Types of Bonds
This type of bond involves the transfer of electrons between atoms.
ionic bond
The suffix “-ide” is used for this part of an ionic compound’s name.
anion
The shape of CH₄ according to VSEPR theory.
tetrahedral
The weakest type of intermolecular force, found in all molecules.
London dispersion forces
The point on a phase diagram where all three states coexist.
triple point
In a metallic bond, positive metal ions are surrounded by this “sea.”
delocalized electrons
What is the correct name for FeCl₃?
iron(III) chloride
A molecule with two bonding pairs and two lone pairs (like H₂O) has this molecular shape.
bent
Hydrogen bonding occurs only when H is bonded to these elements.
N, O, or F
“Like dissolves like” means that polar solutes dissolve best in this kind of solvent.
polar solvent
These bonds form between two nonmetals that share electrons.
covalent bond
Name the compound N₂O₄.
dinitrogen tetroxide
A molecule with five bonding pairs and one lone pair, like BrF₅, has this geometry.
square pyramidal
This IMF is responsible for water’s unusually high boiling point.
hydrogen bonding
The point where the liquid and gas phases become indistinguishable.
critical point
Name one property that distinguishes ionic compounds from covalent compounds.
high melting points / brittleness / electrical conductivity
What is the formula for calcium nitrate?
Ca(NO₃)₂
The total number of electron domains determines this geometry type.
electron geometry
Rank these by strength: hydrogen bond, dipole-dipole, London dispersion.
LDF < dipole-dipole < hydrogen bond
Between n-hexane and 2-methylpentane, which has the higher boiling point and why?
n-hexane, because it has more surface area and stronger LDFs.
Arrange the following by increasing bond strength: metallic, ionic, covalent.
metallic < covalent < ionic
Why do some transition metals require Roman numerals in their names?
Because they can form more than one possible charge.
Describe the difference between electron geometry and molecular geometry.
Electron geometry considers all electron domains; molecular geometry considers only bonded atoms.
Explain why ethanol (CH₃CH₂OH) has a higher boiling point than dimethyl ether (CH₃OCH₃).
Ethanol can form hydrogen bonds; dimethyl ether cannot.
Explain why O₂ can dissolve in water even though it’s nonpolar.
Because a dipole-induced dipole interaction allows temporary polarity in O₂.