SIGNIFICANT FIGURES: 1) ALL non-zero numbers (1‚2‚3‚4‚5‚6‚7‚8‚9) are ALWAYS significant. 2) ALL zeroes between non-zero numbers are ALWAYS significant. 3) ALL zeroes which are SIMULTANEOUSLY to the right of the decimal point AND at the end of the number are ALWAYS significant. 4) ALL zeroes which are to the left of a written decimal point and are in a number >= 10 are ALWAYS significant. 5) If you can/must get rid of the zeroes‚ then they are NOT significant NOTES: -The electron was discovered
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Chemistry SCH3U Unit 1 Lesson 1 Key Questions 1. List three physical properties and one chemical property of a) an iron nail * conducts heat and electricity well * solid at room temperature * ductile * rusts in water (chemical) b) gasoline * liquid at 20deg C * boils between 20 and 200 degrees Celsius * not soluble in water * flammable in the presence of oxygen (chemical) 2. People in a workplace should have access to MSDS sheets so that * chemicals
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“WATER IS A GOOD SOLVENT” Water is very unique in all facets of its nature. The chemical formula for water is H2O as a water molecule consists of two atoms of the chemical element hydrogen (H) and one atom of the element oxygen (O). Water is the most abundant chemical compound on earth as its mass all exists together‚ naturally‚ in its gaseous‚ liquid and solid state. It is the most precious natural resource to man and is essential to life for all discovered living organisms. One of the unusual
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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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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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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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