In a gaseous RbF molecule, the bond length is
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Chapter 3 Solutions
Principles of Modern Chemistry
- In a XeF3Br molecule, why is there a difference in bond length between the Xe-F bond and the Xe-Br bond?arrow_forwardThe potential energy function for either one of the two atoms in a diatomic molecule is often approximated by U(x) a b = x22 x11 where x is the distance between the atoms. a. At what distance of separation does the potential energy have a local minimum (not at x = Express your answer algebraically. xmin b. What is the force on an atom at this separation? F(x = 2min)= N ∞)?arrow_forwardThe strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.(A) N≡N(B) N-N ...... (A,B) fill in the blank 1(C) C=O(D) C≡O ...... (C,D) fill in the blank 2arrow_forward
- Give the ground-state electron configurations and bond orders of(i) F2−, (ii) N2, and (iii) O22−.arrow_forwardWithout consulting tables of data, on the same graph sketch the effective potential energy curves for H2 and He+2.arrow_forwardConsider the molecular hydrogen dimer, HCl···HCl. Suppose that the bond stretching is described using harmonic potentials, and that the van der Waals interactions between non-bonded atoms are described by Lennard-Jones potential. Write the expression of the interatomic forcefield describing the energy of HCl···HCl.arrow_forward
- If the bond in the AB molecule is considered 100% ionic, the absolute value of the partial charge would be equal to the electron charge (1.602 x 10-19 C). If the distance between A and B atoms is taken as 10-10 m (1Å), the dipole moment between two elementary charges of opposite sign at atomic magnitude (1Å) distance between them is = 1.602x10-19 C x 10-10 m = 1.602 x 10- It is available in 29 Cm (or 4.8 x 10-18 esbcm). Dipole moment is given by debye (D) and 1D = 3.34x10-30 Cm (or 1D = 10-18 esbcm) (esb = electrostatic unit). 1. As can be seen, when the HCl covalent molecule is considered ionic and the bond length is 1.27x10-10 m, calculate the dipole moment. The experimental dipole moment of an HCl polar option is = 1.03 D. Calculate the value character of the H-Cl bond according to the bulletin. How many% covalent is the bond, how many% is ionic? Specifyarrow_forwardThe strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.(A) C-O (B) C≡O ...... (A,B) fill in the blank 1 (C) C-C (D) C=C ...... (C,D) fill in the blank 2arrow_forward2. Using the ionization energy of H 1s and CI 3p electrons of 13.6 eV and 13.1 eV, respectively, calculate the (a) energies and (b) compositions of the bonding and antibonding orbitals of HCI. (Use aH = -13.6 eV and acı = -13.1 eV.) Use B=-1.0 eV and S=0.arrow_forward
- Give the ground-state electron configurations of (i) CO, (ii) NO, and (iii) CN−.arrow_forwardWithout consulting tables of data, predict which species has the greater bond length, H2 or He+2.arrow_forward1. Neutrons as well as electrons and x-rays can be used to obtain information about molecular structure through diffraction patterns. What must the velocity of a neutron be for its de Broglie wavelength to be about five times smaller than a bond length? How does this velocity compare (bigger, smaller, or the same) if electrons were diffracted? A typical bond length for C-C is 1.54Å (1.54 x 10-1ºm).arrow_forward
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