#35 balance the following chemical equations a) SiI 4(s) + 2Mg (s)! Si (s) + 2MgI 2(s) Si = 1 I = 4 Mg = 1 2. Si = 1 I = 2 4 Mg = 1 2 (1,2,1,2)

Size: px
Start display at page:

Download "#35 balance the following chemical equations a) SiI 4(s) + 2Mg (s)! Si (s) + 2MgI 2(s) Si = 1 I = 4 Mg = 1 2. Si = 1 I = 2 4 Mg = 1 2 (1,2,1,2)"

Transcription

1 #35 balance the following chemical equations a) SiI 4(s) 2Mg (s)! Si (s) 2MgI 2(s) Si = 1 I = 4 Mg = 1 2 Si = 1 I = 2 4 Mg = 1 2 SiI 4(s) 2Mg (s)! Si (s) 2MgI 2(s) (1,2,1,2) b) MnO 2(s) 2Mg (s)! Mn (s) 2MgO (s) Mn = 1 Mn = 1 O = 2 O = 1 2 Mg = 1 2 Mg = 1 2 MnO 2(s) 2Mg (s)! Mn (s) 2MgO (s) (1,2,1,2) c) 8Ba (s) S 8(s)! 8BaS (s) Ba = 1 8 Ba = 1 8 S =8 S =1 8 8Ba (s) S 8(s)! 8BaS (s) (8,1,8) d) 4NH 3(g) 3Cl 2(g)! 3 Cl (s) NCl 3(g) N = 1 4 N = 1 1 = 2 N = 3 1 = 4 H = 3 12 H = 4 12 Cl = 2 6 Cl = 1 3 = 4 Cl = 3 3 = 6 4NH 3(g) 3Cl 2(g)!3 Cl (s) NCl 3(g) (4, 3, 3, 1)

2 #36 balance the following chemical equations a) Ba( ) 2(aq) Na 2 CrO 4(aq)! BaCrO 4(s) 2Na(aq) Ba = 1 N = 2 O = 6 4 = 10 Na = 2 Cr = 1 Ba = 1 O = 4 3 = 7 O = 4 6 = 10 Na = 1 2 Cr = 1 Ba( ) 2(aq) Na 2 CrO 4(aq)! BaCrO 4(s) 2Na(aq) (1, 1, 1, 2) b) C 2 H 5 OH (l) 3O 2(g)! 2CO 2(g) 3H 2 O (l) C = 2 C = 1 2 H = 6 H = 2 6 O = 1 2 = 3 O = 2 1 = 3 O = 1 6 = 7 O = 4 3 = 7 C 2 H 5 OH (l) 3O 2(g)! 2CO 2(g) 3H 2 O (l) (1, 3, 2, 3) c) CaC 2(s) 2H 2 O (l)! Ca(OH) 2(s) C 2 H 2(g) Ca = 1 Ca = 1 C = 2 C = 2 H = 2 4 H = 2 2 = 4 O = 1 2 O = 2 CaC 2(s) 2H 2 O (l)! Ca(OH) 2(s) C 2 H 2(g) (1, 2, 1, 1)

3 1. water is am important solvent because a. is a polar molecule i. O H bond is polar covalent 1. the oxygen side is partially negative 2. the hydrogen side is partially positive 3. two dipole moments are present ii. tetrahedral arrangement 1. two lone pairs 2. two shared pairs iii. bent or V shape with <109.5! iv. the two dipole moments do not cancel b. has a partially positive region i. which attracts negative ions c. has a partially negative region i. which attracts positive ions d. can dissolve many ionic compounds and polar molecules 2. skip

4 3. precipitate = ionic compounds a. all ionic compounds = net charge zero i. charge cancellation takes place 1. 1:1 ratio :1 ratio :2 ratio :1 ratio :3 ratio :2 ratio :3 ratio

5 4. ions of electrolytes = cations and anions a. in water, the cations and anions separate (dissociate) b. anions = negative ions: move towards the positive end of the wire c. cations = positive ions: move towards the negative end of the wire 5. strong electrolyte = soluble substances a. all particles dissolve/dissociate b. all cations and anions separate c. many ions produced d. strong electric current produced e. examples: i. substances with nitrate ions 1. ii. substances with sodium, potassium, and ammonium ions 1. Na 2. K Na is soluble a. sodium nitrate dissociates b. separates into individual ions, and stay separated c. Na! Na 7. slightly soluble = not soluble a. does not visibly dissolve b. slightly soluble = insoluble i. no difference

6 8. predict whether soluble or insoluble a. barium nitrate i. soluble ii. rule #1 b. potassium carbonate i. soluble ii. rule #2 c. sodium sulfate i. soluble ii. rule #2 d. copper (II) hydroxide i. insoluble ii. rule #5 e. mercury (I) chloride i. insoluble ii. rule #3 (exception) f. ammonium phosphate i. soluble ii. rule #2 g. chromium (III) sulfide i. insoluble ii. rule #6 h. lead (II) sulfate i. insoluble ii. rule #4 (exception)

7 9. predict whether soluble or insoluble a. iron (III) hydroxide i. insoluble ii. rule #5 b. calcium carbonate i. insoluble ii. rule #6 c. cobalt (III) phosphate i. insoluble ii. rule #6 d. silver chloride i. insoluble ii. rule #3 (exception)

