Chemistry NYA Answers Part 3

8/10/2019 Chemistry NYA Answers Part 3

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3.1.1 Exercises:1. Write the electron configuration of the following ions. Are they stable ions?

They are isoelectronic with which neutral element?

Ion Electron Configuration Stable Ion: Y/N Isoelectronic with:

N2- 1s2 2s2 2p5 no fluorine

Mg+ 1s2 2s2 2p63s1 no sodium

O2- 1s2 2s2 2p6 yes neon

P3- 1s2 2s2 2p63s23p6 yes argon

He+ 1s1 no hydrogen

H- 1s2 yes helium

Ca2+ 1s2 2s2 2p63s23p6 yes argon

K+ 1s2 2s2 2p63s23p6 yes argon


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3.2.2 Exercises:

1. Arrange the following groups of atoms in order of their increasing atomic radius (withoutlooking at the chart above):

a) Cl, Na, Al, Mg Cl < Al< Mg < Na

b) I, F, Br, At F < Br < I < At

c) K, Rb, F, B, Be F < B < Be < K < Rb

d) P, Si, N N < S < P

3.2.3 Exercises:

1. Arrange the following isoelectronic ions according to their increasing size: Cl-, K+, S2-, P3-, Ca2+

and explain the arrangement by using the total # of electrons and atomic # in your explanation.

Ca2+ < K+ < Cl- < S2- < P3-

While these are isoelectronic, they have different atomic numbers (Z).

As the # of protons increases, the attraction for electron increases & the radius decreases.


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3.5.1 Exercises:1. Consider the following elements: N, B, Be, K and Fa) Arrange in the above elements in order of increasing atomic radius F < N < B < Be < Kb) Arrange the above elements in order of increasing ionization energy K < B < Be < N < Fc) Arrange the above elements in order of increasing electronegativity K < Be < B < N < F

d) Explain your order in 1b) and 1c).As we move from left to right in a period, the effective nuclear charge increases, which results in thevalence electrons being more strongly attracted by the nucleus (and the radius decreases), so that itrequires more energy to remove these electrons. In a similar manner (from left to right), weunderstand that since the effective nuclear charge increases, the atom has a greater tendency to attractelectrons .

2. Consider the following elements: Ca, F, S, Cl and Pa) Arrange in the above elements in order of increasing atomic radius F < Cl < S < P < Cab) Arrange the above elements in order of increasing ionization energy Ca < S < P < Cl < Fc) Arrange the above elements in order of increasing electronegativity Ca < P < S < Cl < Fd) Explain your order in 2b) and 2c).The answer is similar than above except that in (2) we need to take into account the fact that some of

the elements are from different periods: electronegativity tends to increase from left to right in a period and decrease from top to bottom in agroup.

3. Consider the following ions: N3-, Na+, Mg2+, F- and O2-.Arrange the above ions in order of increasing ionic radius & explain.

Mg2+ < Na+ < F- < O2- < N3-

1st: in a similar period, cations will have a smaller radius than anions (as already explained).


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3.5.1 Exercises:4. Consider the following ions: Si4-, Cl- and Ca2+.Arrange the above ions in order of increasing ionic radius & explain.

Ca2+ < Cl- < Si4-

Cl- and Si4- are of the same 3rd period, and Si4-will have the largest radius as it bears a charge of 4-.

The cation Ca2+ is of the 4th period but has no electrons in that level, and has a charge of +2 and so itwill have the smallest radius.

5. Which has the larger radius: Si2+ or Si4+? Explain.Si2+ has the larger radius since it only has a charge of 2+, and thus has 2 electrons in its 2nd shell (n=2).Si4+ is missing a total of 4 electrons and therefore has no electrons at all in its 2nd shell (the radius isthus smaller).Also, in the case of Si4+ over Si2+, since there are less electrons around the nucleus of the atom, there isless repulsion between the electrons and the electron cloud is smaller, and the attraction by thenucleus for the electrons is greater, therefore also decreasing the radius of the atom.

6. Which has the larger radius: F- or Br-? Explain.Br- has the largest radius as it is in the 4th period (F- is in the 2nd period).

7. Which has the larger radius: Na+ or Mg2+? Explain.Na+ has the largest radius as it only bears a charge of 1+ versus Mg (of the same period) that bears acharge of 2+. The effective nuclear charge for Mg2+ is greater than Na+, hence the attraction for theelectrons is greater for Mg2+ than for Na+.

8. Which has the larger radius: Fe2+ or Fe3+? Explain.

Fe2+ has the largest radius as the effective nuclear charge for Fe3+ is greater than Fe2+, hence theattraction for the electrons is greater for Fe3+ than for Fe2+.


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9. Match each of the following elements with its ionization energy.Explain your choice and explain any irregularities to the general trend:Elements: Li; Be; B; C; N; O; F; Ne:Ionization Energy Values (kJ|mol): 2080; 1681; 1402; 1314; 1086; 900; 800; 560.

