Chapter 9 Flashcards
Molecule
Forms when two or more atoms covalently bond and is lower in potential energy that its constituent atoms
Covalent bond
A chemical bond that results from the sharing of valence ectrons
Lewis structure
A model that uses electron dot structures to show how electrons are arranged in molecules
Pairs of dots or lines represent bonding pairs
Sigma bond
A single covalent bond that is formed when an electron pair is shared by the direct overlap of binding orbitals
Pi bond
A bond that is formed when parallel orbitals overlap to share electrons
Endothermic
A chemical reaction in which a greater amount of energy is required to break the existing bonds in the reactants than is released when the new bonds form in the product molecules
Exothermic
A chemical reaction in which more energy is released than is required to break bonds in the initial reaction
Oxyacid
Any acid that contains hydrogen and an oxyanion
Structural formula
A molecular model that uses symbols and bonds to show relative positions of atoms
Can be predicted for many molecules by drawing the lewis structure
Resonance
Condition that occurs when more than one valid lewis structure exists for the same molecule
Coordinate covalent bond
Forms when one atom donates a pair of electrons to be shAred with an atom or ion that needs two electrons to become stable
VSEPR model
Valence Shell Electron Pair Repulsion
Based on an arrangement that minimizes the repulsion of shared and unshared pairs of electrons around the central atom
Hybridization
The process by which the valence electrons of an Atom are arranged to form four new identical hybrid orbitals
Polar covalent
A type of bond that forms when electrons are not shared equally
Structural formulas
Show atoms
Ball and stick model
Shows shape
Single bond is
Long
Weak
H2
Double bond is
Medium
Medium
O2
Triple bond is
Short
Strong
N2
Structural formulas have
H first
Ionic compound
Metal + nonmetal En difference >1.7 Gives electrons/takes electrons NaCl Attraction of oppositely charged ions
Polar covalent compound
Nonmetal + nonmetal
Unequal sharing of electrons
H-F
Cooperation of valence electrons
Non polar covalent compound
Nonmetal + nonmetal
EN difference <.4
Equal sharing of electrons
Cooperation of valence electrons
Single bond has how many electrons
1 pair of electrons
2 total electrons
