Bonding Test Flashcards
Bond Length
The distance between two bonding atoms in picometers
Bond energy
The amount of energy in kj required to break one mole of bonds
Single bond
Sharing of 2 electrons
Largest bond length
Lowest bond energy
Double bond
Sharing of 4 electrons
Triple bond
Sharing of 6 electrons
Lowest bond length
Highest bond energy
Valence electrons
Highest energy level electrons involved in chemical bonding
Ionic bonding
Electrons are lost or gained Reaction between a metal& nonmetal Only conductive if dissolved in water High melting point Properties- crystal, lattace, brittle Ex salt
Non polar covalent bonding
Even sharing of electrons Reaction between a nonmetal and a nonmetal Not conductive Low melting point Ex butter
Polar covalent bonding
Uneven sharing Non metal and a non metal metal Not conductive Medium melting point Ex sugar
Metalloids
Flow in a sea of electrons Reaction between metals and metals Conductive Pretty high melting point Malliable and ductile Ex aluminum
Surface tension
The clinging together of molecules
Viscosity
The ability to flow or stickiness
Solvation
Ability to dissolve in water
Boiling/ melting point
Higher as the ims increases
How IMFs affect St, V, S BP, MP
As the imf increases, the … Increases (linear)
What are the strengths of IMF
From weakest to strongest
Londoon dispersion forces
Dipole forces
Hydrogen bonding
How does the size of the molecule affect the IMF
The larger the molecule the more permanant the electrons will stay on one side
Tetrahedral shape
Central atom with 4 atoms attached
Bond angle 109
Trigonal pyrimidal
Three atoms attached to the central atom WITH SPRINKLES
Bond angle 107
Little bent
2 atoms connected to the central atom and 2 lone pairs
Bond angle 105
Triogonal planar
3 atoms connected to the central atom WITHOUT SPRINKLES
Bond angle Q120
Big bent
2 central atoms with a double bond connected to the central atom and one lone pair
Linear shape
Straight line with atoms on each side
Bond angle 180
London dispersion theory
The buildup of electrons temporarily on one side of the molecule (teacher vs student)
ONLY NONPOLAR MOLECULES
Dipole force
Two opposite sided molecules that have a partial permanant seperation of charge because the electrons are not evenly shared
ALL POLAR MOLECULES EXCEPT h/f h-n h-o
Hydrogen bonding
Polar bond only woth h-f h-n h-o
Creates a very strong dipole because no other electrons counteract
When is it a nonpolar molecule?
When the bonds are all the same type with the same atom and there are no lone pairs
When is it a polar molecule?
If there is a polar bond
If there is a lone pair
If there is a polar and nonpolar bond
Lewis dot structure
Want 8
Starts with the column it is in on the periodic table
