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Chemistry - Molecular Structure (32 of 45) s-p2 Hybridization - Boron Trifloride, BF3
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will explain the s-p2 hybridization of boron trifloride, BF3.
Views: 14414 Michel van Biezen
sp2-Hybridization; Bonding and Structure of Boron Trifluoride
 
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sp2-Hybridization; Bonding and Structure of Boron Trifluoride
Views: 6072 Sabaq. Pk
SP2 Hybridization
 
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For more information: http://www.7activestudio.com [email protected] http://www.7activemedical.com/ [email protected] http://www.sciencetuts.com/ [email protected] Contact: +91- 9700061777, 040-64501777 / 65864777 7 Active Technology Solutions Pvt.Ltd. is an educational 3D digital content provider for K-12. We also customise the content as per your requirement for companies platform providers colleges etc . 7 Active driving force "The Joy of Happy Learning" -- is what makes difference from other digital content providers. We consider Student needs, Lecturer needs and College needs in designing the 3D & 2D Animated Video Lectures. We are carrying a huge 3D Digital Library ready to use. SP2 hybridization:Definition: "The process of intermixing of one S and two P orbitals to give three identical hybrid orbitals is known as Sp2 or trigonal hybridization". Characteristics Trigonal hybridization:In this hybridization three hybrid orbitals are formed.These hybrid orbitals takes the direction of p-orbitals.Each sp2 hybrid orbitals possess 33.31% of s-character and 66.7% p-character.The hybrid orbitals oriented along the three corners of regular triangle at an angle of 1200. Hence this hybridization is called trigonal hybridization.SP2 hybird orbital is slightly smaller in size than the sp3 hybrid orbital. Therefore the shape of sp2 hybridized atom is trigonal planar with bond angle of 1200.Examples:-BCl3: Boron trichloride BF3: Boron trifluoride. C2H4: Ethylene C6H6: Benzene SO2: Sulphur dioxide.Structure of Boron trichloride Bcl3:Consider Boron trichloride, BCl3.Boron Atom: The central atom in boron trichloride is Boron B.The atomic number of boron is 5.The general electronic configuration is 1s22s22p1 The ground state electronic configuration of is 2s2 2p1.The excited state electronic configuration of Boron is 2s1 2p2.One electron is promoted from 2s to 2py level, then electronic configuration is 1s2 2s12px12py1.The 2s to 2px & 2py orbital undergoes sp2 hybridization and form three sp2 hybrid orbitals. The three sp2 hybrid orbitals possess one electron each.Chlorine Atom: The atomic number of Chlorine is 17. The general electronic configuration is 1s2 2s22p6 3s23p5, which is the ground state electronic configuration.Pz orbital is having unpaired electron. The three hybrid orbitals of boron form three sigma bonds with 3pz orbital of three chlorine atoms and oriented along the three corners of regular triangle at an angle of 1200. Therefore the molecule gets trigonal planar with bond angle of 1200. Hence three sigma sp2-pz bonds are having pair of electrons.
Views: 121435 7activestudio
sp2 hybridisation
 
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Views: 20927 Ribla Moses
Sp2 Hybridization, Bonding and Structure of Boron Trifluoride Hindi/Urdu Chemistry Crash Course #192
 
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Sp2 Hybridization, Bonding and Structure of Boron Trifluoride Hindi/Urdu Chemistry Crash Course #192 Download Notes: http://smartstudyedu.blogspot.com/p/notes.html - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - Hello Everyone! Welcome to our channel Smart Study Education. Here You will Learn Lectures for many subjects of your academic / non academic courses including English, Chemistry, Biology, Physics, Mathematics etc for classes of school, college or university and many more. These Lectures will help you to gain knowledge whether you are a Student or Teacher or Learner. All Lectures will help you throughout your life. Find us on social Networks: Facebook : https://www.facebook.com/Smart-Study-Education-160845007843260 Twitter : https://www.twitter.com/smartstudyedu Google + : https://plus.google.com/116903287599774402171 Website/Blog : http://smartstudyedu.blogspot.com/ Subscribe Our Channel For More Videos: https://www.youtube.com/channel/UCjivnJETneyRvJI0vAHEDWQ Like , Comment and Share video with your friends and relatives to support us. Thanks for Watching
sp2 hybridisation || structure of boron trichloride || bsc chemistry || d's classes
 
