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Electronegativity is the ability within a covalent bond to attract electrons to itself (my definition is the strength an element will take to pull an electron to itself)
Covalent bonds are usually made up of non-metals and equally sharing meaning they share the same electron
When full s and p orbits are full yet they are together and sharing full valence shells
An example of theses would be the diatomic elements H2, Cl2, O2..ect.
When the atoms are attracted to the nuclei then both atoms will become more stable, lowering potential energies. Yet if the atom come to close with the other atom then it will start to repel like magnets with like charge cause thing to lower it from being stable and raising potential energies
Resonance structure is when the Lewis structure is done and one can write more than one meaning that if one does it, they must show both ways or how many ways there are putting an arrow showing that there are equal
When a bonded atom doesn’t share the same electronegativity than the electron will be more attracted to the electronegative causing the molecule to have a less electronegative side and a more electronegative side becoming a dipole also being polar covalent
Metal structures (metallic bonding)
A metal lattice that is packed with positive ions which is surrounded by a sea of electrons. Because of sea of electrons this causes it be a good conductor in electricity and in heat
When one electron is shared it’s a single bond
When two electrons are shared it’s a double bond
When three electrons are shared it’s a single bond
FRQs?
Third bond
Single bond
Double bond
Bond length
Shorter
Shortest
Longest
Bond energy
Stronger
Least
Greatest
Formal charge
The reason for the good conducted is that the energy can easily be passed from one positive ion to the next
Yet with metals and alloys both have different properties from a pure metal showing when there's a reaction with air.
Polar bonds are when a molecule is form but having a dipole when this happens one side is attracted to the electron making one side positive (less electronegative) and one side negative (more electronegative) can also been seen as when electrons are not shared equally
Theses are some of the most recent FRQs asked
The formula shows two things but one is really shown
Ionic bonding- lose or gain an electron to become stable the reason for this to become like the noble gases have a full s and p shell full and also usually metals and non-metals
An example can be The statue of liberty
The statue of liberty was originally made out of copper but due to being oxide it started to turn a greenish color. But the greenish color is a protective layer for the copper because over time the copper would oxide but with the green layer on top the copper would stay in its ways.
Interstitial alloy
Ionic substance can conduct electricity only when in a solution or molten being that in a solid it is hard for the ions to be moving around to conduct electricity
When the charges increase the distance decrease ions have a high charge densities meaning that a strong ionic bond formed
Stronger electrostatic is the force of attraction between the charged particles which ionic bonds are "held by"
Ionic substance can go through hydration meaning that if an ionic bond is polar then the substance will want to go "dissolve" meaning that it will be attracted to the opposite charge
As the radius gets bigger the less electronegativity the molecules have meaning when you move down the periodic table it causes the radius to get bigger causing it to decrease
Is when there is smaller atoms that fill the space of a metallic lattice this causes the structure to be less malleable and ductile making it more rigid and less flexible
Yet if the ionic substance is non-polar it wont react being that i doesn't have a stronger anion or cation so the ionic will stay in its solid from
Noble gases are the most stable ones being that all their p orbital is full
Substitutional alloy
It when one metals atoms are replaced by another metal atoms being with this the only way it could replace another metal atom is if both atoms had a similar radius
02:E
02:G
Yet there really isn’t a full covalent bond or a full ionic bond but a covalent bond with slightly ionic bond behaviors or vice versa
Lewis structures
VSEPR – Valance shell electron pair repulsion
Ionic substance with covalent character
Fajans rule helps us see
This theory can help determine the shape that the molecule/ion might have by knowing the bonding pair and lone pair of electrons
Show cart that is given
When the valence electrons and the atoms are together their electron cloud repel each other having this the molecule will adapt a certain geometry so they can as far away as possible also atoms will do the same thing
this are some of the main ones
Non-bonding – are less restricted being that it could pair with another molecule/ion
Bonding – are more restricted being that it already has the full octet so for molecule/ion to bond its going to be a lot harder
covalent bond with ionic character (polar-covalent)
A covalent bond one can see that in the bond one atom can be more electronegative and a less electronegative creating a dipole which cause a polar covalent bond to be made so the ionic characters come in when the anion gets to big and the cation is to small fajans rule
Sigma bond – single covalent bond
Pi bond – double covalent bond