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PERIODIC TABLE in 1 Shot: All Concepts & PYQs Covered || JEE Main & Advanced

JEE Wallah・191 minutes read

The session covers element classification, historical milestones, and key concepts, emphasizing quick revision and understanding. Concepts like ionization enthalpy, electron gain enthalpy, and electronegativity are explained in detail for group elements, with mnemonic aids provided for memorization.

Insights

  • The session focuses on enhancing studies for 11th class students, covering the classification of elements and periodic properties with an emphasis on important concepts and previous year questions.
  • The historical development of element classification is discussed, starting from Lavoisier's simple classification to Mendeleev's periodic table and the Modern Periodic Table.
  • Uncle Dobereiner introduced triads like Lithium, Sodium, Potassium, Chlorine, Bromine, Iodine, Calcium, Strontium, and Barium, emphasizing quick revision related to 10th standard topics.
  • Lothar Mayer's curve and Moseley's experiment with X-rays are highlighted, providing insights into element classification based on atomic mass and number.
  • The significance of names and symbols in IUPAC nomenclature, as well as mnemonic aids for remembering elements in different groups and blocks, are discussed.
  • The concepts of ionization enthalpy, electron gain enthalpy, and electronegativity are explained, with detailed examples and trends provided to aid in understanding periodic properties.
  • The importance of understanding factors like hydration enthalpy, lattice enthalpy, and ionic mobility in predicting chemical behavior accurately is emphasized, along with specific examples and calculations to illustrate these concepts.

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Recent questions

  • What is the significance of Mendeleev's periodic table?

    Mendeleev's periodic table is a crucial historical development in the classification of elements. Mendeleev arranged elements based on increasing atomic mass and similar properties, leaving gaps for undiscovered elements. His table predicted the properties of these missing elements, showcasing the periodicity of elements' properties. This organization laid the foundation for the Modern Periodic Table, which is based on atomic number rather than atomic mass. Mendeleev's contributions revolutionized the understanding of element classification and paved the way for further advancements in chemistry.

  • How does electron affinity impact stability?

    Electron affinity plays a vital role in determining the stability of an element. If an element has a positive electron affinity, it indicates a desire to gain electrons for stability. Elements like beryllium, magnesium, nitrogen, and noble gases exhibit positive electron affinity. On the other hand, negative electron affinity signifies instability, as the element does not want to accept additional electrons. Understanding electron affinity is crucial in predicting an element's reactivity and chemical behavior, as it directly influences the element's stability and tendency to form bonds.

  • What is the relationship between ionization enthalpy and metallic character?

    Ionization enthalpy and metallic character are inversely related in the periodic table. Lower ionization enthalpy indicates that less energy is required to remove an electron from an atom, leading to higher metallic character. Cesium, for example, has the least ionization enthalpy in the periodic table, contributing to its high metallic character. Elements with low ionization enthalpy tend to readily lose electrons and exhibit metallic properties, such as conductivity and malleability. Understanding this relationship is essential in comprehending the behavior of metals and their properties in chemical reactions.

  • How does electronegativity impact chemical behavior?

    Electronegativity is a crucial concept in chemistry that influences an element's ability to attract bonded electrons towards itself. Elements with higher electronegativity values tend to attract electrons more strongly, leading to polar covalent bonds and specific chemical behaviors. Fluorine, the most electronegative element, exhibits a strong pull on electrons in a bond. Understanding electronegativity values helps predict the nature of chemical bonds, reactions, and the overall behavior of elements in compounds. It provides insights into the distribution of charge in molecules and the reactivity of different elements in various chemical environments.

  • What is the significance of hydration enthalpy in chemistry?

    Hydration enthalpy is a crucial concept in chemistry that relates to the energy released when an ion is surrounded by water molecules. The calculation of hydration enthalpy is proportional to the charge on the ion and inversely proportional to its size. This phenomenon impacts the hydrated radius and ionic mobility of ions in solution, influencing various chemical processes. Understanding hydration enthalpy helps explain the behavior of ions in aqueous solutions, their solubility, and interactions with other substances. It plays a vital role in determining the stability and reactivity of ions in different chemical environments.

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Summary

00:00

Enhancing 11th Class Studies: Element Classification Session

  • The session begins with greetings and a focus on enhancing studies for 11th class students.
  • The topic for the day is the classification of elements and periodic properties.
  • The session will cover important concepts and previous year questions.
  • The duration of the session is estimated to be around 4 to 4.5 hours.
  • The speaker is suffering from a cold and cough but is ready to proceed with the session.
  • The historical development of element classification is discussed, starting with Lavoisier's simple classification of metals and non-metals.
  • Dobereiner's Triad is introduced, focusing on the relationship between atomic masses of elements.
  • Newland's Law of Octaves and Lothar Mayer's curve are mentioned in the historical development.
  • Mendeleev's periodic table and the Modern Periodic Table are highlighted as key milestones.
  • The session emphasizes quick revision of topics and the importance of understanding the historical development of element classification.

