Non Metal Flashcards
1
Q
Hydrogen Discovery
A
Cavendish (1766)
2
Q
Hydrogen Naming
A
Lavoisier (water-former)
3
Q
Hydrogen in Earth’s Crust
A
~1%
4
Q
Hydrogen in Atmosphere
A
0.01% (small amounts)
5
Q
Hydrogen in Sun/Stars
A
Large amounts
6
Q
Hydrogen in Water
A
One ninth by mass
7
Q
Hydrogen in Acids/Alkalis
A
Important constituent
8
Q
Hydrogen in Natural Gas, etc.
A
Combined with carbon
9
Q
Hydrogen in Organic Substances
A
Proteins, carbohydrates, fats
10
Q
Hydrogen Lab Preparation
A
Metals + dilute acids/water/steam, or Zn/Sn/Al + hot concentrated NaOH/KOH
11
Q
Zinc + HCl
A
$Zn(s)+2HCl(aq)\rightarrow ZnCl_{2}(aq)+H_{2}(g)$
12
Q
Zinc + H2SO4
A
$Zn(s)+H_{2}SO_{4}(aq)\rightarrow ZnSO_{4}(aq)+H_{2}(g)$
13
Q
Ionic Representation
A
$Zn(s)+2H^{+}(3q)\rightarrow Zn^{2+}(aq)+H_{2}(g)$
14
Q
Sodium + Cold Water
A
$2Na(s)+2H_{2}O(l)\rightarrow2NaOH(aq)+H_{2}(g)$ (vigorous reaction)
15
Q
Iron + Steam
A
$3Fe(s)+4{H_{2}O(g)\rightleftharpoons Fe_{3}O}{4}(s)+4H{2}(g)$ (reversible)
16
Q
Front
A
Back
17
Q
Hydrogen Preparation Apparatus (Acid + Zinc)
A
Flat-bottomed flask, delivery tube, gas jar over water
18
Q
Acid Used in Zinc Reaction
A
Dilute hydrochloric or tetraoxosulphate(VI) acid
19
Q
Catalyst for Pure Zinc + Acid
A
Copper(II) tetraoxosulphate(VI) solution
20
Q
Drying Hydrogen Gas
A
Fused calcium chloride or concentrated tetraoxosulphate(VI) acid
21
Q
Collecting Dry Hydrogen
A
Over mercury or by downward displacement of air
22
Q
Sodium + Water Experiment
A
Trough with red litmus-colored water, sodium in sodium-spoon or wire gauze
23
Q
Hydrogen Collection (Sodium + Water)
A
Inverted test-tube over sodium in trough
24
Q
Steam + Iron Experiment
A
Combustion tube with iron filings, flask to generate steam
25
Iron Filings Condition
Red-hot
26
Steam Flow
Constant
27
Hydrogen Collection (Steam + Iron)
Over water
28
Hydrogen + Air Mixture
Explosive when heated
29
First Jar of Hydrogen
Discard (mixture with air)
30
Zinc + Acid Observation
Effervescence of hydrogen gas
31
Sodium + Water Observations
Sodium melts, dissolves, water turns blue (NaOH forms)
32
Residue of Steam + Iron Reaction
Iron(II) diiron(III) oxide ($Fe_3O_4$)
33
Front
Back
34
Industrial Hydrogen Production
From water gas (Bosch process) or methane
35
Bosch Process Raw Materials
Water and coke
36
Bosch Process: Steam + Red-hot Coke
$H_{2}O(g)+C(s)\rightarrow CO(g)+H_{2}(g)$ (endothermic), produces water gas
37
Water Gas Composition
Carbon(II) oxide and hydrogen
38
Bosch Process: Water Gas + Excess Steam
$CO(g)+H_{2}(g)+H_{2}O(g) \rightleftharpoons CO_{2}(g)+2H_{2}(g)$ (exothermic), over iron(III) oxide or chromium(III) oxide catalyst at 450°C
39
Bosch Process: CO2 Removal
Dissolving in water (30 atm) or caustic soda solution
40
Bosch Process: Unreacted CO Removal
Ammoniacal solution of copper(I) ethanoate
41
Methane-based Process
Replaces Bosch, uses methane instead of coke
42
Methane-based Process: Steam + Methane
$CH_{4}(g)+H_{2}O(g)\frac{Ni}{800^{\circ}C}>CO(g)+3H_{2}(g)$ , over nickel catalyst at ~800°C, produces synthesis gas
43
Synthesis Gas Composition
Carbon(II) oxide and hydrogen
44
Electrolytic Hydrogen Production
By-product of electrolysis of brine for NaOH and chlorine, or electrolysis of acidified water/dilute NaOH/KOH
45
Metals that Displace Hydrogen from Water/Acids
More active than hydrogen
46
Metals that DO NOT Displace Hydrogen from Water/Acids
Less active than hydrogen (e.g., Cu, Ag)
47
Activity Series: Vigorous Reaction with Cold Water
K, Na
48
Activity Series: Slow Reaction with Cold Water
Ca
49
Activity Series: Reaction with Steam (Heated)
Mg
50
Activity Series: Reaction with Steam (Red Heat)
Al, Zn, Fe
51
Activity Series: No Reaction with Water/Steam
Pb, Cu
52
Front
Back
53
Activity Series: Order of Decreasing Activity
K, Na, Ca, Mg, Al, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Pt, Au
54
Activity Series and Acids
Metals above H displace hydrogen from acids, below H do not.
