Metallic & Ionic Solids. Crystal Lattices. Properties of Solids. Network Solids. Types of Solids. Chapter 13 Solids. Chapter 13

Size: px
Start display at page:

Download "Metallic & Ionic Solids. Crystal Lattices. Properties of Solids. Network Solids. Types of Solids. Chapter 13 Solids. Chapter 13"

Transcription

1 1 Metallic & Ionic Solids Chapter 13 The Chemistry of Solids Jeffrey Mack California State University, Sacramento Crystal Lattices Properties of Solids Regular 3-D arrangements of equivalent LATTICE POINTS in space. Lattice points define UNIT CELLS Unit cells are the smallest repeating internal unit that has the symmetry characteristic of the solid. 1. Molecules, atoms or ions locked into a CRYSTAL LATTICE. 2. Particles are CLOSE together. 3. These exhibit strong intermolecular forces 4. Highly ordered, rigid, incompressible ZnS, zinc sulfide Types of Solids Network Solids Type: Examples: Forces: Ionic Compounds NaCl, BaCl 2, ZnS Ion-Ion (ionic bonding) Diamond Metals Fr, Al Metallic Molecular Ice, I 2, C 12 H 22 O 11 Dipole-Dipole ot Induced Dipoles Network Amorphous Diamond, Graphite Glass, Coal Extended Covalent bonds Covalent; directional electron-pair bonds Graphite

2 2 Cubic Unit Cells Cubic Unit Cells There are 7 basic crystal systems, but we will only be concerned with CUBIC form here. All angles are 90 degrees All sides equal length 1/8 of each atom on a corner is within the cube 1/2 of each atom on a face is within the cube 1/4 of each atom on a side is within the cube Primitive cubic (PC) Bodycentered cubic (BCC) Facecentered cubic (FCC) Cubic Unit Cells Unit Cells for Metals Simple Cubic Unit Cell Atom Packing in Unit Cells Assumes atoms are hard spheres and that crystals are built by PACKING these spheres as efficiently as possible. Each atom is at a corner of a unit cell and is shared among 8 unit cells. Each edge is shared with 4 cells Each face is part of two cells.

3 Atom Packing in Unit Cells Crystal Lattices Packing of Atoms or Ions 3 FCC is more efficient than either BC or PC. Leads to layers of atoms. Crystal Lattices Packing of Atoms or Ions Atomic Radii Packing of C 60 molecules. They are arranged at the lattice points of a FCC lattice. Calcium metal crystallizes in a face-centered cubic unit cell. The density of the solid is 1.54 g/cm 3. What is the radius of a calcium atom? Calcium metal crystallizes in a face-centered cubic unit cell. The density of the solid is 1.54 g/cm 3. What is the radius of a calcium atom? Unit cell volume: g 1 cm 3 1 mol Ca 23 4 Ca atoms = cm 3 1 mol Ca 1.54 g atoms unit cell

4 4 Calcium metal crystallizes in a face-centered cubic unit cell. The density of the solid is 1.54 g/cm 3. What is the radius of a calcium atom? Unit cell volume: g 1 cm 3 1 mol Ca 23 4 Ca atoms = cm 3 1 mol Ca 1.54 g atoms unit cell Unit cell edge length: 22 V = cm = (edge length) Calcium metal crystallizes in a face-centered cubic unit cell. The density of the solid is 1.54 g/cm 3. What is the radius of a calcium atom? Unit cell volume: g 1 cm 3 1 mol Ca 23 4 Ca atoms = cm 3 1 mol Ca 1.54 g atoms unit cell Unit cell edge length: 22 V = cm = (edge length) 3 22 edge length = cm = cm 3 22 edge length = cm = cm face diagonal = 4 radius = 2 edge length radius = 8 2 ( cm) 8 = cm = 197 pm 4 Number of Atoms Per Unit Cell Unit Cell Type PC 1 BCC 2 FCC 4 Net Number Atoms Atom Sharing at Cube Faces & Corners There is 1/8 th of an atom shared in corner. There is 1/2 shared at each face Two Views of CsCl Lattice can be Primitive Cubic lattice of Cl - with Cs + in hole OR a Primitive Cubic of Cs + with Cl - in hole Either arrangement leads to formula of 1 Cs + and 1 Cl - per unit cell Rutile, TiO 2, crystallizes in a structure characteristic of many other ionic compounds. How many formula units of TiO 2 are in the unit cell illustrated here? (The oxide ions marked by an x are wholly within the cell; the others are in the cell faces.) 8 corner Ti 1/8 = 1 Ti 4 face O ½ = 2 O 1 internal Ti = 1 Ti 2 internal O = 2 O = 2 Ti total = 4 O total There are two TiO 2 units per unit cell.

5 5 Common Ionic Solids Titanium dioxide, TiO 2 There are 2 net Ti 4+ ions and 4 net O 2- ions per unit cell. Structure & Formulas of Ionic Compounds Salts with formula MX can have Primitive Cubic structure. Salts with formula MX 2 or M 2 X cannot. The Sodium Chloride Lattice NaCl Construction Many common salts have Face Centered Cubic arrangements of anions with cations in octahedral holes. Example: NaCl FCC lattice of anions: 4 Cl per unit cell Na + in octahedral hole: 1 Na + at center 1 Na + (center) + (12 edges 1/4 Na + per edge) = 4 Na + per unit cell FCC lattice of Cl - with Na + in holes Na + in octahedral holes Octahedral Holes FCC Lattice The Sodium Chloride Lattice Na + ions are in OCTAHEDRAL holes in a face-centered cubic lattice of Cl ions.

