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    • Posted by ???. Pragati 7 years ago

    CBSE > Class 11 > Chemistry
    • 2 answers

    Vaibhav Kumar Gupta 7 years ago

    Because both boron and chlorine are of small size and also of comparable size with each other , hence due to almost comparable size bond formed is more stable , as compared to bond foed between Thallium and chlorine where size/radius difference is more, hence in case of thallium weaker bond is formeand less stable.

    0Thank You

    Ankit Singh 7 years ago

    bcl3 is stable while ticl3 is unstable . Boron and thallium belong to group 13 of the periodic table. In this group, the +1 oxidation state becomes more stable on moving down the group. BCl 3 is more stable than TlCl 3 because the +3 oxidation state of B is more stable than the +3 oxidation state of Tl. Please confirm that my answer is correct .......

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    • Posted by ???. Pragati 7 years ago

    CBSE > Class 11 > Chemistry
    • 4 answers

    Yogita Ingle 7 years ago

    Water gas is produced from synthesis gas, which is composed of carbon monoxide and hydrogen. Syngas is a useful product, but requires careful handling due to its flammability and the risk of carbon monoxide poisoning. The water-gas shift reaction can be used to reduce the carbon monoxide while producing additional hydrogen, resulting in water gas.

    H2O + C → H2 + CO (ΔH = +131 kJ/mol)

    1Thank You

    Ankit Singh 7 years ago

    Hope this answer is helpful to u

    1Thank You

    Ankit Singh 7 years ago

    A fuel gas containing about 5o percent carbon monoxide 40 percent hydrogen and small amount of methane, carbon dioxide and nitrogen made by passing stem and air over heated coke and coal is known as water gas.its composition is (CO+H2).it is used as fuel.

    2Thank You

    Ayushi Ayushi 7 years ago

    A fuel gas containing about 5o percent carbon monoxide 40 percent hydrogen and small amount of methane, carbon dioxide and nitrogen made by passing stem and air over heated coke and coal is known as water gas.its composition is (CO+H2).it is used as fuel.

    2Thank You

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    • Posted by ???. Pragati 7 years ago

    CBSE > Class 11 > Chemistry
    • 3 answers

    Yogita Ingle 7 years ago

    Carbon cannot have a valency beyond four
    C6 =  1s22s22p2
    While silicon can extended covalency from 4 to 6
    Si14 = 1s22s22p63s23p2
    This is because of the absence of d-orbitals in the valence shell of carbon and presence of 3d-orbtials in the valence shell of silicon. Since silicon has vacant 3d- orbitals, it can accept electrons from electron donating species such as F- ion to form complex ion.

    1Thank You

    Ankit Singh 7 years ago

    Hope this answer will help u

    0Thank You

    Ankit Singh 7 years ago

    Catenation is the linkage of atoms of the same element into longer chains. Catenation occurs most readily in carbon, which forms covalent bonds with other carbon atoms to form longer chains and structures.

    2Thank You

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    • Posted by Sweta Kumari 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Aman Sirohi 7 years ago

    CBSE > Class 11 > Chemistry
    • 2 answers

    Yogita Ingle 7 years ago

    Stereoisomers which are related to each other as mirror images are called enantiomers. Enantiomers can contain any number of stereogenic centers, as long as each center is the exact mirror image of the corresponding center in the other molecule.

    1Thank You

    Ayushi Ayushi 7 years ago

    Enantiomers are chiral molecules that are mirror images of one another. Furthermore, the molecules are non-superimposable on one another. This means that the molecules cannot be placed on top of one another and give the same molecule. Chiral molecules with one or more stereocenters can be enantiomers. It is sometimes difficult to determine whether or not two molecules are enantiomers. For introductory purposes, simple molecules will be used as examples.

    2Thank You

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    • Posted by @@Ditya ®°@Thore????? 7 years ago

    CBSE > Class 11 > Chemistry
    • 5 answers

    Ayushi Ayushi 7 years ago

    Your wellcome Aaditya .

    3Thank You

    @@Ditya ®°@Thore????? 7 years ago

    Yhanks ayushi???

    2Thank You

    Ayushi Ayushi 7 years ago

    Your wellcome Ankit.

    2Thank You

    Ankit Singh 7 years ago

    Thanks ayushi ye question meujhe doubt tha

    1Thank You

    Ayushi Ayushi 7 years ago

    Reason for anomalous Behaviour of boron It is extremely hard and black coloured solid. It exists in many allotropic forms. Due to very strong crystalline lattice, boron has unusually high melting point. Rest of the members are soft metals with low melting point and high electrical conductivity.

    3Thank You

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    • Posted by Nishu Godara 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Piyush Jaat 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Kiran Rathore 7 years ago

    CBSE > Class 11 > Chemistry
    • 2 answers

    Ayushi Ayushi 7 years ago

    Antacids Definition Antacids are medicines that neutralize stomach acid. acids may be divided into two classes, those that work by chemical neutralization of gastric acid, most notably sodium bicarbonate; and those that act by adsorption of the acid (non-absorbable antacids), such as calcium and magnesium salts.

