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Maths-

General

Easy

Question

Convert 3/2 into percentage.

15%
1.5%
150%
0.15%

The correct answer is: 150%

3/2= 1.5
1.5*100= 150%

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In octahedral complexes the filling of $t subscript 2 g end subscript$ orbitals decreases the energy of a complex, that is makes it more stable by $negative 0.4 capital delta subscript 0 end subscript$ per electron. Filling the $e subscript g end subscript$ orbitals increases the energy by $plus 0.6 capital delta subscript 0 end subscript$ per electron. The total crystal field stabilization energy is given by
$C F S E invisible function application left parenthesis$ octahedral $right parenthesis equals negative 0.4 capital delta subscript 0 end subscript open parentheses t subscript 2 g end subscript close parentheses plus 0.6 capital delta subscript 0 end subscript open parentheses e subscript g end subscript close parentheses$

The CFSE increases the thermodynamic stability of the complexes i.e it affects the actual lattice energy over the theoretically calculated energy that does not take CFSE it into account. In studying tetrahedral complexes a regular tetrahedron is related to a cube. One atom is at the centre and four of eight corners are occupied by the ligands. The directions of $x comma y comma z$ point to the centres of the faces of the cube . The directions of the approach of the ligands does not coincide exactly with the atomic orbitals.
In these complexes the $e subscript g end subscript$ orbitals are more stable compared to the $t subscript 2 g end subscript$ orbitals.
Considering $M n to the power of 2 plus end exponent$ if the measured lattice energy is XkJ/mol and the calculated lattice energy is YkJ/mol then their relation between X and Y in a strong and a weak ligand field respectively is

In octahedral complexes the filling of $t subscript 2 g end subscript$ orbitals decreases the energy of a complex, that is makes it more stable by $negative 0.4 capital delta subscript 0 end subscript$ per electron. Filling the $e subscript g end subscript$ orbitals increases the energy by $plus 0.6 capital delta subscript 0 end subscript$ per electron. The total crystal field stabilization energy is given by
$C F S E invisible function application left parenthesis$ octahedral $right parenthesis equals negative 0.4 capital delta subscript 0 end subscript open parentheses t subscript 2 g end subscript close parentheses plus 0.6 capital delta subscript 0 end subscript open parentheses e subscript g end subscript close parentheses$

The CFSE increases the thermodynamic stability of the complexes i.e it affects the actual lattice energy over the theoretically calculated energy that does not take CFSE it into account. In studying tetrahedral complexes a regular tetrahedron is related to a cube. One atom is at the centre and four of eight corners are occupied by the ligands. The directions of $x comma y comma z$ point to the centres of the faces of the cube . The directions of the approach of the ligands does not coincide exactly with the atomic orbitals.
In these complexes the $e subscript g end subscript$ orbitals are more stable compared to the $t subscript 2 g end subscript$ orbitals.
Considering $M n to the power of 2 plus end exponent$ if the measured lattice energy is XkJ/mol and the calculated lattice energy is YkJ/mol then their relation between X and Y in a strong and a weak ligand field respectively is

Chemistry-General

parallel

In octahedral complexes the filling of $t subscript 2 g end subscript$ orbitals decreases the energy of a complex, that is makes it more stable by $negative 0.4 capital delta subscript 0 end subscript$ per electron. Filling the $e subscript g end subscript$ orbitals increases the energy by $plus 0.6 capital delta subscript 0 end subscript$ per electron. The total crystal field stabilization energy is given by
$C F S E invisible function application left parenthesis$ octahedral $right parenthesis equals negative 0.4 capital delta subscript 0 end subscript open parentheses t subscript 2 g end subscript close parentheses plus 0.6 capital delta subscript 0 end subscript open parentheses e subscript g end subscript close parentheses$

The CFSE increases the thermodynamic stability of the complexes i.e it affects the actual lattice energy over the theoretically calculated energy that does not take CFSE it into account. In studying tetrahedral complexes a regular tetrahedron is related to a cube. One atom is at the centre and four of eight corners are occupied by the ligands. The directions of $x comma y comma z$ point to the centres of the faces of the cube . The directions of the approach of the ligands does not coincide exactly with the atomic orbitals.
In these complexes the $e subscript g end subscript$ orbitals are more stable compared to the $t subscript 2 g end subscript$ orbitals.
During the formation of a tetrahedral complex the angle between the e_g orbital and the central metal is $X to the power of ring operator end exponent$ and that of $t subscript 2 g end subscript$ orbital and the central metal is $Y to the power of ring operator end exponent$ then $X to the power of 0 end exponent minus Y to the power of ring operator end exponent$ is.

