CHEM 1001 1st Edition Lecture 2Outline of Last Lecture I. Syllabus Outline of Current Lecture I. Definitions a. Chemistry II. Classifications a. States of MatterIII. Properties of Mattera. Physical and Chemical b. Intensive and Extensive IV. Measurement Units a. SI Units V. Measurement Uncertainty a. Significant Figures Current LectureI. Chemistry – the study of matter, its properties, and the changes that matter undergoes a. Matter: the physical material of the universe i. Composition – what atoms?ii. Structure – how are atoms connected?iii. PropertiesThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.1. Macroscopic: properties and behaviors we can see 2. Submicroscopic: properties and behaviors we cannot see b. Atom: the building block of matterc. Element: the unique types of atoms d. Molecule: combination of atoms joined together by chemical bondse. Property: any characteristic that lets us recognizeII. Classifications of Matter a. States of Matteri. Gas1. No fixed volume 2. Conforms to volume and shape of container3. Particles far apart moving rapidlyii. Liquid 1. Distinct volume but no shape 2. Assumes shape of portion of container it occupies3. Particles packed close together and moving rapidly (can be poured)iii. Solid 1. Distinct shape and volume 2. Particles held tightly together with little movement b. Pure Substance i. Matter with distinct properties and constant composition ii. Can be either element or compound (substance formed from two or more elements)c. Mixturei. Combination of two or more pure substances ii. Relative amounts of components can varyiii. Each component retains its own properties iv. Homogenous mixture1. Kool-aid2. Also called a solution v. Heterogeneous 1. Chocolate Chip cookie III. Properties of Matter a. Physical Properties i. Observe without changing the identity or composition of a substanceb. Chemical Propertiesi. Describe the way a substance may change or react to form other substancesc. Intensive Property i. Does not depend on amount of sampleii. Some can be used to identify substancesiii. Ex: Melting Point, density, temperatured. Extensive Propertyi. Depends on the amount of sample ii. Ex: Mass, Volume IV. Measurement Units a. Base Units (SI units)i. Length 1. Meter (m)ii. Mass1. Kilogram (kg)iii. Time 1. Second (s)iv. Temperature1. Kelvin (K)2. Degree C = K – 273.15a. Degree F = 1.8 (Degree C +32)v. Amount of substance1. mole (mol)vi. Electrical current 1. Ampere (A)vii. Luminous intensity 1. Candela (cd)V. Measurement Uncertainty a. Rules for determining which digits are significant i. All digits are significant except zeros that are used only to position the decimal pointii. Make sure that the measured quantity has a decimal pointiii. Start at the left of the number and move right until you reach the first nonzero digit iv. Count that digit and every digit to its right as significant b. Adding and subtracting Significant Figuresi. The answer has the same number of decimal places as there are in the measurement with the fewest decimal placesc. Multiplication and division i. The answer contains the same number of sig figs as there are in the measurement with the fewest sig figs d. Rounding off Numbersi. More then 51. Round upii. Less than 51. Round down iii. Is 51. Followed by other numbers than zero a. Round up only if it is even; odd stays the same b. Ex: 17.75 = 17.8, but 17.65 = 17.62. Followed by all zeros a. Round