Powerpoint 6 Flashcards
What are the two key exceptions to orbital filling?
4s fills before 3d due to energy differences.
d orbitals are one energy level behind, and f orbitals are two levels behind.
How do electron configurations change for Cations?
Remove from the highest energy level (n) first.
How do electron configurations change for anions?
Add extra electrons.
What is atomic radius?
The distance from the nucleus to the outermost valence electron.
What happens to atomic radius down a group?
Increases because new energy levels (n) are added.
What happens to atomic radius across a period?
Decreases due to increased nuclear pull (more protons attract electrons closer).
What three factors affect atomic radius?
More protons = Smaller radius (stronger nuclear pull).
Electron repulsion = Larger radius.
Shielding effect = Inner electrons block nuclear pull.
What happens to atomic size when an atom loses electrons (forms a cation)?
The radius decreases because:
Fewer electrons → Less repulsion.
Higher nuclear pull on remaining electrons.
What happens to atomic size when an atom gains electrons (forms an anion)?
The radius increases because:
More electrons → More repulsion.
Nuclear pull is spread over more electrons.
What is ionization energy?
The energy required to remove an electron from an atom.
How does ionization energy change across a period?
Increases across a period (harder to remove electrons).
How does ionization energy change down a group?
Decreases down a group (easier to remove electrons).
Why does ionization energy jump after removing certain electrons?
A large jump occurs when trying to remove a core electron instead of a valence electron.
What is electron affinity?
The energy released when an atom gains an electron.
What is the trend for electron affinity across a period?
Increases across a period (stronger attraction, except noble gases).
What is the trend for electron affinity down a group?
Decreases down a group (weaker attraction for electrons).
What is electronegativity?
The ability of an atom to attract electrons in a bond.
How does electronegativity change across a period?
Increases across a period (stronger pull).
How does electronegativity change down a group?
Decreases down a group (weaker pull).
