Table of contents

1. Matter and Measurements4h 29m
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 35m
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. Amines38m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 46m
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

4. Molecular Compounds

Dipole Moment (Simplified)

GOB Chemistry

4. Molecular Compounds

Dipole Moment (Simplified)

2:02 minutes

Problem 75McMurry - 8th Edition

Textbook Question

Based on electronegativity differences, would you expect bonds between the following pairs of atoms to be largely ionic or largely covalent? b. Ca and Cl

Verified step by step guidance

insert step 1> Determine the electronegativity values of calcium (Ca) and chlorine (Cl) from the periodic table.

insert step 2> Calculate the difference in electronegativity between Ca and Cl.

insert step 3> Use the electronegativity difference to predict the bond type: if the difference is greater than 1.7, the bond is likely ionic; if it is less, the bond is likely covalent.

insert step 4> Consider the position of Ca and Cl in the periodic table: Ca is a metal and Cl is a non-metal, which typically forms ionic bonds.

insert step 5> Conclude whether the bond between Ca and Cl is largely ionic or covalent based on the electronegativity difference and their positions in the periodic table.

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Key Concepts

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

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It is a key factor in determining the nature of the bond formed between two atoms. The greater the difference in electronegativity between two atoms, the more likely the bond will be ionic, as one atom will attract the shared electrons more strongly than the other.

Ionic vs. Covalent Bonds

Ionic bonds occur when electrons are transferred from one atom to another, resulting in the formation of charged ions that attract each other. In contrast, covalent bonds involve the sharing of electrons between atoms. The type of bond formed depends on the electronegativity difference: a large difference typically leads to ionic bonds, while a small difference results in covalent bonds.

Electronegativity Difference

The electronegativity difference between two atoms can be used to predict the bond type. Generally, a difference of 1.7 or greater indicates an ionic bond, while a difference of less than 1.7 suggests a covalent bond. In the case of calcium (Ca) and chlorine (Cl), the significant electronegativity difference suggests that the bond formed between them would be largely ionic.