AP Chemistry Flashcards: Properties Of Solids

What this deck covers

This deck focuses on Properties Of Solids, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: What are the primary types of crystalline solids?

Answer: Ionic, molecular, covalent network, and metallic. Based on the bonding and structure of constituent particles.

Flashcard 2: Identify the type of solid that diamond is an example of.

Answer: Covalent network solid. Carbon atoms form strong covalent bonds in all three dimensions.

Flashcard 3: State the typical electrical conductivity of molecular solids.

Answer: Generally poor conductors. No mobile charge carriers in the solid state prevents current flow.

Flashcard 4: What is the coordination number for a face-centered cubic lattice?

Answer:

1. Each atom contacts twelve others in this close-packed structure.

Flashcard 5: What type of solid is common table salt an example of?

Answer: Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.

Flashcard 6: Identify the structural characteristic of metallic solids.

Answer: Metal cations surrounded by a sea of delocalized electrons. Electron sea model explains metallic properties like conductivity and malleability.

Flashcard 7: Identify the crystal system where all edges are equal and angles are 90°.

Answer: Cubic system. Three equal axes at right angles define this symmetric crystal system.

Flashcard 8: What is the distinguishing feature of amorphous solids regarding melting?

Answer: No sharp melting point. Random structure softens gradually over a temperature range.

Flashcard 9: Which type of solid has variable hardness and melting points?

Answer: Metallic solids. Properties depend on specific metal and bonding strength variations.

Flashcard 10: What type of solid is common table salt an example of?

Answer: Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.

Flashcard 11: Identify the type of solid that diamond is an example of.

Answer: Covalent network solid. Carbon atoms form strong covalent bonds in all three dimensions.

Flashcard 12: Identify the type of solid with directional covalent bonds.

Answer: Covalent network solids. Bond angles and lengths are fixed, creating rigid structures.

Flashcard 13: What is the feature that distinguishes a crystalline solid at the atomic level?

Answer: Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.

Flashcard 14: What is a common property of covalent network solids regarding melting points?

Answer: Extremely high melting points. Strong covalent bonds throughout require enormous energy to break.

Flashcard 15: Identify the type of solid with directional covalent bonds.

Answer: Covalent network solids. Bond angles and lengths are fixed, creating rigid structures.

Flashcard 16: What is the general solubility of ionic solids in water?

Answer: Generally soluble, depending on specific ions. Polar water molecules interact favorably with separated ions.

Flashcard 17: What kind of solid is dry ice an example of?

Answer: Molecular solid. Solid $CO_2$ held together by weak van der Waals forces.

Flashcard 18: Identify the crystal system where all edges are equal and angles are 90°.

Answer: Cubic system. Three equal axes at right angles define this symmetric crystal system.

Flashcard 19: State one property of solids that distinguishes them from liquids.

Answer: Definite shape. Strong intermolecular forces maintain rigid three-dimensional structure.

Flashcard 20: What is the packing efficiency of a face-centered cubic lattice?

Answer: 74%. Close-packed spheres achieve maximum space utilization in this arrangement.

Flashcard 21: Identify the characteristic property of ionic solids.

Answer: High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.

Flashcard 22: Which type of solid is ice classified as?

Answer: Molecular solid. Water molecules held by hydrogen bonds in hexagonal crystal structure.

Flashcard 23: Identify the crystal system where all edges are equal and angles are 90°.

Answer: Cubic system. Three equal axes at right angles define this symmetric crystal system.

Flashcard 24: What is the primary force holding ionic solids together?

Answer: Electrostatic attractions. Coulombic forces between oppositely charged ions create strong attractions.

Flashcard 25: Identify the characteristic property of ionic solids.

Answer: High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.

Flashcard 26: Which type of solid is characterized by discrete molecules held by intermolecular forces?

Answer: Molecular solids. Van der Waals forces, hydrogen bonds, or dipole interactions hold molecules together.

Flashcard 27: Identify the crystal system where all edges are equal and angles are 90°.

Answer: Cubic system. Three equal axes at right angles define this symmetric crystal system.

Flashcard 28: Identify the structure that graphite is an example of.

Answer: Covalent network solid. Layered structure with delocalized electrons between carbon sheets.

Flashcard 29: What is the distinguishing feature of amorphous solids regarding melting?

Answer: No sharp melting point. Random structure softens gradually over a temperature range.

Flashcard 30: Which type of solid can be reshaped by applying force?

Answer: Metallic solids. Delocalized electrons allow layers to slide past each other without breaking bonds.

Flashcard 31: State the type of bonding present in covalent network solids.

Answer: Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.

