Chemistry: The Study of Matter

1. Chemistry: The Study of Matter Chapter 1

2. Ch. 1 Homework • Ch. 1a on Matter Classification 2, 3a-d, 5-9, 12-15 (both editions) • Ch. 1b on Measurements and Conversions 18, 20, 22-23, 29-31, 33, 35, 39a-c, 40, 43, 47 (both editions)

3. Worldviews The overall perspective with which one sees and interprets the world. • Naturalistic Worldview • Matter is everything and science is the only path to “truth”. • Christian Worldview • Science is the discovery of God's Handiwork in creating matter and all the universe “They exchanged the truth about God for a lie, and worshiped and served created things rather than the Creator-who is forever praised.” Romans 1:25

4. Old Testament Chemistry • Gen. 4:22 • Metallurgy – Extracted pure metals from their minerals/ores (raw earth material). • Created alloys (mixing of metals for desirable properties) • Exod. 30:25 • Apothecary - Used chemicals and herbs for medicinal purposes • “The original pharmacists”

5. Greek Chemistry ~ 430 BC • Democritus's theory – Philosophical atomism (no evidence) • All matter is made up of tiny identical atoms and the difference in materials is based on the shape, position, and arrangement of these atoms. • "Atomos" - indivisible

6. Alchemists • The "original" chemists • Attempted to make gold from other substances. • Impossible challenge • (without nuclear fusion/fission reactions) • Nevertheless, resulted in organized approach to science • Laboratory techniques • Equipment • Terminology

7. Why Study Chemistry? • Creation Mandate • Gen. 1:26, 28 God blessed them, and God said to them, "Be fruitful, multiply, fill the earth, and subdue it. Rule the fish of the sea, the birds of the sky, and every creature that crawls on the earth." (Genesis 1:28 HCSB) • Career Foundation • Pharmacy • Medical • Engineering • Dietician • Agriculture • Environmental • Material science • Critical thinking Skills • Problem solving • Deductive logic • Scientific inquiry

8. Food and Agriculture • Genetically modified crops • “Natural” pesticides • Specialized fertilizers GFP: Green fluorescent protein Chemistry: A Science for the 21st Century • Materials and Technology • Plastics, ceramics, liquid crystals • Room-temperature superconductors? • Molecular computing? • Binary data stored in DNA

9. Fields of Chemistry • Organic - carbon containing compounds (synthesis, plastics, drugs) • Inorganic - all elements minus carbon (metals and coordinating elements)

10. Fields of Chemistry • Biochemistry – organic chemical processes in living things (Biomolecules: proteins, DNA, lipids, carbohydrates) • Analytical – Create/improve chemical techniques used in all branches for precise quantitative measurements. (Purification, sample analysis, water/soil testing) • Physical - foundational theories, detailed study of interaction and energy changes (e- probability, thermodynamics, quantum)

11. 2 Cu + H2O + CO2 + O2 → Cu(OH)2 (s) + CuCO3 (s) The Study of Chemistry: We observe the Macroscopic Macroscopic Microscopic Chemistry explains what’s happening Macroscopically on the Microscopic scale Today 1886 2-6 year Process Oxidized mixture called “Patina”

12. Making Observations List 2 observations of each type you could make • Qualitative observations • Describes the quality of an object • Color, taste, texture, appearance, smell, etc. • Think Adjectives • Quantitative observations • Describes an object using numbers • Count, length, weight, volume • Think Units

13. tested modified The scientific method is a systematic approach to research. Macroscopic Microscopic/Symbolic Explain Observations A hypothesis is a tentative explanation for a set of observations.

14. The scientific method is a systematic approach to research. Hypothetical Method Actual Method * http://www.wired.com/wiredscience/2013/04/whats-wrong-with-the-scientific-method/

15. A theory is a unifying principle that attempts to explain a body of experimental observations. • Theories offer explanations for what we observe. • Theories tell us why we should expect it. • Atomic Theory • Cell Theory • Big bang theory Do not confuse scientific theories as improbable explanations filled with inconsistency. They are often incapable of absoluteproof, but all available data are still in support of them.

16. A law is a concise statement of a relationship between phenomena that is always the same under the same conditions. • Laws describe observations • Often mathematical equations • Laws tell us what we should expect (∝ = directly proportional) Charles’s Law: V ∝ T Newton's 2nd Law: Force = mass x acceleration 2nd law of thermodynamics: Entropy > 0

17. gold ingots silicon crystals liquid nitrogen Chemistry is the study of matter and the changes it undergoes. Matter is anything that occupies space and has mass. A substance is a form of matter that has a definite composition and distinct properties.