Li 560Be 900B 800C 1086N 1402O 1314F 1681

Ne 2080

10. Explain why the 2nd ionization energy of Rb is much greater than the 2nd ionization energy of Sr.The 2nd ionization energy of Sr involves the removal of a valence electron while the 2nd ionizationenergy of Rb involves the removal of a core electron and so requires much more energy.

11. The values for the 1st

, 2nd

, 3rd

ionization energies of an unknown element are found to be asfollows: Ionization Energy: 1st 2nd 3rd

kJ/mol: 897 1782 14820

In which A group of the periodic table would you expect to find this elements? Explain your answer.In the 2nd group as the difference between the 2nd & 3rd ionization is drastically different (thissuggests that there are 2 valence electrons).

3.5.1 Exercises:


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3.6.1 Exercises:

1. Classify the following species as having ionic, polar covalent & non-polar covalent bonds.a) SrS electronegativity = 2.58 0.95 = 1.63 covalent polar

b) K2O electronegativity = 3.44 0.82 = 2.62 ionic

c) HCl electronegativity = 3.16

2.20 = 0.96 covalent polard) H2 electronegativity = 2.20 2.20 = 0 covalent non-polar

e) HBr electronegativity = 2.96 2.20 = 0.76 covalent polar

f) NaCl electronegativity = 3.16 0.93 = 2.23 ionic

g) F2 electronegativity = 3.98 3.98 = 0 covalent non-polar

h) Cl2 electronegativity = 3.16

3.16 = 0 covalent non-polar

i) HF electronegativity = 3.98 2.20 = 1.78 covalent polar

j) H2O electronegativity = 3.44 2.20 = 1.24 covalent polar

k) NCl3 electronegativity = 3.16 3.04 = 0.12 covalent non-polar

l) PH3 electronegativity = 2.20 2.19 = 0.01 covalent non-polar

m) KH electronegativity = 2.20 0.82 = 1.38 covalent polar

n) NH3 electronegativity = 3.04 2.20 = 0.84 covalent polar

o) BaO electronegativity = 3.44 0.89 = 2.55 ionic

p) CO2 electronegativity = 3.44 2.55 = 0.89 covalent polar

q) CsF electronegativity = 3.98 0.79 = 3.19 ionic

r) CH4 electronegativity = 2.55 2.20 = 0.35 covalent polar/non polar


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3.8.1 Exercises:

1. Write the CME, CIE and NIE for the following reaction: Cl2 (g) + NaBr (aq)

Step 1: Is there a reaction? yesStep 2: What are the molecular products? Br2 (NaCl is an ionic product)

Step 3: Balance the equation Cl2 (g) + 2 NaBr (aq)

Br2 (g) + 2 NaCl (aq)Step 4: Complete the CIE Cl2 (g) + 2 Na+ (aq) + 2 Br- (aq) Br2 (aq) + 2 Na

+ (aq) + 2 Cl- (aq)Step 5: Complete the NIE Cl2 (g) + 2 Br

- (aq) 2 Cl- (aq) + Br2 (l)

2. Complete the following:

a) Br2 (l) + 2 NaI (aq) 2 NaBr (s) + I2 (s)

CIE Br2 (l) + 2 Na+

(aq) + 2 I-

(aq)

2 Na+

(aq) + 2 Br-

(aq) + I2 (s)NIE Br2 (l) + 2 I- (aq) 2 Br- (aq) + I2 (s)

b) Cl2 (g) + 2 KI (aq) 2 NaCl (s) + I2 (s)CIE Cl2 (g) + 2 K

+ (aq) + 2 I- (aq) 2 Na+ (aq) + 2 Cl- (aq) + I2 (s)NIE Cl2 (g) + 2 I

- (aq) 2 Na+ (aq) + I2 (s)


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c) Cl2 (g) + NaF (aq)No reactionCIENIE

d) I2 (s) + NaCl (aq)No reactionCIENIE

e) F2 (g) + 2 NaBr (aq) Br2 (l) + 2 NaF (aq)CIE F2 (g) + 2 Na

+ (aq) + 2 Br- (aq) Br2 (l) + 2 Na+ (aq) + 2 F- (aq)

NIE F2 (g) + 2 Br-

(aq) Br2 (l) + 2 F-

(aq)

f) Br2 (l) + NaF (aq) No reactionCIENIE

g) F2 (g) + 2 NaCl (aq) Cl2 (g) + 2 NaF (aq)

CIE F2 (g) + 2 Na+ (aq) + 2 Cl- (aq) Cl2 (g) + 2 Na+ (aq) + 2 F- (aq)NIE F2 (g) + 2 Cl

- (aq) Cl2 (g) + 2 F- (aq)

3.8.1 Exercises:


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3.8.1 Exercises:1. Write the CME, CIE and NIE for the following reaction 2 Na (s) + 2HCl (aq) 2 NaCl (aq) + H2 (g)Step 1: Is there a reaction? yesStep 2: What are the molecular products? H2 (NaCl is the ionic product)Step 3: What is the solubility of the new product AC? NaCl is soluble

