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CHEMISTRY

Matter – 3 states

Elements –

Atom –

Compound –

Molecule –  

COUNTING ATOMS
H₂O -> H = ___; O = ___
2(H₂O) -> H = ___; O = ___

STRUCTURE OF ATOMS:

1.           Protons: ___charged particles

2.           Neutrons: ___charged particles

3.           Electrons: ___charged particles

The Periodic Table of Elements

              6            <-       Atomic # (# protons)

              C           <-       Symbol

          Carbon       <-       Element

          12.011          <-       Atomic Mass (# protons + # neutrons)

# protons = # electrons 

ELECTRON MODELS – Visualizing an atom

The __________________________________ determines how reactive the atom will be (how many things it can bond with)

 Isotope –

 CHEMICAL BONDS –

Atoms want to _________________________ to become more stable.

1.           Ionic Bond –

(Metals + Nonmetals)

Ion:

Ex: NaCl (diagram from class)

2.           Covalent Bond –

(Nonmetals + Nonmetals)

Polar –                                   
Ex: H₂O

Nonpolar –                                   
Ex: H₂

SHARING ELECTRONS BETWEEN ATOMS

Single Bonds: 1 ______________shared (H – H)

Double Bonds: 2 _____________ shared (O = C = O)

Triple Bonds: 3 _______________shared (N = N)

Diatomic Molecules –

(H₂, O₂, N₂)

3.           Hydrogen Bond –

(Force b/w 2 polar H₂O molecules) - see p. 31 in book

STRUCTURAL FORMULAS VS. CHEMICAL FORMULAS 

Solutes:

 

Solvents:

CHEMICAL REACTIONS –

1.           Synthesis/ Dehydration –

Endergonic Rxn: takes in E

See handout

2.           Decomposition/ Hydrolysis –

Exergonic Rxn: releases E

See handout

Activation Energy:

Law of Conservation of Mass: 

Ex:  Mg + 2HCL - - > MgCl₂ + H₂
         C₆H₁₂O₆ + 6O₂ - -> 6CO₂ + 6H₂O

pH Notes

Acids:

Bases:

Ions –

Ionization –

Ex: HCl -> H⁺ + Cl-

Dissociation –

Ex: NaOH -> Na⁺ + OH-

Neutralization –

Ex:
Acid + Base -> H₂O + Salt
HCl + NaOH -> H₂O + NaCl
H⁺ + OH^- -> H₂O

pH Scale:

(see p. 32 in text for scale)

 Indicator-

·       Litmus Paper:

·       Methyl Orange:

·       Phenophthalein:

Living cells must maintain internal levels of H+ and OH– ions.

Buffers –

BIOCHEMISTRY

 Organic Molecules –

Macromolecules –

4 TYPES OF MACROMOLECULES

1.           Carbohydrates:

(see p. 36)

A)Monosaccharides –

Ex: glucose C₆H₁₂O₆

Isomers:

 B)   Disaccharides –

 Ex: sucrose = glucose + fructose

C)   Polysaccharides –

Plants: Starch= energy storage
Animals: Glycogen= energy storage

2.           Lipids –

·       ___ more energy storage than carbs (more C-H bonds)

·       More ____, less ____ than carbs

·       _______ energy source

·       Makes up ______________________

Building Blocks: Glycerol + 3 Fatty Acids (Triglyceride)

(see p.37)

A)Saturated Fat –

(butter, lard)

B)   Unsaturated Fat –

(oils)

C)   Phospholipids –

D)   Cholesterol –

3.           Proteins –

· _________________________ of cells

· ________________ between cells (receptors)

· __________ – promote chemical reactions in cell

· _______________ of energy

· Ex:

Building Blocks are ______________. Basic structure:

Peptide Bonds –

Polypeptide –

Protein Structure

·      Primary Structure –

·      Secondary Structure –

·      Tertiary structure –

·      Quaternary Structure –

4.           Nucleic Acids –

·       A source of __________________ in chromosomes.

·       Building Blocks are long chains of Nucleotides. Basic Structure: (p. 39)

Phosphate                                                 Nitrogen                     Group                                                    Base

                                                 5-carbon sugar

Examples: