Sir. La Rose Chemistry notes on Inorganic Chemistry. 647-5159 contact for private tutoring
Teacher:
Sir. LaRose
1
Sir. La Rose Chemistry notes on Inorganic Chemistry. 647-5159 contact for private tutoring
Table of Contents
Contents
1.
Describe the physical and chemical properties of metals .................................................................... 4
2.
Describe the reactions of metallic oxides, nitrates, carbonates and hydroxides ................................. 6
3.
Describe the extraction of Aluminium and Iron ................................................................................... 7
Aluminium ................................................................................................................................................. 7
Iron extraction .......................................................................................................................................... 9
4 Explain why metal alloys are often used in place of their metals ........................................................... 10
5. Relate the properties of the metals; aluminium, lead, iron, copper and their alloy to their uses. ........ 10
Aluminium ............................................................................................................................................... 10
Lead ......................................................................................................................................................... 10
Iron .......................................................................................................................................................... 11
Copper..................................................................................................................................................... 11
6. Explain the importance of metals and their compounds on living systems and the environment. ....... 12
7. Discuss the harmful effects of metals and their compounds on living systems and the environment.. 12
8. Describe the physical and chemical properties of non-metals ............................................................... 14
9. Describing the laboratory preparation of oxygen, carbon dioxide, ammonia. ...................................... 15
Oxygen .................................................................................................................................................... 15
Carbon Dioxide........................................................................................................................................ 16
Ammonia ................................................................................................................................................. 17
10. Explain the use of gases based on their properties .............................................................................. 18
Oxygen .................................................................................................................................................... 18
Hydrogen................................................................................................................................................. 18
Carbon Dioxide........................................................................................................................................ 18
Nitrogen .................................................................................................................................................. 19
Chlorine ................................................................................................................................................... 19
11. List the usage of non-metals, C, S, P, Si, N, Cl and their compounds.................................................... 20
Carbon ..................................................................................................................................................... 20
Sulphur .................................................................................................................................................... 20
Phosphorous ........................................................................................................................................... 20
Silicon ...................................................................................................................................................... 21
Nitrogen .................................................................................................................................................. 21
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Chlorine ................................................................................................................................................... 21
12. Describe the harmful effects of non-metals on living systems and the environment. ........................ 22
Reactivity Series of Metals ................................................................................................................ 23
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1. Describe the physical and chemical properties of metals
Metal
Zinc (Zn)
Physical Properties
Chemical Properties
•
Bluish-white metal
2Zn(s) + O2(g)
2ZnO(s)
•
Shiny
Zn(s) +H2O(l)
ZnO(s) +H2(g)
•
conductor of electricity
Zn(s) + 2HCl(aq)
•
Iron (Fe)
Sodium
(Na)
ZnCl2(aq) + H2(g)
Zn(s) + H2SO4(aq)
ZnSO4(aq) + H2(g)
•
Silver grey metal
3Fe(s) + 2O2(g)
•
Good transmission of heat
3Fe(s) + 4H2O(l)
Fe3O4(s) + 4H2(g)
or electricity
Fe(s) + 2HCl(aq)
FeCl2(aq) + H2(g)
Fe(s) + H2S04(aq)
FeSO4(aq) +H2(g)
•
•
•
4Na(s)+O2(g)
Silvery white metal with a
Fe3O4(s)
2Na2O(s)
waxy appearance
•
reacts rapidly with water
The surface is bright and
•
2Na(s)+2H20(l)
shiny. Less dense that water
2Na(s)+ 2HCl(aq)
It is soft enough to be cut by
2Na(s)+ H2SO4(aq)
2NaOH(aq) + H2(g)
2NaCl(aq) + H2(g)
Na2SO4(aq) + H2(g)
a knife.
Calcium
(Ca)
•
Silver white metallic
2Ca(s)+ O2(g)
2CaO(s)
•
The surface is shiny
Ca(s) + 2H20(l)
Ca(OH)2(aq)+ H2(g)
•
Relatively soft metal
Ca(s) + 2HCl(aq)
Ca(s) + H2SO4(aq)
Magnesium • Silver or grey coloured
(Mg)
metal
•
•
CaCl2(aq) + H2(g)
CaSO4(aq) + H2 (g)
burns in the presence of oxygen, with a
characteristic blinding bright white flame
Shiny
2Mg(s) + O2(g)
•
2MgO(s)
There is no significant reaction with water. It
reacts slowly with hot water, but however
reacts with steam forming magnesium oxide
or hydroxide.
