Periodic Trends Flashcards
When layers of electrons reduce the pull from the nucleus
shielding effect
Noble gases do not
have electronegativity
The energy required to remove an electron from the valence shell of an atom
ionization energy
The amount of pull on electrons while in a chemical bond
electronegativity
The amount of positive pull from the nucleus on electrons
effective nuclear charge
Period Trend
any characteristic that changes in a regular position across a row (left to right)
Group Trend
any characteristic that changes in a regular pattern down group (top to bottom)
Atomic radius left to right
decreasing
Atomic Radius top to bottom
increasing
Ionization energy left to right
increasing
Ionization energy top to bottom
decreasing
Electronegativity left to right
increasing
Electronegativity top to bottom
decreasing
Which group on the periodic table has the lowest ionization energy?
alkali metals
Which group on the periodic table has the highest ionization energy?
noble gases
atomic radius
size of an atom
ionization energy
amount of energy needed to remove an electron from the valence shell of an atom
valence electrons
in the highest occupied ānā shell, highest energy s+p electrons
electronegativity
amount of pull on an electron an atom has in a chemical bond
electron affinity
amount of energy needed to add an electron to the valence shell of an atom
what is the atomic radius left to right
the more (+) pull, the smaller the atom gets
what is the ionization energy left to right
the more (+) pull makes it harder to remove electrons
what is the electronegativity left to right
the more (+) pull creates more pull on the outside of the electron
what is the atomic radius top to bottom
more layers make the atom bigger with less pull too
what is the ionization energy top to bottom
more layers create less pull making it easier to remove electrons
what is the electronegativity top to bottom
more layers reduce the pull on electrons to the nucleus
How can we add electrons?
Protons pull electrons into the nucleus, so the more (+) pull there is, the harder it is to remove electrons
How can we remove electrons?
The more layers/shields of electrons there are reduce the (+) pull towards the nucleus, making it easier to remove electrons
How do we lose electrons while going down the PT?
As you go down, the IE decreases creating a lesser (+) pull of electrons making them to be easily removed
How do we gain electrons while going up the PT?
As you go up, the energy levels decrease creating a more (+) pull making it harder to remove electrons
The less pull/more layers?
the bigger the atom gets, the easier to remove electrons, and reduces the ability to steal other electrons
When nuclear charge increases?
pulls electrons closer making them harder to remove and making the atom smaller.
