1 / 25

Chemical Equations

Chemical Equations. Counting atoms Balancing chemical equations Classifying chemical reactions Writing word & formula equations. Counting atoms. How many atoms of each element are present in the following: Ca 3 (PO 4 ) 2 H 2 SO 4 H 2 C 6 H 6 O 6 4. 2 Pb (NO 3 ) 2. Counting atoms.

dutch
Download Presentation

Chemical Equations

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. Chemical Equations Counting atoms Balancing chemical equations Classifying chemical reactions Writing word & formula equations

  2. Counting atoms How many atoms of each element are present in the following: • Ca3(PO4)2 • H2SO4 • H2C6H6O6 4. 2 Pb(NO3)2

  3. Counting atoms How many atoms of each element are present in the following: 5. 3 Na2SO4 6. 6 KClO3 7. Al2(SO4)3

  4. Counting atoms In the following equations, one of the reactants is in bold type. Do you find the same number of atoms of this element on both sides of the equation? 8. 2 KCl + Pb(NO3)2 KNO3 + PbCl2 9. (NH4)3PO4 + Sr(OH)2 Sr3(PO4)2 + NH4OH 10. 6 CO2 + 6 H2O  C6H12O6 + 6 O2 11. 4 Si2H3 + 11 O2 4 SiO2 + 6 H2O 12. Fe2(C2O4)3 3 FeC2O4 + 2 CO2

  5. Chemical Equations Read pages 240 – 254 • answer questions p. 254 # 1-5

  6. Balancing Chemical Equations According to the law of conservation of mass, matter cannot be created or destroyed. So… in a chemical reaction atoms cannot be created or destroyed – if there are 4 atoms of nitrogen on the reactants side of an equation, there must be 4 atoms of nitrogen on the products side. Pb(NO3)4 + CaSO4 ---> Pb(SO4)2 + Ca(NO3)2

  7. Balancing Chemical Equations Pb(NO3)4 + CaSO4 ---> Pb(SO4)2 + Ca(NO3)2 Examine the above chemical equation. Is the nitrogen balanced?_____ If not, how many atoms of nitrogen are on the reactants side of the equation?_____ How many atoms of nitrogen are produced?_____ How can the nitrogen atoms be balanced, or equal, on both sides of the equation? (by placing a coefficient of 2 in front of the calcium nitrate product) __Pb(NO3)4 + __ CaSO4 ---> ___ Pb(SO4)2 + 2 Ca(NO3)2

  8. Balancing Chemical Equations One method of balancing is balancing by inspection – also known as trial and error. Most textbooks and many teachers teach this method. It is effective, though may lead to frustration when trying to balance certain types of chemical equations. To balance by trial and error: • Pick one element on the product side and balance it • Then, choose another element and balance • Repeat for each and every element present • The last step is to go back and re-check each element to verify that each is still balanced. • If they are not balanced, continue the process… (hence the name: trial and error).

  9. Balancing Chemical Equations __Pb(NO3)4 +__CaSO4 --->__Pb(SO4)2 + __Ca(NO3)2 To balance the entire reaction you need coefficients of 1, 2, 1, 2 – reading left to right.

  10. TheAmazing sickles’ Seven Step Method! 1. check for diatomic molecules (these exist only in nature bonded together – they do not exist as a single atom) you need to learn these 7 diatomic elements!!! (regardless of the method you use) • they are: H2, N2, O2, F2, Cl2, Br2, and I2 shown here • if these elements are present in a reaction, they must have a subscript of 2 • Fe + O ---> Fe2O3 must be changed to Fe + O2 ---> Fe2O3 2. balance the metal atoms present 3. balance the nonmetal atoms present 4. balance oxygen (if it is present as O2) 5. balance hydrogen (if it is present as H2) 6. recount all atoms to check if they are balanced 7. if the coefficients can be reduced to simpler whole numbers reduce them. for example, if you have coefficients of 4, 2, 4, 4 – reduce them to 2, 1, 2, 2. if the coefficients are 4, 3, 4, 4 – they cannot be reduced

