CHEMISTRY Matter and Change. Chapter 4: The Structure of the Atom
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1 CHEMISTRY Matter and Change Chapter 4: The Structure of the Atom
2 CHAPTER 4 Table Of Contents Section 4.1 Section 4.2 Section 4.3 Section 4.4 Early Ideas About Matter Defining the Atom How Atoms Differ Unstable Nuclei and Radioactive Decay Click a hyperlink to view the corresponding slides. Exit
3 4.1 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 4.1 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 4.1 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 4.1 Early Ideas About Matter Greek Philosophers (cont.) Democritus ( 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 ( 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 4.1 Early Ideas About Matter Greek Philosophers (cont.)
8 4.1 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 4.1 Early Ideas About Matter Greek Philosophers (cont.)
10 4.1 Section Check Who was the first person to propose the idea that matter was not infinitely divisible? A. Aristotle B. Plato C. Dalton D. Democritus
11 4.1 Section Check Dalton s theory also conveniently explained what? A. the electron B. the nucleus C. law of conservation of mass D. law of Democritus
12
13 4.2 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
14 4.2 Defining the Atom The Atom The smallest particle of an element that retains the properties of the element is called an atom. An instrument called the scanning tunneling microscope (STM) allows individual atoms to be seen.
15 4.2 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.
16 4.2 Defining the Atom The Nucleus (cont.) Scientists have determined that protons and neutrons are composed of subatomic particles called quarks.
17 4.2 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.
18 4.2 Section Check Atoms are mostly. A. positive B. negative C. solid spheres D. empty space
19 4.2 Section Check What are the two fundamental subatomic particles found in the nucleus? A. proton and electron B. proton and neutron C. neutron and electron D. neutron and positron
20
21 4.3 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.
22 4.3 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.
23 4.3 How Atoms Differ Atomic Number Each element contains a unique positive charge in their nucleus. The number of protons in the nucleus of an atom identifies the element and is known as the element s atomic number.
24 4.3 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. Atoms with the same number of protons but different numbers of neutrons are called isotopes.
25 4.3 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.
26 4.3 How Atoms Differ Isotopes and Mass Number (Cont.) The mass number is the sum of the protons and neutrons in the nucleus.
27 4.3 How Atoms Differ Mass of Atoms One atomic mass unit (amu) is defined as 1/12 th the mass of a carbon-12 atom. One amu is nearly, but not exactly, equal to one proton and one neutron.
28 4.3 How Atoms Differ Mass of Atoms (cont.) The atomic mass of an element is the weighted average mass of the isotopes of that element.
29 4.3 Section Check An unknown element has 19 protons, 19 electrons, and 3 isotopes with 20, 21 and 22 neutrons. What is the element s atomic number? A. 38 B. 40 C. 19 D. unable to determine
30 4.3 Section Check Elements with the same number of protons and differing numbers of neutrons are known as what? A. isotopes B. radioactive C. abundant D. ions
31
32 4.4 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
33 4.4 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.
34 4.4 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 radioactivity. The rays and particles emitted are called radiation. A reaction that involves a change in an atom's nucleus is called a nuclear reaction.
35 4.4 Unstable Nuclei and Radioactive Decay Radioactive Decay Unstable nuclei lose energy by emitting radiation in a spontaneous process called radioactive decay. Unstable radioactive elements undergo radioactive decay thus forming stable nonradioactive elements.
36 4.4 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.
37 4.4 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 4 He or. Thus, showing mass is conserved in a nuclear equation. 2
38 4.4 Unstable Nuclei and Radioactive Decay Radioactive Decay (cont.) Beta radiation is radiation that has a negative charge and emits beta particles. 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.
39 4.4 Unstable Nuclei and Radioactive Decay Radioactive Decay (cont.)
40 4.4 Unstable Nuclei and Radioactive Decay Radioactive Decay (cont.) Gamma rays are high-energy radiation with no mass and are neutral. They usually accompany alpha and beta radiation. Gamma rays account for most of the energy lost during radioactive decay.
41 4.4 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.
42 4.4 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.
43 4.4 Section Check A reaction that changes one element into another in the nucleus of an atom is called what? A. chemical reaction B. beta radiation C. nuclear reaction D. physical reaction
44 4.4 Section Check Why are radioactive elements rare in nature? A. They do no occur on Earth. B. Most have already decayed to a stable form. C. They take a long time to form. D. They are too hard to detect.
45
46 CHAPTER 4 The Structure of the Atom Resources Chemistry Online Study Guide Chapter Assessment Standardized Test Practice
47 4.1 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 4.2 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 4.3 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 4.4 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.
51 CHAPTER 4 The Structure of the Atom Chapter Assessment Whose work led to the modern atomic theory? A. Dalton B. Rutherford C. Einstein D. Aristotle
52 CHAPTER 4 The Structure of the Atom Chapter Assessment Which particle is not found in the nucleus of an atom? A. neutron B. proton C. gamma ray D. electron
53 CHAPTER 4 The Structure of the Atom Chapter Assessment Two isotopes of an unknown element have the same number of: A. protons B. neutrons C. electrons D. both A and C
54 CHAPTER 4 The Structure of the Atom Chapter Assessment Lithium has an atomic mass of and two isotopes, one with 6 neutrons and one with 7 neutrons. Which isotope is more abundant? A. 6 Li B. 7 Li C. Both isotopes occur equally. D. unable to determine
55 CHAPTER 4 The Structure of the Atom Chapter Assessment What happens when an element emits radioactive particles? A. It gains energy. B. It gains neutrons. C. It loses stability. D. It loses energy.
56 CHAPTER 4 The Structure of the Atom Standardized Test Practice What is the smallest particle of an element that still retains the properties of that element? A. proton B. atom C. electron D. neutron
57 CHAPTER 4 The Structure of the Atom Standardized Test Practice How many neutrons, protons, and electrons does Xe have? A. 124 neutrons, 54 protons, 54 electrons B. 70 neutrons, 54 protons, 54 electrons C. 124 neutrons, 70 protons, 54 electrons D. 70 neutrons, 70 protons, 54 electrons
58 CHAPTER 4 The Structure of the Atom Standardized Test Practice The primary factor in determining an atom's stability is its ratio of neutrons to. A. protons B. electrons C. alpha particles D. isotopes
59 CHAPTER 4 The Structure of the Atom Standardized Test Practice What is the densest region of an atom? A. electron cloud B. nucleus C. isotopes D. atomic mass
60 CHAPTER 4 The Structure of the Atom Standardized Test Practice Why are electrons attracted to the cathode in a cathode ray tube? A. The cathode is more stable. B. The cathode has a positive charge. C. The cathode has a negative charge. D. The cathode has no charge.
61 This slide is intentionally blank.
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