Here's+Dr.+Reich's+Study+Guide+for+2009.

Chapter 1.

Vocab: Hypothesis, experiments, scientific law, law of conservation o fmass, theory, atomic theory

Scientist: Dalton

Chapter 2:

Scientific Notation: Leading number is 1 or more but smaller than 10. The rest of the digits are expressed as 10^x. If you move the decimal point to the left the exponent will increase. Sig Figs: 1. Numbers 0-9 are significant 2. 0s inbetween numbers are significant 3. 0s before numbers are insignificant 4. 0s after numbers, but without a decimal point are insignificant 5. 0s after numbers, and with a decimal point are significant 6. 0s after a decimal point but before a number are insignificant 7. 0s after a decimal point and after a number are significant

Sig Figs: Multiplication and Division, The term with the least number of sig figs in it determines how many the final answer will have and they will be the same number. Addition and Subtraction: Look for the biggest number with the least amount of known digits. Wherever the number is unkown too all other numbers must be rounded to it. see page 19 for more info.

Prefixes: tera, giga, mega, kilo, deci, centi, milli, micro, nano, femto

Units: Seconds, Liter, Meters, Grams

Density= mass / volume

Volume = mass / Density

Mass = Density * Volume

Chapter 3: Matter

Matter= anything that has volume and mass

Elements: The different types of matter atoms: smallest unit of a type of matter molecule: 2 or more atoms put together

State of Matter: Solid- close together, imobile Liquid- spread apart, fluid, will spread out Gas- spread very far apart, fast moving, fills all available space

Solids can be crystalline where there are patterns that the atoms take, or amorphous where they are much more randomly assorted. Crystalline solids tend to be hard, amorphous tend to be malleable or goopy.

Classifying Matter: Pure Substance: only 1 unique element or molecule present Mixture: two or more elements or molecules present Compound: 2 or more elements combined into a molecule in definate proportions

Properties:

Physical Properties: A property where the molecule doesn't change formula or composition. example question What does it look like? Chemical Properties: How the molecule reacts and changes formula when interacting with certain other molecules. Example question: What does it do when?

Physical changes results in a different form o f the same substance, while a chemical change results in a completely new substance.

Reactions:

Reactants --> Products

Separating Mixtures:

Decanting Distillation Filtration

Energy Types: Kinetic Energy Potential Energy Electrical Energy Chemical Energy

Energy Changes: Exothermic: A reaction releases energy... it gets hot Endothermic: A reaction requires energy... it cools down

Temperature: Farenheit Celsius Kelvin

Kelvin = Celcius + 273

Heat Capacity- The quantity of termal energy required to change the temperature of a given amount of the substance by 1C. If the given amount is listed in grams then the term is specific heat capacity.

Heat= Mass x Specific heat Cacity x change in temperature

Chapter 4: Atomic Theory- Dalton Thompson Rutherford

Plum PUdding model Rutherford Gold Experiment

Protons: Mass 1, Charge +1 Nuetrons: Mass 1, Charge 0

Electrons: Mass 0, charge -1

Protons and Nuetrons are in the nucleus, electrons are on the outside Masses are listed in amu, which actually weigh 1.67e-27 kg

Different Elements: atomic number (also called Z), is the number of protons, and chemists use this to tell the difference between elements. Chemical Symbol: the 1 or 2 letter abriviation for an element.

Periodic Table: Periodic Laws repeat Groups: up and down Periods: left to right

Metals: Elements to the left, conduct electricty, can bend, shiny Non-Metals: Elements in the upper right, don't conduct, brittle, dull

metalloids: some properties of both semiconductors: capable of some conductivity

Main group elements: Group 1,2, 13, 14, 15, 16, 17, 18 Transition Metals- Gorup group 3-12

Noble gasses group 18 Halogen group 17 Alkaline Earth group 2 Alkaline group 1

Ions: Charged particles are called ions. If an element or molecules gains an electron it gets a negative charge If an element or molecule loses an electron it gets a positive charge

Basically Ions are the same compound in all aspects except for how many electrons are present

Isotope: Similar atoms that have different number of neutrons are called isotopes

Different isotopes occur in different amounts. The specific amout is referred to as the percent natural abundance.

