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The geometry of H(2)S and its dipole mom...

The geometry of `H_(2)S` and its dipole moment are :

A

angular and non zero

B

angular and zero

C

linear and non zero

D

linear and zero

Text Solution

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The correct Answer is:
To determine the geometry and dipole moment of \( H_2S \), we can follow these steps: ### Step 1: Identify the Central Atom In \( H_2S \), sulfur (S) is the central atom because it is less electronegative than hydrogen (H) and can form two bonds with hydrogen. **Hint:** The central atom in a molecule is usually the least electronegative element that can form multiple bonds. ### Step 2: Determine the Valence Electrons Sulfur is in group 16 of the periodic table and has 6 valence electrons. Each hydrogen atom contributes 1 electron, giving a total of 2 electrons from the two hydrogens. Thus, the total number of valence electrons in \( H_2S \) is \( 6 + 2 = 8 \) electrons. **Hint:** Count the valence electrons of each atom to find the total number of electrons available for bonding. ### Step 3: Draw the Lewis Structure In the Lewis structure of \( H_2S \), sulfur is bonded to two hydrogen atoms with single bonds. Sulfur also has two lone pairs of electrons. The structure can be represented as: ``` H | H--S | (Lone Pair) (Lone Pair) ``` **Hint:** Use dots to represent lone pairs and lines to represent bonds in the Lewis structure. ### Step 4: Determine the Molecular Geometry The presence of two lone pairs and two bonding pairs around the sulfur atom leads to a bent or angular geometry according to the VSEPR theory. The bond angle is approximately 104.5°. **Hint:** Use VSEPR theory to predict the shape based on the number of bonding and lone pairs. ### Step 5: Analyze the Dipole Moment In \( H_2S \), sulfur is more electronegative than hydrogen, which means that the S-H bonds will have a dipole moment directed towards sulfur. Additionally, the two lone pairs on sulfur contribute to the overall dipole moment. - The dipole moments from the S-H bonds do not cancel out due to the bent shape of the molecule. Instead, they add up to produce a net dipole moment that is directed upwards. **Hint:** Consider the direction of the dipole moments based on electronegativity and the geometry of the molecule. ### Step 6: Conclusion The geometry of \( H_2S \) is angular (or bent), and it has a non-zero dipole moment directed upwards. **Final Answer:** The geometry of \( H_2S \) is angular, and its dipole moment is non-zero.
To determine the geometry and dipole moment of \( H_2S \), we can follow these steps: ### Step 1: Identify the Central Atom In \( H_2S \), sulfur (S) is the central atom because it is less electronegative than hydrogen (H) and can form two bonds with hydrogen. **Hint:** The central atom in a molecule is usually the least electronegative element that can form multiple bonds. ### Step 2: Determine the Valence Electrons ...
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Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. A diatomic molecule has a dipole moment of 1.2D. If the bond length is 1.0times10^(-8) cm, what fraction of charge does exist each atom?

Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Arrange the following compounds in increasing order of dipole moments, toluene (I), o-dichlorobenzene (II), m-dichlorobenzene (III) and p-dichlorobenzene (IV) :

Knowledge Check

  • The geometry of H_2S and its dipole moment are:

    A
    Angular and non-zero
    B
    Angular and zero
    C
    Linear and zero
    D
    Linear and non-zero

  • The geometry of H_2 S and its moment are :

    A
    angular and non-zero
    B
    angular and zero
    C
    linear and non-zero
    D
    linear and zero

  • Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length d for the bond. Unit of dipole moment is Debye. One Debye is equal to 10^(-18) esu-cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be used to disinguisd between cis- and trans- isomers, ortho-, meta - and para - forms of a substance, etc. The dipole moment value of H-X molecule is 1.2 Debye. If the internuclear distance between H-X is 0.8Å then the % ionic character in H-X molecules is :

    A
    `31.25%`
    B
    `50%`
    C
    `14%`
    D
    `25%`

    • Similar Questions

    Explore conceptually related problems

    Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Arrange the following compounds in increasing order of dipole moments, toluene (I), o-dichlorobenzene (II), m-dichlorobenzene (III) and p-dichlorobenzene (IV) :

    Chemical bonding between two atoms is necessarily associated with an electrical moment arising out of the difference in electroegativity of two atoms. This means that every bond carries with it an electrical moment called the ''bond moment''. The dipole moment of a molecule is really the vectorial sum of the individual bond moment present in it. To compute the dipole moment it is necessary to find out the values of various bond moment. In the following table, dipole moment of different bonds are as given. {:(,rarr,rarr,rarr),("Bond",H-C,C-Cl,C=0),("Bond moments",0.4 D,1.5 D,2.5 D):} The group moments of few groups as given {:("Group",NO_(2),OH,CN,CH_(3)),("Direction of dipole","Towards N","Towards O","Towards N","Away from "CH_(3)),("Dipole moment",4D,1.6D,3.8D,0.4D):} The bond angle in H_(2)S is 97^(@) and its dipole moment is 1.5 D. The S-H bond distance is 0.15 nm. Therefore, approximate percentrage ionic cjaracter pf S-H bond is (neglect the effect of dipole moment of lone pair on sulphur atom in H_(2)S ). (Given : [cos 97^(@)=-0.121 and sqrt(0.88)=0.94] )

    Chemical bonding between two atoms is necessarily with an electrical moment arising out of the difference in electronegativity of two atoms. This means that every bond carries with it an electrical moment called the bond moment.The dipole moment of a molecule is really the vectorial sum of the individual bond moment present in it. To compute the dipole moment it is necessary to find out the values of various bond moment in the moment of different bonds are as given. {:("Bond",oversetto(H-C), " ",oversetto(C-Cl)," ",oversetto(C=O)),("Bond moments",0.4 D ," ", 1.5 D, " ", 2.5D):} The group moments of few groups as given {:("Group",NO_2,OH,CN,CH_3),("direction of dipole","toward N","towards O","towards N","away from" CH_2),("Dipole moment",4D,1.6D,3.8 D,0.4D):} The bond angle in H_2S is 97^@ and its dipole moments is 1.5 D.The S-H bond distance is 0.15 nm.There fore approximate percentage ionic character of S-H bond is (neglect the effect of dipole moment of lone pair on sulphur atom in H_2S ).(Given [cos 97^@=-0.12 ] and sqrt0.88=0.94 )

    H_(2)O has a net dipole moment while BeF_(2) has zero dipole moment because :

    The molecule (s) that will have dipole moment is/are:

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