1. Chapter 3 Atoms: The Building Blocks of Matter 3.1 The Atom:
The Atom: From Philosophical Idea to Theory
Chapter 3
Atoms:
The Building
Blocks of Matter
3.1 The Atom:
From Philosophical Idea to Theory

2. Democritus (400 BC) Coined the term “atomos”
"The only existing things are atoms and empty space; all else is opinion”
Coined the term “atomos”

3. Law of Conservation of Mass
Mass is neither created nor destroyed during chemical or physical reactions.
Total mass of reactants =
Total mass of products
Antoine Lavoisier

4. Law of Definite Proportions
A chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or the source of the sample

5. Law of Multiple Proportions
If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers
a. CO2 and CO
b. H2O and H2O2

6. Dalton’s Atomic Theory (1808)
All matter is composed of extremely small particles called atoms
Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties
John Dalton

7. Dalton’s Atomic Theory (1808)
Atoms cannot be subdivided, created, or destroyed
Atoms of different elements combine in simple whole-number ratios to form chemical compounds
In chemical reactions, atoms are combined, separated, or rearranged
John Dalton

8. Modern Atomic Theory
Several changes have been made to Dalton’s theory.
Dalton said:
Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties
Modern theory states:
Atoms of an element have a characteristic average mass which is unique to that element.

9. Chapter 3 Atoms: The Building Blocks of Matter 3.2
The Atom: From Philosophical Idea to Theory
Chapter 3
Atoms:
The Building
Blocks of Matter
3.2
The Structure of the Atom

10. Isotopes Elements occur in nature as mixtures of isotopes.
Isotopes are atoms of the same element that differ in the number of neutrons

11. Composition of the nucleus
Atomic Masses
Atomic mass is the average of all the naturally occurring isotopes of that element.
Carbon =
Isotope
Symbol
Composition of the nucleus
% in nature
Carbon-12
12C
6 protons
6 neutrons
98.89%
Carbon-13
13C
7 neutrons
1.11%
Carbon-14
14C
8 neutrons
<0.01%
1 amu (atomic mass unit) = 1/12 the mass of a carbon-12 atom; also = x kg

12. Modern Atomic Theory #2 Dalton said: Modern theory states:
Atoms cannot be subdivided, created, or destroyed
Modern theory states:
Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions!

13. Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube to deduce the presence of a negatively charged particle.
Cathode ray tubes pass electricity through a gas that is contained at a very low pressure.

14. Some Modern Cathode Ray Tubes

15. Thomson’s Atomic Model
Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model.

16. Mass of the Electron
1909 – Robert Millikan determines the mass of the electron.
Mass of the electron is
9.109 x kg
The oil drop apparatus

17. Conclusions from the Study of the Electron
Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged electrons.
Atoms are neutral, so there must be positive particles in the atom to balance the negative charge of the electrons
Electrons have so little mass that atoms must contain other particles that account for most of the mass

18. Rutherford’s Gold Foil Experiment
Alpha particles are helium nuclei
Particles were fired at a thin sheet of gold foil
Particle hits on the detecting screen (film) are recorded

19. Try it Yourself!
In the following pictures, there is a target hidden by a cloud. To figure out the shape of the target, we shot some beams into the cloud and recorded where the beams came out. Can you figure out the shape of the target?

20. The Answers
Target #2
Target #1

21. Rutherford’s Findings
Most of the particles passed right through
A few particles were deflected
VERY FEW were greatly deflected
“Like howitzer shells bouncing off of tissue paper!”
Cool Website!
Conclusions:
The nucleus is small
The nucleus is dense
The nucleus is positively charged

22. Atomic Particles Particle Charge Mass (kg) Location Electron -1
9.109 x 10-31
Electron cloud
Proton +1
1.673 x 10-27
Nucleus
Neutron
1.675 x 10-27

23. The Atomic Scale
Most of the mass of the atom is in the nucleus (protons and neutrons)
Electrons are found outside of the nucleus (the electron cloud)
Most of the volume of the atom is empty space
“q” is a particle called a “quark”