Mg(s) + 2H2O(l)
4
Mg(OH)2(aq) + H2(g)
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Mg(s) + 2HCl(aq)
Mg(s) + H2SO4(aq)
Copper
(Cu)
•
•
Reddish metal; tarnishes to
black or green in air
•
•
•
water.
It is a good conductor of
Cu(s) + H2O(l)
•
•
CuO(s) + H2(g)
It does not react with hydrochloric acid
Cu(s) + 2HCl(aq)
•
2CuO(s)
There is no reaction between copper and
bright metallic
heat and electricity
MgSO4(aq) + H2(g)
oxygen react to form black Cu2O.
2Cu(s) + O2(g)
The lustre of copper is
MgCl2(aq) +H2(g)
CuCl2(aq) + H2(g)
Copper metal dissolves in hot concentrated
sulphuric acid to form solutions containing
the copper sulphate ion together with
hydrogen gas
Cu(s) + 2H2SO4(aq)
CuSO4(aq) + 2H2O(l) +
SO2(g)
Aluminium • Silvery- white metal
(Al)
• Soft with dull lustre
•
4Al(s) + 3O2(g)
Aluminium is an excellent
heat and electricity
conductor
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2Al2O3(s)
2Al(s) + 6H2O(l)
2Al(OH)3(aq) + 3H2(g)
2Al(s) + 6HCl(aq)
2AlCl3(aq) + 3H2(g)
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2. Describe the reactions of metallic oxides, nitrates,
carbonates and hydroxides
Substance Dilute Acid
Metallic
Oxides
Heat
This reaction forms salt and water.
Heat can decompose metal oxides to give oxygen
Na2O + 2 HCl
NaCl + H2O
and metal. The more reactive the metal is, the
MgO + 2 HCl
MgCl2 + H2O
higher the temperature in order to decompose.
2Al2O3
Nitrates
4Al + 3O2
The reaction between a metal nitrate and
Most nitrates tend to decompose on heating to
dilute acid is a double
give the metal oxide, brown fumes of nitrogen
decompositionKNO3(aq) + HCl(aq)
dioxide, and oxygen.
KCl(s) + HNO3(aq)
Mg and Li nitrate tend to decompose completely:
As you go down the Group, the decomposition
gets more difficult
Carbonates
Metal carbonates will react with dilute
Carbonates decompose on heating resulting in a
acids to give salt, water and carbon
metal oxide and carbon dioxide. There are
dioxide gas.
droplets of liquid present from the salt losing
MgCO3(aq)+2HCl(aq)
water in crystallization. Carbon dioxide is
MgCl2(aq)+
evolved showing that the compound is
H2O(l)+CO2 (g)
decomposing. Calcium and Lithium carbonate
react similarly:
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Hydroxides Metal hydroxides react with dilute acid
to form salt and water.
HCl(aq) + NaOH(aq)
Metal hydroxides decompose on heating to yield
metal oxides and water.
NaCl(aq) + H2O(l)
2Mg(OH)2(s)→MgO(s)+H2O(g)
3. Describe the extraction of Aluminium and Iron
Aluminium
The bauxite is purified to produce aluminium oxide, a powder from which aluminium can be
extracted.
The mined bauxite is either:1. Converted to pure alumina (Al2O3), the anhydrous compound, or
2. Heated to 3000 ºC to produce calcined bauxite
Aluminium is obtained from alumina by electrolysis. Aluminium oxide dissolve in molten
cryolite (sodium aluminium fluoride). The addition of cryolite lowers the melting point to 960ºC.
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During the electrolysis of alumina:
•
A molten mixture of cryolite and aluminium oxide is used as the electrolyte
•
5 V and 100000 A are required
•
The positively charger aluminium ions gain electrons from the cathode and form molten
aluminium
Al3+ + 3ē→Al (l)
•
The oxide ions lose electrons at the anode, and form oxygen molecules which is released at
the anode.
2O2+(l) – 4ē → O2 (g)
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Iron extraction
•
•
•
•
•
•
•
•
Iron is produced more than any other metal and most of it is converted to steel.
Iron is extracted from iron ore in a huge container called a blast furnace.
Iron ores such as haematite contain iron (III) oxide, Fe2O3.
Dried heated iron ore, limestone and coke are fed into the top of the furnace.
Near the bottom, hot air is blown into the furnace.
Due to the heat, the coke burns producing carbon dioxide and generating a great deal of
heat.
