Elements and Compounds. Composition of Matter
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1 Elements and Compounds Composition of Matter
2 Elements
3
4 Element Identification
5 Source of Light Elements
6 Solar Spectra
7 Detecting Elements
8 Molecular Spectrum of CO
9 Chemical and Physical Properties Elements An Element is the basic form of matter it cannot be broken down into smaller parts by chemical methods Each element has a unique identity
10 Compounds A Compound is a unique substance that is formed from two or more elements and has different properties from all other substances
11 Pure Substances Pure substances have unchanging, definite compositions and properties. Table Salt: crystalline white substance that is commonly used to modify food taste NaCl : 1 sodium atom + 1 chlorine atom. Two different elements, unique properties.
12 Properties of Substances A physical property is one that can be observed without performing a change to the substance: Color Density Hardness etc.
13 Names of the Elements Latin names from historical context produce unusual symbols for some elements: first letter is capitalized, second is lower case Ferrum: Fe (Iron) Aurum: Au (Gold) Cobalt: Co
14
15 Atomic Theory John Dalton used Greek ideas with experimentation to reveal the atomic nature of the elements The atom is defined as the smallest particle of an element that retains the properties of the bulk element Daltons atomic theory allows the prediction of composition
16 Daltons Atomic Theory Matter is composed of atoms All atoms of each element are identical and possess the same properties Chemical compounds are composed of atoms of different elements in whole number ratio Reactions produce re-arranged atoms
17 Law of Constant Composition Any compound is made up of elements in the same proportion by mass. A compound is identified by a specific formula
18 Compounds and Molecules Two or more elements bonded to each other are molecules or molecular compounds Elements bonded together are polyatomic i.e. Cl 2 Molecules may be formed by both types: compounds or polyatomic elements
19 Chemical Properties Chemical properties are related to the identity of the element or the compound The ability of a substance to undergo a chemical change: reaction Chemical change is a transformation of a substance into a new substance
20 Mixtures of elements and compounds
21 Mixtures Heterogeneous: a non-uniform mixture containing two or more phases Sample of mixture produces different amounts of each substance in container
22 Homogeneous Mixtures One physical state with uniform properties May be a Solution or an Alloy Solution: homogeneous mixture with one liquid phase Alloy: homogeneous mixture of solids with one phase (solid solution)
23 Electrons 1897 J.J. Thompson proves existence of the electron Is common to all atoms Has a charge of -1 Used Plum Pudding analogy : electrons and a positive medium mixed as a solid particle
24 Rutherford Experiment Used positively charged helium ions to bombard thin gold foil Showed a dense positively charged center- not a conglomeration of positive and negative charges Calculated charge to mass ratio =-1.76 x 10 8 coulombs/gram From an electron beam
25
26 Electron Properties R.A. Millikan (Univ. Of Chicago) determined charge magnitude of electrons which led to the determination of the mass q= -1.6 x Coulombs Mass = 9.11 x grams (from charge to mass ratio)
27 The Nuclear Atom
28 Counting The Particles All atoms of each element are not quite the same Mass of atoms of an element is variable, a result of a new particle, the neutron The nuclear mass is the sum of protons and neutrons: isotopes
29 Calculating Isotopic Values Atomic Number = element identity = Protons in nucleus neutrons=mass number protons 90 Sr has 38 protons: = 52 neutrons Still has 38 electrons!
30
31 Atomic Mass Units Isotopic mass is determined by comparison with a standard: AMU = 1/12 the mass of a 12 C atom Boron isotopes: 10 B is times the mass of 12 C: Therefore has AMU 11 B has AMU
32 Table Values for Atomic Mass Since elements exist in nature with isotopic masses, the reported value is the weighted average of all of these isotopes based on their percent abundance
33 Calculating atomic masses Nature contains 19.9% 10 B and 80.1% 11 B. What is the weighted average? 10 B: x AMU = 1.99 AMU 11 B: x AMU = 8.82 AMU AMU
34 End of Chapter 5
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