The sum of protons and neutrons is called the mass number.

Atomic Mass is an average number. You have to average the masses from each different isotope of an element.

(Natural abundance x mass number 1) + (natural abundance x mass number 2) + (etc) = average mass

Chapter 5:

Law of constant composition: All samples of a given compound have the same proportions of their consituent elements

Chemical Formula: Lists all the different elements and the number of atoms of each type of elements

H2O

THere are two H atoms and 1 O atom

Molecular Elements: H2, I2, N2, Cl2, Br2, O2, F2

Ionic Compounds: Metals and Non-Metals come together Covalent or Molecular Compounds: 2 or more Non Metals Come together

Figuring out Ionic Compounds Formulas: Symbols Charges Switcheroo Reduce

Figuring out molecular formulas: read the name figure out what the prefixes mean write the formula like the name suggests

Naming Systems: Ionic Metals in group 1,2, and 13 just get called their names Metals in all other groups get called their names with their charges in parenthensis afterward. Iron +3 = Fe(III). Remember charge in parenthensis is written in Roman Numerals.

The anion gets a slightly different name. Polyatomic names won't change. Sulfates and Sulfites will be called Sulfates and Sulfites. However, if a non-metal combines with a metal like AlCl3 or Fe(II)O, then the non-metal that is not part of a polyatomic group will have it's name changed. The ending will go from -ine to -ide.

You should know the polyatomic ions listed on page 138. Make flash cards. Don't expect any help from us.

Naming Systems: Covalent aka Molecular

use number prefixes. Mono=1, Di=2 etc (page 140)

The order for naming covalent compounds is the following:

1. prefix 2. element 3. prefix 4. element 5. change the ending of the non-metal from -ine to -ide.

Naming Systems: Acids Acids make H+ ions when they are put in water. They are combinations of H atoms and polyatomic anions or monoatomic anions. There are oxy and binary acids. For every negative charge the negative part of an acid has there is 1 H atom to counterbalance the charge.

Oxy Acids: made with a non-metal surrounded by oxygens.

Binary Acid Naming: 1. Add the word Hydro 2. Write the root word of the element 3. change the ending of the word to -ic 4. Add the word acid

Oxyacid Naming: 1. Read the name of the anion out loud. 2. If it ends in -ate; the name of the acid will be the root word of the anion with the ending changed to -ic and then add the word acid 3. If it ends in -ite; the name of the acid will be the root word of the anion with the ending changed to -ous and then add the word acid

Molecular Mass aka Formula Mass: To calculate the molecular mass of a compound you must sum the masses of all the atoms of every element type. (pg 146)

Chapter 6: The mole map should help here.

Grams to Moles: To go from grams to moles multiply your mass of grams by 1 mol of the compound diveded by the molecular mass in grams. Moles to Grams: To go from moles to grams multiply you number of moles of a compound by the molecular mass in grams divided by 1 mol of the compound.

To get into atoms if the molecule is just 1 atom (like Ne or Fe metal): get the value into mols and then multiply by 6.02e23 atoms divided by 1 mol.

To get a molecule into number of atoms you must get the value into moles. Then mulitply that number of moles by 6.02e23 molecules divided by 1 mol. Then multiply by the number of atoms in the molecule divided by 1 molecule.

Mass Percent: Take the mass of one element type (the sum of the masses of all the atoms of one element) divide by the mass of the compound and then multiply by 100.

Percent Composition: Do a mass percent for each and every element in the molecule.

Any time you do a percent it's basically little number divided by big number times 100.

You can turn a percent composition into a chemical formula. It's on the test. It's too hard to explain here. Read in the book the end of chapter 6.7-the end of chapter 6.8. It does an ok job of explaining this.

Chapter 7: Chemical Reactions

Evidence: gas formation, heat and light, smell changes, color changes

Chemical equations: Reactants --> Products

Make sure you can balance a chemical rxn.

