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name:______________________________________________________________per____ ISN III: Building Atoms and Organizing Matter Page Item Check In Value 68 -76 4 3-6 Mini-Rutherford Activity, Video Guide, LHC 4 Text 77-79 4 7-9 Isotopes & Practice Atoms 4 Atom Factory 1 9 12 Atomic Math 2 13 Atom Factory 2 20 What are Ions? & Atomic Dimensions 2 10-11 14-15 16 17-18 Atom Factory 3 sticker here Elements 2 Know & Parts of Atoms 17 2 19 Quarks sticker here 4 20 Atoms Review 4 Text 80-82 4 Text 82-87 4 Text 88-91 2 Text 92-95 2 Text 96-98 2 Text 99-105 4 Text 106--113 4 21-24 Periodic Table and Synthetic Elements 5 Parent signature night before quiz 5 TOTAL 108 1 Parent signature ___________________________________date_______________ Text Pts. Lost Updated Things 2 Know 1. SAFETY FIRST!! (lab walk, fragile things, P.A.S.S., etc) 2. You are required to have a pencil or erasable pen, ISN with cover, and calculator everyday. 3. Any missed labs or in class work should be made up in my room during lunch with Mr. Sato or tutorial with Mrs. Stout as soon as possible after an absence. 4. Sato’s email address: [email protected] 5. Sato’s web site: www1.northbrook28.net/~asato 6. Matter is made of tiny particles that are always in some motion. 7. Matter can exist in several states, the most common are solid, liquid, gas and plasma. 8. Temperature is how fast the particles are vibrating and ... 9. Thermal Energy is how many particles there are and how fast they are moving. 10. Heat is the transfer of thermal energy. 11. An element is the most basic type of matter that is still unique. 2 Atom Basics n Protons- have a positive one electrical charge (+1). Found in the nucleus Neutrons - neutral or zero charge (n or 0). Found in the nucleus Electrons- have a negative one charge(-1). Found outside of nucleus in energy clouds or energy levels. The dotted line in the figure above represents the energy level. Atomic Number- is the number of protons, and is the identifying part of the atom. All atoms of the same element have the same atomic number. Mass Number= the number of protons plus number of neutrons Isotopes: Atoms with the same amount of protons, but different numbers of neutrons. These are basically, slightly different versions of the same element. The mass number is added to the name to identify the isotope, like Carbon-14 Charge = number of protons minus number of electrons Ions: Atoms or molecules with a positive or negative charge due to more or less electrons. 3 Sizes of Particles Mini- Rutherford Activity Draw the shape that you deduce is hidden under the board. Use the marbles to “sense” the objects Newton Galileo Curie Hawking Carson Carver 4 Atom and Elements Video Guide 1.________________________ are the basic building blocks of all matter, living or non-living. 2.Each atom is made up of ____________________ that spin around the nucleus made up of _____________________ & _____________________. 3.Atoms are roughly the same ________________. 4.The _______________________ nuclear force holds the nucleus together. 5.The protons give the nucleus a ____________________________ charge. 6.The ___________________________ is very dense and contains most of the mass of the atom. 7. The protons and neutrons are made up of even smaller particles called _________________. 8._________________________ and ________________________ are considered to be that smallest particles in the universe. 9.The _____________________________ force holds the electrons in their orbits. 10. ______________________________ is the most prevalent (common) element in the universe. 11.Hydrogen has the atomic number 1 because it has ________ proton. It’s symbol is ________. 12. _____________ electrons can fit in the first shell. ____________ electrons fit in the 2nd and 3rd shell. 13.______________________ have the same atomic number but different atomic mass and mass number. 14.If atoms lose or gain an electron they are called _____________________________ WORD BANK: electrons, protons, neutrons, size, hydrogen, ions, isotopes, strong, electromagnetic, atoms, positive, quarks, one, two, eight, H, nucleus 5 PICTURE 1 The Large Hadron Collider (LHC) was built by the European Organization for Nuclear Research (CERN) with the intention of testing various predictions of high-energy physics, including the existence of new particles predicted by supersymmetry. It lies in a tunnel 27 kilometers (17 mi) in circumference, as much as 175 meters (570 ft) beneath the Franco-Swiss border near Geneva, Switzerland. It is funded by and built in collaboration with over 10,000 scientists and engineers from over 100 countries as well as hundreds of universities and laboratories. Picture 1 shows the LHC from the