Atomic Architecture Slides Atomic Architecture
Building the Universe from the Inside Out: Structure, Reactivity, and Bonding
The Atomic Blueprint
The Nucleus
Contains Protons (+) and Neutrons (neutral). This is where the mass lives!
Electron Cloud
Electrons (-) orbit in shells. Valence electrons (outer shell) determine reactivity.
Nucleus
Structure & Placement
Periods (Rows)
Tell you the number of Electron Shells an atom has.
Example: Carbon (Period 2) has 2 shells.
Groups (Columns)
Tell you the number of Valence Electrons (for Groups 1-2, 13-18).
Example: Oxygen (Group 16) has 6 valence electrons.
Valence electrons are the "hands" an atom uses to bond with others!
Ionic Bonding: The Steal
One atom gives electrons, another takes them.
Occurs between Metals and Non-metals .
Atoms become Ions (charged particles).
Opposites attract! (+) and (-) stick together.
"I'll take that! Now we're stuck together."
Na
Metal (Loses)
Cl
Non-metal (Gains)
Na⁺ + Cl⁻ → NaCl
Covalent Bonding: The Share
Atoms share pairs of electrons to fill their outer shells.
Occurs between Non-metals and Non-metals .
Forms Molecules .
Neither atom is strong enough to "steal."
"Let's work together to reach 8 electrons!"
H
H
H — H (H₂)
Bonding Cheat Sheet
Feature Ionic Covalent Action Transfer (Give/Take) Sharing Elements Metal + Non-metal Non-metal + Non-metal Product Ions (Crystals) Molecules Reactivity High (Reactive) Varies
Atomic Blueprint Worksheet Project: Atomic Architect
Atomic Blueprint
IPC.7.A: Structure, Reactivity, and Bonding
Name:
Date:
Part 1: The Inner Workings
Label the subatomic particles and their charges in the diagram below. Then, fill in the table for an atom of Carbon .
Nucleus
A: ________
B: ________
C: ________
Particle Charge Location Proton Neutron Electron
Part 2: Map the First 18
Use your Periodic Table to identify how structure relates to placement.
Sodium (Na)
Period: ____ Shells: ____
Group: ____ Valence e⁻: ____
Oxygen (O)
Period: ____ Shells: ____
Group: ____ Valence e⁻: ____
Argon (Ar)
Period: ____ Shells: ____
Group: ____ Valence e⁻: ____
The Reactivity Rule:
Atoms are most stable with a full outer shell (usually 8 electrons). Why are Noble Gases (Group 18) unreactive while Alkali Metals (Group 1) are highly reactive?
Part 3: Bonding Comparison
IONIC BONDING
COVALENT BONDING
Elements Involved:
Elements Involved:
Action of Electrons:
Action of Electrons:
What is formed?
What is formed?
Complete the Bonding Flowchart:
Atom
Gains or Loses Electrons
Becomes an _______
_______ Bond
Shares Electron Pairs
Forms a _______
_______ Bond
Part 4: Sketching Structures
Draw the Lewis Dot Structures (valence electrons only) for the following atoms and show how they would bond.
A. Ionic: Sodium (Na) + Fluorine (F)
Show the electron transfer arrow!
B. Covalent: Water (H₂O)
Circle the shared electron pairs!
Part 5: Checkpoint Questions
1. Which subatomic particle determines the identity of an element?
A. Electron
B. Proton
C. Neutron
D. Nucleus
2. An atom of Phosphorus (Group 15) has how many valence electrons?
A. 3
B. 5
Atomic Blueprint Answer Key ANSWER KEY
Atomic Architecture Unit
Part 1: The Inner Workings
Diagram Labels:
A: Electron (-)
B: Electron Shell / Energy Level
C: Nucleus (Protons + Neutrons)
<table class="w-full border-collapse border border-slate-400 text-xs"><tbody><tr class="bg-slate-100 font-bold"><td class="border border-slate-400 p-1">Particle</td><td class="border border-slate-400 p-1">Charge</td><td class="border border-slate-400 p-1">Location</td></tr><tr><td class="border border-slate-400 p-1">Proton</td><td class="border border-slate-400 p-1 text-red-600">+1 (Positive)</td><td class="border border-slate-400 p-1 text-red-600">Nucleus</td></tr><tr><td class="border border-slate-400 p-1">Neutron</td><td class="border border-slate-400 p-1 text-red-600">0 (Neutral)</td><td class="border border-slate-400 p-1 text-red-600">Nucleus</td></tr><tr><td class="border border-slate-400 p-1">Electron</td><td class="border border-slate-400 p-1 text-red-600">-1 (Negative)</td><td class="border border-slate-400 p-1 text-red-600">Electron Cloud</td></tr></tbody></table>
Part 2: Map the First 18
Sodium:
Period 3 (3 Shells); Group 1 (1 Valence e⁻)
Oxygen:
Period 2 (2 Shells); Group 16 (6 Valence e⁻)
Argon:
Period 3 (3 Shells); Group 18 (8 Valence e⁻)
Reactivity Rule: Noble gases have a full outer shell (8 e⁻), making them stable/unreactive. Alkali metals have only 1 valence e⁻ and "want" to lose it to reach stability, making them highly reactive.
Part 3: Bonding Comparison
Feature
Ionic / Covalent
Elements
Metal + Non-metal / Non-metal + Non-metal
Action
Transfer (Give/Take) / Sharing Pairs
Result
Ions (Crystals) / Molecules
Part 5: Checkpoint Answers
1. Which subatomic particle determines the identity of an element?
B. Proton
2. An atom of Phosphorus (Group 15) has how many valence electrons?
B. 5
3. What happens to a neutral atom if it loses two electrons?
It becomes a positive ion (cation) with a +2 charge.
4. Which type of bond is formed when atoms of two non-metals combine?
B. Covalent
5. Why do elements in the same Group often react in similar ways?
Because they have the same number of valence electrons, which determines bonding behavior.
6. In an ionic bond, the metal atom usually becomes:
A. Positively charged
7. Carbon (Period 2) and Silicon (Period 3) both have 4 valence electrons. How many electron shells does Silicon have?
