Question

could you help with these 2 questions ?

anions. Element Or has a greater electron affinity value Periodican Elements and Their Properties: 1. Element Ar has a 1s' electron configuration. 2. Elements Or, Me, and R form -1 anions. Element Or has a greater and than Me but a smaller electron affinity value than element R. 3. Elements Te, Es, T, and N are listed in order of increasing and N are listed in order of increasing ionization energy. These elements comprise the group of elements that form the +1 cations. 4. Elements Nt, I, At, Is, and Go compose the group of inert (noble) gases order of decreasing size. E, He, and Fa have an outer shell configuration of ns2 and tend to form +2 cations. The atomic number of Fa is higher than that of He but is lower than that or 6 6. Elements Pi, V, and Le are transition metals and are listed in order of increasing a radius. the group of inert (noble) gases and are listed in This puzzle was adapted from an article in Journal of Chemical Education, original citation is currently not available. Part III: Calculating AHºrx from Bond Enthalpies Using bond enthalpy data in the table below, calculate the enthalpy change for the following reaction. CH3-CH2-CH2-CH3(g) + / 02(8) CH3-CH2-O-CH2-CH2(g) Bond C- HC- CC= C0- 00-0TCOT Bond Enthalpy 414 347 614 204 498 358 (kJ/mol) 745

Answer 1

TABLE - 1(Original Periodic Table)

Group - 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 1 Period Be 328 349 324 190 295 Bh Mt Ag Lanthanides Eu Gd Tb Ho &185 Puli Am ** Actinides Cm Bk Cf Fm Es - -- - - - --- -

TABLE - 2 (Periodic Table for planet Periodus)

ILI IV е м о At He Fa I Pi IR v or Le I Me Es ь Ι Ол Te Nt

For the best comparison I have mentioned both the original periodic table and the new one as Table 1 and 2 respectively.

LET US FIRST GO THROUGH SOME BASICS

1.The horizontal rows are called PERIODS and veritical columns as GROUPS

2.Groups are numbered as roman and periods as numericals in the new table.

3.Atomic/Ionic radius of elements increases DOWN the group and decreases across the PERIOD

4.Ionisation Potential or Energy(IE) – Its is the energy required to completely remove an electron from a gaseous atom or ion. Ionization energy decreases moving down the group (increasing atomic radius).

5.Electron Affinity (EA) - The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion. It also decreases moving down the group (increasing atomic radius).

Now let’s start placing the elements using given data and cross referencing with above concepts

1. Ar has 1s configuration hence it is similar to H of Table 1. So we can place it in top left corner.

2. Or,Me and R forms -1 anions. Hence they can be compared to group 17 of table1 that is F ,Cl, Br. Further Or has greater Electron Affinity than that of Me but smaller than R , hence arranged accordingly as mentioned in point 5 earlier .

3. Ionisation Energy of N>T>Es>Te as given so we arrange according. Again the group can be compared with Group 1 of Table 1 which is H,Li, Na etc. Both these groups form +1 cations so placed accordingly as the first group in table 2

4. Atomic size is given as Go<Is<At<I<Nt and also the group belongs go inert gases. So we may compare it with group 18 of table1 and place as group number V in table 2 arranging as per given size order .

5. We know that outer shell configuration of group 2 of table 1 is ns2 , which is Be,Mg,Ca etc and they form +2 cations. Comparing the same with given data we place them in group II of table 2. Now atomic number of E>Fa>He and we know atomic number of elements increases down the group with size, hence such an arrangement is made.

6. Now if you notice carefully , group 3 to 12 of table 1 are all transition metals and they have such properties that show variable oxidation states, which varies according to their positions. They are naturally placed in the middle of the periodic table, so we did the same for ours.

Another reason to such placement is simply because there was only one vacant group left as all others were occupied. Now we arrange them as per atomic radius Le>V>Pi and place accordingly.

Hence your periodic table for planet Periodus is ready :-)