air, Picture 2 is one place where the particles actually collide. Pictures 3 and 4 are images of the collisions PICTURE 2 PICTURE 3 6 PICTURE 4 ISOTOPES Atoms of the same element always have the same number of protons. But, different versions of atoms of the same element can have different numbers of neutrons. The different possible versions of each element are called isotopes. For example, the most common version or isotope of hydrogen, called hydrogen-1, has no neutrons at all; there's also a hydrogen isotope called hydrogen-2 , with one neutron, and another, hydrogen-3, with two neutrons. Here are the nuclei of those isotopes. + for Proton n, for Neutron, - for electron. Notice that all have 1 proton because the atomic number is 1 for all atoms of hydrogen. hydrogen-1 + hydrogen-2 hydrogen-3 n n + n + Neutrons Here are some Frequently Asked Questions (and answers) Question 1: How many isotopes can one element have? The number of isotopes varies from atom to atom. The average number of stable isotopes is 3.2 per element. But some have only 1 and others up to 10. Question 2: Can an atom have just any number of neutrons? No, there are only a few combinations of neutrons and protons when the forces holding nuclei together seem to balance best. Light elements tend to have about as many neutrons as protons; heavy elements apparently need more neutrons than protons in order to stick together. Atoms with a few too many neutrons, or not quite enough, can sometimes exist for a while, but they're unstable Question 3: I'm not sure what you mean by "unstable." Do atoms just fall apart if they don't have the right number of neutrons? Well, yes, in a way. Unstable atoms are radioactive : their nuclei change or decay by spitting out radiation , in the form of particles or electromagnetic waves. 7 ISOTOPES The table below lists all of the stable isotopes of hydrogen, carbon, and nitrogen. Refer to the table to answer the questions that follow. Atomic Mass Isotope Name % in Nature Atomic Number Mass Number units are atomic mass units (amu)** Hydrogen-1 99.9985 1.00783 1 1 Hydrogen-2 0.0015 2.00141 1 2 ✣ Hydrogen-3 trace* unknown 1 3 Carbon-12 98.8900 12.00000 6 12 Carbon-13 1.1100 13.00300 6 13 ✣ Carbon-14 trace* unknown 6 14 Nitrogen-14 14.00307 7 14 99.6360 Nitrogen-15 0.0036 15.00011 7 15 *trace means a very small quantity, too small to be accurately measured **amu is for atomic mass unit, a unit of mass used for atomic and molecular weights. ✣ radioactive 1. What does the term isotope mean? 2. How many stable isotopes does hydrogen have? Circle answer: ONE TWO THREE 3. How many stable isotopes does nitrogen have? Circle answer: ONE TWO THREE 4. Which isotopes of each of the three elements are the most common in nature? 5. Which isotopes have scientists not been able to determine the atomic mass of and why do you think this is? 6. According to the table, how are isotopes named? 7. What is the atomic number for all the isotopes of hydrogen?_________ 8. What is the atomic number for all the isotopes of carbon? __________ 9. What is the atomic number for all the isotopes of nitrogen? __________ 10.One of these isotopes has been used by scientists as a standard for the atomic mass unit (amu) Guess which one and explain your reasoning. 8 Practice Atoms • Electron orbitals • Number of Protons 3+ 3n • Number of Neutrons • Nucleus • Electrons A) Hydrogen-2 C) H-3 + n + n B) Hydrogen-1 D) Lithium-5 + n + n 9 Atom Factory Instructions READ ME Work by yourself to complete the Atom Factory #1 Lab on the computers. Don’t ask questions until you’ve tried REAL hard... hint the number of protons = electrons, for now 1. Log in as student (if needed) 2. Connect to your server 3. Click on Atom Factory 1 on the links page. 4. Open the downloaded file 5. SAVE the file to Your Server folder or Jump Drive 6. Put your name in the header at the top 7. Read all instructions on the computer copy. 8. Complete both pages on the Computer 9. Save and print to 226-Science 10.Cut out and put over this page and on the next page. YES COVER THIS PAGE WITH PAGE 1 11.Check your work with Mr. Sato after putting the printout into the ISN. 10 page 2 of Atom Factory 1 here 11 Atomic Math Calculate the answers , EACH ANSWER LEADS TO THE NEXT. e number of electrons is the same as the number of protons. 