Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SO3 and SO2 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  1

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(a)

Expert Solution
Check Mark

Answer to Problem 10.57P

SO2 molecule has a greater dipole moment than SO3 molecule.

Explanation of Solution

The shape of SO3 is bent. In SO3, the oxygen atom is more electronegative than sulfur atom so the direction of dipole moment vector is towards oxygen atom.

The dipole moment in SO3 is represented as follows:

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  2

All the SO polar bonds cancel each other’s polarity and thus result in a zero net dipole moment.

The shape of SO2 is bent. In SO2, the oxygen atom is more electronegative than sulfur atom so the direction of dipole moment vector is towards oxygen atom.

The dipole moment in SO2 is represented as follows:

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  3

The individual dipole moment does not cancel each other so the value of net dipole moment is not zero and therefore SO2 is polar in nature.

Hence, SO2 molecule is more polar than SO3 molecule.

Conclusion

Molecules in which individual dipole moment does not cancel each other result in net non-zero dipole moment and the overall molecule is said to be polar. In SO2 individual dipole moment adds up and SO2 is a polar molecule.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ICl and IF is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  4

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electronegativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

  ΔEN=(electronegativity of B)(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(b)

Expert Solution
Check Mark

Answer to Problem 10.57P

IF has greater dipole moment then the ICl molecule.

Explanation of Solution

The formula to calculate ΔEN in ICl bond is as follows:

  (ΔEN)ICl=(electronegativity of Cl)(electronegativity of I)        (1)

Substitute 3.0 for electro negativity of Cl and 2.5 for electro negativity of I in the equation (1).

  (ΔEN)ICl=(3.0)(2.5)=0.5

The formula to calculate ΔEN in IF bond is as follows:

  (ΔEN)IF=(electronegativity of F)(electronegativity of I)        (2)

Substitute 4.0 for electro negativity of F and 2.5 for electro negativity of I in the equation (2).

  (ΔEN)IF=(4.0)(2.5)=1.5.

Bond polarity and dipole moment are directly related to the electronegativity difference.  Therefore, IF molecule has greater dipole moment than ICl molecule.

Conclusion

Greater the electronegativity difference between the two bonding atoms more polar will be the bond.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among SiF4 and SF4 is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  5

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(c)

Expert Solution
Check Mark

Answer to Problem 10.57P

SF4 molecule has a greater dipole moment than SiF4 molecule.

Explanation of Solution

The shape of SiF4 is tetrahedral. In SiF4, the F  atom is more electronegative than Si atom so the direction of dipole moment vector is towards oxygen atom.

The dipole moment in SiF4 is represented as follows:

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  6

All the SiF polar bonds canceled each other’s polarity with net dipole moment Zero.

The shape of SF4 is see-saw. In SF4, the fluorine atom is more electronegative than sulfur atom so the direction of dipole moment vector is towards fluorine atom.

The dipole moment in SF4 is represented as follows:

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  7

The individual dipole moment does not cancel each other so the value of net dipole moment is not zero and therefore SF4 is polar in nature.

Hence, SF4 molecule has greater dipole moment than SiF4 molecule.

Conclusion

Molecules in which individual dipole moment does not cancel each other result in net non-zero dipole moment and the overall molecule is said to be polar. In SF4 individual dipole moment adds up and SF4 is a polar molecule.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among H2O and H2S is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Chemistry: The Molecular Nature of Matter and Change, Chapter 10, Problem 10.57P , additional homework tip  8

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by ΔEN. ΔEN is the electro negativity difference between the atoms bonded to each other. The formula to calculate ΔEN in AB bond is as follows:

  ΔEN=(electronegativity of B)(electronegativity of A)

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(d)

Expert Solution
Check Mark

Answer to Problem 10.57P

H2O has greater dipole moment then the H2S molecule.

Explanation of Solution

The formula to calculate ΔEN in OH bond is as follows:

  (ΔEN)OH=(electronegativity of O)(electronegativity of H)        (3)

Substitute 3.5 for electro negativity of O and 2.1 for electro negativity of H in the equation (3).

  (ΔEN)OH=(3.5)(2.1)=1.4

The formula to calculate ΔEN in SH bond is as follows:

  (ΔEN)SH=(electronegativity of S)(electronegativity of H)        (4)

Substitute 3.5 for electro negativity of O and 2.1 for electro negativity of H in the equation (4).

  (ΔEN)SH=(2.5)(2.1)=0.4.

Both H2O and H2S has polar bonds and have a similar shape but HO has a larger electronegative difference than H2S. Therefore H2O has a greater dipole moment.

Conclusion

Greater the electronegativity difference between the two bonding atoms more polar will be the bond.

