Unit 6 Chemical Reactions
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failing123 on January 21, 2012
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Terms | Definitions |
|---|---|
 Chemical Reaction | is a chemical change, which is any change in matter that results in the formation of a new substance. Which is a change in identity. |
| Reactant | Any substance made out of atoms that undergoes a chemical reaction. |
| Products | The substances made out of atoms that are formed in a reaction. |
| differences of the reactant and of the product | When the reaction takes place, the reactant transforms into the product. the product and the reactant are different substances, which have different composition, structure and properties. |
| Reactants → Products | Reactants yield Products |
| The first part of the reactants to products transformation | The atoms of the reactants become rearranged (this is when the existing bonds break and new bonds form). |
| The second part of the reactants to products transformation | Once the atoms are in new arrangement, new substances (the products) exist. |
| Conservation of Mass in Chemical Reactions | In reaction equations, no atoms can be created or destroyed; atoms can only be rearranged in the process. |
| Importance of the Law of Conservation of Mass in Chemical Reactions | The number of atoms on the left side must equal the number of atoms on the right side. (the total number of atoms of any given element in the reactants must equal the number of atoms of that element in the products. ) |
| Counting Atoms in Formulas and Reaction Equations | with and without prentheses |
| The subscript that immediately follows an atomic symbol shows what? | It shows how many of that atom is present in the formula unit. |
| How many atoms are in CO₂ | C:1 atom (1 carbon atom) O: 2 atoms (2 oxygen atoms) |
| The subscript outside those parentheses shows what? | it shows how many atoms each of those elements inside the parentheses are present. |
| How many atoms are in Mg(OH)₂ | Mg: 1 atom (1 magnesium atom) O: 2 atoms (2 oxygen atoms) H: 2 atoms (2 hydrogen atoms) |
| Reaction Coefficient | it is the number written before a formula in a reaction equation. |
| when there are reaction coefficients, how do you count the atoms? | when counting atoms, reaction coefficients distribute to all atoms in the formula unit |
| How many atoms are in 3 Mg(OH)₂ | Mg: 3 atoms (3 magnesium atoms) O: 6 atoms (6 oxygen atoms) H: 6 atoms (6 hydrogen atoms) |
| How many atoms of each element are in the formula and what is the name of the formula ? | answer the following questions |
| SO₃ | Sulfur Oxide S: 1, O: 3 |
| K₃PO₄ | Potassium Phosphate K: 3, P: 1, O: 4 |
| (NH₄)₂SO₄ | Ammonium Sulfate N: 2, H: 8, S: 1, O:4 |
| 2 N₂O₅ | Dintrogen Pentoxide N: 4, O: 10 |
| 5 Cr(C₂H₃O₂)₆ | Cr:5, C: 60, H: 90, O: 60 |
| B₂O₃ | diboran trioxide B: 2, O: 3 |
| Mg₃(PO₄)₂ | Magnesium Phosphate Mg: 3, P: 2, O: 8 |
| 3 Mn₂ O₅ | Manganese (V) Oxide Mn: 6, O: 15 |
| 6 (NH₄)₂H₂PO₄ | N:12, H:60, P:6, O:24 |
| 5 Fe₂(C₂O₄)₃ | Fe:10, C:30, O:60 |
| Balancing Reactions | the reactants side (left side) have to same amount of atoms of each element as the Products (right side) |
| Balance (Hydrogen + Oxygen → Water) H₂ + O₂ → H₂O | 2 H₂ + O₂ → 2 H₂O |
| Balance (Sodium + Oxygen → Sodium Oxide) Na + O₂ →Na₂O | 4 Na + O₂ → 2 Na₂O |
| Balance (Aluminum + Oxygen → Aluminum Oxide) Al + O₂ → Al₂O₃ | 4 Al + 3 O₂ → 2 Al₂O₃ |
| Strategy to balance equations | balance the elements starting with those who appear the least and finishing with the most abundant. |
| CHO | when carbon, hydrogen and oxygen are the elements, then you always balance C first, H second and O last |
| CH₄ + O₂ → CO₂ + H₂O | CH₄ + 2 O₂ → CO₂ + 2 H₂O |
| C₃H₈ + O₂ → CO₂ + H₂O | C₃H₈ +5 O₂ → 3 CO₂ + 4 H₂O |
| Balancing reactions with Polyatomic Ionic Compounds | If the same polyatomic ion is on both sides of the reaction, then it is counted as if it were an element. |
| Al + Cu(NO₃)₂ → Cu + Al(NO₃)₃ | 2 Al + 3 Cu(NO₃)₂ → 3 Cu + 2 Al(NO₃)₃ |
| (NH₄)₂SO₄ + Pb(NO₃)₂ → NH₄NO₃ + PbSO₄ | (NH₄)₂SO₄ + Pb(NO₃)₂ → 2 NH₄NO₃ + PbSO₄ |
| (NH₄)₃PO₄ + AgNO₃ → NH₄NO₃ + Ag₃PO₄ | (NH₄)₃PO₄ + 3 AgNO₃ → 3 NH₄NO₃ + Ag₃PO₄ |
| States of Matter in Chemical Reactions | The state of matter for each reactant and product is often presented in a reaction equation. |
| (s) | solid |
| Cu(s) | solid copper metal |
| (l) | pure liquid |
| H₂O(l) | pure liquid water |
| (g) | gas |
| O₂(g) | oxygen gas |
| (aq) | aqueous solution (a solution where water is the solvent) |
| NaCl (aq) | aqueous sodium chloride, which is sodium chloride dissolved in water which is salt water. |
| the mole | is the unit of measurement that is used in all substances that are in a chemical reaction. |
| 1 mole = ? atoms | 6.022x10²³ atoms |
| 2 H₂ + O₂ → 2 H₂O | 2 moles of hydrogen + 1 mole of Oxygen yields 2 moles of water |
| Mole Ratios and Conversions | ??? |
| 2 H₂ + O₂ → 2 H₂O | use this in the following questions |
| what is the mole ratio of H₂ to O₂? | 2:1 |
| what is the mole ratio of O₂ to H₂O? | 1:2 |
| what is the mole ratio of H₂ to H₂O? | 2:2 or 1:1 |
| mole to mole conversions | ???? |
| If you need 100 moles of water to serve everyone, then how many moles of Hydrogen will you need? | 100 H₂ + 50 O₂ → 100 H₂O 100 moles of Hydrogen and 50 moles of Oxygen |
| C₈H₁₈ + O₂ → CO₂ + H₂O | 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O |
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