Uploaded August 2025 | Updated September 2026, 2 weeks ago
Types of Chemical Bonds
Dr. DeBacco
What is a Bond?
A chemical bond is essentially the force that holds atoms together to form molecules and compounds.
Most chemical reactions you see (rusting iron, baking bread, digesting food) are just atoms rearranging their bonds.
Ionic Bonds
One atom donates an electron to another, creating positive and negative ions that attract each other.
The atom that loses electrons becomes a cation (positive), and the atom that gains electrons becomes an anion (negative).
Typically between Metals and nonmetals.
Example: Sodium chloride (NaCl) — table salt.
Covalent Bonds
Atoms share electrons to reach a stable electron configuration.
Typically between Nonmetals.
Example: Water (H₂O), carbon dioxide (CO₂).
Covalent Bonds- Single, Double or Triple
Can be single, double, or triple bonds
Resulting molecules are often gases or liquids.
Single Bond: One pair of electrons shared
Ex. H₂
Double Bond: Two pairs of electrons shared
Ex. O₂
Triple Bond: Three pairs of electrons shared
Ex. N₂
Types of Covalent Bonds
Polar Covalent: Electrons are shared unequally due to differences in electronegativity, creating partial charges
H₂O, where oxygen is more electronegative, pulling electrons closer and creating a δ⁻ charge on O and δ⁺ on H).
Nonpolar Covalent: Electrons are shared equally because the atoms have similar electronegativities
Cl₂, where the electronegativity difference is ~0)
Non-Polar Covalent Bonds
Electrons are shared equally between atoms.
No dipole (no partial charges).
Atoms involved have similar or identical electronegativity (tendency to attract electrons) with the molecule often symmetrical shape.
These molecules tend to have low boiling and melting points and are not soluble in water.
They can dissolve in other non-polar substances like oils.
Examples:
Hydrogen molecule (H₂)
Methane (CH₄)
Oxygen molecule (O₂)
Polar Covalent Bonds
Electrons are shared unequally between atoms.
Partial positive and negative charges are created (δ⁺ and δ⁻).
One atom has greater electronegativity and pulls electrons closer creating a molecule that has an asymmetrical shape.
These molecules have moderate boiling/melting points, and exhibit interesting behavior like hydrogen bonding and are usually soluble in water
Examples:
Water (H₂O) — oxygen pulls electrons more than hydrogen.
Ammonia (NH₃)
Hydrogen fluoride (HF)
Metallic Bond
Metal atoms share a “sea” of delocalized electrons that flow freely.
The strength of the bond depends on the number of delocalized electrons and the charge of the metal ions.
Examples:
Copper (Cu): Used in electrical wiring due to its excellent conductivity.
Iron (Fe): Strong metallic bonding contributes to its use in construction.
Link to Lecture Slides: drive.google.com/file/d/1CLZEOkOPfO33qrKXstPy1rU7xLq46rB1/view?usp=drive_link
*Due to the description character limit the full work cited for "Types of Chemical Bonds" can be viewed at... docs.google.com/document/d/1d2lti1-E59NzEMSqGSlgbTN22L5hb838/edit?usp=drive_link&ouid=104237452697237972847&rtpof=true&sd=true
Types of Chemical Bonds
Dr. DeBacco
What is a Bond?
A chemical bond is essentially the force that holds atoms together to form molecules and compounds.
Most chemical reactions you see (rusting iron, baking bread, digesting food) are just atoms rearranging their bonds.
Ionic Bonds
One atom donates an electron to another, creating positive and negative ions that attract each other.
The atom that loses electrons becomes a cation (positive), and the atom that gains electrons becomes an anion (negative).
Typically between Metals and nonmetals.
Example: Sodium chloride (NaCl) — table salt.
Covalent Bonds
Atoms share electrons to reach a stable electron configuration.
Typically between Nonmetals.
Example: Water (H₂O), carbon dioxide (CO₂).
Covalent Bonds- Single, Double or Triple
Can be single, double, or triple bonds
Resulting molecules are often gases or liquids.
Single Bond: One pair of electrons shared
Ex. H₂
Double Bond: Two pairs of electrons shared
Ex. O₂
Triple Bond: Three pairs of electrons shared
Ex. N₂
Types of Covalent Bonds
Polar Covalent: Electrons are shared unequally due to differences in electronegativity, creating partial charges
H₂O, where oxygen is more electronegative, pulling electrons closer and creating a δ⁻ charge on O and δ⁺ on H).
Nonpolar Covalent: Electrons are shared equally because the atoms have similar electronegativities
Cl₂, where the electronegativity difference is ~0)
Non-Polar Covalent Bonds
Electrons are shared equally between atoms.
No dipole (no partial charges).
Atoms involved have similar or identical electronegativity (tendency to attract electrons) with the molecule often symmetrical shape.
These molecules tend to have low boiling and melting points and are not soluble in water.
They can dissolve in other non-polar substances like oils.
Examples:
Hydrogen molecule (H₂)
Methane (CH₄)
Oxygen molecule (O₂)
Polar Covalent Bonds
Electrons are shared unequally between atoms.
Partial positive and negative charges are created (δ⁺ and δ⁻).
One atom has greater electronegativity and pulls electrons closer creating a molecule that has an asymmetrical shape.
These molecules have moderate boiling/melting points, and exhibit interesting behavior like hydrogen bonding and are usually soluble in water
Examples:
Water (H₂O) — oxygen pulls electrons more than hydrogen.
Ammonia (NH₃)
Hydrogen fluoride (HF)
Metallic Bond
Metal atoms share a “sea” of delocalized electrons that flow freely.
The strength of the bond depends on the number of delocalized electrons and the charge of the metal ions.
Examples:
Copper (Cu): Used in electrical wiring due to its excellent conductivity.
Iron (Fe): Strong metallic bonding contributes to its use in construction.
Link to Lecture Slides: drive.google.com/file/d/1CLZEOkOPfO33qrKXstPy1rU7xLq46rB1/view?usp=drive_link
*Due to the description character limit the full work cited for "Types of Chemical Bonds" can be viewed at... docs.google.com/document/d/1d2lti1-E59NzEMSqGSlgbTN22L5hb838/edit?usp=drive_link&ouid=104237452697237972847&rtpof=true&sd=true
