Use the following data and the Born-Haber cycle to calculate the first ionization energy (ΔH IE1) of K(g) K(s) → K(g) 89 kJ mol-1 Cl(g) + e– → Cl–(g) -349 kJ mol-1 K(s) + ½ Cl2(g) → KCl(s) -437 kJ mol-1 K(g) → K+(g) + e– ΔH IE1 Cl2(g) → 2Cl(g) 244 kJ mol-1 K+(g) + Cl–(g) → KCl(s) -717 kJ mol-1

Explain why the third ionization energy of Al is significantly larger than its first ionization energy. (2744 vs 577 kJ/mol)

The quantum numbers for the electron(s) in the valence shell of thallium (81TI) are: NOTE: the designation electron(s) with brackets around the s means that there might be only one: "electron" or there might be more than one: "electrons" O (6,1,-1,2) (6,1,0,½) (6,1,1,½) O (6,1,-1,12) O (6,0,0,±12) (6,1,-1,½) O (6,0,0,±½/2)

The graph below represents successive ionization energies (IEs) in kJ/mol for a particular element in period 3. Identify the element. 35000 30000 ll 25000 20000 15000 10000 5000 IE1 IE2 IE3 IE4 IES IE6 E7 E8 O Chlorine O Aluminum O Phosphorous Silicon O Argon Oxygen

Calculate the change in energy for the following processes: Na(g) + Cl(g) → Na^+1(g) + Cl^-1(g) Ca(g) + 2Br(g) → Ca^+2(g) + 2Br-1(g)

What element has the electron configuration [He]2s22p4? What element has the electron configuration [Rn]7s²5f¹2?

Briefly explain the errors in each of the three noble gas core configurations below and give the correct noble gas core configurations.   Potassium: [Ar] 4s2 Iodine: [Kr] 5s2 5d10 5p5 Chromium: [Ar] 4s2 3d4

1) How much energy (in MJ) is required to ionize 21.14 moles of hydrogen atoms?

Which of the following ions has the largest radius?      Br-     S2-     B3+     Mg2+     Li+

Using the figure below, write the electron configuration of the following Carbon (C) 1s22s22p2 Aluminum ( Al) 1s22s22p63s23p1 Chlorine (Cl) 1s22s22p63s23p5 Write the molecular formula resulted due to the sharing of the following, name the compounds. Carbon + Chlorine = Aluminum + Chlorine = What is the type of bond in each compound?