Inorganic Chemistry - P Block Elements

Name: Inorganic Chemistry - P Block Elements
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Complete Chemistry for Engg and Medical Entrance Exam Preparation. ( IIT JEE Main | Advanced | BITSAT | SAT | NEET etc.)

Created bystudi live

Last updated 3/2022

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What you'll learn

Appreciate the general trends in the chemistry of p-block elements
Describe the trends in physical and chemical properties of group 13 and 14 elements
Explain anomalous behaviour of boron and carbon
Describe allotropic forms of carbon
Know the chemistry of some important compounds of boron, carbon and silicon
List the important uses of group 13 and 14 elements and their compounds

Course content

1 section • 36 lectures • 5h 9m total length

Anomalous Behavior of Nitrogen7:57
Explore the anomalous behavior of nitrogen, the first element in group 15, its diatomic nature and variable oxidation states from minus three to plus five, with ammonia, most stable hydride.
Anomalous Behavior of Fluorine7:36
Explain the anomalous behavior of fluorine among the group 17 halogens, highlighting its permanent -1 oxidation state, strong hydrogen-fluorine bond, weak hydrofluoric acid, and hydrogen bonding from its small size.
Anomalous Behavior of Boron5:57
Boron shows anomalous behavior in group 13: the hardest, smallest element with higher electronegativity; it exists as a monomer, forms covalent compounds, and has acidic oxides and hydroxides.
Allotropic Forms of Carbon10:39
Explore the three allotropic forms of carbon—diamond, graphite, and buckyball. Learn their bonding and structures: diamond with sp3, graphite with sp2, and buckyball's geometry and conductivity.
Allotropy of Phosphorus8:34
Explore the allotropy of phosphorus: white (yellow) phosphorus glows in the dark and is poisonous and insoluble; red phosphorus forms P4 structure; black phosphorus has a layered, less reactive form.
Chemical Properties of Chlorine9:19
Explore the chemical properties of chlorine, including its reactions with metals to form chlorides, with non-metals, hydrocarbons, ammonia, and water, and its effects on turpentine.
Compound of Phosphorous (PCl3 and PCl5)8:35
Explains preparation methods for phosphorus trichloride and phosphorus pentachloride from white phosphorus, using chlorine gas, with balancing steps and byproduct considerations.
Chemical Properties of PCl37:28
Explore the chemical properties of PCl3, including reaction with chlorine to form PCl5, hydrolysis to phosphorus acid, and formation of acid chlorides and alcohol chlorides from carboxylic acids and alcohols.
Chemical Properties of PCl59:20
Phosphorus pentachloride decomposes to PCl3 and Cl2 and hydrolyzes to phosphoric acid; it forms acid chlorides with carboxylic acids, alkyl chlorides with alcohols, and forms metal chlorides.
Compounds of Oxygen - Ozone7:29
Explains the ozone molecule (O3), its photochemical formation from O2 under light, and its role as a UV protection umbrella, with resonance structures across three oxygen atoms.
Anomalous Behavior of Carbon9:43
Explore the anomalous behavior of carbon in group 14, highlighting its small size, high electronegativity, tetravalence with four covalent bonds, and allotropes like diamond, graphite, and fullerene.
Anomalous Behavior of Oxygen6:52
Explores the anomalous behavior of oxygen in group 16, highlighting its gaseous diatomic nature, distinct oxidation states, hydrogen bonding, liquid water formation, and paramagnetic character.
Compounds of Nitrogen - Ammonia Preparation8:36
Explore ammonia preparation via laboratory methods using ammonium chloride with calcium hydroxide and ammonium sulfate with alkali, and industrial synthesis of nitrogen and hydrogen over a catalyst at high pressure.
Chemical Properties of Dinitrogen5:41
Examine the chemical properties of dinitrogen: metal nitride formation, ammonia synthesis with hydrogen, oxidation to nitric oxide, and reaction with calcium carbide.
Uses of Noble Gases6:00
Explore noble gas uses: helium for breathing mixtures and cryogenics, neon for signs, argon for inert atmospheres, krypton for airport lighting, xenon for flash tubes, and radon for cancer therapy.
Inter Halogen Compounds7:43
Explore inter halogen compounds’ characteristics, including their bonding with small electronegativity differences, their oxidizing behavior, hydrolysis with water to form halide ions, and addition to unsaturated hydrocarbons.
