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239 Terms

1

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equation for density of gas

p= PM/RT

p= density of gas (g x L^-1)

P= pressure (atm)

M= molar mass (g)

R= ideal gas constant [0.0821 (L x atm/mol x K)]

T= temperature (K)

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2

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diatomic ions

hydrogen, nitrogen, oxygen, bromine, chlorine, iodine, fluorine

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3

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allotropes

molecules with different formulas whose atoms are all of the same element (ex. O2 and O3; S6, S8, and S12)

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4

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charge of NH4==+== (ammonium)

+1

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5

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charge of H3O==+== (hydronium)

+1

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6

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charge of Hg22+ (mercury I)

+1

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7

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charge of H2PO3==-== (dihydrogen phosphite)

-1

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8

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charge of H2PO4==-== (dihydrogen phosphate)

-1

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9

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charge of HCO3==-== (hydrogen carbonate)

-1

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10

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charge of HSO3==-== (hydrogen sulfite)

-1

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11

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charge of HSO4==-== (hydrogen sulfate)

-1

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12

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charge of NO2==-== (nitrite)

-1

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13

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charge of NO3==-== (nitrate)

-1

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14

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charge of OH==-== (hyrdoxide)

-1

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15

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charge of CH3COO==-== (acetate)

-1

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16

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charge of CrO2==-== (chromite)

-1

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17

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charge of CN==-== (cyanide)

-1

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18

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charge of CNO==-== (cyanate)

-1

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19

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charge of CNS==-== (thiocyanate)

-1

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20

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charge of MnO4==-== (permanganate)

-1

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21

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charge of ClO==-== (hypochlorite)

-1

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22

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charge of ClO2==-== (chlorite)

-1

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23

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charge of ClO3==-== (chlorate)

-1

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24

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charge of ClO4==-== (perchlorate)

-1

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25

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charge of BrO==-== (hypobromite)

-1

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26

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charge of BrO2==-== (bromite)

-1

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27

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charge of BrO3==-== (bromate)

-1

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28

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charge of BrO4==-== (perbromate)

-1

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29

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charge of IO==-== (hypoiodite)

-1

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30

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charge of IO2==-== (iodite)

-1

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31

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charge of IO3==-== (iodate)

-1

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32

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charge of IO4==-== (periodate)

-1

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33

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charge of N3==-== (azide)

-1

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34

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charge of HPO32- (hydrogen phosphite)

-2

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35

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charge of HPO42- (hydrogen phosphate)

-2

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36

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charge of CO32- (carbonate)

-2

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37

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charge of SO32- (sulfite)

-2

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38

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charge of SO42- (sulfate)

-2

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39

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charge of S2O32- (thiosulfate)

-2

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40

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charge of C2O42- (oxalate)

-2

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41

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charge of CrO42- (chromate)

-2

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42

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charge of Cr2O72- (dichromate)

-2

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43

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charge of O22- (peroxide)

-2

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44

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charge of S22- (disulfide)

-2

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45

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charge of O2- (oxide)

-2

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46

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charge of S2- (sulfide)

-2

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47

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charge of PO43- (phosphate)

-3

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48

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charge of AsO33- (arsenite)

-3

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49

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charge of AsO43- (arsenate)

-3

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50

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charge of N3- (nitride)

-3

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51

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SI unit: terra

10^12

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52

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SI unit: giga

10^9

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53

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SI unit: mega

10^6

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54

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SI unit: kilo

10^3

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55

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SI unit: centi

10^-2

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56

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SI unit: milli

10^-3

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57

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SI unit: micro

10^-6

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58

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SI unit: nano

10^-9

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59

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p-orbitals have __ shapes/p-orbitals per shell

3

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60

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d-orbitals have __ shapes/p-orbitals per shell

5

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61

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f-orbitals have __ shapes/p-orbitals per shell

7

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62

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quantum numbers formula

n, l, ml, ms

n= principal; the energy level/distance from nucleus; range is 1-infinity

l= azimuthal; the type of orbital it is (l=0=s, l=1=p, l=2=d, l=3=f); range is 0, 1, 2, or 3

ml= magnetic; shares which p, d, or f orbital you have (oriental space); range is [-l -→ +l]

ms= spin; shares the electrons spin; range is either +1/2 or -1/2

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63

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paramagnetic

has unpaired electrons, attracted to magnets, odd or even number of electrons (ex. O2)

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64

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diamagnetic

has no unpaired electrons, repelled by magnets, even number of electrons (ex. N2)

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65

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equation for the energy of a photon

E photon= hf= hc/w

h= Planck’s constant= 6.63 x 10^-34 J x sec

f= photon’s frequency= c/w

c= speed of light= 3.0 x 10^8 m/sec

w= photon’s wavelength

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66

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kinetic energy of electrons equation

