Lecture 5 - Valence Electrons, Ions, and Lewis Dot Structures

Monday, January 22, 2024

6:45 PM

 

 

"(To account for) the total difference between the maximum negative and positive valences of an element (which) is frequently eight and is in no case more than eight, I designed what may be called the theory of the cubical atom." ﷟HYPERLINK "https://pubs.acs.org/doi/epdf/10.1021/ja02261a002"The Atom and the Molecule - G.N. Lewis 1916. 
Historical textbook by Lewis: ﷟HYPERLINK "https://www.google.com/books/edition/Valence_and_the_Structure_of_Atoms_and_M/2hxDAAAAIAAJ?hl=en&gbpv=1&pg=PA107&printsec=frontcover"Valence and the Structure of Atoms and Molecules (1923)
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﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28698/discussion_topics/658275"This week's overview
Assignments this week:
﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28698/assignments/984055"Activity 1 (Elemental Exploration: A Personal Journey through the Periodic Table).
Write-up by due tomorrow Wednesday (1/24)
Peer reviews due Sunday (1/28).
﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28698/assignments/984618"HW 3 (2.1-2.2) on Aktiv Chemistry due tomorrow Wednesday (1/24) Covers periodic table, electron configurations, and valence electrons
﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28698/assignments/986501"Reading quiz 4 (2.3-2.6) due Friday.
﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28698/assignments/986593"HW 4 (2.3-2.6) on Aktiv Chemistry due Sunday (1/28). Covers ions, Lewis dot, and periodic trends

Office Hours: 
Friday 11-1 CIC 
﷟HYPERLINK "https://calendly.com/bricejurban/office-hours"By appointment
Tuesday (1/23) Schedule:
Finish up last week's discussion
Ions
Lewis Dot Diagrams
Looking Ahead
Thursday (1/25) Schedule:
Share our research of the elements 
Periodic Properties (radius, ionization)
Review of Chapters 1 and 2
Tuesday (1/30) Schedule
Midterm 1 (in-class) chapters 1 and 2
Paper and Pencil Exam
Scientific/Graphing calculator allowed
One single-sided 8.5" x 11" sheet of notes.
Practice Exam posted by Thursday
Study by completing and reviewing the homework assignments, studying the end of chapter questions from chapter 1 and 2, and reviewing the lecture notes and reading quizzes


Elaboration: What notation is used to indicate the electrons in an atom
Electron Configuration Notation
Hydrogen

Long Form:

# of Protons:

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# of Total Electrons:


# of Valence Electrons:
Oxygen
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Long Form:





Short Form:
# of Protons:


# of Total Electrons:


# of Core electrons: 


# of Valence Electrons:
Silicon 
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Is 
Long Form:





Short Form:


# of Protons:


# of Total Electrons:


# of Core electrons: 


# of Valence Electrons:




Untitled picture.png QX)Qč 
Long Form:





Short Form:
# of Protons:


# of Total Electrons:


# of Core electrons: 
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Short Form:


# of Core electrons: 


# of Valence Electrons:
Arsenic
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IS 

Long Form:





Short Form:
# of Protons:


# of Total Electrons:


# of Core electrons: 


# of Valence Electrons:

 

Uranium
Untitled picture.png Energy of Atomic Orbitals (A 
7006000000000000 
6000b0000boocooo 
6s 
500000000 
0000000 
36000 
Is 





# of Total Electrons:



Long Form:





Short Form:
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Untitled picture.png Energy of Atomic Orbitals (A 
7006000000000000 
6000b0000boocooo 
6s 
500000000 
0000000 
36000 
Is 

Short Form:
Evaluate: How can we relate electron configuration to the periodic properties?
Valence Electrons!
Untitled picture.png Isl 
2sl 
3s1 
General 
Form: 
ns 
# of 
Valence 
Electrons: 
Ion 
Formed 
Mg 
ns 
2S2 2pl 
3s2 3p1 
ns n 
2s2 2p2 
Si 
3s2 3p2 
ns n 
2s2 2p3 
3s2 3p3 
ns n 
2s2 2p4 
3s2 3p4 
ns n 
2s2 2p5 
3s2 3p5 
ns n 
He 
2p2 2p6 
3s2 3p6 
ns n 

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The valence electrons of an element determine its properties. Elements in each family across the Periodic Table have the same number of valence electrons. This explains why elements in the same group have similar chemical properties. 

