1. Chapter 10 States of Matter Pages 329 - 351

2. The Kinetic-Molecular Theory of Matter …states that particles of matter are always in motion. An _____________ is a hypothetical gas that perfectly fits all assumptions of the kinetic-molecular theory (KMT). Five assumptions of the KMT of gases: 1.Gases consist of large numbers of tiny particles that are __________relative to their size. 2.Collisions between gas particles and between particles and container walls are _____________ which exhibit no net loss of total kinetic energy. 3.Gas particles are in continuous, rapid, random motion, therefore they possess __________ which is energy of __________. 4.There are no __________________ between gas particles. 5.Gas temperatures depend on the _______________________ of the gas particles.

3. The Kinetic-Molecular Theory of Matter Physical properties of gases: 1.Expansion: completely fill any container in which they are enclosed 2.Fluidity: particles glide easily past one another because attractive forces (in ideal gases) are insignificant 3.Low Density: particles are so far apart from each other, exhibit low density 4.Compressibility: particles are so far apart from each other, they can be compressed 5.Diffusion: because of random and continuous motion of gas molecules, they spread and mix with one another without being stirred.

4. The Kinetic-Molecular Theory of Matter Do all gases behave ideally? A _________ is a gas that does not behave completely according to the assumptions of the KMT. At high pressure and low temperature, gas particles are ______________ and kinetic energy is insufficient to overcome attractive forces. Real gas = non-ideal gas ≠ ideal gas Gas molecules that have polarity will be most likely to behave _________(ideally or non-ideally?) For the following gas molecules, which will exhibit polarity? Which will not? N 2, H 2, O 2, H 2 O(g), NH 3, CH 3 Cl, Ar, Ag

5. Liquids …are the least common state of matter because they have a ____________ of temperature/pressure. Liquid particles are also in constant motion but are ______________ than gas particles – thus, forces of attraction (or intermolecular forces) are more significant. Some of these already discussed are ________________, London dispersion and ________________. Molecules at the surface of liquids have enough _______________ to overcome these forces. What happens to these liquid molecules?

6. Liquids Physical Properties: 1.High Density: because of the close arrangement of liquid particles. Water becomes _______________ when it solidifies and is an exception to most liquids. 2.Incompressibility: while they do transmit pressure equally in all directions, because their molecules are so much _______ together, they resist compression. 3.Diffusion: because the molecules also have ___________motion, they mix with other liquids. (refer to fig 5 page 334) 4.Surface Tension: results from the _____________ between liquid particles; causes droplets to take a spherical shape 5.Evaporation/Boiling: occurs because liquid particles have different _____________. Boiling is the change of a liquid to _______________ appearing throughout the liquid (fig 8 page 336) 6.Solid Formation: when liquid is cooled, the average energy of its particles ____________. Do all liquids freeze at the same temperature? Why do you think this is?

7. Solids Solid particles are more ____________ than those of liquid or gas particles – thus, they have the most significant forces of ___________. What are these forces? Unlike liquids and gases, solid particles are not in constant random motion but they do have _________ movement. Do you think this can be described as unordered or ordered structure? What are the two types of solids?

8. Solids Physical Properties: 1.Definite Shape and Volume: because particles are ____________ together – thus, there is very little empty space into which particles can be compressed. 2.Definite Melting Point (crystalline only): when melting occurs, ___________ of particles within the solid overcome the _____________ holding them together and a phase change occurs. Substance changes from a ______ to a _______. 3.High Density/Incompressibility: because particles are ____________ together – thus they are more dense than liquids and MUCH more dense than gases. 4.Low Diffusion Rates: though diffusion has been observed between solids, it is MUCH ________ than liquids and gases.

9. Solids Crystalline vs. Amorphous: CRYSTALLINE SOLIDS AMORPHOUS SOLIDS Particles are orderly, geometric and repeating patterns of atoms held together by ionic or covalent bonds. Particles are arranged randomly without geometric patterns. Have definite melting points. Do not have the ability to flow. Do NOT have definite melting points. Have the ability to flow over a range of temperatures. Arrangement of particles in a crystal is represented by a coordinate system called a lattice. Are sometimes referred to as supercooled liquids because particles are arranged randomly much like a liquid. Smallest portion of a crystal lattice that shows the 3-D pattern of the entire lattice is called a unit cell. Plastics and glass are examples of amorphous solids.

