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Interpret the non-linear shape of H(2)S ...

Interpret the non-linear shape of `H_(2)S` molecule and non-planar shape of `PCl_(3)` using valence shell electron pair repulsion (VSEPR) theory.
(Atomic number `:H=1, P=15, S=16, Cl=17`)

Text Solution

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In `H_(2) O ` atomic number of central atom (S) = 16
Electronic arrangment of S = 2, 8, 6
Out of 6 valence eletrons , two electrons are shared with two H atoms and the remaining four electrons are
present as two lone pairs . Thus, we hgave

i.e., it is a molecule of the type `AB_(2)L_(2)` . Due to repulsions between bond pairs and lone pairs the shape is
bent (non-linear).
In `PCl_(3)` atomic number of central atom (P) = 15
Electronic arrangement of P = 2, 8, 5
Out of 5 valence eleectrons , three electrons are shared with three Cl atoms and the remaining 2 electrons are
Present as one lone pair. thus, we have

i.e., it is a molecule of the type `AB_(3) L `. To minimise repulsions between lone pairs bond pairs, the shape
becomes pyramidal (non-planar).
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Interpret non-linear shape of H_(2)S and non-planar shape of PCl_(3) on the basis of VSEPR theory.

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?

Knowledge Check

  • The shape of ClO_3^- according to valence shell electron pair repulsion theory will be

    A
    Planar triangle
    B
    Pyramidal
    C
    Tetrahedral
    D
    Square planar.

  • 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 among the following molecules have sp^(3)d hybridization with one lone pair of electron on the central atom? (P) SF_(4) (Q) [PCl_(4)]^(+) (R) XeO_(2)F_(2) (S) ClOF_(3)

    A
    P, Q and R only
    B
    P, R and S only
    C
    P and Q only
    D
    Q and R only

  • 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 :

    A
    The same with 2, 1 and 0 lone pair of electrons respectively
    B
    Different with 2, 1 and 0 lone pair of electrons respectively
    C
    Different with 0, 1 and 2 lone pair of electrons respectively
    D
    The same with 2,0 and 1 lone pair of leectrons respectively

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    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. Among the following molecules. (P) XeO_(3)" (Q)"XeOF_(4) (R) XeO_(2)F_(2)" (S)"XeF_(5) Those having different molecular geometry but same number of lone pairs on Xe are :

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