All the Group 1 elements are silvery-coloured metals. They are soft, and can be easily cut with a knife to expose a shiny surface which dulls on oxidation.
These elements are highly reactive metals. The reactivity increases on descending the Group from lithium to cesium. There is a closer similarity between the elements of this Group than in any other Group of the Periodic Table.
These elements are too reactive to be found free in nature. The alkali metals are so reactive they cannot be displaced by another element, so are isolated by electrolysis of their molten salts.
The alkali metals differ from other metals in several ways. They are soft, with low melting and boiling temperatures. They have low densities - Li, Na and K are less dense than water. They have low standard enthalpies of melting and vaporization. They show relatively weak metallic bonding as only one electron is available from each atom.
Alkali metals colour flames. When the element is placed in a flame the heat provides sufficient energy to promote the outermost electron to a higher energy level. On returning to ground level, energy is emitted and this energy has a wavelength in the visible region: Li red Na yellow K lilac Rb red Cs blue
The ionic radii of the alkali metals are all much smaller than the corresponding atomic radii. This is because the atom contains one electron in an s level relatively far from the nucleus in a new quantum shell, and when it is removed to form the ion the remaining electrons are in levels closer to the nucleus. In addition, the increased effective nuclear charge attracts the electrons towards the nucleus and decreases the size of the ion.
The alkali metals are strong reducing agents. The standard electrode potentials all lie between -2.7V and -3.0V, indicating a strong tendency to form cations in solution. They can reduce oxygen, chlorine, ammonia and hydrogen. The reaction with oxygen tarnishes the metals in air, so they are stored under oil. They cannot be stored under water because they react with it to produce hydrogen and alkali hydroxides:
All group one elements have a single valence electron, which means that they form ions by losing that electron. This event confers a +1 charge on the atom that has lost the electron. Because of the fact that these elements only need to lose a single electron to ionize, they are very reactive and are never found in their elemental state in nature.
1
Group 1 elements have +1 oxidation number (except for hydrogen) All group 2 elements have +2 oxidation number Fluoride ion always has -1
An outer electron shell with only one electron.
+1 only for all elements (except for hydrogen) hydrogen can have +1 and -1 as their oxidation numbers.
yes
-1.
Main group or Alkali metals
these elements are found in all institutions of the world societies: 1: it is a group of people who are inerrelated through social interaction. 2:this is a group of people is united under common interest.
They are all reactive metals with one valence electron in their outermost s sublevel.
1
Elements in the same family (or group) have the same amount of electrons in their outer shell. For Example, all elements in Group 1 have 1 electron in their outer shells.
Group 1 elements have +1 oxidation number (except for hydrogen) All group 2 elements have +2 oxidation number Fluoride ion always has -1
All the atoms in group 1.
An outer electron shell with only one electron.
All elements in group 1 have 1 valence electron.
+1 only for all elements (except for hydrogen) hydrogen can have +1 and -1 as their oxidation numbers.
Hydrogen is an alkali metal just like all the other elements in group 1. The difference is that hydrogen is a nonmetal and a gas which seperates it from the rest of group 1's elements. The rest of the elements in group 1 are metals and solid. (this was done by #41 for all u ppl at sjs who have no idea what the hell this worksheet was about.)