I'm happy to help with your question! Let's break it down step by step:
32. An element 'X' has the same number of electrons in the first and the fourth shell as well as in the second and the third shell.
(a) The electronic configuration of the element 'X' would be:
- First and fourth shell: 2 electrons
- Second and third shell: 8 electrons
So, the electronic configuration is 2, 8, 8, 2.
(b) The group number for this element would be Group 2 since it has 2 valence electrons in the outermost shell. The period where it belongs in the periodic table would be Period 3.
(c) The valency of the element 'X' is 2 because it has 2 valence electrons.
(d) Element 'X' will most likely form an ionic bond with oxygen because it can lose its 2 valence electrons to achieve a stable configuration.
(e) The oxides of element 'X' are likely to be basic in nature due to the tendency of Group 2 elements to form basic oxides.
33. The first ionization energy of Na is lower than that of Mg because Na has a larger atomic size than Mg, which makes it easier to remove an electron from Na compared to Mg. However, the second ionization energy of Na is higher than that of Mg because removing the second electron from Na requires breaking into a stable electronic configuration, making it harder than removing the first electron.
