Chemistry Homework Help at e-Assignmenthelp

Chemistry Assignment Help
e-Assignmenthelp

Topic: Organic and Inorganic
Compounds
Problem Statement:
Discuss the following properties of various inorganic
and organic compounds:
• General Formula
• Nomenclature
• Chemical Properties
• Industrial Uses
• Examples
© e-Assignmenthelp, 2014

Binary Salts
1. Binary salts have the general formula (M+Nm).
2. In the nomenclature, the metal is first followed by the non-metal, whose name is
then changed to “-ide”.
3. Non-metallic oxides such as nitrides, carbides, phosphides and hydrides can
react with moisture and water to produce flammable gases, toxic gases and heat.
Apart from these common hazards, they also have some special hazards. For
instance, nitrides release ammonia gases when they come in contact with
moisture.
– Higher nitrogen oxides such as azides are shock sensitive and poisonous.
– Carbides release highly unstable and explosive acetylene gas when they come
in contact with moisture.
– Hydrides release large amounts of heat and hydrogen gas when they come in
contact with moisture.
– Phosphides release large amounts of highly poisonous phosphine gas when
they come in contact with moisture.

Binary Salts (Contd.)
4. Binary salts are commonly used in fertilizers, developers in
photography, protection from harmful gamma radiation.
5. Some common examples of binary salts are
Potassium Chloride (KCl)
Mercury II Chloride (HgCl2)
Sodium Floride (NaF)
Calcium Sulfide (CaS)
Sodium Hydride (NaH)
Sodium Sulfide (Na2S)

Metal Oxides
1. Metal Oxides have the general formula (M+O).
2. In the nomenclature, the metal is named first, followed by the
oxygen, which is then altered to be named “oxide”.
3. Metal oxides might be prone to hygroscopic hazards. When mixed
with water, these salts produce intense heat and a caustic liquid.
The farther the metal is to the left in the periodic table, the more
intense the reaction will be.
4. Metal oxides find their use in batteries as well as industrial
applications such as lead oxide which provides protection from
sound and vibrations.
5. Some common examples of metal oxides are Sodium Oxide
(Na2O), Magnesium Oxide (MgO), Potassium Oxide (K2O) and
Calcium Oxide (CaO).

Hydroxide Salts
1. Hydroxide salts have the general suffix (OH).
2. In the nomenclature, the metal is named first followed by
the hydroxide.
3. Solutions of hydroxide salts, much like the metal
oxides, produce caustic liquids and generate intense heat.
4. One major application of hydroxide salts is that they are
used in industries to provide a strong base and is also
used in agriculture in fertilizers like ammonia.
5. Some common examples of hydroxide salts include
Potassium Hydroxide (KOH), Sodium Hydroxide
(NaOH), Calcium Hydroxide (Ca(OH)2).

Oxy-salts
1. Oxy salts have the general formula (M+ oxy-anion).
2. In the nomenclature, the metal is named first followed by
the oxy anion, depending upon its oxy state.
3. These salts are potent oxidizers. When introduced to
heat, they liberate oxygen and intensify the combustion of
materials.
4. One of the common forms of oxy salts is Epsom
salt, which is used for health issues and other
applications.
5. Some common examples of oxy salts are Sodium
Perchlorate (NaClO2), Potassium Nitrate
(KNO3), Potassium Nitrite (KNO2), Calcium Hypochlorite
(Ca(ClO)2).

Cyanide Salts
1. Cyanide salts are mixtures of cyanides and
ammonium salts, with a general formula (CN).
2. In the nomenclature, the metal is named first
followed by adding the word cyanide to the ion. All
cyanides are toxic through every route.
3. When they are mixed with an acid, they liberate
hydrogen cyanide gas, which is highly toxic in nature.
4. Cyanide salts are used in electroplating, photography
development, and as a chemical for gas chamber
executions.
5. Some common examples of cyanide salts are Sodium
Cyanide (NaCN), Potassium Cyanide (KCN).

Ammonium Salts
1. Ammonium salts have the general formula
(NH₄⁺¹).
2. In the nomenclature, the ammonium ion comes
first, followed by the non-metal.
3. Since ammonium salts contain a positive
charge, they easily react and release a toxic gas.
4. Ammonium salts are used in many fertilizers.
5. Some common examples of ammonium salts are
Ammonium Chlorate ( NH4ClO), Ammonium
Fluoride (NH4F), Ammonium Bisulfate
(NH4HSO2).

Binary Non-salts
1. Binary Non Salts have the general formula (Nm+Nm).
2. In their nomenclature, the element donating the least
amount of atoms comes first. It is then followed by the
second element ending in “ide”.
3. Any of these salts containing halogens are considered
toxic. The ones containing hydrogen are water reactive in
addition to being toxic. They are also able to release
hydrogen gas during this, and thereby sufficient to ignite
the gas.
4. Despite high toxicity and reactivity, binary non-salts are
used in fertilizers and for other agricultural purposes.
5. A popular example of a binary non-salt is ammonia
(NH3).

