InterviewSolution
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InterviewSolution
This section includes InterviewSolutions, each offering curated multiple-choice questions to sharpen your Class 11 knowledge and support exam preparation. Choose a topic below to get started.
| 101. |
Why is it not possible to cool a gas to 0 k ? |
| Answer» Because 0k is equal to the 273c | |
| 102. |
What is kolbe reactions |
| Answer» Kolbe’s reaction: When phenol is treated with sodium hydroxide, sodium phenoxide is produced. This sodium phenoxide when treated with carbon dioxide, followed by acidification, undergoes electrophilic substitution to give ortho-hydroxybenzoic acid as the main product. This reaction is known as Kolbe’s reaction. | |
| 103. |
Why did Heisenberg replace the concept of definite orbit by the concept of probabilty |
| Answer» Because if we have definite orbit then we can find out momentum and position of an moving electron simultaneously but he proved experimentally that it is impossible to find out both position and momentum simultaneously<br>Because I don\'t know | |
| 104. |
What is quarks |
| Answer» A quark is a type of elementary particle and a fundamental consitutent of matter quarks combine to form composite particles called hadrons,the most stable of which are protons and neutrons,the component of atomic nuclic. SPIN_1/2COMPOSITION_ elementary particle | |
| 105. |
Electroconifergution |
| Answer» Name the element then i send u electroniconfiguration of it.... OK Mahesh | |
| 106. |
Diffrence between sigma bond and pi bond. |
| Answer» Sigma bond is single bond n pi bond is double bond.<br>Sigma bond is formed by axial overlapping while pi bond is formed by side to side overlapping of two orbitals<br>Pi bond is weak bond<br>Sigma bond is strong bond | |
| 107. |
What is hybridization and its types? |
| Answer» Hybridization happens when atomic orbitals mix to form a new atomic orbital. The 3 types r sp3 single bond, sp2 double bond and sp triple bond. | |
| 108. |
How the atomic radii changes across the period? |
| Answer» Increase in Nuclear charge and decrease in atomic size.......both are inversely proportional<br>The atomic radii decreases because when we move from left to right in a period the no. of electron increases and charge of proton also increase then the proton charge also attract the valence electron then that lead to the decrease in atomic radii.??????<br>because when we move left to right then size of atom decrease due increase in atomic nuclear charge and no. of electron on orbit | |
| 109. |
Hey buddy Can u explain me formal charge? |
| Answer» It denotes the difference in valence electrons in free atom and number of electrons assigned to that atom in lewis dot structureNo of valence electrons in free atom - number of bonding electrons - half of no. of bonding electrons | |
| 110. |
What is plank quantum theory |
| Answer» According to plank energy trevels in the form of small packets called quanta.In case of light these quantas are known as photon and the energy of each quanta is directly proportional to the frequency of radiation.E is proportional to VE = h newWhere h is plank constant which is 6.62×10*-34 JS<br>-346.626*(10) | |
| 111. |
Characteristics of groups and period in periodic table |
| Answer» All elements of a single group have similar physical and chemical properties.While in a period, all elements have same number of shells or orbits. | |
| 112. |
What are completely filled orbital |
| Answer» Orbitals having 0 valency and which are fully stable.<br>It means fully stabled | |
| 113. |
Describe the absorption and emission spectra of atom |
| Answer» | |
| 114. |
Question no 2 |
| Answer» | |
| 115. |
How much iron can be obtain by the reduction of 1 kg of fe2o3 |
| Answer» 700 grams iron can be obtained by the reduction of 1 kg of Fe2o3. | |
| 116. |
