 Bond radius  Ionization Energy  Electronegativity  Electron Affinity*

 The distance from the center of the nucleus to the outermost energy level  Bond radius – used to measure atomic radius

A. Increases B. Decreases C. Stays the same D. No direct pattern

A. Negative B. Positive C. Neutral D. Depends on the atom

A. Smaller B. Larger C. Same size D. Depends on the atom

 The energy required to remove an electron from the outermost energy level

 Increases as you move from left to right across the periodic table  Why? Stronger attraction between protons and electrons

 Increases as you move up a group  Why? ◦ There are more energy levels as you move down a group ◦ The inner electrons block the force of the protons from the outer electrons  This is called electron shielding

 How much an atom in a molecule attracts electrons  A higher value represents that an atom has a stronger pull on the electrons

 Increases as you move up a group  Why? ◦ Less electron shielding ◦ Outer electrons are closer to the nucleus

 Increases as you move from left to right  Why? ◦ More pull from added protons

A. Energy required to remove an electron from outermost energy level B. Energy required to add an electron to outermost energy level C. Inner electrons blocking the charge of the nucleus from the outer electrons D. Outer electrons blocking the charge of surroundings from the nucleus

A. Energy required to remove an electron from outer most energy level B. Energy required to shield electrons C. The energy cations use when forming bonds D. The energy anions use when forming bonds

A. Fluorine B. Chlorine C. Iodine D. Bromine

A. Lithium B. Beryllium C. Boron D. Fluorine

 The energy gained by a neutral atom when it accepts an electron to become an anion  Increases as you move up a group  Increases as you move left to right