Which of the following statements is correct about covalent radii in 3d-series of transition elements?
Correct answer: C. First it decreases in the start, constant in the middle and then increases at the end of series
- A. It decreases continuously
- B. First it decreases then increases rapidly
- C. First it decreases in the start, constant in the middle and then increases at the end of series
- D. It remains almost constant in the series
Explanation
The covalent radii of transition elements generally follow this trend. As you move from left to right across the 3D series of transition elements, the covalent radii initially decrease due to increasing effective nuclear charge. However, once you reach the middle of the series (around the element chromium), there's a relatively stable region where the covalent radii remain almost constant. This is because the added electron goes to the 4s orbital rather than the 3d orbital, resulting in a relatively constant increase in atomic size. Toward the end of the series, the covalent radii start to increase as electron-electron repulsions become more significant.
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About Transition Elements
Transition elements are identified by their partially filled d subshells in atoms or common ions. The topic covers the electronic structure of d-block elements, including the filling order of 4s and 3d orbitals, variable oxidation states and the distinction between transition elements and elements with completely filled d subshells.
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