28864
Which among the following is a paramagnetic complex?$($At. No. \(Mo = 42, Pt = 78)\)
1 \([Co(NH_3)_6]^{3+}\)
2 \([Pt(en)Cl_2]\)
3 \([CoBr_4]^{2-}\)
4 \(Mo(CO)_6\)
Explanation:
Magnetic Moments (spin only)- \(\sqrt{n(n+2)}\) where \(n=\) number of unpaired electron. Number of unpaired \(e^{-} s\) and corresponding magnetic moments \(1 \rightarrow 1.7\) \(2 \rightarrow 2.8\) \(3 \rightarrow 3.9\) \(4 \rightarrow 4.9\) \(5 \rightarrow 5.9\) since \(B r^{-}\) is a weak feild ligand, so electrons in \(C o^{2+}\) will not pair up. the complex has \(3\) unpaired electrons leaving it paramagnetic in nature.
COORDINATION COMPOUNDS
28865
Which is diamagnetic ?
1 \([Co(F)_6]^{3-}\)
2 \([Ni(CN)_4]^{2-}\)
3 \([NiCl_4]^{2-}\)
4 \([Fe(CN)_6]^{3-}\)
Explanation:
Diamagnetic substance have all paired electron. (a) [Fe(CN)6]3- Oxidation state of Fe=+3 It has one unpaired electron and is paramagnetic. (b) It has two unpaired electrons and is paramagnetic (c) It has no unpaired electron and is diamagnetic (d) \(\therefore\) It is paramagnetic as it has five unpaired electrons.
28864
Which among the following is a paramagnetic complex?$($At. No. \(Mo = 42, Pt = 78)\)
1 \([Co(NH_3)_6]^{3+}\)
2 \([Pt(en)Cl_2]\)
3 \([CoBr_4]^{2-}\)
4 \(Mo(CO)_6\)
Explanation:
Magnetic Moments (spin only)- \(\sqrt{n(n+2)}\) where \(n=\) number of unpaired electron. Number of unpaired \(e^{-} s\) and corresponding magnetic moments \(1 \rightarrow 1.7\) \(2 \rightarrow 2.8\) \(3 \rightarrow 3.9\) \(4 \rightarrow 4.9\) \(5 \rightarrow 5.9\) since \(B r^{-}\) is a weak feild ligand, so electrons in \(C o^{2+}\) will not pair up. the complex has \(3\) unpaired electrons leaving it paramagnetic in nature.
COORDINATION COMPOUNDS
28865
Which is diamagnetic ?
1 \([Co(F)_6]^{3-}\)
2 \([Ni(CN)_4]^{2-}\)
3 \([NiCl_4]^{2-}\)
4 \([Fe(CN)_6]^{3-}\)
Explanation:
Diamagnetic substance have all paired electron. (a) [Fe(CN)6]3- Oxidation state of Fe=+3 It has one unpaired electron and is paramagnetic. (b) It has two unpaired electrons and is paramagnetic (c) It has no unpaired electron and is diamagnetic (d) \(\therefore\) It is paramagnetic as it has five unpaired electrons.
28864
Which among the following is a paramagnetic complex?$($At. No. \(Mo = 42, Pt = 78)\)
1 \([Co(NH_3)_6]^{3+}\)
2 \([Pt(en)Cl_2]\)
3 \([CoBr_4]^{2-}\)
4 \(Mo(CO)_6\)
Explanation:
Magnetic Moments (spin only)- \(\sqrt{n(n+2)}\) where \(n=\) number of unpaired electron. Number of unpaired \(e^{-} s\) and corresponding magnetic moments \(1 \rightarrow 1.7\) \(2 \rightarrow 2.8\) \(3 \rightarrow 3.9\) \(4 \rightarrow 4.9\) \(5 \rightarrow 5.9\) since \(B r^{-}\) is a weak feild ligand, so electrons in \(C o^{2+}\) will not pair up. the complex has \(3\) unpaired electrons leaving it paramagnetic in nature.
COORDINATION COMPOUNDS
28865
Which is diamagnetic ?
1 \([Co(F)_6]^{3-}\)
2 \([Ni(CN)_4]^{2-}\)
3 \([NiCl_4]^{2-}\)
4 \([Fe(CN)_6]^{3-}\)
Explanation:
Diamagnetic substance have all paired electron. (a) [Fe(CN)6]3- Oxidation state of Fe=+3 It has one unpaired electron and is paramagnetic. (b) It has two unpaired electrons and is paramagnetic (c) It has no unpaired electron and is diamagnetic (d) \(\therefore\) It is paramagnetic as it has five unpaired electrons.
28864
Which among the following is a paramagnetic complex?$($At. No. \(Mo = 42, Pt = 78)\)
1 \([Co(NH_3)_6]^{3+}\)
2 \([Pt(en)Cl_2]\)
3 \([CoBr_4]^{2-}\)
4 \(Mo(CO)_6\)
Explanation:
Magnetic Moments (spin only)- \(\sqrt{n(n+2)}\) where \(n=\) number of unpaired electron. Number of unpaired \(e^{-} s\) and corresponding magnetic moments \(1 \rightarrow 1.7\) \(2 \rightarrow 2.8\) \(3 \rightarrow 3.9\) \(4 \rightarrow 4.9\) \(5 \rightarrow 5.9\) since \(B r^{-}\) is a weak feild ligand, so electrons in \(C o^{2+}\) will not pair up. the complex has \(3\) unpaired electrons leaving it paramagnetic in nature.
COORDINATION COMPOUNDS
28865
Which is diamagnetic ?
1 \([Co(F)_6]^{3-}\)
2 \([Ni(CN)_4]^{2-}\)
3 \([NiCl_4]^{2-}\)
4 \([Fe(CN)_6]^{3-}\)
Explanation:
Diamagnetic substance have all paired electron. (a) [Fe(CN)6]3- Oxidation state of Fe=+3 It has one unpaired electron and is paramagnetic. (b) It has two unpaired electrons and is paramagnetic (c) It has no unpaired electron and is diamagnetic (d) \(\therefore\) It is paramagnetic as it has five unpaired electrons.