What are the two main properties that the group 2 elements have in common?

Some of the properties of group 2 elements are that they have low boiling points, low melting points, and low densities.

What are the properties and uses of the elements in Group 2 of the periodic table?

Being a metal, they are obviously good conductors of heat and electricity. The general electronic configuration of Group 2 elements is ns2. Alkali earth metals have the capability to lose the two electrons in their outer shell. Thus, they react with other elements and form ionic compounds.

Which element in Group 2 is most reactive?

The alkali metals are the most reactive metals. Group 2 consists of the alkaline Earth metals. They are very reactive but less so than the alkali metals.

Why does the reactivity of group 2 elements increase?

As you progress down Group 2, the reactivity increases. This is due to a decrease in ionisation energy as you progress down the group. As it requires less energy to form the ions, the reactivity increases.

Why does Group 2 have similar properties?

Being in group 2 means they all have two valence electrons, or the electrons that are furthest away from the nucleus. Having two valence electrons makes this group reactive, meaning the elements want to combine with other elements, not just water. Other characteristics most share include being soft and silvery.

Which properties are characteristic of the Group 2 metals?

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.

Why is group 2 less reactive?

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.

Which element in group 2 is most metallic?

radium
Among the group 2 elements, radium is known to have the greatest metallic character and it can, therefore, be considered the most metallic group 2 element. This is because the metallic character of elements increases while traversing down a group, and radium is at the bottom of group 2 in the modern periodic table.

What is the reactivity of Group 2?

Reactivity of Group II elements increases down the group. This can be explained by the increase in ease at losing two outer electrons as we descend the group. The loss of electrons becomes easier due to the decreasing ionisation energy required.

What happens to the reactivity of Group 2?

The reactivity of the group 2 elements increase as you go down the group. This is because, as explained previously, it is much easier to remove an outer shell electron as you go further down the group (lower ionisation energies).

Why do group 2 metals have higher melting points than Group 1 metals?

Consequently, stronger metallic bonding exists in group 2 metals which results in higher cohesive energy and close packing of the atoms. This accounts for the greater hardness and higher melting and boiling points of group 2 metals as compared to group 1 metals.

Why be is different from the rest of the group 2 members?

1) Beryllium is harder than other members of its group. 2) Beryllium has higher melting and boiling point than other members of its group. 3) Beryllium does not react with water even at high temperature while other metals do. 4) Beryllium forms covalent compounds whereas other members form ionic compounds.

What is beryllium in the periodic table?

Beryllium (Be), formerly (until 1957) glucinium, chemical element, the lightest member of the alkaline-earth metals of Group 2 (IIa) of the periodic table, used in metallurgy as a hardening agent and in many outer space and nuclear applications. Element Properties. atomic number.

How is the beryllium atom analogous to helium?

The beryllium atom is analogous to helium in that both atoms have two outer electrons, but the atom is not chemically similar to helium. The reason is that the n = 2 shell…

What are the similarities between beryllium and aluminium?

In fact, there are several similarities between beryllium and aluminium in Group 3. This is known as a diagonal relationship and is discussed on the page about electronegativity. Beryllium chloride, BeCl 2, melts at 405°C and boils at 520°C. That compares with 714°C and 1412°C for magnesium chloride.

Does beryllium react with sulfuric acid?

When exposed to higher temperatures, it burns rapidly to form beryllium oxide. It reacts with hydrochloric and sulfuric acid but not with nitric acid. Beryllium also reacts with non-metals and form binary compounds with them, including sulfur, fluorine, iodine and bromine. The oxidation state of beryllium is +2.