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https://www.facebook.com/Ds-classes-1391615131088506/ https://www.facebook.com/amit.dw.1 https://www.facebook.com/mahadevsss2016/ यह चैनल मुख्य रूप से उन लोगों के लिए बनाया गया है जो प्रतियोगी परीक्षा की तैयारी कर रहे हैं और इसके आलावा वह विद्यार्थी जो ग्रेजुएशन कर रहे हैं उनके केमिस्ट्री ( रसायन विज्ञान ) विषय से सम्बंधित भी सारे लेक्चर लाइव मिलेंगे , इस कक्षा का मुख्य उद्देश्य उन सभी को पढ़ाना है जो कहीं न कहीं से आर्थिक रूप से कमजोर हैं। Amit Dwivedi D's Classes 9993265131 , 8962564211
Lewis Structure For BCl3, Molecular Geometry, Bond Angle, Hybridization, Polar or Nonpolar
 
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This video shows you how to draw the lewis structure for BCl3. It provides the molecular geometry, bond angle, and hybridization of BCl3. It also tells you if BCl3 is polar or nonpolar.
sp2- Hybridization ; Bonding and Structure of Boron Trifluoride | Chemistry Guider | Swap
 
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Subscribe to get more videos 1st year chemistry in urdu/hindi first time on intertnet , Swap will share more and more videos with you Guys please Subscribe And appricate this effort God Bless You MOre And More visit SWAP faCEBOOK PAGE www.facebook.com/swap.pk
Views: 32 Once More
Chemistry - Molecular Structure (34 of 45) s-p3-d Hybridization - Phosphorus Pentachloride, PCl5
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will explain the s-p3-d hybridization of phosphorus pentachloride, PCl5.
Views: 18667 Michel van Biezen
Chemistry - Molecular Structure (40 of 45) Hybridization with 2 Free Electron Pairs - Water - H2O
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will explain the hybridization with 2 free electron pairs (water, H2O).
Views: 11376 Michel van Biezen
Sp2 Hybridization in urdu FSc part 1 and part 2
 
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Sp2 Hybridization in urdu FSc part 1 and part 2, What is hybridization ? What do you mean by hybridization ? Define hybridization , Definition of Hybridization.
Views: 2951 Ibtihaj Ahmad
Chemistry - Molecular Structure (38 of 45) Hybridization and the Triple Bond (2 Pi-Bonds)
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will explain the hybridization and the triple bond of ethyne, C2H2 (2 Pi-bonds).
Views: 5393 Michel van Biezen
14.2 Lewis, hybridization (sp3,sp2,sp) , shapes and angles [HL IB Chemistry]
 
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14.2.3 Identify and explain the relationships between Lewis structures, molecular shapes and types of hybridization (sp, sp2 and sp3). If your teacher taught that single bonds means sp3, double means sp2 and triple is sp, break the news that they are wrong! 4 charge centers = sp3, 109.5 / 107 / 105 degree bond angles, 4 sigma 3 charge centers = sp2, 120 degree bond angle, 3 sigma, 1 pi (normally) 2 charge centers = sp, 180 degree bond angle, 2 sigma, 2 pi
Views: 67958 Richard Thornley
Quantum Chemistry 11.2 - sp2 Hybridization
 
