chapter 14 chemical raection

7/28/2019 chapter 14 chemical raection

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Liberty Christian Academy

General Chemistry

Miss Kostura

Chapter 14

Chemical Reactions


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What is the difference?

Forming New Substances
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Leaves change colors in the fall but what

is happening to cause this change?

Leaves contain a compound called

chlorophyll. Chlorophyll undergoes a

chemical change and forms simplersubstances that have no color.

http://images.google.com/imgres?imgurl=http://www.travelsandjourneys.com/images/fall-leaves.jpg&imgrefurl=http://greenopolis.com/myopolis/blogs/hlund05/climate-change-ruining-fall-foliage&usg=__ZAUmi7jzgWIOKmhSJzPCQrXmQgM=&h=426&w=640&sz=55&hl=en&start=5&um=1&tbnid=6Of5K6pIDEq2zM:&tbnh=91&tbnw=137&prev=/images?q=leaves&um=1&hl=en&sa=Nhttp://images.google.com/imgres?imgurl=http://www.hsv.k12.al.us/schools/middle/wtms/student/cell/chlorophyll.jpg&imgrefurl=http://www.hsv.k12.al.us/schools/middle/wtms/student/cell/cell_energy.html&usg=__zZo7OnlqCgveBcdvmXxn7bLsDLQ=&h=300&w=300&sz=17&hl=en&start=2&um=1&tbnid=NWCuMA-l-ytu3M:&tbnh=116&tbnw=116&prev=/images?q=chlorophyll&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.usoe.k12.ut.us/curr/Science/sciber00/8th/energy/images/chloro.jpg&imgrefurl=http://www.usoe.k12.ut.us/curr/Science/sciber00/8th/energy/sciber/chloroph.htm&usg=__O-m7ncNW-0WHVaIFEUaAhQOfreE=&h=279&w=288&sz=28&hl=en&start=3&um=1&tbnid=GpHS0pWU00GPlM:&tbnh=111&tbnw=115&prev=/images?q=chlorophyll&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.steve.gb.com/images/molecules/porphyrins/chlorophyll-a.png&imgrefurl=http://www.steve.gb.com/science/photosynthesis.html&usg=__i_o3gKkCu2XdxBZPFLm6GSWJJmY=&h=327&w=287&sz=4&hl=en&start=9&um=1&tbnid=PtJXGqV1G87WcM:&tbnh=118&tbnw=104&prev=/images?q=chlorophyll&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.steve.gb.com/images/molecules/porphyrins/chlorophyll-a.png&imgrefurl=http://www.steve.gb.com/science/photosynthesis.html&usg=__i_o3gKkCu2XdxBZPFLm6GSWJJmY=&h=327&w=287&sz=4&hl=en&start=9&um=1&tbnid=PtJXGqV1G87WcM:&tbnh=118&tbnw=104&prev=/images?q=chlorophyll&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.usoe.k12.ut.us/curr/Science/sciber00/8th/energy/images/chloro.jpg&imgrefurl=http://www.usoe.k12.ut.us/curr/Science/sciber00/8th/energy/sciber/chloroph.htm&usg=__O-m7ncNW-0WHVaIFEUaAhQOfreE=&h=279&w=288&sz=28&hl=en&start=3&um=1&tbnid=GpHS0pWU00GPlM:&tbnh=111&tbnw=115&prev=/images?q=chlorophyll&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.hsv.k12.al.us/schools/middle/wtms/student/cell/chlorophyll.jpg&imgrefurl=http://www.hsv.k12.al.us/schools/middle/wtms/student/cell/cell_energy.html&usg=__zZo7OnlqCgveBcdvmXxn7bLsDLQ=&h=300&w=300&sz=17&hl=en&start=2&um=1&tbnid=NWCuMA-l-ytu3M:&tbnh=116&tbnw=116&prev=/images?q=chlorophyll&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.travelsandjourneys.com/images/fall-leaves.jpg&imgrefurl=http://greenopolis.com/myopolis/blogs/hlund05/climate-change-ruining-fall-foliage&usg=__ZAUmi7jzgWIOKmhSJzPCQrXmQgM=&h=426&w=640&sz=55&hl=en&start=5&um=1&tbnid=6Of5K6pIDEq2zM:&tbnh=91&tbnw=137&prev=/images?q=leaves&um=1&hl=en&sa=N


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You see the red, orange, and yellow colors

because the green color of the chlorophyll

no longer hides them.

