(a)
Interpretation:
Types of attractive intermolecular interactions that arise between molecules of
Concept Introduction:
Intermolecular forces are forces that are responsible for interaction between molecules. Such forces include both attractive as well as repulsive forces.
Types of intermolecular forces:
1. Ion-dipole forces: These forces come into play when ions interact with polar molecules. Ion gets attracted to oppositely charged end of polar molecule.
2. Dipole-dipole forces: These forces arise when there is interaction between oppositely charged ends of different dipoles.
3. London forces: These forces exist when there is interaction between nonpolar molecules. There occurs distortion in symmetry of electron clouds when two nonpolar molecules come closer to each other. Such forces exist in all molecules and therefore London forces are called universal.
4. Hydrogen bonding: This intermolecular force exists when hydrogen atoms are connected to highly electronegative elements like
(b)
Interpretation:
Types of attractive intermolecular interactions that arise between molecules of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Types of attractive intermolecular interactions that arise between molecules of
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
Types of attractive intermolecular interactions that arise between molecules of
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemical Principles: The Quest for Insight
- 3C. Restate the assumptions of the kinetic molecular theory.arrow_forward(a) How do the structures of these molecules account for these differences in boiling point? Provide a full account of the structures and their influence on the differences in this physical property. Name Boiling Point methane -161.6 °C methanol 64.7 °C propane -42 °C propan-1-ol 97 °Carrow_forward2S03(g) →2SO2(g) + O2(g); AH° =arrow_forward
- The energy of the van der Waals bond, which is responsible for a number of the characteristics of water, is about 0.50 eV. (a) At what temperature would the average translational kinetic energy of water molecules be equal to this energy? (b) At that temperature, would water be liquid or gas? Under ordinary everyday conditions, do van der Waals forces play a role in the behavior of water?arrow_forwardWrite the difference between ferromagnetism and anti-ferromagnetism.arrow_forward7. (a) What effect do the polarity, size, and shape of a molecule have on the physical properties of the molecule? (b) How do these factors influence intermolecular forces? K/UT/Iarrow_forward
- (a) How do the viscosity and surface tension of liquids change as intermolecular forces become stronger? (b) How do the viscosity and surface tension of liquids change as temperature increases? Accounts for these trendsarrow_forwardRank the following substances in increasing boiling points (left-to-right). (a) CH4, C,H6, C;Hs, C4H10; (b) HF, HCI, HBr, and HI; (c) NH3, PH3, ASH3, and SbH3; (c) CH3OH, CH;CH;OH, CH3CI, and CH;CH;Cl; 2.arrow_forwardName the type(s) of intermolecular forces that exists between molecules (or basic units) in each of the following species: (a) LiF, (b) CH4, (c) SO2 (a) benzene (C6H6), (b) CH3Cl, (c) PF3, (d) NaCl, (e) CS2arrow_forward
- Ethanol, C2H5OH, and carbon dioxide, CO2, have approximately the same molecular mass,yet carbon dioxide is a gas at STP and ethanol is a liquid. How do you account for thisdifference in physical property?arrow_forwardExplain each of these properties of water, and describe how each is conferred by the dipolar nature of a water molecule: high specific heat capacity; high heat of vaporization; unique density behavior; high surface tension; capacity to be a good solvent for ions of salts.arrow_forwardQ2.2a - Identify the type of atomic bonds and intermolecular attractions present in each of the following scenarios: A compound made of positively-charged magnesium and negatively-charged sulfide atoms. The balanced bonds holding together the carbons and hydrogens in a molecule of Ethane. Hydrogen Fluoride is added to an aqueous solution. It dissolves due to interactions between partially-charged atoms in the Hydrogen Fluoride and Water molecules. The fatty acid tails on phospholipids are strongly attracted to each other because they are strongly repelled by water. This allows them to form phospholipid bi-layer structures. Ethanol contains an alcohol group with an oxygen atom that is strongly electronegative. This causes the molecule's electrons to be unbalanced, resulting in a partially-charged molecule. Hydrogen Attraction Non-polar Covalent Bond lonic Bond Hydrogen Attraction Polar Covalent Bond 4 >arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning