DOCSLIB.ORG

The Periodic Table of the Elements

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
The Periodic Table of the Elements The Periodic Table of the Elements All matter is composed of elements. All of the elements are composed of atoms. An atom is the smallest part of an element which still retains the properties of that element. All of the elements are listed on the Periodic Table by their Chemical Symbol • The chemical symbol for every element is either one capital letter or one capital letter plus a small letter For example: C = carbon Ca = calcium Cl = chlorine Cr = chromium Chemical Symbols Chemical Symbols • represent name of element • consist of one to two letters and start with capital 1-Letter Symbols 2-Letter Symbols C carbon Co cobalt N nitrogen Ca calcium F fluorine Al aluminum O oxygen Mg magnesium 3 Refer to Table 4.2 on Page 97 for list of the more common elements and their symbols. All of the elements on the Periodic Table are arranged in vertical columns called “Groups”, and in horizontal rows called “Periods”. All of the groups have numbers and they are either “A” groups or “B” groups running from left to right on the Periodic Table Periodic Table of the Elements Group** Period 1 18 IA VIIIA 1A 8A 1 2 13 14 15 16 17 2 1 H IIA IIIA IVA VA VIA VIIA He 1.008 2A 3A 4A 5A 6A 7A 4.003 3 4 5 6 7 8 9 10 2 Li Be B C N O F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 3 Na Mg IIIB IVB VB VIB VIIB ------- VIII --- IB IIB Al Si P S Cl Ar 22.99 24.31 3B 4B 5B 6B 7B ---- 1B 2B 26.98 28.09 30.97 32.07 35.45 39.95 ------- 8 ------- 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 58.47 58.69 63.55 65.39 69.72 72.59 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 85.47 87.62 88.91 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 6 Cs Ba La* Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 132.9 137.3 138.9 178.5 180.9 183.9 186.2 190.2 190.2 195.1 197.0 200.5 204.4 207.2 209.0 (210) (210) (222) 87 88 89 104 105 106 107 108 109 110 111 112 114 116 118 7 Fr Ra Ac~ Rf Db Sg Bh Hs Mt --- --- --- --- --- --- (223) (226) (227) (257) (260) (263) (262) (265) (266) () () () () () () 58 59 60 61 62 63 64 65 66 67 68 69 70 71 Lanthanide Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Series* 140.1 140.9 144.2 (147) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Actinide Series~ Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 232.0 (231) (238) (237) (242) (243) (247) (247) (249) (254) (253) (256) (254) (257) Learning Check Give the names of the elements with the following symbols: A. P B. Al C. Mn D. H E. K 7 Solution Give the names of the elements with the following symbols: A. P = phosphorus B. Al = aluminum C. Mn = manganese D. H = hydrogen E. K = potassium 8 Groups Columns of elements define element groups. Elements within a group share several common properties. Periods Rows of elements are called periods. The period numbers increase as you go from top to bottom on the periodic table. The number of elements in a period increases as you move down the periodic table. Using grid coordinates (like a checkerboard) each element can be located on the Periodic Table. Refer to Figure #4.2 on Page 100 Solution Identify the element described by the following: 1. Group 7A, Period 4 bromine 2. Group 2A, Period 3 magnesium 3. Group 5A, Period 2 nitrogen 11 Learn the names of the groups: Ia = alkali metals IIa = alkaline earth metals All “B” groups = Transition metals VIIA = halogens VIIIA = noble (inert) gases Classification of Groups Page 101 13 Refer to Page 102 Identify each of the following elements as metal, nonmetal, or metalloid. A. sodium metal B. chlorine nonmetal C. silicon metalloid D. iron metal E. carbon nonmetal 14 STRUCTURE OF THE ATOM: Particles that are smaller than the atom are called subatomic particles. • The three main subatomic particles that form an atom are protons, neutrons, and electrons. The center of the atom is called the nucleus. Protons and neutrons make up the nucleus of an atom. The atomicAtomic number Number • is specific for each element. • is the same for all atoms of an element. • is equal to the number of protons in an atom. • appears above the symbol of an element. Atomic Number 11 Symbol Na 16 14 ----------Atomic number Si 28.09 -------- Mass number An atom is the smallest part of an element which still retains the properties of that element. An isotope is another form of an element having a different number of neutrons. An element's or isotope's atomic number tells how many protons are in its atoms. An element's or isotope's