Types of chemical reactions Knowing the different types of reactions gives you the ability to predict what the products will be after the chemical reactions.

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Types of chemical reactions Knowing the different types of reactions gives you the ability to predict what the products will be after the chemical reactions. Remember: In all chemical reactions mass, charge and energy are conserved. Slide 2 Synthesis NOTES 2 or more substances combine to form a more complex substance Can be written in the general form: Also called a combination reaction A + B AB Slide 3 Putting Puzzle Pieces Together Synthesis Reaction Slide 4 Fe + S FeS 2Mg + O 2 H 2 O + SO 3 H 2 SO 4 2MgO Slide 5 NOTES Decomposition 1 substance breaks down into 2 or more simpler substances Can be written in the general form: Also known as an analysis reaction. AB A + B Slide 6 Breaking Apart a Puzzle Decomposition Reaction Slide 7 FeS Fe + S 2NaCl CaCO 3 CaO + CO 2 2Na + Cl 2 Slide 8 NOTES Single Replacement 1 element replaces another that is in a compound. There is ALWAYS a single element and a compound reacting. This can be written in the general form: A + BX B + AX Slide 9 Sharing among Children Single Replacement Reaction Slide 10 Zn + 2HCl ZnCl 2 + H 2 2Na + CuSO 4 Na 2 SO 4 + Cu Cl 2 + 2KBr 2KCl + Br 2 Slide 11 NOTES Double Replacement 2 substances in two compounds switch partners. A compound always reacts with a compound. This can be written in the general form: AB + CD AD + CB Slide 12 Trading Double Replacement Reaction Slide 13 NaCl + AgNO 3 NaNO 3 + AgCl 2K 3 PO 4 + 3CaS Ca 3 (PO 4 ) 2 + 3K 2 S Slide 14 Solving Synthesis Reactions Slide 15 Formula Writing In ionic bonds, an electron is transferred between the atoms. Example: Na Cl +1+1 Slide 16 Formula Writing We can get the charge of an atom by looking at the periodic table. Slide 17 What is the charge of a phosphorous ion? What is the charge of a magnesium ion? What are the charges of the ions Lithium and Fluorine? Slide 18 Formula Writing Once we have the charges, we crisscross the numbers to the subscript position. NaCl +1+1 Slide 19 Formula Writing So the final formula for sodium and chlorine is just NaCl Slide 20 What is the formula for Na and Br? What is the formula for Mg and Cl? What is the formula for Rh and O? Slide 21 Solving Equations So now we can write formulas We can identify synthesis reactions Lets put it all together. H 2 + 0 2 ???? Slide 22 Solving Equations H 2 + 0 2 Step 1: Look up the oxidation states for each element on the periodic table. Slide 23 Solving Equations H 2 + 0 2 Step 2:Crisscross Slide 24 Solving Equations H 2 + 0 2 Step 3: Rewrite Slide 25 Solving Equations H 2 + 0 2 Step 4: Balance the Equation H2OH2O Slide 26 Solve the following equation Na + F 2 ??? Slide 27 Solve the following equation H 2 + P ??? Slide 28 Solve the following equation Sr + N ??? Slide 29 NOTES Decomposition 1 substance breaks down into 2 or more simpler substances AB A + B Slide 30 Breaking Apart a Puzzle Decomposition Reaction Slide 31 FeS Fe + S 2NaCl CaCO 3 CaO + CO 2 2Na + Cl 2 Slide 32 Decomposition Reactions Decomposition reactions are the same as synthesis reactions, only in reverse. 2H 2 + O 2 2H 2 O 2H 2 O 2H 2 + O 2 Slide 33 Diatomic Atoms When breaking a compound apart, you must remember that not all elements stay alone. Elements that naturally bond with themselves are called Diatomic H2H2 O2O2 N2N2 Br 2 I2I2 F2F2 Cl 2 I 2 Br 2 ing Cl 2 ay F 2 rom O 2 ur N 2 ew H 2 ouse Slide 34 Decomposition Reactions NaCl SrF 2 Slide 35 Practice: Complete the following decomposition reactions 1. MgBr 2 2. Na 2 O 3. HCl Slide 36 NOTES Single Replacement 1 substance in a compound replaces another. An element reacts with a compound. AB + C AC + B AB + C CB + A Slide 37 Sharing among Children Single Replacement Reaction Slide 38 Why do single replacement reactions occur? A more reactive element replaces a less reactive element NOTES Slide 39 Zn + 2HCl ZnCl 2 + H 2 2Na + CuSO 4 Na 2 SO 4 + Cu Cl 2 + 2KBr 2KCl + Br 2 Slide 40 Single Replacement Reactions In a single replacement reaction, one element replaces another in a compound. Sr + 2HCl H 2 + SrCl 2 Slide 41 Formulas Remember, the first element in a compounds formula is the cation (positively charged ion). The second element in a compounds formula is the anion (negatively charged ion) Slide 42 Who to Replace? Step 1: What is the potential charge on the single element? Step 2: Which element in the compound has the same type of charge? Be + NaCl 2+ 1+ 1- BeCl 2 + Na Slide 43 Complete the following reaction: Li + NaCl Complete the following reaction: O 2 + NaCl Slide 44 But will it happen? In order for one element to replace another, it must be higher on Table J than Slide 45 Check Your Homework Any Questions? 5. 2Na + 2HOH H 2 + 2NaOH 6. B + 3KF 3K + BF 3 7. Ba + BaS Ba + BaS 8. Ca + 2HOH H 2 + Ca(OH) 2 Slide 46 NOTES Double Replacement 2 substances in a compound switch partners. A compound reacts with a compound. AB + CD AD + CB Slide 47 Trading Double Replacement Reaction Slide 48 Why do double replacement reactions occur? One of the products must form as a gas, a precipitate or as water NOTES Slide 49 Also known as ionic reaction or solution reaction Slide 50 NaCl + AgNO 3 NaNO 3 + AgCl 2K 3 PO 4 + 3CaS Ca 3 (PO 4 ) 2 + 3K 2 S Slide 51 Double Replacement Reactions In a double replacement reaction, two ions switch places in two compounds. NaFLiCl Slide 52 Double Replacement Reactions Once you have identified which two will switch (by looking at the charges), complete the switch and rewrite the formula. NaN+Mg O 3 Slide 53 Double Replacement Reactions KF + SrO Slide 54 Practice: NaCl + BeF 2 Slide 55 Practice: MgO + KCl Slide 56 Practice: BaBr 2 + K 2 O Slide 57 Polyatomic Ions Polyatomic Ions are multinuclear ions that can be treated as a group of atoms with a charge. Slide 58 KCNSr SO 3 1+1-2+ 2- 1+ 1- 2+2- 22 ( ) Slide 59 Complete: Ba(NO 3 ) 2 + K 2 C 2 O 4 Slide 60 Complete: NaHCO 3 + HCl