Textbook Question
Compare the Lewis structures of CH4 and H2O Why do these molecules have similar bond angles but different molecular shapes?
1
views
Ch.6 Ionic and Molecular Compounds
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 Chemistry in Our Lives11
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy54
- Ch.4 Atoms and Elements51
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions41
- Ch.8 Gases29
- Ch.9 Solutions51
- Ch.10 Acids and Bases and Equilibrium65
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons78
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones83
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides90
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis83
- Ch.18 Metabolic Pathways and ATP Production67
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353Not the one you use?Change textbook
Chapter 6, Problem 74c
Complete each of the following statements for a molecule of H2S:
c. The number of atoms attached to the central S atom is _______.
Verified step by step guidance1
Identify the central atom in the molecule H₂S. In this case, sulfur (S) is the central atom because it is less electronegative than hydrogen and can form multiple bonds.
Determine the number of hydrogen atoms bonded to the sulfur atom. The molecular formula H₂S indicates that there are two hydrogen atoms in the molecule.
Recognize that each hydrogen atom forms a single covalent bond with the sulfur atom. Therefore, there are two atoms (hydrogen) attached to the central sulfur atom.
Verify the molecular geometry of H₂S. Sulfur has two lone pairs of electrons and two bonding pairs (from the hydrogen atoms), resulting in a bent molecular shape, which confirms the bonding arrangement.
Conclude that the number of atoms attached to the central sulfur atom is 2, as there are two hydrogen atoms directly bonded to it.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Structure
Molecular structure refers to the arrangement of atoms within a molecule, including the types of bonds and the spatial orientation of the atoms. In H₂S, the central sulfur (S) atom is bonded to two hydrogen (H) atoms, which influences the molecule's shape and properties.
Recommended video:
Guided course
00:34
Molecular Models Example 1
Valence Electrons
Valence electrons are the outermost electrons of an atom that are involved in forming bonds with other atoms. Sulfur has six valence electrons, and in H₂S, it shares two of these with two hydrogen atoms, allowing it to form two single covalent bonds.
Recommended video:
Guided course
01:55Valence Electrons of Elements (Simplified) Concept 1
Coordination Number
The coordination number of an atom in a molecule refers to the number of atoms directly bonded to it. For the sulfur atom in H₂S, the coordination number is two, as it is bonded to two hydrogen atoms, which is essential for understanding its chemical behavior and reactivity.
Recommended video:
Guided course
03:13Calculate Oxidation Numbers
Related Practice
Textbook Question
Compare the Lewis structures of CF4 and NF3 Why do these molecules have different shapes?
1
views
Textbook Question
Which electronegativity difference (a, b, or c) would you expect for a nonpolar covalent bond?
a. from 0.0 to 0.4
b. from 0.5 to 1.8
c. from 1.9 to 3.3
Textbook Question
Why is CCl4 a nonpolar molecule, but is PCl3 a polar molecule?
Textbook Question
Choose the shape (1 to 6) that matches each of the following descriptions (a to c):
1. linear
2. bent (109°)
3. trigonal planar
4. bent (120°)
5. trigonal pyramidal
6. tetrahedral
b. a molecule with a central atom that has four electron groups and three bonded atoms
1
views
Textbook Question
For each of the following bonds, indicate the positive end with 𝛿⁺ and the negative end with 𝛿⁻ . Draw an arrow to show the dipole for each.
a. N and F