CHEM 1211K 1st EditionExam # 1 Study Guide Lectures: 1 - 4Lecture 1 (January 14)Composition of MatterWhat is Chemistry? What is matter and how do you classify it? What are the fundamental building blocks of matter? How are atoms related to molecules? Chemistry is defined as the science that seeks to understand the behavior of matter by studyingthe behavior of atoms and molecules.Matter: anything that occupies space and has mass. Classify matter according to its state (physical form: solid, liquid, gas) and its composition (basic components that make it up: example CO) Atom: submicroscopic particles, and the fundamental building blocks of matter. Molecules: two or more atoms combined in a specific geometrical arrangement. Scientific Approach to KnowledgeHow do scientists learn about the world around them? How do you classify observations? What are the steps of the scientific method? How can a hypothesis become a theory? How can a hypothesis become a law? What’s the difference between a law and a theory? Scientists observe the world around them and conduct experiments to gain knowledge. Two types of observations: qualitative and quantitative.Qualitative: observations that describe the behavior or certain characteristics found in nature. Involve information gathered through your senses. Describes how a procedure happens. Quantitative: observations that compare a behavior to a standard numerical scale. Measuring something about the procedure. -Observations lead to hypothesis, which leads to experimentation to try to see if hypothesis is valid/invalid. Hypothesis: tentative explanation of observations. Experiments: highly controlled procedures created to see if idea is valid/invalid.Scientific Law: short statement that summarizes past observations and predicts future observations. Subject to experimentation. Scientific Theory: generalized model for the way nature is, and why. Subject to experimentation.The difference between scientific law and scientific theory is what and why. Scientific law explains what happens in nature; scientific theory explains why things act the way they do in nature. How is matter classified? What is a pure substance? If a pure substance can be decomposed intoa simpler substance what is it called? What is a mixture? What is the difference between homogeneous and heterogeneous mixtures? Matter is classified by its state and its composition. Three different states of matter: 1. Solid: fixed volume, rigid shape, not compressible, doesn’t flow. Crystalline (atoms/molecules form patterns with long range, repeating order. Ex: sugar, salt, diamonds) or amorphous (atoms/molecules do not have any long-range order. Ex: glass, plastic, charcoal)2. Liquid: assumes container’s shape, maintains volume, not compressible, flows.3. Gas: assumes container’s shape, assumes container’s volume, is compressible, flows.Pure Substance: made of only one component and its composition doesn’t vary from sample to sample. -Two categories: element or compoundElement: pure substance that cannot be decomposed into simpler substances. Ex: Gold, Helium Compound: pure substance that can be decomposed into simpler substances.What is a mixture? What is the difference between homogeneous and heterogeneous mixtures?Mixture: made of two or more components in varying proportions depending on the sample.-Mixtures are classified by the uniformity of its composition. Homogeneous Mixture: uniform composition throughout the mixture, identical characteristics. Ex: gasoline, water, tea with sugar Heterogeneous Mixture: composition varies throughout the mixture. Ex: wet sand, chicken noodle soupWhat are possible ways of separating mixtures?Decanting: pouring off water into separate containerDistillation: mixture is boiled to remove more volatile (easily vaporized) liquids.Filtration: mixture is poured through filter paper inside a funnel to separate insoluble solid and the liquid. What’s the difference between physical changes and chemical changes? What are some examples of physical and chemical changes? What’s the difference between physical properties and chemical properties?Physical Changes: changes that don’t alter composition of matter, just state or appearance. Can be reversed. -Ex: water boiling, water freezing, sugar dissolving, ice subliming, Chemical Changes: changes that alter composition of matter, creates different substance. -Ex: rusting of iron, gas burning, Physical Property: substance shows this property without changing compositionChemical Property: substance shows this property after a chemical change and the substance’s original composition has been alteredLecture 2 (January 16)What is energy? How are energy and work related? How are kinetic energy, potential energy, and thermal energy connected to total energy? What is the law of conservation of energy? Energy: the capacity to do work -Any change in matter (physical and/or chemical) results in matter gaining/releasing energyWork: action of a force through a distance-The total energy in an object = kinetic energy + potential energy. Thermal energy is also connected to total energy because thermal energy is a form of kinetic energy. Kinetic Energy: energy associated with object’s motionPotential Energy: energy associated with object’s position/composition-Systems with high potential energy tend to change in a direction that lowers potential energy causing the release of energy into the surrounding areaThermal Energy: energy associated with object’s temperature -form of kinetic energy Law of Conservation of Energy: energy is neither created nor destroyed -Energy can be converted from one form to another-Total amount of energy always remains the sameWhat does SI stand for? What are the base units’ symbols and quantities? Standard Units of Measure (SI units):What is the SI unit for temperature? What are the formulas for converting temperature scales? What are the boiling points, freezing points, and absolute zeros for Fahrenheit, Celsius, and Kelvin? -There are three basic formulas for converting Celsius, Fahrenheit, and Kelvin.Fahrenheit to Celsius: °C = (°F-32) 1.8 Celsius to Fahrenheit: °F = 1.8(°C) + 32Celsius to Kelvin: K = °C + 273.15°- Celsius, Fahrenheit, and Kelvin have separate boiling points, freezing points, and absolute zeros. Temperature scale Boiling Point Freezing Point Absolute ZeroCelsius 100 °C 0.00 °C -273 °C Fahrenheit 212 °F 32 °F