Acids and Bases Lab 2 Compound |Observations |Type of Compound (Acid/base? Ionic/Covalent?) |Amount (Drops) |Conductor of Electricity? Yes/ No | |NaOH (0.5 mol/L) Reactant |Clear‚ odourless‚ liquid |Base Ionic |20 |Not tested | |Phenolphthalein Indicator |Clear‚ liquid‚ alcohol odour |pH indicator |1 |Not Tested | |HCl (0.5 mol/L) Reactant |Clear‚ liquid‚ sour odour |Acid Ionic |44 |Not tested | |H2O (water) Product |Clear‚ liquid‚ odourless |Non-reactive Covalent |Not measured |No
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– Mr Most substances exist as; - compounds if ionic - molecules if covalent We can use Ar’s to calculate the ‘average mass of ONE unit of a substance’ this is called the Mr (see also topic 9) E.g. Calculate the Mr for sodium carbonate 3Na2CO3. Ar (Na) = 23 Ar (C) = 12 Ar (O) = 16 The number 3 in front of the formula has been ignored because by definition Mr is the mass of ONE unit of a substance whether the substance is ionic or covalent. Molar mass This is the mass of one
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HF – hydrogen fluoride is a covalent bond and shares one pair of electrons. The hydrogen end of the molecule is slightly positive and the fluorine end is slightly negative. This causes hydrogen bonding between other hydrogen fluoride molecules. KCl – potassium chloride is a metal halide salt. The bonding between potassium and chloride is an ionic bond. The potassium becomes a cation and the chloride an anion. The potassium end of the molecule becomes slightly positive and the other end slightly
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Assessment 1) Describe the difference between ionic and covalent bond. Ionic bonds have electrostatic forces that hold cations and anions together‚ and are electronic neutral. Covalent bonds are bonds that don’t give or take any electrons. In stead they share the elctrons 50) Which of these compounds contain elements that do not follow the octet rule? Explain. a) NF3: 5 + (7*3) = 26 b) PCl2F3: 5 + (7*2) + (7*3) = 40 c) SF4: 6 + (7 *4) = 24 d) SCl2: 6 + (7*2) = 20 The answer is “d”
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Study guide for exam 3 Chem 1212 Fall 2014 (chapters 3‚4‚ 14‚15) Chapter 3 Nomenclature ionic compounds‚ molecular compounds‚ simple organic compounds‚ hydrates‚ acids Know the names and charges of the polyatomic ions Calculation molecular weight mw Molar mass of compound Number particles = NA x n Mass % Determination of empirical formula and molecular formula Combustion analysis Balancing equations Chapter 4 Limiting reactant Mole to mole conversion from reaction stoichiometry Theoretical yield
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Organic chemistry is the study of essentially all substances containing carbon. Organic compounds that contain only carbon and hydrogen are called hydrocarbons. The simplest hydrocarbons are the alkanes which contain only single covalent bonds. Methane is the simplest alkane. It is also the major component of natural gas. Methane contains only 1 carbon in the molecular formula and the structural formula. There is ethane which is 2 carbons‚ propane that is 3‚ butane which is 4‚ pentane which is 5
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the periodic table tell you about a Group A element? Define molecule Define compound Define ionic bond and describe how they are formed Define ion Define cation Define anion Define polyatomic ion Define covalent bond and describe how they are formed Define electronegativity and describe how it is used to determine if a bond is ionic‚ polar covalent or nonpolar covalent Define polar covalent bond Define nonpolar covalent bond What kind of bonds are found within a water molecule? What kind of bond
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200 Things to Know to Pass the Chemistry Exam 1. Protons are positively charged (+) with a mass of 1 amu. Example: Which has the greatest nuclear charge? Cl-35 Ar-40 K-39 Ca-40 2. Neutrons have no charge and a mass of 1 amu. 3. Electrons are small and are negatively charged (-) with a mass of almost 0 amu.. 4. Protons & neutrons are in an atom’s nucleus (nucleons). Which has the greatest number of nucleons? Sn-119 Sb-122 Te-128 I-127 5. Electrons are found in “clouds”
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1: Identifying the ionic compound By visual inspection‚ the compound in bottle A was pure element‚ and the compound in bottle D was heterogeneous mixture because the mixture does not mix well and the proportions of substances were uneven visually. To determine the ionic compound from compound B and compound C‚ a conductivity test and solubility test were carried out. Both compounds were mixed with water. Both compounds were soluble in water. Therefore‚ the type of compounds could not yet be determined
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molecules‚ energy‚ rate‚ temperature) Name some compounds: H2O (Hydrogen and Oxygen elements - Water) CH4 (Carbon and Hydrogen elements - Methane) NaCl (Sodium Chloride- salt) Different types of compounds: Metal + Metal = Metallic Compound Metal + Non-Metal = Ionic compound Non-Metal + Non-Metal = Covalent compound Different types of reactions: Metal+ non-metal ionic compound Non-metal + non-metal covalent compound Metal + metal metallic compound Respiration‚ oxidation‚ photosynthesis and precipitation:
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