55
Activity Series and Electropositivity
Metals high in series are electropositive and chemically active.
56
Activity Series and Metal Displacement
Any metal displaces metals below it from their salt solutions.
57
Hydrogen's Unusual Nature
Has 1 valence electron like Group 1 but is a non-metal gas like Group 7.
58
Hydrogen's Placement in Periodic Table
Usually Group 1, sometimes between Group 1 and 7
59
Hydrogen's Electron Configuration
Achieves stable duplet like helium
60
Hydrogen's Electron Gain
Accepts electron to form hydride ion (H-)
61
Hydrogen's Electron Sharing
Forms covalent bond (H-H)
62
Hydrogen's Electron Donation
Donates electron to form H+ and coordinate bonds (e.g., with $H_2O$ to form $H_3O+$)
63
Hydrogen's Test with Test-tubes
Demonstrates it's lighter than air
64
Test-tube Experiment Setup
4 test-tubes (A, B with H2, C, D with air), remove corks, test with burning splinter
65
Test-tube Result: A, C
Hydrogen rises, displaces air, pop sound in C
66
Test-tube Result: B
Pure hydrogen, burns quietly, pale blue flame, extinguished splinter
67
Test-tube Result: D
Air present, splinter burns, no pop
68
Front
Back
69
Hydrogen Combination Reactions
Forms electrovalent and covalent hydrides
70
Hydrogen's Electron Gain in Reactions
Achieves stable helium configuration
71
Hydrogen + Active Metals
Forms ionic hydrides (H-)
72
$2Na(s)+H_{2}(g)\rightarrow2NaH(s)$
Example of hydrogen + active metal
73
Hydrogen + Oxygen
Pure hydrogen burns with pale blue flame to form steam: $2H_{2}(g)+O_{2}(g)\rightarrow2H_{2}O(g)$
74
Hydrogen + Halogens
Forms halides
75
$Cl_{2}(g)+H_{2}(g)\rightarrow2HCl(g)$
Example of hydrogen + halogen
76
$Br_{2}(g)+H_{2}(g)\rightarrow2HBr(g)$
Another example of hydrogen + halogen
77
Hydrogen + Chlorine Reaction Speed
Spontaneous in bright sunlight, slower in diffused light
78
Hydrogen Reducing Agent Ability
Strong
79
Hydrogen + Metal Oxides
Reduces oxides of Cu, Pb, Fe, Zn to metals, forms water
80
$CuO(s)+H_{2}(\mathfrak{g})\rightarrow Cu(s)+H_{2}O(g)$
Example of hydrogen reducing metal oxide
81
$Fe_{2}O_{3}(s)+3H_{2}(\mathfrak{g})\rightarrow2Fe(s)+3H_{2}O(g)$
Another example of hydrogen reducing metal oxide
82
Front
Back
83
Hydrogen Test
Insert lighted splinter into test-tube
84
Hydrogen Test Result
Pop sound (due to mixing with air)
85
Hydrogen Test Caution
Use small quantities of gas
86
Hydrogen Use: Ammonia, HCl, Methanol
Manufacture
87
Hydrogen Use: Vegetable Oils
Hydrogenation (margarine, etc.)
