1.1 INTRO TO MATTER-solids ,liquids and gases

matter

1. TOPIC 1 STOICHIOMETRIC RELATIONSHIPS 1.1 INTRODUCTION TO THE PARTICULATE NATURE OF MATTER AND CHEMICAL CHANGE

2. ESSENTIAL IDEA Physical and chemical properties depend on the ways in which different atoms combine. NATURE OF SCIENCE (3.1) Making quantitative measurements with replicates to ensure reliability – definite and multiple proportions.

3. INTERNATIONAL-MINDEDNESS Chemical symbols and equations are international, enabling effective communication amongst scientists without need for translation. IUPAC (International Union of Pure and Applied Chemistry) is the world authority in developing standardized nomenclature for both organic and inorganic compounds,

4. THEORY OF KNOWLEDGE Chemical equations are the “language” of chemistry. How does the use of universal languages help and hinder the pursuit of knowledge? Lavoisier’s discovery of oxygen, which overturned the phlogiston theory of combustion, is an example of a paradigm shift. How does scientific knowledge progress?

5. UNDERSTANDINGS/KEY IDEA 1.1.A Atoms of different elements combine in fixed ratios to form compounds, which have different properties from their component elements.

6. UNDERSTANDINGS/KEY IDEA 1.1.B Mixtures contain more than one element and/or compound that are not chemically bonded together and so retain their individual properties.

7. UNDERSTANDINGS/KEY IDEA 1.1.C Mixtures are either homogeneous or heterogeneous.

8. Chemistry: Chemistry is the study of what things are made up of, and the changes that they undergo

9. MATTER (Pure) Substances Mixtures Homogeneous Heterogeneous Anything that has mass and takes up space Physical combinations of two or more substances Uniform throughout, aka “solution”; Think: smoothie Not uniform throughout, distinct pieces; Think: fruit salad

10. Pure Substances: Elements & Compounds occur naturally, same composition throughout the substance and everywhere in the world

11. MATTER (Pure) Substances Mixtures Elements Compounds Homogeneous Heterogeneous Stuff that has mass and takes up space Have a specific or definite composition (homogeneous) Physical combinations or two or more substances Uniform throughout, aka “solution”; Think: smoothie Not uniform throughout, distinct pieces; Think: fruit salad

12. Elements Elements: The simplest form of matter Cannot be broken down or separated into a simpler substance Building blocks for all other substances Found on the periodic table of elements

13. MATTER (Pure) Substances Mixtures Elements Compounds Homogeneous Heterogeneous Anything that has mass and takes up space Have a specific or definite composition (homogeneous) Physical combinations of two or more substances Examples: iron sulfur, carbon, Hydrogen, oxygen Uniform throughout, aka “solution”; Think: smoothie Not uniform throughout, distinct pieces; Think: fruit salad

14. Compounds Compounds: Chemical combination of 2 or more substances Cannot be physically separated Have properties different than the elements that are combined

15. MATTER (Pure) Substances Mixtures Elements Compounds Homogeneous Heterogeneous Stuff that has mass and takes up space Have a specific or definite composition (homogeneous) Physical combinations of two or more substances Examples: iron sulfur, carbon, Hydrogen, oxygen Examples: water, salt, sugar Uniform throughout, aka “solution”; Think: smoothie Not uniform throughout, distinct pieces; Think: fruit salad

16. APPLICATION/SKILLS Be able to deduce chemical equations when reactants and products are specified.

17. Atoms cannot be created or destroyed in a chemical reaction, they can only be rearranged. The reactants (substances on the left side of the arrow) are transformed into products (substances on the right side of the arrow). All chemical reactions must be balanced – the number of atoms of each element must be the same on each side of the equation.

18. The coefficients in an equation give the molar ratios of the reactants and products. 2H 2(g) + O 2(g) 🡪 2H 2 O (l) This tells us that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.

19. 2H 2(g) + O 2(g) 🡪 2H 2 O (l) The mole ratio is a ratio of the coefficients in the balanced chemical equation. When working stoichiometry problems, the coefficient for the unknown is always on top. The mole ratio of hydrogen to oxygen is 2 to 1. The mole ratio of oxygen to water is 1 to 2.

20. APPLICATION/SKILLS Be able to apply the state symbols (s), (l), (g) and (aq) in equations.

21. 2H 2(g) + O 2(g) 🡪 2H 2 O (l) The states of substances are indicated in parenthesis next to the formula. Solid (s) Liquid (l) Gas (g) Aqueous solution (aq) – indicates that the ions are dissolved in water. A single arrow 🡪 means the rxn essentially goes to completion. A double arrow means equilibrium.

22. APPLICATION/SKILLS Be able to explain the observable changes in physical properties and temperature during changes of state.

23. Heating/Cooling Curve www.gcps.desire2learn.com

24. APPLICATION/SKILLS Be able to name the changes of state – melting, freezing, vaporization (evaporation and boiling), condensation, sublimation and deposition.

25. Melting: solid to liquid Freezing: liquid to solid Vaporization: liquid to gas Condensation: gas to liquid Sublimation: solid to gas Deposition: gas to solid

26. APPLICATION/SKILLS Be able to balance a variety of reaction types.

27. 5 Basic Types of Reactions 1. Combination or synthesis 2. Decomposition 3. Single Replacement 4. Double Replacement 5. Combustion

28. Combination Reaction where 2 substances combine into a single substance. A + B → AB

29. Decomposition Reaction where 1 substance breaks into 2 or more substances. AB → A + B

30. Single Replacement Reaction where an element replaces a similarly charged ion in a compound. A + BC → B + AC

31. Double Replacement Reaction where two compounds react to produce two new compounds. AD + BC → BD + AC Write the charges on top of the elements in the reactants and exchange the positive ions to make new compounds. You must have a positive followed by a negative to make a compound.

32. Combustion Reaction where an element or compound(usually a hydrocarbon) reacts with oxygen. A + O 2 → AO 2 CH 2 + O 2 → CO 2 + H 2 O The first example is simply a combination reaction. The second example with the hydrocarbon always produces CO 2 and H 2 O.

33. Citations International Baccalaureate Organization. Chemistry Guide, First assessment 2016. Updated 2015. Brown, Catrin, and Mike Ford.  Higher Level Chemistry . 2nd ed. N.p.: Pearson Baccalaureate, 2014. Print. ISBN 978 1 447 95975 5 eBook 978 1 447 95976 2 Most of the information found in this power point comes directly from this textbook. The power point has been made to directly complement the Higher Level Chemistry textbook by Brown and Ford and is used for direct instructional purposes only.