Structural and electronic effects Acids and Bases Acknowledgement Some material have been sourced from the following websites and books Reference • http://facstaff.gpc.edu/~matteya/organicppt/Ch2.ppt • http://atom.chem.wwu.edu/dept/facstaff/pavia/351pavia.html • www.fccj.us/chem1212/powerpoint/Ch17_Lewis_B.ppt • CH102 Course book • Organic Chemistry 7th Edition by John McMurry 2 Acids & Base Definitions Definition #3 – Lewis • Lewis acid - a substance that accepts an electron pair • All BrØnsted-Lowry
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huge impact on the polarity of this section. I’m just going to draw up the electronegativity values of the atoms we’re concerned with. So carbon has a value of 2.55‚ hydrogen with 2.2 and nitrogen with 3.04. Carbon to hydrogen bonds are nonpolar because the electronegativity difference is 0.35 when 2.55 is taken away from 2.2. A carbon to nitrogen bond highly favours nitrogen that is polar because of its electronegativity value. Therefore‚ it can be concluded that this half of the molecule is polar
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This is due to either what group or period it is in and periodic trends also affect this. Whether the element is metallic or non metallic the elements differ. Metallic elements have higher atomic weight and radius while non-metallic have high electronegativity and ionization trends. With each being so different we tested each element given and saw what happened when dropped into a certain solution to determine how periodic trends related to this
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a. which has bonds that are the most polar? b. which molecules have a dipole moment ? Answer Plan to arrange the polarity: The most polar bond is the one that has greatest difference in electronegativity (EN) between the atoms. Florin has the highest EN(4.0) electronegativity increase across the period and decrease down the group to identify the dipole moment : draw the Lewis structure and show the vector (arrow ) of the atoms. the vectors move from the atom of high EN to
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semiconductor devices that can convert electrical energy directly into light due to the nature of the bonding that occurs in the semiconductor solid. Type of bonding is directly related to conductivity of solid. Bonding in Elemental Solids Electronegativity – the ability of an atom to attract electrons to itself. Atoms with low e.n. (metals) don’t hold valence electrons tightly valence electron orbitals are diffuse (large distances away from nucleus) Atoms with high e.n. (nonmetals)
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Chemistry Notes: Metals: • A metal consists of a lattice of positive ions surrounded by a ‘sea’ of mobile delocalised valence electrons. • Metallic bonding is the electrostatic attraction between the delocalised electrons and the positive ions in the metallic lattice. Properties of metals: Property Explanation Relatively high density The particles are very close together. This is because of high electrostatic forces between the sea of valence electrons and the positively charged nucleus.
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suitable data Topic 1.3 Can you: a) define an ionic bond‚ covalent bond‚ metallic bond‚ and predict the type of bonding present in simple substances b) explain the difference between normal and dative covalent bonds c) define electronegativity and use it to explain why some bonds are covalent‚ others polar covalent and others ionic d) draw dot-cross diagrams to show
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D) H3C–CH2–C H3 8) The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately __________. A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal 9) Given the electronegativities below‚ which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5 A) C–H B) N–H C) O–H D) O–C E) O–N 10) Using the table of bond dissociation energies‚ the ΔH for the following gas-phase reaction is __________ kJ. A) -44
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Chem 11 Study Guide SCH3U Unit 1 Definitions: * SATP: Standard Ambient Temperature and Pressure ( 100kpa and 25 degrees C) * STP: Standard Temperature and Pressure (101.325kp and 0 deg C) * IUPAC: Intn’l Union of Pure and Applied Chem (approves‚ makes chem names symbols‚ etc. * Representative Elements: an element in any of groups 1‚2‚13-18 * Transition Metal: element of groups 3-12 * Energy level: a space with definite and fixed energy in which an electron is allowed to
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REVIEW a. I‚. • • C • • c. • C 3. The effective nuclear charge is a. equal to the suns of the charges of the protons in the nucleus b. equal to the suns of the charges of the protons in the nucleus minus the sum of the electrons in the Outer shell c. lest than tire sum of the charges of the protons in the nucleus due to shielding by the electrons in the outer shell d. lest than the sum of the charges of the protons in tire nucleus due to nisielding by the
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