AP Chem Unit 1 Tough Stuff

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Atomic radius

Distance from nucleus to outermost electron

Effective nuclear charge

Net positive charge “felt” by an electron after shielding by inner electrons (I don’t get this either)

Ionization energy

Energy required to remove an electron

As ionization energy increases, atomic radius…

decreases

Electron affinity

Energy change when gaining an election → actual change

As electron affinity increases, atomic radius…

decreases

Electronegativity

Atom’s ability to attract electrons in a bond → relative pulling power

As electronegativity increases, atomic radius…

decreases

Removing an electron from a stable arrangement requires _______ ionization energy

more

Electron repulsion

Repulsion between electrons in orbitals

As electron repulsion increases, atomic radius…

increases

As electron repulsion increases, ionization energy…

decreases (electrons fighting → want to LEAVE)

Binding energy

Energy holding electron to the nucleus

Valance electrons have a _______ binding energy

lower

Core electrons have a _______ binding energy

higher

As binding energy increases, ionization energy…

increases

As binding energy increases, effective nuclear charge…

increases

As binding energy increases, atomic radius…

decreases (more coulombic attraction!)

Smaller atoms (lower atomic radius, higher effective nuclear charge) generally have a ______ ionization energy, electronegativity, binding energy, and electron affinity

higher → more tightly held together

Larger atoms (higher atomic radius, lower effective nuclear charge) generally have a _______ ionization energy, electronegativity, binding energy, and electron affinity

lower → electrons loosely held together

As we go left to right across a period, what happens to ionization energy, atomic radius, electron affinity, and electronegativity?

IE → increases

AR → decreases

EA → increases

EN → increases

As we go top to bottom across a group, what happens to ionization energy, atomic radius, electron affinity, and electronegativity?

IE → decreases

AR → increases

EA → decreases

EN → increases

More protons generally means a _______ effective nuclear charge

higher

A larger atomic radius generally signifies a _______ effective nuclear charge

lower

Any element that as less than _______ valence electrons gives away an electron (ionic charges)

4

The _______ element in an ionic bond gains electrions

nonmetal

The most _______ element in an ionic bond gains the electrons

electronegative

A positive cation is _______ than its parent atom because it has lost a…

smaller, valence shell

A negative anion is _______ than its parent atom because…

larger, electrons added to same valance shell = greater electron-electron repulsion = larger AR

Noble gas configurations are…

stable

When electrons are removed from an atom to form a cation, they are removed from the _______ energy shell

highest