Hydrocarbons: Types and Properties

Study Notes

Definition: Hydrocarbons are compounds consisting only of hydrogen and carbon atoms.
Types:
- Saturated hydrocarbons (alkanes): single bonds between carbon atoms, general formula CnH2n+2
- Unsaturated hydrocarbons (alkenes and alkynes): multiple bonds between carbon atoms, general formula CnH2n (alkenes) and CnH2n-2 (alkynes)
Properties:
- Low melting and boiling points
- Insoluble in water, soluble in organic solvents
- Combustible, producing CO2 and H2O upon burning

Definition: Covalent bonds are chemical bonds formed by sharing one or more pairs of electrons between atoms.
Types:
- Sigma (σ) bonds: formed by end-to-end overlap of atomic orbitals
- Pi (π) bonds: formed by sideways overlap of atomic orbitals
Characteristics:
- Strong and stable bonds
- Directional, resulting in specific molecular shapes
- Typically found in molecules with multiple atoms, including carbon compounds

Definition: Halogenated compounds are organic compounds containing halogen atoms (F, Cl, Br, I).
Examples:
- Chloroform (CHCl3)
- Carbon tetrachloride (CCl4)
- Freon (CF2Cl2)
Properties:
- Often toxic and hazardous to human health and the environment
- Used as solvents, refrigerants, and pesticides
- Can be persistent pollutants in the environment

Definition: Aldehydes and ketones are organic compounds containing a carbonyl group (C=O).
Aldehydes:
- General formula: RCHO
- Examples: formaldehyde (HCHO), acetaldehyde (CH3CHO)
Ketones:
- General formula: RCOR'
- Examples: acetone (CH3COCH3), methyl ethyl ketone (CH3CH2COCH3)
Properties:
- Often have a characteristic pungent smell
- Used in perfumes, flavorings, and pharmaceuticals
- Can be synthesized through various chemical reactions

Definition: Allotropes are different physical forms of the same element, in this case, carbon.
Examples:
- Diamond: rigid and crystalline, extremely hard
- Graphite: soft and slippery, used in pencil lead
- Fullerenes: spherical or tube-shaped, consisting of 60 or more carbon atoms
- Carbon nanotubes: tubular structures with unique properties
- Amorphous carbon: non-crystalline, often found in charcoal and soot
Properties:
- Varying hardness, density, and conductivity
- Wide range of applications, including electronics, materials science, and biology

Hydrocarbons are compounds consisting only of hydrogen and carbon atoms.
Saturated hydrocarbons (alkanes) have single bonds between carbon atoms, with a general formula of CnH2n+2.
Unsaturated hydrocarbons (alkenes and alkynes) have multiple bonds between carbon atoms, with general formulas of CnH2n (alkenes) and CnH2n-2 (alkynes).
Hydrocarbons have low melting and boiling points, are insoluble in water, soluble in organic solvents, and are combustible, producing CO2 and H2O upon burning.

Covalent bonds are chemical bonds formed by sharing one or more pairs of electrons between atoms.
Sigma (σ) bonds are formed by end-to-end overlap of atomic orbitals.
Pi (π) bonds are formed by sideways overlap of atomic orbitals.
Covalent bonds are strong and stable, directional, resulting in specific molecular shapes, and are typically found in molecules with multiple atoms, including carbon compounds.

Halogenated compounds are organic compounds containing halogen atoms (F, Cl, Br, I).
Examples of halogenated compounds include chloroform (CHCl3), carbon tetrachloride (CCl4), and Freon (CF2Cl2).
Halogenated compounds are often toxic and hazardous to human health and the environment, and are used as solvents, refrigerants, and pesticides.
They can be persistent pollutants in the environment.

Aldehydes and ketones are organic compounds containing a carbonyl group (C=O).
Aldehydes have a general formula of RCHO, with examples including formaldehyde (HCHO) and acetaldehyde (CH3CHO).
Ketones have a general formula of RCOR', with examples including acetone (CH3COCH3) and methyl ethyl ketone (CH3CH2COCH3).
Aldehydes and ketones often have a characteristic pungent smell, are used in perfumes, flavorings, and pharmaceuticals, and can be synthesized through various chemical reactions.

Allotropes are different physical forms of the same element, in this case, carbon.
Examples of allotropes of carbon include diamond, graphite, fullerenes, carbon nanotubes, and amorphous carbon.
Diamond is rigid and crystalline, extremely hard, while graphite is soft and slippery, used in pencil lead.
Fullerenes are spherical or tube-shaped, consisting of 60 or more carbon atoms, while carbon nanotubes are tubular structures with unique properties.
Amorphous carbon is non-crystalline, often found in charcoal and soot.
Allotropes of carbon have varying hardness, density, and conductivity, with a wide range of applications, including electronics, materials science, and biology.