Properties of Covalent (Molecular) Substances

Slides:

Advertisements

Similar presentations

Intermolecular forces

Advertisements

Properties of Covalent (Molecular) Substances. Properties Depend on strength of IMF between “particles” or separate units covalent substances: – units.

Condensed Phases and Intermolecular Forces

TOPIC: Intermolecular Forces Part 2: Dipole- Dipole and Hydrogen Bonding Do Now: List the 4 categories of Nonpolar Molecules – all of these have DISPERSION.

INTERMOLECULAR FORCES. Three types of force can operate between covalent (not ionic) molecules:  Dispersion Forces also known as London Forces as Weak.

TOPIC: Intermolecular Forces Part 1: Dispersion Forces Do Now: How do particle diagrams of liquids & solids compare to those of gases?

Intermolecular Forces Chemistry Mrs. Coyle. Intermolecular Forces The forces with which molecules attract each other.

Intermolecular Forces Forces Between Molecules. Why are intermolecular forces important? They determine the phase of a substance at room temperature.

Sec. 8.5: Electronegativity and Bond Polarity

Topic: Covalent Bonds and Properties 1.Why do atoms form bonds? 2. How do atoms form bonds? To attain a noble gas configuration By gaining, losing, or.

TOPIC: Intermolecular Forces How do particle diagrams of liquids & solids compare to those of gases?

1 Mr. ShieldsRegents Chemistry U07 L01 2 Forces of attraction There exist between Molecules of gases and liquids Forces of attraction. Some forces may.

 Intramolecular Bond  (Bond within a molecule)  Intermolecular force of attraction  (Attraction between 2 molecules)  Usually Dipoles (H- bonds)

Intermolecular Forces Forces Between Molecules. Why are intermolecular forces important? They determine the phase of a substance at room temperature.

Intermolecular Forces Chapter 11.2 Pages

Recall from Ionic Bonding…

Polarity and Intermolecular Forces

Chemical Bonding Topic 5 Chemical Bonding Metallic Metal atoms only Ionic Metal + nonmetal atoms Covalent Nonmetal + nonmetal atoms Polar covalent Nonpolar.

Between.  Intra- › strong forces that hold the atoms in a molecule together  takes 464 kJ/mol to break the H-O bonds within a water molecule › responsible.

Properties of Covalent (Molecular) Substances. Poor conductors of heat & electricity in any phase. No charged particles! Low melting & boiling points:

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.

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.

1 POLARITY  POLAR BONDS  Bonds between atoms  POLAR MOLECULES  Polarity between molecules  Occurs when polar bonds create a dipole moment.

Polar Bonds and Molecules. Bond Polarity  Not all covalent bonds are equal in their sharing of electrons  A lot depends on the type of atoms involved.

Condensed Phases and Intermolecular Forces. Fundamentals How do particle diagrams of liquids & solids compare to those of gases?

Intermolecular Forces By Peter Demkowicz. Why? Intermolecular Forces.

Properties of Ionic Compounds. Properties high melting points –strong electrostatic interactions between oppositely charged ions.

TOPIC: Intermolecular Forces How do particle diagrams of liquids & solids compare to those of gases?

1 2 Forces of attraction There exist between Molecules of gases and liquids Forces of attraction. Some forces may be strong other forces may be weak.

Condensed Phases and Intermolecular Forces. Fundamentals How do particle diagrams of liquids & solids compare to those of gases?

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.

Condensed Phases and Intermolecular Forces. Let’s look at particle diagrams of liquids & solids and compare them to particle diagrams of gases.

Electronegativity ++ –– 00 00 HClHH Electronegativity Electronegativity describes how electrons are shared in a compound Consider the compound.

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.

Intermolecular Forces Forces Between Molecules. Why are intermolecular forces important? They determine the phase of a substance at room temperature.

Chapter 6.2. Two Types of Forces with Compounds Intramolecular Forces the forces of attraction that hold the atoms together in a molecule. Ex. ionic bonds,

9-9 Intermolecular Forces (IMFs) ~ (Section 14.3) And you.

Intermolecular Forces

Covalent Properties Polarity and IMF.

Intermolecular forces

8.4 Bond Polarity Bonding Ionic Covalent.

Intermolecular forces

I. Intermolecular Forces

Section 2: Intermolecular Attractive Forces

Intermolecular Forces

8.4 Bond Polarity Bonding Ionic Covalent.

Forces between Particles

Intermolecular Forces

7.13 – NOTES Solubility of Molecules

I. Intermolecular Forces

I. Intermolecular Forces

Properties of Covalent (Molecular) Substances

Notes: 13.2 OBJECTIVES: Students will be able to (SWBAT)

8.4 Bond Polarity Bonding Ionic Covalent.

Intermolecular Forces,

Intermolecular Forces

INTERMOLECULAR FORCES

Intermolecular forces

Intermolecular Forces

Attractions Within & Between Molecules

Intermolecular Forces

Intermolecular forces

Intermolecular forces

9-9 Intermolecular Forces (IMFs) ~ (Section 14.3)

Aim: What attracts molecules to each other?

7.11 – NOTES Solubility of Molecules

Intermolecular Forces (Ch6)

Intermolecular forces

Properties of Covalent (Molecular) Substances

Presentation transcript:

Properties of Covalent (Molecular) Substances

Properties Depend on strength of IMF between “particles” or separate units covalent substances: units are molecules

Intermolecular Forces Dispersion forces occur between nonpolar molecules (Van der Waals) Dipole-dipole forces occur between polar molecules Hydrogen bonding occurs between molecules with an H-F, H-O, or H-N bond Intermolecular forces determine phase!

Dispersion forces ↑ as size molecule ↑ weakest IMF = dispersion forces - occur between nonpolar molecules Monatomic molecules: He, Ne, Ar, Kr, etc. Diatomics of same element: O2, H2, N2 Symmetric molecules: C4H10 Dispersion forces ↑ as size molecule ↑

Dipole-dipole forces occur between: - polar molecules (permanent charge separation) HCl and HBr are examples of polar diatomic molecules

Hydrogen bonding occurs between molecules containing an H-F, H-O, or H-N bond H-bonding: strongest IMF

Properties of Covalent (Molecular) Substances Poor conductors of heat & electricity no charged particles! Low mp & low bp easy to pull molecules apart from each other Majority of solids are soft Low Hf and Hv compared to ionic & metallic substances High VP compared to ionic & metallic substances

mp, bp, Hf and Hv and vapor pressure depend on how hard it is to pull particles apart Weak IMF – easy to pull particles apart Strong IMF – more difficult to pull apart

Which substance has the strongest intermolecular forces? The weakest? Water Ether