1. Ch.2&3, Chemistry, the Central Science

2. Recall the discovery of the atom and origin of atomic number and mass (pp.39-44). Atomic masses are relative; Carbon-12 is the standard. The atom is very small, the unit Angstrom (10 -10 m) is used when discussing atomic measurements.

3. Recall isotopes and isotopic notation (pp.46-47): Remember, isotopes vary in their numbers of neutrons. In an isotope name, the number following the dash is the mass number, p + n. In isotopic notation, atomic number goes to bottom left of element symbol, mass number to upper left, and charge (if there is one) to upper right.

4. Fill in the following table: Isotope Name Isotopic Notation # of protons # of neutrons charge# of electrons Iodine-128 128 I -1 53 7554 8713686 Bismuth- 210 +3

5. Recall periodic table structure and nomenclature (pp.49-52)… names of groups, classifications (metal, nonmetal, metalloid), common charges, etc.

6. Recall molecules, ions, formula units (pp.52-56). Recall the diatomic elements (BrINClHOF), how to name compounds and write formulas (pp.59-65). There are two systems… the Roman numeral system for ionic and the prefix system for molecular. Remember how to name/write acids too. (Chem I flow charts and rules attached.) Know molecular compound prefixes from p.65

7. The following polyatomic ions and oxyanion rules must FOREVER be committed to memory. They will not be provided for you ever again. ammoniumNH 4 +1 hydroxideOH -1 acetateC 2 H 3 O 2 -1 or CH 3 COO -1 bromate *BrO 3 -1 chlorate *ClO 3 -1 cyanideCN -1 iodate *IO 3 -1 nitrate *NO 3 -1 carbonateCO 3 -2 sulfate *SO 4 -2 phosphate*PO 4 -3

8. * Rules for the oxyanions (the …ate polyatomics): 1 less O than …ate → …ite Ex: ClO 2 -1 is chlorite 2 less O than …ate → hypo…ite Ex: ClO -1 is hypochlorite 1 more oxygen than …ate → per…ate Ex: ClO 4 -1 is perchlorate (Note: ion charges do not change) Be familiar with common anions on p.63 and listed on your periodic table that are not included in the must- knows.

9. Recall how to predict oxidation states for monatomic ions based on position in the periodic table: Alkali metals (Group 1) always +1 charged. Alkaline earth metals (Group 2) always +2 charged. Group 13, most common charge is +3. Group 14, common charges are +4 & +2. C, Si, and Ge can be –4 also. Group 15, common charges are –3, +3, and +5. Group 16, most common charge is –2. Others are +2, +4 and +6. Halogens (Group 17) almost always –1 charged. Noble gases (Group 18) tend to remain neutral.

10. Recall how to write and balance chemical equations and basic classifications of reactions… synthesis, decomposition, combustion, single replacement, double replacement (pp.78-84).

11. NEW: Expanding on predicting products: alkali metal + water → metal hydroxide + hydrogen gas Ex: 2Na + 2H 2 0 → 2NaOH + H 2 combustion of a hydrocarbon (even containing oxygen): hydrocarbon + oxygen → carbon dioxide + water Ex: C 6 H 12 O 6 + 40 2 → 6CO 2 + 6H 2 O metal and nonmetal synthesis: metal + nonmetal → metal salt Ex: 2K + Cl 2 → 2KCl

12. decomposition of metal carbonates: metal carbonate → metal oxide + carbon dioxide Ex: MgCO 3 → MgO + CO 2 decomposition of metal chlorates: metal chlorate → metal chloride + oxygen gas Ex: 2KClO 3 → 2KCl + 3O 2 nonmetal oxides and water produce acids: nonmetal oxide + water → acid Ex: N 2 O 5 + H 2 O → 2HNO 3

13. metal oxides and water produce bases: metal oxide + water → base Ex: MgO + H 2 O → Mg(OH) 2 nonmetal oxides form salts: metal oxide + nonmetal oxide → metal salt Ex: MgO + N 2 O 5 → Mg(NO 3 ) 2

14. Recall how to calculate atomic and molar (molecular) masses (pp.84-86). Recall % composition (% by mass) (pp.85-86) Recall how to use the mole to convert to and from the microscopic (molecular) and the macroscopic (measurable) worlds (pp.86-92) using the factor-label method. Mole to mass, mass to mole…use molar mass. Mole to particle, particle to mole… use Avogadro’s Number.

15. Recall that correct terminology for the mole depends on the identity of the substance: Substance Identity Correct Terminology monatomic element1 mole is 6.02x10 23 atoms of the element molecular compound or diatomic element 1 mole is 6.02x10 23 molecules of the compound or element ionic compound 1 mole is 6.02x10 23 formula units of the compound ions 1 mole is 6.02x10 23 ions or particles

16. Recall stoichiometry problem solving (pp.96- 99). Recall limiting reactant problem solving and %yield (pp.99-103).