Properties of Solids - AP Chemistry

What are the primary types of crystalline solids?

Ionic, molecular, covalent network, and metallic. Based on the bonding and structure of constituent particles.
Identify the type of solid that diamond is an example of.

Covalent network solid. Carbon atoms form strong covalent bonds in all three dimensions.
State the typical electrical conductivity of molecular solids.

Generally poor conductors. No mobile charge carriers in the solid state prevents current flow.
What is the coordination number for a face-centered cubic lattice?

12. Each atom contacts twelve others in this close-packed structure.
What type of solid is common table salt an example of?

Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.
Identify the structural characteristic of metallic solids.

Metal cations surrounded by a sea of delocalized electrons. Electron sea model explains metallic properties like conductivity and malleability.
What is the distinguishing feature of amorphous solids regarding melting?

No sharp melting point. Random structure softens gradually over a temperature range.
Which type of solid has variable hardness and melting points?

Metallic solids. Properties depend on specific metal and bonding strength variations.
What type of solid is common table salt an example of?

Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.
What is the feature that distinguishes a crystalline solid at the atomic level?

Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.
What is a common property of covalent network solids regarding melting points?

Extremely high melting points. Strong covalent bonds throughout require enormous energy to break.
Identify the type of solid with directional covalent bonds.

Covalent network solids. Bond angles and lengths are fixed, creating rigid structures.
What is the general solubility of ionic solids in water?

Generally soluble, depending on specific ions. Polar water molecules interact favorably with separated ions.
What kind of solid is dry ice an example of?

Molecular solid. Solid $CO_2$ held together by weak van der Waals forces.
Identify the crystal system where all edges are equal and angles are 90°.

Cubic system. Three equal axes at right angles define this symmetric crystal system.
State one property of solids that distinguishes them from liquids.

Definite shape. Strong intermolecular forces maintain rigid three-dimensional structure.
What is the packing efficiency of a face-centered cubic lattice?

74%. Close-packed spheres achieve maximum space utilization in this arrangement.
Identify the characteristic property of ionic solids.

High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.
Which type of solid is ice classified as?

Molecular solid. Water molecules held by hydrogen bonds in hexagonal crystal structure.
Identify the crystal system where all edges are equal and angles are 90°.

Cubic system. Three equal axes at right angles define this symmetric crystal system.
What is the primary force holding ionic solids together?

Electrostatic attractions. Coulombic forces between oppositely charged ions create strong attractions.
Identify the characteristic property of ionic solids.

High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.
Identify the crystal system where all edges are equal and angles are 90°.

Cubic system. Three equal axes at right angles define this symmetric crystal system.
Identify the structure that graphite is an example of.

Covalent network solid. Layered structure with delocalized electrons between carbon sheets.
What is the distinguishing feature of amorphous solids regarding melting?

No sharp melting point. Random structure softens gradually over a temperature range.
Which type of solid can be reshaped by applying force?

Metallic solids. Delocalized electrons allow layers to slide past each other without breaking bonds.
State the type of bonding present in covalent network solids.

Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.
State the simplest repeating unit in a crystal lattice.

Unit cell. Smallest portion that shows the complete crystal pattern when repeated.
Which property differentiates crystalline from amorphous solids?

Regular repeating pattern in crystalline solids. Long-range order creates distinct X-ray diffraction patterns in crystals.
State the unit cell type for a hexagonal close-packed structure.

Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.
Which property is common in amorphous solids?

Lack of long-range order. Random atomic arrangement distinguishes them from ordered crystalline structures.
What is a distinguishing feature of metallic solids?

Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.
State the unit cell type for a hexagonal close-packed structure.

Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.
Identify the type of solid with the highest thermal conductivity.

Metallic solids. Mobile electrons efficiently transfer thermal energy through the structure.
State the type of bonding present in covalent network solids.

Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.
State the coordination number for a body-centered cubic lattice.

8. Each atom touches eight nearest neighbors in this packing arrangement.
What is the feature that distinguishes a crystalline solid at the atomic level?

Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.
What is the typical hardness of covalent network solids?

Very hard. Extensive covalent bonding throughout makes them extremely resistant to deformation.
What type of crystal lattice does sodium chloride form?

Cubic lattice. Each ion has six nearest neighbors in this common ionic structure.
What is a distinguishing feature of metallic solids?

Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.
State the unit cell type for a hexagonal close-packed structure.

Hexagonal. Six-fold symmetry with layers stacked in ABAB pattern.
What type of solid is common table salt an example of?

Ionic solid. Sodium and chloride ions held together by strong electrostatic forces.
State the packing efficiency of a simple cubic lattice.

52%. Inefficient packing with spheres touching only along cube edges.
Identify the type of solid that exhibits the highest melting points.

Covalent network solids. Extensive covalent bonding requires the most energy to break.
What is the distinguishing feature of amorphous solids regarding melting?

No sharp melting point. Random structure softens gradually over a temperature range.
What is the primary structural feature of graphite?

Layers of carbon atoms in a hexagonal arrangement. Planar layers allow electrons to move freely within sheets.
Identify the characteristic property of ionic solids.

High melting points and electrical conductivity in molten state. Strong ionic bonds require high energy to break and ions become mobile when melted.
What is the typical electrical conductivity of ionic solids?

Conductive when molten or dissolved. Ions become mobile charge carriers when lattice breaks down.
What is a distinguishing feature of metallic solids?

Good electrical and thermal conductivity. Mobile electron sea allows efficient heat and electric current transfer.
What type of solid is glass considered to be?

Amorphous solid. Lacks ordered crystalline structure with random atomic arrangement.
Which type of solid is characterized by discrete molecules held by intermolecular forces?

Molecular solids. Van der Waals forces, hydrogen bonds, or dipole interactions hold molecules together.
Identify the type of solid that is typically soft and has low melting points.

Molecular solids. Weak intermolecular forces make them easily deformable and meltable.
What defines the anisotropic nature of crystalline solids?

Different properties in different directions. Ordered atomic arrangement creates directional variation in physical properties.
State the type of bonding present in covalent network solids.

Covalent bonding throughout the structure. Extended network of covalent bonds creates very strong structures.
What is the feature that distinguishes a crystalline solid at the atomic level?

Ordered atomic arrangement. Repeating three-dimensional pattern defines crystal structure.
What is the coordination number in a simple cubic lattice?

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

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