General Chemistry Flashcards
1
Q
Nitrate Ion
A
NO3-
2
Q
Nitrite Ion
A
NO2-
3
Q
Thiosulphate Ion
A
S2O32-
4
Q
Sulphate Ion
A
SO42-
5
Q
Sulfite Ion
A
SO32-
6
Q
Sulphide Ion
A
S2-
7
Q
Carbonate Ion
A
CO32-
8
Q
Hydrogen Carbonate Ion
A
HCO3-
9
Q
Phosphate Ion
A
PO43-
10
Q
Hydroxide Ion
A
OH-
11
Q
Oxide Ion
A
O2-
12
Q
Nitric Acid
A
HNO3
13
Q
Nitrous Acid
A
HNO2
14
Q
Sulphurous Acid
A
H2SO3
15
Q
Dihydrogen Sulphide
A
H2S
16
Q
Carbonic Acid
A
H2CO3
17
Q
Phosphoric Acid
A
H3PO4
18
Q
The Four Halide Ions
A
Flouride (F-)
Chloride (Cl-)
Bromide (Br-)
Iodide (I-)
19
Q
Chromate Ion
A
CrO42-
20
Q
Dichromate Ion
A
Cr2O72-
21
Q
Permanganate Ion
A
MnO4-
22
Q
Hydrogen Fluoride
A
HF
23
Q
Hydrogen Chloride
A
HCL
24
Q
Ammonium Ion
A
NH4+
25
Iron(II) Ion
Fe2+
26
Iron(III) Ion
Fe3+
27
Mercury(I) Ion
Hg22+
28
Mercury(II) Ion
Hg2+
29
Zinc Ion
Zn2+
30
Alkali Metals
Group 1 Elements
Form Me+ Ions
31
Alkali Earth Metals
Group 2 Elements
Form Me2+ Ions
32
Density (ρ) Units
g/dm3
33
Mass Concentration Unit
g/dm3
34
Mass Fraction Unit
g/g
35
What are the conjugated acid and base pair of water
Acid: H3O+ Base: OH-
36
What is the Tyndall-effect
Scattering the light on the colloid size particles
37
Define the bond order. How much is it for O2 molecule.
*The half of the difference between the number of bonding and antibonding electrons in the given molecule.*
For O2: (10-6)/2 = 2
38
Write the base dissociation constant, Kb (Equation) for ammonia in water?
Kb = [NH4+][OH-]/[NH3] mol/dm3
39
Write the ideal gas law and name the symbols.
**p•V = n•R•T**
* p=Pressure,*
* V=Volume,*
* T=Temperature,*
* n=Mole number,*
* R=Universal gas constant*
40
Give a typical example for a complex formation (balanced reaction) with hydroxide ion as aligand!
4Na**OH** + ZnSO4 = Na2[Zn(**OH**)4] + Na2SO4
41
Give the formulas of three oxyacids of phosphorus
H3PO2
H3PO3
H3PO4
42
SnCl4
Tin (IV) Chloride
43
Al2O3
Aluminium (III) Oxide
44
KH2PO4
Potassium Dihydrogenphosphate
45
N2H4
Hydrazine
46
Give the formula for mercury(II) amido-chloride
Hg(NH2)Cl
47
Give the formula for Orthophosphate ion
PO43-
48
Write the reaction for potsassium iodide and acidic hydrogen peroxide (with sulphuric acid)
2KI + H2O2 + H2SO4 → I2 + K2SO4 + 2H2O
49
How can sulphide ions be detected?
Lead Ions (PbS [Black ppt.])
50
How can barium ions be detected?
Sulphate ions (BaSO4 [White ppt.])
51
Give an example of a chalcogen
Oxygen (O2)
52
N2O5
Dinitrogen pentoxide
53
N2O5 + H2O =
2 HNO3
54
Detect oxoacids of nitrogen with
Griess-Ilosvay reagent
55
Phosphorus (V) Oxide
P4O10 white solid, strong dehydrating agent
56
Phosphonic Acid
H3PO3, dibasic, reducing agent
57
Give two soluble gases
Nitric Oxide, Carbon monoxide
58
What does amphoteric mean? Give an example.
A compound that can react as an acid and a base, Zinc.
59
Calculate pressure
Pressure = Force/Area (Pascals)
60
Pressure is measured with a…
Barometer
61
Boyle's Law
PV = k = P1V1=P2V2
62
Charles' Law
At constant pressure, the volume of any samle of gas varies with tempereature
63
Ideal Gas Law
P•V = n•R•T
(R=8.3143 J/mol•K)
64
What is Critical pressure?
The minimum pressure needed to liquefy a gas at its critical temperature
65
What is critical temperature?
The temperature above which it is impossible to liquefy the gas
66
Compressed gases allowed to expand causing cooling
Joule-Thompson Effect
67
Equilibrium Vapour Pressure
Pressure of vapour in equilibrium with a liquid
68
Henry's Law
C = Kh • p
69
Calculate osmotic pressure
π= c•R•T
70
In rate law, what is 'k'?
The Rate Constant - Characteristic for each reaction; Depends on the temperature exclusively
71
Formula for the first order reactions
Unit: 1/s
72
Formula for the second order reactions
Unit: dm3/mol•s
73
Formula for half life of first order reaction.
74
Formula for half life of second order reaction.
75
Give the Arrhenius Equation
76
What is Molecularity?
The number of molecules that participate in a single step
77
How is the overall rate of a multistep reaction determined
By the slowest Step
78
Formula for the law of mass action
79
80
Formula to calculate the solubility product
81
Solubility product for NaCl
37.2
82
Calculate the ionic prouduct of water
83
Calculate heat capacity
84
Second law of thermodynamics
The entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process.
85
Formula for the first law of thermodynamics
* q= heat absorbed from the surroundings *
* w= work done by the system*
86
Formula for Gibbs free energy
G = H-T•S
## Footnote
* H= enthalpy*
* T= Kelvin temp.*
* S=Entropy*
87
Give the reaction of a galvanic cell with Copper and Zinc.
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
88
Where does oxidation occur in a voltaic cell?
The Anode
## Footnote
*Loss of electrons*
89
What is corrosion?
Where metals are oxidised to their oxides and sulfides
90
Formula to calculate the mass of discharged substances
* M: Molecular Mass*
* z: Number of electrons involved*
* Q: Quantity of electric charge used*
* F: Faraday*
91
What is the Tyndall-Effect?
The scattering of light by colloidal particles in a liquid
92
Name three stabilising factors for colloids (Allows coagulation of colloids)
Electrical charge
Hydration
Protective colloids
93
What is 'Hard Water'?
Water containing a high amount of calcium and magnesium ions
94
**Give an example of a protective colloid**
**Protein Polysaccharide**
