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Transcript

UV Light

Chemical Bonding

Polarity and Forces

Adam Hogue / IB Chemistry

Ionic Bonding

Metals with nonmetals

Electrostaic attraction between oppositely charged ions

Strongest bond

Ionic Bonding

Title

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

Covalent Bonding

Between non-metals and non-metals

Atoms share electrons

Covalent Bonding

Lewis structures

The Octet Rule

Thh

2

CO2

o

C

Coordinate Covalent Bonds

- Coordinate covalent bonding takes place when 2 electrons come from one atom, but are both shared between the atom and another

Resonance Structures

O3 (ozone)

Method of Forming Lewis Structures

C 4 (valance) -> 8 - 4 = 4 (bonds)

O 6 -> 8 - 6 = 2

Bonding Angles

Bonding Angles

109.5°

Molecules with multiple central atoms

Parent/basic shape: triagonal planar

Actual shape: V-shaped

Domains: 3

Bonding pairs: 2

Loan pairs: 1

Electron Repulsion

Force

NH3

Domains: 4

Bonding pairs: 3

Loan pairs:1

107°

Tetrahedral (ussually) = 109.5°

109.5 - 2 ≈ 107°

Hybridization

Hybridization

- 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

Valence Shells

2p

Valence electrons

2s

sp3

sp2

sp

s

p

COH2

C

1s2 2s2 2p2

2p

2s

π

σ

2p

(non-hybridized)

σ

sp2

Diamond

Giant Covalent Structures

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

E

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

Exceptions to octet rule

Explanation

Expanded Octate

Period 3 and below can expand octet if needed

Metalic Bonding

Metalic Bonding

- 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

Determinants of higher melting point

Melting Points

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

Ductlicity

- 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

Alloys

Alloy Examples

- Bronze

- Brass

- Steel

- Solder

... and more!

Polarity

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

Determining Polarity

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

Wavelength of UV Light

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

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

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