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Understanding the Chemistry of Life: Atoms, Elements, and Compounds

This chapter covers the fundamental concepts of chemistry essential for understanding life. It explains the nature of matter, focusing on atoms as the smallest units and their unique properties defined by the number of protons. Key elements in living organisms such as oxygen, carbon, hydrogen, and nitrogen are discussed, alongside the concept of isotopes and radioactive decay. The chapter also explores chemical compounds, their formulas, and the primary types of chemical bonds including covalent, ionic, and van der Waals forces that hold molecules together.

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Understanding the Chemistry of Life: Atoms, Elements, and Compounds

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  1. Honors BiologyChapter 2 The Chemistry Of life

  2. The Nature of Matter • Essential Question: • How would you explain the relationship between atoms, elements, and compounds?

  3. Atoms smallest unit of matter each element has its own unique # of protons (atomic #)

  4. Elements • Only ~ 24 elements found in living things • 4 most abundant: • Oxygen • Carbon • Hydrogen • Nitrogen

  5. Isotopes atoms of same element with different # of neutrons #p + #n = atomic mass (mass #)

  6. Radioactive Isotopes some isotopes have unstable nuclei so they undergo “decay”

  7. Chemical Cpds compound: substance formed by chemical combination of 2 or more elements in definite proportions cpd has different properties than elements alone had

  8. Chemical Formulas

  9. Chemical Bonds Atoms form chemical bonds with other atoms to ________________. The 2 main types of bonds are ________ and ____________.

  10. Types of Bonds

  11. Chemical Bonds Covalent Bonds Polar Covalent Bonds share valence e- unequal sharing e-

  12. Ionic bonds • transfer of e-  atom with a charge (ion) • (+) ions = cations • (-) ions = anions • opposite charges attract • charges must be balanced • stronger bonds than covalent

  13. van der Waals Forces • Because atoms do not share e- equally, there are polar bonds • This causes the (+) end of one molecule to be attracted to the (-) end of another molecule • This attraction is called van derwaals forces • Very weak compared to covalent bonds but are still able to hold molecules together

  14. Van der Waals Forces in action

  15. What type of bond is shown here?

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