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This section includes 7 InterviewSolutions, each offering curated multiple-choice questions to sharpen your Current Affairs knowledge and support exam preparation. Choose a topic below to get started.
| 1. |
Which element is the strongest oxidising agent ? |
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Answer» F- flourine Flourine The oxidizing agent is a term which is used to describe a reactant in the oxidation and reduction reactions which include the transfer of electrons between the reactants in order to form a product. The elemental fluorine is an example of the strongest agent. |
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| 2. |
all compounds of lithium mentioned in s block with their properties |
| Answer» Can u please elaborate | |
| 3. |
Why Chemistry is big Mistory |
| Answer» Everything which you study by heart will become mystrious and interesting for u | |
| 4. |
What is Spatial arrangements of atoms (easy define).. |
| Answer» | |
| 5. |
Molarity of H+ ions if 49g of H2SO4 is dissolved in 250ml solution. |
| Answer» 4M | |
| 6. |
how to find the iupac names |
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Answer» Learn all rules Seniority table must be by heart and then word root and a few tricks that will be developed by practice First of all learn all functional groups.. I dont know |
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| 7. |
Lithium salts are most hydrated give reason |
| Answer» Due to high hydration enthalapy of lithium | |
| 8. |
Formula of h2o |
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Answer» Water ??It must be H2O |
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| 9. |
Nitrogen does not form pentachloride. Why ? |
| Answer» 1. Due to its small size...2 . Absence of vacant d orbitals.. Due to these reasons nitrogen cannot hold five huge atoms of Cl.....? | |
| 10. |
Explain fajans rule. |
| Answer» Fajans\' rule states that a compound with low positive charge, large cation and small anion has ionic bond where as a compound with high positive charge, small cation and large anion are covalently bonded. NaCl is correctly predicted to be ionic since Na+ is a larger ion with a low charge and Cl− is a smaller anion. | |
| 11. |
What is the action of heating on borax? |
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Answer» It first looses water of crystallization and then on furthr heating it forn a transparent liquid which solidifies to form bead like structure known as borax bead See ncert |
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| 12. |
Name the most powerful reducing agent and give reason for it? |
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Answer» LiAlH4 Lithium is strongest Reducing agent because of lowest standard reduction potential. When something is oxidized, it reduces another substance, becoming a reducing agent. Hence lithium is the strongest reducing agent. |
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| 13. |
Hypophosphorus acid formula? |
| Answer» Hypophosphorous acid is a phosphorus oxyacid and a powerful reducing agent with molecular formula H3PO2. It is a colorless high-melting compound, which is soluble in water, dioxane, and alcohols. The formula for blue acid is generally written H3PO2, but a more descriptive presentation is HOP(O)H2 which highlights its monoprotic character. | |
| 14. |
What we obtain by burning orthophosphorous |
| Answer» When Orthophosphorus acid is heated, then following reaction takes place, 4H3PO3 → 3H3PO4 + PH3it forms phosphoric acid and phosphine this reaction yields a number of undefined phosphorus suboxides as well. | |
| 15. |
How would you calculate the ph of 0.001M NaOH?? |
| Answer» NaOH is a strong base that dissociates completely Therefore [OH-] = [NaOH] = 0.001M First calculate the pOH of the solution : pOH = -log [OH-] pOH = -log 0.001 pOH = 3.00 pH = 14.00 - pOH pH = 14.00 - 3.00 pH = 11.00 | |
| 16. |
How we express scientific notation if n>1 |
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| 17. |
1ml of 13.6 molar HCl is diluted to give 1litre of solution find pH of solution? |
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| 18. |
Which is most strong electron withdrawing group among NO2 and O-CH3? |
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Answer» No2 because nitrogen is bonded with two second most electronegative elements, it generates a strong partial positive charge on nitrogen He it is NO2 |
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| 19. |
How find standard enthalpy |
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| 20. |
Differentiate between butane and butene |
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Answer» Butane is alkane ..1. it is saturated 2. It has only sigma bondand butene is alkene..1. it is unsaturated In butane , there is single bond between carbon atoms and in butene there is double bond between carbon atoms . Butane is saturated hydrocarbon (alkane) while butene is unsaturated hydrocarbon |
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| 21. |
Calculate the molarity of H2O2 labeled as 10 volume H2O2? |
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| 22. |
How many sigma and pi bond in a molecule of ethylene |
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Answer» 5 sigma 1 pi bonda 5 sigma 1 pi bonds |
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| 23. |
Write the electronic configuration of O2 |
