GRADE_9_CHEMISTRY.pptx

Properties of
Covalent and Ionic
Compounds
Properties of
Carbon Atom,
Structure, and
Isotopes
Hydrocarbon
Derivatives
Organic Chemistry
and Structures
01 02 03
05
04
Hydrocarbons and
Nomenclature

Properties of
Covalent and Ionic
Compounds
01
How are compounds different from one
another?

Highly Flammable Mostly Inflammable
Insulator of Electricity Conductor of Electricity
Nonpolar Polar
Insoluble in water Soluble in water
Low Melting Point High Melting Point
High Boiling Point Low Boiling Point

Properties of
Carbon Atom,
Structure, and
Isotopes
02

Carbon (𝑪𝟔
)
 Carbon came from the Latin word carbo
which means “charcoal”.
 6th most abundant element in the
universe and has been known since
ancient times.
 Carbon is commonly obtained from coal
deposits.

Properties of Carbon
Atom
 Atomic number: 6
 Atomic mass: 12.0211 𝑔/𝑚𝑜𝑙
 Density: 2.267 𝑔/𝑐𝑚3
 Melting point: 3652 °𝐶
 Boiling point: 4827 °𝐶
 Isotopes: 3 (12C, 13C, & 14C)
 Electronic shell: [ 𝐻𝑒 ] 2𝑠22𝑝2

Carbon has four valence electrons, so
it can achieve a full outer energy level by
forming four covalent bonds. When it
bonds only with hydrogen, it forms
compounds called hydrocarbons. Carbon
can form single, double, or triple covalent
bonds with other carbon atoms.
Types of Bond Carbon
Makes

4 single bonds
1 double bond and 4
single bond or 2 double
bond
1 triple bond and 2
single bond
Types of Bond Carbon
Makes

6 total number of Electrons
(e-)
2 e- on the inner shell (1𝑠2
)
4 e- on the outer shell
(2𝑠2
2𝑝2
)
How many electrons does an
atom need to be stable?
Structure of Carbon
Atom

Aliphatic Structure
Atom bonded to two other atoms placed at a
bond-angle and joined together in straight chains, and
branched chains.
Structure of Carbon
Atom
C C
e- e-
e-
e-
e- e-
e-
e-
C e-
e-
e-
e-
C
e-
e-
e- e

Cyclic Structure
Ring compound is a
compound in which at
least some its atoms are
connected to form a ring.
Structure of Carbon
Atom
C C
e- e-
e-
e-
e- e-
e-
e-
C
e- e-
e- e-

12C
6 Electrons (e-), 6 Protons (p+),
6 Neutron (n°)
13C
7 Neutron (n°)
14C
8 Neutron (n°)
Isotopes of Carbon
Atom

Carbon-12
6 Neutron (n°)
 Stable Isotope
 Most Abundant Carbon Isotope
 Almost 99% of all carbon on
Earth
Isotopes of Carbon
Atom

Carbon-13
7 Neutron (n°)
 Stable Isotope
 2nd Most Abundant Carbon
Isotope
 Slightly 1% of all carbon on
Earth
Isotopes of Carbon
Atom

Carbon-14
8 Neutron (n°)
 Most Abundant Radioactive
Isotope at 1 ppt (parts per
trillion)
 Half Life of 5,730 years
 Used in Radioactive Dating
Isotopes of Carbon
Atom

Organic
Chemistry and
Structures
03

Organic chemistry is the study of the structure,
properties, composition, reactions, and preparation of
carbon-containing compounds.
Most organic compounds contain carbon and
hydrogen, but they may also include any number of
other elements (e.g., nitrogen, oxygen, halogens,
phosphorus, silicon, sulfur).
Organic Chemistry

Difference between Organic &
Inorganic Compounds
Highly Flammable Mostly Inflammable
Insulator of Electricity Conductor of Electricity
Nonpolar Polar
Insoluble in water Soluble in water
Low Melting Point High Melting Point
High Boiling Point Low Boiling Point

Vitamin A (Retinol)
Structure of Organic
Molecule
A.
Straight-Line
Structure
B.
Bond-Line
Structure

Hydrogen wants to have 2 e- to be stable.
While Carbon, Oxygen and Nitrogen wants 8 e- to
be stable.
NOTE: When looking at representation of atoms
and making your own always remember the
OCTET RULE
Structure of Organic
Molecule

Proposed by Gilbert N. Lewis. It is a
representation of the valence electrons of an atom
that uses dots around the symbol of the element.
The number of dots equals the number of valence
electrons in the atom.
Lewis Electron Dot

