Concept explainers
(a)
Interpretation:
Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Answer to Problem 4.73P
The bond between H and Br atom is polar covalent.
Explanation of Solution
The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be polar covalent in nature.
(b)
Interpretation:
Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Answer to Problem 4.73P
The bond between Na and S atom is polar covalent.
Explanation of Solution
The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be polar covalent in nature.
(c)
Interpretation:
Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Answer to Problem 4.73P
The bond between N and C atom is polar covalent.
Explanation of Solution
The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be polar covalent in nature.
(d)
Interpretation:
Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Answer to Problem 4.73P
The bond between Li and O is ionic.
Explanation of Solution
The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be ionic in nature.
Want to see more full solutions like this?
Chapter 4 Solutions
EBK GENERAL, ORGANIC, & BIOLOGICAL CHEM
- • define electronegativity and state how electronegativity varies with position in the periodic table.arrow_forwardClassify each bond as nonpolar covalent or polar covalent or state that ions are formed. (a) SH (b) PH (c) CF (d) CClarrow_forwardA representative element (X) forms an ion with a 2 charge. What is the a. Roman numeral group number for element X b. Lewis symbol for element X c. number of valence electrons possessed by X d. the chemical formula of the compound formed between X and the Ca2+ ionarrow_forward
- Many monatomic ions are found in seawater, including the ions formed from the following list of elements. Write the Lewis symbols for the monatomic ions formed from the following elements: (a) Cl (b) Na (c) Mg (d) Ca (e) K (f) Br (g) Sr (h) Farrow_forwardUsing a periodic table, but not a table of electronegativity values, arrange each of the following sets of atoms in order of increasing electronegativity. a. Be, N, O, B b. Li, C, B, K c. S, Te, Cl, Se d. S, Mg, K, Caarrow_forwardWithout actually drawing the Lewis structure, determine how many valence electrons are available for covalent bonding in each of the following molecules. a. SiH4 b. NCl3 c. H2S d. Cl2Oarrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax