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CHEM 11 Chapter Notes - Chapter 1: Chemical Compound, Decimal Mark, Boiling Point

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21 Oct 2016

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Chemistry : the study of nature, properties, and transformations of matter. Matter : the physical material that makes up the universe; anything that has mass and. Properties : a characteristic useful for identifying a substance or object. Size, color, temperature, chemical composition, chemical reactivity. Physical change : a change that does not affect the chemical makeup of a substance or object; does not result in a change in the identity of the substance. ; sugar heated in a saucepan to make caramel. A substance that has a definite shape and volume. A substance that has a definite volume but assumes the shape of its container. A substance that has neither a definite volume nor a definite shape. Every sample of matter is either throughout. Pure substance: a substance that has a uniform chemical composition. Element : a fundamental substance that cannot be broken down.

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I need help doing my lab homework, I missed lab that day because, I was sick and it's due.

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.

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Lab B4 Le ChÃ¢telier's Principle Introduction All chemical reactions proceed until equilibrium is reached, provided none of the reactants or the products are removed from the reaction mixture. Le ChÃ¢telier's principle describes what happens to an equilibrium after it has been disturbed (Ebbing/Gammon, Sections 14.7, 14.8, and 14.9) Purpose You will study the application of Le ChÃ¢telier's principle by seeing the effect of the addition of Fe" and SCN to an equilibrium mixture of Fe ,SCN, and Fe(SCN); the effect of the addition of an acid to an equilibrium mixture of Ni2, NHs, and Ni(NHs the effect of the addition of an acid and a base on the cquilibrium involving an indicator, the effect of acids and bases on the solubility of Ca(OH): in water; and the effect of temperature on an equilibrium mixture of Co, CI, and CoCl New Substances In this experiment you will encounter some substances that you may not have seen before. The reaction between Fe" and SCN (thiocyanate ion) gives Fe(SCN)2+ This substance is adeeply colored complex ion. Other complex ions that you will encounter are Ni(NHs)% and CoCLThese substances result from the reaction between Ni and NH, and from the reaction between Co? and CI, respectively. You will also study an equilibrium involving methyl orange, an indicator. Indicators are discussed in Appendix D. Read the second, third, and fourth paragraphs of that appendix to gain an understanding of the physical and chemical properties of this indicator Concept of the Experiment Le ChÃ¢telier's principle can be described in the following way: "When a system in chemical equilibrium is disturbed by a change of temperature, pressure, or concentration, equilibrium composition in a way that tends to counteract this change of variable" (Ebbing/Gammon, Section 14.7) This statement explains the effects that you will encounter in this experiment. the system shifts in Procedure Getting Started 1. Obtain 3 small test tubes and a piece of filter paper 2. in directions for discarding the solutions that you will use in this experiment from your laboratory instructor. 3. Be careful handling the solutions used in this CAUTION: Solutions of ammonia, hydrochlorie acid, and sodium hydroxide can cause chemiÃ©al burns, in addition to Do not use y mixing these solutions. If you spill any of these solutions on you, wash the contaminated area thoroughly and immediately report the incident to your laboratory instructor. You may require further treatment.

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Lab B4 Le ChÃ¢telier's Principle Introduction All chemical reactions proceed until equilibrium is reached, provided none of the reactants or the products are removed from the reaction mixture. Le ChÃ¢telier's principle describes what happens to an equilibrium after it has been disturbed (Ebbing/Gammon, Sections 14.7, 14.8, and 14.9). 05 Purpose You will study the application of Le ChÃ¢telier's principle by seeing the effect of the addition of Fe and SCN-to an equilibrium mixture of Fe", SCN, and Fe(SCN)ê³¼, the effect of the addition of an acid to an equilibrium mixture of Ni2, NHs, and Ni(NH)% the effect of the addition of an acid and a base on the equilibrium involving an indicator; the effect of acids and bases on the solubility of Ca(OH)2 in water and the effect of temperature on an equilibrium mixture of Co', cr, and CoCla 2- New Substances In this experiment you will encounter some substances that you may not have seen before. The reaction between Fe and SCN (thiocyanate ion) gives Fe(SCN)2. This substance is a deeply colored complex ion. Other complex ions that you will encounter are Ni(NHs)6 and CoCl These substances result from the reaction between Ni? and NH3 and from the reaction between Co and CI, respectively. You will also study an equilibrium involving methyl orange, an indicator. Indicators are discussed in Appendix D. Read the second, third, and fourth paragraphs of that appendix to gain an understanding of the physical and chemical properties of this indicator. Concept of the Experiment Le ChÃ¢telier's principle can be described in the following way: "When a system in chemical equilibrium is disturbed by a change of temperature, pressure, or concentration, the system shifts in equilibrium composition in a way that tends to counteract this change of variable" (Ebbing/Gammon, Section 14.7). This statement explains the effects that you will encounter in this experiment. Procedure lib Getting Started 1. Obtain 3 small test tubes and a piece of filter paper Obtain directions for discarding the solutions that you will use in this experiment from your laboratory instructor. Be careful handling the solutions used in this experiment. 2. 3. CAUTION: Solutions of ammonia, hydrochloric acid, and sodium hydroxide can cause chemical burns, in addition to ruining your clothing. Do not use your finger as a stopper when mixing these solutions. If you spill any of these solutions on you, wash the contaminated area thoroughly and immediately report the incident to your laboratory instructor. You may require further treatment. May not be scanned, copied or duplicated, or posted to a publily accessible website, in whole or in part be o 2013 Cengage Leaming All Rights Reserved. custom page 125