The carbon dioxide formed is then reduced the carbon monoxide by the hot coke;
CO2 (g) + C(S)→ 2CO (g).The carbon monoxide reduces the hot iron ore to molten iron;
Fe2O3(s) + 3CO (g) → 2Fe (l) + 3CO2 (g).
The molten iron runs to the bottom of the furnace. The iron produced in the blast furnace would
have very large amounts of impurities if limestone was not used. The limestone then breaks
down; CaCO3(s)→ CaO(s)+ CO2(g). The calcium oxide then combines with silicon dioxide which is
the main impurity in iron ore, to form a molten slag; CaO(s) + SiO2(s) →CaSiO3(l).
The molten metal is then allowed to solidify in shallow trays known as casts. Because of this, the
iron is referred to as ‘cast iron’.
Extraction of Iron THE BLAST FURNACE
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4 Explain why metal alloys are often used in place of their metals
An alloy is a combination of metals or a combination of one or more metals with nonmetallic elements.
Metal alloys are used because they are often harder than the pure metal and more resistant to
corrosion, more flexible and may have better electrical and thermal conductivity. When the
combination occurs, a stronger item is created.
5. Relate the properties of the metals; aluminium, lead, iron,
copper and their alloy to their uses.
Aluminium
Pure aluminium is soft, ductile, and corrosion resistant and has a high electrical conductivity.
It is widely used for foil and conductor cables. It is use in cans, kitchen utensils, window frames,
beer kegs and aeroplane parts but
alloying with other elements is necessary. manufacturers mix aluminium with other metals to
strengthen it, forming several different aluminium alloys. Aluminium alloys are widely used in
automotive engines, particularly in cylinder blocks and crankcases due to the weight savings that
are possible. Some alloys include Magnalium and Duralumin.
Lead
The properties of lead are lubricity, malleability, density, electrical conductivity, and coefficient
of thermal expansion, which are all high. It is also characterised by its low elastic modulus,
elastic limit, strength, hardness, and melting point. Lead also has good resistance to corrosion
under a wide variety of conditions. Lead is easily alloyed with other metals.
The high density of lead makes it effective when shielding again x-rays and gamma radiation.
The primary consumption of lead is for Lead- Acid batteries, rolled extrusions, cable sheathing
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and ammunition. Seamless pipes are usually made from lead alloys because of its corrosion
resistance and flexibility. Anodes made from lead alloys are used in electro-winning and plating
of metals e.g. manganese. An example of a lead alloy is Solder.
Iron
Iron is very strong but rusts easily. It also forms a wide range of alloys. It is used to manufacture
steel and also used in civil engineering like reinforced concrete, girders etc. Iron is used to make
bridges, electricity pylons, bicycle chains, cutting tools and rifle barrels.
Iron alloys are arguably the most important class of engineering materials. The most wellknown alloy of iron is steel which contains carbon as its supplemental element. The carbon helps
prevent the iron from rusting, and makes it stronger. People use the material widely in
construction, such as for making screws, nails and beams for buildings and bridges. A common
alloy of iron is steel.
Copper
Copper is soft, malleable, easy to bend and a good conductor of heat and electricity as well as
being resistant to corrosion.
Alloy e.g. brass, a copper alloy, contains about 20% zinc. These alloys are used jewellery, nuts
and bolts.
Copper’s most common use is in electrical equipment like wiring and motors. Due to its
resistance to corrosion, it is used in roofing and guttering. It is also used in plumbing, cookware
and cooking utensils.
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6. Explain the importance of metals and their compounds on
living systems and the environment.
Metal
Importance
Iron
Iron is found in haemoglobin, giving blood cells their red colour. Haemoglobin carries
oxygen from our lungs to the cells, where the oxygen is used to release energy from
food.
A lack of haemoglobin causes anaemia to develop.
It is needed for the body’s defensive system to properly work. It has a role in cell
Zinc
division, cell growth, wound healing and the breakdown of carbohydrates. Senses of
smell and taste rely on zinc as well. Zinc, an essential trace element is essential for the
normal growth and reproduction of humans and plants. It is vital for the functionality
of more than 300 enzymes, for the stabilization of DNA, and for gene expression.
Magnesium Magnesium helps to maintain normal nerve and muscle function, helps bones remain
strong, supports a healthy immune system and keeps the heartbeat steady. It is a part
of chlorophyll.
