General Introduction of Group 2 Elements
General Introduction of Group 2 Elements: Overview
This topic covers concepts, such as, Alkaline Earth Metals, Occurrence of Alkaline Earth Metals, Electron Gain Enthalpy of Alkaline Earth Metals & Standard Reduction Potentials of Alkali Earth Metals etc.
Important Questions on General Introduction of Group 2 Elements
Due to their stable configuration, _____ metals have very little tendency to gain electrons.
Why alkaline earth metals have low electron gain enthalpy values?
Which of the following metal has low electron gain enthalpy?
Due to their stable configuration, alkaline earth metals have very little tendency to gain electrons.
Explain the electron gain enthalpy in alkaline earth metals?
The reducing character of alkaline earth metals _____ down the group.
Explain the trend of reducing property among alkaline earth metals.
Standard reduction potential values of alkaline earth metals decreases down the group.
Explain the trend of standard reduction potentials among alkaline earth metals.
Identify the sequence representing the correct order of ionic mobility in aqueous solution.
The atomic and ionic radii of the alkaline earth metals are smaller than those of the corresponding alkali metals in the same periods.
Answer the following question with respect to the Modern Periodic Table:
What are Group elements called?
The elements of group are known as _____ metals.
What is the name of the family of reactive metals having valency two?
An alkaline earth metal.
Name an alkaline earth metal in the third period. (Sodium/ Magnesium)
The compounds of alkaline earth metals have the following magnetic nature:
Alkali and alkaline earth metals along with hydrogen and helium constitute s-block elements. They have low ionization enthalpies and hence exhibit characteristic flame colourations. They have highly negative electrode potentials and hence are strong reducing agents. Their solutions in liquid ammonia are conducting and also act as strong reducing agents. Being stronger reducing agents than hydrogen, they are usually prepared by electrolysis of their fused chlorides. Their oxides are basic and the basic strength increases down the group. The solubility of carbonates and sulphates of alkali and alkaline earth metals show opposite trends. The carbonates of alkaline earth metals and lithium carbonate decompose on heating while the carbonates of other alkali metals do not decompose on heating The bicarbonates of both alkali and alkaline earth metals on heating give carbonates.
Which of the following processes is used in the extractive metallurgy of magnesium?
Alkali and alkaline earth metals along with hydrogen and helium constitute s-block elements. They have low ionization enthalpies and hence exhibit characteristic flame coloration. They have highly negative electrode potentials and hence are strong reducing agents. Their solutions in liquid ammonia are conducting and also act as strong reducing agents. Being stronger reducing agents than hydrogen, they are usually prepared by electrolysis of their fused chlorides. Their oxides are basic and the basic strength increases down the group. The solubility of carbonates and sulphates of alkali and alkaline earth metals show opposite trends. The carbonates of alkaline earth metals and lithium carbonate decompose on heating while the carbonates of other alkali metals do not decompose on heating The bicarbonates of both alkali and alkaline earth metals on heating give carbonates.
The element that produces red-violet colour in the non-luminous flame is
Strong reductants in and group in the aqeous phase are:
