Ok so I have this table on my book (I uploaded a picture here, can you see it?)And there are these questions beside the tableMy teacher answered them but I couldn't understand a word, the answers don't make sense to mePlease explain AS SIMPLE AS POSSIBLE.1) What are the values for the first, second, and third ionization energies for sodium and aluminum ANSWER: Ionization energy for Al is greater than Na because Al is smaller in size (Period Trend)2) Is it easier to remove an electron from a sodium (Na) or aluminum (Al) atom? From Na^+ or Al^+? From Na^2^+ or Al^2^+?ANSWER: 3rd IE gt; 2nd IEgt; 1st IE IE ionization energy By the way3) Which ion is more common? Na^3^+ or Al^3+?Answer : Al^3^+ is more commonNa^3+ is less common because it is breaking stability (Breaking complete energy level)Honestly the answers of the 1st and 2nd questions don't make sense to me at allAnd in the third question what does quot;breaking stabilityquot; mean?
Understanding ionisation energy trends will help with later topics like electronegativity and bonding, and properties of elements, so you do need to get your head round thisAll those numbers in the table represent the ionisation energy of the different elementsThat's the energy needed to remove one outer electronRemoving the outer electron from an atom produces an ion with a +1 chargeRemoving an electron from a +1 ion results in a +2 ion, and so onThat's why you have the first, second, and third ionisation energiesLooking at sodium and aluminium, it's easier to remove the first electron from sodiumSodium only has one electron in its outer shell, And a mere 11 protons in the nucleusAluminium has 13 protons, which attract the electrons more strongly, and hold them closerSo it takes more energy to remove the first electron from aluminiumHowever, once you make the +1 ion, all of sodium's remaining electrons are from the shell below(The next 6 are 2p electrons) Because they are closer to the nucleus, they are harder to remove than the outermost of aluminium's electrons, which are 3s electronsSo the second and third ionisation energies are higher for sodiumThe more electrons you remove, the harder it is to remove the next oneThat's because the thing you're taking it from has an extra + charge, and holds the electron more tightlyIt'll also be smaller in sizeThe smaller the atomic (orionic) radius, the harder it is to remove an electronIn question 3, they talk about breaking stabilityWhat it means is the inert gas configurationWhen atoms have a full outer shell, they are most stableThey don't accept any more electrons, and it's difficult to remove themNote that the inert gases have the highest first ionisation energiesOnce you strip off the outer electrons and are left with an inert gas configuration, the next ionisation energy is REALLY highShown in the chart where the stepped solid lines go acrossYou need a lot of energy to remove an electron from a full outer shell.
Foil made from a thin leaf of tin was commercially available before the aluminium counterpartIn the late 19th century and early 20th century, tin foil was in common use, and some people continue to refer to the new product by the name of the old oneTin foil is stiffer than aluminium foilIt tends to give a slight tin taste to food wrapped in it, which is one major reason it has largely been supplanted by aluminium and other materials for wrapping foodTin was first replaced by aluminium in 1910, when the first aluminium foil rolling plant, “DrLauber, Neher Cie., Emmishofen.” was opened in Kreuzlingen, SwitzerlandThe plant, owned by J.GNeher Sons (aluminium manufacturers) started in 1886 in Schaffhausen, Switzerland, at the foot of the Rhine Falls - capturing the falls’ energy to produce aluminiumNeher's sons together with DrLauber discovered the endless rolling process and the use of aluminium foil as a protective barrierFrom there began the wide use of aluminium foil in the packaging of chocolate bars and tobacco productsProcesses evolved over time to include the use of print, colour, lacquer, laminate and the embossing of the aluminium.