6 6 Comparing NaCl with CsCl Common Ionic Solids Even though their formulas have one cation and one anion, the lattices of CsCl and NaCl are different. The different lattices arise from the fact that a Cs + ion is much larger than a Na + ion. Zinc sulfide, ZnS The S 2 ions are in facecentered cubic (FCC) structure. 1/8 of each corner S 2- ½ of each face S 2- Each Zn 2+ is in a hole between S 2-. The holes are tetrahedral 1 atom in ½ of the holes. Zn = (4 1) = 4 S = (1/8 8) + (½ 6) = 4 Zn:S = 4:4 = 1:1 Therefore the formula is ZnS Common Ionic Compounds Fluorite or CaF 2 FCC lattice of Ca 2+ ions This gives 4 net Ca 2+ ions. F ions in all 8 tetrahedral holes. This gives 8 net F ions. Bonding in Metals & Semiconductors Molecular orbital (MO) theory was introduced in Chapter 9 to rationalize covalent bonding in molecules MO theory can also be used to describe metallic bonding. Metals can be thought of as a supermolecule. Metallic bonding is described as delocalized: The electrons are associated with all the atoms in the crystal and not with specific bonded atoms. This theory of metallic bonding is called band theory. Bonding in Metals & Semiconductors Band Theory An energy-level diagram shows the bonding and antibonding molecular orbitals blending together into a band of molecular orbitals. Molecular orbitals are constructed from the valence orbitals on each atom and are delocalized over all the atoms. When sufficient energy is added, electrons are excited to the conduction band. (Thermal energy provides this for metals)

7 7 Band Theory Classifications of Solids Solids can be classified on the basis of the bonds that hold the atoms or molecules together. This approach categorizes solids as either: Molecular orbitals are constructed from the valence orbitals on each atom and are delocalized over all the atoms. When sufficient energy is added, electrons are excited to the conduction band. (Thermal energy provides this for metals) molecular Network (covalent) ionic metallic Molecular Solids Molecular solids are characterized by relatively strong intramolecular bonds between the atoms that form the molecules The intermolecular forces between these molecules are much weaker than the bonds. Because the intermolecular forces are relatively weak, molecular solids are often soft substances with low melting points. Examples: I 2 (s), sugar (C 12 H 22 O 11 ) and Dry Ice, CO 2 (s) Network (Covalent) Solids In Network solids, conventional chemical bonds hold the chemical subunits together. The bonding between chemical subunits is identical to that within the subunits resulting in a continuous network of chemical bonds. Two common examples of network solids are diamond (a form of pure carbon) and quartz (silicon dioxide). In quartz one cannot detect discrete SiO 2 molecules. Instead the solid is an extended threedimensional network of...-si-o-si-o-... bonding. Ionic Solids Ionic solids are salts, such as NaCl, that are held together by the strong force of attraction between ions of opposite charge. q( + ) q( -) F» 2 r Because this force of attraction depends on the square of the distance between the positive and negative charges, the strength of an ionic bond depends on the radii of the ions that form the solid. As these ions become larger, the bond becomes weaker. Metallic Solids In Molecular, ionic, and covalent solids the electrons in these are localized within the bonding atoms. Metal atoms however don't have enough electrons to fill their valence shells by sharing electrons with their immediate neighbors. Electrons in the valence shell are therefore shared by many atoms, instead of just two. In effect, the valence electrons are delocalized over many metal atoms. Because these electrons aren't tightly bound to individual atoms, they are free to migrate through the metal. As a result, metals are good conductors of electricity.

8 8 Bonding in Ionic Compounds: Lattice Energy The energy of an ion pair (cation/anion) is described by Coulombs law: U ion pair ( n + e - )( n - e + ) = C d n + = cation charge, n = anion charge d = distance between ion centers lattice U is the energy of formation of one mole of the solid crystaline compound from its ions in the gas phase. + - M ( g) + X ( g) MX( s) The Lattice Energy of a salt is dependant upon the charge and size of the ions. U ion pair Lattice Energy ( n + e - )( n - e + ) = C d Lattice Energy Calculation of lattice energy via the Born Haber cycle, an application of Hess s law. Solution: Approach this problem using Hess s Law. You need to find the enthalpy for the reaction: Start by drawing the Born-Haber cycle for the reaction: Li(s) + ½ F 2 (g) LiF(s)

