Solids and Liquids Chapter 14 Kinetic Molecular Theory

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Solids and Liquids Chapter 14

Solids and Liquids Chapter 14

Kinetic Molecular Theory • Solids-particles are highly ordered and packed closely together. They have

Kinetic Molecular Theory • Solids-particles are highly ordered and packed closely together. They have slight vibrational movement. A solid maintains its shape regardless of the container. • Liquids-particles are more disordered and are spread further than in a solid. They more closely resemble solids than gases.

Phases Heat is added Endo • Evaporation-liquid to gas (100°C for waterboiling point) •

Phases Heat is added Endo • Evaporation-liquid to gas (100°C for waterboiling point) • Melting-solid to liquid • Sublimation-solid to gas (dry ice directly to a gas) Heat is removed Exo • Condensing-gas to liquid • Freezing-liquid to solid (0°C for waterfreezing point) • Deposition-gas to solid (water vapor directly to ice)

It takes 7 times more energy to vaporize a mole of water than to

It takes 7 times more energy to vaporize a mole of water than to melt a mole of water.

Phase Diagram of Water

Phase Diagram of Water

Water One gram of ice has a greater volume than one gram of water.

Water One gram of ice has a greater volume than one gram of water. liquid water 1. 00 g = 1. 00 g/m. L 1. 00 m. L solid water 1. 00 g = 0. 917 g/m. L 1. 09 m. L

All phase changes are physical changes because a new substance is not created.

All phase changes are physical changes because a new substance is not created.

What keeps the molecules together? • Intramolecular forces (within the molecule)-holds the atoms of

What keeps the molecules together? • Intramolecular forces (within the molecule)-holds the atoms of a molecule together Ex: H bonds with O to make H 2 O • Intermolecular forces (between the molecules)-forces between molecules Ex: H 2 O bonds are broken with other H 2 O molecules when making steam.

Intermolecular Forces • Hydrogen bonding-special type of strong dipole-dipole bond where H is bonded

Intermolecular Forces • Hydrogen bonding-special type of strong dipole-dipole bond where H is bonded to a highly electronegative element Ex: H 2 S, HCl • Dipole-dipole attraction-polar molecules line up so the positive and negative poles attract (1% as strong as covalent or ionics) • London dispersion forces-forces that exist among noble gas atoms and nonpolar molecules (weakest force) Ex: H 2, N 2, I 2

Intermolecular Forces: Hydrogen Bonding Forces Click in this box to enter notes. Go to

Intermolecular Forces: Hydrogen Bonding Forces Click in this box to enter notes. Go to Slide Show View (press F 5) to play the video or animation. (To exit, press Esc. ) This media requires Power. Point® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete. ] Copyright © Houghton Mifflin Company. All rights reserved.

Types of crystalline solids • Ionic-contains cations and anions, conduct electricity Ex: Salt (Na.

Types of crystalline solids • Ionic-contains cations and anions, conduct electricity Ex: Salt (Na. Cl). Have high melting points. • Molecular-contains covalent bonds (molecules) Ex: Sugar (C 12 H 22 O 11). Intermolecular forces are weak so they melt at low temperatures. • Atomic-1 element covalently bonded to itself Ex: Diamond (Carbon)

Structure of an Ionic Solid (Na. Cl) Click in this box to enter notes.

Structure of an Ionic Solid (Na. Cl) Click in this box to enter notes. Go to Slide Show View (press F 5) to play the video or animation. (To exit, press Esc. ) This media requires Power. Point® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete. ] Copyright © Houghton Mifflin Company. All rights reserved.

Molecular Solids Click in this box to enter notes. Go to Slide Show View

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Comparison of a Molecular Compound an Ionic Compound Click in this box to enter

Comparison of a Molecular Compound an Ionic Compound Click in this box to enter notes. Go to Slide Show View (press F 5) to play the video or animation. (To exit, press Esc. ) This media requires Power. Point® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete. ] Copyright © Houghton Mifflin Company. All rights reserved.

Metallic Solids • Metals have strong, nondirectional bonding. • Electron sea model-metal atoms are

Metallic Solids • Metals have strong, nondirectional bonding. • Electron sea model-metal atoms are located in a sea of valence electrons that are shared • Alloy-a substance that contains a mixture of elements and has metallic properties.

Alloys • Substitutional alloy-metal atoms are replaced by other metal atoms of similar size

Alloys • Substitutional alloy-metal atoms are replaced by other metal atoms of similar size Ex: sterling silver (93% silver, 7% copper) Analogy: Substitute teacher • Interstitial alloy-some of the interstices (holes) among metal atoms are occupied by smaller atoms Ex: steel (carbon and iron) Analogy: Tutor

Electron Sea Model Click in this box to enter notes. Go to Slide Show

Electron Sea Model Click in this box to enter notes. Go to Slide Show View (press F 5) to play the video or animation. (To exit, press Esc. ) This media requires Power. Point® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete. ] Copyright © Houghton Mifflin Company. All rights reserved.