Atomic Radius
Ionization Energy
Electronegativity
Electron Affinity
Element Symbols
100
On the Periodic Table, atomic radius does this as you move down a group.
What is "increases"?
100
The energy needed to do this to an atom while in the gaseous state.
What is "remove an electron"?
100
Electronegativity is the ability of an atom to attract electrons toward itself in this.
What is "a chemical bond"?
100
Electron affinity is a measure of the energy absorbed when an electron is added to a neutral atom to form this.
What is "a negative ion"?
100
"F"
What is "Fluorine"?
200
Atomic radius is half the distance between the nuclei of two like atoms in this type of molecule.
What is "a diatomic molecule"?
200
The 1st Ionization Energy is the energy it takes to remove this many electrons.
What is "one electron"?
200
Electronegativity increases going this direction on the Periodic Table.
What is "left to right"?
200
The more negative the value, the more this the ion is.
What is "stable?"
200
"Ma"
What is "Manganese"?
300
The size trend in horizontal periods is less prominent than in vertical groups because of this effect.
What is "the electron shielding effect"?
300
This distance between two atoms is a factor affecting Ionization Energy.
What is "atomic radius"?
300
Going down a group, electronegativity does this.
What is "decreases"?
300
Electron affinity is virtually the opposite of this.
What is "ionization energy"?
300
"Er"
What is "Erbium"?
400
There are more electrons in these energy levels, thus the atomic radii increase.
What are "principal energy levels"?
400
Atoms that are smaller cling to these tighter, thus having higher ionization energy.
What are "valence electrons"?
400
These are increasingly distant from the attraction of the nucleus.
What are "bonding electrons"?
400
Atoms that have a more negative electron affinity are more attracted to these.
What are "extra electrons"?
400
"Sb"
What is "Antimony"?
M
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