Zeo Lites7:16
Explore zeolites as sodium aluminum silicate frameworks with cavities that trap cations, enabling ion exchange and wide industrial uses. Discover applications in water purification, laundry detergents, and nuclear waste reprocessing.
Uses of Diborane6:23
Investigate how diborane (B2H6) acts as a rocket propellant and a reducing agent. It also enables synthesis of silicate glass, catalysis in reactions, rubber vulcanization, and doping in semiconductors.
Preparation of Sulphuric Acid9:12
Outline the contact process for industrial sulfuric acid production, from roasting and oxidation to so2 and so3, catalyzed by vanadium pentoxide, forming oleum and dilution.
Preparation of Chlorine13:33
Explore chlorine preparation methods, including the oxidation of hydrogen chloride with manganese dioxide, bleaching powder with acids, the decon process, and electrolysis of brine to release chlorine gas.
Compounds of Sulphur - Sulphur Dioxide (Preparation)9:00
This lecture explains how to prepare so2 from sulfur via a laboratory method, from sodium sulfide with hydrochloric acid, copper turnings with sulfuric acid, and industrial roasting of sulfide ores.
Uses of Aluminium4:18
Explore aluminium's wide range of applications from packaging and food containers to transport, construction, coins, watches, and electrical wires.
Compounds of Phosphorus - Phosphine (Chemical Properties)6:18
Examine the chemical properties of phosphine, a key phosphorus compound, through its reactions with copper sulfate, mercuric chloride, bromine, and chlorine, balancing equations and noting its basic character.
Physical Properties of Group 15th Elements9:17
Explore the physical properties of the group 15 elements (nitrogen, phosphorus, arsenic, antimony, bismuth), including trends in atomic radius, ionization energy, electronegativity, density, and the shift from nonmetals to metals.
Uses of Nitrogen5:59
Nitrogen, a diatomic gas in the air, serves as a refrigerant and to synthesize ammonia, nitric acid, and calcium cyanide; it provides inert atmospheres in metallurgy.
Preparation of Dinitrogen10:03
Explore methods to prepare dinitrogen, including the laboratory method with ammonium chloride and sodium nitrite, industrial thermal decomposition of ammonium nitrate, and bleaching powder and metal azide routes.
Preparation of Nitric Acid6:32
Learn two methods for preparing nitric acid: a laboratory method using sodium nitrate with concentrated sulfuric acid, and the all swirls process for large-scale production.
Compounds of Elements of Group 18 - Xenon Fluorides Part - 110:20
Examine xenon difluoride formation from xenon and fluorine, including preparation methods and its fluoridation of benzene and oxidizing actions.
Compounds of Elements of Group 18 - Xenon Fluorides Part - 29:19
Explore xenon fluorides in group 18, detailing synthesis of XeF4 from xenon and fluorine at 400 °C and XeF6 from discharge at −80 °C, plus properties and fluorinating oxidizing behavior.
Classification of Oxides10:48
Classify oxides into acidic, basic, amphoteric, and neutral oxides, noting nonmetal oxides form acids with water, metal oxides form bases, and zinc oxide is amphoteric.
Compounds of phosphorus - Phosphine (Preparation)8:52
Learn practical methods to prepare phosphine (PH3) from metal phosphides with water or acids, from white phosphorus with water, and from phosphine iodide routes, with gas evolution noted.
Preparation of Dioxygen12:11
Learn how to prepare dioxygen through thermal decomposition of oxygen-rich salts and metal oxides, electrolysis of water, and peroxide and laboratory methods.
Chemical Properties of Nitric Acid11:42
Explore the chemical properties of nitric acid through reactions with copper and zinc, balancing equations and noting by-products such as nitrogen oxides and water, and nitration of benzene.
Clathrates5:07
Learn how noble gases form clathrates, with xenon as a key example, trapping gases in cages for uses in anesthesia, isotope handling, and separating helium and neon from mixtures.
Chemical Properties of Dioxygen12:30
Examine the chemical properties of dioxygen, including metal oxidation to oxides, nonmetal oxidation to CO2, SO2, and NO, and catalyzed reactions with ammonia and hydrocarbon combustion.
Compounds of Elements of Group 18 - Xenon Oxides12:54
Explore xenon oxides in group 18, including xenon dioxide and xenon tetroxide, their hydrolysis from xenon fluorides XeF4 and XeF6, geometry, and their oxidizing properties.

