CHM 103 1nd EditionExam # 1 Study Guide Lectures: 1 - 5Lecture 1 (September 3)Introduction to Atoms and Molecules What is an atom? What is a molecule? How do these two things correlate with matter?Atom:- An atom is the fundamental building blocks of ordinary matter. They are minuscule particles that can also bind together. An example of an atom would be an oxygen atom or a carbon atom.Molecule: - A molecule is a combination of atoms held together in specific shapes. The properties ofsubstances depend on the atoms and molecules that compose the substance. An example of a molecule would be a carbon monoxide molecule.How they Correlate with Matter:- Matter is built up of molecules and atoms. Matter is what occupies space and without molecules and atoms there would be no matter. The science of chemistry studies the behavior of matter by studying the behavior of atoms and molecules. Lecture 2 (September 5)More on Matter What are the three different classifications of matter? Describe the molecules state in each classification. Describe what a chemical and physical property is. Describe what a chemical andphysical change is. Classify matter according to its composition.Three Classifications of Matter:- Solid: Molecules are tightly packed together and vibrate but do not move. The solid hasa fixed volume and a rigid shape.- Liquid: Molecules and atoms are still packed closely together but are free to move around each other. Therefore, liquids have a fixed volume but not a fixed shape. They assume the shape of their container.- Gas: Molecules and atoms have a lot of room to move around rapidly. This cause a lot of collisions between the molecules and atoms. Gasses are compressible and always assume the shape and volume of the container they are in. Physical and Chemical Properties:- Physical Properties: Property that a substance displays without changing its composition. Examples would be color, odor, density, hardness, melting and boiling point, conductivity or solubility.- Chemical Properties: Property that a substance displays only by changing its composition via a chemical change. Examples would be corrosiveness, flammability, acidity, toxicity, etc...Physical and Chemical Changes:- Physical Changes: Changes that alter only state or appearance but not composition. Atoms or molecules making up a substance do not change their identity in a physical change. An example would be when water boils, it changes its state from a liquid to a gas but the gas remains composed of water molecules.- Chemical Changes: Changes that alter the composition of matter. Atoms rearrange, transforming the original substances into different substances. An example would be the burning of propane gas. Propane changes to carbon dioxide and water when it is burned. Matter according to its composition:- Pure substance: Composed of only a single type of atom or molecule. Pure substances can be categorized into two types; elements and compounds.- Element: Substance that cannot be chemically broken down into a simpler substance. An example would be Helium.- Compound: Substance composed of two or more elements in fixed, definite proportions. An example would be pure water. - Mixture: Composed of two or more types of atoms or molecules that can be combined in variable proportions. Mixtures can also be categorized into two types (heterogeneousand homogeneous) depending on how uniformly the substances within them mix. - Heterogeneous: Composition varies from one region of the mixture to another. An example would be wet sand. - Homogeneous: Holds the same composition throughout the entire mixture. An example would be tea with sugar.Lecture 3 (September 8)Units, Significant Figures and DensityMemorize specific units of measurements. What is a prefix multiplier? What are the formulas for converting different temperatures? How does one measure density? What are significant figures and how do they work? How does one solve a chemical problem?Units of Measurements to Remember:Quantity Unit SymbolLength Meter mMassKilogramkgTime Second sTemperature Kelvin KAmount ofSubstance Mole molPrefix Symbol Multiplier 10xkilo k 1000 10³centi c 0.01 10¯²milli m 0.001 10¯³micro μ 0.000001 10¯⁶nano n0.00000000110¯⁹Prefix Multiplier:- Prefix multipliers change the value of the unit by powers of 10 such as an exponent doesin scientific notation. For example, 1 kilometer = 1000 meters = 10³ meters.Formulas for Converting Temperature:Celsius  Fahrenheit = (°C × 9/5) + 32 = °FFahrenheit  Celsius = (°F − 32) x 5/9 = °CCelsius  Kelvin = °C + 273.15 = KDensity Formula:- Density (d) of a substance is the ratio of its mass (m) to its volume (V). So by knowing the volume and mass of a substance, one can divide the two to find the density. It is an example of an intensive property or one that is independent of the amount of the substance. - Mass in measure in grams (g) and volume is measured in either centimeters cubed (cm³) or milliliters (mL).Significant Figures and their Rules:- Significant figures (sig figs) are the non-holding-place digits that are not marking the decimal place recorded in any measurement. - Certain rules to follow when using sig figs are as follows:1. All nonzero digits are significant.2. Interior zeroes are significant.3. Leading zeroes, or zeroes to the left of the first nonzero digit, are not significant. They only serveas place holders for the decimal point. 4. Trailing zeroes after a decimal point are always significant.5. Trailing zeroes before a decimal point but also after a nonzero number are always significant. 6. Trailing zeroes before an implied decimal point are ambiguous and should be changed to scientific notation. - Examples for each rule are as follows:1. 23.05 and 0.02302. 503 and 4.04013. 0.0032 and 0.0000054. 43.000 and 2.34005. 120.00 and 3400.446. 1200 – ambiguous 1.2 X 10³ - 2 sig figs1.20 X 10³ - 3 sig figs1.200 X 10³ - 4 sig figsSolving Chemical Problems:- Units behave just like numbers in math.- What data are we given?- What quantity do we need?- What conversion factors are available to take us from what we are given to what we need?Formula: Given Unit ×Desired UnitGiven Unit=Desired UnitLecture 4 (September 10)The Atomic Theory, Elements and the Periodic Table What is the Atomic Theory? What were the laws that led up to the Atomic Theory? What is the structure of an atom? What is an Isotope? What is an Ion?