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Chapter 2 Chemistry of Life

Chapter 2 Chemistry of Life. Can you list the levels of organization?. Matter. Matter – Anything that has mass and takes up space – made up of atoms. States of matter Solid – has definite shape and volume Liquid – has definite volume, changeable shape Gas – has changeable shape and volume.

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Chapter 2 Chemistry of Life

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  1. Chapter 2 Chemistry of Life • Can you list the levels of organization?

  2. Matter Matter – Anything that has mass and takes up space – made up of atoms. States of matter Solid – has definite shape and volume Liquid – has definite volume, changeable shape Gas – has changeable shape and volume

  3. Atom - The smallest particle into which a substance can be broken by ordinary chemical means. • Remember an atom has a nucleus that consists of neutrons (neutral) and protons (positive) • Electrons (negative) are found orbiting the nucleus Levels Reviewed

  4. Element – Groups of the same type of atom Compound – Two or more elements chemically combined ex. H2O

  5. MOLECULE- GROUPS OF ATOMS BONDED TOGETHER & ACTING AS A GROUP ORGANELLES- BASIC STRUCTURES WITHIN CELLS – has a specific function CELL- BASIC UNIT OF LIVING ORGANISMS

  6. TISSUE- TISSUES ARE GROUPS OF CELLS WITH A COMMON FUNCTION. • ORGAN- OFTEN LARGE AND COMPOSED OF SEVERAL DIFFERENT TISSUES • ORGAN SYSTEM- A GROUP OF ORGANS CARRYING OUT A MAJOR BODY PROCESS • ORGANISM- (A GROUP OF ORGAN SYSTEMS IN AN INDIVIDUAL) – any living thing

  7. Mixtures • Mixtures – two or more substances not chemically combined – therefore they retain their own properties • Solutions – evenly combined • Solvent – does the dissolving ex. Water • Solute – the substance being dissolved ex. Sugar

  8. Suspensions –The particles will spread out and eventually settle – large particles (saturated, unsaturated, and supersaturated) • Example sand in water (whole blood) • Colloid – a mixture that has medium particles – held in solution by their association with water • ex. Liquid jello….. Mayonnaise

  9. Mixtures Compared with Compounds • No chemical bonding takes place in mixtures • Most mixtures can be separated by physical means • Mixtures can be heterogeneous or homogeneous • Compounds cannot be separated by physical means • All compounds are homogeneous

  10. Writing Chemical Equations • The left side of an equation is called the reactants. • The right side of an equation is called the products • An arrow separates the reactants from the products. The arrow is called a “yields” sign Ex. Na + Cl  NaCl

  11. TYPES OF BONDS(Bonds store energy) IONIC BONDS- ELECTRONS ARE TRANSFERRED FROM ONE ATOM TO ANOTHER AND IONS ARE FORMED Ions are charged atoms resulting from the gain or loss of electrons Anions have gained one or more electrons Cations have lost one or more electrons

  12. COVALENT BONDS- WHEN ATOMS SHARE ELECTRONS (the strongest bond) • e.x. Peptide bonds – between C and N in proteins

  13. HYDROGEN BONDS- A BOND BETWEEN HYDROGEN AND 2 SMALL ELECTRONEGATIVE ATOMS ex. F, N, O (the weakest bond)

  14. Polar and Nonpolar Molecules Electrons shared equally between atoms produce nonpolar molecules Unequal sharing of electrons produces polar molecules (ex. Water!) (unequal causes a “charge” on each molecule)

  15. Types of Reactions • Chemical Reactions – the process of breaking down chemical bonds and/or forming new ones (a chemical equations shows this) • To do this an activation energy is needed ( the energy that is needed to get the reaction going) • Exothermic – there is a net release of energy (it feels warm) • Endothermic – there is a net absorption of energy (feels cool)

  16. . Two or more elements or compounds combine to make a more complex substance (ex. Dehydration synthesis – takes H2O away) A + B → AB AB → A + B Compounds break down into simpler substances (ex hydrolysis – puts H2O back) Occurs when one element replaces another one in a compound AB + C → AC + B AB + CD → AC + BD Occurs when different atoms in two different compounds trade places A = Red B = Blue C = Green D = Yellow

  17. Identifying Chemical Reactions 2. Use colored pencils to circle the common atoms or compounds in each equation to help you determine the type of reaction it illustrates. Use the code below to classify each reaction. S = Synthesis D = Decomposition SR = Single Replacement DR = Double Replacement ____ P + O2 → P4O10 ____ Mg + O2 → MgO ____ HgO → Hg + O2 ____ Al2O3 → Al + O2 ____ Cl2 + NaBr → NaCl + Br2 ____ H2 + N2 → NH3

  18. ____ Na + Br2 → NaBr ____ CuCl2 + H2S → CuS + HCl ____ HgO + Cl2 → HgCl + O2 ____ C + H2 → CH4 ____ KClO3  →   KCl  +  O2  ____ S8 + F2 → SF6 ____ BaCl2   +   Na2 SO4 →     NaCl   +   BaSO4

  19. Types of Reactions 1. Synthesis – small molecules are combined into larger molecules – always involves the formation of new chemical bonds • Ex. A + B  AB

  20. Ex. Dehydration synthesis (condensation) – the formation of complex molecules by the removal of H2O A-B-C-H + HO-D-EA-B-C-D-E + H20

  21. Anabolism – Energy requiring building phase of metabolism in which simpler substances are combined to form more complex substances

  22. 2. Decomposition – breaks large molecules into smaller ones AB A + B • Ex. Food broken down • If water is used to breakdown the bonds then it is called hydrolysis (opposite of dehydration synthesis) Ex A-B-C-D-E + H20  A-B-C-H + HO-D-E

  23. Ex Hydrolysis – is an example of a decomposition reaction where water is added back into the molecule

  24. Catabolism – Process in which living cells break down substances into simpler substances

  25. Additional Vocabulary • Valence – number of electrons in the outer energy level. Ex. 7 • Oxidation Number – number of electrons an atom has gained or lost and the charge associated. Ex. Looking at the above valence: 1- • Octet Rule - filling the outer energy level to 8 electrons (exception is the first energy level that can only hold two electrons)

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