Ionic Bonding - process of dissolving in water and how it explains conductivity and solubility.

Solid, high melting point, conductive only if dissolved, and high solubility in water - held together by electrostatic forces that are in many directions which allows lattice formation and can only vibrate when solid so cannot conduct.

Covalent (includes polar and non-polar) - everything depends on polarity.

Any state of matter at room temp, depends on the compound. Not conductive, but solubility depends on the compound and true for all states of matter for each compound - since covalent compounds share, they are neutral and there are no free electrons t

It is solid at room temperature, conductive, but not soluble at room temperature - electrostatic force is strong but electrons are not bound to any atom and delocalized and move freely allowing them to conduct (lattice),. H2O cannot break electron.

Polar, non-polar, and ionic classifications and bonding triangle.

NP=0.0-0.4, P=0.5-1.7, I=1.7+, since the numbers are a spectrum, the bonding triangle aids in providing boundaries. X axis -s avg en, while y is en difference.

Polar and non polar bonds versus polar and non-polar : watch out for induced dipoles

Polarity of a bond is about atoms sharing electrons equally while polarity of a molecule is about the overall shape of the entire molecule. Bond dipole versus net dipole movement of the whole thing, keep in mind: all polar = nonpolar but not vice versa

Even though the molecules have non-polar bonds and a net dipole of zero, they possess polarizable electron clouds that form temporary, induced dipoles, allowing them to attract each other and condense into a liquid or solid.

Potential energy graphs

X is the inter nuclear distance , while the y is the potential energy. Internuclear distance decreases as more electrons are involved so triple bond, double, single, etc.

How to interpret the potential energy and dips of the graphs

When is near the dotted line,/0 : the electrons show no chemical relationship and moving past. Less than 0: stability because energy is released. Minimum: strength of bond energy, greater than 0: forced close together and repel.

Exact distance where the pulling forces and pushing forces perfectly balance each other out. Atomic radii: As larger atoms have longer bond lengths, smaller has shorter. , and bond order increases, length decreases,

First covalent bond formed between any atoms pi comes after double and triple; there is only sigma bond.

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Types of Bonds CHEM

Term	Definition
Ionic Bonding - process of dissolving in water and how it explains conductivity and solubility.	Solid, high melting point, conductive only if dissolved, and high solubility in water - held together by electrostatic forces that are in many directions which allows lattice formation and can only vibrate when solid so cannot conduct.
Covalent (includes polar and non-polar) - everything depends on polarity.	Any state of matter at room temp, depends on the compound. Not conductive, but solubility depends on the compound and true for all states of matter for each compound - since covalent compounds share, they are neutral and there are no free electrons t
Metallic bonds	It is solid at room temperature, conductive, but not soluble at room temperature - electrostatic force is strong but electrons are not bound to any atom and delocalized and move freely allowing them to conduct (lattice),. H2O cannot break electron.
Polar, non-polar, and ionic classifications and bonding triangle.	NP=0.0-0.4, P=0.5-1.7, I=1.7+, since the numbers are a spectrum, the bonding triangle aids in providing boundaries. X axis -s avg en, while y is en difference.
Polar and non polar bonds versus polar and non-polar : watch out for induced dipoles	Polarity of a bond is about atoms sharing electrons equally while polarity of a molecule is about the overall shape of the entire molecule. Bond dipole versus net dipole movement of the whole thing, keep in mind: all polar = nonpolar but not vice versa
induced dipole	Even though the molecules have non-polar bonds and a net dipole of zero, they possess polarizable electron clouds that form temporary, induced dipoles, allowing them to attract each other and condense into a liquid or solid.
Potential energy graphs	X is the inter nuclear distance , while the y is the potential energy. Internuclear distance decreases as more electrons are involved so triple bond, double, single, etc.
How to interpret the potential energy and dips of the graphs	When is near the dotted line,/0 : the electrons show no chemical relationship and moving past. Less than 0: stability because energy is released. Minimum: strength of bond energy, greater than 0: forced close together and repel.
Bond Length	Exact distance where the pulling forces and pushing forces perfectly balance each other out. Atomic radii: As larger atoms have longer bond lengths, smaller has shorter. , and bond order increases, length decreases,
Sigma Bonds and pi	First covalent bond formed between any atoms pi comes after double and triple; there is only sigma bond.

Created by: nuhaSalim

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