9 9 Start by drawing the Born-Haber cycle for the reaction: Li + (g) Li(g) IE sub H + EA D o F (g) F(g) Li(s) + ½ F 2 (g) LiF(s) Using Hess s Law, the enthalpy of formation is found by: Li + (g) + F (g) Li(g) IE sub H EA D o F(g) Li(s) + ½ F 2 (g) LiF(s) f H o = sub H + I 1 + D o + EA + lattice U f H o = sub H + IE + D o + EA + lattice U Li(s) Li(g) sub H = kj/mol Li(g) Li + (g) + e IE = kj/mol ½ F 2 (g) F(g) D o = kj/mol F(g) + e F (g) EA = kj/mol Li + (g) + F (g) LiF(s) lattice U = 1037 kj/mol f H = = 607 kj/mol Phase Changes Involving Solids Melting: Conversion of Solid into Liquid The melting point of a solid is the temperature at which the lattice collapses into a liquid. Like any phase change, melting requires energy, called the enthalpy of fusion. Energy absorbed as heat on melting = enthalpy of fusion fusion H (kj/mol) Energy evolved as heat on freezing = enthalpy of crystallization fusion H (kj/mol) Enthalpies of fusion can range from just a few thousand joules per mole to many thousands of joules per mole. Enthalpies of Fusion Are a Function of Intermolecular Forces Phase Changes Involving Solids Sublimation: Conversion of Solid into Vapor Molecules can escape directly from the solid to the gas phase by sublimation Solid Gas Energy required as heat = sublimation H Sublimation, like fusion and evaporation, is an endothermic process. The energy required as heat is called the enthalpy of sublimation.

10 10 Sublimation Sublimation entails the conversion of a solid directly to its vapor. Here, iodine (I 2 ) sublimes when warmed. Transitions Between Phases: Phase Diagrams Phase diagrams are used to illustrate the relationship between phases of matter and the pressure and temperature. Phase Diagram for Water Phase Equilibria Water Liquid phase Solid-liquid Gas-Liquid Solid phase Gas phase Gas-Solid Triple Point Water Phases Diagrams: Water At the TRIPLE POINT all three phases are in equilibrium. T( C) P(mmHg) Normal boil point (at 1atm): Normal freeze point (at 1atm): Triple point:

11 11 Phases Diagrams: Water Water has its maximum density at 4 C, in the liquid phase. Most substances have a maximum density in the solid phase. Hydrogen bonding accounts for water s deviation from normal behavior. Phases Diagram: Water At constant temp, an increase in pressure can bring about a phase change from solid to liquid! Phases Diagrams: Water At constant temp, an increase in pressure can bring about a phase change from solid to liquid! This occurs when the blade of an ice skate runs on the ice. Ice skaters actually ride on a film of water, not the ice! CO 2 Phase Diagram Notice the CO 2 has a forward slope of the solid/liquid boundary. This is seen because CO 2 does not exhibit hydrogen bonding. CO 2 Phases Separate phases Increasing pressure More pressure Supercritical CO 2

Chapter 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids

Chapter 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids Chapter 12 Insert picture from First page of chapter Intermolecular Forces and the Physical Properties of Liquids and Solids Copyright McGraw-Hill 2009 1 12.1 Intermolecular Forces Intermolecular forces

More information

Properties of Liquids and Solids. Vaporization of Liquids. Vaporization of Liquids. Aims:

Properties of Liquids and Solids. Vaporization of Liquids. Vaporization of Liquids. Aims: Properties of Liquids and Solids Petrucci, Harwood and Herring: Chapter 13 Aims: To use the ideas of intermolecular forces to: Explain the properties of liquids using intermolecular forces Understand the

More information

Properties of Liquids and Solids. Vaporization of Liquids

Properties of Liquids and Solids. Vaporization of Liquids Properties of Liquids and Solids Petrucci, Harwood and Herring: Chapter 13 Aims: To use the ideas of intermolecular forces to: Explain the properties of liquids using intermolecular forces Understand the

More information

Chapter 11. Intermolecular Forces and Liquids & Solids

Chapter 11. Intermolecular Forces and Liquids & Solids Chapter 11 Intermolecular Forces and Liquids & Solids The Kinetic Molecular Theory of Liquids & Solids Gases vs. Liquids & Solids difference is distance between molecules Liquids Molecules close together;

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chapter 11 Intermolecular Forces, Liquids, and Solids Dissolution of an ionic compound States of Matter The fundamental difference between states of matter is the distance between particles. States of

More information

CHAPTER ELEVEN KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS

CHAPTER ELEVEN KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS CHAPTER ELEVEN AND LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS Differences between condensed states and gases? KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS Phase Homogeneous part

More information

Chapter 11: Intermolecular Forces. Lecture Outline

Chapter 11: Intermolecular Forces. Lecture Outline Intermolecular Forces, Liquids, and Solids 1 Chapter 11: Intermolecular Forces Lecture Outline 11.1 A Molecular Comparison of Gases, Liquids and Solids Physical properties of substances are understood

More information

Solids. properties & structure

Solids. properties & structure Solids properties & structure Determining Crystal Structure crystalline solids have a very regular geometric arrangement of their particles the arrangement of the particles and distances between them is

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 A phase is a homogeneous part of the system in contact

More information

Diamond. There are four types of solid: -Hard Structure - Tetrahedral atomic arrangement. What hybrid state do you think the carbon has?

