Test Review: Periodic Trends & Electrons

Learning Standards 11-14

  1. Explain the use of chemical and physical properties in the historical development of the Periodic Table. (Think Mendeleev)
  2. Use the Periodic Table to identify and explain the properties of chemical families, including alkali metals, alkaline earth metals, halogens, noble gases, and transition metals.
  3. Use the Periodic Table to identify & explain periodic trends including atomic & ionic radii, electronegativity, & ionization energy.
  4. Express the arrangement of electrons in atoms through electron configurations & Lewis valence electron dot structures.
  1. Essential Vocabulary

You should be familiar with the following vocabulary.

Energy level

Sublevel

Atomic orbital

Periodic law

Periodicity

Chemical family

Representative element

Alkali metal

Alkaline earth metal

Main group metal

Transition metal

Inner transition metal

Halogen

Noble gas

Electron configuration

Aufbau principle

Hund’s rule

Pauli exclusion principle

Periodic trend

Atomic radius

Ionic radius

Electronegativity

Ionization energy

Effective Nuclear Charge

Shielding

  1. Periodic Table Basics
  1. Who conceived of and created the first periodic table of elements?
  2. By what two metrics did he arrange the elements in his table?
  3. He predicted the discovery of several elements, and even described some of their physical and chemical properties. Gallium was one of those elements. The predictions that he made about gallium were based on which element?
  4. Classify the following as Metals, Nonmetals, or Metalloids:

  1. Potassium
  2. Silicon
  3. Sulfur

  1. Name the group to which the following elements belong (Alkali Metals, Alkaline Earth Metals, Halogens, Noble Gases):
  2. Fluorine
  3. Magnesium
  4. Argon
  5. Cesium
  6. To what larger category does each of the following elements belong? {Representative Elements, Transition Metals, Inner Transition Metals}
  7. Uranium
  8. Carbon
  9. Iron
  10. How many energy levels contain electrons for the following neutral atoms?

(Occupied energy level = period number)

  1. Helium
  2. Zinc
  3. Aluminum
  1. How many valence electrons are found in neutral atoms of the following elements?

(Valence electrons = Group A number)

  1. Phosphorus
  2. Bromine
  3. Lithium
  4. Boron
  1. How are elements with similar properties arranged on the periodic table?

III.Periodic Trends

  1. Define shielding
  2. State the trend for shielding
  1. Across a period
  2. Down a group
  1. Define atomic radius
  2. State the trend for atomic radius
  3. Across a period
  4. Down a group
  5. Explain the trends for atomic radius at the atomic level.
  6. Define electronegativity
  7. State the trend for electronegativity
  8. Across a period
  9. Down a group
  10. Explain the trends for electronegativity at the atomic level.
  11. Define ionization energy
  1. State the trend for ionization energy
  2. Across a period
  3. Down a group
  4. Explain the trends for ionization energy at the atomic level
  5. Define reactivity
  6. State the trend for reactivity of metals
  7. Across a period
  8. Down a group
  9. State the trend for reactivity of nonmetals
  10. Across a period
  11. Down a group
  12. Explain the trends for reactivity at the atomic level.
  13. How does the ionic radius of a metal cation compare to its neutral atom? Explain.
  14. How the ionic radius of a nonmetal anion compare to its neutral atom? Explain.
  15. Arrange the following ions in order of increasing size.
  16. K +, Fe +3, Ca +2
  17. Cl -, Br-, F-
  1. Electron Configuration
  1. Define principle energy level/quantum number. How is principle energy level related to position on the periodic table?
  2. How many and what type of sublevels are in each principal energy level?

  1. 1
  2. 2
  3. 3
  4. 4

  1. How many orbitals can be found within each sublevel?

  1. s
  2. p
  3. d
  4. f

  1. How many electrons can be found within a single orbital?
  2. How many electrons can be found within each sublevel?

  1. s
  2. p
  3. d
  4. f

  1. How many electrons can be found within each principal energy level?

  1. 1
  2. 2
  3. 3
  4. 4

  1. Define Aufbau principle.
  2. State the Pauli Exclusion Principle.
  3. State Hunds Rule.
  1. Write unabbreviated and abbreviated electron configurations of neutral atoms:
  2. V
  3. C
  4. Rb
  5. For each of the atoms in #35, identify the energy level of the highest energy electrons.
  6. For each of the atoms in #35, identify the energy level of the OUTERMOST electrons.
  7. Write non-core orbital notation for atoms in question number 35.
  8. Identify atoms based on their electron configurations:
  9. 1s22s22p63s23p1
  10. 1s22s22p63s23p64s23d6
  11. Define valence electrons. How is the number of valence electrons for the representative elements related to position on the periodic table?