Solid Solutions and Phase Diagrams

What is a solid solution?

• A liquid phase with dispersed ions

• A solid phase with a single type of atom

• A solid phase containing two or more types of atoms or ions dispersed uniformly

• A gaseous phase with mixed elements

What are alloys?

• Pure metals with no engineering applications

• Materials made from a single element

• Materials that exhibit metallic properties and are made from multiple elements

• Non-metallic compounds used in engineering

What is a phase in the context of solid solutions?

• A region of atoms with varying structures

• A region of atoms with the same structure throughout, roughly the same composition and properties, and a boundary between its surroundings

• A liquid region with mixed properties

• A gaseous region with no defined boundary

When combining two substances, why is it important to know the solid solubility limit?

• To determine the boiling point

• To predict the formation of a new phase

• To measure the density

• To calculate the melting point

Which of the following pairs of substances exhibit unlimited solubility?

• Water and oil

• Salt and water

• Copper and nickel

• Sand and water

What is an example of a combination with limited solubility?

• Water and ethanol

• Copper and nickel

• Salt and water

• Oil and water

Which set of rules must an alloy system follow to exhibit unlimited solubility?

• Hume-Rothery rules

• Euler's Method

• Avogadro's principles

• Boyle's laws

What is the maximum size difference allowed between atoms in an alloy system to avoid excessive lattice strain according to the Hume-Rothery rules?

• 15%

• 25%

• 10%

• 5%

According to the Hume-Rothery rules, what property must be similar between materials to avoid forming compound phases?

• Valence

• Density

• Color

• Hardness

Why do interstitial atoms always have limited solubility according to the Hume-Rothery rules?

• They violate the size restriction

• They have different colors

• They are too dense

• They are too light