1. The particles in solids and liquids have a limited range of motion and are not easily compressed. Section 3: Liquids and Solids K What I Know W What I Want to Find Out L What I Learned

2. 4(C) Compare solids, liquids, and gases in terms of compressibility, structure, shape, and volume. 10(A) Describe the unique role of water in chemical and biological systems. 2(H)Organize, analyze, evaluate, make inferences, and predict trends from data. 2(I) Communicate valid conclusions supported by the data through methods such as lab reports, labeled drawings, graphs, journals, summaries, oral reports, and technology–based reports. 3(A)In all fields of science, analyze, evaluate, and critique scientific explanations by using empirical evidence, logical reasoning, and experimental and observational testing, including examining all sides of scientific evidence of those scientific explanations, so as to encourage critical thinking by the student. Liquids and Solids Copyright © McGraw-Hill Education

3. Essential Questions How do the arrangements of particles in liquids and solids differ? What are the factors that affect viscosity? How are the unit cell and crystal lattice related? Liquids and Solids Copyright © McGraw-Hill Education

4. Review meniscus Liquids and Solids Copyright © McGraw-Hill Education Vocabulary New viscosity surface tension surfactant crystalline solid unit cell allotrope amorphous solid

5. Liquids Forces of attraction keep molecules closely packed in a fixed volume, but not in a fixed position. Liquids are much denser than gases because of the stronger intermolecular forces holding the particles together. Large amounts of pressure must be applied to compress liquids to very small amounts. Fluidity is the ability to flow and diffuse; liquids and gases are fluids. Liquids and Solids Copyright © McGraw-Hill Education

6. Viscosity Viscosity is a measure of the resistance of a liquid to flow and is determined by the type of intermolecular forces, size and shape of particles, and temperature. The stronger the intermolecular attractive forces, the higher the viscosity. In this diagram of glycerol, it is the hydrogen bonding that makes it so viscous. The hydrogen atoms attached to the oxygen atoms in each molecule are able to form hydrogen bonds with other glycerol molecules. Liquids and Solids Copyright © McGraw-Hill Education

7. Viscosity Particle size and shape: Larger molecules create greater viscosity. Long chains of molecules result in a higher viscosity: cooking oils and motor oils. Temperature: Increasing the temperature decreases viscosity because the added energy allows the molecules to overcome intermolecular forces and flow more freely. Liquids and Solids Copyright © McGraw-Hill Education

8. Surface Tension Surface tension is the energy required to increase the surface area of a liquid by a given amount. Surface tension is the a measure of the inwards pull by particles in the interior. The stronger the attraction between particles the stronger the surface tension. Example: Water Surfactants are compounds that lower the surface tension of water. Surface tension is why water alone will not clean your clothes, you need soap to break down the hydrogen bonds so the water will carry the dirt away. Liquids and Solids Copyright © McGraw-Hill Education

9. Enzymes and Surfactants Video Enzymes and Surfactants Add link to concepts video from page 419 here. Liquids and Solids Copyright © McGraw-Hill Education

10. Cohesion, Adhesion, and Capillary Action Cohesion is the force of attraction between identical molecules. Adhesion is the force of attraction between molecules that are different. Capillary action is the upward movement of liquid into a narrow cylinder, or capillary tube. Liquids and Solids Copyright © McGraw-Hill Education

11. Solids Solids contain particles with strong attractive intermolecular forces. Particles in a solid vibrate in a fixed position. Most solids are more dense than liquids. One exception to this is water. Ice is less dense than liquid water. The hydrogen bonding in ice results in an open symmetrical structure that keeps the water molecules in ice farther apart than in water in a liquid state. Liquids and Solids Copyright © McGraw-Hill Education

12. Crystalline Solids Crystalline solids are solids with atoms, ions, or molecules arranged in an orderly, geometric shape. A unit cell is the smallest arrangement of atoms in a crystal lattice that has the same symmetry as the whole crystal. Liquids and Solids Copyright © McGraw-Hill Education

13. Unit Cells Interactive Table FPO Add link to concepts in motion interactive table from page 421 here. Liquids and Solids Copyright © McGraw-Hill Education

14. Crystalline Solids Liquids and Solids Copyright © McGraw-Hill Education

15. Types of Crystalline Solids Interactive Table FPO Add link to concepts in motion interactive table from page 422 here. Liquids and Solids Copyright © McGraw-Hill Education

16. Amorphous Solids Amorphous solids are solids in which the particles are not arranged in a regular, repeating pattern. Amorphous solids form when molten material cools quickly. Gas, rubber, and many plastics are amorphous solids. Liquids and Solids Copyright © McGraw-Hill Education

17. Liquids and Solids Copyright © McGraw-Hill Education Review Essential Questions How do the arrangements of particles in liquids and solids differ? What are the factors that affect viscosity? How are the unit cell and crystal lattice related? Vocabulary viscosity surface tension surfactant allotrope amorphous solid crystalline solid unit cell