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"Chemistry of Group Elements: Videos"

00:00:02 [Music] As a part of my lecture series on the chemistry of main group elements, today I would like to drive our attention to the chemistry of group one elements that is alkalary elements. You all know that electronic configuration of alkaly metals is ns1. uh that means they have only one s electron in their veence shell and that since these electrons are loosely held one can readily remove it and hence all these alkaly metal elements show plus one oxygen state and you can see from here we have lithium sodium potassium


00:


00:57 rubidium cium and franchium lithium shows little different chemistry compared to rest of the elements in the group due to its smaller size and with water they readily form hydroxides which are strongly alkaline in nature and hence they are called alkaline metals. Sodium and potassium are abundant whereas lithium, rubidium and cium are less abundant and they are in trace amounts and franchium is highly radioactive. uh you can imagine by just looking into the half-life of one of the isotopes that is 223 franchium that has about 21


00:01:42 minutes that indicates the extent of radioactivity franchium source as a result not much chemistry one can think of about franchium chemistry of lithium is little different from those of other group members as I said going to smaller size but lithium shows similarities to magnesium in terms of its properties usually known as diagonal relationship. I would discuss about those aspects at the end of this series of this lecture and sodium, potassium, calcium and magnesium ions are in large proportions


00:02:18 in biological fluids. In fact, they perform very very important biological functions such as maintenance of ion balances and nerve impulse conditions. Okay. and loosely held S electrons can be readily removed and hence they have low ionation energy or ionation enthalpies and all are most electropositive elements in the periodic table. In fact, alkaly metals are most electrol electropositive among the elements in the periodic table. They readily form M plus ion and obviously M plus ion size is much smaller than the M


00:02:58 ion as a result of shrinkage of its size due to the removal of that electron and hence the increase in the effective nuclear charge. Atomic and ionic radi increases down the group as the size increases. In fact, they have the largest size in their respective periods or rows and ionization enthalpy decreases down the group due to the increase in the size. And due to the increase in the size, hydration enthalpy also decreases down the group. And lithium plus ion has larger hydration enthalpy and CCM shows minimum hydration


00:03:37 enthalpy. And the order follows this uh sequence. This is the order of hydration enthalpy. uh lithium plus has maximum degree of hydration and hence all lithium salts are hydrated. For example, if you take lithium uh chloride, it is solvated with two molecules of water. Okay. And due to the presence of only one veence electron, metal metal bonds are very weak and hence they are soft metals. That means one can easily cut using a knife. And the other interesting aspect of these alkaline metals is they


00:04:54 import characteristic color to an oxidizing flame. This is essentially due to the exitation of s electron to the p orbital. And of course when we talk about electronic transitions we have two important selection rules that is electrons within the same orbital cannot be transmitted that is it is prohibited that means S2S transition P2P transition D2D transition is forbidden whereas S2P P2 D2F are allowed they are called leopard allowed and another selection rule is spin selection rule. So during


00:05:31 electronic transition the spin should not change. This is quite opposite to the selection rule that we use in the case of nuclear magnetic resonance where the spin should change that is delta s equals plus or minus1 whereas in case of electronic transition delta s equals zero. That means essentially this flame test the color comes as a result of NS1 electron getting promoted exited to NP1. So as a result of this one, what happens when these electrons are coming back to the ground state? They emit radiation in


00:06:18 the visible region. As a result, color can be seen for the flames. For example, you can see lithium shows crimson red color. Sodium shows golden yellow color, potassium shows violet color and rubidium shows red violet and cium shows blues. In the respective wavelengths I have given here. For lithium it is 670.8. In case of sodium it is 589.2 in case of potassium it is 766.5. And in case of rubidium and CCM it is 780 and 455.5 nanometers. The color also you can see from the slide that is shown there.