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Short lecture on sp2 hybrid orbitals in non-linear polyatomic molecules. In trigonal planar molecules such as BH3, the valence 2s and 2p orbitals overlap in a linear combination to form sp2 hybrid orbitals oriented towards the three external hydrogen atoms. Notes Slide: http://i.imgur.com/9FHH79Y.png --- About TMP Chem --- All TMP Chem content is free for everyone, everywhere, and created independently by Trent Parker. Email: [email protected] --- Video Links --- Chapter Playlist: https://www.youtube.com/playlist?list=PLm8ZSArAXicImNhMOwgaSfDkVxKtZSLW8 Course Playlist: https://www.youtube.com/playlist?list=PLm8ZSArAXicL3jKr_0nHHs5TwfhdkMFhh Course Review: https://www.youtube.com/playlist?list=PLm8ZSArAXicLTRn3cJyyU1TiU7n_Pp4X1 Other Courses: https://www.youtube.com/playlist?list=PLm8ZSArAXicIXArfap9Tcb8izqRPvE0BK Channel Info: https://www.youtube.com/playlist?list=PLm8ZSArAXicLlGO4Rvpz-D6vX8MFbOn4V --- Social Links --- Facebook: https://www.facebook.com/tmpchem Twitter: https://www.twitter.com/tmpchem LinkedIn: https://www.linkedin.com/in/tmpchem Imgur: https://tmpchem.imgur.com GitHub: https://www.github.com/tmpchem --- Equipment --- Microphone: Blue Yeti USB Microphone Drawing Tablet: Wacom Intuos Pen and Touch Small Drawing Program: Autodesk Sketchbook Express Screen Capture: Corel Visual Studio Pro X8
Views: 1904 TMP Chem
BH3 Hybridization Molecular Geometry and Lewis Structure
 
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The hybridization of BH3 is sp2. BH3 has a trigonal planar molecular geometry when you draw its lewis structure. BH3 stands for Boron Trihydride
Drawing Hybrid Orbitals on central atom
 
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This video addresses the pi bonding we see when there is a double bond in a molecule (or triple bond). Pi bonding will occur when there is an Un-hybridized p-atomic orbital. Pi bonding can be localized (if no resonance structures are possible) or delocalized (if the molecule has resonance structures).
Views: 28092 Michele Berkey
Depicting Hybridization of Atomic Orbitals - Ammonia (NH3) 001
 
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For the molecule ammonia (NH3): a) Draw the filled atomic orbitals of the central atom. b) What should the bond angle around the central atom be if the atomic orbitals do not hybridize? c) Which atomic orbitals are used for hybridization and eventual bonding? d) Draw the process of hybridization for the central atom. e) What are type of hybridized orbitals are formed? f) Draw a depiction of the orbitals that overlap to form a covalent bond in the molecule. Interviews 1) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part I” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-1 2) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part II” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-2
sp2 hybridization
 
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sp2 hybridization for AISG HL Chem students
Views: 31 Scott Seiple
NH3 Hybridization: Hybrid Orbitals for NH3 (ammonia)
 
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A description of the hybridization of NH3. Note that the NH3 hybridization is sp3 for the central Nitrogen (N) atom.
Views: 28785 Wayne Breslyn
Hybridization of Atomic Orbitals, Sigma and Pi Bonds, Sp, Sp2 & Sp3 - Chemical bonding
 
