Quizlet Guide Flashcards
(232 cards)
1
Q
Chemicals Everything—including you
A
me
2
Q
Elements Pure substances that cannot be broken down into other substances.
A
3
Q
Chemical Cycle Water changing state and moving through ecosystems in a cycle.
A
4
Q
Fertilizer A substance that enriches soil; the NPK ratio (Nitrogen-Phosphorus-Potassium).
A
5
Q
Pesticides Chemicals that kill pests. Herbicides (weeds)
A
insecticides (insects)
6
Q
Organic Compounds Molecules containing carbon bonded to hydrogen. Examples: fossil fuels
A
sugar.
7
Q
Inorganic Compounds Compounds that mostly do not contain carbon. Examples: salt
A
quartz.
8
Q
Macronutrients for Plants Carbon
A
hydrogen
9
Q
Macronutrients for Humans Carbon
A
hydrogen
10
Q
Micronutrients Needed in trace amounts. Examples: selenium
A
iron
11
Q
Optimum Amounts The ideal amount of a substance for best health—too much or too little is harmful.
A
12
Q
Carbohydrates Made of carbon
A
hydrogen
13
Q
Lipids Organic compounds like fats
A
oils
14
Q
Proteins Made of carbon
A
hydrogen
15
Q
Nucleic Acids Complicated molecules made of phosphate
A
ribose
16
Q
Glucose Test Benedict’s solution turns from blue to red/orange/yellow.
A
17
Q
Starch Test Iodine solution turns blue-black.
A
18
Q
Fat/Oil Test Use brown paper; fat leaves a translucent spot.
A
19
Q
Protein Test Biuret solution turns purple/mauve.
A
20
Q
Groundwater Water beneath the surface in spaces between rock and soil.
A
21
Q
Pores Tiny spaces in soil; permeable soil allows quick movement of water.
A
22
Q
Leachate Solution formed when water dissolves substances from soil.
A
23
Q
Chemical Movement Example Hydrocarbons in soil are toxic and difficult to clean.
A
24
Q
Nitrogen Fixation Nitrogen must be fixed into ammonia (NH3) to be useful to plants.
A
25
Nitrogen Fixers Bacteria in root nodules and lightning.
26
Nitrifying and Denitrifying Bacteria Nitrify: ammonia → nitrite/nitrate. Denitrify: nitrate → free nitrogen.
27
Sewage Wastewater from household sources like kitchen and bathroom.
28
Effluent Treated wastewater released into rivers/lakes.
29
pH A measure of hydrogen ions (H+) in a solution.
30
Acids and Bases Acids: pH < 7
taste sour. Bases: pH > 7
31
pH Scale Logarithmic; each step = 10x change in H+ concentration.
32
Neutralization Reaction of acid + base = neutral solution + salt + water.
33
Acid Rain Caused by the presence of acids in the atmosphere.
34
What causes acid rain? SO2 and NOx from industrial processes mix with water to form acids.
35
What does water quality depend on? pH
dissolved oxygen
36
What is PPM? Parts per million = (solute/solution) x 1
0
37
What are biological indicators? Bacteria
invertebrates used to assess water quality.
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What affects dissolved oxygen? Temperature
turbulence
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How do nitrogen and phosphorus affect water? They cause algae growth → bacteria eat algae → oxygen drops → fish die.
40
What is spring acid shock? Sudden drop in pH from acidic snowmelt.
41
What is LD50? Dose of toxin that kills 50% of test subjects.
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What are heavy metals? Toxic metals like mercury
lead
43
What affects chemical spread in water? Source
chemical properties
44
What are 5 ways to reduce chemical concentration? Dispersion
dilution
45
What is biodegradation? Breakdown of material by organisms like bacteria or fungi.
46
What is phytoremediation? Use of plants to absorb harmful chemicals from soil or water.
47
What is photolysis? Breakdown of compounds by sunlight.
48
What is a chemical? Everything around us is made of chemicals
vital to survival but can also cause harm.
49
What is cellulose? A chemical compound with the formula C6H10O5
found in wooden materials.
50
What is calcium silicate? A chemical compound with the formula Ca2SiO4
found in concrete.