00:07:01 So when we talk about the chemical reactivity we can think of few things that comes to our mind. First of all, how it reacts with air. Air means it's quite obvious that how they are going to interact with oxygen. Next, how they interact with water. And then what kind of interaction one can anticipate when it is treated with hydrogen, nitrogen or halogens. And lastly, we can also look into their interaction with organic moities and also behavior in liquid ammonia. Okay. So, let us uh look into the


00:07:34 chemical reactivity here. uh due to the high reactivity uh of these positively charged ions they are exposure to air they tarnish due to the formation of oxides which in turn react with moisture to form hydroxides. For example, if we take lithium, it readily reacts with oxygen to form lithium oxide. This is called oxide. We have O2 minus. And sodium reacts with oxygen to form peroxide. not oxide. Other heavier elements react with oxygen to form super oxides. where M is potassium, rubidium and CCM.


00:09:01 So you can see from this slide uh compounds and their interaction with oxygen and the resulting compounds. For example, lithium gives lithium oxide and here anion is O2 minus that is oxide and and the hydrarolysis product that means when they are treated with water what would happen in case of lithium oxide O minus hydrarolysis sodium lithium hydroxide is formed in case of sodium peroxide is there as a result when it is reacted with water it forms hydroxide and then hydrogen peroxide in case of


00:09:37 potassium rubidium and cium we get super oxide. So super oxide on treatment with water gives hydroxide, oxygen and hydrogen peroxide. So let me write those uh reactions. It is for this reason they are called alkaly metals. Na2o plus H2O gives 2 NaOH. Similarly, sodium peroxide reacts with one equivalent of water to give initially sodium oxide plus H2O2. And this Na2O again reacts with another molecule of water to give sodium hydroxide. And also they react with nitrates to give the corresponding oxides.


00:10:47 In this case N2 nitrogen will be liberated. And these alkali metals can also react with wone to form wenate salts. So these wenate salts have a unpaired electron. As a result all wasinate salts are paramagnetic in nature. Similar reactions one can anticipate when they are treated with sulfur and in in those reactions they form sulfides and polyulfides of composition M2 SX. Let me write few reactions. Sodium on treatment with sulfur gives sodium sulfide. This sodium sulfide on further treatment with elemental sulfur.


00:12:01 Similarly, sodium can also react with the tourum to give the corresponding toleres. It it gives Na2 TE2 plus Na2 TE3. CCM also reacts in a similar fashion to give CCM sulfide. Of course, further treatment of CCM sulfide with sulfur, elemental sulfur leads to the formation of CS2 S5. So these are the some these are some of the reactions uh with oxygen as well as sulfur. They reacts with almost all halogens to give the corresponding halides and alkalates are well-known compounds. For example, sodium


00:13:10 chlorides, potassium chloride, all combinations one can think of. Uh, CCM chloride, CCM bromide, CCM hydide have the same structure and sodium chloride has a different structure. In case of CCM chloride structure, the cation and annions both are eight coordinate that you can see from the structure I have shown on the right side. In NaCCl there are six coordinate. Both are acted coordinate. sodium and chlorine with a ratio of 1 is to 1. Okay. So you can see and simply by looking into the radius ratio that mean


00:13:51 radius of cation alkal metal cation and allied annions one can predict the nature of the structures and the structure adopted by a salt M plus X minus can be readily predicted considering the following rule. For example, if you consider the radius ratio that is R + to R minus and if it falls in the range of.25 to 414, they assume zinc sulfide asparate structure. On the other hand, if they have in the range of 414 to 0.732, they have sodium chloride structure. And if the radius ratio is greater than


00:14:35 0.732, they assume CCM chloride structure. Uh radius ratio rules provides a reasonably general means of assessing the likely structure adapted by an ionic solid but gives incorrect predictions usually when there is a significant coalent bonding. For example, in case of lithium hallides, there is some coalent character is there. It's not purely ionic. In those cases probably this uh method of prediction may not be correct. And also when there is a borderline in case of radius ratio for example if the radius ratio falls in


00:15:17 the range of 414 to 420. So it it can have either zinc sulfide structure or sodium chloride structure. Same thing is true in between sodium chloride as well chloride. So ionic radi not known accurately. So the values vary with coordination number since ionic radi essentially varies with the type of other ion we have in its vicinity. Lithium reacts with nitrogen to form nitrate. It is very interesting to look into lithium nitrate. The salt is highly stable because of very high latis energy from the very small lithium plus and


00:16:05 highly charged N3 minus ions coming together. So, Li plus is highly charged and smaller in size and N3 minus is highly charged and also smaller in size and in fact N3 minus is formed by breaking a very strong NN triple bond having energy of about 941 kiloj per mole. Essentially the combination of these two gives the energy that is sufficient to break this NN triple bond. And of course uh lithium nitrate is highly reactive and it readily underos hydraysis on treatment with water or on exposure to moisture.


