H2S, H2O, CH4, H2, KBr Solution: KBr is an ionic solid (metal and non-metal) so it has the highest boiling point of the listed compounds. See the figure (Bp of Hydrides) on page 42. fill in the missing particles and determine the decay type. CH 4 is a nonpolar molecule and has a weak dispersion force (10 electrons), (bp −161°C). The variation in boiling point can be explained by intermolecular bonding Explain why H2S has a lower boiling point than H20 and H2Se. Since H2Se … Well the simplest answer is..."because God wanted in that way.." As you know, the normal boiling points of water, 100 ""^@C, and ammonia, -33.3 ""^@C..are EXCESSIVELY HIGH....especially given these are molecules of paltry molecular mass, the which gives rise to negligible dispersion force. Among H2O, H2S, H2 Se and H2 Te the one with highest boiling point. H2O, 100oC; H2S, -60oC; H2Se, -41oC; H2Te, -2oC (2 marks) Generally, the boiling points in a series increases with the molecular mass and this would put the boiling point of water below -60o C. The boiling point of water is high because of the extensive H-bond between the water molecules. H2Se has the higher boiling point because it has a larger mass and more electrons. This because H2O have intensive HYDROGEN BONDING within its molecules × Enroll For Free Now & Improve Your Performance. Examples are boiling and melting points compared to $\ce{H2S}$, $\ce{H2Se}$, density anomaly at 4 °C and many others. 1 answer. asked Apr 21, 2019 in Chemistry by Simrank (72.0k points) p - block element ; jee; jee mains; 0 votes. Re: Boiling Point . Because Se has more electrons, it is more polarizable and therefore has stronger London Dispersion Forces than H2S. It is poisonous, corrosive, and flammable. The reason is the enhanced electronegative character of N, O and F. That is why, water is liquid at room temperature, but H 2 S and H 2 Se are gases. That is, The $\ce{S-H}$ and $\ce{Se-H}$ bonds use pure $\ce{p}$-orbitals from sulfur and selenium respectively. Find out more about how we use your information in our Privacy Policy and Cookie Policy. The boiling point of hydrogen compounds of group 16 is into the order of H2O > H2S . $\endgroup$ – TAR86 Jun 20 '19 at 17:56. 6.54. Note also that the boiling point for toluene is 111 o C, well above the boiling point of benzene (80 o C). The threshold limit value is 0.05 ppm. The key factor for the boiling point trend in this case is size (toluene has one more carbon), whereas for the melting point trend, shape plays a much more important role. k..VS.. Ad-pd. Information about your device and internet connection, including your IP address, Browsing and search activity while using Verizon Media websites and apps. 13d) All four molecules are molecular solids. 1 $\begingroup$ Freezing is tricky, it can't be justified as easily as boiling. This causes it to have a higher boiling point. × Thank you for registering. 30,747 results, page 2 chemistry. It also shows the saturation pressure with changes in temperature. Two $\ce{p}$-orbitals are used, one for each of the two $\ce{X-H}$ bonds; this leaves another $\ce{p}$-orbital and an $\ce{s}$-orbital to hold the two lone pairs of electrons. [5] Select one: A. HCl B. H2S C. CH3OH D. CH4 E. NH3. Which one of the following should have the lowest boiling point? On the other hand, both $\ce{H2S}$ and $\ce{H2Se}$ have no orbital hybridization. Sample Problem: Place the following compounds in order of increasing boiling point. katie_sutton1B Posts: 61 Joined: Fri Sep 28, 2018 7:17 am. What the molar enthalpy of the reaction? ) From the following pairs of compounds, determine which one has the highest boiling point. The graph below shows the variation in boiling points of the Group 16 hydrides. However, in the chemistry textbook version 6 p.484, H2Se is expected to be a stronger acid than H2S because H2Se … Journal of Chemical Education 2011 , 88 (7) , 937-943. However, when we measure the boiling points for these compounds, we find that they are dramatically higher than the trends would predict, as shown in Figure 11. Explain your reasoning a) H2S vs H2Se b) CH3Cl vs CH3F c) CO2 vs NO2 d) H2S vs H2O e) HF vs HCl f) NH3 vs BF3 1 Bromine is a reactive element. Post by katie_sutton1B » Fri Dec 07, … When we consider the hydrides of group VA, VIA, VIIA then NH 3, HF and H 2 O show maximum boiling points in the respective series. H2se H2Te, Amongst H2O, H2S, H2Se and H2Te, the one with the highest boiling point is (a) H2O because of hydrogen bonding, Classification of elements and periodicity in properties. d. The dry atmosphere is made up almost entirely of 3 species: N2 (78%), O2 (21%), and Ar (1%). H2S = 212 K. H2Se = 232 K. H2STe = 271 K (- 2.2 oC) the boiling points as some other contributors have said is an indication of intermolecular forces. One of our academic counsellors will contact you within 1 working day. So why so? What is the freezing point of a solution that contains 10.0 g of glucose (C6H12O6)in 100.g of H20? Chemistry. If we use this trend to predict the boiling points for the lightest hydride for each group, we would expect NH3 to boil at about 120 °C, H2O to boil at about 80 °C, and HF to boil at about 110 °C. H2Se has stronger London forces than H2S because it has more electrons meaning the induced dipoles will be stronger - more energy is needed to break them so … Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get … The stark contrast between our naïve predictions and reality provides compelling evidence for the strength of hydrogen bonding. Which has highest boiling point? H20, H2S, H2Se, H2Te i know its H20, but why? Hydrogen selenide is hazardous, being the most toxic selenium compound and far more toxic than its congener hydrogen sulfide. Favorite Answer I find in a handbook a different Bp for H2Se, it is, -41.25 degrees C. The boiling point for H2Te is given as the same as the previous answer. What is the partial pressure of Ar (in kPa) when the atmospheric pressure is 654 kPa? Kf for water is 1.86C/m. An Analytical Approach for Relating Boiling Points of Monofunctional Organic Compounds to Intermolecular Forces. 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