Alkali metals are among the most reactive metals. This is due in part to their larger atomic radii and low ionization energies. They tend to donate their electrons in reactions and have an oxidation state of +1. These metals are characterized by their soft texture and silvery color.

The vertical columns on the periodic table are called groups or families because of their similar chemical behavior. All the members of a family of elements have the same number of valence electrons and similar chemical properties.

Reactivity of Group 1 Elements Hydrogen is a very reactive gas, and the alkali metals are even more reactive. In fact, they are the most reactive metals and, along with the elements in group 17, are the most reactive of all elements.

The outermost electrons of the alkaline earth metals (group 2) are more difficult to remove than the outer electron of the alkali metals, leading to the group 2 metals being less reactive than those in group 1. The reactivity of group 1 elements increases as you go down the group because: the atoms become larger.

Revision notes on the topic ‘Group 7: Reactivity’ for Edexcel IGCSE Chemistry

• Reactivity of Group 7 non-metals increases as you go up the group.
• Out of the 3 halogens, chlorine, bromine and Iodine, chlorine is the most reactive and iodine is the least reactive.

Group 2A (or IIA) of the periodic table are the alkaline earth metals: beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). In most cases, the alkaline earth metals are ionized to form a 2+ charge.

The two most reactive families of elements are the halogens and the alkali metals.

The Group 2 alkaline earth metals include Beryllium, Magnesium, Calcium, Barium, Strontium and Radium and are soft, silver metals that are less metallic in character than the Group 1 Alkali Metals. All the elements in Group 2 have two electrons in their valence shells, giving them an oxidation state of +2.

radium

Beryllium, magnesium, calcium, strontium, barium and radium are the elements in Group 2. For two reasons, these elements are referred to as Alkaline Earth metals, Their oxides remain in the crust of the earth and are very heat-stable.

Chalcogens means ore forming, as most of the ores in the earth crust are either oxides or sulphides, group 16 elements are called chalcogens. for example: Oxygen is the most abundant of all the elements on earth. Oxygen forms about 46.6% by mass of earth’s crust.

transition metals

Beryllium fulfills the first criterion but not the second one, since its oxides and hydroxides show amphoteric behavior, rather than alkaline. So, it is not considered an alkaline earth metal in the true sense, even though it does resemble them in various other properties.

Alkaline-earth metal, any of the six chemical elements that comprise Group 2 (IIa) of the periodic table. The elements are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).

The alkaline earth metals are six chemical elements in group 2 of the periodic table. They are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).

5.2 Alkaline earth metals The alkaline earth metals (beryllium, magnesium, calcium, strontium, barium, and radium) are the second most reactive metals in the periodic table (Table 3.7), and, like the Group 1 metals, have increasing reactivity in the higher periods.

Alkaline earth metals share many similar properties including: They are silvery, shiny, and relatively soft metals. They are fairly reactive under standard conditions. They have two outer valence electrons which they readily lose.

This group includes beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). Alkaline earth metals have only two electrons in their outermost electron layer. Alkaline earth metals get the name ‘alkaline’ because of the basic nature of the compounds they form when bonded with oxygen.

The alkaline-earth elements are highly metallic and are good conductors of electricity. They have a gray-white lustre when freshly cut but tarnish readily in air, particularly the heavier members of the group. Beryllium is sufficiently hard to scratch glass, but barium is only slightly harder than lead.

Properties of Alkaline Earth Metals

• shiny.
• silvery-white.
• somewhat reactive metals at standard temperature and pressure.
• readily lose their two outermost electrons to form cations with a 2+ charge.
• low densities.
• low melting points.
• low boiling points.

Transition metals are also high in density and very hard. Most of them are white or silvery in color, and they are generally lustrous, or shiny. The compounds that transition metals form with other elements are often very colorful.

Alkaline Earth metals are very reactive because they readily give up their two valence electrons to achieve a full outer energy level, which is the most stable arrangement of electrons. Reactivity increases from the top to the bottom of the group.

Beryllium

Problems

• Metal oxides form basic solutions in water.
• Difluorine does not react with water.
• Beryllium has a large atomic radius.
• Sodium is the alkali element that reacts most violently with water.