24. Chapter 3 Atoms: The Building Blocks of Matter 3.3 Counting Atoms
The Atom: From Philosophical Idea to Theory
Chapter 3
Atoms:
The Building
Blocks of Matter
3.3
Counting Atoms

25. Atomic Number
Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element.
Element
# of protons
Atomic # (Z)
Carbon 6
Phosphorus 15
Gold 79

26. Isotopes…Again (must be on the test)
Isotopes are atoms of the same element having different masses due to varying numbers of neutrons.
Isotope
Protons
Electrons
Neutrons
Nucleus
Hydrogen–1
(protium) 1
Hydrogen-2
(deuterium)
Hydrogen-3
(tritium) 2

27. Mass Number
Mass number is the number of protons and neutrons in the nucleus of an isotope.
Mass # = p+ + n0
Nuclide p+ n0 e-
Mass #
Oxygen - 10 - 33 42
- 31 15 18 8 8 18
Arsenic 75 33 75
Phosphorus 16 15 31

28. 6 protons, 6 electrons & 7 neutrons
Practice
1. How many protons, neutrons & electrons make up an atom of carbon-13?
2. Write the nuclear symbol for oxygen-16.
3. Write the hyphen notation for the element whose atoms have 7 electrons & 9 neutrons.
6 protons, 6 electrons & 7 neutrons
Nitrogen-16

29. The Mole
In chemistry, we use a new unit to quantify an amount of a substance.
This unit is called the mole; abbreviated mol.
(no, not an animal or a dermatological spot)
The same way the supermarket uses a dozen to quantify 12 objects, we use a mole to quantify
6.02 x 1023 objects.
This unit helps chemists determine the number of particles in a sample of matter without counting them.

30. The Mole 1 dozen = 12 1 gross = 144 1 ream = 500 1 mole = 6.02 x 1023
There are exactly 12 grams of carbon-12 in one mole of carbon-12.

31. I didn’t discover it. Its just named after me!
Avogadro’s Number
6.02 x 1023 is called “Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro ( ).
I didn’t discover it. Its just named after me!
Amadeo Avogadro

32. Calculations with Moles: Converting moles to grams
How many grams of lithium are in 3.50 moles of lithium?
3.50 mol Li
6.94 g Li X
= g Li
24.3
1 mol Li

33. Calculations with Moles: Converting grams to moles
How many moles of lithium are in 18.2 grams of lithium?
1 mol Li
18.2 g Li X
= mol Li
2.62
6.94 g Li

34. Calculations with Moles: Using Avogadro’s Number
How many atoms of lithium are in 3.50 moles of lithium?
3.50 mol Li
6.022 x 1023 atoms Li X
= atoms Li
2.11 x 1024
1 mol Li

35. Calculations with Moles: Using Avogadro’s Number
How many atoms of lithium are in 18.2 g of lithium?
6.022 x 1023 atoms Li
1 mol Li
18.2 g Li X X
6.94 g Li
1 mol Li
(18.2)(6.022 x 1023)/6.94
= atoms Li
1.58 x 1024

36. More Practice What is the mass is grams of 3.6 mol of carbon?
What is the mass in grams of mol of sulfur?
How many moles of copper are in 3.22 g copper?
How many moles of lithium are in 2.72 x 10-4 g lithium?
How many moles of carbon are in 2.25 x 1022 atoms of carbon?
43 g
23.5 g
mol
3.92 x 10-5 mol
mol

37. Even More Practice!
6. How many moles of oxygen, O, are in 2,000,000 atoms oxygen? 7. How many atoms of sodium are in 3.80 mol sodium? 8. What is the mass in grams of 5.0 x 109 atoms of neon? 9. How many atoms of carbon are in g carbon? 10. What mass of silver contains the same number of atoms as 10.0 g of boron?
3 x mol
2.29 x 1024 atoms
1.7 x g
1.0 x 1021 atoms
99.8 g