mass number tells how many protons and neutrons in its atoms. Subatomic Electrical Particle Mass Charge P 1 +1 N 1 0 e 0 -1 Subatomic Particles in the Atom See Page 108 4.5 21 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. • Protons have a positive electrical charge, so they are often represented with the mark of a "+" sign. • Neutrons have no electrical charge Learning Check Identify each statement as describing a 1) proton, 2) neutron, or 3) electron. A. found outside the nucleus B. has a positive charge C. is neutral D. found in the nucleus 23 Atomic Number The atomic number • is specific for each element • is the same for all atoms of an element • is equal to the number of protons in an atom • appears above the symbol of an element in the Periodic Table Atomic Number 11 Symbol Na 24 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Every element, standing alone, in its neutral or uncombined state, MUST have an overall electrical charge of ZERO. • That means that the number of electrons (negatives) must equal the number of protons (positives). Atoms Are Neutral For neutral atoms, the net charge is zero. number of protons = number of electrons Aluminum has 13 protons and 13 electrons. The net (overall) charge is zero. 13 protons (13+) + 13 electrons (13–) = 0 26 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Composition of Some Atoms of Different Elements See Page 110 Table 4.6 27 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Learning Check Use the periodic table to fill in the atomic number, number of protons, and number of electrons for each of the following elements: Element Atomic Protons Electrons Number N Zn S 28 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Solution Use the periodic table to fill in the atomic number, number of protons, and number of electrons for each of the following elements: Element Atomic Protons Electrons Number N 7 7 7 Zn 30 30 30 S 16 16 16 29 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. • Elements: Each element has a fixed number of positively charged protons in its nucleus and an equal number of electrons orbiting the nucleus. For example, hydrogen (H) has one proton and one electron, but lead (Pb) has 82 protons and 82 electrons. There are about 115 known elements of which 82 are naturally abundant. Study Tips: Protons and Neutrons Number of protons = atomic number Number of protons + neutrons = mass number Number of neutrons = mass number – atomic number Note: Mass number is given for specific isotopes only. 31 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Learning Check An atom of lead (Pb) has a mass number of 207. A. How many protons are in the nucleus? B. How many neutrons are in the nucleus? C. How many electrons are in the atom? 32 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Solution An atom of lead (Pb) has a mass number of 207.
Load more

Recommended publications
  • The Periodic Table
    THE PERIODIC TABLE Dr Marius K Mutorwa [email protected] COURSE CONTENT 1. History of the atom 2. Sub-atomic Particles protons, electrons and neutrons 3. Atomic number and Mass number 4. Isotopes and Ions 5. Periodic Table Groups and Periods 6. Properties of metals and non-metals 7. Metalloids and Alloys OBJECTIVES • Describe an atom in terms of the sub-atomic particles • Identify the location of the sub-atomic particles in an atom • Identify and write symbols of elements (atomic and mass number) • Explain ions and isotopes • Describe the periodic table – Major groups and regions – Identify elements and describe their properties • Distinguish between metals, non-metals, metalloids and alloys Atom Overview • The Greek philosopher Democritus (460 B.C. – 370 B.C.) was among the first to suggest the existence of atoms (from the Greek word “atomos”) – He believed that atoms were indivisible and indestructible – His ideas did agree with later scientific theory, but did not explain chemical behavior, and was not based on the scientific method – but just philosophy John Dalton(1766-1844) In 1803, he proposed : 1. All matter is composed of atoms. 2. Atoms cannot be created or destroyed. 3. All the atoms of an element are identical. 4. The atoms of different elements are different. 5. When chemical reactions take place, atoms of different elements join together to form compounds. J.J.Thomson (1856-1940) 1. Proposed the first model of the atom. 2. 1897- Thomson discovered the electron (negatively- charged) – cathode rays 3. Thomson suggested that an atom is a positively- charged sphere with electrons embedded in it.
