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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. |
What is the difference between polar and non polar covalent bonds? |
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Answer» Polar covalent bond means there is electronegativity difference in the atoms forming covalent bond.for example HCI, H is electropositive in nature whereas Cl is electronegative .Non polar covalent bond means there is no electronegativity difference between the atoms forming covalent bond.for example Cl2\xa0 Ans.\xa0Polar covalent bonding\xa0is a type of chemical bond where a pair of electrons is unequally shared between two atoms. In a polar covalent bond, the electrons are not equally shared because one atom spends more time with the electrons than the other atom. In polar covalent bonds, one atom has a stronger pull than the other atom and attracts electrons. e.g. H2ONonpolar covalent bonds\xa0are a type of bond that occurs when two atoms share a pair of electrons with each other. These shared electrons glue two or more atoms together to form a molecule. e.g. Cl2 |
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| 2. |
Calculate the mass of 1 molecule of O3 and Na\xa0 |
| Answer» 1) 1mole of O3\xa0weighs 48g. 1mole contains 6.022*10^23 molecules.So 1molecule of O3 weighs (48*1)/6.022*10^23 g. =7.97*10^-23g.2) 1 mole of Na weighs 23g. The same way,1molecule of Na weighs (23*1)/6.022*10^23 g. =3.81*10^-23g. | |
| 3. |
IUPAC\xa0name\xa0of\xa0compound CH3-O-CH2-O-CH2-CH2-O-CH3 |
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Answer» Sorry : Correct name is\xa01-Methoxy-2-(MethoxyMethoxy)Ethane\xa0 Solution : IUPAC Name of\xa0compound CH3-O-CH2-O-CH2-CH2-O-CH3 is 1-methoxy-2-(2-methoxymethoxy)ethane.\xa0 Ans.\xa01-Methoxy-2-(2-MethoxyMethoxy)Ethane |
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| 4. |
Give examples of intramolecular hydrogen bonding\xa0 |
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Answer» Ans.\xa0When the hydrogen bond is present between two atoms of the same molecule, then it is known as intramolecular hydrogen bond.For example, intramolecular hydrogen bonding occurs in ethylene glycol (C2H4(OH)2) between its two hydroxyl groups due to the molecular geometry. When the hydrogen bond is present between two atoms of the same molecule, then it is called as intramolecular hydrogen bond.Eg. In the above image, the dotted line represents the intramolecular bonding between hydrogen and oxygen of the same molecule. |
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| 5. |
IUPAC NAME OF CH3COCH2CH2CH2COOH |
| Answer» Ans.\xa05-oxohexanoic acid | |
| 6. |
What is buffer solution\xa0 |
| Answer» Ans.\xa0A buffer solution is one which resists changes in pH when small quantities of an acid or an alkali are added to it.A common example would be a mixture of ethanoic acid and sodium ethanoate in solution. | |
| 7. |
HF is more polar than HCl give reason? |
| Answer» Fluorine is more electronegative than chlorine. Hence, HF has more polarity than HCl.\xa0 | |
| 8. |
Arrange in increasing order of non metallic character\xa0Nitrogen,phosphorus,oxygen,sulphur |
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| 9. |
Meaning of neucleophile |
| Answer» Ans.\xa0A Nucleophile\xa0is a chemical species that donates an electron pair to an electrophile to form a chemical bond in relation to a reaction. All molecules or ions with a free pair of electrons or at least one pi bond can act as Nucleophiles. Because\xa0nucleophiles\xa0donate electrons, they are by\xa0definition\xa0Lewis bases. | |
| 10. |
Did noble gases have largest size in their own period ? |
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| 11. |
What is scrondinger equation. |
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| 12. |
How is that silicon atoms can have a coordination number more than four but carbon atom cannot? |
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| 13. |
Define entropy and show entropy is a state function\xa0 |
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| 14. |
Define entropy\xa0 |
| Answer» Ans.\xa0Entropy is a thermodynamic state quantity which is a measure of randomness or disorder of the molecules of the system. | |
| 15. |
Balance the equation by basic medium by ion electron method\xa0P4 \xa0+OH-\xa0-> PH3 + HPO2-\xa0 |
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| 16. |
What is redox reactions ? All chemical reactions are redox ,if not why? |
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| 17. |
