Consider the reaction \(Cu^{2+} + X^- → Cu_2X_2 + X_2\).
X2 will be predominantly?
X2 will be predominantly?
- Cl2
- Br2
- I2
- All halogens are possible.
The Correct Option is C
Solution and Explanation
Top Questions on d -and f -Block Elements
Complete the following ionic equations:
$5\text{SO}_3^{2-} + 2\text{MnO}_4^{-} + 6\text{H}^+ \longrightarrow$
- CBSE CLASS XII - 2025
- Chemistry
- d -and f -Block Elements
Answer the following questions:
Name two elements of 3d series for which the third ionisation enthalpies are quite high.
Out of KMnO$_4$ and K$_2$MnO$_4$, which one is paramagnetic and why?
Write any one consequence of lanthanoid contraction.
How do you prepare potassium manganate from pyrolusite ore?
Why is the ability of oxygen more than fluorine to stabilise higher oxidation states of transition metals?- CBSE CLASS XII - 2025
- Chemistry
- d -and f -Block Elements
- Account for the following :The $E^\circ_{\text{Mn}^{3+}/\text{Mn}^{2+}}$ value for manganese is highly negative, whereas $E^\circ_{\text{Mn}^{4+}/\text{Mn}^{3+}}$ is highly positive.
- CBSE CLASS XII - 2025
- Chemistry
- d -and f -Block Elements
- Assertion (A): Actinoids show irregularities in their electronic configurations.
Reason (R): Actinoids are radioactive in nature.- CBSE CLASS XII - 2025
- Chemistry
- d -and f -Block Elements
- Which of the following transition metal ion is not coloured?
- CBSE CLASS XII - 2025
- Chemistry
- d -and f -Block Elements
Questions Asked in JEE Main exam
- Suppose that the number of terms in an A.P. is \( 2k, k \in \mathbb{N} \). If the sum of all odd terms of the A.P. is 40, the sum of all even terms is 55, and the last term of the A.P. exceeds the first term by 27, then \( k \) is equal to:
- JEE Main - 2025
- Arithmetic Progression
- If \( \alpha + i\beta \) and \( \gamma + i\delta \) are the roots of the equation \( x^2 - (3-2i)x - (2i-2) = 0 \), \( i = \sqrt{-1} \), then \( \alpha\gamma + \beta\delta \) is equal to:
- JEE Main - 2025
- Complex numbers
- Let \( [x] \) denote the greatest integer function, and let \( m \) and \( n \) respectively be the numbers of the points, where the function \( f(x) = [x] + |x - 2| \), \( -2<x<3 \), is not continuous and not differentiable. Then \( m + n \) is equal to:
- JEE Main - 2025
- Differential Equations
- Let \( f(x) = \frac{x - 5}{x^2 - 3x + 2} \). If the range of \( f(x) \) is \( (-\infty, \alpha) \cup (\beta, \infty) \), then \( \alpha^2 + \beta^2 \) equals to.
- JEE Main - 2025
- Functions
- Let \( P_n = \alpha^n + \beta^n \), \( P_{10} = 123 \), \( P_9 = 76 \), \( P_8 = 47 \), and \( P_1 = 1 \). The quadratic equation whose roots are \( \frac{1}{\alpha} \) and \( \frac{1}{\beta} \) is:
- JEE Main - 2025
- Sequences and Series
Concepts Used:
d block elements
The elements, in the columns of the periodic table in which d subshells are being occupied are known as d block elements.
These are the elements that have the capability of forming stable cations with incompletely filled d orbitals. Elements like mercury and Zinc are not considered transition metals because they have electronic configurations: (n-1)d10 ns2. These elements have filled d-orbitals in their ground state and, therefore, even in some of their oxidation states.
General Properties Of d-Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behaviour and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high. This is because of the presence of unpaired electrons and partially filled d orbitals. Because of these two things, they form strong bonds and therefore have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements