The bond strength, bond length, and bond order of N − N bond in N 2 H 4 , N 2 H 2 and N 2 is to be compared. Concept introduction: To draw the Lewis structure of the molecule there are following steps: Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom. Step 2: Calculate the total number of valence electrons. Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond. Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons. Step 5: Convert the lone pair into bond pair. Bond strength is directly proportional to the bond order. While the bond length is inversely proportional to the bond order thus higher bond order means smaller bond length. A single bond is weaker and longer than a double bond and a triple bond is most stronger and shorter.
The bond strength, bond length, and bond order of N − N bond in N 2 H 4 , N 2 H 2 and N 2 is to be compared. Concept introduction: To draw the Lewis structure of the molecule there are following steps: Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom. Step 2: Calculate the total number of valence electrons. Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond. Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons. Step 5: Convert the lone pair into bond pair. Bond strength is directly proportional to the bond order. While the bond length is inversely proportional to the bond order thus higher bond order means smaller bond length. A single bond is weaker and longer than a double bond and a triple bond is most stronger and shorter.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
Chapter 10, Problem 10.61P
(a)
Interpretation Introduction
Interpretation:
The bond strength, bond length, and bond order of N−N bond in N2H4, N2H2 and N2 is to be compared.
Concept introduction:
To draw the Lewis structure of the molecule there are following steps:
Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.
Step 2: Calculate the total number of valence electrons.
Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.
Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.
Step 5: Convert the lone pair into bond pair.
Bond strength is directly proportional to the bond order. While the bond length is inversely proportional to the bond order thus higher bond order means smaller bond length.
A single bond is weaker and longer than a double bond and a triple bond is most stronger and shorter.
Interpretation Introduction
Interpretation:
The Lewis structure for tetrazene (H2NNNNH2) is to be drawn. Also ΔHrxn° for the decomposition of tetrazene is to be calculated.
Concept introduction:
To draw the Lewis structure of the molecule following steps are used.
Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.
Step 2: Calculate the total number of valence electrons.
Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.
Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.
Step 5: Convert the lone pair into bond pair.
The heat of the reaction (ΔHrxn°) is defined as the heat released or absorbed during a chemical reaction as a result of the difference in the bond energies (BE) of reactant and product in the reaction. ΔHrxn° is negative for exothermic reaction and ΔHrxn° is positive for an endothermic reaction.
The formula to calculate ΔHrxn° of reaction is as follows:
ΔHrxn°=∑ΔHreactant bond broken°+∑ΔHproduct bond formed°
Or,
ΔHrxn°=∑BEreactant bond broken−∑BEproduct bond formed
The bond energy of reactants is positive and the bond energy of products is negative.
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