What is the effect of increased nuclear charge on atomic radius (across a period)?
Decreases atomic radius due to stronger attraction between nucleus and electrons.
What is the effect of adding electron shells on atomic radius (down a group)?
Increases atomic radius because valence electrons are farther from the nucleus.
What is the effect of losing electrons on ionic radius?
Decreases ionic radius due to reduced electron-electron repulsion.
What is the effect of gaining electrons on ionic radius?
Increases ionic radius due to increased electron-electron repulsion.
What is the effect of increased atomic size on electronegativity (down a group)?
Decreases electronegativity because the nucleus is farther from bonding electrons.
What is the effect of increased nuclear charge on electronegativity (across a period)?
Increases electronegativity because the nucleus has a stronger attraction for electrons.
Define 'Effective Nuclear Charge (Zeff)'
The net positive charge experienced by an electron in an atom, considering shielding effects of inner electrons.
Define 'Atomic Radius'.
The distance between the nucleus and the valence electrons of an atom.
Define 'Ionic Radius'.
The distance between the nucleus and the valence electrons of an ion.
Define 'Electronegativity'.
The ability of an atom to attract electrons in a chemical bond.
What is a 'Period' in the Periodic Table?
A horizontal row of elements in the periodic table; elements in the same period have the same number of electron shells.
What is a 'Group' in the Periodic Table?
A vertical column of elements in the periodic table; elements in the same group have the same number of valence electrons.
Compare atomic radius trend across a period vs. down a group.
Across a period: Decreases | Down a group: Increases
Compare electronegativity trend across a period vs. down a group.
Across a period: Increases | Down a group: Decreases
Compare the size of a cation to its parent atom.
Cation: Smaller due to loss of electrons and reduced electron-electron repulsion. | Parent Atom: Larger.
Compare the size of an anion to its parent atom.
Anion: Larger due to gain of electrons and increased electron-electron repulsion. | Parent Atom: Smaller.
Differentiate between nuclear charge and effective nuclear charge.
Nuclear charge: Total positive charge of the nucleus due to protons. | Effective nuclear charge: Net positive charge experienced by an electron, accounting for shielding.
