Atomic Blueprint Flashcards
Chemistry Study Cards
Investigation 1B • Atomic Structure
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○ CARD 1
Question
Reading a Bohr Model
11 P 12 N
1. What element is this? (Look at protons: 11 P)
2. What is the Mass Number? (Protons + Neutrons)
3. How many valence electrons on the outer ring?
4. What Period (rings) and Group (outer e⁻)?
Try to answer all 4 before flipping! FOLD ╎
Answer
CARD 1 KEY ○
1. Element: Sodium (Na)
11 Protons = Atomic Number 11.
2. Mass Number = 23
11 Protons + 12 Neutrons = 23.
3. Valence Electrons: 1
Only 1 red electron in the outside ring.
4. Table Position:
• Period 3 (it has 3 rings)
• Group 1 (it has 1 valence electron)
💡 Big Rule: In a neutral atom, Protons = Electrons!
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○ CARD 2
Question
When is an Atom Stable?
1. Full Ring Rule: What does an atom need to be stable?
2. Octet Rule: How many valence electrons do most atoms want?
3. Exception: Which element only needs 2 electrons?
Practice: Sulfur-32 (\(^{32}\text{S}\))
Sulfur has 16 electrons (2 in 1st, 8 in 2nd, 6 in 3rd).
Is Sulfur stable or unstable?
Remember: "Octet" means 8! FOLD ╎
Answer
CARD 2 KEY ○
1. Full Outer Ring = Stable
An atom is stable when its outside shell is completely filled with electrons.
2. The Rule of 8
Almost all atoms need 8 valence electrons to be happy and stable.
3. Helium (He) is the Exception
Helium needs only 2 electrons because its only ring holds a maximum of 2.
Sulfur Answer:
Sulfur has 6 valence electrons. It is UNSTABLE because it needs 2 more to make 8!
⭐ Noble Gases (Group 18) already have 8 electrons (stable!).
Chemistry Study Cards
Investigation 1B • Flame Lab & Orbitals
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○ CARD 3
Question
How Does Fire Make Colored Light?
Put these 4 steps of electron movement in the correct order:
Step ? • Electron falls back down
Step ? • Electron starts in Ground State
Step ? • Energy added \(\rightarrow\) Electron jumps to Excited State
Step ? • While falling, it emits a Photon (Colored Light!)
⚡ Key Test: Is light emitted when jumping UP or falling DOWN?
Think: Fireworks release light as energy drops! FOLD ╎
Answer
CARD 3 KEY ○
The 4-Step Pathway:
1
Ground State:
Electron rests in the lowest/inner ring.
2
Absorbs Fire & Jumps:
Electron jumps up to an Excited State.
3
Falls Back Down:
Excited state is unstable, so it falls back.
4
Emits a Photon (Light!):
Energy is released as a specific colored wavelength.
🚨 Golden Rule: Light is ONLY emitted when falling down!
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○ CARD 4
Question
The 4 Sublevels: s, p, d, f
Match each sublevel letter to its shape and max electrons:
| Sublevel | Shape | Max Electrons |
|---|
| s | ? | ? |
| p | ? | ? |
| d | ? | ? |
| f | Complex | 14 |
Question: How many electrons can one single orbital hold?
Odd numbers of orbitals: 1, 3, 5, 7! FOLD ╎
Answer
CARD 4 KEY ○
| Sublevel | Shape | Boxes | Max e⁻ |
|---|
| s | Sphere | 1 | 2 e⁻ |
| p | Dumbbell | 3 | 6 e⁻ |
| d | 4-Leaf Clover | 5 | 10 e⁻ |
| f | Complex | 7 | 14 e⁻ |
• Max per Single Orbital = 2 electrons
Any single orbital box can hold at most 2 electrons, and they must spin in opposite directions (↑↓).
💡 Total if 1s, 2s, 2p, 3s are full:
\(2 + 2 + 6 + 2 = \mathbf{12\text{ electrons}}\) (Magnesium, Mg).
Pattern: 1, 3, 5, 7 boxes \(\rightarrow\) Double them to get 2, 6, 10, 14!
Chemistry Study Cards
Investigation 1B • Lewis Dots & The 3 Rules
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○ CARD 5
Question
Drawing Lewis Dot Structures
How many dots do these elements get, and are they stable or unstable?