What is the photo electric effect |
| Answer» It is the phenomenon in which the surface of alkali metal like potassium and calcium emit electron on their own when the beam of light with high frequency is made to fall on them<br>“The phenomenon of ejection of electrons from the surface of a metal when light of suitable frequency strikes on it, is called photoelectric effect.The emitted electrons are called photoelectrons.”Experimental studies of photoelectric effect under different conditions led to the following important observations—(i) The electrons are ejected from the metal surface as soon as the beam of light strikes the surface. .(ii) For each metal, certain minimum frequency of light is needed to eject the electrons. This is known as threshold frequency and it is different for different metals.(iii) The kinetic energy of the ejected electrons is directly proportional to the frequency of the incident radiation and it is independent of its intensity.(iv) The number of electrons ejected per second from the metal surface depends upon the intensity or brightness of incident radiation but does not depend upon its frequency | |
| 117. |
List of no of valence electrons of elements having atomic number 1 to 30. |
| Answer» 1-12-03-14-25-36-47-38-29-110-0 | |
| 118. |
why is neurton is not attracting to electron ? |
| Answer» Because it is neutral in nature.<br>Because its neither positive niether negative | |
| 119. |
Zeema effect in magnetic quantum number. |
| Answer» It is the phenomenon of splitting up of spectral lines on influencing through magnetic field. | |
| 120. |
Biogas contains CH4. How much mass of dioxygen is needed to burn 2kg of it? |
| Answer» 1 mol CH4 = 12+4 =16g1g=1÷16mol 1kg = 1÷16×2000 = 125 mol1 mol CH4 requires 2 mol of O2.Therefore, 125 mol of CH4 requires O2 = 125 ÷2 = 62.5 mol OR62.5 × 16 = 1000 g OR 1Kg. | |
| 121. |
What is the limitation of mendeleeve periodic table? |
| Answer» Yogita Ingle has written all the points..so i think we should not ans it again??<br>Limitations of Mendeléev’s classification\tNo fixed position could be assigned to hydrogen in the Periodic Table.\tIsotopes discovered long after Mendeléev periodic classification of\telements imparted a challenge to Mendeleev’s Periodic Law.\tThe atomic masses of elements did not increase in a steady manner while going from one element to other which made it difficult to predict the number of elements that could be discovered between two elements. | |
| 122. |
What is difference between molar and molecular mass |
| Answer» What is mole.?<br>Thanks<br>\tMOLAR MASSMOLECULAR MASSRefers to mass of a mole of a substanceRefers to the mass of moleculesAlso known as molecular weightIt determines the mass of single moleculeSI unit is g/mol to use in higher calculationsMeasured in amuIt is defined as the mass of Avogadro number of atoms/molecules or compoundsNo particular melting pointMeasurement given to compounds, atoms or moleculesDetermined only in moleculesLess accurate than molecular massAccurate to use in higher calculationsExample: Mass of 1 mole of oxygen is 15.9994 grams. Therefore the molar mass = 15.9994 g/molExample: Molecular mass of Ca(OH)2 = 74 atomic mass units\t<br>Molar mass is mass of 1 mole of that substance and molecular mass is mass of one molecule of that substance | |
| 123. |
Kmno4+koh=k2mno4+mno2+o2 balance this equation |
| Answer» Equation is wrong because In reactent h is present but not present in product | |
| 124. |
How do atomic radius vary in a period & in a group? How do you explain the variation |
| Answer» Atomic radius decreases in periods because of the increasing of effective nuclear charge and increases in the groups because of formation of new shells. | |
| 125. |
Addition of significant figures |
| Answer» What do you mean by this | |
| 126. |
Calculate the mass of one mole of KNO3 |
