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reaction between fluorine and hydrogen is an explosive reaction even when it is cold and dark.  (II) The reaction between CHLORINE and hydrogen is an explosive reaction but only when it occurs in the presence of heat and light.  (iii) The reaction between BROMINE and hydrogen is a little less explosive and this explosion occurs only when exposed to flames. (iv) There is only partial reaction happening between Iodine and hydrogen ACHIEVING the STATE of chemical equilibrium .Hence, the order of reactivity would be HF > HCl > HBr > HI.

TION :- GIVE the name of TWO metals having MELTING point less than 310 kelvin ?__________________________________ANSWER :- Gallium and caesium are metals with melting POINTS less than 310 K (37℃).__________________________________

NOW THE CORRECT ORDER OF THERMAL OF STABILITY OF ALKYL HALIDE, FIRST OF ALL WE SHOULD KNOW THAT THE SIZE OF HALOGEN ATOM INCREASES FROM F (flourine) to I (iodine) then HX BOND LENGTH ALSO INCREASES FROM H-F to H-Ithen the correct order will be, (H – F < H – Cl < H – Br < H – I)

TION:-Nor EPINEPHRINE and epinephrine DERIVED from which aminoacid_________________________________ANSWER:- epinephrine and nor epinephrine are derive from "TYROSIN" amino ACID._________________________________

electrons in the valence shell of the alkali metals easily absorb energy from the flame and consequently, they get excited to higher energy levels. When such excited electrons get back to the "ground state", an "energy" is released in the FORM of LIGHT. (ii) There EXISTS very high LATTICE enthalpy in LiF which makes it insoluble in water. However, it is the opposite in the case of LiCl. There exists comparatively low lattice enthalpy in LiCl and thus, there is a higher hydration enthalpy which makes it easily soluble in water. As acetone is polar in nature, LiCl is ALSO soluble in acetone because of the effect of dipolar attraction.

re is a diagonal relationship existing between lithium and magnesium. That's why they both show similar properties. There are many reasons for this diagonal relationship (a) In the PERIODIC table, the elements from top to bottom in any particular group exhibit an ascending order of their electropositive nature. On the other hand, the elements from left to right, the same nature WOULD be in decreasing order. This is one of the reason why diagonal elements LIKE magnesium and lithium have similarities. (b) Size of the atom in a group from top to bottom increases. This implies that the polarizing power of the elements in the group is in descending order. But, from left to right in a periodic table, the polarising power increases.  This is another reason why lithium and magnesium are said to be strong elements and possess similarities (ii) Alkali metals have only one electron in their outermost shell. When an alkali metal loses that single electron, it  achieves stable configuration of a noble gas. Thus  these alkali metals exhibit an oxidation state of +1. (iii) Alkali metals are located at the extreme left side of the periodic table.  The introduction of new valence shells BEGIN from these alkali metals and then moves over to the remaining elements in the respective periods. Additionally, "alkali metals" have the lowest nuclear charge when COMPARED to the other elements in the respective periods.  That is why the alkali metals are largest size when compared to the other elements in the respective periods.

formation of ionic compounds, one of the atoms should have high electron affinity. Electron affinity is a property of an atom to accept an electron in its valence shell.  COMPARED to other elements, the halogens possess the "highest electron affinity". This property helps the halogens to get CONVERTED as anions and forming ionic bonds readily. There are other elements that have high electron affinities and that are capable of forming ionic compounds like the elements of GROUP VI. These elements need to accept 2 electrons for the achievement of a STABLE configuration.  During the process of accepting of electrons, one electron is added to the atom along with release of energy, thereby forming a single charged negative ion. This produced anion repels the next electron that is yet to be accepted by the atom. Hence, an energy greater than the repulsion has to be applied for adding the second electron.  Therefore, double charged negative ions do not get formed in ionic compounds of halogens.