1. Multiply the atomic number of hydrogen by the number of electrons in mercury answer:___________ 2. Divide this number by the number of neutrons in helium-4. answer:___________ 3. Add the number of protons in potassium to the answer to #2 answer:___________ 4. Add the mass number of the most common isotope of carbon. (see Isotopes on ISN 8) answer:___________ 5. Subtract the number of neutrons in sulfur-32. answer:___________ 6. Divide by the number of electrons in boron-11. answer:___________ 7. is number is the atomic number of which of these elements ? fluorine: atomic number 9 neon: atomic number 10 sodium: atomic number 11 final answer:_______________ 12 Atom Factory 2 Attach Here 13 What are ions? ion (pronounced: “EYE-on”) An atom (or group of atoms)that has either lost or gained one or more electrons, so that it has an electrical charge. Ions are either positively or negatively charged. A neutral atom( or group of atoms) becomes an ion by gaining or losing one or more electrons. Since the electron and proton have equal but opposite charges(negative 1 and positive 1), the charge of an ion is always expressed as a whole number of charge and is either positive or negative. If an atom or group of atoms loses electrons it will have a net positive charge and is called a cation(cat-eye-on). If an atom or group gains electrons or loses protons, it will have a net negative charge and is called an anion(an-eye-on). Let’s take a Lithium (Li) atom. It has an atomic number of 3. That means it has 3 protons. Each proton in positively charged. For Lithium to have zero net or overall charge it must have a balanced number of negatively charged electrons, thus it needs 3 electrons to be electrically neutral, demonstrated here. 14 Atomic Dimensions The table below contains information about several elements. Use this table to review the concepts of atomic number, mass number, subatomic particles, isotopes, ions, neutrality and atoms. In each case, use the information has provided for you and a periodic table to fill in all the blanks. # 1 Aluminum 2 Bromine 35 3 Uranium 92 4 Helium 2 4 5 Helium 2 5 2 6 Lithium 3 7 2 7 Tungsten 8 Xenon 9 Magnesium 12 10 Carbon 6 11 Carbon 12 Nitrogen 7 14 0 13 Potassium 19 40 -2 14 Gold 197 -3 15 Sodium 22 0 Symbol Atomic Number Mass Number Number Number of Number of of neutrons Electrons Protons Element Name 27 13 80 Charge 13 45 36 146 92 -1 184 110 74 79 54 24 0 or neutral +2 14 6 6 0 8 +3 The “Full name” of question #2 is -1 bromine-80 16. What is the “full name” of number #4? ___________________________ 15 Atom Factory 3 Attach here 16 ELEMENTS 2 KNOW Use the Elements Names & Symbols on Quia to study and know the names and symbols for this list. Mn manganese Fe iron H hydrogen He helium Li lithium Co cobalt Be beryllium Ni nickel B boron Cu copper C carbon Zn zinc N nitrogen Pb lead O oxygen Bi bismuth F fluorine Br bromine Ne neon 17 Sr strontium Na sodium Ag silver Mg magnesium Sn tin Al aluminum I iodine Si silicon P phosphorus S sulfur Cl chlorine Ar argon K potassium Ca calcium Cr chromium Ba barium W tungsten Pt platinum Au gold Hg mercury U uranium What are the parts of an atom? Complete the following. Use Text pages and ISN 3 for help. 1. The first scientist to suggest that atoms contain smaller particles was_____________. 2. Positively charged particles are called____________________. 3. Bohr proposed that electrons in an atom are found in _________________________. 4. Negatively charged particles are called_______________ 5. Rutherford found that an atom is made up mostly of_____________________ 6. The center, or core, of an atom is called the ______________________ 7. Surrounding the core of an atom is a cloud of very small particles called ______________ 8. Today, orbitals and energy levels are used to predict the location of ___________________. 9. Neutral particles are called ____________________ 10. Rutherford found that___________________are located in the core of an atom. Write "Yes" or "No" in the correct columns to identify whether each statement is true for protons, neutrons, and electrons. Proton 1. Found in the nucleus 2. Positively charged 3. Moves in orbitals around nucleus. 4. Negatively charged 5. Does not have an electric charge 18 Neutron Electron QUARKS & Other Weird Particles As you have read, many scientists have contributed to our knowledge of atoms and particles even smaller than atoms. From the early ideas of Democritus to the modern Cloud model of atoms, we have made quite a journey! This has been the journey to answer a “simple” question...What is the fundamental particle? In other words, what is the most basic particle of matter? The smallest thing? The thing that can’t be broken down any further? We have discovered protons, neutrons and electrons. Great, but scientists weren’t finished yet! In the 1930s, 40s, and 50s nuclear physicists studied the forces that held atoms together. The field of Particle Physics developed as an outgrowth of this investigation. These scientists were interested in the make-up of nuclear particles, like protons & neutrons. However, to study these particles, great energy had to be generated. Giant accelerators were built, like the one at Fermi Lab in Batavia, Illinois, just 