Ionic Bonds
The rule explains why atoms form ions to reach 8 valence electrons.
The octet rule.
The attraction between metal cations and free electrons.
A metallic bond.
Covalent bonds occur when atoms do this with electrons.
Share them.
Electronegativity is an atom’s ability to do this in a bond.
Attract electrons.
Name the compound CaCl₂.
Calcium chloride.
The type of ions attract to form an ionic bond.
Oppositely charged ions (cation + anion).
The model that describes electrons flowing freely around metal ions.
The sea of electrons model.
Type of bond where there are one pair of shared electrons.
A single covalent bond.
A bond with equal electron sharing.
Nonpolar covalent bond.
Name the molecular compound N₂O₄
Dinitrogen tetroxide.
Ionic compounds form large repeating 3D structures.
Crystal lattices.
The property that describes a metal that can be pulled into wires.
Ductility (Ductile).
This theory explains molecule shape based on electron repulsion.
VSEPR Theory.
Two factors that determine whether a molecule is polar overall.
Bond polarity + molecular geometry.
Name FeO using Roman numerals.
Iron(II) oxide.
This happens to electrons when a metal becomes a cation.
It loses electrons.
The property that ionic and metallic solids share (think molecules).
They are not made of discrete molecules.
The bond type formed between two oxygen atoms in O₂.
A double covalent bond.
For the bond C–H (EN: C = 2.5, H = 2.1), calculate the EN difference and classify the bond.
EN difference = 0.4 → Nonpolar covalent.
Write the formula for ammonium sulfate.
(NH₄)₂SO₄.
Name an example of an ionic compound.
NaCl2
(cation + anion)The reason why metals are good conductors of electricity.
Mobile valence electrons allow charge flow.
The reason hydrogen is an exception to the octet rule.
It only needs 2 electrons for stability.
Name the bond that would be the most polar.
Fluorine = 4.0
Carbon = 2.5
Hydrogen = 2.1
H–F (ΔEN = 1.9) → most polar
Write the formula for aluminum oxide.
Al₂O₃