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lide experience nucleophilic displacement responses promptly when a strong el' withdrawal group i.e. nitro is AVAILABLE at ortho or para positions. Whenever p - NITROCHLOROBENZENE responds with caustic soda, p - NITROPHENOL is synthesized. As caustic soda is NAOH and OH group is el' donating. Its impact is visible in given reaction. At the point when NUCLEOPHILE attacks p - nitrochlorobenzene, it will make negative charge on carbon nearby nitro group which is delocalized outside of the ring and this intermediate will turn out to be more steady than chlorobenzene and thus the product for example p - nitrophenol formed.

is an example of a salt produced from a strong acid and a weak base. When this salt reacts with the moisture in the air, it undergoes HYDROLYSIS and forms fumes of hydrogen chloride GAS.  (ii)        There are many factors that make beryllium chloride different from other halides of ALKALINE earth METALS. a.        Beryllium chloride are covalent whereas the others "halides" of all other alkaline earth metals are ionic. b.       Hydrates can be formed by any of the chlorides of Group 2 except c.        There would be some colour characteristics in the FLAMES of "chlorides" of "alkaline earth metals" except

ringer.comMagnetic iron oxide nanoparticles: synthesis and surface functionalization strategiesWei Wu, Quanguo He, Changzhong JiangNanoscale RESEARCH letters 3 (11), 397, 2008Surface functionalized magnetic iron oxide nanoparticles (NPs) are a kind of NOVEL functional materials, which have been widely used in the biotechnology and catalysis. This review focuses on the recent development and various strategies in preparation, structure, and magnetic PROPERTIES of naked and surface functionalized iron oxide NPs and their corresponding application briefly. In order to implement the practical application, the particles must have combined properties of high magnetic saturation, stability, biocompatibility, and interactive functions at the surface. Moreover, the surface of iron oxide NPs could be modified by organic materials or inorganic materials, such as polymers, biomolecules, silica, metals, etc. The problems and major challenges, along with the directions for the synthesis and surface functionalization of iron oxide NPs, are considered. FINALLY, some future trends and prospective in these research AREAS are also discussed.

dation of Ferrous to Ferric Ion by in acidic medium This is a redox equation in which two processes happen .a) Ferrous Ion is OXIDIZED to Ferric Ion. The oxidation half-reaction is as follows:                        [oxidation] B) Hydrogen peroxide is reduced to WATER. The reduction half-reaction is as follows:                                [reduction] The OVERALL redox reaction is as follows: (ii) Oxidation of Iodide to IODINE Ion by in acidic medium This is a redox equation in which two processes happena) Iodide Ion is oxidized Iodine. The oxidation half-reaction  is as follows:                  [oxidation] b) Hydrogen peroxide is reduced to water. The reduction half-reaction is as follows:                                [reduction] The overall redox reaction is as follows:

hin PROTECTIVE LAYER of aluminium oxide is formed on the surfaces of the aluminium containers due to the chemical reaction taking place between Aluminium and Concentrated . Now this oxide layer prevents further reaction thereby making aluminium passive.  (ii) When sodium hydroxide is made to react with aluminium, it forms sodium tetrahydroxoaluminate (III). During this reaction, hydrogen is also liberated. The pressure of this hydrogen gas HELPS in OPENING the blocked drains. (iii) The structure of graphite is a layered ONE. The Van-der-Waal's forces that hold the layers together are weak. This will lead to slipping over one another. This is the reason why graphite acts as a lubricant.

ubstance is known to be a reducing agent, if  a. It causes reduction in the "oxidation number" of the other substance involved in the chemical reaction. b. Its oxidation number is increased. "Alkali metals" have only one electron in their "valence SHELLS" which they WOULD lose easily to attain stability and become oxidized. Hence, their oxidation numbers would increase whereas on giving that electron, the substance that gets this electron will have its oxidation number reduced.  Hence, alkali metals are termed as strong reducing agents. (ii) There are three main reasons: a. As alkali metals are strong reducing agents, they cannot be isolated by the chemical reaction of their oxides b. As alkali metals are highly electropositive, they cannot be PREPARED  by reactions involving displacement of one element over another in their salt solutions c. During electrolysis of  aqueous solutions of their salts, the liberated metals REACT with water and eventually hydrogen gets liberated at the cathode.  Thus, in order to extract alkali metals, electrolysis of their fusion chloride is implemented as shown below: During electrolysis At anode At cathode (iii) During the process of electrolysis of the aqueous SOLUTION of any alkali metal like for example sodium, it would produce sodium hydroxide by immediately reacting with water. Thus, hydrogen gets liberated at the cathode. This happens because the standard electrode potential of water is much higher than that of alkali metals. (iv) When an alkali metal gets dissolved in liquid , the atom of the alkali metal loses its only electron in its valence shell very easily. Now, the cation so formed will merge with ammonia to form ammoniated cation.   The solvated electron so formed, absorbs energy from the red region of the visible light in order to get excited to higher energy levels. Eventually, the blue colour is imparted to the solution due to the transmitted light. (v) The blue colour gets disappeared on standing for some time because the solvated electrons reacts with ammonia which will thus liberate hydrogen