50 miles southwest from Northbrook and the Large Hadron Collider in France/Switzerland. Particles were accelerated at tremendous speed and then shot at a target or directed into the path of another particle traveling in the opposite direction. As a result of these collisions, hundreds, yes hundreds, of new particles were discovered that were smaller than protons & neutrons. Therefore, protons and neutrons are not the fundamental particles either. Quarks are particles that make up protons and neutrons. Here are some of the weird names of other particles: hadrons, leptons, quarks, neutrinos, muons(moo-ons), positrons, photons, gluons(glue-ons), and Higgs bosons. Currently we know of 36 types of quarks and 12 types of leptons(including electrons). These particles, quarks & leptons are all about the same size and so far we have not been able to break these particles apart. Particle physicists are striving to find a link between the particles and the four forces. This is called the Unification Theory, even Einstein couldn’t figure this one out! The four forces are gravity, electromagnetic, weak, and strong. Gravity is the attraction of all matter to all other matter. The electromagnetic force is the attraction or repulsion of charged(positive or negative) matter. The weak force is responsible for radioactive decay of a nucleus. The strong force is the force that hold quarks and the nucleus of atoms together. The answer to this seemingly simple question is closer than ever before, but also much more complex. Scientists are hard at work all over the world trying to find the final answer! Maybe you will help to lead the world to the final answer... Question for Quia: Will we ever find out what is the fundamental particle? In other words, what is the most basic particle of matter? Explain your answer on Quia in a few sentences. Click on Quiz: QUARK QUESTION to answer in QUIA. 19 Review Write the letter of the correct answer on the line at the left. 1. The positively charged particle in an atom’s nucleus is the A electron B neutron C proton D isotope 2. An element’s identity can only be determined from its A atomic number B number of neutrons C number of isotopes D energy levels 3. The smallest particle an element can be divided into and still be the element is the ... A electron B neutron C isotope D atom 4. The model of the atom that described electrons scattered throughout a ball of positive charge was proposed by A Niels Bohr B Ernest Rutherford C J. J. Thomson D John Dalton If the statement is true, write T. If the statement is false, change the underlined word or words to make the statement true. 5. ______________An element’s mass number tells the number of protons in its nucleus. 6.____________Negatively charged particles in an atom are called electrons. 7.__________The cloud model of the atom describes the location of electrons as specific orbits around the nucleus. 8._________Atoms with the same number of protons but different numbers of neutrons are called isomers. 9.__________The sum of the protons and neutrons in an atom is called the atomic number. 10._________An object that helps explain ideas about the natural world is called a model. 11.How many different isotopes can an element have? Give the Element Symbol: Give the Element Name: 12.Hydrogen ___________ 15. W _____________________ 13.Oxygen ___________ 16. Au _____________________ 14.Lead ___________ 17. Mg _____________________ 20 Periodic Table Assignment 1. Use Periodic Table and Textbook to Color in the following table. 2. Write in all the symbols. Put a star in the boxes of the Metalloids 3. Color the following lightly so you can still see the symbol and #. 4. If you need to substitute colors, make a note on this list. 5. Find information for each family with information from Text or Internet. Halogen family- Blue Carbon family- Yellow Hydrogen alone- Light blue Alkaline Earth Metals- Red Alkali Metals- Orange Transition Metals- White Inert (Noble) Gases- Purple Lanthanide Series- Light Green Actinide Series- Green Oxygen Group Brown Nitrogen Group Grey Boron group Red-orange 21 22 Synthetic Elements As of today, there are 117 known elements. Opinions differ, but about 93 occur naturally on earth (including technetium and plutonium), and 94 (including promethium) have been detected so far in the universe. The other elements not found on earth are made artificially; the first claim of a synthesized element was technetium, in 1937. Later, trace amounts of naturally occurring technetium were found. Scientists have been hard at work attempting to produce new elements since that time. The first transuranium element (element with atomic number greater than 92) discovered was neptunium in 1940. The heaviest element that has been