The value for astatine, At, is missing in this figure. To the nearest 100 kJ/mol,what estimate would you make for the first ionization energy of At?
The ionization energies of halogens are as given below.
Halogen | Ionization energy |
Fluorine | 1681 |
Chlorine | 1251 |
Bromine | 1140 |
Iodine | 1008 |
Astatine |
The ionization energies of astatine is not given. It is estimated to be 900 kJ/mol.
Halogen | Ionization energy |
Fluorine | 1681 |
Chlorine | 1251 |
Bromine | 1140 |
Iodine | 1008 |
Astatine | approx 900 |
We can observe that the ionization energy of halogen decreases by about 100 kJ/mol from chlorine to iodine. Hence, the ionization energy of Astatine will be about 100 kJ/mol lower than that of iodine.
The value for astatine, At, is missing in this figure. To the nearest 100 kJ/mol,what estimate...
A hypothetical element X has the following properties: First Ionization energy: 850 kJ/mol Second Ionization energy: 1700 kJ/mol Third Ionization energy: 13,999 Kj/mol a) if you were to react element X with oxygen, what would be the chemical formula of the resulting compound? b) write the balanced chemical reaction of X reacting with the oxygen to give the product from part a c) would you expect the product of the chemical reaction of X with oxygen to be basic, an...
39) A ficticious atom, Up, has the following ionization energies: 234 kJ/mol, 324 kJ/mol, 524 kJ/mol, 725 kJ/mol, 3187 kJ/mol, 4851 kJ/mol. What is the largest value of x expected in the following formula: UpCI, a) 1 b) 2 Explain the energetics of ionic bond formation and covalent bond formation When the two atoms sodium (Na) and chlorine (Cl) combine to make NaCl, one could imagine a number of steps that the atoms go through. For each of the steps...
The first three ionization energies for element Z are 320 kJ/mol, 640 kJ/mol, 10,200 kJ, mol. What is the likely charge of Z Z+ Z2+ Z3+ Z4+
The C1-C1 bond energy is 243 kJ/mol. Therefore the breaking of the bond between chlorine atoms should require the absorption of 243 kJ per mote of Cl_2 formed. should require the absorption of486 kJ per mole of Cl_2 formed should result in the release of 243 kJ per mole of Cl_2 formed. should result in the release of 486 Id per mole of Cl_2 form A reactive element with a relatively high electronegativity would be expected to have a relatively...
An atom with a first ionization energy of 939 kJ/mol, requires a photon of what maximum wavelength (nm) in order to remove a single electron from a single atom?
Consider the following information. • The lattice energy of NaCl is AHlattice = –788 kJ/mol. • The enthalpy of sublimation of Na is AHsub = 107.5 kJ/mol. • The first ionization energy of Na is IE1 = 496 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for NaCl(s). AH= kJ/mol
Consider the following information. • The lattice energy of KCl is AHlattice = -701 kJ/mol. • The enthalpy of sublimation of K is AHsub = 89.0 kJ/mol. • The first ionization energy of K is IE1 = 419 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for KCl(s). AHư= kJ/mol
Part C The ionization energy for rubidium is 403 kJ/mol The electron affinity for iodine is-295 kJ/mol. Use these values and Hess's law to calculate the change in enthalpy for the following reaction per mole of reagent: Rb(g) +I(g)Rb+ (g) +I (8), AH=? Express your answer with the appropriate units. ► View Available Hint(s) AH per mole = Value Units Submit
The first ionization energy, E, of a boron atom is 8.01 x 10 kJ/mol. What is the wavelength of light, in nanometers, that is just sufficient to ionize a boron atom? Refer to the values for constants.
Consider the following information. The lattice energy of LiCl is ΔH lattice = −834 kJ/mol. The enthalpy of sublimation of Li is ΔH sub = 159.3 kJ/mol. The first ionization energy of Li is IE 1 = 520 kJ/mol. The electron affinity of Cl is ΔH EA = -349 kJ/mol. The bond energy of Cl2 is BE = 243 kJ/mol. Determine the enthalpy of formation, ΔHf, for LiCl(s).