Lewis Electron Dot
𝑪𝟔 𝑶𝟖
𝑵𝟕

Kekulé structures, Straight-Line Structures
or Expanded Structural Structures are like Lewis
Structures, but instead of covalent bonds being
represented by electron dots, the two shared
electrons are shown by a line.
e.g., methane
Kekulé Structures

A condensed structure shows all atoms, but
it omits the vertical bonds and most or all of the
horizontal single bonds.
e.g., Ethane
𝑪𝑯𝟐 − 𝑪𝑯𝟐
𝑪𝑯𝟐𝑪𝑯𝟐
Condensed Structures

A representation of molecular structure in
which covalent bonds are represented with one
line for each level of bond order.
e.g., methyl-2-butane
Bond Line or Zigzag
Formula

Dashed lines show atoms and bonds that go
into the page, behind the plane, away from you.
e.g., dimethyl-2-propanol
Dashed-Wedge Line
Structure

Hydrocarbons
and
Nomenclature
04

Organic compound, any of a large
class of chemical compounds in which one
or more atoms of carbon are covalently
linked to atoms of other elements, most
commonly hydrogen, oxygen, or nitrogen.
The few carbon-containing compounds not
classified as organic include carbides,
carbonates, and cyanides.
Organic Compounds

Organic
Compounds
Hydrocarbons
Alkanes
Alkenes
Alkynes
Hydrocarbon
Derivatives
Alcohols (-OH)
Aldehydes
(𝑅 − 𝐶−𝐻
=𝑂
)
Ketones
(𝑅 − 𝐶−𝑅
=𝑂
)
Carboxylic Acid
(𝑅 − 𝐶−𝑂𝐻
=𝑂

A hydrocarbon is an organic chemical
compound composed exclusively of
hydrogen and carbon atoms.
Hydrocarbons are naturally-occurring
compounds and form the basis of crude
oil, natural gas, coal, and other important
energy sources.
HydroCarbons

Is a saturated hydrocarbon. In other words,
an alkane consists of hydrogen and carbon atoms
arranged in a tree structure in which all the
carbon–carbon bonds are single.
General Formula for an Alkane:
𝑪𝒏𝑯𝟐𝒏+𝟐
Alkanes

Alkanes
# of
Carbon
Name
Formula
(𝑪𝒏𝑯𝟐𝒏+𝟐)
1 Methane 𝑪𝟏𝑯𝟒
2 Ethane 𝑪𝟐𝑯𝟔
3 Propane 𝑪𝟑𝑯𝟖
4 Butane 𝑪𝟒𝑯𝟏𝟎
5 Pentane 𝑪𝟓𝑯𝟏𝟐
6 Hexane 𝑪𝟔𝑯𝟏𝟒
7 Heptane 𝑪𝟕𝑯𝟏𝟔
8 Octane 𝑪𝟖𝑯𝟏𝟖
9 Nonane 𝑪𝟗𝑯𝟐𝟎
10 Decane 𝑪𝟏𝟎𝑯𝟐𝟐
# of Carbon Name
Formula
11 Undecane 𝑪𝟏𝟏𝑯𝟐𝟒
12 Dodecane 𝑪𝟏𝟐𝑯𝟐𝟔
13 Tridecane 𝑪𝟏𝟑𝑯𝟐𝟖
14 Tetradecane 𝑪𝟏𝟒𝑯𝟑𝟎
15 Pentadecane 𝑪𝟏𝟓𝑯𝟑𝟐
16 Hexadecane 𝑪𝟏𝟔𝑯𝟑𝟒
17 Heptadecane 𝑪𝟏𝟕𝑯𝟑𝟔
18 Octadecane 𝑪𝟏𝟖𝑯𝟑𝟖
19 Nondecane 𝑪𝟏𝟗𝑯𝟒𝟎
20 Eicosane 𝑪𝟐𝟎𝑯𝟒𝟐

Straight-Chain Cyclic
Branched
Alkanes

IUPAC stands for International Union of Pure
& Applied Chemistry. A neutral and objective
scientific organization, IUPAC was established in
1919 by academic and industrial chemists who
shared a common goal – to unite a fragmented,
global chemistry community for the advancement
of the chemical sciences via collaboration and the
free exchange of scientific information.
IUPAC Nomeclature

#1. Find the Longest
Carbon Chain
1
2
3 4
5 6
7

#2. Name the Longest
Carbon Chain
1
2 3
4
5
6
7
Carbon
Atom (#)
Root
Name
1 Meth
2 Eth
3 Prop
4 But
5 Pent
6 Hex
7 Hept
8 Oct
9 Non
10 Dec

