The energy used in the excitation of an electron from a lower energy d-orbital to a higher energy d-orbital lies in
The energy used in the excitation of an electron from a lower energy d-orbital to a higher energy d-orbital lies in
A
UV range.
B
IR range.
C
X-ray range.
D
Visible range.
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The correct Answer is:
D
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Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired electrons in the (n-1)d orbitals, most of the transition metal ions and their compounds are paramagnetic. Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from '"Spin only formula"' viz. mu = sqrt(n(n+2)) B.M. n = no . of unpaired electrons Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1)d subshell. When an electron from a lower energy of d-orbital is excited to a higher energy d-orbital, the energy of excitation corresponding to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed correponds to complementary colour of the light absorbed. The frequency of the light absorbed is determined by the nature of the ligand. Which of the following pair of compounds is expected to exhibit same colour in aqueous solution.
Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired electrons in the (n-1)d orbitals, most of the transition metal ions and their compounds are paramagnetic. Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from '"Spin only formula"' viz. mu = sqrt(n(n+2)) B.M. n = no . of unpaired electrons Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1)d subshell. When an electron from a lower energy of d-orbital is excited to a higher energy d-orbital, the energy of excitation corresponding to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed correponds to complementary colour of the light absorbed. The frequency of the light absorbed is determined by the nature of the ligand. Titanium shows magnetic moment of 1.7 BM in its compound. What is the oxidation state of titanium in the compound?
Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired contain unpaired electrons in the (n-1) d orbitals , most of the transition metal ions and their compounds are paramagnetic . Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from spin only formula' Vz mu=sqrt(n(n+2)) B.M n="number of unpaired electrons" Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1) d sub-shell. When an electron from a lower energy of d-orbitals is excited to a higher energy d-orbital, the energy of excitation corresponds to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed corresponds to complementry colour of the light obserbed. The frequency of the light absorbed is determined by the nature of the ligand. Which of the following pair of Compounds is expected to exhibit same colour in aqueous solution
Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired contain unpaired electrons in the (n-1) d orbitals , most of the transition metal ions and their compounds are paramagnetic . Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from 'spin only formula' Vz mu=sqrt(n(n+2)) B.M n="number of unpaired electrons" Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1) d sub-shell. When an electron from a lower energy of d-orbitals is excited to a higher energy d-orbital, the energy of excitation corresponds to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed corresponds to complementry colour of the light obserbed. The frequency of the light absorbed is determined by the nature of the ligand. The colourless species is:
Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired contain unpaired electrons in the (n-1) d orbitals , most of the transition metal ions and their compounds are paramagnetic . Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from 'spin only formula' Vz mu=sqrt(n(n+2)) B.M n="number of unpaired electrons" Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1) d sub-shell. When an electron from a lower energy of d-orbitals is excited to a higher energy d-orbital, the energy of excitation corresponds to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed corresponds to complementry colour of the light obserbed. The frequency of the light absorbed is determined by the nature of the ligand. Titanium shows magnetic moments of 1.73 BM in its compound. What is the oxidation state of titanium in the compound?
Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired contain unpaired electrons in the (n-1) d orbitals , most of the transition metal ions and their compounds are paramagnetic . Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from 'spin only formula' Vz mu=sqrt(n(n+2)) B.M n="number of unpaired electrons" Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1) d sub-shell. When an electron from a lower energy of d-orbitals is excited to a higher energy d-orbital, the energy of excitation corresponds to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed corresponds to complementry colour of the light obserbed. The frequency of the light absorbed is determined by the nature of the ligand. Identify the correct statement.
When an electron from a lower energy d-orbital is excited to a higher energy d-orbital (i)The energy of excitation corresponds to the frequencey of light absorbed. (ii) This frequency generally lines in the visible region. (iii) The colour observed corresponds to the compementary colour of the light absorbed. (iv) The frequencey of the light absorbed is determined by the nature of the ligand. Which one of the above mentioned statements are correct?
Amount of energy required to excite an electron of an atom from the lower energy state to its next higher energy state is defined as:
When an electron from a lower energy d-orbital is excited to a higher energy d-orbital I. The energy of excitation corresponds to the frequency of light absorbed. II. This frequency generally lies in the visible region. III. The colour observed corresponds to the complementary colour of the light absorbed. The above mentioned statements which are correct choose the appropriate option.
4s orbitals has less energy than 3d orbital
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