18. cement, oil and water, iron filings in sand, insoluble compounds Solutions (soft drink), gas mixtures (air), solder (Sb/Pb alloy) A mixture is a combination of two or more substances in which the substances retain their distinct identities. • Homogenous mixture – composition of the mixture is the same throughout • Heterogeneous mixture – composition is not uniform throughout

19. Heterogeneous or Homogenous? • Chicken Broth • Vegetable beef soup • Air • Vinaigrette dressing (oil/water base) • Salt water

20. Separating Sand/Iron via a magnet Mixture Mixtures can be separated into their pure components by some physical means. *Distillation - Separating two liquid substances by their differing boiling points Pure

21. Physical Properties: can be measured or observed without changing the composition or identity of a substance. • Density: amount of mass per volume of space • Malleability: Hammered into a thin sheet • Ductility: Drawn into long thin strings • Conductivity: Ability to transfer either heat and/or electricity • Phase transition temperatures: temp. where melting/boiling occurs • Appearance: color, luster • Solubility: amount dissolvable in solvent (water) • Hardness: measured by Mohs scale (1: Talc - 10: diamond)

22. Extensive and Intensive Properties of matter An extensive property depends upon how much matter is being considered. • mass • length • volume An intensive property of a material does not depend upon how much matter is being considered. • Density • Temperature • Color • Viscosity

23. sugar dissolving in water ice melting Hydrogen burns in air to form water Types of Changes A physical change does not alter the composition or identity of a substance. A chemical change alters the composition or identity of the substance(s) involved. Metal rusting

24. Chemical Properties: A chemical change must occur to observe: • Temperature change • Color change • Gas production (effervescence) (at constant P&T) • Solid production from solution (precipitation) • Flammability • Toxicity • Acidity/Basicity

25. Physical or Chemical Change? • Grinding coffee beans • Food rotting • Lighting a match • Cutting paper in half • water evaporating to vapor • Jewelry tarnishing • Dissolving salt in water

26. An element is a substance that cannot be separated into simpler substances by chemicalmeans. The first person to discover an element using scientific inquiry was Hennig Brand, a German scientist who discovered phosphorus (P) in 1649. In 1789, a French scientist, Antoine Lavoisier defined what was meant by a chemical element and drew a table that contained 33 known elements • 118 elements have been identified • 98 elements occur naturally (some only in trace amounts) • 20 elements have been synthetically created by scientists

27. Atoms: the basic particles that make up the different elements • Ex. Li, Be, B, C, N, O, F, Ne, Au • Either 1 or 2 letter symbol; first letter capitalized Atoms possess subatomic particles: Neutrons (N0) - no charge, but have mass Protons (P+) - positively charged and have mass Electrons (e-) - negatively charged, but little mass When an atom has equal Protons and Electrons it is Neutral ex. a neutral Helium atom contains 2 P+ and 2 e- Ion: When P+ and e- are unbalanced in an atom, it is Charged. ex. an ionized Sodium ion (Na+1) has 11 P+ and 10 e-

28. Elemental symbols Si ≠ SI aurum Kalium Ferrum Plumbum Argentum Natrium * * *Many are derived from their Latin names *Hydrargyros "water silver" *Wolframite: W containing ore

29. Quartz: SiO4 Lithium fluoride: LiF dry ice – CO2 (carbon dioxide) A compound is a substance composed of atoms of two or more different elements chemically united (bonded) in fixed proportions. Compounds can only be separated (broken down) into their pure components (elements) by chemical means. *Non-compounds are not necessarily always monoatomic (C, He): Can have many element atoms in a substance: P4, S8, Cl2

30. Review of the Nucleus: The Nucleus: Crash Course Chemistry #1 https://www.youtube.com/watch?v=FSyAehMdpyI

31. Classifications of Matter CO2 C O2 H2 ex. Carbonated Water + H2O

32. gas solid liquid The Three States of Matter: Effect of a Hot Poker on a Block of Ice

33. Lab Glassware Non-Quantitative • Borosilicate Glass (SiO2+ B2O3) • Withstands higher temperatures • Lower thermal expansion (hot to cold) • Less likely to shatter • Used to contain chemicals/reactions • Used to heat liquids • Not used to heat solids Erlenmeyer Flask Beaker Used Quantitatively Crucible used instead Graduated Cylinder Volumetric Flask Buret