Flashcard 32: State the simplest repeating unit in a crystal lattice.

Answer: Unit cell. Smallest portion that shows the complete crystal pattern when repeated.

Flashcard 33: Which property differentiates crystalline from amorphous solids?

Answer: Regular repeating pattern in crystalline solids. Long-range order creates distinct X-ray diffraction patterns in crystals.

Flashcard 34: State the unit cell type for a hexagonal close-packed structure.

Answer: Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.

Flashcard 35: Which property is common in amorphous solids?

Answer: Lack of long-range order. Random atomic arrangement distinguishes them from ordered crystalline structures.

Flashcard 36: What is a distinguishing feature of metallic solids?

Answer: Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.

Flashcard 37: State the unit cell type for a hexagonal close-packed structure.

Answer: Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.

Flashcard 38: Identify the type of solid with the highest thermal conductivity.

Answer: Metallic solids. Mobile electrons efficiently transfer thermal energy through the structure.

Flashcard 39: What is the feature that distinguishes a crystalline solid at the atomic level?

Answer: Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.

Flashcard 40: State the type of bonding present in covalent network solids.

Answer: Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.

Flashcard 41: State the coordination number for a body-centered cubic lattice.

Answer:

1. Each atom touches eight nearest neighbors in this packing arrangement.

Flashcard 42: What is the feature that distinguishes a crystalline solid at the atomic level?

Answer: Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.

Flashcard 43: What is the typical hardness of covalent network solids?

Answer: Very hard. Extensive covalent bonding throughout makes them extremely resistant to deformation.

Flashcard 44: What type of solid is common table salt an example of?

Answer: Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.

Flashcard 45: What is a distinguishing feature of metallic solids?

Answer: Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.

Flashcard 46: What type of crystal lattice does sodium chloride form?

Answer: Cubic lattice. Each ion has six nearest neighbors in this common ionic structure.

Flashcard 47: What is a distinguishing feature of metallic solids?

Answer: Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.

Flashcard 48: State the unit cell type for a hexagonal close-packed structure.

Answer: Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.

Flashcard 49: What type of solid is common table salt an example of?

Answer: Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.

Flashcard 50: State the packing efficiency of a simple cubic lattice.

Answer: 52%. Inefficient packing with spheres touching only along cube edges.

Flashcard 51: State the type of bonding present in covalent network solids.

Answer: Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.

Flashcard 52: Identify the type of solid that exhibits the highest melting points.

Answer: Covalent network solids. Extensive covalent bonding requires the most energy to break.

Flashcard 53: What is the distinguishing feature of amorphous solids regarding melting?

Answer: No sharp melting point. Random structure softens gradually over a temperature range.

Flashcard 54: What is the primary structural feature of graphite?

Answer: Layers of carbon atoms in a hexagonal arrangement. Planar layers allow electrons to move freely within sheets.

Flashcard 55: Identify the characteristic property of ionic solids.

Answer: High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.

Flashcard 56: Identify the structural characteristic of metallic solids.

Answer: Metal cations surrounded by a sea of delocalized electrons. Electron sea model explains metallic properties like conductivity and malleability.

Flashcard 57: What is the typical electrical conductivity of ionic solids?

Answer: Conductive when molten or dissolved. Ions become mobile charge carriers when lattice breaks down.

Flashcard 58: Identify the characteristic property of ionic solids.

Answer: High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.

Flashcard 59: What is a distinguishing feature of metallic solids?

Answer: Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.

Flashcard 60: State the unit cell type for a hexagonal close-packed structure.

Answer: Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.

Flashcard 61: What type of solid is glass considered to be?

Answer: Amorphous solid. Lacks ordered crystalline structure with random atomic arrangement.

Flashcard 62: What is the distinguishing feature of amorphous solids regarding melting?

Answer: No sharp melting point. Random structure softens gradually over a temperature range.

Flashcard 63: Which type of solid is characterized by discrete molecules held by intermolecular forces?

Answer: Molecular solids. Van der Waals forces, hydrogen bonds, or dipole interactions hold molecules together.

Flashcard 64: Identify the type of solid that is typically soft and has low melting points.

Answer: Molecular solids. Weak intermolecular forces make them easily deformable and meltable.

Flashcard 65: What defines the anisotropic nature of crystalline solids?

Answer: Different properties in different directions. Ordered atomic arrangement creates directional variation in physical properties.

Flashcard 66: State the type of bonding present in covalent network solids.

Answer: Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.

Flashcard 67: What is the feature that distinguishes a crystalline solid at the atomic level?

Answer: Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.

Flashcard 68: What is the coordination number in a simple cubic lattice?

Answer:

1. Each sphere touches six others along the cube faces and edges.