1. For each compound given here, write what type of compound it is (molecular or ionic or acid).
(a) NH4Cl (b) AlH3 (c) O2 (d) CH4 (e) NH3 (f) H2O (g) PCl5
(h) SF4 (I) ClF3 (j) XeF2 (k) SF6 (l) BrF5 (m) XeF4 (o) CS2 (p) CH2Cl2
2. Write a chemical equation that goes with Lattice energy of CaCl2(s).
3. Draw the Lewis Dot structure of ..
(a) Na
(b) Cl
(c) O-2
(d) Mg+2
4. What is the relationship between bond strength and bond energy?
5. Nitrogen and hydrogen combine to form ammonia in the Haber process. Calculate (in kJ) the standard enthalpy change H° for the reaction written below, using the bond energies given.
N2(g) + 3H2(g) ? 2NH3(g)
Bond: |
NN |
H–H |
N–H |
Bond energy (kJ/mol): |
945 |
432 |
391 |
6. Acetone can be easily converted to isopropyl alcohol by addition of hydrogen to the carbon–oxygen double bond. Calculate the enthalpy of reaction using the bond energies given.
Bond: |
C=O |
H–H |
C–H |
O–H |
C–C |
C–O |
Bond energy (kJ/mol): |
745 |
436 |
414 |
464 |
347 |
351 |
7. Define electronegativity.
8. Select the most polar bond amongst the following. |
A) C–O B) Si–F C) Cl–F D) C–F E) C–I |
9. Based on electronegativity trends in the periodic table, predict which of the following compounds will have the greatest % ionic character in its bonds. |
A) H2O B) LiI C) CaO D) RbF E) HCl |
10. a) For each reaction given here, give at least one NAME for the energy. For example, the first one will be called ‘heat of sublimation”
Mg(s) → Mg(g) ΔH° = 148 kJ ‘heat of sublimation”
Mg(g) → Mg2+(g) + 2e- ΔH° = 2186 kJ ?
S8(s) → 8S(g) ΔH° = 2232 kJ ?
S(g) + 2e- → S2-(g) ΔH° = 450 kJ ?
8Mg(s) + S8(s) → 8MgS(s) ΔH°= -2744 kJ ?
b) What is the NAME for the energy associated with Mg2+(g)
+ S2-(g) → MgS(s) ?
c) Using Hess’s Law with equations given in (a), calculate the enthalpy change for Mg2+(g) + S2-(g) → MgS(s) .
11. What is the relationship between (directly, inversely, not related?) …
Effective nuclear charge and atomic size
Energy and n
Stability and n
Effective nuclear charge and shielding
Ionization energy and atomic size
Number of electrons and size
Number of protons and size
Bond length and bond energy
Bond strength and bond energy
Bond length and bond order
SOLN 1
(a) NH4Cl : ionic (NH4+ and Cl-)
(b) AlH3 : Molecular (Lewis Acid)
(c) O2 : Molecular
(d) CH4 : Molecular
(e) NH3: Molecular
(f) H2O : Molecular
(g) PCl5 : Molecular (also lewis acid)
(h) SF4 : Molecular
(I) ClF3 :Molecular
(j) XeF2 : Molecular
(k) SF6 : Molecular
(l) BrF5: Molecular
(m) XeF4 : Molecular
(o) CS2 : Molecular
(p) CH2Cl2 : Molecular
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1. For each compound given here, write what type of compound it is (molecular or ionic...
