Early Models of the Atom
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1 Early Models of the Atom An atom is the smallest particle of an element that retains its identity in a chemical reaction. Although early philosophers and scientists could not observe individual atoms, they were still able to propose ideas about the structure of atoms.
2 Early Models of the Atom Democritus s Atomic Philosophy The Greek philosopher Democritus (460 BC 370 BC) was among the first to suggest the existence of atoms. Democritus reasoned that atoms were indivisible and indestructible.
3 Early Models of the Atom Dalton s Atomic Theory The modern process of discovery regarding atoms began with John Dalton ( ), an English chemist and schoolteacher. By using experimental methods, Dalton transformed Democritus s ideas on atoms into a scientific theory.
4 Early Models of the Atom Dalton s Atomic Theory Dalton studied the ratios in which elements combine in chemical reactions. The result of his work is known as Dalton s atomic theory.
5 Early Models of the Atom Dalton s Atomic Theory 1. All elements are composed of tiny indivisible particles called atoms. Atoms of element A
6 Early Models of the Atom Dalton s Atomic Theory 1. Atoms of the same element are identical. The atoms of any one element are different from those of any other element. Atoms of element A Atoms of element B
7 Early Models of the Atom Dalton s Atomic Theory 1. Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds. Mixture of atoms of elements A and B
8 Early Models of the Atom Dalton s Atomic Theory 1. Chemical reactions occur when atoms are separated from each other, joined, or rearranged in different combinations. Atoms of one element are never changed into atoms of another element as a result of a chemical reaction. Compound made by chemically combining atoms of elements A and B
9 How was Jon Dalton able to study atoms even though he couldn t observe them directly? What evidence did he use to formulate his atomic theory? Dalton studied the ratios in which elements combine in chemical reactions. He observed that when atoms mix, they maintain their own identity unless they combine in a chemical reaction.
10 Sizing up the Atom This liquid mercury illustrates Dalton s concept of the atom. Every drop, no matter its size has the same properties. Even if you could make a drop the size of one atom, it would still have the chemical properties of mercury.
11 Much of Dalton s atomic theory is accepted today. One important change, however, is that atoms are now known to be divisible. They can be broken down into even smaller, more fundamental particles, called subatomic particles.
12 Electrons In 1897, the English physicist J. J. Thomson ( ) discovered the electron. Electrons are negatively charged subatomic particles.
13 Electrons Thomson found that a cathode ray is deflected by electrically charged metal plates. A positively charged plate attracts the cathode ray, while a negatively charged plate repels it.
14 Electrons Thompson knew that opposite charges attract and like charges repel, so he hypothesized that a cathode ray is a stream of tiny negatively charged particles moving at high speed. Thompson called these particles corpuscles. Later they were named electrons.
15 Electrons Thompson concluded that electrons are a component of the atoms of all elements.
16 Electrons An electron has one unit of negative charge, and its mass is 1/1840 the mass of a hydrogen atom.
17 Protons and Neutrons If cathode rays are electrons given off by atoms, what remains of the atoms that have lost the electrons? For example, after a hydrogen atom (the lightest kind of atom) loses an electron, what is left?
18 Protons and Neutrons You can think through this problem using four simple ideas about matter and electric charges. 1. Atoms have no net electric charge; they are electrically neutral. 2. Electric charges are carried by particles of matter. 3. Electric charges always exist in whole-number multiples of a single basic unit; that is, there are no fractions of charges. 4. When a given number of negatively charged particles combines with an equal number of positively charged particles, an electrically neutral particle is formed.
19 Protons and Neutrons In 1886, Eugen Goldstein ( ) observed a cathode-ray tube and found rays traveling in the direction opposite to that of the cathode rays. He concluded that they were composed of positive particles. Such positively charged subatomic particles are called protons.
20 Protons and Neutrons In 1932, the English physicist James Chadwick ( ) confirmed the existence of yet another subatomic particle: the neutron. Neutrons are subatomic particles with no charge but with a mass nearly equal to that of a proton.
