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CHM 131 Lecture Notes - Lecture 3: Ionic Compound, Ion, Covalent Bond

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peachwoodchuck721

9 Aug 2018

School

University of Rochester

Department

Course

Professor

Benjamin Hafensteiner

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Document Summary

Due to the conservation of mass, a chemical reaction completely converts the reagents/reactants into the products. In other words, the number of atoms in the reactants is the same as the number of atoms in the products. As a result, the mass of the products are equivalent to the mass of the reactant. The law of conservation of mass states that mass is neither created nor destroyed, it transforms from one state to other and is constant because atoms can be neither created nor destroyed. The law of definite proportion says that atoms are present in specific ratios in compounds. The law of multiple proportions says that elements are in integer ratios of mass proportions in different compounds. N the former compound, barium is only capable of forming one cation with a charge of. In the latter compound, however, iron where is capable of forming more than one type of cation, 2+ and 3+.

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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.