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Dr. Collins Pcat Chem > Part 1- Inorganic Chemistry > Flashcards

Part 1- Inorganic Chemistry Flashcards

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1
Q

Hydroxide

A

OH 1-

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2
Q

Carbonate

A

CO3 2-

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3
Q

Perchlorate

A

ClO4 1-

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4
Q

Cyanide

A

CN 1-

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5
Q

Bicarbonate

A

HCO3 1-

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6
Q

Chlorate

A

ClO3 1-

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7
Q

Sulfate

A

SO4 2-

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8
Q

Peroxide

A

O2 2-

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9
Q

Chlorite

A

ClO2 1-

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10
Q

Phosphate

A

PO4 3-

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11
Q

Superoxide

A

O2 1-

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12
Q

Hypochlorite

A

ClO 1-

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13
Q

Nitrate

A

NO3 1-

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14
Q

Permanganate

A

MnO4 1-

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15
Q

Ammonium

A

NH4 1+

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16
Q

IA IIA

A

Na 1+ K 1+ Mg 2+ Ca 2+ Ba 2+

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17
Q

Important B group element

A

Fe 2+ or Fe 3+ Co 2+ or Co 3+ Ni 2+ Zn 2+ Ag 1+

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18
Q

IIIA VIA

A

Al 3+ O 2- S 2-

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19
Q

VIIA

A

F 1- Cl 1- Br 1- I 1-

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20
Q

Electron shell

A

1s, 2s, 3s, 4s, 5s, 6s, 7s

2p, 3p, 4p, 5p, 6p, 7p

3d, 4d, 5d, 6d, 7d

4f, 5f, 6f, 7f

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21
Q

Pv=nRT

A

P, Pressure if in mmHg or torr divide it by 760

R, gas constant .082 L atm/mole

K n, number of moles T, temperature kelvin if in C ad 273

V, is volume is in L

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22
Q

Dalton’s law of partial pressures

A

The total pressure of a gas is a simple sum of the partial pressures of the individual gases that are present in the gas mixture

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23
Q

London forces (Van Der Waal’s forces)

A

Are the weakest intermolecular forces Are by which the means by which neutral, non-polar molecules attract each other.

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24
Q

Dipole dipole

A

Polar molecules attract each other strong

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25
Q

Hydrogen bonding

A

Very strong F, O, or N Polar molecules

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26
Q

Diatomic atoms

A

Not polar example H2 O2 N2 F2 Cl2 Br2 I2

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27
Q

Water

A

H2O Bent polar Hydrogen bonding

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28
Q

Carbon dioxide

A

CO2 Linear non-polar

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29
Q

Sulfur dioxide

A

Bent and polar SO2

30
Q

Sulfur trioxide

A

Trigonal planar and non polar SO3

31
Q

Ammonia

A

NH3 Pyramidal and polar and hydrogen bonding

32
Q

Methane

A

Tetrahedral and non polar

33
Q

Sulfur hexafluoride

A

SF6 Octahedral and non polar

34
Q

Ionic bonds

A

1) metal/nonmetal NaCl 2) common polyatomic ions NH4NO3, NH4Cl

35
Q

Strength of intermolecular forces

A

Ion-ion > h-bonding > dipole-dipole > London

36
Q

Stronger IMF mean

A

Higher boiling and meting

37
Q

Size on IMF

A

Neutral, nonpolar atoms- larger molecules the stronger attraction Polar molecules- smaller molecules the stronger the attraction

38
Q

homogenous

A

completely uniform (sugar dissolved in water)

39
Q

solvent solute

A

solvent= the which does the dissolving solute= being dissolved solution always takes on the physical state of the solvent

40
Q

concentration

A

solute/solvent

41
Q

Molarity

A

moles of solute/ V of solution in L Moles x V(L)= # of moles Moles x M(ml) = # of mmoles

42
Q

colligative properties raoult’s law

A

solution value is based on number of solutes molecules not the nature of the solute molecules example: adding non-volatile to volatile solvent lowest he vapor pressure. P= Xsolvent x P degree