8 10. predict the identity of the precipitate formed a. calcium sulfate rule #4 (exception) Na Cl Na Cl 2 SO 4 Ca 2! Na Na Cl Cl Na Na Cl Cl Na 2 SO 4 Ca 2! Cl Na CaSO 4 Cl Na 2 SO 4(aq) CaCl 2(aq)! 2NaCl (aq) CaSO 4(s) CaSO 4 b. silver Na iodide 2 SO 4(aq) CaCl 2(aq)! 2NaCl (aq) CaSO 4(s) rule #3 (exception) I Ag! AgI I (aq) Ag(aq)! (aq) AgI (s) K K Pb 2! PO 4 3 K Pb 3 (PO 4 ) 2 K K 3 PO 4(aq) Pb( ) 2(aq)! K(aq) Pb 3 (PO 4 ) 2(s) 2K 3 PO 4(aq) 3Pb( ) 2(aq)! 6K(aq) Pb 3 (PO 4 ) 2(s) K = 3 6 K = 1 6 P = 1 2 P = 2 O = 4 6 = 10 O = 3 8 = 11 O = 8 18 = 26 O = 18 8 = 26 Pb = 1 3 Pb = 3 N = 2 6 N = 1 6 2K 3 PO 4(aq) 3Pb( ) 2(aq)! 6K(aq) Pb 3 (PO 4 ) 2(s) (2,3,6,1)

9 c. lead (II) phosphate rule #6 K K Pb 2! PO 4 3 K Pb 3 (PO 4 ) 2 K K 3 PO 4(aq) Pb( ) 2(aq)! K(aq) Pb 3 (PO 4 ) 2(s) 2K 3 PO 4(aq) 3Pb( ) 2(aq)! 6K(aq) Pb 3 (PO 4 ) 2(s) K = 3 6 K = 1 6 P = 1 2 P = 2 O = 4 6 = 10 O = 3 8 = 11 O = 8 18 = 26 O = 18 8 = 26 Pb = 1 3 Pb = 3 N = 2 6 N = 1 6 2K 3 PO 4(aq) 3Pb( ) 2(aq)! 6K(aq) Pb 3 (PO 4 ) 2(s) (2,3,6,1)

10 Cl Fe(OH) 3 d. iron (III) hydroxide rule #5 sodium hydroxide iron (III) chloride NaOH FeCl 3 Cl Na Fe 3 OH Cl! Na Cl NaOH (aq) FeCl 3(aq)! NaCl (aq) Fe(OH) 3(s) 3NaOH (aq) FeCl 3(aq)! 3NaCl (aq) Fe(OH) 3(s) Na = 1 3 Na = 1 3 O = 1 3 O = 3 H = 1 3 H = 3 Fe = 1 Fe = 1 Cl = 3 Cl =1 3 3NaOH (aq) FeCl 3(aq)! 3NaCl (aq) Fe(OH) 3(s) (3,1,3,1) e. no precipitate formed rule #2 potassium sulfate sodium nitrate K 2 SO 4 Na K K Na 2 SO 4! Na K 2 SO 4 Na K 2 SO 4(aq) Na(aq)! K(aq) Na 2 SO 4 (aq) K 2 SO 4(aq) 2Na(aq)! 2K (aq) Na 2 SO 4 (aq) K = 2 K = 1 2 O = 4 3 = 7 O = 3 4 = 7 O = 4 6 = 10 O = 6 4 = 10 Na =1 2 Na = 2 N =1 2 K 2 SO 4(aq) 2Na(aq)! 2K(aq) Na 2 SO 4(aq) (1,2,2,1)

11 f. barium carbonate rule #6 sodium carbonate barium nitrate Na 2 CO 3 Ba( ) 2 Na 2 CO 3 Ba 2! Na Na Na BaCO 3 Na 2 CO 3(aq) Ba( ) 2(aq)! Na(aq) BaCO 3(s) Na 2 CO 3(aq) Ba( ) 2(aq)! 2Na(aq) BaCO 3(s) Na = 2 C = 1 O = 3 6 = 9 Ba = 1 N = 2 Na = 1 2 C = 1 O = 3 3 = 6 O = 6 3 = 9 Ba = 1 Na 2 CO 3(aq) Ba( ) 2(aq)! 2Na(aq) BaCO 3(s) (1,1,2,1)

12 11. write a balanced molecular equation a. nitric acid barium chloride! H BaCl 2! Cl Ba 2 H Cl H Cl Ba 2! H(aq) BaCl 2(aq)! HCl (aq) Ba( ) 2(aq) 2H(aq) BaCl 2(aq)! 2HCl (aq) Ba( ) 2(aq) H = 1 2 H = 1 2 H N = 12 2 N O = N O = 26 O Ba = = 316 O Ba = = 61 Ba Cl = 21 Ba Cl = 1 2 Cl = 2 Cl = 1 2 2H(aq) BaCl 2(aq)! 2HCl (aq) Ba( ) 2(aq) 2HNO (2,1,2,1) 3(aq) BaCl 2(aq)! 2HCl (aq) Ba( ) 2(aq) (2,1,2,1) no precipitate no rule precipitate # 1 and rule #3 b. ammonium rule # 1 and sulfide rule #3 cobalt (II) chloride! ( ) 2 S CoCl 2! Cl S 2 Co 2! Cl Cl CoS ( ) 2 S (aq) CoCl 2(aq)! Cl (aq) CoS (s) ( ) 2 S (aq) CoCl 2(aq)! 2 Cl (aq) CoS (s) N = 2 H = 8 H = 4 8 Co = 1 Co = 1 Cl = 2 Cl = 1 2 ( ) 2 S (aq) CoCl 2(aq)! 2 Cl (aq) CoS (s) (1,1,2,1) precipitate = CoS (s) rule #6

