Chemical Reactions Physical Science Chemical Reactions When 2
- Slides: 25
Chemical Reactions Physical Science
Chemical Reactions • When 2 or more elements chemically combine to form a “new” substance
Chemical Equation • Is a representation of a chemical reaction • Two Parts • Reactants • Products
Reactants vs Products C + O 2 CO 2 The arrow ( ) divides an equation in half • Reactants – The substance(s) that undergo the change – All things on the left side of the “ ” – Ex: C & O 2 • Products – The new substance(s) that form – All things on the right side of the “ ” – Ex: CO 2
Id the Reactants and Products 1) 2 Cu + O 2 2 Cu. O 2) 2 KCl. O 3 2 KCl + 3 O 2 3) HCl + Na. OH Na. Cl + H 2 O 4) N 2 H 4 + O 2 N 2 + 2 H 2 O
Endothermic vs Exothermic • Endothermic – Reaction absorbs energy from its surrounding – Surrounding becomes cooler • Exothermic – Reaction releases energy to the surrounding – Surrounding becomes warmer
Signs of a Reaction • Production of a GAS – Fizzing, bubbling • Formation of a Precipitate – Insoluble solid • Energy is released – EX: Light, heat • Color Change
Counting Atoms • Number in front is called a coefficient • Coefficients are multiplied to all elements behind it • Subscripts go to what they follow
Counting Atoms Practice 1) 2 CO 2 2) Mg(OH)2 3) 3 Ca(NO 3)2 4) NH 4 OH
End of Day One
How Do I Balance an Equation? • ID the elements present • Count the amount of atoms on both sides of the “ ” for each element • Place coefficients in front of compounds and multiply to any subscript • Recount the atoms on both sides of the “ ” to see if they are equal. If not equal, adjust the coefficients LEFT has to equal RIGHT
Balancing Practice #1 ____Cu + ____O 2 ____Cu. O
Balancing Practice #2 ____N 2 H 4 + ____O 2 ____N 2 + ____H 2 O
Balancing Practice #3 ____KCl. O 3 ____KCl + ____O 2
Choose the Balanced Equation • KCl. O 2 KCl + 2 O 2 • 4 Al + 3 O 2 2 Al 2 O 3 • N 2 + 3 H 2 2 NH 3 • H 2 + O 2 H 2 O • 2 Na. Cl 2 Na + Cl 2
Why Balance? • The Law of Conservation of Matter – Matter is neither created nor destroyed – Start = Finish
End of Day Two
Types of Reactions • 4 Main Types – Synthesis – Decomposition – Single Replacement – Double Replacement • 2 Special Types – Combustion Reaction – Neutralization Reaction
Synthesis Reaction A + B AB • When 2 or more substances react to form a single substance • 2 1 • Dating: Becoming a Couple
Decomposition Reaction AB A + B • When a compound breaks down into two or more substances • 1 2 • Dating: Breaking Up
Single Replacement Reaction A + BC B + AC • A reaction in which one element trades places with another element in a compound • Element and Compound • Dating: CHEATING
Double Replacement Reaction AB + CD AD + BD • Where two different compounds exchange positive ions (cations) to form two new compounds • All compounds – (4 of them) • Dating: Swingers
Type Of Reaction Practice 1. Na 3 PO 4 + 3 KOH 3 Na. OH + K 3 PO 4 2. P 4 + 3 O 2 2 P 2 O 3 3. Pb + Fe. SO 4 Pb. SO 4 + Fe 4. Ca. CO 3 Ca. O + CO 2
Special Reaction: Combustion Reaction • When a hydrocarbon (hydrogen and carbon together) reacts with Oxygen • Products are always CO 2 & H 2 O • Ex: CH 4 + 2 O 2 CO 2 + H 2 O
End of Unit!
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- Chemical reactions section 1 chemical changes
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- The science duo physical and chemical changes
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- Predicting products of chemical reactions
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