Mention the most important metals and non-metals from the following products. annapurna salt,liquid uses in thermometer,lead of the pencil,chlorophyll,filament in electric buld,enamel layer on teeth.

Mention the most important metals and non-metals from the following products.a) Annapurna salt.

Mention the most important metals and non-metals from the following products : Chlorophyll.

Mention the most important metals and non-metals from the following products : Liquid used in thermometer.

Mention the most important metals and non-metals from the following products : Lead of the pencil.

Mention the most important metals and non-metals from the following products : Enamel layer on teeth.

Mention the most important metals and non-metals from the following products : filament in electric bulb.

For a spontaneous reaction, the free energy change must be negative. DeltaG=DeltaH-TDeltaS is the enthalpy change during the reaction. T is absolute temperature, and AS is the change in entropy during the reaction. Consider a reaction such as the formation ofan oxide . M+O_(2) MO Dloxygen is used wp in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids consequently gases have a higher entropy than liquids and solids, in this reaction (entropy or randomness) decreases, hence is negative. Thus, the temperature is raised the DeltaS becomes more negative. Since, TDeltaS is subtracted in the equation, then SG becomes less negative. Thus, the free energy changes increases with the increase in temperature. The free energy changes that occur when one mole of common reactant in this case dioxygen) is we may e plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. Free energy change of Hg and Mg for the convertion to oxides the slope of DeltaG . T has been changed above the boiling points of the given metal because

Ozone layer acts as one of the most important life support system. The major cause of ozone layer destruction is believed to be the release of chlorofluorocarbon compounds. UV radiation causes the chlorofluouocarbons to dissociate : CF_(2) Cl overset(hv)(rarr) Cl* +CF_(2) CI A highly reactive chlorine atomis responsible for the decomposition of ozone. Cl* + O_(3) (g) rarr ClO* + O_(2) (g) ClO* + O(g) rarr Cl* + O_(2) (g) Free radicals of chlorine decompose ozone molecules in a chain reaction. The depletion of ozone layer leading to ozone hole has, however, been mainly observed in the stratosphere over Antarctica. Special type of cloud called polar stratospheric colouds are formed over Antarctica.These clouds (contain solid HNO_(3).3H_(2)O ) play an important role in ozone depletion. ClO* + NO_(2) rarr ClONO_(2) ClONO_(2) + H_(2) O rarr HOCl + HNO_(3) ClONO_(2) + HCl rarr Cl_(2) + HNO_(3) HOCl overset(hv)(rarr) HO* + Cl* The reactive chlorine atoms thus formed are rendered to deplete ozone layer. Peeling of ozone umbrella, which protects us from UV rays is caused by:

For a spontaneous reaction, the free energy change must be negative. DeltaG=DeltaH-TDeltaS is the enthalpy change during the reaction. T is absolute temperature, and AS is the change in entropy during the reaction. Consider a reaction such as the formation ofan oxide . M+O_(2) MO Dloxygen is used wp in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids consequently gases have a higher entropy than liquids and solids, in this reaction (entropy or randomness) decreases, hence is negative. Thus, the temperature is raised the DeltaS becomes more negative. Since, TDeltaS is subtracted in the equation, then SG becomes less negative. Thus, the free energy changes increases with the increase in temperature. The free energy changes that occur when one mole of common reactant in this case dioxygen) is we may e plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. As per the Ellingham diagram of oxides which of the following conclusion is true?

For a spontaneous reaction, the free energy change must be negative. DeltaG=DeltaH-TDelaS is the enthalpy change during the reaction. T is absolute temperature, and AS is the change in entropy during the reaction. Consider a reaction such as the formation ofan oxide . M+O_(2) MO Dloxygen is used wp in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids consequently gases have a higher entropy than liquids and solids, in this reaction (entropy or randomness) decreases, hence is negative. Thus, the temperature is raised the DeltaS becomes more negative. Since, TDeltaS is subtracted in the equation, then SG becomes less negative. Thus, the free energy changes increases with the increase in temperature. The free energy changes that occur when one mole of common reactant in this case dioxygen) is we may e plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. For the conversion of Ca(s) to CaO(s) which of the following represent the DeltaG vs T :