1) The order of IMFs vary as H-bonding >> dipole-dipole interactions > dispersio

Question

1) The order of IMFs vary as H-bonding >> dipole-dipole interactions > dispersion forces. Ammonia, NH3 molecule can show all the three IMFs; however; (a) H-bonding is the strongest IMF present in NH3.

2) The higher the electronegativity of the central atom in a polyatomic molecule, the greater is the boiling point of the molecule. O atom is more electronegative than N atom which is turn is more electronegative than C atom. Consequently, O atom can form stronger H-bonds with the hydrogen atom of a neighboring H2O molecule and therefore, it requires a large amount of energy to break apart the H2O molecules; hence, H2O has the highest boiling point. C atom cannot participate in H-bonding and will have the lowest boiling point while NH3 lies in between.

3) The atomic masses of the noble gases increase in the order He < Ne < Ar < Kr < Xe. As the atomic mass increases, the dispersion forces increase (dispersion forces are related to the molecular mass of a gas). The larger the dispersion forces, the greater are the interaction between the gas molecules. The ideal gas law assumes that there is minimum interaction between the gas molecules; hence (E) Xe will show the largest deviation from ideal behavior.

4) The ideal gas law assumes that the gas molecules are point masses and do not interact with each other; the only interaction that the gas molecules show is collisions with the walls of the container. These collisions are responsible for the pressure of the gas. The molecular theory also assumes that the distance between the molecules is large compared to the diameter of the molecules; hence, the molecules show minimum interactions.

At low pressures, the collisions are significantly reduced; at high temperatures, the gas molecules are in rapid motions and the distances between the molecules is so large that they can hardly interact. Therefore, the set of conditions under which a real gas behaves like an ideal gas are (C) low pressure, high temperature.

Explanation / Answer

1. Which IMF is the most important in NH,? A. H-bonding B. dispersion C. dipole-dipole 2. Rank the boiling points of the following molecules from least to greatest HyO, NHs, CH 3. Which of the following gases has the largest deviation from ideal behavior? A. He B. Ne C. Ar D. Kr E. Xe 4. Under which set of conditions will a real gas behave most like an ideal gas? A. high pressure, high temperature B. low pressure, low temperature C. low pressure, high temperature D. high pressure, low temperature 5. FeCls is a/an substance. A. metallic B. ionic C. network covalent D. molecular covalent 6. Rank the following ionic compounds from lowest to highest melting point: Naci, KBr, CaCl Mgo 7. Which set of parameters goes together? A. weak IMF, low BP, high VP B. weak IMF, low BP, low VP C. strong IMF, low BP, high VP D. weak IMF, low BP, low VP E. weak IMF, high BP, low VP compared to 8. When a liquid evaporates, the potential energy of the particles when the liquid remains liquid. A. increases B. decreases C. stays the same 9. Circle the 2 correct parts. When silicon is doped with Ga, a/an n/p type semiconductor is created. The Ga adds mobile-charges, + holes 10. Which of the following explains why CS, has a higher boiling point than Co,? ent while CO2 is molecular covalent B. CS2 is polar, CO, is nonpolar. C. A. CS is network coval cs, has stronger dispersion forces. D. CS, is more polar than CO2 11. Which of the following explains why KCI has a lower melting point than Nacr? A. KCI is less polar than NaCI B. K' is larger than Na* C. NaCl is network covalent 12. Each of these flasks contains water at 25C. Which flask has the highestvP? B. C. D. A. E. all are equal

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

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