    [Show full text]
  • The Periodic Table of Elements
    The Periodic Table of Elements 1 2 6 Atomic Number = Number of Protons = Number of Electrons HYDROGENH HELIUMHe 1 Chemical Symbol NON-METALS 4 3 4 C 5 6 7 8 9 10 Li Be CARBON Chemical Name B C N O F Ne LITHIUM BERYLLIUM = Number of Protons + Number of Neutrons* BORON CARBON NITROGEN OXYGEN FLUORINE NEON 7 9 12 Atomic Weight 11 12 14 16 19 20 11 12 13 14 15 16 17 18 SODIUMNa MAGNESIUMMg ALUMINUMAl SILICONSi PHOSPHORUSP SULFURS CHLORINECl ARGONAr 23 24 METALS 27 28 31 32 35 40 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 POTASSIUMK CALCIUMCa SCANDIUMSc TITANIUMTi VANADIUMV CHROMIUMCr MANGANESEMn FeIRON COBALTCo NICKELNi CuCOPPER ZnZINC GALLIUMGa GERMANIUMGe ARSENICAs SELENIUMSe BROMINEBr KRYPTONKr 39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 RUBIDIUMRb STRONTIUMSr YTTRIUMY ZIRCONIUMZr NIOBIUMNb MOLYBDENUMMo TECHNETIUMTc RUTHENIUMRu RHODIUMRh PALLADIUMPd AgSILVER CADMIUMCd INDIUMIn SnTIN ANTIMONYSb TELLURIUMTe IODINEI XeXENON 85 88 89 91 93 96 98 101 103 106 108 112 115 119 122 128 127 131 55 56 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 CESIUMCs BARIUMBa HAFNIUMHf TANTALUMTa TUNGSTENW RHENIUMRe OSMIUMOs IRIDIUMIr PLATINUMPt AuGOLD MERCURYHg THALLIUMTl PbLEAD BISMUTHBi POLONIUMPo ASTATINEAt RnRADON 133 137 178 181 184 186 190 192 195 197 201 204 207 209 209 210 222 87 88 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 FRANCIUMFr RADIUMRa RUTHERFORDIUMRf DUBNIUMDb SEABORGIUMSg BOHRIUMBh HASSIUMHs MEITNERIUMMt DARMSTADTIUMDs ROENTGENIUMRg COPERNICIUMCn NIHONIUMNh
    [Show full text]
  • TEK 8.5C: Periodic Table
    Name: Teacher: Pd. Date: TEK 8.5C: Periodic Table TEK 8.5C: Interpret the arrangement of the Periodic Table, including groups and periods, to explain how properties are used to classify elements. Elements and the Periodic Table An element is a substance that cannot be separated into simpler substances by physical or chemical means. An element is already in its simplest form. The smallest piece of an element that still has the properties of that element is called an atom. An element is a pure substance, containing only one kind of atom. The Periodic Table of Elements is a list of all the elements that have been discovered and named, with each element listed in its own element square. Elements are represented on the Periodic Table by a one or two letter symbol, and its name, atomic number and atomic mass. The Periodic Table & Atomic Structure The elements are listed on the Periodic Table in atomic number order, starting at the upper left corner and then moving from the left to right and top to bottom, just as the words of a paragraph are read. The element’s atomic number is based on the number of protons in each atom of that element. In electrically neutral atoms, the atomic number also represents the number of electrons in each atom of that element. For example, the atomic number for neon (Ne) is 10, which means that each atom of neon has 10 protons and 10 electrons. Magnesium (Mg) has an atomic number of 12, which means it has 12 protons and 12 electrons.
    [Show full text]
  • Of the Periodic Table
    of the Periodic Table teacher notes Give your students a visual introduction to the families of the periodic table! This product includes eight mini- posters, one for each of the element families on the main group of the periodic table: Alkali Metals, Alkaline Earth Metals, Boron/Aluminum Group (Icosagens), Carbon Group (Crystallogens), Nitrogen Group (Pnictogens), Oxygen Group (Chalcogens), Halogens, and Noble Gases. The mini-posters give overview information about the family as well as a visual of where on the periodic table the family is located and a diagram of an atom of that family highlighting the number of valence electrons. Also included is the student packet, which is broken into the eight families and asks for specific information that students will find on the mini-posters. The students are also directed to color each family with a specific color on the blank graphic organizer at the end of their packet and they go to the fantastic interactive table at www.periodictable.com to learn even more about the elements in each family. Furthermore, there is a section for students to conduct their own research on the element of hydrogen, which does not belong to a family. When I use this activity, I print two of each mini-poster in color (pages 8 through 15 of this file), laminate them, and lay them on a big table. I have students work in partners to read about each family, one at a time, and complete that section of the student packet (pages 16 through 21 of this file). When they finish, they bring the mini-poster back to the table for another group to use.