21 The table below summarizes the properties of these subatomic particles. Properties of Subatomic Particles Particle Symbol Relative charge Relative mass (mass of proton = 1) Actual mass (g) Electron e 1 1/ Proton p Neutron n
22 Although protons and neutrons are extremely small, theoretical physicists believe that they are composed of yet smaller subnuclear particles called quarks.
23 When subatomic particles were discovered, scientists wondered how the particles were put together in an atom. Most scientists including J. J. Thompson thought it likely that the electrons were evenly distributed throughout an atom filled uniformly with positively charged material. In Thomson s atomic model, known as the plumpudding model, electrons were stuck into a lump of positive charge, similar to raisins stuck in dough.
24 This model of the atom turned out to be short-lived, however, due to the work of a former student of Thomson, Ernest Rutherford ( ). Born in New Zealand, Rutherford was awarded the Nobel Prize for Chemistry in His portrait appears on the New Zealand $100 bill.
25 Rutherford s Gold-Foil Experiment In 1911, Rutherford and his co-workers wanted to test the existing plum-pudding model of atomic structure. They devised the gold-foil experiment. Their test used alpha particles, which are helium atoms that have lost their two electrons and have a double positive charge because of the two remaining protons.
26 The Rutherford Atomic Model Based on his experimental results, Rutherford suggested a new theory of the atom. He proposed that the atom is mostly empty space. Thus explaining the lack of deflection of most of the alpha particles.
27 The Rutherford Atomic Model The Rutherford atomic model is known as the nuclear atom. In the nuclear atom, the protons and neutrons are located in the positively charged nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom.
28 The Rutherford Atomic Model According to this model, the nucleus is tiny and densely packed compared with the atom as a whole. If an atom were the size of a football stadium, the nucleus would be about the size of a marble.
29 Key Concepts Three kinds of subatomic particles are electrons, protons, and neutrons. In the nuclear atom, the protons and neutrons are located in the nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom.
30 Glossary Terms atom: the smallest particle of an element that retains its identity in a chemical reaction electron: a negatively charged subatomic particle proton: a positively charged subatomic particle found in the nucleus of an atom neutron: a subatomic particle with no charge and a mass of 1 amu; found in the nucleus of an atom nucleus: the tiny, dense central portion of an atom, composed of protons and neutrons
31 What makes one element different from another?
32 Atomic Number Elements are different because they contain different numbers of protons. An element s atomic number is the number of protons in the nucleus of an atom of that element. The atomic number identifies an element.
33 Atomic Number Remember that atoms are electrically neutral. Thus, the number of electrons (negatively charged particles) must equal the number of protons (positively charged particles).
34 Understanding Atomic Number The element nitrogen (N) has an atomic number of 7. How many protons and electrons are in a neutral nitrogen atom?
35 Identify the atomic number. Then use the atomic number to find the number of protons and electrons. The atomic number of nitrogen is 7. So, a neutral nitrogen atom has 7 protons and 7 electrons.
36 Mass Number The total number of protons and neutrons in an atom is called the mass number.
37 Mass Number If you know the atomic number and mass number of an atom of any element, you can determine the atom s composition. Number of neutrons = mass number atomic number
38 For each element listed in the table below, the number of protons equals the number of electrons. Atoms of the First Ten Elements Name Symbol Atomic number Protons Neutrons Mass number Electrons Hydroge Helium n H He Lithium Li Berylliu Boron m Be B Carbon C Nitrogen N Oxygen O Fluorine F Neon Ne
39 Mass Number The composition of any atom can be represented in shorthand notation using atomic number and mass number. The atomic number is the subscript. Au is the chemical symbol for gold. The mass number is the superscript.
40 Mass Number You can also refer to atoms by using the mass number and the name of the element. Au may be written as gold Au is the chemical symbol for gold.