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Chapter 10 Solutions

Chemistry: The Molecular Nature of Matter and Change

Ch. 10.2 - Prob. 10.6AFPCh. 10.2 - Prob. 10.6BFPCh. 10.2 - Prob. 10.7AFPCh. 10.2 - Prob. 10.7BFPCh. 10.2 - Prob. 10.8AFPCh. 10.2 - Prob. 10.8BFPCh. 10.3 - Prob. 10.9AFPCh. 10.3 - Prob. 10.9BFPCh. 10.3 - Prob. B10.1PCh. 10.3 - Prob. B10.2PCh. 10 - Prob. 10.1PCh. 10 - When is a resonance hybrid needed to adequately...Ch. 10 - Prob. 10.3PCh. 10 - Prob. 10.4PCh. 10 - Draw a Lewis structure for (a) SiF4; (b) SeCl2;...Ch. 10 - Draw a Lewis structure for (a) ; (b) C2F4; (c)...Ch. 10 - Prob. 10.7PCh. 10 - Prob. 10.8PCh. 10 - Prob. 10.9PCh. 10 - Draw Lewis structures of all the important...Ch. 10 - Prob. 10.11PCh. 10 - Draw Lewis structures of all the important...Ch. 10 - Prob. 10.13PCh. 10 - Prob. 10.14PCh. 10 - Draw the Lewis structure with lowest formal...Ch. 10 - Draw the Lewis structure with lowest formal...Ch. 10 - Prob. 10.17PCh. 10 - Prob. 10.18PCh. 10 - Prob. 10.19PCh. 10 - Prob. 10.20PCh. 10 - These species do not obey the octet rule. Draw a...Ch. 10 - These species do not obey the octet rule. Draw a...Ch. 10 - Molten beryllium chloride reacts with chloride ion...Ch. 10 - Prob. 10.24PCh. 10 - Prob. 10.25PCh. 10 - Phosgene is a colorless, highly toxic gas that was...Ch. 10 - If you know the formula of a molecule or ion, what...Ch. 10 - In what situation is the name of the molecular...Ch. 10 - Prob. 10.29PCh. 10 - Prob. 10.30PCh. 10 - Consider the following molecular shapes. (a) Which...Ch. 10 - Use wedge-bond perspective drawings (if necessary)...Ch. 10 - Prob. 10.33PCh. 10 - Determine the electron-group arrangement,...Ch. 10 - Determine the electron-group arrangement,...Ch. 10 - Prob. 10.36PCh. 10 - Prob. 10.37PCh. 10 - Prob. 10.38PCh. 10 - Prob. 10.39PCh. 10 - Determine the shape, ideal bond angle(s), and the...Ch. 10 - Prob. 10.41PCh. 10 - Determine the shape around each central atom in...Ch. 10 - Prob. 10.43PCh. 10 - Prob. 10.44PCh. 10 - Prob. 10.45PCh. 10 - Prob. 10.46PCh. 10 - Arrange the following ACln species in order of...Ch. 10 - State an ideal value for each of the bond angles...Ch. 10 - Prob. 10.49PCh. 10 - Prob. 10.50PCh. 10 - Prob. 10.51PCh. 10 - Prob. 10.52PCh. 10 - How can a molecule with polar covalent bonds not...Ch. 10 - Prob. 10.54PCh. 10 - Consider the molecules SCl2, F2, CS2, CF4, and...Ch. 10 - Consider the molecules BF3, PF3, BrF3, SF4, and...Ch. 10 - Prob. 10.57PCh. 10 - Prob. 10.58PCh. 10 - Prob. 10.59PCh. 10 - Prob. 10.60PCh. 10 - Prob. 10.61PCh. 10 - Prob. 10.62PCh. 10 - Prob. 10.63PCh. 10 - Prob. 10.64PCh. 10 - Prob. 10.65PCh. 10 - Prob. 10.66PCh. 10 - When SO3 gains two electrons, forms. (a) Which...Ch. 10 - The actual bond angle in NO2 is 134.3°, and in it...Ch. 10 - Prob. 10.69PCh. 10 - Propylene oxide is used to make many products,...Ch. 10 - Prob. 10.71PCh. 10 - Prob. 10.72PCh. 10 - Prob. 10.73PCh. 10 - Prob. 10.74PCh. 10 - Prob. 10.75PCh. 10 - Prob. 10.76PCh. 10 - Prob. 10.77PCh. 10 - A gaseous compound has a composition by mass of...Ch. 10 - Prob. 10.79PCh. 10 - Prob. 10.80PCh. 10 - Prob. 10.81PCh. 10 - Prob. 10.82PCh. 10 - Pure HN3 (atom sequence HNNN) is explosive. In...Ch. 10 - Prob. 10.84PCh. 10 - Prob. 10.85PCh. 10 - Oxalic acid (H2C2O4) is found in toxic...Ch. 10 - Prob. 10.87PCh. 10 - Hydrazine (N2H4) is used as a rocket fuel because...Ch. 10 - Prob. 10.89PCh. 10 - Prob. 10.90PCh. 10 - Prob. 10.91PCh. 10 - Consider the following molecular shapes: Match...Ch. 10 - Prob. 10.93PCh. 10 - Prob. 10.94PCh. 10 - Prob. 10.95PCh. 10 - Phosphorus pentachloride, a key industrial...
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