Carbon Chain
1
2 3
4
5
6
7
7 –
Hept-

#3. Figure out what the
ending (suffix) should be
This is
an
Alkane
Use the –ane suffix to
attach to the root name

#4. Number your Carbon
Atoms
1
2 3
4
5
6
7
Note 1: Find any side
groups or any molecule
attached
Note 2: Always start
counting where the
branched side is nearer

#5. Name the Side
Groups
1
2 3
4
5
6
7
In naming a side group,
you must include the root
name, suffix and the
carbon number it is
attached
Remember: Side groups of
carbon are considered as
Alkyl Group (-yl)
Methyl-4- or
4-methyl

#6. Apply all the steps &
Name the Alkane
1
2 3
4
5
6
7
Note: In naming a
compound, the alkyl group
always comes first. If there
are multiple alkyl group,
they are arranged in an
alphabetical order
Methyl-4 or
4-methyl
7 - Hept Alk-ane

Name the compound
1
2 3
4
5
6
7
Methyl-4-heptane
or
4-methylheptane
Methyl-4- or
4-methyl
7 - Hept Alk-ane

In organic chemistry, the cycloalkanes are
the monocyclic saturated hydrocarbons. In other
words, a cycloalkane consists only of hydrogen
and carbon atoms arranged in a structure
containing a single ring (possibly with side
chains), and all the carbon-carbon bonds are
single.
What is a
Cycloalkane?

#1. Locate the Longest
Cyclic Carbon Chain
1
2
3
4 5
5 Carbon
Cyclic Chain

Cyclic Carbon Chain
1
2
3
4 5
5 – Pent-
Note: It is a cycloalkane.
Use the prefix cyclo-
before the root name
Cyclopent-

Atoms
attached
counting where the
branched side is nearer

#5. Name the Side
Groups
1
2
carbon number it is
attached
Alkyl Group (-yl)
1-ethyl or
ethyl

Name the Alkane
1-
ethylcyclopentane
or
ethylcyclopentane
1-ethyl or
ethyl
5 – cyclopent-
Alk-ane
1
2
3
4 5

#1. Locate the Longest
Carbon Chain
1
2
3
4
5
6 Carbon
Straight
Chain
6
1
2
3
4 5

Carbon Chain
1 2 3 4
5
6 – Hex-
6

Atoms
1
2
3
4
5
6

#5. Name the Side
Groups
1
2
3
4
5 6
Note: In this case, the
cycloalkane is a
substituent. Use it as the
alkyl group as

Name the Alkane
1
2 3 4 5 6
Alk-ane
6 – Hex-
1-
cyclopentylhexane
Or
Cyclopentylhexane

1. Most Alkanes are Colorless and Odorless
2. Alkanes are less dense than water (They will
float on top of water)
3. Alkanes are non-polar
4. Has weak intermolecular forces between alkane
molecules
5. Insoluble in water
Properties of Alkanes

6. Alkanes are relatively unreactive, but they will
combust. Commonly used as fuels since large
amounts of energy is released (the longer the
chain, more bonds to be broken, the greater
energy released).
7. The first 4 alkanes are gases at room
temperature, and solids do not begin to appear
until about 𝑪𝟏𝟕𝑯𝟑𝟔
Properties of Alkanes

Propane and butane can be liquefied at low
pressures, and are used, for example, in the
propane gas burner, or as propellants in aerosol
sprays. Butane in used in cigarette lighters.
Uses of Alkanes

The alkanes from pentane to octane are
highly volatile liquids and good solvents for
nonpolar substances. They are used as fuels in
internal combustion engines.
Uses of Alkanes

Alkanes from nonane to hexadecane are
liquids of higher viscosity, being used in diesel
and aviation fuel (kerosene). The higher melting
points of these alkanes can cause problems at low
temperatures and in polar regions, where the fuel
becomes too viscous.
Uses of Alkanes

Alkanes with a chain length above 35 carbon
atoms are found in bitumen (as it is used in road
surfacing). These higher alkanes have little
chemical and commercial value and are usually
split into lower alkanes by cracking.
Uses of Alkanes

In chemistry, an alkene is an unsaturated
hydrocarbon compound. This compound may
contain one or more carbon-carbon double bond.
General Formula for an Alkane:
𝑪𝒏𝑯𝟐𝒏
Alkenes

