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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`)

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Central atoms of `H_(2)` is S. There are 6 electrons in its valence shell`(._16S=2,8,6)` Two electrons are shared with two H-atoms and the remaining four electrons are present as two lone pairs.

Hence, total pairs of electrons are four (2 bond pairs and 2 lone pairs). Due to the presence of 2 lone pairs the shape becomes distorted tetrahedral or angular or bent (non-linear).

`PCl_(3)` - Central atom is phosphorous. There are 5 electrons in the valence shell `(._(15)P=2,8,5)`. Three electrons are shared with three Cl-atoms and the remaining two electrons are present as one lone pair.
Hence, total pairs of electrons are four (1 lone pair and 3 bond pairs). Due to the presence of one lone pair, 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.

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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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