(a) Interpretation: The percent ionic character for LiBr and NaCl bonds separately needs to be determined. Concept introduction: Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic. In a bond, the dipole moment can be calculated as follows: µ = δ × d Here, µ = Dipole mment δ = Partial charge d = Distance
(a) Interpretation: The percent ionic character for LiBr and NaCl bonds separately needs to be determined. Concept introduction: Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic. In a bond, the dipole moment can be calculated as follows: µ = δ × d Here, µ = Dipole mment δ = Partial charge d = Distance
The percent ionic character for LiBr and NaCl bonds separately needs to be determined.
Concept introduction:
Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic.
In a bond, the dipole moment can be calculated as follows:
µ=δ×d
Here,
µ = Dipole mment
δ = Partial charge
d = Distance
Interpretation Introduction
(b)
Interpretation:
The calculated ionic characters of LiBr and NaCl needs to be compared with given theoretical values of figure based on electronegativity values.
Concept introduction:
Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic.
In a bond, the dipole moment can be calculated as follows:
µ=δ×d
Here,
µ = Dipole mment
δ = Partial charge
d = Distance
Interpretation Introduction
(c)
Interpretation:
The reason for equality of calculated percentage ionic values and given data based on electronegativity needs to be explained.
Concept introduction:
Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic.
In a bond, the dipole moment can be calculated as follows:
how would I identify which of these Lewis structures (A, B, C or D) is correct for PO33- and what is the VSEPR shape of the compound?
The hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main componentof rocket propellants. Draw Lewis structures for both ions.
(a) What is the formal charge of Cl in the hypochlorite ion?(b) What is the formal charge of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (c) What is theoxidation number of Cl in the hypochlorite ion? (d) Whatis the oxidation number of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (e) In a redox reaction,which ion would you expect to be more easily reduced?
Write Lewis structures that obey the octet rule for each of thefollowing, and assign oxidation numbers and formal chargesto each atom: (a) OCS, (b) SOCl2 (S is the central atom),(c) BrO3-, (d) HClO2 (H is bonded to O).
Chapter 10 Solutions
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell