State where in the periodic table these elements appear: (a) elements with the valence-shell electron configuration ns2np5 (b) elements that have three unpaired p electrons (c) an element whose valence electrons are 4s24p1 (d) the d-block elements [Section 6.9]

Verified step by step guidance

1. Identify the general electron configuration for each case and relate it to the periodic table sections: s-block, p-block, d-block, and f-block.
2. For part (a), recognize that the electron configuration ns2np5 corresponds to halogens, which are located in Group 17 of the p-block.
3. For part (b), elements with three unpaired p electrons typically have a p3 configuration, placing them in Group 15 of the p-block.
4. For part (c), the electron configuration 4s24p1 indicates an element in the 4th period of the p-block, specifically in Group 13.
5. For part (d), understand that the d-block elements are transition metals, which are found in the central block of the periodic table, specifically Groups 3 through 12.

Key Concepts

Valence Electron Configuration

Valence electron configuration describes the distribution of electrons in the outermost shell of an atom. The notation 'ns2np5' indicates that the element has two electrons in the s subshell and five in the p subshell of its highest energy level, which corresponds to the halogens in Group 17 of the periodic table.

Unpaired Electrons

Unpaired electrons are those that occupy an orbital alone rather than in pairs. Elements with three unpaired p electrons typically belong to Group 15 of the periodic table, where the p subshell has three electrons, leading to unique chemical properties and reactivity.

d-block Elements

The d-block elements, also known as transition metals, are found in Groups 3 to 12 of the periodic table. These elements are characterized by the filling of d orbitals and exhibit properties such as variable oxidation states and the ability to form colored compounds, making them essential in various chemical reactions and applications.