What 2 factors account for the stability of the H2 molecule?
The fact that the attractive energy between the electrons and protons of opposite atoms is slightly greater than the repulsive energy between the proton-proton and electron-electron interactions.
The fact that the electrons are spread over the entire volume of the H2 molecule itself and not just the confines of it's atom's orbital
What are the electrons in the outer-most principal energy level shell of an atom called?
In a Lewis Dot Diagram of an atom, which electrons of the atom are shown as dots around it?
Are they the only ones involved in covalent bonding?
Only the valence electrons of the atom
All molecules form covalent bonds to achieve the electron configurations of which atoms?
How can you identify the amount of valence electrons in an atom on the periodic table?
It is equal to the last digit of the group number the atom is in on the periodic table
What are the 2 types of pairs possibly shown on a Lewis Structure and how are they represented?
Covalent Bond pairs
Shown as dash between the bonded atomsUnshared pairs
Shown as separate dots outside the corresponding atom
For molecules that are ionized despite covalent bonds, how are they're charges shown in Lewis structures?
The bonded atoms are placed in brackets and the charge is shown in the top right corner outside the bracket.
Ex: [ ]2-
What does the octet rule state?
What is its exception?
Says that atoms in covalently bonded species tend to have the electron structures of noble gases.
The exception is hydrogen, which need only be surrounded by 2 electrons to be stable.
Which elements never form multi-covalent bonds in Lewis structures?
Hydrogen and the halogens
What is the procedure for writing Lewis structures?
1) Count # of valence electronsif polyatomic ion add/stubtract # of electrons equal to its charge
2) Draw skeleton structure using covalent bonds
# of electrons to use for covalent bonds is equal to # needed for noble gas structure - # of valence e-
3) Determine # of electrons still available
equal to # of electrons - 2 for each covalent bond
4) Fill each atom with remaining unpaired electrons until octets are reached
remember hydrogen only needs two electrons to be stable
How can you denote resonance in a Lewis structure?
Place a double arrow between the two resonant structures
Does resonance imply that there are 2 different kinds of the same molecule?
No, the molecule is intermediate between the two forms
What is the "charge an atom would have if valence electrons in bonds were distributed evenly"?
If you found it possible to write more than one Lewis structure arrangement for a molecule, how would you go about telling the difference between which one would exist in nature?
Find the formal charges of each important atom so that the more realistic arrangement of molecules would be the one where the formal charges are closest to 0
What is the equation for formal charge and what doe each variable represent?
Cf = X-(Y + Z/2) = X-Y-Z/2
X = # of valence electrons in the atom alone
Y = # of unpaired electrons in the atom within the Lewis structure
Z = # of electrons used to form the covalent bonds around the atom
Where should negative formal charges be in a set of formal charge equations?
Should be on the element that is most electronegative
When do there tend to be exceptions to the octet rule of Lewis Structures?
1) When the amount of valence electrons in the molecule add up to an odd number
aka: free radicals2) When the octets must be expanded to fit more than 4 covalent bonds
When are there typically Expanded Octets?
When a nonmetal of the Third, Fourth, or Fifth period is combined with a halogen
These nonmetals have d orbitals available for extra electron pairs
How would you know that an Expanded Octet is needed for a Lewis Structure?
If you find that the number of electrons needed to fill all octets is less than the amount of electrons remaining after the skeleton structure is drawn, then you need to add the left over electrons to the central atom
What does the VSEPR model say about electron pairs surrounding an atom?
It says that the pairs repel one another, and through this repulsion they are oriented to be at angles that are as far away from each other as possible
For the notation AXbEc, what does each part of that designate?
A - Central atom in the molecule
X - Terminal atom surrounding the central atom
b - Number of terminal atoms present
E - Number of unshared electron pairs that central atom has
c - Nnumber of these unshared pairs
What is the shape of a molecule with the formula AX4 and what angle are its covalent bonds at? Also give an example.
Tetrahedron shape and the bonds
are 109.5 degrees apart
CH4 is like this
Tell me what orientation the Electron pairs in each of these molecules have: BeF2 BF3 CH4 PF5 SF6
For a molecule with the formula AX2, if the central atom has unshared electrons then what shape will it take?
What about if the central atom in AX3 had unshared electrons?
What are the predicted VSEPR model shapes of each of these molecule types: AX5 AX4E AX3E2 AX2E3 AX6 AX5E AX4E2
Do multiple bonds affect the predicted shape of molecule? How do they act?
They don't affect the shape because they occupy space the exact same way a single bond would.
What are the 2 types of covalent bonds?
Polar Covalent bonds
These are a result of an asymmetrical distribution of electrons that causes a positive and negative poleNon-polar Covalent bonds
The distribution of electrons in these are symmetrical and thus have no poles
When do polar and non-polar bonds typically occur?
Non-polar bonds happen when the atoms joined are identical or the same element (as in H2 or F2).
Polar bonds happen when the atoms joined aren't of the same element thus creating a higher electron density on one side than the other.
How do you find whether or not a covalent bond is strongly polar?
Calculate the difference in electronegativities of the bonded atoms
What is the dipole moment?
This is a measure of the extent to which molecules tend to orient themselves in a magnetic field.
What is the dipole moment of F2?
How many hybrid orbitals are created by an sp3d hibridization?
True/False: All single bonds are sigma bonds?
In a multiple bond, how many bonds are sigma bonds and how many are pi bonds?
Only one bond is a sigma bond...the rest are pi bonds.
Which two elements are known to need less than 8 electrons to reach stability, and how many electrons do they need specifically?
Are pi bonds made up of hybrid orbitals?
If you have a molecule with 2 single bonds and 1 double bond, what is the hybridization of its orbitals?
sp2 because two p orbitals are combined with an s orbital to create 3 sigma bonds, leaving one p orbital available for the pi bond that creates the double bond.