Alkenes
# of
Carbon
Name
Formula
(𝑪𝒏𝑯𝟐𝒏)
2 Ethene 𝑪𝟐𝑯𝟒
3 Propene 𝑪𝟑𝑯𝟔
4 Butene 𝑪𝟒𝑯𝟖
5 Pentene 𝑪𝟓𝑯𝟏𝟎
6 Hexene 𝑪𝟔𝑯𝟏𝟐
7 Heptene 𝑪𝟕𝑯𝟏𝟒
8 Octene 𝑪𝟖𝑯𝟏𝟔
9 Nonene 𝑪𝟗𝑯𝟏𝟖
10 Decene 𝑪𝟐𝟎𝑯𝟐𝟎
11 Undecene 𝑪𝟏𝟏𝑯𝟐𝟐
# of Carbon Name
Formula
12 Dodecene 𝑪𝟏𝟐𝑯𝟐𝟒
13 Tridecene 𝑪𝟏𝟑𝑯𝟐𝟔
14 Tetradecene 𝑪𝟏𝟒𝑯𝟐𝟖
15 Pentadecene 𝑪𝟏𝟓𝑯𝟑𝟎
16 Hexadecene 𝑪𝟏𝟔𝑯𝟑𝟐
17 Heptadecene 𝑪𝟏𝟕𝑯𝟑𝟒
18 Octadecene 𝑪𝟏𝟖𝑯𝟑𝟔
19 Nonadecene 𝑪𝟏𝟗𝑯𝟑𝟖
20 Eicosene 𝑪𝟐𝟎𝑯𝟒𝟎

Carbon Chain
1
2
3
4

Carbon Chain
1
2
3
4
4- but-

This is
an
Alkene
Use the –ene suffix to

Atoms
attached
counting where the
carbon-carbon double
bond is nearer
1
2
3
4

#5. Name the Side
Groups
carbon number it is
attached
Alkyl Group (-yl)
1
2
3
4

Name the compound
1-Butene or
but-1-ene or
butene
1
2
3
4
Alk-ene
4 – but-

Carbon Chain
1
2
3
4
5

Carbon Chain
1
2
3
4
5- pent-
5

Atoms
attached
counting where the
carbon-carbon double
bond is nearer
1
2
3
4
5

#5. Name the Side
Groups
carbon number it is
attached
Alkyl Group (-yl)
1
2
3
4
5

Name the compound
4-methyl-2-pentene or
methyl-4-pent-2-ene
Alk-ene
5 – pent-
1
2
3
4
5

1. Alkenes are lighter than water, therefore, are
insoluble in water. Alkenes are only soluble in
polar solvent.
2. Alkenes are virtually insoluble in water, but
dissolve in organic solvents. The reasons for this
are the same as for the alkanes.
Properties of Alkenes

3. The boiling point of each alkene is very similar
to that of the alkane with the same number of
carbon atoms. Ethene, propene, and the various
butene are gases at room temperature. All the rest
that you are likely to come across are liquids (i.e.,
ethylene glycol)

4. Melting points of alkenes depends
on the packaging of molecules.
Alkenes have similar melting points
to that of alkanes, however, there are
some isomers that low melting
points.

Alkenes are extremely
important in the manufacture of
plastic. All plastics are in some way
related to alkenes. The names of
some plastics (Polythene or Poly
Ethene, Polypropene), relate to their
alkene partners. Plastics are used
for all kinds of tasks, from
packaging and wrapping, to
clothing and outdoor apparel.
Uses of Alkenes

Lower alkenes are used as fuel and
illuminant. These may be obtained by the
cracking of kerosene or petrol.
Alkenes are also used as artificial
ripening of fruits (Ethylene or Ethene), as a
general anesthetic, for making poisonous
mustard gas (war gas) and ethylene-
oxygen flame.
Uses of Alkenes

In organic chemistry, an alkyne is an
unsaturated hydrocarbon containing at least one
carbon—carbon triple bond. The simplest acyclic
alkynes with only one triple bond and no other
functional groups form a homologous series with
the General Formula for an Alkyne:
𝑪𝒏𝑯𝟐𝒏−𝟐
Alkynes

Alkynes
# of Carbon Name
Formula
(𝑪𝒏𝑯𝟐𝒏)
2 Ethyne 𝑪𝟐𝑯𝟒
3 Propyne 𝑪𝟑𝑯𝟔
4 Butyne 𝑪𝟒𝑯𝟖
5 Pentyne 𝑪𝟓𝑯𝟏𝟎
6 Hexyne 𝑪𝟔𝑯𝟏𝟐
7 Heptyne 𝑪𝟕𝑯𝟏𝟒
8 Octyne 𝑪𝟖𝑯𝟏𝟔
9 Nonyne 𝑪𝟗𝑯𝟏𝟖
10 Decyne 𝑪𝟐𝟎𝑯𝟐𝟎
11 Undecyne 𝑪𝟏𝟏𝑯𝟐𝟐