88
Hydrogen Use: Balloons
Low density
89
Hydrogen Use: Synthetic Petrol
From oil and powdered coal
90
Hydrogen Use: Gaseous Fuels
Water gas, coal gas
91
Hydrogen Use: Rocket Fuel
Liquid hydrogen
92
Hydrogen Use: High Temperatures
Oxy-hydrogen flames (>2000°C)
93
Hydrogen Use: Atomic Hydrogen Flames
Electric arc breaks $H_2$ to H, recombination releases heat
94
Hydrogen Isotopes
Protium (H), Deuterium (D or $^2_1H$), Tritium (T or $^3_1H$)
95
Protium Atomic Mass
1
96
Deuterium Atomic Mass
2
97
Tritium Atomic Mass
3
98
Deuterium vs. Protium
Similar chemistry, less reactive
99
Deuterium Oxide
$D_2O$, heavy water, 1.1x heavier than $H_2O$
100
Tritium Property
Radioactive
101
Front
Back
102
Ionic Hydrides
Formed by alkali and alkali-earth metals with hydrogen
103
Ionic Hydride Properties
Crystalline solids, high melting points, conduct electricity (molten)
104
Ionic Hydride Reaction with Water
Forms hydroxides and hydrogen gas
105
$CaH_{2}(s)+2H_{2}O(l)\rightarrow Ca(OH)_{2}(aq)+2H_{2}(g)$
Example of ionic hydride reaction with water
106
Ionic Hydride Reaction (Ionic)
$H^{-}(s)+H_{2}O(l)\rightarrow OH^{-}(aq)+H_{2}(g)$
107
Complex Covalent Hydrides
Formed by Boron and aluminium
108
Complex Covalent Hydride Use
Reducing agents (organic chemistry)
109
Examples of Complex Hydrides
Lithium tetrahydridoaluminate(III), sodium tetrahydridoborate(III)
110
Simple Covalent Hydrides
Formed by most non-metallic elements (e.g., chlorine, nitrogen)
111
Simple Covalent Hydride State
Volatile gases (at room temperature)
112
Exceptions to Simple Covalent Hydride State
HF, $H_2O$ (liquids, hydrogen bonding)
113
Hydrides of Electronegative Elements
Form acidic solutions with water (e.g., chlorine, sulphur)
114
Front
Back
115
Halogens Group
Group 7 of the Periodic Table
116
Halogens Valence Electrons
Seven
117
Halogens Reactivity
Very reactive non-metals
118
Chlorine Discovery
Scheele (1774)
119
Chlorine Naming
Davy (1810), from Greek 'chloros' (greenish-yellow)
120
Chlorine Occurrence
Combined state as chlorides
121
Most Abundant Chloride
Sodium chloride (common salt)
122
Chlorine Lab Preparation
Oxidation of concentrated hydrochloric acid
123
Oxidizing Agents for HCl Oxidation
Manganese(IV) oxide, potassium tetraoxomanganate(VII), lead(IV) oxide
124
MnO2 + HCl Reaction
$MnO_{2}(s)+4HCl(aq) \xrightarrow{heat} MnCl_{2}(aq)+2H_{2}O(l)+Cl_{2}(g)$
125
MnO2 + HCl Reaction (Ionic)
$Mn^{4+}(O^{2-})_{2}(s)+4H^{+}(aq)+2Cl^{-}(aq) \rightarrow Mn^{2+}(aq)+2H_{2}O(l)+Cl_{2}(g)$
126
Alternative Chlorine Preparation
$2NaCl(s)+MnO_{2}(s)+2H_{2}SO_{4}(aq) \rightarrow Na_{2}SO_{4}(aq)+MnSO_{4}(aq)+2H_{2}O(l)+Cl_{2}(g)$
127
Alternative Chlorine Preparation (Ionic)
$2Cl^{-}(s)+Mn^{4\div}(O^{2-})_{2}(s)+4H^{+}(aq) \rightarrow Mn^{2+}(aq)+2H_{2}O(l)+Cl\cdot\frac{1}{2}$
128
KMnO4 + HCl Reaction
$2KMnO_{4}(aq)+16HCl(aq) \rightarrow 2MnCl_{2}(aq)+2KCl(aq)+8H_{2}O(l)+5Cl=\frac{1}{3}$
129
KMnO4 + HCl Reaction (Ionic)
$2MnO_{4}^{-}(aq)+16H^{+}(aq)+10Cl^{-}(aq) \rightarrow 2Mn^{2+}(aq)+8H_{2}O(l)+5Cl_{2}(\underline{g})$
130
Front
Back
131
Industrial Chlorine Production
Electrolysis of brine or molten chlorides
132
Brine Electrolysis Products
Chlorine (anode), hydrogen and sodium hydroxide (cathode)
133
Brine Electrolysis Equation
$2NaCl(aq)+2H_{2}O(l)\xrightarrow{electricity}2NaOH(aq)+H_{2}(g)+Cl_{2}(g)$
134
Molten Chloride Electrolysis
Chlorine at anode, metal at cathode
