SCH4U - Molecular Shapes Flashcards
Ionic bond?
The electrostatic attraction between oppositely charged ions.
Covalent bond?
A chemical bond in which atoms share the bonding electrons.
Bonding electron pair?
An electron pair that is involved in bonding, found in the space
between 2 atoms.
Lewis structure?
A diagram that represents the arrangement of covalent electrons and
bonds in a molecule or polyatomic ion.
Duet rule?
The observation that the complete outer shell of valence electrons when
hydrogen and period 2 metals are involved in bonding.
Octet rule?
The observation that many atoms tend to form the most stable substances
when they are surronded by 8 electrons in their valence shells.
Lone electron pair?
A pair of valence electrons that is localized to a given atom but not
involved in bonding.
Valence shell electron-pair repulsion theory (VSEPR)?
A method to determine the
geometry of a molecule based on the idea that electron pairs are as far apart as possible.
Electron-pair repulsion?
The repulsive force that occurs between electron pairs, causing
them to be positioned as far apart as possible in a molecule.
Non-polar covalent bond?
A covalent bond in which the electrons are shared equally
between atoms.
Polar covalent bond?
A covalent bond in which the electrons are not shared equally
because 1 atom attracts them more strongly than the other atom.
Electronegativity?
The ability of an atom in a molecule to attact shared electrons to itself.
Dipole?
A seperation of positive and negative charges in a region in space.
Polar molecule?
A molecule that has a net dipole.
Non-polar molecule?
A molecule that has only non-polar bonds, or a bond dipole sum of
zero?
Hybrid orbital?
An orbital that forms from the combination of at least 2 different orbitals.
Hybridization?
The process of forming hybrid orbitals from the combination of at least 2
different orbitals.
Sigma bond?
A bond that is formed when the lobes of 2 p orbitals directly overlap end
to end.
Pi bond?
A bond that is formed when the sides of the lobes of 2 p orbitals overlap.
Intramolecular force?
They are chemical bonds within a molecule. (Intra = “In-between”)
Intermolecular Forces?
forces that occurs in between molecules, they can cause large number of molecules to interact.
Van der waals forces?
Many types of intermolecular forces, including dipole - dipole
forces, London dispersion forces, and hydrogen bonding.
Dipole-dipole force?
The intermolecular force that is caused when the dipoles of polar
molecules position their positive and negative ends near each other.
Hydrogen bond?
The strong dipole-dipole force that occurs when a hydrogen atom
bonded to a highly electronegative atom (oxygen, nitrogen, or fluorine) is attracted to a
partially negative atom on a nearby molecule.
London dispersion forces?
The intermolecular forces that exist in non-polar molecules;
they increase as the molecular mass increases.
Surface tension?
The resistance of a liquid to increase its surface area.
Capillary action?
The spontaneous rising of a liquid in a narrow tube.
Composite material?
A material composed of two or more distinct materials that remain
separate from each other in the solid phase.
Metallic crystals?
A solid with closely packed atoms held together by electrostatic
interactions and free-moving electrons.
Electron sea theory?
A theory that states that the electrons in a metallic crystal move
freely around the positively charged nuclei.
Metallic bonding?
The bonding that holds the nuclei and electrons of metals together.
Molecular crystals?
A solid composed of individual molecules held together by
intermolecular forces of attraction.
Covalent network crystals?
A solid in which the atoms form covalent bonds in an
interwoven network.
Buckyball?
A spherical arrangement of carbon atoms that forms a hollow, cage-like
structure.
Carbon nanotube?
A solid made of carbon atoms similar to graphite rolled into a cylinder.
Strongest to least bonding
- Ionic Bonds
2.Covalent Bonds
3.Hydrogen bonds
4.Dipole Dipole - LDF