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In chemistry, orbital hybridisation (or hybridization) is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory. Hybrid orbitals are very useful in the explanation of molecular geometry and atomic bonding properties. Although sometimes taught together with the valence shell electron-pair repulsion (VSEPR) theory, valence bond and hybridisation are in fact not related to the VSEPR model. Hybridisation describes the bonding atoms from an atom's point of view. For a tetrahedrally coordinated carbon (e.g., methane CH4), the carbon should have 4 orbitals with the correct symmetry to bond to the 4 hydrogen atoms. Carbon's ground state configuration is 1s2 2s2 2p2 or more easily read: C ↑↓ ↑↓ ↑ ↑ 1s 2s 2p 2p 2p The carbon atom can use its two singly occupied p-type orbitals, to form two covalent bonds with two hydrogen atoms, yielding the singlet methylene CH2, the simplest carbene. The carbon atom can also bond to four hydrogen atoms by an excitation of an electron from the doubly occupied 2s orbital to the empty 2p orbital, producing four singly occupied orbitals. C* ↑↓ ↑ ↑ ↑ ↑ 1s 2s 2p 2p 2p The energy released by formation of two additional bonds more than compensates for the excitation energy required, energetically favouring the formation of four C-H bonds. Quantum mechanically, the lowest energy is obtained if the four bonds are equivalent, which requires that they are formed from equivalent orbitals on the carbon. A set of four equivalent orbitals can be obtained that are linear combinations of the valence-shell (core orbitals are almost never involved in bonding) s and p wave functions,which are the four sp3 hybrids. C* ↑↓ ↑ ↑ ↑ ↑ 1s sp3 sp3 sp3 sp3 In CH4, four sp3 hybrid orbitals are overlapped by hydrogen 1s orbitals, yielding four σ (sigma) bonds (that is, four single covalent bonds) of equal length and strength. Other carbon compounds and other molecules may be explained in a similar way. For example, ethene (C2H4) has a double bond between the carbons. For this molecule, carbon sp2 hybridises, because one π (pi) bond is required for the double bond between the carbons and only three σ bonds are formed per carbon atom. In sp2 hybridisation the 2s orbital is mixed with only two of the three available 2p orbitals, C* ↑↓ ↑ ↑ ↑ ↑ 1s sp2 sp2 sp2 2p forming a total of three sp2 orbitals with one remaining p orbital. In ethylene (ethene) the two carbon atoms form a σ bond by overlapping two sp2 orbitals and each carbon atom forms two covalent bonds with hydrogen by s–sp2 overlap all with 120° angles. The π bond between the carbon atoms perpendicular to the molecular plane is formed by 2p–2p overlap. The hydrogen–carbon bonds are all of equal strength and length, in agreement with experimental data. The chemical bonding in compounds such as alkynes with triple bonds is explained by sp hybridisation. In this model, the 2s orbital is mixed with only one of the three p orbitals, C* ↑↓ ↑ ↑ ↑ ↑ 1s sp sp 2p 2p resulting in two sp orbitals and two remaining p orbitals. The chemical bonding in acetylene (ethyne) (C2H2) consists of sp–sp overlap between the two carbon atoms forming a σ bond and two additional π bonds formed by p–p overlap. Each carbon also bonds to hydrogen in a σ s–sp overlap at 180° angles.
Views: 201 Abdullah SanaUllah
Orbital diagrams
 
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Views: 75298 Sonya Birazian
CO2 Hybridization: Hybrid Orbitals for CO2
 
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A description of the hybridization of CO2 including sigma and pi bonds. Note that the CO2 hybridization is sp for the central carbon atom. It's sp2 for each of the oxygen atoms as well.
Views: 109036 Wayne Breslyn
Hybridization of orbitals with sigma and pi bonds (1st half)
 
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sp3, sp2, sp hybridization sigma bonds pi bonds
Views: 33 chemtaiji
Orbitals, the Basics: Atomic Orbital Tutorial — probability, shapes, energy; Crash Chemistry Academy
 
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A crash course tutorial on atomic orbitals, quantum numbers and electron configuration + practice problems explained. CC Academy videos are easy 101 crash course tutorials for step by step Chemistry help on your chemistry homework, problems, and experiments. Check out our best lessons: - Solution Stoichiometry Tutorial: How to use Molarity - Stoichiometry - Quantum Numbers - Rutherford's Gold Foil Experiment, Explained - Covalent Bonding Tutorial: Covalent vs. Ionic bonds - Metallic Bonding and Metallic Properties Explained: Electron Sea Model - Effective Nuclear Charge, Shielding, and Periodic Properties - Electron Configuration Tutorial + How to Derive Configurations from Periodic Table - Orbitals, the Basics: Atomic Orbital Tutorial — probability, shapes, energy - Metric Prefix Conversions Tutorial - Gas Law Practice Problems: Boyle's Law, Charles Law, Gay Lussac's, Combined Gas Law --- More on Atomic Orbitals -- Wikipedia "An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom.[1] This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term, atomic orbital, may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.[2] Each orbital in an atom is characterized by a unique set of values of the three quantum numbers n, ℓ, and m, which respectively correspond to the electron's energy, angular momentum, and an angular momentum vector component (the magnetic quantum number). Any orbital can be occupied by a maximum of two electrons, each with its own spin quantum number s. The simple names s orbital, p orbital, d orbital and f orbital refer to orbitals with angular momentum quantum number ℓ = 0, 1, 2 and 3 respectively. These names, together with the value of n, are used to describe the electron configurations of atoms. They are derived from the description by early spectroscopists of certain series of alkali metal spectroscopic lines as sharp, principal, diffuse, and fundamental. ... Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model), a modern framework for visualizing the submicroscopic behavior of electrons in matter. In this model the electron cloud of a multi-electron atom may be seen as being built up (in approximation) in an electron configuration that is a product of simpler hydrogen-like atomic orbitals. The repeating periodicity of the blocks of 2, 6, 10, and 14 elements within sections of the periodic table arises naturally from the total number of electrons that occupy a complete set of s, p, d and f atomic orbitals, respectively, although for higher values of the quantum number n, particularly when the atom in question bears a positive charge, the energies of certain sub-shells become very similar and so the order in which they are said to be populated by electrons (e.g. Cr = [Ar]4s13d5 and Cr2+ = [Ar]3d4) can only be rationalized somewhat arbitrarily." Wikipedia contributors. "Atomic orbital." Wikipedia, The Free Encyclopedia. Wikipedia, The Free Encyclopedia, 17 May. 2016. Web. 27 May. 2016.
Views: 869855 Crash Chemistry Academy
Depicting Hybridization of Atomic Orbitals - Boron Trifluoride (BF3)
 
