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- At large interatomic separations, an alkali halide molecule MX has a lower energy as two neutral atoms, M+X ; at short separations, the ionic form (M+)(X) has a lower energy. At a certain distance, Rc , the energies of the two forms become equal, and it is near this distance that the electron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atoms are weak at large distances, a reasonably good approximation can be made by ignoring any variation in potential V(R) for the neutral atoms between Rc and R= . For the ions in this distance range, Rc is dominated by their Coulomb attraction. (a) Express Rc for the first ionization energy of the metal M and the electron affinity of the halogen X. (b) Calculate Rc for LiF, KBr, and NaCl using data fromAppendix F.cacl calcudate the dowest pssible of Calculate ++ energy also 1on and the energy vequired electron to vemuve an from hi ions ++For each of the following pairs of atoms, state which youexpect to have the higher electron affinity: (a) Rb or Sr;(b) I or Rn; (c) Ba or Te; (d) Bi or C
- [Ne] 3s2 3P3 is a electronic configuration of Select one: of O phosphorous tion silicon O aluminium O nitrogen fvalence19 of 44 > © Macmillan Learning In the given three-dimensional molecular structure, the differently colored spheres represent different types of atoms. Write a molecular formula for this molecule. molecular formula: 4 R % 67 68 5 1 SPECIAL xº (g) ΔΣΩ λμπ X₁ X () 6 [] (s) Y (1) (aq) →>>> MacBook Pro The 11 7 U t CLR 8 K →>> 9 Rotate X You 9 Rotate Y ( 0 ☐C □H D Rotate Z 0 Zoom In P O Zoom Out Attempt A Label Atoms C8) Arrange affinity (less negative Na,S, and CI the following inorder of increasiing electron tomore negative).
- Group the electronic configurations of neutral elements in sets according to those you would expect to show similar chemical properties. 1s²2s²2p63s²3p6 1s²2s²2p²³: Set A 1s²2s²2p 3s²3pº: 1s²2s²2p³ 1s²2s²2p 3s ²3 pº 4s²3d¹⁰4p⁰: 1s²2s²2p 3s²3p³: Determine the chemical symbols for the neutral elements corresponding to the electronic configurations. Use proper formatting; letter case matters. Answer Bank 1s²2s²2p 3s²3 p4s²3d¹04p6 1s²2s²2p 3s²3p³ Set BWhat's the full electron configuration of O2-? O 1s2s2p4 O 1s2252p2 O 1s?2s2p63s2 O 1s22s2p65.) Electron Configurations for Ions: Supply the ground state electron configurations for the following ions. You many use the short-hand notation (e.g. Na*: [He]2s 2p°). (a) N (b) Mg*. (c) O (d) Sc* (e) Sn2+ (f) Ar 6.) Formulas of Ions: Predict the formulas of the most stable ions of the following elements (a) Na (b) Mg (c) S (d) Al (e) Br (f) P
- Write the charge and full ground-state electron configuration of the monatomic ion most likely to be formed from each atom: (a) CI (b) Na (c) Ca Which of the formed ions will be least stable? -- --(a) What are valence electrons? (b) How many valence electrons does a nitrogen possess? (c) An atom has the electron configuration 1s22s22p63s23p2. How many valence electrons does the atom have?Give three examples of ions that have an electron configurationof nd6 1n = 3, 4, 5,c2.