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O.A # 60. Write the formula for each of the following: Silicon Dioxide ___________ Magnesium Iodide ___________ Aluminum Sulfide ___________. SiO 2. MgI 2. Al 2 S 3. O.A # 61 Surface Tension. O.A # 62 Phase Diagram. Chapter 13- States of Matter. 13.1 Gases.
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O.A # 60 Write the formula for each of the following: • Silicon Dioxide ___________ • Magnesium Iodide ___________ • Aluminum Sulfide ___________ SiO2 MgI2 Al2S3
O.A # 61 Surface Tension
O.A # 62 Phase Diagram
13.1 Gases 1. Define the kinetic-molecular theory. Definition: The kinetic-molecular theory describes the behavior of gases in terms of particles in motion. Assumptions: a. Size: Gases consist of small particles that are separated from one another by empty space. The volume is small compared with the volume of the empty space.
b. Motion: Gas particles are in constant random motion. Particles move in straight line until they collide with other particles and the walls of their container. c. Energy: The kinetic energy can be represented by KE= 1/2mv2, in a sample of a gas all particles have the same mass but do not have the same velocity.
2. What is meant by an elastic collision? Collisions between particles are elastic. An elastic collision is one in which no kinetic energy is lost. 3. How is kinetic energy and temperature related? Temperature is a measure of the average kinetic energy. At a given temperature, all gases have the same average kinetic energy
13.2 Forces of Attraction 1. Differentiate intramolecular and intermolecular forces. There are three main types of intramolecular force: Ionic, covalent, and metallic. The prefix “inter” means ‘between” or “among.” Intermolecular forces can hold together identical particles such as water molecules in a drop of water. All intermolecular forces are weaker than intramolecular or bonding forces.
2. Describe the three types of intermolecular forces in order from weakest to strongest. a) Dispersion forces: Dispersion forces are weak forces that result from temporary shifts in the density of electrons in electron clouds. b) Dipole-dipole forces: Dipole-dipole forces is the attraction between oppositely charged regions of polar molecules.
c) Hydrogen bonds: A hydrogen bond is a dipole-dipole attraction that occurs between molecules containing a hydrogen atom bonded to a small, highly electronegative atom with at least one lone pair of electrons.
13.3 Liquids and Solids Not fixed Not fixed Fixed Indefinite Definite Definite Relatively high Extremely low Medium Extremely low Relatively high Low does not flow flows flows rapid medium none
I2, H2O,NH3, CO2, C12H22O11 Very soft, very low melting point and poor conductivity Inter- molecular molecules Atoms connected by covalent bonds Fairly soft, low melting point, and poor conductivity Diamond and quartz Intra- molecular Very hard, high melting point, and poor conductivity NaCl, KBr, CaCO3 Ions Intra- molecular Atoms surrounded by mobile valence e- Soft to hard, low to high melting point, and excellent conductivity All metallic elements Intra- molecular
3. What is surface tension and how is it influenced by intermolecular forces? Surface tension is the energy required to increase the surface area of liquid by a given amount, results from an uneven distribution of attractive forces Summary:
13.4 Phase Changes 1. Define the following phase changes Gas Sublimation Condensation Deposition Vaporization Solid Melting Liquid Freezing
2. What is vapor pressure and what is its relation to boiling point? The pressure exerted by a vapor over a liquid is called vapor pressure. Thetemperature at which the vapor pressure of a liquid equals the external or atmospheric pressure is called the boiling point.
3. What is a phase diagram and what information does it provide? A phase diagram is a graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure. Summary:
