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What is the biggest difference between the Lewis and the AO-model in terms of the localisation of electrons in atoms?
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- Which of the following bonds are polar: (a) P—O; (b) S—F; (c) Br—Br; (d) O—Cl? Which is the more electronegative atom in each polar bond?Some chemical reactions proceed by the in it ial loss or transfer of an electron to a diatomic species. Which of the molecules N2, NO. O2, C2, F2, and CN would you expect to be stabil ized by (a) the addit ion of an electron to form AB-. (b) the removal of an electron to form AB+?What is the biggest difference between the Lewis and the AO-model in terms of the localisation ofelectrons in atoms?
- If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?The length of a covalent bond depends upon the size of the atoms and the bond order. For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) C≡O(B) C-O ...... (A,B) fill in the blank 1(C) N=N(D) N≡N ...... (C,D) fill in the blank 2The 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?
- The 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 2If 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)?Hydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.
- The 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 2Calculate the ionic resonance energy of HCl, given that: χH = 2.2 and χCl = 3.16.The compounds ethyne, ethene and ethane contain, respectively, C≡C, C=C and C–C bonds. What is the expected sequence of carbon–carbon bond lengths and bond enthalpies. Select one: a. Bond lengths: C≡C > C=C > C–C; bond enthalpies: C≡C < C=C < C–C b. Bond lengths: C≡C < C=C < C–C; bond enthalpies: C≡C < C=C < C–C c. Bond lengths: C≡C < C=C < C–C; bond enthalpies: C≡C > C=C > C–C d. Bond lengths: C≡C > C=C > C–C; bond enthalpies: C≡C > C=C > C–C