AP Chemistry Quiz: Properties Of Solids

20 questions · exam conditions

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Properties Of SolidsQuestion 1 of 20

A student heats two solids to compare melting behavior. Solid P is a molecular solid made of polar molecules capable of hydrogen bonding. Solid Q is an ionic solid. Which statement best describes their melting behavior?

P melts at a higher temperature than Q because hydrogen bonds are stronger than ionic bonds

P melts at a lower temperature than Q because intermolecular forces are weaker than ionic attractions

P and Q melt at similar temperatures because both are crystalline solids

P melts at a higher temperature than Q because polar molecules have mobile electrons

P and Q both do not melt but decompose because strong bonds prevent phase changes

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AP Chemistry Quiz

AP Chemistry Quiz: Properties Of Solids

Practice Properties Of Solids in AP Chemistry with focused quiz questions that help you check what you know, review explanations, and build confidence with test-style prompts.

What this quiz covers

This quiz focuses on Properties Of Solids, giving you a quick way to practice the rules, question types, and explanations that matter most for AP 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.

All questions

Question 1

P melts at a higher temperature than Q because hydrogen bonds are stronger than ionic bonds
P melts at a lower temperature than Q because intermolecular forces are weaker than ionic attractions (correct answer)
P and Q melt at similar temperatures because both are crystalline solids
P melts at a higher temperature than Q because polar molecules have mobile electrons
P and Q both do not melt but decompose because strong bonds prevent phase changes

Explanation: This question evaluates the comparison of melting behaviors between molecular and ionic solids based on bonding strengths. Solid P, with polar molecules and hydrogen bonding, has intermolecular forces that are weaker than the ionic attractions in solid Q, leading to a lower melting point for P. Ionic solids like Q require more energy to disrupt the lattice of charged ions, resulting in higher melting temperatures. This is accurately stated in choice B, as seen in comparisons like water (molecular) versus NaCl (ionic). A tempting distractor is choice A, reversing the strengths by claiming hydrogen bonds exceed ionic bonds, due to the misconception of overestimating intermolecular forces. To predict melting points, assess the type and strength of forces holding particles together, whether intermolecular or ionic.

Question 2

A student tests an unknown solid. It is dull, soft, and has a low melting point. It does not conduct electricity as a solid, and the liquid also does not conduct. Which classification is most consistent with these observations?

Metallic solid
Covalent network solid
Molecular solid (correct answer)
Intermetallic compound
Ionic solid

Explanation: This question tests the skill of classifying solids using a set of observed properties. The correct answer is C, molecular solid, because the dull appearance, softness, low melting point, and lack of conductivity in both states indicate discrete neutral molecules held by weak intermolecular forces, without mobile charges or strong bonds. Molecular solids melt easily and are often soft. The nonconductivity rules out ionic or metallic types. A tempting distractor is A, ionic solid, which is incorrect as ionics have high melting points; the misconception is attributing low melting to ionic lattices. Compile all properties and eliminate solid types that don't match the full set.

Question 3

A solid is composed of discrete molecules that are polar and capable of hydrogen bonding. Compared with a similar-sized nonpolar molecular solid, which property is most likely to be higher for the hydrogen-bonding solid?

Melting point (correct answer)
Electrical conductivity in the solid state
Malleability
Hardness comparable to a covalent network solid
Electrical conductivity when melted

Explanation: This question tests the skill of relating intermolecular forces to physical properties in molecular solids. The correct answer is B, melting point, because hydrogen bonding in the polar solid creates stronger intermolecular attractions than London dispersion forces in a nonpolar solid of similar size, requiring more energy to melt. This leads to a higher melting point for the hydrogen-bonding solid. Other properties like conductivity and malleability are similar as both are nonconductive and brittle molecular solids. A tempting distractor is A, electrical conductivity in the solid state, which is incorrect as neither conducts due to lack of charge carriers; the misconception is assuming hydrogen bonding enables charge mobility like in ionic solids. Compare properties of similar compounds differing only in intermolecular force type to predict trends like melting points.

