The first five ionization energies (IE, through IE5) of a Period 6 element have the following pattern: II լօա/

Which element below will have an exothermic electron affinity?  Group of answer choices   Ar O Kr Xe none of these

Arrange the following set of elements in order of increasing first ionization energies. Ne N Li B C O

Arrange the following in order of increasing ionization energy: P, Ca, Cs, Ge, O, Ba

Out of these sentances , choose the one that is correct (there may be multiple correct statements) 1. Sodium has a bigger first ionization energy than potassium  2. sodium has a bigger atomic size than clorine 3.calcium has a bigger fist ionization energy than fluorine does 4. sulfur has a bigger electronegativity than chlorine

Write the complete electron configuration of the following and indicate the number of valence electrons in each. Provide the electron-dot structure of each. a) P(Z=15): b) Ar (Z-18)

Select all correct statements dealing with electron affinity. O It is the enthalpy change associated with the removal of an electron from a gaseous atom or ion. O It is the enthalpy change associated with the addition of an electron to a gaseous atom or ion. O In general the first electron affinity is: X(g)X(g) + e O In general the first electron affinity is: X(g) + e - Why are electron affinities usually exothermic? O the incoming electron experiences a repulsion from the nucleus, lowering the potential energy of the electron. O the incoming electron experiences an attraction to the nucleus, lowering the potential energy of the electron O the incoming electron experiences a repulsion from the nucleus, increasing the potential energy of the electron. O the incoming electron experiences an attraction to the nucleus, increasing the potential energy of the electron J E O étv NOV 11

Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization energy ionization energy required required Cs - Cs + e Se » Se - e Не — Не +e ? Ci Cl' + e Rb - Rb + e v ? Те — Те +e ? 1 (least) 3 (most)

Write the full electron configuration of the Period 2 element with the following successive IEs (in kJ/mol):IE₁=801 ,IE₂=2427 ,IE₃=3659 ,IE₄=25,022 ,IE₅=32,822

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