Chapter 2: The Periodic Table Flashcards
What are periods?
- Rows
- Same principle energy level, n
What are groups?
- Columns
- Same valence electron configuration
Where are the valence electrons of the lanthanide and actinide series?
s and f subshells
What are metals? Where are they found?
- Shiny (lustrous, except for mercury), conduct electricity well, and are malleable and ductile;
easily give up their electrons - Metals are found on the left side and middle of the Periodic Table.
What are non-metals? Where are they found?
- Dull, poor conductors of electricity, and are brittle.
- Nonmetals are found on the right side of the Periodic Table.
What are metalloids? Where are they found?
- Possess characteristics of both metals and non-metals and are found in a stair-step pattern starting with boron.
What is the effective nuclear charge (Zeff)?
The net positive charge experienced by electrons in the valence shell and forms the foundation for all periodic trends.
How does Zeff change from left to right in a period?
Increases
How does Zeff change from top to bottom in a group?
Little change
What is the atomic radius?
The size of a neutral element
How does the atomic radius change from left to right in a period?
Decreases
How does the atomic radius change from top to bottom in a group?
Increases
What is the ionic radius?
The size of a charged species
Are cations generally smaller or larger than their corresponding neutral atom? Where are they located?
- Smaller
- Metals close to the metalloid line
Are anions generally smaller or larger than their corresponding neutral atom? Where are they located?
- Larger
- Non-metals close to the metalloid line
What is the ionization energy?
The amount of energy (endothermic) necessary to remove an electron from the valence shell of a gaseous species
How does the ionization energy change from left to right in a period?
Increases
How does the ionization energy change from top to bottom in a group?
Decreases
What happens if you remove a subsequent electron after attaining a noble gas-like configuration?
Removing the subsequent electron will cost much more energy
What is electron affinity?
The amount of energy released (exothermic) when a gaseous species gains an electron in its valence shell
How does the electron affinity change from left to right in a period?
Increases
How does the electron affinity change from top to bottom in a group?
Decreases
What is electronegativity?
measure of the attractive force of the nucleus for electrons within a bond
How does the electronegativity change from left to right in a period?
Increases
How does the electronegativity change from top to bottom in a group?
Decreases
What oxidation state do alkali metals take?
- +1
- To lose an electron and gain a noble gas-like configuration
What oxidation state do alkali metals take?
- +2
- Lose two electrons to achieve a noble gas-like configuration
What oxidation state do chalcogens take?
- -2 (metals) or +6 (non-metals)
Which group is biologically important?
Chalcogens
What oxidation state do halogens take?
- -1
- Highest electronegativities
Which groups has the highest ionization energies and virtually non-existent electronegativities?
Noble gases
What explains the ability of transition metals to form colorful complexes with non-metals in solution?
The fact that they take on multiple oxidation states