Question 4

A covalent network solid is heated strongly. It does not melt under typical laboratory heating and remains nonconductive. Which explanation best accounts for its very high melting point?

Breaking the solid requires overcoming strong covalent bonds throughout the lattice (correct answer)
Melting requires separating ions from a lattice stabilized by ion-dipole forces
Melting requires disrupting metallic bonds formed by localized electrons
Melting requires breaking hydrogen bonds within each molecule
Melting requires overcoming only London dispersion forces between atoms

Explanation: This question tests the skill of explaining high melting points in covalent network solids. The correct answer is A, breaking the solid requires overcoming strong covalent bonds throughout the lattice, because the entire structure is interconnected by covalent bonds, demanding high energy to disrupt, unlike weaker forces in other solids. Nonconductivity persists as there are no mobile charge carriers. This accounts for the extreme thermal stability. A tempting distractor is E, melting requires overcoming only London dispersion forces between atoms, which is incorrect as it applies to atomic solids, not networks; the misconception is underestimating the strength of covalent lattices. Relate melting behavior to the type and extent of bonding across the solid's structure.

Question 5

A shiny gray solid can be hammered into thin sheets and drawn into wires. It conducts electricity well as a solid and remains conductive when melted. Which type of solid is it, and which property best supports that classification?

Molecular; it has a low melting point and is brittle
Covalent network; it is nonconductive and soft
Metallic; it is malleable and conductive as a solid (correct answer)
Ionic; it conducts electricity only when melted
Ionic; it is malleable and conductive as a solid

Explanation: This question tests the skill of classifying solids by type and supporting properties. The correct answer is C, metallic; it is malleable and conductive as a solid, because the solid's ability to be hammered into sheets and drawn into wires indicates malleability, a hallmark of metallic bonding where cations slide in a sea of delocalized electrons without breaking the structure. Conductivity in both solid and molten states arises from mobile electrons that remain free even in the liquid. The shiny appearance further supports metallic classification. A tempting distractor is E, ionic; it is malleable and conductive as a solid, which is incorrect as ionic solids are brittle, not malleable; the misconception is equating metallic ductility with ionic lattices. Always match multiple properties like ductility, luster, and conductivity across phases to confirm solid type.

Question 6

A metallic solid and an ionic solid are both heated above their melting points. Which statement correctly compares their electrical conductivity in the molten state?

Only the metallic liquid conducts because ions cannot carry current
Only the ionic liquid conducts because electrons are no longer mobile
Both conduct because metals have mobile electrons and ionic melts have mobile ions (correct answer)
Neither conducts because melting disrupts all charge carriers
Both conduct only if dissolved in water first

Explanation: This question tests the skill of comparing conductivity in different phases for metallic and ionic solids. The correct answer is C, both conduct because metals have mobile electrons and ionic melts have mobile ions, as metallic liquids retain delocalized electrons for charge transport, while ionic melts free ions from the lattice to move. Melting does not eliminate charge carriers in either case. This highlights similarities in molten conductivity despite different mechanisms. A tempting distractor is B, only the ionic liquid conducts because electrons are no longer mobile, which is incorrect for metals; the misconception is assuming melting localizes electrons in metallics. Compare phase-dependent conductivity to distinguish charge carrier types in solids.

Question 7

A crystalline solid is brittle and has a high melting point. In a conductivity test, the solid does not conduct, but an aqueous solution of the solid conducts strongly. Which conclusion is best supported?

