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Chemistry Survival Guide

Chemistry Survival Guide. A Visual Guide to Understanding Chemistry. Table of Contents. Intro to Chemistry. Nuclear Chemistry. Atomic Structure. Gas Laws. Periodic Table. Thermochemistry. Compounds. Solutions. Quantitative Chemistry. Acids & Bases. “Chemistry in the Real World”.

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Chemistry Survival Guide

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  1. Chemistry Survival Guide A Visual Guide to Understanding Chemistry

  2. Table of Contents Intro to Chemistry Nuclear Chemistry Atomic Structure Gas Laws Periodic Table Thermochemistry Compounds Solutions Quantitative Chemistry Acids & Bases “Chemistry in the Real World”

  3. Rationale The science community* has increasingly identified the content focus and the instructional practices as the two areas most in need of change (McCleery & Tindal, 1999). *(National Science Teachers Association, the American Association for the Advancement of Science, and the National Science Foundation Education Association)

  4. Methods of Instruction Explicit Instruction Teaching in Small Steps Guiding Students During Initial Practice Providing High Levels of Successful Practice Rule-Based Approach Focusing the Content Sequencing Activities Minimizing Learner Demands

  5. Principles of Universal Design Flexible Curricula Multiple Representations of Presented Information Multiple Means of Expression and Control Multiple Means of Motivating and Engaging Students (Orkwis, 1999)

  6. Curriculum Models Intensified: Hands-On Theme-Based: Long Term Activities Interrelationships Among Unifying Processes (Cawley, Foley, & Miller, 2003)

  7. Introduction to Chemistry Classifying Matter Calculating Density Accuracy & Precision Calculating Percent Error Metric System & UnitConversion Scientific Notation Physical vs. Chemical Properties Pure Substances Mixtures & Compounds

  8. Classification of Matter Matter Mixture Substance Element Compound Hetero geneous Homo geneous

  9. Classification of Matter

  10. Calculating Density DENSITY: A physical property of matter, measured in: grams, or g/ml or g/cm3 D = M/V Density = Mass divided by Volume (g or g/ml or g/cm3) M = D  V Mass = Density times Volume (in grams) V = M/D Volume = Mass divided by Density ( in ml, l, cm3) V = LWH Volume = Length times Width times Height (cm3) M D V

  11. Calculating Density M D V Density = Mass / Volume

  12. Calculating Density M D V Mass = Density x Volume

  13. Calculating Density M D V Volume = Mass / Density

  14. Accuracy & Precision Accuracy = How close a measured value is to the true or accepted value. Precision = How close together a group of measurements actually are to each other.

  15. Inaccurate & Imprecise

  16. Inaccurate & Precise

  17. Accurate & Precise

  18. Calculating Percent Error ( Accepted Value - Measured Value = Error) 1.0 - .98 = .02 (Error / Accepted Value x 100% = % Error) .02/1.0 = .02 x 100 = 2%

  19. Metric System & Unit Conversion

  20. Metric System & Unit Conversion

  21. Scientific Notation 6028 006 . .

  22. Physical vs. Chemical Properties

  23. Physical Changes Chemical Changes

  24. Pure Substances, Mixtures & Compounds

  25. Atomic Structure Atomic Scientists Atomic Structure Orbital Filling Diagram

  26. Atomic Scientists John Dalton Atoms are indestructible, indivisible, and identical. Combine in simple ratios called the Law of Definite Proportions. Atoms are not created or destroyed during a reaction. JJ Thomson Cathode Ray tube experiment Plum Pudding model Opposite charged particles (electrons) attract

  27. Atomic Scientists Ernest Rutherford Alpha Particles and Gold Foil experiment Atoms are mostly “empty space” Nucleus is small but has almost all of atom’s mass Niels Bohr Planetary model Electrons occupy specific orbits around the nucleus

  28. Atomic Structure

  29. Atomic Structure ATOMIC NUMBER 8 ELEMENT SYMBOL O MASS NUMBER 15.999 ELECTRON CONFIGURATION 1S22S22P4

  30. Orbital Filling Diagram ALUMINUM Z=13 1S2 2S2 2P6 3S2 3P1 3P1 3S2 2P6 2S2 1S2

  31. Periodic Table Protons, Electrons & Neutrons Periodic Table of the Elements Periods & Groups Blocks Trends Ions

  32. Periodic Table Atomic Number = Number of Protons Number of Protons = Number of Electrons Mass Number – Atomic Number = Number of Neutrons # of P’s = # of E’s Mass # - Atomic # = # of N’s

  33. Periodic Table

  34. Periodic Table Arranged horizontally in PERIODS Arranged vertically in GROUPS

  35. Periodic Table Arranged in BLOCKS (S, D, P, F) D P S F

  36. Periodic Trends Atomic Radius & Metallic Character Ionization Energy & Electronegativity DECREASES ACROSS A PERIOD INCREASES ACROSS A PERIOD INCREASES DOWN A GROUP DECREASES DOWN A GROUP

  37. Ions 1+ 2+ 3+ 3- 2- 1- Group 13 Group 15 Group 16 Group 17 Group 1 Group 2

  38. Compounds Binary Ionic Compounds Bonding Writing Formulas Lewis Dot Structures

  39. Compounds IONIC COMPOUNDS: Any chemical compound that is composed of oppositely charged ions NAMING BINARY IONIC COMPOUNDS: The name of the CATION followed by The name of the ANION + IDE

  40. Compounds NAMING BINARY COMPOUNDS OF TWO NONMETALS (Given formula, write name) Do Not use the prefix “mono” for the 1st element Use the prefixes (1-10) and end in IDE N2O = Dinitrogen Monoxide NO2 = Nitrogen Dioxide

  41. Bonding BONDING IONIC MOLECULAR COVALENT BOND Metal & Non-Metal Non – Metal & Non-Metal 1, Name the 1st element 1. Do not use Roman Numerals 2. Make the 2nd element = IDE2. Use Prefixes ( Mono, Di, Tri) 3. Use Roman Numerals ( I, II, III) 3. 2nd element ALWAYS has if Transition Element (3-12) PREFIX & IDE 4. Reduce to lowest terms 4. Do Not Reduce

  42. Comparing Bond Types

  43. Bonding e Sodium Nitride e e e e Na e e e e e e e e e e e e e e Na e N e e e e e e e e e e e e e e Na Na3N e e e e e e

  44. Writing Formulas Formulas are created by the “CROSS-OVER” Method Sodium (Na) & Nitrogen (N) - + N Na 3 Na3N Sodium Nitride =

  45. Writing Formulas Transition Metals Groups (3-12) & The Ions They Form Cation Anion Iron = Fe3+ Chlorine = Cl - - + 3 Fe Cl Fe Cl3 Iron (III) Chloride =

  46. Transition Metals Lead (Pb) & Flourine (F) - 2 + Pb F Lead (II) Fluoride = Pb F2

  47. Lewis Dot Structures O H H Oxygen has 6 valence electrons Hydrogen has 1 valence electron Hydrogen has 1 valence electron 8 electrons in the valence shell is stable Obey the Octet Rule

  48. Lewis Dot Structures H2O H H O Dihydrogen Monoxide =

  49. Quantitative Chemistry ( Moles! ) Moles & the Mole Concept Stoichiometry Percent (%) Composition Molecular & Empirical Formulas Balancing Chemical Equations Types of Reactions

  50. Quantitative Chemistry ( Moles! ) Moles & #’s of Particles Multiply by 6.02 x 1023 Moles # of Atoms Particles Molecules Divide by 6.02 x 1023

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