135
Physical State of Chlorine
Gas
136
Chlorine Color
Greenish-yellow
137
Chlorine Smell
Unpleasant, choking
138
Chlorine Solubility in Water
Moderate
139
Chlorine Density
2.5 times denser than air
140
Chlorine Liquefaction
Easily liquefied under pressure (~6 atm)
141
Chlorine Toxicity
Poisonous, damages mucous lining of lungs
142
Chlorine Valence Electrons
Seven
143
Chlorine Reactivity
Very reactive
144
Chlorine Electron Gain
Forms Cl- ion in electrovalent compounds
145
Chlorine Electron Sharing
Forms single covalent bond
146
Front
Back
147
Chlorine's Dual Bonding Ability
Gains an electron (Cl-) or shares electrons (Cl-Cl, H-Cl)
148
Chlorine's Displacement Ability
Displaces other halogens (except fluorine) from their compounds
149
Reason for Chlorine's Displacement
More reactive than the halogen it replaces
150
Chlorine Displacement Example
$Cl_{2}(g)+2NaBr(aq)\rightarrow2NaCl(aq)+Br_{2}(l)$
151
Chlorine Displacement with HI
$Cl_{2}(g)+2HI(aq)\rightarrow2HCl(aq)+I_{2}(s)$
152
Chlorine Displacement with NaI
$Cl_{2}(g)+2NaI(aq)\rightarrow2NaCl(aq)+I_{2}(s)$
153
Chlorine's Direct Combination
Reacts directly with most elements to form chlorides
154
Chlorine + Metals
Forms corresponding chlorides (often with heating)
155
Chlorine + Sodium Equation
$2Na(s)+Cl_{2}(g)\rightarrow2NaCl(s)$
156
Chlorine + Zinc Equation
$Zn(s)+Cl_{2}(g)\rightarrow ZnCl_{2}(s)$
157
Chlorine + Iron Equation
$2Fe(s)+3Cl_{2}(g)\rightarrow2FeCl_{3}(s)$
158
Anhydrous Metallic Chloride Preparation
Direct combination of metal and chlorine
159
Chlorine and Variable Metal Chlorides
Forms the higher chloride (e.g., FeCl3, not FeCl2)
160
Chlorine + Non-metals
Non-metals burn in chlorine to form chlorides (except noble gases, O2, N2, C)
161
Front
Back
162
Hydrogen + Chlorine Reaction Condition
Explosive in bright sunlight
163
Hydrogen + Chlorine Reaction Speed in Diffused Light
Slower
164
Hydrogen + Chlorine Product
$H_{2}(g)+Cl_{2}(g)\rightarrow2HCl(g)$
165
Hydrogen + Hydrocarbons
Chlorine removes hydrogen, forms soot and HCl
166
Turpentine + Chlorine Reaction
$C_{10}H_{16}(l)+8Cl_{2}(g)\rightarrow1OC(s)+16HCl(g)$
167
Chlorine + Burning Hydrocarbons
Forms HCl fumes and soot
168
Chlorine + Saturated Hydrocarbons
Substitution reaction, forms chlorinated hydrocarbons and HCl
169
Methane + Chlorine Example
$CH_{4}(g)+Cl_{2}(g)\rightarrow CH_{3}Cl(g)+HCl(g)$
170
Chlorine + Ammonia Reaction
$2NH_{3}(g)+3Cl_{2}(g)\rightarrow N_{2}(g)+6HCl(g)$
171
Chlorine + Excess Ammonia Product
Ammonium chloride ($NH_4Cl$)
172
Chlorine + Hydrogen Sulphide Reaction
$H_{2}S(g)+Cl_{2}(g)\rightarrow2HCl(g)+S(s)$
173
Chlorine + Water Reaction
$Cl_{2}(\mathfrak{g})+H_{2}O(l)\rightarrow HCl(aq)+HOCl(aq)$
174
Chlorine Water in Sunlight Product
Oxygen ($O_2$)
175
Chlorine's Oxidizing Ability
Strong
176
Chlorine's Oxidizing Action
Removes hydrogen, accepts electrons
177
Front
Back
178
Chlorine as a Bleaching Agent
Bleaches most dyes/inks (except carbon-based) in the presence of water
179
Chlorine's Bleaching Mechanism
Forms unstable oxochlorate(I) acid (HOCl), releases oxygen to oxidize the dye
180
HOCl Decomposition
$HOCl(aq)\rightarrow HCl(aq)+[O]$
181
Bleaching Equation
$Dye+[O]\rightarrow(Dye+O)$ (colored to colorless)
182
Chlorine + Dilute Alkali Product
холодный разбавленный раствор гидроксида натрия, бледно-желтоватая смесь оксохлората(I) и хлорида металла.