Step 4: What is the state of pure B? H2 is a gasStep 3: Balance the equation see aboveStep 4: Complete the CIE: 2 Na (s) + 2 H+ (aq) + 2 Cl- (aq) 2 Na+ (aq) + 2 Cl- (aq) + H2 (g)Step 5: Complete the NIE: 2 Na (s) + 2 H+ (aq) 2 Na+ (aq) + H2 (g)


a) Ca(s) + H2SO4 (aq)

H2 (g) + CaSO4 (s)CIE Ca(s) + 2H+ (aq) + SO42- (aq)H2 (g) + CaSO4 (s)

NIE Ca(s) + 2H+ (aq) + SO42- (aq)H2 (g) + CaSO4 (s)

b) Cu (s) + 2 AgNO3 (aq) Cu(NO3)2 (aq) + 2 Ag (s)CIE Cu (s) + 2 Ag+ (aq) + 2 NO3

-(aq) Cu2+ (aq) + 2 NO3-(aq) + 2 Ag (s)

NIE Cu (s) + 2 Ag+ (aq) Cu2+ (aq) + 2 Ag (s)

c) Zn (s) + Cu(NO3)2 (aq) Cu (s) + Zn(NO3)2CIE Zn (s) + Cu2+ (aq) + 2 NO3 (aq) Cu (s) + Zn

2+ (aq) + 2 NO3-(aq)

NIE Zn (s) + Cu2+ (aq) Cu (s) + Zn2+ (aq)

d) Mg (s) + Ni(NO3)2 (aq) Ni (s) + Mg(NO3)2 (aq)CIE Mg (s) + Ni2+ (aq) + 2 NO3 (aq)Ni (s) + Mg

2+ (aq) + 2 NO3 (aq)NIE Mg (s) + Ni2+ (aq) Ni (s) + Mg2+ (aq)


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e) Pb (s) + Ca(NO3)2 (aq) No reaction.CIENIE

f) Al (s) + 3 AgNO3 (aq) 3 Ag (s) + Al(NO3)3 (aq)CIE Al (s) + 3 Ag+ (aq) + 3 NO3 (aq) 3 Ag (s) + Al

3+ (aq) + 3 NO3 (aq)

NIE Al (s) + 3 Ag+ (aq) 3 Ag (s) + Al3+ (aq)

g) Zn(s) + BaCl2 (aq) No reaction.CIENIE

h) Zn(s) + Ni(NO3)2 (aq) Ni (s) + Zn(NO3)2 (aq)CIE Zn(s) + Ni2+ (aq) + 2 NO3 (aq) Ni (s) + Zn

2+ (aq) + 2 NO3 (aq)

NIE Zn(s) + Ni2+

(aq)

Ni (s) + Zn2+

(aq)i) Ag(s) + Cu(NO3)2 (aq) No reaction.CIENIE

j) H2 (g) + 2 AgNO3 (aq) 2 Ag (s) + 2 HNO3 (aq)CIE H2 (g) + 2 Ag

+ (aq) + 2 NO3-(aq) 2 Ag (s) + 2 H+ (aq) + 2 NO3

- (aq)NIE H2 (g) + 2 Ag

+ (aq) 2 Ag (s) + 2 H+ (aq)

k) H2 (g) + Cu(NO3)2 (aq) Cu (s) + 2 HNO3 (aq)CIE H2 (g) + Cu

2+ (aq) + 2 NO3 (aq) Cu (s) + 2 H+ (aq) + 2 NO3

-(aq)NIE H2 (g) + Cu

2+ (aq) Cu (s) + 2 H+ (aq)

l) H2 (g) + KCl (aq) No reaction.CIENIE

3.8.1 Exercises:


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3.8.2 Exercises:

1. Write the CME, CIE & NIE for the following reaction: NaCl (aq) + AgNO3 (aq)AgCl (s) + NaNO3 (aq)Step 1: What are the molecular products? AgCl & NaNO3Step 2: What is the state of these products? (s) (aq)Step 3: Is there a reaction? Yes

Step 3: Balance the equation: NaCl (aq) + AgNO3 (aq) AgCl (s) + NaNO3 (aq)Step 4: Complete the CIE: Na+(aq) + Cl-(aq) + Ag+(aq) + NO3

-(aq)AgCl(s) + Na+(aq) + NO3-(aq)

Step 5: Complete the NIE: Cl-(aq) + Ag+(aq)AgCl(s)


a) NaCl (aq) + AgNO3 (aq) AgCl (s) + NaNO3 (aq)CIE Na+(aq) + Cl-(aq) + Ag+(aq) + NO3

-(aq)AgCl(s) + Na+(aq) + NO3-(aq)

NIE Cl-(aq) + Ag+(aq)AgCl(s)

b) LiCl (aq) + H3PO4 (aq) No reaction


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c) 3 Mg(ClO3)2 (aq) + 2 (NH4)3PO4 (aq) Mg3(PO4)2 (s) + 6 NH4ClO3 (aq)CIE 3 Mg2+(aq) + 6 ClO3

