Chapter 2 - Periodic Table Flashcards
Periods
Rows
- Based on same principal energy level, n
Groups
Columns
- Same valence shell electron configuration
Metals
Shiny (lustrous), conduct electricity well, and are malleable and ductile
- Left side and middle of table
Nonmetals
Dull, poor conductors of electricity, and are brittle
- Right side of table
Metalloids
Characteristics of both metals and nonmetals
- Stair pattern starting with element B
Effective Nuclear Charge (Zeff)
Net positive charge experienced by electrons in the valence shell and forms the foundation of all periodic trends
- increases from left to right
Atomic Radius
Average distance between a nucleus and its outermost electron
- Increases down and left (opposite of other trends)
Ionic Radius
Size of a charged species
- Cations smaller than neutral
- Anions larger than neutral
Ionization Energy (IE)
Amount of energy necessary to remove an electron from the valence shell of a gaseous species
- Increases from left to right
- Decreases from top to bottom
Electron Affinity
Amount of energy released when a gaseous species gains an electron in its valence shell
- Increases from left to right
- Decreases from top to bottom
Electronegativity
Measure of the attractive force of the nucleus for electrons within a bond
- Increases from left to right
- Decreases from top to bottom
Alkali Metals
Typically take on an oxidation sate of +1 and prefer to lose an electron to achieve a noble gas-like configuration
- Most reactive of all metals
Alkaline Earth Metals
Take on oxidation state of +2 and can lose 2 electrons to achieve noble gas-like configurations
Chalcogens
Take on oxidation states of -2 or +6
Noble Gases
Fully filled valence shell in their standard state and prefer not to give up or take on additional electrons
- Very high IE
- Virtually nonexistent electronegativities and affinities
Halogens
Take on oxidation state of -1 and prefer to gain an electron
- Highest electronegativity
Transition Metals
Take on multiple oxidation states
