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Principles of Chemistry 1 Test 1 Review

Principles of Chemistry 1 Test 1 Review. As Understood by Bo… http://www.searchles.com/channels/show/3584. Chapter 1. Follow along in notes… Significant Figures SI Units to Know Kilo = 10 3 = 1000 Centi = 10 -2 (ex. 100 cm = 1 m) Milli = 10 -3 (ex. 1000 mm = 1 m)

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Principles of Chemistry 1 Test 1 Review

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  1. Principles of Chemistry 1Test 1 Review As Understood by Bo… http://www.searchles.com/channels/show/3584

  2. Chapter 1 • Follow along in notes… • Significant Figures • SI Units to Know • Kilo = 103 = 1000 • Centi = 10-2 (ex. 100 cm = 1 m) • Milli = 10-3 (ex. 1000 mm = 1 m) • Micro = 10-6 (ex. 100,000 µm = 1 m) • Nano = 10-9 • Know how to use temp. conversion eqns too!

  3. Chapter 1 • Precision vs. Accuracy • Ex. - Target • Questions on Chapter 1?

  4. Chapter 2 • Describing atoms… • Z = atomic # = p+ • A = mass # = p+ + n0 • Therefore…# of n0 = A-Z

  5. Chapter 2 • Ex. 20Ne and 21Ne, how many neutrons and protons in each • Z = 10 = p+ for both • 20Ne => A = 20 = p+ + n0 • n0 = A - Z => 20 - 10 = 10 • 21Ne => A = 21 = p+ + n0 • n0 = A - Z => 21 - 10 = 11 • What does that make these two forms of Ne?

  6. Chapter 2 • ISOTOPES! • Same element with different mass • Same Z (# of p+) but different number of n0 • Ex in class of Carbon-12 and Carbon-14

  7. Chapter 2 • How to find atomic mass (average of masses of the isotopes) based on % abundances… • How to find % abundance of and element of an based on atomic masses of the isotopes…

  8. Chapter 2 • Periodic Table • Where Z # Located, Atomic symbol, atomic mass • www.dayah.com/periodic • Chalocogens (6A) - “Ore Forming” • Charges based on Groups (1A, 2A, 3A, 5A, 6A, 7A) • Staircase

  9. Chapter 2 • Now for some entertainment • http://www.youtube.com/watch?v=GFIvXVMbII0&NR=1

  10. Chapter 2 • List of elements to know • Al, Ar, As, Ba, B, Br, Ca, C, Cl, Cr, Co, Cu, F, Au (Like Akron U, the gold standard!!!) • He, H, I, Kr, Fe, Pb, Li, Mg, Mn, Hg, Ne, N, Ni, O, P, Pt, Pu, K, Rn, Si, Ag, Na, S, Sn, U, Xe, Zn • Which exist as diatomic molecules?

  11. Chapter 2 • The 7 (Plus H) on the periodic table are all diatomic in nature • H2, N2, O2, F2,Cl2, Br2, I2 • These are all covalent compounds, they share e- equally • Ionic Compounds • Usually a metal and a nonmetal • One cation (+) and one anion (-)

  12. Chapter 2 • IF YOU DO NOT MEMORIZE THESE, CHEMISTRY WILL BE VERY DIFFICULT FOR YOU AND YOU WILL DO POORLY ON THIS EXAM!!! • Chapter 2

  13. Chapter 2 • Why do chemists like Nitrates so much? They’re cheaper than day rates!

  14. Chapter 2 • IF YOU DO NOT MEMORIZE THESE, CHEMISTRY WILL BE VERY DIFFICULT FOR YOU AND YOU WILL DO POORLY ON THIS EXAM!!!

  15. Chapter 2 • Another one to know…

  16. Chapter 2 • Acids… • “-ate” ion = “-ic” acid (CH3COOH) • “-ide” ion = hydro____ic acid [HCl (aq)] • Ionic Compound Naming (Metal and Nonmetal) • CaCl2, NaCl, etc. Don’t use di-tri, etc. • Lowest ratio of components • Binary Covalent Naming (Two non-metals) • Don’t need prefix for 1st element • 2nd element has “-ide” ending • 2nd element has di, tri, etc prefix • So name BF3…

  17. Chapter 2

  18. Chapter 2 • Calculating molecular (and formula) mass • Molecular for covalently bonded compounds, formula for ionic compounds • Ex. Calculate the molar mass of Ca(BO2)2*6H2O

