1. Basic Concepts: Matter and Measurement Introduction: The scientific method Macro and Particulate Concepts Goals: 1.Classify matter. 2.Recognize elements, atoms, compounds, and molecules. 3.Identify physical and chemical properties and changes. 4.Apply the kinetic-molecular theory to the properties of matter. 5.Use metric units and significant figures correctly. 6.Understand and use the math’s of chemistry.

2. The scientific method InquiryInquiry – pose a reasonable QUESTION: ? –Look for what others have done. _____________Form a _____________ – tentative explanation or prediction of experimental observations. –Perform experiments. –Summarize observations in the form of a general rule. If the hypothesis is always true it may become a _______ – concise verbal or mathematical statement of a relation that seems always to be the same under the same conditions. If the human mind conceives a __________ – a unifying principle - to explain the observations. Always changing!!!

3. Chemist’s views of matter

4. What is matter? What are the states of matter? Matter is __________________________. There are other two states of matter. Do you know what are they? SOLID: rigid shape, fixed volume LIQUID: no shape of its own, fixed volume GAS: no fixed volume, it is determined by the size of the container

5. What is the kinetic-molecular theory? The theory which describes matter as extremely tiny particles (atoms and molecules) in constant motion. Also, the higher the temperature the ________ the particles move. The kinetic energy (energy of motion) acts to overcome the forces of _________ between the particles.

6. What are physical properties? Physical properties:Physical properties: properties which can be observed and measured without changing the identity composition of a substance. Examples: Color, state of matter, melting point, boiling point, density, hardness, odor. Physical changes:Physical changes: - boiling of a liquid - melting of a solid - dissolving a solid into a liquid to give a homogeneous mixture (a solution).

7. Density: important and useful physical property. –ratio of the mass of an object to its volume. Which one has more mass per unit volume? Which one would be heavier on Earth? Density 21.5 g/cm 3 Aluminum 2.7 g/cm 3 Platinum Density = mass volume

8. Density Density is an INTENSIVE property of matter – does NOT depend on quantity of matter. EXTENSIVE properties – depend on the quantity of matter analyzed. Students should become familiar with using density in calculations. Temperature Mass Melting PointLength ColorVolume Hardness

9. Mercury (Hg) has a density of 13.6 g/cm 3. What is the mass of 95 mL of Hg in grams? In kilograms? Solve the problem using DIMENSIONAL ANALYSIS -carrying on UNITS-

10. *Calculations need to be done in same units. 1 cm 3 = 1mL 1. Calculate mass: 2. Calculate mass in Kg: Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg in grams? In kilograms? Density = mass volume

11. What are chemical properties? Chemical properties:Chemical properties: those which describe the way a substance may change, or react, to form other substances. Example: Flammability Chemical change or Chemical reaction:Chemical change or Chemical reaction: transformation of one or more atoms or molecules into one or more different molecules.

12. Chemical vs. Physical Properties Explosiveness Corrosiveness Flammability Toxicity Temperature Mass Volume Color Density

13. How do we classify matter? Ask: Do the substance has an even texture (to the microscopic level)? YES – homogeneous NO - heterogeneous

14. How can we separate mixtures? Filtration Distillation Chromatography

15. What is an element? Element: substance composed of ____________ ______________. Pure substance that cannot be decomposed by ordinary means to other substances. Students should become familiar with the periodic table - symbols and names of the elements. Aluminum Bromine

16. The Periodic Table Dmitri Mendeleev (1834 - 1907) Try to answer: Why are elements organized in such a way?

17. What is an atom? An atom is ___________________ _______that retains the chemical properties of that element. Copper atoms on silica surface. Distance across = 1.8 nanometer (1.8 x 10 -9 m)

18. What are atoms composed of? An atom consists of a nucleus –of _________ and __________ and _____________ in space around the nucleus. Electron cloud Nucleus

19. What is a compound? Compounds: substance composed of two or more different ________; it can be decomposed into those __________. –Have distinctly different properties from their parent elements. –Have a definite percentage composition (my mass) of their combining atoms. –Might be composed of ions (electrically charged atoms, or group of atoms) or molecules (the smallest discrete units that retain the chemical characteristics of the compound). –Can be represented by their formula.

20. A compound: The red compound is composed of nickel (Ni) (silver) carbon (C) (black) hydrogen (H) (white) oxygen (O) (red) nitrogen (N) (blue)

21. What is a molecule? A molecule is the ___________ ________that retains the chemical characteristics of the ____________. Composition of molecules are given by a MOLECULAR FORMULA. H2OH2OH2OH2O C 8 H 10 N 4 O 2 - caffeine

22. Label: Elements vs. Compounds

23. What are SI base units? International System of Units metric systemSI – International System of Units. It is based on the metric system. Give the units with their symbol for: Masskilogram (kg) Length___________ Time___________ Temperature___________ Learn Table 1.2 in your textbook (page 26).

24. Length 1 m = 100 cm = 1000 mm 1 mm = 1x 10 -3 m 1 nm = 1 x 10 -9 m O—H distance = 9.58 x 10 -11 m 9.58 x 10 -9 cm 0.0958 nm O—H distance = 9.58 x 10 -11 m 9.58 x 10 -9 cm 0.0958 nm Students should become familiar with: 1. equivalents of units and their conversions. 2. exponential notation and prefixes.

25. Unit Conversion 0.0958 nm to m Look for conversion factor(s):

26. Temperature Scales 1 kelvin = 1 degree Celsius Notice that 1 kelvin = 1 degree Celsius Boiling point of water Freezing point of water Celsius 100 ˚C 0 ˚C 100˚C Kelvin 373 K 273 K 100 K Fahrenheit 32 ˚F 212 ˚F 180˚F Students should learn the rules for significant figures!

27. Temperature Scales 100 o F 38 o C 311 K oFoF oCoCK T( o C) = 5oC5oC 9oF9oF [T( o F) – 32] T(K) = 1 K 1oC1oC [T( o C) + 273.15 o C]

28. Remember Go over all the contents of your textbook. Practice with examples and with problems at the end of the chapter. Practice with OWL tutor. Practice with the quiz on CD of Chemistry Now. Work on your assignment for Chapter 1.