00:16:50 It forms lithium hydroxide and ammonia. So just as sodium hydroxide is a base in water, sodium amide is a base in liquid ammonia because it is able to deprotonate acidic organic molecules especially when they have a acidic proton bound to carbon. One can easily deproinate it. That is the reason the sodium amids are widely used in organic synthesis to generate sodium salts. You take a typical alkali metal treat with ammonia. They form amides of this type or one can get amide plus H2 Of course uh if you take any of these


00:18:11 alkaly metals especially if you take sodium and put into liquid ammonia the color turns blue because of the solvated electrons. What happens there is when the sodium is put into liquid ammonia. So it forms n plus and these electrons are released. So now ammonia what happens because of the polar bonds they have it generate delta minus on nitrogen and delta plus positive charge on hydrogen. So now this sodium will be attracted uh towards uh nitrogen and whereas electrons will be coming towards this one. So because of


00:18:59 this salivated electrons the color is blue in nature and how it activates a acidic hydrogen in carbon can be seen from this reaction. For example, if you take a typical hydrocarbon where H is slightly acidic and treat with sodium amide, it readily forms a sodium salt with the formation of ammonia. So now this can be used in various organic synthetic reactions. So all these alkali metals reacts with hydrogen to form the ionic hydrides. So at 701073 Kelvin lithium reacts whereas rest potassium reacts at 673


00:20:19 K for potassium and other higher elements. Since lithium is very smaller in size, okay, it requires little higher temperature to induce reaction with hydrogen molecule to form metal hydride or lithium hydride. Whereas in in the case of sodium potassium, one can perform this reaction at 673 Kelvin to form the corresponding metal hydrides. And these metal hydrates are also very sensitive towards water and they readily undergo hydraysis to form the corresponding base hydroxide with the liberation of hydrogen.


00:21:12 And this sodium hydide can also activate acidic CH proton similar to sodium amide. For example, sodium hydide on treatment with CH3 SOC3 dimethile sulfur oxide to form a salt of this type. So H anion is a strong base can be used to deproinate organic molecules as I said containing relatively acidic CH groups. How about the reaction of alkali metals with carbon? So they react with uh carbon species to form the corresponding carbides. Let me write a couple of reactions. For example, uh acetylene on treatment with


00:22:21 alkaline metals liberate hydrogen gas to form the corresponding acetylide. Of course, which in turn react can react with another mole of metal to give fully substituted or this reaction. So, ethane acts as an acid. You can see this is deeprotonated and it gives the corresponding carbide. And of course extensive organic chemistry is associated with alkaline metals especially with lithium and organoliththium reagents are extensively used in organic synthesis and they find numerous applications in in all aspects


00:23:24 of organic transformations and these lithium readily reacts with alkalides in dry hydrocarbons. You should remember nonacqueous medium when we are reacting all these alkali metals with organic moities we should not use wet solvents we have to use highly dry hydrocarbons. So reaction of lithium with RX a typical alkalhalide in a dry hydrocarbon like benzene hexane etc. Or one can also use ethers like diilether or tetrahydrofuron. It forms R LI plus LI X comes out. This LIX will prosperate depending upon the


00:24:17 nature of the solvent we are using and then can be filtered off and our LI remains in solution that can be used for further synthetic utility. Okay, this organo lithium reagents are extensively aggregated together in the solid and in solution. For example, if you consider methile lithium, how to make methile lithium? Methile chloride when it's reacted with two equivalents of lithium. Methile lithium is formed and lithium chloride is formed. So lithium chloride can be taken out. This methile lithium when you solidify or


