Periodic Table Trends Flashcards
can be understood as chemical property describing an atom’s ability to attract and bind with electrons
electronegativity
energy required to remove an electron from a neutral atom in its gaseous phase
ionization energy
energy change when electron is added
electron affinity
right to left due to valence shell and increased protons, down-up due to shielding
electron affinity and ionization energy
right-left due to protons sucking electrons in as you go right; up-down due to increasing number of orbitals
atomic radius
level of reactivity of a metal. metals tend to lose electrons in chemical reactions.
right to left
nonmetallic character
level of reactivity of a metal. metals tend to lose electrons in chemical reactions.
left to right
metallic character
rows
periods
columns
groups
why do elements in the same group behave similarly
same num. of valence electrons
size of atom
atomic radius
as we go down the periodic table, atomic size ____
increases
because we add shells
as we go to the right, atomic size ______
decreases
because we are moving within a shell and each element to the right has one more proton in the nucleus than the last
electrons repel each other so adding an electron makes an atom bigger
ionic radius
ions with the same electron configuration will have their radii _____ as the atomic number increases
decrease