| Answer» 1 mole of kno3 .We know that no.of moles = mass/ molecular mass then here mole if given.(1)mole of kno3 then 1=m/atomic mass of k+n+o3. Then 1=m/39+14+48.1=M/101. Then M=1×101 then mass of one mole of kno3 is 101. | |
| 127. |
What are magic ions? From chapter 3rd |
| Answer» | |
| 128. |
Why electron are filled up in 4s orbital before 3d orbital |
| Answer» Hello bisvanath can u tell me ur real name because this is so large and teeepical<br>Because if you take any element whose electron also move in 4th shell then you first write 1s to 4s.<br>Hello ,Do you understand my answer ? Please tell me . I am waiting for ur answer biswanath<br>Because electrons are filled by serial wise like maths counting 1,2,3.......100 so electronic configuration is starts from 1s,2s,2p,3s,3p,3d,3f ,4s ,4p and so on | |
| 129. |
Calculate the percentage composition of CuSo4.5H2O |
| Answer» | |
| 130. |
Why KHF2 exist but KHCl 2 does not? |
| Answer» Due to the presence of hydrogen bonding in HF, the structure is converted to,\xa0This can dissociate to give\xa0{tex} \\mathrm{HF}_{2}^{-} {/tex}\xa0ion.If we add K+\xa0to\xa0{tex} \\mathrm{HF}_{2}^{-} {/tex}\xa0ion, we get\xa0KHF2.Due to the absence of hydrogen bonding in HCl,\xa0{tex} \\mathrm{HCl}_{2}^{-} {/tex}\xa0ion is not formed.Hence, KHCI2\xa0does not exist.Therefore,\xa0KHF2\xa0exists but KHCl2\xa0does not exist. | |
| 131. |
Which of the following has the shortest bond length? NO, NO+, NO2+, NO-. |
| Answer» NONumber of electrons\xa0= 15Electronic configuration =\xa0{tex} \\sigma \\mathrm{1s}^{2}, \\sigma^{*} \\operatorname{1s}^{2}, \\sigma 2 s^{2}, \\sigma^{*} 2 s^{2}, \\sigma 2 p_{z}^{2}, {/tex}{tex} \\pi 2 p_{x}^{2}=\\pi 2 p_{y}^{2}, \\pi^{*} 2 p_{x}^{1} {/tex}Bond order\xa0=\xa0{tex}\\frac {1} {2}{/tex}(10 - 5) = 2.5Magnetic property = Paramagnetic.NO+Number of electron = 14Electronic configuration =\xa0{tex} \\sigma \\mathrm{1s}^{2}, \\sigma^{*} \\mathrm{1s}^{2}, \\sigma 2 s^{2}, \\sigma^{*} 2 s^{2}, {/tex}{tex} \\sigma 2 p_{z}^{2}, \\pi 2 \\rho_{x}^{2}=\\pi 2 p_{y}^{2} {/tex}Bond order =\xa0{tex}\\frac {1} {2}{/tex}(10 - 4) = 3Magnetic property = Diamagnetic.{tex} \\mathrm{N} O^{2+} {/tex}Number of electrons = 13Electronic configuration =\xa0{tex} \\sigma \\mathrm{1s}^{2}, \\sigma^{*} \\mathrm{1s}^{2}, \\sigma 2 s^{2}, \\sigma^{*} 2 s^{2}, {/tex}{tex} \\sigma 2 p_{z}^{2}, \\pi 2 \\rho_{x}^{2}=\\pi 2 p_{y}^{1} {/tex}Bond order =\xa0{tex}\\frac {1} {2}{/tex}\xa0(9 - 4) = 2.5Magnetic property = ParamagneticNO-Number of electrons = 16Electronic configuration =\xa0{tex} \\sigma \\mathrm{1s}^{2}, \\sigma^{*} \\mathrm{1s}^{2}, \\sigma 2 s^{2}, \\sigma^{*} 2 s^{2}, {/tex}{tex} \\pi 2 p_{x}^{2}=\\pi 2 p_{y}^{2}, \\pi^{*} 2 p_{x}^{2} {/tex}Bond order =\xa0{tex}\\frac {1} {2}{/tex}(10 - 6) = 2Magnetic property = DiamagneticSince\xa0{tex} \\mathrm{NO}^{+} {/tex}\xa0has the highest bond order and therefore, it has\xa0the shortest bond length. | |
| 132. |
4g naoh dissolve in 90 gm of water find mole fraction of solute as well as solvant |
| Answer» | |
| 133. |
How many isotopes in periodic table |
| Answer» Every chemical element has one or more radioactive isotopes. For example, hydrogen, the lightest element, has three isotopes with mass numbers 1, 2, and 3. | |
| 134. |
Whats the difference between mole and molecule |
| Answer» Mole is a measurement of quantity whereas molecules is the part or chemical species of atom and molecules is made up of by combining of two or more atoms. | |
| 135. |
nacl becl2 and alcl3 which one is more covalent |
| Answer» | |
| 136. |
Al3+,Be2+,Na+ which is smaller cation. Why? |
| Answer» Al3+ because the ion with greater positive magnitude of charge is the smallest cation | |
| 137. |
Difference between mendeleev periodic table and modern periodic table |