-(aq) + 6 NH4+(aq) + 2 PO4

3-(aq)Mg3(PO4)2 (s) + 6 NH4+(aq) + 6 ClO3

-(aq)NIE 3 Mg2+(aq) + 2 PO4

3-(aq)Mg3(PO4)2 (s)

d) Al2(SO4)3 (aq) + LiBr (aq) no reaction

e) AgF (aq) + Cu(NO3)2 (aq) no reaction

f) Ni(NO3)2 (aq) + Na2CO3 (aq) Ni(CO3)2 (s) + 2 NaNO3 (aq)CIE Ni2+ (aq) + 2 NO3

-(aq) + 2 Na+ (aq) + CO32- (aq)Ni(CO3)2 (s) + 2 Na

+ (aq) + 2 NO3-(aq)

NIE Ni2+ (aq) + CO3

2- (aq) Ni(CO3

)2

(s)

3.8.2 Exercises:


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1. Write the CME, CIE and NIE for the following reaction HCl (aq) + NaOH (aq) CME HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l)CIE H+ (aq) + Cl- (aq) + Na+ (aq) + OH- (aq)Na+ (aq) + Cl- (aq) + H2O (l)NIE H+ (aq) + OH- (aq) H2O (l)

2. Complete the followinga) KOH (aq) + H2SO4 (aq) CME 2 KOH (aq) + H2SO4 (aq) K2SO4 (aq) + H2O (l)CIE 2 K+ (aq) + 2 OH- (aq) + 2H+ (aq) + SO4

2-(aq) 2 K+ (aq) + SO42-(aq) + H2O (l)

NIE 2 OH- (aq) + 2H+ (aq)H2O (l)

b) H2SO3 (aq) + Ba(OH)2 (aq) CME H2SO3 (aq) + Ba(OH)2 (aq) BaSO4 (s) + 2 H2O (l)CIE 2 H+ (aq) + SO3

2-(aq) + Ba2+ (aq) + 2 OH- (aq) BaSO4 (s) + 2 H2O (l)NIE 2 H+ (aq) + SO3

2-(aq) + Ba2+ (aq) + 2 OH- (aq) BaSO4 (s) + 2 H2O (l)

c) H2CO3 (aq) + LiOH (aq)

CME H2CO3 (aq) + 2 LiOH (aq)

Li2CO3 (aq) + 2 H2O (l)CIE 2 H+ (aq) + CO32-(aq) + 2 Li+ (aq) + 2 OH- (aq) 2 Li+ (aq) + CO3

2-(aq) + 2 H2O (l)NIE 2 H+ (aq) + 2 OH- (aq) 2 H2O (l)

d) NaOH (aq) + H3PO4 (aq) CME 3 NaOH (aq) + H3PO4 (aq)Na3PO4 (aq) + 3 H2O (l)CIE 3 Na+ (aq) + 3 OH- (aq) + 3 H+ (aq) + PO4

3-(aq) 3 Na+ (aq) + PO43-(aq) + 3 H2O (l)

NIE 3 OH- (aq) + 3 H+ (aq) 3 H2O (l)

3.8.3 Exercises:


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e) Ba(OH)2 (aq) + H3PO4 (aq) CME 3 Ba(OH)2 (aq) + 2 H3PO4 (aq) Ba3(PO4)2 (s) + 6 H2O (l)CIE 3 Ba2+ (aq) + 6 OH- (aq) + 6 H+ (aq) + 2 PO4

3-(aq) Ba3(PO4)2 (s) + 6 H2O (l)NIE 3 Ba2+ (aq) + 6 OH- (aq) + 6 H+ (aq) + 2 PO4

3-(aq) Ba3(PO4)2 (s) + 6 H2O (l)

f) Fe(OH)2 (s) + H2SO4 (aq) CME Fe(OH)2 (s) + H2SO4 (aq) FeSO4 (s) + H2O (l)CIE Fe(OH)2 (s) + 2 H

+ (aq) + SO42-(aq) FeSO4 (s) + H2O (l)

NIE Fe(OH)2 (s) + 2 H+ (aq) + SO4

2-(aq) FeSO4 (s) + H2O (l)

g) Fe(OH)3 (s) + HCl (aq) CME Fe(OH)3 (s) + 3 HCl (aq) FeCl3 (aq) + 3 H2O (l)CIE Fe(OH)3 (s) + 3 H

+ (aq) + 3 Cl- (aq) Fe3+ (aq) + 3 Cl- (aq) + 3 H2O (l)NIE Fe(OH)3 (s) + 3 H

+ (aq) Fe3+ (aq) + 3 H2O (l)

h) HClO3 (aq) + Ca(OH)2 (s) CME 2 HClO3 (aq) + Ca(OH)2 (s) Ca(ClO3)2 (s) + 2 H2O (l)

CIE 2 H+

(aq) + 2 ClO3-

(aq) + Ca(OH)2 (s)

Ca(ClO3)2 (s) + 2 H2O (l)NIE 2 H+ (aq) + 2 ClO3-(aq) + Ca(OH)2 (s) Ca(ClO3)2 (s) + 2 H2O (l)

i) H2CO3 (aq) + Mg(OH)2 (s) CME H2CO3 (aq) + Mg(OH)2 (s)MgCO3 (s) + 2 H2O (l)CIE 2 H+ (aq) + CO3

