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44 Cards in this Set
- Front
- Back
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N,O,F,H,Cl,Br,I |
Always appears in doubles |
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Covalent bond |
Created by two atoms sharing electrons. Between 2 non metals |
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Ionic compound |
Oppositly charged ions bound by colombs law |
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Metallic bonding |
Cations suspended in sea of valence electrons. Hold electrons near cations but don't impede flow |
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Metallic bonding properties |
Conductivity Deformation |
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Polarity strengths |
F biggest. Right to left, top to bottom weakens |
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Lattice energy |
The energy that holds ions together |
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Center atom fir Lewis structures? |
Least electronegative except for H |
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Lewis structure -1 means |
Add an electron |
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Lewis structure +1 means |
Lose an electron |
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What to do first to balance an equation |
Look for element that appears only once on both sides |
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London dispersion forces |
Momentary occilations if electron clouds. Non polar. Make atom form temporary dipoles when electrons contact positive nucleus. |
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Where are dispersion forces |
Everywhere in every molecule |
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How do dispersion forces strengthen |
Larger and heavier atoms Molecules that are easily polarized |
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Dipole dipole forces |
Positive pole of one molecule is attracted to the negative pole of the other. Polar |
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Hydrogen bonding |
From electronegativity of N, O, F. Hydrogen is small so the molecules are close. H nucleus exposed due to unequal sharing |
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Ion dipole forces |
Dipole attracted to oppositely charged ion |
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Polar solvents and ion dipole |
Force is stronger in the water (solvent) than the lattice energy in the salt (solute) |
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Dipole dipole forces and boiling point |
Stronger intermolecular forces have higher melting/ boiling points |
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Hydrogen bonds more significant because |
Form extremely strong bonds because H so low and O F N so high |
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Solubility |
Like dissolves like. Polar dissolves polar. Non polar dissolves non polar. Do not react |
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Miscible |
Can be mixed in any proportion like water and alcohol |
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Water solubility |
Polar substances |
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Viscosity |
Increases with stronger intermolecular forces |
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Surface tension |
Molecules attracted by all other molecules in all directions. Pulls towards center. |
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Capillaries |
Forces of cohesive and adhesive battle. If adhesive forces are more, liquid will be drawn up |
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VSEPR theory |
Assumes that pairs of valence electrons are arranged around central atom in a way that minimizes repulsion |
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Trigonal planar |
Flat triangle. Sn 3. 2 atoms= bent 120° |
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Tetrahedal |
3d pyramid. Sn 4. 109.5° 3 atoms= pyramidal 109.5° 2 atoms= bent 109.5° |
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Trigonal bipyramidal |
Sn 5. 90° 120° |
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Octahedral |
Sn 6. 90° |
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Solids |
Closer together and structured |
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Liquids |
Not structured but close togetherish |
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Gases |
No structure. Lots of space |
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Phase diagram, triple point |
Where solid liquid gas meet |
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Vapor pressure |
Partially liquid/gas etc. Half and half |
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Hybridization |
Double bonds, switch out a p orbital for d. After 5 p orbitals need a d orbital. Only 1 s orbital. Go by stearic number |
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Trigonal bipyramidal missing atoms |
4 atoms = seesaw 90° 120° 3 atoms= t shape 90° 2 atoms= linear 180° |
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Octahedral is missing atoms |
5 atoms= square pyramidal 90° 4 atoms= spare planar 90° |
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Covalent bond with out Roman numerals |
Cd, Zn, Hg |
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Exceptions to octet rule |
1. Period three can have more 2. Hydrogen, boron and beryllium 3. Odd number of electrons |
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Fluorine a bitch why |
Can only have one electron sharing |
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Lattice energy |
Double bonds strongers than single |
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More electronegative |
Pokariz.ed and bigger |
