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Understanding Electron Dot Diagrams and Mass Calculations in Chemistry

This lesson focuses on important chemistry concepts such as electron dot diagrams and mass calculations from equations. Students will learn how to accurately represent electron configurations, including the correct number of neutrons and electrons, and how to draw electron dot diagrams for various elements and molecules. Additionally, the session will cover how to calculate masses from chemical equations, adhering to the principle of conservation of mass. Engaging worksheets and examples will reinforce learning, preparing students for future assessments in chemistry.

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Understanding Electron Dot Diagrams and Mass Calculations in Chemistry

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  1. Equations – Computer Says No! http://www.roystoncartoons.com/2009/11/cartoon-illustration-computer-says-no.html

  2. Today’s Lesson • Go through answers to test • Review of electron dot diagrams • Drawing electron dot diagrams • Working out masses from equations

  3. Electron Dot Diagrams • In an electron dot diagram, you need to include the following: • Number of Neutrons and Electrons in the nucleus • The correct number of electrons in each shell • Up to 2 electrons in first shell • Up to 8 electrons in second shell • Up to 18 electrons in third shell • Etc – but your last shell normally has 8 electrons unless it has only 1 electron shell

  4. Sharing Electrons • For molecules, they like to share (covalent) or donate (ionic) electrons. • This is what we will be focusing on. I’ll draw some examples on the board. • Now we can complete a fun worksheet • I will also be collecting your workbooks around every 2-3 weeks from now on. As such, you need to write your answers in your books.

  5. The Mole • In Chemistry, we measure the mass of objects through ‘the mole’. • The mole is the mass of how many atoms or molecules there are. • It’s known as Avogadro’s Constant. There are 6.02 X 10^23 atoms of molecules in a mole. • Eg, there are 602000000000000000000000 atoms of Hydrogen in 1g.

  6. Masses From Equations • In an equation, both sides need to have the same mass or same amount of stuff • Eg; C (s) + O2 (g) -> CO2 (g) • 1 C Atom + 1 Oxygen Molecule = 1 molecule of Carbon Dioxide • 12 + 32 = 44g • See the pattern – both sides have the same mass 

  7. Calculating Mass From Equations • You need to do the following steps: • Write the balanced equation for the reaction • Write down the relative atomic mass (Ar) or formula mass for each substance • From the equation, write down the reacting amount in grams • Once you know these, you can find out the actual mass. • Next slide has an example

  8. H2OOOOH! • 2H2 (g) + O2 (g) -> 2H2O (l) • 2X2g + 32g 2 X 18g • 4g + 32g 36 g • We only have 1 g of H, so much Oxygen and water will we make?? • 4/4g + 32/4g 36/4g • 1 g 8g 9g • Complete Q 1, 2 & 3 on P 118/119

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