Multiple Choice
List the following elements in order of decreasing density under standard conditions:
a) Magnesium, Mg
b) Bromine, Br
c) Calcium, Ca
d) Barium, Ba
e) Hydrogen, H
23. Chemistry of the Nonmetals
Main Group Elements: Density
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Which of the following diatomic molecules would be expected to have the greatest density?
A
Chlorine
B
Selenium
C
Bromine
D
Iodine
E
Argon
Verified step by step guidance1
Identify the diatomic molecules from the list: Chlorine (Cl2), Selenium (Se2), Bromine (Br2), Iodine (I2), and Argon (Ar2). Note that Argon is a noble gas and typically exists as a monatomic gas, not diatomic.
Recall that density is defined as mass per unit volume. For diatomic molecules, the density can be influenced by the molar mass of the molecule and its physical state at a given temperature and pressure.
Determine the molar mass of each diatomic molecule: Chlorine (Cl2) has a molar mass of approximately 70.9 g/mol, Bromine (Br2) has a molar mass of approximately 159.8 g/mol, and Iodine (I2) has a molar mass of approximately 253.8 g/mol. Selenium (Se2) is less common but has a molar mass of approximately 157.0 g/mol.
Consider the physical state of each molecule at room temperature. Chlorine is a gas, Bromine is a liquid, Iodine is a solid, and Selenium is less common but can be a solid or gas depending on conditions.
Compare the densities based on the molar mass and physical state. Generally, solids have higher densities than liquids and gases. Since Iodine (I2) is a solid with the highest molar mass among the options, it is expected to have the greatest density.
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