Calcium
Calcium is an important part of structure of plant cell walls and cell membranes. It is
essential when building strong bones and teeth. It is involved in muscle contraction
and prevents muscle cramp. Calcium is also involved in vascular contraction,
vasodilation, nerve transmission, intracellular signalling, and hormonal secretion. If
someone does not take in sufficient amounts of calcium in his or her diet, the body
will demineralize which would make the bones weak and reduce body mass.
7. Discuss the harmful effects of metals and their compounds on
living systems and the environment
Metal
Harmful Effects
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Lead
Exposure to high levels of lead can cause anaemia, hypertension, kidney and brain
damage. Lead attacks the brain and central nervous system to cause coma,
convulsions and even death.
Children who survive lead poisoning may be left with mental retardation and
behavioural disorders.
Mercury
The inhalation of mercury vapour can cause neurological and behavioural
disorder such as tremors, emotional instability, insomnia, memory loss, neuromuscular changes and headaches. They can also harm kidneys and thyroids.
Mercury is released into the atmosphere from the burning of fossil fuels in
power stations and domestic and industrial wastes in incinerators. Mercury
compounds are released directly into the land from many fungicides.
Nickel
The most serious effects from exposure to nickel are chronic bronchitis, reduced
lung function, cancer in the lung and nasal sinus.
Cadmium
Exposure to cadmium can result in flu like symptoms (chills, fever and
muscle pains) and can damage the lungs.
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8. Describe the physical and chemical properties of non-metals
NonMetal
Physical properties
Chemical properties
Hydrogen
•
•
Colourless, odourless gas
•
Chlorine
•
Hydrogen molecules violently react
with oxygen
Pale Green-yellow gas with a sharp
•
odour (Choaking smell)
H2+ O2→ H2O
Reacts with metals is direct
combination.
2Fe(s) + 3Cl2(g) → 2FeCl3(s)
M + Cl2 → MCl
H2(g) + Cl2(g) → 2HCl(g)
Oxygen
•
•
Colourless, odourless gas
•
reacts with metals, to form the
corresponding metal oxide.
2Mg(s) + O2(g) → 2MgO(s)
Carbon
•
•
•
•
Black solid (graphite) conducts
electricity, brittle
there is the formation of carbon
Colourless crystal (diamond),
dioxide.
extremely hard
C(s) + O2(g) → CO2(g)
•
High boiling and melting point
•
•
Yellow solid (soft)
it reduces metal oxides below
aluminium such as iron oxide
3367ºC and the boiling point 4827ºC
Sulphur
When carbon reacts with oxygen,
•
Reacts with oxygen resulting in
sulphur dioxide.
S(s) + O2(g) → SO2(g)
•
With metals, to produce metallic
sulphides which are ionic compounds
Mg(s)+ S(s) → MgS(s)
Nitrogen
•
3Mg(s) + N2(g) → Mg3N2(s)
Colourless, odourless gas
•
•
Nitrogen prevents substances from
being oxidised.
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9. Describing the laboratory preparation of oxygen, carbon
dioxide, ammonia.
Oxygen
•
Concentrated hydrogen peroxide is dropped slowly from a dropping funnel into a flask
containing manganese (IV) oxide catalyst, 2H2O2 (aq)→O2(g) +2H2O(l).
•
The oxygen is collected in the gas jar by downward displacement of water.
•
Oxygen is slightly soluble in water so most of the oxygen produced will be collected
in the gas jar.
•
The oxygen collected in the gas jar will contain some water vapour because it is
collected over water.
•
If the oxygen is required dry, it can be passed over anhydrous calcium chloride in a Utube.
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Carbon Dioxide
•
Carbon dioxide is prepared by dropping dilute hydrochloric acid onto marble chips.
•
In this preparation, carbon dioxide is denser than air, hence it is collected in the gas jar
by upward displacement of air.
•
It is soluble in water so it is preferable not collect it over water.
•
The carbon dioxide entering from the reaction flask will contain some water vapour.
•
This then arises from the water in the dilute hydrochloric acid.
•
The carbon dioxide can be passed over anhydrous calcium chloride in a U-tube to dry
it.
Test: Bubble the gas through lime water (calcium hydroxide). Goes from
colourless to milky white
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Ammonia
•
•
Ammonia is an alkaline gas which is very soluble in water.
•
It can be prepared by warming any alkali with ammonium salt.
•
In the diagram below, calcium hydroxide and ammonium chloride is heated gently.
