1. Chemistry by the numbers Units of Measurement – The Metric System Length: Mass: Volume: Temperature: Pressure: Kilo-Hecta-Deka-BaseDeci-Centi-Milli- 0.0010.010.11101001000 meter(m) gram(g) liter(L) Celsius(ºC) atmosphere(atm)

2. Chemistry by the numbers ● How do you convert 100 grams into kilograms? ● Use dimensional analysis (aka Unit Factor Method) ● Multiply the value by its conversion factor ● Kilo- means 1000 of something (in this case, grams) ● Therefore, the conversion factor is 1000 grams = 1 kilogram 100 grams x 1 kilogram 1000 grams We know 1000grams = 1kilogram, but why use a fraction? Why is kilogram on the top? The fraction makes the math easy. We can cancel out the ‘grams’ unit like it was a variable. The kilogram unit goes on the top because it is the unit we want. 100 grams x 1000 grams 1 kilogram Conversions = 0.1 kilograms The unit we want! ??? Can’t cancel out the units!

3. Chemistry by the numbers ● Convert the following ● 1.5 Liters to kiloLiters ● 20,000 micrograms to grams ● 1950 centimeters to meters ● 1.501 kg to grams ● 0.009 L to mL Conversions

4. Chemistry by the numbers ● What is the mass of an electron? 0.000,000,000,000,000,000,000,000,000,000,911 kg ● What is the distance between our sun and Pluto? 5,913,520,000,000 m ● Is there a better way to write these numbers? YES! Scientific Notation

5. Chemistry by the numbers ● First, locate the first significant digit Scientific Notation Move this decimal......to just after the first significant digit ● Then count the places the decimal moved...

6. Chemistry by the numbers ● Your new number is then written times 10 to the number of places you moved the decimal Scientific Notation ● The number is negative because the original number is a decimal So try it with the other number: 5,913,520,000,000 m → kg

7. Accuracy vs. Precision Chemistry involves making measurements with tools Accuracy - measurements that are close to the true value. Which tool is more accurate to measure the width of a penny; a meter stick or a caliper? Precision - measurements that are consistent. Measurements are the same or close to the same every time you measure. No tool is 100% accurate. Tools can be precise.

9. Percent Error How good are your measurements? Percent error: formula used to determine how close(or how far) the experimental value is to the accepted value. % error = |accepted value – experimental value| x 100 accepted value Experimental value = the measurement or calculation you made in the experiment Accepted value = the measurement that is accepted by the scientific community as true and exact.

10. % Error Calculations ● A student measures the mass and volume of a block of iron and calculates its density as 8.50 g/cm 3. The accepted value is 7.86 g/cm 3. What is the % error? % error = |7.86 g/cm 3 - 8.50 g/cm 3 | x 100 7.86 g/cm 3 % error = 8.14% ● A chemical reaction produced a solid with a mass of 0.455 grams. However, the expected amount was supposed to be 1.000 grams. What is the percent error for this experiment? % error = |1.000g -.455 g/cm 3 | x 100 1.000g % error = 54.5%

11. Significant Figures ● 2 kinds of numbers: – Exact: The precise amount. – (ie Money in your pocket) – Approximate: Anything MEASURED. – No measurement is perfect ● Scientists only use numbers that are reliable. Example: Mass of a coin on a triple-beam balance is 2.7g Mass of the same coin on a digital scale is 2.700g ● Are they the same number? ● To a mathematician, yes. ● To a scientist, No!

12. ● 2.700g to a scientist means the measurement is accurate to within one thousandth of a gram, but the measurement of 2.7g is only accurate to the 10 th of a gram. ● The more accurate a measurement is, the greater the number of significant numbers. When to use Significant figures

13. ● Rule 1: All numbers are significant starting with the first non-zero digit on the left. ● 1st Exception: In whole numbers that end in zero, the zeros at the end are not significant. Determining Significant Figures Has 4 sig figs Has 3 sig figs ??? Has 1 sig fig

14. How many sig figs?  7  40  0.5  0.00003  7 x 10 5  7,000,000 11 11 11 11 11 11

15. How do I know how many?  2nd Exception: Any zeroes between two non-zero numbers are significant.  2002 sec  3rd Exception: Zeroes to the right of a decimal are significant.  11.4000kg  4th Exception: decimal points make all zeroes to the left significant.  90100. m Has 4 sig figs Has 6 sig figs Has 5 sig figs

16. How do I know how many? Sig Figs & Scientific Notation Count all the numbers before the x10 9.3x10²cm = 4.1000x10³³kg = 2 5

17.  1.2  2100  56.76  4.00  0.0792  7,083,000,000 22 22 44 33 33 44 How many sig figs?

18. 3401 2100 2100.0 5.00 0.00412 8,000,050,000. 4 2 5 3 3 10 How many sig figs?

19. When Adding or subtracting measurements – Answer will have the same decimal place as the least accurate number – Ex: 2.45 cm + 1.2cm = 3.65cm? – 1.2cm is least accurate so… round to the one decimal 7.432L + 2L Sig Fig Calculations  3.7cm = 9.432L round to  9L

20. 123.0cm – 99.82cm = 2100.mL + 101mL = 88.772g – 17.1g = 24.00cm – 18cm = 7234.1m + 1000.0m = 708g – 8.4g = 23.2cm 2201mL 71.7g 6cm 8234.1m 700.g Sample Problems

21. ● Multiplying or dividing, significant figures Answer will have the same sig. figs as the least reliable measurement. 56.780cm x 2.45cm = Sig Fig Calculations 5 sig figs 3 sig figs 139.111 cm 2 139.111 cm 2 → 139 cm 2 Round to 3 sig figs... If two numbers have the same reliability, use the least amount of sig figs. 12.00km x 1.01km = 12.12km 2 → 12.1km 2

22.  1.0cm x 4cm =  4.00cm x 18cm =  7234.1m ÷ 100.0sec =  708g ÷ 8.1L =  298.01kg + 34.112kg =  84m/s x 31.221s =  4cm²  72cm²  72.34m/sec  87.4g/L  332.12kg  2600 m Sample Problems