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The linear structure is possessed by...

The linear structure is possessed by

A

`SnCl_(2)`

B

`CS_(2)`

C

`NO_(2)^(+)`

D

`SF_(2)`

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given compounds possesses a linear structure, we will analyze each option step by step, focusing on their hybridization and molecular geometry. ### Step 1: Analyze Cl2 (Chlorine gas) - **Hybridization**: Chlorine is a diatomic molecule (Cl2). Each chlorine atom has 7 valence electrons, and they share one pair of electrons to form a single bond. Since there are no lone pairs on the central atom, it can be considered as having sp hybridization. - **Structure**: The structure of Cl2 is simply a straight line between the two chlorine atoms. However, since there are no central atoms with lone pairs, it can be considered linear. ### Step 2: Analyze SnCl2 (Tin(II) chloride) - **Hybridization**: Tin (Sn) has 4 valence electrons. For SnCl2, there are 2 chlorine atoms (monovalent), so the formula for hybridization is: \[ \text{Hybridization} = \frac{(4 + 2)}{2} = 3 \] This indicates sp² hybridization. - **Structure**: SnCl2 has 2 bond pairs and 1 lone pair, leading to a bent shape (not linear). ### Step 3: Analyze CS2 (Carbon disulfide) - **Hybridization**: Carbon (C) has 4 valence electrons. In CS2, sulfur is divalent, so we can calculate: \[ \text{Hybridization} = \frac{(4 + 0)}{2} = 2 \] This indicates sp hybridization. - **Structure**: The structure of CS2 is linear, with carbon in the center and double bonds to each sulfur atom (C=S=S). ### Step 4: Analyze NO2+ (Nitronium ion) - **Hybridization**: Nitrogen (N) has 5 valence electrons. The positive charge indicates one less electron: \[ \text{Hybridization} = \frac{(5 - 1)}{2} = 2 \] This indicates sp hybridization. - **Structure**: The NO2+ ion has a linear structure due to the presence of two double bonds and no lone pairs on nitrogen. ### Step 5: Analyze SF2 (Sulfur difluoride) - **Hybridization**: Sulfur (S) has 6 valence electrons. For SF2: \[ \text{Hybridization} = \frac{(6 + 2)}{2} = 4 \] This indicates sp³ hybridization. - **Structure**: SF2 has 2 bond pairs and 2 lone pairs, resulting in a bent shape (not linear). ### Conclusion: From the analysis, the compounds with linear structures are: - CS2 (Carbon disulfide) - NO2+ (Nitronium ion) ### Final Answer: The linear structure is possessed by **CS2 and NO2+**.

To determine which of the given compounds possesses a linear structure, we will analyze each option step by step, focusing on their hybridization and molecular geometry. ### Step 1: Analyze Cl2 (Chlorine gas) - **Hybridization**: Chlorine is a diatomic molecule (Cl2). Each chlorine atom has 7 valence electrons, and they share one pair of electrons to form a single bond. Since there are no lone pairs on the central atom, it can be considered as having sp hybridization. - **Structure**: The structure of Cl2 is simply a straight line between the two chlorine atoms. However, since there are no central atoms with lone pairs, it can be considered linear. ### Step 2: Analyze SnCl2 (Tin(II) chloride) - **Hybridization**: Tin (Sn) has 4 valence electrons. For SnCl2, there are 2 chlorine atoms (monovalent), so the formula for hybridization is: ...
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Knowledge Check

  • The crown structure is possessed by

    A
    Phosphorous
    B
    Cyclo-octaring of sulphur
    C
    Cyclic trimer of `SO_3`
    D
    Cyclic tetrameric form of `SeO_3`
  • The linear structure is assumed by

    A
    `SnCl_(2)`
    B
    `NCO^(-)`
    C
    `NO_(2)^(+)`
    D
    `CS_(2)`
  • The linear structure is assumed by

    A
    `CO_(3)^(2-)`
    B
    `NCO^(-)`
    C
    `CS_(2)`
    D
    `NO_(2)^(+)`
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