Using the following information, calculate the heat of sublimation of S(s) to S(g). ?H°f MgS= -343 kJ/mol, ?H°sublimation Mg(s) = 148 kJ/mol, The lattice energy MgS = 3406 kJ/mol ?Mg(g) ? Mg2+(g) + 2 e ??st + 2nd IE = 2186 kJ/mol, S(g) +2e ? S2-(g) ????H = 450 kJ/mol, A. 575 kJ/mol B. 1179 kJ/mol C. 279 kJ/mol D. 965 kJ/mol E. 4651 kJ/mol
16. Using the following information, calculate the sublimation of S(s) to S(g). Mg(s) + S(s) + MgS(s) AH° = -343 kJ/mol Mg(s) + Mg(g) AH° = 148 kJ/mol Mg(g) → Mg2+(g) + 2e AH° = 2186 kJ/mol S(s) + S(g) AH° = ? S(g) + 2e → S2-(g) AH° = 450 kJ/mol Mg2+(g) + SP-(g) + MgS(s) AH° = -3406 kJ/mol A) 279 kJ/mol B) 575 kJ/mol C) 1179 kJ/mol D) 965 kJ/mol E) 4651 kJ/mol
16. Using the following information, calculate the sublimation of S(s) to S(g) Mg(s) S(s) MgS(s) AHo 343 kJ/mol Mg(s) Mg(g) Mg(g) Mg (g) 2e S(s)> S(g) 2e > S2(g) Mg2 (g) S2g) -> MgS(s) A) 279 kJ/mol B) 575 kJ/mol C) 1179 kJ/mol D) 965 kJ/mol E) 4651 kJ/mol AHo 148 kJ/mol 2+ AH° 2186 kJ/mol ΔΗ S(g) AHo 450 kJ/mol AHo3406 kJ/mol _
Consider an ionic compound, MX,, composed of generic metal M and generic, gaseous halogen X. • The enthalpy of formation of MX, is AH; = -841 kJ/mol. • The enthalpy of sublimation of Mis AH sub = 111 kJ/mol. • The first and second ionization energies of M are IE = 615 kJ/mol and IE2 = 1353 kJ/mol. The electron affinity of X is AHEA = -319 kJ/mol. (Refer to the hint). • The bond energy of X, is BE...
Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X. The enthalpy of formation of MX2 is ΔH∘f=−831 kJ/mol. The enthalpy of sublimation of M is ΔHsub=129 kJ/mol. The first and second ionization energies of M are IE1=691 kJ/mol and IE2=1401 kJ/mol The electron affinity of X is ΔHEA=−307 kJ/mol. The bond energy of X2 is BE=153 kJ/mol. Determine the lattice energy of MX2. ΔHlattice=ΔHlattice= kJ/mol
Determine the lattice energy of MX2. Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X. The enthalpy of formation of MX2 is ΔH∘f=−681 kJ/mol. The enthalpy of sublimation of M is ΔHsub=145 kJ/mol. The first and second ionization energies of M are IE1=607 kJ/mol and IE2=1444 kJ/mol. The electron affinity of X is ΔHEA=−315 kJ/mol. The bond energy of X2 is BE=247 kJ/mol. Determine the lattice energy of MX2. I've been stuck on this question...
Which of the following statements are FALSE, given the following bond dissociation energies? Assume that bond energies accurately determine heats of reaction. Check all that are false. BE[H-H] = 436 kJ/mol BE[H-N] = 393 kJ/mol BE[H-O] = 460 kJ/mol BE[O=O] = 499 kJ/mol 1. NH(g) + H2(g) ---> NH2(g) + H(g) is an exothermic reaction. 2.ΔH°f[H(g)] = 218 kJ/mol 3. ΔH°[H2O(g) ---> 2 H(g) + O(g)] = 920 kJ/mol 4. An H-H bond is stronger than an H-O bond. 5....
Using bond enthalpies (given as Average Bond Energies in the Data Sheet) estimate the enthalpy change (ΔH, heat of reaction) for the following gas-phase reaction. (The bond energy value for S−C is 259 kJ mol-1 and that for S−H is 339 kJ mol-1.) HS CH2CH2 SH + 2HF F CH2CH2 F + 2 HSH.
7.5 lonic Bonding and Lattice Energy 1. Organize the following in terms of increasing magnitude of lattice energy: KСI Mgs NaF Mgo SrSe 7.5 Bond Energies 2. a. Choose the covalent bond below that is the strongest (largest bond energy) b. Choose the covalent bond below that is the longest. a. N-O d. N-N e. N-C b. N-O c. N-N 3. a) Given the following bond energies, estimate the AH of the reaction: 2 NH3 (g)N2 (g) + 3 Hz...
Acetone can be easily converted to isopropyl alcohol by addition of hydrogen to the carbon-oxygen double bond. Calculate the enthalpy of reaction using the bond energies given. Enter your answer in kilojoules. HC-C-CH, (g) + H2 (8) HC-C-CH, %) Bond: C=O H-H C-HO-H C-C C-O Bond energy (kJ/mol): 745 432 413 467 347 358