The first ionisation enthalpy of C atom is greater than that of boron atom whereas the reverse is true for the second IE. How will you substantiate this anomally?

Give justification, The first lonisation enthalpy of carbon is greater than that of boron, whereas the reverse is correct for the second ionisation enthalpy.

The first ionization enthalpy of sodium is lower than that of magnesium but its second ionisation enthalpy is higher than that of magnesium. Explain.

How would you explain that the first ionisation energy of Na is lawer than that of Mg but is second inoisation enthalpy is higher than that of Mg ?

A quantitative measure of the tendency of an element to lose electron is given by its ionisation enthalpy (I.E.). I.E. increases from left to right in a period of the periodic table. However, in second period, the I.E of oxygen is less than that of nitrogen. Why?

The reactivity of an element is very much related to its ionization enthalpy. Observe the following graph in which the first ionization enthalpies (DeltaH_1) of elements of the second period are plotted against their atomic numbers (Z): Identify the anomalour values and justify.

Among the elements B , Al , C and Si . a. Which has the highest first ionization enthalpy? b. Which has most negative electron gain enthalpy? c. Which has the largest atomic radius? d. Which has the most metallic character?

Name of elements with atomic numbers greater than 100 are given by IUPAC the first inoisation enthalpies of second period element generally increase from lewft to right along the period. Give reason for this general trend.

Ionisation is the removal of electron from an.atom. What is ionisation enthalpy? How is it related to electronic configuration of atoms.

Compare the general characteristics of the first series of the transition metals with those of the second and third series metals. in the respective vertical columns. Give special emphasis on the following points: (i) electronic configurations (ii) oxidation states iii) Ionisation enthalpies and iv) atomic sizes.

Monosaccharides containing an aldehyde group are called aldoses while those containing aketo group are called ketoses. The aldehyde group is always present at C_1 while the keto group is usually present at C_2 . All monosaccharides containing five and six carbon atoms have cyclic structures, furnaose (five membered) and pyranose (six membered). During ring formation, C_1 in aldoses and C_2 in ketoses becomes chiral and hence all these monosaccharides exist in two stereoisomeric forms called the alpha -anomer and the beta -anomer while C_1 and C_2 are called glycosidic or anomeric carbon atoms. In contrast, stereoisomers, which differ in configuration at any other chiral carbon other than the glycosidic carbon are called epimers. Two molecules of the same or different monosaccharides combine together through glycosidic linkage to form disaccharides. All monosaccharides (aldoses and ketoses) and most disaccharides reduce Tollens'reagent and Fehling's solution, undergo mutarotation and form osazones. Two forms of D-glucopyranose are called