14:11

"Periodic Table: Elements, Trends, and History"

  • The average of two numbers is 23.
  • Dobra Ener Uncle presented triads like Lithium, Sodium, Potassium, Chlorine, Bromine, Iodine, Calcium, Strontium, and Barium.
  • These triads are related to 10th standard topics for quick revision.
  • Uncle Dobereiner was a pioneer in arranging elements based on similar properties and increasing atomic mass.
  • Lothar Mayer arranged elements in a graph form, focusing on atomic volume versus atomic mass.
  • The graph showed peaks for elements like Lithium, Sodium, Potassium, and Rubidium.
  • The ascending and descending positions in the graph represent alkali metals, halogens, and alkaline earth metals.
  • Transition elements were also discussed in the context of the periodic table.
  • Uncle Mendeleev's tabular periodic table is considered a significant historical development.
  • The periodic function of elements' properties in relation to their atomic mass is a key concept in the periodic table.

28:14

"Periodic Table Evolution and Mnemonic Devices"

  • The group named Hai Zero Bhai is discussed, emphasizing the impact of names on perception and behavior.
  • The text delves into the origins of the periodic table, starting with Mendeleev's corrections to atomic mass calculations.
  • Mendeleev's predictions of certain elements and their properties are highlighted, showcasing his method of element classification.
  • The significance of Eka elements and their properties, like gallium's low melting point, is explained.
  • The concept of isotopes and their impact on the periodic table's structure is detailed.
  • The text introduces the idea of precious pairs in the periodic table, emphasizing the relationship between atomic numbers and masses.
  • Moseley's experiment with X-rays and the revelation of the direct proportionality between X-ray frequency and atomic number are discussed.
  • The transition to the modern periodic table based on atomic number is explained, highlighting its organization into groups, blocks, and periods.
  • An analysis of the periodic table's structure, including the positioning of elements and mnemonic devices for memorization, is provided.
  • The text concludes with a discussion on the elements in different groups and blocks of the periodic table, offering mnemonic aids for remembering their order.

42:12

Element Groups and Mnemonics in Chemistry

  • Elements are grouped together, with groups three, four, five, six, eight, ten, eleven, and twelve being mentioned.
  • The Fadi series starts in period five, followed by the 4d series.
  • Group six elements start with Lanthum, with a mnemonic provided for remembering the elements.
  • A sheikh named Rahman from Iran is mentioned, known for having a lot of money and purchasing gold and mercury.
  • Group three elements include Scandium, Trion, Lantham, and Actinium, with a mnemonic for remembering them.
  • Group 12 elements are important, including Zinc, Adam, and Mercury, known as coin age metals.
  • P Block Elements are discussed, starting with group 13 and mnemonic for remembering Borol.
  • Group 14 elements are associated with Kashi Esan Prabhu, while group 15 starts with nitrogen.
  • The Oxygen family is mentioned, with a mnemonic for remembering the elements.
  • The Lanthanide and Actinide series are detailed, with mnemonics provided for remembering the elements.

58:45

"Periodic Table: Elements, Patterns, and Nomenclature"

  • The sum of 18 and 14 equals 32, which is the maximum number in any period.
  • Element x in a group where the maximum element is y leads to questions about x/y, x*y, or x+y.
  • 71 people correctly answered a question in a poll, emphasizing participation and engagement.
  • Locating elements in the Modern Periodic Table involves identifying their period, group, and block.
  • The Modern Periodic Table includes seven periods, with specific ranges of elements in each.
  • The atomic number of noble gases follows a pattern in each period, aiding in element identification.
  • The "magic number" method simplifies determining an element's period based on its atomic number.
  • F block elements belong to groups 3-12, with specific ranges for Lanthanides and Actinides.
  • Electron configuration helps identify an element's period, block, and group in the Periodic Table.
  • IUPAC nomenclature provides a systematic way to name elements with atomic numbers over 100.