1. Beryllium (Be)
Group 2
? dots
2. Oxygen (O)
Group 16
? dots
3. Neon (Ne)
Group 18
? dots
💡 Shortcut: Look at the last digit of the Group number!
Lewis dots ONLY show valence electrons! FOLD ╎
Answer
CARD 5 KEY ○
Beryllium (Be): 2 Dots
Group 2 \(\rightarrow\) 2 valence e⁻
•Be• Unstable
Oxygen (O): 6 Dots
Group 16 \(\rightarrow\) 6 valence e⁻
:Ö• • Unstable
Neon (Ne): 8 Dots
Group 18 \(\rightarrow\) 8 valence e⁻
:N̈e: STABLE (8)
Group 1 = 1 dot • Group 2 = 2 dots • Group 13–18 = 3 to 8 dots!
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○ CARD 6
Question
The 3 Electron Rules
Match each rule name to its simple real-life nickname:
1. Aufbau Principle Which energy orbitals fill first?
2. Pauli Exclusion Principle What direction must the 2 arrows point?
3. Hund's Rule Why is it called the "Bus Seat Rule"?
🚌 Think: Do people sit next to strangers or take empty seats first?
Aufbau = German for "building up"! FOLD ╎
Answer
CARD 6 KEY ○
🧱 1. Aufbau = "Start at the Bottom"
Electrons always fill the lowest energy levels first (1s before 2s, 4s before 3d).
🔄 2. Pauli = "Opposite Spins"
Max 2 electrons per box, and they must point in opposite directions (↑↓).
🚌 3. Hund's = "The Bus Seat Rule"
Electrons spread out and sit alone first (↑) before they are forced to pair up (↑↓)!
Aufbau = Bottom First • Pauli = Opposite Spins • Hund = Spread Out!
Chemistry Study Cards
Investigation 1B • Arrows & Configurations
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○ CARD 7
Question
Orbital Arrow Diagrams
How do you draw the arrow boxes for these elements?
1. Nitrogen (N, atomic # 7)
Boxes: 1s, 2s, 2p (3 boxes).
Do the three 2p arrows pair up or spread out?
2. Iron (Fe, atomic # 26)
Which orbital fills first: 4s or 3d?
📌 Remember: Hund's rule says single arrows first!
Arrow pointing up = ↑, down = ↓ FOLD ╎
Answer
CARD 7 KEY ○
Nitrogen (7 electrons):
↑↓ 1s ↑↓ 2s ↑ ↑ ↑ 2p
All 3 2p electrons sit alone pointing UP!
Iron (26 electrons):
1s[↑↓] 2s[↑↓] 2p[↑↓][↑↓][↑↓] 3s[↑↓] 3p[↑↓][↑↓][↑↓] 4s[↑↓] 3d[↑↓][↑][↑][↑][↑]
4s has lower energy, so 4s fills before 3d!
Rule: Always put 2 arrows in 4s before touching 3d!
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○ CARD 8
Question
Decoding Configurations
An unknown neutral element has this configuration:
[Kr] 5s² 4d¹⁰ 5p²
1. How many valence electrons? (outer shell n=5)
2. How many total electrons? (Kr has 36)
3. Which element on the Periodic Table is it?
4. Where are the s, p, d, f blocks?
Add: 36 (Kr) + 2 + 10 + 2! FOLD ╎
Answer
CARD 8 KEY ○
1. Valence Electrons = 4
Only count outer shell \(n=5\): \(5s^2 + 5p^2 = 4\). (The 4d is inside!).
2. Total Electrons = 50
36 (Kr) + 2 (5s) + 10 (4d) + 2 (5p) = 50 electrons.
3. Element: Tin (Sn)
Atomic number 50, Group 14, Period 5.
Periodic Table Blocks:
• s-block: Groups 1 & 2 (left side)
• p-block: Groups 13–18 (right side)
• d-block: Groups 3–12 (middle transition metals)
• f-block: Bottom two detached rows
Noble Gas Shorthand examples: Vanadium is [Ar] 4s² 3d³ • Iodine is [Kr] 5s² 4d¹⁰ 5p⁵