Non-metallic oxides
1. Non-metal oxides have the general formula (Nm +
O).
2. In the nomenclature, the non-metal is named
followed by the oxide, which is then followed by a
prefix (di or tri) that designates the number of
oxygen atoms present.
3. Non-metal oxides are respiratory irritants and form
oxy-acids with water. They are also responsible for
producing much of the "acid rain" making the
environmental news.
4. Sulphur dioxide is a common example of such a
non-metal oxide.

Inorganic Oxides
1. Inorganic oxides, as the as the name
suggests, have a general formula (Nm +Ozy
Radical).
2. They are more commonly known for their
ability to react in the instant formation of
very corrosive oxy-acids when contacting
moisture, toxicity, being strong
oxidizers, stimulation of combustion.

Binary Acids
1. Binary acids have the general formula (H +
Halogen).
2. In the nomenclature, the "hydrogen" name
changes to "hydro" and non-metal changes from
"ide" to "ic" and then word acid is added, based
on the basisity, though, the suffix may vary.
3. Binary acids, like most common laboratory
chemicals, are toxic in nature.
4. Some common examples of binary acids are
Hydrogen fluoride HF, Hydrogen chloride
HCl, Hydrobromic acid HBr, Hydrogen iodide HI.

Inorganic Cyanides
1. Inorganic Cyanides are chemical compounds
with the general formula (Nm+CN).
2. In the nomenclature, the non metal is named
first followed by ‘cyanide’, or ‘cyanogen’ as a
prefix.
3. All of these chemicals are extremely toxic. They
prevent cells in the body from using oxygen.
4. They find a prominent application as military
warfare agents.
5. A common example of an inorganic cyanide is
HCN.

Alkanes
1. Alkanes are hydrocarbons with the general
formula (H+C).
2. In nomenclature, the name of the compound
ends in “ane” after a suitable Latin prefix
showing the number of carbon atoms in the
alkane.
3. Alkanes are the most common materials found
in hazardous materials, though they have a wide
range of industrial applications.
4. Some common examples of alkanes are
methane, ethane and propane.

Alkenes
1. Alkenes are unsaturated hydrocarbons with
the general formula (H+C).
2. In the nomenclature, they are named similar
to alkanes, except that the suffix is „ene‟.
3. Alkenes are highly toxic.
4. They are used as oxidisers, energy sources as
well as in the field of plastic manufacturing.
5. Some common examples are propene and
ethene.

Alkynes
1. Alkynes are hydrocarbons with general formula:
(CnH2n – 2).
2. In the nomenclature, they are named similar to
alkanes and alkenes except for the fact that the suffix
is ‘yne’.
– In the IUPAC system of nomenclature, the parent chain
must include the double bond even if it makes it shorter
than the others.
– And the parent alkene chain must be numbered from
whichever end gives the first carbon of the double bond
the lower of two possible numbers.
– Also, the location number should be given as to where the
double bond is.

Alkynes
3. Alkynes take part in very violent decomposition
reactions.
4. They find a wide range of applications in high
energy fuels, high temperature
processes, chemical intermediates.
5. A common example of an alkyne is acetylene.

Aromatic Hydrocarbons
1. Aromatic hydrocarbons have the general formula
(CnHn).
2. In the classical nomenclature, they are named
Benzene, Toluene, and Xylene based on the position
of the prominent substituent.
3. They are very highly toxic and combustible, while
some aromatic hydrocarbons are found to be
carcinogenic.
4. In the field of experimental chemistry, they are
extensively used as carriers and intermediates.
5. Some common examples are Benzene, Toluene, and
Xylene.

Hydrocarbon Radicals
1. Hydrocarbon Radicals are hydrocarbons with
general formula (R-X).
2. These radicals are named based on number of
carbon atoms (Latin suffix) followed by ‘yl’.
3. They are volatile at different temperatures and
also undergo cracking.

Fuel Families
1. Fuel Families are hydrocarbons (H + C) which are
more commonly used in fuel sources, such as in
petroleum and crude oils.
2. They are chemically volatile at different
temperatures, giving rise to the phenomenon of
‘cracking’.
3. Some common examples of fuel families are
petroleum, crude oils, methane, ethane.

Halogenated Hydrocarbons
1. Halogenated hydrocarbons have the general formula
(R-X).
2. In the classical nomenclature, the prefix is followed
by ‘ide’.
3. They are toxic, flammable, carcinogenic, and take
part in polymerization reactions.
4. They also find a wide range of industrial applications
such as solvents, refrigerants, anesthetics, and
insecticides.
5. Examples of halogenated hydrocarbons include
Alkyl Halide, Aryl Halide

Amines
1. Amines are ammonium derivatives with general
formula (R-NH₂)
2. In the nomenclature, they are named ‘amides’.
3. Amines are used in chemical warfare, as blistering
agents etc. They are very irritating to the tissue, very
toxic to the kidneys. They are also highly flammable.
4. Amines are found very widely in nature. Industrial
applications of amines include manufacturing of
plastics, insecticides, etc.
5. Nitrogen mustard is a common example of amines.