  • Xsolvent= mole fraction of the solvent, (moles of solvent is moles of solvent/total moles of solution)
  • P is vapor pressure
  • P degree is vapor pressure of solvent
43
Q

boiling point elevetation freezing point

A

delta Tb= Kb x m delta Tb= how much boiling point elevated Kb= constant characteristic of solvent how much the boiling point is elevated per unit of molarity m= molarity of solute add this amount to the regular BP of water or solution….. this will give you the new BP delta Tf= Kf x m subtract this form regular freezing temp for new temp

44
Q

greatest colligative effect

A

the greatest colligative effect is the solution with the largest solute concentration this includes lowest vapor pressure or highest BP, or the lowest FP or the largest osmotic pressure

45
Q

osmotic pressure

A

the flow of solvent through a semi-permeable membrane, in an effort to equalize concentration proportional to solute concentration…. so more concentraiton, more ion the better. like KCl vs. K2SO4

46
Q

solute concentration

A

ionic solutes (electrolytes) - will have a greater concentration than non-ionic solutes (non-electrolytes)

47
Q

common strong electrolyte solute

A

water soluble strong acids- HCl, HNO3, H2SO4 water soluble strong bases- NaOH, KOH Water soluble salts- NaCl, KNO3, K2SO4

48
Q

common weak electrolyte solutes

A

water soluble molecular weak acids- CH3COOH water soluble molecular weak bases- NH3

49
Q

Common non-electrolyte solutes

A

glucose C6H12O6 or sucrose sugar alcohols such as methanol CH3OH

50
Q

common strong acid

A

hydrochloric acid HCL nitric acid HNO3 Sulfuric acid H2SO4 Perchloricacid HClO4

51
Q

common weak acid

A

acetic acid HC2H3O2 or CH3COOH carbonic acid H2CO3 hydrofluoric acid HF phosphoric acid H3PO4

52
Q

common strong base

A

IA and IIAA hydroxide salts, KOH NaOH etc.

53
Q

common weak bases

A

NH3

54
Q

calorie

A

defined as the energy needed to raise the temperature of one gram of liquid water by one degree Celcius

55
Q

joule

A

is the SI unit of energy and is defined as one cal= 4.18 J

56
Q

SH specific heat

A

is defined as the heat needed to raise the temperature of one gram of the substance by one degree Celsius SH of h2o = 1 cal/g degrec celsius= 4.18 J/g degree celsius

57
Q

heat calculations involving no change in physical state

A

q (heat)= mass x SH x change in temp

58
Q

heat of fusion

A

q (FUS) amount of heat needed to convert one gram of solid to liquid at the substance’s melting point water q (fus)= 80 cal/g= 334 J/q

59
Q

heat of vaporation

A

amount of heat needed to convert one gram of liquid to vapor at the liquid’s boiling point q vap= 540 cal/g= 2260 J/g

60
Q

entropy

A

delta s positive- disorder increases

negative- disorder decrease

change in delta is= product- reactant

61
Q

enthalpy

A

delta H, heat change in the reaction exothermic- negative endothermic- positive

62
Q

gibbs free energy delta G

A

delta G= delta H - T delta S

63
Q

what is not in the equilibrium

A

solids, pure liquids and water

64
Q

LeChatelier’s principle

A
  1. changes in concentration 2. changes in pressure 3. changes in temperature
65
Q

decrease in pressure

A

equalibritim will shift to the side with more moles of gase this change means there is an increase in volume

66
Q

anhydride

A

formed by the removal of one of H2O from the molecuels H2SO4 turning into SO3 plus H20

67
Q

what phsyical state does helium fail to exhibit

A

solid

68
Q

sublimation deposition

A

sublimation= solid to gas deposition= gas to solid

69
Q

K(sp)

A

smaller K(sp) the less soluble the slat will be

70
Q

one salt disolving in pure water

A

x=solubilty= sq(K(sp))

71
Q

common ion effect

A

if salt is initially present in solution, the solubility of the salt in the solution will be significantly less than its solubility in pure water

72
Q

oxidation reduction ocurres to waht

A

oxidation occurs to anod reduction occurs to cathode

Dr. Collins Pcat Chem (9 decks)

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