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Chapter 1 Chemistry: the study of the composition of matter and the changes it undergoes (what stuff is made of, and how it reacts) Chapter 3 Quantitative vs. Qualitative Pure chemistry: studying chemistry just for the sake of knowing -Quantitative = QUANTITY = NUMBERS (It is 39 degrees Organic Chemistry: study of substances containing CARBON Inorganic Chemistry: study of substances the DO NOT contain carbon Analytical Chemistry: the study of the composition of substances Physical Chemistry: study of theories and experiments that describe the BEHAVIOR of chemicals Celsius) -Qualitative = QUALITY = NO NUMBERS (it is hot) Scientific Notation -Move the decimal behind the first non-zero digit -Count the number of ‘jumps’ Biochemistry: study of the chemistry of living organisms -Jump right? Negative exponent Scientific Method: a logical approach to the solution of scientific problems -Jump left? Positive exponent Steps: Observe, form a hypothesis, experiment, repeat Accuracy/Precision/Error Hypothesis: proposed explanation for what is observed -Accuracy: How close your values are to the ‘true value’ Theory: a broad and extensively tested explanation as to why experiments give certain results (almost certainly true) Scientific law: describes a natural phenomenon without explaining the why -Precision: How close your measurements are to each other. -Error: ‘How wrong were you?’ … This is the difference between your value and the accepted value (difference means SUBTRACT) Chapter 2 -Percent Error: Error/accepted value x 100 Matter: anything that has mass and takes up space Significant figures Mass: amount of matter an object contains KNOW THE RULES! Substance: matter that has a definite and uniform composition 1. Physical Property: a quality of an object that can be observed without changing the substances composition (color, weight, boiling point) Physical Changes: a change that alters a material without changing its composition (ex. Water is still water, even when frozen) 2. 3. 4. Mixture: physical blend of two or more substances 5. Heterogeneous: not uniform (salad) 6. Homogeneous: uniform (salt water) also called SOLUTIONS Phase: any part pf a system with uniform composition and properties Elements: simplest forms of matter that cannot be separated by chemical means Compound: substances that can be separated into simpler substances by chemical means Chemical Reaction: when one or more substances change into new substances Reactants: the starting substances (the ones that REACT) Products: the substances formed (or the ones that are PRODUCED) Chemical property: the ability of a substance to undergo a chemical reaction and to form new substances Chemical change: always results in a change of composition of the substance (burning) Law of Conservation of Mass: in any physical change or chemical reaction, mass is neither created or destroyed; it is conserved 7. Every non-zero digit is significant= 1,234 has 4 significant figures Zeros between non-zero digits are significant = 1001 has 4 significant figures Leftmost zeros before a nonzero digit are NOT significant = 0.000012 has 2 significant figures Zeros at the end of a number AND to the right of a decimal point ARE significant 100.23 has 5 significant figures Zeros at the end with no decimal point are NOT significant = 1,000,000 has 1 significant figure When adding/subtracting, line up decimal point and round your answer to the least number of DECIMAL places in the problem = 2.14 + 2.1 = 4.2 (The answer has 1 decimal place because that is the lowest number of decimal places) When Multiplying/dividing, round your answer to the least number of significant figures SI system of Measurement Length = meter Volume = cubic meter Mass = Kilogram Temperature = kelvin Time = second Convert!!! mega (M) 1,000,000 times larger than the unit kilo (k) 1,000 times larger than the unit deci (d) 1/10 the size of the unit cent (c) 1/100 the size of the unit milli (m) 1/1000 the size of the unit Atomic Mass Unit (amu): unit for atomic mass micro ( ) 1/1,000,000 the size of the unit. Periodic Table Mendeleev: Arranged by atomic mass Density Mosely: arranged by atomic number Density= relationship between and objects mass and volume Periods: horizontal rows Density = mass/volume Groups/Families: Vertical columns Temperature Periodic law: when the elements are arranged by increasing atomic number, there is a pattern to their properties Temperature shows us the heat transfer Group 1A; Alkali Metals Feels cold to you? Heat going to that object Group 2A: Alkaline Earth Metals Feels hot to you? Heat going from object to you Group 7A: Halogens Temperature scales Group 8: Noble Gases Celsius = based on freezing point and boiling point of water Metals to the left, nonmetals to the right, metalloids on the zigzag line Kelvin = based on ABSOLUTE ZERO Know how to find the # of protons, neutrons, electrons K = Degrees Celsius + 273 Degrees Celsius = K – 273 What type of questions will you see? 1. 2. 3. 4. 5. 6. Conversion questions. For example, how many grams in 27.4 kilograms? Significant figures a. Count them, round to a specific significant figure, add/subtract/multiply/divide Write in scientific notation Is it accurate? Precise? What is the percent error? Be able to solve for the missing value in a density problem Temperature conversion: kelvin-Celsius and reverse Chapter 5 Democritus: reasoned that all things were made up of ATOMS Dalton: developed the ATOMIC THEORY 1. 2. 3. 4. All elements are made up of atoms Atoms of the same element are identical Atoms can be combined with other atoms Chemical reactions occur when atoms are separated or combined J.J. Thompson: ELECTRON Millikan: charge and mass of the electron Goldstein: PROTON Chadwick: NEUTRON Rutherford: Most of an atom is empty space Atomic Number: number of protons in the nucleus of an atom (also electrons) Mass Number: the total number of protons and neutrons in an atom Neutrons = mass number – atomic number Isotopes: Atoms with the same number of protons, but different numbers of neutrons