The Periodic Table III Flashcards
Specific patterns in the
physical and chemical
properties of the elements
that can be observed in the Periodic Table
Periodic Trends
What are the 5 Common Periodic Trends?
Atomic Radius, Ionization Energy, Metallic Property, Electron Affinity, Electronegativity
We determine the radius by placing two atoms of one element side-by-side; We get the distance between the two nuclei (plural of nucleus), obtaining the diameter so we divide by 2, to get the atomic radius
Atomic Radius
Atomic Radius increases as you go…
Southwest
Refers to the level of reactivity of a metal, since metals tend to lose electrons when bonding or reacting with another atom
Metallic Property
Metallic Property increases as you go…
Southwest
The energy required to
remove electron from an atom; The larger the atom, the lesser the energy required to remove an electron
Ionization Energy
Ionization Energy increases as you go…
Northeast
The energy required to
accept electron from an atom; The higher the valence electrons an atom has, the higher their electron affinity
Electron Affinity
“Rule of eight”; When they have eight electrons, they are less likely to react with other atoms
Octet Rule
The special “outermost” electrons in an atom, and they play a big role in how atoms interact with each other; They determine how it can connect with other atoms to form compounds and molecules
Valence Electrons
The electrons in the inner shells of the atom; They are not involved in chemical reactions or bonding; Closer to the nucleus and are more tightly held by the positive charge of the protons in the nucleus.
Core Electrons
Electron Affinity increases as you go…
Northeast
The tendency of an atom to attract electron (Atoms need a total of 8 valence electrons to follow the Octet Rule and become stable)
Electronegativity
Electronegativity increases as you go…
Northeast
