When the ionization energies (IE) of a series of isoelectronic atoms and ions in the second ow (that is, species that contain the same number of electrons, in this case three) are compared, the following relationship is observed (IE are in kJ/mol, and Z is the atomic number):| VIE = 18.4Z – 32.0 What is the expected ionization energy for Be*? A) 1730 kJ/mol 3) 23.2 kJ/mol C) 538 kJ/mol D) 41.6 kJ/mol E) 6.4 kJ/mol

The first five ionization energies (IE, through IE,) of a Period 4 element have the following 1 ll IE, IE, IE3 IEĄ IE, Make a reasonable guess about which element this is. Enter its chemical symbol below. kJ/mol

Which of the following atoms has the lowest first ionization energy? OSi Cs Са

Which one of the following pairs contains isoelectronic species? Ca2+, Cl- Br", CI Cr3+, V3+ O Ca?+, Br

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

O Macmillan Learning Consider an ionic compound, MX₂, composed of generic metal M and generic, gaseous halogen X. • The enthalpy of formation of MX₂ is AH = -987 kJ/mol. • The enthalpy of sublimation of M is AH sub • The first and second ionization energies of M are IE₁ • The electron affinity of X is AHEA = −351 kJ/mol. (Refer to the hint.) • The bond energy of X₂ is BE = 201 kJ/mol. Determine the lattice energy of MX₂. ΔΗ lattice = x10 = 125 kJ/mol. TOOLS = 677 kJ/mol and IE2 = 1.390 × 10³ kJ/mol. kJ/mol

Consider the following set of successive ionization energies: IE1=578kJ/mol IE2=1,820kJ/mol IE3=2,750kJ/mol IE4=11,600kJ/mol To which third-period element do these ionization values belong?

An element has the following electron configuration, [Ar]3d104s²4p3. This element is a _-- O transition metal O metal noble gas nonmetal O metalloid

Consider a hypothetical ionic compound AB (comprised of A* and B ions). Given the following enthalpy data and using a Born-Haber cycle calculation, predict AHiattice in kJ mol. AG) + Bs) - AB 4H = -384 kJ mol As) → Ag) ArH = 105 kJ mol B(s) - Bg) A,H = 101 kJ mol1 First ionization energy of Ag) = 501 kJ mol" Answes=? Electron affinity enthalpy of Bro (exothermic) = -348 kJ mol

F and F are both stable ions. What does this imply about the signs of the first ionization energy (IE₁) and electron affinity (EA) of F? IE₁ (F) 0, EA(F) > 0 IE₁ (F) = 0, EA(F) > 0 IE₁ (F) > 0, EA(F) 0