Types of Bonds and Electronegativity
This type of bond is between a metal and another metal
What is a metallic bond with a "sea of electrons." An ionic bond is between a metal and nonmetal and involves electron transfer. A Covalent bond is between two nonmetals and can be polar covalent or nonpolar covalent
As Two atoms get closer to eachother
There potential energey decreases and vice versa
This is the kind of alloy a metal is when its atomic radus is much smaller than the metal it interacts with
What is an interstitial alloy
This is what is added to elements in a lewis diagram other than H to fill the 8 valence electrons and give it a full shell
What are Lone Pairs
2 Electrons
2 Electron Domains
0 Lone Pairs
180O Bond Angle
sp Hybridization
What is a Linear Bond
The O-H Bond in H2O
What is a polar bond
This decreases the strength of Coloumbic Attraction
Increasing the distance between charges and vice versa
The Properties of Ionic Solids
1) Ionic Solids have high melting points
2) Ionic Solids do not conduct electricity
3) Ionic Solids are soluble in polar solvents
This set of 4 molecules is abbreviated by HONC
H - Hydrogen 1 Bond
O - Oxygen 2 Bonds
N - Nitrogen 3 Bonds
c - Carbon 4 Bonds
This is the Bond Shape of a BF3 molecule with an sp2 hybridization
What is Trigonal Planar
In this bond, the electrons are not equally shared
What is a polar covalent bond. A nonpolar covalent bond is where the electrons are shared equally between the molecules
This bond length is the strongest yet shortest
What is a triple bond
This happens as the charge of the cations and the number of electrons increase
The attractions are greater and vice versa
This is included around a lewis dot diagram of an ion with resonance structures
Brackets with the charge as the exponent outside. In a resonant structure a double or triple bond may be placed in multiple areas so draw as many necessary to account for all possible configurations.
If a single or double bond can be placed in the same spot, you may draw a double bond with the top line being dashed into two, signifying a single and double bond possibility.
Divide the actual number of bonds (singe - 1 double - 2) by the number of bond domains (single - 1 double - 1) for the estimated bond length. (i.e. 4/3 = about 1.3 bond length)
5 Electrons
5 Electron Domains
0 Lone Pairs
sp3d Hybridization
What is a Trigonal Bipyrimidal Bond
This kind of bond has an electronegativity difference of 0.0-0.4
What is a Nonpolar Covalent Bond
Electronegativityhigher - Electronegativitylower
Polar Covalent (0.4-1.7)
Ionic (1.7- Greater)
As bond length decreases
Bond strength increases and vice versa
What happens to ions at higher charges
Larger Charges = More Attraction = More energy required to break ions
Smaller Charges = Less Attraction = Less energy required to break ions
These are the steps to creating a lewis dot diagram
What are:
1) Determine the total number of valence elctrons in an atom by adding the valence electrons of all elements together (i.e. H-2 0-6)
2) Draw a Skeleton structure of elements with their corresponding amounts of bonds. Each single bond is equal to 2 Electrons subtracted from the total
3) Add the remaining lone pairs until all electrons are gone and all shells of elements are filled, each lone pair is two electrons
4) If electrons run out before filling octets, create double or triple bonds accordingly
4 Electrons
2 Electron Domains
2 Lone Pairs
104.5O Bond Angle
sp3 Hybridization
What is a Tetrahedral Bond
This Kind of Bond has lower melting points and do not condut electricity well when dissolved
What is an Ionic Bond
A Covalent Bond has more brittle compounds, high melting points, and conduct electricity when dissolved into a solution
What is Lattice Energy
The energy to separate ion from ionic compounds
Two metals that interact with similar radii are substitutional alloys
This is how you calculate formal charge of a molecule that has a resonant structure and desiring to find which is most valid
Formal Charge = (#Valence Electrons) - (#Lone Pairs) - (1/2)(bonding Electrons)
The sum of formal charges should be zero or the charge of the polyatomic ion
Example HCN
H [1 (valence electron) - 0 (lone pairs) - 1( two bonding electrons divided 2)]
C [4 (valence electron) - 0 (lone pairs) - 4( eight bonding electrons divided 2)]
N[5 (valence electron) - 2 (lone pairs) - 3( six bonding electrons divided 2)]
0-0-0 Closer to all zeroes This Structure is more valid
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H [1 (valence electron) - 0 (lone pairs) - 1( two bonding electrons divided 2)]
N[5 (valence electron) - 0 (lone pairs) - 4( eight bonding electrons divided 2)]
C [4 (valence electron) - 2 (lone pairs) - 3( six bonding electrons divided 2)]
0 + 1 - 1 This structure is less valid because there is variation from zero (it is still a valid resonance structure however)
This is the SF6 bond shape with a hybridization of sp3d2
What is an Octohedral Bond