| Answer» It is not important for exm<br>Mendeleev periodic table is not complete table because he can not explain the position of hydrogen and not full fill the all gap in periodic table. But modern periodic table is a table who gives the scientist NEILS BOHR . Now we used the atomic no. Of periodic table . Ok.<br>Somebody plz tell me where it is necessary or not<br>Not necessary from examination point of view | |
| 138. |
What is aufbau principal , hund rule , pauli rule |
| Answer» Aufbau principle : the electrons are filled in the orbital according to their increasing order of energyHund rule : no pairing of electrons can take place until and unless each of the orbital is singly occupiedPauli rule : no two electrons can have same set of four quantum numbers or two electrons in an orbital must different spins to attain stability in an atom where one electron revolves anti clockwise and the other clockwise or vice versa with charge +1/2 or -1/2 or vice versa accordingly | |
| 139. |
Which of the following is the smallest cation? Na+ , Mg2+ , Ca2+ , Sc3+. |
| Answer» Na+ as Na is smallest also it is cationOn comparing it with sc3+ .sc is much larger than na<br>Scandium 3+ | |
| 140. |
Why atoms with half filled and completely filled have extra stability? |
| Answer» Atoms are half filled and completely filled because of two reasons : 1. Symmetry distribution : we know that symmetry leads to stability. And an atom always tries to gain stability to remain balanced so half filled and complete orbitals are more stable2. Energy exchange : the stabilising effect arises whenever two or more than two electrons have same spin are present in the degenerate orbitals of a subshell these electrons tends to exchange their places and hence releases more energy which is calledvas exchange energy More the exchange of places more is the exchange energy and as a result the orbital or atom will be more stable | |
| 141. |
What is bond parameters? |
| Answer» Bond parameters refer to the characterization of covalent bond on the basis of various parameters like bond length, bond angle, bond enthalpy. | |
| 142. |
Balance this equation NH3 + O2 = NO + H2O |
| Answer» No this is wrong ans.<br>4NH3 + 5O2 = 4NO + 6H2O<br>4NH3 + 5O2=4NO + 6H2O<br>4NH3 + 5O2 = 4NO + 6H2O | |
| 143. |
What is the difference between atomic radii and ionic radii |
| Answer» Atomic radius is calculated by measuring the distance between the two atoms of the same element if the combined by single covalent bond.Ionic radius is calculated by measuring the distance between the two positive and negative ions enough compound formed by exchange of charges | |
| 144. |
Write short note on H-bonding in simple language. |
| Answer» Also explain its type.<br>H- bonding is the bonding of hydrogen with other atoms with a line from one side and a dotted line from other side.Types:-1.Intermolecular H-bonding.2.Intramolecular H-bonding. | |
| 145. |
Atomic theory |
| Answer» English | |
| 146. |
Explain with suitable example 1.molarity2.Limiting reagent |
| Answer» Molarity is defined as the number of moles with solute /disolve per litre solution | |
| 147. |
Properties of cathode and anode rays |
| Answer» Cathode rays consist of negatively charged particles.Anode rays consist of positively charged particles<br>Cathode rays travel in straight line. | |
| 148. |
A gas undergoes in volume from 1*10^-3 |
| Answer» | |
| 149. |
What is neutrino and antineutrino in atom?? |
| Answer» A Neutrino\xa0is an electrically neutral, weakly interacting\xa0subatomic particle\xa0with half integer spins.The neutrino (meaning "small neutral one" in Italian) is denoted by ?(nu).\xa0 | |
| 150. |
What is subatomic particle. |
| Answer» A Subatomic particle is nothing but a particle which is smaller than an atom in size. Typically, an atom can be broken down into three subatomic particles, namely: protons, electrons, and neutrons.<br>Subatomic particles are particles much smaller than atom i.e. electrons, protons and neutrons. | |