1.1: Matter
1.1.1: Properties of Matter
1.1.1.1: Extensive versus Intensive Properties
Read the "Extensive and Intensive Properties" section. Remember that extensive properties, such as volume and mass, rely on the "extent" to which matter is present. Intensive properties, such as density and viscosity, are independent of the quantity of matter and are inherent to the matter.
1.1.1.2: Physical versus Chemical Properties
Read the "Physical and Chemical Properties" section. Note that, because the two properties of matter are closely related, the distinction can become difficult to discern; however, for our purposes, we will define a physical property as one that can be observed without changing the matter's composition.
1.1.2: States of Matter
Read the "Solids, Liquids, and Gases" section. Note the differences between these three phases of matter on both the microscopic and macroscopic level. Solids, like wooden blocks, have definite shape and definite volume, and the particles are ordered and close together. Liquids have definite volume and indefinite shape, meaning they take on the shape of the container. Imagine the differences between iced tea in a pitcher versus in a glass. A liquid's particles are less ordered, but still relatively close together. Gases, such as the air inside balloons, have indefinite shape and indefinite volume and their particles are highly disordered.
1.1.3: Density
Read the first two sections: "So What Is Density?" and "Densities of Common Substances." Note that density is temperature dependent and the units differ for solids (g/cm3), liquids (g/mL) and gases (g/L).
1.1.4: Energy and Work
Read this webpage. Notice the distinctions made between heat and temperature. While both deal with kinetic energy, the energy of motion, "heat" refers to thermal energy transfer, while "temperature" is a measure of the kinetic energy of a system. Potential energy, the energy of position, in chemistry usually refers to the energy stored in chemical bonds. This material will be discussed in more detail in Unit 6.
1.1.5: Composition
1.1.5.1: Homogeneous versus Heterogeneous
Read the "How do we classify matter?" section. All matter can be classified as either a pure substance or a mixture. Furthermore, for a pure substance a subcategory of either single element or compound can be applied. Mixtures are further categorized as either homogeneous (e.g., single phase) or heterogeneous (e.g., multiple phases). The distinction between homogeneous and heterogeneous mixtures presented here is dependent on phase, or physical, boundaries. This section also contains material relevant to the next section of the course.
1.1.5.2: Mixtures and Pure Substances
Read the "Chemical Composition" section. Keep in mind that mixtures, whether homogeneous or heterogeneous, can be separated by physical means into pure substances. Techniques of separation were discussed in the previous section. Pure substances comprise elements and compounds.
1.1.6: Chemical versus Physical Changes
Read the "Chemical Change," "Energetics of Chemical Change," and "Dynamics of Chemical Change" sections. The energetics of chemical change will be discussed more thoroughly in Unit 6. To determine if you are dealing with a physical or chemical change, ask yourself if you can reverse the process to recover the original material. For example, ice melting is a physical change, because you can re-freeze the water; however, cooking a steak is a chemical change, because you cannot recover the raw meat.