00:25:04 when you crystallize it, it does not exist in monomeic form. It exists in tetromeic form. Alkyhides, there are several ways to make them. One of the methods is treatment of lithium metal directly with alkyle halides in dry hydrocarbon. or ethers such as dethyl ether or tetrahydrofuron etc. The reaction leads to the formation of argan lithium reagents with the precipitation of lithium helide. So here one can conveniently use chloro brmo or even iodo derivatives. So these organo lithium compounds are


00:26:07 usually extensively aggregated together in the solid state and solution state. The reason is very simple. If you just look into a typical RI say CH3 Li or methile lithium here we have one bond between carbon and lithium and the rest of the surface of lithium is exposed since lithium is coordinatively unsaturated and also you know the fact that lithium can get solvated. So in absence of any other Louis bases or donor solvents what it does is it try to undergo association to make some sort of electrondeicient bonds to give


00:26:57 temporarily coordinative saturation. This methile lithium exists as a tetrome. So how this tetrome gives extra stability we can look into it. If you just recall your understanding of the methane using veance bond theory. So we have here methane uh you know the concept of hybridization and before methane molecule is formed carbon having s2 p2 electronic configuration. What it does is it promotes the s electron to the p orbital to have this kind of situation. Now we have one electron in S and three


00:27:46 electrons in P orbital. And these four electrons orbital combine together to generate new kind of hybrid orbitals called sp3 hybrid orbitals and each one having one electron. So now this four sp3 hybrid orbitals combine with one s one orbital of hydrogen to form four CH bonds. Okay. So now in case of CH3 what happens? We have C H3 and one with one electron is there. And of course this one very similar to another hydrogen. It combines with lithium 1s electron to form CH3 LI. So now if you just look into it


00:28:48 S of lithium combined with sp3 of carbon to form methile lithium. It is similar to methane but lithium is not coordinatively saturated in in the tetramic form. What it does is it has a structure like this. So it assumes a cubain type structure. So that means uh in cubain we have eight corners are there. Each corner is occupied by methile groups as well as lithium groups. That means alternate corners are occupied by lithium and methile groups. So if you see uh the position of four lithium atoms that can


00:30:11 be compared to a typical a tetraedron. So now in this one in tetraedrron we have four triangular faces are there. You can consider any of these triangular faces and each triangular faces now interacts with one sp3 from CH3 and this eventually gives a cubain structure and and of course it's not exactly regular cubain it it it's a distort started cubain. So here if you just look into it since four lithium atoms are there in the tetraedron and each one has one electron. So that means for one triangular phase only one of the


00:31:16 lithium atoms can donate one electron. So that means essentially when three lithiums are there in this particular triangular phase three are there one of the lithium gives. So that means basically here you have four centered two electron bond. That means four centered two electron bonds are formed. They are highly electron deficient. However, it gives some stability to methile lithium. And this how it looks like methile lithium. And you can see the acru structure of methile lithium. You can clearly see that is in purple is lithium


00:32:01 atom and this methile groups are there with the CH shown coming out of the cube and this is how the association gives some stability in solid state. Of course uh when you take methyl lithium and add donor solvents like pyodine tetromethyl ethylene diamine this association breaks up and you get individual entities coordinating to some of these louisis bases and alkaly metal complexes form relatively very few complexes with neutral liants. Uh lithium salts are more soluble in solvents such as ethanol, ethers than those of other


00:32:42 group members and lithium is four coordinate whereas sodium and potassium are six coordinate in nature. So we can look into some simple coordination complexes here. As I said stable complexes can be formed by multi-ented liants uh which can encapsulate the metal ion. For example, if we have like EDTA, ethylene diametra acidic acid. Of course, there we are not using for lithium. Of course, in case of calcium, we are using that one. But here in this case, extensively we use a multi-ented liance called


00:33:20 chrome ethers and cryptants. Then you may be asking what is chron ether and what is crypt? They nothing but the poly ethers. I would come to that one later. For example here as I said lithium can be tetracoordinated. So lithium readily forms tetramine lithium complex and and these are all the crown ethers. In this crown ether you can see variable number of oxygen atoms are there and it is a poly ether and since this is not planer and when it is puckered it appears like crown and hence the name crone ether and the first one


