Covalent Bond | Bond Pair and Lone Pair | Coordinate Bond

Introduction|Octet Rule|Covalent Bond|Bond Pair And Lone Pair

Introduction|Octet Rule|Covalent Bond|Bond Pair And Lone Pair

Covalent Bond|Bond Pair & Lone Pair|Lewis Representation Of Simple Molecular (The Lewis Structures)|Example|Summary

Electrovalent Or Ionic Bond|Example|Conditions To Form Ionic Bond|Formation Of Lattice|Properties Of Ionic Compounds|Lewis Symbols|Covalent Bond|Bond Pair & Lone Pair|Lewis Representation Of Simple Molecules (The Lewis Structures)|Example|Summary

Hybridisation And Shapes Of Molecules Containing Bond Pairs And Lone Pairs Of Electrons

The approximate shape of a molecule can often be predicted by using what is called the valence-shell electron-pair repulsion (VSEPR) model. Electrons in bonds and in lone pairs can be thought of a ''charge cloud'' that repel one another nad stay as far apart as possible, thus causing molecules to assume specific shapes. The repulsive interactions of electron pairs decrease in the order: Lone pair - Lone pair gt Lone pair - Bond pair gt Bond pair - Bond pair These repulsive effects result in deviations from idealised shapes and alteration in bond angles in molecules. Which of the following statement is correct with respect ot bond angles?

The approximate shape of a molecule can often be predicted by using what is called the valence-shell electron-pair repulsion (VSEPR) model. Electrons in bonds and in lone pairs can be thought of a ''charge cloud'' that repel one another nad stay as far apart as possible, thus causing molecules to assume specific shapes. The repulsive interactions of electron pairs decrease in the order: Lone pair - Lone pair gt Lone pair - Bond pair gt Bond pair - Bond pair These repulsive effects result in deviations from idealised shapes and alteration in bond angles in molecules. Which of the following statements is incorrect?

The approximate shape of a molecule can often be predicted by using what is called the valence-shell electron-pair repulsion (VSEPR) model. Electrons in bonds and in lone pairs can be thought of a ''charge cloud'' that repel one another nad stay as far apart as possible, thus causing molecules to assume specific shapes. The repulsive interactions of electron pairs decrease in the order: Lone pair - Lone pair gt Lone pair - Bond pair gt Bond pair - Bond pair These repulsive effects result in deviations from idealised shapes and alteration in bond angles in molecules. Molecular shape of XeF_(3)^(+),SF_(3)^(+) and CF_(3)^(+) are :

Predict the correct order among the following Lone pair - lone pair > Ione pair - bond pair > bond pair - bond pair Lone pair - lone pair > bond pair -bond pair> Lone pair - bond pair Bond pair - bond pair > Ione pair - bond pair > Lone pair - bond pair lone pair- bond pair > bond pair-bond pair> lone pair - lone pair