Elements- the building blocks of all matter. (118 total)

Atoms- the smallest particle of an element.

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Elements:

Atomic Number and Atomic Mass (P.18)

Atomic Number- Number of Protons

Atomic Mass- Number of Protons + Nuetrons

AM is measures in daltons

(6.02 x 10²³) daltons makes one gram

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Neutral atoms have the same amount of electrons and protons.

Ions are charged particles; number of electrons does not equal the number of protons.

Cation⁺- More protons than electrons.

Anion^-- More electrons than protons.

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Same number of protons; different number of neutrons

(think carbon)

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Carbon Isotopes (P.19-20)

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Carbon 12- ¹²C

6 Protons; 6 Nuetrons- Stable; over 99% found in nature

Carbon 13- ¹³C

6 Protons; 7 Nuetrons- Unstable; Make up majority of remaining 1%

Carbon 14- ¹⁴C

6 Protons; 8 Neutrons- Unstble and Radioactive

Radioactive decay- used in carbon dating

0.5grams or half-life= 5730 years

0.25grams=11460years

0.125grams= 17190years

Eletrons Determine the Elemental Behavior and Shape of an Atom (P.20)

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Atoms are 3D

1st Energy Level (1st Orbital)

     2 electrons max

2nd Energy Level (2nd Orbital)

     8 electrons max

     2S 2Px 2Py 2Pz

3rd Energy Level (3rd Orbital)

     8 electrons max

     3s 3Px 3Py 3Pz

Redox Reactions

Oxidation and Reduction (P.21)

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Remember: OiL RiG

Oxidation Loss Reduction Gain

The Periodic Table (P.22)

Dmitri Mendeleev - 19th Century Chemist

• Organized elements by atomic number and chemical properties
• Repeates in 8s due to valence electrons
• Octet Rule - 8 valence electrons make atoms happy
• 118 elements
• 90 naturally occuring elements
• C H O N P S (organic compounds) - make up 96.3% of body weight 

12 Elements to Remember 

C H O N P S Fe Na Ca Cl Mg K

1. ⁶C_12.01           Carbon 
2. ¹H_1.01            Hydrogen
3. ⁸O_16.00          Oxygen 
4. ⁷N_14.01          Nitrogen
5. ¹⁵P_30.96         Phosphorous 
6. ¹⁶S_32.06         Sulfur 
7. ²⁶Fe_55.93        Iron 
8. ¹¹Na_22.99       Sodium
9. ²⁰Ca_40.08       Calcium 
10. ¹⁷Cl_35.45        Chlorine 
11. ¹²Mg_24.31       Magnesium 
12. ¹⁹K_39.10          Potassium 

Chemical Bonds and Interactions (P.23)

(Table 2.1)

• Covalent Bond- Sharing of electron pairs (Strong Bond)
• Ionic Bond- Opposites attract (Strong Bond)
• Hydrogen Bond- Sharing of H atom (Weak Bond)
• Hydrophobic Interaction- Forcing hydrophobic protons of a molecule together in the presence of a polar molecule.

Water Chemistry

Cohesion vs Adhesion

Cohesion 

Water molecules stick to other Water molecules

Adhesion

Water molecules stick to other Polar molecules

6 Properties of Water (P.27)

(Table 2.3)

1. High Specific Heat- Takes a high temp to change water temp.
2. High Heat of Vaporization- Evaporative cooling (sweating).
3. Solid is Less Dense than Liquid- Water freezes top to bottom.
4. Solvent- breaks weak bonds
5. Organizes Nonpolar Molecules
6. Water Ionizes- H₂O -> OH^- + H⁺

A solute dissolves into solvent and makes a solution.

Think Saltwater Solution.

Solute= Salt

Solvent= Water

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More acidic= More [H⁺]; Less OH^-

More Basic= More OH^-; Less [H⁺]

Buffers help maintain homeostasis.

• Finding Protons- Same as Atomic Number
• Finding Electrons- Same as Protons (if stable)
• Finding Neutrons- Protons Minus Number of Protons
• Finding Valence Electrons- Number of Electrons Minus 2 (first energy level), then minus 8 (second energy level).

(Know elements 1-18)