The solid is covalent network because it conducts only when dissolved
The solid is ionic because it forms mobile ions in solution (correct answer)
The solid is metallic because it is brittle and has a high melting point
The solid is metallic because its ions carry charge in the crystal
The solid is molecular because it dissolves and forms mobile electrons

Explanation: This question tests the skill of inferring solid type from conductivity and physical properties. The correct answer is C, the solid is ionic because it forms mobile ions in solution, as the brittleness and high melting point suggest strong lattice forces, while nonconductivity in the solid indicates fixed particles, but aqueous conductivity implies dissociation into mobile ions. Ionic solids conduct in solution or melt due to free ions carrying charge. This matches the observation of strong conductivity only in solution. A tempting distractor is A, the solid is metallic because its ions carry charge in the crystal, which is incorrect as metallics conduct in the solid state via electrons; the misconception is attributing solution conductivity to metallic properties. Use conductivity tests in solid, molten, and dissolved states to differentiate ionic from other solids.

Question 8

A shiny gray solid can be hammered into thin sheets and drawn into wires. It conducts electricity well as a solid and also conducts when molten. Which type of solid is most consistent with these properties?

Ionic solid
Molecular solid
Covalent-network solid
Metallic solid (correct answer)
Hydrated ionic solid

Explanation: This question tests identification of metallic solids through their characteristic mechanical and electrical properties. The solid is shiny, can be hammered into sheets (malleable), drawn into wires (ductile), and conducts electricity both as a solid and when molten - these are all defining properties of metallic solids. Metallic solids consist of metal atoms arranged in a lattice with valence electrons delocalized in a "sea of electrons" that can move freely throughout the structure. This electron sea accounts for the electrical conductivity in both solid and liquid states, while the non-directional metallic bonding allows atoms to slide past each other when force is applied, explaining malleability and ductility. A common misconception is choosing ionic solid (A) because students might focus only on conductivity, but ionic solids are brittle rather than malleable and only conduct when molten or dissolved. To identify metallic solids, look for the unique combination of malleability/ductility with electrical conductivity in the solid state.

Question 9

Two solids, X and Y, are tested. Solid X is brittle and conducts electricity only when molten. Solid Y is soft, has a low melting point, and does not conduct electricity as a solid or as a liquid. Which identification is most consistent with these results?

X is metallic and Y is ionic
X is ionic and Y is molecular (correct answer)
X is covalent-network and Y is metallic
X is molecular and Y is ionic
X is metallic and Y is covalent-network

Explanation: This question tests the ability to distinguish between different solid types based on their properties. Solid X is brittle and conducts only when molten - classic ionic solid behavior where ions are fixed in the solid but mobile when melted. Solid Y is soft, has a low melting point, and never conducts electricity - typical of molecular solids held together by weak intermolecular forces. Ionic solids conduct when molten because the ions become free to move and carry charge, while molecular solids don't conduct because they lack mobile charge carriers even when melted. The brittleness of X versus the softness of Y reflects the different bonding: ionic crystals shatter when layers shift due to electrostatic repulsion, while molecular solids can deform more easily. Students often incorrectly choose option D, reversing the identifications because they associate low melting points with ionic compounds, forgetting that ionic bonds are actually very strong. Use conductivity when molten as a key test: ionic solids conduct when melted, molecular solids don't.

Question 10

A sample of solid Z is very hard, does not melt in a Bunsen burner flame, and does not conduct electricity as a solid. Which classification best fits solid Z?

Molecular solid
Covalent-network solid (correct answer)
Metallic solid
Ionic solid
Amorphous solid

Explanation: This question tests recognition of covalent-network solid properties based on hardness, melting point, and electrical conductivity. Solid Z is very hard, doesn't melt in a Bunsen burner flame (indicating extremely high melting point), and doesn't conduct electricity - these properties uniquely identify covalent-network solids. Covalent-network solids consist of atoms connected by continuous networks of strong covalent bonds extending throughout the entire crystal, as seen in diamond (carbon), quartz (SiO₂), and silicon carbide (SiC). The extensive covalent bonding makes these solids extremely hard and gives them very high melting points, often above 1000°C, well beyond typical Bunsen burner temperatures. Students might incorrectly choose ionic solid (D) because ionic solids can also be hard, but ionic solids typically have lower melting points than covalent-network solids and would conduct electricity when molten. To identify covalent-network solids, look for the combination of extreme hardness, very high melting point, and non-conductivity in all states.

