Assign the position of the element having outer electronic configuration:
(i) ns2np4 for n = 3
(ii) (n-1)d2ns2 for n = 4, and
(iii) (n-2) f7 (n-1)d1ns2 for n = 6, in the periodic table.
Give the atomic number and electronic configuration of the following elements:
(i) The third alkali metal
(ii) The second transition element
(iii) The fourth noble gas
(iv) The first halogen.
Elements A, B, C and D have atomic numbers 7, 19, 29 and 36 respectively. Write the electronic configuration and also predict their period, group and block.
The elements Z = 107 and Z = 109 have been made recently; element Z = 108 has not been made. Indicate the groups in which you will have the above elements.
An element belongs to third period of the p-block. It has four valence electrons. Predict its group. How many unpaired electrons does it has?
The elements with Z = 117 and 120 have not yet been discovered. In which family/group would you place these elements. Also give the electronic configuration in each case.
Metal | Non-metal |
Metals have a strong tendency to lose electrons to form cations. Thus, metal is strong reducing agent. | Non-metals have a strong tendency to accept electrons to form the anion. Thus, non-metal are the strong oxidising agent. |
Metal have low ionization enthalpies. | Non-metal have high ionization enthalpies. |
Less negative electron gain enthalpies. | High negative electron gain enthalpies. |
Metal have low electronegativity. | Non-metal have high electronegativity. |
Metal have less negative electron gain enthalpies. | Non-metal high negative electron gain enthalpies. |
Metal forms a basic oxide and ionic compounds. | Non-metal forms acidic oxides and covalent compounds. |
Arrange the following elements in the increasing order of their metallic character: Si, Be, Mg, Na, P.
What are periodic properties of the elements? Name a few important periodic properties.