1. Chapters 4.3 & 5.1-3 Notes A. Atomic Review B. Ch. 4.3: Modern Atomic Theory C. Ch. 5.1: Organizing the Elements D. Ch. 5.2: The Modern Periodic Table E. Ch 5.3: Representative Groups

2. A. Atomic Review Subatomic particles (p, n, e) Symbols Atomic # Mass # Isotopes

3. Diagram of an atom p – Proton e – Electron n - Neutron

4. B. Ch. 4.3: Modern Atomic Theory Energy levels: the possible energies that electrons in an atom can have (staircase analogy) Electron Cloud: visual model of the most likely locations for electrons in an atom (windmill analogy) Orbital: a region of space around the nucleus where an electron is likely to be found (map of dots analogy) The most stable electron configuration is when electrons are in orbitals with the lowest possible energies.

5. Energy Levels Outer level electrons have more energy. Different levels hold different numbers of electrons.

6. Nucleus Energy Level 1 2 electrons Energy Level 2 8 electrons Energy Level 3 18 electrons

7. C. Ch 5.1: Organizing the Elements How did Mendeleev use solitaire to help him organize 63 elements? Compare and contrast Mendeleev’s periodic table to the table we use today.

8. D. Ch. 5.2: The Modern Periodic Table

9. Families (Groups) and Periods (Rows)

10. Group or Family Trends Up and down; columns Elements in the same group have similar properties (have same # of valence electrons). Group 1, very reactive (only 1 valence electron) Group 8A, not very reactive (has all 8 valence electrons)

11. Row or Period Trends As you go to the right, you add 1 proton and 1 electron. The row ends when there are 8 electrons in the outer energy level Increasing Energy Levels

12. Variation Across a Period From left to right, the elements become less metallic and more nonmetallic in their properties. Na – reacts quickly and violently with water Mg – reacts with hot water Al – doesn’t react with water, but reacts w/oxygen Si – least reactive (except Ar) P & S – normally don’t react w/water, but react w/O and Cl, which is a highly reactive nonmetal. Ar – hardly reacts at all

13. SOME TRENDS OF THE PERIODIC TABLE

14. Periodic Table Trends Electronegativity – measure of attraction for electrons Ex: High electronegativity = strong attraction Ionization energy – energy required to remove an electron Ex: Low ionization E = easy to remove electron Electron affinity – ability of an atom to accept an electron Ex: High electron affinity = good at accepting e - Metallic character – same as atomic radii trend *Atomic radius – see next slide * Reactivity *Oxidation numbers – shows # of e - gained or lost *Valence electrons – see group number *Energy levels – see row number (* = characteristics you need to know)

15. Atomic Radii Pattern

16. Reason for atomic radii pattern? As you move down a group, the radii increases… The number of energy levels increases, and each subsequent energy level is further from the nucleus than the last As you move across a row, the radii decreases… More electrons are added to the same energy level, and more protons are added to the nucleus. Thus, there is a stronger force of attraction pulling the electrons closer to the nucleus.

17. How to draw an Electron Dot Diagram 1. Find element on table. 2. Write symbol. 3. Look at the group number to determine the number of dots. 4. Draw dots. HUND Rule: Every orbital in a subshell is singly occupied w/1 electron before any one orbital is doubly occupied…

19. E. Ch. 5.3: Representative Groups Valence Electron – electron that is in the highest occupied energy level of an atom (outermost energy level) Elements in a group have similar properties because they have the same number of valence e- The number of valence electrons help us predict how atoms will interact with each other (bonding).

20. Representative Groups, cont. Group 1A – Alkali Metals 1 valence electron, very reactive Group 2A – Alkaline Earth Metals 2 valence electrons, harder than alkali Group 4A – Carbon Family 4 valence electrons, metal, nonmetal, metalloid Group 5A – Nitrogen Family 5 valence electrons Group 6A – Oxygen Family 6 valence electrons Group 7A – Halogens 7 valence electrons, highly reactive nonmetals Group 8A – Noble Gases 8 valence electrons, colorless, odorless, unreactive