Standards Project
Charlotte Koberg
Table of Contents
Structure of Atoms
a. Atomic Structure
b. Atomic Nucleus
c. Isotopes
Structure and Properties of Matter
a. Valence Electronsb. Chemical Bonds
- Ionic
- Covalent
- Hydrocarbon Compounds
c. Periodic Table/Trends
d. Physical/Chemical Properties of Chemical Compounds
e. States of Matter
f. Relationship between Pressure and Volume of gases
Chemical Reaction
a. Conservation of Matter
b. Common Reactions/Types of Reactions
c. Acids and Bases
Problem Solving
a. Metric System Conversions
b. Stoichiometry
Structure of Atoms
Nucleus
Isotopes
Structure and Properties of Matter
Valence Electrons
Examples on Finding the Number of Valence Electrons
Chemical Bonds
- Strongest type of bonding, crystal lattice structure, occurs between metals and nonmetals or polyatomic ions, they are formed from the transfer of electrons to attain a full outer shell, most polar bond
- Properties: high boiling/melting points, they are soluble in water and high conductors in solutions, no odor
- Determination: if the first element given is to the left of the stair step, it is ionic
Covalent
- It is determined by polarity, which describes the distributions of electrons in a bond
- Nonpolar Covalent: the least polar bond, has even sharing of electrons
- Polar Covalent: middle polar bond, has uneven sharing of electrons
- Properties: low conductivity, low boiling/melting points, odor
- Determination: if the first element given is to the right of the stair step, it is covalent
Hydrocarbon Compounds
Only hydrogen and carbon elements are used
- Alkanes: single bond, saturated, maximum number of hydrogens, carbons 1-4 used
- Alkenes: 1 double bond, unsaturated, carbons 2-5 used
- Alkynes: 1 triple bond, unsaturated, carbons 2-5 used
Electronegativity
Stairstep Rule
Covalent- right of the stair step
Exception- Hydrogen, because it's a nonmetal
Hydrocarbons
Alkanes
Takes up the most space
Alkenes
Saves space from the double bond
Alkynes
Saves space from the triple bond
Periodic Table & Trends
- Periodic Law: repetition of physical and chemical properties when the elements are arranged by atomic number
- A group in the periodic table are the vertical columns, going down, groups behave the same way with their similar properties, the numbers above the group tells you how many valence electrons those elements have
- A period is the horizontal columns, going left to right, they have the same atomic orbitals (how many shells the element has for its electrons)
- Atomic Radius Trend (the distance from the nucleus to the outer shell of electrons): decreases from left to right when moving across the period; when moving down a group the atomic radius increases
- Electronegativity Trend: from left to right in a period, electronegativity increases; when moving down a group, the electronegativity decreases
- Ionization Trend: from left to right in a period; the ionization energy increases; when moving down a group, the ionization energy decreases
Organization
The periodic table is made up of;
Metals: shiny, solid, good conductors and react with acid
Non-metals: gases, brittle if solid, dull and poor conductors (exceptions: Hydrogen and Aluminum)
Metalloids: share properties of metals and non-metals, share a side with stair step
Families
Alkali Metals (1A, except Hydrogen): very reactive with metals, soft metals, not found naturally, low densities
Alkali Earth Metals (2A): reactive with metals, found in earth's crust
Halogens (7A): highly reactive, diatomic (gives the element a subscript of 2), gases
Noble Gases (8A): nonreactive, found in small quantities in the atmosphere, monatomic because of their full valence shells
Physical/Chemical Properties of Chemical Compounds
Physical Change: no new substance is created
examples: ice melting, cutting an apple, mixing a salad
Physical Properties: can be observed or measured without changing the chemical compositionexamples: density, mass, color and volume
Chemical Change: new substance is formed
- Indicators: color change, bubbles, odor, solid forming, temperature change
examples: frying an egg, metal rusitng, burning paper
Chemical Properties: observed when the substance interacts with one another
examples: flammability, reactivity with acid, reactivity with base, toxicity
Extensive Properties: external, depends on the quantity of the substance
examples: mass, volume
Intensive Properties: internal, does not depend on the quantity of the substance
examples: density, melting point
States of Matter
Liquid: particles in a liquid assumes the shape of the container it occupies, not easily compressible, particles slide past each other, flows easily, fixed volume
Gas: particles in a gas assume the shape and volume of the container it occupies, compressible, flows easily, particles move very fast and bounce off each other
Phase Changes
Relationship between Pressure and Volume of gases
P1V1=P2V2
Chemical Reactions
Conservation of Matter
Common Reactions
Types of Reactions
2. Decomposition- when one substance breaks up into two or more products
3. Single Replacement- when one element replaces another in a compound
4. Double Replacement- when two compounds exchange elements
5. Combustion- when fuel is burned in the presence of oxygen to produce water vapor and carbon dioxide
Double Replacement
Combustion
Acids and Bases
Bases: feel slippery, taste bitter, corrosive, accept the H+ ions
Litmus Paper: when using red litmus paper, and a drop of base is added, it will turn the paper blue; when using blue litmus paper, and a drop of acid is added, it will turn the paper red
pH scale: measure of hydrogen ion concentration in a solution
Conjugate acid: base plus H+
Conjugate base: acid minus H+
Acid base reactions: forms water and salt, neutralization, no excess acid or base
Problem Solving
Metric System Conversions
Stoichiometry
Mole ratio- a relationship connecting or relating the molar amounts of two substances in a balanced equation
Steps for Stoichiomety
1. Balance the equation
2. Identify the starting point
3. Convert to moles
4. Multiply by mole ratio
5 Convert to ending point
Example of Stoichiometry
Equation: KClO3 --> KCl + O2
1. Balance the equation: 2KClO3 --> 2KCl + 3O2
2. Identify the starting point: 138.6 g of KClO3
3. Convert to moles: 138.6 g of KClO3 / 122 g/mol = 1.136 mol of KClO3
4. Multiply by mole ratio: 1.136 mole KClO3 * 3 mol O2 = 1.704 mol O2
2 mol KClO3
5. Convert to ending unit: 1.704 mol O2 * 32 g O2 = 5453 g O2 is produced
Websites Used/Work Cited
- www.wpclipart.com
- blogs.plos.org
- socratic.org
- becuo.com
- 2012books.lardbucket.org
- surfguppy.com
- www.grandinetti.org
- chemistry.tutorvista.com
- 2012books.lardbucket.org
- hydrocarbonsalkanealkene4p104.blogspot.com
- www.learnnext.com
- simple.wikipedia.org
- antoine.frostburg.edu
- www.studyblue.com
- ykonline.yksd.com
- pixgood.com
- www.elmhurst.edu