2 electrons in the outermost shell.
Alkali gases only have 1 electron needing to be removed to reach a stable noble gas configuration. Alkaline earths have two electrons. Alkali metals thus have the lower ionization energy of the two groups.
All atoms want to do is make their valence shell full. In alkali metals they have all of their shells completely full except one valence electron. The alkali metals REALLY want to get rid of that electron, so they will react with many elements/compounds to get rid of that electron. In alkaline earth metals they have all of their shells completely full except for two valence electrons. They also want to get rid of those electrons but the alkaline earth metals are not as desperate to do so as the alkali earth metals which make the alkaline much less reactive than the alkali metals.
Alkali metals (group 1 elements) have one valence electron. Hence have one ionization energy Alkaline earth metals (group 2 elements) have two valence electron. Hence have two ionization energy
The electronegativityÊ of alkaline earth metals decreases as you go down the group due to increase in atomic radius. The earth alkaline metals are beryllium, magnesium, strontium, barium and radium. Radium has the smallest electronegative.
YEP! remember In science in order for the Alkali metals and Alkaline earth metals to become stable they must give AWAY electrons. The Earth metals have a Plus 2 charge because they give away 2 electrons on there outer shell!
ns^2
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
All alkaline earth metals have electron configurations ending in s2; 6s2 would be the alkaline earth metal in period 6 of the PTE, which is barium.
All halogens have 7 valence electrons. They gain one electron and achieve noble gas electronic configuration
Alkaline metals
They don't, they actually have a greater tendency to lose electrons. This is for a number of reasons. First of all, the alkali metals form a stable cation by losing one electron, while the alkaline-earth metals need to lose two to form a stable ion. It takes more energy to remove one electron from an atom than it does to remove two. Additionally an alkaline earth metal has a greater positive charge on its nucleus and a smaller atomic radius than an alkali metal in the same row of the periodic table. This make it even harder to remove valence electrons. ------------ ?? WRONG: Alkali metals have a valence electron configuration of ns1 so they can accept another electron in the ns orbital. On the other hand, alkaline earth metals have a valence electron configuration of ns2. Alkaline earth metals have little tendency to accept another electron, as it woudl have to go into a higher energy p orbital.
Be (berylium) berylium Mg (magnesium) magnesium Ca (calcium) calcic Sr (strontium) strontium Ba (barium) baryum Ra (radium) radium All the elements' general valence electron configuration is ns2 "n" is a number from 2 (for Be) to 7 (for Ra).
alkali metals have one valence electron, whereas alkaline earth metals have two valence electrons.
The valance electron configuration is the same in each at ns1 where n = the period number.
This is [noble gas] 2s2 to 7s2.
No. All the alkaline earth metals have 2 valence electrons, meaning they have two electrons in the outermost shells. No two alkaline earth metals have the same number of electron shells. Beryllium is the only one with two shells.
Alkali metals