http://images.google.com/imgres?imgurl=http://www.freepicturesfreepictures.com/free-pictures-fall-autumn-colors-leaves-Mexicanwave.jpg&imgrefurl=http://www.freepicturesfreepictures.com/free_pictures_autumn_leaves_fall_colors.htm&usg=__tY70fgqfzz5WJ_8EFbjQbyiQtsI=&h=768&w=1025&sz=263&hl=en&start=2&um=1&tbnid=9NWBYrgaVIqYJM:&tbnh=112&tbnw=150&prev=/images?q=fall+leaves&um=1&hl=enhttp://images.google.com/imgres?imgurl=http://www.betterbudgeting.com/images/ph03642i.jpg&imgrefurl=http://www.betterbudgeting.com/frugalcrafts/preservingleaves.htm&usg=__h9RtFCNFjsYCoBdliRk2CGVlt78=&h=434&w=600&sz=166&hl=en&start=9&um=1&tbnid=1bhDug91dJjs7M:&tbnh=98&tbnw=135&prev=/images?q=fall+leaves&um=1&hl=en


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Leaves changing colors in the fall are an

example of a chemical reaction.

def: the process by which one or more

substances undergo change to produce

one or more different substances.

Recall, the new substances have different

chemical and physical properties.



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Examples of chemical reactions

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Clues to help you recognize a chemical

reaction

1. Gas formation

2. Solid formation3. Color change

4. Energy change



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Carbon dioxide (CO2) is great heres

why!

Dissolved under pressure = carbonated

beverages

CO2 gas is not combustible & is denserthan air= fire extinguishers

dry ice/solid CO2 = cooling effect, better

than ice

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New substances form because chemical

bonds in the starting substance break.

Then atoms rearrange.

Finally, a new bond forms in the newsubstance.



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Remember a chemical symbol is

shorthand for writing an element.

Oxygen = O

Nitrogen = N

Carbon = C



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Chemical formula

def: a shorthand way of writing a compound

or a diatomic element using chemical

symbols and numbers.

Example: H2O, CO2, C6H12O6



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the number represents how many of each

kind of atom is present in a molecule.

H2O tells you that a water molecule is

composed of 2 hydrogen atoms and 1

oxygen atom.

The 2 is a subscript. Subscripts are

written below and to the right of a chemical



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When no subscript is present after a

symbol it indicates only one atom of the

element.

Example: H2O, N2O



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Lets try a compound a little more

difficult how many atoms of each element

are in this formula?

Na2SO4

Ca(NO3)2



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Writing Formulas for Covalent Compounds

The prefix used in the name represents the

number of atoms in that compound.



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Prefixes to memorize

mono- 1di- 2

tri- 3

tetra- 4

penta- 5

hexa- 6



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How to write a chemical formula from the

name of a covalent compound

The lack of a prefix indicates only 1 atom.

The prefix di indicates 2 atoms etc.

Example: carbon dioxide = CO2dinitrogen monoxide = N2O



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Writing Formulas for Ionic Compounds

If the name contains a metal and

nonmetal the compound is probably ionic.



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Heres how

1. Make sure the overall charge is zero.2. The formula may need subscripts to

cause the charges of the ions to cancel

out. (Remember the charge of manyions can be determined by looking at the

periodic table.)

Example: Mg is in column 2, it has a +2



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Practice

Sodium Chloride NaCl

sodium ion has 1+ charge

chloride ion has a 1- charge

** one sodium ion & one chloride ion have

an overall charge of zero*** (+1) + (-1) = 0



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Practice

Magnesium Chloride - MgCl2magnesium ion has a 2+ charge

chloride ion has a 1- charge

** one magnesium ion & two chlorideions have an overall charge of zero** (+2) +

2(-1) = 0



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How do all chemists know what each othermeans?

chemical equation

def: a shorthand description of achemical reaction using chemical

formulas and symbols.

This form is understood around the world andneeds no explanation.

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Chemical reactions involve two sides of

the equation.

Reactants yield Products

Reactants Products

Reactants- starting materials

Products- substances formed from a



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Reactants Products

Example: C + O2 CO2

Charcoal for barbecuing contains C. The C

reacts with O in the air, and the primaryproduct is CO2.

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Make sure you are accurate in writing thesubstances of a reaction carefully.

Remember to use the proper chemicalsymbol.

MISTAKES CO2 vs. CO vs. Co

Dont forget to write a subscript of 2 for thediatomic elements.

( 7 total: H2, N2, O2, F2, Cl2, Br2, I2 )

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What about hydrogen gas, H2, as fuel for

vehicles.

Mode: as H burns, water is the only

product.

Benefits: cheaper, less air pollution.

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An equation MUST BE BALANCED!!!

Every atom in the reactants becomes part of

the products.

Atoms are never lost or gained in a chemical

equation.