The ammonia is less dense than air so it is collected in the gas jar by downward displacement
of air.
• NH4Cl + Ca(OH)2 → NH3 + H2O + CaCl2
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10. Explain the use of gases based on their properties
Oxygen
Oxygen is an odourless, colourless and tasteless gas. It is made up of 22% of the air. Oxygen
gas can generate temperatures of 3000ºC making it suitable for oxy-hydrogen and oxyacetylene blow torches. This is used in industry for cutting, welding and melting metals.
Oxygen does not burn but supports combustion. It is used to produce energy in industrial
processes, generators and ships. Oxygen is also used in airplanes and cars. Liquid oxygen is
burnt by spacecraft for thrust. Oxygen is slightly soluble in water; astronauts, mountaineers
and scuba divers use breathing apparatus that contain oxygen gas. Oxygen is used to destroy
bacteria, treat victims of carbon monoxide, and for aerobic respiration.
Hydrogen
Hydrogen is colourless and odourless gas. It is less dense than air, due to this it is used in
weather balloons that are fitted with equipment to record information necessary to study the
climate. Hydrogen is used in fertilisers, food and chemical and paint industries. Hydrogen
fuel cells are used to generate electricity from oxygen and hydrogen. Hydrogen gas is used in
the processing of petroleum products to break down crude oil into fuel oil, gasoline and such.
Hydrogen is important in creating ammonia (NH3) for use in making fertilizer. Hydrogen gas
is used as a hydrogenating agent to for polyunsaturated fats, such as used in margarine.
Carbon Dioxide
Carbon Dioxide is a colourless and odourless gas. Carbon dioxide does not burn and is
denser than air. Some fire extinguishers contain CO2 when sprayed on fire. Since it is denser
than air and the ‘blankets’ of fire, it’s sealed off from the oxygen. Carbon dioxide
extinguishers are especially useful for dealing with fires involving flammable liquids and
electrical equipment. Carbon dioxide is used make drink ‘fizz’ by pumping carbon dioxide
into the drink under pressure. Solid Carbon Dioxide is used to keep materials cold. It is also
used in pressurising oil wells and as an aerosol propellant.
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Nitrogen
Nitrogen gas is used in handling explosive mixtures, to anneal metals at high temperatures.
This is because of the inertness of nitrogen which prevents premature explosions. It is used to
flush out boilers and pipes during non-use periods since it reduces the chance of corrosion.
Nitrogen protects food from spoilage because bacteria cannot survive in an atmosphere of
nitrogen. Used to make ammonia
Chlorine
This green-yellow gas is soluble in water and has bleaching properties and so turns red
litmus, colourless. Chlorine is used to make sodium hypochlorite which is present in many
bleaches because it is a powerful oxidant. It is involved in cotton and paper manufacture of
polychloroethene since it adds readily to alkenes.
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11. List the usage of non-metals, C, S, P, Si, N, Cl and their
compounds
Carbon
•
Carbon, in the form of graphite, is used as a lubricant and is also used as ‘lead’ in
lead pencils. This is possible because there are weak forces between the layers
allowing the plates of graphite to slide past each other.
•
As diamond, it is used in drill tips for high speed drills because of its hardness.
•
Diamond is also used in jewellery because of its lustre.
•
Carbon fibres are used to strengthen some types of plastic as well.
•
Used to cut glass
•
Graphite is used as electrodes
Sulphur
•
Sulphur is used in the production of chemicals e.g. sulphuric acid which is normally used
in the manufacture of fertilisers and detergents.
•
Matches and gun power contain sulphur since it burns easily and quickly.
•
Sulphur forms links between polymer chains hence it is used in the manufacture of tyres to
make the rubber harder, known as vulcanisation.
•
Sulphur powder is used as a fungicide on plant materials.
Phosphorous
•
Phosphorous is used to make flares and fireworks and
•
phosphorous sulphide is used to make the heads of ‘strike anywhere’ matches because of
its spontaneous inflammable nature.
•
Phosphates are used in fertilisers and pesticides, cleaning agents and water softeners.
•
Phosphorous is an essential element for plant growth and contains particle binding
properties.
•
A small amount of phosphorous is used to make the alloy, phosphor bronze.
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Silicon
•
Silicon is used in electronic devices like transistors and calculators due to its semiconducting property.
•
Silicon in its highly purified form is used to make silicon chips for computers.
•
Sand contains silicon oxide which is used in the manufacture of glass. The glass is made
by heating the sand with calcium oxide and sodium carbonate.
