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01:160:159 Lecture Notes - Lecture 1: Significant Figures, Kilogram, Fokker E.Ii

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apricotherring648

3 Apr 2016

School

Rutgers University

Department

Course

Professor

Saterah Marvasti

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Document Summary

Chapter 1: keys to the study of chemistry: some fundamental definitions i. Physical properties - substance shows by itself, without changing into or interacting with another substance. Physical change - substance alters its physical form, not composition: ex. Chemical properties - substance shows as it changes into or interacts with another substance. Chemical change/chemical reaction - substance converted into different substance: ex. Lower potential energy is more stable: opposite charges attract each other and like charges repel each other viii. Observations - quantitative are most useful: natural law - same observation with no clear exceptions. Hypothesis - proposal made to explain an observation; must be testable. Experiment - procedural steps that test a hypothesis; must be reproducible ii. iii: model - formulates theories based on experiments, chemical problem solving, units and conversion factors in calculations i. ii. Conversion factors - ratios that express a measured quantity in different units. Dimensional analysis - factor label method: measurement in scientific study i.

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Chemical Reactions and Equations Learning objectives To observe physical and chemical properties associated with chemical changes To be able to give evidence for the occurrence of a chemical reaction To write a balanced chemical equation To identify areaction as a combination, decomposition, precipitation, single or double replacement, or combustion reaction ntroduction When a substance undergoes a physical change, it changes its appearance but not its composition. For example, when ice melts to form water, it undergoes a physical change from solid to liquid. In a chemical change, the composition of a substance is changed to give a new substance with different physical and chemical properties. For example, when silver tarnishes, the shiny silver (Ag) changes to a dull gray silver sulfide (AgaS). Not only has the chemical formula changed from Ag to Agus, but also the physical properties (shininess) of the substance have changed. Some examples of physical and chemical changes are listed in Table 1 below. Table 1. Comparison of Physical and Chemical Changes Examples of Physical changes Examples and Evidence of Chemical Changes Change in state (melting, freezing, evaporating Formation of a gas (bubbles) subliming) Formation of a solid (precipitate) Change in size Tearing Change in Color Heat is given off or absorbed A solid dissolving in a solvent In a chemical reaction, atoms in the reactants are rearranged to produce new combinations of atoms in the products. However, the total number of atoms of each element in the reactants is equal to the total number of atoms in the products. This is true according to the Law of Conservation of Mass, which states that the total mass remains constant during a chemical reaction. In other words, matter cannot be created or destroyed in a chemical reaction. In a chemical equation, the reactants are shown on the left and the products are on the right. An arrow in between indicates that a chemical reaction occurs. Finally, the physical state of each compound is designated in parentheses after the chemical formula. Solid, liquid, gas, and aqueous (dissolved in water) are shown as(s,(n,(g), and (aq), respectively.