41 Determining the Composition of an Atom How many protons, electrons, and neutrons are in each atom? a. 4Be b. 10Ne c. 11Na
42 Use the definitions of atomic number and mass number to calculate the numbers of protons, electrons, and neutrons. KNOWNS Beryllium (Be) atomic number = 4 mass number = 9 UNKNOWNS protons =? electrons =? neutrons =? Neon (Ne) atomic number = 10 mass number = 20 Sodium (Na) atomic number = 11 mass number = 23
43 Use the atomic number to find the number of protons. atomic number = number of protons a. 4 b. 10 c. 11
44 Use the atomic number to find the number of electrons. atomic number = number of electrons a. 4 b. 10 c. 11
45 Use the mass number and atomic number to find the number of neutrons. number of neutrons = mass number atomic number a.number of neutrons = 9 4 = 5 b.number of neutrons = = 10 c. number of neutrons = = 12
46 Isotopes are atoms that have the same number of protons but different numbers of neutrons. Neon-20, neon-21, and neon 22 are three isotopes of neon.
47 Why are atoms with different numbers of neutrons still considered to be the same element? Despite differences in the number of neutrons, isotopes are chemically alike. They have identical numbers of protons and electrons, which determine chemical behavior.
48 Atomic Mass How do you calculate the atomic mass of an element? It is useful to compare the relative masses of atoms using a reference isotope as a standard. The reference isotope chosen is carbon- 12.
49 A carbon-12 atom has six protons and six neutrons in its nucleus, and its mass is set at 12 amu. The six protons and six neutrons account for nearly all of this mass. Therefore, the mass of a single proton or a single neutron is about one-twelfth of 12 amu, or about 1 amu.
50 In nature, most elements occur as a mixture of two or more isotopes. Each isotope of an element has a fixed mass and a natural percent abundance.
51 Name Hydrogen Helium Carbon Oxygen Chlorine Symbol H H H He He C C O O O Cl Cl Natural Percent Abundance of Stable Isotopes of Some Elements Natural percent abundance negligible Mass (amu) Atomic mass
52 Chlorine occurs as two isotopes: chlorine- 35 and chlorine-37.
53 Because there is more chlorine-35 than chlorine- 37 in nature, the atomic mass of chlorine, amu, is closer to 35 than to 37.
54 The atomic mass of an element is a weighted average mass of the atoms in a naturally occurring sample of the element. A weighted average mass reflects both the mass and the relative abundance of the isotopes as they occur in nature.
55 Key Concepts Elements are different because they contain different numbers of protons. Because isotopes of an element have different numbers of neutrons, they also have different mass numbers.
56 Key Equation number of neutrons = mass number atomic number
57 Glossary Terms atomic number: the number of protons in the nucleus of an atom of an element mass number: the total number of protons and neutrons in the nucleus of an atom isotopes: atoms of the same element that have the same atomic number but different atomic masses due to a different number of neutrons
58 Glossary Terms atomic mass unit (amu): a unit of mass equal to one-twelfth the mass of a carbon-12 atom atomic mass: the weighted average of the masses of the isotopes of an element
59 Electrons and the Structure of Atoms Atoms of the same element have the same number of protons, which is equal to an atom s atomic number. But atoms of the same element can have different numbers of neutrons. Atoms of the same element with different numbers of neutrons are isotopes.
60 Subatomic Particles A review using a Graphic Organizer
61 Subatomic Particles ATOM
62 Subatomic Particles ATOM NUCLEUS
63 Subatomic Particles ATOM NUCLEUS PROTONS
64 Subatomic Particles ATOM NUCLEUS PROTONS POSITIVE CHARGE
65 Subatomic Particles ATOM NUCLEUS PROTONS NEUTRONS POSITIVE CHARGE
66 Subatomic Particles ATOM NUCLEUS PROTONS NEUTRONS POSITIVE CHARGE NEUTRAL CHARGE
67 Subatomic Particles ATOM NUCLEUS ELECTRONS PROTONS NEUTRONS POSITIVE CHARGE NEUTRAL CHARGE
68 Subatomic Particles ATOM NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE
69 Subatomic Particles ATOM NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE Most of the atom s mass.
70 Subatomic Particles ATOM NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE Atomic Number equals the # of...
71 Subatomic Particles ATOM NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE equal in a neutral atom
72 Subatomic Particles ATOM NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE QUARKS
73 Quarks Subatomic Particles component of protons & neutrons 6 types 3 quarks = 1 proton or 1 neutron He
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