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

4. Molecular Compounds

Dipole Moment (Simplified)

GOB Chemistry

4. Molecular Compounds

Dipole Moment (Simplified)

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Problem 135c

Textbook Question

Calculate the electronegativity difference and classify each of the following bonds as nonpolar covalent, polar covalent, or ionic:
c. Na and Cl

Verified step by step guidance

Determine the electronegativity values for sodium (Na) and chlorine (Cl) using the periodic table or a reference chart. Sodium typically has an electronegativity of approximately 0.9, and chlorine has an electronegativity of approximately 3.0.

Calculate the electronegativity difference (ΔEN) between the two elements using the formula:

Δ E N = | E N

_Cl - EN_Na|. Substitute the values for chlorine and sodium into the formula.

Compare the calculated electronegativity difference to the standard ranges for bond classification: nonpolar covalent (ΔEN ≈ 0 to 0.4), polar covalent (ΔEN ≈ 0.5 to 1.9), and ionic (ΔEN ≥ 2.0).

Based on the calculated ΔEN, determine whether the bond between Na and Cl is nonpolar covalent, polar covalent, or ionic.

Conclude the classification of the bond and explain that the large difference in electronegativity between Na and Cl typically results in an ionic bond, where electrons are transferred from Na to Cl.

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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 higher the electronegativity value, the stronger the atom's pull on electrons. This concept is essential for classifying bonds as nonpolar covalent, polar covalent, or ionic based on the difference in electronegativity between the bonded atoms.

Bond Classification

Bonds can be classified into three main types based on the electronegativity difference between the two atoms involved. Nonpolar covalent bonds occur when the difference is negligible (typically less than 0.4), polar covalent bonds form with a moderate difference (0.4 to 1.7), and ionic bonds arise when the difference is significant (greater than 1.7). Understanding these classifications helps predict the properties and behaviors of compounds.

Sodium and Chlorine Interaction

In the case of sodium (Na) and chlorine (Cl), sodium has a low electronegativity, while chlorine has a high electronegativity. The significant difference in their electronegativities (approximately 3.0) indicates that the bond formed between them is ionic. This means that sodium donates an electron to chlorine, resulting in the formation of Na+ and Cl- ions, which are held together by strong electrostatic forces.