Conceptual Physics Matter Atoms
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1 Conceptual Physics Matter Atoms Lana Sheridan De Anza College July 20, 2017
2 Last time projectile motion orbits escape speed heliocentric model Kepler s laws review
3 Overview matter atoms elements atomic structure charge
4 Dividing Matter What happens when you cut a loaf of bread in half and then in half again, and again, and again...?
5 Dividing Matter What happens when you cut a loaf of bread in half and then in half again, and again, and again...? Can you just keep cutting bread forever?
6 Dividing Matter What happens when you cut a loaf of bread in half and then in half again, and again, and again...? Can you just keep cutting bread forever? Or is there some smallest bit of bread, that you can t cut further?
7 Dividing Matter What happens when you cut a loaf of bread in half and then in half again, and again, and again...? Can you just keep cutting bread forever? Or is there some smallest bit of bread, that you can t cut further? Or at some point, does it stop being bread?
8 Some History People have speculated on the underlying nature of matter for far longer than there has been good evidence to decide the question. Ancient Greece: Plato (c. 427-c. 347 BCE) thought there were 4 basic kinds of corpuscles, each in a different geometric shape Aristotle (sometime before 330 BCE) decided that the 4 basic elements (earth, water, fire, air) were continuous Democritus, Leucippus, and Epicurus ( BCE) believed all matter was composed of small indivisible particles and that there was empty space, void, in between them to allow for motion Ancient Rome: Lucretius observed that everything decays, but that everything can also be reconstituted, suggesting that there are underlying building blocks of matter that are eternal.
9 Some History Ancient India: thinking about atomic concepts seems to have sprouted from reasoning about linguistics in India anor (atom) is mentioned in the Bhavagad Gita ( BCE) Nyaya-Vaisesika school developed an early idea about atoms ( BCE) and how they combine Buddhist school (prior to 400 BCE?) had a concept of 4 kinds of atoms very similar to Aristotle s idea of 4 elements Jaina school ( BCE) conceived of atoms as the basic building blocks of matter, and had some concepts of sub-atomic constituents
10 Some History Later thinkers in the Middle East were influenced by Greek and Indian ideas. In Europe philosophers were exposed to Greek and Roman ideas, with Aristotle s continuous matter idea very popular for a long time. Nevertheless, ideas about corpuscles (small particles) were important for Newton and his contemporaries. A chemist, Robert Boyle ( ) speculated that if atoms / corpuscles made up matter, that much resolve problems arising in chemistry. He proved correct.
11 Understanding from Chemical Reactions John Dalton, a physicist and chemist in 1803 started trying to understand the patterns of chemical reactions. Dissociating pure water: water oxygen + hydrogen and always hydrogen and oxygen were produced in the same proportions! This lead him to suppose that matter was composed of atoms chemical substances that could not be dissociated were elements chemical substances that could be dissociated were formed from combinations of atoms
12 Understanding from Chemical Reactions Rules of Dalton s theory 1 : Elements are made 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. 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. 1 Wikipedia, Dalton, A New System of Chemical Philosophy (1808)
13 Understanding from Chemical Reactions 1 Images from Dalton, A New System of Chemical Philosophy (1808) and Wikimedia.
14 Elements
15 Brownian Motion In 1827 Robert Brown, a botanist, observed pollen grains suspended in water through a microscope. He expected to see them suspended at rest, but did not. Instead the grains of pollen seemed to jump and wiggle about for no discernible reason.
16 Brownian Motion In 1827 Robert Brown, a botanist, observed pollen grains suspended in water through a microscope. He expected to see them suspended at rest, but did not. Instead the grains of pollen seemed to jump and wiggle about for no discernible reason. He wondered if it was something peculiar that pollen did so he tried again with dust and soot and saw the same thing! This motion is called Brownian Motion.
17 Brownian Motion Brownian motion remained a mystery until Einstein, building on tools he had just developed in his doctoral thesis, developed a theory describing Brownian motion. It is the result of fast-moving water molecules (too small to see) colliding with the pollen molecules, and jostling them.
18 About Atoms Facts about atoms: atoms are very small: m there are in just a gram of water! they move around when not at absolute zero temperature (which is always) atoms of heavier elements are formed in stars. Most atoms are very stable and therefore almost as old as the universe.
19 Electric Charge Charge is an intrinsic (essential) property of subatomic particles. Charge can be positive or negative. Particles can also be chargeless, ie. have zero net charge.
