Group I and group II elements

The alkali metals are in group I, the alkaline earth metals are in group II, the pnictogens are in group 16, the chalcogens are in group 17, the halogens are in group 18, and the noble gases are in group 18.

Group I elements – 

The alkali metals are made up of the chemical elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr) (Fr). They are part of group 1, which, along with hydrogen, is located in the periodic table’s s-block. The outermost electron of all alkali metals is in an s-orbital configuration; due to this shared electron configuration, their distinguishing features are quite similar. And yes, the alkali metals are good examples of periodic table group trends in characteristics, with elements exhibiting well-defined homologous behaviour. This family of elements is called the lithium family after its leading element at room temperature and pressure. The alkali metals are all lustrous, soft, and highly reactive metals that readily lose their outermost electron to form cations with charge +1. Due to their pliability, they can all be easily sliced with a knife, revealing a gleaming surface that tarnishes quickly in the air due to oxidation by atmospheric moisture and oxygen (and in the case of lithium, nitrogen). Because of their high reactivity, they must be stored in oil to avoid reactions with air, and they are only found in nature as salts, never as free elements. As the fifth alkali metal, caesium is the most reactive of all metals. All alkali metals react with water, but heavier alkali metals react more vigorously than lighter alkali metals.

Group 2 elements

The alkaline earth metals are a collection of six chemical elements found in Periodic Table Group 2 of the periodic table. The elements in question are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra) (Ra). The elements have very similar properties at standard temperature and pressure: they are all lustrous, silvery-white, and moderately reactive metals. They (along with helium) share a complete outer s-orbital structurally, which has its full complement of two electrons, which the alkaline earth metals rapidly lose to form cations with charge +2 and oxidation state +2. All of the known alkaline earth metals can be found in nature, though radium is only found as a byproduct of uranium and thorium decay, rather than as a primordial element. Several attempts to synthesize element 120, the group’s next potential member, have all failed.

Uses of alkaline earth metals

Alkaline earth metals have a variety of applications, including:

The element is utilized in the production of alloys. Cu-Be alloys are commonly used to make high-strength springs. Mg is utilized in the production of alloys containing Al, Zn, Mn, and Sn. Mg-Al alloys are used in aircraft construction. Metals are extracted from their oxides using calcium. Radium salt is used in radiotherapy, such as for cancer treatment. 

Uses of Alkali Metals

Lithium, sodium, and potassium have a wide range of applications, although rubidium and cesium are only helpful in academic settings. Lithium oxide can aid in the processing of silica, which is commonly used in batteries. Lithium is also used in the production of lubricating greases, air treatment, and aluminum. The use of pure sodium in sodium-vapor lamps, which provide very efficient light, is one of its many applications. In the biological system, potassium plays a critical role. KOH is used in the production of soap, while KCl is utilized as a fertilizer. Photoelectric cells are made of cesium.

Group of elements

Alkali metals Group 1: highly reactive metals that do not occur naturally.

There is one electron in the outer shell.

Metals from the Alkaline Earth

Group 2: the following reactive metals, which are found in the earth’s crust but not in elemental form.

In the outer shell, there are two electrons.

Group 3-12 Transition Elements: metals with varying reactivities. Group 3 elements have a higher density than Group 1 or 2 elements.

In the outer shell, there are 1-2 electrons.

Actinides and Lanthanides

Lanthanides, also known as rare earth elements, have periods 6-7 and are soft and malleable with high conductivity; the only actinides found in significant quantities on Earth are thorium and uranium.

Boron Group 13 is reactive and contains metal and metalloid.

There are three electrons in the outer shell.

Metalloids, metals, and nonmetals are all found in Carbon Group 14.

Metalloids, metals, and nonmetals are found in Nitrogen Group 15.

In the outer shell, there are 5 electrons.

Metalloids, metals, and nonmetals are all found in Group 16 of the Oxygen Group. Reactive

In the outer shell, there are 6 electrons.

Halogens

Group 17 halogens are nonmetals that are extremely reactive.

There are 7 electrons in the outer shell.

Group 18 Nobel gases are non-metals and non-reactive.

There are 8 electrons in the outer shell.

Highest melting point element

Heavy metals include tantalum, iridium, platinum, gold, tungsten, hafnium, and silver. The melting point of the densely packed metallic structures is extremely high. Tungsten, for example, has the highest melting point of any metal.

Conclusion 

Alkali metals are members of Group 1, alkaline earth metals are members of Group 2, halogens are members of Group 17, and noble gasses are members of Group 18. The number of electrons in the outermost orbital differs between Groups 1 and 2. The primary distinction between group 1 and group 2 elements is that group 1 elements all have unpaired electrons in their outermost orbitals, whereas group 2 elements all have paired electrons in their outermost orbitals.