51
What are elements? Pure substances that cannot be broken down into other substances.
52
What is a fertilizer? A substance that enriches soil so that plants will grow better.
53
How are fertilizers identified? By 3 numbers.
54
What is the significance of chemical cycles in the environment? Many elements and compounds
like oxygen and carbon
55
NPK ratio These stand for the percent of the fertilizer that is nitrogen
phosphorus
56
Pesticides Chemicals that are used to kill pests.
57
Pests Organisms that harm crops.
58
Herbicides Chemicals that control weeds.
59
Insecticides Chemicals that control insects.
60
Fungicides Chemicals that control fungi.
61
Organic Compounds Molecules that contain carbon bonded to hydrogen.
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Inorganic Compounds Compounds that do not contain carbon (mostly).
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Macronutrients Chemicals that organisms need in large amounts.
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Macronutrients for plants Carbon
hydrogen
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Macronutrients for humans Carbon
hydrogen
66
Micronutrients Chemicals that organisms need in small (aka trace) amounts.
67
Examples of Micronutrients Selenium
iron
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Optimum Amounts The amount of a substance that provides the organism with the best health.
69
Carbohydrates Organic molecules made up of carbon
hydrogen
70
Simple carbohydrates Monosaccharides or sugars
including glucose
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Disaccharides Formed when two simple carbohydrates link together.
72
Complex carbohydrates Large chains of monosaccharides
such as starch or cellulose.
73
Lipids Organic compounds made up of many carbon
hydrogen
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Proteins Very large organic molecules made up of nitrogen
hydrogen
75
Amino Acids The building blocks of proteins
with 20 different kinds that the body digests from food.
76
Nucleic Acids The largest and most complicated molecules found in living things.
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DNA Deoxyribonucleic acid
a cell's instruction book on how to make proteins.
78
RNA Ribonucleic acid
a cell's post it note for holding copies of the instructions from DNA.
79
Testing for Glucose Use Benedict's solution; turns from blue to yellow/orange/red in the presence of organic molecules.
80
Testing for Starch Use iodine solution; turns from red/yellow to blue-black in the presence of starch.
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Testing for Fat/oil Use brown paper; fats leave a translucent spot.
82
Testing for Proteins Use biuret solution; turns from blue to purple to mauve in the presence of proteins.
83
Carbohydrates Includes glycogen
starch
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Sugar Includes DNA
phosphate
85
Fats Includes waxes
oils
86
Solid Waste Chemicals may be introduced into the environment when we dispose of solid waste or wastewater.
87
Sanitary Landfills Waste is often put in these
which need to be properly lined with plastic and clay to prevent leakage.
88
Groundwater Water found beneath the surface in the spaces between rock and soil.
89
Water Table The top of the groundwater zone.
90
Pores The tiny spaces between grains of soil; larger pores allow faster groundwater movement.
91
Permeable Soil Soil that contains interconnected pores that allow for quick movement of groundwater.
92
Leachate A solution formed when water moves through soil and dissolves substances from the soil.
93
Evaporation/Residue Water evaporates and leaves chemical compound on top of soil as a residue.
94
Collection Chemical solution flows over top of soil
eventually collecting in nearby streams
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Absorption into Plants Chemical solution soaks into the soil and is absorbed by plants via its roots
possibly harming/burning plants.
96
Absorption into Soil Chemical solution is absorbed into the soil rather than plants
may sit within the pores or move downward.
97
Hydrocarbons Contaminate soil and are carried by water in the soil; toxic to plants and animals.
98
Nitrogen Cycle Nitrogen is important for all living things
including plants.
99
Free Nitrogen Nitrogen in the atmosphere is in the form N2 and cannot be used directly by plants.
100
Nitrogen Fixation The process of changing free nitrogen into ammonia (NH3).
101
Nitrification The process where bacteria convert ammonia into nitrite (NO2-) and nitrate (NO3-).
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Denitrification The process where some bacteria can reverse the nitrifying reaction.
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Denitrifying bacteria Bacteria that convert nitrate back into free nitrogen.
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Nitrates and nitrites Compounds that wash off the soil or deep down where roots can't reach.
