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Understanding Matter and Energy: The Basics of Chemistry

This overview explores the fundamental concepts of matter and energy in chemistry. It defines energy as the capacity to do work or produce heat, explaining its forms including kinetic, potential, mechanical, and chemical energy. Matter is defined as anything with mass and volume, classified into elements and compounds. The text also introduces the law of conservation of energy and matter, emphasizing that neither can be created or destroyed. Furthermore, it discusses physical and chemical properties, changes in matter, and the importance of mixtures along with their classifications.

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Understanding Matter and Energy: The Basics of Chemistry

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  1. Matter and Energy Applied Chemistry

  2. Matter and Energy • The universe is made of matter and energy. • Energy • Definition: The capacity to do work or produce heat. • Common unit: calorie abbreviated cal • SI unit: Joule abbreviated J

  3. Types of Energy • Radiant Energy is energy transferred through waves without matter. • Ex. Sunlight • Kinetic Energy is energy of motion. • Walking, Running, Water flowing • Potential Energy is energy of position or stored energy. • Ball at the top of a hill, battery

  4. Potential and Kinetic Energy

  5. Forms of Energy Mechanical, Heat, Chemical, Electrical, Radiant, Sound, Nuclear

  6. Law of Conservation of Energy • Energy is neither created nor destroyed. • Energy can change from one form to another.

  7. Matter • Definition: anything that has mass and volume. • States of matter: • Solid s • Liquid l • Gas g • Plasma -----

  8. Identification Table

  9. Matter • Change is state is also known as a phase change. Temperature vs. Heat Animation

  10. States of Matter Solid deposition melting sublimation freezing condensing evaporating Liquid Gas

  11. Properties or Characteristics of Matter • A physical property is a property observed or measured without changing the material. • Example: color, density, shape, melting point, boiling point • A chemical property is a property that refers to the ability of a material to undergo a change that alters its structure. • Examples: flammability, light sensitivity

  12. Changes in Matter • All changes involve a change in energy. • Physical changes: Do NOT change the identity of a substance. • Ex) size, shape, state, and dissolving • Chemical changes: Do change the identity of a substance. • Ex) burning, digesting food, rusting

  13. Signs of a chemical change • Change in color • Formation of a precipitate (cloudiness; solid formed from 2 solutions) • Production of a gas (bubbles; fizzing) • Increase or decrease in temperature • Change or production of an odor

  14. Chemical Equation – a shorthand way to • write a chemical change • Starting materials are called reactants • Newly formed materials are called products • Reactants products yields Iron + Oxygen Rust

  15. Law of Conservation of Matter • Matter is neither created nor destroyed. • Shown by the French chemist Antoine Lavoisier in the 1700s. He is known as the Father of Chemistry. mass of reactants = mass of products

  16. Classification of Matter

  17. Elements • Contain only 1 type of atom. • Cannot be broken down by ordinary means. (physical or chemical) • Ancient Greeks believed there were only 4 elements. (earth, air, fire, and water) • 92 naturally occurring elements. Others are short-lived, man-made elements.

  18. Elements • A symbol is a shorthand way of writing the name of an element. represents 1 atom of an element • Consists of 1 or 2 letters. • 1st letter is ALWAYS capitalized. • Subsequent letter is lower case. • 3-letter symbols are temporary designations assigned by IUPAC.

  19. Elements • Using your periodic table, find the symbols for the following elements: • Hydrogen • Helium • Carbon • Chlorine • The number of elements as a solid, liquid, or gas at room temperature • 2 liquids • 11 gases • Others are solids H He C Cl

  20. Compounds • Contain 2 or more different elements that are chemically combined. • Can be broken down by chemical processes, such as heat and electricity. • Smallest part of a compound is a molecule.

  21. Compounds • A formula is a shorthand way of writing the name of a compound. It shows… • Which elements are present • The ratio of the elements present.

  22. Examples of Formulas • H2O: the 2 is called a subscript that tells you that 2 atoms of hydrogen combine with 1 atom of oxygen to form 1 molecule of water. • 3H2O is read as 3 molecules of water. The 3 is called the coefficient. There are 6 hydrogen atoms and 3 oxygen atoms

  23. Identify the following substances as elements or compounds. • Co Element • CS Compound • CO Compound • Mg Element • Note: If two capital letters are present, it is a compound.

  24. Counting Atoms in Compound • Step 1: List all elements present • Step 2: Identify the coefficient • Step 3: Count the number of atoms of each element in the compound. • Step 4: Multiply the coefficient by the subscript • Step 5: Add up all the atoms

  25. Counting Atoms • Na2SO4 7 atoms • Ca(OH)25 atoms • 3 Fe2(SO3)342 atoms

  26. Pure Substances

  27. Mixtures • Mixtures contain elements or compounds that are mixed together but not chemically joined. • Types of Mixtures • Homogeneous Mixture or Solution • Heterogeneous Mixture or Mechanical Mixture

  28. Homogeneous Mixtures • Uniform throughout • Not visibly different • Examples: • Gasoline • Food coloring • 14 caret gold • Air • Brass • lemonade

  29. Examples of Alloys Brass is an alloy of copper and zinc. Steel is an alloy of carbon and iron. Bronze is an alloy of copper and tin.

  30. Heterogeneous Mixtures • Not uniform throughout • Visibly different • Examples: • Oil & vinegar • Salad • Concrete • Soup • Sand and water

  31. Homogeneous vs. Heterogeneous Mixtures

  32. Separationof Heterogeneous Mixtures:Filtration • Separate suspended particles from a clear liquid by pouring through a screen, filter, or porous substance. • Filtrate: the liquid that passes through the filter • Residue: the solid left on the filter • Examples: car filter, pool filter

  33. Filtration

  34. Separation of Heterogeneous Mixtures: Magnetic Method & Decanting • Magnetic Method • Separate magnetic substances from nonmagnetic substances. • Examples: iron filings and sulfur recycling center • Decanting • Separate liquids due to a difference in density • Example: oil from water

  35. Heterogeneous liquids can be decanted.

  36. Decanting Diagram

  37. Separation of Homogeneous Mixtures: Chromotography • Separate pigments of ink using strips of paper. • Remember Pete Cheat Lab • Examples: dyes and chlorophyll

  38. Chromatography

  39. Separation of Homogeneous Mixtures: Distillation • Separate solution by a difference in boiling point. The liquids will evaporate and then condense back to a liquid. • Ex. Salt water, crude oil • Distillation Demo • A Closer Look at Distillation

  40. Distillation

  41. Separation of Homogeneous Mixtures: Crystallization • Separate a solution by evaporating the liquid and the solid will recrystallize. • Examples: rock candy, salt water

  42. Crystallization

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