| Answer» 1S2 2S2 2P4 | |
| 24. |
What are oxidising flame?? |
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Answer» I have asked oxidising flame not radioactive elements... Read the question carefully Krishna radioactive element. an element subject to spontaneous degeneration of its nucleus accompanied by the emission of alpha particles, beta particles, or gamma rays. All elements with atomic numbers greater than 83 are radioactive. Naturally occurring radioactive elements include radium, thorium, and uranium. |
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| 25. |
What are radioactive elements?? |
| Answer» radioactive element. an element subject to spontaneous degeneration of its nucleus accompanied by the emission of alpha particles, beta particles, or gamma rays. All elements with atomic numbers greater than 83 are radioactive. Naturally occurring radioactive elements include radium, thorium, and uranium. | |
| 26. |
How to convert benzoic acid into benzene? |
| Answer» react benzene with NaOH then it will form sodium benzenoatethen again react sodium benzenoate in the presence of soda lime it will give benzene and Na2CO3. | |
| 27. |
How to convert benjoic acid into benjene?Plz help |
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| 28. |
Under what conditions of temperature and pressure real gas tend to behave ideally? |
| Answer» 1. At very high temperature2. At very low pressureReal gases acts as ideal gases b/c due to very high temperature inter molecular distance become very large thus potential energy remove and only kinetic energy remain which is characteristic of ideal gas. | |
| 29. |
What are polar and non polar solvents ?explain with example. |
| Answer» \tMolecules in which dipole moment is not ‘zero’ are called polar solvents. Example: NaCl, HF, H2O…etc. The non-zero dipole moment in these molecules is mainly due to electronegativity difference between bonding atoms.\tMolecules in which dipole moment is ‘zero’ are called non-polar solvents. Example: CCl4, H2, Cl2, O2…etc. In non-polar molecules the dipole moment is zero due nearly equal in electronegativity of bonding atoms and also due to symmetry in structure. | |
| 30. |
What do you mean by steric crowding ? |
| Answer» | |
| 31. |
Out of Benzene, metadinitrobenzene and toluene which will undergo nitration most easily and why???? |
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Answer» Thank u Gaurav for ur help Nitration of benzene is an electrophilic substitution reaction. Presence of electron releasing group such as —CH3 activates the benzene nucleus towards electrophilic substitution while presence of electron withdrawing group such as —NO2 deactivates the benzene nucleus towards electrophilic substitution. Therefore, the ease of nitration decreases in the orderToluene > benzene > m-dinitrobenzeneThus, toluene will undergo nitration most easily. |
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| 32. |
Electronic configuration of CU + |
| Answer» 1s2 2s2 2p6 3s2 3p6 4s0 3d10 | |
| 33. |
Divide 9 hours for revision of Thermodynamics, states of matter and Redox reactions pls Answer |
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Answer» 1.5 for states of matter,2 hrs for redox,5.5 for thermodynamics 2 hourse states of matter3 hours for redox4 hours for thermo |
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| 34. |
Advantages and disadvantages of fuel cell please tell me |
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Answer» Welcome aditya .disadvantages of fuel cell : 1. Nitrogen Dioxide EmissionCritics of hydrogen fuel cells argue that although these cells do not emit carbon after burning, they give out nitrogen dioxide and other emissions. Nitrogen dioxide is a toxic gas and can still be harmful when ingested by humans.2. Storage IssuesApart from taking much time to separate the compounds of hydrogen, this element is also a challenge to move and transport. 3.High CostAside from having to spend a lot of money to transport hydrogen, the time it takes to break down its elements makes the process expensive as well. Advantages of fuel cell :1.Fuel cells have a higher efficiency than diesel or gas engines.2.Most fuel cells operate silently, compared to internal combustion engines. They are therefore ideally suited for use within buildings such as hospitals.3.Fuel cells can eliminate pollution caused by burning fossil fuels; for hydrogen fuelled fuel cells, the only by-product at point of use is water.4.if the hydrogen comes from the electrolysis of water driven by renewable energy, then using fuel cells eliminates greenhouse gases over the whole cycle.5.Fuel cells do not need conventional fuels such as oil or gas and can therefore reduce economic dependence on oil producing countries, creating greater energy security for the user nation. |
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| 35. |
Please sir provide me a model paper of chemistry for hindi medium |
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| 36. |
What are the similarities of hydrogen with alkali metals and halogen |
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Answer» Similarity to Halogens: hydrogen can also form both ionic and covalent bond. Both H and Halogens form compound with metals and non-metals. Similarity to alkali metals:hydrogen has 1 electron in its outermost shell and can form compounds with non-metals (such as HCl, etc.). |
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| 37. |