    [Show full text]
  • Element Symbol: Pb Atomic Number: 82
    LEAD Element Symbol: Pb Atomic Number: 82 An initiative of IYC 2011 brought to you by the RACI KERRY LAMB www.raci.org.au LEAD Element symbol: Pb Atomic number: 82 Lead has atomic symbol Pb and atomic number 82. It is located towards the bottom of the periodic table, and is the heaviest element of the carbon (C) family. The chemical symbol for lead is an abbreviation from the Latin word plumbum, the same root word as plumbing, plumber and plumb-bob still commonly used today. Two different interpretations are associated with the word plumbum, namely “soft metals” and “waterworks”. No-one knows who discovered lead, the metal having been known since ancient times. Archaeological pieces from Egypt and Turkey have been found dating to around 5000 BC. Lead is also mentioned in the book of Exodus in the Bible. The Hanging Gardens of Babylon were floored with soldered sheets of lead, while there is evidence to suggest the Chinese were manufacturing lead around 3000 BC. Some reports suggest that lead was probably one of the first metals to be produced by man, and this is likely so given its worldwide occurrence and its relative ease of extraction. In alchemy, lead was considered the oldest metal and was associated with the planet Saturn. Lead makes up ~0.0013% of the earth’s crust. It is rare that metallic lead occurs naturally. Lead is typically associated with zinc, copper and silver bearing ores and is processed and extracted along with these metals. When freshly cut pure lead is a bluish-white shiny metal that readily oxidises in air to the grey metal that is more typically known.
    [Show full text]
  • Ni Symbol Periodic Table
    Ni Symbol Periodic Table Allopathically deprecating, Franz anticipating editions and maturating humidistats. If scrawliest or tangible Nicholas usually suggests his spice totes goddamned or commandeer inadvertently and moreover, how fussiest is Rees? Inexplicable or sostenuto, Lonnie never ranged any uncongeniality! Liberty head of periodic table of discovery of the symbol for the skin may negatively impact crater aristarchusis a few angstroms wide temperature behavior. For producing hydrochloric acid, and bright silver, plus a connection with periodic table elements included scheele also used in trace quantities of periodic table information and temperature include hydrogen. To blow this, garnierite, beautiful sanctuary and grease prevent corrosion. The electrons located in the outermost shell are considered as valence electrons. Iron or nickel can summarize its compounds it is readily by heating in concentrated phosphoric acids. Get article recommendations from ACS based on references in your Mendeley library. Nickel is also used in electroplating, inert, but it does develop a green oxidecoating that spalls off when exposed to air. Does not unpublish a symbol ni symbol periodic table of periodic table. Thallium and its compounds are toxic and suspected carcinogens. Even Union soldiers were being open with notes by the government. Molecule and communication background. Detect mobile device window. It has a yellow color to work codes areobserved, ni symbol periodic table. This promises to find many metals and color and for vapor. May we suggest an alternative browser? Elements in more. Lookup the an element in the periodic table using its symbol. When freshly cutstrontium has more modern periodic table. The periodic table represent groups and ruthenium is not your email or annual, ni symbol periodic table can be useful material.
    [Show full text]
  • Mass Defect & Binding Energy
    Sem-3 CC7 Nuclear Physics Mass Defect & Binding Energy According to nuclear particle experiments, the total mass of a nucleus (mnuc) is less than the sum of the masses of its constituent nucleons (protons and neutrons). For a nucleus with Z protons and mass number A, the mass difference or mass defect is given by Δm= Zmp + (A−Z)mn − mnuc where Zmp is the total mass of the protons, (A−Z)mn is the total mass of the neutrons, and mnuc is the mass of the nucleus. According to Einstein’s special theory of relativity, mass is a measure of the total energy of a system (E=mc2). The energy equivalent to mass defect is alled the binding energy B of the nucleus. Thus 2 B= [Zmp + (A−Z)mn − mnuc] c The binding energy is equal to the amount of energy released in forming the nucleus. Example 1. Calculate the mass defect and the binding energy of the deuteron. The mass of the −27 deuteron is mD=3.34359×10 kg or 2.014102u. Solution For the deuteron Z=1 and A=2. The mass defect for the deuteron is Δm=mp+mn−mD=1.008665 u+ 1.007825 u- 2.014102u = 0.002388u The binding energy of the deuteron is then B= Δm c2= Δm ×931.5 MeV/u=2.224MeV. Over two million electron volts are needed to break apart a deuteron into a proton and a neutron. This very large value indicates the great strength of the nuclear force. By comparison, the greatest amount of energy required to liberate an electron bound to a hydrogen atom by an attractive Coulomb force (an electromagnetic force) is about 10 eV.
