the cental atom has 6 electron pairs, it has d²sp³ hybridization
Back
Why are metals good conductors of electricity?
Front
Valence electrons on each atom do not belong to a specific atom and are very mobile.
Back
Where are electrons localiyed in a network solid?
Front
in colvalent bonds between particular atoms
Back
Molecular Geometry
Front
The shape of a molecule that is assumes to keep different electron pairs as far apart as possible
Back
Doping
Front
a process in which an impurity is added to an existing lattice
Back
Network (covalent) Bonds
Front
hold together atoms in a network solid
Back
Which molecules are more likely to experience greater London-Dispersion forces?
Front
molecules with more electrons
Back
London Dispersion forces
Front
very weak attractions that occur because of the random motions of electrons on atoms within molecules
Back
Trigonal Bipyramidal
Front
The central atom has 5 electron pairs, it has dsp³ hybridization
Back
The larger the dipole moment...
Front
... The more polar the molecule
Back
How can you determine the length and strength of a bond in a resonance structure?
Front
using a bond order calculation
pick one of the bonds in the resonance structure and add up the total bond order across the ressonance forms then divide that by the sum
Back
What give the molecule a dipole?
Front
One of the atoms (the more electronegative one) will exert a stronger pull on the electrons in the bond -- not enough to make the bond ionic, but enough to keep the electrons on one side of the molecule more than the other side
Back
Substitutional Alloy
Front
Forms between atoms of similar radii.
ie. Brass
Back
What is p-doping?
Front
a missing bond (''hole'') creates a positive charge in the lattice and attracts other electrons to it to increase conductivity
Back
Hydrogen bonds
Front
the positively charged hydrogen end of a molecule is attracted to the negatively charged end of another molecule conatining an extremely electronegative element
Back
Sigma bond σ
Front
First covalent bond formed between two atoms
Back
What is the phase of a sunstance related to?
Front
the strength of the intermolecular forces
Back
Po bond π
Front
Additional bonds between two atoms that are formed
Back
Tetrahedral
Front
The central atom has 4 electron pairs, it has sp³hybridization, bond angles are about 109.5°
Back
Double and triple bonds are _____ and _____ than single bonds, but they are not _____ or _____ the strength
Front
Stronger
Shorter
Twice
Triple
Back
Example of hydrogen bonds
Front
H-F
H-N
H-O
Back
What is n-doping?
Front
An extra valence electron is added to allow it to move freely in the lattice
Back
Intermolecular forces
Front
bonds that only exist in covalently bonded molecules
Back
What us the kinetic energy of an ideal gas related to?
Front
it is directly proportional to its absolute temperature:
the greater the temperature, the greater the average kinetic energy
Back
Properties of Network Solids
Front
very hard, high melting and boiling points
Back
Why are network solids poor conductors of electricity?
Front
Their electrons are not free to move about the lattice
Back
Interstitial Alloy
Front
Metal atoms with two vastly different radii combine.
ie. Steel
Back
State and Boiling/Melting point of ionic bonds
Front
Solid at room temp
Very high melting and boiling points
Back
Which side of the molecule is positive?
Front
The side where the electrons spend less time
Back
Dipole-dipole Forces
Front
positive of one polar molecule is attracted to the negative end of another polar molecule
Back
Expanded octets
Front
in molecules that have the d subshells available, the central atom can have more than 8 valence electrons but never more than 12
Back
Resonance forms
Front
Back
Average kinetic energy of a gas single molecule
Front
Back
Properties of London Dispersion forces
Front
weaker than dipole dipole
low melting and boiling points
gases at room temp
Back
Lewis Dot Structure
Front
Back
Trigonal Planar
Front
The central atom has 3 electron pairs, and it has sp² hybridization, bond angles are about 120°
Back
Covalent bonds
Front
Two atoms share electrons
Back
Why do ionic liquids conduct electricity?
Front
The ions are free to move about in the liquid phase
Back
Why are ionic solids poor conductors of electricity?
Front
Each electron is localized around a particular atom and do not move around the lattice
Back
Incomplete octets
Front
atoms that are stable with less than 8electrons in their outer shell
Back
Hybrid orbitals
Front
In a molecule with more than two atoms, the shape of the molecule is determined by the number of electron pairs on the central atom
Back
The melting/boiling point of a covalent susbtance is based entirely on ... but the melting point 0f an ionic substance is based on...
Front
the strength of its intermolecular forces
its lattice energy
Back
VSEPR Valence Shell Ectron-Pair Repulsion
Front
Predicting the geometries of a molecule
Back
Properties of dipole-dipole forces
Front
high melting and boiling points
relatively weak
Back
Linear Shape
Front
the central atom has 2 electron pairs, then it has sp hybridization
Back
Which side of the molecule is negative?
Front
The side where the electrons spend more time
Back
Number of covalent bonds an atom can form
Front
The number of unpaired electrons in its valence shell
Back
Ionic bonds
Front
Held together by the electrostatic attractions between ions that are next to one another in a lattice structure. They often occur between metals and nonmetals.
Back
Hydrogen bond properties
Front
high melting and boiling points
Back
How do you calculate the formal charge?
Front
take the number of valence electrons for that atom and subtract the number of assigned electrons in the Lewis Structure
The total formal charge should be 0
Back
Section 2
(14 cards)
Dalton's Law equation
Front
Back
Mole fraction
Front
gives the fraction of moles of a given substance out of the total moles present in a sample
.
Back
Ideal gas equation
Front
R= .0821
Back
What two things happen when molecules are packed to tightly?
Front
1. The volume of the gas molecules becomes insignificant
2. Gas molecules attract one another and stick together
Back
In what do polar/ ionic solutes dissolve in?
Front
Polar solvents
Back
Partial Pressure
Front
Xa= moles gas A/ total moles of gas
Back
What is dissociation?
Front
Ionic substance dissolves and breaks up into ions
Back
P₁V₁/T₁
Front
P₂V₂/T₂
Back
What dissolves in solvents?
Front
Like dissolves like
Back
Density of a gas
Front
Back
What does molarity express?
Front
concentration of a solution in terms of volume
Back
When do you use the ideal gas constant?
Front
to calculate any of the four variatbles relating to the gas, provided you already know the other 3
Back
Molarity
Front
Back
Dalton's Law
Front
the total pressure of a mixture of gases is just the sum of all the partial pressures of the individual gases in a mixture