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Quantum Atom

sphere shaped orbitals s orbitals
blank spaces in orbitals where electrons cannot be nodes
dumbbell shaped orbitals p orbitals
number of p orbital shapes three (x, y, and z)
number of types of d orbital shapes five
mostly clover shaped (except one)orbitals d orbitals
maximum number of electrons each orbital can hold two
states that the two electrons in any orbital have opposite spins Pauli exclusion principle
charge an atom has if an atom gains an electron negative
charge an atom has if it loses an electron positive
an atom that gains or loses an electron ion
uses dots to show the number of valence electrons Lewis structure
the electrons in the outer shell of an atom valence electrons
states that an atom gains or loses electrons until it has eight electrons in its valence shell octet rule
bonds formed between oppositely charged ions ionic bond
bond formed between two atoms that share a pair of electrons covalent bond
bond formed between two atoms that share two pairs of electrons double covalent bond
bond formed between two atoms that share three pairs of electrons triple covalent bond
the ability of an atom in a molecule to attract the electrons closer to itself electronegativity
when two atoms with different electronegativities bond polar covalent bond
states that electrons fill the lowest energy level first Aufbrau principle
When electrons occupy orbitals of equal energy, they don’t pair up until they have to. They will have the same spin. Hund's rule
Created by: ad_g