1. Chapter 6.1 Biology

2. Bio NOTES: Intro to the Chemistry Your life DEPENDS on chemistry! 1.When you inhale oxygen, your body uses it in chemical reactions! 2.When you eat food, your body breaks it down and uses it in chemical reactions!

3. 6.1: Atoms, Elements, and Compounds Chemistry is the study of matter. Matter is anything that has mass and takes up space. Atoms are the building blocks of matter. Brain Pop -Atoms

4. THE STRUCTURE OF ATOMS: Billions of atoms could fit on the head of a pin! Atoms are made up of even smaller particles – 1. Neutrons 2. Protons 3. Electrons

5. The Structure of Atoms: Nucleus – the center of an atom Within this nucleus are protons and neutrons. Neutrons – particles that have no charge Protons – particles with a positive charge Electrons – negatively charged particles located outside the nucleus. Constantly move around the nucleus in energy levels

6. Elements: An element is the name for a specific Atom It is a pure substance that cannot be broken down into other substances by chemical or physical means. But Elements can be joined together to form compounds

7. All living things are made up of chemical compounds A compound is made of atoms of different elements bonded together, such as H 2 O or CO 2 These compounds are the building blocks of our body and the world around us. The bonds that can hold compounds together are ionic, covalent, and hydrogen bonds.

8. 3 Types of Bonds: 1. Ionic bond – forms between oppositely charged ions 2. Covalent bond – forms when atoms share a pair of electrons 3. Hydrogen bond – Type of covalent bond forms between slightly positive hydrogen atoms and slightly negative atoms. Think WATER O HH _ ++ covalent bonds Oxygen atom (O) Carbon atom (C) Oxygen atom (O) Carbon dioxide (CO 2 ) Sodium ion (Na + ) Chloride ion (CI - ) ionic bond gained electron Ion = atom that has lost or gained electrons

9. POSITIVE IONS: *Formed when an atom loses an electron. *Lose the negative electron = atom is more positive NEGATIVE IONS: *Formed when an atom gains an electron. *Gain a negative electron = atom is more negative

10. Types of Compounds: 1. Molecule - a compound in which the atoms are held together by covalent bonds. 2. Ionic compound – a substance formed by ionic bonds.

11. Water and Solutions 6.3 pgs. 161-163

12. Why is water so important??

13. Water is a molecule: H2O Covalent bonds hold a water molecule together. The electrons are pulled towards the bond. This leaves one side slightly more positive than the other. This makes water….

14. Water is a polar molecule Polarity: Opposite charges on opposite sides of a molecule

15. Water’s Polarity Molecules that have an unequal distribution of charges are called polar molecules. Polarity is the property of having two opposite poles. The oxygen and hydrogen in water share electrons, oxygen is bigger and holds the electrons closer so oxygen becomes a little negative and hydrogen becomes a little positive.

16. The Polarity of Water Creates Hydrogen Bonds Attraction between the H on one molecule and an electronegative atom on another molecule. Electronegative= negative charge

17. It is because of Waters’ Polarity and Hydrogen Bonding that water is able to do Extraordinary things!!

18. Extraordinary Properties of Water 1. Adhesion Water molecules cling to other surfaces. Example: Capillary action, as in water moving up a plant stem

19. Extraordinary Properties of Water 2. Cohesion Water molecules stick together Water LOVES itself, therefore it clings to itself! - this creates Surface Tension

21. Extraordinary Properties of Water 3. Water is less dense as a solid Most substances gain density when frozen. This allows for aquatic life to live under the ice in the extreme cold.

22. Why ice really does float:

23. Liquid water has hydrogen bonds that are constantly being broken and reformed. Frozen water forms a crystal-like lattice whereby molecules are set at fixed distances.

24. Extraordinary Properties of Water 4. Water is a good solvent Solvent = a substance in which another substance is dissolved in Solute = a substance dissolved in a solvent Solution = when a solvent and solute are combined

25. Water is a Solvent Water is polar so it dissolves all polar molecules (example salt, sugar) Water will not dissolve non-polar molecules (example Oil, grease) polar = has slightly charged regions nonpolar = does not have charged regions

26. Water is polar Water molecules are held together with hydrogen bonds Properties Adhesion Cohesion Less dense when frozen Good Solvent Review

27. Pg 164-165

28. The pH Scale **Some compounds form acids or bases Scientists use something called the pH scale to measure how acidic or basic a liquid is The scale looks at the concentration of positively charged hydrogen ions (H+) in a solution vs. the amount of negatively charged hydroxide ions (OH-) The scale goes from values 0 through 14. Brain pop

29. Acids Taste sour Corrode metals An acid releases a hydrogen ions when it dissolves in water. -high H + concentration -Low OH- concentration - pH less than 7

30. Bases Taste bitter, chalky Feel soapy, slippery A base releases hydroxide ions

31. A B Left to right

32. Ok in English please! If you have an ionic compound and you put it in water, it will break apart into two ions. If one of those ions is H+, the solution is acidic. If one of the ions is OH-, the solution is basic. There are other ions that make acidic and basic solutions, but we won't be talking about them here.

33. ACIDBASE

34. Neutral Pure water contains small, but equal amounts of ions: H+ and OH- On the pH scale the number is 7