how to be successful in second semester chemistry
TRANSCRIPT
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How To Be Successful in Second Semester
Chemistry
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Skills
• Chances are, you are good at video games, sports, playing an instrument, or some extra curricular activity.
• But how did you get good at that?
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Video Games
• Was anyone born good at video games?• Could anyone who has never played Halo or
Black Ops beat the last level first try?
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Video Games
• So how does someone get good at video games?
• What happens if you can’t get past a level?
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The Video Game of Chemistry
• You are starting the second half of the game of Chemistry.
• You are Level 4 students.• You have 5 more levels to pass
before you beat the game
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The Video Game of Chemistry
• Games teach us that different choices have different outcomes and we control the choices we make.
• Your grade is not something that just “happens”.
• No one is just “good” at chemistry.Some people just have to
practice less.
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The Video Game of Chemistry
• You have unlimited lives. • You have someone who beat the game before
to show you pointers.• The game is designed to be won.
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Chemistry Lies
• “I am just not good at math”• “I can just do better on the next test”• “It doesn’t matter what I do I always get the
same grade on the test”• “There is nothing I can do
to bring up my grade”
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Chemistry Truth
• I strongly believe that everyone here can win this game and have a good grade this semester.
• I will do everything in my power to make sure that happens.
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First Semester Review• Substances can be classified as elements, compounds, or mixtures.
– Elements are substances made of _____type of atom
– Compounds are two or more elements chemically combined by sharing or transferring __________.
– Mixtures are elements and compounds physically mixed together.
• Atoms are the smallest part of an element that has the same properties.
• Atoms are made of _________________________________.
one
electrons
protons, neutrons, and electrons
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First Semester Review• The model of the atom has changed over time as ____________have
given us new knowledge about the atom.
• The periodic table contains all the known elements in the universe.
– The periodic table is arranged by atomic number, the number of ___________.
– The periodic table is also arranged with all of the elements in the same column have similar properties.
– Patterns in the periodic table exist with atomic size and electronegativity. Metals and Nonmetals are separated by the dark zigzag line running through the “p” block.
experiments
protons
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First Semester Review• Elements make bonds to become more stable by sharing or
transferring _______________.
– All elements want to have the same number of valence electrons as the ____________________.
– Energy is given off when bonds are formed and energy is required to break bonds.
• Compounds are named using the ionic naming system or the covalent naming system.
– Ionic compounds are named using the ________________.
• FeCl2 is Iron (II) chloride
– Covalent compounds are named using ______________.
• P2O5 is diphosphorus pentoxide
electrons
noble gases
ion sheet
prefixes
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Ch. 8 Notes -- Chemical Reactions • Chemical equations give information in two major areas:
1. _____________ and ______________ of the reaction.
2. Coefficients of a balanced chemical equation tell us the ______ of the substances involved.
Example of a Balanced Chemical Equation: 2H2 (g) + O2 (g) 2H2O (g)
Reactants are on the ______ side of the arrow, and theproducts are on the __________ side. The arrow means “________”,or “reacts to produce” when read aloud.
• From our example, hydrogen reacts with oxygen in a ___:___ ratio.
• The coefficients represent either the number of _________ or molecules present.
Reactants products
amount
leftyieldsright
2 1
moles
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• Remember, the number of atoms of each element must be ___________ on both sides.
Example: __ H2 + __O2 __H2O
Balancing Chemical Equations
equal
2 1 2
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Six General Types of Reactions1) ________________________:
• A reaction that breaks apart ______ ______________ into simpler substances, (usually two elements or an element and a smaller compound.)
General Form: _____ ___ + ___
Examples: H2O _____ + _____
KCl _____ + _____
Remember that “HONClBrIF” elements are diatomic when alone!!
Decomposition
one compound
AX A X
H2 O2
+
K
Cl2
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2) _______________: (sometimes called “Combination” or “Synthesis”)
• A reaction of _____ __________________, typically a metal and a nonmetal to form ______ ______________.
• It is the opposite of decomposition.
General Form: ___ + ___ _____
Examples: Al + Cl2 _______
K + S ___
General Types of Reactions (Continued)
Composition
two substancesone compound
A X AX
+
AlCl3
K2S
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3) _____________ Replacement:
• A reaction between ____ ______________ and ___ ____________ that produces a different _____________ and ______________.
General Forms: ____ + __ ____ + __
____ + __ ____ + __
• The element that is trying to replace the other must be ________ _______________ than the one it is replacing.
• You must use the Activity Series to see if the reaction will happen.
• Activity Series _________ ___ = more reactive
• Elements from ____ to ____ can displace hydrogen in water to form a metallic hydroxide and H2 gas.
General Types of Reactions (Continued)
Single
one compound one elementcompound element
Y
B
X
A
AX AY
BXAX
morereactive
Higher up
Li Na
+
+
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Activity Series
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Single Replacement Reactions
Examples:
NaCl + F2 _____ + _____
FeCl2 + K _____ + _____
HCl + Zn _____ + _____
HCl + Au _____ + _____
H2O + Na _____ + _____
AgNO3 + Cu _____ + _____
H(OH)
NaF Cl2
KCl Fe
ZnCl2 H2
No Reaction
NaOH H2
CuNO3 Ag
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4) _______________ Replacement: (sometimes called “Ionic”)
• A reaction between _____ ________________ that are dissolved in water that produces _____ ________________ , one of which is ________________.
• Water or a gas may be one of the two compounds being produced.
General Form: ____ + ____ ____ + ____
• You must use the Solubility Chart to see which product is the precipitate.
• Solubility Chart ___ or _____= precipitate
Examples: CaCl2 (aq) + AgNO3 (aq) _________ + ________
NaOH (aq) + HCl (aq) ________ + ________
General Types of Reactions (Continued)
Double
two compounds two compounds
insoluble
AX(aq) BY(aq) AY(aq) BX(s)
I sS
++
Ca(NO3)2 (aq) AgCl(s)
NaCl(aq) H2O (l)
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General Types of Reactions (Continued)5) _________________:
• A reaction between a Carbon/Hydrogen (and sometimes Oxygen) _________________ with _____.
• The products are always the same… ________ + ________
• This reaction is too easy!! Don’t miss it!
General Form: CxHy + O2 ____ + ____
Examples: C2H2 + O2 _______ + _______
C7H6O + O2 _______ + _______
Combustion
compound O2
CO2 H2O
CO2 H2O
CO2 H2O
CO2 H2O
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General Types of Reactions (Continued)6) _________________:
• There are two types of Nuclear reactions, ________________
– Fission reactions involve a heavy nucleus that will split into two or three pieces.
– Fusion reactions involve two light nuclei that combine into a heavier one.
– New elements are formed!
• You will not be asked to predict products!• Examples of nuclear fission reactions:
Nuclear
Fission and Fusion
Nuclear Weapons (atom bomb)
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General Types of Reactions (Continued)
• More examples of nuclear fission reactions:
Nuclear Medicine /Medical Imaging
Nuclear Power Plants
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General Types of Reactions (Continued)
• Examples of nuclear Fusion reactions:
Hydrogen on the sun becomes Helium
Fusion