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Study Notes
Ch 4 p124-157: p164-166
Ch 7 pg 256-285
Ch 5 pg 176-207
Ch 8 pg 297; 307; 316-323
Ch 6 pg 214-241; p246-249
Strategies for Studying:
• DO your study notes!!
• Look at the figures (pictures) and read the captions.
• Read the chapter summary.
• Practice with the chapter review.
• Review pages in Reading-Note Taking Guide (workbook)
Location in atom
Electric charge
Size - mass
Proton
Neutron
Electron
An isotope is
Atomic
Number
Ag
Au
An ion is
Atomic Mass
How do you calculate the
atomic mass of an atom?
What is the difference
between Atomic
Number and Atomic
Mass of an element?
Why are atoms
electrically neutral?
C
O
For the following compounds, name all the elements and count the number of atoms in these
compounds.
NH4NO3
C6H12O6
NaCl
4FeCl2
•
•
•
•
Most elements are __________
Metalloids/Semi metals are located in groups _______________
Nonmetals are located ___________
Elements are arranged by increasing _________________
What are characteristics of the following types of matter?
Metals
Nonmetals
Semimetals / Metalloids
Pure substance
Element
Compound
Mixture
What are some methods to separate mixtures?
Solubility
Solute
Solvent
***______________ is a universal solvent.
Homogeneous
Heterogeneous
Concentration
Dilute
Define:
Define:
Unsaturated
Saturated
Define:
Define:
Solution
Colloid
Suspension
Define:
Define:
Define:
Example:
Example:
Example:
Ways to speed up the dissolving process/increase solubility:
•
Chemical bonding
•
Valence electrons:
•
Atoms bond by :
•
Polymers:
•
Covalent Bonds
•
Ionic Bonds:
Chemical Reactions
•
What are four signs of a chemical reaction?
1. ___________________________________________________________________
2. ___________________________________________________________________
3. ___________________________________________________________________
4. ___________________________________________________________________
What are the 4 types of chemical reactions?:
1. ___________________________________________________________________
2. ___________________________________________________________________
3. ___________________________________________________________________
4. ___________________________________________________________________
•
•
Reactants :
•
•
Exothermic :
•
Ex. Give an example:
•
Endothermic:
•
Ex. Give an example:
Products :
Law of Conservation of Mass / Matter :
Ex. Is mass conserved in the following chemical reactions?
2Na + Cl2 è 2NaCl
Yes or No
H2O + CO2è C6H12O6 + O2
Yes or No
Catalyst :
Inhibitor
(how do you know?) ---
List four factors that affects the rate of reactions :
1.
2.
3.
4.
Acids and Bases
Acid
Base
Neutral
Define
Taste / Feel
Release of ______
ions
pH Range
Weak pH #
Strong pH #
Example:
7
7
Indicator
Define:
Examples:
What happens when an acid and a base are combined?
Why can acids and bases conduct electricity?
Chemical Compounds
•
Inorganic vs. Organic
Ex. Circle the organic compound. Cross out the inorganic compound.
2NaCl
C6H12O6
NH4NO3
CO2
•
Carbon
Write 3 facts about carbon
1.
2.
3.
Carbohydrates :
Proteins
Nucleic Acids
H2 O