2-(aq) + Mg(OH)2 (s)MgCO3 (s) + 2 H2O (l)NIE 2 H+ (aq) + CO3

2-(aq) + Mg(OH)2 (s)MgCO3 (s) + 2 H2O (l)

3.8.3 Exercises:


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3.8.4 Exercises:1. Complete the following:

a) HBr (aq) + Na2CO3 (aq) CME 2 HBr (aq) + Na2CO3 (aq) 2 NaBr (aq) + H2O (l) + CO2 (aq) [H2CO3 (aq) CO2 (g) + H2O (l)]CIE 2 H+ (aq) + 2 Br- (aq) + 2 Na+ (aq) + CO3

2-(aq) 2 Na+ (aq) + 2 Br- (aq) + H2O (l) + CO2 (aq)NIE 2 H+ (aq) + CO

3

2-(aq) H2

O (l) + CO2

(aq)

b) HCl (aq) + NaHCO3 (aq) CME HCl (aq) + NaHCO3 (aq) NaCl (aq) + H2O (l) + CO2 (g)CIE H+ (aq) + Cl- (aq) + Na+ (aq) + HCO3

-(aq) Na+ (aq) + Cl- (aq) + H2O (l) + CO2 (g)NIE H+ (aq) + HCO3

-(aq) H2O (l) + CO2 (g) [H2CO3 (aq) CO2 (g) + H2O (l)]

c) HNO3 (aq) + CaCO3 (s)

CME 2 HNO3 (aq) + CaCO3 (s) Ca(NO3)2 (aq) + H2O (l) + CO2 (g)CIE 2 H+ (aq) + 2 NO3

-(aq) + CaCO3 (s) Ca2+ (aq) + 2 NO3

-(aq) + H2O (l) + CO2 (g)NIE 2 H+ (aq) + CaCO3 (s) Ca

2+ (aq) + H2O (l) + CO2 (g)

1. Complete the following

a) HNO3 (aq) + NaC2H3O2 (aq) CME HNO3 (aq) + NaC2H3O2 (aq) HC2H3O2 (aq) + NaNO3 (aq)CIE H+ (aq) + NO3

-(aq) + Na+ (aq) + C2H3O2- (aq) HC2H3O2 (aq) + Na

+ (aq) + NO3- (aq)

NIE H+ (aq) + C2H3O2- (aq) HC2H3O2 (aq)

b) HCl (aq) + Ca(C2H3O2)2 (aq) CME 2 HCl (aq) + Ca(C2H3O2)2 (aq) CaCl2 (aq) + 2 HC2H3O2 (aq)

CIE 2 H+

(aq) + 2 Cl-

(aq) + Ca2+

(aq) + 2 C2H3O2-

(aq)

Ca2+

(aq) + 2 Cl-

(aq) + 2 HC2H3O2 (aq)NIE 2 H+(aq) + 2 C2H3O2-(aq) 2 HC2H3O2 (aq)

3.8.5 Exercises:

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a) KOH (aq) + NH4Cl (aq) CME KOH (aq) + NH4Cl (aq) NH3 (g) + KCl (aq) + H2O (l)

CIE K+

(aq) + OH-

(aq) + NH4+

(aq) + Cl-

(aq)

NH3 (g) + K+

(aq) + Cl-

(aq) + H2O (l)NIE OH- (aq) + NH4+ (aq) NH3 (g) + H2O (l)

b) Ca(OH)2 (aq) + NH4Br (aq) CME Ca(OH)2 (aq) + 2 NH4Br (aq) CaBr2 (aq) + 2 NH3 (g) + 2 H2O (l)CIE Ca2+ (aq) + 2 OH- (aq) + 2 NH4

+ (aq) + 2 Br- (aq) Ca2+ (aq) + 2 Br -(aq) + 2 NH3 (g) + 2 H2O (l)NIE 2 OH- (aq) + 2 NH4

+ (aq) 2 NH3 (g) + 2 H2O (l)

3.8.6 Exercises:

3.9.1 Exercises:1. Complete the following:

a) Al(OH)3 (s) + HCl (aq)

CME Al(OH)3 (s) + 3 HCl (aq) AlCl3 (aq) + 3 H2O (l)CIE Al(OH)3 (s) + 3 H

+ (aq) + 3 Cl- (aq) Al3+ (aq) + 3 Cl- (aq) + 3 H2O (l)NIE Al(OH)3 (s) + 3 H

+ (aq)Al3+ (aq) + 3 H2O (l)

b) Al(OH)3 (s) + NaOH (aq) NaAl(OH)4 (aq) (sodium aluminate)CME Al(OH)3 (s) + NaOH (aq) NaAl(OH)4 (aq)

CIE Al(OH)3 (s) + Na+

(aq) + OH-

(aq)

Na+

(aq) + Al(OH)4-

(aq)NIE Al(OH)3 (s) + OH- (aq) Al(OH)4

-(aq)

