Interpretation:
Compare the estimated values with the experimental values have to be done.
Concept Introduction:
Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.
Bond distance: In molecular geometry, bond length or bond distance is the average distance between nuclei of two bonded atoms in a molecule. It is a transferable property of a bond between atoms of fixed types, relatively independent of the rest of the molecule.
Increase and decrease electro negativity: The less vacancy electrons an atoms has the least it will gain of electrons. Moreover the
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Chemistry & Chemical Reactivity
- The bond length in HI(1.62) is close to the sum of the atomic radii of H (0.37 Å) and I (1.33 Å). What does this fact indicate about the polarity of the bond?arrow_forwardThe bond energy of C2 is 599 kJ/mol, the bond distance is 110 pm. Take a rough estimate of the Coulomb repulsion in doubly ionized C2 (i.e., C22+). How far would the C-C bond have to stretch for the Coulomb repulsion to be less than the bond energy in neutral C2? Do you think that the C22+ molecule will still be stable?arrow_forwardIf the dipole moment of a diatomic molecule is found to be 1.04 D, and its bond length is found to be 124 pm, what is the fractional charge on the atoms of the molecule in Coulombs (C)?arrow_forward
- “Inert” xenon actually forms several compounds, especially with the highly electronegative elements oxygen and fluorine. The simple fluorides XeF2, XeF4, and XeF6 are all formed by direct reaction of the elements. As you might expect from the size of the xenon atom, the Xe-F bond is not a strong one. Calculate the Xe-F bond energy in XeF6, given that the enthalpy of formation is - 402 kJ/mol.arrow_forward(c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observationsarrow_forwardBased on average bond enthalpies, would you expect a photon capable ofdissociating a C¬Cl bond to have sufficient energy to dissociate a C¬Br bond?arrow_forward
- To explain why AHan for RbCl is different than that for KCI, the student investigates factors that affect AHoln and finds that ionic radius and lattice enthalpy (which can be defined as the AH associated with the separation of a solid crystal into gaseous ions) contribute to the process. The students consults references and collects the data shown in the table below. lonic Radius (pm) lon к' 138 Rb* 152 b. Using principles of atomic structure, explain why the Rb' ion is larger than the K' ionarrow_forwardb) Answer the following question and give a brief explanation for your answers. a. Which one is more reactive : cesium, Cs or potassium, K? Explain b. Which one is more electronegative silicon, Si or tellurium, Te? Explain c. Arrange the following according to their size : smallest to largest. Justify your answer. O2 , F, Nearrow_forwardUse average bond enthalpy values to calculate ΔrH for the following reaction: 2NH3 + 3Cl2 → N2 + 6HClarrow_forward
- Which is the bonding and which is the anti-bonding orbital? Describe the differences in these two orbitals with respect to the number of nodes present, the relative electron density located between the atoms versus that located outside the inter-nuclear region, and the overall size of regions with the same phase. How do you expect the wavelength of the electron to vary between these two orbitals? What about the relative energy of the electron in these two states? Explainarrow_forwardThe bond lengths in Cl2, Br2, and I2 are 200, 228, and 266 pm, respectively. Knowing that the silicon radius is 111 pm, estimate the bond distances in Si-Cl, Si—Br, and Si—I. (Express your answer as an integer.) Si-Cl: Si-Br: Si-I: pm pm pmarrow_forwardConsider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule?arrow_forward
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