1. Chapter 2 Of Atoms and Molecules: Chemistry Basics

2. All organisms consist of matter and energy. LIFE- based on chemical principles. MATTER – The basis for everything

3. A. Matter Material that takes up space. Matter broken down to pure substances- Elements 1. Elements Pure chemical substances composed of atoms. Examples? Oxygen, sodium, copper, potassium How many elements exist? (92)

4. How many of these elements are essential to life? (25) The essential elements are divided into: Bulk elements: needed in relatively large amounts Examples: C, O, H, N Trace elements: needed in relatively small amounts Examples: Fe, K, Na, Zn, Ca

5. Periodic Table of Elements

7. 2. Atom The smallest “piece” of an element that retains the characteristics of that element. Composed of 3 subatomic particles: Protons Neutrons Electrons

8. Atoms of each element – characteristic number of protons # of protons – determines size and character of each atom. Charge- attraction between opposite types of particles. Atom – electrically neutral Electron – small compared to proton and neutron Orbital- location for an electron relative to its nucleus.

9. Element – has a symbol. He- Helium Na- Sodium Atomic number- shows the # protons in the atom- identity of the atom. Elements are arranged sequentially in the periodic table by atomic number.

10. Characteristics of Subatomic Particles

11. Atomic number # protons in nucleus of an atom (establishes identity of the atom) Since most atoms are electrically neutral, atomic number indicates # of electrons as well. Atomic mass # protons plus # neutrons in nucleus of an atom

12. Periodic table information on carbon: Atomic mass given in table is average mass of all the element’s isotopes.

13. How can we determine the number of neutrons in an atom? # neutrons = atomic mass - atomic # Determine # neutrons in a carbon atom (atomic mass = 12; atomic # = 6). # neutrons = 12 - 6 = 6 Do all carbon atoms have the same number of protons? Do all carbon atoms have the same number of neutrons?

14. Isotopes Atoms having the same number of protons, but differing numbers of neutrons. Same charge & characteristics but different masses. Often one isotope is very abundant and others are rare. If an isotope is unstable, it is termed radioactive Ex. Carbon isotopes carbon 12 ( 12 C)  6 neutrons carbon 13 ( 13 C)  7 neutrons carbon 14 ( 14 C)  8 neutrons

15. 3. Compound A pure substance formed when atoms of different elements bond. The number of atoms of each element is written as a subscript. Examples: CO 2 carbon dioxide H 2 Owater CH 4 methane C 6 H 12 O 6 glucose Atoms bound together – molecules

16. 4. Molecule Smallest piece of a compound that retains characteristics of that compound. The number of molecules is written as a coefficient. Examples: 4CO 2 4 molecules of carbon dioxide 2C 6 H 12 O 6 2 molecules of glucose 6O 2 6 molecules of oxygen

17. Chemical Reactions The reactants of a reaction are written to the left of the arrow. The products of a reaction are written to the right of the arrow. Example: 6O 2 + C 6 H 12 O 6  6H 2 O + 6CO 2 + energy

18. 5. Chemical Bonds Type of bond formed is determined by the number of valence electrons in the interacting atoms [octet rule]. The goal of chemical bonding is for all atoms involved to complete or eliminate their outer electron shells.

20. a) Covalent bonds - form when atoms share electron pairs. strongest type of bond tend to form when atoms have 3, 4 or 5 valence electrons the number of electron pairs shared determines whether the covalent bond is single, double or triple can be nonpolar or polar

22. Nonpolar covalent bonds - electrons are shared equally between atoms. Ex. methane

23. Types of diagrams to represent molecules

24. Polar covalent bonds - electrons are not shared equally. They are drawn more strongly to 1 atom’s nucleus than the other. Form when less electronegative atoms bond with more highly electronegative atoms. Ex. water

25. b) Ionic bonds - form when oppositely charged ions are attracted to each other. weaker than covalent bonds atoms with 1, 2 or 3 valence electrons give up electrons to atoms with 7, 6 or 5 valence electrons which forms ions form salts which break apart in water Ex. NaCl

26. c) Hydrogen bonds - form when opposite charges on two molecules are attracted to each other. weakest type of bond* Ex. DNA H2OH2O

27. 6. Attractive forces van der Waals attraction Attraction between molecules or within molecules that occur when oppositely charged regions approach each other Often used to shape molecules

28. Interactions with water hydrophobic: parts of a molecule that do not have charges cannot interact with water hydrophilic: parts of a molecule that have charges can interact with water

29. B. The Importance of Water 1. Properties Cohesion - the attraction of water molecules for each other. Adhesion - the attraction of water molecules for other compounds. Imbibition – the tendency to absorb water and swell

30. High heat capacity – takes a great deal of heat to raise the temperature of water. High heat of vaporization - a lot of heat is required to evaporate water. Exists as solid, liquid or gas - solid (ice) is less dense than liquid.

31. 2. Solutions A solution is a mixture of one or more solutes dissolved in a solvent. If solvent is water, then it is an aqueous solution. Water is a strong solvent because it separates charged atoms or molecules.

32. 3. Acids & Bases Acids - substances that add H + to a solution. Bases - substances that remove H + from solution. Buffer systems: help stabilize pH pH scale is measure of acidity/alkalinity based on H + concentration.