1 / 48

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)

adrina
Télécharger la présentation

Principles of Chemistry 1 Test 1 Review

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related