Free Electronic Structure of d-Block Elements MCQs with Answers
154 Electronic Structure of d-Block Elements MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
The electronic structure of d-block elements covers the filling of the (n-1)d and ns orbitals, general electronic configurations, and the exceptions shown by chromium and copper. It explains how partially filled d orbitals produce variable oxidation states, coloured ions, magnetic behaviour and complex formation, while distinguishing transition elements from elements with completely filled d subshells.
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154 questions · page 5 of 8
- A. Cu-Zn
- B. Cu-Zn-Sn
- C. TiH1.73
- D. V2O5
Explanation: V2O5 is not an interstitial compound. Interstitial compounds are those that do not have an exact composition as shown in V2O5.
Correct answer: V2O5- A. Involvement of inner d-orbitals
- B. Due to the presence of unpaired electrons
- C. d-d transition of electrons
- D. Variable oxidation state
- E. Suitable surface area
Explanation: Transition metals and their compounds act as catalysts because their electronic configurations are variable that enables them to…
Correct answer: Variable oxidation state- A. 3.87 B.M
- B. 2.68 B.M
- C. 5.92 B.M
- D. 6.92 B.M
Explanation: A d7 electron configuration in an octahedral or tetrahedral field will typically have 3 unpaired electrons (t2g5e_g2 or e4t23).
Correct answer: 3.87 B.M- A. The ion absorbs visible light in the region of ~ 5000 Å
- B. The colour results from an electronic transition of one electron from the t2g to an eg orbital
- C. The low colour-intensity is because of a low probability of transition
- D. The transition is the result of metal-ligand back bonding
Explanation: [Ti(H2O)6]3+ has one unpaired electron in its d-subshell which gives rise to the d-d transition to impart colour.
Correct answer: The transition is the result of metal-ligand back bonding- A. Small size of metal ion
- B. Highly charged metal ion
- C. Availability of empty d orbitals
- D. All of these
Explanation: A. Small size of metal ion:Smaller metal ions have a higher charge density, which enhances their ability to attract and hold onto ligands…
Correct answer: All of these- A. [Ar]3d5, 4s2
- B. [Ar]3d6, 4s2
- C. [Ar]3d5, 4s1
- D. [Ar]3d10, 4s2
Explanation: [Ar] 3d5 4s2 is electronic configuration of Mn. It shows maximum +7 oxidation state because it belongs to group VIIB of periodic table.
Correct answer: [Ar]3d5, 4s2- A. Sc
- B. Zn
- C. Cu
- D. Co
Explanation: "Zn" is non-typical transition element it does not show variable oxidation state. So, it shows only +2 oxidation state.i.e Zn2+=[Ar]4so 3d10
Correct answer: Zn- A. Cu+1
- B. Sc+3
- C. Zn+2
- D. All of the above
Explanation: Following ions of 3d-series contain no unpaired electrons. So, these don't show d-d transition and certain colourSe+3, Ti+4, Cu+1 and Zn+2
Correct answer: All of the above- A. Ag2SO4
- B. ZnCl2
- C. MgF2
- D. CuF2
Explanation: Copper in +2 state contain one unpaired electron so it shows d-d transition and certain colour. Cu+2 18[Ar] 4s↿⥮⥮3d⥮⥮
Correct answer: CuF2- A. d-d transitions of electrons
- B. Paramagnetic nature of transition elements
- C. Ionization
- D. Loss of s-electrons
Explanation: The color of transition metal complexes is primarily due to d-d transitions.
Correct answer: d-d transitions of electrons- A. Ti
- B. Cr
- C. Cu
- D. Zn
Explanation: Zinc has complete d-subshell. There is no d-d transition, therefore zinc form a colorless complex.
Correct answer: Zn- A. Colorless
- B. Purple
- C. Blue
- D. Green
Explanation: As colour of transition metals is due to d- transition of electrons but in ionic state Sc does not have electrons in it's d orbital as a…
Correct answer: Colorless- A. 1
- B. 3
- C. 2
- D. 4
Explanation: [Ti+3(H2O)60]+3 22Ti [Ar] 4s2 3d2 22Ti+3 18[Ar] 4s0 3d1 As per the electronic configuration of Ti in [Ti(H2O)6]+3, their is one electron…
Correct answer: 1- A. Yellow, Green
- B. Red, Yellow
- C. Blue, Green
- D. Red, Blue
Explanation: In [Ti (H2O6)+3, yellow light is absorbed while most of the red and blue lights are transmitted, therefore the solution of [Ti (H2O)6]+3…
Correct answer: Red, Blue- A. Sc+3
- B. Cu+1
- C. Fe+3
- D. Zn+2
Explanation: Fe+3 is correct because iron (III) ions can form yellow colored complex compounds under certain conditions.
Correct answer: Fe+3- A. 4
- B. -4
- C. 6
- D. 2
Explanation: The number of lone pair of electrons provided by the ligands to the central metal atom or ion is called the coordination number of the…
Correct answer: 6- A. Monodentate
- B. Bidentate
- C. Tridentate
- D. Hexadentate
Explanation: EDTA is a hexadentate ligand, meaning it can form six bonds with a metal ion.
Correct answer: Hexadentate98. Label the element in the first series of outer transition elements that has highest binding energy.
- A. Titanium
- B. Vanadium
- C. Chromium
- D. Manganese
Explanation: When we move from left to right in the 3d series, the number of unpaired electrons increases upto V-B (vanadium) and VI-B (Chromium).
Correct answer: Chromium- A. +2
- B. +3
- C. -1
- D. +1
Explanation: Certainly! The oxidation state of the central metal (Mn) in the complex Na[Mn(CO)5(F)2] is +2.
Correct answer: +2- A. Neutral ligand
- B. Anionic ligand
- C. Cationic ligand
- D. None of the above
Explanation: This is the correct answer. An amine (NH2) is a neutral ligand because it does not carry a net charge.
Correct answer: Neutral ligand