Diamond. There are four types of solid: -Hard Structure - Tetrahedral atomic arrangement. What hybrid state do you think the carbon has? Bonding in Solids Bonding in Solids There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network - very hard with

More information

Intermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for

Intermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw Hill Companies, Inc. Permission required for 1 A phase is a homogeneous part of the system in contact with other parts of the

More information

There are four types of solid:

There are four types of solid: Bonding in Solids There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network - very hard with very high melting

More information

Chapter 12 INTERMOLECULAR FORCES. Covalent Radius and van der Waals Radius. Intraand. Intermolecular Forces. ½ the distance of non-bonded

Chapter 12 INTERMOLECULAR FORCES. Covalent Radius and van der Waals Radius. Intraand. Intermolecular Forces. ½ the distance of non-bonded Chapter 2 INTERMOLECULAR FORCES Intraand Intermolecular Forces Covalent Radius and van der Waals Radius ½ the distance of bonded ½ the distance of non-bonded Dipole Dipole Interactions Covalent and van

More information

The Solid State. Phase diagrams Crystals and symmetry Unit cells and packing Types of solid

The Solid State. Phase diagrams Crystals and symmetry Unit cells and packing Types of solid The Solid State Phase diagrams Crystals and symmetry Unit cells and packing Types of solid Learning objectives Apply phase diagrams to prediction of phase behaviour Describe distinguishing features of

More information

SOLID STATE CHEMISTRY

SOLID STATE CHEMISTRY SOLID STATE CHEMISTRY Crystal Structure Solids are divided into 2 categories: I. Crystalline possesses rigid and long-range order; its atoms, molecules or ions occupy specific positions, e.g. ice II. Amorphous

More information

Solids. Adapted from a presentation by Dr. Schroeder, Wayne State University

Solids. Adapted from a presentation by Dr. Schroeder, Wayne State University Solids Adapted from a presentation by Dr. Schroeder, Wayne State University Properties of Solids Definite shape, definite volume Particles are CLOSE together, so Attractive forces (bonds or IMF s) are

More information

Some Properties of Solids, Liquids, and Gases

Some Properties of Solids, Liquids, and Gases AP Chemistry: Intermolecular Forces, Liquids, and Solids Sec 1. A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These are forces

More information

- intermolecular forces forces that exist between molecules

- intermolecular forces forces that exist between molecules Chapter 11: Intermolecular Forces, Liquids, and Solids - intermolecular forces forces that exist between molecules 11.1 A Molecular Comparison of Liquids and Solids - gases - average kinetic energy of

More information

Ch 11: Intermolecular Forces, Liquids, and Solids

Ch 11: Intermolecular Forces, Liquids, and Solids AP Chemistry: Intermolecular Forces, Liquids, and Solids Lecture Outline 11.1 A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A phase is a homogeneous part of the system in contact

More information

Some Properties of Solids, Liquids, and Gases

Some Properties of Solids, Liquids, and Gases AP Chemistry: Intermolecular Forces, Liquids, and Solids Lecture Outline 11.1 A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These

More information

CHEMISTRY The Molecular Nature of Matter and Change

CHEMISTRY The Molecular Nature of Matter and Change CHEMISTRY The Molecular Nature of Matter and Change Third Edition Chapter 12 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 11 INTERMOLECULAR FORCES

More information

Metallic and Ionic Structures and Bonding

Metallic and Ionic Structures and Bonding Metallic and Ionic Structures and Bonding Ionic compounds are formed between elements having an electronegativity difference of about 2.0 or greater. Simple ionic compounds are characterized by high melting

More information

Ionic Bonding. Chem

Ionic Bonding. Chem Whereas the term covalent implies sharing of electrons between atoms, the term ionic indicates that electrons are taken from one atom by another. The nature of ionic bonding is very different than that

More information

Chapter 10. Liquids and Solids

Chapter 10. Liquids and Solids Chapter 10 Liquids and Solids Chapter 10 Table of Contents 10.1 Intermolecular Forces 10.2 The Liquid State 10.3 An Introduction to Structures and Types of Solids 10.4 Structure and Bonding in Metals 10.5

More information

General Chemistry 202 CHM202 General Information. General Chemistry 202 CHM202 Policies. General Chemistry 202 CHM202 Laboratory Guidelines

General Chemistry 202 CHM202 General Information. General Chemistry 202 CHM202 Policies. General Chemistry 202 CHM202 Laboratory Guidelines General Chemistry 202 CHM202 General Information Instructor Meeting times and places Text and recommended materials Website Email Grading Schedule 1 General Chemistry 202 CHM202 Policies Equipment Instruction

More information

Liquids, Solids and Phase Changes

Liquids, Solids and Phase Changes Chapter 10 Liquids, Solids and Phase Changes Chapter 10 1 KMT of Liquids and Solids Gas molecules have little or no interactions. Molecules in the Liquid or solid state have significant interactions. Liquids

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids PowerPoint Lecture Presentation by J. David Robertson University of Missouri Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction

More information

4. Interpenetrating simple cubic

4. Interpenetrating simple cubic 2 1. The correct structure t of CsClCl crystal is 1. Simple cubic 2. Body centered cubic 3. Face centered cubic 4. Interpenetrating simple cubic If corner as well as the particle at the center are same

More information

Chapter 10: Liquids and Solids

Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids *Liquids and solids show many similarities and are strikingly different from their gaseous state. 10.1 Intermolecular Forces Intermolecular

More information

States of Matter; Liquids and Solids. Condensation - change of a gas to either the solid or liquid state

States of Matter; Liquids and Solids. Condensation - change of a gas to either the solid or liquid state States of Matter; Liquids and Solids Phase transitions - a change in substance from one state to another Melting - change from a solid to a liquid state Freezing - change of a liquid to the solid state

More information

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules?