Ions
The-Periodic-Table-of-Common-Ions-v2.png THE PERIODIC TABLE OF COMMON IONIC CHARGES 
HYDROGEN 
HYDRIDE 
LITHIUM 
SODIUM 
POTASSIUM 
RUBIDIUM 
BERYLLIUM 
Be2+ 
MAGNESIUM 
CALCIUM 
Ca2+ 
STRONTIUM 
BARIUM 
Ba2+ 
RADIUM 
Ra2+ 
KEY 
Name of ion 
LITHIUM 
Ion formula 
When there is more than one common ion, 
the more common ion is shown on top. 
Elements for which no ion is shown are 
those which do not commonly form 
ions, or superheavy elements whose 
chemistry is currently unknown. 
CAESIUM 
FRANCIUM 
Ci 
SCANDIUM 
YTTRIUM 
La-Lu 
Ac-Lr 
TITANIUM(IV) 
TITANIUM(III) 
Ti3+ 
ZIRCONIUM 
HAFNIUM 
Hf4+ 
RUTHERFORDIUM 
LANTHANUM 
La3+ 
ACTINIUM 
Ac3+ 
VANADIUM(III) 
VANADIUM(V) 
NIOBIUM(V) 
NIOBIUM 
Nb3+ 
TANTALUM 
Ta5+ 
OUBNIUM 
Db5+ 
CERIUM 
Ce3+ 
THORIUM 
Th4+ 
CHROMIUM(III) 
Cr3+ 
CHROMIUM(II) 
MOLYBDENUM 
TUNGSTEN 
SEABORGIUM 
PRASEODYMIUM 
PROTACTINIUM(V) 
PROTACTINIUM(IV) 
MANGANESE(II) 
Mn2+ 
MANGANESE(IV) 
Mn4+ 
TECHNETIUM 
RHENIUM 
Re7+ 
BOHRIUM 
Bh7+ 
NEODYMIUM 
Nd3+ 
URANIUM(VI) 
URANIUM(IV) 
IRON(III) 
RUTHENIUM(III) 
RUTHENIUM(IV) 
OSMIUM 
Os4+ 
HASSIUM 
Hs4+ 
PROMETHIUM 
Pm3+ 
NEPTUNIUM 
COBALT(II) 
C02* 
COBALT(III) 
C03+ 
RHODIUM 
Rh3+ 
IRIDIUM 
MEITNERIUM 
Mt 
SAMARIUM(III) 
Sm3+ 
SAMARIUM(II) 
Sm2+ 
PLUTONIUM(IV) 
Pu4+ 
PLUTONIUM(VI) 
Pu6+ 
NICKEL(II) 
NICKEL(III) 
PALLADIUM(II) 
Pd2+ 
PALLADIUM(IV) 
PLATINUM(IV) 
Pt4+ 
PLATINUM(II) 
Pt2+ 
DARMSTADTIUM 
EUROPIUM(III) 
Eu3+ 
EUROPIUM(II) 
Eu2+ 
AMERICIUM(III) 
Am3+ 
AMERICIUM(IV) 
Am4+ 
COPPER(II) 
Cu2+ 
COPPER(I) 
SILVER 
GOLD(III) 
Au3+ 
GOLD(I) 
ROENTGENIUM 
GADOLINIUM 
Gd3+ 
CURIUM 
Cm3+ 
ZINC 
Zn2+ 
CADMIUM 
Cd2+ 
MERCURY(II) 
MERCURY(I) 
COPERNICIUM 
Cn 
TERBIUM 
Tb3+ 
BERKELIUM(III) 
BERKELIUM(IV) 
BORON 
ALUMINIUM 
A13+ 
GALLIUM 
Ga3+ 
INDIUM 
In3+ 
THALLIUM(I) 
THALLIUM(III) 
NIHONIUM 
DYSPROSIUM 
DY3+ 
CALIFORNIUM 
Cf3+ 
CARBON 
SILICON 
GERMANIUM 
Ge4+ 
TIN(IV) 
Sn2+ 
LEAD(II) 
LEAD(IV) 
FLEROVIUM 
HOLMIUM 
H 03+ 
EINSTEINIUM 
Es3+ 
NITRIDE 
PHOSPHIDE 
ARSENIDE 
As3— 
ANTIMONY(III) 
ANTIMONY(V) 
Sb5+ 
BISMUTH(III) 
BISMUTH(V) 
MOSCOVIUM 
Mc 
ERBIUM 
FERMIUM 
Fm3+ 
OXIDE 
02- 
SULFIDE 
SELENIOE 
Se2- 
TELLURIDE 
POLONIUM(II) 
P02+ 
POLONIUM(IV) 
P04+ 
LIVERMORIUM 
THULIUM 
MENDELEVIUM(II) 
Md2+ 
MENDELEVIUM(III) 
Md3+ 
FLUORIDE 
CHLORIDE 
BROMIDE 
IODIDE 
ASTATIDE 
TENNESSINE 
YTTERBIUM(III) 
YTTERBIUM(II) 
NOBELIUM(II) 
N 02+ 
NOBELIUM(III) 
N03+ 
HELIUM 
NEON 
ARGON 
Ar 
KRYPTON 
XENON 
RADON 
OGANESSON 
LUTETIUM 
Lu3+ 
LAWRENCIUM 
O Andy Brunning/Compound Interest 2019 1 www.compoundchem.com I @compoundchem 
Shared under a Creative Commons 4.0 Attribution-NoDerivatives-NonCommercial licence. 
BY 
NC 
ND 
#1YPT2019 
