19 Jan Chem 1008 Halogens Boiling Poin 85.1 238.6 332.0 457.6 ie thebist of f gy

Question

19 Jan Chem 1008 Halogens Boiling Poin 85.1 238.6 332.0 457.6 ie thebist of f gy the observed incrase in boing point rele F2 Cl2 Brz 4. Given the 3 compounds below all have comparable molecular masses. List the dominant type of IME for each substances, then rank the strength of each compound based on the IMF you have assigned (i-strongest, 2 = in between, 3 = weakest) IMF Relative Strength Compo und HBr CH OH 5. Circle all of the species below that can form a hydrogen bond in its pure form. Briefly explain why the other species cannot hydrogen bond A. C2He B. HF C. CHsOCH D. KCI E. CH;CH CH2OH 6. List the intermolecular force that would occur in each of the following A. CO B. CO2 C. BrF D. CsBr E. SiCl Rank the following compounds, H2S, C2, Nal, N2, H:0, from weakest intermolecular forces to strongest. Justify your answer 7.

Explanation / Answer

3. Due to increasing the strength of Van der Waal's forces as the sizes and relative atomic mass of the atoms increases.

4. CH3OH (hydrogen bonding-strongest) > HBr (Dipole-Dipole- in between)> O2 (London Dispersion -weakest).

5. Hydrogen bond formed between H and more electronegative atoms like F, O and N etc. Options B and E , HF & propanol exhibit H-bond.

While remaing not formed.

6. CO-dipole-dipole forces, CO2- London Dispersion Force

BrF- dipole-dipole, CsBr- Ionic bonding and SiCl4- dipole-dipole

7. H2S and H2O- Hydrogen bond, Cl2 and N2- London Dispersion forces, NaI - Ionic bonding.

Strongest NaI > H2O > H2S>Cl2> N2 weakest.

Order of intermolecular forces' Ionic bonding>H-Bond >dipole-dipole> London Dispersion forces

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