discuss the diagonal relationship between Be\xa0and Al |
| Answer» Ans. The ionic radius of Be2+\xa0is estimated to be 31 pm : the charge/ radius ratio is nearly the same as that of the Al3+\xa0ion. Hence beryllium resembles aluminium in some ways. Some of the similarities are:\tLike aluminum, beryllium is not readily attacked by acids because of the presence of an oxide film on the surface of the metal.\tBeryllium hydroxide dissolves in excess of alkali to give a beryllate ion, just as aluminium hydroxide gives aluminate ion.\tThe chlorides of both beryllium and aluminium have Cl- bridged chloride structure in vapour phase. Both the chlorides are soluble in organic solvents and are strong Lewis acids. They are used as Friedel Craft catalysts.\tBeryllium and aluminium ions have strong tendency to form complexes. | |
| 18. |
compare the structure of water molecule and ice? |
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| 19. |
Limiting reagent\xa0 |
| Answer» The\xa0limiting reagent\xa0(or\xa0limiting reactant) in a chemical reaction is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this\xa0reagent, since the reaction cannot continue without it. | |
| 20. |
what is syn gas and how it is prepared nowdays |
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| 21. |
Oxidation number of N in (NH4)2 SO4\xa0 |
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| 22. |
Explanation of hydrogen spectrum and equation\xa0 |
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| 23. |
Calculate lemda neu and energy for the last line of each Series\xa0 |
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| 24. |
Five\xa0properties of electromagnetic spectrum.\xa0 |
| Answer» \xa0\tElectromagnetic waves are propagated by oscillating electric and magnetic fields oscillating at right angles to each other.\tElectromagnetic waves travel with a constant velocity of 3 x 108\xa0ms-1\xa0in vacuum.\t\xa0Electromagneticwaves are\xa0not deflected\xa0by electric or magnetic field.\tElectromagneticwaves can show\xa0interference\xa0or\xa0diffraction.\tElectromagneticwaves are\xa0transverse waves. | |
| 25. |
5 differences between a pure substance and a mixture |
| Answer» \tPropertiesPure SubstanceMixtureDefineThe substances that are made of a single element or compound are called pure substancesSeveral elements & compounds together form a mixtureCategorizationSolid, liquid, gasHeterogeneous, homogeneousPhysical propertiesConstantVaryPurityPureImpureSeparation by a physical processNot possiblePossible to separate by evaporation, magnetic separation, etc.Chemical propertiesConstantVaryExampleGold, pure water, hydrogen gasOil & water, sand & sugar\t | |
| 26. |
What mass of carbon will be present in 342gram sample of sucrose(C12H22O11) |
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| 27. |
Find the no. Of molecules of 4.25g ammonia |
| Answer» Molar mass NH3 = 14+3 = 17g/mol4.25g = 4.25/17 = 0.25 molNH3 1mol = 6.022 {tex}\\times {/tex}1023 molecules0.25 mol = 0.25 {tex}\\times{/tex}6.022 {tex}\\times {/tex}1023Number of molecules = 1.51 {tex}\\times{/tex}1023\xa0 | |
| 28. |
Find no. Of moles of.25g of ammonia |
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| 29. |
Find mass of 3g atom magnesium |
| Answer» Ans. Molecular mass if Magensium = 24.3\xa0So No of Atoms in 24.3 g of Magnesium =\xa0{tex}6.022 \\times 10^{23}{/tex}No of Atoms in 1 g of Magnesium = {tex}6.022\\times 10^{23}\\over 24.3{/tex}No of Atoms in 3 g of Magnesium =\xa0{tex}{6.022\\times 10^{23}\\over 24.3}\\times 3{/tex}\xa0=\xa0{tex}0.743 \\times 10^{23}{/tex} | |
| 30. |
Find the no. Of atoms in 24g sample of C12 |
| Answer» Molecular Mass of 12C = 12\xa0No of Atoms in 12g of\xa012C = 6.022 × 1023No of Atoms in 1g of\xa012C ={tex}{1\\over 12 }\\times {/tex} 6.022 × 1023No of Atoms in 20g of\xa012C ={tex}{20\\over 12}\\times {/tex}6.022 × 1023 =\xa0{tex}10.036 \\times 10^{23}{/tex}\xa0 | |
| 31. |
Why metals are melleable and ductile?give sutaible reason. |
| Answer» Metals are malleable and ductile because they are made of hexagonal and cubic packed structures that can be moved by applying force to them. When force is applied, the atoms slide from one plane past atoms in a different plane. | |
| 32. |
400 ml\xa0 |
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| 33. |
What is equivalent mass? |
| Answer» It is defined as the mass of an element/compound/ion which combines or displaces 1 part of hydrogen or 8 parts of oxygen or 35.5 parts of chlorine by mass.It is not always possible to apply this classic definition to determine equivalent weights of chemical entities. | |