h +2 and +4 oxidation states are adopted by the element tin. The same is true for Lead as well. But there is a difference between tin and lead regarding the context of oxidation states. Tin (IV) oxidation state is more stable.  HENCE, the conversion of tin (II) compounds to tin (IV) compounds is very easy as two ELECTRONS are lost easily by the tin(II). Hence, tin is a reducing agent. (ii) This is best illustrated in the below chemical reaction where tin (II) ions reduces iron (III) to iron(II) ions. During this process, the tin (II) ions (less stable ions) are oxidized to the tin(IV) ions (more stable ions) .(iii) But it is REVERSE in the case of Lead because the lead (II) is more stable than lead (IV). Thus, Lead will not be losing any electrons easily. Hence, lead cannot be a reducing agent. (iv) As we have proved in (i) that tin is a reducing agent, it can REDUCE mercuric salts to mercurous salts. Thus is best illustrated in the below chemical reaction where tin(II) chloride reacts with mercuric chloride to form mercurous chloride

ct elements like nitrogen, sulphur, and HALOGENS in organic compounds, we use Lassaigne's Test. This test was invented by the French Chemist named J.L. Lassaigne.  In this test, the organic compound that is under study is being fused with metallic sodium for converting the elements into sodium salts. These sodium salts would be soluble in WATER. Now this extract would then undergo qualitative tests to detect the required element .Now here, the test is for detecting sulphur in an organic compound. The preparation of Lassaigne's extract involves the fusion process of metallic sodium and the sulphur from organic compound. This reaction FORMS sodium SULPHIDE.This sodium sulphide gives deep violet colour when it reacts with sodium nitroprusside because the product FORMED due to the reaction is sodium thionitroprusside. This indicates the presence of sulphur.

n affinity MEANS ENERGY released by gas during it changes to ION STATE from gas state. Here, chlorine releases 3.7eV energy when it transforms from chlorine gas to chlorine ion. For 1 mole chlorine, the released energy is                                           3.7eV = 357.013 kJ/mole Now, 1 mole Chlorine = 35.5 gm. 35.5 gm chlorine when changes completely into ion releases 357.013 kJ energy 7.1 gm chlorine when changes completely into ion releases

re assuming the equal probabilities of a reaction : 1 mol of methyl BROMIDE and ethyl bromide will PRODUCE CH3CH2CH3 (propane). The reaction of both reactants in the PRESENCE of sodium is GIVEN below : CH3Br + CH3CH2Br + 2 Na----------> CH3CH2CH3 + CH3CH2CH2CH3 +                                                                    2NaBr 1 mol of propane = molar mass  = 44.0 g Mass of CH3CH2CH3 = 44 / 3 = 14.67 g

that,                           First and SECOND ionization energies of Mg are and (GIVEN). Therefore, the TOTAL energy REQUIRED to convert magnesium atoms to magnesium ions is                                                                                          =22⋅681eV  Total required energy in TERMS of kJ is   22⋅68×96⋅49=2188⋅39 kJ Now, molar mass of magnesium is 24 gm/mol means 24 X 103 mg/mol So, 12 mg of magnesium = Therefore, total energy required to convert all Mg atoms to ions is