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The-Periodic-Table-of-Common-Ions-v2.png THE PERIODIC TABLE OF COMMON IONIC CHARGES 
HYDROGEN 
HYDRIDE 
LITHIUM 
SODIUM 
POTASSIUM 
RUBIDIUM 
BERYLLIUM 
Be2+ 
MAGNESIUM 
CALCIUM 
Ca2+ 
STRONTIUM 
BARIUM 
Ba2+ 
RADIUM 
Ra2+ 
KEY 
Name of ion 
LITHIUM 
Ion formula 
When there is more than one common ion, 
the more common ion is shown on top. 
Elements for which no ion is shown are 
those which do not commonly form 
ions, or superheavy elements whose 
chemistry is currently unknown. 
CAESIUM 
FRANCIUM 
Ci 
SCANDIUM 
YTTRIUM 
La-Lu 
Ac-Lr 
TITANIUM(IV) 
TITANIUM(III) 
Ti3+ 
ZIRCONIUM 
HAFNIUM 
Hf4+ 
RUTHERFORDIUM 
LANTHANUM 
La3+ 
ACTINIUM 
Ac3+ 
VANADIUM(III) 
VANADIUM(V) 
NIOBIUM(V) 
NIOBIUM 
Nb3+ 
TANTALUM 
Ta5+ 
OUBNIUM 
Db5+ 
CERIUM 
Ce3+ 
THORIUM 
Th4+ 
CHROMIUM(III) 
Cr3+ 
CHROMIUM(II) 
MOLYBDENUM 
TUNGSTEN 
SEABORGIUM 
PRASEODYMIUM 
PROTACTINIUM(V) 
PROTACTINIUM(IV) 
MANGANESE(II) 
Mn2+ 
MANGANESE(IV) 
Mn4+ 
TECHNETIUM 
RHENIUM 
Re7+ 
BOHRIUM 
Bh7+ 
NEODYMIUM 
Nd3+ 
URANIUM(VI) 
URANIUM(IV) 
IRON(III) 
RUTHENIUM(III) 
RUTHENIUM(IV) 
OSMIUM 
Os4+ 
HASSIUM 
Hs4+ 
PROMETHIUM 
Pm3+ 
NEPTUNIUM 
COBALT(II) 
C02* 
COBALT(III) 
C03+ 
RHODIUM 
Rh3+ 
IRIDIUM 
MEITNERIUM 
Mt 
SAMARIUM(III) 
Sm3+ 
SAMARIUM(II) 
Sm2+ 
PLUTONIUM(IV) 
Pu4+ 
PLUTONIUM(VI) 
Pu6+ 
NICKEL(II) 
NICKEL(III) 
PALLADIUM(II) 
Pd2+ 
PALLADIUM(IV) 
PLATINUM(IV) 
Pt4+ 
PLATINUM(II) 
Pt2+ 
DARMSTADTIUM 
EUROPIUM(III) 
Eu3+ 
EUROPIUM(II) 
Eu2+ 
AMERICIUM(III) 
Am3+ 
AMERICIUM(IV) 
Am4+ 
COPPER(II) 
Cu2+ 
COPPER(I) 
SILVER 
GOLD(III) 
Au3+ 
GOLD(I) 
ROENTGENIUM 
GADOLINIUM 
Gd3+ 
CURIUM 
Cm3+ 
ZINC 
Zn2+ 
CADMIUM 
Cd2+ 
MERCURY(II) 
MERCURY(I) 
COPERNICIUM 
Cn 
TERBIUM 
Tb3+ 
BERKELIUM(III) 
BERKELIUM(IV) 
BORON 
ALUMINIUM 
A13+ 
GALLIUM 
Ga3+ 
INDIUM 
In3+ 
THALLIUM(I) 
THALLIUM(III) 
NIHONIUM 
DYSPROSIUM 
DY3+ 
CALIFORNIUM 
Cf3+ 
CARBON 
SILICON 
GERMANIUM 
Ge4+ 
TIN(IV) 
Sn2+ 
LEAD(II) 
LEAD(IV) 
FLEROVIUM 
HOLMIUM 
H 03+ 
EINSTEINIUM 
Es3+ 
NITRIDE 
PHOSPHIDE 
ARSENIDE 
As3— 
ANTIMONY(III) 
ANTIMONY(V) 
Sb5+ 
BISMUTH(III) 
BISMUTH(V) 
MOSCOVIUM 
Mc 
ERBIUM 
FERMIUM 
Fm3+ 
OXIDE 
02- 
SULFIDE 
SELENIOE 
Se2- 
TELLURIDE 
POLONIUM(II) 
P02+ 
POLONIUM(IV) 
P04+ 
LIVERMORIUM 
THULIUM 
MENDELEVIUM(II) 
Md2+ 
MENDELEVIUM(III) 
Md3+ 
FLUORIDE 
CHLORIDE 
BROMIDE 
IODIDE 
ASTATIDE 
TENNESSINE 
YTTERBIUM(III) 
YTTERBIUM(II) 
NOBELIUM(II) 
N 02+ 
NOBELIUM(III) 
N03+ 
HELIUM 
NEON 
ARGON 
Ar 
KRYPTON 
XENON 
RADON 
OGANESSON 
LUTETIUM 
Lu3+ 
LAWRENCIUM 
O Andy Brunning/Compound Interest 2019 1 www.compoundchem.com I @compoundchem 
Shared under a Creative Commons 4.0 Attribution-NoDerivatives-NonCommercial licence. 
BY 
NC 
ND 
#1YPT2019 

