Define valence electrons.
Outermost electrons involved in chemical bonding, residing in the *s* and *p* orbitals of the outermost shell.
Define electronegativity.
An atom's ability to attract electrons in a chemical bond.
Define ionic bond.
A chemical bond involving the transfer of electrons, typically between a metal and a nonmetal, resulting in the formation of ions.
Define covalent bond.
A chemical bond involving the sharing of electrons, typically between two nonmetals.
Define polar covalent bond.
A covalent bond with unequal sharing of electrons due to differing electronegativities, creating partial charges.
Define nonpolar covalent bond.
A covalent bond with equal sharing of electrons due to similar electronegativities.
Compare and contrast ionic and covalent bonds.
Ionic: Transfer of electrons, typically between metal and nonmetal, high melting/boiling points. | Covalent: Sharing of electrons, typically between nonmetals, lower melting/boiling points.
Differentiate between polar and nonpolar covalent bonds.
Polar: Unequal sharing of electrons, electronegativity difference between 0.4 and 1.7, creates partial charges. | Nonpolar: Equal sharing of electrons, electronegativity difference between 0 and 0.4.
Compare the electrical conductivity of ionic compounds in solid vs. liquid states.
Solid: Do not conduct electricity due to immobile ions. | Liquid: Conduct electricity due to mobile ions.
Compare the melting points of compounds with +1/-1 charges vs +2/-2 charges based on Coulomb's Law.
+1/-1: Lower melting point due to weaker electrostatic attraction. | +2/-2: Higher melting point due to stronger electrostatic attraction.
Compare the impact of charge versus size on the melting point of ionic compounds.
Charge: Greater impact on melting point due to stronger electrostatic forces. | Size: Smaller impact, but smaller ions lead to higher melting points.
What is the effect of a large electronegativity difference between two atoms?
Formation of a polar covalent bond or an ionic bond, depending on the magnitude of the difference.
What is the effect of increased charge on the melting point of an ionic compound?
Increased melting point due to stronger electrostatic attractions, as described by Coulomb's Law.
What is the effect of increased distance between ions on the strength of an ionic bond?
Decreased strength of the ionic bond due to weaker electrostatic attraction, as described by Coulomb's Law.
What is the effect of similar electronegativities between two atoms?
Formation of a nonpolar covalent bond with equal sharing of electrons.
What is the effect of dissolving an ionic compound in water?
The compound conducts electricity because the ions become mobile.
What is the effect of an atom losing an electron?
The atom becomes a positively charged ion (cation).
What is the effect of an atom gaining an electron?
The atom becomes a negatively charged ion (anion).