20 Electric Charge Charge is an intrinsic (essential) property of subatomic particles. Charge can be positive or negative. Particles can also be chargeless, ie. have zero net charge. Static electric charge can be experienced on a large scale through static electricity.
21 Charge on larger objects F Most large objects around us have (approximately) zero net charge. 62 CHAPTER 21 ELECTRIC CHARGE Objects can become charged when rubbed against one another. F F (a) Glass F Glass 1 Diagrams from Halliday, Resnick, Walker, 9th ed (a) Glass Glass These examples reveal that w carpets, doorknobs, faucets, and co amount of electric charge. Electr fundamental particles making up t automatically with those particles w The vast amount of charge in the object contains equal amounts Glass negative charge. With such an equa F to be electrically F Plastic neutral; that is, i charge are not in balance, then th charged to indicate (b) that it has a cha Fig always (a) much Two charged smaller rods than of the the to same sign charge repel contained each other. in (b) the Twoobject
22 Electrostatic force Charged objects exert a force (the electrostatic force) on one another. Charges with the same electrical sign repel each other. Charges with opposite electrical signs attract each other.
23 Electrostatic force Charged objects exert a force (the electrostatic force) on one another. Charges with the same electrical sign repel each other. Charges with opposite electrical signs attract each other. The unit for charge is the Coulomb, written with the symbol C.
24 realignment of charges in the molecules of the wall. Induced Charge Polarization because in the m Charged balloon Wall Induced charge separation Charged objects can a also be attracted to neutrally-charged objects b because neutral objects are composed of charged particles. 1 Fig from Serway & Jewett, Physics for Scientists and Engineers, 9th ed.
25 Fundamental Unit of Charge The smallest unit of charge is called e. e = C
26 Electrons Electrons are tiny negatively charged particles. J.J. Thompson is credited with their discovery, because he determined their charge and mass, which showed that they were not a kind of charged atom of molecule, but a new kind of particle. Symbol: e Negatively charged: charge e Very low mass: kg
27 Atomic Structure Thompson knew that electrons could be extracted from atoms. The remaining portion of the atom was positively charged. He developed a model of what the atom could look like, called the Thompson Model or the Plum Pudding Model. 1 Left: whatscookingamerica.net/cake/plumpuddingtips.htm; Right:
28 Atomic Structure Because of an experiment by Rutherford, Geiger, and Marsden, we know that Thompson s model is not correct. There are other kinds of particles in atoms also. Atoms are made up of subatomic particles: protons neutrons electrons Atoms of different elements have different numbers of protons. 1 Figure from Wikipedia.
29 Protons Symbol: p (or p + ) Positively charged: charge +e Much larger mass than an electron: kg
30 Protons Symbol: p (or p + ) Positively charged: charge +e Much larger mass than an electron: kg This is 1837 times the mass of the electron!
31 Neutrons Symbol: n (or n 0 ) The neutron has no electric charge. (It is neutral.) Very similar mass to a proton: kg. (Just slightly heavier.)
32 Atomic Structure Atoms have a compact nucleus composed of protons and neutrons. The nucleus therefore has an overall positive charge. A cloud of electrons surrounds the nucleus, attracted by the electrostatic force. 1 Figure from Wikipedia.
33 Nuclei Usually, atoms have a similar number of neutrons to the number of protons in their nuclei. 1 Figure from UC Davis ChemWiki.
34 Kinds of Atoms Atoms are neutral (net charge 0), so each atom has the same number of protons and electrons. The atomic mass is the sum of the number of protons and neutrons ( kg). Electrons can be neglected because they have so little mass.
35 Kinds of Atoms Element # Protons/Electons # Neutrons Atomic Mass Hydrogen Helium Lithium Berylium Boron Carbon Nitrogen Oxygen Fluorine Neon
36 Elements
37 How to read each element square 1 Diagram from WikiPhoto, WikiHow
38 How to read each element square Boron has a mass of 11 amu or atomic mass units. 1 amu = 1/12 of the mass of one carbon atom. 1 Diagram from WikiPhoto, WikiHow
39 Summary matter atoms atomic structure elements Homework charge worksheet (see website or course studio) Hewitt, Ch 11, onward from page 211. Ranking: 1; Exercises: 1, 9, 11, 13, 15, 17, 21, 27 Ch 22, onward from page 403. Exercises: 3.
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