| 34. |
Calculate the mole fraction of nitrogen when 28 g of nitrogen is mixed with 64 g of oxygen gas . |
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| 35. |
what is NTP and STP???\xa0\xa0 |
| Answer» STP stands for Standard Temperature and Pressure.NTP stands for Normal Temperature and Pressure.\xa0At STP: Pressure = 1 bar = 0.987 atmTemperature = 273 K or 0°CAt NTP:\xa0Pressure = 1 atmTemperature = 293 K or 20°C\xa0 | |
| 36. |
When water is added, pH of acidic solution...A) remains sameB) increasesC) decresesD) becomes zero |
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Answer» Increase\xa0 B) IncreaseExplanation : When you add pure water to an acidic solution, the solution becomes less acidic and the pH goes up -- to a point. For example, if you add pure water to a relatively acidic solution that has a pH of 3.5, the pH level might go up to a 4 or 5. You cannot, though, turn an acidic solution into a base solution or make it neutral just by adding water. As a result, pure water can only raise the pH of an acidic solution to a maximum of a 6.9. |
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| 37. |
How has Avogadro\'s hypothesis helped in making distinguish between atom and molecules |
| Answer» Avogadro’s assertion is a “law” rather than a “hypothesis” or a “theory” precisely because it has withstood two centuries of rigorous usage and observation. Indeed the point of the law is that the volume of a gas does NOT depend on the size of the molecules. That said, it has been recognized from the start that Avogadro’s Law presumes an “ideal gas”. Deviations from ideal behavior are expected, for example, when gas molecules reversibly interact with one another or when gases are highly compressed. | |
| 38. |
JJ thomson model explain\xa0 |
| Answer» J.J Thomson gave the first model of an atom in which its model is compared with a water melon or Christmas pudding. The reddish part of water melon represents positive charge ( protons ) and seeds embedded in it reflect negative charge ( electrons) . The total amount of positive charge is equal to total amount of negative charge. An atom as a whole is electrically neutral.Limitations:-\xa01. This model didn\'t get experimental support and hence discarded.2. This model could not explain the stability of an atom as there is no boundary of separation between positive and negative charge | |
| 39. |
What is the difference between oxygen gas and dioxygen and their masses? |
| Answer» Dioxygen means O\u200b\u200b\u200b\u200b\u200b\u200b2 Oxygen basically exists as a diatomic gas, that is two oxygen atoms chemically combine to form an oxygen molecule which is denoted by\xa0O\u200b\u200b\u200b\u200b\u200b\u200b2 In other words, dioxygen is the elemental form of oxygen. So, if in a question only oxygen gas has been mentioned then we will consider O\u200b\u200b\u200b\u200b\u200b\u200b2 and take 32g as the molar mass because atomic mass of oxygen = 16uSo molecular mass of of oxygen gas (O\u200b\u200b\u200b\u200b\u200b\u200b2) = 2 X 16 = 32 u and hence molar mass of oxygen gas = 32gOtherwise, if oxygen molecule is mentioned, then it is quite clear that you will consider dioxygen and take 32g as the molar mass. However, if in the question specifically oxygen atom has been mentioned, then O atoms will be considered and the molar mass will be taken as 16g, because here we are talking about oxygen atoms, and not oxygen molecules. | |
| 40. |
What is difference between molality and molarity |
| Answer» Molality vs. Molarity:\xa0These two words sound similar but they are not synonyms, even though both of them are used for representing solution concentration. By definition, molarity is the number of moles of solute dissolved per liter of solution. We use capital letter “M” to represent molarity and its formula is M= (# mol SOLUTE)/ (Liters of SOLUTION).Molality is then the number of moles of solute per kilogram of the SOLVENT, NOT solution! We use lower case letter “m” to represent molality and its formula can be represented as: m= (# mole SOLUTE) / (Kilograms of SOLVENT).Most of the time scientists use either molarity or molality to represent solution concentration, but MOLALITY is preferred when the temperature of the solution varies. That is because MOLALITY does not depend on temperature, (Neither number of moles of solute nor mass of solvent will be affected by changes of temperature.) while MOLARITY changes as temperature changes. (Volume of solution in the formula changes as temperature changes, and that is why.) | |
