(a)
Interpretation:
The element that has a high
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
(b)
Interpretation:
The element that has a high electron affinity from Pm and F should be predicted.
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
(c)
Interpretation:
The element that has a high electron affinity from Ca and K should be predicted.
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
(d)
Interpretation:
The element that has a high electron affinity from Po and At should be predicted.
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
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OWLV2 FOR OXTOBY/GILLIS/BUTLER'S PRINCI
- For each of the following pairs of atoms, state which youexpect to have the higher first ionization energy: (a) Bi orXe; (b) Se or Te; (c) Rb or Y; (d) K or Ne.arrow_forwardUsing only the periodic table, arrange each set of atoms inorder of increasing radius: (a) Ba, Ca, Na; (b) In, Sn, As; (c) Al,Be, Si.arrow_forwarda) what is meant by the term polarizability? (b) Which of the following atoms would you expect to be most polarizable: O, S, Se, or Te? Explain.arrow_forward
- The following equations represent the chemical process to determine electron affinity of atoms. Identify the process expected to be the most exothermic (that releases the most energy). (A) F(g) + e– --> F– (g); (B) Cl(g) + e– --> Cl–(g); (C) Br(g) + e– --> Br–(g) ; (D) I(g) + e– --> I–(g);arrow_forward(a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic compounds in Section 2.7:K2O, CaO, Sc2O3, TiO2, V2O5, CrO3. (b) Name these oxides.(c) Consider the metal oxides whose enthalpies of formation(in kJ mol - 1) are listed here.Oxide K2O1s2 CaO1s2 TiO21s2 V2O51s2ΔHf° -363.2 -635.1 -938.7 -1550.6Calculate the enthalpy changes in the following general reactionfor each case:MnOm1s2 + H21g2¡nM1s2 + mH2O1g2(You will need to write the balanced equation for each caseand then compute ΔH°.) (d) Based on the data given, estimatea value of ΔHf° for Sc2O31s2.arrow_forwardUsing only the periodic table as your guide, select the mostelectronegative atom in each of the following sets: (a) Na,Mg, K, Ca; (b) P, S, As, Se; (c) Be, B, C, Si; (d) Zn, Ge, Ga, As.arrow_forward
- la) For each of the following pairs indicate which element you would expect to have the larger First Ionization Energy and which one would have the larger radius: (a) Ca and Cl; (b) Sn and Tl; (c) Ba and Bi (d) Fr and Cs b) For each pair indicate which Ion you would expect to have the largest Radius: (a) 0²- and O; (b) N³ and Mg²+ (c) Al3* and Al ne Elearrow_forward7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°arrow_forwardConsider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?arrow_forward
- (a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic K2O, CaO, Sc2O3, TiO2, V2O5, CrO3. (b) Name these oxides.(c) Consider the metal oxides whose enthalpies of formation(in kJ mol -1) are listed here. Calculate the enthalpy changes in the following general reactionfor each case:MnOm(s) + H2(g)----->nM(s) + mH2O(g)(You will need to write the balanced equation for each caseand then compute ΔH°.) (d) Based on the data given, estimatea value of ΔHf° for Sc2O3(s).arrow_forward(ii) How would you expect the second ionization energies for Na and Mg to compare? Explain using both a qualitative and quantitative (Slater’s rules) argument. (iii) Does your answer for (ii) correspond to what you know about the common ions formed by Na and Mg? Explain.arrow_forwardChoose the option in each that has the desired characteristic. Briefly explain each of your choices. (a) Larger Size? Si or Cl (b) Lower IE1? P or Po (c) Better Electron Affinity? O or F (d) Smaller Size? Br or Te2-arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning