Skyler Wild - Final Chemistry Notebook

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Determine the Type of Reaction for each equation. Then predict the products of each of the following chemical reactions. If a reaction will not occur, explain why not. Then Balance the equation. AB + CD 1) __Ag2SO4 + __NaNO3 → NO REACTION For this reaction t occur, both reactants and only one of the products must be soluble in water. Ag2SO3 is partly soluble in water, and the other compounds are soluble in water. Which says that the reaction will not occur. 2) __NaI + __CaSO4 → NO REACTION Both products are soluble in water, and CaSO4 is only partially soluble in water, meaning that the conditions for a successful double displacement reaction are not met, a reaction will not occur. 3) __HNO3 + __Ca(OH)2 → 2 1 1 Ca(NO3)2 + 2 H2O acid-base reaction 4) __CaCO3 → 1 1 CaO + 1 CO2 decomposition reaction 5) __AlCl3 + __(NH4)PO4 → AlPO4 + 3 NH4Cl double displacement reaction 6) __Pb + __Fe(NO3)3 → NO REACTION Lead is lower on the activity serioes than the iron that would replace it in the reaction, the reaction does not occur. 7) __C3H6 2 + __O2 9 → 6 CO2 + 6 H2O combustion reaction 8) __Na 2 + __CaSO4 1 → 1 Na2SO4 + 1 Ca single displacement reaction 105
The Learning Goal for this assignment is: Apply the mole concept and the law of conservation of mass to calculate quantities of chemicals particles in reactions. Stoichiometry and Balancing Reactions Stoichiometry is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data. In Greek, stoikhein means element and metron means measure, so stoichiometry literally translated means the measure of elements. In order to use stoichiometry to run calculations about chemical reactions, it is important to first understand the relationships that exist between products and reactants and why they exist, which require understanding how to balanced reactions. Balancing In chemistry, chemical reactions are frequently written as an equation, using chemical symbols. The reactants are displayed on the left side of the equation and the products are shown on the right, with the separation of either a single or double arrow that signifies the direction of the reaction. The significance of single and double arrow is important when discussing solubility constants, but we will not go into detail about it in this module. To balance an equation, it is necessary that there are the same number of atoms on the left side of the equation as the right. One can do this by raising the coefficients. Reactants to Products A chemical equation is like a recipe for a reaction so it displays all the ingredients or terms of a chemical reaction. It includes the elements, molecules, or ions in the reactants and in the products as well as their states, and the proportion for how much of each particle is create relative to one another, through the stoichiometric coefficient. The following equation demonstrates the typical format of a chemical equation: 2Na(s) + 2HCl(aq) → 2NaCl(aq) + H2(g) In the above equation, the elements present in the reaction are represented by their chemical symbols. Based on the Law of Conservation of Mass, which states that matter is neither created nor destroyed in a chemical reaction, every chemical reaction has the same elements in its reactants and products, though the elements they are paired up with often change in a reaction. In this reaction, sodium (Na), hydrogen (H), and chloride (Cl) are the elements present in both reactants, so based on the law of conservation of mass, they are also present on the product side of the equations. Displaying each element is important when using the chemical equation to convert between elements. Stoichiometric Coefficients In a balanced reaction, both sides of the equation have the same number of elements. The stoichiometric coefficient is the number written in front of atoms, ion and molecules in a chemical reaction to balance the number of each element on both the reactant and product sides of the equation. These stoichiometric coefficients are useful since they establish the mole ratio between reactants and products. In the balanced equation: 2Na(s)+2HCl(aq)→2NaCl(aq)+H2(g) 106
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Reference Tables for Physical Setti
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150. 140. Table G Solubility Curves
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Table I Heats of Reaction at 101.3
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Table O Symbols Used in Nuclear Che
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0 6.941 +1 Li 3 2-1 Na 39.0983 K +1
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First Atomic Symbol Name Ionization
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Collier County CHEMISTRY EXAM FORMU
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Honors Chemistry Class Policies and
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Unit 1 (22 days) Chapter 1 Introduc
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4 Lorenzo Walker Technical High Sch
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MUSTANG LABORATORIES COMMITMENT TO
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Chapter 1 Unit 1 Introduction to Ch
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The Learning Goal for this assignme
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2. One cereal bar has a mass of 37
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1. How many meters are in one kilom
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RULE #3: To add/subtract in scienti
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Rule 3: A final zero or trailing ze
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24 For addition and subtraction, lo
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Dimensional Analysis This is a way
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Chapter 4 Unit 2 Atomic Structure T
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Looking at Ions We haven’t talked
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Neutron Madness We have already lea
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Create groups for these Scientist a
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38
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In the space below, write the unabb
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Skyler Wild Name __________________
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The Learning Goal for this Assignme
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Atomic Size Define Atomic Size: The
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Define Electronegativity: Electrone
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Learning Goal for this section: Exp
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Beta Particle Decay Beta decay is a
Page 76 and 77: Inside the sun, fusion reactions ta
Page 78 and 79: 58 Chapter 7 Unit 3 Ionic and Metal
Page 80 and 81: The Learning Goal for this assignme
Page 82 and 83: Ion Charge? What is the charge on f
Page 84 and 85: Here are some examples for you: Zn
Page 88 and 89: C 2 H 6 O Ethanol CH 3 CH 2 O Step
Page 90 and 91: Name Formula Charge Dichromate Cr
Page 93 and 94: Name Skyler Wild Date Example: Xeno
Page 95 and 96: Trioxygen Chemical Name O 3 Chemica
Page 97 and 98: Phosphorus Pentafluoride Chemical N
Page 99 and 100: 78 Finding Bond Angles, Shapes, and
Page 101 and 102: case, we count two things stuck to
Page 103 and 104: Unit 4 Chapter 22 Hydrocarbon Compo
Page 105 and 106: 84 https://www.bbc.co.uk/education/
Page 107 and 108: Introduction to Organic Chemistry T
Page 109 and 110: Carbon Prefix Alkane Name Chemical
Page 111 and 112: Unit 5 Chapter 10 Chemical Quantiti
Page 113 and 114: Learning Goal for this section: Des
Page 115 and 116: Example: Converting between mass an
Page 119 and 120: Step 5 Balance the hydrogen atoms n
Page 121 and 122: 6) ___ 1 Mn(NO2)2 + ___ 1 BeCl2 __
Page 125: Single Disp ----------> A+BC x BOTH
Page 129 and 130: Stoichiometry and Balanced Equation
Page 131 and 132: Step 1: 200g C3H8 is equal to 4.54
Page 133 and 134: Stoichiometry and balanced equation
Page 135 and 136: Discussion Due to chemical equilibr
Page 137 and 138: Stoichiometry Skyler Wild Molecu
Page 139 and 140: Unit 6 Chapter 13 States of Matter
Page 141 and 142: Name: Skyler W. Name: Jahrew P. Gra
Page 143 and 144: Lesson #2: A Model for Liquids: Ess
Page 145 and 146: The Learning Goal for this is: Stud
Page 147 and 148: Then substitute them into the const
Page 149 and 150: P1V1 = P2V2 T1 It is important to n
Page 153 and 154: 132 Unit 7 Chapter 16 Solutions The
Page 159 and 160: The Time-Temperature Graph We are g
Page 161 and 162: Step Two: solid ice melts Now, we c
Page 163 and 164: Step Four: liquid water boils Now,
Page 165 and 166: 144 The following table summarizes
Page 169 and 170: Phase Diagram Information on a Phas
Page 171 and 172: Heating Curve Information on a Phas
Page 173 and 174: Unit 8 Chapter 19 Acid and Bases Th
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This would be a generic base: XOH -
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HCl + H2O ⇌ H3O + + Cl¯ HCl - th
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Several categories of substances ca
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1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
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2. What is the oxidation number of
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One point of concern: notice that e
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Skyler Wild - Final Chemistry Notebook

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