Question 11

A clear, hard solid is an electrical insulator and has an extremely high melting point. The solid is composed only of silicon and oxygen atoms in a continuous 3D arrangement. Which statement best describes its brittleness and melting behavior?

It is malleable and has a low melting point because layers can slide past one another.
It is brittle and has a very high melting point because covalent bonds extend throughout the solid. (correct answer)
It is brittle and has a low melting point because only weak intermolecular forces are present.
It is malleable and has a very high melting point because ions are free to move in the lattice.
It is malleable and has a low melting point because electrons are localized on each atom.

Explanation: This question tests understanding of covalent network solid properties. The silicon-oxygen solid with continuous 3D arrangement describes a covalent network solid like quartz (SiO₂), where atoms are connected by strong covalent bonds extending throughout the structure. Breaking these solids requires breaking covalent bonds, resulting in extremely high melting points. The rigid, directional nature of covalent bonds makes these solids brittle - when stress is applied, bonds break rather than allowing layers to slide. Answer choice A incorrectly suggests malleability and low melting point, confusing network solids with metallic solids. To identify network solids, look for continuous covalent bonding, extreme hardness, brittleness, and very high melting points.

Question 12

A student compares two solids at room temperature: Solid X is brittle and conducts electricity only when molten; Solid Y is malleable and conducts electricity as a solid. Which pairing of solid types best matches X and Y?

X: molecular; Y: covalent network
X: ionic; Y: metallic (correct answer)
X: metallic; Y: ionic
X: covalent network; Y: molecular
X: molecular; Y: ionic

Explanation: This question tests distinguishing between solid types based on mechanical and electrical properties. Solid X (brittle, conducts only when molten) exhibits typical ionic solid behavior - ions are fixed in the solid but become mobile when melted. Solid Y (malleable, conducts as solid) shows metallic properties - delocalized electrons enable conductivity and non-directional bonding allows malleability. Answer choice A incorrectly identifies X as molecular, but molecular solids don't conduct when molten since they lack ions. To differentiate solid types, use the combination of mechanical properties (brittle vs malleable) and conductivity patterns (never, when dissolved/molten, or always).

Question 13

A solid is made of an extended 3D network of covalent bonds between silicon and oxygen atoms (no discrete molecules or ions). Which property is most consistent with this type of solid?

Low melting point, soft, conductive as a solid due to mobile electrons
Moderate melting point, soft, nonconductive as a solid but conductive when melted
High melting point, brittle, nonconductive as a solid and nonconductive when melted (correct answer)
Low melting point, brittle, conductive when dissolved in water due to ions
High melting point, malleable, conductive as a solid and conductive when melted

Explanation: This question assesses understanding of covalent network solids and their distinctive properties derived from extended bonding. The solid is a silica-like network of covalent bonds between silicon and oxygen atoms, requiring significant energy to break bonds for melting, thus having a high melting point and brittleness due to the rigid 3D structure. It remains nonconductive as a solid and when melted because there are no free ions or delocalized electrons, only localized covalent bonds. This is consistent with choice C, as seen in quartz or diamond. A tempting distractor is choice D, which implies malleability and conductivity like metals, based on the misconception that high melting points always indicate metallic bonding with mobile electrons. To identify covalent network solids, look for high hardness, high melting points, and consistent nonconductivity across phases, distinguishing them from ionic or metallic solids.

Question 14

A solid is composed of $\text{Na}^+$ and a large polyatomic anion. The solid is hard and crystalline, and it shatters when struck. Which observation would best support classifying this solid as ionic rather than metallic?

