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Unit 1 review

Unit 1 review. By: Makoto Bowering and Nick Ennen. Charges. Anions (has excess electron)– Has a negative charge Most common -1 charge : H-, F-, Cl -, Br-, I-, OH- -2 charge : O, O2, S -3 charge : N. Charges. Cations (has a less electrons) Has a positive charge Most common

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Unit 1 review

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  1. Unit 1 review By: Makoto Bowering and Nick Ennen

  2. Charges • Anions (has excess electron)– Has a negative charge • Most common -1 charge : H-, F-, Cl-, Br-, I-, OH- -2 charge : O, O2, S -3 charge : N

  3. Charges Cations (has a less electrons) Has a positive charge Most common 1+ : H, Li, Na, K, Cs, Ag 2+ : Mg, Ca, Sr, Ba, Zn, Cd 3+ : Al

  4. Bonds Covalent 2 non-metals Ex: FO H2O CH4 HCl

  5. Bonds Ionic 1 metal and 1 non-metal EX: NaCl NaF MgO

  6. Bonds Metallic 2 Metal EX: Diamond Bronze Copper

  7. Organic compounds 1 = meth- 2 = eth- 3 = prop- 4 = but- 5+ = a normal binary scale Alcohols have suffix ol and are and O-H bond

  8. Percent composition CH2O C= 40% H= 6.72% O= 53.28% Assume that the percent can be changed into grams and perform stoichiometry to get it to Moles. Once in moles divide by the lowest value to get the empirical forulma.

  9. Universal Gas Law PV=NRT P=Pressure (1.000 atm) V=Volume (L) N=Moles R=constant (0.08206 L*atm/Mol*K) T= Temperature (K = Tc + 273.15)

  10. Standard temperature and pressure STP- 273.15 k 1.00 atm 1 mole of gas 22.4 L

  11. Real gas equation (P+a(n/V)’2)(V-bn)= nRT First part = The factor that the regular PV=nRT value is off because of the fact that IMFA was not included Second part = The factor that the regular PV=nRT value is off because it now does not include the molecules themselves

  12. Partial Pressure P(molecule)=(n(a)/n(total))

  13. Root-Means-Square Speed This is the speed at which a molecule is moving. Urms= 3RT/M (all under a square root sign) M=Molar mass (Kg/mol) R= constant (8.314 J/Mol*K) T= Temperature (K)

  14. Limiting Reagent The limiting reagent limits the reaction from producing the greatest it can. The limiting reagent runs out before the excess reagent does. To find the value of the limiting reagent and excess reagent, all that is needed is stochiometery

  15. Limiting Reagent EX: A 2.00g sample of ammonia is mixed with 4.00g of oxygen. Which is the limiting reactant and how much excess reactant remains after the reaction has stopped?

  16. Limiting Reagent Step 1: write a balanced reaction 4NH3 + 5O2 4NO + 6H2O

  17. Limiting Reagent Step 2: finding which is limiting Use stoichiometry to calculate how much product is produced by each reactant. You can start with either reactant, and you can calculate for either product, but the product must be the same for both in order for the amounts to be compared.

  18. Limiting Reagent Step 3: finding the excess To find the amount of excess reactant, we must calculate how much of the non-limiting reactant actually did react with the limiting reactant.

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