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The transition elements are more metallic than the representative elements, because they are
- a)electrons in d-orbitals
- b)electrons pairs in d-orbitals
- c)availibility of d-orbitals for bonding
- d)unpaired electrons in metallic orbitals
Correct answer is option 'C'. Can you explain this answer?
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The transition elements are more metallic than the representative elem...
Option C is correct.
TE have good metallic properties also due to low ionisation energy
TE have good metallic properties also due to low ionisation energy
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The transition elements are more metallic than the representative elem...
Availability of d-orbitals for bonding
The transition elements are more metallic than the representative elements mainly due to the availability of d-orbitals for bonding. Here's why:
1. D-orbitals in transition elements:
Transition elements have partially filled d-orbitals in their valence shell. These d-orbitals can participate in bonding with other atoms, leading to the formation of complex structures and compounds. This ability to form multiple bonds and coordinate with ligands contributes to their metallic nature.
2. Increased electron configurations:
The transition elements have more complex electron configurations compared to the representative elements. This allows for a greater variety of bonding possibilities, leading to the formation of colorful compounds and complex structures.
3. Variable oxidation states:
Transition elements exhibit variable oxidation states due to the presence of d-orbitals. This allows them to form a wide range of compounds with different properties, enhancing their metallic behavior.
4. Transition metal complexes:
Transition elements can form coordination complexes due to the availability of d-orbitals. These complexes exhibit unique properties such as color, magnetism, and catalytic activity, which are characteristic of metallic behavior.
In conclusion, the availability of d-orbitals for bonding in transition elements plays a crucial role in their metallic nature compared to representative elements. Their ability to form complex structures, exhibit variable oxidation states, and form coordination complexes contributes to their metallic properties.
The transition elements are more metallic than the representative elements mainly due to the availability of d-orbitals for bonding. Here's why:
1. D-orbitals in transition elements:
Transition elements have partially filled d-orbitals in their valence shell. These d-orbitals can participate in bonding with other atoms, leading to the formation of complex structures and compounds. This ability to form multiple bonds and coordinate with ligands contributes to their metallic nature.
2. Increased electron configurations:
The transition elements have more complex electron configurations compared to the representative elements. This allows for a greater variety of bonding possibilities, leading to the formation of colorful compounds and complex structures.
3. Variable oxidation states:
Transition elements exhibit variable oxidation states due to the presence of d-orbitals. This allows them to form a wide range of compounds with different properties, enhancing their metallic behavior.
4. Transition metal complexes:
Transition elements can form coordination complexes due to the availability of d-orbitals. These complexes exhibit unique properties such as color, magnetism, and catalytic activity, which are characteristic of metallic behavior.
In conclusion, the availability of d-orbitals for bonding in transition elements plays a crucial role in their metallic nature compared to representative elements. Their ability to form complex structures, exhibit variable oxidation states, and form coordination complexes contributes to their metallic properties.
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The transition elements are more metallic than the representative elements, because they area)electrons in d-orbitalsb)electrons pairs in d-orbitalsc)availibility of d-orbitals for bondingd)unpaired electrons in metallic orbitalsCorrect answer is option 'C'. Can you explain this answer?
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