Unit 2 part 2 - Atomic radii and ionization energy Flashcards
21MAR25 P 291-99 (19 cards)
What does the periodic law state?
That after certain regular but varying intervals, the chemical elements show an approximate repetition in their properties
What is the position of an element in the periodic table based on?
The sublevel of the highest - energy electron in the ground state form
Groups?
Columns
Periods?
Rows
Where are metals found?
Left hand side of the table in the s block, central d block, and island of f block
Where are non metals found?
Upper right hand side of p block
What are metalloids?
Elements that have characteristics of both metals and non-metals
What do metalloids look like?
Mainly resemble metal
What do metalloids chemically have more in common with?
Non metals
Group 1?
Alkali metals
Group 17?
Halogen
Where are transition metals?
D block
Group 18?
Noble gases
What does the period of an element give?
The number of occupied energy levels
Two ways to calculate radius?
- Bonded diameter
AKA covalent radius - Non-bonded diameter
AKA Vander walls radius
Ionization energy down a column?
- Electrons are in higher energy levels and further from nucleus meaning they experience greater shielding from electrons
- Atomic radius increases
Ionization energy across a period?
- Atomic radii = decreasing
- Zeff increases across a row
= This pulls valence electrons together making it harder to remove
Why is there a larger jump between Ne and Na?
B/c as we move to the next row of the periodic table energy levels are being added
- Higher energy levels are further from the nucleus and easier to
remove
Pairing energy?
Paired electrons that require energy when paired in same orbital
- Can overcome a larger effective charge from the nucleus which results in lower ionization energy
