Every alkali metal has only one electron in the outermost energy level. They give it away to form monopositive ions which have stable electron configurations ending with ns2 np6 (where n is a counting number between 2 and 7 inclusive).
Alkali metals, have only one valence electron so they will "want" to lose it to achieve a stable electron arrangement.
they lose one electron
This is because they only have on valance electron. This makes it easier to react with other elements and more often also.
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.
Group I elements (that is alkali metals)
Alkali metals, have only one valence electron so they will "want" to lose it to achieve a stable electron arrangement.
they lose one electron
Alkali metals lose one electron in chemical reactions.
Lithium would be most likely to lose electrons in a chemical bond.
Sodium is an alkali metal. All alkali metals have 1 electron in the valence shell. This means that the "desired state" is to have a full valence shell configuration. So, in order for sodium and other alkali metals to reach this state, it has to LOSE one electron, making it a positive ion (cation).
This is because they only have on valance electron. This makes it easier to react with other elements and more often also.
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.
Group I elements (that is alkali metals)
Alkali metals
Groups 3-12 do not have individual names. Instead, all of these groups are called transition metals. The atoms of transition metals do not give away their electrons as easily as atoms of the Group 1 and Group 2 metals do. So, transition metals are less reactive than alkali metals and alkaline-earth metals are.
The key to this answer is the phrase "valence electrons". Alkali metals are in the first column of the periodic table and include elements such as Lithium, Sodium and Potassium. These elements typically lose ONE electron when they participate in a chemical reaction, therefore they have ONE valence electron.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.