Transcript Chemical Reactions

• Name:
•
•
•
•
Na2O
BaS
CO2
NF3
Sodium Oxide
_____________________
Barium Sulfide
_____________________
_____________________
Carbon Dioxide
_____________________
Nitrogen Triflouride
Take Out Homework
1. Which ones would conduct
electricity?
Ionic Compounds- Na2O, BaS
Na2O
2. Which ones are not very hard, and
have an easier bond to break?
Covalent Compounds CO2, NF3
Those with Phys Science Book with Satellite Dish
1. Go to page 602-604 - Answer: Why do atoms combine?
2. Explain the 2 types of covalent bonds (polar and non-polar)
3. Go to page 616 – what are the charges (oxidation numbers) for
transition metals Copper (I), Iron (III) and Lead (II)?
4. Go to p. 626 Do 1-18. Write out the word and the phrase for 1-10
Just answer 11-18, no need to write it out
Those with Phys Science Book with Roller Coaster
1. Go to page 298-300 - Answer: Why do atoms combine?
2. Explain the 2 types of covalent bonds (polar and non-polar)
3. Go to page 315 – what are the charges (oxidation numbers) for
transition metals Copper (I), Iron (III) and Lead (II)?
4. Go to p. 321 Do 1-10. Write out the word and the phrase for 1-10
Go to page 322 answer 1-10 (answer only)
Things to know for the quiz tomorrow…
Know differences between Ionic and Covalent bonds
Melting points, electricity conduction, which elements
know that metallic bonds are bonds between metals only
Know what covalent bonds look like when sharing electrons
with dot diagrams
Be able to identify correct formula for an ionic bond, you need
to memorize the charges in groups 1, 2, 13, 15, 16, 17
Be able to identify correct formula and names of covalent
bonds
Tips on Ionic and Covalent Compounds– stuff in
your notes…
Ionic or Covalent? If you only have formula of a compound,
see if it contains a metal. Ionic if it has a metal, Covalent if
no metals
Naming compounds from formulas:
Rule for both: 2nd part ends with “ide” unless it is a
polyatomic ion (it keeps its given name)
Covalent, you need prefixes: mono, di, tri, tetra…
IONIC Formula writing, total + charges must equal
total – charges **Use charge of one ion to decide the
subscript of the other one
Be+2
P-3
Be3P2
Chemical Reactions
• Indicators:
–Fizzing (gas produced)
–Color change
–Gets cloudy/precipitant (solid produced)
–Heat released or absorbed
–Light emitted
–Odor changes
Chemical Reactions
http://ed.ted.com/lessons/if-molecules-were-people-george-zaidan-and-charles-morton
• Reactants  Products
• H2O2  H2O + O2
–What are the reactants? What are the
products?
Chemical Reactions
There are 4 kinds of Chemical
Reactions that occur:
Synthesis
Decomposition
Single
Replacement
Double
Replacement
Types of Chemical Reactions
•Synthesis
–Two or more reactants are
combined to form one
product.
+
Types of Chemical Reactions
•Decomposition
–One reactant breaks down
into two or more products.
+
Types of Chemical Reactions
• Single Replacement
–An element and a compound
combine.
–One element from the reactants
replaces another in the products.
+
+
Types of Chemical Reactions
•Double replacement
–Two compounds combine.
–Two elements in the reactants
switch places in the products.
+
+
Chemical Reactions-Practice
Identifying
• Example #1
• H2 + O2  H2O
Which is it?
• Synthesis
• Decomposition
• Single Replacement
• Double
Replacement
Chemical Reactions
• Example #2
• Li3P  Li + P
Which is it?
• Synthesis
• Decomposition
• Single
Replacement
• Double
Replacement
Chemical Reactions
• Example #3
Which is it?
• Na + MgCl2  Mg + NaCl• Synthesis
• Decomposition
• Single
Replacement
• Double
Replacement
Chemical Reactions
• Example #4
Which is it?
• SiCl4 + O2  SiO + Cl2
• Synthesis
• Decomposition
• Single Replacement
• Double
Replacement
Chemical Reactions
• Example #5
• C5O3  C + O2
Which is it?
• Synthesis
• Decomposition
• Single Replacement
• Double
Replacement
Chemical Reactions
• Example #6
• Rb2O + AlF3  RbF + Al2O3
Which is it?
•
Synthesis
•
Decomposition
•
Single
Replacement
•
Double
Replacement
Chemical Reactions
• Law of conservation of Matter
–Atoms are not created or destroyed
–The number of atoms at the START
of a reaction, there must be the same
number of atoms AFTER the
reaction.
–Equations must be balanced!
Chemical Reactions
• Balancing Chemical Equations STEPS:
–Count the number of atoms for each
element in the reactants and in the
products.
–Compare the numbers to see if each
element is balanced (equal) with itself.