183
Chlorine + Dilute NaOH Equation
$Cl_{2}(g)+2NaOH(aq)\rightarrow NaOCl(aq)+NaCl(aq)+H_{2}O(l)$
184
Chlorine + Dilute Alkali Ionic Equation
$Cl_{2}(g)+20H^{-}(aq)\rightarrow OCl^{-}(aq)+Cl^{-}(aq)+H_{2}O(l)$
185
Bleaching Powder Formation
Chlorine + slaked lime
186
Bleaching Powder Equation
$Cl_{2}(g)+Ca(OH)_{2}(s)\rightarrow CaOCl_{2}.H_{2}O(s)$
187
Chlorine + Concentrated Alkali Product
Горячий концентрированный раствор гидроксида натрия, смесь триоксохлората(V) и хлорида металла.
188
Front
Back
189
Chlorine + Hot Concentrated Alkali
$Cl_{2}(g)+6NaOH(aq) \xrightarrow{hot, conc.} 5NaCl(aq)+NaClO_{3}(aq)+3H_{2}O(l)$
190
Chlorine as a Disinfectant
Kills bacteria and germs in water
191
Chlorine Uses
Bleaching, sterilizing water, manufacturing HCl, plastics, etc.
192
Test for Chlorine
Bleaches damp litmus paper
193
Chlorine Test Result
Paper turns red then colorless
194
Chlorine Test Mechanism
Forms HCl and HOCl, HOCl releases oxygen that bleaches
195
Front
Back
196
Nitrogen Discovery
Daniel Rutherford (1772)
197
Nitrogen Occurrence in Air
About 78% by volume
198
Other Nitrogen Sources
Sodium nitrate, potassium nitrate
199
Nitrogen in Proteins
Essential constituent
200
Nitrogen in Protoplasm
Essential constituent
201
Nitrogen Laboratory Preparation
From ammonium nitrite
202
Ammonium Nitrite Decomposition Equation
$NH_{4}NO_{2}(s)\xrightarrow{heat}2H_{2}O(g)+N_{2}(g)$
203
Alternative Nitrogen Preparation
Aqueous ammonium chloride + sodium nitrite
204
Alternative Nitrogen Preparation Equation
$NH_{4}Cl(aq)+NaNO_{2}(aq)\rightarrow2H_{2}O(l)+N_{2}(g)+NaCl(aq)$
205
Nitrogen Preparation Method
Heating a mixture of ammonium chloride and sodium trioxonitrate(III) (nitrite)
206
Nitrogen Preparation Apparatus
Same as figure 19.1
207
Purity of Nitrogen Prepared from Ammonium Nitrite
Pure
208
Purity of Nitrogen Prepared from Ammonium Chloride and Sodium Nitrite
Contains impurities
209
Impurities in Nitrogen from NH4Cl/NaNO2
NO, $NO_2$
210
Nitrogen Drying Agent
Concentrated tetraoxosulphate(VI) acid
211
Nitrogen Collection Method
Over water
212
Front
Back
213
Nitrogen Preparation Caution
Ammonium nitrite is unstable and explodes on heating.
214
Nitrogen Preparation Alternative Caution
Use ammonium chloride and sodium nitrite, heat gently.
