Atomic Structure Study Notecards
Set 1 of 4
Atomic Structure & Light Emission
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Card 01 • Question Bohr Anatomy
Deciphering the Bohr Model
Examine a neutral atom with 11 protons and 12 neutrons (3 electron shells: 2, 8, 1):
11 P 12 N
- What element is shown? Mass #?
- Total e⁻ vs. Valence e⁻?
- Periodic Table Period & Group?
Investigation 1B Turn card for answer ➜
Answer & Breakdown Sodium (Na)
• Element: Sodium (Na) — atomic number 11
• Mass Number: 23 (11 protons + 12 neutrons)
• Total Electrons: 11 (neutral atom: P = E)
• Valence Electrons: 1 (outermost ring)
• Atom or Ion? Atom (neutral, 11 P = 11 E)
• Stability: Unstable (needs 8 valence e⁻)
• Periodic Table: Period 3 (3 energy rings) & Group 1 (1 valence electron)
Key Concept: Number of occupied rings = Period; number of outer valence electrons = Group number (Group 1).
Card 02 • Question Octet & Stability
Atomic Stability & Electron Counts
1. What does it mean for an atom to be stable? How many valence electrons are needed?
2. How many electrons does a neutral atom of Potassium (K) have?
3. For a neutral atom of Sulfur-32 (atomic #16):
- How many protons & neutrons?
- How are its 16 electrons arranged in rings?
- How many valence electrons does it have?
Investigation 1B Turn card for answer ➜
Answer & Breakdown Stability Rules
• Atomic Stability: An atom is stable when it has a full outer ring of valence electrons. Most atoms require 8 valence electrons (Octet Rule). Exception: Helium only needs 2 (its 1st shell is full).
• Potassium (K): 19 electrons (protons = 19; neutral atom has P = E).
• Sulfur-32 Structure:
• Nucleus: 16 Protons & 16 Neutrons (32 - 16 = 16)
• Electron Rings: 2 (ring 1), 8 (ring 2), 6 (ring 3)
• Valence Electrons: 6 (unstable, needs 2 more for octet)
Rule: Shell capacities are Ring 1: max 2e⁻, Ring 2: max 8e⁻, Ring 3: holds 8e⁻ before opening shell 4.
Card 03 • Question Emission Spectra
Atomic Emission & The Flame Test
1. What is an atomic emission spectrum?
2. True or False: Each element produces its own unique emission spectrum (like a DNA fingerprint)?
3. Trace the journey of an electron producing light in the flame lab using all 6 terms:
ground state • energy • jump • excited state • fall • photon
Investigation 1B Turn card for answer ➜
Answer & Breakdown Light Emission
• Definition: The pattern formed when light emitted by energized atoms is separated into the specific wavelengths it contains.
• Fingerprint: TRUE — Every element has a unique set of electron energy transitions.
• The 5-Step Flame Test Cycle:
- Electron starts in ground state (inner low-energy ring).
- Heat adds energy, causing the electron to jump.
- Electron arrives in unstable excited state.
- Electron must fall back down to ground state.
- While falling, it releases energy by emitting a photon (visible light)!
Bohr Model Ground State: Electrons occupy the innermost possible rings closest to the nucleus.
Investigation 1B Review • Chemistry Notecards • Page 1 of 4
Set 2 of 4
Quantum Theory & Dot Structures
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Card 04 • Question Quantum Model
Modern Atomic Theory
1. What is the formal name of the current, modern atomic model?
2. How many electrons can any single individual orbital hold total?
3. If all orbitals in the nested shell diagram below are completely filled, how many total electrons are there?
Orbitals Present: 1s, 2s, 2p, 3s
Calculate maximum electron capacity for each!
Experience 4 Turn card for answer ➜
Answer & Breakdown Model Details
• Current Model: Quantum Mechanical Model (replaces circular orbits with 3D mathematical probability regions called orbitals).
• Orbital Capacity: Each individual orbital holds up to 2 electrons (with opposite spins).
• Electron Total Calculation:
• 1s: 1 orbital × 2 e⁻ = 2 e⁻
• 2s: 1 orbital × 2 e⁻ = 2 e⁻
• 2p: 3 orbitals × 2 e⁻ = 6 e⁻
• 3s: 1 orbital × 2 e⁻ = 2 e⁻
Total = 2 + 2 + 6 + 2 = 12 total electrons (Magnesium!)
