Exam Prep Flashcards
(10 cards)
What is atomic radius?
The distance from the nucleus to the outermost electron shell.
How does atomic radius change across a period?
It decreases because the nuclear charge increases, pulling electrons closer.
How does atomic radius change down a group?
It increases due to the addition of electron shells.
What is ionization energy?
The energy required to remove one electron from a gaseous atom.
What is the trend for ionization energy across a period?
It increases due to a stronger attraction between the nucleus and electrons.
What is the trend for ionization energy down a group?
It decreases as electrons are farther from the nucleus and more shielded.
What is electronegativity?
An atom’s ability to attract shared electrons in a chemical bond.
What is the trend for electronegativity across a period?
It increases due to increased nuclear charge and effective nuclear attraction.
What is the trend for electronegativity down a group?
It decreases due to greater atomic size and more shielding.
What is effective nuclear charge (Zₑff) and its impact?
It’s the net positive charge felt by valence electrons; increases across a period and causes smaller radii and higher ionization energy.
