Periodic Trends Flashcards
Nuclear charge
+ pull in on electrons from the nucleas
Group
Trends that increase or decrease as u move down a group on the PT
Shielding effect
There is a reduced pull on valence electrons because of the number of electrons between the nucleus and the valence shell
Atomic radius
Size of the atom
Periodic trend for atomic radius
Why
Decrease from left to right
A greater nuclear charge pulls the electrons closer than a weaker nuclear charge
Group trends atomic radius
Why
Increases in size from top to bottom
Each row has another layer of electrons adding to the shielding affect (reduces the pull from the nucleas on valence electron)
Ionization energy
Amount of energy needed to remove an electron from the orbitals (stealing an electron)
High energy
Hard to take electron
Low energy
Easier to take electron
Ionization energy periodic trend
Increase (gets harder to steal an electron)
Nuclear charge increase moving electrons closer to nuclear and holding them more firmly
Group trend ionization energy
Decrease (easier to steal electron)
Each period adds another layer of electron which decrease the pull from the nucleas
Electronegativity
The ability of an atom in a molecule to attract electrons to itself in a chemical bond
Electro negativity periodic Trend
Increase (more likely to steal an electron)
Increase in nuclear charge increase the pull on all electrons
Group trends Electronegativity
Decrease (less likely to take electron)
Shielding effect reduces pull on all electrons
Electron affinity
Amount of energy needed to add an electron to an atom (easy low energy hard high energy)