Carbon Chain
5- pent-
1
2
3
4
5

This is
an
Alkyne
Use the –yne suffix to

Atoms
attached
counting where the
carbon-carbon triple bond
is nearer
5
4
3
2
1

#5. Name the Side
Groups
carbon number it is
attached
Alkyl Group (-yl)
5
4
3
2
1

Name the compound
1-pentyne
or pent-1-
yne or
pentyne
Alk-yne
5 – Pent-
5
4
3
2
1

Carbon Chain
1
2
3
4
5
6

Carbon Chain
6- hex-
1
2
3
4
5
6

Atoms
attached
counting where the
carbon-carbon triple bond
is nearer
1
2
3
4
5
6

#5. Name the Side
Groups
carbon number it is
attached
Alkyl Group (-yl)
1
2
3
4
5
6

Name the compound
5,5-dimethyl-3-hexyne
or dimethyl-5,5-hexa-3-
yne
Alk-yne
6 – hex-
1
2
3
4
5
6

Alkynes are nonpolar, unsaturated
hydrocarbons with physical properties like
alkanes and alkenes. Alkynes dissolve in organic
solvents, have slight solubility in polar solvents,
and are insoluble in water. Compared to alkanes
and alkenes, alkynes have slightly higher boiling
points.
Properties of Alkynes

1. The properties of alkynes pretty much
follow the same pattern of those of alkanes and
alkenes.
2. Alkynes are unsaturated carbon that
shares a triple bond at the carbon site
3. All alkynes are odorless and colorless
except for ethylene which has a slight distinctive
odor.
4.The first three alkynes are gases, and the
next eight are liquids. All alkynes higher than

5. Alkynes are slightly polar in nature
6. The boiling point and melting point of
alkynes increases as their molecular structure
grows bigger. The boiling point increases with
increase in their molecular mass
7. Also, the boiling points of alkynes are
slightly higher than those of their corresponding
alkenes, due to the one extra bond at the carbon
site.

1.The most common use of Ethyne is for making
organic compounds like ethanol, ethanoic acid, acrylic acid,
etc.
2. It is also used for making polymers and its beginning
materials. For instance, vinyl chloride is used as the starting
material for PVC and chloroprene is used for synthetic rubber
neoprene.
3. Ethyne is used for preparing many organic solvents.
4. Alkynes are commonly used to artificially ripe fruits.
Uses of Alkynes

Aromatic hydrocarbons, or arenes, are
aromatic organic compounds containing
solely carbon and hydrogen atoms. The
configuration of six carbon atoms in
aromatic compounds is called a "benzene
ring", after the simple aromatic compound
benzene, or a phenyl group when part of a
larger compound.
Aromatic Hydrocarbon

The group of hydrocarbons, such as
alkane, alkene and alkynes, have unique
characteristics to distinguish them from the
rest of the other organic compounds. They
are composed merely of carbon and
hydrogen and the bonding my be single,
double or triple carbon-carbon bonds. All
hydrocarbons are combustible.
Reaction of
Hydrocarbons

𝟐𝑪𝟐𝑯𝟔 + 𝟕𝑶𝟐 → 𝟒𝑪𝑶𝟐 + 𝟔𝑯𝟐𝑶
𝑬𝒕𝒉𝒂𝒏𝒆 + 𝑶𝒙𝒚𝒈𝒆𝒏 → 𝑪𝒂𝒓𝒃𝒐𝒏 𝑫𝒊𝒐𝒙𝒊𝒅𝒆 + 𝑾𝒂𝒕𝒆𝒓
𝑪𝟐𝑯𝟒 + 𝟑𝑶𝟐 → 𝟐𝑪𝑶𝟐 + 𝟐𝑯𝟐𝑶
𝑬𝒕𝒉𝒚𝒏𝒆 + 𝑶𝒙𝒚𝒈𝒆𝒏 → 𝑪𝒂𝒓𝒃𝒐𝒏 𝑫𝒊𝒐𝒙𝒊𝒅𝒆 + 𝑾𝒂𝒕𝒆𝒓
𝟐𝑪𝟐𝑯𝟔 + 𝟓𝑶𝟐 → 𝟒𝑪𝑶𝟐 + 𝟐𝑯𝟐𝑶
𝑬𝒕𝒉𝒚𝒏𝒆 + 𝑶𝒙𝒚𝒈𝒆𝒏 → 𝑪𝒂𝒓𝒃𝒐𝒏 𝑫𝒊𝒐𝒙𝒊𝒅𝒆 + 𝑾𝒂𝒕𝒆𝒓
Reaction of
Hydrocarbons

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