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Chapter 14 Liquids and Solids

Chapter 14 Liquids and Solids. How do the particles of a gas behave? Motion? Attraction? Arrangement? As a result, gases have low densities, are highly compressible and conform completely to the shape of a container. Let’s compare that to solids

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Chapter 14 Liquids and Solids

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  1. Chapter 14Liquids and Solids

  2. How do the particles of a gas behave? • Motion? • Attraction? • Arrangement? As a result, gases have low densities, are highly compressible and conform completely to the shape of a container. • Let’s compare that to solids • High densities, basically incompressible, rigid, maintain their own shapes • The properties of liquids are in-between • Liquids are more closely related to solids than they are to gases.

  3. When a liquid turns solid it becomes denser (except water)

  4. Which state of matter is illustrated? Solid

  5. Which state of matter is illustrated? Liquid

  6. Which state of matter is illustrated? Gas

  7. What process is illustrated? Melting

  8. What process is illustrated? Boiling / Evaporation

  9. 14.1 intermolecular forces • Most substances consisting of small molecules are gasses at room temperature and pressure (a notable exception is water) • Intermolecular forces are sources of attraction between molecules. • Dipole-dipole attraction • Hydrogen Bonding • London Dispersion Forces

  10. dipole-dipole attraction • polar molecules get together b/c of mutual attraction • the ∂+ of one is attracted to the ∂- of the other • they find the best orientation, too, for maximum “stickiness” • only about 1% as strong as covalent

  11. hydrogen bonding • Particularly strong intermolecular force • Occurs when hydrogen is bound to a highly electronegative atom (e.g. F, N) • The extremely unequal sharing of the Hydrogen’s one electron creates a very strong dipole

  12. water molecules have a strong attraction for each other • their attraction is called an H-bond • represented by------ lines • [not true bonds, just really strong attractions]

  13. This also happens with molecules which have N-H and F-H bonds • water, ethanol, ammonia all have H-bonding • it’s the reason they all are liquids when they aren’t supposed to be (i.e. similar sized molecules without H-bonding are all gases)

  14. it has a significant affect on the properties of H-bonded molecules by making them cling to each other more • boiling points are higher because it is so hard to separate them

  15. londondispersionforces • what about nonpolar substances? how can they be attracted to each other and form a liquid? • they are attracted by london dispersion forces • some atoms, although nonpolar overall can experience temporary, instantaneous dipoles

  16. it is short-lived and weak but it can add up

  17. nonpolar moleculescanform these attractions • they have to be slow and close for any significant effect, but… • large molecules (e.g. I2) form them more easily because of all the electrons involved

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