13 c. sulfuric acid lead (II) nitrate! H 2 SO 4 Pb( ) 2! H 2 SO 4 Pb 2! H H PbSO 4 H 2 SO 4(aq) Pb( ) 2(aq)! H(aq) PbSO 4(s) H 2 SO 4(aq) Pb( ) 2(aq)! 2H(aq) PbSO 4(s) H = 2 H = 1 2 S H = 11 2 O = 4 6 = 10 O S = 31 4 = 7 O = 63 4 = 10 7 Pb = 1 Pb O = 61 4 = 10 N Pb = = 21 N Pb = = 112 N = 2 H 2 SO 4(aq) Pb( ) 2(aq)! 2H(aq) PbSO 4(s) H(1,1,2,1) 2 SO 4(aq) Pb( ) 2(aq)! 2H(aq) PbSO 4(s) precipitate (1,1,2,1) = PbSO 4(s) rule precipitate #4 (exception) = PbSO 4(s) rule #4 (exception) d. calcium chloride potassium carbonate! CaCl 2 K 2 CO 3! Cl K K Cl Ca 2 2 CO 3! Cl K CaCO 3 CaCl 2(aq) K 2 CO 3(aq)!!"#$ (aq) %!CaCO 3(s) CaCl 2(aq) K 2 CO 3(aq)! &"#$ (aq) %!''CaCO 3(s) Ca = 1 Ca = 1 Cl = 2 Cl = 1 2 K = 2 K = 1 2 C = 1 C = 1 O = 3 O = 3 CaCl 2(aq) K 2 CO 3(aq)!!&"#$ (aq) %!CaCO 3(s) (1,1,2,1) precipitate = CaCO 3(s) rule #6

14 Na Cl CrPO 4 e. sodium acetate ammonium nitrate! NaC 2 H 3 O 2! Na C 2 H 3 O 2! Na C 2 H 3 O 2 NaC 2 H 3 O 2(aq) (aq)! Na(aq) C 2 H 3 O 2(aq) NaC 2 H 3 O 2(aq) (aq)! Na(aq) C 2 H 3 O 2(aq) Na = 1 Na = 1 C = 2 C Na = = 21 H = 3 4 = 7 H C = 27 O H = = 57 O H =3 = 7 2 = 5 N O = 2 3 = 5 N O = = = 52 N = 2 N = 1 1 = 2 NaC 2 H 3 O 2(aq) (aq)! Na(aq) C 2 H 3 O 2(aq) NaC (1,1,1,1) 2 H 3 O 2(aq) (aq)! Na(aq) C 2 H 3 O 2(aq) no (1,1,1,1) precipitate rule no precipitate #1 and rule #2 rule #1 and rule #2 f. sodium phosphate chromium (III) chloride! Na 3 PO 4 CrCl 3! Na Cl Na Cl Na PO 4 3 Cr 3 Cl! Na 3 PO 4(aq) CrCl 3(aq)!!NaCl (aq) CrPO 4(s) Na 3 PO 4(aq) CrCl 3(aq)! 3NaCl (aq) CrPO 4(s) Na = 3 Na = 1 3 P = 1 P = 1 O = 4 O = 4 Cr = 1 Cr = 1 Cl = 3 Cl = 1 3 Na 3 PO 4(aq) CrCl 3(aq)!!"NaCl (aq) CrPO 4(s) (1,1,3,1) precipitate = CrPO 4(s) rule #6

15 12. balance each of the following equations a. Ag(aq) H 2 SO 4(aq)! Ag 2 SO 4(s) H(aq) 2Ag(aq) H 2 SO 4(aq)! Ag 2 SO 4(s) 2H(aq) Ag = 1 2 Ag = 2 O = 3 4 = 7 O = 4 3 = 7 O = 6 4 = 10 O = 4 6 = 10 H = 2 H = 1 2 S =1 2Ag(aq) H 2 SO 4(aq)! Ag 2 SO 4(s) 2H(aq) (2,1,1,2) b. Ca( ) 2(aq) H 2 SO 4(aq)! CaSO 4(s) H(aq) Ca( ) 2(aq) H 2 SO 4(aq)! CaSO 4(s) 2H(aq) Ca = 1 N = 2 O = 6 4 = 10 H = 2 Ca = 1 O = 4 3 = 7 O = 4 6 = 10 H = 1 2 Ca( ) 2(aq) H 2 SO 4(aq)! CaSO 4(s) 2H(aq) (1,1,1,2) c. Pb( ) 2(aq) H 2 SO 4(aq)! PbSO 4(s) H(aq) Pb( ) 2(aq) H 2 SO 4(aq)! PbSO 4(s) 2H(aq) Pb = 1 N = 2 O = 6 4 = 10 H = 2 Pb = 1 O = 4 3 = 7 O = 4 6 = 10 H = 1 2 Pb( ) 2(aq) H 2 SO 4(aq)! PbSO 4(s) 2H(aq) (1,1,1,2)