In octahedral complexes the filling of $t subscript 2 g end subscript$ orbitals decreases the energy of a complex, that is makes it more stable by $negative 0.4 capital delta subscript 0 end subscript$ per electron. Filling the $e subscript g end subscript$ orbitals increases the energy by $plus 0.6 capital delta subscript 0 end subscript$ per electron. The total crystal field stabilization energy is given by
$C F S E invisible function application left parenthesis$ octahedral $right parenthesis equals negative 0.4 capital delta subscript 0 end subscript open parentheses t subscript 2 g end subscript close parentheses plus 0.6 capital delta subscript 0 end subscript open parentheses e subscript g end subscript close parentheses$

The CFSE increases the thermodynamic stability of the complexes i.e it affects the actual lattice energy over the theoretically calculated energy that does not take CFSE it into account. In studying tetrahedral complexes a regular tetrahedron is related to a cube. One atom is at the centre and four of eight corners are occupied by the ligands. The directions of $x comma y comma z$ point to the centres of the faces of the cube . The directions of the approach of the ligands does not coincide exactly with the atomic orbitals.
In these complexes the $e subscript g end subscript$ orbitals are more stable compared to the $t subscript 2 g end subscript$ orbitals.
During the formation of a tetrahedral complex the angle between the e_g orbital and the central metal is $X to the power of ring operator end exponent$ and that of $t subscript 2 g end subscript$ orbital and the central metal is $Y to the power of ring operator end exponent$ then $X to the power of 0 end exponent minus Y to the power of ring operator end exponent$ is.

Chemistry-General

In octahedral complexes the filling of $t subscript 2 g end subscript$ orbitals decreases the energy of a complex, that is makes it more stable by $negative 0.4 capital delta subscript 0 end subscript$ per electron. Filling the $e subscript g end subscript$ orbitals increases the energy by $plus 0.6 capital delta subscript 0 end subscript$ per electron. The total crystal field stabilization energy is given by
$C F S E invisible function application left parenthesis$ octahedral $right parenthesis equals negative 0.4 capital delta subscript 0 end subscript open parentheses t subscript 2 g end subscript close parentheses plus 0.6 capital delta subscript 0 end subscript open parentheses e subscript g end subscript close parentheses$

The CFSE increases the thermodynamic stability of the complexes i.e it affects the actual lattice energy over the theoretically calculated energy that does not take CFSE it into account. In studying tetrahedral complexes a regular tetrahedron is related to a cube. One atom is at the centre and four of eight corners are occupied by the ligands. The directions of $x comma y comma z$ point to the centres of the faces of the cube . The directions of the approach of the ligands does not coincide exactly with the atomic orbitals.
In these complexes the $e subscript g end subscript$ orbitals are more stable compared to the $t subscript 2 g end subscript$ orbitals.
In which of the following complex ion, the metal ion will have $t subscript 2 g end subscript superscript 6 end superscript e subscript g end subscript superscript 0 end superscript$ configuration according to CFT:

In octahedral complexes the filling of $t subscript 2 g end subscript$ orbitals decreases the energy of a complex, that is makes it more stable by $negative 0.4 capital delta subscript 0 end subscript$ per electron. Filling the $e subscript g end subscript$ orbitals increases the energy by $plus 0.6 capital delta subscript 0 end subscript$ per electron. The total crystal field stabilization energy is given by
$C F S E invisible function application left parenthesis$ octahedral $right parenthesis equals negative 0.4 capital delta subscript 0 end subscript open parentheses t subscript 2 g end subscript close parentheses plus 0.6 capital delta subscript 0 end subscript open parentheses e subscript g end subscript close parentheses$

The CFSE increases the thermodynamic stability of the complexes i.e it affects the actual lattice energy over the theoretically calculated energy that does not take CFSE it into account. In studying tetrahedral complexes a regular tetrahedron is related to a cube. One atom is at the centre and four of eight corners are occupied by the ligands. The directions of $x comma y comma z$ point to the centres of the faces of the cube . The directions of the approach of the ligands does not coincide exactly with the atomic orbitals.
In these complexes the $e subscript g end subscript$ orbitals are more stable compared to the $t subscript 2 g end subscript$ orbitals.
In which of the following complex ion, the metal ion will have $t subscript 2 g end subscript superscript 6 end superscript e subscript g end subscript superscript 0 end superscript$ configuration according to CFT:

Chemistry-General

The complexes given below show:

The complexes given below show:

Chemistry-General

parallel

The correct IUPAC name of the complex:

The correct IUPAC name of the complex:

Chemistry-General

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Find the gcf of 2 and 3

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Express 6/8 as a decimal.

Multiply the fractions with the whole number. 3 * 7/8

Multiply the fractions with the whole number. 3 * 7/8

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