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Introduction To Chemistry

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Published in: Chemistry
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Introduction to Organic Chemistry

Sachin S / Pune

14 years of teaching experience

Qualification: M.Sc (Pune University - 2008), B.Sc (Yashwant College - 2006)

Teaches: Chemistry, AIEEE, BITSAT, CET, IIT JEE Advanced, IIT JEE Mains, AIPMT, Medical Entrance Exams, NEET

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  1. Chapter 1 An lnWOduction to Chemistry By Mark Bishop
  2. Chemistry The that deals with the structure and behavior of matter
  3. Summary Study Strategies— The will to succeed is important, but what 's more important is the will to prepare. Bobby Knight, basketball coach Read the chapter in the textbook before it is covered in the lecture. Attend the class meetings, take notes, and participate in class discussions. Reread the textbook, working the exercises, and marking important sections.
  4. More Study——--.-- Strategies • Use the chapter objectives as a focus of study. • Use the computer-based tools that accompany the course. • Work some of the problems at the end of the chapter. • Ask for help when you need it. • Review for the exam.
  5. Scientific Method Observation Collection of information leads to •Ille hypothesis a testable hypothesis. is subjected to New bservations are ma l)isproof Hypothesis Further rese IS done to refine the aprlications. Application lications are Sought. Ion •11tat10n. "[he ex fails. Experimentation s cation ssful tsare lished. is repeated repeated successfully.
  6. Chapter Map Base units Reporting values from measurements Measurement and units International system (SI) of measurement ngth Volum Metric prefixes emperatu Accuracy Precision 'Relationshi between mass an weight
  7. Val I-.leS from Measurements • A value is a quantitative description that includes both a unit and a number. For 100 meters, the meter is a unit by which distance is measured, and the 100 is the number of units contained in the measured distance. Units are quantities defined by standards that people agree to use to compare one event or object to another.
  8. Type length mass time temperature Base Unit meter kilogram second kelvin Abb. m kg s K Defined in terms of the fixed numerical value of the speed of light in vacuum c to be 299,792,458 when expressed in the unit m s-1, where the second is defined as below. the fixed numerical value of the Planck constant, h, to be 6.62607015 x 10-34 when expressed in the unit J s, which is equal to kg m2 s-l, where the meter and the second are defined in terms of c and Avcs• the fixed numerical value of the cesium frequency, Avcs, which is the unperturbed ground-state hyperfine transition frequency of the cesium-133 atom, to be 9, 192,631 , 770 when expressed in the unit Hz, which is equal to s-1 the fixed numerical value of the Boltzmann constant, k, to be 1.380 649x10-23 when expressed in the unit J K-1, which is equal to kg m2 s-2 K-l, where the kilogram, meter and second are defined in terms of h, c and Avcs.
  9. Derived Unit cubic meter one meter I cubic meter = 1000 liters eeq ooe liter 10-3 m3 103 1 m3
  10. Some Base Units and-Their Abbreviations for the International System of Measurement*-æ. Type Length Mass Volume Energy Base Unit meter gram liter joule Abbreviation m L or I
  11. Metric Prefixes Prefix giga mega kilo centi milli micro nano pico Abbreviation k c m n p Number 109 or 106 or 103 or 1000 10-2 or 0.01 10-3 or 0.001 10-6 or 0.000001 10-9 or 0.000000001 10-12 or 0.000000000001
  12. Scientific Notation Numbers expressed in scientific notation have the following form. Exponent, a positive or negative integer ax 10 Coefficient, Exponential term a number with one nonzero digit to the left of the decimal point
  13. Scientific (Example) 5.5 x 1021 carbon atoms in a 0.55 carat diamond. — 5.5 is the coefficient — 1021 is the exponential term — The 21 is the exponent. • The coefficient usually has one nonzero digit to the left of the decimal point.
  14. Uncertainty The coefficient reflects the number' s uncertainty. • It is common to assume that coefficient is plus or minus one in the last position reported unless otherwise stated. Using this guideline, 5.5 x 1021 carbon atoms in a 0.55 carat diamond suggests that there are from 5.4 x 1021 to 5.6 x 1021 carbon atoms in the stone.
  15. Size (Magnitudéj•----" of Number The exponential term shows the size or magnitude of the number. Positive exponents are used for large numbers. For example, the moon orbits the sun at 2.2 x 104 or 22,000 mi/hr. 2.2 x 104=2.2 x 10 x 10 x 10 x 22,000
  16. Size of Number Negative exponents are used for small numbers. For example, A red blood cell has a diameter of about 5.6 x 10-4 or 0.00056 inches. 5.6 10 1 104 5.6 0.00056
  17. From Decimal- Nurfibéöto Scientific Notation—.--..m Shift the decimal point until there is one nonzero number to the left of the decimal point, counting the number of positions the decimal point moves. Write the resulting coefficient times an exponential term in which the exponent is positive if the decimal point was moved to the left and negative if the decimal position was moved to the right. The number in the exponent is equal to the number of positions the decimal point was shifted.
