| A | B |
|---|
| Define Ionization Energy | The energy needed to remove an electron from a gaseous atom. |
| When moving down a group of the periodic table, what happens to atomic size? | It increases |
| When moving across a period of the periodic table from left to right, what does atomic size generally do? | decrease |
| What is the difference between an ion and an atom? | An ion can be negative or positive while an atom is always neutral. |
| Define Electronegativity. | The tendency for an atom to attract electrons to itself when it is chemically combined with another element. |
| How many electrons are there in the outer shell of the most stable electron configuration? | eight |
| What is the name of the group on the periodic table with the most stable electron configuration? | Noble Gases |
| Define electron affinity. | The energy change that accompanies the addition of an electron to a gaseous atom. |
| Does ionization energy increase or decrease with atomic number within a period? | Increase |
| Does ionization energy increase or decrease with atomic number within a group? | Decrease |
| Does electronegativity increase or decrease with atomic number within a period? | Increase |
| Does electronegativity increase or decrease with atomic number within a group? | Decrease |
| Which group of elements has the most negative electron affinities? | Halogens |
| What are atoms trying to accomplish when they bond? | To become more stable |
| Are molecules made up of atoms that are bonded ionically or covalently? | Covalently |
| Ionically bonded substances are made up of what? | Ions |
| Define valence electrons | Electrons in the highest occupied energy level of an element's atoms. |
| Are covalent or ionic compounds usually crystalline solids? | Ionic |
| Do most ionic compounds have high or low melting points? | High |
| What does "most stable" mean in terms of energy? | Lowest energy |
