General Chemistry B - Week 2
General Chemistry B - Week 2 CHM 111
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This 3 page Class Notes was uploaded by Hailey N Detrick on Monday September 12, 2016. The Class Notes belongs to CHM 111 at Elon University taught by Amanda Watson in Fall 2016. Since its upload, it has received 5 views.
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Date Created: 09/12/16
General Chemistry B Week Two: 9/5 – 9/11 1. Stoichiometry: a. Based on the conversation of mass b. Depends on the property balanced equation i. Balance the equation: H 2 O à 2 O 2 ii. Answer: H +2O à 2H O 2 c. Rules: i. Write the complete chemical reaction ii. Count the total amount of each atom on each side a. i.e. H:2 O:2 à H:2 (4) O:1 (2) iii. balance the elemtents one at a time a. start with elements OTHER than C, O, and H b. balance C,O, and H last c. use whole number coefficiants d. i.e. 2H not 2.345H iv. Edit previously placed coefficient if necessary v. Reduce coefficients 2. Calculate the formula weight of a molecule: a. H 2: i. H (1 amu) x 2 (for 2 H atoms) + O (16 amu) x 1 (for 1 O atom) = 18 amu b. C 6 O12 6: i. C (12 amu) x 6 + H (1 amu) x 12 + O (16 amu) x 6 = 180 amu 3. Conversion from amu to grams: a. 1 amu = 1.66 x 10 -24 4. Mols: a. Conversion to mols i. 1 mole = 6.02 x 10 23 23 a. ex. If I have 1 mole of students, I would have 6.02 x 10 students b. Conversion from amu to g using mols: i. 1 mol C = 12 grams // C = 12 amu ii. 1 mol Pb = 207 grams // Pb = 207 amu iii. .5 mol C = 6 grams // .5C = 6 amu iv. .5 mol Pb = 103.5 grams // .5Pb = 103.5 amu 5. Atomic Theory of Mass: a. Law of conservation of mass: i. the total # of mass before the reaction will always be the same # of mass after the reaction ii. when two elements A and B combine to form more than one compound 6. Radioactivity: a. The spontaneous emission of radiation 7. Atomic Structure: -19 a. Electronic charge: 1.602 x 10 C -24 b. The atomic mass unit: amu = 1.66054 x 10 g c. Atomic number: the number of protons in an element 8. Atomic Weight: a. Determines the average atomic mass of an element b. (▯▯▯▯▯▯▯ ▯▯▯▯) (▯▯▯▯▯▯▯▯▯ ▯▯ ▯▯▯▯▯▯▯) ▯▯▯ ▯▯ ▯▯▯ ▯▯▯▯▯▯▯▯ ▯▯ ▯▯▯▯ ▯▯▯▯▯▯▯ 9. Molecules and Chemical Formulas: a. Halogens: H , O , N , F , Cl , Br , I 2 2 2 2 2 2 2 b. Molecular compounds: i. Composed of molecules containing more than 1 type of atom c. Chemical Formulas: i. Indicate the actual number of atoms in a molecule d. Empirical Formula: i. Relative number of atoms of each type of molecule 10. Ions and Ionic Compounds: a. Ion: when electrons are added/removed from an atom b. Cations: positive charge (lose electron) c. Anions: negative charge (gain electron) d. Polyotomic Ion: atoms joined together with a net positive/negative charge 11. Predicting Ionic Charges: a. Noble gas: nonreactive elements that form very few compounds b. Many atoms gain/lose electrons to end up with the same number of electrons as their closest noble gas 12. Ionic Compounds: a compound made up of cations and anions a. Identify an Ionic Compound: i. Cations are metal ions ii. Anions are non-metal ions iii. Generally combines (cat + an) 13. Names and Formulas 1. mono- 6. hexa- 7. hepta- 2. di- 8. octa- 3. tri- 9. nona- 4. tetra- 5. penta- 10. deca-
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