215
Absence of Air Test
Burning splinter extinguishes
216
Absence of Oxygen Test
Glowing splint does not relight
217
Nitrogen Odor
Odorless
218
Nitrogen Color
Colorless
219
Nitrogen Effect on Litmus Paper
Neutral
220
Nitrogen Solubility in Water
Slightly soluble
221
Nitrogen Density Compared to Air
Slightly less dense
222
Nitrogen Diffusion Rate
Slightly faster than air
223
Nitrogen Boiling Point
Very low (-196°C)
224
Nitrogen Liquefaction
Difficult
225
Front
Back
226
Nitrogen Inertness Reason
Strong triple bond between atoms (N≡N)
227
Nitrogen Combination Condition
High temperature
228
Nitrogen Combination Examples
With oxygen, hydrogen, metals
229
Nitrogen + Oxygen Product
Oxides of nitrogen
230
Nitrogen + Magnesium Product
Magnesium nitride ($Mg_3N_2$)
231
Nitrogen + Hydrogen Condition
High temperature, pressure, catalyst
232
Nitrogen + Hydrogen Product
Ammonia ($NH_3$)
233
Nitrogen's Direct Combination Elements
Only lithium and boron at room temperature
234
Nitrogen's Reducing/Oxidizing Ability
Poor
235
Hot Magnesium in Nitrogen Gas Observation
Burns with bright flame
236
Hot Magnesium in Nitrogen Gas Product
Yellowish-green magnesium nitride powder
237
Magnesium Nitride + Water Product
Ammonia gas
238
Magnesium Nitride + Water Equation
$Mg_{3}N_{2}(s)+3H_{2}O(l)\rightarrow3Mg(OH)_{2}(aq)+2NH_{3}(g)$
239
Front
Back
240
Uses of Nitrogen
Ammonia production (Haber process)
241
Haber Process Conditions
High temperature, pressure, catalyst
242
Nitrogen Use in Liquid Form
Refrigerant
243
Liquid Nitrogen Temperature
−196°C
244
Nitrogen Use in Light Bulbs
Inert atmosphere to prevent filament burning
245
Nitrogen Use in Food Packaging
Inert atmosphere to prevent spoilage
246
Nitrogen Oxidation States
−3 to +5
247
Nitrogen Oxidation State in $N_2O$
1
248
Nitrogen Oxidation State in NO
2
249
Nitrogen Oxidation State in $NO_2$
4
250
Nitrogen Oxidation State in $N_2O_5$
5
251
Nitrogen Oxidation State in $NH_3$
−3
252
Nitrogen Oxidation State in $N_2H_4$
−2
253
Nitrogen Oxidation State in $NH_2OH$
−1
254
Front
Back
255
Ammonia Formula
$NH_3$
256
Ammonia Shape
Pyramidal
257
Ammonia Bond Angle
107°
258
Ammonia Solubility in Water
Very soluble
259
Ammonia Density
Lighter than air
260
Ammonia Test
Turns damp red litmus paper blue
261
Ammonia Test Gas
Alkaline gas
262
Ammonia Reaction with Hydrogen Chloride
Forms white fumes of ammonium chloride
263
Ammonia + HCl Equation
$NH_3(g) + HCl(g) \rightarrow NH_4Cl(s)$
264
Ammonia Use
Manufacture of fertilizers
265
Front
Back
266
Ammonium Chloride Formula
$NH_4Cl$
267
Ammonium Chloride State
White solid
268
Ammonium Chloride Solubility in Water
Very soluble
269
Ammonium Chloride Solution's Nature
Slightly acidic
270
Ammonium Chloride Decomposition Products
Ammonia and hydrogen chloride
271
Ammonium Chloride Decomposition Equation
$NH_4Cl(s) \rightleftharpoons NH_3(g) + HCl(g)$
272
Ammonium Chloride Decomposition Condition
Heated strongly
273
Reversible Reaction
A reaction that can proceed in both the forward and reverse directions.
274
Conditions Favoring Forward Reaction in Ammonium Chloride Decomposition
Low temperature
275
Conditions Favoring Backward Reaction in Ammonium Chloride Decomposition
High temperature
276
Front
Back
277
Nitrogen Oxides
Five well-defined oxides
278
Nitrogen Oxides Formulae
$N_2O, NO, N_2O_3, NO_2, N_2O_5$
279
Oxidation States of Nitrogen Oxides
+1 to +5
280
Nitrogen Oxides Nature
Unstable (except $N_2O$, NO)
281
Nitrogen Oxides State
Gaseous (except $N_2O_5$)
282
Dinitrogen Oxide Other Name
Nitrous oxide
283
Dinitrogen Oxide Formula
$N_2O$
284
Dinitrogen Oxide Preparation
Careful heating of ammonium nitrate
285
Ammonium Nitrate Decomposition Equation
$NH_4NO_3(s) \xrightarrow{heat} N_2O(g) + 2H_2O(g)$
286
Dinitrogen Oxide Test
Relights glowing splint (like oxygen)
287
Dinitrogen Oxide Uses
Anaesthetic ('laughing gas')
288
Front
Back
289
Nitrogen(II) Oxide Other Name
Nitric oxide
290
Nitrogen(II) Oxide Formula
NO
291
Nitrogen(II) Oxide Preparation
Direct combination of nitrogen and oxygen (lightning)
292
Nitrogen(II) Oxide Preparation (Lab)
Reduction of dilute trioxonitrate(V) acid with copper
293
Dilute HNO3 + Copper Equation
$3Cu(s) + 8HNO_3(aq) \rightarrow 3Cu(NO_3)_2(aq) + 4H_2O(l) + 2NO(g)$
294
Nitrogen(II) Oxide Appearance
Colorless gas
295
Nitrogen(II) Oxide in Air
