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Chapter 4 Vocabulary

Across
An atom, ion, or molecule with unpaired electron.
The electrostatic attraction of a cation for an anion.
The energy a charged particle has because of its position relative to another charged particle. (AKA ELECTROSTATIC POTENTIAL ENERGY)
A bond resulting from unequal sharing of bonding pairs of electrons between atoms.
[(# of valence e-)-(# of e- in a lone pairs + .5(# of shared e-)]
Delocalization of electrons that lead to molecular stability.
Two atoms share two pairs of electrons.
The # of covalent bonds an atom forms to have an octet of electrons in its valence shell.
Atoms of main group elements make bonds by gaining, losing, or sharing electrons to achieve a full valence shell.
A characteristic of electron distribution when two or more equivalent Lewis structures can be drawn for one compound.
Two atoms share three pairs of electrons.
An ordered 3D array of particles.
Down
One of two or more Lewis Structures with the same arrangement of atoms but different arrangements of bonding pairs of electrons.
The number of bonds between two atoms
A bond resulting from equal sharing of bonding pairs of electrons between atoms.
The energy needed to break one mole of a specific covalent bond in the gas phase.
A relative measure of the ability of an atom to attract electrons to itself within a bond.
A polyatomic anion that contains at least one nonoxygen central atom bonded to one or more oxygen atoms.
The capacity of the atoms of an element to form chemical bonds.