General Chemistry 1 PDF

General Chemistry 1 1ST SEMESTER / FIRST QUARTER / LECTURE AND PPT-BASED Mikaela Kristel Alcon (Mika) 1.3.1. Pure Substance LESSON 1 : Matter and its Properties...

General Chemistry 1 1ST SEMESTER / FIRST QUARTER / LECTURE AND PPT-BASED Mikaela Kristel Alcon (Mika) 1.3.1. Pure Substance LESSON 1 : Matter and its Properties > based on the number of kinds of 1. Matter atoms present > anything that occupies space (volume) and > has fixed and definite composition, has mass consists of only one type of particle 1.1. Particles > chemically bonded 1.1.1. Atoms 1.3.1.1. Element > smallest unit of matter, derived from > simplest form of substance atomos (indivisible) > can no longer be broken down into > particle of an element constituent parts by chemical 1.1.2. Molecules means > aggregation of two or more atoms, 1.3.1.2. Compound chemically bonded > aggregation of two or more > particle of a compound elements 1.1.3. Ions > can be broken down into elements > atoms that have a net charge, by chemical means positive or negative 1.3.2. Mixture > can be monatomic or polyatomic > based on the uniformity of 1.1.3.1. Cation composition and properties > positively charged (metals) > combination of two or more 1.1.3.2. Anion substances which retain their identities > negatively charged (non-metals) > physically bonded 1.2. Properties 1.3.2.1. Homogenous 1.2.1. Physical Property > composition is same throughout > can be measured and observed 1.3.2.1.1. Solution without changing the composition or > dispersed particles are identity of a substance intermediate in size, less than 1 1.2.1.1. Intensive Property nanometer > does not depend on the amount of > doesn’t scatter light substance 1.3.2.2. Heterogenous > density, color, temperature, etc. > composition is not uniform 1.2.1.2. Extensive Property 1.3.2.2.1. Colloid > depends on the amount of > dispersed particles are substance intermediate in size between 1 > mass, volume, weight and 1000 nanometer 1.2.2. Chemical Property > scatters light (Tyndall effect) > can be measured and observed by 1.3.2.2.2. Suspension changing the composition or identity > dispersed particles settle out, of substance intermediate in size over 1000 1.3. Classification nanometer > based on the number of components > typically does not scatter light General Chemistry 1 1ST SEMESTER / FIRST QUARTER / LECTURE AND PPT-BASED Mikaela Kristel Alcon (Mika) 1.4. Separating Mixtures > mobile phase - liquid; carries the 1.4.1. Solid-Solid Mixture components 1.4.1.1. Magnetic Separation > stationary phase - paper; allows > uses magnets to attract metals components to travel > example: mixture of iron filings and 1.4.3. Liquid-Liquid Mixture sulfur powder 1.4.3.1. Using Separatory Funnel 1.4.1.2. Sublimation > uses funnel to separate immiscible > requires heating wherein one must liquids sublime (solid to gas) > example: oil and water > example: Ammonium chloride 1.4.3.2. Distillation 1.4.1.3. Sieving > exploits boiling points of liquids > separates larger particles from > distillate - the product; liquid smaller ones > example: ethanol and water > example: sifting rice LESSON 2 : Significant Figures 1.4.2. Solid-Liquid Mixture 1.4.2.1. Filtration 1. Significant Figures > separates insoluble solid from > a number or figure that is certain to give a liquid reliable and/or reasonable information > filtrate - passed through filter 1.1. Rules > residue - solid left in filter 1.1.1. Non-zero digits > example: sand and water > All non-zero digits are significant 1.4.2.2. Decantation > example: 101 - 3 SF > pouring out the liquid after the 1.1.2. Captured/Captive Zeros solid settled at the bottom > If 0 is captured between two non-zero > example: oil and water digits, it is significant 1.4.2.3. Evaporation > example: 101 - 3 SF > requires heating to separate liquid 1.1.3. Leading Zeros from solid > If 0 comes before a non-zero, it is > example: table salt and water insignificant 1.4.2.4. Crystallization > example: 013 - 2 SF > retrieving solids after evaporation 1.1.4. Trailing Zeros > example: table salt 1.1.4.1. Significant 1.4.2.5. Centrifugation > it is significant if it is found at the > denser particles move outward right of a decimal point while less dense are displaced > example: 