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d-block Elements PPT Chemistry Class 12
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Page 1 SS CI 11.5 The d block 1 1s 2s 3s 4s 2p 3p 3d Energy Ar 1s 2 2s 2 2p 6 3s 2 3p 6 4p Page 2 SS CI 11.5 The d block 1 1s 2s 3s 4s 2p 3p 3d Energy Ar 1s 2 2s 2 2p 6 3s 2 3p 6 4p SS CI 11.5 The d block 2 1s 2s 3s 4s 2p 3p 3d Energy Sc 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 4s 2 4p Page 3 SS CI 11.5 The d block 1 1s 2s 3s 4s 2p 3p 3d Energy Ar 1s 2 2s 2 2p 6 3s 2 3p 6 4p SS CI 11.5 The d block 2 1s 2s 3s 4s 2p 3p 3d Energy Sc 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 4s 2 4p Electronic Arrangement Element Z 3d 4s Sc 21 [Ar] ? ?? Ti 22 [Ar] ? ? ?? V 23 [Ar] ? ? ? ?? Cr 24 [Ar] ? ? ? ? ? ? Mn 25 [Ar] ? ? ? ? ? ?? Fe 26 [Ar] ?? ? ? ? ? ?? Co 27 [Ar] ?? ?? ? ? ? ?? Ni 28 [Ar] ?? ?? ?? ? ? ?? Cu 29 [Ar] ?? ?? ?? ?? ?? ? Zn 30 [Ar] ?? ?? ?? ?? ?? ?? SS CI 11.5 The d block 3 Page 4 SS CI 11.5 The d block 1 1s 2s 3s 4s 2p 3p 3d Energy Ar 1s 2 2s 2 2p 6 3s 2 3p 6 4p SS CI 11.5 The d block 2 1s 2s 3s 4s 2p 3p 3d Energy Sc 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 4s 2 4p Electronic Arrangement Element Z 3d 4s Sc 21 [Ar] ? ?? Ti 22 [Ar] ? ? ?? V 23 [Ar] ? ? ? ?? Cr 24 [Ar] ? ? ? ? ? ? Mn 25 [Ar] ? ? ? ? ? ?? Fe 26 [Ar] ?? ? ? ? ? ?? Co 27 [Ar] ?? ?? ? ? ? ?? Ni 28 [Ar] ?? ?? ?? ? ? ?? Cu 29 [Ar] ?? ?? ?? ?? ?? ? Zn 30 [Ar] ?? ?? ?? ?? ?? ?? SS CI 11.5 The d block 3 Chromium and Copper • Cr and Cu don’t fit the pattern of building up the 3d sub-shell, why? – In the ground state electrons are always arranged to give lowest total energy – Electrons are negatively charged and repel each other – Lower total energy is obtained with e - singly in orbitals rather than if they are paired in an orbital – Energies of 3d and 4s orbitals very close together in Period 4 Page 5 SS CI 11.5 The d block 1 1s 2s 3s 4s 2p 3p 3d Energy Ar 1s 2 2s 2 2p 6 3s 2 3p 6 4p SS CI 11.5 The d block 2 1s 2s 3s 4s 2p 3p 3d Energy Sc 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 4s 2 4p Electronic Arrangement Element Z 3d 4s Sc 21 [Ar] ? ?? Ti 22 [Ar] ? ? ?? V 23 [Ar] ? ? ? ?? Cr 24 [Ar] ? ? ? ? ? ? Mn 25 [Ar] ? ? ? ? ? ?? Fe 26 [Ar] ?? ? ? ? ? ?? Co 27 [Ar] ?? ?? ? ? ? ?? Ni 28 [Ar] ?? ?? ?? ? ? ?? Cu 29 [Ar] ?? ?? ?? ?? ?? ? Zn 30 [Ar] ?? ?? ?? ?? ?? ?? SS CI 11.5 The d block 3 Chromium and Copper • Cr and Cu don’t fit the pattern of building up the 3d sub-shell, why? – In the ground state electrons are always arranged to give lowest total energy – Electrons are negatively charged and repel each other – Lower total energy is obtained with e - singly in orbitals rather than if they are paired in an orbital – Energies of 3d and 4s orbitals very close together in Period 4 Chromium and Copper • At Cr – Orbital energies such that putting one e - into each 3d and 4s orbital gives lower energy than having 2 e - in the 4s orbital • At Cu – Putting 2 e - into the 4s orbital would give a higher energy than filling the 3d orbitals SS CI 11.5 The d block 5Read More
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FAQs on d-block Elements PPT Chemistry Class 12
| 1. What are d-block elements? |  |
Ans. D-block elements, also known as transition elements, are a group of elements in the periodic table that occupy the d-block. These elements have partially filled d orbitals and are characterized by their ability to form colored compounds, exhibit variable oxidation states, and form complex ions.
| 2. What are the properties of d-block elements? | |
Ans. D-block elements have several unique properties, including high melting and boiling points, good thermal and electrical conductivity, and high densities. They also exhibit variable oxidation states and form complex compounds due to the availability of d orbitals for bonding.
| 3. How do d-block elements contribute to the color of compounds? | |
Ans. The color of compounds formed by d-block elements is due to their partially filled d orbitals. When light falls on these compounds, electrons in the d orbitals absorb specific wavelengths of light, resulting in the transmission of complementary colors. This absorption and transmission of light give rise to the observed colors of d-block element compounds.
| 4. What are the uses of d-block elements in daily life? | |
Ans. D-block elements find numerous applications in our daily lives. For example, iron (Fe) is used in the production of steel, which is widely used in construction and manufacturing. Copper (Cu) is used in electrical wiring and plumbing, while silver (Ag) is used in jewelry and coins. Other d-block elements, such as titanium (Ti) and chromium (Cr), are used in various industries for their unique properties.
| 5. How do d-block elements form complex ions? | |
Ans. The availability of partially filled d orbitals in d-block elements allows them to form complex ions. These complex ions are formed when ligands, which are molecules or ions with lone pairs of electrons, coordinate with the central d-block element through coordinate bonds. This coordination results in the formation of a complex ion with a central d-block element surrounded by ligands. The formation of complex ions enhances the reactivity and stability of d-block elements.
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