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules? Polar Bonds and Polar Molecules Chapter 10 Liquids, Solids, and Phase Changes Draw Lewis Structures for CCl 4 and CH 3 Cl. What s the same? What s different? 1 Polar Covalent Bonds and Dipole Moments Bonds

More information

Atomic Arrangement. Primer Materials For Science Teaching Spring

Atomic Arrangement. Primer Materials For Science Teaching Spring Atomic Arrangement Primer Materials For Science Teaching Spring 2016 31.3.2015 Levels of atomic arrangements No order In gases, for example the atoms have no order, they are randomly distributed filling

More information

Liquids and Solids Chapter 10

Liquids and Solids Chapter 10 Liquids and Solids Chapter 10 Nov 15 9:56 AM Types of Solids Crystalline solids: Solids with highly regular arrangement of their components Amorphous solids: Solids with considerable disorder in their

More information

CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey

CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS Chemistry 1411 Joanna Sabey Forces Phase: homogeneous part of the system in contact with other parts of the system but separated from them by a

More information

CRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS

CRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS CRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS CRYSTAL STRUCTURE CRYSTALLINE AND AMORPHOUS SOLIDS Crystalline solids have an ordered arrangement. The long range order comes about from an underlying

More information

London Dispersion Forces (LDFs) Intermolecular Forces Attractions BETWEEN molecules. London Dispersion Forces (LDFs) London Dispersion Forces (LDFs)

London Dispersion Forces (LDFs) Intermolecular Forces Attractions BETWEEN molecules. London Dispersion Forces (LDFs) London Dispersion Forces (LDFs) LIQUIDS / SOLIDS / IMFs Intermolecular Forces (IMFs) Attractions BETWEEN molecules NOT within molecules NOT true bonds weaker attractions Represented by dashed lines Physical properties (melting points,

More information

Experiment 7: Understanding Crystal Structures

Experiment 7: Understanding Crystal Structures Experiment 7: Understanding Crystal Structures To do well in this laboratory experiment you need to be familiar with the concepts of lattice, crystal structure, unit cell, coordination number, the different

More information

Intermolecular Forces and Liquids and Solids Chapter 11

Intermolecular Forces and Liquids and Solids Chapter 11 Intermolecular Forces and Liquids and Solids Chapter 11 A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well defined boundary. Phases

More information

Chapter 10 Liquids and Solids. Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, , 113

Chapter 10 Liquids and Solids. Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, , 113 Chapter 10 Liquids and Solids Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, 104-106, 113 Recall: Intermolecular vs. Intramolecular Forces Intramolecular: bonds between

More information

ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes

ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes ก ก ก ก Mc-Graw Hill 1 Intermolecular Forces: Liquids, Solids, and Phase Changes 12.1 An Overview of Physical States and Phase Changes 12.2

More information

Intermolecular Forces and States of Matter AP Chemistry Lecture Outline

Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Name: Chemical properties are related only to chemical composition; physical properties are related to chemical composition AND the

More information

2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation).

2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation). A. Introduction. (Section 11.1) CHAPTER 11: STATES OF MATTER, LIQUIDS AND SOLIDS 1. Gases are easily treated mathematically because molecules behave independently. 2. As gas P increases and/or T is lowered,

More information

Atomic Arrangement. Primer in Materials Spring

Atomic Arrangement. Primer in Materials Spring Atomic Arrangement Primer in Materials Spring 2017 30.4.2017 1 Levels of atomic arrangements No order In gases, for example the atoms have no order, they are randomly distributed filling the volume to

More information

Chapter 10. Liquids and Solids

Chapter 10. Liquids and Solids Chapter 10 Liquids and Solids Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Metallic bonds Covalent bonds Ionic

More information

AP* Chapter 10. Liquids and Solids. Friday, November 22, 13

AP* Chapter 10. Liquids and Solids. Friday, November 22, 13 AP* Chapter 10 Liquids and Solids AP Learning Objectives LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses

More information

UNIT-1 SOLID STATE. Ans. Gallium (Ga) is a silvery white metal, liquid at room temp. It expands by 3.1% on solidifica-tion.

UNIT-1 SOLID STATE. Ans. Gallium (Ga) is a silvery white metal, liquid at room temp. It expands by 3.1% on solidifica-tion. UNIT-1 SOLID STATE 1 MARK QUESTIONS Q. 1. Name a liquefied metal which expands on solidification. Ans. Gallium (Ga) is a silvery white metal, liquid at room temp. It expands by 3.1% on solidifica-tion.

