1. “I’ll believe it when I see it…” What have you learned about in science that is either too small or too big to fully perceive with your senses?

2. What have you learned about in science that is either too small or too big to fully perceive with your senses? Examples: water molecule, earth’s rotation, water cycle, germs, photosynthesis, plate tectonics, lunar tides “I’ll believe it when I see it…”

3. The Biochemical Basis of Life Essential Questions: —What are atoms and what they are composed of? —How do the components of an atom vary? —How do atoms interact with each other?

4. Why learn about atoms? How can we eat such different kinds of animals and plants and then use those materials to construct or our bodies? Plants don't eat as we do. How do they construct themselves? Why doesn't all the water on earth simply disappear through evaporation?

5. Your turn! What do you know about atoms? What do they look like?

6. Where are they? Are they in solids? Are they in liquids? Are they alive? Are they in dead things? Your turn! What do you know about atoms?

7. Scale: micro to macro

8. Atoms An atom is the smallest unit of an element that has all of the characteristic properties of that element. Everything living and non-living is made of atoms. An individual atom of a substance, like gold, has all the characteristics of that substance. A gold atom is made up of smaller components called protons, neutrons, and electrons. By themselves, these subunits do not have the properties of gold.

9. Atomic Structure # protons=# neutrons Atomic Mass= # protons + # neutrons Atomic Number= # protons ComponentChargeLocationMass Neutron No charge (0)Nucleus= mass of proton Proton Positive (+)Nucleus= mass of neutron Electron Negative (-)Energy levels/ Surrounding Shells = 0 (very light)

10. Valence electrons – Electrons travel around the nucleus in regions called energy levels – There are 2 electrons in the innermost energy level or shell – Valence electrons are the electrons that travel in the outermost energy level or shell – Atoms are in a stable “happy” state when they have a complete outer shell (2, 8, or 18 electrons)

11. Your Turn! How many Valence Electrons are in each atom?

12. 354

13. Periodic Table of Elements …a crash course An element is the most simple chemical substance. It is composed of one type of atom.

14. “…‘Our schoolchildren, some as young as the fourth grade, are being exposed to this deadly element in their science classes,’ said Tricia Montcalm, president of the Grand Rapids Parents Association.”

15. Periodic Table of Elements …a crash course An element is the most simple chemical substance. It is composed of one type of atom. # protons = # electrons (+) = (-)  Elements have no charge Elements below and to the left of the purple “staircase” line on the table are metals (except for H). Elements above and to the right of the purple “staircase” line on the table are non-metals. ElementColumn # valence electrons Hydrogen11 Carbon144 Oxygen166 Neon*188 The column number gives the number of valence electrons in the element:

16. Patterns in the Periodic Table ElementColumn # valence electrons Hydrogen11 Carbon144 Oxygen166 Neon *188

17. Scale – from micro to macro How do atoms interact to form the components of our bodies and the earth?

18. Scale – from micro to macro How do atoms interact to form the components of our bodies and the earth? Bonds!

19. Ionic Bonds 1.Ionic bonding occurs between metals and non-metals. 2.Atoms held together by ionic bonds form a compound. 3.The opposite charges of the elements (ions) attract. 4.Atoms are in a stable “happy” state when they have a complete outer shell of valence electrons (2, 8, or 18). 5.If atoms have 1 or 2 electrons too few or too many, they gain or lose electrons in order to achieve a complete outer shell of valence electrons.

20. Covalent Bonds 1.Ionic bonding occurs between non-metals. 2.Atoms held together by covalent bonds form a molecule (like water!). 3.Covalent bonds are the most common in Biology. 4.Atoms are in a stable “happy” state when they have a complete outer shell (2, 8, or 18). 5.If atoms have more than 3 electrons too few or too many, they share electrons in order to achieve a complete outer shell of valence electrons. 6.Sharing electrons is easier because it takes less energy than fully gaining or losing them.

21. Isotopes Isotopes are atoms of the same element that contain different numbers of neutrons. Your turn! How many neutrons are in each isotope of Carbon?

22. Isotopes Isotopes are atoms of the same element that contain different numbers of neutrons. Your turn! How many neutrons are in each isotope of Carbon? 678

23. Bonds at a glance… http://www.youtube.com/watch?v=QqjcCvzWwww Your turn! 1.What type of bonding occurs when electrons are transferred (gained or lost)? 2.What type of bonding occurs when more electrons are shared? 3.What part of the atom is responsible for how an atom interacts with another atom? 4.In what case will an atom not react to another atom?

24. Bonds at a glance… http://www.youtube.com/watch?v=QqjcCvzWwww Your turn! 1.What type of bonding occurs when electrons are transferred (gained or lost)? Ionic bonding 2.What type of bonding occurs when more electrons are shared? Covalent bonding 3.What part of the atom is responsible for how an atom interacts with another atom? Electrons (e-) 4.In what case will an atom not react to another atom? When the valence electron shell is complete on its own, or when it is complete because it is bonded (ionic or covalent) with 1 or more atoms)

25. Case Study: Affect of Carbon Monoxide on the Function of Hemoglobin Why is it important that these O 2 and CO 2 bond well to Iron atoms in the heme molecules? How does Oxygen & Carbon Dioxide bond to the Iron in your blood cells?

26. Question/Problem: Why is Carbon Monoxide deadly? 1.Compare CO 2 and CO. Which is more stable? How do you know? Record your observation in your notes Hint: How many electrons does Carbon need to have a complete outer shell? Hint: Are atoms stable if they have do not have a complete outer shell? What do atoms do when they do not have a complete outer shell? 2. What do you think will happen if you breathe in Carbon Monoxide instead of Carbon Dioxide? Record your hypothesis in your notes, make sure to state something about bonding.

27. Experiment & Conclusions Background: – http://www.youtube.com/watch?v=wKIrbq2pWvw http://www.youtube.com/watch?v=wKIrbq2pWvw Conclusions: 1.Why is CO more unstable than CO 2 ? Carbon does not have its valence shell full. 2.What does that instability mean for the hemoglobin? CO will bond to heme more quickly and tightly. But won’t let go to let normal O 2 and CO 2 in. 3.Why are bonding properties of atoms, compounds and molecules important? In this example, your body needs to get Oxygen to cells and get rid of CO 2 properly. If not, the cells and eventually the body will die.