Flashcard library · General Chemistry
Chemistry: Periodic Table Trends
Master the essential concepts of periodic table trends with this comprehensive flashcard set. Understand how atomic structure dictates properties like atomic radius, ionization energy, and electronegativity across periods and down groups. Perfect for reviewing core material for exams and building a strong foundation in chemistry.
Want to actually learn these?
Save this deck to your NoteFren library and study it with spaced repetition — or turn your own notes into cards like these.
How does atomic radius change across a period?
It decreases, because rising effective nuclear charge pulls electrons closer.
How does atomic radius change down a group?
It increases, because electrons occupy shells farther from the nucleus.
What is (first) ionization energy?
The energy needed to remove one electron from a gaseous atom.
How does ionization energy change across a period?
It generally increases, as effective nuclear charge rises.
How does ionization energy change down a group?
It decreases, because the outer electrons are farther out and more shielded.
What is electronegativity?
An atom's ability to attract shared electrons in a bond.
How does electronegativity change across a period and down a group?
It increases across a period and decreases down a group; fluorine is the most electronegative.
How does metallic character change across the table?
It decreases across a period and increases down a group.
Is a cation larger or smaller than its neutral atom?
Smaller: it loses electrons, often a whole shell, and the rest are pulled closer.
Is an anion larger or smaller than its neutral atom?
Larger: added electrons increase repulsion and the cloud expands.
How does alkali metal reactivity change down Group 1?
It increases, because the single valence electron is lost more easily.
How does halogen reactivity change down Group 17?
It decreases, because gaining an electron becomes less favorable.
What is effective nuclear charge?
The net positive charge an electron actually feels after shielding by other electrons.
What is electron shielding?
Inner electrons reducing the nucleus's pull on outer electrons.
How many valence electrons do elements in the same main group have?
The same number, which is why they behave alike.