  11. Balancing equations ws 1 • ___ NH3 + ___ O  ___ NO + ___ H20 • __ HNO3 + __ Mg(OH)2 __ H2O + __ Mg(NO3)2

  12. Balancing equations ws 1 • ___ H3PO4 + ___ NaBr ___ HBr + ___ Na3PO4 4. ___ C + ___ H2 ___ C3H8

  13. TheAmazing sickles’ Seven Step Method! ‘Advanced’ 1. check for diatomic molecules (these exist only in nature bonded together – they do not exist as a single atom) you need to learn these 7 diatomic elements!!! (regardless of the method you use) • they are: H2, N2, O2, F2, Cl2, Br2, and I2 shown here • if these elements are present in a reaction, they must have a subscript of 2 • Fe + O ---> Fe2O3 must be changed to Fe + O2 ---> Fe2O3 2. balance the metal atoms present 3. balance the nonmetal atoms present 3.5 balance polyatomic ions as a group (*IF they appear on both sides of the equation) 4. balance oxygen (if it is present as O2) 5. balance hydrogen (if it is present as H2) 6. recount all atoms to check if they are balanced • if the coefficients can be reduced to simpler whole numbers reduce them.

  14. Balancing equations ws 1 9. _ CuSO4 + __ NaOH __ Cu(OH)2 + __ Na2SO4

  15. Classifying Chemical Reactions Read pages 256 – 263 • answer questions p. 264 # 1-4

  16. Classifying Chemical Reactions 5 Types of Chemical Reactions: • Synthesis • Decomposition • Single Replacement (Displacement) • Double Replacement (Displacement) • Combustion

  17. Classifying Chemical Reactions Synthesis reactions: Two (or more) elements (or compounds) combining to form a compound simple + simple (+simple)  complex H2 + O2  H2O CaO + H2O  Ca(OH)2

  18. Classifying Chemical Reactions Decomposition reactions: A compound breaks down to form two (or more) elements (or compounds) complex  simple + simple (+simple) H2O  H2 + O2 KClO3  KCl + O2

  19. Classifying Chemical Reactions Single Replacement reactions: One element replaces a second element in a compound to form a new compound and a different element. element A + compound X element B + compound Y Al + CuCl2  Cu + AlCl3

  20. Classifying Chemical Reactions Double Replacement reactions: One element in a compound replaces an element in another compound (& the 2nd element takes the 1st element’s place). compound A + compound B compound X + compound Y Cu(NO3)2 + NaOH  Cu(OH)2 + NaNO3

  21. Classifying Chemical Reactions Combustion reactions: A hydrocarbon (CxHy) reacts with oxygen to form carbon dioxide and water CxHy + O2  CO2 + H2O CH4 + O2  CO2 + H2O C2H5OH + O2  CO2 + H2O

  22. Classifying Chemical Reactions 5 Types of Chemical Reactions: • Synthesis a + b  1 product • Decomposition 1 reactant  x + y • Single Replacement element + cmpd element + cmpd • Double Replacement (Displacement) cmpd + cmpd cmpd+ cmpd • Combustion CxHy + O2  CO2 + H2O

  23. Classifying Chemical Reactions D • HgO Hg + O • Na + H2O NaOH + H2 • S8 + O2 SO3 • HNO3 + Mg(OH)2 H2O + Mg(NO3)2 • CF4 + Br  CBr4 + F • C7H16 + O2 CO2 + H2O • Si2H3 + O2 SiO2 + H2O SR S DR SR C DR

  24. TheAmazing sickles’ Combustion Method! ‘Super’ 1. double the hydrocarbon 2. balance the C 3. balance the H • balance the O (using 02…) • reduce, if necessary

  25. TheAmazing sickles’ Combustion Method! ‘Super’ ___C7H16 + ___O2 ___CO2 + ___H2O ___ C3H7OH + ___ O2 ___ CO2 + ___ H2O

More Related