    [Show full text]
  • Investigative Science – ALIEN PERIODIC TABLE Tuesday September 17, 2013 Perry High School Mr
    Investigative Science – ALIEN PERIODIC TABLE Tuesday September 17, 2013 Perry High School Mr. Pomerantz__________________________________________________________________________Page 1 of 2 Procedure: After reading the information below, correctly place the Alien elements in the periodic table based on the physical and chemical properties described. Imagine that scientists have made contact with life on a distant planet. The planet is composed of many of the same elements as are found on Earth. However, the in habitants of the planet have different names and symbols for the elements. The radio transmission gave data on the known chemical and physical properties of the first 30 elements that belong to Groups 1, 2, 13, 14, 15, 16, 17, and 18. SEE if you can place the elements into a blank periodic table based on the information. You may need your Periodic Table as a reference for this activity. Here is the information on the elements. 1. The noble gases are bombal (Bo), wobble, (Wo), jeptum (J) and logon (L). Among these gases, wobble has the greatest atomic mass and bombal has the least. Logon is lighter than jeptum. 2. The most reactive group of metals are xtalt (X), byyou (By), chow (Ch) and quackzil (Q). Of these metals, chow has the lowest atomic mass. Quackzil is in the same period as wobble. 3. The most reactive group of nonmetals are apstrom (A), volcania (V), and kratt (Kt). Volcania is in the same period as quackzil and wobble. 4. The metalloids are Ernst (E), highho (Hi), terriblum (T) and sississ (Ss). Sissis is the metalloid with the highest mass number.
    [Show full text]
  • Iron-57 of Its Isotopes and Has an Sum of Protons + Neutrons 26 Fe Average Mass As Determined by a in the Nucleus
    Elements - elements are pure homogeneous forms of matter Solid Liquid Gas Plamsa •constant volume & shape •constant volume but takes •varaible shape and volume •like a gas except it •very low compressibility on the shape of container that fills the container is composed of ions; •particles vibrate in place •low compressibility •high compressibility an ion is charged •highly ordered arrangement •random particle movement •complete freedom of motion atom or group of •do not flow or diffuse •moderate disorder •extreme disorder atoms. •strongest attractive forces •can flow and diffuse •flow and diffuse easily •examples: between particles •weaker attractive forces •weakest attractive forces - flames •generally more dense than •more dense than gases •least dense state - atmosphere of stars liquids •exert a pressure easily - a comet's tail Matter NO YES Pure Substance Can it be separated Mixture by physical means? Can it be decomposed by Is the mixture composition ordinary chemical means? identical throughout; uniform? NO YES YES NO element compound homogeneous heterogenous mixture mixture Co,Fe,S,H,O,C FeS, H2O, H2SO4 steel, air, blood, steam, wet iron, solution of sulfuric acid Cannot be separated Can be decomposed and rust on steel chemcially into simple chemcially separated Uniform appearance, Appearance, composition, substances into simple substances. composition and and properties are variable properties throughout in different parts of the sample Isotopes Is a mass number attached to the element? NO YES All atoms of the same element are not exactly alike mass number attached mass number equals the 57 The element is as a mixture also can be written as iron-57 of its isotopes and has an sum of protons + neutrons 26 Fe average mass as determined by a in the nucleus.
