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Polarity and Forces
Adam Hogue / IB Chemistry
Metals with nonmetals
Electrostaic attraction between oppositely charged ions
Strongest bond
Aluminum needs 3 electrons, Oxygen needs 2 for complete octet
O gives Al, but mathematically 2 Aluminums bonded with 3 oxygens will need to exist in order for the octates to be complete
Between non-metals and non-metals
Atoms share electrons
Thh
2
o
C
- Coordinate covalent bonding takes place when 2 electrons come from one atom, but are both shared between the atom and another
O3 (ozone)
C 4 (valance) -> 8 - 4 = 4 (bonds)
O 6 -> 8 - 6 = 2
109.5°
Parent/basic shape: triagonal planar
Actual shape: V-shaped
Domains: 3
Bonding pairs: 2
Loan pairs: 1
Force
NH3
Domains: 4
Bonding pairs: 3
Loan pairs:1
107°
Tetrahedral (ussually) = 109.5°
109.5 - 2 ≈ 107°
- The mixing of atomic orbitals to produce a new set of orbitals keeping the charcateristics of the original orbitals, but are set up in space for covalent bonding
2p
Valence electrons
2s
sp3
sp2
sp
s
p
C
1s2 2s2 2p2
2p
2s
π
σ
2p
(non-hybridized)
σ
sp2
Diamond
Giant covalent bonds-
Bonds made up of the same atom creating a new molecular structure or allotrope
London force - Weak force between adjaent atoms that are in positions of temporary dipoles
Graphite
Ccccff
Cases occur when an atom does not have enough room to obtain a full valence shell or when atoms must go above the octet limit in order to complete the octet ofits bonded atoms
Period 3 and below can expand octet if needed
- Between metals and metals
- Electrons are unnatached and travel amongst positive ions
- The more positive he ions are, the more electrostatic attraction exists between them and the electrons
1. Stronger electrostatic attraction leads to higher boiling point
2. Smaller (more positively charged) ions have electrons closer to the nucleus and are more attracted
3. The more delocalized electrons per atom, the higher attraction between them and the ions
- The delocalization of the electrons in metals make them ductile, meaning that two metals slide together, the bonding in the structure stays the same
- If ionic solids are brought together, they are brittle because of their charges repelling eachother
- Alloys are combinations of pure metals which together form a new type of metal
- Alloys are ussually made to achieve desirable properties, such as alloys often being stronger than pure metals
- The strength from alloys is due to combination of bigger atoms with smaller ones. Bigger atoms prevent smaller atoms from moving around as easily
Polarity - Difference of electromagitivity between two atoms resulting in electrons lying more towards one atom than the other
A molecule must have a positive and negative end in order to be polar
The direction to where the electrons lean towards is the dipole movement
Symmetry cancles out dipole movement and make a molecule nonpolar
Difference of 0.8 in electronegativity means polarity
CO
- The measure of an atom's ability to attract shared electrons to itself
3.5 - 2.5 = 1
1 > 0.5
CO is polar
Nobal gasses = Nonpolar
Single and diamtomic molecules = nonpolar
Symmetric molecules = nonpolar
Symmetric molecules having a difference in shape can make the compound polar
O2 - Oxygen
O3 - Ozone
- O2 absorbs highest energy of `uv radiation
- O3 bond is weaker than O2, absorbs low energy of UV radiation
O=O = 498 kj mol^-1
Free radicals are compounds in the stratosphere that break down ozone molecules
(Free radical)
Chlorocarbons
CCl2F2 -UV-> CClF2 + Cl
ClO + O3 -> ClO + O2
ClO + O -> O2 + Cl
Nitrogen Oxides
NO + O3 -> NO2 + O2
NO2 + O -> O2 + NO