01:12:22

Naming and Symbolizing Numbers in Mathematics

  • The text discusses assigning symbols and names to numbers, starting with "p" for one, "six" for six, and "hex" for six as well.
  • It introduces the name "hept" for seven, explaining that "hept" won't give "sept," which is named for seven.
  • The text then moves on to naming "et" for seven and assigning the symbol "s" to it.
  • It continues by naming "chota o nine" for eight and assigning the symbol "E 10" to it.
  • The text emphasizes that the number ten will be represented by one and zero, symbolizing everything.
  • It discusses the significance of name endings, using examples like adding "um" to names in local languages.
  • The text then delves into a numerical exercise, asking for the name and symbol of 108, with participants providing answers like "Rahul Yum" and "Nikhilam."
  • It transitions to a chemistry question about an element's atomic number, with participants engaging in the exercise.
  • The text further engages participants in a question related to atomic numbers, with a focus on identifying elements based on their atomic numbers.
  • Finally, the text shifts to discussing effective nuclear charge, explaining the concept and introducing Slater's rule for calculating effective nuclear charge.

01:25:52

"Sigma Forest: Orbit Donations and Periodic Properties"

  • The forest in Sigma is called the whole forest, where everyone will contribute money.
  • Each person will donate money based on their potential, with donations coming into orbit.
  • Donations will be 35 paise for n-1 orbit, 85 paisa for n-2 orbit, and ₹1 for each electron.
  • Contributions are related to the penetration power of orbitals, with s having the highest and f the lowest.
  • The closest orbitals to the nucleus are s orbitals, while f orbitals are the farthest.
  • Shield power refers to the ability to shield electrons, with different orbitals having varying abilities.
  • Group 13 elements have many exceptions, with the 13th floor often omitted due to superstitions.
  • Periodic properties include atomic and ionic sizes, ionization enthalpy, electron gain enthalpy, and electronegativity.
  • Atomic size decreases left to right and increases top to bottom, with noble gases having the largest size.
  • Wonder Wall radius is used to compare metallic and intermolecular distances, especially in gases.

01:40:06

Size Trends in Elemental Groups: Key Findings

  • Moving from scandium to manganese in the 3d series, the size initially decreases.
  • Iron, cobalt, and nickel maintain a constant size in the 3d series.
  • Copper and zinc show an increase in size compared to other elements in the 3d series.
  • The size order in group 13 elements is significant, indicating danger.
  • Lanthanide contraction is crucial in understanding the size variations in elements.
  • Europium stands out as an exception in the A block elements, being the largest in size.
  • Ionic size varies based on the charge of the element, with positive charges indicating smaller sizes.
  • The size trend in group one elements follows a pattern where larger arrows indicate smaller sizes.
  • The cationic radius of elements in group 16 shows a unique trend, with tellurium being larger than phosphide and carbide ions.
  • Understanding ionization enthalpy involves considering the energy required to remove electrons from isolated gaseous atoms.

01:54:27

Ionization Enthalpy: Trends and Mnemonics

  • Ionization enthalpy is the energy required to remove an electron from an isolated gaseous atom.
  • Enthalpy is represented by delta H, and it is not defined for molecules but for isolated gaseous atoms.
  • The enthalpy change for ionization is not the same as the enthalpy change for a reaction.
  • The order of ionization enthalpy increases from top to bottom in a group and from left to right in a period.
  • Factors affecting ionization enthalpy include size, effective nuclear charge, and the region from which electrons are removed.
  • The order of ionization enthalpy in a period is larger than lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon.
  • Scams and deceptions in the order of ionization enthalpy occur due to the region from which electrons are removed.
  • The trend of ionization enthalpy from top to bottom in a group is exemplified by group 13 elements, remembered by the mnemonic "RBI."
  • The order of ionization enthalpy for group 13 elements is aluminum, gallium, indium, and thallium.
  • The mnemonic "W Make Mouth Breaking" helps remember the order of ionization enthalpy for group 14 elements: carbon, silicon, germanium, tin, and lead.

02:08:39

"3D and 5D Elements: Valence, Ionization, Size"

  • The confusion arises between two answers, with Dhoom's sir providing clarification.
  • The reason behind the confusion is the inert pair effect, affecting the oxidation state.
  • In the 3D series, the order remains normal, with elements like scandium, trion, lantham, and acton following a decreasing trend.
  • Moving from group three to group four to twelve, the 3D elements increase, followed by 4D and 5D elements.
  • The relationship between these elements varies, with sometimes 3D elements being more dominant and other times 5D elements.
  • The number of valence electrons can be predicted by analyzing the ionization enthalpy gaps.
  • The element with the highest first ionization enthalpy belongs to the eighth group of the periodic table.
  • The ionic radii order can be determined by the maximum positive charge affecting the size.
  • Isoelectronic species' size is influenced by the nuclear charge, with more protons leading to smaller sizes.
  • Understanding these concepts is crucial for answering JE Mains questions accurately.