    2Thank You

    Aditya Rai 7 years ago

    Opposite of acid 

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    • Posted by Ramesh Verma 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Yogita Ingle 7 years ago

    Like Li and Be, boron – the first member of group 13 – also shows anomalous behavior due to its low size and high nuclear charge/size ratio, high electronegativity and non – availability of d electrons. The main point of differences is:-
    1.   Boron is a typical non-metal whereas other members are metals.
    2.   Boron is a bad conductor of electricity whereas others are good conductors.
    3.   Boron shows allotropy and exists in two forms—crystalline and amorphous. Aluminum is a soft metal and does not exist in different forms.
    4.   Like other non metals, the melting point and boiling point of boron are much highr than those of others elements of group 13.
    5.   Boron forms only covalent compounds whereas aluminum and other elements of group 13 also do form some ionic compounds.
    6.   Hydroxides and oxides of boron are acidic in nature whereas those of others are amphoteric and basic.
    7.   The trihalides of boron exist as monomers. On the other hand, aluminium halides exist as dimmers.
    8.   The hydrides of boron i.e. boranes are quite stable while those of alumimium are unstable.
    9.   Dilute acids have no action on boron. Other members of group 13 liberate h2 from dilute acids.
    10.  Borates are more stable than aluminates.
    11.  Boron exhibit maximum covalency of four e.g., BH4- ion while other members exhibit a maximum covalency of six e.g.
    12.  Boron does not decompose steam while other members do so.

    2Thank You

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    • Posted by Jatin Nayak 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Ankit Singh 7 years ago

    CBSE > Class 11 > Chemistry
    • 5 answers

    Ankit Singh 7 years ago

    Thank u

    1Thank You

    Aman Kumar 7 years ago

    Nice

    2Thank You

    Priya Dharshini ? 7 years ago

    1. Shape, hybridisation and structure representation of carbon compounds 2. Classification of organic compounds focusing on the concepts revolving around aromaticity 3. Nomenclature and isomerism of organic compounds 4. Homolytic and heterolytic cleavage 5. Nucleophile and electrophile 6. Electron displacement effects 7. Purification of organic compounds esp. focussing on types of chromatography and distillation and its types

    1Thank You

    Ankit Singh 7 years ago

    Please

    0Thank You

    Ankit Singh 7 years ago

    Please help

    2Thank You

    ANSWER

    • Posted by Anand Raj 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Prakhar Jadaun ? 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Mini Azad 7 years ago

    CBSE > Class 11 > Chemistry
    • 2 answers

    Ayushi Ayushi 7 years ago

    The inert pair effect is defined as the tendency of electrons in the outermost atomic s orbital to remain unionized or unshared in compounds of post-transition metals. ... When we say that electrons are inert, we essentially mean that they are spin paired. An example is in helium, with two electrons.

    2Thank You

    Anurag Mishra 7 years ago

    Decrease in oxidation state by 2. (In p block)

    3Thank You

    ANSWER

    • Posted by @@Ditya ®°@Thore????? 7 years ago

    CBSE > Class 11 > Chemistry
    • 3 answers

    Ritu Thapliyal 7 years ago

    Ur wlcm

    1Thank You

    @@Ditya ®°@Thore????? 7 years ago

    Thanks Ritu

    3Thank You

    Ritu Thapliyal 7 years ago

    Li forms monoxide bcz of its small size it has strong field therefore it only combines with one oxygen atom to form monoxide while Na has large size due to which the field become weak and it can't prevent oxide ion to combine with another O2 atom to form peroxide

    4Thank You

    ANSWER

    • Posted by Sundram Yadav 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Ayushi Ayushi 7 years ago

    Aluminium and gallium belongs to group 13.Generally, atomic radii increases on moving down in a group.But the atomic size of gallium is less than aluminium although it lies below aluminium in the group.This because of the poor shielding or screening effect of electrons in the 3d orbital of gallium.

    3Thank You

    ANSWER

    • Posted by Kajol Verma 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Ayushi Ayushi 7 years ago

    First of all we react methyl bromide with ethyl bromide and sodium in presence of dry ether (wurtz reaction) ....it gives propane ...react propane with CI2...in presence of li8...Then react with aq KOH...then oxidise it with KMnO4 to give propanone.....

