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Chapter 1 Matter, Energy and Measurement

Chemistry B11. Chapter 1 Matter, Energy and Measurement. Chemistry and our life. Chemistry & Matter. Matter: has mass and takes space. Chemistry: science that deals with matters and their changes . Central Science. All sciences are connected to chemistry. Changes.

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Chapter 1 Matter, Energy and Measurement

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  1. Chemistry B11 Chapter 1 Matter, Energy and Measurement

  2. Chemistry and our life

  3. Chemistry & Matter Matter: has mass and takes space. Chemistry:science that deals with matters and their changes. Central Science All sciences are connected to chemistry.

  4. Changes Chemical change (chemical reaction): substance(s) are used up (disappear) → other forms burning a paper or cooking an egg Physical change: identities of the substances do not change. (change of state) evaporation of water or melting

  5. Scientific method fact:is a statement based on direct experience. hypothesis:is statement that is proposed without actual proof. theory:is the same as a hypothesis except that we have a stronger belief in it because of more evidence supports it. serendipity:observation by chance.

  6. Exponential notation based on powers of 10 10000 = 1×104 0.0001 = 1×10-4 4500000 = 4.5×106 0.000078 = 7.8×10-5 94800 = 9.48×104 0.0121 = 1.21×10-2 Positive power: greater than 1 Negative power: Less than 1

  7. Exponential notation Power, Exponent 9.23 1025 Base Coefficient

  8. Exponential notation (3.62 ×106)(7.43 ×103) = 26.90 ×109 = 2.69 ×1010 3.62 ×107 = 2.68 ×102 1.35 ×105 Decreasing the power one point Moving the decimal point to right Increasing the power one point Moving the decimal point to left

  9. Measurements

  10. Measurements Measurement consists of two parts: Number - Unit 2 pounds Unit Number

  11. Measurement and Units Metric system or SI (International System of Units) meter, liter, gram … English system (use in the United States) miles, gallons, pounds … Advantages of SI:we have base unit for each kind of measurement. Other units are related to the base unit by powers of 10.

  12. base unit of mass: gram (g) 1 kilogram (kg) = 1000 gram (g) 1 milligram (mg) = 0.001 gram (g) base unit of volume: liter (L) base unit of time: second (s) 1 milliliter (mL) = 0.001 liter (L) 1000 milliliter (mL) = 1 liter (L) 1 mL = 1 cc = 1cm3 1L = 1dm3 60 seconds (s) = 1 minute (min) 60 minutes (min) = 1 hour (h) base unit of length: meter (m) 1 kilometer (km) = 1000 meter (m) 1 centimeter (cm) = 0.01 meter (m) 1 nanometer (nm) = 1×10-9 meter (m)

  13. Tools (equipment) of measurement Length: Meterstick or Ruler Volume: Graduated cylinder, Pipette Mass: Balance

  14. °F = 1.8 °C + 32 °C = °F – 32 1.8 Kelvin scale or absolute scale (K) K = °C +273 °C = K – 273 Temperature Fahrenheit (°F) English system Celsius or centigrade (°C) metric system or SI

  15. Temperature

  16. 2.205 lb = 55.12 lb 25kg × 25kg = ? lb 1 kg 1.609 km 78 mile = ? km = 125.50 km 78mi × 1 mi 45 m/h = ? in/min 39.37 in 1 h m 45 × × = 29.53 in/min h 1 m 60min Conversion of Units Factor-Label method

  17. States of Matter

  18. m d = V Specific gravity: dsubstance SG = dwater Hydrometer No units (dimensionless) Density and Specific gravity density: mass per unit volume d: density (g/mL or g/L) m: mass V: volume

  19. Energy Kinetic energy (KE): energy of motion KE = ½ mV2V: velocity Potential energy: stored energy Law of conservation of energy

  20. Amount of heat = specific heat × mass × change in temperature Amount of heat = SH × m × (T2 – T1) T2 = final temperature T1 = initial temperature SH = Specific heat (cal/g °C) Heat and Temperature units of heat: calorie (cal) or joule (J) 1 cal = 4.184 J

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