Explore ionic bonding, lattice enthalpy, and the properties of ionic compounds. This category explains how ions form and how their arrangement affects physical and chemical behavior.
Carbon has 4 valence electrons, and oxygen has 6. Total = 4 + 6 = 10 valence electrons in CO .
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
In TeF₆ , tellurium is sp³d² hybridized with 6 bonding pairs and no lone pairs, resulting in an octahedral shape.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
Nitrogen (N) in Group 15 has 1s² 2s² 2p³ . Gaining 3 electrons forms N³⁻ with 1s² 2s² 2p⁶ , matching Ne .
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
In C₂H₂ (ethyne), the C#C triple bond has a bond length of ~120 pm, shorter than typical double or single bonds.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
In OF₂ , oxygen is sp³ hybridized with two bonding pairs and two lone pairs, resulting in a bent (V-shaped) geometry.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
For Ne₂ : (sigma 1s)² (sigma^* 1s)² (sigma 2s)² (sigma^* 2s)² (sigma 2pz)² (pi 2px)² (pi 2py)² (pi^* 2px)² (pi^* 2py)² (sigma^* 2pz)² . Bonding = 10, antibonding = 10. Bond order = (10 - 10/2) = 0 .
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
In IF₇ , iodine is sp³d³ hybridized with 7 bonding pairs and no lone pairs, forming a pentagonal bipyramidal shape.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
In BeCl₂ , beryllium uses one s and one p orbital to form two sp hybrid orbitals, resulting in a linear geometry.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
Fluorine (F) in Group 17 has 1s² 2s² 2p⁵ . Gaining 1 electron forms F⁻ with 1s² 2s² 2p⁶ , matching Ne .
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
For He₂ : (sigma 1s)² (sigma^* 1s)² . Bonding = 2, antibonding = 2. Bond order = (2 - 2/2) = 0 , making it unstable.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
Cl₂ has a bond enthalpy of ~243 kJ/mol, higher than F₂ (159 kJ/mol), Br₂ (193 kJ/mol), or I₂ (151 kJ/mol) due to optimal bond strength.
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
For N₂ : (sigma 1s)² (sigma^* 1s)² (sigma 2s)² (sigma^* 2s)² (pi 2px)² (pi 2py)² (sigma 2pz)² . Bonding = 10, antibonding = 4. Bond order = (10 - 4/2) = 3 .
Ref: NCERT Class 11 Chemistry > Chapter 4: Chemical Bonding and Molecular Structure > Topic: Ionic Bonding - Lattice Enthalpy and Properties of Ionic Compounds