00:34:04 is 18 crown six and the next one we have along with oxygen we also have nen donor atoms are there this is called krypton and in this one the krypton left hand uh in the bracket square bracket 2.2.2 two is given that essentially represents between two nitrogen how many oxygen atoms are there and each uh line if you consider that way you have two oxygen two oxygen and two oxygen totally six oxygen are there uh in the palm of that alky chain and hence the name krypton 222 and if we have in between


00:34:48 two nitrogen atoms we have three oxygen atoms it can be krypton 3 33 3 or if you have 2 32 it can be called 2 3 4 depending upon the number of oxygen atoms the whatever the numeral we are showing that changes and here how it is 18 crown 6 I will show you this one let's write uh they are all linked by ethylene groups If you start counting from here, 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18. So that means there are 18 atoms in the ring and so it is a 18 crown and six oxygen atoms are there. So this


00:36:01 is how one can write the name for these crown ethers and these crown ethers depending upon the the size and how many oxygen atoms are there they can comfortably encapsulate these alkali metals to stabilize them. and cryptand if you take again cation if you take this one and treat with a cryptand of course it's always reversible since this is a neutral liant the whole complex will be kionic in nature okay stability of these complexes increased inreases if the size of M plus matches the cavity size. That means if


00:36:54 if whatever the cavity that that is generated in case of these crown ethers if it is fits exactly the size of the cation then those complexes are more stable. So that's the reason whenever we are using some of these cations to be stabilized by crown ethers we are taking the right size uh crown ethers that you can see from this slide. uh for encapsulating or trapping lithium you need a smaller crown ether that is 12 crown 4 and sodium is little larger so one should use 15 crown 5 e crown ether in


00:37:37 case of potassium one can comfortably use 18 crown 6 the one I wrote here and in case of rubidium because of smaller bigger size and also it's Coordination number also more one can use 21 crown 7 and CCM is the largest among all elements in the periodic table. Uh leaving franchium. uh one can use 24 crown 8 ether to capture CCM and you can see how this encapsulates can be show seen from that the last uh structure I have shown where potassium is encapsulated by 18 crown 6 o ether other oxygen is


00:38:25 opposite sides so that you may not be able to see it similarly krypton can also encapsulate these cations and let's look into the similarities between lithium and magnesium. I was telling you in the beginning lithium rather showing similarities with its own group predecessors it shows much similarity with the next group okay uh element magnesium that is diagonally opposite to that one. So when we come across this kind of relationship uh in chemical and physical behavior we call them as diagonal relationship. And


00:39:05 lithium shows many similarities to magnesium rather than to the heavier alkal such as sodium or potassium. And if you consider lithium that readily forms uh lithium oxide and similarly magnesium forms magnesium oxide and whereas sodium forms sodium peroxide. So that means there is a difference in the chemistry of lithium and sodium but similarity is there between the lithium and magnesium and similarly if you take lithium carbonate and heat it forms lithium oxide and CO2 is liberated. Similarly, magnesium carbonate on


00:39:43 heating it forms magnesium oxide and carbon dioxide is liberated. Whereas sodium carbonate is quite resistant and it is stable. And in order to decompose that one to form sodium oxide, you have to use very high temperature. And when we look into the complexes, lithium forms four coordinated complexes. Similarly, magnesium also forms four coordinated complexes. Tetramine lithium cation is known. Similarly, tetramine magnesium cation is also known. And let's look into some uses of alkaline metals and their compounds. In fact, we


00:40:20 find extensive utility of most of the alkaly metals and most of their compounds in one or the other aspects in day-to-day life. For example, lithium is used in metal alloys with lead that is called white metals and they are used in bearings for motor engines. And also when lithium is mixed with aluminium in a in a definite proportion that alloy is used in aircraft parts and with magnesium they are used in armor plates and of course in thermonuclear reactions lithium is used and also in electrochemical series and dry cells. We


