Chemistry U1 11
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Last updated 7:56 PM on 1/29/23
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4 Terms
1
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Ionic bonds: properties
* b/t metal cation and non metal anion; held together by electrostatic forces
* Cannot form a molecule/ more than 1 bond bc of ionic bond
* Form crystal lattices/ solids at room temperature
* High melting and boiling points: strong forces hold atoms together
* Very hard and brittle: when structure shifts, similar changes line up
* Soluble in water, conduct electricity in it/ solvents by disassociating as ions that move to conduct it
* Cannot form a molecule/ more than 1 bond bc of ionic bond
* Form crystal lattices/ solids at room temperature
* High melting and boiling points: strong forces hold atoms together
* Very hard and brittle: when structure shifts, similar changes line up
* Soluble in water, conduct electricity in it/ solvents by disassociating as ions that move to conduct it
2
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covalent bonds: properties
* b/t 2 or more non metals
* No transfer of electrons, sharing forms a molecule
* Can form more than 1 bond
* Much lower melting and boiling points than ioic compounds
* Softer and squishier than ionic bonds
* More flammable than ionic compounds
* Dont conduct electricity and not v soluble in water
* No transfer of electrons, sharing forms a molecule
* Can form more than 1 bond
* Much lower melting and boiling points than ioic compounds
* Softer and squishier than ionic bonds
* More flammable than ionic compounds
* Dont conduct electricity and not v soluble in water
3
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top-bottom periodic trend
* atomic radius is increased
* increase in energy levels
* e- are far away from nucleus
* weaker pull; attraction from nucleus on e is less
* easier to remove e
* ionization energy decreases
* larger atomic radius = less attraction for e
* lower affinity
* lower electronegativity
* increase in energy levels
* e- are far away from nucleus
* weaker pull; attraction from nucleus on e is less
* easier to remove e
* ionization energy decreases
* larger atomic radius = less attraction for e
* lower affinity
* lower electronegativity
4
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left - right
* atomic radius is decreased
* inner e cannot shield valence electrons from positive charge of nucleus
* nuclear charge increases
* ve moves closer to nucleus
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* inner e cannot shield valence electrons from positive charge of nucleus
* nuclear charge increases
* ve moves closer to nucleus
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