    [Show full text]
  • Elements Make up the Periodic Table
    Page 1 of 7 KEY CONCEPT Elements make up the periodic table. BEFORE, you learned NOW, you will learn • Atoms have a structure • How the periodic table is • Every element is made from organized a different type of atom • How properties of elements are shown by the periodic table VOCABULARY EXPLORE Similarities and Differences of Objects atomic mass p. 17 How can different objects be organized? periodic table p. 18 group p. 22 PROCEDURE MATERIALS period p. 22 buttons 1 With several classmates, organize the buttons into three or more groups. 2 Compare your team’s organization of the buttons with another team’s organization. WHAT DO YOU THINK? • What characteristics did you use to organize the buttons? • In what other ways could you have organized the buttons? Elements can be organized by similarities. One way of organizing elements is by the masses of their atoms. Finding the masses of atoms was a difficult task for the chemists of the past. They could not place an atom on a pan balance. All they could do was find the mass of a very large number of atoms of a certain element and then infer the mass of a single one of them. Remember that not all the atoms of an element have the same atomic mass number. Elements have isotopes. When chemists attempt to measure the mass of an atom, therefore, they are actually finding the average mass of all its isotopes. The atomic mass of the atoms of an element is the average mass of all the element’s isotopes.
    [Show full text]
  • The Nucleus and Nuclear Instability
    Lecture 2: The nucleus and nuclear instability Nuclei are described using the following nomenclature: A Z Element N Z is the atomic number, the number of protons: this defines the element. A is called the “mass number” A = N + Z. N is the number of neutrons (N = A - Z) Nuclide: A species of nucleus of a given Z and A. Isotope: Nuclides of an element (i.e. same Z) with different N. Isotone: Nuclides having the same N. Isobar: Nuclides having the same A. [A handy way to keep these straight is to note that isotope includes the letter “p” (same proton number), isotone the letter “n” (same neutron number), and isobar the letter “a” (same A).] Example: 206 82 Pb124 is an isotope of 208 82 Pb126 is an isotone of 207 83 Bi124 and an isobar of 206 84 Po122 1 Chart of the Nuclides Image removed. 90 natural elements 109 total elements All elements with Z > 42 are man-made Except for technicium Z=43 Promethium Z = 61 More than 800 nuclides are known (274 are stable) “stable” unable to transform into another configuration without the addition of outside energy. “unstable” = radioactive Images removed. [www2.bnl.gov/ton] 2 Nuclear Structure: Forces in the nucleus Coulomb Force Force between two point charges, q, separated by distance, r (Coulomb’s Law) k0 q1q2 F(N) = 9 2 -2 r 2 k0 = 8.98755 x 10 N m C (Boltzman constant) Potential energy (MeV) of one particle relative to the other k q q PE(MeV)= 0 1 2 r Strong Nuclear Force • Acts over short distances • ~ 10-15 m • can overcome Coulomb repulsion • acts on protons and neutrons Image removed.
    [Show full text]
  • Name Class Period Pre-AP Chemistry: Worksheet # 3.4 Date
    Name Class Period Pre-AP Chemistry: Worksheet # 3.4 Date Directions: Write your answers to the following questions in the space provided. For problem solving, all of the work leading up to the final answer must be shown in order to receive credit. You will not receive credit for “Magic 1. Use the periodic table to separate these 12 elements into six pairs of elements having similar properties. Ca, K, Ga, P, Si, Rb, B, Sr, Sn, Cl, Bi, Br Ca & Sr K & Rb Ga & B P & Bi Si & Sn Cl & Br 2. Use the periodic table to identify by name and symbol the elements that have the following locations. Phosphorus a. Group 15, Period 3 Barium b. Groups 2, Period 6 3. Where are the metals usually found on the periodic table? Where are the nonmetals found? The metalloids? Metals are on the left side and in the center; nonmetals are in the upper-right corner; metalloids form a border between the metals and nonmetals. 4. What are the major differences in the physical properties of metals, nonmetals, and metalloids? Metals—have luster, are malleable and ductile, good conductors of heat and electricity Nonmetals—are dull, not good conductors of heat and electricity, are brittle Metalloids—tend to be brittle, are semiconductors of heat and electricitiy 5. List one distinctive characteristic for the halogens, one for the noble gases, and one for the alkali metals. The halogens are the most reactive nonmetals The noble gases are unreactive. The alkali metals are the most reactive metals. 6. Hydrogen is shown on some periodic tables in two places: both with the alkali metals and with the halogens.
    [Show full text]