00:40:56 know that lithium is extensively used and sodium lead alloy in making tetromethile lead and tetrathile lead and earlier uh in order to increase the utility of petrol for better combustion. Tetrathyl lead used to be added as a additive and it was called as anti-in reagents. Nowadays because of the toxicity of tetraal lead uh is no longer used as additive in petrol and that's the reason if you go and see in the petrol banks you can see the writing unled petrol. So that means liquid sodium usually has a


00:41:40 coolant in fast breeder nuclear reactors and potassium plays a vital role in biological systems along with sodium and potassium chloride is used in fertilizers and also potassium hydroxide sodium hydroxide are also used in the manufacturer of soap detergents and other things and also to absorb carbon dioxide and CCM is used in photoelectric cells and we come across many more utilities probably you can look into any standard textbook to find out more applications of alkaline metals and their compounds and sodium carbonate. Uh


00:42:18 that's also called washing soda. Okay. And sodium bicarbonate Na H CO3 is baking soda. It reacts with acidic compounds to release carbon dioxide which causes expansion of batters if it is used in the bakery products giving characteristic texture and grain for fermentation and all those things we use it. How that happens? sodium bicarbonate and heating to uh modest temperature it forms sodium carbonate and liberates carbon dioxide. This is responsible for the expansion of the batter in bakery


00:43:19 products. And now you can ask yourself a question related to alkaly metal elements. For example, what is the oxen state of sodium in sodium oxide or sodium peroxide? In the gas phase, the alkali metals form dimer M2. Then draw a MO diagram for M2 molecule. That means how to draw a MO diagram for M2 molecule. And how would you synthesize sodium perchlorate starting from sodium carbonate and also cescium per chlorate. And if you assume the following facts that lithium plus has 74 and ccm has 167 pometer and fluoride has 133 and iodide


00:44:11 has 222. So predict what structures type will be adopted by the following alkaline metal salts for example CCM hydide and lithium fluoride. So we know the radius ratio rule and also for a particular ratio what is the standard structure it prefers to adopt under normal circumstances once when we look into those things we should be able to tell. Let us try to do one at a time. Okay. So what is the oxy state of? So of course whether you take sodium oxide or sodium peroxide the oxy state of sodium is + one.


00:44:53 And and the next question uh how would you synthesize? I would come back to the MO diagram for M2 molecule later. Let us look into the preparation of sodium uh per chlorate starting from sodium carbonate. So you can take sodium carbonate and treat this one with perchloric acid. It gives sodium perchlorate with the formation of CO2 and H2O. So this is how starting from sodium carbonate one can prepare sodium per chloride and since cesium chloride and and it salts are sparingly soluble one can think of a precipitation reaction


00:45:47 that means cium chloride on treatment with sodium per chloride it forms cm ium perchlorate plus sodium chloride. Of course, one can also here it respirates out. So this can be separated. One can also start from cium carbonate way similar to sodium carbonate. Treat cmium carbonate with perchloric acid. It gives CCM per chlorate and CO2 plus H2O comes out. or one can also start from CCM hydroxide. So in this case along with CCM per chloride water will be formed and there's no formation of carbon dioxide.


00:46:49 So now uh try to look into the problem I gave you to find out the type of structure cium chloride and lithium fluoride would have. So look into that radius ratio. Let me write for uh so now what is given is u ccm iate it is 167 by 220 so it gives 76 and similarly in case of lithium fluoride the same ratio will come to this 74 for lithium and 133 for fluoride this comes around.56. So now if you compare so this value is 076. So that means it comes very close to 0.732. So it will have that means cium iodide


00:47:57 has a structure similar to cesium chloride. And similarly lithium fluoride has a structure very similar to it comes 56 between 0.414 414 to 0.732 it comes Ncl structure it has a NCL structure so about in the gas phase the combination to give M2 MO diagram so MO diagram writing is very easy uh n S1 one electron is there you assume this is where this atomic orbital you consider another ns1 from another alkaline metal and both have one electron each. So now they combine together to form a bonding and