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For the molecule boron trifluoride (BF3): a) Draw the filled atomic orbitals of the central atom. b) What should the bond angle around the central atom be if the atomic orbitals do not hybridize? c) Which atomic orbitals are used for hybridization and eventual bonding? d) Draw the process of hybridization for the central atom. e) What are type of hybridized orbitals are formed? f) Draw a depiction of the orbitals that overlap to form a covalent bond in the molecule. ———————————— INTERVIEW 1) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part I” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-1 2) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part II” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-2 ———————————— INTERDISCIPLINARY ART LECTURE: 1) Giesbrecht, H., Peet, K. (January 20, 2016) “Translating Failure” WEDGE_SPACE https://vimeo.com/152432030 ———————————— FACEBOOK: https://www.facebook.com/profheath/ TWITTER: https://twitter.com/prof_heath
Depicting Hybridization of Atomic Orbitals - Beryllium Dichloride (BeCl2)
 
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For the molecule beryllium dichloride (BeCl2): a) Draw the filled atomic orbitals of the central atom. b) What should the bond angle around the central atom be if the atomic orbitals do not hybridize? c) Which atomic orbitals are used for hybridization and eventual bonding? d) Draw the process of hybridization for the central atom. e) What are type of hybridized orbitals are formed? f) Draw a depiction of the orbitals that overlap to form a covalent bond in the molecule.
Hybridization Pi Bonds
 
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Views: 1125 Moleqlar
Hybridisation of Carbon in Organic Compounds
 