  18. From Decimal-Nühber to Scientific Notation-(Examples). e • For example, when 22,000 is converted to scientific notation, the decimal point is shifted four positions to the left so the exponential term has an exponent of 4. 4 22,000 - 2.2 x 10 When 0.00056 is converted to scientific notation, the decimal point is shifted four positions to the right so the exponential term has an exponent of -4. 0.00056 - 5.6 x 10
  19. Scientific Notätifito Decimal Numbers—.-.—__ Shift the decimal point in the coefficient to the right if the exponent is positive and to the left if it is negative. The number in the exponent tells you the number of positions to shift the decimal point. 2.2 x 104 goes to 22,000 5.6 x 104 goes to 0.00056
  20. Reasons for Using-" Scientific Notation—.--..m • Convenience - It takes a lot less time and space to report the mass of an electron as 9.1096 x 10-28, rather than 0.00000000000000000000000000091096 g. • To more clearly report the uncertainty of a value - The value 1.4 x 103 kJ per peanut butter sandwich suggests that the energy from a typical peanut butter sandwich could range from 1.3 x 103 kJ to 1.5 x 103 kJ. If the value is reported as 1400 kJ, its uncertainty would not be so clear. It could be 1400 ± 1, 1400 ± 10, or 1400 ± 100.
  21. Exponential Terms—. • When multiplying exponential terms, add exponents. 103 x 106 = 103+6 = 109 103 x 10-6 = 10-3 3.2 x 10-4 x 1.5 x 109 3.2 1.5 = 4.8 x 105
  22. When dividing-exponential terms, subtract exponents. 1012 = 109 103 6 10 = 106-(-3) = 109 10-3 9.0 x 1011 -6 1.5 x 10 102. 10 —3 106 9.0 x 1011-(-6) = 6.0 x 101 7 1.5 _ 10—7 1.5 x 104. 4.0 x 105 2.0 x 1012. 103 1.5 . 4.0 x 104+5—12 3 2.0 3.0 x 10-6
  23. Raising Exponemal Terms to a When raising exponential terms to a power, multiply exponents. (104)3 = 104•3 = 1012 (3 x 105)2 = (3)2 x (105)2 = 9 x 1010
  24. Length kilometers miles I km = 0.6214 mi I km I ft = 0.3048 m 3.281 ft I in. = 2.54 cm 25.4 mm I cm 0.3937 in. I mm 0.03937 in. centimeters I mm inches A mile is times around a typical high school track. I meter I centimeter i meter
  25. Range of Lengths 10-15 10-10 10—5 10 1015 20 10 25 10 30 10
  26. Volume 29.57 rnL = about 20 drops 1 gal = 3.785 L I gallon (gal) or 4 quarts (qt) 1 qt = 0.9464 L I qt or 32 fl oz 1 1.057 qt = 0.2642 gal I liter (L) or 1000 mL
  27. Range of Volumes 10 10-30 -10 10-20 1010 1020 30 10 liters
  28. M ss and Weight Mass is usually defined as a measure of the amount of matter in an object. Mass can be defined as the property of matter that leads to gravitational attractions between objects and therefore gives rise to weight. Matter is anything that occupies a volume and has a mass. The weight of an object, on the Earth, is a measure of the force of gravitational attraction between the object and the Earth.
  29. Comparison of_the Mass and Weight of a 65 kg Person On Earth Mass 65 kg Weight 637 N Between Earth and Moon 65 kg On Moon 65 kg 1/6(637 N) = 106 N
  30. Mass I 28.35 g About 2.5 grams (g) or about 0.088 ounce (oz) 1 1b 453.6 g 1 kg 2.205 1b About 1 kilogram (kg) or about 2.2 pounds (1b) I Mg = 1000 kg = It About 1 megagram (Mg) or 1 metric ton (t)
  31. Electron in an atom, 9.1096 x 10-28 g Atom, 1.6735 x g • Basketball, 612 g Egyptian pyramid, 1013 g Earth, 1027 g -Ibe universe,
  32. Celsius and Fahrenheit Temperature 100 oc— 32 —212 OF Boiling water Ice water
  33. Comparing Temperature Scales Celsius Boiling water units Freezing water Absolute zero 100 OC -273. 100 units Kelvin 373.15K 180 units 273.15 K OK Fahrenheit 212 OF 32 OF
  34. Accuracy Precision describes how closely a series of measurements of the same object resemble each other. The closer the measurements are to each other, the more precise the measurement. The precision of a measurement is not necessarily equal to its accuracy. Accuracy is a measurement' s relationship to the property' s true value.
  35. Accuracy 000 This archer is precise but not accurate. This archer is precise and accurate. This archer is imprecise and inaccurate.
  36. Reporting from Measurements-. • One of the conventions that scientists use for reporting numbers from measurements is to report all of the certain digits and one estimated (and thus uncertain) digit.
  37. Graduated Cylinder — Comparing the position of the bottom of the meniscus and the milliliter scale yields a measurement of 8.74 mL.
  38. Accurate to — If the graduated cylinder is only accurate to ±0.1 mL, we report 8.7 mL.
  39. Trailing Zeros — We report 8.00 mL to show an uncertainty of ±O.OI mL.
  40. Trailing Zeros (2) — If the graduated cylinder is only accurate to +0.1 mL, we report 8.0 mL.
  41. Digital Readout CAL Report all digits unless otherwise instructed.
  42. Digital Readout (2) CAL In many cases, it is best to round the number in the value to fewer decimal positions than displayed. For the mass displayed above, 100.432 g would indicate ±0.001 g.

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