| 41. |
Structure of SO42- |
| Answer» https://youtu.be/lEjQKATnI2A | |
| 42. |
What do you mean by hybridization of carbon |
| Answer» Hybridization happens when atomic orbitals mix\xa0to form new atomic orbitals. The new orbitals have the same total electron capacity as the old ones. The properties and energies of the new, hybridized orbitals are an \'average\' of the original unhybridized orbitals. | |
| 43. |
who founded chemistry |
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Answer» The distinction began to emerge when a clear differentiation was made between chemistry and alchemy by Robert Boyle in his work The Sceptical Chymist (1661) Robert boyle is the father of chemistry.\xa0 |
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| 44. |
How many gram molecules are present in 49 grams of h2so4 |
| Answer» calculate molecular mass of H2SO4\xa0\xa0that is = (1*2)+(1*32)+(4*16)=2+32+64=98so 98 gram of\xa0H2SO4= 1 mole49 gram of\xa0H2SO4 = X moleX=(1*49)/98=.5 moles\xa0\xa0 | |
| 45. |
All special cases of electronic configuration of elements?\xa0 |
| Answer» An atom\'s electron configuration is a numeric representation of its electron orbitals. Electron orbitals are differently-shaped regions around an atom\'s nucleus where electrons are mathematically likely to be located. An electron configuration can quickly and simply tell a reader how many electron orbitals an atom has as well as the number of electrons populating each of its orbitals. Once you understand the basic principles behind electron configuration, you will be able to write your own configurations and tackle those chemistry tests with confidence.Method1 Assigning Electrons Using a Periodic Table1 Find your atom\'s atomic number. Each atom has a specific number of electrons associated with it. Locate your atom\'s chemical symbol on the periodic table. The atomic number is a positive integer beginning at 1 (for hydrogen) and increasing by 1 for each subsequent atom. The atom\'s atomic number is the number of protons of the atom - thus, it is also the number of electrons in an atom with zero charge.2 Determine the charge of the atom. Uncharged atoms will have exactly the number of electrons as is represented on the periodic table. However, charged atoms will have a higher or lower number of electrons based on the magnitude of their charge. If you\'re working with a charged atom, add or subtract electrons accordingly: add one electron for each negative charge and subtract one for each positive charge.For instance, a sodium atom with a +1 charge would have an electron taken away from its basic atomic number of 11. So, the sodium atom would have 10 electrons in total.3 Memorize the basic list of orbitals. As an atom gains electrons, they fill different orbitals sets according to a specific order. Each set of orbitals, when full, contains an even number of electrons. The orbital sets are:The s orbital set (any number in the electron configuration followed by an "s") contains a single orbital, and by Pauli\'s Exclusion Principle, a single orbital can hold a maximum of 2 electrons, so each s orbital set can hold 2 electrons.The p orbital set contains 3 orbitals, and thus can hold a total of 6 electrons.The d orbital set contains 5 orbitals, so it can hold 10 electrons.The f orbital set contains 7 orbitals, so it can hold 14 electrons. Remember the order of the letters with this mnemonic:[1]Sober Physicists Don\'t Find Giraffes Hiding In Kitchens.For atoms with even more electrons, the orbitals continue alphabetically past K, skipping letters already used.4 Understand electron configuration notation. Electron configurations are written so as to clearly display the number of electrons in the atom as well as the number of electrons in each orbital. Each orbital is written in sequence, with the number of electrons in each orbital written in superscript to the right of the orbital name. The final electron configuration is a single string of orbital names and superscripts.For example, here is a simple electron configuration: 1s2 2s2 2p6. This configuration shows that there are two electrons in the 1s orbital set, two electrons in the 2s orbital set, and six electrons in the 2p orbital set. 2 + 2 + 6 = 10 electrons total. This electron configuration is for an uncharged neon atom (neon\'s atomic number is 10.)5 Memorize the order of the orbitals. Note that orbital sets are numbered by electron shell, but ordered in terms of energy. For instance, a filled 4s2 is lower energy (or less potentially volatile) than a