Ionization Energy and Electron Affinity
Ionization energy ____________ from left to right across the periodic table.
Increases
Atomic radius _______ from left to right across a period.
Decreases
Shiny, hard, dense, good conductor of heat and electricity, solids at room temp (except Hg), ductile, malleable
The original periodic table was arranged by
similar properties
The ability of an atom to attract electrons from another atom.
Electron affinity __________ down a group
Decreases
Atomic radius ______ down a group.
Increases
Give one property of a nonmetal
Dull, not ductile, not malleable, not good conductor of heat and electricity, most are gases at room temperature
Who created the first periodic table?
Dmitri Mendeleev
Put the following elements in order of increasing electronegativity: Y, Cl, Ni, P
Y < Ni < P < Cl
The higher ionization energy between Mn and P
P
Put the following elements in order of increasing atomic radii: Ca, F, Fe, Al
F < Al < Fe < Ca
Metals are located on the ______ side of the periodic table.
Left
increasing atomic number
Put the following elements in order of effective nuclear charge (Zeff): F, C, B, Li
Li < B < C < F
The lower electron affinity between Be and Sr
Sr
Which is bigger, a parent atom or an anion?
Nonmetals are located on the _______ side of the periodic table.
Right
Who created the modern periodic table?
Henry Mosely
Increases, increase slightly
Give the definitions of both ionization energy and electron affinity
Electron affinity is the energy change when an atom gains an electron.
Parent atom
List the six metalloids
Boron, silicon, arsenic, tellurium, germanium, antimony
What element spots were left empty on the original periodic table?
Ga and Ge
Effective nuclear charge takes into account two things. What are they?
The pull of the nucleus on the valence electrons and the screening electrons repelling the valence electrons.