On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br
On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. msp; a . H — F or H — Cl c . H — Br or H — Cl b . H — Cl or H — I d . H — I or H — Br
Solution Summary: The author explains the chemical bond between two atoms in which electrons are distributed in an unequal amount is known as polar bond.
On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs.
msp;
a
.
H
—
F or H
—
Cl
c
.
H
—
Br or H
—
Cl
b
.
H
—
Cl or H
—
I
d
.
H
—
I or H
—
Br
Expert Solution
Interpretation Introduction
(a)
Interpretation:
On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.
Concept Introduction:
The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.
The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.
Answer to Problem 17QAP
On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−F.
Explanation of Solution
The given pair of bonds is H−F and H−Cl.
The electronegativity value of hydrogen is 2.1.
The electronegativity value of chlorine is 3.0.
The electronegativity value of fluorine is 4.0.
The difference in the electronegativity values for H−F bond is,
Differenceinelectronegativity for H−F bond=4.0−2.1=1.9
The difference in the electronegativity values for H−Cl bond is,
Differenceinelectronegativity for H−Cl bond=3.0−2.1=0.9
The difference in the electronegativity values for H−F bond is 1.9 and for H−Cl bond is 0.9.
The difference in the electronegativity values for H−F bond is higher than the difference in the electronegativity values for H−Cl bond. Hence, H−F bond is more polar than H−Cl bond.
Expert Solution
Interpretation Introduction
(b)
Interpretation:
On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.
Concept Introduction:
The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.
The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.
Answer to Problem 17QAP
On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.
Explanation of Solution
The given pair of bonds is H−Cl and H−I.
The electronegativity value of hydrogen is 2.1.
The electronegativity value of chlorine is 3.0.
The electronegativity value of iodine is 2.5.
The difference in the electronegativity values for H−I bond is,
Differenceinelectronegativity for H−I bond=2.5−2.1=0.4
The difference in the electronegativity values for H−Cl bond is,
Differenceinelectronegativity for H−Cl bond=3.0−2.1=0.9
The difference in the electronegativity values for H−I bond is 0.4 and for H−Cl bond is 0.9.
The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Cl bond is more polar than H−I bond.
Expert Solution
Interpretation Introduction
(c)
Interpretation:
On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.
Concept Introduction:
The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.
The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.
Answer to Problem 17QAP
On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Cl.
Explanation of Solution
The given pair of bonds is H−Cl and H−Br.
The electronegativity value of hydrogen is 2.1.
The electronegativity value of chlorine is 3.0.
The electronegativity value of bromine is 2.8.
The difference in the electronegativity values for H−Br bond is,
Differenceinelectronegativity for H−Br bond=2.8−2.1=0.7
The difference in the electronegativity values for H−Cl bond is,
Differenceinelectronegativity for H−Cl bond=3.0−2.1=0.9
The difference in the electronegativity values for H−Br bond is 0.7 and for H−Cl bond is 0.9.
The difference in the electronegativity values for H−Cl bond is higher than the difference in the electronegativity values for H−Br bond. Hence, H−Cl bond is more polar than H−Br bond.
Expert Solution
Interpretation Introduction
(d)
Interpretation:
On the basis of electronegativity values, the more polar bond in the given pair of bonds is to be stated.
Concept Introduction:
The chemical bond that exists between two atoms in which electrons are distributed in an unequal amount is known as polar bond. Due to this unequal distribution of electrons, the molecule will possess the dipole moment in which one end will have partial positive charge and the other end will have partial negative charge.
The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.
Answer to Problem 17QAP
On the basis of electronegativity values, the more polar bond in the given pair of bonds is H−Br.
Explanation of Solution
The given pair of bonds is H−I and H−Br.
The electronegativity value of hydrogen is 2.1.
The electronegativity value of iodine is 2.5.
The electronegativity value of bromine is 2.8.
The difference in the electronegativity values for H−I bond is,
Differenceinelectronegativity for H−I bond=2.5−2.1=0.4
The difference in the electronegativity values for H−Br bond is,
Differenceinelectronegativity for H−Br bond=2.8−2.1=0.7
The difference in the electronegativity values for H−Br bond is 0.7 and for H−I bond is 0.4.
The difference in the electronegativity values for H−Br bond is higher than the difference in the electronegativity values for H−I bond. Hence, H−Br bond is more polar than H−I bond.
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(f) SO:
Best Lewis Structure
3
e group geometry:_
shape/molecular geometry:,
(g) CF2CF2
Best Lewis Structure
polarity:
e group arrangement:_
shape/molecular geometry:
(h) (NH4)2SO4
Best Lewis Structure
polarity:
e group arrangement:
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
Sketch (with angles):
1.
Problem Set 3b
Chem 141
For each of the following compounds draw the BEST Lewis Structure then sketch the molecule (showing
bond angles). Identify (i) electron group geometry (ii) shape around EACH central atom (iii) whether the
molecule is polar or non-polar (iv)
(a) SeF4
Best Lewis Structure
e group arrangement:_
shape/molecular geometry:
polarity:
(b) AsOBr3
Best Lewis Structure
e group arrangement:_
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
(c) SOCI
Best Lewis Structure
2
e group arrangement:
shape/molecular geometry:_
(d) PCls
Best Lewis Structure
polarity:
e group geometry:_
shape/molecular geometry:_
(e) Ba(BrO2):
Best Lewis Structure
polarity:
e group arrangement:
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
Sketch (with angles):
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