The first five ionization energies of an atom X are 6, 19, 28,120, and 154...

The first five ionization energies of an atom X are 6, 19, 28, 120, and 154 eV. Sugust what 3rd row element X is and give reasons for your choice.

Expert Solution

3rd row series contains;

Na Mg Al Si P S Cl Ar

First we will look for the difference in the magnitude of I.E

1st-2nd 2nd-3rd 3rd-4th 4th-5th

13 9 92 34

So as we can see on the above scale is that after removal of 3rd electron, a huge amount of energy is needed to remove the 4th electron from the shell.

Hence, number of valence electron present in the element = 3e

If we carefully look for the electronic configuration for above series, Al = 3s² 3p¹

As removal of an extra electron (basically from 2nd shell) needs a much higher amount of energy compare to 3rd (valence shell).

Our proposed element X is Aluminium

queen_honey_blossom answered 2 years ago

Table 4.1: Ionization Energies Complete the ionization energies for each element.

Table 4.1: Ionization EnergiesComplete the ionization energies for each element.ElementHHeLiBeBCNOFNeNaMgAlAtomic Number12345678910111213Ioni zationEnergies1st1312237252090080110872nd-52517298175723532856338833743952456214513rd--118151484946204578530160506122691077334th---21007622374757469840893719543105435th----37831944510990110231217713354136306th-----472775326713327151641523816613180207th------6436071330178681999920117217118th-------84078920382307025496256619th--------106434115380289323165310th---------1314321413623545811th----------15907516998812th-----------1893682. Explain how the successive (first, second, third, etc) ionization potentials change in each atom.3. For most atoms, there are one or two huge jumps in the ionization potential. Explain why these occur. In aluminum, explain these huge increases using the valence electrons.4. Explain any trend you observe when looking at only the first ionization energies of each of the 13 elements.

The ionization energies for a hypothetical element are listed below. Based on these ionization energies, identify...

The ionization energies for a hypothetical element are listed below. Based on these ionization energies, identify which group the element would be from on the Periodic Table. IE1 (kJ/mol) IE2 (kJ/mol) IE3 (kJ/mol) IE4 (kJ/mol) IE5 (kJ/mol) IE6 (kJ/mol) 600 1200 7300 9580 12,600 14,640

Explain the reason for the unexpected values of the first ionization energies of the group 3A...

Explain the reason for the unexpected values of the first ionization energies of the group 3A and group 6A elements, relating the apparent decrease from the previous group in terms of the orbital electron configuration. Explain how ionization energy relates to electronegativity, and explain that property. Be sure to define the two properties, and discuss their trends the relationship between each property and the size of atomic shells, as well as the reason for the numeric difference in electronegativity, both...

Select all true statements regarding Ionic Radii and Ionization Energies Group of answer choices first ionization...

Select all true statements regarding Ionic Radii and Ionization Energies Group of answer choices first ionization energy increases down the group because the larger atom has more positively charged protons the valence electrons of a cation experience a lower effective nuclear charge than in the neutral atom formation of an anion is accompanied by an increase in the size of the atom when atoms form cations the valence electrons are removed the larger the effective nuclear charge on the electron,...

The first and second ionization energies of two elements from the 3rd row of the periodic...

The first and second ionization energies of two elements from the 3rd row of the periodic table are given below. Element A: 738 kJ/mol and 1451 kJ/mol Element B: 496 kJ/mol and 4562 kJ/mol What is element B?

The first two ionization energies of an unknown element are as follows: 1st I.E = 496...

The first two ionization energies of an unknown element are as follows: 1st I.E = 496 kJ/mol 2nd I.E = 4560 kJ/mol Predict which group this element belongs to and write down the electron configuration of its valence electrons Q2. Explain why the first ionization energy of sulfur is inferior to that of phosphorus

The first ionization energies of the elements __________ as you go from left to right across...

The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table.

An unknown element has the following ionization energies:

An unknown element has the following ionization energies:Please answer all questionsIE1 = 570 kJ/mol IE2 = 1431 kJ/mol IE3 = 2023 kJ/mol IE4 = 10,521 kJ/mol IE5 = 13,288 kJ/mol a) Based on this information, how many valence electrons does this element have?Explain your answer.b) In view of your answer in part a), what charge would this element likely form, and would it be a metal or non-metal? (Assume it is not a metalloid). Explain.

The following table gives the first ionization energies for the second period elements. Using electron configurations,...

The following table gives the first ionization energies for the second period elements. Using electron configurations, explain why boron and oxygen have lower ionization energies than would be expected based on the general trend. Element Li Be B C N O F NE IE (KJ/mol) 520 899 801 1086 1402 1314 1681 2081

Question 1: a. The first four ionization energies of an element are approximately: 738 kJ mol-1,...

Question 1: a. The first four ionization energies of an element are approximately: 738 kJ mol-1, 1450 kJ mol-1, 7.7 x 103 kJ mol-1, and 1.1 x 104 kJ mol-1. Which family (group) of elements does this element belong? Explain. b. In a photoelectron spectroscopy experiment the kinetic energy of the ejected electron from a potassium atom is found to be 5.34 x 10-19 J using a UV source of wavelength 162 nm. Calculate the ionization energy. i. It is...

Question