02:23:36

"Understanding Ionization and Electron Enthalpy"

  • The speaker emphasizes the importance of correcting any errors promptly and efficiently.
  • The speaker mentions the need to complete tasks within a specific timeframe.
  • Metallic character is discussed in relation to ionization enthalpy, with a focus on lower ionization enthalpy leading to higher metallic character.
  • Cesium is highlighted as having the least ionization enthalpy in the periodic table.
  • The concept of ionization enthalpy is explained, with specific values provided for lithium and sodium.
  • The speaker discusses the complications related to ionization enthalpy and metallic character.
  • The process of electron gain enthalpy is introduced, emphasizing the stability gained through electron gain.
  • The speaker explains the difference between positive and negative electron gain enthalpy.
  • Affinity for electrons is discussed, with positive affinity leading to stability and negative affinity causing instability.
  • The speaker uses relatable examples to explain the concepts of electron gain enthalpy and electron affinity.

02:37:57

Electron Affinity and Periodic Trends

  • Affinity for someone is positive if the electron wants it and it wants the electron for stability by taking electrons.
  • Stability is achieved by taking electrons, leading to negative electron gain enthalpy.
  • If an electron does not want electrons, it will be unstable by taking them, requiring positive electron gain enthalpy.
  • Beryllium, magnesium, nitrogen, and noble gases have positive electron gain enthalpy.
  • Electron removal is always endothermic, requiring energy.
  • Trend of electron affinity decreases from top to bottom in p-block elements.
  • Fluorine lags behind chlorine due to its small size causing repulsion.
  • Inert gases have positive electron gain enthalpy, with neon having the highest value.
  • The order of electron affinity in group 18 is helium, neon, argon, krypton, and xenon.
  • Electronegativity is the last periodic property, representing the tendency to attract electrons.

02:53:13

"Crucial concept: Electronegativity in chemistry"

  • Electronegativity is a crucial concept in chemistry, with a fine line between electron gain enthalpy and electronegativity.
  • Electronegativity is a scale measuring an element's ability to attract bonded electrons towards itself.
  • Different scales like Malikan, Pauling, and Polling are used to measure electronegativity.
  • The Malikan scale formula involves dividing the sum of Ionization Enthalpy and Electron Affinity by two.
  • The Polling scale is essential for calculating electronegativity values accurately.
  • The order of electronegativity follows a specific trend, with fluorine being the most electronegative element.
  • The values of electronegativity decrease from fluorine to hydrogen in period 2 of the periodic table.
  • Group 13 elements exhibit exceptions in electronegativity trends, with Boron having an electronegativity of 2.0.
  • Electronegativity values for group 13 elements like Boron, Aluminum, Gallium, Indium, and Thallium vary following specific trends.
  • Understanding electronegativity values is crucial for organic chemistry and helps in predicting chemical behavior accurately.

03:06:22

Electronegativity, Hydration Enthalpy, and Ionic Mobility

  • The order of electronegativity in Group 13 is discussed, with the most electronegative element first, followed by the second, third, fourth, and fifth in order.
  • The order of electronegativity in Group 14 is questioned, with the correct order provided as 3.5, 2.5, 1.9, 1.8, and 1.8.
  • The application of electronegativity is explained through formulas like the Stevenson Schumacher Formula and the Henny Smith equation.
  • Factors affecting electronegativity are detailed, including positive charge, hybridization, and the terminal atom's electronegativity.
  • The Fajan Rule, which is the opposite of the Henny Smith Equation, is mentioned.
  • Hydration enthalpy, related to the energy released when an ion is surrounded by water molecules, is discussed.
  • The calculation of hydration enthalpy is explained as proportional to the charge on the ion and inversely proportional to its size.
  • The order of hydrated radius and ionic mobility is highlighted as important questions related to hydration enthalpy.

03:20:19

"Size, Charge, and Mobility of Lithium"

  • Lithium has a small size and a tiny lithium charge.
  • Water carries a plus one charge and fiercely attacks lithium.
  • Water forms layers on lithium when attacking it.
  • The layers increase the size of lithium.
  • Sodium has a larger size compared to lithium.
  • Ionic radius is larger when hydrated radius is smaller.
  • Ionic mobility is higher for smaller ions.
  • Lithium Plus has the lowest molar conductivity due to its large hydrated radius.
  • Lattice enthalpy can be viewed in two ways: lattice formation and lattice breaking.
  • Lattice enthalpy formula involves charges and sizes of ions.

03:35:45

Electron gain enthalpy exceptions and examples

  • Electron gain enthalpy is positive for sulfur and negative for all other elements except Beryllium, Magnesium, Nitrogen, and Noble Gases.
  • The process of electron gain enthalpy is endorsed for all elements except sulfur, which follows the assort process. Understanding this concept requires examining two to three examples to grasp it fully.
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