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End of unit exercises:1. Complete and balance the following equation and classify as: combination (C), decomposition (D),burning of organic compound (B), single replacement (SR) or double replacement (DR).

a) H2SO4 (aq) + 2 KOH (aq) K2SO4 (aq) + H2O (aq) DRb) 2 H3PO4 (aq) + 3 Mg(OH)2 (s) Mg3(PO4)2 (aq) + H2O (l) DR

c) CaCl2 (aq) + Na2CO3 (aq) CaCO3 (s) + 2 NaCl (aq) DRd) HCl (aq) + KHCO3 (aq) KCl (aq) + H2O (l) + CO2 (g) DRe) S8 (s) + 8 O2 (g) 8 SO2 (g) Cf) Si (s) + O2 (g) SiO2 (s) Cg) 2Al (s) + 3/2 O2 (g) Al2O3 (s) Ch) Li2O (s) + H2O (l) 2 LiOH (aq) SRi) CO

2(g) + H

2O (l) H

2CO

3(aq) C

j) Na (s) + H2O (l) NaOH (aq) + H2 (g) Ck) 2 Na (s) + H2 (g) 2 NaH (s) Cl) Ba (s) + Cl2 (g) BaCl2 (s) Cm) H2 (g) + Cl2 (g) 2 HCl (g) Cn) K2CO3 + 2 HCl (aq) 2 KCl + CO2 (g) + H2O (l) DRo) 2AgNO3 (aq) + BaCl2 (aq) 2 AgCl (s) + Ba(NO3)2 (aq) DR

p) (NH4)2CO3 (aq) + 2 HCl (aq) 2 NH4Cl (aq) + H2O (l) + CO2 (g) DRq) Li (s) + O2 (g) Li2O (s) Cr) C2H6 (g) + 7/2 O2 (g) 2 CO2 (g) + 3 H2O (l) Bs) HgO (s) + heat Hg (s) + O2 (g) Dt) CaI2 (aq) + Br2 (l) CaBr2 (aq) + I2 (s) SR

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End of unit exercises:1. Complete and balance the following equation and classify as: combination (C), decomposition (D),burning of organic compound (B), single replacement (SR) or double replacement (DR).

u) BaCl2 (aq) + H2SO4 (aq) BaSO4 (s) + 2 HCl (aq) DRv) NH4NO3 (aq) + NaOH (aq) NaNO3 (aq) + H2O (l) + NH3 (g) DR

w) Ca(CH3CO2)2 (s) + 2 HCl (aq) CaCl2 (aq) + 2 CH3CO2H (aq) DRx) Na2CO3 (aq) + H2SO4 (aq) Na2SO4 (aq) + H2O (l) + CO2 (g) DRy)3 KOH (aq) + H3PO4 (aq) 3 H2O (l) + K3PO4 (aq) DRz) Ba(OH)2 (aq) + H2SO4 (aq) Ba(OH)2 (aq) + H2SO4 (aq) DRaa) Mg (s) + H2SO4 (aq) H2 (g) + MgSO4 (s) SRbb) MgO (s) + H2O (l) + heat Mg(OH)2 (aq) Ccc) NaCl (s) + heat Na (s) + Cl

2(g) D

dd) 2 H3PO4 (aq) + 3 Mg(s) Mg3(PO4)2 (aq) + 3 H2 (g) SRee) N2O5 (s) + 2 H2O (l) 2 HNO3 (aq) Cff) P4O6 (s) + 6 H2O (l) 4 H3PO4 (aq) Cgg) Cl2 (aq) + CaBr2 (aq) Br2 (aq) + CaCl2 (aq) SRhh) Na2O (s) + H2O (l) 2 NaOH (aq) Cii) Al (s) + 3 HCl (aq) AlCl3 (aq) + 3/2 H2 (g) SR

jj) CaCO3 + heat Ca (s) + CO2 (g) D

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2. Write the CME, CIE & NIE for the following reactions (all soluble reactants are in aq. solutions).a) Sulphuric acid with barium hydroxideCME H2SO4 (aq) + Ba(OH)2 BaSO4 (s) + 2 H2O (l)CIE 2 H+ (aq) + SO4

2-(aq) + Ba2+ (aq) + 2 OH (aq) BaSO4 (s) + 2 H2O (l)

NIE 2 H+ (aq) + SO42-(aq) + Ba2+ (aq) + 2 OH

(aq) BaSO4 (s) + 2 H2O (l)

b)Barium chloride & sodium sulfateCME BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2 NaCl (aq)CIE Ba2+ (aq) + 2 Cl-(aq) + 2 Na+ (aq) + SO4

2-(aq) BaSO4 (s) + 2 Na+ (aq) + 2 Cl-(aq)

NIE Ba2+ (aq) + SO42-(aq) BaSO4 (s)

c) Sodium carbonate & nitric acidCME Na2CO3 (aq) + 2 HNO3 (aq) 2 NaNO3 (aq) + CO2 (g) + H2O (l)CIE 2 Na+(aq) + CO3

