(mass=145g) with change in velocity of 0.11 m/s. 4. Fill in the following. | Number of orbitals | Number of electrons that can be held | n=3 | | | 4p subshell | | | 3px | | | 2f subshell | | | 5. Give the full electron configuration of the followings. For (a)‚ indicate the inner and valence electrons. (a) 14Si (b) 25Mn3+ 6. Give the condensed electron configuration and orbital diagram for 22Ti. Then determine whether the atom is paramagnetic or diamagnetic. 7. Determine
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‘It is often suggested that the source for many of William Wordsworth’s poems lies in the pages of Dorothy Wordsworth’s journal. Quite frequently‚ Dorothy describes an incident in her journal‚ and William writes a poem about the same incident‚ often around two years later.’ It is a common observation that whilst Dorothy is a recorder – ‘her face was excessively brown’ – William is a transformer – ‘Her skin was of Egyptian brown’ . The intertextuality between The Grasmere and Alfoxden Journals and
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Topic 5 – Bonding and Structure Revision Notes 1) Introduction • Atoms form bonds to get a full outer shell of electrons • There are three types of bonding: ionic‚ covalent and metallic • The structures produced by forming bonds are either giant or simple • The possible combinations of structure and bonding are giant ionic‚ simple covalent‚ giant covalent and giant metallic • Simple covalent is sometimes called simple molecular • Giant covalent is sometimes called giant
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SCH4U-C 1 UNIT Structure and Properties of Matter Unit 1 Introduction Chemisty SCH4U-C Table of Contents Unit 1: Structure and Properties of Matter Lesson 1: Atomic Structure Lesson 2: Introduction to Chemical Bonding Lesson 3: Molecular Shape and Polarity Lesson 4: Intermolecular Forces and Their Applications Unit 2: Organic Chemistry Lesson 5: Saturated Hydrocarbons Lesson 6: Unsaturated Hydrocarbons Lesson 7: Functional Groups Lesson 8: Acids‚ Esters‚ Amides
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s-character‚ 66% p-character sp i.e. CO2 2 regions of e- linear 180° 50% s-character‚ 50% p-character Orbitals Einstein: photoelectric effect → photons de Broglie → wave-particle duality Schrodinger → wave functions ?→ orbitals Atomic orbitals Simple Molecular Orbital Theory # MO’s = #AO’s MO’s arranged by relative E Filling follows (1: Aufbau‚ 2: Pauli) Bond Order (e- in bonding orbital - e- in antibonding) / 2 Valence Bond Theory places e- pairs between atoms problems incorrect bond
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Molecular Structure or "The Shape Molecules are In" Directions: Make a copy of this document and change the file name to “your last name‚ VSEPR Lab.” Place the document in the Google folder with your name on it. Follow each instruction to build molecular models and answer the following questions. Make sure your notes‚ comments‚ and answers are in a different text color. When you have finished with the lab questions attach a 12 page conclusion that summarizes and explains the main points of the lab
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molecules. If you are interested in electronegativity in an organic chemistry context‚ you will find a link at the bottom of this page. What is electronegativity Definition Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The Pauling scale is the most commonly used. Fluorine (the most electronegative element) is assigned a value of 4.0‚ and values range down to caesium and francium which are the least electronegative at 0.7. What happens if two
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The Beer-Lambert LawWhat the Law looks likeYou will find that various different symbols are given for some of the terms in the equation - particularly for the concentration and the solution length. I’m going to use the obvious form where the concentration of the solution is "c" and the length is "l". | | Note: That’s obviously "l" for length. The font I’m using won’t distinguish between "l" for length and a capital letter "I" (for Intensity). That problem disappears in the equation below - where
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PAGE 2 8. Which of the following represents an sp3 hybridized atomic orbital containing the lone pair of electrons of ammonia‚ NH3? (a) 1 (b) 2 (c) 3 (d) 4 9. How many electrons are there in the valence shell of the carbon atom of a methyl cation‚ CH3+? (a) 4 (b) 5 (c) 6 (d) 7 10. Which atomic orbitals overlap to form the C-H â bonding molecular orbitals of ethane‚ CH3CH3? (a) C2p + H1s (b) Csp + H1s (c) Csp2 + H1s (d) Csp3 + H1s 11. Which
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assigned by your lab instructor. Student Learning Outcomes: Learn how to draw Lewis structures. Learn how to draw Lewis structures for atoms which violate the octet rule. Learn how to use Lewis structures and VSEPR and to predict the shapes of molecules. Learn how to use the shape of a molecule to predict whether or not it is polar. Experimental Goals: The purpose of this lab is to learn how to draw Lewis structures for molecules‚ and‚ from those structures‚ to predict the shape
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