---
title: "A student analyzes the particulate representations of two solid iron-based alloys, Alloy 1 and Alloy 2, shown in the diagrams below.  Which alloy is an interstitial alloy, and why is this alloy typically less malleable than pure \\(\\text{Fe}\\)?"
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date_modified: "2026-08-23T05:04:50+00:00"
---

# A student analyzes the particulate representations of two solid iron-based alloys, Alloy 1 and Alloy 2, shown in the diagrams below.

Which alloy is an interstitial alloy, and why is this alloy typically less malleable than pure \(\text{Fe}\)?

A student analyzes the particulate representations of two solid iron-based alloys, Alloy 1 and Alloy 2, shown in the diagrams below.

Which alloy is an interstitial alloy, and why is this alloy typically less malleable than pure \(\text{Fe}\)?

![Two side-by-side rectangular boxes labeled Alloy 1 on the left and Alloy 2 on the right. At the top, a legend shows: large open circle = Fe atom, large shaded gray circle = Cr atom, small solid black circle = C atom. In the Alloy 1 box, there is a regular 4 by 4 square grid of 16 closely packed large circles in total: exactly 13 large open circles and 3 large shaded gray circles that occupy lattice sites directly replacing open circles. In the Alloy 2 box, there is a regular 4 by 4 square grid of 16 closely packed large open circles, with exactly 3 small solid black circles located in the interstitial gaps between adjacent large open circles. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787461489-pYgFNh.jpg)

- **A.** Alloy 1, because the solute atoms have an atomic radius similar to \(\text{Fe}\) and occupy lattice sites, which allows the layers of metal atoms to slide past one another more easily.
- **B.** Alloy 1, because the solute atoms replace \(\text{Fe}\) atoms in the lattice, which increases the density of free valence electrons and weakens the metallic bonding.
- **C.** Alloy 2, because the significantly smaller solute atoms occupy the spaces between the \(\text{Fe}\) atoms, which disrupts the regular lattice planes and makes it more difficult for layers of atoms to slide past one another.
- **D.** Alloy 2, because the smaller solute atoms form rigid, directional covalent bonds with adjacent \(\text{Fe}\) atoms, which prevents the delocalization of valence electrons.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121493/*