Matter Builder Anchor Charts
Anchor Chart 1
Atomic Structure & Subatomic Particles
Building Blocks
1. Anatomy of the Atom (The Building Block of Matter)
Bohr Model & Cloud
0
0
0
-
-
-
-
Nucleus (p⁺ + n⁰) & Electrons (e⁻)
- Proton (p⁺) Charge: +1 • Mass: 1 amu
Location: Nucleus • Role: Determines the element's identity (Atomic Number).
0 Neutron (n⁰) Charge: 0 • Mass: 1 amu
Location: Nucleus • Role: Stabilizes the nucleus and adds atomic mass.
- Electron (e⁻) Charge: -1 • Mass: ~0 amu
Location: Electron Cloud • Role: Forms chemical bonds with other atoms.
2. Reading a Periodic Table Tile (The A-P-E M-A-N Strategy)
Quick Calculation Strategy
6
C
Carbon
12.011 (Mass)
A = P = E Neutral Atom
- • Atomic Number = 6
- • Protons = 6
- • Electrons = 6
M - A = N Finding Neutrons
- • Mass Number (12)
- • Minus Atomic # (6)
- • Equals Neutrons = 6
Key Rule to Remember
Protons give the atom its identity, electrons control chemical bonding, and neutrons hold the nucleus together.
Anchor Chart 2
Matter Hierarchy & Chemical Formulas
Particle Models
1. The 4 Levels of Matter (From Single Atoms to Compounds)
Progressive Models
Level 1
Single Atom
One individual building sphere.
H
Single Particle Ex: 1 Hydrogen (H)
Level 2
Element
Only ONE type of atom.
O
O
Pure Substance Ex: O₂, Au, Fe
Level 3
Molecule
2+ atoms bonded together.
O
O
Bonded Cluster Ex: O₂, N₂, H₂O
Level 4
Compound
2+ DIFFERENT elements.
O
H
H
Different Elements Ex: H₂O, CO₂
The Golden Rule:
All compounds are molecules (because they contain bonded atoms), but not all molecules are compounds (e.g., O₂ is a molecule, but NOT a compound because it contains only one element type).
2. Decoding Chemical Formulas (Subscripts vs. Coefficients)
Counting Atoms
3H₂O
3 Molecules of Water
3 (Big)
Coefficient = Number of Molecules
Multiplies all atoms across the entire molecule.
₂ (Small)
Subscript = Count of Specific Atom
Applies ONLY to the element right before it.
H: 3 × 2 = 6 atoms O: 3 × 1 = 3 atoms Total = 9
Color Code Key:
Hydrogen (H) Oxygen (O) Carbon (C) Nitrogen (N)
Anchor Chart 3
Chemical Bonds & Classifying Matter
Bonds vs. Mixes
1. The Two Main Chemical Bonds (How Atoms Lock Together)
Valence Electrons
Sharing Electrons Nonmetal + Nonmetal
Covalent Bonding
Atoms overlap shells to share pairs of electrons for stability.
H
H
Examples: Water ($H_2O$), Oxygen ($O_2$), Carbon Dioxide ($CO_2$).
Transferring Electrons Metal + Nonmetal
Ionic Bonding
One atom transfers electron(s), forming +/- charged ions that attract.
Na +
Gives 1 e⁻
attracts
Cl -
Takes 1 e⁻
Examples: Table Salt ($NaCl$), Calcium Chloride ($CaCl_2$).
2. Classifying All Matter: Pure Substances vs. Mixtures
Particle Visual Guide
Pure Substances Chemical Bond
Fixed composition; separated ONLY by chemical reactions.
Element
All identical atoms
Compound
Fixed bonded ratio
Mixtures Physical Blend
Not bonded; separated easily by physical methods (filtering, boiling).
Homogeneous
Uniform (Salt water)
Heterogeneous
Uneven (Salad, Sand)
Quick Identification Test
Did combining them create a new substance with new properties? YES = Chemical Bond (Compound) • Can you physically separate them? YES = Mixture