Combines with oxygen to form $NO_2$
296
Nitrogen(IV) Oxide Formula
$NO_2$
297
Nitrogen(IV) Oxide Appearance
Brown fumes
298
Nitrogen(IV) Oxide Preparation
$2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
299
Front
Back
300
Trioxonitrate(V) Acid Formula
$HNO_3$
301
Trioxonitrate(V) Acid Other Name
Nitric acid
302
Trioxonitrate(V) Acid Preparation
Large scale: catalytic oxidation of ammonia
303
Catalytic Oxidation of Ammonia Equation
$4NH_3(g) + 5O_2(g) \rightarrow 4NO(g) + 6H_2O(g)$
304
Nitrogen(II) Oxide Oxidation
$2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
305
Nitrogen(IV) Oxide + Water
$3NO_2(g) + H_2O(l) \rightarrow 2HNO_3(aq) + NO(g)$
306
Nitric Acid Appearance
Colorless liquid
307
Nitric Acid Fuming
Fumes in moist air
308
Nitric Acid Solubility
Very soluble in water
309
Nitric Acid Strength
Strong acid
310
Nitric Acid Action on Skin
Turns yellow
311
Front
Back
312
Dinitrogen Trioxide Formula
$N_2O_3$
313
Dinitrogen Trioxide Preparation
Mixing equal volumes of NO and $O_2$ below -20°C
314
Dinitrogen Trioxide State
Blue liquid
315
Dinitrogen Pentoxide Formula
$N_2O_5$
316
Dinitrogen Pentoxide Preparation
Action of phosphorus(V) oxide on concentrated $HNO_3$
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Dinitrogen Pentoxide State
Colorless solid
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Nitrogen(IV) Oxide Other Names
Nitrogen dioxide
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Acidic Oxides of Nitrogen
$N_2O_3, NO_2, N_2O_5$
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Acidic Oxides of Nitrogen Reaction
Dissolve in water to form acids
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Uses of Nitrogen Compounds
Fertilizers, explosives, nylon
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Nitric Acid Action as Acid
Typical acid reactions
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Nitric Acid + Metal Product
Salt, water, hydrogen
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Nitric Acid + Base Product
Salt, water
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Nitric Acid + Carbonate Product
Salt, water, carbon dioxide
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Nitric Acid Oxidizing Ability
Strong
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Nitric Acid Oxidizing Action
Attacks metals (except Au, Pt)
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Dilute Nitric Acid + Copper Equation
$3Cu(s) + 8HNO_3(aq) \rightarrow 3Cu(NO_3)_2(aq) + 4H_2O(l) + 2NO(g)$
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Concentrated Nitric Acid + Copper Equation
$Cu(s) + 4HNO_3(aq) \rightarrow Cu(NO_3)_2(aq) + 2H_2O(l) + 2NO_2(g)$
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Nitric Acid + Hydrogen Sulfide Equation
$H_2S(g) + 2HNO_3(aq) \rightarrow S(s) + 2H_2O(l) + 2NO_2(g)$
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Nitric Acid + Iron(II) Sulfate Equation
$2FeSO_4(aq) + H_2SO_4(aq) + 2HNO_3(aq) \rightarrow Fe_2(SO_4)_3(aq) + 2H_2O(l) + 2NO_2(g)$
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Fertilizers
Substances that restore soil fertility and increase crop yield.
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Fertilizer Types
Natural (manure) and artificial (chemical compounds).
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Essential Elements for Plants
Nitrogen, phosphorus, potassium.
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Nitrogen's Role in Plants
Promotes healthy leaf and stem growth.
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Phosphorus's Role in Plants
Stimulates root growth and fruit development.
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Potassium's Role in Plants
Strengthens resistance to diseases.
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Common Nitrogen Fertilizers
Ammonium salts, nitrates, urea.
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Ammonium Salts Examples
Ammonium sulfate ((NH4)2SO4), ammonium chloride (NH4Cl).
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Nitrates Examples
Sodium nitrate (NaNO3), potassium nitrate (KNO3).
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Urea Formula
(NH2)2CO
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Urea Properties
Soluble in water, easily absorbed by plants.
