Introduction to Chemistry: Matter, Elements, and Changes

1. Chemistry – Matter and Change Chapter ONE

2. Objectives for Unit 2 SPI 3221.1.2 – Interpret the periodic table to describe an element’s atomic makeup. SPI 3221.2.1 – Distinguish among elements and compounds. SPI 3221.2.4 – Classify as physical or chemical change. SPI 3221.2.5 – Compare and contrast heat/temperature changes in chemical/physical processes. SPI 3221.2.6 – Investigate solids, liquids, and gasses in terms of energy and particle spacing.

3. More Objectives for Unit 2 You will also be able to… - Define and describe “Chemistry” - List the different types of Chemistry - Describe how to separate a mixture - Describe the periodic table and how it is arranged

4. Chemistry: the study of composition, structure, and properties of matter* and the changes it undergoes. *Matter: composed of mass and takes up space.

5. Branches of Chemistry Organic Chemistry – carbon-containing compounds. Inorganic Chemistry – no carbon Physical Chemistry – properties and changes of matter and their relation to energy. Analytical Chemistry – identification of components and composition of materials. Biochemistry – substances and processes occurring in living things. Theoretical Chemistry – use of math and computers to understand chemical behavior and to design/predict the properties of NEW compounds.

6. Elements and Compounds All matter is composed of atoms. Copper pipe is made of copper atoms. Oxygen gas is made of oxygen atoms. An elementis a pure substance made of only one kind of atom. Carbon is an element made of only carbon atoms. Atoms of two or more elements bond together to make compounds. CO2 (___ carbon atom and ___ oxygen atoms) H2O2 (___ hydrogen atoms & ___ oxygen atoms)

7. Physical Properties A characteristic that can be observed or measured without changing the identity of the substance. Examples: boiling and freezing points Physical Change: does not involve a change in identity of the substance…cutting, melting, boiling, freezing, tearing. Change of State: physical change from one state to another. Solid  Liquid (Melting) Liquid  Solid (Freezing) Solid  Gas (Subliming) Gas  Solid (Deposition) Liquid  Gas (Evap./Boil) Gas  Liquid (Condensing) SOLID - LIQUID - GAS - PLASMA

8. STATES OF MATTER • SOLID: • Definite Shape • Definite Volume • Particles move slowly and are close together Video: Potassium • Examples • Sodium metal (Na) • Ice (H2O) • Gold at room temp. (Au)

9. STATES OF MATTER • LIQUID: • No Definite Shape • Definite Volume • Particles move a little faster than solids and more freely. Video: Mercury • Examples • Mercury (Hg) • Bromine (Br2) • Water (H2O) • Gold at high temp. (Au)

10. STATES OF MATTER • GAS: • No Definite Shape • No Definite Volume • Particles move very quickly and are far apart. Video: Chlorine • Examples • Neon (Ne) • Steam (H2O) • Chlorine gas (Cl2)

11. STATES OF MATTER • PLASMA: • High Temperature • Atoms lose electrons easily Video: What is Plasma? • Examples • Sun • Fluorescent Bulbs

12. STATES OF MATTER LIQUID SOLID GAS

13. Group Questions 1. Using microscopic drawings (molecular level), show the difference between a gaseous element and a gaseous compound.

14. Group Questions 2. Heat is applied to an ice cube. Eventually, only steam is present. Draw a molecular-level representation of this process. What happens to the size of the molecules? If you could collect all of the steam, how would the mass of the steam compare to the mass of the original ice cube?

15. Group Questions 3. When you are in the room next to your kitchen, you can smell soup cooking. Why is this??

16. Group Questions 4. Which of the following is true about the state of an individual atom? A) An individual atom can be a solid. B) An individual atom can be a liquid. C) An individual atom can be a gas. D) The state of the atom depends on which element it is (for example, an iron atom is solid, but a helium atom is gaseous.) E) An individual atom cannot be a solid, liquid, or gas.

17. Group Questions 5. Using microscopic drawings (molecular level), show the difference between an atomic element and a molecular element. Explain your drawings.

18. Chemical Properties… …relate how chemicals undergo change. Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant  product carbon + oxygen  carbon dioxide C + O2 CO2 Alkali Metals in Water

19. Chemical Properties… …relate how chemicals undergo change. Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant  product sodium + water  sodium hydroxide + hydrogen gas Na + H2O NaOH + H2

20. Chemical Properties… …relate how chemicals undergo change. Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant  product Potassium + water  potassium hydroxide + hydrogen gas K + H2O KOH + H2

21. Chemical Properties… …relate how chemicals undergo change. Chemical Change (reaction): when substances are converted into NEW substances. Reactants REACT. Products are PRODUCED. reactant + reactant  product Rubidium + water  rubidium hydroxide + hydrogen gas Rb + H2O RbOH + H2

22. Classification of Matter Mixtures Pure Substances Homogeneous (air, sugar in water) Heterogeneous (wood, blood) Compounds (water, salt, sugar) Elements (gold, oxygen) “Solutions”

23. MIXTURES Blend of two or more types of matter (each retains its own identities and properties.) Salt-Water…is both salt and water. Tastes like salt and tastes like water. Mixture of metals: alloy -24 k. gold = only gold -18 k. gold = gold, silver, copper PURE SUBSTANCES Every sample has exactly the same properties. Every sample has exactly the same composition. Pure water is always 11.2% hydrogen and 88.8% oxygen. Mixtures vs. Pure Substances

24. Classification of Matter Mixtures Pure Substances Homogeneous (air, sugar in water) Heterogeneous (wood, blood) Compounds (water, salt, sugar) Elements (gold, oxygen) “Solutions”

25. DISTILLATION Boil mixture. Liquid boils off, leaving solid minerals behind. Collect the boiled vapor in a condenser. Collected liquid is pure(er). Ex: Seawater or Moonshine FILTRATION Pour mixture onto a mesh, like filter paper. Liquid passes through paper. Solid is left on the paper. Ex: Charcoal water filters Separation of Mixtures

26. INTRO to the Periodic Table

27. GROUPS (or families) are VERTICAL

28. PERIODS are HORIZONTAL.

29. Metals are Left. Nonmetals are Right METALLOIDS are on Zig-Zag Line.

30. Groups you should know… • Alkali Metals • Alkaline Earth Metals • Transition Metals • Rare Earth Metals • Metalloids • Nonmetals • Halogens (Group 17) • Inert “Nobel” Gases

31. Label your periodic table… • Group numbers (1-18) • Period numbers (1-7, 6-7) • Metals (except H) • Nonmetals • Metalloids (except Al) • Hydrogen is *special* • Group 1: Alkali Metals • Group 2: Alkaline Earth Metals • Groups 3-12: Transition Metals • Group 17: Halogens • Group 18: Inert “Nobel” Gases • Rare Earth Metals • (Top) Lanthanide Series • (Bottom) Actinide Series

32. Vocabulary Review • Solid • Liquid • Gas • Plasma • Reactant • Product • Pure Substance • Group (Family) & Period • Metal • Nonmetal • Metalloid • Chemistry • Atom • Compound • Element (atomic/molecular) • Change of State • Physical Change • Mass, Matter • Chemical Change • Chemical Reaction • Mixture • Homogeneous • Heterogeneous

33. Important Information Test on Thursday! - Chapter 2 - Scientific Method Review - Lab Safety & Equipment - Graphing Review Bring: Pencil & Calculator Book (for after test)

34. Next Unit… Chapter 5 Measurements & Calculations