Chapter 8 Flashcards
How does matter take form in nature?
In many forms
Covalent Bond
Sharing electrons.
Molecule
A group of atoms joined by covalent bonds.
Diatomic Molecule
A molecule consisting of two of the same atoms.
Molecular Compound
Compounds composed of molecules.
They have relatively lower melting and boiling points.
Molecular Formula
The chemical formula of a molecular compound.
In covalent bonds, why does electron sharing occur?
To attain the electron configuration of a noble gas.
Single Covalent Bond
Two atoms held together by sharing a pair of electrons.
Structural Formula
Represents the covalent bonds by dashes and shows the arrangement of the covalently bonded atoms.
Unshared Pair
A pair of valence electrons that are not shared between atoms.
Double Covalent Bond
A bond that involves two shared pairs of electrons.
Triple Covalent Bond
A bond by sharing three pairs of electrons.
Diatomic Elements
Hydrogen, Nitrogen, Oxygen, and group 17.
Coordinate Covalent Bond
A covalent bond in which one atom contributes both bonding electrons.
Polyatomic Ion
Tightly bonded group of atoms that has a charge and behaves as a unit.
Bond Dissociation Energy
The energy required to break the bond between two covalently bonded atoms.
Resonate
Electron pairs rapidly flip back and forth between atoms.
Resonance Structure
The structure that occurs when it is possible to draw two or more valid electron got structures.
When can the octet rule not be satisfied?
IN molecules whose total number of valence electrons is an odd number.
Molecular Orbitals
Orbitals that apply to the entire molecule.
Bonding Orbital
Molecular orbital that can be occupied by two elements of a covalent bond.
Sigma Bond
Two atomic orbital combines to form a molecular orbital.
Pi Bond
Bonding electrons are most likely to be found in the sausage-shaped regions.
What is weaker, Pi or Sigma?
A pi bond is weaker than sigma.
VSEPR Theory
Valence shell electron pair repulsion theory.
The repulsion between electron pairs causes molecular shapes.
Orbital Hybridization
Provides info about both molecular bonding and molecular shape.
Hybridization
Atomic orbitals mix to form the same total number of equivalent hybrid orbitals.
Non-Polar Covalent Bond
Bonding electrons are shared equally.
Polar Covalent Bond
Electrons are shared unequally.
Polar Molecule
One end of the molecule is slightly negative while the other end is slightly positive.
Dipole/Dipolar Molecule
Has two poles
Can molecules attract by a variety of forces?
Yes
Are intermolecular attractions stronger or weaker than ionic or covalent bonds?
Weaker
Skip
Consists of two forces
Dipole Interactions
Occurs when polar molecules are attracted to one another.
Dispersion Forces
Caused by the motion of electrons.
Hydrogen Bonds
Hydrogen is attracted to negative oxygen and its electrons.
This is extremely important in determining the properties of water.
Important in proteins.
Network Solids/ Network Crystals
Solids in which all of the atoms are covalently bonded to each other.
Example diamond.