105
Farming The process where plants uptake nitrogen from the soil and are then harvested
taking the nitrogen with them.
106
Sewage Wastewater from your kitchen
bathroom
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Septic tank An underground container where bacteria break down the organic material in sewage.
108
Effluent Treated wastewater that is released into lakes or rivers
which may contain extra nitrogen or phosphorus.
109
Storm sewers Large pipes that take rainwater directly into a lake or river during a big storm.
110
pH A measure of the amount of hydrogen ions (H+) in a solution.
111
Acids Compounds that dissolve in water to form a solution with pH lower than 7 and taste sour (e.g.
lemon juice or vinegar).
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Bases Compounds that dissolve in water to form a solution with pH higher than 7 and taste bitter and feel slippery (e.g.
bleach or soap).
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pH Scale Ranges from 0-14
where 1 is very acidic (e.g.
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Logarithmic scale Each step on the pH scale represents a 10x change in acidity.
115
pH meter A probe attached to a meter that provides a pH reading when submerged in liquid.
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Acid-Base Indicators Substances that change color when placed in solutions (e.g.
blue litmus paper turns red in an acid).
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Universal Indicator A group of indicators that change color over a wide range of pH
available in paper form or as a solution.
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Neutralization The reaction when acids and bases create a neutral solution along with a salt and water.
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Neutral solution A solution that does not have the properties of either acids or bases.
120
Acid Rain Ordinary rainwater that is slightly acidic (pH 5.6) due to dissolved carbon dioxide forming carbonic acid.
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Calcium hydroxide A base used to treat acidic lakes to neutralize the acid.
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Bromothymol Blue An indicator used to predict pH changes when bubbles are blown into it.
123
Sulfuric acid A strong acid (H2SO4(aq)) that can react with sodium hydroxide (NaOH(aq)).
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Sodium hydroxide A strong base (NaOH(aq)) that can react with sulfuric acid (H2SO4(aq)).
125
Water Quality Water quality cannot be determined by clarity of the water alone. A large variety of factors including pH
dissolved oxygen
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Water Quality Standards The government sets water quality standards for different categories of water use such as human drinking water
recreation (swimming)
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Biological Indicators of Water Quality Scientists can use organisms that live in water to help determine water quality.
128
Microbiological Indicators Bacteria and other microorganisms can cause problems in large numbers. Water is sampled to ensure these populations do not get too large.
129
Aquatic Invertebrates Invertebrates are animals without backbones including worms
shrimp
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Parts Per Million (ppm) Chemicals in the environment are measured in parts per million (ppm). 1 ppm of chlorine means that for every 1 part (ex. 1 mL) of chlorine
there are 1 million parts of the chlorine/water solution.
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PPM Formula PPM = (amount of solute/ amount of solution) x 1
0
132
Defective Toys Example Example: what is the concentration in ppm of 25 defective toys in a shipment of 1
000 toys? 25/1000 = 0.025 (2.5% of the toys are broken). Now calculate the amount of 1
133
Food Coloring Example Example: what is the concentration in ppm if you add 1 mL of food coloring to 99 mL of water?
134
Salt Solution Example If you have 100g of salt solution
and the solution has 205 ppm of salt
135
Parts Per Billion (ppb) Parts per billion and parts per trillion are also measurements used by scientists.
136
Food Coloring in Bathtub 1 drop of food coloring in a half-full bathtub is about 1 ppm.
137
Food Coloring in Swimming Pool 1 drop of food coloring in a full swimming pool is about 1 ppb.
138
Food Coloring in Multiple Pools 1 drop of food coloring in the amount of water needed to fill 1000 swimming pools is about 1 ppt.
139
Chemical Factors Affecting Water Quality Dissolved oxygen
acidity
140
Dissolved Oxygen Dissolved oxygen is necessary for aquatic life. The level of dissolved oxygen depends on temperature
turbulence due to moving water
141
Good Dissolved Oxygen Level 5 mg per L (5 ppm) is good for most living things.
142
Nitrogen and Phosphorus Impact The amount of nitrogen and phosphorus in the water can affect the amount of dissolved oxygen. This can enter the water from sewage or fertilizer runoff.
