12th Grade > Chemistry
D AND F BLOCK ELEMENTS MCQs
Total Questions : 43
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Answer: Option A. -> The +4 oxidation state of cerium is not known in solutions
:
A
(+4) oxidation state of cerium is also known in solution.The formation of Ce(+4) is favoured by its noble gas configuration, but it is a strong oxidant reverting to thecommon +3 state.
:
A
(+4) oxidation state of cerium is also known in solution.The formation of Ce(+4) is favoured by its noble gas configuration, but it is a strong oxidant reverting to thecommon +3 state.
Answer: Option C. -> Zr and Hf have about the same radius
:
C
Atomic radii down the group for transition elements first increases, becomes almost equal and then decreases. This is due to poor shielding ofone of 4felectron by another in the subshellwhich results in greater effective nuclear charge; this effect is called lanthanide contraction.
:
C
Atomic radii down the group for transition elements first increases, becomes almost equal and then decreases. This is due to poor shielding ofone of 4felectron by another in the subshellwhich results in greater effective nuclear charge; this effect is called lanthanide contraction.
Answer: Option D. -> Manganese (Z = 25)
:
D
25Mn = 3d54s2
After losing two electron electronic configuration will be like this Mn2+(3d5)and this is most stable configuration due to half filled orbitals hence third ionization enthalpy will be highest in this case.
:
D
25Mn = 3d54s2
After losing two electron electronic configuration will be like this Mn2+(3d5)and this is most stable configuration due to half filled orbitals hence third ionization enthalpy will be highest in this case.
Answer: Option C. -> 1s2,2s2p6,3s2p6d2,4s2
:
C
d1−9configuration is transition element.
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C
d1−9configuration is transition element.
Answer: Option B. -> Cr
:
B
V = 1s2,2s2,2p6,3s2,3p6,3d3,4s2
Cr = 1s2,2s2,2p6,3s2,3p6,3d3,4s1
V = 1s2,2s2,2p6,3s2,3p6,3d5,4s2
Fe = 1s2,2s2,2p6,3s2,3p6,3d6,4s2
In second ionization enthalpy Cr+has exact half filledd-sub shell.
:
B
V = 1s2,2s2,2p6,3s2,3p6,3d3,4s2
Cr = 1s2,2s2,2p6,3s2,3p6,3d3,4s1
V = 1s2,2s2,2p6,3s2,3p6,3d5,4s2
Fe = 1s2,2s2,2p6,3s2,3p6,3d6,4s2
In second ionization enthalpy Cr+has exact half filledd-sub shell.
Answer: Option C. -> Due to d5 configuration, metallic bonds are weak
:
C
Due to d5configuration, metallic bonds are weak.d5 orbital is half filled as a result 3delectrons are more tightly held by the nucleus and this reduces the de-localization of electrons resulting in weaker metallic bonding.
:
C
Due to d5configuration, metallic bonds are weak.d5 orbital is half filled as a result 3delectrons are more tightly held by the nucleus and this reduces the de-localization of electrons resulting in weaker metallic bonding.
Answer: Option B. -> MnO2 when treated with fused KOH and oxidized in air, it gives KMnO4(purple)
:
B
MnO2 when treated with fused KOH and oxidized in air, it gives K2MnO4(purple)
2MnO+4KOH+O2⟶2K2MnO4+2H2O
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B
MnO2 when treated with fused KOH and oxidized in air, it gives K2MnO4(purple)
2MnO+4KOH+O2⟶2K2MnO4+2H2O
Answer: Option C. -> Eu2+
:
C
Lanthanoids exhibitf0(Ce4+) and thef14(Yb2+and Lu3+) configurations with no unpaired electron, thus, they are diamagnetic, whereas, Eu2+exhibits f7 configuration with seven unpaired electrons.
:
C
Lanthanoids exhibitf0(Ce4+) and thef14(Yb2+and Lu3+) configurations with no unpaired electron, thus, they are diamagnetic, whereas, Eu2+exhibits f7 configuration with seven unpaired electrons.
Answer: Option D. -> Cr
:
D
Strength of metallic bond depends upon number of unpaired electrons. As number of unpaired electrons increases, the bond strength increases. So Cr,Mo,Wshow stronger bonding due to maximum number of unpaired electron.
:
D
Strength of metallic bond depends upon number of unpaired electrons. As number of unpaired electrons increases, the bond strength increases. So Cr,Mo,Wshow stronger bonding due to maximum number of unpaired electron.
Answer: Option A. -> Yb+3
:
A
Due to Lanthanoid contraction order will beYb+3<Pm+3<Ce+3<La+3
:
A
Due to Lanthanoid contraction order will beYb+3<Pm+3<Ce+3<La+3