College Chemistry Quiz: Structure Of Metals And Alloys

What this quiz covers

This quiz focuses on Structure Of Metals And Alloys, giving you a quick way to practice the rules, question types, and explanations that matter most for College Chemistry.

How to use this quiz

Try each quiz question before looking at the correct answer. Use the explanations to review missed ideas, then come back to similar questions until the pattern feels familiar.

Question 1

1. Metallic bonding involves delocalized electrons shared among many cations, unlike fixed cation–anion attractions in ionic solids. (correct answer)
2. Metallic bonding forms alternating cations and anions, while ionic bonding shares electrons equally.
3. Metallic bonding occurs only in liquids, while ionic bonding occurs only in gases.
4. Metallic bonding requires localized electron pairs, while ionic bonding requires delocalized electrons.

Question 2

1. Attraction between metal cations and delocalized electrons produces cohesive, non-directional bonding. (correct answer)
2. Attraction between alternating cations and anions forms directional bonds within the lattice.
3. Localized electron pairs form fixed bonds that prevent layers from sliding.
4. Neutral atoms pack randomly and remain held together only by weak dispersion forces.

Question 3

1. Solute atoms have similar atomic radii to the host atoms and compatible packing. (correct answer)
2. Solute atoms are much smaller than the host atoms and easily fit into holes.
3. Solute atoms are nonmetals that form covalent bonds with the host metal.
4. Solute atoms force electrons to become localized, creating directional bonding.

Question 4

1. Substitutional alloy with altered lattice packing, often improving hardness and corrosion resistance. (correct answer)
2. Interstitial alloy with Sn atoms in lattice holes, greatly increasing conductivity.
3. Ionic compound with alternating Cu+ and Sn− ions, producing brittleness like salts.
4. Pure metal with no lattice changes, so properties match those of pure Cu.

Question 5

1. Increased hardness and strength due to hindered dislocation motion in the lattice. (correct answer)
2. Decreased melting point because metallic bonds are replaced by covalent bonds.
3. Loss of conductivity because electrons become confined to individual atoms.
4. Guaranteed brittleness because all alloys are more brittle than pure metals.

Question 6

1. They disrupt lattice regularity and hinder layer slippage and dislocation motion. (correct answer)
2. They convert metallic bonding into ionic bonding, locking ions in place.
3. They create empty space that allows metal layers to slide more easily.
4. They eliminate the electron sea, preventing metallic cohesion under stress.

Question 7

1. Strong attraction between cations and delocalized electrons stabilizes an extended lattice, requiring energy to disrupt. (correct answer)
2. Metals melt easily because their lattices are held together by weak dispersion forces only.
3. Melting points are high because metals form discrete molecules with strong covalent bonds.
4. Melting points depend only on density, not on bonding or lattice arrangement.

Question 8

1. Zn atoms substitute into Cu lattice sites, altering packing and impeding layer motion compared with pure Cu. (correct answer)
2. Zn atoms occupy interstitial holes only, leaving the Cu lattice sites unchanged.
3. Zn forms covalent chains through the Cu lattice, eliminating metallic bonding.
4. Zn converts the solid into an ionic crystal with alternating Zn2+ and Cu2− ions.

Question 9

1. Metal atoms form molecules, and electrons circulate only within each molecule.
2. Metal cations occupy lattice sites, and valence electrons are delocalized and mobile throughout the solid. (correct answer)
3. Metal anions occupy lattice sites, and electrons remain localized on the anions.
4. Metal ions float in a liquid of protons, so conductivity occurs only when molten.

Question 10

1. Non-directional bonding allows cation layers to slide while remaining attracted to the electron sea. (correct answer)
2. Directional bonds prevent movement, so deformation occurs only by bond breaking.
3. Electrons are fixed in place, so stress is relieved by forming new ions.
4. Malleability occurs only in metals with simple cubic lattices, not in bcc or fcc metals.

Question 11

1. Substitutional alloys replace host metal atoms with similar-sized atoms, while interstitial alloys place small atoms in lattice gaps. (correct answer)
2. Substitutional alloys require nonmetals, while interstitial alloys contain only metals.
3. Substitutional alloys form by trapping electrons between ions, while interstitial alloys form by electron transfer.
4. Substitutional alloys place small atoms in lattice gaps, while interstitial alloys replace host atoms in the lattice.

Question 12

1. Substitutional alloy, because Cr atoms can replace Fe atoms at lattice sites. (correct answer)
2. Interstitial alloy, because Cr atoms fit into holes between Fe atoms.
3. Covalent network, because Cr forms directional bonds with Fe throughout.
4. Ionic solid, because Cr donates electrons completely to Fe in the lattice.

Question 13

1. Alloy atoms disrupt regular packing and can hinder dislocation motion, often increasing strength. (correct answer)
2. Alloying always increases ductility because it makes the lattice more uniform.
3. Alloying has no effect because metallic bonds are identical in all compositions.
4. Alloying strengthens metals only by increasing the number of free protons in the electron sea.

Question 14

1. Electrons are shared as localized pairs between specific neighboring metal atoms.
2. Electrons are delocalized and mobile, attracting many metal cations and holding the lattice together. (correct answer)
3. Electrons are transferred completely to form alternating cations and anions in a rigid lattice.
4. Electrons remain fixed on each atom, so bonding depends mainly on magnetic alignment.