Textbook Question
Consider the following solids. The solids A, B, and C represent aluminum (D = 2.70g/mL), and silver (D = 10.5 g/mL). If each has a mass of 10.0 g, what is the identity of each solid? (2.7)
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2. Measurement and Problem Solving
Density
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At standard temperature and pressure (STP), which element has the greatest density?
A
Mercury (Hg)
B
Iron (Fe)
C
Aluminum (Al)
D
Osmium (Os)
Verified step by step guidance1
Understand that density is defined as mass per unit volume, given by the formula \(\text{density} = \frac{\text{mass}}{\text{volume}}\).
Recognize that at standard temperature and pressure (STP), the density of an element in its solid or liquid state depends on its atomic mass and how closely its atoms are packed in the structure.
Note that Mercury (Hg) is a liquid at STP, while Iron (Fe), Aluminum (Al), and Osmium (Os) are solids, so their densities are based on their solid-state atomic packing.
Compare the atomic masses and atomic packing of the elements: Osmium has a very high atomic mass and a very tightly packed crystal structure, which contributes to its high density.
Conclude that among the given elements, Osmium (Os) has the greatest density at STP because of its combination of high atomic mass and compact atomic arrangement.
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