1. T HE C HEMISTRY O F L IFE Chapter 6

2. A TOMS AND T HEIR I NTERACTIONS Section 6.1

3. O BJECTIVES FOR THIS SECTION Relate the structure of an atom to the identify of elements. Relate the formation of covalent and ionic chemical bonds to the stability of atoms. Distinguish mixtures and solutions Define acids and bases and relate their importance to biological systems.

4. W HAT MAKES A LIVING THING DIFFERENT FROM A NONLIVING THING ? H OW ARE THE PARTICLES THAT MAKE UP A ROCK SIMILAR TO THOSE OF A CORAL ?

5. Living things and non living things are all made of atoms. It is the way the atoms combine into different elements that affects their physical and chemical properties and whether they are living or nonliving. That particles that form a rock and the hard outer covering of the coral are made of similar substances that are combined differently.

6. E LEMENTS EVERYTHING….. Is made of substances called elements. Element is a substance that cant be broken down into simpler chemical substances. Fun Fact: of the naturally occurring elements on Earth, only about 25 are essential to living organisms. Hydrogen, Oxygen, Nitrogen and Carbon

7. T HE PERIODIC TABLE

8. A TOMS : T HE BUILDING BLOCKS OF ELEMENTS An atom is the smallest particle of an element that has the characteristics of that element. They are the basic building blocks of all matter. All atoms have the same general structure that includes the center of an atom which is called the nucleus. http://www.youtube.com/watch?v=lP57g EWcisY

10. Energy levels are what exist around the nucleus holding electrons. The first energy level can hold only two electrons. The second energy level can hold a maximum of eight electrons. The third level can hold up to 18 electrons.

11. E XAMPLES

12. P ART 2

14. I SOTOPES OF AN E LEMENT Atoms of the same element that have different numbers of neutrons are called isotopes of that element Example: Carbon Carbon normally has the atomic mass of 12 which is why it is usually called carbon-12. This means it has 6 protons and 6 neutrons. Other isotopes of carbon are carbon-13 and carbon-14. How many neutrons do those have?

15. C OMPOUNDS AND B ONDING Salt is very common to our everyday life but it is not an element. Salt is a type of substance called a compound. A compound is a substance that is composed of atoms of two or more different elements that are chemically combined. Table salt is a compound composed of element sodium and chlorine (NaCl)

16. H OW DO COMPOUNDS FORM ? Atoms combine with other atoms only when the resulting compound is more stable that the individual atom is by itself. How does it become stable? For most elements, an atom becomes stable when its outermost energy level is full. How do the energy levels become stable? By sharing electrons with other atoms!

17. E XAMPLE OF A COMPOUND H2O H2 = Two atoms of Hydrogen O = One atom of Oxygen When two atoms share electrons that force the hold of them together is called an Covalent Bond A molecule is a group of atoms held together by covalent bonds

18. I ONIC B ONDS Not all atoms bond with each other by sharing electrons. Sometimes they will combine with each other by first gaining or losing electrons in their out energy levels. An atom that gains or loses electrons has an electrical charge and is called an ion. An ion is a charged particle made of atoms.

19. E XAMPLE OF AN IONIC BOND NaCl =Table salt A sodium atom (Na) contains11 electrons including one in the third energy level. A chlorine atom (Cl) contain 17 electrons with the out level holding seven electrons.

20. The positive charge of the sodium ion attracts the negative charge of a chlorine ion. Therefore, sodium will give One electron to chlorine for each atom to become stable. The attractive force between two ions of opposite charge is known as an ionic bond.

21. C HEMICAL R EACTIONS Chemical reactions occur when bonds are formed or broken, making substances to recombine into different substances. All the chemical reactions that occur within an organism are referred to as that organism’s metabolism. Scientist show these reactions by writing chemical equations

22. W RITING CHEMICAL EQUATIONS H2O H + H+ O  H2O NH3 N+H+H+H-->NH3

23. M IXTURES AND S OLUTIONS A mixture is a combination of substances in which the individual components retain their own properties. A solution is a mixture in which one or more substances are distributes evenly in another substance.

24. A CIDS AND B ASES Chemical reaction in organisms also depends on the pH of the environment with the organism. The pH is a measure of how acidic or basic a solution is. A scale with values ranging from below 0 to above 14 is used to measure Ph.

25. A CID Substances with a pH below 7 are acidic. An acid is any substance that forms hydrogen ions in water. A solution is neutral if is pH equals 7 Substances with a pH above 7 are basic. A base is any substance that forms hydroxide ions in water.

26. Q UESTIONS OVER 6.1 Describe where the electrons are located in the atom. How does the formation of an ionic bond differ from the formation of a covalent bond? A nitrogen atom contains seven protons, seven neutrons, and seven electrons. Make a labeled drawing of the structure of a nitrogen atom. How can this atom become stable?