More information

Intermolecular Forces, Liquids, Solids. IM Forces and Physical Properties

Intermolecular Forces, Liquids, Solids. IM Forces and Physical Properties Intermolecular Forces, Liquids, Solids Interactions Between Molecules: What does it take to separate two (or more) molecules from one another? or What holds molecules close to one another? Structure/Property

More information

Report Form for Experiment 6: Solid State Structures

Report Form for Experiment 6: Solid State Structures Report Form for Experiment 6: Solid State Structures Note: Many of these questions will not make sense if you are not reading the accompanying lab handout. Station 1. Simple Cubic Lattice 1. How many unit

More information

Chapter 12 Intermolecular Forces and Liquids

Chapter 12 Intermolecular Forces and Liquids Chapter 12 Intermolecular Forces and Liquids Jeffrey Mack California State University, Sacramento Why? Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature

More information

SOLID STATE MODULE - 3. Objectives. Solid State. States of matter. Notes

SOLID STATE MODULE - 3. Objectives. Solid State. States of matter. Notes Solid State MODULE - 3 8 SOLID STATE Y ou are aware that the matter exists in three different states viz., solid, liquid and gas. In these, the constituent particles (atoms, molecules or ions) are held

More information

What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction

What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Liquids and Solids What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Types of Interparticle Forces Ionic Bonding Occurs between cations and anions Metallic

More information

Chem 112 Dr. Kevin Moore

Chem 112 Dr. Kevin Moore Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11 Intermolecular Forces, Liquids, and Solids John D. Bookstaver St. Charles Community

More information

1051-3rd Chem Exam_ (A)

1051-3rd Chem Exam_ (A) 1051-3rd Chem Exam_1060111(A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The molecular-orbital model for Ge shows it to be A) a conductor,

More information

1051-3rd Chem Exam_ (B)

1051-3rd Chem Exam_ (B) 1051-3rd Chem Exam_1060111(B) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In liquids, the attractive intermolecular forces are. A) strong enough

More information

1051-3rd Chem Exam_ (C)

1051-3rd Chem Exam_ (C) 1051-3rd Chem Exam_1060111(C) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The hybridizations of iodine in IF3 and IF5 are and, respectively.

More information

Chemistry 101 Chapter 14 Liquids & Solids

Chemistry 101 Chapter 14 Liquids & Solids Chemistry 101 Chapter 14 Liquids & Solids States of matter: the physical state of matter depends on a balance between the kinetic energy of particles, which tends to keep them apart, and the attractive

More information

CHAPTER 11 INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS

CHAPTER 11 INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS CAPTER 11 INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS 11.7 ICl has a dipole moment and Br 2 does not. The dipole moment increases the intermolecular attractions between ICl molecules and causes that substance

More information

Chapter 9. Liquids and Solids

Chapter 9. Liquids and Solids Chapter 9 Liquids and Solids Chapter 9 Table of Contents (9.1) (9.2) (9.3) (9.4) (9.5) (9.6) (9.7) (9.8) (9.9) (9.10) Intermolecular forces The liquid state An introduction to structures and types of solids

More information

Liquids and Solids. H fus (Heat of fusion) H vap (Heat of vaporization) H sub (Heat of sublimation)

Liquids and Solids. H fus (Heat of fusion) H vap (Heat of vaporization) H sub (Heat of sublimation) Liquids and Solids Phase Transitions All elements and compounds undergo some sort of phase transition as their temperature is increase from 0 K. The points at which these phase transitions occur depend

More information

INTERMOLECULAR FORCES: LIQUIDS, SOLIDS & PHASE CHANGES (Silberberg, Chapter 12)

INTERMOLECULAR FORCES: LIQUIDS, SOLIDS & PHASE CHANGES (Silberberg, Chapter 12) INTERMOLECULAR FORCES: LIQUIDS, SOLIDS & PASE CANGES (Silberberg, Chapter 12) Intermolecular interactions Ideal gas molecules act independently PV=nRT Real gas molecules attract/repulse one another 2 n

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11, Liquids, and Solids John D. Bookstaver St. Charles Community College Cottleville,

More information

Upon successful completion of this unit, the students should be able to:

Upon successful completion of this unit, the students should be able to: Unit 9. Liquids and Solids - ANSWERS Upon successful completion of this unit, the students should be able to: 9.1 List the various intermolecular attractions in liquids and solids (dipole-dipole, London

More information

They are similar to each other

They are similar to each other They are similar to each other Different than gases. They are incompressible. Their density doesn t change much with temperature. These similarities are due to the molecules staying close together in solids

More information

Structure of Crystalline Solids

Structure of Crystalline Solids Structure of Crystalline Solids Solids- Effect of IMF s on Phase Kinetic energy overcome by intermolecular forces C 60 molecule llotropes of Carbon Network-Covalent solid Molecular solid Does not flow

More information

HW# 5 CHEM 281 Louisiana Tech University, POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Structures of Ionic Solids. Why?

HW# 5 CHEM 281 Louisiana Tech University, POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Structures of Ionic Solids. Why? HW# 5 CHEM 281 Louisiana Tech University, POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Structures of Ionic Solids. Why? Many ionic structures may be described as close-packed

More information

Notes on Solids and Liquids

Notes on Solids and Liquids THE LIQUID STATE Notes on Solids and Liquids Why do liquids tend to bead up when on a solid surface? The effect of uneven pull on surface molecules draws them into the body of the liquid causing droplet

More information

Critical Temperature - the temperature above which the liquid state of a substance no longer exists regardless of the pressure.