2-(aq) + 2 H+(aq) + 2 NO3-(aq) 2 Na+(aq) + NO3

-(aq) + CO2(g) + H2O(l)NIE CO3

2-(aq) + 2 H+(aq) CO2(g) + H2O(l)

d) Silver nitrate & ammonium chloride

CME AgNO3 (aq) + NH4Cl (aq)

AgCl (s) + NH4Cl (aq)CIE Ag+ (aq) + NO3- (aq) + NH4

+ (aq) + Cl- (aq)AgCl (s) + NH4+ (aq) + Cl- (aq)

NIE Ag+ (aq) + Cl- (aq)AgCl (s)

e) Ammonium hydroxide & sulphuric acidCME 2 NH4OH (aq) + H2SO4 (aq) (NH4)2SO4 (aq) + 2 H2O (l)CIE 2 NH4

+ (aq) + 2 OH- (aq) + 2 H+ (aq) + SO42-(aq) 2 NH4 (aq) + SO4

2- (aq) + 2 H2O (l)

NIE 2 OH- (aq) + 2 H+ (aq)) 2 H2O (l)

End of unit exercises:

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f) Aluminum hydroxide & perchloric acidCME Al(OH)3 (aq) + 3 HClO4 (aq)Al(ClO4)3 (aq) + 3 H2O (l)CIE Al3+ (aq) + 3 OH-(aq) + 3 H+ (aq) + 3 ClO4

- (aq)Al3+ (aq) + 3 ClO4- (aq) + 3 H2O (l)

NIE 3 OH-(aq) + 3 H+ (aq)3 H2O (l)

g) Potassium carbonate & strontium chlorideCME K2CO3 (aq) + SrCl2 (aq) 2 KCl (aq) + SrCO3 (s)CIE 2 K+ (aq) + CO3

2- (aq) + Sr2+ (aq) + 2 Cl- (aq) 2 K+ (aq) + 2 Cl- (aq) + SrCO3 (s)NIE CO3

2- (aq) + Sr2+ (aq) SrCO3 (s)

h) Aluminum & hydrochloric acidCME Al (s) + 3 HCl (aq)AlCl3 (aq) + 3/2 H2 (g)CIE Al (s) + 3 H+ (aq) + 3 Cl- (aq)Al3+ (aq) + 3 Cl- (aq) + 3/2 H2 (g)NIE Al (s) + 3 H+ (aq)Al3+ (aq) + 3/2 H2 (g)

i) Potassium acetate & sulphuric acidCME 2 KOAc (aq) + H2SO4 (aq) K2SO4 (aq) + 2 HOAc (aq)

CIE 2 K+

(aq) + 2 AcO-

(aq) + 2 H+

(aq) + SO42-

(aq)

2 K+

(aq) + SO42-

(aq) + 2 H+

(aq) + 2 AcO-

(aq)NIE 2 AcO-(aq) + 2 H+(aq) 2 HOAc (aq)

j) Calcium sulfite & sodium hydroxideCME CaSO3 (aq) + 2 NaOH (aq) Ca(OH)2 (s) + Na2SO3 (aq)CIE Ca2+ (aq) + SO3

2- (aq) + 2 Na+ (aq) + 2 OH- (aq) Ca(OH)2 (s) + 2 Na+ (aq) + SO3

2- (aq)NIE Ca2+ (aq) + 2 OH- (aq) Ca(OH)2 (s)


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k) Magnesium metal & sulphuric acidCME Mg (s) + H2SO4 (aq)MgSO4 (aq) + H2 (g)CIE Mg (s) + 2 H+ (aq) + SO4

2- (aq)Mg2+ (aq) + SO42- (aq) + H2 (g)

NIE Mg (s) + 2 H+ (aq)Mg2+ (aq) + H2 (g)

l) Potassium carbonate & hydrochloric acidCME K2CO3 (aq) + 2 HCl (aq) 2 KCl (aq) + H2O (l) + CO2 (g)CIE 2 K+ (aq) + CO3

2- (aq) + 2 H+ (aq) + 2 Cl- (aq) 2 K+ (aq) + 2 Cl- (aq) + H2O (l) + CO2 (g)NIE CO3

2- (aq) + 2 H+ (aq)H2O (l) + CO2 (g)

m) Aluminum metal with calcium hydroxide [skip this question]CMECIENIE

n) Phosphoric acid & potassium hydroxideCME H3PO4 (aq) + 3 KOH (aq) K3PO4 (aq) + 3 H2O (l)

CIE 3 H+

(aq) + PO43-

(aq) + 3 K+

(aq) + 3 OH-

(aq)

3 K+

(aq) + PO43-

(aq) + 3 H2O (l)NIE 3 H+ (aq) + 3 OH- (aq)3 H2O (l)

o) Potassium hydroxide with ammonium bromideCME KOH (aq) + NH4Br (aq) KBr (aq) + H2O (l) + NH3 (g)CIE K+ (aq) + OH- (aq) + NH4

+ (aq) + Br- (aq) K+ (aq) + Br- (aq) + H2O (l) + NH3 (g)NIE OH- (aq) + NH4

+ (aq)H2O (l) + NH3 (g)


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3. Sodium metal reacts with atmospheric oxygen to form compound A, compound A reacts with waterto give compound B, compound B reacts with carbon dioxide to give compound C and water,compound C reacts with barium chloride to give solid D and NaCl and solid D reacts withhydrochloric acid to give water, compound E and barium chloride. Identify A, B, C, D, E and write the

equation for each reaction.

