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Chemistry I > General Chemistry > Flashcards

General Chemistry Flashcards

1
Q

Nitrate Ion

A

NO3-

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2
Q

Nitrite Ion

A

NO2-

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3
Q

Thiosulphate Ion

A

S2O32-

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4
Q

Sulphate Ion

A

SO42-

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5
Q

Sulfite Ion

A

SO32-

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6
Q

Sulphide Ion

A

S2-

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7
Q

Carbonate Ion

A

CO32-

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8
Q

Hydrogen Carbonate Ion

A

HCO3-

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9
Q

Phosphate Ion

A

PO43-

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10
Q

Hydroxide Ion

A

OH-

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11
Q

Oxide Ion

A

O2-

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12
Q

Nitric Acid

A

HNO3

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13
Q

Nitrous Acid

A

HNO2

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14
Q

Sulphurous Acid

A

H2SO3

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15
Q

Dihydrogen Sulphide

A

H2S

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16
Q

Carbonic Acid

A

H2CO3

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17
Q

Phosphoric Acid

A

H3PO4

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18
Q

The Four Halide Ions

A

Flouride (F-)

Chloride (Cl-)

Bromide (Br-)

Iodide (I-)

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19
Q

Chromate Ion

A

CrO42-

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20
Q

Dichromate Ion

A

Cr2O72-

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21
Q

Permanganate Ion

A

MnO4-

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22
Q

Hydrogen Fluoride

A

HF

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23
Q

Hydrogen Chloride

A

HCL

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24
Q

Ammonium Ion

A

NH4+

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25
Q

Iron(II) Ion

A

Fe2+

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26
Q

Iron(III) Ion

A

Fe3+

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27
Q

Mercury(I) Ion

A

Hg22+

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28
Q

Mercury(II) Ion

A

Hg2+

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29
Q

Zinc Ion

A

Zn2+

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30
Q

Alkali Metals

A

Group 1 Elements

Form Me+ Ions

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31
Q

Alkali Earth Metals

A

Group 2 Elements

Form Me2+ Ions

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32
Q

Density (ρ) Units

A

g/dm3

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33
Q

Mass Concentration Unit

A

g/dm3

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34
Q

Mass Fraction Unit

A

g/g

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35
Q

What are the conjugated acid and base pair of water

A

Acid: H3O+ Base: OH-

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36
Q

What is the Tyndall-effect

A

Scattering the light on the colloid size particles

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37
Q

Define the bond order. How much is it for O2 molecule.

A

The half of the difference between the number of bonding and antibonding electrons in the given molecule.

For O2: (10-6)/2 = 2

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38
Q

Write the base dissociation constant, Kb (Equation) for ammonia in water?

A

Kb = [NH4+][OH-]/[NH3] mol/dm3

39
Q

Write the ideal gas law and name the symbols.

A

p•V = n•R•T

  • p=Pressure,*
  • V=Volume,*
  • T=Temperature,*
  • n=Mole number,*
  • R=Universal gas constant*
40
Q

Give a typical example for a complex formation (balanced reaction) with hydroxide ion as aligand!

A

4NaOH + ZnSO4 = Na2[Zn(OH)4] + Na2SO4

41
Q

Give the formulas of three oxyacids of phosphorus

A

H3PO2

H3PO3

H3PO4

42
Q

SnCl4

A

Tin (IV) Chloride

43
Q

Al2O3

A

Aluminium (III) Oxide

44
Q

KH2PO4

A

Potassium Dihydrogenphosphate

45
Q

N2H4

46
Q

Give the formula for mercury(II) amido-chloride

47
Q

Give the formula for Orthophosphate ion

48
Q

Write the reaction for potsassium iodide and acidic hydrogen peroxide (with sulphuric acid)

A

2KI + H2O2 + H2SO4 → I2 + K2SO4 + 2H2O

49
Q

How can sulphide ions be detected?

A

Lead Ions (PbS [Black ppt.])

50
Q

How can barium ions be detected?

A

Sulphate ions (BaSO4 [White ppt.])

51
Q

Give an example of a chalcogen

A

Oxygen (O2)

52
Q

N2O5

A

Dinitrogen pentoxide

53
Q

N2O5 + H2O =

54
Q

Detect oxoacids of nitrogen with

A

Griess-Ilosvay reagent

55
Q

Phosphorus (V) Oxide

A

P4O10 white solid, strong dehydrating agent

56
Q

Phosphonic Acid

A

H3PO3, dibasic, reducing agent

57
Q

Give two soluble gases

A

Nitric Oxide, Carbon monoxide

58
Q

What does amphoteric mean? Give an example.

A

A compound that can react as an acid and a base, Zinc.

59
Q

Calculate pressure

A

Pressure = Force/Area (Pascals)

60
Q

Pressure is measured with a…

61
Q

Boyle’s Law

A

PV = k = P1V1=P2V2

62
Q

Charles’ Law

A

At constant pressure, the volume of any samle of gas varies with tempereature

63
Q

Ideal Gas Law

A

P•V = n•R•T

(R=8.3143 J/mol•K)

64
Q

What is Critical pressure?

A

The minimum pressure needed to liquefy a gas at its critical temperature

65
Q

What is critical temperature?

A

The temperature above which it is impossible to liquefy the gas

66
Q

Compressed gases allowed to expand causing cooling

A

Joule-Thompson Effect

67
Q

Equilibrium Vapour Pressure

A

Pressure of vapour in equilibrium with a liquid

68
Q

Henry’s Law

A

C = Kh • p

69
Q

Calculate osmotic pressure

A

π= c•R•T

70
Q

In rate law, what is ‘k’?

A

The Rate Constant - Characteristic for each reaction; Depends on the temperature exclusively

71
Q

Formula for the first order reactions

72
Q

Formula for the second order reactions

A

Unit: dm3/mol•s

73
Q

Formula for half life of first order reaction.

74
Q

Formula for half life of second order reaction.

75
Q

Give the Arrhenius Equation

76
Q

What is Molecularity?

A

The number of molecules that participate in a single step

77
Q

How is the overall rate of a multistep reaction determined

A

By the slowest Step

78
Q

Formula for the law of mass action

80
Q

Formula to calculate the solubility product

81
Q

Solubility product for NaCl

82
Q

Calculate the ionic prouduct of water

83
Q

Calculate heat capacity

84
Q

Second law of thermodynamics

A

The entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process.

85
Q

Formula for the first law of thermodynamics

A
  • q= heat absorbed from the surroundings *
  • w= work done by the system*
86
Q

Formula for Gibbs free energy

A

G = H-T•S

  • H= enthalpy*
  • T= Kelvin temp.*
  • S=Entropy*
87
Q

Give the reaction of a galvanic cell with Copper and Zinc.

A

Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)

88
Q

Where does oxidation occur in a voltaic cell?

A

The Anode

Loss of electrons

89
Q

What is corrosion?

A

Where metals are oxidised to their oxides and sulfides

90
Q

Formula to calculate the mass of discharged substances

A
  • M: Molecular Mass*
  • z: Number of electrons involved*
  • Q: Quantity of electric charge used*
  • F: Faraday*
91
Q

What is the Tyndall-Effect?

A

The scattering of light by colloidal particles in a liquid

92
Q

Name three stabilising factors for colloids (Allows coagulation of colloids)

A

Electrical charge

Hydration

Protective colloids

93
Q

What is ‘Hard Water’?

A

Water containing a high amount of calcium and magnesium ions

94
Q

Give an example of a protective colloid

A

Protein Polysaccharide

Chemistry I (5 decks)

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