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Lewis models
________ are limited because they make it seem like electrons are equally shared between two atoms.
transfer of an electron
The ________ causes energy to be absorbed.
Metals
________ become cations and nonmetals are anions.
best structures
The ________ will have the least electronegative atom in the middle.
Valence electrons
________ are represented with dots.
chemical bond
A(n) ________ is the sharing or transferring of an electron in order to reach a stable electron configuration.
Lattice energy
What is larger when the magnitude of the ionic charge increases? Answer with a single words or term.
Ionic bonds
________ deal with electrons being transferred.
Free radicals
________ can be expressed as Lewis structures because resonance shows the different places the electron could be located.
Hydrogen atoms
________ can never be in the center.
Dashes lines
________ represent a bonding pair.
Scientists
________ tried to develop a molecule that would disable the HIV- protease.
electronegative element
The more ________ should be in the center.
Lewis symbol of an anion
The ________ is represented with brackets around the model and the charge in the upper right corner.
Incomplete octets
________ are molecules or ions with less than 8 electrons.
enthalpy change
What is the lattice energy? Answer with a single words or term.
Francium
What is the least electronegative element? Answer with a single words or term.
Any lone pairs
________ should be given to the middle atom.
electron sea model models
Metals have low ionization energies, so they lose their electrons very easily. The ________ metallic bonding.
Fluorine
What is the most electronegative element? Answer with a single words or term.
Helium
What is an exception because it can only hold 2 valence electrons? Answer with a single words or term.
Boron
________ has 6 electrons.
model
The ________ does not account for the nonconductitvty of ionic solids.
Electronegativity
________ decreases going down a column.
Formal charge
________ can be found by finding the difference between the number of valence electrons in the atom and the number of electrons that it "owns "in a Lewis Structure.
Note
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