Uploaded August 2025 | Updated September 2026, 2 weeks ago
Valence Electrons per Family
Dr. DeBacco
General Trends
Left to right across a period: Valence electrons increase by one per group.
Top to bottom in a group: Valence electron count stays the same, but energy levels increase.
Cations
Alkali Metals
1 valence electron
Alkaline Earth Metals
2 valence electrons
Boron Family
3 valence electrons
Carbon Family
Carbon has four electrons in its outermost shell, which are its valence electrons.
These elements have a tendency to form covalent bonds sharing electrons allowing for a stable octet (8 electrons) in its outermost shell.
This makes these elements versatile for building diverse molecules
Anions
Nitrogen Family
Forms -3 to +5 oxidation states
Oxygen Family
Often form -2 ions, reactive nonmetals
Halogens
Forms -1 ions and is very reactive
Noble Gases
Noble gases have either 2 or 8 valence electrons.
Helium has 2, following the "duet rule", while all other noble gases (Neon, Argon, Krypton, Xenon, Radon, and Oganesson) have 8, following the "octet rule".
This full valence shell makes them exceptionally stable and unreactive
Transition Metals (Groups 3–12)
Have variable oxidation states due to d-orbital involvement
Generally, more complex and less predictable than main-group elements.
Lanthanides and Actinides (f-block)
Valence electrons vary widely, often involving 4f or 5f orbitals.
Commonly show +3 oxidation states, but can range from +2 to +6 depending on the element.
Link to Lecture Slides: drive.google.com/file/d/1cPUUUvDpIK4p42iBHhU-km8-lDlYP19k/view?usp=drive_link
*Due to the description character limit the full work cited for "Valence Electrons per Family" can be viewed at... docs.google.com/document/d/1N8Ode4Rc6puhHMMS38gDNn_1xrLSDQVY/edit?usp=drive_link&ouid=104237452697237972847&rtpof=true&sd=true
Valence Electrons per Family
Dr. DeBacco
General Trends
Left to right across a period: Valence electrons increase by one per group.
Top to bottom in a group: Valence electron count stays the same, but energy levels increase.
Cations
Alkali Metals
1 valence electron
Alkaline Earth Metals
2 valence electrons
Boron Family
3 valence electrons
Carbon Family
Carbon has four electrons in its outermost shell, which are its valence electrons.
These elements have a tendency to form covalent bonds sharing electrons allowing for a stable octet (8 electrons) in its outermost shell.
This makes these elements versatile for building diverse molecules
Anions
Nitrogen Family
Forms -3 to +5 oxidation states
Oxygen Family
Often form -2 ions, reactive nonmetals
Halogens
Forms -1 ions and is very reactive
Noble Gases
Noble gases have either 2 or 8 valence electrons.
Helium has 2, following the "duet rule", while all other noble gases (Neon, Argon, Krypton, Xenon, Radon, and Oganesson) have 8, following the "octet rule".
This full valence shell makes them exceptionally stable and unreactive
Transition Metals (Groups 3–12)
Have variable oxidation states due to d-orbital involvement
Generally, more complex and less predictable than main-group elements.
Lanthanides and Actinides (f-block)
Valence electrons vary widely, often involving 4f or 5f orbitals.
Commonly show +3 oxidation states, but can range from +2 to +6 depending on the element.
Link to Lecture Slides: drive.google.com/file/d/1cPUUUvDpIK4p42iBHhU-km8-lDlYP19k/view?usp=drive_link
*Due to the description character limit the full work cited for "Valence Electrons per Family" can be viewed at... docs.google.com/document/d/1N8Ode4Rc6puhHMMS38gDNn_1xrLSDQVY/edit?usp=drive_link&ouid=104237452697237972847&rtpof=true&sd=true