  19. Chapter 2 • Ca(BO2)2*6 H2O • How many Calcium atoms? What is atomic mass of Calcium? • 1 Calcium at 40.08g/mol • How many Borons? • 2 @ 10.81 g/mol • How many Oxygens? • 4 from Ca(BO2)2 and 6 from H2O @ 16 g/mol • How many Hydrogens? • 12 @ 1.008 g/mol

  20. Chapter 2 • Ca(BO2)2*6 H2O • 40.08(1 Ca)+10.81(2 B)+16(10 O)+1.008(12 H) = 233.796 g/mol

  21. Chapter 3 • Do you have a mole problem? • Call Avagadro at 602-1023

  22. Chapter 3 • Recommend programing Avagadro’s Number into your calculator • TI-83 • Put in number, STO->, ALPHA, A • Atomic mass in amu = mass of one mole in grams • Ex. Atomic for carbon is 12.01 amu, molar mass is 12.01 g/mol

  23. Chapter 3 Chemistry Island Gram island Avagadro’s Bridge M.W. Bridge Mol Island “Entity” Island

  24. Practice • Which formula of an ionic compound would NOT be correct • ( a) Na2SO4 • ( b) MgCO3 • ( c) Ca2NO3 • ( d) NH4Cl

  25. Practice • Ca2+ and NO3-, should be Ca(NO3)2

  26. Practice • Calculate the number of oxygen atoms in 29.34 g of sodium sulfate.

  27. Practice • What does sodium sulfate look like • Na2SO4 • Now what? • Formula weight of Na2SO4

  28. Practice • What is the % of C in sucrose (C12H22O11) by mass? • Pretend you have 1 mol of sucrose • 12 C atoms in 1 mol • 12.01 g/mol for C • M.W. for sucrose = 342.296

  29. Practice • Which is a chemical change? • Melting wax • Boiling water • Broiling steak on a grill • Carving a piece of wood • Condensing water vapor into rainfall

  30. Practice • Grilling a steak • Give the correct formula and type of bonding for sodium oxide.

  31. Practice • Metal and non-metal, probably ionic • Na = Sodium, Charge 1+ • Oxide = O, Charge 2- • Na2O

  32. Practice • What is the correct name for KClO3? • Potassium Chlorate • Potassium Chloride • Potassium Chlorite • Potassium (I) Chlorite • Potassium (I) Chlorate

  33. Practice • K+ and ClO3- • Potassium ion and chlorate ion • Potassium Chlorate

  34. Practice • Balance the Equation • B2O3 + HF BF3 + H2O B = 2 B = 1 O= 3 O = 1 H = 1 H = 2 F = 1 F = 3 Lets start with the B, make them equal on both sides, add 2 to BF3

  35. Practice • B2O3 + HF 2 BF3 + H2O B = 2 B = 2 O= 3 O = 1 H = 1 H = 2 F = 1 F = 6 Now lets fix the F’s, add 6 to HF on Left side

  36. Practice • B2O3 + 6HF 2 BF3 + H2O B = 2 B = 2 O= 3 O = 1 H = 6 H = 2 F = 6 F = 6 Now H2O is all that is left to fix…add a 3 to H2O, it will give same # of H’s and O’s on right and left

  37. Practice • B2O3 + 6HF 2 BF3 + 3H2O B = 2 B = 2 O= 3 O = 3 H = 6 H = 6 F = 6 F = 6

  38. Practice • Bromine-81 (81Br) isotope. Select the combination which lists the correct atomic #, neutron #, and mass #, respectively • 46,81,35 • 35,46,81 • 81,46,35 • 35,81,116

  39. Practice • Z = atomic # = 35 for Br from periodic table • A = mass # = p+ + n0 = 81 • n0 = A-Z = 81-35 = 46

  40. Practice • What volume, in L, of 10 M HCl is needed to make 2.00L of a 2.00 M HCl solution by dilution with water?

  41. Practice • M1=10 M • V1= Unkn • M2= 2.00 M • V2 = 2.00 L

  42. Practice • Which of the following is a metalloid? • Z • S • Br • C • Ge

  43. Practice • Remember where metalloids are? • Staircase… • Ge is a Metalloid

  44. Practice • Empirical Formula • Elemental analysis of an Ionic compound done, shows 2.82 g Na, 4.35 g Cl, 7.83 g O. What is the empirical formula of the compound? • Start => Find moles of each element present.

  45. Practice • Now divide by the smallest to find the ratio of each element to the others What is this compound called?

  46. Practice • NaClO4 • Na+ and ClO4- • Sodium and Perchlorate • Sodium Perchlorate

  47. Questions? http://www.youtube.com/watch?v=a45dXztokZM&feature=related

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