16 Cl Fe(OH) write a balanced molecular equation a. ( ) 2 S (aq) CoCl 2(aq)! Cl S 2 Co 2! Cl Cl CoS ( ) 2 S (aq) CoCl 2(aq)! Cl (aq) CoS (s) ( ) 2 S (aq) CoCl 2(aq)! 2 Cl (aq) CoS (s) N = 2 H = 8 H N = S H = 14 8 Co = 1 Co S = = 11 Cl Co = 21 Cl Co = 12 Cl = 2 Cl = 1 2 ( ) 2 S (aq) CoCl 2(aq)! 2 Cl (aq) CoS (s) (NH (1,1,2,1) 4 ) 2 S (aq) CoCl 2(aq)! 2 Cl (aq) CoS (s) precipitate (1,1,2,1) = CoS (s) rule precipitate #6 = CoS (s) rule #6 b. NaOH (aq) FeCl 3(aq)! Cl Na Fe 3 OH Cl! Na Cl NaOH (aq) FeCl 3(aq)! NaCl (aq) Fe(OH) 3(s) 3NaOH (aq) FeCl 3(aq)! 3NaCl (aq) Fe(OH) 3(s) Na = 1 3 Na = 1 3 O = 1 3 O = 3 H = 1 3 H = 3 Fe = 1 Fe = 1 Cl = 3 Cl =1 3 3NaOH (aq) FeCl 3(aq)! 3NaCl (aq) Fe(OH) 3(s) (3,1,3,1) precipitate = Fe(OH) 3(s) rule #5

17 c. CuSO 4(aq) Na 2 CO 3(aq)! Na Na Cu CO 3! SO 4 2 SO 4 Na Na CuCO 3 CuSO 4(aq) Na 2 CO 3(aq)!!Na 2 SO 4(aq) "!CuCO 3(s) CuSO 4(aq) Na 2 CO 3(aq)! Na 2 SO 4(aq) "!CuCO 3(s) Cu = 1 Cu = 1 O = 4 3 = 7 O = 4 3 = 7 Na = 2 Na = 2 C = 1 C = 1 CuSO 4(aq) Na 2 CO 3(aq)!!Na 2 SO 4(aq) "!CuCO 3(s) (1,1,1,1) precipitate = CuCO 3 (s) rule #6

18 14. write balanced net ionic equation a. K 2 SO 4 Ca 2! K K CaSO 4 K 2 SO 4(aq) Ca( ) 2(aq)! K(aq) CaSO 4(s) K 2 SO 4(aq) Ca( ) 2(aq)! 2K(aq) CaSO 4(s) K = 2 O = 4 6 = 10 Ca = 1 N = 2 K = 1 2 O = 3 4 = 7 O = 6 4 = 10 Ca = 1 ME: K 2 SO 4(aq) Ca( ) 2(aq)! 2K(aq) CaSO 4(s)!"#$% &' 2 (aq)%(%so 4 (aq) Ca 2 (aq) 2 (aq)! &' (aq)% 2 (aq) CaSO 4(s) NIE: Ca 2 2 (aq) (%SO 4 (aq)! CaSO 4(s) )*,%.%/,01, % %

19 b. Fe 3 Na CO 3 2 Na! Na Fe 2 (CO 3 ) 3!"( ) 3(aq) Na 2 CO 3(aq)! Na(aq) Fe 2 (CO 3 ) 3(s) #!"( ) 3(aq) 3Na 2 CO 3(aq)! 6Na(aq) Fe 2 (CO 3 ) 3(s) Fe = 1 2 N = 3 6 O = 9 3 = 12 O = 18 9 = 27 Na = 2 6 C = 1 3 Fe = 2 N = 1 6 O = 3 9 = 12 O = 18 9 = 27 Na = 1 6 C = 3 ME: 2!"( ) 3(aq) 3Na 2 CO 3(aq)! 6Na(aq) Fe 2 (CO 3 ) 3(s) $%&'( #Fe 3 (aq)()(* (aq) 6Na 2 (aq) 3CO 3 (aq)! 6Na (aq) * (aq) Fe 2 (CO 3 ) 3(s) NIE: #Fe 3 2 (aq)()(3co 3 (aq)! Fe 2 (CO 3 ) 3(s),"(.*(

20 c. Ag I Ca 2! Ca 2 I AgI!"(aq) CaI 2 (aq)! Ca( ) 2(aq) AgI (s) #!"(aq) CaI 2 (aq) $!$ Ca( ) 2(aq) 2AgI (s) $!"$%$&$#$ '$%$&$#$ ($%$)$*$,$%$&$ $%$#$ $!"$%$&$#$ '$%$#$ ($%$*$,$%$&$ $%&$#$ $ ME: 2!"(aq) CaI 2 (aq)! Ca( ) 2(aq) 2AgI (s)./$ #Ag (aq)$0$# (aq) Ca 2 (aq) 2I (aq)! Ca 2 (aq) # (aq) 2AgI (s) #Ag (aq)$0$2i (aq)! 2AgI (s) [lowest combinations of coefficients required] './$ Ag (aq)$0$i (aq)! AgI (s) 1234$5)$647849:;<=>?$ $ $

