Chemistry 2 Wiki | RecentChanges | Preferences
Essential Question: Do you believe that? (theory explains observations)
Each student will be able to:
- Explain the difference between Medeleev and Moseley's Periodic Table. [3.1]
- Explain the relationship of an element's position on the Periodic Table to its atomic number (i.e. Periodic law)[3.1](3.1).
- Describe the Modern Periodic Law
- Define Isoelectronic species and determine them for an element or ion.
- Relate the position of an element on the Periodic Table to its Electron Configuration.[3.2](3.3).
- Relate the chemical charateristics (reactivity) to the Family elements and how Electron configuration detemines it.(3.3)
- Give appropriate Elements for the Groups, Periods, and other designated elements including metals, non-metals, and metalloids (semi-metals). [3.2](3.1,3.2).
- Describe what Coulombic force (both attractive & repelsion) and the two major factors that affect the strength of the Coulombic Force (charge on the nucleus & electron).
- Define covalent atomic radius, van der Waals radius, and atomic radius in metals. State and explain why (using Coulombic force, C.F.) how the atomic radii changes as you go down a Group and across a Period. [3.4](3.4).
- Define 1st Ionization Energy (IE) and give the trends for IE as you go down a Group and across a Period. Be able to explain the trend using C.F.(not Shielding effect). Also, state the two Exceptions for Period 2 & 3 (2 for each period). [3.4](3.4).
- Define Higher Ionization Energies (IE) and explain how they can explain the charge on the element's ion. (i.e. Al3+) [3.4]
- Define Electronegativity (EN) and state(including why using C.F.)the general trends as you go down a Group and across a Period. [3.4](3.4)
- Explain how the ionic radius compares to the atomic radius for Metals and then for Non-metals. 'DO NOT usually explain general trends across Period'. Down a Group is same as Atomic radii. [3.4](3.4)
- State the difference between Metals and Non-metals for the characteristics of IE,EN,Luster, Deformability,heat/electrical conductivity, charge, and phase (at room temp). [3.4].
- State and explain why (using other trends)the trends for Metallic Characteristics as you go down a Group and across a Period. [3.4].
Students need to be able to define (most are also stated above):
- Modern Periodic Law
- Period / Row
- Group / Family / Column
- Coulombic Force
- Ionization Energy (IE)
- Higher IE
- Covalent atomic radius
- van der Waals radius
- Atomic radius in metals
- Isoelectronic species
- Shielding Effect
- Malleable and ductile and deformability
Students need to be able to locate the following on the Periodic Table
- Period,Group,Alkali metal, Alkaline Earth metals, Transition Elements, Inner Transition Elements,Lanthanoid series, Actinoid series, Noble or Inert Gases, Halogen, Nitrogen Family, Oxygen Family, metals, non-metals, semi-metals or Metalloids, (s-,p-,d-,f-block elements), phase of elements @20degreeC.