Na (s) + O2 (g)Na2O (s) [A]Na2O (s) + H2O (l) 2 NaOH (aq) [B]NaOH (aq) + CO2 (g)NaHCO3 (aq) [C]2 NaHCO3 (aq) + BaCl2 (aq) 2 NaCl (s) + Ba(HCO3)2 (s) [D]Ba(HCO3)2 (s) + 2 HCl (aq) 2 H2O (l) + BaCl2 (aq) + 2 CO2 (g) [E]


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4. How would calcium oxide react with:

a) Water CaO (s) + H2O (l) Ca(OH)2 (aq)b) Sulfuric acid CaO (s) + H2SO4 (aq) CaSO4 (s) + H2O (l)c) How would the product in 4a) react with:

i) Hydrochloric acid Ca(OH)2 (aq) + 2 HCl (aq) CaCl2 (aq) + 2 H2O (aq)ii) Carbon dioxide Ca(OH)2 (aq) + CO2 (g) CaCO3 (aq) + H2O (l)iii) Ammonium chloride Ca(OH)2 (aq) + 2 NH4Cl (aq)CaCl2 (aq) + 2 NH3 (g) + 2 H2O (l)

5. Write the equation for the reaction of each of the following elements with oxygen.a) Barium Ba (s) + O2 (g) BaO (s)b) Sulphur S (s) + O

2

(g) SO2

(g)S (s) + 3/2 O2 (g) SO3 (g)

6. Write the equation for the reaction of the products of 5) with water.a) Barium BaO (s) + H2O (l) Ba(OH)2 (aq)b) Sulphur SO2 (g) + H2O (l)H2SO3 (aq)

SO3 (g) + H2O (l)H2SO4 (aq)

7. How would the products of 6) react with sodium hydroxide?a) Barium Ba(OH)2 (aq) + NaOH (aq) no reactionb) Sulphur H2SO2(aq) + 2 NaOH (aq)Na2SO3 (aq) + 2 H2O (l)

H2SO4 (aq) + 2 NaOH (aq)Na2SO4 (aq) + 2 H2O (l)



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11. What would you expect to happen if you added concentrated sodium hydroxide solution to asolution of aluminum chloride?Formation of a precipitate: NaOH (aq) + AlCl3 (aq)NaCl (aq) + Al(OH)3 (s)

12. Write the CME, CIE and NIE for the following:a) Aqueous NaOH is added to AlCl3 until a white precipitate appearsb) Excess NaOH is added to the precipitate from a) until the precipitate disappearsa) CME: 3 NaOH (aq) + AlCl3 (aq)3 NaCl (aq) + Al(OH)3 (s)

CIE: 3 Na+ (aq) + 3 OH- (aq) + Al3+ (aq) + 3 Cl- (aq)3 Na+ (aq) + 3 Cl- (aq) + Al(OH)3 (s)NIE: 3 OH- (aq) + Al3+ (aq)Al(OH)3 (s)

b) CME: NaOH (aq) + Al(OH)3 (aq)NaAl(OH)4 (aq)CIE: Na+ (aq) + OH- (aq) + Al(OH)3 (s)Na

+ (aq) + Al(OH)4- (aq)

NIE: OH- (aq) + Al(OH)3 (s)Al(OH)4- (aq)

13. For the following elements: Sulphur, chlorine, phosphorus, potassium, carbon, aluminuma)Write the formula of its oxide. List only the highest oxidation state oxides (the one with the most

oxygens), b)Classify each oxide as acidic, basic or amphoteric.a) b)SO3 acidicCl2O7 acidicP4O10 acidicK2O basicCO2 acidic

Al2O3 amphoteric (acidic or basic)




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14. Predict whether a reaction will happen or not. If a reaction occurs, complete & balance theequation.

a) 2 NaOH (aq) + H2SO4 (aq) Na2SO4 (aq) + 2 H2O (l)

b) H2 (g) + O2 (g) H2O (l)

c) C5H12 (l) + 8 O2 (g) 5 CO2 (g) + 6 H2O (l)

d) H2O (l) (electrolysis) H2 (aq) + O2 (g)

e) Al (s) + KCl (aq) no reaction

f) K (s) + Cl2 (g) KCl (s)

g) AgF (aq) + Cu(ClO3)2 (aq) no reaction

h) AlBr3 (aq) + (NH4)3PO4 (aq) AlPO4 (s) + 3 NH4Br (aq)

i) F2 (g) + 2 KBr (aq) Br2 (l) + 2 KF (aq)


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Chemistry NYA Answers Part 3