If you change the number of protons you get a different element
If you change the number of neutrons you get a different isotope
If you change the number of electrons you get an ion
Adding electrons (which are negative) makes the atom negatively ﷐−﷯ charged. 
These are known as anions
Element suffix is replaced with -ide e.g. nitride ion ﷐𝑁﷮3−﷯
Removing electrons consequently causes the atom to be positively ﷐+﷯ charged.
These ions are known as cations
Element suffix is kept same e.g. sodium ion ﷐𝑁𝑎﷮+﷯

CationsandAnions.png Cations vs Anions - Difference Between Cations and Anions with Examples
Untitled picture See related image detail. "Cation - science pun cat new" by linkitty | Redbubble
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Untitled picture See related image detail. "Cation - science pun cat new" by linkitty | Redbubble

Untitled picture.png Isotopic Notation (with charges) 
15 3- 
Mass Number (A) 
Charge 
Atomic Number (Z) 
7 
Element Symbol 

# of
protons
# of 
neutrons
# of
total
electrons
type of ion 
(cation, anion
Or not an ion)
Short-form electron configuration
e.g. [Ne]2s2
 ﷐﷐﷮𝟏﷮𝑯﷯﷮﷮−﷯





﷐﷐﷮𝟑𝟓﷮𝑪𝒍﷯﷮﷮−﷯





﷐﷐﷮𝟒𝟎﷮𝑪𝒂﷯﷮﷮𝟐+﷯





﷐﷮𝟒𝟎﷮𝑨𝒓﷯





﷐﷐﷮𝟔𝟎﷮𝑭𝒆﷯﷮﷮𝟐+﷯





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Lewis Dot Structures
Untitled picture.png Na 
val e- 
1 
val e- 
Mg 
val e- 
2 
val e- 
0 
AI 
val e- 
3 
val e- 
0 
Si 
val e- 
4 
val e- 
5 
val e- 
8 
s 
val e- 
6 
val e- 
8 
Cl 
val e- 
7 
val e- 
8 
Ar 
val e- 
8 
Maximum of eight valence electrons
Four areas (top, bottom, left, right) (one s + three p orbitals)
One electron dot in each area before pairing
Helium and Hydride are exceptions (only has s orbital)



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