34. A Comparison: The Three States of Matter Undefined shape, incompressible • Undefined shape • Compressible Defined shape, incompressible

35. A Comparison: The Three States of Matter Four Kinetic Molecular Theory: describes motion of particles in states of matter Random, fast movement of particles (non-interacting) Greater freedom of motion “particles shift/slide” Little particle motion “locked in place” only vibrations Plasma: Charged Gas, effected by magnetic field, Interacting particles

36. Energyis the capacity to do work or produce heat. • Mechanical energy is sum of kinetic (energy of motion) and potential (energy of position). • Thermal energy is the energy associated with the random motion of atoms and molecules (heat). • Encompasses all kinetic energy of particles.

37. Electrical energy – derived from electron potential energy • (Ni → Ni+2 + 2e-) • Chemical energy is the energy stored within the bonds of chemical substances • Nuclear energy is the energy stored within the collection of neutrons and protons in the atom (very exothermic)

38. Electromagnetic energy is the energy associated with electricity and magnetic fields. (visible light, Infrared, UV, Gamma, radiowaves). • Acoustic energy is the movement of particles (kinetic) moving in periodic waves (sound waves).

39. Mass – Energy Equivalence • Matter can be converted to energy • First proposed relationship by Isaac Newton (1717) • Related by a constant • Einstein was the first to derive the equivalence (1905)

40. 1st Law of Thermodynamics: Conservation of Energy • Energy (or matter) is nevergained or lost in a closed system • Energy is only converted from one form to another • Gasoline – Stored chemical energy (in the bonds) • Gasoline + Oxygen combusts → CO2 + H2O + ... • Produces steam to drive pistons (kinetic energy) • Produces heat (thermal energy) • Produces light • Produces sound

41. Thermochemistry is the study of heat change in chemical reactions. Thermal Energy includes all collective kinetic movements & vibrations of particles. • Heat is the transfer of thermal energy between two bodies that are at different temperatures. • Always flows from high to low energy Temperature is a relative measure of the thermal energy. Temperature  Thermal Energy As Temp ↑, Thermal Energy ↑ (particles move faster/collide more)

42. °F = x °C + 32 9 5 A Comparison of Temperature Scales K = 0C + 273.15 0 K = -273.15 0C 0 K = -460 ° F “Water based” (1742) Absolute Scale (1848) (1724) “Weather/human based” Absolute Zero: Theoretical temp where all atomic movements stops

43. Example • Solder is an alloy made of tin and lead that is used in electronic circuits. A certain solder has a melting point of 224°C. What is its melting point in degrees Fahrenheit? • Helium has the lowest boiling point of all the elements at -452°F. Convert this temperature to degrees Celsius. • Mercury, the only metal that exists as a liquid at room temperature, melts at -38.9°C. Convert its melting point to Kelvins. 1.3 Temperature conversion

44. Example • This conversion is carried out by writing • Here we have • The melting point of mercury in Kelvins is given by 1.3 Solution

45. 2H2(g) + O2(g) 2H2O (l) + energy H2O (g) H2O (l) + energy energy + NH4NO3(s) NH4+1 (aq) + NO3-1 (aq) energy + H2O (s) H2O (l) Exothermic process is any process that gives off heat – transfers thermal energy from the system to the surroundings. (Feels hot to the touch) Endothermic process is any process in which heat has to be supplied to the system from the surroundings. (Feels cool to the touch) H2O

46. Review of Energy: Energy and Chemistry: Crash Course Chemistry #17 www.youtube.com/watch?v=GqtUWyDR1fg

47. A 1 kg bar will weigh weight = mass x g (F = m•a) 1 kg on earth on earth, g = 1.0 0.1 kg on moon on moon, g ~ 0.1 Matter - anything that occupies space and has mass • mass – measure of the quantity of matter • SI unit of mass is the kilogram (kg) • 1 kg = 1000 g = 1 x 103 g La Grande K 1 Kg Pt/Ir alloy World’s Roundest Object https://www.youtube.com/watch?v=ZMByI4s-D-Y weight – force that gravity exerts on an object

48. International System of Units (SI) Base Units Used as Relative Standards for comparison Utilized in this class All other units are derived from these units and are known as Derived Units Velocity: m/s Force: 1 Newton = 1 kg•m/s2 Volume: m3

49. Prefixes can be used to simplify for extremely large or small quantities of base units “mu” Used most often in this class, be sure to memorize.

50. *not true