Key takeaway: Sublevels contain 1 (s), 3 (p), 5 (d), or 7 (f) orbitals, each holding a maximum of 2 electrons.
Card 05 • Question Orbital Shapes
Sublevels s, p, d, f Capacities
Complete the sublevel inventory table. For each type, state its general shape and max electron capacity:
| Orbital | Shape | # Orbitals | Max e⁻ |
|---|
| s | ? | ? | ? |
| p | ? | ? | ? |
| d | ? | ? | ? |
| f | ? | ? | ? |
Experience 4 Turn card for answer ➜
Answer & Breakdown Sublevel Table
| Orbital | Shape | # Orbitals | Max e⁻ |
|---|
| s | Sphere | 1 | 2 |
| p | Dumbbell | 3 | 6 |
| d | Cloverleaf | 5 | 10 |
| f | Complex | 7 | 14 |
• Pattern: Orbitals increase by odd numbers: 1, 3, 5, 7.
• Electrons: Multiply orbitals by 2: 2, 6, 10, 14.
Memory Trick: "Some People Drive Fast" = s, p, d, f (2, 6, 10, 14 electrons).
Card 06 • Question Lewis Dots
Lewis Dot Structures
For each element below, determine its Valence Electrons, Group #, Period #, Lewis Dot diagram, and whether it is Stable or Unstable:
1. Beryllium (Be)
2. Oxygen (O)
3. Neon (Ne)
Experience 4 Turn card for answer ➜
Answer & Breakdown Lewis Dot Solutions
Be: 2 valence e⁻ | Grp 2, Per 2 | Unstable
•Be•
O: 6 valence e⁻ | Grp 16, Per 2 | Unstable
••:O:•
Ne: 8 valence e⁻ | Grp 18, Per 2 | Stable
:Ne: (8)
Drawing Rule: Place dots one by one on the 4 sides of the element symbol before pairing them up!
Investigation 1B Review • Chemistry Notecards • Page 2 of 4
Set 3 of 4
Electron Configurations & Diagrams
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Card 07 • Question The 3 Rules
Fundamental Electron Rules
1. Fill in the blanks:
"Electrons always fill the _______ (lowest / highest) energy orbitals first and have _______ (same / opposite) spins."
2. Name the three scientific principles that guide how electrons populate orbitals:
- Which principle dictates energy order?
- Which principle limits 2 electrons with opposite spins?
- Which rule explains why electrons spread out in p orbitals?
Experience 5 Turn card for answer ➜
Answer & Breakdown Filling Principles
Answer: Electrons always fill the LOWEST energy orbitals first and have OPPOSITE spins (↑↓).
• Aufbau Principle: Orbitals fill in order of increasing energy (1s → 2s → 2p → 3s → 3p → 4s → 3d...).
• Pauli Exclusion Principle: An orbital holds at most 2 electrons, and they must have opposite spins (↑ and ↓).
• Hund's Rule ("Bus Seat Rule"): For sublevels with multiple orbitals (like p, d, f), electrons occupy orbitals singly with parallel spins before pairing up.
Analogy: People sit alone in empty bus seats first (Hund's rule) before sharing a seat!
Card 08 • Question Orbital Diagrams
Drawing Orbital Diagrams
Draw the orbital diagrams (using boxes and arrows ↑ / ↓) for the following neutral elements:
a. Nitrogen (N) Atomic # 7 • 7 total electrons
b. Iron (Fe) Atomic # 26 • 26 total electrons
Be sure to follow Aufbau, Pauli, and Hund's rules!
Experience 5 Turn card for answer ➜
Answer & Breakdown Arrow Diagrams
a. Nitrogen (7 e⁻):
↑↓1s
↑↓2s
↑ ↑ ↑
2p has 3 separate unpaired electrons (Hund's Rule)!
b. Iron (26 e⁻):
↑↓1s ↑↓2s ↑↓ ↑↓ ↑↓2p ↑↓3s ↑↓ ↑↓ ↑↓3p ↑↓4s ↑↓ ↑ ↑ ↑ ↑3d
4s fills before 3d. 3d holds 6 e⁻: 1 pair + 4 unpaired.
