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Understanding Key Concepts in Chemistry: Measurements, Significant Figures, and Scientific Notation

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This chapter delves into essential mathematical vocabulary and concepts in chemistry, focusing on the scientific method as a means to address problems. Learn the difference between qualitative and quantitative observations, and understand accuracy, precision, and significant figures (SF). We cover the importance of the metric system, SI units, and demonstrate methods for addition, subtraction, multiplication, and division of measurements with appropriate significant figures. Finally, the chapter reinforces how to convert units and use scientific notation effectively.

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Understanding Key Concepts in Chemistry: Measurements, Significant Figures, and Scientific Notation

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  1. Chemistry Chapter 2 Math

  2. Vocabulary • Scientific method : the strategy to explore a problem • Qualitative : words • Quantitative: numbers • Accuracy : the measurement approaches true value of quantity • Precision : the same quantity, made in same ways, and agrees with one another • Significant Figures (SF) : consists of all the digits known with certainty plus final digits * Zeros in the beginning never, zeros in the middle always, zeros in the end sometimes if following a decimal point. • Addition/Subtraction with SF and SN : must have the same number of digits to right of the decimal point as there are in measurement having fewest digits • Multiplication/Division with SF and SN : D = M V ; no more SF’s than what are in the measurement with fewest number of SF. • Density : the ratio of mass to volume, or mass divided by volume. D = M V • Factor Label Method (Conversion Factors) : change one unit into another; converting numbers • Metric System : system of measurements • SI units : terms of standard measurement

  3. Math • “Sig figs” : 305 = 3 sf’s 0.1 = 1 sf , 0.01090 = 4 sf’s • Adding/ subtracting Sig Figs: 2.44cm +100. cm +14.5667 =117.0067 = 117. cm / 3.467 mm – 0.02 = 3.447 = 3.45 mm • Multiplying/ dividing Sig Figs : (4.50 cm)(2) = 9. cm / (64.0 g) / (10. mL)= .64g/mL • Density : volume = 55 cm3 & mass = 170 g ; 170g 55cm3 = 3.1g/cm3 • Addition/ subtraction SN : 4 • Multiplying/ dividing SN : 4.67 X 104 = 0.000467

  4. UNITS SI system of units Length Meter m Mass Kilogramkg Time Second s Temperature Kelvin K Amount of substance Mole mol Electric Current Ampere A Intensity of Light Candela cd METRIC PREFIXES PREFIX Unit abbreviation Exponent Factor Tera T 1012 Giga G 109 MegaM 106 Kilok 103 Hecto h 102 Dekada101 Base * 100 Decid 10 -1 Centic10-2 Millim 10-3 Microu 10-6 Nanon 10-9 Pico p 10-12 Femto f 10-15 Atto a 10-18

  5. Scientific Notation 1. Standard form is #.# X 10n . 1.2 X 103 2. A positive exponent is a large number. 1.2 X 103 = 1200 3. A negative exponent is a small number. 5.7 X 10-2 = 0.057 4. The number of sig figs does not change when converting between expanded and scientific notation. 1200 has 2SF as does 1.2 X 103 1200. has 4SF as does 1.200 X 103

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