The number of atoms of each element on the

reactants side must equal the number of atoms



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Remember

You CAN NOT CHANGE SUBSCRIPTS

You can change coefficients



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French chemist, Antoine Lavoisier (1700s)performed experiments and determined that the

total mass of reactants equaled the total mass

of the products.

Law of conservation of mass

def: mass is neither created nor destroyed

in ordinary chemical and physical changes



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Therefore a chemical equation musthave the same number and kind of atom on

both sides.

Example: 2H2 + O2 2H2O



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Review Questions

Page 357 #1 - 5



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Types of Chemical Reactions

1. Synthesis Reactions2. Decomposition Reactions

3. Single-Replacement Reactions

4. Double-Replacement Reactions



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What happens when somethingdecomposes?

What happens when something

synthesizes?

http://images.google.com/imgres?imgurl=http://blog.mlive.com/watershedwatch/2008/02/large_landfill.jpg&imgrefurl=http://blog.mlive.com/watershedwatch/2008/02/&usg=__V-bN9U1RoghVLmBO7QiNnJpmVJc=&h=284&w=452&sz=44&hl=en&start=8&um=1&tbnid=sUaeso9Ecv7TTM:&tbnh=80&tbnw=127&prev=/images?q=garbage+decomposing&um=1&hl=en


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Synthesis Reaction

def: a reaction in which two or moresubstances combine to form a single

compound.

Example: A + B AB

2Na + Cl2 2NaCl



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Decomposition Reaction

def: a reaction in which a singlecompound breaks down to form two or more

simpler substances.

Example: AB A + B

H2CO3 H2O + CO2



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Single-Replacement Reaction

def: a reaction in which an element takesthe place of another element that is part of acompound.

Note: the products are a new compound and adifferent element.

Example: A + BC AC + B



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Double Replacement Reaction

def: a reaction in which ions in twocompounds switch places. One of the

products of this reaction is often a gas or a

precipitate.

Example: AB + CD AD + CB

NaCl + AgF NaF + AgCl



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Review Questions

Page 360 # 1 & 2



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Every chemical reaction involves chemical

ENERGY!

During a reaction, the chemical bonds that

hold the reactants together are broken as

they absorb energy.

When new bonds form in the products, the

energy is released.

Energy & Rates of Chemical

Reactions


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If the reactants contain more chemicalenergy than the products energy will be

released during the reaction this is called

exothermic.

def: a chemical reaction in which

energy is released or removed.


Reactions


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This energy can be released in severaldifferent forms such as light, electrical, orthermal.

2Na + Cl2 2NaCl + energy

Example: Campfire (light & thermal energy

are released)


Reactions
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If the reactants contain less chemicalenergy than the products energy is

absorbed during the reaction this is called

endothermic.

def: a chemical reaction in which

energy is absorbed.


Reactions


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Written as2H2O + energy 2H2 + O2

Example: Photosynthesis plants use energyfrom the sun

6CO2 + 6H2O + energy C6H12O6 +

6O2


Reactions
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Just like mass is never created ordestroyed in chemical reactions the same

is true for energy.

Law of conservation of energy

def: energy can neither be created or

destroyed


Reactions


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All substances need energy to start a

reaction.

Example: a match contains all the reactants

needed to burn, but it will not burn until

energy is added. This energy comes from

the friction of striking it.

Activation energy

def: the minimum amount of energy


Reactions
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Example: an electric spark in a carsengine provides activation energy to begin

the burning of gasoline.


Reactions
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Look at 2 diagrams on page 363


Reactions


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Factors affecting rates of reactions-

measure of how rapidly the reaction takes

place.

1. Temperature

2.Concentration3. Surface area

4. Catalyst or Inhibitor


Reactions


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Temperature- increasing the temperaturemakes particles move faster increase rate

of reaction.

temperature = rate of reaction


Reactions


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Concentration- increase the number ofreactant particles increase rate of

reaction*.

concentration = rate of

reaction


Reactions


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Surface area- increase the amount ofexposed surface of a solid reactant

increases rate of reaction.

surface area = rate of

reaction


Reactions


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Some reactions occur too slow for us sowe need to use a catalyst.

Catalyst- a substance that speeds up areaction without being permanently

changed.


Reactions


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Most reactions in your body are sped upusing catalysts called enzymes.

Everything your body does involves anenzyme.


Reactions
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Amylase- an enzyme in your salivanecessary for digestion of food its starts

working as soon as the food enters your

mouth.


Reactions

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Inhibitor- substance that slows down orstops a chemical reaction.

Example: preservatives added to foodsare inhibitors that slow down the rates of

bacteria or fungus which spoils food.


Reactions

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Review Questions

Page 365 # 1, 2, & 4


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E & R t f Ch i l


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Chapter Review Quesitons

Page 368 # 1-13, 15, 17-19, 21


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