143
Acidity of Rain Rain and snow has a pH of 5.6 because the water dissolves carbon dioxide from the air creating carbonic acid.
144
Acid Rain Effect If the pH of the rain gets too low and makes lake and river pH less than 4.5
fish die.
145
Spring Acid Shock Spring acid shock occurs when snow that has built up in places where acid rain falls enters waterways and drops the pH.
146
Pesticides Pesticides can lead to pesticide resistant insects and may end up in waterways where they can mix together and become increasingly toxic to living things.
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Toxins Toxins are poisonous substances that produce serious health problems or death for living things.
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Toxicity Toxicity describes how poisonous a substance is.
149
LD50 LD50 stands for lethal dose-50%. It is the amount of a substance that
if given to a group of test animals
150
LD50 The lower the LD50 number
the more toxic it is.
151
Heavy Metals Heavy metals include mercury
copper
152
Heavy Metals in Everyday Items They occur and are made into everyday items like tires
batteries
153
Toxicity of Heavy Metals Toxic to many living things including humans.
154
Impact on Children Effect the normal development of children and cause permanent brain damage.
155
Acidity and Heavy Metals Changes in the acidity of water can allow heavy metals to be absorbed into plants and animals more easily.
156
Water Quality Guidelines Governments set water quality guidelines for five categories of water use.
157
Spring Acid Shock What effect does spring acid shock have on aquatic organisms?
158
Concentration Calculation A student put 0.03 mL of food colouring into water to make 1000 mL of solution. Calculate the concentration of food colouring in parts per million.
159
Phosphorus in Water Systems Explain what happens when a high concentration of phosphorus enters a water system.
160
Waterborne Chemicals When a chemical substance is dumped into any body of water it's considered to be waterborne.
161
Factors Affecting Chemical Scattering Waterborne chemicals will scatter in the water; how far they scatter depends on a few factors: source
chemical's characteristics
162
Source of Waterborne Chemicals Chemical substances can enter surface water from air
groundwater
163
Chemical Characteristics Weight
size
164
Solubility How well a chemical substance dissolves in water.
165
Currents Direction and speed of water flow; ocean currents (ex. gulf stream) or river currents spread chemicals far
ground water moves slowly.
166
Changing Concentration of Pollutants The concentration of pollutants can be changed using different techniques: dispersion
dilution
167
Dispersion The scattering of a substance away from its source.
168
Dilution Reduces the concentration of the pollutant by mixing it with a large amount of air or water.
169
Biodegradation The breakdown of materials by organisms such as earthworms
and micro-organisms like bacteria
170
Types of Biodegradation Two types of biodegradation are aerobic and anaerobic.
171
Aerobic Biodegradation Aerobic means the bacteria need air to function.
172
Anaerobic Biodegradation Anaerobic bacteria do not require oxygen (ex. Deep underground).
173
Factors Affecting Biodegradation Temperature
soil moisture
174
Phytoremediation A technique that can be used to reduce the concentration of harmful chemicals in soil and groundwater by planting plants that absorb or accumulate large amounts of chemicals from the soil.
175
Photolysis The breakdown of compounds by sunlight.
176
Photodegradable Plastic Made up of chemicals that when they react with sunlight
they turn the plastic into a fine powder.
177
Fertilizer A substance that enriches soil so plants will grow
identified by 3 numbers (ex. 10-30-20)
178
Pesticides Chemicals used to kill pests
organisms that harm crops.
179
Organic Compounds Molecules that contain carbon bound to hydrogen.
180
Nutrients Elements and compounds that organisms need for living
growing
181
Carbohydrates Organic molecules made of carbon
hydrogen
182
Lipids Organic molecules made up of many carbon
hydrogen
183
Proteins Large organic molecules made up of nitrogen
hydrogen
184
Amino Acids Building blocks of protein
with 20 kinds that your body digests from food and uses to make protein.
185
Nucleic Acids The largest and most complicated molecules found in living things
made of phosphate
186
Groundwater Water found beneath the surface in the space between rock and soil.
187
Pores The tiny spaces between grains of soil.
188
Permeable soil Soil that contains interconnected pores that allow for the quick movement of groundwater.