00:48:44 anti-bonding you call sigma. This is sigma star. And here both electrons will there. And this is how the mo diagram can be written for a typical M2 molecule very similar to hydrogen molecule. So uh one can readily write this kind of MO diagrams just by looking into the valence electrons and their right combination can give ammo diagrams for the molecules we are looking for. So this completes about alkali metal chemistry and four important aspects I had discussed. When we talk about chemical reactivity, one


00:49:39 can look into the reaction with air that means oxygen and reaction with water. how it reacts with water and then how it reacts with hydrogen and then how it reacts with halogens because whatever the compounds we come across will be either oxides or hydrides or halides and then one should also look into how one can make a element to carbon bond that means argonometallic chemistry. So here I showed one method of formation of organo lithium reagents. uh one can take alkyhalide and treat with two equivalents of lithium and presspirate


00:50:20 out one equivalent of lithium halid and form one equivalent of organo lithium compound and organoliththium compounds and these reactions has to be carried out strictly under inert atmospheric conditions using very dry solvents because of their tendency to undergo hydraysis to form lithium oxide and eventually more water is there lithium hydroxide and organoliththium ium chemistry is very extensive and that is also very similar to grian reagents. Probably I would give more information about the utility of organo


00:50:54 lithium reagents when I discuss about the organometric chemistry of main group elements. Let me summarize the chemistry of group one elements. So group one elements and their compounds follow the periodic properties and trends with very little or no variations. And as you know alkali metals are highly reactive and form basic oxide oxides and water soluble halides containing M plus cations. The group oxidation state is plus one. So they all form M plus cations. Among alkaly metal compounds whether we consider hydrides, oxides,


00:51:32 halides or even argonometric compounds ionic properties dominate the chemistry. Uh except in case of lithium because of its smaller size all compounds of lithium have some coalent character. Nevertheless, the rest of the elements uh ionic property dominates and in case of lithium it resembles more of magnesium uh due to the diagonal relationship that means the chem chemistry of lithium can be uh compared with the chemistry of magnesium. So this completes the discussion on uh group one elements. In my next lecture I'll be


00:52:18 dealing with the chemistry of group two elements. Thank you very much.

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NEET Class 11 Chemistry NCERT Chemistry of Group Elements

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In this video, we will cover:

1. Physical Properties of Group 1 & Group 2 ( Melting & Boiling  Point ,Density , Conductivity ,Flame test, Photoelectric effect )

2. Standard Oxidation Potential (Group 1 & Group 2 )

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11. NEET The s-Block Elements Concepts

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22. Class 11 Chemistry The s-Block Elements NEET Concepts

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28. The s-Block Elements NEET for 2026-2027

29. The s-Block Elements NEET Coaching

30. NEET Concepts NCERT Class 11 Chemistry

27. Neetbharath.in Tutorials NEET pe Jeet

28. FREE NEET The s-Block Elements

29. FREE of Cost NEET Coaching 2026-2027

30. The s-Block Elements NEET 2026-2027

31. Inorganic Chemistry for NEET

32. Inorganic Chemistry NEET

 

Chapter 10 The s-Block Elements Class 11 NEET Chemistry deals with:

The elements in which the last electron enters the outermost s-orbital are called s-block elements. s-block has two groups (1 and 2).

Diagonal Relationship

  •     The similarity in the properties of definite pairs of diagonally adjacent elements in the second and third periods of the periodic table is called diagonal relationship.
  •     In s-block elements Lithium is the first element of group 1 whereas Beryllium is the first elementsof Group 2.
  •     Some of their properties do not match with the properties exhibited by other elements of their group.
  •     Instead their properties resemble the properties of the second element of the following group due to the similarity in ionic sizes and /orcharge/radius ratio of the elements.
  •     Consequently lithium and magnesium have similar properties whereas Beryllium and Aluminium exhibit similar properties.
  •     This relation is called diagonal relationship.