The strongest type of covalent chemical bonds are sigma-bonds which are FORMED by head-on overlap between two atomic orbitals. π bonds: Side to side OVERLAPPING of two atomic orbitals forms a pi-bonds which is a covalent bonds. Pi-bonds are easily broken. A single sigma-bond and one or two pi-bonds are usually formed double or TRIPLE bonds.  The number of sigma-bonds in the above chemical structure is 9. And, the number of pi-bonds in the above chemical structure is 3. Explanation: C-C sigma-bonds = 3                       C-H sigma-bonds = 5                       C-N sigma bonds = 1                       C-C pi-bonds = 1                        C-N pi-bonds = 2

ncipal QUANTUM number n describes the energy of an electron and the size of the orbital. Whereas, the angular momentum quantum number (Azimuthal) specifies the shape of an orbital. The secondary quantum number divides a shell into sub-shells , a smaller group of orbitals. A LETTER CODE l represents sub-shells with specified names and numbers.           Values of l          0     1     2     3     4     5   Names of sub-shells     s     p     d     f      g      H The number of sub-shells DEPEND on the mathematical value of . For example, the s sub-shell ‘l’ equals to 0.

cathodeCu2+ (aq) + 2e-  ---> CU(s)At the anode4OH-(aq) ----> 2H2O (L) + O2(g) + 4e-Faraday’s constant = 96500C/molTo DEPOSIT 1 MOLE of copper, we need 2x96500CSo, 96500C will deposit 0.5 moles of copper = 0.5x63.5 = 31.75gTo LIBERATE one mole of oxygen molecules,we need  4x96500CSo, 96500C will liberate = ¼  = 0.25 moles = 0.25x32 = 8g

lecule has 14 ELECTRONS totally. Three is the bond order in   . In NO molecule ,2.5 is the bond order. So, the order of bond for    molecule is greater than NO molecule. Hence   molecule has higher bond dissociation ENERGY than NO.(ii) “Three is the order of bond for CO” .   molecule which is EQUAL to CO. Both    and CO are isoelectronic. Because of high electronegativity difference, CO is highly reactive than   . And CO is also more polar than  .

ate means that a SET of orbitals or electron shells which are having the same energy value. The LOCATIONS of the shells can be different around the nucleus. The number of degenerate orbitals depends on Azimuthal Quantum Number. For example, the azimuthal quantum number is L = 1.The total number of magnetic number of a sub-shell can process, i.e., no. of degenerate orbitals are from –l to +l or mathematically expressed as 2l+1.Therefore, for p shell, there are 3 degenerate atomic orbitals ( -1 , 0 , +1 ) called and they all have EXACTLY the same energy value. To calculate number of orbitals one should know the FOLLOWING data :The azimuthal quantum number (l) of  i)        s sub-shell is 0  ii)        p sub-shell is 1 iii)        d sub-shell is 2  iv)        f sub-shell is 3 The total number of degenerate atomic orbitals of d sub-shell is 5 ( -2 , -1 , 0 , +1 , +2 ).

ides are metallic elements in the periodic table from “Lanthanum to lutetium”. Lanthanides are elements of f-block in which 4F electron shell are filled. The atomic numbers RUN from 51 to 71. All the Lanthanide elements contain the +3 cations and forms the stable compounds.    The ELECTRONIC configuration of Cerium is   and it is stable at +4  cation.   can lose one 'f' electron to form   with the fixed Xenon configuration.      The Europium configuration  is   and it is stable at +2 cation.   earn an electron for the formation of with the configuration and has the additional “stability of a partially-filled shell”.

ng electrophilic reagents like , HBr Alkanes are more reactive than Alkynes.This is because, In alkynes the pie-electrons are  TIGHTLY HELD by the  atoms of carbon due to the triple bond. And in ALKENES the pie electrons are not held tight because of hybridilized carbon atoms. The electrons become more delocalized and stable, so the pie electrons are less available for adding electrophilic reagents.  THEREFORE, Alkynes reacts less than the Alkenes with ELECTROPHILES.

fference – Formic Acid vs Acetic Acid Both formic acid and acetic acid are ORGANIC molecules that can be categorized as CARBOXYLIC ACIDS due to the presence of a carboxyl group. Therefore, both compounds are ACIDIC compounds. However, in aqueous solutions, these are weak acids that are partially dissociated into their conjugated base form by releasing a proton. The main difference between formic acid and acetic acid is that formic acid is COMPOSED of a carboxyl group attached to a hydrogen atom WHEREAS acetic acid is composed of a METHYL group attached to a carboxyl group.