There are 5 types of chemical reactions:

Composition/synthesis: 2 things come together to make 1 Decomposition: 1 things falls apart to make 2 combustion: fuel + O2 --> H2O and Water Single replacement: element A + Compound --> Element B + New Compound Double replacement: metals switch Places AB + CD --> AD + BD be sure to balance correctly. FIgure out each formula first, and then figure out the

For Double displacement reactions the two compound going in are typically solid. One of the products formed is generally insoluble. You can determine which of the products is insoluble if you know the following:

1. Compounds that have Li, Na, K, NH4, NO3, or C2H3O2 (acetate) are always soluble 2. Compounds with Cl, Br, and I are soluble unless with Ag, Hg2, or Pb+2 3. SO4 compouns are soluble, except with Sr, Ba, Pb, or Ca 4. OH and S compounds are insoluble in general, but with a bunch of exceptions 5. CO3, and PO4 compounds are typically insoluble

Total Ionic Equations:

Ionic compounds in water will break up into ions. Molecular compounds will not.

Ios that appear on both sides of the chemical equation are called spectator ions.

To make the net ionic equation cancel out the spectator ions, and copy down whatever is left over.

Read 218-220 in your book for gas evolution reactions and Oxidation Reduction Reactions.

Chapter 8:

Use your mole map here again, study it, memorize it, be ready to use it on the test.

Mole to Mole conversions: Look at the balanced chemical reaction. Use the coefficients from the balanenced chemical reaction to figure out the molar ratio. You can then use this to help convert from Grams of A to moles of A to moles of B to grams of B.

Limiting reagent: Figure out which element would run out first. The easy way is to run the reaction twice using the two different reagents in question. Whichever makes less product is the limiting reagent. The harder way is to compare the two to each other and see which you have more of.

Theoretical yield. The most you could have possibly made of a certain product. Actual yield: The amount of product you actually made Percent yeild: Actual yield divided by theoretical yield times 100

Read Chapter 8.7

Chapter 9 Bohr Model Full Quantum Model

Electromagnetic Waves (light) run over a broad spectrum When hydrogen emits light it only comes in a few colors, not a billion. That was a problem and no one could explain it. Until the quantum model. Electrons can't be everywhere. Only in certain energy shells (Bohr's model). That explained hydrogen. So, atoms are quantized.

Bohr's Model: 1 quantum number, energy shell Full Quantum Model: 4 Quantum Numbers, energy shell, shape, orientation, spin

New Orbitals, s orbitals, p orbitals, d orbitals, f orbitals

electron configuration: List the orbitals in order of how they show up and the numbers in each orbital, 1s22s22p6 etc

s block, p block, d block, f block

Periodic trends:

Shielding stays the same across the periodic table Shielding increases going down the periodic table

Nuclear charge increases from left to right

Atomic size decreases left to right Atomic size increases top to bottom

Ionization energy increases from left to right Ionization energy decreases from top to bottom

metallic character increases from top to bottom metallic character decreases from left to right

Chapter 10:

Bonding Theory: Covalent Bonding and ionic bonding

Covalent Bonding happens between non-metals and electrons are shared Ionic Bonding is between metals and non-metals and electrons go from the metal to the non-metal and they are not shared

Lewis Dot Thoery: Electron Dots represent valence electrons. 1 dot =1 electron. Group 1a= 1 ve, group 2a =2ve etc...

Make sure you know how to place electrons and draw their bonds

Octet Rule: Metals want 0 valence electrons, non-metals want 8. He wants 2. H wants 0 or 2.

Exceptions to the octet rule. Elements like B, S, P, and N, often break the octet rule and are still stable. Just be able to recognize why they are exceptions.

Resonance. If two structure models of molecules look the same except they are flipped around they are called resonance structures. The model will look like any and all of the resonance strucutres

VSEPR: bent, linear, trigonal planer, trigonal pyramidal, tetrahedral. Know which is which and why.

Electronegativity and polarity. Understand that electrons aren't shared equally. They are shared based on electronegativity. The more electronegative element will pull electrons toward it even from adjacent atoms.

Polarity. If electrons are pulled in a such a way that it's asymetrical in the molecule then the molecule will be polar.

Element Naming: