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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3.1 & 3.2 Chemistry Notes Dalton * In 1805‚ John Dalton reintroduced the idea to explain 3 fundamental principles Experimental Work * Atoms of different elements have different properties * Law of definite proportion and multiple compositions: atoms of 2 or more elements can combine in a fixed ratio to form new substances depending on their combining capacities (eg. H2O vs H2O2) * Law of conservation of mass: atoms cannot be created or destroyed during a chemical reaction
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atom and its particle behaviour through mathematics * Heralded “quantum physics” * electrons as wavelengths‚ not particles * 3D description of an atom * It is possible to predict where electrons would probably be found but impossible to predict EXACTLY where you could find them * “wave function” a mathematical function * James Chadwick – discovered the particle neutrons * Werner Karl Heisenberg – “Quantum Theory” * Probabilities of electron’s behaviour and location in
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concerning gravitation (Newton’s laws and General relativity) return great results when explaining rotation of galaxies‚ gravitational pull‚ etc. however these theories rely upon classical quantum field theory physics and completely break down as we approach the subatomic scale. The standard model mainly relies on the quantum branch of physics which deals with subatomic particles and force carriers but this theory mainly relies on probability (particles such as electrons behave like a wave). Nevertheless
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Jean-Luc Fernandez 9.4 The start of the atom. The atom is the basic unit of matter and all life. The history of the study of the atomic nature of matter is the thinking process that goes on in the scientist’s heads. Further progress in the understanding of atoms did not occur until very famous scientist created the atomic theory. Here are some scientists who changed the way we learn about the atom‚ and the atomic nature of all life. Ernest Rutherford. Ernest Rutherford was another scientist
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traveling at 30 cm/s. A) car B) planet C) hydrogen atom D) uranium atom E) marble 5. Which of the subshells below do not exist due to the constraints upon the l quantum number? A) 2s B) 2p C) 2d D) all of the above E) none of the above 6. Which of the subshells below do not exist due to the constraints upon the l quantum number? A) 4f B) 4p C) 4d D) 4s E) none of the above 2 Ghiladi - Exam 1 Name: ______________‚ ______________ ID #:______________ (last) (first) 7.
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Jonsson shot electrons through two holes to observe how subatomic particles react in stress. As you would imagine‚ an electron couldn’t possibles go through both holes at the same time... or could it? Jonssons discovery was a major break through in quantum physics. Heres the peculiar part‚ when you were directly observing the electrons‚ they would go through either one hole or the other‚ but the what we couldn’t see‚ the results showed electrons traveling through both holes‚ leading physicists to believe
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Chemistry: A Molecular Approach (Tro) Chapter 8 Periodic Properties of the Elements 1) Give the ground state electron configuration for Se. A) [Ar]4s23d104p4 B) [Ar]4s24d104p4 C) [Ar]4s23d104p6 D) [Ar]4s23d10 E) [Ar]3d104p4 Answer: A 2) Give the ground state electron configuration for I. A) [Kr]5s24d105p6 B) [Kr]5s24d105p5 C) [Kr]4d105p6 D) [Kr]5s25p6 E) [Kr]5s25d105p6 Answer: B 3) Give the ground state electron configuration for Sr. A) [Kr]5s24d2
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By placing atoms of a metal into a flame‚ electrons can be induced to absorb energy and jump to an excited energy state‚ this is called a quantum jump. They then return to their ground state by emitting a photon of light. The amount of energy in the photon of light determines its color. For example‚ when a photon gives off red light‚ you can determine that it does not have a lot of energy
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absolute zero (0 K or −273.15 °C[1]). Under such conditions‚ a large fraction of the bosons occupy the lowest quantum state‚ at which point quantum effects become apparent on a macroscopic scale. These effects are called macroscopic quantum phenomena. This state of matter was first predicted by Satyendra Nath Bose and Albert Einstein in 1924–25. Bose first sent a paper to Einstein on the quantum statistics of light quanta (now called photons). Einstein was impressed‚ translated the paper himself from
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