Why are the elements of group IA called alkali metals?

Sodium $Na_11^23$ is so reactive that if sodium metal is placed in water it will react vigorously to produce Hydrogen gas and heat often causing an explosion. All of...

The main reason the noble gases do not need to bond with other is that their outermost subshells are filled. These are known as . Take helium for example. It...

The metal becomes more reducing........and MUCH MORE reactive. Lithium is fairly zippy in water; sodium is even zippier. Potassium will give you bangs and pops and flames. The metal...

It is well known that ionization energies INCREASE across a Period from left to right as we observe the Table, but decrease down a Group. Across the Period, as nuclear...

Hydrogen is commonly grouped with the alkali metals, the which all have the one valence electron in the $s$ shell. Under extreme, high pressure conditions, metallic hydrogen has been claimed....

A metalloid is an element whose properties are "in between" those of . For example, metals are excellent electothermal conductors, and nonmetals are non-conductors. Metalloids are described as semiconductors....

The realization that earths were in fact oxides was attributed to Lavoisier. And the Group 2 metals form a stable series of sparingly soluble binary oxides. I am told that...

Given the $ns^1$ configuration, the metals are strongly reducing. Their reaction with water reflects this: $M(s) + H_2O(l) rarr M(OH)(aq) + 1/2H_2(g)$ They also react quantitatively with liquid ammonia (another...

Two factors are important here. $"A priori"$ we would expect that it would be harder to remove an electron from a cation than from a neutral species. This is from...

As you know, metallic results from the delocalization of electrons from the parent metal atom so that positive ions are conceived to swim in a sea of electrons. This view...