lon-dipole interaction Dipole-dipole interaction lon-ion interaction Induced dipole-dipole interaction Decane is liquid while Ethane is gas at room temperature. This can be as the carbon chain increases. explained by stronger O London dispersion force hydrogen bond induced dipole-dipole interaction dipole-dipole interaction
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- TRUE OR FALSE 1. Molecules with temporary dipole moment tend to align with opposite polarities in the solid phase for maximum attractive interaction. 2. The boiling points of compounds containing elements in the same periodic group is inversely proportional to the element's molar mass. 3. When adhesion is greater than cohesion, a convex appearance of the liquid in a tube is evident.Choose from: A = intermolecular H-bonding B = London dispersion forces C = intramolecular H-bonding D = dipole-dipole interaction E = ion-dipole interaction Benzoic acid and aniline are both sparingly soluble in water. Their respective salts, however, are both very soluble. This is because their salts can exhibit _____ interaction with water.Show hydrogen bonds and the dipole-dipole moments.
- The table below shows the normal boiling points of benzeneand benzene derivatives.(a) How many of these compounds exhibit dispersion interactions?(b) How many of these compounds exhibitdipole-dipole interactions? (c) How many of these compoundsexhibit hydrogen bonding? (d) Why is the boilingpoint of bromobenzene higher than that of chlorobenzene?(e) Why is the boiling point of phenol the highest of all?Solvent-solvent interaction between acetyl chloride dissolved in HF? ion-dipole dipole-dipole london h bonding ionicWhat is the strongest interparticle force in each of the following substances?a) CH3Clhydrogen bondingdipole―dipoledispersion(b) CH3CH3dipole―dipoledispersionhydrogen bondingc) NH3hydrogen bondingdispersiondipole―dipole
- A miscible solution of cyclopentane and cyclooctane is capable of ___________. dispersion force dispersion force, dipole-dipole interactions dispersion force, dipole-dipole interactions, hydrogen bonding dispersion force, dipole-dipole interactions, hydrogen bonding, ion-dipole interactionsUse the normal boiling pointspropane 1C3H82 -42.1 °Cbutane 1C4H102 -0.5 °Cpentane 1C5H122 36.1 °Chexane 1C6H142 68.7 °Cheptane 1C7H162 98.4 °Cto estimate the normal boiling point of octane 1C8H182.Explain the trend in the boiling points.A chloride ion and a sodium ion are separated by a center–center distance of 0.5 nm. Calculate the interaction energy (the energy required to pull them infinitely far apart) if the medium between them is (a) water and (b) n-pentane . Express the energy in joules per mole of ion pairs. [Note: The charge on an electron is 1.602 * 10-19 C, Avogadro’s number is 6.02 * 1023 molecules/mol.]
- A. DIRECTION: Define the following and give an example of each:1. Dispersion force2. Dipole-dipole attraction3. Hydrogen bond B. DIRECTION: Open the PhET States of Matter Simulation to answerthe following questions: Link: https://phet.colorado.edu/en/simulation/states-of-matter 1. Select the Solid, Liquid, Gas tab. Explore by selecting differentsubstances, heating and cooling the systems, and changing thestate. What similarities do you notice between the foursubstances for each phase (solid, liquid, gas)? What differencesdo you notice? 2. For each substance, select each of the states and record the giventemperatures. How do the given temperatures for each statecorrelate with the strengths of their intermolecular attractions?Explain.NaNO2 (aq) + HSO3NH2 (aq) ----> NaHSO4(aq) +N2(g) + H2O (l) Calculate Atmospheric pressure (mmHg), Pc (mmHg), Vapour pressure of water (mmHg) and PN2 (mmHg) Given: weight of Sulfamic acid= 0.678g and weight of NaNO2= 0.888g Vapour pressure of water at 25°C = 23.8 (mmHg) and 26°C = 25.2 (mmHg) height = 14.2mm, T= 25.1 °C, Volume of acid= 25.5mL, Volume of Gas= 28.80mLGive the major force between acetone and chloroform. dipole-dipole dispersion hydrogen bonding ion-ion ion-dipole