21 d.!""#$%&"'()#*()!,''.#/!0'1223'*&04!,' PO 4 3 Co 2 2! SO 4 2 SO 4 Co 3 (PO 4 ) PO 4(aq) ''CoSO 4(aq)!'1 3 2 SO 4(aq) 'Co 3 (PO 4 ) 2(s) ' PO 4(aq) ''6CoSO 4(aq) '!' SO 4(aq) '77Co 3 (PO 4 ) 2(s) ' 8'9'6':' ;'9'<5'5=' >'9'<'5'?'9'=''='9'@'?'9'@''<5'9'5A' B#'9'<'6' C'9'<'6' ' 8'9'5':' ;'9'@'5=' >'9'5'?'9'=''@'9'<5'?'9'<5''@'9'5A' B#'9'6' C'9'<'6' ' ME: PO 4(aq) ''6CoSO 4(aq)!' SO 4(aq) 'Co 3 (PO 4 ) 2(s) ' B2DE' 3 : (aq) ''5PO 4 (aq) 3Co (aq) 3SO 4 (aq)! 6 (aq) 3SO 4 (aq) Co 3 (PO 4 ) 2(s) 82DE' 3Co 2 3 (aq) '5PO 4 (aq)! Co 3 (PO 4 ) 2(s) F&0,'G:' '

22 e.!"#$%"&'()*,$#&.)/)(.#*'#0)123)%&"#4".) Cl Sr 2 2 Hg 2 Cl! Sr 2 Hg 2 Cl 2 5#6,7(aq) )/)Hg (aq)!)Sr1 3 2(aq) /)Hg 2 Cl 2(s) ) 885#6,7(aq) )/)88Hg (aq) )!) Sr1 3 2(aq) /)88Hg 2 Cl 2(s) ) 5#)9):) 6,)9)7) ;<)9)7) =)9)7) >)9)?) ) 5#)9):) 6,)9)7) ;<)9)7) =)9)7) >)9?) ) ME: 5#6,7(aq) )/)Hg (aq)!)Sr1 3 2(aq) /)Hg 2 Cl 2(s) ) 62@A) Sr 2 (aq))/)7cl 2 (aq) Hg 2 (aq) 2 (aq)! Sr 2 (aq)) 2 (aq) Hg 2 Cl 2(s) =2@A) 2 Hg 2 (aq) /)7Cl (aq)! Hg 2 Cl 2(s) #',.)BC)1.D*.E"&$%!3) ) )

23 f. image ) F4#&'()F#$(&.)/),.4)1223)%&"#4".) Br Ba 2 Pb 2! Ba Br PbBr 2 G4G#7(aq) )/)Pb1 3 2(aq)!)Ba1 3 2(aq) /)PbBr 2(s) ) skip #44 88G4G#7(aq) )/)88Pb1 3 2(aq) )!) Ba1 3 2(aq) /)88PbBr 2(s) ) G4)9):) G#)9)7) HF)9):) =)9)7) >)9)?) ) G4)9):) G#)9)7) HF)9):) =)9)7) >)9)?) ) ME: G4G#7(aq) )/)Pb1 3 2(aq)!)Ba1 3 2(aq) /)PbBr 2(s) ) 62@A) Ba 2 aq))/)7br (aq) Pb 2 (aq) 2 (aq)! Ba 2 (aq)) 2 (aq) PbBr 2(s) =2@A) Pb 2 (aq) /)7Br (aq)! PbBr 2(s) #',.)BC)1.D*.E"&$%!3) ) )

insoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water

insoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of

More information

CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY

CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans

More information

elemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.

elemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another. CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two

More information

Chapter 8 Chemical Reactions

Chapter 8 Chemical Reactions Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate

More information

EXPERIMENT 10: Precipitation Reactions

EXPERIMENT 10: Precipitation Reactions EXPERIMENT 10: Precipitation Reactions Metathesis Reactions in Aqueous Solutions (Double Displacement Reactions) Purpose a) Identify the ions present in various aqueous solutions. b) Systematically combine

More information

5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES

5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES 5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES LEARNING OUTCOMES a) Be able to write formulae of simple compounds b) Be able to write

More information

HW 7 KEY!! Chap. 7, #'s 11, 12, odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones)

HW 7 KEY!! Chap. 7, #'s 11, 12, odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones) HW 7 KEY!! Chap. 7, #'s 11, 12, 15-21 odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, 72-75 all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones) 11) NOTE: I used the solubility rules that I have provided

More information

(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion

(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single

More information

IONIC CHARGES. Chemistry 51 Review

IONIC CHARGES. Chemistry 51 Review IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can

More information

Chapter 4 Suggested end-of-chapter problems with solutions

Chapter 4 Suggested end-of-chapter problems with solutions Chapter 4 Suggested end-of-chapter problems with solutions a. 5.6 g NaHCO 1 mol NaHCO 84.01 g NaHCO = 6.69 10 mol NaHCO M = 6.69 10 mol 50.0 m 1000 m = 0.677 M NaHCO b. 0.1846 g K Cr O 7 1 mol K 94.0 g

More information

CH 4 AP. Reactions in Aqueous Solutions

CH 4 AP. Reactions in Aqueous Solutions CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,

More information

The solvent is the dissolving agent -- i.e., the most abundant component of the solution

The solvent is the dissolving agent -- i.e., the most abundant component of the solution SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout

More information

Practice questions for Chapter 4

Practice questions for Chapter 4 Practice questions for Chapter 4 1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar

More information

Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent

Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,

More information

TYPES OF CHEMICAL REACTIONS

TYPES OF CHEMICAL REACTIONS TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility

More information

9/24/09 Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter

9/24/09 Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter 4.1-4.4 KEY VOCABULARY: 1. Ionic compound a compound composed of cations (+) and anions (-). Many ionic compounds dissociate