partially-filled or filled 3d10, so the 4s shell is listed first. Once you know the order of orbitals, you can simply fill them according to the number of electrons in the atom. The order for filling orbitals is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s.An electron configuration for an atom with every orbital completely filled would be written: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d107p6Note that the above list, if all the shells were filled, would be the electron configuration for Og (Oganesson), 118, the highest-numbered atom on the periodic table - so this electron configuration contains every currently known electron shell for a neutrally charged atom.6 Fill in the orbitals according to the number of electrons in your atom. For instance, if we want to write an electron configuration for an uncharged calcium atom, we\'ll begin by finding its atomic number on the periodic table. Its atomic number is 20, so we\'ll write a configuration for an atom with 20 electrons according to the order above.Fill up orbitals according to the order above until you reach twenty total electrons. The 1s orbital gets two electrons, the 2s gets two, the 2p gets six, the 3s gets two, the 3p gets 6, and the 4s gets 2 (2 + 2 + 6 +2 +6 + 2 = 20.) Thus, the electron configuration for calcium is: 1s2 2s2 2p6 3s2 3p6 4s2.Note: Energy level changes as you go up. For example, when you are about to go up to the 4th energy level, it becomes 4s first, then 3d. After the fourth energy level, you\'ll move onto the 5th where it follows the order once again. This only happens after the 3rd energy level.7 Use the periodic table as a visual shortcut. You may have already noticed that the shape of the periodic table corresponds to the order of orbital sets in electron configurations. For example, atoms in the second column from the left always end in "s2", atoms at the far right of the skinny middle portion always end in "d10," etc. Use the periodic table as a visual guide to write configurations - the order that you add electrons to orbitals corresponds to your position in the table. See below:Specifically, the two leftmost columns represent atoms whose electron configurations end in s orbitals, the right block of the table represents atoms whose configurations end in p orbitals, the middle portion, atoms that end in d orbital, and the bottom portion, atoms that end in f orbitals.For example, when writing an electron configuration for Chlorine, think: "This atom is in third row (or "period") of the periodic table. It\'s also in the fifth column of the periodic table\'s p orbital block. Thus, its electron configuration will end ...3p5Caution - the d and f orbital regions of the table correspond to energy levels that are different than the period they\'re located in. For instance, the first row of the d orbital block corresponds to the 3d orbital even though it\'s in period 4, while the first row of the f orbital corresponds to the 4f orbital even though it\'s in period 6.8 Learn shorthand for writing long electron configurations. The atoms along the right edge of the periodic table are called noble gases. These elements are very chemically stable. To shorten the process of writing a long electron configuration, simply write the chemical symbol of the nearest chemical gas with less electrons than your atom in brackets, then continue with the electron configuration for the following orbital sets. See below:To understand this concept, it\'s useful to write an example configuration. Let\'s write a configuration for Zinc (atomic number 30) using noble gas shorthand. Zinc\'s full electron configuration is: 1s2 2s2 2p6 3s2 3p6 4s2 3d10. However, notice that 1s2 2s2 2p6 3s2 3p6 is the configuration for Argon, a noble gas. Just replace this portion of Zinc\'s electron notation with Argon\'s chemical symbol in brackets ([Ar].)So, Zinc\'s electron configuration written in shorthand is [Ar]4s2 3d10.Method2 Using an ADOMAH Periodic TableUnderstand the ADOMAH Periodic Table. This method of writing electron configurations doesn\'t require memorization. However, it does require a rearranged periodic table, because in traditional periodic table, beginning with fourth row, period numbers do not correspond to the electron shells. Find an ADOMAH Periodic Table, a special type of periodic table designed by scientist Valery Tsimmerman. It\'s easily found via a quick online search.