Chemistry SL
6
Chapters
243
Notes
Chapter 1 - Models Of The Particulate Nature Of Matter
Chapter 2 - Models Of Bonding & Structure
Chapter 3 - Classification Of Matter
Chapter 4 - What Drives Chemical Reactions?
Chapter 5 - How Much, How Fast & How Far?
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Chemistry SL
Chapter 1 - Models Of The Particulate Nature Of Matter
Empirical vs. Molecular Formulas: Unlocking Chemical Secrets
452 words
3 mins read
Last edited on 5th Nov 2024
Table of content
Molecular formula vs empirical formula🧪
- Molecular Formula: This shows the actual number of atoms of each element in the molecule of a substance. It's like a detailed recipe!
- Empirical Formula: This shows the simplest ratio of atoms in the substance. Think of it as a simplified recipe!
- Real-World Example: For glucose (sugar you use in your kitchen), the molecular formula is C6H12O6, but the empirical formula is CH2O.
Ionic compounds🧲
- For ionic compounds (like salt), the empirical formula is the same as the formula unit, representing the simplest ratio of ions.
- Real-World Example: For table salt (NaCl), the empirical formula and the formula unit are both NaCl.
Moles & atomic ratio🧮
- The number of atoms is proportional to the amount in moles (N = n × NA).
- Real-World Example: In water (H2O), the atomic ratio of hydrogen to oxygen is 2:1. So, one molecule of water has 2 atoms of hydrogen and 1 atom of oxygen!
Percentage composition (ω)⚖️
- Expresses the elemental composition of a compound in percent by mass.
- Mole ratio can be used to calculate this.
- Real-World Example: If you're baking a cake, the percentage composition would tell you what percent of the cake's weight is flour, sugar, eggs, etc.
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Chemistry SL
Chapter 1 - Models Of The Particulate Nature Of Matter
Empirical vs. Molecular Formulas: Unlocking Chemical Secrets
452 words
3 mins read
Last edited on 5th Nov 2024
Table of content
Molecular formula vs empirical formula🧪
- Molecular Formula: This shows the actual number of atoms of each element in the molecule of a substance. It's like a detailed recipe!
- Empirical Formula: This shows the simplest ratio of atoms in the substance. Think of it as a simplified recipe!
- Real-World Example: For glucose (sugar you use in your kitchen), the molecular formula is C6H12O6, but the empirical formula is CH2O.
Ionic compounds🧲
- For ionic compounds (like salt), the empirical formula is the same as the formula unit, representing the simplest ratio of ions.
- Real-World Example: For table salt (NaCl), the empirical formula and the formula unit are both NaCl.
Moles & atomic ratio🧮
- The number of atoms is proportional to the amount in moles (N = n × NA).
- Real-World Example: In water (H2O), the atomic ratio of hydrogen to oxygen is 2:1. So, one molecule of water has 2 atoms of hydrogen and 1 atom of oxygen!
Percentage composition (ω)⚖️
- Expresses the elemental composition of a compound in percent by mass.
- Mole ratio can be used to calculate this.
- Real-World Example: If you're baking a cake, the percentage composition would tell you what percent of the cake's weight is flour, sugar, eggs, etc.
Unlock the Full Content!
Dive deeper and gain exclusive access to premium files of Chemistry SL. Subscribe now and get closer to that 45 🌟