Critical Temperature - the temperature above which the liquid state of a substance no longer exists regardless of the pressure. Critical Temperature - the temperature above which the liquid state of a substance no longer exists regardless of the pressure. Critical Pressure - the vapor pressure at the critical temperature. Properties

More information

Solid to liquid. Liquid to gas. Gas to solid. Liquid to solid. Gas to liquid. +energy. -energy

Solid to liquid. Liquid to gas. Gas to solid. Liquid to solid. Gas to liquid. +energy. -energy 33 PHASE CHANGES - To understand solids and liquids at the molecular level, it will help to examine PHASE CHANGES in a little more detail. A quick review of the phase changes... Phase change Description

More information

compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due

compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due Liquids and solids They are similar compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due to the molecules being close together in solids

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of

More information

They are similar to each other. Intermolecular forces

They are similar to each other. Intermolecular forces s and solids They are similar to each other Different than gases. They are incompressible. Their density doesn t change much with temperature. These similarities are due to the molecules staying close

More information

Solid Type of solid Type of particle Al(s) aluminium MgCl2 Magnesium chloride S8(s) sulfur

Solid Type of solid Type of particle Al(s) aluminium MgCl2 Magnesium chloride S8(s) sulfur QUESTION (2017:1) (iii) Sodium chloride, NaCl, is another compound that is excreted from the body in sweat. Use your knowledge of structure and bonding to explain the dissolving process of sodium chloride,

More information

M7 Question 1 Higher

M7 Question 1 Higher M7 Question 1 Higher Explain why carbon dioxide is a compound by oxygen is an element Carbon dioxide contains two elements carbon and oxygen. Oxygen contains only one type of atom. M7 Question 2 Higher

More information

EXAM TWO PART ONE CHM 451 (INORGANIC CHEMISTRY) DR. MATTSON 1 NOVEMBER 2012

EXAM TWO PART ONE CHM 451 (INORGANIC CHEMISTRY) DR. MATTSON 1 NOVEMBER 2012 EXAM TWO PART ONE CHM 451 (INORGANIC CHEMISTRY) DR. MATTSON 1 NOVEMBER 2012 NAME: Instructions: This exam has two parts. In Part One, only a pencil and a non-programmable calculator may be used. When you

More information

States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces

States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces States of matter Chapter 11 Intermolecular Forces Liquids and Solids By changing the T and P, any matter can exist as solid, liquid or gas. Forces of attraction determine physical state Phase homogeneous

More information

E12 UNDERSTANDING CRYSTAL STRUCTURES

E12 UNDERSTANDING CRYSTAL STRUCTURES E1 UNDERSTANDING CRYSTAL STRUCTURES 1 Introduction In this experiment, the structures of many elements and compounds are rationalized using simple packing models. The pre-work revises and extends the material

More information

Intermolecular Forces. Chapter 16 Liquids and Solids. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces

Intermolecular Forces. Chapter 16 Liquids and Solids. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces Big Idea: Systems that form macromolecules (ionic, metallic, and covalent network) have the strongest interactions between formula units. Systems that cannot form macro molecules still contain intermolecular

More information

Intermolecular Forces, Liquids and Solids Chap. 10

Intermolecular Forces, Liquids and Solids Chap. 10 Page III-10-1 / Chapter Ten Lecture Notes Intermolecular Forces, and Solids Chap. 10 States of Matter The fundamental difference between states of matter is the distance between particles. Chemistry 222

More information

Metal Structure. Chromium, Iron, Molybdenum, Tungsten Face-centered cubic (FCC)

Metal Structure. Chromium, Iron, Molybdenum, Tungsten Face-centered cubic (FCC) Metal Structure Atoms held together by metallic bonding Crystalline structures in the solid state, almost without exception BCC, FCC, or HCP unit cells Bodycentered cubic (BCC) Chromium, Iron, Molybdenum,

More information

Chapter 12. Solids and Modern Materials

Chapter 12. Solids and Modern Materials Lecture Presentation Chapter 12 Solids and Modern Materials Graphene Thinnest, strongest known material; only one atom thick Conducts heat and electricity Transparent and completely impermeable to all

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in the solid and liquid states particles

More information

Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments

Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments P a g e 1 Unit 3: Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments Liquids and solids are quite different from gases due to their attractive forces

More information

Chapter 9 MODELS OF CHEMICAL BONDING

Chapter 9 MODELS OF CHEMICAL BONDING Chapter 9 MODELS OF CHEMICAL BONDING 1 H H A + B H H A B A comparison of metals and nonmetals 2 9.1 Atomic Properties & Chemical Bonds Chemical bond: A force that holds atoms together in a molecule or

More information

Intermolecular forces (IMFs) CONDENSED STATES OF MATTER

Intermolecular forces (IMFs) CONDENSED STATES OF MATTER Intermolecular forces (IMFs) CONDENSED STATES OF MATTER States of Matter: - composed of particles packed closely together with little space between them. Solids maintain a. - any substance that flows.

