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Nitrogen difluoride
Nitrogen difluoride, also known as difluoroamino, is a reactive radical molecule with formula NF2. This small molecule is in equilibrium with its dimer tetrafluorohydrazine.
As the temperature increases the proportion of NF2 increases.
The molecule is unusual in that it has an odd number of electrons, yet is stable enough to study experimentally.
The energy needed to break the N–N bond in N2F4 is 20.8 kcal/mol (87 kJ/mol), with an entropy change of 38.6 eu. For comparison, the dissociation energy of the N–N bond is 14.6 kcal/mol (61 kJ/mol) in N2O4, 10.2 kcal/mol (43 kJ/mol) in N2O2, and 60 kcal/mol (250 kJ/mol) in N2H4. The enthalpy of formation of N2F4 (ΔfH) is 8.227 kcal/mol (34.421 kJ/mol).
At room temperature N2F4 is mostly associated with only 0.7% in the form of NF2 at 5 mmHg (670 Pa) pressure. When the temperature rises to 225 °C, it mostly dissociates with 99% in the form of NF2.
In NF2, the N–F bond length is 1.3494 Å and the angle subtended at F–N–F is 103.33°.
In the infrared spectrum the N–F bond in NF2 has a symmetrical stretching frequency of 1075 cm−1. This compares to 1115 cm−1 in NF, 1021 cm−1 in NF3 and 998 cm−1 in N2F4.
The microwave spectrum shows numerous lines due to spin transitions, with or without nuclear spin transitions. The lines form set of two triplets for antisymmetric singlet, or two triplets of triplets for symmetric triplet. Lines appear around 14–15, 24, 25, 26, 27, 28–29, 33, 60, 61, 62, and 65 GHz. The rotational constants for the NF2 molecule are A = 70496 MHz, B = 11872.2 MHz, and C = 10136.5 MHz. The inertial defect Δ = 0.1204 mu·Å2. The centrifugal distortion constants are τaaaa = −7.75, τbbbb = −0.081, τaabb = 0.30, and τabab = −0.13.
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Nitrogen difluoride
Nitrogen difluoride, also known as difluoroamino, is a reactive radical molecule with formula NF2. This small molecule is in equilibrium with its dimer tetrafluorohydrazine.
As the temperature increases the proportion of NF2 increases.
The molecule is unusual in that it has an odd number of electrons, yet is stable enough to study experimentally.
The energy needed to break the N–N bond in N2F4 is 20.8 kcal/mol (87 kJ/mol), with an entropy change of 38.6 eu. For comparison, the dissociation energy of the N–N bond is 14.6 kcal/mol (61 kJ/mol) in N2O4, 10.2 kcal/mol (43 kJ/mol) in N2O2, and 60 kcal/mol (250 kJ/mol) in N2H4. The enthalpy of formation of N2F4 (ΔfH) is 8.227 kcal/mol (34.421 kJ/mol).
At room temperature N2F4 is mostly associated with only 0.7% in the form of NF2 at 5 mmHg (670 Pa) pressure. When the temperature rises to 225 °C, it mostly dissociates with 99% in the form of NF2.
In NF2, the N–F bond length is 1.3494 Å and the angle subtended at F–N–F is 103.33°.
In the infrared spectrum the N–F bond in NF2 has a symmetrical stretching frequency of 1075 cm−1. This compares to 1115 cm−1 in NF, 1021 cm−1 in NF3 and 998 cm−1 in N2F4.
The microwave spectrum shows numerous lines due to spin transitions, with or without nuclear spin transitions. The lines form set of two triplets for antisymmetric singlet, or two triplets of triplets for symmetric triplet. Lines appear around 14–15, 24, 25, 26, 27, 28–29, 33, 60, 61, 62, and 65 GHz. The rotational constants for the NF2 molecule are A = 70496 MHz, B = 11872.2 MHz, and C = 10136.5 MHz. The inertial defect Δ = 0.1204 mu·Å2. The centrifugal distortion constants are τaaaa = −7.75, τbbbb = −0.081, τaabb = 0.30, and τabab = −0.13.