More information

Solubility Rules and Net Ionic Equations

Solubility Rules and Net Ionic Equations Solubility Rules and Net Ionic Equations Why? Solubility of a salt depends upon the type of ions in the salt. Some salts are soluble in water and others are not. When two soluble salts are mixed together

More information

Reaction Writing Sheet #1 Key

Reaction Writing Sheet #1 Key Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium

More information

Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11)

Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) 1 Solubility vs. Temperature 2 Solubility Table Anions SOLUBILITY Table 8.3 page 363 in MHR Cl Br I S OH SO CO 3 PO 3 SO 3 C 2 H 3

More information

Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions

Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are

More information

Chemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11

Chemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11 Chemical Reactions CHM 1032C Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. The Hindenburg Reaction Reactants are on left, products to the right. Arrow

More information

Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)

Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and

More information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 4. Aqueous Reactions and Solution Stoichiometry Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)

More information

EXPERIMENT 5 Double Replacement Reactions

EXPERIMENT 5 Double Replacement Reactions EXPERIMENT 5 Double Replacement Reactions PURPOSE a) To identify the ions present in various aqueous solutions. b) To systematically combine solutions and identify the reactions that form precipitates

More information

Solubility & Net Ionic review

Solubility & Net Ionic review Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds

More information

Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.

Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution. Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look

More information

Reactions in aqueous solutions Redox reactions

Reactions in aqueous solutions Redox reactions Reactions in aqueous solutions Redox reactions Redox reactions In precipitation reactions, cations and anions come together to form an insoluble ionic compound. In neutralization reactions, H + ions and

More information

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined). Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are

More information

D O UBLE DISPL Ac EMENT REACTIONS

D O UBLE DISPL Ac EMENT REACTIONS Experiment 8 Name: D O UBLE DISPL Ac EMENT REACTIONS In this experiment, you will observe double displacement reactions and write the corresponding balanced chemical equation and ionic equations. Double

More information

Chapter 6. Naming Compounds Writing Formulas

Chapter 6. Naming Compounds Writing Formulas Chapter 6 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell

More information

**The partially (-) oxygen pulls apart and surrounds the (+) cation. The partially (+) hydrogen pulls apart and surrounds the (-) anion.

**The partially (-) oxygen pulls apart and surrounds the (+) cation. The partially (+) hydrogen pulls apart and surrounds the (-) anion. #19 Notes Unit 3: Reactions in Solutions Ch. Reactions in Solutions I. Solvation -the act of dissolving (solute (salt) dissolves in the solvent (water)) Hydration: dissolving in water, the universal solvent.

More information

Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON

Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the

More information

Chapter 4. Types of Chemical Reactions and Solution Stoichiometry

Chapter 4. Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition

More information

Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry

Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry 13. Determine the concentrations of the solutions Solution A 4 particles 1.0 L Solution B 6 paticles 4.0 L Solution C 4 particles

More information

Types of Reactions: Reactions

Types of Reactions: Reactions 1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous

More information

Chapter 4. The Major Classes of Chemical Reactions 4-1

Chapter 4. The Major Classes of Chemical Reactions 4-1 Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions

More information

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because

More information

UNIT 12: Solutions Lesson 3: Table F Solubility Guidelines

UNIT 12: Solutions Lesson 3: Table F Solubility Guidelines Name: Period: Date: General Chemistry KIPP NYC College Prep UNIT 12: Solutions Lesson 3: Table F Solubility Guidelines By the end of today, you will have an answer to: How do we determine if a substance

More information

Chapter 5. Naming Compounds Writing Formulas

Chapter 5. Naming Compounds Writing Formulas Chapter 5 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell

More information

Review 7: Solubility Equilibria

Review 7: Solubility Equilibria Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both

More information

TOPIC 6. CHEMICAL REACTIONS AND IONIC EQUATIONS.

TOPIC 6. CHEMICAL REACTIONS AND IONIC EQUATIONS. TOPIC 6. CHEMICAL REACTIONS AND IONIC EQUATIONS. Reactions involving ionic compounds. As discussed earlier, ionically bonded compounds consist of large aggregations of cations and anions which pack together

More information

Solubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization

Solubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization Chem 30S Review Solubility Rules Solubility Equilibria Salts are generally more soluble in HOT water(gases are more soluble in COLD water) Alkali Metal salts are very soluble in water. NaCl, KOH, Li 3

More information

TOPIC 6. CHEMICAL REACTIONS AND IONIC EQUATIONS.

TOPIC 6. CHEMICAL REACTIONS AND IONIC EQUATIONS. TOPIC 6. CHEMICAL REACTIONS AND IONIC EQUATIONS. Reactions involving ionic compounds. As discussed earlier, ionically bonded compounds consist of large aggregations of cations and anions which pack together

More information

AP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry

AP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance

More information

SOLUBILITY REVIEW QUESTIONS

SOLUBILITY REVIEW QUESTIONS Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver

More information

SCH 3UI Unit 5 Outline Chemical Reactions Homework Questions and Assignments complete handouts: Balancing Equations #1, #2, #3, #4

SCH 3UI Unit 5 Outline Chemical Reactions Homework Questions and Assignments complete handouts: Balancing Equations #1, #2, #3, #4 Lesson Topics Covered 1 Note: Chemical Reactions and Chemical Equations definition of chemical reaction four signs of chemical change the Law of Conservation of Mass balancing chemical equations SCH 3UI

More information

Name of Anion. (aq) NaCl NaNO 3 NaOH Na 2 SO 4 Na2CO3. MgSO4. AgNO 3. Ba(NO 3 ) 2. Pb(NO 3 ) 2. CuSO (1) AgNO 3 ( ) + NaCl( )

