Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

2. Atoms and the Periodic Table

Electronic Structure

GOB Chemistry

2. Atoms and the Periodic Table

Electronic Structure

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1:54 minutes

Problem 44c

Textbook Question

Distinguish between the following:
c. A lone pair and a shared pair of electrons

Verified step by step guidance

Understand the concept of a lone pair: A lone pair refers to a pair of valence electrons that are not involved in bonding and are localized on a single atom. These electrons are not shared with another atom and remain as non-bonding electrons.

Understand the concept of a shared pair: A shared pair of electrons, also known as a bonding pair, refers to a pair of valence electrons that are shared between two atoms to form a covalent bond. These electrons contribute to the bond that holds the atoms together.

Visualize the difference: In a Lewis structure, lone pairs are typically represented as dots around the atom, while shared pairs are represented as a line (or two dots) between two atoms, indicating a covalent bond.

Relate to molecular geometry: Lone pairs can influence the shape of a molecule because they occupy space around the central atom, often causing bond angles to adjust. Shared pairs, on the other hand, directly determine the connectivity between atoms in the molecule.

Apply the knowledge: When analyzing a molecule, identify lone pairs and shared pairs by counting the valence electrons of each atom and determining which are involved in bonding and which remain unshared.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lone Pair of Electrons

A lone pair of electrons refers to a pair of valence electrons that are not shared with another atom. These electrons are localized on a single atom and play a crucial role in determining the geometry and reactivity of molecules. For example, in water (H2O), the oxygen atom has two lone pairs that influence its bent shape.

Shared Pair of Electrons

A shared pair of electrons, also known as a bonding pair, occurs when two atoms share a pair of electrons to form a covalent bond. This sharing allows each atom to attain a more stable electron configuration, often resembling that of noble gases. For instance, in a hydrogen molecule (H2), each hydrogen atom shares one electron, resulting in a stable bond.

Covalent Bonding

Covalent bonding is a type of chemical bond that involves the sharing of electron pairs between atoms. This interaction typically occurs between nonmetals and is fundamental to the structure of many organic and inorganic compounds. The strength and number of shared pairs can affect the properties of the resulting molecule, such as its shape and reactivity.

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