189
Leachate Solution formed when water moves through the soil and dissolves substances from the soil.
190
Transport of Chemicals in Soil Things that can happen when chemicals move through the soil.
191
Evaporation/residue Water evaporates and leaves chemical compounds on top of the soil as a residue.
192
Collection A chemical solution flows over the top of the soil
eventually collecting in nearby streams
193
Absorption into soil Chemical solution is absorbed into the soil rather than the plants; the chemical solution may sit within the pores of the soil.
194
Absorption into plants Chemical solution is absorbed by plants from the soil.
195
Nitrogen cycle Nitrogen is important for all living things
including plants; plants can use nitrogen if it is combined with other elements like O2 or hydrogen.
196
Sewage Water waste from your kitchen
bathroom
197
Effluent Treated wastewater that is released into lakes or rivers; it may contain extra nitrogen or phosphorus from the sewage.
198
Storm sewage Large pipes that take rainwater directly into a lake or river during a big storm
carrying chemicals from streets and cars.
199
pH A measure of the amount of hydrogen ions (H+) in a solution; a solution with a lot of hydrogen ions is called acidic
and a solution with few hydrogen ions is called basic.
200
Acidity Compounds that dissolve in water to form a solution with pH lower than 7; they taste sour like lemon juice or vinegar.
201
Basic/alkaline Compounds that dissolve in water to form a solution with pH higher than 7; they taste bitter and feel slippery like bleach or soap.
202
pH number Indicates the acidity of a solution; it measures the concentration of the acidity.
203
Logarithmic scale Each bump on the acidity scale represents a x10 difference.
204
Acid-Base Indicators Substances that change color when placed in solutions; blue turns paper red in an acid
and red litmus paper turns blue in a base.
205
Universal Indicator A group of indicators that change color over a wide range of pH in paper form or solution.
206
Neutralization When acids and bases react to create a neutral solution
salt
207
Acid Rain Rain that is slightly acidic (pH 5.6) due to the dissolution of carbon dioxide in water
which forms carbonic acid.
208
Acidic lakes treatment Acidic lakes can be treated with calcium hydroxide (lime)
which is a base that neutralizes the acid in the lake.
209
Biological Indicators of Water Quality Organisms that live in water can help determine water quality.
210
Microbiological indicators Bacteria and other microorganisms that can cause problems in large numbers; water is sampled to ensure these populations do not get too large.
211
Aquatic Invertebrates Animals without backbones
including worms
212
Parts per million (ppm) A measurement of chemicals in the environment
calculated as PPM = Amount of solute / Amount of solution x 1
213
Dissolved Oxygen Necessary for aquatic life; the level of dissolved oxygen depends on temperature.
214
Dissolved Oxygen 5 mg per L (5 ppm) is good for most living things.
215
Acidity If the pH of the rain gets too low and makes the lake and river pH less than 4.5
fish die.
216
Spring Acid Shock Occurs when snow that has built up acid enters waterways and drops the pH.
217
Heavy Metals Heavy metals include mercury
copper
218
Toxicity Describes how poisonous a substance is.
219
LD50 The amount of a substance
that if given to a group of test animals
220
Waterborne Chemicals When a chemical substance is dumped into any body of water
it's considered to be waterborne.
221
Biodegradation The breakdown of materials by organisms.
222
Aerobic Bacteria Bacteria needing air.
223
Anaerobic Bacteria Bacteria that don't need oxygen.
224
Phytoremediation A technique that can be used to reduce the concentration of harmful chemicals in soil and groundwater by planting plants that absorb or accumulate large amounts of chemicals.
225
Photolysis Breakdown of compounds by sunlight.
226
Toxins Poisonous substances that produce serious health problems or death for living things.
227
Plant Nutrients Like nitrogen and phosphorus
they can affect the amount of dissolved oxygen.
228
Pesticides Some pesticides last a long time in the environment and may end up in waterways.
229
Current Direction and speed of water flow that can spread chemicals.
230
Temperature for Bacteria Bacteria like it warm.
231
Soil Moisture Soil should be damp for effective biodegradation.
232
Nutrient Availability Ex. cut grass will have more nutrients than paper
however both decompose.
