Unit 7.5 Comparing Intermolecular Forces Teacher: Dr. Van Der Sluys.

Slides:



Advertisements
Similar presentations
Intermolecular Attractions
Advertisements

INTERMOLECULAR FORCES. Three types of force can operate between covalent (not ionic) molecules:  Dispersion Forces also known as London Forces as Weak.
Intermolecular Forces and the Physical Properties of Liquids and Solids.
Chem-To-Go Lesson 18 Unit 4 COVALENT BONDING – POLARITY & INTERMOLECULAR FORCES.
Bonding in compounds Overview Learn how the elements can form bonds in compounds.
2.4 Intermolecular Forces
Electronegativity and Polarity.  Describe how electronegativity is used to determine bond type.  Compare and contrast polar and nonpolar covalent bonds.
Melting Point and Boiling Points of Ionic and Covalent Compounds
Intermolecular Forces a.k.a. van der Waal’s Forces O ++ -- H H O ++ -- H H Intermolecular Intramolecular.
How many valence electrons does magnesium have? 2.
UNIT: BONDING TIER 5 -Determine if a molecule is polar or nonpolar
Intermolecular Forces: relationships between molecules
Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chapter 10 Structures of Solids and Liquids 10.4 Attractive Forces between Particles 1.
Functional Groups The great majority of organic compounds have C—C and C—H bonds. These are strong, non-polar bonds. They provide a non-reactive framework.
Define a Solution Summary Activity Read pp. 266 – 268 Define the following terms: solution, homogeneous mixtures, solute, solvent, alloy, and aqueous.
Interparticle Bonding
Intermolecular Forces. How are molecules held together? There are two types of attraction in molecules: ◦ Intramolecular forces ◦ Intermolecular forces.
Polarity and Intermolecular Forces
Intermolecular Forces and Liquids and Solids Chapter 11.
Liquids Properties of liquids are similar to solids’, and way different from gas properties density compressibilities enthalpy changes attractive forces.
Attractions Between Molecules or Intermolecular Forces (IM Forces) Chapter 8.4.
Types of Solids Intra V Inter. Intramolecular Type of bonding within the molecule Covalent Ionic Metallic Covalent Simple molecular solids with different.
Chapter 2: Organic Compounds: A First Look Common Bonding Situations Hydrogen1 bond Carbon4 bonds (neutral and 8 electrons) Reactive Carbon Species.
Functional Groups.
Intermolecular Forces... explaining the properties of liquids.
Intermolecular Forces Topic 4.4
CHEMICAL BONDING. Why do bonds form? To complete the valence or outer energy level Octet Rule – 8 is great! A bond forms when 2 atoms attract the same.
Intermolecular Forces of Attraction (IMFs)
Solubility: Molecular Polarity. How do molecules stay together?
Intermolecular Forces Chemistry 11 Ms. McGrath. Intermolecular Forces The forces that bond atoms to each other within a molecule are called intramolecular.
Why do some solids dissolve in water but others do not? Why are some substances gases at room temperature, but others are liquid or solid? The answers.
Why do some solids dissolve in water but others do not? Why are some substances gases at room temperature, but others are liquid or solid? The answers.
A chemical bond’s character is related to each atom’s attraction for the electrons in the bond. Section 5: Electronegativity and Polarity K What I Know.
Objectives Contrast ionic and molecular substances in terms of their physical characteristics and the types of forces that govern their behavior. Describe.
1 Section 8.1The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes (Hybridization and VSEPR model)
1 Organic Chemistry MDL233 Chapter 2 BY Mahwash Hafeez.
Intermolecular Forces Glenn V. Lo Department of Physical Sciences Nicholls State University.
Intermolecular Forces
The atom has a centrally located nucleus with a positive charge. + surrounded by a cloud of electrons (with a negative charge).
Intermolecular Forces Chemistry 11 Ms. McGrath. Intermolecular Forces The forces that bond atoms to each other within a molecule are called intramolecular.
Intermolecular Forces
Materials Science Lesson 8.
Intermolecular forces
UNIT 6 Solution Chemistry.
Chemical Bonding `.
Ch. 6.5b Hybrid Orbitals and Intermolecular Forces
Polarity within a Molecule
Explaining Solutions SCH3U.
Intermolecular Forces
IONIC VS. COVALENT COMPOUNDS
Intermolecular Forces
Ionic and Metallic Bonding
8.4 Bond Polarity Bonding Ionic Covalent.
Intermolecular Forces
Physical Properties Physical properties such as boiling point and solubility are largely determined by intermolecular forces.
Electronegativity and Polarity
Bellwork Tuesday Draw the Lewis Structure and name the correct shaped molecule for all of the following. BF3 CH4 HBr NH3.
UNIT VIII PPT #1 Solution Chemistry.
Intermolecular Forces,
Intermolecular Forces
Section 6.5 – Molecular Geometry
Intermolecular Forces
Intra vs Inter The prefix intra- means “within”
Hydrogen bonds What are they?
Intra vs Inter The prefix intra- means “within”
12.1 Intramolecular Forces
Mission B6 - Intermolecular Bonding
Intermolecular forces
Presentation transcript:

