Which of the following molecules would have the most polar bonds (Ch 9.6 pg 396)

Question

Which of the following molecules would have the most polar bonds (Ch 9.6 pg 396) and which would produce the largest ions when dissolved in water (pg. 359-360 figure 8.12-13)? Rbcl HBr Explain why the Rb ion is smaller than the Bryon (you can use periodic trends of ions) A 1.50 L glass vessel contains 0.112 mol of Cl_2 (g) and 0.117 mol of HI (g) at 110_degree C. Starting with the ideal gas law, PV = nRT (pg 208), solve for P/RT. What are the units for P/RT (when simplified)? Calculate the molarities of the gases and convert those values into pressure using the ideal gas low. (wait for lab lecture before trying this) Assuming moles, temperature, and pressure stated above, if the following reaction goes to completion, what is the total pressure in the container? Assume constant temperature and volume (pg 221-223). Cl_2 (g) ? 2 HI (g) -I_2 (s) ? 2 HC1 (g)

Explanation / Answer

Solved Q6 completely, post multiple question to get the remaining answers

Q6)

a) HF

Electronegativity of H = 2.1

Electronegativity of F = 4

Difference in electronegativity = 1.9

b) RbCl

Electronegativity of Rb = 0.82

Electronegativity of F = 3.16

Difference in electronegativity = 2.34

c) HBr

Electronegativity of H = 2.1

Electronegativity of Br = 2.96

Difference in electronegativity = 0.86

The highest electronegativity difference exists between Rb and Cl, since Rb is an metal and Cl is highly electronegative element

d) The size of Rb ion s smaller than Br ion, because in water Rb will exists as Rb+ and it will lose the electron from outer octet whereas Br will accept an electron from outer octet to reach nearest noble gas configuration

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.