It conducts electricity well in the solid state and can be hammered into sheets
It is nonconductive as a solid but conducts when molten (correct answer)
It has a low melting point and is nonconductive in both solid and liquid states
It is malleable and conducts electricity in both solid and molten states
It sublimates easily and conducts electricity only when dissolved in a nonpolar solvent

Explanation: This question examines the differentiation between ionic and metallic solids using conductivity and mechanical observations. The solid has Na⁺ ions and a polyatomic anion, forming an ionic lattice that is hard and brittle, shattering due to like-charge repulsion upon impact. It is nonconductive as a solid with fixed ions but conducts when molten as ions become mobile, supporting ionic classification over metallic, as in choice B. This contrasts with metals, which conduct in the solid state due to delocalized electrons. A tempting distractor is choice A, suggesting malleability and solid conductivity, based on the misconception that ionic solids with cations behave like metals. To distinguish ionic from metallic solids, prioritize testing conductivity in solid versus molten states alongside brittleness.

Question 15

A student compares two solids. Solid X is a crystalline salt that forms a clear, conducting solution in water. Solid Y is a crystalline solid that does not dissolve in water and is an electrical insulator as a solid. Solid Y is known to be composed of carbon atoms in a tetrahedral network. Which statement correctly compares X and Y?

X and Y both have low melting points because their particles are held by weak intermolecular forces
X is malleable because ions can slide, while Y is brittle because electrons are localized
X conducts as a solid due to mobile electrons, while Y conducts when dissolved due to ions
X is brittle and has a high melting point, while Y is very hard and has a very high melting point (correct answer)
X and Y both conduct electricity as solids because both are crystalline

Explanation: This question tests the comparison of ionic and covalent network solids based on solubility, conductivity, and mechanical properties. Solid X is an ionic salt with high melting point and brittleness due to electrostatic lattice forces, conducting when dissolved as ions mobilize in water. Solid Y is diamond, a covalent network with extremely high melting point and hardness from strong, directional covalent bonds, remaining insoluble and nonconductive. This comparison is accurately described in choice D, highlighting the differences in durability and thermal stability. A tempting distractor is choice C, which incorrectly attributes solid conductivity to X via mobile electrons, reflecting the misconception of confusing ionic with metallic bonding. To compare solids, evaluate solubility and conductivity in various states to distinguish bonding types and predict properties like hardness.

Question 16

A solid is made of atoms arranged in layers. The solid is soft and slippery, and it conducts electricity along the planes of the layers. Which bonding description best explains these properties?

Covalent bonds within layers and weak forces between layers (correct answer)
Metal cations in a sea of localized electrons that cannot move
Neutral molecules held together by hydrogen bonding between molecules
Ions held by strong electrostatic attractions in a 3D lattice
Discrete molecules held together only by covalent bonds between molecules

Explanation: This question tests the skill of linking bonding models to macroscopic properties of solids. The correct answer is C, covalent bonds within layers and weak forces between layers, because the layered structure with strong covalent bonds in planes allows conductivity along layers via delocalized electrons, as in graphite, while weak van der Waals forces between layers explain the soft, slippery nature. This bonding permits sliding of layers without breaking strong bonds. The directional conductivity aligns with the anisotropic structure. A tempting distractor is D, metal cations in a sea of localized electrons that cannot move, which is incorrect as it misapplies metallic bonding to layered structures; the misconception is assuming all conductive solids have fully delocalized electrons like metals. Examine anisotropy in properties like conductivity and texture to infer layered bonding in solids.

Question 17

A student is told that a solid is metallic. Which set of observations would be least consistent with that classification?

Lustrous appearance and high electrical conductivity as a solid
Malleable behavior and moderate to high melting point
Nonconductive as a solid and brittle when struck (correct answer)
Conductive as a solid and conductive when molten
Can be drawn into a wire and conducts heat well

Explanation: This question tests the skill of evaluating consistency of properties with metallic classification. The correct answer is C, nonconductive as a solid and brittle when struck, because metals are defined by solid-state conductivity via delocalized electrons and malleability from sliding cation layers, so nonconductivity and brittleness contradict metallic nature. Other choices like luster, malleability, and conductivity align with metals. This set is least fitting. A tempting distractor is D, conductive as a solid and conductive when molten, which is actually consistent with metals; the misconception is thinking molten conductivity is unique to non-metals. Verify classifications by checking if all observed properties align with the defining traits of the solid type.

