Electrons
The idea that electrons can behave both like particles and waves.
wave–particle duality
The maximum number of electrons the first energy level can hold.
2 electrons
The tendency of an atom to attract electrons in a bond.
electronegativity
Elements in this group already have full valence shells and rarely react.
noble gases
This type of energy transfer occurs when electrons absorb energy and move to a higher energy level.
excited state
This model uses probability clouds instead of fixed circular paths for electrons.
quantum mechanical model
This trend increases as you move down a group due to added energy levels.
atomic radius
A positively charged ion formed when an atom loses electrons.
cation
The stable, lowest-energy arrangement of electrons in an atom.
ground state
This law states that electrons fill the lowest-energy orbitals first.
Aufbau Principle
This effect explains why outer electrons feel less nuclear attraction in larger atoms.
shielding effect
This diagram shows only the valence electrons of an atom.
Lewis dot structure
Atoms become more stable by gaining, losing, or sharing these subatomic particles.
electrons
This block of the periodic table begins filling in the fourth period, making electron configurations more complex.
d block
According to Coulomb’s law, this increases as nuclear charge increases and distance decreases.
electrostatic attraction
This group of elements almost always forms a +1 oxidation state.
Group 1
Draw a Bohr model and a Lewis Structure for Sulfur
Must show 16 electrons total and 6 valence electrons
The noble-gas electron configuration for sulfur.
[Ne]3s23p4
A bond formed when the electronegativity difference between two atoms is large, such as Na and Cl.
ionic bond
If Atom A has a higher electronegativity than Atom B, electrons in a bond are pulled closer to this atom.
Atom A