Chapter 5. Early Atomic Theory and Structure
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1 Chapter 5 Early Atomic Theory and Structure Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott Pattison, and Susan Arena Lightning occurs when electrons move to neutralize a charge difference between the clouds and the Earth
2 Chapter Outline 5.1 Early Thoughts 5.2 Dalton s Model of the Atom 5.3 Composition of Compounds 5.4 The Nature of Electric Charge 5.5 Discovery of Ions 5.6 Subatomic Parts of the Atom 5.7 The Nuclear Atom 5.8 Isotopes of the Elements 5.9 Atomic Mass
3 Early Thoughts The earliest models of the atom were developed by the ancient Greek philosophers. Empedocles (about 440 B.C.) stated that all matter was composed of four elements earth, wind, fire and water. Democritus (about B.C.) thought all forms of matter were composed of tiny indivisible particles, called atoms, derived from the Greek work for indivisible.
4 Dalton s Model of the Atom ( ) 1. Elements are composed of minute, indivisible particles called atoms. Atoms are made up of smaller particles 2. Atoms of the same element are alike in mass and size. Isotopes of elements exist 3. Atoms of different elements have different masses and sizes. Isotopes like C-14 and N-14 make this incorrect
5 Dalton s Model of the Atom (cont.) 5. Chemical compounds are formed by the union of two or more atoms of different elements. 6. Atoms combine to form compounds in simple numerical ratios. 7. Atoms of two elements may combine in different ratios to form more than one compound. H 2 O H 2 O 2
6 Composition of Compounds Law of definite composition states that a compound always contains two or more elements chemically combined in a definite proportion by mass. Water Hydrogen Peroxide H 2 O H 2 O %H 5.9% H 88.8% O 94.1% O 2H + 1O 2H + 2O
7 Law of Multiple Proportions Atoms of two or more elements may combine in different ratios to produce more than one compound.
8 Natural Law versus Theory Natural Law summary of observed behavior Laws do not undergo modification Example: Law of Definite Composition Theory (model) explanation of the behavior Theories are often modified or discarded over time Example: Dalton s Atomic Theory
9 Your Turn! Which of the following statements in Dalton s atomic theory has had to be modified or discarded in modern atomic theory? a. Atoms of the same element are alike in mass and size. b. Chemical compounds are formed by the union of two or more atoms of different elements. c. Atoms combine to form compounds in simple numerical ratios.
10 Your Turn! Which pair of formulas illustrates the law of multiple proportions? a. CH 3 Cl and CH 3 OH b. H 2 O and HOH c. CuCl 2 and CuBr d. Na 2 O and Na 2 O 2
11 The Nature of Electric Charge 1. Charge may be of two types: positive and negative. 2. Unlike charges attract and like charges repel. 3. Charge may be transferred by contact or induction. 4. Force of attraction between ions is Reduced by distance between charges (r) Increased by increasing charge (q) Coulomb's Law : F = kq q r where k is a constant.
12 Your Turn! Which of the following sets of ions have the greatest force of attraction? a. Fe 2+ and Na + b. Fe 2+ and O 2- c. Fe 3+ and O 2- Coulomb's Law : F = kq q r 1 2 2
13 Your Turn! As the distance between two oppositely charged particles increases, the force of attraction will a. Increase b. Decrease c. Remain the same Coulomb's Law : F = kq q r 1 2 2
14 Discovery of Ions Michael Faraday ( ) Discovered that compounds dissolved in water contain charged particles. These charged particles conduct electricity. Coined the term ion from the Greek word wanderer.
15 Discovery of Ions Svante Arrhenius ( ) He reasoned that an ion is an atom carrying a positive or negative charge. Both positive and negative ions are present in a compound so the molten compound conducts electricity. Cations move toward negative electrode (cathode) Anions move toward positive electrode (anode)
16 Subatomic Parts of the Atom Cathode Rays (Electrons) Discovered by J. J. Thomson in 1897 Travel in straight lines Are negatively charged Are deflected by electrical and magnetic fields
17 Electrons The electron (e - ) is a particle with a mass of g or 1/1837 mass of a hydrogen atom. a relative charge of -1. a diameter of less than cm.