Similarity of beryllium and aluminium

  • The charge/radius ratio of Be2+ ion is nearly the same as that of the Al3+ ion and hence exhibit similar properties.
  • Both remains unaffected by acids due to the presence of an oxide film on the metallic surface.
  • Hydroxide of both the elements dissolves in excess of alkali to produce beryllate ion[Be (OH)4]2– and aluminate ion [Al(OH)4]–
  • Chlorides of both the elements are soluble in organic solvents and act as strong Lewis acids
  • The ions of both the elements have strong tendency to form complexes like BeF42–, AlF63–.

 

NEET Class 11 Chemistry NCERT Chapter 11 The p-Block Elements

In this video, we will cover:

1. PYQs NEET The p-Block Elements

2. The p-Block Elements PYQs

3. NEET The p-Block Elements Previous Year

4. Questions from NEET The p-Block Elements

5. Chemistry NEET Chapter 11

6. NEET Class 11 Chemistry

7. CBSE Class 11 Chemistry The p-Block Elements NCERT Chapter 11 NEET

8. NEET Mains Concepts Chemistry

9. The p-Block Elements NEET Concepts for 2026-2027

10. The p-Block Elements NEET Concepts 2026-2027

11. NCERT Class 11 Chemistry Chapter 11 NEET Concepts

12. The p-Block Elements NEET for 2026-2027

13. NEET Chemistry Question

14. The p-Block Elements NEET

15. The p-Block Elements NEET Coaching

16. The p-Block Elements NEET 2026-2027

17. NEET from Chapter 11 Class 11 Chemistry

18. Neetbharath.in Tutorials NEET pe Jeet LH Chemistry

19. NEET Class 11 Chapter 11 Chemistry The p-Block Elements

20. NEET The p-Block Elements Chapter 11 Class 11 Chemistry

21. Class 11 Chapter 11 The p-Block Elements NEET Coaching

22. The p-Block Elements NEET Class 11 Chapter 11 Chemistry

23. FREE NEET The p-Block Elements

24. FREE of Cost NEET Coaching 2026-2027

25. NEET Chemistry Practice Questions

26. Neetbharath.in Tutorials NEET Chemistry

27. The p-Block Elements NEET 2026-2027

28. NEET Chemistry Class 11 Practice Questions

29. Class 11 Chemistry Chapter 11 The p-Block Elements NEET Questions

30. Chapter 11 Class 11 Chemistry NEET

31. The p-Block Elements Class 11 Chemistry NEET

32. Neetbharath.in Tutorials NEET pe Jeet LH Chemistry

 

Chapter 11 The p-Block Elements Class 11 NEET Chemistry deals with:

  • P block is present at extreme right of periodic table.
  • It has general electronic configuration ns2np1-6.
  • It includes solids, liquids and gases.
  • The elements of this group are metal, non- metal and metalloids.
  • If we move along period in periodic table, non-metallic character increases and if we move down the group, the non-metallic character decreases.
  • In this group: As we move down, the lower oxidation state becomes more stable due to” Inert pair effect.”

Inert pair effect : It is “reluctance in the participation of s electrons in bond formation due to poor shielding effect by d and f orbital .As a result, s electrons are tightly bounded .

1st member is different from its congeners due to:

  • Small size
  • Highest ionization energy.
  • High electro-negativity.
  • No vacant d orbital.
  • They show maximum co-valence of 4 because of no vacant d orbital.
  • First member also has tendency to form multiple bonds because in them p can takes place (because of its small size) .

Group -13

This group includes following elements:

  • Boron (B)
  • Aluminum (Al)
  • Gallium (Ga)
  • Indium(In)
  • Thallium (Tl)

Boron occurs as Borax, kernite, orthoboric acid etc. Aluminum occurs as bauxite, Cryolite, Corundum etc.

General electronic configuration of this group: ns2np1

 

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Class 11 Chemistry Chemistry of Group Elements NCERT


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  1. - Retention and Memory: Regularly reviewing and revisiting the material of Class 11 Chemistry Chemistry of Group Elements helps reinforce the concepts in student's minds. It strengthens memory pathways, making it easier to recall information during exams and beyond.
  2. - Consolidation of Knowledge: When you revise notes, you are essentially consolidating your knowledge. This means connecting new information with what you already know, making the overall understanding more robust.
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