Input interpretation
![dinitrogen pentoxide](../image_source/11fbc79585aae3006281d3338b3ced34.png)
dinitrogen pentoxide
Chemical names and formulas
![formula | N_2O_5 name | dinitrogen pentoxide IUPAC name | nitro nitrate alternate names | dinitrogen pentoxide | nitrogen oxide | nitrogen oxide (2:5) mass fractions | N (nitrogen) 25.9% | O (oxygen) 74.1%](../image_source/3acf6c0c516066927e1d0f0188094689.png)
formula | N_2O_5 name | dinitrogen pentoxide IUPAC name | nitro nitrate alternate names | dinitrogen pentoxide | nitrogen oxide | nitrogen oxide (2:5) mass fractions | N (nitrogen) 25.9% | O (oxygen) 74.1%
Lewis structure
![Draw the Lewis structure of dinitrogen pentoxide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the nitrogen (n_N, val = 5) and oxygen (n_O, val = 6) atoms: 2 n_N, val + 5 n_O, val = 40 Calculate the number of electrons needed to completely fill the valence shells for nitrogen (n_N, full = 8) and oxygen (n_O, full = 8): 2 n_N, full + 5 n_O, full = 56 Subtracting these two numbers shows that 56 - 40 = 16 bonding electrons are needed. Each bond has two electrons, so in addition to the 6 bonds already present in the diagram add 2 bonds. To minimize formal charge oxygen wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: To fully fill its valence shell, nitrogen will donate one of its electrons, allowing it to form four bonds (the maximum number an element on period 2 can form). Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding nitrogen to the other highlighted oxygen atoms would result in an equivalent molecule: Answer: | |](../image_source/c6a593d5d04168e0a4ed06c4b528cd30.png)
Draw the Lewis structure of dinitrogen pentoxide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the nitrogen (n_N, val = 5) and oxygen (n_O, val = 6) atoms: 2 n_N, val + 5 n_O, val = 40 Calculate the number of electrons needed to completely fill the valence shells for nitrogen (n_N, full = 8) and oxygen (n_O, full = 8): 2 n_N, full + 5 n_O, full = 56 Subtracting these two numbers shows that 56 - 40 = 16 bonding electrons are needed. Each bond has two electrons, so in addition to the 6 bonds already present in the diagram add 2 bonds. To minimize formal charge oxygen wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: To fully fill its valence shell, nitrogen will donate one of its electrons, allowing it to form four bonds (the maximum number an element on period 2 can form). Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding nitrogen to the other highlighted oxygen atoms would result in an equivalent molecule: Answer: | |
3D structure
![3D structure](../image_source/a42bf070d29e91fe1de0a84ec547f9f3.png)
3D structure
Basic properties
![molar mass | 108.01 g/mol phase | solid (at STP) melting point | 30 °C boiling point | 47 °C density | 2.05 g/cm^3](../image_source/f01f3cb0cfce098abe9c07012411d4dc.png)
molar mass | 108.01 g/mol phase | solid (at STP) melting point | 30 °C boiling point | 47 °C density | 2.05 g/cm^3
Units
Solid properties (at STP)
![density | 2.05 g/cm^3](../image_source/f3b916ec923cfc5d8e2263e4ed61172b.png)
density | 2.05 g/cm^3
Units
Thermodynamic properties
![specific heat capacity c_p | gas | 0.8823 J/(g K) | solid | 1.325 J/(g K) molar heat capacity c_p | gas | 95.3 J/(mol K) | solid | 143.1 J/(mol K) specific free energy of formation Δ_fG° | gas | 1.084 kJ/g | solid | 1.055 kJ/g molar free energy of formation Δ_fG° | gas | 117.1 kJ/mol | solid | 113.9 kJ/mol specific heat of formation Δ_fH° | gas | 0.1231 kJ/g | solid | -0.399 kJ/g molar heat of formation Δ_fH° | gas | 13.3 kJ/mol | solid | -43.1 kJ/mol specific entropy S° | solid | 1.648 J/(g K) molar entropy S° | solid | 178 J/(mol K) molar heat of fusion | 34.7 kJ/mol | specific heat of fusion | 0.3213 kJ/g | (at STP)](../image_source/9083f20a818d4e8c5e8b8f97e5c601f6.png)
specific heat capacity c_p | gas | 0.8823 J/(g K) | solid | 1.325 J/(g K) molar heat capacity c_p | gas | 95.3 J/(mol K) | solid | 143.1 J/(mol K) specific free energy of formation Δ_fG° | gas | 1.084 kJ/g | solid | 1.055 kJ/g molar free energy of formation Δ_fG° | gas | 117.1 kJ/mol | solid | 113.9 kJ/mol specific heat of formation Δ_fH° | gas | 0.1231 kJ/g | solid | -0.399 kJ/g molar heat of formation Δ_fH° | gas | 13.3 kJ/mol | solid | -43.1 kJ/mol specific entropy S° | solid | 1.648 J/(g K) molar entropy S° | solid | 178 J/(mol K) molar heat of fusion | 34.7 kJ/mol | specific heat of fusion | 0.3213 kJ/g | (at STP)
Chemical identifiers
![CAS number | 10102-03-1 PubChem CID number | 66242 SMILES identifier | [N+](=O)([O-])O[N+](=O)[O-] InChI identifier | InChI=1/N2O5/c3-1(4)7-2(5)6 EU number | 233-264-2 Gmelin number | 2466](../image_source/a4b5edf0e4f11c37fdb36fff083b2586.png)
CAS number | 10102-03-1 PubChem CID number | 66242 SMILES identifier | [N+](=O)([O-])O[N+](=O)[O-] InChI identifier | InChI=1/N2O5/c3-1(4)7-2(5)6 EU number | 233-264-2 Gmelin number | 2466
NFPA label
![NFPA label](../image_source/723f3260050eb2d5e8bee50b40a6d12c.png)
NFPA label
![NFPA health rating | 3 NFPA fire rating | 0 NFPA reactivity rating | 0 NFPA hazards | oxidizing agent](../image_source/6694c5f3c472a1fae6ad124b103a43b0.png)
NFPA health rating | 3 NFPA fire rating | 0 NFPA reactivity rating | 0 NFPA hazards | oxidizing agent