Name of Anion. (aq) NaCl NaNO 3 NaOH Na 2 SO 4 Na2CO3. MgSO4. AgNO 3. Ba(NO 3 ) 2. Pb(NO 3 ) 2. CuSO (1) AgNO 3 ( ) + NaCl( ) Name of Compound Prelab #1 Formula Cation (Metal) Name of Cation silver nitrate Ag Ag + silver magnesium sulfate barium nitrate lead nitrate copper sulfate Cation = (+)positive ion Anion = ()negative ion

More information

Reactions in Aqueous Solutions Chang & Goldsby modified by Dr. Hahn

Reactions in Aqueous Solutions Chang & Goldsby modified by Dr. Hahn Reactions in Aqueous Solutions Chang & Goldsby modified by Dr. Hahn Chapter 4 Copyright McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of

More information

Chapter 4 Chemical Formulas, Reactions, Redox and Solutions

Chapter 4 Chemical Formulas, Reactions, Redox and Solutions Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution

More information

The Copper Cycle. HCl(aq) H + (aq) + Cl (aq) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq)

The Copper Cycle. HCl(aq) H + (aq) + Cl (aq) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq) The Copper Cycle Introduction Many aspects of our lives involve chemical reactions from the batteries that power our cars and cell phones to the thousands of processes occurring within our bodies. We cannot

More information

ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13

ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13 ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)

More information

Unit Learning Targets (L.T.):

Unit Learning Targets (L.T.): Unit 9: Chemical Equations and Reactions Chapters 8 and 19 Name Block Unit Learning Targets (L.T.): By the end of the unit, students will be able to: Chapter 8: 1. Correctly write and balance chemical

More information

Types of Reactions: Reactions

Types of Reactions: Reactions 1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous

More information

Chemical Bonding. Comparison of Properties Ionic Compounds Covalent Compounds Metals

Chemical Bonding. Comparison of Properties Ionic Compounds Covalent Compounds Metals Chemical Bonding Comparison of Properties Ionic Compounds Covalent Compounds Metals Essential Questions Why/How do atoms combine with one another to form the vast array of chemical substances that exist?

More information

CHEMISTRY - CLUTCH CH.4 - CHEMICAL QUANTITIES & AQUEOUS REACTIONS

CHEMISTRY - CLUTCH CH.4 - CHEMICAL QUANTITIES & AQUEOUS REACTIONS !! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute

More information

Chapter 4 Reactions in Aqueous Solution

Chapter 4 Reactions in Aqueous Solution Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances

More information

Experiment 8 - Double Displacement Reactions

Experiment 8 - Double Displacement Reactions Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

CHEMISTRY - ZUMDAHL 2E CH.6 - TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY

CHEMISTRY - ZUMDAHL 2E CH.6 - TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY !! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute

More information

Unit 1 - Foundations of Chemistry

Unit 1 - Foundations of Chemistry Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its

More information

UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)

UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.

More information

AP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry

AP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,

More information

Chapter 3 Chemical Reactions

Chapter 3 Chemical Reactions Chapter 3 Chemical Reactions Jeffrey Mack California State University, Sacramento Chemical Reactions Reactants: Zn + I 2 Product: ZnI 2 Chemical Reactions Evidence of a chemical reaction: Gas Evolution

More information

Double Displacement (Exchange or Metathesis) Reactions Practicum

Double Displacement (Exchange or Metathesis) Reactions Practicum Double Displacement (Exchange or Metathesis) Reactions Practicum Part I: Instructions: Write the molecular, complete ionic and net ionic equations for every one of the following reactions. If a reaction

More information

SCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A

SCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute

More information

Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions

Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are two

More information

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement 13. Is the following sentence true or false? Hydrocarbons, compounds of hydrogen and carbon, are often the reactants in combustion reactions. 14. Circle the letter of each compound that can be produced

More information

Funsheet 9.1 [VSEPR] Gu 2015

Funsheet 9.1 [VSEPR] Gu 2015 Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015

More information

D O UBLE DISPL Ac EMENT REACTIONS

D O UBLE DISPL Ac EMENT REACTIONS Experiment 8 Name: D O UBLE DISPL Ac EMENT REACTIONS In this experiment, you will observe double displacement reactions and write the corresponding balanced chemical equation and ionic equations. Double

More information

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. Atomic mass

More information

Law of conservation of mass: Chemical reaction: conversion of substances into different substances (by rearranging atoms) H 2 + O 2 H 2 O

Law of conservation of mass: Chemical reaction: conversion of substances into different substances (by rearranging atoms) H 2 + O 2 H 2 O Chapter 7: Chemical Reactions Chemical reaction: conversion of substances into different substances (by rearranging atoms) Reactants: substances present before reaction Products: substances present after

More information

Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary

Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)

More information

NAMING IONIC COMPOUNDS

NAMING IONIC COMPOUNDS NAMING IONIC COMPOUNDS There are a few general rules that apply when naming ionic compounds. 1. Most ionic compounds are also called salts. 2. Most ionic compounds exist as solids and many dissolve to

More information

Types of Chemical Reactions

Types of Chemical Reactions Types of Chemical Reactions 1) Combination (Synthesis) Reaction 2) Decomposition 3) Single Replacement 4) Double Replacement 5) Combustion 6) Oxidation-Reduction (Redox) Combination (Synthesis) Reactions

More information

DOUBLE DISPLACEMENT REACTIONS. Double your pleasure, double your fun

DOUBLE DISPLACEMENT REACTIONS. Double your pleasure, double your fun DOUBLE DISPLACEMENT REACTIONS Double your pleasure, double your fun Industrial processes produce unwanted by-products. Dissolved toxic metal ions-copper, mercury, and cadmium-are common leftovers in the

More information

H H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent.