Nitroso-compounds
1. Nitros are nitrogen oxide derivatives with
general formula (R-NO₂).
2. In the nomenclature, the positive radical is
named first, followed by ‘amine’.
3. They are highly unstable and often considered
ideal explosives.
4. They are also used as racing fuels.
5. Some common examples are
trinitrobenzene, trinitrotoluene and picric acid.

Organic Cyanides
1. Organic Cyanides are cyanide derivatives with
general formula (R-CN).
2. In IUPAC nomenclature, these are named nitriles
while in classical nomenclature, they end with
the suffix ‘cyanide’.
3. They are very toxic and very irritating to the
human body, causing direct damage to the
respiratory tract.
4. They are used in the extraction of metals and as
pesticide fumigants.

Ethers
1. Ethers have the general formula (R- O-R1).
2. In the nomenclature, the hydrocarbon is
named first, followed by the suffix ‘ether’.
– In the IUPAC system of nomenclature, simple
ethers can be named by naming the alkyl groups
alphabetically followed by the word "ether".
– A more efficient way of naming ethers would be
by adding -oxy- to the prefix for the smaller
hydrocarbon group and joining it to the alkane
name of the larger hydrocarbon group.

Ethers
3. Since ethers have oxygen in a very unstable
arrangement, they have a very wide flammable
range.
4. Ethers are used as solvents, gas additives;
formerly they were also used as anesthetics.
5. Ethyl Ether and ethoxyethane are common
examples of ethers.

Sulfides
1. Sulfides are sulphur-hydrocarbon derivatives
with general formula (R- S-R1).
2. In the nomenclature, the hydrocarbon is
followed by ‘sulfide’
3. The common hazards of sulfides include
toxicity, flammability and irritation.
4. Sulfides are primarily chemical intermediates or
additives by nature.
5. Some common examples are thiomethyl ether
and thioethyl ether.

Mercaptans
1. Mercaptans or “thiols” are sulphur-hydrocarbon
derivatives with general formula (R- SH).
2. In the nomenclature, the hydrogen is named
first, followd by the suffix „mercaptan‟.
3. The common hazards from mercaptans include
toxicity, flammability and irritation.
4. Mercaptans are primarily chemical
intermediates or additives by nature.
5. Some common examples are ethyl
mercaptan, grapefruit mercaptan and
monoterpenoid thiol.

Organic Peroxides
1. Organic Peroxides have the general formula (R- O2-R).
2. In the nomenclature, they are named by naming the
hydrogen first, followed by the suffix „peroxide‟.
3. They may become violently
unstable, oxidizers, flammable.
4. Common uses of organic peroxides include use as
initiators in chemical manufacturing processes.
5. Examples of organic peroxides are methyl peroxide
and methyl ethyl peroxide.

Alcohols
1. Alcohols have the general formula (R- OH).
2. In classical nomenclature, alcohols are
named by mentioning the hydrocarbon first,
followed by „ol‟.
3. Alcohols can be toxic. They oxidize to form
aldehydes or organic acids.
4. Menthol, ethanol, 2-propanol, etc. are
common examples of alcohols.

Ketones
1. Ketones have the general formula (R- CO-R).
2. In the classical nomenclature, they are named
by mentioning the hydrocarbon first, followed
by „one‟.
3. Ketones tend to be toxic, narcotic and
flammable by nature.
4. They are widely used as industrial and
laboratory-grade solvents.
5. Some common examples are Dimenthyl ketone
and methyl ethyl ketone.

Aldehydes
1. Aldehydes have the general formula (R- CHO).
2. In the nomenclature, they are named by naming
the hydrocarbon first, followed by the suffix „-
al‟.
3. Aldehydes are toxic by all routes.
– They oxidize to from organic acids.
– They are also highly flammable.
– Some aldehydes are suspected carcinogenic agents
(HCHO).

Aldehydes
4. Aldehydes are used as solvents, disinfectants
and preservatives.
– Unsaturated aldehydes are used in the
manufacture of plastics.
5. Some common examples of aldehydes
include Methanal (Formaldehyde); Ethanal
(Acetaldehyde); Propanal (Propionaldehyde);
Butanal (butyraldehyde).

Organic Acids
1. Organic acids have the general formula (R- COOH).
2. In the nomenclature, the hydrocarbon is named
first, followed by „-ic acid‟.
3. While some are very toxic, some are mild irritants.
Organic acids are highly flammable and form mild
corrosive solutions when mixed with water.
4. They are used as solvents in plastic production and
water purification.
5. Some common examples of organic acids are benzoic
acid, acetic acid, formic acid, oxalic acid, citric acid.

Esters
1. Esters have the general formula (R- CO2-R).
2. Unlike most other organic compounds, they have a
unique naming system based upon materials used in
etherification process.
3. Since they are highly unsaturated, they tend to be
very toxic and participate in polymerization reactions.
All esters are combustible/ flammable.
4. They are used as food additives and as esterification
agents (plastic manufacturing).
5. Some common examples are ethyl acetate, ethyl
acetate ester, propyl ethanoate .

Chemistry Homework Help at e-Assignmenthelp

Recommended

Recommended

More Related Content

Viewers also liked

Viewers also liked (14)

Recently uploaded

Recently uploaded (20)

Chemistry Homework Help at e-Assignmenthelp