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In this video we want to discuss the concept of excitation and hybridisation of Carbon in Organic Compounds. We can use hybridisation to explain the shape of organic molecules with respect to carbon. 1. Methane, CH4 Let's consider carbon in methane, CH4. We know that the shape with respect to carbon is tetrahedral according to Valence Shell Electron Pair Repulsion Theory (VSEPR). Let's try to explain the shape via the electronic configuration of carbon instead. Carbon in the ground state has the following electronic configuration: 1s2 2s2 2p2. Carbon has only 2 unpaired electrons in this case, so therefore it can only form 2 bonds in its ground state. Of course we know that carbon always forms 4 bonds, so the concept of excitation comes in where an electron is promoted from the paired 2s orbital which is lower in energy to an empty 2p orbital which is higher in energy. Carbon in its excited state now has 4 unpaired electrons so can form 4 bonds. However, if carbon just uses these 2s and 2p orbitals for bond formation, the shape with respect to carbon will not be tetrahedral since 2s orbital is more stable and closer to the nucleus so bond formed will be shorter, while 2p orbital is less stable and further away from the nucleus so bond formed will be longer. This means we will have one shorter C-H bond (from 2s orbital) and 3 longer C-H bonds (from the 2p orbitals), which is hardly the highly symmetrical tetrahedral shape that we see in methane. Therefore we need another concept to connect between excitation and the final shape of methane - hybridisation. Hybridisation is the mixing of valence orbitals to form sigma bonds. Since carbon in methane forms 4 sigma bonds, it will mix 4 of its valence orbitals (2s, 2px, 2py, 2pz) to form 4 identical orbitals with equal shape and energy. The name of the hybridised orbitals will be sp3 hybridised orbitals and since they have the same shape and energy, they repel each other equally and give sp3 hybridised carbon in CH4 its highly symmetrical tetrahedral shape. 2. Ethene, C2H4 Carbon in ethene forms 3 sigma bonds and 1 pi bond. Since carbon forms 3 sigma bonds, it will mix 3 of its valence orbitals (2s, 2px, 2py) to form 3 identical orbitals with equal shape and energy. The name of the hybridised orbitals will be sp2 hybridised orbitals and since they have the same shape and energy, they repel each other equally and give sp2 hybridised carbon in C2H4 its trigonal planar shape. Remainder 2pz orbital is unhybridised and is used in pi bond formation. 3. Ethyne, C2H2 Carbon in ethyne forms 2 sigma bonds and 2 pi bonds. Since carbon forms 2 sigma bonds, it will mix 2 of its valence orbitals (2s, 2px) to form 2 identical orbitals with equal shape and energy. The name of the hybridised orbitals will be sp hybridised orbitals and since they have the same shape and energy, they repel each other equally and give sp hybridised carbon in C2H2 its linear shape. Remainder 2py and 2pz orbitals are unhybridised and used in pi bond formation. 4. Summary for State of Hybridisation for Carbon The following table will summarise what we need to know for hybridisation. Based on the number of sigma bonds that carbon forms, we can determine its state of hybridisation. For the detailed discussion and explanation on excitation and hybridisation, check out this video now! Topic: Introduction to Organic Chemistry, Organic Chemistry, A Level Chemistry, Singapore Found this video useful? Please LIKE this video and SHARE it with your friends! SUBSCRIBE to my YouTube Channel for new A Level Chemistry video lessons every week at https://www.youtube.com/ChemistryGuru Any feedback, comments or questions to clarify? Suggestions for new video lessons? Drop them in the COMMENTS Section, I would love to hear from you! If you are looking for A Level Chemistry Tuition, do consider taking up my classes at Bishan. More info at https://chemistryguru.com.sg/ -~-~~-~~~-~~-~- Please watch my latest video: "Ideal Gas Graph Sketching" https://www.youtube.com/watch?v=G4_PSne7kE0 -~-~~-~~~-~~-~-
sp3 hybridized orbitals in methane, diamond
 
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This video is about sp3 hybridized orbitals in methane, diamond.
Views: 1457 Scott Ramsay
Bonding and Structure of Ammonia
 
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Bonding and Structure of Ammonia
Views: 5612 Sabaq. Pk
CHEMISTRY 101 - Valence Bond Theory: hybridization in larger molecules
 
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In this example problem, we determine the hybridization on atoms in arginine, determine the bonding scheme of bonds within arginine, and determine the total number of sigma and pi bonds.
Views: 553 Matthew Gerner
Chemistry - Molecular Structure (37 of 45) Hybridization and the Double Bond
 
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Visit http://ilectureonline.com for more math and science lectures! In this video I will explain the hybridization and the double bond of ethylene, C2H4.
Views: 4161 Michel van Biezen
Carbon atom hybridization within a molecule
 
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How to determine the hybridization of a carbon atom within a molecule.
Views: 267 LHSAtkins
How to identify hybridization of atoms
 
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How to identify hybridization of atoms
Views: 87 winscience
Depicting Hybridization of Atomic Orbitals - Phosphorous Pentachloride (PCl5)
 
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For the molecule phosphorous pentachloride (PCl5): a) Draw the filled atomic orbitals of the central atom. b) What should the bond angle around the central atom be if the atomic orbitals do not hybridize? c) Which atomic orbitals are used for hybridization and eventual bonding? d) Draw the process of hybridization for the central atom. e) What are type of hybridized are formed? f) Draw a depiction of the orbitals that overlap to form a covalent bond in the molecule.
Hybridization in Methane (CH4)
 
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This explains how valence bond theory without hybridization doesn't "work" and how using hybridization "solves" the issue.
Views: 898 Jon Gittins
Methane hybridization
 
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Describing the hybridization in the bonding of methane.
Views: 865 StudentFriendlyChem
Hybridization Informization
 
