Name the factors that affect the thermal stability of alkali metal salts. Explain the stability trend observed in case of nitrates of these metals.

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call
The thermal stability of a substance depends heavily on the structure of the substance which, in turn, is dependent on the bonds between atoms that hold that structure together. Group 1 nitrates decompose to form products: MeNO2 + O2 Going down Groups 1, nitrates become more stable. Higher temperatures are needed to decompose them. Cations (positively charged ions) can affect anions such as NO3-. They can lower the energy needed to break a N–O bond. This effect increases: • the smaller the cation • the greater the cation’s charge. The small positive ions at the top of the Group polarise the nitrate more than the larger positive ions at the bottom.
0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
Describe and suggest an explanation for the trend in the thermal decomposition of the nitrates of the Group II elements magnesium to barium, writing equations and using diagrams where appropriate

Both carbonates and nitrates of Group 2 elements become more thermally stable down the group. The larger compounds further down require more heat than the lighter compounds in order to...

1 Answers 1 views
while is second ionization energy of alkaline earth metals is less than that of corresponding alkali metals

Although IE1 (first ionization energy) values of alkaline earth metals are higher than that of alkali metals, the IE2 (second ionization energy) values of alkaline earth metals are much smaller...

1 Answers 1 views
The second ionization energy of alkaline earth metals is less than that of corresponding alkali metals because

First ionization energy values of alkaline earth metals are higher than that of alkali metals, but second ionization energy values of alkaline earth metals are much smaller than those of...

1 Answers 1 views
What is the trend for ionic character of the group 2 compounds going down the group? Can you explain this trend?

In this series, the ionic character of the compounds increases with increasing ionic radius of the metal atom. Electronegativity atoms decreases, and therefore the difference between the electronegativity of the...

1 Answers 1 views
Explain the trends in the thermal stability of the oxosalts of alkali and alkaline earth metals

For Group 1 and Group 2 oxosalts the thermal stability increases down the group as the ionic radius of the cation increases, and its polarising power decreases.Group 1 oxosalts tend...

1 Answers 1 views
Explain the trend in the thermal stability of the oxosalts of alkali and alkaline earth metal

As we move along the period the radii of atoms decrease, i.e. radii of alkaline earth metals are smaller than the radii of alkali metals. The smaller the radius of...

1 Answers 1 views
Indicate the solubility in water of each of the following groups of compounds: Salts of the alkali metals Hydroxides Chlorides Carbonate Sulphates Nitrate

Salts of the alkali metals:Hydroxides-solubleChlorides-solubleCarbonate-soluble(Lithium carbonate is limited soluble in water).Sulphates-solubleNitrate-soluble

1 Answers 1 views
the discovery of ---------- rejected law of octave.. A. Halogens B. Inert gases C. Alkali Metals D. Heavy metals

The Law of Octaves was published by John Newland in 1864. He proposed that some of the physical and chemical properties of the elements must be repeated after every seven...

1 Answers 1 views
Which of the alkali earth metal is not collected as alkali earth metals because its oxide is not alkaline ?

Beryllium.Beryllium oxide is amphoteric

1 Answers 1 views
What are alkali metals? Why do these metals not occur in free state in nature? List the principal ores of alkali metals.

Alkali metals are: - Lithium (Li); - Sodium (Na); - Potassium (K); - Rubidium (Rb); - Cesium (Cs); - Francium (Fr). All alkali metals have their outmost electron in the s-orbital. This pre-determines their high chemical...

1 Answers 1 views
X