10. Solids Four Types of Crystalline Solids Classified by Binding Forces: 1.Ionic crystals: consists of positive and negative ions arranged in a regular pattern. Examples: ___________ and __________ 2.Covalent network crystals: each atom is covalently bonded to its nearest neighboring atom. Examples: __________ and ________. 3.Metallic crystals: consists of metal cations (charge?) surrounded by a ________________ valence electrons. Do you think metallic crystals conduct electricity? What about the other types? 4.Covalent molecular crystals: covalently bonded molecules held together by intermolecular forces. What are the two types of these crystals? _______________________. Identify the following as polar or nonpolar: NH 3, C 6 H 6, H 2 O, CH 4, CH 3 Cl, CCl 4

11. Changes of State

12. Ice  liquid water is ____________ Dry ice  CO 2 gas is ____________ Water  Ice is _______________ Liquid bromine  bromine vapor is _______________ Water vapor  liquid water is _______________ ____________ is a dynamic condition in which two opposing changes occur at equal rates in a closed system. The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature is the liquid’s ________________________.

13. Changes of State

14. Liquids that evaporate readily are called __________. They escape the liquid phase quickly because of their weak ______________. What is an example of this type of liquid? The ___________of a liquid is the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure. Can the pressure of a substance affect the temperature at which said substance boils? During boiling, added energy is used to overcome _______________ between molecules during the phase change and is stored in vapor as _______________. Remember!! Law of Conservation of ____________.

15. Changes of State The amount of energy as heat that is needed to vaporize one mole of a liquid at the liquid’s boiling point at constant pressure is called the liquid’s _______________________________. The stronger the attraction between molecules (intermolecular forces), the _________ (more or less?) energy is required to overcome the liquid state and escape to the gas phase. Why do we sweat to cool our body temperature? Energy is needed for water to change from a liquid to a gas. When perspiration evaporates from our skin, body heat is absorbed by the liquid water – thus cooling the surface of our skin. Freezing involves the LOSS of energy in the form of heat by the liquid. Liquid  solid + energy

16. Changes of State At the ____________, particles of the liquid and the solid have the same average kinetic energy. Thus, melting is the reverse: solid + energy  liquid : but consider, which phase of matter (solid or liquid) has more motion and movement? What type of energy can describe motion or movement? Thus, a liquid has more or less energy? The amount of energy as heat required to melt one mole of solid at the solid’s melting point is the solid’s ____________________. As a result of melting, there is a ____________ in particle order as substance transforms from solid to liquid. The magnitude of this quantity of heat energy is dependent on the forces of ____________ between the molecules of the substance.

17. Changes of State A ________________ is a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist and how states of a system change with changing temperature/pressure. The point on a phase diagram where temperature/pressure conditions are such that a substance exists as a _______, a ________ and a _________ is called the triple point. Critical point = critical _________ & critical __________ The ______________ is the temperature above which the substance cannot exist in the liquid state. The _______________ is the lowest pressure at which the substance can exist as a liquid at the critical temperature.

18. Changes of State

19. Water

20. Water …is an essential component of all _____________ - chemical reactions of most life processes take place in water and is usually a _________ or a _________ in these reactions. What type of bonds exist between the 2 hydrogen atoms to the 1 oxygen atom? What is the geometry of a water molecule? What is the bond angle between the two atoms of hydrogen? What is the hybridization of a water molecule? Water molecules are linked between one another by _________ but as the temperature increases, the number of linked molecules __________. If not for hydrogen bonding, water would be a _____ at room temperature.

21. Water In ice, water molecules are in __________ arrangements. How can we account for the fact that solid water (ice) is less dense than liquid water (thus, ice floats in liquid water)? In what state of matter is this molecular illustration of water?