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Here's some practice problems for you: Draw CO2 What is the hybridization of BeF2 What about NH3?
SC128 Promotion & Hybridization
 
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Views: 115 jaj e
hybridization ammonia sp3
 
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describing the nitrogen of ammonia as sp3 hybridized
Views: 70 Erland Stevens
Chemistry Hybridization
 
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lesson on hybridztion and how to show hybridization when drawing orbital box diagrams
Views: 375 97Omar97
Aromatic, Antiaromatic, or Nonaromatic, Huckel's Rule, 4n+2, Heterocycles, Aromaticity
 
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This organic chemistry video tutorial shows you how to tell if a compound is aromatic, antiaromatic or nonaromatic by using huckel's rule / number of 4n+2 pi electrons, and features of the compound such as whether or not if it's cyclic, conjugated, sp2 hybridized and planar. Organic Chemistry Video Playlist: https://www.youtube.com/watch?v=n5vjCqnVb6s&index=1&t=25s&list=PL0o_zxa4K1BU3gxU8RwqkEET2ilZ80Znj Access to Premium Videos: https://www.patreon.com/MathScienceTutor Facebook: https://www.facebook.com/MathScienceTutoring/ Examples and practice problems in this video include cyclobutadiene, benzene, cyclooctatetraene, pentalene, 1,3,5-hexatriene, naphthalene, anthracene, tropylium ion, cyclopropenyl cation radical & anion, cyclopentadienyl radical cation & anion, cyclooctarienyl dianion, cyclohexatrienyl cation, radical, & anion, pyrrole, furan, pyran, isoxazole, tub conformation of cyclooctatetraene, heterocycles such as thiophene, 1,3-thiazole, pyrimidine, purine, pyrylium ion, & imidazole. This video also helps you to see which nitrogen atom is basic and which is not. It clearly helps you to see the difference in aromaticity vs antiaromaticity.
sp2 Hybridization of Ethylene - Nature of Chemical Bond - Chemistry Class 11
 
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sp2 Hybridization of Ethylene Video Lecture from Chapter Nature of Chemical Bond of Subject Chemistry Class 11 for HSC, IIT JEE, CBSE & NEET. Watch Previous Videos of Chapter Nature of Chemical Bond:- 1) sp3 Hybridization of H2O - Nature of Chemical Bond - Chemistry Class 11 - https://youtu.be/9o5c0LOVhsY 2) sp3 Hybridization of Ammonia (NH3) - Nature of Chemical Bond - Chemistry Class 11 - https://youtu.be/jl2_0M04o3k Watch Next Videos of Chapter Nature of Chemical Bond:- 1) sp2 Hybridization of Boron Trifloride - Nature of Chemical Bond - Chemistry Class 11 - https://youtu.be/1DgoG4lsXxE Access the Complete Playlist of Chapter Nature of Chemical Bond:- http://gg.gg/Nature-of-Chemical-Bond Access the Complete Playlist of Chemistry Class 11:- http://gg.gg/Chemistry-Class-11 Subscribe to Ekeeda Channel to access more videos:- http://gg.gg/Subscribe-Now #NatureofChemicalBond #ChemistryClass11 #ChemistryClass11JEE #ChemistryClass11Lectures #ChemistryClass11Tutorial #OnlineVideoLectures #EkeedaOnlineLectures #EkeedaVideoLectures #EkeedaVideoTutorial Nature of Chemical Bond Chemistry Class 11 Nature of Chemical Bond Class 11 Chemistry Class 11 Nature of Chemical Bond 11 Chemistry Nature of Chemical Bond Nature of Chemical Bond 11th Std Class 11 Nature of Chemical Bond Class 11 Chemistry Chemistry for Class 11 Thanks For Watching. You can follow and Like us on following social media. Website - http://ekeeda.com Parent Channel - https://www.youtube.com/c/ekeeda Facebook - https://www.facebook.com/ekeeda Twitter - https://twitter.com/Ekeeda_Video LinkedIn- https://www.linkedin.com/company-beta/13222723/ Instgram - https://www.instagram.com/ekeeda_/ Pinterest - https://in.pinterest.com/ekeedavideo You can reach us on [email protected] Happy Learning : )
Views: 92 Ekeeda

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