[2]1 In the ADOMAH Periodic Table, horizontal rows represent groups of elements, such as halogens, inert gases, alkali metals, alkaline earths, etc. Vertical columns correspond to electron shells and so called “cascades” (diagonal lines connecting s,p,d and f blocks) correspond to periods.Helium is moved next to Hydrogen, since both of them are characterized by the 1s orbital. Blocks of periods (s,p,d and f) are shown on the right side and shell numbers are shown at the base. Elements are presented in rectangular boxes that are numbered from 1 to 120. These numbers are normal atomic numbers that represent total number of electrons in a neutral atom.2 Find your atom in the ADOMAH table. To write electron configuration of an element, locate its symbol in ADOMAH Periodic Table and cross out all elements that have higher atomic numbers. For example, if you need to write electron configuration of Erbium (68), cross out elements 69 through 120.Notice numbers 1 through 8 at the base of the table. These are electron shell numbers, or column numbers. Ignore columns which contain only crossed out elements. For Erbium remaining columns are 1,2,3,4,5 and 6.3 Count orbital sets up to your atom. Looking at the block symbols shown on the right side of the table (s, p, d, and f) and at the column numbers shown at the base and ignoring diagonal lines between the blocks, break up columns into column-blocks and list them in order from the bottom up. Again, ignore column blocks where all elements are crossed out. Write down the column-blocks beginning with the column number followed by the block symbol, like this: 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 6s (in case of Erbium).Note: The above electron configuration of Er is written in the order of ascending shell numbers. It could also be written in the order of orbital filling. Just follow cascades from top to bottom instead of columns when you write down the column-blocks: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f12.4Count electrons for each orbital set. Count elements that were not crossed out in each block-column, assigning one electron per element, and write down their quantity next to the block symbols for each block-column, like this: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f12 5s2 5p6 6s2. In our example, this is is the electron configuration of Erbium.5 Know irregular electron configurations. There are eighteen common exceptions to electron configurations for atoms in the lowest energy state, also called the ground state. They deviate from the general rule only by last two-to-three electron positions. In these cases, the actual electron configuration keeps the electrons in a lower-energy state than in a standard configuration for the atom. The irregular atoms are:Cr (..., 3d5, 4s1); Cu (..., 3d10, 4s1); Nb (..., 4d4, 5s1); Mo (..., 4d5, 5s1); Ru (..., 4d7, 5s1); Rh (..., 4d8, 5s1); Pd (..., 4d10, 5s0); Ag (..., 4d10, 5s1); La (..., 5d1, 6s2); Ce (..., 4f1, 5d1, 6s2); Gd (..., 4f7, 5d1, 6s2); Au (..., 5d10, 6s1); Ac (..., 6d1, 7s2); Th (..., 6d2, 7s2); Pa (..., 5f2, 6d1, 7s2); U (..., 5f3, 6d1, 7s2); Np (..., 5f4, 6d1, 7s2) and Cm (..., 5f7, 6d1, 7s2). | |
| 46. |
Why ionization energy is less for oxygen than nitrogen? |
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Answer» This is due to an electron being added to an already half full orbital in oxygen, which results in electron electron repulsion, which will lower the ionisation energy. Nitrogen also has the added stability of a half filled shell of electrons in the 2p shell This is due to an electron being added to an already half full orbital in oxygen, which results in electron electron repulsion, which will lower the ionisation energy. Nitrogen also has the added stability of a half filled shell of electrons in the 2p shell. |
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| 47. |
What is atomic scale?? In work function\xa0 |
| Answer» This group focuses on probing the atomic scale structure and electronic properties of molecules and nanostructures using low-temperature scanning tunnelling microscopy (STM) and atomic force microscopy (AFM). We have a particular interest in fabricating and characterizing atomically well-defined nanostructures to study physical phenomena at the nanoscale.\xa0 | |
| 48. |
What is effective nuclear charge\xa0 |
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| 49. |
Difference b/w ionization potential and work function |
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| 50. |
how to find the electronic configuration of element in organic chemistry |
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Answer» |
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