found to date is element 118, ununoctium, which was successfully synthesized on October 9, 2006, in Russia. Element 117, ununseptium, has not yet been created or discovered, although its place in the periodic table is pre-established, and likewise for possible elements beyond 118. In order to study and better understand the characteristics and properties of the elements, scientists have organized them on a special chart known as the periodic table. Uranium is element 92 on this table. Most of the synthetic elements have numbers greater than 92 and are thus called the transuranic elements. All synthetic elements exist for very short periods of time, are incredibly expensive to produce, and are radioactive. To produce a new element, a scientist places atoms of a naturally occurring element in a device called a particle accelerator. (like the one at Fermi labs in Illinois and the LHC at CERN) These atoms are bombarded by other atoms or parts of other atoms moving at incredibly high speeds. The collision that occurs forces the atoms to fuse together, forming atoms of a new element. Collisions are not guaranteed, however, and billions of bombardments are usually required before the desired collision occurs. Synthetic elements are usually named by the scientist or team of scientists that produces them. Some of these elements have been named for famous scientists. Some examples include element 99, einsteinium (after Albert Einstein), element 100, fermium (after Enrico Fermi), and element 102, nobelium (after Alfred Nobel). Other synthetic elements are named for places, such as element 95, americium (America) and element 98, californium (California). Sometimes it takes years before the name of a new element is agreed upon. 23 Synthetic Elements Continued This is especially true if more than one scientist or team of scientists claims to have produced the same element. No final agreement has yet been reached on names for elements 117 through 118. Until some decision is made, these elements are identified by the Latin terms for their numbers in the table. For example, element 110 was designated ununnilium before it was named. Scientists believe it is only a matter of time before more elements are produced. These yet unseen elements will be products of the bombarding and fusing of elements with higher numbers on the periodic table. ANSWER THE FOLLOWING IN COMPLETE SENTENCES 1. What do all synthetic elements have in common? 2. What are transuranic elements? 3. Why might scientists be interested in producing new elements? 4. Why are synthetic elements so difficult to study? 24 Things to know about the Periodic Table of Elements 1. periodic refers to the repeating properties of the elements. 2. elements are put in order by their atomic number 3. atomic number = the number of protons. 4. vertical column is a group or family (similar properties) 5. horizontal row is a period (completes electron shell/cloud) 6. metals on left , non-metals on the right (staircase divides) 7. group 1 =alkali metals 8. group 2 = alkaline earth metals 9. group 17 = halogens 10. group 18 = inert gases (noble gases) 11. other groups are known by the head of the family (such as the oxygen family) 12. transition elements - metals, middle groups (3-12) 13. __117__ known elements, 94 naturally occur in the universe 14. Dmitri Mendeleev organized the first useful periodic table. 15. How new elements are produced/discovered 16. Characteristics of metals, nonmetals, and metalloids 25 this page is blank 26 My Element name:____________________________Element #____________ Web Element Project • Home Page Requirements “Welcome to the Page” statement YOUR FIRST NAME, Last initial Your Science period Element name • Three Pictures or Images (one can be the background) Picture/image 1 Picture/image 2 Picture/image 3 • Info Page Element Name Symbol Family or Group Metal/nonmetal/metalloid Who discovered it? (if unknown then specify as such) Year discovered (if unknown then specify as such) Where discovered (if unknown then specify as such) Origin of name (if unknown then specify as such) Uses(if none then specify as such) Price per gram you might have to convert units(find a unit converter on internet, if unknown then specify as such) • Physical Properties(also in Info Page) State at room temperature (20˚C) Atomic Number Atomic Weight Melting Point in K, ˚C and ˚F (if unknown then specify as such) Boiling Point in K, ˚C and ˚F (if unknown then specify as such) Color (if unknown then specify as such) Chemical Properties (if unknown then specify as such) • Sources Page in MLA style (use your NoodleTools™ for this) Source 1 Source 2 Source 3 Diagram of atom(like atom factory, but you can find one not make it) • Effort/Creativity/Design 4 points Add 4 3 2 1 27