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Brown Ring Test
Test for nitrate ion ($NO_3^-$)
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Brown Ring Test Reagents
Freshly prepared iron(II) sulfate, concentrated sulfuric acid
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Brown Ring Test Procedure
Add iron(II) sulfate, then carefully add sulfuric acid to form a brown ring at the junction
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Brown Ring Formula
[Fe(H2O)5NO]2+
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Nitric Acid Uses
Fertilizers, explosives, plastics
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Nitrates Use
Fertilizers
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Ammonium Nitrate Use
Fertilizer
353
Potassium Nitrate Use
Gunpowder
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Sodium Nitrate Use
Meat preservative
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Nitrogen Cycle Importance
Maintains nitrogen balance in atmosphere
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Nitrogen Fixation
Conversion of nitrogen gas to nitrogen compounds
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Nitrogen Fixation Types
Atmospheric, industrial, biological
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Atmospheric Nitrogen Fixation
Lightning converts nitrogen and oxygen to nitrogen oxides
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Industrial Nitrogen Fixation
Haber process
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Biological Nitrogen Fixation
Bacteria in root nodules convert nitrogen to ammonia
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Nitrification
Conversion of ammonia to nitrites and nitrates
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Nitrification Bacteria
$Nitrosomonas$ (ammonia to nitrites), $Nitrobacter$ (nitrites to nitrates)
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Assimilation
Plants absorb nitrates from soil to make proteins
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Decomposition
Bacteria/fungi break down dead organisms, releasing ammonia
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Denitrification
Bacteria convert nitrates back to nitrogen gas
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Contact Process Catalyst
Vanadium(V) oxide ($V_2O_5$)
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Raw Materials for Sulfuric Acid Production
Sulfur, air, water
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Sulfur Burning Equation
$S(l) + O_2(g) \rightarrow SO_2(g)$
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Sulfur Dioxide Oxidation Equation
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$
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Sulfur Trioxide Absorption Equation
$SO_3(g) + H_2SO_4(l) \rightarrow H_2S_2O_7(l)$
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Oleum Formula
$H_2S_2O_7$
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Dilution of Oleum Equation
$H_2S_2O_7(l) + H_2O(l) \rightarrow 2H_2SO_4(l)$
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Ostwald Process Steps
Ammonia oxidation, NO oxidation, $NO_2$ absorption
376
Ammonia Oxidation Catalyst
Platinum-rhodium gauze
377
Ammonia Oxidation Equation
$4NH_3(g) + 5O_2(g) \rightarrow 4NO(g) + 6H_2O(g)$
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Fertilizer Disadvantage
Can be washed away by rain, causing water pollution.
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Eutrophication
Excessive nutrient enrichment of water bodies, leading to algal blooms.
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Effects of Eutrophication
Depletion of oxygen, harm to aquatic life.
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Preventing Fertilizer Pollution
Use appropriate amounts, apply at the right time.
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Organic Fertilizers
Compost, manure.
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Organic Fertilizer Advantages
Improve soil structure, water retention.
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Organic Fertilizer Disadvantages
Bulky, slow to release nutrients.
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Inorganic Fertilizers
Chemically manufactured.
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Inorganic Fertilizer Advantages
High nutrient content, easy to apply.
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Inorganic Fertilizer Disadvantages
Can harm soil organisms, contribute to pollution.
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Nitrogen Fixation
The process by which atmospheric nitrogen is converted into nitrogen compounds.
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Nitrogen Cycle
The series of processes by which nitrogen and its compounds are interconverted in the environment and in living organisms, including nitrogen fixation and decomposition.
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Nitrification
The biological oxidation of ammonium to nitrite and then nitrate, performed by microorganisms.
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Denitrification
The reduction of nitrates or nitrites by bacteria in soil that results in the release of nitrogen back into the atmosphere.
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Assimilation
The process by which plants absorb nitrogen (nitrates and ammonium) from the soil and use them to form organic nitrogen compounds such as amino acids, proteins, and nucleic acids.
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Ammonification
The process by which microorganisms break down organic nitrogen-containing compounds into ammonia.
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Haber-Bosch Process
An industrial process for producing ammonia from nitrogen and hydrogen, using an iron catalyst at high temperature and pressure.
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Le Chatelier's Principle
States that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change to reestablish an equilibrium.
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Contact Process
The industrial process for producing sulfuric acid, involving the catalytic oxidation of sulfur dioxide to sulfur trioxide.
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Ostwald Process
A chemical process used for the industrial production of nitric acid ($HNO_3$).