    2Thank You

    ANSWER

    • Posted by Jyotya Sachan 7 years ago

    CBSE > Class 11 > Chemistry
    • 3 answers

    Nancy Rajput 7 years ago

    ethan -1-1- dialdehyde

    1Thank You

    Prakhar Jadaun ? 7 years ago

    Sorry..... ...... Right answer is - ethane - 1,1 - dial

    0Thank You

    Prakhar Jadaun ? 7 years ago

    Eth - 1,1 - dialdehyde

    0Thank You

    ANSWER

    • Posted by Saumya Sb Bhandari 7 years ago

    CBSE > Class 11 > Chemistry
    • 3 answers

    Prakhar Jadaun ? 7 years ago

    1 . Elements like H and He exist since they donot complete their octet. They complete their duplate. 2 . Formation of hypervalent compound i.e. compounds having more than 8 electrons in their valence shell. Eg. SiF6 , in this Si have 12 shared pair electrons ( 6 of Si and 6 of F) . 3 . Formation of compound having less than 8 electrons in their valence shell. Eg. AlCl3, in which aluminum donot complete their octet, after been combined with three Cl, it has only 6 electrons in its valence shell

    0Thank You

    Ankit Singh 7 years ago

    It cannot be applied to the nonmetals after silicon in the Periodic Table. These elements can “expand their octet” and have more than eight valence electrons around the central atom. Molecules with an odd number of electrons such as NO and NO₂ cannot satisfy the octet rule.

    1Thank You

    Aman Kumar 7 years ago

    ????

    1Thank You

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    • Posted by Naman .. 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Ayushi Ayushi 7 years ago

    in SiCl6(2-) the chlorine atom is much larger than flourine which does not allow the six chlorines to surround the silicon due to repulsions between chlorine atoms. silicon cannot acomodate 6 chlorines around it. Hence , due to interelectron repulsions between chlorine atoms the compound SiCl6(2-) is unstable and not known.

    2Thank You

    ANSWER

    • Posted by Akash Kumar 7 years ago

    CBSE > Class 11 > Chemistry
    • 2 answers

    Ayushi Ayushi 7 years ago

    The electron gain enthalpy of halogens is highly negative because it needs only one electron to achieve nearest noble gas configuration. And for noble gases, it is highly positive because the extra electron has to be placed in the next higher principal quantum level which requires lots of energy.

    4Thank You

    Ayushi Ayushi 7 years ago

    Electron gain enthalpy (ΔegH) is defined as the enthalpy change associated with an isolated gaseous atom (X) when it gains an electron to form its corresponding anion. The reaction can be given as below: X(g)+e−→X−(g) On the basis of nature of the element, the process of accepting electron in an atom can either be exothermic or endothermic. In general, energy is released when an electron is added to an atom and the electron gain enthalpy for such elements is negative.

    3Thank You

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    • Posted by Ashutosh Yadav 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Mukesh Chand 7 years ago

    CBSE > Class 11 > Chemistry
    • 3 answers

    Ankit Singh 7 years ago

    No. Of moles

    1Thank You

    Karan Yadav 7 years ago

    No. Of moles

    1Thank You

    Divya Tripathy 7 years ago

    no. Of moles

    3Thank You

    ANSWER

    • Posted by Shikha Rai 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Ankit Singh 7 years ago

    The hydrogen economy is a proposed system of delivering energy using hydrogen. The term hydrogen economy was coined by John Bockris during a talk he gave in 1970 at General Motors Technical Center. The concept was proposed earlier by geneticist J.B.S. Haldane

    1Thank You

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    • Posted by Pratiksha Vinayak 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Yogita Ingle 7 years ago

    We know that in ice, each oxygen atom is surrounded by four hydrogen atoms in such a way that the two hydrogen atoms are linked to an oxygen atom by covalent bonds whereas the other two hydrogen atoms are linked by hydrogen bonds. In ice (solid state), a water molecule is associated with four other water molecules through hydrogen bonding in a tetrahedral manner. This gives rise to open cage-like structure which prevents the close packing of molecules (lower density). When ice absorbs heat and melts to form water, the hydrogen bonds break and close packing of water molecules takes place. Due to this close packing, the density of water is higher than that of ice and hence ice floats over water.

    2Thank You

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    • Posted by Vijay Singh 7 years ago

    CBSE > Class 11 > Chemistry
    • 3 answers

    Ankit Singh 7 years ago

    Isothermal is a process in which change in temperature remains constant ,,, ∆T =0 .......

    1Thank You

    Paranjeet Singh 7 years ago

    In this process temperature remains constant so there no change in temperature hence, internal energy of the system do not change so in this process amount of heat ∆Q = ∆W

    1Thank You

    Rudransh Kalia 7 years ago

    An isothermal process is a change of a system, in which the temperature remains constant: ΔT = 0.

    3Thank You

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    • Posted by Nikhil Yadav 7 years ago

    CBSE > Class 11 > Chemistry
    • 0 answers
    ANSWER

    • Posted by Paras Paras 7 years ago

    CBSE > Class 11 > Chemistry
    • 2 answers

    Aditi Singh 7 years ago

    No it is not in syllabus

    1Thank You

    Shweta Chaudhary 7 years ago

    Yes

    5Thank You

    ANSWER

    • Posted by Arjun Thakur 7 years ago

    CBSE > Class 11 > Chemistry
    • 1 answers

    Sweta Kumari 7 years ago

    because both Na and H2 have 0 change it is on ground state after in product they have + and - charge so redox rxn occurs here

    2Thank You

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