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E!HERE IS YOUR ANSWER 17. (B) Phosgene18. (b) -OH19. (c) or (d)HOPE IT WILL HELP YOU.........

eactions in which HEAT is ABSORBED is CALLED ENDOTHERMIC reaction..

of the large size, these ELEMENTS have LOW density which increases down the GROUP from LI to CS.

g water sources available to North Americans may contain high levels of Ca2+, MG2+, and Na+ and may provide clinically important portions of the RECOMMENDED dietary intake of these minerals. Physicians should encourage PATIENTS to CHECK the mineral content of their drinking water, whether tap or bottled, and CHOOSE water most appropriate for their needs.

________________Which of the FOLLOWING are LEWIS ACIDS ? , , , ✔✔✔_______________________

-7strongly ALKALINE -11strongly ACIDIC -1weakly acidic -4weakly alkaline -9

ompare hydrogen and HALOGENS on the basis of physical STATE then both are gas in the basis of information both FORM negative FORMATION of IRON and in the basis of valency both have valency 1 and reaction with oxygen to form water vapour and the reaction is not very harmful

riend ♥♥✌✌Please Edit The QUESTION With the FigureThe edit option is in the three VERTICAL DOTS at the upper RIGHT SIDE

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ngle COVALENT bond consist one pair of shared electron . In other words a single bond is formed by sharing one sharing of one pair of electron between two atoms . A single and covalent COMPOUND is formed by the sharing two electrons between the ATOM each atom CONTRIBUTING one electron of sharing . ii) A double covalent bond consists of two PAIRS of shared electrons . In other words a double bond is formed by sharing two pairs of electrons between two atoms .Double covalent bond is formed by sharing of electrons between two atoms and each atoms contributing to electrons for sharing .

n No.01       A= H2 (Hydrogen Gas Is Colorless at STP),       B= CuO(Cupric oxide is a Black Colored Metallic Oxide)c= neutral gas H0 hydrogen oxide       D= CU (Copper is a pinkish RED metal)Question No.02The BALANCED Chemical Equation of Reaction          2CuO (s) + H2 (g) ---> 2CU (s) + 2HO (g)

is WOULD help you mate,SIMPLY when the elements react , they lose their affinity or negativitye.g. in the ionic bond of Na+ and CL- ,both are harmful substances ,but due to the bond they neutralize each other and we EAT them on daily BASIS.

her PROPORTION of carbon dioxide in atmosphere has increased  where more fossil fuel burning TAKE place.Dry air comprises 78.09 % of Carbon Dioxide. Deforestation is the root cause for the carbon STORED in trees and ALSO results in less carbon dioxide being clean off from the atmosphere.

ng to AVOGADRO's law, one MOLE of a GAS at STP occupies 22.4L. 1 g of Hydrogen Gas (H2) = 0.5 mole of Hydrogen gas since 2 gm. is the molar mass of DIHYDROGEN! Now by Avogadro's Law, 1 mole of any gas at STP would occupy 22.7 litres of volume.

n Lassaigne’s solution, Ferric CHLORIDE (FeCl3) reacts with Sodium thiocyanate to GIVE Ferric thiocyanate [Fe(CNS)3] which is blood red.The test is usually USED as a confirmatory test for organic compounds containing NITROGEN and Sulfur Compounds(essential amino acids). Blood red color indicates the FORMATION of Ferric thiocyanate.Hope it helped.

Here is ur answerethanol=C2H5OHethanoic acid=CH3COOHester=CH3COOCH2CH3esterification reaction= ethanol+ethanoic acid----->esterde esterification reaction is the OPPOSITE of esterification reaction and is also known as Saponification reactionIts chemical EQUATION followsCH3COOCH2CH3--------> (in the presence of NAOH GIVES) C2H5OH+CH3COOHhope it will help u...

hatic AMINES the amine GROUP -NH2 is attached to an alkyl group which is an electron donating group. ie., They have a +I EFFECT. So they increase the availability of a pair of electron on the Nitrogen Atom and hence Aliphatic amines will be more basic than Ammonia and aromatic amines.In aromatic amines the -NH2 Group is attached to PHENYL Group (-C6H5 ) is which is electron attracting. So the availability of the lone pair of electron on the Nitrogen atom will be less and hence will be less basic than Aliphatic amines.is stronger but more basic in nature...hope it helps u mate....pls mark me brainliest