Question 18

Two solids are compared at $25^\circ\text{C}$ . Solid X is brittle, has a high melting point, and is nonconductive as a solid. Solid Y is malleable, lustrous, and conductive as a solid. Which pairing of solid types is most consistent with these observations?

X: molecular; Y: covalent network
X: ionic; Y: metallic (correct answer)
X: metallic; Y: ionic
X: covalent network; Y: molecular
X: molecular; Y: ionic

Explanation: This question tests the skill of comparing and classifying different types of solids based on observed properties. The correct answer is B, X: ionic; Y: metallic, because Solid X's brittleness, high melting point, and nonconductivity as a solid are typical of ionic lattices with fixed ions and strong electrostatic forces. Solid Y's malleability, luster, and solid-state conductivity indicate metallic bonding with delocalized electrons allowing deformation and charge flow. These properties distinctly separate the two types. A tempting distractor is C, X: metallic; Y: ionic, which reverses the classifications incorrectly; the misconception is swapping brittleness for malleability between ionic and metallic solids. Systematically list key properties for each solid type to match observations accurately.

Question 19

A student compares two molecular solids of similar molar mass: Solid P is nonpolar, and Solid Q is polar and capable of hydrogen bonding. Both are nonconductive. Which trend is most likely correct?

Solid P has the higher melting point because nonpolar molecules form stronger bonds
Solid Q has the higher melting point because stronger intermolecular forces are present (correct answer)
Solid P has the higher melting point because it forms an ionic lattice
Solid Q has the lower melting point because hydrogen bonding weakens attractions
Both have identical melting points because all molecular solids melt at low temperatures

Explanation: This question tests the skill of predicting melting point trends based on intermolecular forces in molecular solids. The correct answer is B, Solid Q has the higher melting point because stronger intermolecular forces are present, as hydrogen bonding in the polar Solid Q provides stronger attractions than London dispersion in nonpolar Solid P, requiring more energy to melt despite similar molar masses. Both are nonconductive due to lack of charge carriers. This explains the difference in thermal stability. A tempting distractor is A, Solid P has the higher melting point because nonpolar molecules form stronger bonds, which is incorrect; the misconception is reversing the strength of hydrogen bonding versus dispersion forces. Assess intermolecular force types and strengths to forecast relative physical properties in molecular compounds.

Question 20

A solid sample is made of discrete neutral molecules held together primarily by London dispersion forces. It melts near room temperature and does not conduct electricity in either the solid or liquid state. Which description best matches its macroscopic properties?

Low melting point and nonconductive in both solid and liquid states (correct answer)
High melting point and conductive as a solid but not as a liquid
High melting point and conductive in both solid and liquid states
High melting point and nonconductive in both solid and liquid states
Low melting point and conductive only when melted

Explanation: This question tests the skill of identifying properties of molecular solids based on intermolecular forces. The correct answer is A, low melting point and nonconductive in both solid and liquid states, because the solid consists of discrete neutral molecules held by weak London dispersion forces, leading to low melting points as little energy is needed to separate molecules. Molecular solids do not conduct electricity in either state since there are no free charge carriers like ions or delocalized electrons. The description of melting near room temperature aligns with weak intermolecular forces typical of nonpolar molecular solids. A tempting distractor is E, low melting point and conductive only when melted, which is incorrect as it mistakes molecular solids for ionic ones where melting frees ions; the misconception is assuming conductivity arises from melting alone without charge carriers. When analyzing solids, distinguish molecular types by checking for conductivity and relating melting point to intermolecular force strength.