p3
Iodine will gain one electron to form iodide anion which has the electronic configuration of the nearest noble gas (xenon): [Kr] 5s2 4d10 5p6 or 2, 8, 18, 18, 8.
It compares to those of the nearest noble gases by adding electrons to those groups. Hope it`s useful :)
Fluorine attains the electron configuration of neon (the nearest noble gas).
They have one valence electron. If this electron is lost, the atoms form cations with the electronic configuration of the nearest noble gas.
Group 17 elements need one more electron to achieve the nearest noble gas electronic configuration. Hydrogen also needs one electron. Hence hydrogen behaves like a group 17 element when forming covalent bond.
[He] 2s1
"Noble gas configuration" means that in writing out an electron configuration for an atom, rather than writing out the occupation of each and every orbital specifically, you instead lump all of the core electrons together and designate it with the symbol of the corresponding noble gas on the periodic table (in brackets). For example, the noble gas configuration of phosphorus will be [Ne]3s23p3
Iodine will gain one electron to form iodide anion which has the electronic configuration of the nearest noble gas (xenon): [Kr] 5s2 4d10 5p6 or 2, 8, 18, 18, 8.
Lithium (Li) should lose 1 electron to get the configuration of the nearest noble gas (He).
Argon has completely filled valence orbitals and hence is unreactive. Sodium has one valence electron. If sodium loses this electron it will attain the stable electron configuration of the nearest noble gas (argon) and hence is reactive.
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.
Positive. It wants to lose two electrons to get to the electron configuration of its nearest noble gas, Ne (Neon).
If alkali metals loses one electron, they achieve the electronic configuration of the nearest noble gases.