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Unit two:Molecular and Ionic Compound Structure and Properties

02:ABC

02:F

02:D

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 (Molecules)

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

Oxygen reacts with metal?

Formal charge

  • Formal charge = (number of valence electrons)-(lone electrons)-(number of bonds)

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

Ionic bonding (ions)

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.

  • Forms a lattice making it solid form every brittle

Interstitial alloy

  • Ionic bonding has a high melting/ boiling point and low vapor pressure
  • To show where the charges lay and the most likely separation of charge meaning the value for each charge
  • To show the most plausible structure from a set of resonance structures use

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

  • 2019 2a, 1a
  • 2018 2d, 3a-b
  • 2017 1c, 2a
  • 2015 2d-c

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:ABC

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

Electron deficient species

is when the central atom doesn’t complete the full octet meaning that it has to find another compound to complete the octet Ex. BF3 and NH3, yet at the end when both end us sharing both compounds form a dative or co-ordinate bond meaning they use other compounds to make normal covalent bonds

  • when the cation is small and highly charged
  • when the anion is highly charged

Polar and non-polar bonds

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

A molecule can only be a polar bond if it has two things

  • A dipole moment must exist
  • Dipoles that are present must not cancel out due to symmetry

Non-polar bonds cancel out due to symmetry

Also when writing a Lewis structure one can use an arrow to show which side is more electronegative

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

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