Question | Answer |
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 |