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Unit 10: Periodic Table and Trends
Guiding Questions:
- Why is the periodic table so important?
- Why is the periodic table shaped the way it's shaped?
- Why do elements combine? Why do elements react?
- What other patterns are there in the world and how do they help us?
What you should learn:
- When elements are listed in order according to the number of protons, repeating patterns of physical and chemical properties result and can be used to make predictions
- The ability to create a model and then make predictions that prove to be correct, based upon that model, is what science is all about.
More Specifically...:
IB Objectives: SL
HL
- Trends - Physical Properties
- Associate rows with periods and columns with families or groups.
- Identify the seven diatomic gases
- Give locations and list characteristic properties of metals, non-metals, metalloids, and noble gases.
- Label the following areas on a periodic chart
- a. Alkali metals
- b. Alkaline Earth Metals
- c. Transition Metals
- d. Metalloids
- e. Halogens
- f. Noble gases
- g. Lanthanides
- h. Actinides
- Trends - Chemical Properties
- Define and give the general trends on the periodic table forthe following properties for alkali metals (Li to Cs), halogens (F to I, and period 3 elements (Na to Ar)
- a. Ionization energy
- b. Electronegativity
- c. Atomic radius / Ion radius
- d. Electron affinity
- e. Reactivity
- i. Of alkali metals (Li, Na, K) with water and halogens (Cl2 and Br2)
- ii. Of Halogens (Cl2, Br2, I2) with halid ions (Cl-1, Br-1, I-1)
- iii. Of halide ions with silver ions
- f. Atomic Number
- g. Melting point
- h. Electron configurations
- i. Intermolecular forces
- j. kind of bonding
- k. Change in nature from metallic to non-metallic
- l. Change from basic to amphoteric to acidic oxides and their reaction with water for period 3
- Define ionization energy as the minimum energy requires to remove one electron from an isolated gaseous atom
- Define shielding effect and use it to explain trends in families
- Define effective nuclear charge and use it to explain trends in periods
- Predict location on periodic table given ionization energy data
- Explain zig-zag of ionization energy diagram in terms of nuclear charge, shielding, Hund's rule.
- Deduce relationship between electron configuration and position in the periodic table
- State that the noble gas configuration is the most stable electron configuration
- Predict oxidation states for various elements based on their proximity to a noble gas in the periodic table
- Write electron configurations and orbital diagrams of ions
- Explain why there are multiple oxidation states
Lecture Notes:
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