AP Chemistry 1.7: Periodic Trends

Practice AP Chemistry 1.7 questions on periodic trends in atomic and ionic radius, ionization energy, shielding, effective nuclear charge, and Coulombic attraction.

Exam points

Use intermolecular forces and structure to explain boiling point, solubility, phase behavior, and properties.
Relate polarity, bonding, and particle interactions to observed properties and separation or purification outcomes.

Covered syllabus points

1.7.A—Explain the relationship between trends in atomic properties of elements and electronic structure and periodicity

[Maximum number: 1]

Sterling silver is an alloy that is commonly used to make jewelry and consists of 92.5\% silver and 7.5\% other metals, such as copper, by mass. Over time, the alloy can form a tarnish of $\mathrm{Ag}_{2} \mathrm{~S}(s)$ when it reacts with hydrogen sulfide, as represented by the following equation.

2 \mathrm{Ag}(s)+\mathrm{H}_{2} \mathrm{~S}(g) \rightarrow \mathrm{Ag}_{2} \mathrm{~S}(s)+\mathrm{H}_{2}(g)

The following table contains the atomic radii for silver and copper.

Table for Question 1.7 Periodic Trends question 1 — AP Chemistry

Using principles of atomic structure and Coulomb's law, explain why silver has a larger atomic radius than copper does.

The $\mathrm{Ag}_{2} \mathrm{~S}$ tarnish on sterling silver can be removed until only sterling silver remains. A student weighs a tarnished sterling silver sample both before and after removing the $\mathrm{Ag}_{2} \mathrm{~S}(s)$ (molar mass 247.80 g / mol) and records the data in the following table.

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Covered syllabus points

1.7 Periodic Trends question 1