In H2O, H2S, H2Se, H2Te, the bond angle decreases though all have the same bent shape. Why does the angle never drop below 90? (B) The polarizability of the group 16 elements increases going down the group. Expert Answer: Effect of electronegativity of the surrounding atom on the bond angle of … In H2O, H2S, H2Se, H2Te, the bond angle decreases though all have the same bent shape. H2Te is the most acidic among the three. Arrange in decreasing order of bond angle. In H2O, H2S, H2Se, H2Te, the bond angle decreases though all have the same bent shape. Why? H2S, H2Se and H2Te exhibit dipole-dipole intermolecular forces while H2O exhibits hydrogen bonding. What is a functional group in organic chemistry? H2Se, H2O, H2Te, H2S. (A) The electronegativity of the group 16 elements increases going down the group. asked May 29, 2019 in Chemistry by Ruksar (68.7k points) chemical bonding; molecular structure; class-11; Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Students (upto class 10+2) preparing for All Government Exams, CBSE Board Exam, ICSE Board Exam, State Board Exam, JEE (Mains+Advance) and NEET can ask questions from any subject and get quick answers by subject teachers/ experts/mentors/students. Explain why there is an increase in bond angle in the series PF3H2S>H2Se>H2Te. In all the four cases, the molecules undergo Sp, Arrange in decreasing order of bond angle. Why? The lone pair of electrons takes up more space than a regular bonding pair since it it is not confined to be between two atoms, so it adds coulombic repulsion to the bonding pairs and compresses the angle. See h20 has 104.5 degrees bond angle , h2s has 92degrees , h2se has 91degrees and h2te has 90degrees bond angles Answer:The lone pair of electrons takes up more space than a regular bonding pair since it it is not confined to be between two atoms, so it adds coulombic repulsion to the bonding pairs and compresses the angle. Hence, H2Te can release H-ion more easily than H2S, making it more acidic. Predict the correct order of bond angles: a)H2S>H2O>H2Se>H2Te b)H2O>H2S>H2Se>H2Te c)H2Te>H2Se>H2S>H2O d)H2O>H2Se>H2S>H2Te 2 See answers nverma0811 nverma0811 May be c is correct.. In diatomic nitrogen (N≡N), for instance, the bond order is 3 because there are 3 chemical bonds linking the two nitrogen atoms. In H2O, H2S, H2Se, H2Te, the bond angle decreases though all have the same bent shape. Arrange H2O, H2S, H2Se, H2Te. Can't explain that with Lewis. To learn how to determine a bond order at a glance, keep reading! Why? In the decreasing order of boiling point. Valence bond theory explains bond angles in terms of hybridization of orbitals. Amongst H2O, H2S, H2Se and H2Te, the one with the highest boiling point is (a) H2O because of hydrogen bonding asked Mar 12, 2019 in Chemistry by Daisha ( 70.5k points) s-block elements The sizes increase in the order S H2S > H2Se > H2Te (104.5) (92.5) (91.0) (89.5) in inorganic chemistry Arrange the following in order of property indicated for each set : H2O, H2S, H2Se, H2Te – increasing acidic character HF, HCl, HBr, HI – decreasing bond enthalpy So, they have minimum bond angles group In all the four cases, the molecules undergo Sp3 hybridization forming four hybrid orbitals, two of which are occupied by 1p of electrons and two by bp electrons. Arrange in decreasing order of bond angle. The trend in bond angles in H2O, H2S, H2Se, H2Te of 104.5, 92.3, 91 and 90 respectively. asked May 29, 2019 in Chemistry by Ruksar (68.7k points) chemical bonding; molecular structure; class-11; 0 votes. In H2O, H2S, H2Se, H2Te, the bond angle decreases though all have the same bent shape. (a) H2O, H2S, H2Se. In case of H2O molecule, as oxygen is small in size and has high electronegativity value, the bp are closer due to which it is subjected to larger repulsion (bo-bp). ), Arrange the following in order of property indicated for each set: (a) H2O, H2S, H2Se, H2Te – increasing acidic character. Thus they are expected to have 109°28' angle but this does not happen. Which is the best explanation for this trend? In H2O, H2S, H2Se, H2Te, the bond angle decreases though all have the same bent shape. The reason for this is that the repulsions between lone pair increases by size and the size increases down in the group .Also the molecules have no hybridisation. Arrange the following sets of molecules in the decreasing order of bond angle –  (i) SF6, H2O, NH3, CH4. Why the sudden and dramatic jump from almost tetrahedral angle to almost orthogonal? This can be explained by the application of VSEPR with some hand waving steric and inductive electronic arguments thrown in. Looking at the table, when we go from AX2, AX3 and all the way down to AX2N2, we will find out that the bond angle is going to be 109.5 degrees. In H2O, oxygen is more electronegative, electrons of two O-H bonds are more attracted towards oxygen atom. H2Se is a bent molecule with a bond angle of 91 0. H2O Bond Angles. In the decreasing order of boiling point. H2O would be the highest, I think, due to the hydrogen bonding that occurs when hydrogen is bonded to an N, O, or F atom. Arrange the following in order of the property mentioned against each: (a) PH3, NH3, SbH3, AsH3 (Increasing basic strength)(b) H2O, H2S, H2Se, H2Te (Increasing bond angle)(c) HClO4, HClO3, HClO2, HClO (Increasing oxisidsing ability) - Chemistry - The p-Block Elements H2O, H2S, H2Te, H2Se (acidic strength), Arrange in the increasing properties of H2O, H2S, H2Se, H2Te (B.P. 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