To identify the sample, we can calculate its density using the formula:
\[ \text{Density} = \frac{\text{Mass}}{\text{Volume}} \]
Given that the mass is 17.6 g and the volume is 1.96 cm³, we can calculate the density:
\[ \text{Density} = \frac{17.6 , \text{g}}{1.96 , \text{cm}^3} \approx 8.98 , \text{g/cm}^3 \]
Now, we can compare this density with the given densities of the metals:
- Aluminum: 2.70 g/cm³
- Zinc: 7.14 g/cm³
- Iron: 7.87 g/cm³
- Copper: 8.96 g/cm³
- Silver: 10.49 g/cm³
- Lead: 11.34 g/cm³
- Mercury: 13.55 g/cm³
- Gold: 19.32 g/cm³
The density we calculated (approximately 8.98 g/cm³) is closest to the density of copper (8.96 g/cm³).
Thus, the identity of the sample is:
A. copper.