1.0 - 2 SF > centrifuge - device which uses 1.1.4.2. Insignificant centrifugal force to separate > it is insignificant if it is found at the > example: DNA banding left of a decimal point 1.4.2.6. Chromatography > example: 0.1 - 1 SF > uses fluid solvent to separate a > it is insignificant if it is found after a mixture to its components non-zero digits General Chemistry 1 1ST SEMESTER / FIRST QUARTER / LECTURE AND PPT-BASED Mikaela Kristel Alcon (Mika) > example: 100 - 1 SF LESSON 3 : Scientific Notation 1.2. Rounding Numbers 3. Scientific Notation 1.2.1. Greater than 5 > method of effectively and efficiently > if the digit to be removed is greater expressing very small or extremely large than 5, then the preceding digit will numbers into powers of 10 increase by 1 2 > 1. 6 × 10 > example: 9.88- 9.9 3.1. Parts 1.2.2. Less than 5 3.1.1. Coefficient > if the digit to be removed is less than > 1. 6 5, then the preceding digit will retain > a number that is equal to or more than > example: 9.81 - 9.8 one but less than ten 1.2.3. Equal to 5 3.1.2. Base 1.2.3.1. Even Number > 10 > if the digit to be removed is even, > a number that is always 10 then the preceding digit will retain 3.1.3. Exponent > example: 0.45 - 0.4 >2 1.2.3.2. Odd Number > a number that determines how many > if the digit to be removed is odd, times the decimal point should be then the preceding digit will moved increase by 1 3.2. Conversion > example: 0.35 - 0.4 3.2.1. Standard Form to Scientific Notation 1.2.3.3. Non-zero Digit > to get the coefficient, move the > if the digit that follows 5 is a decimal point until you get a number non-zero, then the preceding digit that is equal to or more than 1 but less will increase by 1 than 5 > example: 9.755 - 9.8 3.2.1.1. Large Number 1.2.3.4. Zero 4 > if the digit that follows 5 is a zero, > 45000 = 4. 5 × 10 then the preceding digit will retain > move decimal point to left > example: 9.850 - 9.8 > positive exponent 1.3. Calculation 3.2.1.2. Small Number −4 1.3.1. Addition/Subtraction > 0. 00076 = 7. 6 × 10 > final answer must follow the number > move decimal point to right with least decimal places > negative exponent > example: 15. 333 + 15. 23 = 30. 563 3.2.2. Scientific Notation to Standard Form final answer: ≈ 30. 56 3.2.2.1. Positive Exponent 4 1.3.2. Multiplication/Division > 4. 5 × 10 = 45000 > final answer must follow the number > move decimal point to right with least significant figures 3.2.2.2. Negative Exponent −4 > example: 25. 05 ÷ 5. 0 = 5. 01 > 7. 6 × 10 = 0. 00076 final answer: ≈ 5. 0 > move decimal point to left General Chemistry 1 1ST SEMESTER / FIRST QUARTER / LECTURE AND PPT-BASED Mikaela Kristel Alcon (Mika) 3.3. Calculation 4.1.1. Percent Accuracy 3.3.1. Addition/Subtraction > %𝐴 = 𝑚𝑒𝑎𝑛 × 100 𝑠𝑡𝑎𝑛𝑑𝑎𝑟𝑑 𝑣𝑎𝑙𝑢𝑒 3.3.1.1. Same Exponent 2 2 > %𝐴 = 100 − %𝐸 > 2. 5 × 10 + 3. 8 × 10 4.2. Precision > add the coefficients > closeness of every observed value to one > 2. 5 + 3. 8 = 6. 3 another > rewrite in scientific notation 2 4.2.1. Percent Error > 6. 3 × 10 |𝑠𝑡𝑎𝑛𝑑𝑎𝑟𝑑 𝑣𝑎𝑙𝑢𝑒−𝑜𝑏𝑠𝑒𝑟𝑣𝑒𝑑 𝑣𝑎𝑙𝑢𝑒| > %𝐸 = × 100 3.3.1.2. Different Exponent 𝑠𝑡𝑎𝑛𝑑𝑎𝑟𝑑 𝑣𝑎𝑙𝑢𝑒 3 2 4.2.2. Range > 2. 75 × 10 + 7. 5 × 10 >𝑅 =𝑥 − 𝑥𝑚𝑖𝑛 > rewrite the coefficient to have the 𝑚𝑎𝑥 same power of 10 4.2.2.1. Interpretation 3 > 2. 75 × 10 + 0. 75 × 10 3 > 𝑃 = 𝑚𝑒𝑎𝑛 ± 𝑟𝑎𝑛𝑔𝑒 𝑅 > add the coefficients 4.2.3. Average Deviation > 2. 75 + 0. 75 = 3. 5 Σ|𝑜𝑏𝑠𝑒𝑟𝑣𝑒𝑑 𝑣𝑎𝑙𝑢𝑒−𝑚𝑒𝑎𝑛| > 𝐴𝐷 = 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑜𝑏𝑠𝑒𝑟𝑣𝑎𝑡𝑖𝑜𝑛𝑠 > rewrite in scientific notation 3 4.2.3.1. Interpretation > 3. 5 × 10 >𝑃 = 𝑚𝑒𝑎𝑛 ± 𝐴𝐷 3.3.2. Multiplication/Division 𝐴𝐷 3.3.2.1. Same Exponent 4.2.4. Standard Deviation 2 2 2 > 2. 5 × 10 × 3. 8 × 10 Σ(𝑜𝑏𝑠𝑒𝑟𝑣𝑒𝑑 𝑣𝑎𝑙𝑢𝑒−𝑚𝑒𝑎𝑛) > 𝑆𝐷 = 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑜𝑏𝑠𝑒𝑟𝑣𝑎𝑡𝑖𝑜𝑛𝑠 > multiply the coefficients 4.2.4.1. Interpretation > 2. 5 × 3. 8 = 9. 5 >𝑃 = 𝑚𝑒𝑎𝑛 ± 𝑆𝐷 > add the coefficients 𝑆𝐷 2+2 4 > 10 = 10 > rewrite in scientific notation 4 > 9. 5 × 10 3.3.2.2. Different Exponent 3 2 > 8. 0 × 10 × 9. 0 × 10 > multiply the coefficients > 8. 0 × 9. 0 = 72 > add the exponents 3+2 5 > 10 = 10 > rewrite in scientific notation 5 6 > 72 × 10 → 7. 2 × 10 LESSON 4 : Accuracy and Precision 4. Accuracy and Precision 4.1. Accuracy > closeness of observed value to the standard value