(a) Alkali metals: ns¹
(b) Alkaline earth metals: ns²
(c) Noble gases: ns² np⁶
(d) Halogens: ns² np⁵
Related Questions:
- Write the valence shell electronic configuration of the atoms of the following elements:
- Write the valence shell electronic configuration of an element present in the 3rd period and Group IIA.
- Arrange the elements in each of the following in order of decreasing shielding effect:
- Specify which of the following elements you would expect to have the greatest electron affinity: S, P, Cl
- Electronic configurations of some elements are given below. Group the elements in pairs that would represent similar chemical properties:
- Arrange the elements in groups and periods from Q. No. 6:
- For normal elements, the number of valence electrons of an element is equal to the group number. Find the group number of the following elements:
- In which block, group, and period in the periodic table would you place each of the following elements with the given electronic configurations?
- Explain the trends of atomic size, ionization energy, and electron affinity in the periodic table with suitable examples.
- Describe the significance of Mendeleev’s periodic law and how it helped in the development of the modern periodic table.
- Explain the position and properties of alkali metals and halogens in the periodic table. Why do they react so easily with each other?
- Define halogens.
- Which atom has a higher shielding effect, Li or Na?
- Explain why Na has higher ionization energy than K.
- Alkali metals belong to the S-block in the periodic table. Why?
- Arrange the elements in each of the following groups in order of increasing ionization energy:
- Why does atomic radius decrease across a period from left to right?
- Why do noble gases have high ionization energy?
- Why are alkali metals highly reactive?
- What is periodicity in the periodic table?