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General Chemistry Lecture 1 Notes (Week 1)

by: nichl

General Chemistry Lecture 1 Notes (Week 1) 01:160:161

Marketplace > Rutgers University > Chemistry > 01:160:161 > General Chemistry Lecture 1 Notes Week 1
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About this Document

Introduction to the class and beginning of chapter 1 notes.
General Chemistry I
Class Notes
General Chemistry




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This 2 page Class Notes was uploaded by nichl on Sunday September 11, 2016. The Class Notes belongs to 01:160:161 at Rutgers University taught by in Fall 2016. Since its upload, it has received 97 views. For similar materials see General Chemistry I in Chemistry at Rutgers University.


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Date Created: 09/11/16
General Chemistry Lecture 1 9/7/16 General Course Guidelines:  Office hours: 12-6 PM  Online recitations are available through:  Recitation Schedule:  Dr. G. Govindarajoo o Email: o Office hours:  Monday 12:20-1:20 Hickman 131  Wednesday 12:35-1:35 Heldrich Science Building 204  Textbook: Chemistry Structure – Properties by Nivaldo Tro  Exams: o Recitations Quiz = 5% o Exam Dates:  October 15 9:40 – 11:00 pm  November 2 9:40 – 11:00 pm  December 7 9:40 – 11:00 pm Chapter 1 Notes:  Definitions: o Chemistry: Study of composition, structure, and properties of matter and the changes that occur when matter interacts o Matter: Anything that has mass and occupies space o Atom: Smallest distinctive units of matter o Substance: a type of matter that has a definite or fixed composition that does not vary from one sample to another (e.g2 H O) o Element: A substance that cannot be broken down into simpler substances through a chemical reaction (e.g. He) o Compound: Substance made of two or more types of elements in fixed proportions (e.g. H2O)  States of Matter: o Solid: Strongest attractions between particles, rigid shape, fixed volume o Liquid: Fixed volume, no fixed shape, free to move (fluid) o Gas: Weakest attraction between particles, doesn’t clump together, no fixed shape/volume  Mixtures: General Chemistry Lecture 1 9/7/16 o No fixed composition or ratios o Homogeneous mixtures (solutions):  Mixture that has the same composition and properties throughout the sample (i.e. a sugar water solution has same amount of sugar at top and bottom of a column) o Heterogeneous mixture:  Varies in composition and/or varies in properties between different parts of the mixture (i.e. granite)  Scientific method: o Hypothesis: Tentative explanation or prediction that must be testable by experimentation and create scientific data o Scientific data: provides patterns that can be summarized into scientific laws o Scientific Theory: Provides explanations for a natural phenomenon that can be tested by further experimentation Questions Findings Hypothesis Questions o Hypothesis and theories can be disproved by better tech, etc.  Chemical reactions: Chemical change process that changes to composition of a material (i.e. burning gasoline)  Law of Conservation of Mass: In a chemical reaction. Matter is neither created nor destroyed. Mass stays the same. Combined mass of reactants must equal combined mass of products  Law of Definite Proportions: All samples of a given compound (pure) regardless of the source at preparation have the same proportion of their constituent elements Practice 1.1 Pg. 11 2 samples of Carbon Monoxide (CO) Sample 1 – 17.2g O + 12.9g C 17.2/12.9 = 1.33g O/1g C Sample 2 – 10.5g O + 7.8g C 10.5/7.8 = 1.3g O/1g C Suggested Problems: Ch. 1.1 – 1.7 # 35, 41, 49, 53, 59, 61


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