–Use WHOLE NUMBER coefficients to
“fix” unbalanced elements.
• Do not change the subscripts!
Chemical Reactions
• Example #1
• H2 + O2  H2O
Chemical Reactions
• Example #2
• Li3P  Li + P
Chemical Reactions
• Example #3
• Na + MgCl2  Mg + NaCl
Chemical Reactions
• Example #4
• SiCl4 + O2  SiO + Cl2
Chemical Reactions
• Example #5
• C5O3  C + O2
Chemical Reactions
• Example #6
• Rb2O + AlF3  RbF + Al2O3
Chemical Reactions
• Example #7
SnO2 + H2 → Sn + H2O
Chemical Reactions
• Example #8
• Mg(ClO3)2 + Na  NaClO3 + Mg
Chemical Reactions
• Example #9
• Al2(SO4)3 + RbF  AlF3 + Rb2SO4
Chemical Reactions
• Identify and Balance
•
Al + F2  AlF3
Chemical Reactions
• Identify and Balance
•
Ca(MnO4)2 +
FeCl4 
CaCl2 +
Fe(MnO4)4
Chemical Reactions
• Identify and Balance
•
Si3O  Si8 + O2
Chemical Reactions
• Identify and balance
•
Cs2O + N2  Cs3N + O2
Schedule for the week:
Welcome Back!
Monday: Classify types of Chemical Reactions and
Balance Chemical Equations
Tuesday: Acids and Bases – quick lab and practice more
chemical equations
Wednesday: Radioactive Decay – review Acids/Bases
and Chemical Reactions
Thursday: 1st and 3rd period: Recap Radioactive
Decay: quiz on Chemical Reactions and
Acids/Bases REVIEW PACKET –Test Practice
Friday 4th period: Recap Radioactive Decay: quiz
on Chemical Reactions and Acids/Bases
REVIEW PACKET –Test Practice
Warm Up
Chemical Reactions
• Law of conservation of Matter
–Atoms are not created or destroyed
–The number of atoms at the START
of a reaction, there must be the same
number of atoms AFTER the
reaction.
–Equations must be balanced!
Chemical Reactions
• Balancing Chemical Equations STEPS:
–Count the number of atoms for each
element in the reactants and in the
products.
–Compare the numbers to see if each
element is balanced (equal) with itself.
–Use WHOLE NUMBER coefficients to
“fix” unbalanced elements.
• Do not change the subscripts!
Acids and Bases
Draw a Line Like this in the
middle of your paper
c
0
7
NEUTRAL
0
\
7
14
Acids and Bases
Acids and Bases pH scale
c
0
7
NEUTRAL
0
7
\
Bases get
weaker as
you go toward
the #7
Acids get
weaker as
you go toward
the #7
ACIDIC
14
pH 7
Basic (Alkaline)
Acids & Bases-pH Scale
Acids properties
1.
2.
3.
Conduct electricity
(electrolytes)
Produce H+ ions
Sour taste
4. Corrosive
5.
pH values 0-6.9
Acids
Acids
pH range = 0-6.9
• Examples: Citric Acids,
Gastric Acid, Battery Acid,
Sodas, tomatoes, etc.
• Examples of Formulas: HCl,
H2SO4, H3PO4, HNO3, etc
SPOILED
MILK
Bases
properties
1.
Conduct electricity
(electrolytes)
2.
OH- ions
3.
Bitter taste
4. Corrosive
5.
Have a slippery feeling (like
soap)
6.
pH values 7.1-14
Bases
Bases pH range 7.1 to 14
• Examples: Soaps, Cleaning supplies,
Hair Relaxers, etc.
• Examples of Formulas: NaOH,
KOH, Mg(OH)2, Al3(OH), NH3,
NH OH
Acids & Bases
• Neutralization Reactions
Only an Acid can neutralize a base
Only a Base can neutralize an acid
• H+ comes off of the Acid and OHcomes off of the Base (OH and H
make water!)
• Acid + Base  Water + Salt
Ex: HCl + KOH  H2O + KCl
NEUTRALIZATION
REACTION In your stomach
CaCO3
+ 2HCl
Hydrchloric
ACID
==> CaCl2(salt) + H2O + CO2
Acid/Base Neutralization
• HBr + LiOH  _________ + _________
• FrOH + HCl  _________ + _________
• H2S + Mg(OH)2  ________ + _______
• ______ + HF  H20 + KF
• ______ + CsOH  H20 + CsI
Acids and Bases—Identify
Acid, Base, Both or Neutral
1.
2.
3.
4.
5.
6.
7.
8.
pH =2
HF
pH= 7
RbOH
Ca(OH)2
pH= 9
Sour taste
Slippery feel
9. Electrolyte
10.pH = 13
11.pH = 4
12.H2SO4
13.HBr
14.FrOH
15.Corrosive
16.Bitter taste
Acids and Bases-Compare & Contrast