• Save
Chemical Reactions
Upcoming SlideShare
Loading in...5
×

Like this? Share it with your network

Share
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
  • nice concept
    Are you sure you want to
    Your message goes here
No Downloads

Views

Total Views
6,912
On Slideshare
3,061
From Embeds
3,851
Number of Embeds
12

Actions

Shares
Downloads
0
Comments
1
Likes
15

Embeds 3,851

http://learning.ssis.edu.vn 3,282
http://chemistry10th.blogspot.com 330
http://omsvikings.pbworks.com 111
http://www.chemistry10th.blogspot.com 59
http://chemistry10th.blogspot.mx 19
http://cppchem.pbworks.com 14
http://blackboard.cpsb.org 13
http://longenbergerchemistry.wikispaces.com 7
http://www.slideshare.net 6
https://cv.scoca-k12.org 5
http://www.chemistry10th.blogspot.mx 3
http://chemistry10th.blogsopt.com 2

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
    No notes for slide

Transcript

  • 1. Chemical Reactions
  • 2. Chemical reaction
    • a chemical change
    • bonds of reactants are broken and bonds of product are formed
    • reactants products
    • (yield or make)
  • 3.
    • when some chemicals come into contact with each other, they break apart, join, or rearrange to form new chemicals ( always to become more stable)
  • 4. Evidence of Chemical Rxn
    • change in color (unexpected)
    • change in temperature
    • change in smell
    • change in taste
    • formation of a precipitate (appears cloudy)
    • production of a gas (bubbles)
    • production of heat, light, sound
  • 5. Chemical equations
    • shorthand representations of chemical reactions
    • H 2 + O 2 H 2 O
    • ( skeleton equation )
  • 6. Parts of a chemical equation . . .
    • Reactants the elements or compounds that enter into a reaction
    • Products are the elements or compounds that are formed as a result of a chemical reaction
    • Arrow means yields, produces or forms
    • reactants products
    • yield
  • 7. Formula Equation
    • 2 H 2 (g) + O 2 (g) 2 H 2 O (l)
    • includes states of matter
      • (s) – solid
      • (l) – liquid
      • (g) – gas
      • (aq) – aqueous
    • chemical equation must be balanced
  • 8. Word equation
    • hydrogen gas and oxygen gas form liquid water
    • 2 H 2 (g) + O 2 (g) 2 H 2 O (l)
  • 9. Types of Chemical Reactions
    • Synthesis
    • Decomposition
    • Double Replacement
    • Single Replacement
    • Combustion
  • 10. 1. Synthesis
    • A + B AB
    • two or more substances react to form a single product
    • example :
      • 2 H 2 (g) + O 2 (g) 2 H 2 O (l)
  • 11. 2. Decomposition
    • AB A + B
    • a single compound breaks down into two or more substance
    • example :
      • 2 H 2 O (l) 2 H 2 (g) + O 2 (g)
  • 12. 3. Single Replacement
    • A + BC AC + B
    • the atoms of one element replace the atoms of another element in a compound
    • example :
    • Zn (s) + Cu(NO 3 ) 2 (aq) Zn(NO 3 ) 2 (aq) + Cu (s)
  • 13. 4. Double Replacement
    • AB + CD AD + CB
    • metal cations exchange position between two compounds (dissolved in water)
    • example :
    • AgNO 3 (aq) + NaCl (aq) AgCl (aq) + NaNO 3 (aq)
  • 14. 5. Combustion
    • reactant(s) + O 2 product(s)
    • oxygen combines with a substance and releases energy (heat & light)
    • example :
    • CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (l)
  • 15. What is the purpose of balancing chemical equations?
    • The Law of Conservation of Mass states that matter is neither created nor destroyed during a chemical reaction. Therefore, when writing a chemical equation, the reactants must be equal to the products. So you must add any necessary coefficients to show that matter is conserved.
  • 16. METAL ACTIVITY SERIES
    • During a Single Replacement reaction, a metal will not always replace another metal. This is because metals differ in their reactivities.
    MOST ACTIVE Fr Li Rb K Ca Na Mg Zn Fe Ni Sn Pb Cu Ag Pt Au LEAST ACTIVE
  • 17.
    • For example : Francium (Fr) is the most active metal on the table. It will replace (or kick out) any other metal.
      • NOTE : it’s the highest on the Activity Series list.
    • So in the reaction below, the Fr metal with replace the Fe in the iron (II) chloride, resulting in pure iron metal as a product.
    • 2 Fr + FeCl 2 2 FrCl + Fe
  • 18. A Metal Activity Series helps you determine if a reaction will occur.
    • Au + FeCl 2 no reaction
    • * gold is one of the least active metals, so it will not be able to replace (kick out) the iron metal, and the reaction will not take place.
  • 19.
    • 2 Al + 3 FeCl 2 2 AlCl 3 + 3 Fe
    • * Al is more reactive than iron, so it will replace (kick out) the iron metal, and the reaction will take place.
  • 20. Write out and balance the following
    • Sulfur solid reacts with iron solid to form solid iron(III) sulfide.
  • 21. Magnesium metal reacts with hydrochloric acid to form magnesium chloride solution and hydrogen gas.
  • 22. Oxygen gas reacts with solid copper metal to form copper(II) oxide solid.
  • 23. Oxygen gas reacts with hydrogen gas to form liquid water.
  • 24. Hydrogen gas and aluminum chloride solution are produced when solid aluminum is reacted with hydrochloric acid.
  • 25. Answer Key
    • 3S (s) + 2Fe(s)------> Fe 2 S 3 (s)
    • Mg(s) + 2HCl(aq)------> MgCl 2 (aq) + H 2 (g)
    • O 2 (g) + 2Cu(s)------> 2CuO(s)
    • 2H 2 (g) + O 2 (g)------> 2H 2 O(l)
    • 2Al(s) + 6HCl(aq)------> 3H 2 (g) + 2AlCl 3 (aq)
  • 26. Try the following Write out the formula and balance.
    • Dinitrogen pentoxide gas in the presence of a platinum catalyst and high enough temperature forms nitrogen gas and oxygen gas.
    • Sulfur solid reacts with iron solid to form solid iron(III) sulfide.
    • Hydrogen gas and iron(III) oxide powder react to form liquid water and solid iron powder.
    • Magnesium metal reacts with hydrochloric acid to form magnesium chloride solution and hydrogen gas.
    • Magnesium sulfide solid and hydrochloric acid react to form hydrogen sulfide gas and magnesium chloride solution.
  • 27. Key
    • 2N 2 O 5 (g)------> 2N 2 (g) + 5O 2 (g)
    • 3S (s) + 2Fe(s)------> Fe 2 S 3 (s)
    • 3H 2 (g) + Fe 2 O 3 (s)------> 3H 2 O(l) +2Fe(s)
    • Mg(s) + 2HCl(aq)------> MgCl 2 (aq) + H 2 (g)
    • MgS(s) + 2HCl(aq)------> MgCl 2 (aq)+ H 2 S(g)
  • 28. Finding Formula Mass
    • H 3 PO 4
    • AlCl 3
    • K 2 C 4 H 4 O 6
    • N 2 O 5
    • K 3 SO 4
    • Nd 2 O 3