18 Your Turn! Cathode rays are a. Ions b. Electrons c. Protons d. Neutrons
19 Subatomic Parts of the Atom Protons A relative charge of +1. Mass is 1837 times the mass of an electron. Thompson s Plum Pudding Model (proposed in 1904)
20 Subatomic Parts of the Atom J. J. Thompson proposed that ions result from the loss and gain of electrons
21 Subatomic Parts of the Atom Neutrons Discovered by James Chadwick in Neutral charge
22 Your Turn! A proton is a a. Cation b. Anion c. None of the above
23 Your Turn! A neutron is a a. Cation b. Anion c. None of the above
24 Your Turn! What is the relative mass of an electron? a. Slightly larger than a proton b. Slightly smaller than a proton c. 1/1837 the mass of a proton
25 Mass and Number of Atoms Calculate number of atoms in 25 g of hydrogen, if each hydrogen atom has a mass of g. 1 atom 25g = 1.5x10 atoms g
26 Your Turn! The mass of a copper atom is 1.045x10-22 g. How many copper atoms are present in a 94.5g sample of copper? a X b X c d. 94.5
27 The Nuclear Atom
28 Rutherford s Experiment Observation Most alpha rays passed through Au as if nothing was there! Some alpha rays were deflected as if repelled by a like charge particle. Some bounced back as if they encountered something very dense. Hypothesis Most of the volume of an atom is empty space The nucleus or center of the atom is positive. Most of the mass of the atom is in the nucleus.
29 Nuclear Atom Protons and neutrons make up the dense, positive nucleus. Electrons occupy the empty space outside the nucleus. A neutral atom contains the same number of electrons and protons.
30 Your Turn! The mass of an atom is primarily determined by the mass of its a. Protons b. Neutrons c. Electrons d. Protons and neutrons e. Protons, neutrons and electrons
31 Atomic Number of the Elements The atomic number of an element is the number of protons in the nucleus. The atomic number determines the identity of the element. Example: Sodium has an atomic number of 11 so every sodium atom has 11 protons. Since a neutral atom of Na has 11 protons, it also has 11 electrons.
32 Your Turn! Use a periodic table to determine the atomic number of potassium. Which of the following is true? a. Potassium has 15 protons and 15 electrons. b. Potassium has 15 protons and 31 electrons. c. Potassium has 19 protons and 19 electrons. d. Potassium has 19 protons and 39 electrons.
33 Isotopes of the Elements Isotopes are atoms of an element with the same atomic number but different masses. Isotopes have different numbers of neutron. The mass number is the sum of protons and neutrons.
34 Isotopic Notation Phosphorus-31 is the only stable P isotope. The neutral atom has 15 protons and 15 electrons. Number of neutrons = = P
35 Isotopes Complete the table: Element Symbol Atomic No. Mass No. No. of Protons No. of Electrons No. Of Neutrons 37 chlorine Cl lead Pb argon Ar
36 Your Turn! Carbon-14 dating involves measuring the amount of C-14 remaining in a fossil. How many neutrons does this radioactive isotope have? a. 14 b. 6 c. 8 d C
37 Your Turn! Approximately 50.70% of all atoms of bromine are atoms. How many neutrons, protons and electrons does this isotope of bromine have? a. 79 neutrons, 35 protons and 35 electrons b. 44 neutrons, 35 protons and 35 electrons c. 35 neutrons, 79 protons and 35 electrons d. 44 neutrons, 35 protons and 44 electrons e. 79 neutrons, 35 protons and 44 electrons 79 Br 35
38 Your Turn! What is the mass number of an atom that contains 30 protons, 30 electrons, and 35 neutrons? a. 35 b. 30 c. 65 d. 95
39 Atomic Mass The mass of an atom is so small that a table of relative atomic masses using atomic mass units was devised. The atomic mass unit (amu) is defined as 1/12 mass of a C-12 atom. 1 amu = x10-24 g Atomic mass is a weighted average of the naturally occurring isotopes of an element compared to the atomic mass of carbon-12.
40 Atomic Mass Isotope 12 C 6 13 C 6 Isotopic mass (amu) Abundance (%) Average atomic mass (amu) Atomic mass of Carbon: 98.97% 12 C ( amu) % 13 C ( amu) = amu
41 Your Turn Bromine has two stable isotopes: Br-79 (50.70%) and Br-81 (49.32%). The atomic masses are amu and amu respectively. Determine the average atomic mass of bromine. a amu b amu c amu d amu
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