Unit 7.5 Comparing Intermolecular Forces Teacher: Dr. Van Der Sluys

Objectives To determine –Relative melting and boiling points –Relative solubility of various combinations of compounds

Vocabulary Solution - a homogeneous mixture of two or more compounds. Solvent - The compound that comprises the majority of a solution. Solute - A minor component of a solution. Aqueous solution - A mixture of liquid water and one or more solutes.

Types of Bonding IntramolecularIntermolecular Nonpolar CovalentLondon Dispersion Forces Polar Covalent London Dispersion when symmetric Dipole-Dipole when asymmetric Extremely Polar Covalent: H-N, H-O or H-F bonds Hydrogen Bonding Weakly Ionic: NaCl Soluble in water due to ion-dipole interactions Extremely Ionic: Fe 2 O 3 Insoluble in water due to high crystal lattice energies

Like Dissolves Like In order for a mixture to combine and become homogeneous on the molecular level, the compounds must have similar intermolecular bonding properties, i.e. ethanol and water. Two compounds that have very different intermolecular forces will not mix and will produce a heterogeneous mixture, i.e. Italian salad dressing.

Comparing Intermolecular Forces CompoundLondon Dispersion Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O)

Comparing Intermolecular Forces CompoundLondon Dispersion Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) CH 4 methane H 2 O water

Comparing Intermolecular Forces CompoundLondon Dispersion Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) NH 3 ammonia H 2 O water

Comparing Intermolecular Forces CompoundLondon Dispersion Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) Fe 2 O 3 Iron(III) oxide C 8 H 18 octane

Comparing Intermolecular Forces CompoundLondon Dispersion Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) CO 2 Carbon dioxide H 2 O water

Melting and Boiling Points The relative melting and boiling of various compounds are due to the strength of intermolecular forces. If two compounds have the same types of intermolecular forces, the total number of electrons can usually be used to predict the degree of London dispersion forces. The compound with more electrons usually has the higher melting and boiling points. For compounds with hydrogen bonding, the ratio of hydrogen atoms to lone pairs can be important.

Comparing Intermolecular Forces Compound London Dispersion (Total number of electrons?) Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) CH 4 methane C 2 H 6 ethane

Comparing Intermolecular Forces Compound London Dispersion (Total number of electrons?) Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) CO 2 Carbon dioxide H 2 O water

Comparing Intermolecular Forces Compound London Dispersion (Total number of electrons?) Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) NaCl Sodium chloride C 6 H 14 Hexane

Comparing Intermolecular Forces Compound London Dispersion (Total number of electrons?) Dipole- Dipole (AXE?) Hydrogen Bonding (H-F, H-N, H-O) Weakly Ionic (Ions with low charges) Strongly ionic (Both ions have charges >2 Usually Insoluble in H 2 O) CO 2 Carbon dioxide H 2 O water

Summary If compounds have similar intermolecular forces they tend to form homogeneous solutions, “like dissolves like.” The strength of intermolecular forces can be used to predict relative melting and boiling points