Download Balancing Chemical Equations Bkt p

p. 3 Balancing Chemical Equations –Coefficients:
Numbers in front of each chemical formula
1) 1, 3, 2
2) 2, 2, 3
3) 2, 1, 2, 1
4) 2, 1, 2
5) 2, 1, 2, 1 6) 2, 3, 6, 1
7) 1, 2, 1, 2 8) 1, 5, 3, 4 9) 2, 25, 16, 18
10) 1, 3, 1, 3 11) 4, 5, 2
12) 2, 2, 2, 1
13) 2, 4, 1
14) 1, 12, 8 15) 6, 6, 1, 6
16) 2, 1, 2, 1 17) 2, 1, 1, 1, 1
Notes of Chemical Reactions’ Abbreviations Nov 18th, 2014
Hof Brincl: diatomic molecules/in pairs also gaseous (g)
H2, O2, F2, Br2, I2, N2, Cl2
aqueous: dissolved in water, in solution (aq)
liquid: pure covalent compound Ex: H2O(l)
**pure metallic element: uncharged and solid Ex: Cu(s)
CuSO4 : ionic and Cu2+ (aq) (charged)
pure copper sprinkles: Cu (s) (uncharged)
p. 4 Word Equations: Watch for Hof Brincl!!
1) Zn + Pb(NO3)2  Zn(NO3)2 + Pb
2) 2AlBr3 + 3Cl2  2AlCl3 + 3Br2
3) 2Na3PO4 + 3CaCl2  6NaCl + Ca3(PO4)2
4) 2KClO3  2KCl + 3O2
5) 2Al + 6HCl  2AlCl3 + 3H2
6) 3Ca(OH)2 + 2H3PO4  Ca3(PO4)2 + 6H2O
7) Cu + 2H2SO4  CuSO4 + 2H2O + SO2
8) 2H2 + 2NO  2H2O + N2
p. 5 Word Equations (Hof Brincl)
1) 2AlBr3 + 3Cl2  2AlCl3 + 3Br2
2) 2H2 + O2  2H2O
3) N2 + 3H2  2NH3
4) HCl + NaF  NaCl + HF
5) Fe + PbS  FeS + Pb
6) H2SO4  SO3 + H2O
7) 2Na2O + 2F2  4NaF + O2
8) 2KI + Br2  2KBr + I2
9) 3Zn + 2FeCl3  3ZnCl2 + 2Fe
10) 4Al + 3O2  2Al2O3
11) 2N2 + 5O2  2N2O5
p.6 More Word Equations (Include the states: s, l, aq, g)
1) 2O2(g) + N2(g)  2NO2(g)
2) 2BeI2(aq) + Sn(NO3)4(aq)  2Be(NO3)2(aq) + SnI4(s)
3) 2Fe(s) + 3F2(g)  2FeF3(s)
4) 2HCl(aq) + Mg(OH)2(aq)  MgCl2(aq) + 2H2O(l)
5) 2(NH4)3N(aq) + 3Pb(ClO3)2(aq) 6NH4ClO3(aq) + Pb3N2(s)
6) H2CO3(aq)  CO2(g) + H2O(l)
7) 2Na3PO4(aq) + 3CuSO4(aq)  3Na2SO4(aq) + Cu3(PO4)2(s)
8) H2O(l) + CO(g)  H2(g) + CO2(g)
p.7 Concept Attainment-Classifying Chemical Rxns
Examples of synthesis:
b, c use a highlighter
Synthesis:
2 compounds combining to form a larger substance.
p.8
Examples of single replacement: a, d use a highlighter
Single replacement:
One element replaces another element in a compound.
Examples of decomposition:
b, e use a highlighter
Decomposition:
Large substance is breaking down into smaller compounds.
Examples of double replacement: c, d use a highlighter
Double replacement:
An ion of a compound is switched with another metal or non metal
to form another compound.
p.9 Examples of combustion: a, d, e
use a highlighter
Combustion: Reaction with oxygen as a reactant.
Examples of neutralization: a, d use a highlighter
Neutralization: An acid(H-) is reacting with a base(-OH) to
produce a salt(cation + anion) and water.
p. 10 Classification of Chemical Reactions
1) synthesis
2) decomposition
3) single replacement
4) synthesis, combustion
5) decomposition
6) single replacement
7) synthesis
8) double replacement
9) decomposition
10)neutralization(special type of DR)
p.11 Classifying Reactions Practice
1) combustion
2) single replacement
3) double replacement
4) decomposition
5) synthesis
6) single replacement
7) neutralization (DR)
9) decomposition
11) single replacement
13) single replacement
15) neutralization (DR)
8) synthesis, combustion
10) combustion
12) decomposition
14) single replacement
**T** p.12 Predicting Products of Chemical Reactions
1) MgBr2 + Cl2  MgCl2 + Br2
single replacement
2) 2Al + Fe2O3 2Fe + Al2O3
single replacement
3) 2AgNO3 + ZnCl2  2AgCl + Zn(NO3)2 double replacement
MnO2 (catalyst)
4) 2H2O2 ---
2H2O + O2
decomposition
elephant toothpaste demo
5) Zn + 2HCl ZnCl2 + H 2
single replacement
6) H2SO4 + 2NaOH  Na2SO4 + 2H2O
neutralization
7) 2Na + H2 2NaH
synthesis
8) 2CH3COOH + Cu  NR
s(no reaction)
**T** p. 13 Balancing Equations and Classifying Rxns
All the rxns below are single replacement rxns
i) Zn + MgSO4  NR
(Zn is below Mg)
ii) 2Al(s) + Fe2O3(aq)  Al2O3(aq) + 2Fe(s) (Al is above Fe)
iii) Pb + KNO3 NR (Pb is below K)
iv) Ni + FeSO4 NR
(Ni is below Fe)
v) Zn(s) + CuCl2(aq)  ZnCl2(aq) + Cu(s) (Zn is above Cu)
vi) F2(g) + 2KCl(aq)  2KF(aq) + Cl2(g)
(F2 is above Cl2)
vii) I2 + FeBr3 NR
(I2 is below Br2)
viii) 3Zn(s) + 2H3PO4(aq)  Zn3(PO4)2(aq) + 3H2(g)
(Zn is above H2)