1. CHEMISTRY Matter and Change
Chapter 4: The Structure of the Atom

2. Table Of Contents Section 4.1 Early Ideas About Matter
CHAPTER4
Table Of Contents
Section 4.1 Early Ideas About Matter
Section 4.2 Defining the Atom
Section 4.3 How Atoms Differ
Section 4.4 Unstable Nuclei and Radioactive Decay
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3. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Compare and contrast the atomic models of Democritus, Aristotle, and Dalton.
Understand how Dalton's theory explains the conservation of mass.
theory: an explanation supported by many experiments; is still subject to new experimental data, can be modified, and is considered successful if it can be used to make predictions that are true

4. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Dalton's atomic theory
The ancient Greeks tried to explain matter, but the scientific study of the atom began with John Dalton in the early 1800's.

5. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Greek Philosophers
Many ancient scholars believed matter was composed of such things as earth, water, air, and fire.
Many believed matter could be endlessly divided into smaller and smaller pieces.

6. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Greek Philosophers (cont.)
Democritus (460–370 B.C.) was the first person to propose the idea that matter was not infinitely divisible, but made up of individual particles called atomos, from which the English word atom is derived.
Aristotle (484–322 B.C.) disagreed with Democritus because he did not believe empty space could exist.
Aristotle’s views went unchallenged for 2,000 years until science developed methods to test the validity of his ideas.

7. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Greek Philosophers (cont.)

8. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Greek Philosophers (cont.)
John Dalton revived the idea of the atom in the early 1800s based on numerous chemical reactions.
Dalton’s atomic theory easily explained conservation of mass in a reaction as the result of the combination, separation, or rearrangement of atoms.

9. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Greek Philosophers (cont.)

10. Defining the Atom Define atom.
SECTION4.2
Defining the Atom
Define atom.
Distinguish between the subatomic particles in terms of relative charge and mass.
Describe the structure of the atom, including the locations of the subatomic particles.
model: a visual, verbal, and/or mathematical explanation of data collected from many experiments

11. Defining the Atom atom cathode ray electron nucleus proton neutron
SECTION4.2
Defining the Atom
atom
cathode ray
electron
nucleus
proton
neutron
An atom is made of a nucleus containing protons and neutrons; electrons move around the nucleus.

12. Defining the Atom The Atom *is called an atom.
SECTION4.2
Defining the Atom
The Atom
*is called an atom.
An instrument called the scanning tunneling microscope (STM) allows individual atoms to be seen.

13. Defining the Atom The Electron
SECTION4.2
Defining the Atom
The Electron
When an electric charge is applied, a ray of radiation travels from the cathode to the anode, called a cathode ray.
Cathode rays are a *.
The particles carrying a negative charge are known as *.

14. Defining the Atom The Electron (Cont.)
SECTION4.2
Defining the Atom
The Electron (Cont.)
This figure shows a typical cathode ray tube.

15. Defining the Atom The Electron (Cont.)
SECTION4.2
Defining the Atom
The Electron (Cont.)
J.J. Thomson measured the effects of both magnetic and electric fields on the cathode ray to determine the charge-to-mass ratio of a charged particle, then compared it to known values.
The mass of the charged particle was much less than a hydrogen atom, then the lightest known atom.
Thomson received the Nobel Prize in 1906 for identifying the first subatomic particle—the electron

16. Defining the Atom The Electron (Cont.)
SECTION4.2
Defining the Atom
The Electron (Cont.)
In the early 1910s, Robert Millikan used the oil-drop apparatus shown below to determine the charge of an electron.

17. the mass of a hydrogen atom
SECTION4.2
Defining the Atom
The Electron (Cont.)
Charges change in discrete amounts—1.602  10–19 coulombs, the charge of one electron (now equated to a single unit, 1–).
With the electron’s charge and charge-to-mass ratio known, Millikan calculated the mass of a single electron.
the mass of a hydrogen atom

18. Defining the Atom The Electron (Cont.)
SECTION4.2
Defining the Atom
The Electron (Cont.)
Matter is neutral. You know that matter is neutral from everyday experiences. You do not receive an electric shock (except under certain conditions) when you touch an object.
If electrons are negative, then how is matter, which is made up of electrons, neutral?
J.J. Thomson proposed a model of the atom to answer this question.

19. Defining the Atom The Electron (Cont.)
SECTION4.2
Defining the Atom
The Electron (Cont.)
J.J. Thomson's plum pudding model of the atom states that the atom is a uniform, positively charged sphere containing electrons.

20. Defining the Atom The Nucleus
SECTION4.2
Defining the Atom
The Nucleus
In 1911, Ernest Rutherford studied how positively charged alpha particles interacted with solid matter.
By aiming the particles at a thin sheet of gold foil, Rutherford expected the paths of the alpha particles to be only slightly altered by a collision with an electron.

21. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
Although most of the alpha particles went through the gold foil, a few of them bounced back, some at large angles.

22. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
Rutherford concluded that atoms are mostly empty space.
*in a dense region in the center of the atom called the nucleus.
Electrons are held within the atom by their attraction to the positively charged nucleus.

23. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
The repulsive force between the positively charged nucleus and positive alpha particles caused the deflections.

24. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
Rutherford refined the model to include positively charged particles in the nucleus called *.
James Chadwick received the Nobel Prize in 1935 for discovering the existence of neutrons, *.

25. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
All atoms are made of three fundamental subatomic particles: the electron, the proton, and the neutron.
Atoms are spherically shaped.
Atoms are mostly empty space, and electrons travel around the nucleus held by an attraction to the positively charged nucleus.

26. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
Scientists have determined that protons and neutrons are composed of subatomic particles called quarks.