•
Glass fibres are silicates which are used to strengthen plastics (fibreglass). Fibreglass has
a low density, it is strong and is used to make pipes and storage tanks.
•
Traces of transition element atoms found in silicates are used for jewellery.
Nitrogen
Done above
Chlorine
Chlorine is also used to sterilise swimming pools and in water treatment. The active
ingredients of some insecticides are chlorine-containing compounds. A major use of
chlorine is to make the monomer for the plastic, PVC. Some dry cleaning and industrial
solvents and refrigerants contain compounds of chlorine.
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12. Describe the harmful effects of non-metals on living systems
and the environment.
Non- Metal
Carbon Dioxide
Harmful Effects
global warming and changes in rainfall pattern. This then leads to
polar ice caps melting, rise in sea levels, more violent and
unpredictable weather patterns, formation of more desserts and an
increase in the temperature of the oceans.
Carbon Monoxide
If CO is inhaled, it can cause headache, dizziness, vomiting, and
nausea. If CO levels are high enough, you may become
unconscious or die.
Chlorofluorocarbons
The breakdown of ozone causes the formation of holes in the
ozone layer.
This results in the increased risk of getting skin cancer, eye
cataracts and reduced resistance to some disease. Warming of the
earth
Nitrates and
Eutrophication is caused by the excessive amounts of nitrates and
Phosphates
phosphates in lakes and rivers. The nitrates and phosphates from
fertilisers applied to the fields dissolve in groundwater and get
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Reactivity Series of Metals
•
•
•
•
The chemistry of the metals is studied by analysing their reactions with water and acids
and oxygen
Based on these reactions a reactivity series of metals can be produced
The series can be used to place a group of metals in order of reactivity based on the
observations of their reactions with water and acids oxygen
The non-metals hydrogen and carbon are also included in the reactivity series as they are
used to extract metals from their oxides
Table of Metal Reactions
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The reactivity series mnemonic
•
•
Observations from the table above allow the following reactivity series to be deduced
The order of this reactivity series can be memorised using the following mnemonic
o “Please send cats, monkeys and cute zebras into hot countries signed Gordon"
You can learn the reactivity series with the help of a silly phrase
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Deducing the order of reactivity
•
•
•
•
•
•
The order of reactivity of metals can be deduced by making experimental observations
of reactions between metals and water, acids and oxygen
The more vigorous the reaction of the metal, the higher up the reactivity series the metal
is
A combination of reactions may be needed, for example, the order of reactivity of the
more reactive metals can be determined by their reactions with water
The less reactive metals react slowly or not at all with water, so the order of reactivity
would need to be determined by observing their reactions with dilute acid
Temperature change in a reaction can also be used to determine the order of reactivity
The greater the temperature change in a reaction involving a metal, the more reactive
the metal is
5 Unique Properties Of Water
Water is one of the most important sources of life for us, and not only is it healthy, but it is also a
unique substance with some interesting properties.
▪
When water begins to evaporate off of a surface, it creates a cooling effect.
▪
Lower density of ice allows for only the tops of lakes to be frozen.
▪
Water is an extremely potent solvent due to its characteristic of high polarity.
5. Attraction To Other Polar Molecules
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Cohesion is what we call the ability of water to
attract other water molecules. It is one of its most
important properties
There is also the ability of water to bind with
molecules of different substances. This is called
adhesion. Through this property, water can be
adhesive to any other molecule it can form a
hydrogen bond with.
4. High Specific Heat
Water manages to stay liquid because of two of its properties, high specific heat, and its high
heat of vaporization.
3. High Heat Of Evaporation
This is another unique property that allows water to
maintain its temperature.
When water starts evaporating off of a surface, it
creates an effect of cooling. This is similar to
humans and sweating.
2. Lower Density Of Ice
Also, it allows for only the tops of lakes to be
frozen, which is the fact that not many are aware
of. While most people are aware that the reason
icebergs float is the lower density, not many
know about the reason why only the tops of
lakes are frozen.
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Sir. La Rose Chemistry notes on Inorganic Chemistry. 647-5159 contact for private tutoring
1. High Polarity -The universal solvent
Water dissociates salts by separating the cations
and anions and forming new interactions
between the water and ions.
•
Water dissolves many biomolecules,
because they are polar and therefore
hydrophilic.
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Sir. La Rose Chemistry notes on Inorganic Chemistry. 647-5159 contact for private tutoring
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