More information

What factors affect whether something is a solid, liquid or gas? What actually happens (breaks) when you melt various types of solids?

What factors affect whether something is a solid, liquid or gas? What actually happens (breaks) when you melt various types of solids? States of Mattter What factors affect whether something is a solid, liquid or gas? What actually happens (breaks) when you melt various types of solids? What external factors affect whether something is

More information

Chapter 10: Liquids, Solids, and Phase Changes

Chapter 10: Liquids, Solids, and Phase Changes Chapter 10: Liquids, Solids, and Phase Changes In-chapter exercises: 10.1 10.6, 10.11; End-of-chapter Problems: 10.26, 10.31, 10.32, 10.33, 10.34, 10.35, 10.36, 10.39, 10.40, 10.42, 10.44, 10.45, 10.66,

More information

SOLIDS AND LIQUIDS - Here's a brief review of the atomic picture or gases, liquids, and solids GASES

SOLIDS AND LIQUIDS - Here's a brief review of the atomic picture or gases, liquids, and solids GASES 30 SOLIDS AND LIQUIDS - Here's a brief review of the atomic picture or gases, liquids, and solids GASES * Gas molecules are small compared to the space between them. * Gas molecules move in straight lines

More information

Chapter 16: Phenomena. Chapter 16 Liquids and Solids. intermolecular forces? Intermolecular Forces. Intermolecular Forces. Intermolecular Forces

Chapter 16: Phenomena. Chapter 16 Liquids and Solids. intermolecular forces? Intermolecular Forces. Intermolecular Forces. Intermolecular Forces Chapter 16: Phenomena Phenomena: The tables below show melting points and boiling points of substances. What patterns do you notice from the data? Melting Boiling Substance Point Point CaO 2886 K 4123

More information

Chapter 10. Liquids and Solids. Copyright 2017 Cengage Learning. All Rights Reserved.

Chapter 10. Liquids and Solids. Copyright 2017 Cengage Learning. All Rights Reserved. Chapter 10 Liquids and Solids Chapter 10 Table of Contents (10.1) (10.2) (10.3) (10.4) (10.5) Intermolecular forces The liquid state An introduction to structures and types of solids Structure and bonding

More information

Chap. 12 INTERMOLECULAR FORCES

Chap. 12 INTERMOLECULAR FORCES Chap. 12 INTERMOLECULAR FORCES Know how energy determines physical properties and how phase changes occur as a result of heat flow. Distinguish between bonding (intermolecular) and nonbonding (intermolecular)

More information

The Liquid and Solid States

The Liquid and Solid States : The Liquid and Solid States 10-1 10.1 Changes of State How do solids, liquids and gases differ? Figure 10.4 10-2 1 10.1 Changes of State : transitions between physical states Vaporization/Condensation

More information

Structures of Solids. Unit Cells - Not(?) Chapter 4 Ionic and Other Inorganic Solids. CHEM 462 Wednesday, September 22 T.

Structures of Solids. Unit Cells - Not(?) Chapter 4 Ionic and Other Inorganic Solids. CHEM 462 Wednesday, September 22 T. Chapter 4 Ionic and Other Inorganic Solids CHEM 462 Wednesday, September 22 T. Hughbanks Structures of Solids Many dense solids are described in terms of packing of atoms or ions. Although these geometric

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids 11.2 Intermolecular Forces Intermolecular forces are much weaker than ionic or covalent bonds (e.g., 16 kj/mol versus 431 kj/mol for HCl). Melting or boiling = broken intermolecular forces Intermolecular

More information

Liquids, Solids, and Phase Changes

Liquids, Solids, and Phase Changes C h a p t e r 10 Liquids, Solids, and Phase Changes KMT of Liquids and Solids 01 Gases have little or no interactions. Liquids and solids have significant interactions. Liquids and solids have well-defined

More information

S.No. Crystalline Solids Amorphous solids 1 Regular internal arrangement of irregular internal arrangement of particles

S.No. Crystalline Solids Amorphous solids 1 Regular internal arrangement of irregular internal arrangement of particles Classification of solids: Crystalline and Amorphous solids: S.No. Crystalline Solids Amorphous solids 1 Regular internal arrangement of irregular internal arrangement of particles particles 2 Sharp melting

More information

Chapter 12: Structures & Properties of Ceramics

Chapter 12: Structures & Properties of Ceramics Chapter 12: Structures & Properties of Ceramics ISSUES TO ADDRESS... Bonding and structure of ceramic materials as compared with metals Chapter 12-1 Atomic Bonding in Ceramics Bonding: -- Can be ionic

More information

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 11 Liquids and Intermolecular Forces John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Gases, Liquids, and Solids State Volume Shape of State Density

More information

Ch 9 Liquids & Solids (IMF) Masterson & Hurley

Ch 9 Liquids & Solids (IMF) Masterson & Hurley Ch 9 Liquids & Solids (IMF) Masterson & Hurley Intra- and Intermolecular AP Questions: 2005 Q. 7, 2005 (Form B) Q. 8, 2006 Q. 6, 2007 Q. 2 (d) and (c), Periodic Trends AP Questions: 2001 Q. 8, 2002 Q.

More information