Requirements

Basic understanding of chemistry and math's

Description

SUMMARY

p-Block of the periodic table is unique in terms of having all types of elements – metals, non-metals and metalloids. There are six groups of p-block elements in the periodic table numbering from 13 to 18. Their valence shell electronic configuration is ns2 np1–6 (except for He). Differences in the inner core of their electronic configuration greatly influence their physical and chemical properties. As a consequence of this, a lot of variation in properties among these elements is observed. In addition to the group oxidation state, these elements show other oxidation states differing from the total number of valence electrons by unit of two. While the group oxidation state is the most stable for the lighter elements of the group, lower oxidation states become progressively more stable for the heavier elements. The combined effect of size and availability of d orbitals considerably influences the ability of these elements to form π-bonds. While the lighter elements form pπ–pπ bonds, the heavier ones form dπ–pπ or dπ–dπ bonds. Absence of d orbital in second period elements limits their maximum covalence to 4 while heavier ones can exceed this limit.

Boron is a typical non-metal and the other members are metals. The availability of 3 valence electrons (2s 2 2p1 ) for covalent bond formation using four orbitals (2s, 2px, 2py and 2pz ) leads to the so called electron deficiency in boron compounds. This deficiency makes them good electron acceptor and thus boron compounds behave as Lewis acids. Boron forms covalent molecular compounds with dihydrogen as boranes, the simplest of which is diborane, B2H6. Diborane contains two bridging hydrogen atoms between two boron atoms; these bridge bonds are considered to be three-centre two-electron bonds. The important compounds of boron with dioxygen are boric acid and borax. Boric acid, B(OH)3 is a weak monobasic acid; it acts as a Lewis acid by accepting electrons from hydroxyl ion. Borax is a white crystalline solid of formula Na2[B4O5(OH)4]·8H2O. The borax bead test gives characteristic colours of transition metals.

Aluminium exhibits +3 oxidation state. With heavier elements +1 oxidation state gets progressively stabilised on going down the group. This is a consequence of the so called inert pair effect.

Carbon is a typical non-metal forming covalent bonds employing all its four valence electrons (2s 2 2p2 ). It shows the property of catenation, the ability to form chains or rings, not only with C–C single bonds but also with multiple bonds (C=C or C≡C). The tendency to catenation decreases as C>>Si>Ge ~ Sn > Pb. Carbon provides one of the best examples of allotropy. Three important allotropes of carbon are diamond, graphite and fullerenes. The members of the carbon family mainly exhibit +4 and +2 oxidation states; compouds in +4 oxidation states are generally covalent in nature. The tendency to show +2 oxidation state increases among heavier elements. Lead in +2 state is stable whereas in +4 oxidation state it is a strong oxidising agent. Carbon also exhibits negative oxidation states. It forms two important oxides: CO and CO2. Carbon monoxide is neutral whereas CO2 is acidic in nature. Carbon monoxide having lone pair of electrons on C forms metal carbonyls. It is deadly poisonous due to higher stability of its haemoglobin complex as compared to that of oxyhaemoglobin complex. Carbon dioxide as such is not toxic. However, increased content of CO2 in atmosphere due to combustion of fossil fuels and decomposition of limestone is feared to cause increase in ‘green house effect’. This, in turn, raises the temperature of the atmosphere and causes serious complications. Silica, silicates and silicones are important class of compounds and find applications in industry and technology.

Who this course is for:

Parents whose wards are students preparing for Indian Engineering and Medical Entrance Exams
IIT JEE | JEE Main | JEE Advanced | BITSAT | NEET | AIPMT | KVPY | SAT | GATE | MSAT