How and why do all in elements in Group 1A belong there?

Question

Chemistry, I can't seem to find the reason how.

Answer 1

The are all akali metals therefore:
Properties

The alkali metals exhibit many of the physical properties common to metals, although their densities are lower than those of other metals. Alkali metals have one electron in their outer shell, which is loosely bound. This gives them the largest atomic radii of the elements in their respective periods. Their low ionization energies result in their metallic properties and high reactivities. An alkali metal can easily lose its valence electron to form the univalent cation. Alkali metals have low electronegativities. They react readily with nonmetals, particularly halogens.

Summary of Common Properties


Lower densities than other metals
One loosely bound valence electron
Largest atomic radii in their periods
Low ionization energies
Low electronegativities
Highly reactive

Answer 2

Going in the time of team A a million+, 2+, 3+, 4+ or 4-, 5+ and 3-, 2-, a million-. Going around the B communities. all of them have a valence of two+ because of the 2s2 electrons which could be donated because of the fact the completed team are metals. Then there is an further valence because of the three-d electrons Sc 2+, 3+, Ti 2+, 4+, V 2+, 5+, Cr2+, 6+ Mn 2+, 7+ Fe 2+, 3+ Co 2+, N1 2+, Cu a million+, 2+ Zn 2+ the 1st 5 can donate their outer electrons, which by how each and every have an analogous spin quantum no. After that ,beginning it in basic terms loses1 extra electron from the three-d's because of the fact After Mn the d's are precisely a million/2 filled,, so the guideline variations. i'm hoping this facilitates..

Answer 3

They all have the same outer electron configuration - ns1. As such, their chemistries are very similar, probably more so than any other similar group in the Periodic Table (with the possible exception of the noble gases).

Answer 4

The alkali metals are the series of elements in Group 1 (IUPAC style) of the periodic table (excluding hydrogen in all but one rare circumstance): lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr).

The alkali metals are silver-colored (caesium has a golden tinge), soft, low-density metals, which react readily with halogens to form ionic salts, and with water to form strongly alkaline (basic) hydroxides. These elements all have one electron in their outermost shell, so the energetically preferred state of achieving a filled electron shell is to lose one electron to form a singly charged positive ion.

Answer 5

Similar electronic configuration

Answer 6

group 1 or 1a
Alkali metals
One valence electron

Answer 7

they are all alkali metals and they have one valence electron.