Textbook Question
Arrange the bonds in each of the following sets in order of increasing polarity: (c) C—S, B—F, N—O.
697
views
Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 8, Problem 43a
(a) From the data in Table 8.2, calculate the effective charges on the H atom of the HBr molecule in units of the electronic charge, e.
Verified step by step guidance1
Identify the concept of electronegativity and how it relates to effective charge. Electronegativity is a measure of an atom's ability to attract and hold onto electrons.
Look up the electronegativity values for hydrogen (H) and bromine (Br) from Table 8.2. These values will help determine the polarity of the H-Br bond.
Calculate the difference in electronegativity between Br and H. This difference will indicate the direction and magnitude of the dipole moment in the HBr molecule.
Use the concept of partial charges to express the effective charge on the H atom. The partial charge (δ) can be estimated using the formula: δ = (ΔEN / 4), where ΔEN is the electronegativity difference.
Express the effective charge on the H atom in units of the electronic charge, e, by considering the partial charge calculated in the previous step.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Effective Charge
Effective charge refers to the net charge experienced by an electron in an atom, taking into account the shielding effect of other electrons. In molecules, this concept helps to understand how the distribution of electron density affects the behavior of atoms within a compound, such as HBr, where the hydrogen atom's effective charge can be influenced by the presence of bromine.
Recommended video:
Guided course
01:51
Effective Nuclear Charge
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. In the case of HBr, bromine is significantly more electronegative than hydrogen, which leads to a polar covalent bond. This difference in electronegativity is crucial for calculating the effective charge on the hydrogen atom.
Recommended video:
Guided course
02:10Electronegativity Trends
Molecular Dipole Moment
The molecular dipole moment is a vector quantity that represents the separation of positive and negative charges in a molecule. It is influenced by the effective charges on the atoms and their spatial arrangement. In HBr, the dipole moment arises from the unequal sharing of electrons, which is essential for understanding the effective charge on the hydrogen atom.
Recommended video:
Guided course
01:25Dipole Moment
Related Practice
Textbook Question
(b) If you were to put HBr under very high pressure, so its bond length decreased significantly, would its dipole moment increase, decrease, or stay the same, if you assume that the effective charges on the atoms do not change?
821
views
Textbook Question
In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) SiF4 and LaF3 (for ionic or molecular substances) to assign a name to each compound: (b) FeCl2 and ReCl6 (c) PbCl4 and RbCl.
550
views
Textbook Question
The iodine monobromide molecule, IBr, has a bond lengthof 249 pm and a dipole moment of 1.21 D. (a) Which atom ofthe molecule is expected to have a negative charge?
1344
views
Textbook Question
Arrange the bonds in each of the following sets in order of increasing polarity: (a) C—F, O—F, Be—F (b) O—Cl,S—Br, C—P
1222
views
Textbook Question
By referring only to the periodic table, select (d) the element in the group K, C, Zn, F that is most likely to form an ionic compound with Ba.
591
views