The table below includes the bond enthalpy (the energy required to separate the diatomic molecule into its atoms) and the bond length for each diatomic molecule. Diatomic Molecule Bond Enthalpy (kJ/mol) Bond Length (pm) Cl2 243 199 O2 498 121 N2 945 110   Identify the observed trend between bond enthalpy and number of shared electrons: as the number of electrons shared between two atoms increases, the bond enthalpy (  increases  /  decreases  /  remains unchanged  ).   Identify the observed trend between bond length and number of shared electrons: as the number of electrons shared between two atoms increases, the bond length (  increases  /  decreases  /  remains unchanged  ).

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Chapter1: Chemical Foundations
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The table below includes the bond enthalpy (the energy required to separate the diatomic molecule into its atoms) and the bond length for each diatomic molecule.

Diatomic Molecule

Bond Enthalpy (kJ/mol)

Bond Length (pm)

Cl2

243

199

O2

498

121

N2

945

110

 

  • Identify the observed trend between bond enthalpy and number of shared electrons: as the number of electrons shared between two atoms increases, the bond enthalpy (  increases  /  decreases  /  remains unchanged  ).

 

  • Identify the observed trend between bond length and number of shared electrons: as the number of electrons shared between two atoms increases, the bond length (  increases  /  decreases  /  remains unchanged  ).

 

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