Methyl chloride to ethyl chloride |
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| 38. |
What are expected products when hydrogen react with metals And halogen |
| Answer» Ionic hydrides and covalent hydrides respectively. | |
| 39. |
Main topic of equilibrium chapter please urgent ???? |
| Answer» Relation between kp and kcLaw of mass actionLe chatliers principleSolubility numericalsBuffer solution Common ion effect and it\'s application | |
| 40. |
Explain buffer solution |
| Answer» It is a kind of solution which helps in maintaining the ph of that substance if some acids or bases is added in that substance Ex-blood is the best example of buffer solution | |
| 41. |
How to find group and period |
| Answer» For period :no.of valenced shell for all elements.GroupFor s block element :valences electron.For p block:12+valenced electron.For d clock:valenced e– of s +valenced e– of d.For f:just write f block elwment.For eg: predict grp and period of an elwmwnt having atomaic no.17Electrknic conf.is 1s2 2s2 2p6 3s1Grp is 3Period is 1 | |
| 42. |
Easy definition of buffer solution |
| Answer» Buffers are solutions that resist change in pH on dilution or on the addition of small amounts of acids or alkali.\xa0A lot of biological and chemical reactions need a constant pH for the reaction to proceed. Buffers are extremely useful in these systems to maintain the pH at a constant value. This does not mean that the pH of buffers does not change. It only means that the change in pH is not as much as it would be with a solution that is not a buffer. | |
| 43. |
Out of Na and Na+1 which has higher atomic size and why? |
| Answer» Na+ is smaller than Na because Na+ is formed when an electron is lost from the Na atom,Thus the effective nuclear charge increases bcz the number of protons exceeds the number of electrons .This results in bringing the valence shell a little closer to the nucleus because of a very strong nuclear pull. | |
| 44. |
Difference between endothermic and exothermic reactions? |
| Answer» \tEndothermic ReactionExothermic ReactionA reaction that the system absorbs energy from its surrounding in the form of heat.A reaction that releases energy from the system in the form of heat.The energy is absorbed from the surround into the reactionThe energy is released from the system to its environment.Energy in the form of heatEnergy is released as heat, electricity, light or sound.Melting ice, evaporation, cooking, gas molecules, photosynthesis are few examplesRusting iron, settling, chemical bonds, explosions, nuclear fission are few examples.\t | |
| 45. |
Give all possible values of l , me and ms for the orbital 3d? |
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| 46. |
Give an example of reaction of preparation of alkyne |
| Answer» Polymerisation | |
| 47. |
Diagonal relationship in periodic table |
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Answer» It applies to all the periods or only second period ?? The diagonal relationship is due to the similarity in ionic sizes and / or charge/radius ratio of the elements.eg.lithium shows similarity to magnesium and berilliyum to aluminium in many of their properties. |
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| 48. |
Find the wave number of the radiation of energy if n=1 jumps to n=2 |
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| 49. |
CH2=cH2+NaNH2 gives |
| Answer» | |
| 50. |
Explain f-centre |
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Answer» A compound may have excess metal ion. When negative ion is absent from its lattice side and compound have excess metal ion and leaving a hole which occupied by electron to maintain electrical neutrality , the ionic sites are called F center .Colour in these crystals are impart by unpaired electrons.These types of defects are found in crystals which have electric neutrality and Schoottky defects .The hole occupied by electron is called F–center. This F center is responsible for most of the interstitial properties of compound .For example We observe this effect when Crystals of NaCl heated in an atmosphere of sodium vapour. An F-Center or Farbe (German for colour) center is a type of crystallographic defect in which an anionic vacancy in a crystal is filled by one or more electrons, depending on the charge of the missing ion in the crystal or mainly due to the reason that when a compound is heated to a high temperature (mainly metallic oxides) the ions get excited and get displaced from their respective positions in their crystal structure but while doing so these ions leave behind some electrons in the vacated spaces. This leads to the phenomenon of colouring of compounds. This is used to identify many compounds, especially zinc oxide (yellow). Electrons in such a vacancy tend to absorb light in the visible spectrum such that a material that is usually transparent becomes colored. Thus the origin of the name, F-center, which originates from the German Farbzentrum. The translation of this term also provides the synonym color center, which can also refer to such defects. F-centers are often paramagnetic and can then be studied by electron paramagnetic resonance techniques. The greater the number of F-centers, the more intense is the color of the compound. A way of producing F centers is to heat a crystal in the presence of an atmosphere of the metal that constitutes the material, e.g.: NaCl heated in a metallic Na atmosphere. |
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