Chemistry 11 Some Study Materials for the Final Exam
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1 Chemistry 11 Some Study Materials for the Final Exam Prefix Abbreviation Exponent giga G 10 9 mega M 10 6 kilo k 10 3 hecto h 10 2 deca da 10 1 deci d 10-1 centi c 10-2 milli m 10-3 micro µ 10-6 nano n 10-9 pico p Density M D V Precision -The number of significant digits to which a value has been reliably measured. -The more decimal places, the more precise the measurement. -The greater the precision, the less the uncertainty. The accuracy of a measurement is how close the measurement is to an accepted standard. Significant Digits Rules: 1. All non-zero digits are significant 2. Zero s between non-zero digits are significant 3. All zero s to the LEFT of the 1st non-zero digit are NOT significant. (called leading zero s) 4. Zero s to the RIGHT of the last non-zero digit ARE significant IF the decimal point is SHOWN. 5. Zero s to the RIGHT of the last non-zero digit (trailing zero s) ARE NOT significant if there is an UNDERSTOOD decimal point. 6. In Scientific Notation, the exponent part of the number is NOT significant. Chemistry 11 - Page 1
2 For Multiplication or Division: Answer is rounded to the LOWEST # OF SD S in the data. For Addition or Subtraction: Answer is rounded to the LOWEST # OF DECIMAL PLACES in the data. Some Terms in Unit 3: Observation, Interpretation, Qualitative, Quantitative, Data, Experiment, Hypothesis, Theory, Laws, Matter, Chemistry, Physical and Chemical Properties, Malleability, Ductility, Lustre, Viscosity and Diffusion. Review the Phases of Matter. Define: Observation, Interpretation, Qualitative, Quantitative, Data, Experiment, Hypothesis, Theory, Laws, Matter, Chemistry, Physical and Chemical Properties, Malleability, Ductility, Lustre, Viscosity and Diffusion. Review the Phases of Matter. The Methods of Separation of Mixtures: 1. Filtration 2. Distillation 3. Solvent Extraction 4. Recrystallization 5. Gravity Separation 6. Paper Chromatography Temperature Time Graph Melting solid Warming liquid Warming solid Covalent names and Formulas Chemistry 11 - Page 2
3 Chemistry 11 - Page 3
4 Percent Composition Chemistry 11 - Page 4
5 Chemistry 11 - Page 5
6 Chemistry 11 - Page 6
7 Chemistry 11 - Page 7
8 Chemistry 11 - Page 8
9 Chemistry 11 - Page 9
10 Chemistry 11 - Page 10
11 Excess and Limiting Reactant Problems Chemistry 11 - Page 11
12 Chemistry 11 - Page 12
13 Chemistry 11 - Page 13
14 Electron-Dot Formulas Electronegativity the tendency of an atom to attract electrons from a neighbouring atom. When the electronegativities of two atoms are quite different from each other: One atom loses an electron (or electrons) The other atom gains an electron (or electrons) This results in an Ionic Bond. Crystal Lattice Chemistry 11 - Page 14
15 When Electronegativities of bonding atoms are the same (as they are in diatomic molecules) or close to the same, they SHARE electrons. Bonds formed when atoms share electrons are called Covalent Bonds. In diatomic molecules (like H2 or Cl2), the electronegativities of both atoms are exactly the same so electrons are shared equally! Bonds within molecules that hold the atoms of a molecule together are called intramolecular bonds. They are strong covalent bonds. Covalent Bonds A dipole is a partial separation of charge which exists when one end of a molecule has a slight positive charge and the other end has a slight negative charge When electrons are shared unequally between two atoms, the bond is called Polar Covalent. Chemistry 11 - Page 15
16 Chemistry 11 - Page 16
17 Chemistry 11 - Page 17
18 An enthalpy diagram for an exothermic reaction: Enthalpy (H) 2C 8 H O 2 16CO H 2 O H is Negative Reaction Proceeds So, to summarize, in an exothermic reaction: H is negative Products are lower than Reactants on the Enthalpy Diagram Heat is released to the surroundings In an endothermic reaction: Heat is absorbed from the surroundings and converted into enthalpy. Here is an enthalpy graph for an endothermic reaction: Enthalpy (H) H 2 O + CO 2 + NaCl NaHCO 3 + HCl H is Positive Heat and Moles in Equations Find the amount of heat released during the formation of 14.6 moles of NH 3, given the reaction: N 2 + 3H 2 2NH kj Solution: 14.6 mol NH 3 x 46.2kJ 2molNH 3 = 337 kj Calorimetry: Example: Given that the heat capacity of water: C 2 = 4180 J/kg. o C Calculate the heat required to warm g of water from 20 o C to 50 o C. Solution: First we have to change g to kg and calculate the temperature change ( t) 50 o C - 20 o C = 30 o C Next, we write the equation: Heat = m. C. t Then we plug in the data: Reaction Proceeds H O Heat (J) = kg x 4180 J/kg. o C x 30 o C = J Chemistry 11 - Page 18
AP Chemistry A. Allan Chapter 1 Notes - Chemical Foundations
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