1 / 16

Quiz #5 Chemical Rxns and Safety

Why is it important to avoid eating in a chemistry lab? What is the correct way to write the formula for Hydrogen? In the formula Ca 3 (PO 4 ) 2 What elements are present? How many of each element is present in the formula of Calcium phosphate (in question 3)? Balance the following:

janice
Download Presentation

Quiz #5 Chemical Rxns and Safety

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. Why is it important to avoid eating in a chemistry lab? What is the correct way to write the formula for Hydrogen? In the formula Ca3 (PO4)2 What elements are present? How many of each element is present in the formula of Calcium phosphate (in question 3)? Balance the following: __N2 + __H2 __NH3 What does C2H6 (g) symbolize if this is the symbol for ethane? Predict the following reaction: __Al + __Cl2______ Poisonous chemicals could be left on the desk from previous experiments, eating in lab makes it likely that you will poison yourself. H2 Calcium, phosphorous, oxygen 3 Ca, 2 P, 8 O N2 + 3 H2 2 NH3 Gaseous ethane 2 Al+ 3 Cl2  2 AlCl3 Quiz #5 Chemical Rxns and Safety

  2. Practice Synthesis Rxns • Active metal oxides react with water to form hydroxides. ex: • K2O + H2O  ________ • Many oxides of nonmetals react with water to form oxyacids. ex: • P2O5 + 3 H2O  _________ • Some metal oxides react with nonmetal oxides to form salts. • CaO + SO3  ________ • Active metals react with halogens to form salts. • __Cs + Br2-  2KOH 2 H3PO4 CaSO4 2 2 CsBr

  3. __CsOH  __Al(OH)3  __Na2CO3  __CsClO3  __Mg(ClO3)2  __Ba(OH)2  2 CsOH  Cs2O + H2O 2 Al(OH)3  Al2O3 + 3H2O Na2CO3  Na2O + CO2 2 CsClO3 -> 2CsCl + 3 O2 Mg(ClO3)2  MgCl2 + 3 O2 Ba(OH)2  BaO + H2O Practice Decomposition reactions

  4. O O O O O O N N N N N N O O O O O O O O O O O O Single DisplacementA+ BX AX + Bor:Y + BX  BY + X • Replacement of a metal in a compound by another metal. 2 Al (s) + 3Pb(NO3)2 3Pb +2 Al(NO3)3 Pb2+ Al Pb2+ Al Pb2+

  5. O O O O O O N N N N N N O O O O O O O O O O O O Single DisplacementA+ BX AX + Bor:Y + BX  BY + X • Replacement of a metal in a compound by another metal. 2 Al (s) + 3Pb(NO3)2 3Pb +2 Al(NO3)3 Pb Al3+ Al3+ Pb Pb

  6. Single DisplacementA+ BX AX + Bor:Y + BX  BY + X • Replacement of a hydrogen in a compound by a metal. 2 Na (s) + 2 H2O (l) 2 NaOH (aq) + H2(g) H O Na Na H H O H

  7. Single DisplacementA+ BX AX + Bor:Y + BX  BY + X • Replacement of a hydrogen in a compound by a metal. Mg (s) + 2 HCl (aq) MgCl2(aq) + H2(g) Cl Mg H Cl H

  8. Single DisplacementA+ BX AX + Bor:Y + BX  BY + X • Replacement of halogens Cl2(g) + 2 KBr (aq) 2 KCl (aq) + Br2(g) Br Cl K Cl Br K

  9. http://ncsdweb.ncsd.k12.wy.us/roden/Chemistry/Forms%20PDF/Activity%20Series%20Chart.pdfhttp://ncsdweb.ncsd.k12.wy.us/roden/Chemistry/Forms%20PDF/Activity%20Series%20Chart.pdf

  10. Practice: Single Replacement Less active  • Lithium Fluorine • Potassium Chlorine • Barium Bromine • Strontium Iodine • Calcium • Sodium • Magnesium • Aluminum • Manganese • Zinc • Iron • Cadmium • Cobalt • Nickel • Tin • Lead • Hydrogen • Copper • Silver • Mercury • Gold • Elements CANNOT replace anything Above them. The reaction does NOT occur in this situation • Mg + 2 HCl  • 2 Fe + 6 HCl  • Zn + CuCl2  • Cu + ZnCl2  • Ni + PbCl2  • Sn + PbCl2  • Fe + 3 AgNO3  H2 + MgCl2 3 H2 + 2 FeCl3 Cu + ZnCl2 No reaction Pb + NiCl2 SnCl2 + Pb Fe(NO3)3 + 3Ag

  11. O O N N O O O O Double Replacement Reactions (double displacement) • Formation of a precipitate. • 2 KI (aq) + Pb(NO3)2 (aq)  PbI2 (s) + 2 KNO3 (aq) I Pb2+ I K K

  12. Double Replacement Reactions (double displacement) • Formation of a gas. • FeS (s) + 2 HCl(aq)  H2S (g) + FeCl2 (aq) S Fe2+ Cl Cl H H

  13. Double Replacement Reactions (double displacement) • Formation of a water. • NaOH (s) + HCl(aq)  H2O (l) + NaCl2 (aq) H O Na+ Cl H

  14. Combustion Reactions • A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. 2 H2 (g) + O2 (g)  2 H2O O H O H H H

  15. Combustion Reactions • A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. C3H8 (g) +5 O2 (g)  4 H2O + 3 CO2 O O O O H O H H H C O C C O H O H H O H O

  16. Combustion Reactions • A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. C3H8 (g) +5 O2 (g)  4 H2O + 3 CO2 O O H C O O H H H O H H O C H O O C O O H

More Related