How To Be Successful in Second Semester

Chemistry

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?

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?

Video Games

• So how does someone get good at video games?

• What happens if you can’t get past a level?

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

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.

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.

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”

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.

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

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

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

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

• Remember, the number of atoms of each element must be ___________ on both sides.

Example: __ H2 + __O2 __H2O

Balancing Chemical Equations

equal

2 1 2

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

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

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

+

+

Activity Series

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

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)

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

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)

General Types of Reactions (Continued)

• More examples of nuclear fission reactions:

Nuclear Medicine /Medical Imaging

Nuclear Power Plants

General Types of Reactions (Continued)

• Examples of nuclear Fusion reactions:

Hydrogen on the sun becomes Helium

Fusion