atoms to moles powerpoint presentation.pptx

the conversion of atoms to moles

1. GOOD AFTERNOON

2. LET’S RECALL!

3. 1.What is avogadros number?

4. 2. what is the equivalent or value of 1 mole?

5. 3. what is the formula in converting the moles into molecules?

6. LET’S PLAY! ATOMIC COUNTDOWN!

7. INSTRUCTIONS: Explain that they have exactly 5 minutes to find and join with other students to create a "molecular group" by forming a molecule using the elements on their cards.

8. INSTRUCTIONS: Encourage them to share their element names with others and work together to create a valid molecule. For example, if a student has a card with "H" and another has "O," they can form a water molecule (H₂O).

9. INSTRUCTIONS: As the timer approaches the 5-minute mark, ask a few groups to share the molecules they've formed. Validate if they have correctly combined the elements to create a stable molecule.

10. Hydrogen chloride (HCl) Nitrogen dioxide (NO2) Carbon monoxide (CO) Sulfur hexafluoride (SF6) Water (H2O) Hydrogen sulfide (H2S) Methane (CH4) Nitrous oxide (N2O) Carbon dioxide (CO2) Ammonia (NH3) Sodium chloride (NaCl) Oxygen (O2) 13. Hydrogen peroxide (H2O2) 14. Sodium hydroxide (NaOH) 15. Potassium chloride (KCl) 16. Hydrochloric acid (HCl) 17. Phosphorus pentoxide (P4O10) 18. Calcium carbonate (CaCO3) 19. Nitric oxide (NO) 20. Silicon dioxide (SiO2) 21. Magnesium oxide (MgO) 22. Dinitrogen trioxide (N2O3) 23. Dinitrogen tetroxide (N2O4) 24. Hydrogen bromide (HBr) 25. Sulfur dioxide (SO2)

11. OBJECTIVES: At the end of the lesson the student should be able to; 1.Analyze the given compounds to determine the quantities of atoms present and the molecular mass; 2.Convert molecular formulas into atoms using the Avogadro’s number; and 3.Demonstrate a sense of curiosity into the application of the conversion of molecules into atoms.

12. atoms to moles

13. WHY IS IT IMPORTANT TO CONVERT ATOMS INTO MOLES? This is an easy way of determining how much of one substance can react with a given amount of another substance. From moles of a substance, one can also find the number of atoms in a sample and vice versa.

14. how to convert the moleS into atoms? USE THE GUFSA METHOD FORMULA: 1 MOL # OF ATOMS x 6.02x10 23

15. PRACTICE PROBLEM HOW MANY MOLES ARE THERE IN 5.10x10 24 ATOMS OF GOLD? 1. GIVEN 5.10 x 10 24 ATOMS OF GOLD 2. UNKNOWN NO. OF MOLES? 3. FORMULA # OF ATOMS X 1 MOL 6.02x10 23

16. PRACTICE PROBLEM HOW MANY MOLES ARE THERE IN 5.10x10 24 ATOMS OF GOLD? 4. SOLUTION = 5.10X10 24 ATOMS X 5. ANSWER = 8.47 MOLES OF GOLD NO OF MOLES 1 MOLE 6.02x10 23 ATOMS

17. PRACTICE PROBLEM HOW MANY MOLES ARE THERE IN 2.80 x 10 24 ATOMS OF SILICON? 1. GIVEN 2. UNKNOWN 3. FORMULA 4. SOLUTION 5. ANSWER

18. MOLAR MASS

19. WHAT IS MOLAR MASS? Molecular mass is the total mass of a compound. It is equal to the sum of the atomic masses or mass numbers of each element present in a compound or molecule.

20. HOW TO SOLVE THE MOLAR MASS FOR EXAMPLE: METHANE = CH 4 = 1 C ATOM + 4 H ATOMS ATOMIC MASS OF C = 1 x 12.01 G/MOL = 12.01 G/MOL ATOMIC MASS OF H = 4 x 1.00 G/MOL = 4.00 G/,OL MOLAR MASS OF CH 4 = 12.01 G/MOL + 4.00 G/MOL = 16.01 G/MOL

21. LETS TRY! GIVE THE MOLAR MASS OF FE 2 O 3

22. activity Activity Get the molecular mass of the following: 1.Ammonia: NH3 2.Sodium chloride: NaCl 3.Methane: CH4 4.Ethanol: C2H5OH 5.Sulfur Hexafloride: SF6 Solve for the atoms present in the following: HOW MUCH MOLES ARE PRESENT IN 2.23x10 23 ATOMS OF ALUMINUM

23. analysis Guide questions: 1.How do we get the molecular mass? 2.What are the particles present in compounds? How about in elements? 3.Why do we need to convert atoms into moles?

24. application 1.How important is the conversion of molecules into atoms? 2.If we convert the atoms into moles does this means that we are also breaking down chemical compounds? 3.Can we calculate the molar mass of an element in a compound?

25. thankyou for listening!