Check: Count your arrows! Nitrogen: 2+2+3 = 7. Iron: 2+2+6+2+6+2+6 = 26.
Card 09 • Question Longhand
Longhand Electron Configurations
Write the full, complete longhand electron configuration for each element:
a. Phosphorus (P) Atomic Number: 15
b. Germanium (Ge) Atomic Number: 32
Experience 5 Turn card for answer ➜
Answer & Breakdown Configuration Solutions
a. Phosphorus (15 e⁻): 1s² 2s² 2p⁶ 3s² 3p³ Sum: 2 + 2 + 6 + 2 + 3 = 15 | Valence: 3s² 3p³ (5 valence e⁻)
b. Germanium (32 e⁻): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p² Sum: 2+2+6+2+6+2+10+2 = 32 | Valence: 4s² 4p² (4 valence e⁻)
Notice: 3d lies between 4s and 4p in filling order, but only 4s and 4p electrons count as valence electrons!
Investigation 1B Review • Chemistry Notecards • Page 3 of 4
Set 4 of 4
Shorthand & Periodic Table Blocks
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Card 10 • Question Noble Gas Shorthand
Noble Gas Configurations
How does noble gas configuration shorthand work? Write the noble gas configuration for:
1. Iodine (I) Atomic Number: 53 (Period 5, Group 17)
2. Vanadium (V) Atomic Number: 23 (Period 4, Group 5)
Experience 5 Turn card for answer ➜
Answer & Breakdown Shorthand Method
Method: Find the noble gas (Group 18) in the row above the element. Put its symbol in brackets, then write the remaining electron configuration!
Iodine (53 e⁻): [Kr] 5s² 4d¹⁰ 5p⁵ Previous noble gas: Krypton (36 e⁻) | 36 + 2 + 10 + 5 = 53
Vanadium (23 e⁻): [Ar] 4s² 3d³ Previous noble gas: Argon (18 e⁻) | 18 + 2 + 3 = 23
Golden Rule: Never use a noble gas from the same row or a lower row—always the row directly above!
Card 11 • Question Configuration Clues
Decoding Mystery Elements
Use the mystery electron configuration below to answer all three questions:
[Kr] 5s² 4d¹⁰ 5p²
- a. How many valence electrons does this element have?
- b. How many total electrons does this element have?
- c. Which element is this?
Experience 5 Turn card for answer ➜
Answer & Breakdown Tin (Sn)
• a. Valence Electrons: 4
Only the highest energy level (n=5) counts: 5s² + 5p² = 4 valence electrons. The 4d¹⁰ subshell is completely filled and part of the inner core!
• b. Total Electrons: 50
Krypton core (36) + 2 (from 5s) + 10 (from 4d) + 2 (from 5p) = 50 total e⁻.
• c. Element Identity: Tin (Sn)
Atomic number 50 on the Periodic Table.
Key Trap: Never count full d or f orbitals as valence electrons—only outer s and p orbitals count!
Card 12 • Question Periodic Geography
Periodic Table Anatomy & Blocks
On a blank periodic table, define and locate:
- Period Numbers: What do rows 1–7 tell you?
- Group Numbers: What do columns 1–18 tell you?
- Valence Electrons: What is the group shortcut?
- The 4 Blocks: Where are s, p, d, f blocks?
s-block d-block p-block
f-block (bottom 2 rows)
Periodic Mastery Turn card for answer ➜
Answer & Breakdown Block Reference
• Periods (Rows 1–7): Indicate the number of energy shells and highest principal energy level (n).
• Groups (Columns 1–18): Elements in the same group have similar chemical properties and identical valence electron counts.
• Valence Shortcut: Grp 1 = 1 | Grp 2 = 2 | Grp 13 = 3 | Grp 14 = 4 | Grp 15 = 5 | Grp 16 = 6 | Grp 17 = 7 | Grp 18 = 8 (except He = 2).
• s-block: Groups 1, 2, and Helium
• d-block: Groups 3–12 (Transition Metals)
• p-block: Groups 13–18
• f-block: Lanthanides & Actinides (bottom 2 rows)
Summary: The periodic table is shaped directly by electron orbital filling (2 cols in s, 10 in d, 6 in p, 14 in f)!
Investigation 1B Review • Chemistry Notecards • Page 4 of 4
