1. Inorganic Chemistry Notes

2. Physical & Chemical Changes

3. Phases of Matter

4. Structure of an atom

5. Chemical Bonding

6. Chemical bond – force that joins atoms to form a stable substance
Compound – substance made of the joined atoms of two or more different elements
identified by a chemical formula Ex. CO2, H2O, C6H12O6, NaCl

7. Types of Chemical Bonds
Covalent bonds – when atoms share electrons to form molecules Ex. H2O
Ionic bond – formed when ions of opposite charge interact (are attracted to each other) Ex. NaCl
Ion – atom or molecule that has gained or lost one or more electrons
Cation (aka. positive ion) – has lost electrons, i.e. : K+, Na+, Ca2
Anion (aka negative ion) – has gained electrons, i.e. Cl¯, F¯, O2¯

9. Types of Chemical Bonds
Hydrogen bonds – Weak attractions between polar molecules (i.e. water)

10. Mixtures

11. Mixtures
Mixtures - combination of substances that can be separated into its individual substances by appropriate physical changes
Homogenous mixture – completely uniform in composition, its components are not distinguishable
Heterogenous mixture - not uniform in composition, its components are distinguishable; Ex. Salad dressing, concrete

12. Mixtures
Homogenous mixture – completely uniform in composition, its components are not distinguishable
Solution - type of homogeneous mixture in which solutes are dissolved in a solvent; Ex. Air, seawater
Suspension – type of homogenous mixture in which particles are suspended in another substance; ex. blood, river water

13. SECTION 2 – WATER AND SOLUTIONS

14. 70% of your body is made of water
Water in Living Things
70% of your body is made of water
2/3 of the molecules in your body are water molecules
cells are filled with water and surrounded by water
water is known as the “universal solvent”
Solvent - the substance that dissolves the solute when making a solution
Solute - the substance that is being dissolved when making a solution

15. 10 Properties of Water

16. Water is inorganic—because it does not contain carbon, H2O
Water has a set molecular
structure— H2O
3. A Water molecule is held
together by covalent bonds
4. Water molecules are held to
each other by hydrogen bonds
+/- charge

17. Water has a high specific heat
5. Water is polar - because of its uneven distribution of charge; results in most of the other unique properties of water
Polar molecules (like water) dissolve polar and ionic molecules
(“like dissolves like”)
Nonpolar molecules do not dissolve well in water
Important in membrane structure and function
Water has a high specific heat
Water heats slowly and retains heat longer than many other substances
Important in helping organisms maintain body temperature through evaporation of water, which carries the heat away O _ H H + +

18. 7. Cohesion and adhesion
Water’s polar nature makes it exhibit both cohesion and adhesion
Cohesion – attraction between water molecules (hydrogen bonds)
causes surface tension
causes drops of water to form
Adhesion – attraction between a water molecule and another substance
causes substances to get wet
causes capillary action

19. Adhesion – things get wet
Cohesion – surface tension
Adhesion – capillary action
Cohesion

20. liquid water has a density of 1 g/ml - In general, solid water is less dense than liquid water

22. Periodic Table Number of Protons? Number of Neutrons? Atomic Mass?
Atomic Number?

23. Acids and Bases

24. Acid – compound that forms hydrogen ions in water
Base – compound that forms hydroxide ions in water, or removes hydrogen ions from water
pH—(stands for pondus hydrogenii meaning “potential hydrogen”) a value used to express the acidity or alkalinity of a solution

25. pH scale – measures the concentration of hydrogen ions in solutions; scale of 0 to 14
0 to 6.9 is acidic
7.0 is neutral
7.1 to 14 is basic or alkaline
a solution of pH of 3 has 10 times more hydrogen ions than one with a pH of 4

27. Neutralization - the reaction of an acid with a base, so called because the properties of both the acid and base are diminished or neutralized.
Buffer - a solution that resists changes in pH when moderate amounts of acids or bases are added to it.
Is your whole body at a pH of 7, or does the pH change from one place to another? What do you think is the purpose of this arrangement?
Answer – It changes, not just within a body but within a cell, too. The purpose is to create unique environments, each with a specific purpose. For example, enzymes in the stomach are only functional at a pH between 1 and 2 to prevent them from digesting the body.