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Slide 2

A _________ is a substance that speeds up a chemical reaction without being permanently consumed in the reaction. catalyst

Slide 3

List the naturally occurring diatomic molecules. H 2, O 2, N 2, Cl 2, Br 2, I 2, F 2

Slide 4

Using collision theory, EXPLAIN why increasing the temperature of a reaction increases the reaction rate? Increasing the temperature also increases the kinetic energy of the reacting molecules. So molecules are moving faster and will collide more often. More collisions = faster reaction rate!

Slide 5

_____________ is the speed of the disappearance of a reactant or the rate of the appearance of a product in a chemical reaction. Reaction rate

Slide 6

Equations must always be balanced because a certain law of chemistry cannot be violated. What is the name of the law that cannot be violated? Law of Conservation of Matter

Slide 7

The arrow between the reactants and products means__________. yields

Slide 8

List the four indicators that a chemical reaction occurred. Heat/light Precipitate Gas (bubbles) Color change

Slide 9

In a chemical equation, what is indicated by the symbol? Heat is added to the reaction

Slide 10

In a chemical equation, what is indicated by the symbol? A precipitate is formed

Slide 11

What are the 4 factors that affect the reaction rate? Temperature Concentration Nature of Reactants Catalyst

Slide 12

List the reactants in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) CH 4 + 2O 2

Slide 13

Using collision theory, EXPLAIN why increasing the concentration of a reactant increases the reaction rate? More molecules are present as the concentration is increased. So more molecules present equals more collisions between reacting molecules. More collisions = faster reaction rate!

Slide 14

In a chemical equation, what is indicated by the H 2 SO 4 symbol? That H 2 SO 4 was used as a catalyst is this reaction

Slide 15

List the products in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) CO 2 + 2H 2 O

Slide 16

How many atoms of O are in 2H 2 O following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2

Slide 17

What is does the represent in the following equation: 2H 2 + O 2 2H 2 O A reversible reaction. The reaction can go both ways- reactants yield products and product can yield reactants

Slide 18

What type of reaction would the following be classified as? AB + CD AD + CB Double displacement

Slide 19

Suppose in the following reaction that 10g of Mg was added to 14g of O 2, how many grams of MgO would be produced? 2Mg (s) + 2O 2 (g) 2MgO (s) 24 g b/c the Law of Conservation of Matter (the amount of matter you start with is the same amount that you end with!)

Slide 20

How many atoms of C are in CO 2 following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1

Slide 21

How many moles of CH 4 are present following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1

Slide 22

What ions are present for H 2 0? H+ and OH-

Slide 23

How many molecules of 2O 2 are present following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2

Slide 24

Which of the following substances would be a gas that is produced in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) CO 2

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What type of reaction would the following be classified as? A + B AB Synthesis

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Which type of reaction has only one REACTANT? Decomposition

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What type of reaction would the following be classified as? A + BC AC + B Single displacement

Slide 28

Which of the following substances would be a liquid in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2H 2 O

Slide 29

How many molecules of CH 4 are present following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1

Slide 30

What ion is ALWAYS present in any acid? H+

Slide 31

Which type of reaction has only one PRODUCT being produced? Synthesis

Slide 32

What does (aq) represent after a substance? Aqueous substance was dissolved in water

Slide 33

Is the following reaction correct? Explain. 2Mg (s) + 2O 2 (g) 2PbO (s) NO! b/c the Law of Conservation of Matter (the same types of atoms must be present on both sides of the equation. Mg cant be changed into Pb!

Slide 34

What type of reaction would the following be classified as? AB A + B Decomposition

Slide 35

Balance the following equation: potassium + water potassium hydroxide + hydrogen 2K + 2H 2 O 2KOH + H 2

Slide 36

Balance the following equation: fluorine + aluminum oxide aluminum fluoride + oxygen 6F 2 + 2Al 2 O 3 4AlF 3 + 3O 2

Slide 37

Identify the type of reaction. Finish the word equation & write the balanced equation: Aluminum + hydrochloric acid Single Displacement Aluminum chloride + hydrogen 2Al + 6HCl 2AlCl 3 + 3H 2

Slide 38

Identify the type of reaction. Finish the word equation & write the balanced equation: calcium fluoride + water Double Displacement Calcium hydroxide + hydrogen fluoride CaF 2 + 2H 2 O Ca(OH) 2 + 2HF

Slide 39

Identify the type of reaction. Finish the word equation & write the balanced equation: potassium oxide Decomposition potassium + oxygen 2K 2 O 4K + O 2

Slide 40

Identify the type of reaction. Finish the word equation & write the balanced equation: strontium + chlorine synthesis Strontium chloride Sr + Cl 2 SrCl 2 *Balanced