E photon- work function

work function= the minimum amount of energy required to ionize the electrons

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67

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types of compounds

ionic, molecular, network covalent, and metallic

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68

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features of ionic compounds

high melting points, high boiling points, brittle, hard, held together by ionic interactions (lattice energy), examples include NaCl and MgO

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69

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features of molecular compounds

low melting points, do not conduct electricity, held together by IMFs, examples include H2O and Cl-Cl and CH2

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70

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features of network covalent compounds

high melting points, high boiling points, hard, do not conduct electricity, held together by a network of covalent bonds, examples include C (diamond and graphite) and SiO2 (quartz)

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71

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features of metallic compounds

variable hardness and melting points, conducts electricity, conducts heat, lustrous (shiny), malleable, ductile, held together by metallic bonding, examples include Fe and Mg

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72

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lattice energy equation

[(cation charge) x (anion charge)]/bond distance

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73

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if there are two “things” surrounding the atom…

electron domain: 2

hybridization: sp

bond angles: 180 degrees

electron-domain geometry: linear

non-bonding electron pairs: 0

molecular geometry: linear

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74

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if there are three “things” surrounding the atom…

electron domain: 3

hybridization: sp2

bond angles: 120 degrees

electron-domain geometry: trigonal planar

non-bonding electron pairs: 0 or 1

molecular geometry: trigonal planar or bent

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75

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if there are four “things” surrounding the atom…

electron domain: 4

hybridization: sp3

bond angles: 109.5 degrees

electron-domain geometry: tetrahedral

non-bonding electron pairs: 0, 1, or 2

molecular geometry: tetrahedral, trigonal pyramid, bent

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76

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if there are five “things” surrounding the atom…

electron domain: 5

hybridization: sp3d

bond angles: 90, 120, or 180 degrees

electron-domain geometry: trigonal bipyramid

non-bonding electron pairs: 0, 1, 2, or 3

molecular geometry: trigonal bipyramid, see-saw, t-shaped, linear

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77

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if there are six “things” surrounding the atom…

electron domain: 6

hybridization: sp3d2

bond angles: 90 degrees

electron-domain geometry: octahedral

non-bonding electron pairs: 0, 1, or 2

molecular geometry: octahedral, square pyramid, square planar

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78

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features to know about alkali metals

group 1 on PT, low ionization energies, very reactive with water, readily form compounds

reaction with water: M (s) + H2O (l) -→ MOH (aq) + 1/2H2 (g); VERY exothermic reaction

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79

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features to know about alkaline earth metals

group 2 on PT, low ionization energies (not as low as alkali metals), reacts with H2O (not as violently as alkali metals), becomes more reactive with H20 as you go down the group

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80

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features to know about halogens

group 7A on PT, high electronegativities and electron affinities, easily reduced because they really want an extra electron, highly reactive with metals, good oxidizing agents

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81

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features to know about noble gases

group 8 on PT, unreactive gases, they have a full octet so are happy

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82

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features to know about transition metals

found in the d-block of PT, often form brightly colored compounds, can have multiple oxidation states

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83

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features to know about oxygen group/chalcogens

group 6A on PT, two forms of molecular oxygen: O2 and O3, metals like to react with oxygen to form metal oxides

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84

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boyle’s law

as pressure decreases, volume increases and vice versa

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85

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charles’ law

as volume decreases, temperature decreases; as volume increases, temperature increases

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86

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avogadro’s law

as volume decreases, the number of moles decreases; as volume increases, the number of moles increases

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combined gas law

P1 x V1/n1 x T1=P2 x V2/ n2 x T2

P= pressure

V= volume

n= number of moles

T= temperature

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ideal gas law

PV=nRT

P= pressure (atm)

V= volume (L)

n= number of moles

R= ideal gas constant= 0.0821 L x atm/ mol x K

T= temperature (Kelvins)

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89

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Heisenberg uncertainty principle

you cannot simultaneously know everything about an electron’s location and momentum

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90

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dalton’s law

total pressure inside a container filled with multiple gases = sum of the gases’ individual pressures

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91

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kinetic energy equation

(1/2 x mass) x (velocity)^2

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92

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graham’s law

effusion rate 1/effusion rate 2= sqaure root of mw2/mw1

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93

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unit cells: simple cubic

only one total atom inside the cell

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94

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unit cells: body centered cubic

two atoms per cell

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95

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unit cells: face centered cubic

four atoms per cell

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96

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sublimation

solid -→ gas (endothermic, +deltaH; create disorder, +deltaS)

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97

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melting (fusion)

solid -→ liquid (endothermic, +deltaH; create disorder, +deltaS)

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98

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boiling (vaporization)

liquid -→ gas (endothermic, +deltaH; create disorder, +deltaS)

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99

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deposition

gas -→ solid (exothermic, -deltaH; create order, -deltaS)

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100

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condensation

gas -→ liquid (exothermic, -deltaH; create order, -deltaS)

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