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Exploring Atoms and Compounds: Chemistry of Life

Discover the fundamentals of matter and atoms in Chapter 6 of the Chemistry of Life. Learn about isotopes, compounds, chemical bonds, and reactions. Dive into the unique properties of water, its role in solutions, and the concept of pH. Enhance your understanding of the building blocks of life through engaging text and examples.

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Exploring Atoms and Compounds: Chemistry of Life

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  1. Chemistry of Life Chapter 6

  2. Atoms • Matter- anything that has mass and takes up space • Atom- smallest particle into which a substance can be divided and still retain its chemical properties

  3. What makes up an atom? • Proton- subatomic particle in atom that has positive charge • Neutron- subatomic particle in atom that has no charge • Electron- subatomic particle in atom that has negative charge

  4. Understanding atoms • Nucleus- center of the atom where protons and neutrons are located • Electrons are found in the electron cloud

  5. Understanding atoms • Element- atoms with the same atomic number have the same chemical properties

  6. Isotopes • Isotopes- Atoms that have the same number of protons but different numbers of neutrons

  7. Uses of radioactive Isotopes • Medical • Tracer- a radioactive substance that is taken up and used by the body • Ex. An overactive thyroid gland may be a symptom of cancer and can easily be detected using radioactive tracers

  8. Compound • Elements can combine to form more complex structures • Compound- is a pure substance formed when two or more different elements combine

  9. Combining atoms • Covalent bond-chemical bonds that forms when electrons are shared • Molecule- is a compound held together by covalent bonds

  10. Covalent Bond

  11. Ionic bonds • Ionic Bond- chemical bond between two atoms that are attracted to each other by opposite charges • Think of how the positive and negative pole of a magnet attract

  12. Ionic Bonds

  13. Van der Waals forces • Van der Waals forces- attractive forces between positive and negative regions pull on molecules and hold them together

  14. Chemical Reactions • Chemical reactions- process by which atoms or groups of atoms in substances are reorganized into different groups • Reactants- starting substances • Left side of the arrow • Products- substance formed during reaction • Right side of the arrow

  15. Chemical reactions 2H2 + O2 2H20 Energy Reactants Products

  16. Chemical reactions • Activation energy- minimum amount of energy needed to start reaction • Enzyme- protein that can speed up the reaction

  17. Hydrogen bonds • Hydrogen bond- weak chemical bonds of a very special sort; play a key role in biology • A hydrogen bond occurs when the positive end of one polar molecule is attracted to the negative end of another • Think of two magnets

  18. Hydrogen bonds

  19. Water’s unique properties • H2O- oxygen atom linked to two hydrogen atoms by single covalent bond • Water is a polar molecule • Hydrogen bonds allow these properties

  20. Water’s unique properties • Heat storage • Many hydrogen bonds water molecules form together require large amount of thermal energy to disrupt organization • Water heats up slower than most compounds and holds temperature longer

  21. Water’s unique properties • Ice Formation • If temperature is low enough, very few hydrogen bonds will break Why is ice dense? • Hydrogen bonds keep water molecules spaced apart preventing them from approaching each other

  22. Water’s unique properties • High heat of vaporization • Temperature is high enough, many hydrogen bonds break in water, changing it from a liquid to a gas • How does sweating cool you off?

  23. Water’s unique properties • Cohesion- when a water molecule is attracted to another water molecule • Adhesion- when a water molecule is attracted to a different polar molecule • Capillary action is created by adhesion

  24. Water’s unique properties • High polarity • Water molecules in a solution always try to form maximum hydrogen bonds possible • Hydrophilic- polar molecules that attracted to water molecules • Soluble- dissolve in water • Hydrophobic-nonpolar compounds shrink from contact with water

  25. Water and solutions • Mixture- combination of two or more substances which each keeps its own properties • Homogenous mixture or solution- mixture that is uniform (same) composition

  26. Mixtures Homogenous Heterogeneous

  27. Homogenous mixture • Solvent- substance in which another substance is being dissolved • Water • Solute- substance that is dissolved in the solvent • powder

  28. pH • Acid- substances that release hydrogen ions (H+) when dissolved in water • Base- substance that release hydroxide ions (OH-) when dissolved in water • pH- concentration (amount) of H+ in a solution

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