Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

1. Intro to General Chemistry

Density of Geometric Objects

General Chemistry

1. Intro to General Chemistry

Density of Geometric Objects

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Multiple Choice

Palladium crystallizes with a face-centered cubic unit cell. The edge length of palladium is 390 pm, and the molar mass of palladium is 106.42 g/mol. What is the density of palladium in g/cm³?

11.8 g/cm³

13.2 g/cm³

12.0 g/cm³

10.5 g/cm³

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Verified step by step guidance

Understand that palladium crystallizes in a face-centered cubic (FCC) unit cell. In an FCC unit cell, there are atoms at each corner and one atom at the center of each face of the cube.

Calculate the number of atoms per unit cell in an FCC structure. Each corner atom is shared by eight unit cells, and each face atom is shared by two unit cells. Therefore, the total number of atoms per unit cell is: \( \text{Number of atoms} = 8 \times \frac{1}{8} + 6 \times \frac{1}{2} = 4 \).

Convert the edge length from picometers to centimeters. Since 1 pm = \( 10^{-12} \) m, and 1 m = 100 cm, the edge length in cm is: \( 390 \text{ pm} \times 10^{-12} \text{ m/pm} \times 100 \text{ cm/m} = 3.90 \times 10^{-8} \text{ cm} \).

Calculate the volume of the unit cell using the edge length: \( \text{Volume} = (3.90 \times 10^{-8} \text{ cm})^3 \).

Determine the density using the formula \( \text{Density} = \frac{\text{Mass of atoms in unit cell}}{\text{Volume of unit cell}} \). First, calculate the mass of the atoms in the unit cell using the molar mass and Avogadro's number: \( \text{Mass} = \frac{4 \text{ atoms} \times 106.42 \text{ g/mol}}{6.022 \times 10^{23} \text{ atoms/mol}} \). Then, divide this mass by the volume calculated in the previous step to find the density in g/cm³.