2. Matter must Have mass Have volume (take up space)

3. Matter exists in three phases Solids (s)- fixed shape & volume Liquid (l)- fixed volume, takes the shape of the container Gas (g)- takes both the volume and the shape of the container

4. Matter is divided into 2 categories. Pure Substances Fixed composition Unique set of properties Mixtures Composed of two more substances physically mixed

5. Pure Substances Elements-type of matter than cannot be broken down into two or more pure substances Elements can be divided into many categories Metals Nonmetals Metalloids Families (Periodic Table) Compounds-more than one element Have new properties after chemically combined

6. Mixures Homogeneous-composition is the same throughout A solution is a liquid homogeneous mixture made of solvents & solutes. Most solvents are liquids; however it can be a gas Heterogeneous- does not have a uniform composition

7. Separation Techiques We are going to look at 3 types. There are more. Filtration Used for a heterogeneous solid-liquid mixture Distillation Homogeneous solid-liquid mixture Also liquid-liquid mixtures in which one liquid can be evaporated Chromatography Liquid-liquid mixture Liquid-gas mixture Gas-gas mixture

8. Significant Figures Uncertainty of at least one unit in the last digit 2.00 mL = 3 SF 2.0 mL = 2 SF 2 mL = 1 SF 0.002 mL= 1 SF

9. Rules Zeros appearing between nonzero digits are significant Zeros appearing in front of all nonzero digits are NOT significant. Zeros at the end of a number and to the right of a decimal point are significant. A decimal point placed after zeros indicates that they are significant. Trailing zeros without decimals are questionable 75000 may be 2-5 SF 7.5 x 10 4 = 2 SF 7.50 x 10 4 = 3 SF Assume not significant in the book therefore 75000= 2SF

10. Rules Multiplying & Dividing The # of SF in the result is the same as quantity of smallest # of SF Adding & Subtracting The number of decimal places in the result is the same with the smallest decimal Rounding If less than 5… leave last digit unchanged If greater than 5…add one to the last digit If equal to 5…round even Round 14.575 to 2SF= 14

11. Rules Multiple Operations Carry out all steps with complete number of digits Go back to find the # of SF at each step Round at the end ALWAYS SHOW WORK AND USE YOUR UNITS!!!

12. How many Sig Figs? 1. 0.00800 in 2. 52.000 nm 3. 800 ns 4. 4.30 x 10 4 kg 5. 5060 g

13. Solve the problem with correct SF. Box in your answer. 1. 2.505 x 0.0920 x 451.08= 2. 0.0810 + 7.168 + 1.50 = 3. 5.20/8.973= ***When putting in your calculator remember to use () to make calculator do order of operations correctly.

14. When you make a conversion, choose the factor that cancels out the initial unit. The actual conversion factor does not count on significant figures Use the number of significant figures in the initial measurement given Remember what % means mathematically. When given a % use the unit shown in the problem. 52% mL = 52 mL/ 100 mL 0.07% L = 0.07 L/ 100 Conversions

15. 3 hr to sec 5.27 Mg to lb (Mg= mega grams) 0.53 mi to m 55.25 mi to km 11.6 mL to in 3 Examples

16. Every pure substance has its own unique set of properties Chemist use these properties for identification 2 ways of grouping these properties Properties of Substances

17. Intensive Properties (do not depend on amount) ***chemist use these to identify These are a few examples Density Melting pt Boiling pt Extensive Properties (depend on amount ) Mass Volume Intensive & Extensive Properties

18. Physical- do not change the substance Theses are just a few examples Density Melting pt Boiling pt Solubility Color Chemical-when a new substance is formed Reactivity Flammability Physical & Chemical Properites

19. Denisty= mass/volume Mass= grams Volume= cm 3, mL, L Be sure to show all work and units!!!!! Density

20. The density of Al is 2.70 g/mL. What is the volume of 8.21 grams? The density of Hg is 13.5 g/mL. How many grams are in 5.0 mL? Examples

21. A sample of metal in a small weighing dish had a mass of 59.61g. The dish had a mass of 0.58 g. When the metal was added to the water, the water level rose 9 mL. What is the mass of the metal? What is the density of the metal? Examples

22. A sample of metal with a mass of 10.06g was placed in a flask with a volume of 65.0 mL. To fill the flask, 35.7 g Hg (density= 13.5 g/mL) must be added to the metal. What is the density of the metal? Examples

23. Atomic Mass= mass on the periodic table Avogadro’s Number Symbol N A 6.022 x 10 23 It represents the number of atoms of an element in a samples whose mass in grams is equal to the atomic mass of that element 6.022 x 10 23 H atoms= 1.008 g H 6.022 x 10 23 N atoms = 14.001 g N Moles to grams to particles

24. Find the mass of a N atom Find the number of N atoms in 7.00 grams. Examples

25. Moles 1 mole = Avogadro’s Number 1 mole = 6.022 x 10 23 Molar Mass Units are g/mol Same as formula mass Moles and Molar Mass

26. 13 g of caffeine, C 4 H 5 N 2 O Convert to moles Convert from moles to atoms Convert from atoms to Number of Carbon atoms Examples