27. Defining the Atom The Nucleus (cont.)
SECTION4.2
Defining the Atom
The Nucleus (cont.)
Scientists do not yet understand if or how quarks affect chemical behavior.
Chemical behavior can be explained by considering only an atom's electrons.

28. SECTION4.3
How Atoms Differ
Explain the role of atomic number in determining the identity of an atom.
Define an isotope.
Explain why atomic masses are not whole numbers.
Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number.

29. SECTION4.3
How Atoms Differ
periodic table: a chart that organizes all known elements into a grid of horizontal rows (periods) and vertical columns (groups or families) arranged by increasing atomic number
atomic number
isotopes
mass number
atomic mass unit (amu)
atomic mass
The number of protons and the mass number define the type of atom.

30. How Atoms Differ Atomic Number
SECTION4.3
How Atoms Differ
Atomic Number
Each element contains a unique positive charge in their nucleus.
*is known as the element’s atomic number.

31. Isotopes and Mass Number
SECTION4.3
How Atoms Differ
Isotopes and Mass Number
All atoms of a particular element have the same number of protons and electrons but the number of neutrons in the nucleus can differ.
*isotopes.

32. Isotopes and Mass Number (Cont.)
SECTION4.3
How Atoms Differ
Isotopes and Mass Number (Cont.)
In nature, most elements are found as mixtures of isotopes. Usually, the relative abundance of each isotope is constant.
Ex. In a banana, 93.26% is potassium-39, 6.73% is potassium-41 and 0.01% is potassium-40. In another banana or in a different source of potassium, the percentage composition of the potassium isotopes will still be the same.
Isotopes containing more neutrons have a greater mass.
Isotopes of an atom have the same chemical behavior.

33. Isotopes and Mass Number (Cont.)
SECTION4.3
How Atoms Differ
Isotopes and Mass Number (Cont.)
The mass number is *.

34. How Atoms Differ Mass of Atoms
SECTION4.3
How Atoms Differ
Mass of Atoms
One atomic mass unit (amu) is defined as 1/12th the mass of a carbon-12 atom.
One amu is nearly, but not exactly, equal to one proton and one neutron.

35. How Atoms Differ Mass of Atoms (cont.) The atomic mass of an element *
SECTION4.3
How Atoms Differ
Mass of Atoms (cont.)
The atomic mass of an element *

36. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Explain the relationship between unstable nuclei and radioactive decay.
Characterize alpha, beta, and gamma radiation in terms of mass and charge.
element: a pure substance that cannot be broken down into simpler substances by physical or chemical means

37. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
radioactivity
radiation
nuclear reaction
radioactive decay
alpha radiation
alpha particle
nuclear equation
beta radiation
beta particle
gamma rays
Unstable atoms emit radiation to gain stability.

38. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactivity
Nuclear reactions can change one element into another element.
In the late 1890s, scientists noticed some substances spontaneously emitted radiation, a process they called *
*are called radiation.
*is called a nuclear reaction.

39. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay
Unstable nuclei lose energy by emitting radiation in a spontaneous process called *
Unstable radioactive elements undergo radioactive decay thus forming stable nonradioactive elements.

40. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)
Alpha radiation is made up of positively charged particles called alpha particles.
Each alpha particle contains two protons and two neutrons and has a 2+ charge.

41. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)
The figure shown below is a nuclear equation showing the radioactive decay of radium-226 to radon-222.
An alpha particle is equivalent to a helium-4 nucleus and is represented by 4He or
Thus, showing mass is conserved in a nuclear equation. 2

42. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)
Beta radiation is *.
Each beta particle is an electron with a 1– charge.
During Beta decay, a neutron is converted to a proton and an electron. The electron is emitted and the proton stays in the nucleus.

43. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)

44. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)
Gamma rays are *.
They usually accompany alpha and beta radiation.
Gamma rays account for most of the energy lost during radioactive decay.

45. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)
Because gamma rays are massless, the emission of gamma rays by themselves cannot result in the formation of a new atom.

46. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Radioactive Decay (cont.)
Atoms that contain too many or two few neutrons are unstable and lose energy through radioactive decay to form a stable nucleus.
Few exist in nature—most have already decayed to stable forms.

47. Early Ideas About Matter
SECTION4.1
Early Ideas About Matter
Study Guide
Key Concepts
Democritus was the first person to propose the existence of atoms.
According to Democritus, atoms are solid, homogeneous, and indivisible.
Aristotle did not believe in the existence of atoms.
John Dalton’s atomic theory is based on numerous scientific experiments.

48. Defining the Atom Key Concepts
SECTION4.2
Defining the Atom
Study Guide
Key Concepts
An atom is the smallest particle of an element that maintains the properties of that element.
Electrons have a 1– charge, protons have a 1+ charge, and neutrons have no charge.
An atom consists mostly of empty space surrounding the nucleus.

49. How Atoms Differ Key Concepts
SECTION4.3
How Atoms Differ
Study Guide
Key Concepts
The atomic number of an atom is given by its number of protons. The mass number of an atom is the sum of its neutrons and protons.
atomic number = number of protons = number of electrons
mass number = atomic number + number of neutrons
Atoms of the same element with different numbers of neutrons are called isotopes.
The atomic mass of an element is a weighted average of the masses of all of its naturally occurring isotopes.

50. Unstable Nuclei and Radioactive Decay
SECTION4.4
Unstable Nuclei and Radioactive Decay
Study Guide
Key Concepts
Chemical reactions involve changes in the electrons surrounding the nucleus of an atom. Nuclear reactions involve changes in the nucleus of an atom.
There are three types of radiation: alpha (charge of 2+), beta (charge of 1–), and gamma (no charge).
The neutron-to-proton ratio of an atom’s nucleus determines its stability.