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CHAPTER 2 Matter and Atoms 2.2 Molecules and Compounds.

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1 CHAPTER 2 Matter and Atoms 2.2 Molecules and Compounds

2 If you cut a piece of wax, is it still wax?
If you cut that smaller piece again, is it still wax? When does it stop being wax?

3 One O2 molecule One H2 molecule molecule: a group of atoms chemically bonded together.

4 One H2 molecule One O2 molecule One H2O molecule molecule: a group of atoms chemically bonded together. compound: a substance containing more than one element in which atoms of different elements are chemically bonded together.

5 What do all these have in common?

6 What do all these have in common?
They are made up of only 3 types of atoms: carbon, oxygen and hydrogen.

7 The alphabet of chemistry
More than 200,000 words in the English language Trillions of substances that make up the universe

8 The chemical formula

9 The chemical formula

10 Write a chemical formula for a compound that has three hydrogen (H) atoms for each atom of nitrogen (N).

11 Write a chemical formula for a compound that has three hydrogen (H) atoms for each atom of nitrogen (N). Asked: Chemical formula Given: 3 hydrogen (H) and 1 nitrogen (N) Relationships: The subscript tells the number of each element in the compound.

12 Write a chemical formula for a compound that has three hydrogen (H) atoms for each atom of nitrogen (N). Asked: Chemical formula Given: 3 hydrogen (H) and 1 nitrogen (N) Relationships: The subscript tells the number of each element in the compound. Answer: NH3

13 The properties of a compound depend more on
the exact structure of the molecule than on the individual elements from which it is made.

14 The arrangement of letters matters!
U L F U N E R A L R E A L F U N The arrangement of letters matters!

15 The arrangement of atoms matters!

16 Representation There are many ways of representing the same thing.

17 Representation

18 Ionic compounds Salt (NaCl) is not a molecule!

19 ionic compound: a compound such as a salt in which positive and negative ions attract each other to keep matter together. ion: an atom or small molecule with an overall positive or negative chare as a result of an imbalance of protons and electrons.

20 Formula mass The formula mass of water (H2O) is 18 g.

21 What is the mass of 1 mole of methane (CH4)?

22 What is the mass of 1 mole of methane (CH4)?
Asked: The mass of 1 mole of methane Given: Methane (CH4) contains 1 carbon (C) and 4 hydrogen (H) atoms Relationships: The formula mass is the sum of the atomic masses for each atom in the compound

23 What is the mass of 1 mole of methane (CH4)?
Asked: The mass of 1 mole of methane Given: Methane (CH4) contains 1 carbon (C) and 4 hydrogen (H) atoms Relationships: The formula mass is the sum of the atomic masses for each atom in the compound Solve: Answer: One mole of methane (CH4) has a mass of g.

24 How many moles are in 100 grams of water (H2O)?

25 How many moles are in 100 grams of water (H2O)?
Asked: The moles in 100 g of water Given: Water (H2O) contains 2 hydrogen (H) atoms and 1 oxygen (O) atom. Relationships: The formula mass is the sum of the atomic masses for each atom in the compound.

26 How many moles are in 100 grams of water (H2O)?
Asked: The moles in 100 g of water Given: Water (H2O) contains 2 hydrogen (H) atoms and 1 oxygen (O) atom. Relationships: The formula mass is the sum of the atomic masses for each atom in the compound. Solve: Answer: 100 g of water (H2O) contains 5.55 moles.

27 How many grams are in 2. 300 moles of butane (C4H10)
How many grams are in moles of butane (C4H10)? Butane is used as a lighter fluid in disposal lighter.

28 How many grams are in 2. 300 moles of butane (C4H10)
How many grams are in moles of butane (C4H10)? Butane is used as a lighter fluid in disposal lighter. Asked: The mass in grams of moles of butane Given: moles of C4H10 Relationships: The formula mass is the sum of the atomic masses for each atom in the compound.

29 How many grams are in 2. 300 moles of butane (C4H10)
How many grams are in moles of butane (C4H10)? Butane is used as a lighter fluid in disposal lighter. Asked: The mass in grams of moles of butane Given: moles of C4H10 Relationships: The formula mass is the sum of the atomic masses for each atom in the compound. Solve: Answer: g are in moles of butane (C4H10).

30 Remember: How many oxygen atoms are in 200.0 g of glucose (C6H12O6)?
Asked: Number of oxygen atoms Given: g of C6H12O6 Relationships: Formula mass of glucose: Remember: Avogadro’s number indicates that one mole contains 6.02 x 1023 atoms

31 Solve: First we find how many moles are in 200.0 g of glucose:

32 Solve: First we find how many moles are in 200.0 g of glucose:
Next we find how many molecules are contained in 1.11 moles of glucose:

33 Solve: First we find how many moles are in 200.0 g of glucose:
Next we find how many molecules are contained in 1.11 moles of glucose: Then we find how many O atoms are contained in x 1023 molecules of glucose:

34 Solve: First we find how many moles are in 200.0 g of glucose:
Next we find how many molecules are contained in 1.11 moles of glucose: Then we find how many O atoms are contained in x 1023 molecules of glucose: Answer: There are x 1024 atoms of O in g of glucose (C6H12O6).

35 We can build compounds using atoms
- The type of atom matters - The arrangement of atoms also matters We can calculate the formula mass of compounds:

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