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Matter – Properties and Changes (chapter 3)

Learn about the properties of substances, including atoms and compounds, and explore physical and chemical properties. Discover the different states of matter, the law of conservation of mass, and the various techniques for separating mixtures.

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Matter – Properties and Changes (chapter 3)

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  1. Matter – Properties and Changes(chapter 3) • Substances – matter that has a uniform and unchanging composition • Atoms and Compounds like table salt, sugar, CO2 • Physical properties can be observed without changing the sample’s composition • Color, texture, density, melting point • Chemical properties are the result when a sample composition is altered • Color “changes”, rusting, odor

  2. States of Matter Solids Liquids Gases

  3. Law of Conservation of Mass Mass cannot be created nor destroyed. Consider the following decomposition reaction 2 H2O2 2 H2O + O2 If 72 grams of water and 64 grams of oxygen are produced, what mass of H2O2 decomposed? a. 72 grams b. 136 grams c. 64 grams d. Not enough information given

  4. Mixtures • Heterogeneous mixture • Individual components are often easily separated

  5. Homogenous mixtures Also known as solutions. Individual components are non-identifiable. Solvents do the dissolving Solutes are what get dissolved.

  6. Separating mixtures Filtration Distillation Crystallization Chromatography

  7. Elements • Pure substances not separated into anything simpler. • 91 naturally occurring elements • Rules for writing symbols • 1st letter is capitalized • The Periodic Table…a quick look…

  8. Compounds A combination of 2+ different elements that are chemically combined

  9. Law of Definite Proportions • Individual compounds are composed of the same elements and proportion by mass. • Glucose (C6H12O6) • C = 42.2% • H = 6.5% • O = 51.3%

  10. Law of Multiple Proportions Question: What does the law of multiple proportions mean? Answer: Let's see an example: Hydrogen can react with oxygen in a couple of different ways. One way occurs when you take two moles of hydrogen and react it with one mole of oxygen. When you do this, you make H2O. Another way occurs when you take one mole of hydrogen and react it with one mole of oxygen: When you do this, you make H2O2. In the first case, two moles of hydrogen weigh 4 grams and one mole of oxygen weighs 32 grams. The ratio of oxygen to hydrogen is 8:1. In the second case, one mole of hydrogen weighs 2 grams and one mole of oxygen weighs 32 grams. The ratio of oxygen to hydrogen is 16:1. Since 16 is equal to 8 x 2, this satisfies the law of multiple proportions. What you'll find is that any time two elements can form more than one compound with each other, this kind of relationship between the masses takes place.

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