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Peter Li Period 4 (Bonding (Bonding Types (Ionic: Cations gives…
Peter Li Period 4
Bonding
Bonding Types
Covalent: Share electron pairs to usually form octets, only involves atoms of non-metals, "molecule" used exclusively for covalent bonding
Polar= unequally shared electrons (electronegativity difference between .3 and 1.7)
Nonpolar=equally shared electrons(electronegativity different between 0 and 0.3)
Metallic "sea of electrons" good conductors of electricity because of free moving electrons also generally high melting points
Forms Alloys: mixture of metals and metals/nonmetals, creates a stronger/better substance
Ionic: Cations gives electron(s), Anions takes electron(s) form between nonmetals and metals, strongest bond type
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In molten state, conduct electricity
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Honc Rule: Hydrogen(and Halogens) form 1 covalent bond Oxygen (and sulfur) form 2 covalent bonds Nitrogen(and phosphorus) form 3 covalent bonds and carbon (and silicon) form 4 covalent bonds
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Type of bonds
Sigma Bonds
s to s, p to p, hybrid to hybrid, s to hybrid
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Stronger than pi bond because linear overlapping, compared to parallel overlapping in pi bonds
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Molecular Geometry
VSEPR (Valence Shell Electron Pair Repulsion) Geometry, AXE Formula. Used to determine atomic shape (molecular geometry) of an compound
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Resonance
A molecule having more than one lewis structure possibility, usually due to multiple bonds
SOme molecules may be written as having resonance, but their actual structure is a hybrid between those resonance structure
Octet rule: elements tend to combine in such a way that each atom has eight electrons in its valence shell, giving it the same electron configuration as a noble gas
Common exceptions: aluminum, boron, hydrogen, lithium
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Chemical bonds form because they lower the potential energy between the charged particles that compose atoms
Hybridization
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Standard atomic orbitals are combined to form new, hybrid orbitals
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Equilibrium
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le chatelier's principle
Increase concentration=move away
Heat=move away
Increase pressure to lower moles
Increase heat=away from heat
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Kinetics
Reaction rate
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Integrated rate law
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Intermediates: substances that are produced in a multi-step reaction but are used by the end of the steps, doesn't appear in final equation
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Pseudo 1st Order
Dependent on one reactant, making other reactant(s)' concentration much larger so it would almost have no affect on the rate
Graphical Analysis
Graph zero order, concentration
Graph first order, ln concentration
Graph second order, 1/concentration
Which ever is more linear is the correct order
Mechanisms
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Consist of multiple, elementary, steps; coefficient is order
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Atomic Structure
Periodic Trends
Atomic radius
Decreases from left to right. Increase protons across a period pulls electrons closer because increase nuclear charge
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Electron affinity
Increases from left to right within a period. This is caused by the decrease in atomic radius.
Decreases from top to bottom within a group. This is caused by the increase in atomic radius.
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Electron negativity
From left to right across a period of elements, electronegativity increases.
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