Periodic Trends Flashcards
Valence electrons
Electrons on the outermost orbitals
Atomic radii
Half the distance between 2 nuclei
Electronegativity
The tendency of an atom to attract electrons to itself when bonded to other elements
Ionic radii
The distance from a nucleus and its outermost electron
Periods
The horizontal row of elements on the periodic table
Groups/rows/collums
The vertical rows of elements in the periodic table
What is the trend of atomic radii
Top to bottom gets bigger: because there are more electrons Left to right gets smaller: same level/period, but more protons to pull the Electrons in slightly
What is the trend of ionization energy
Left to right, ionization energy increases: more protons in nucleus to have a stronger grip on the electrons. Requires more energy to remove one. Top to bottom ionization energy decreases: we are increasing energy levels/periods, so it is easier to remove an electron
What is the trend of Electronegativity
Left to right electronegativity increases: as we go left to right the atoms get smaller however have more protons so they have a stronger/increased nuclear charge. Top to bottom electronegativity decreases: as you go down the periodic table the elements get physically larger. The size makes it more difficult to attract other electrons.
What does the stair step on the periodic table do?
It separates the metals and the nonmetals
How to determine how large the atomic radii is on an atom
The more negative it is, the larger it will be.
Halogens are located where
Noble gassesare located where
Alkali metals are located where
Alkaline earth metals are located where
Atomic radii arrows
Ionization energy arrows
Electronegativity arrows
Transition metals
Inner transition metals
The 2 strips of elements below the others.