H H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent. Role of Water Role of Water Chemical Reactions in Aqueous Solution Role of H 2 O(l) as solvent The polar nature of water molecule Two key features: 1. The distribution of bonding electrons O H covalent

More information

5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3

5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3 Chemistry 11 Solution Chemistry II Name: Date: Block: 1. Ions in Solutions 2. Solubility Table 3. Separating Ions Ions in Solutions Ionization Equation - Represents the salt breaking apart into ions. Practice:

More information

AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:

AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: Water as a solvent Strong and Weak Electrolytes Solution Concentrations How to Make up a solution Types of Reactions Introduction

More information

BIG IDEA TWO. October 13, 2016

BIG IDEA TWO. October 13, 2016 BIG IDEA TWO October 13, 2016 Topics to Cover in Big Idea 2 1. Ionic, metallic, and covalent bonds 2. Polarity and dipole moment 3. Intermolecular forces (IMF): 4. Lewis dot structures 5. Resonance forms

More information

26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O

26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +

More information

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong

More information

2. The reaction of carbon monoxide and diiodine pentoxide as represented by the equation

2. The reaction of carbon monoxide and diiodine pentoxide as represented by the equation 1. The complete combustion of phenylhydrazine, C 6 H 5 NHNH 2, with the oxidizer dinitrogen tetraoxide is shown in the equation C 6 H 5 NHNH 2 + N 2 O 4 CO 2 + H 2 O + N 2 When balanced, the sum of all

More information

Chemical Reactions and Equations

Chemical Reactions and Equations Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new

More information

Net Ionic Equations. Making Sense of Chemical Reactions

Net Ionic Equations. Making Sense of Chemical Reactions Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are

More information

NCEA Chemistry 2.2 Identify Ions AS 91162

NCEA Chemistry 2.2 Identify Ions AS 91162 NCEA Chemistry 2.2 Identify Ions AS 91162 What is this NCEA Achievement Standard? When a student achieves a standard, they gain a number of credits. Students must achieve a certain number of credits to

More information

Unit 3: Solubility Equilibrium

Unit 3: Solubility Equilibrium Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM

More information

Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)

Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility

More information

AP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section

AP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction

More information

You have mastered this topic when you can: CHEMICAL REACTIONS AND THE KINETIC MOLECULAR THEORY AQUEOUS SOLUTIONS

You have mastered this topic when you can: CHEMICAL REACTIONS AND THE KINETIC MOLECULAR THEORY AQUEOUS SOLUTIONS CH 11 TOPIC 32 CLASSIFYING CHEMICAL REACTIONS PART 2 1 You have mastered this topic when you can: 1) define or describe these terms: aqueous solution, solvent, solute, solubility, soluble, low solubility,

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Chapter 4 Reactions in Aqueous Solutions Some typical kinds of chemical reactions: 1. Precipitation reactions: the formation of a salt of lower solubility causes the precipitation to occur. precipr 2.

More information

CHEMICAL REACTIONS. Introduction. Chemical Equations

CHEMICAL REACTIONS. Introduction. Chemical Equations CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions

More information

A reaction in which a solid forms is called a precipitation reaction. Solid = precipitate

A reaction in which a solid forms is called a precipitation reaction. Solid = precipitate Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons

More information

Chap. 4 AQUEOUS RXNS. O H δ+ 4.1 WATER AS A SOLVENT 4.2 AQUEOUS IONIC REACTIONS. Page 4-1. NaOH(aq) + HCl(g) NaCl(aq) +H 2 O

Chap. 4 AQUEOUS RXNS. O H δ+ 4.1 WATER AS A SOLVENT 4.2 AQUEOUS IONIC REACTIONS. Page 4-1. NaOH(aq) + HCl(g) NaCl(aq) +H 2 O Chap. AQUEOUS RXNS.1 WATER AS A SOLVENT Describe solution composition in terms of molarity Describe strong and weak electrolyte solutions, including acids and bases Use ionic equations to describe neutralization

More information

WRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included.

WRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. WRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,

More information

CHM152LL Solution Chemistry Worksheet

CHM152LL Solution Chemistry Worksheet Name: Section: CHM152LL Solution Chemistry Worksheet Many chemical reactions occur in solution. Solids are often dissolved in a solvent and mixed to produce a chemical reaction that would not occur if

More information

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most

More information

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3? 1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K

More information

Cations have a positive charge and anions have a negative charge. 3. Complete the following table.

Cations have a positive charge and anions have a negative charge. 3. Complete the following table. Name Pre-AP Chemistry: Ionic Bonding and Nomenclature Period Homework #1: Ionic Bonding 1. Use Lewis Dot Diagrams to predict the ionic compound formed between each of the following atoms. Use arrows to

More information

7.01 Chemical Reactions

7.01 Chemical Reactions 7.01 Chemical Reactions The Law of Conservation of Mass Dr. Fred Omega Garces Chemistry 100 Miramar College 1 Chemical Reactions Making Substances Chemical Reactions; the heart of chemistry is the chemical

More information