CHAPTER #2 - Atoms, Molecules, and Ions
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1 CHAPTER #2 - Atoms, Molecules, and Ions 2.1 The Early History of Chemistry - Ancient Greeks - thought matter was composed to 4 substances earth, air, fire, water ( vs. ) Alchemy - (discovered many elements; learned to prepare mineral acids) Metallurgy - extraction of metals from ore Robert Boyle - ( Skeptical Chymist) - first quantitative experiments; current concept of element Georg Stahl suggested phlogiston flowed out of burning material Joseph Priestley - ( ) discovered oxygen (not phlogiston) Fundamental Chemical Laws/ Dalton s Atomic Theory - NATURAL LAWS: 1. Conservation of Mass - In any chemical reaction, mass is neither created nor destroyed 2. Constant Composition a given compound always contains exactly the same proportion of elements by mass. 3. Multiple Proportions - When two elements form a series of compounds, the ratios of the masses of the 2 nd element that combine with 1 gram of the 1 st element can always be reduced to small whole numbers. Mass Oxygen w/ 1 g C Cpd I 1.33 g Cpd II 2.66 g Mass Nitrogen w/ 1 g O Cpd I g Cpd II g Cpd III g John Dalton (1808) Father of Atomic Theory Essentials of his theory An element is composed of tiny particles called atoms. All atoms of a given element show the same chemical properties. 2. Atoms of different elements have different properties. In an ordinary chemical reaction, no atom of any element disappears or is changed into an atom of another element. 3. Compounds are formed when atoms of two or more elements combine. In a given compound, the relative numbers of atoms of each kind are
2 definite and constant. In general, these relative numbers can be expressed as integers or simple fractions. IN GENERAL - Elements consist of tiny particles called, which retain their identity in. In a compound, atoms of two or more elements are combined in a fixed ratio of. Gay-Lussac - (1809) Combining Volumes of Gases Performed experiments in which he measured (under same T & P) the that reacted with each other. Amadeo Avogadro - (1811) Avogadro s Hypothesis Equal volumes of different gases contain the at the same temperature and pressure. 2.4 Early Experiments to Characterize the Atom JJ Thomson ( ): English physicist Experiment (late 1890 s) Important Observations Inferences This lead to the Model
3 Robert Milikan ( ) Experiment (1909) Important Observations Inferences Sir James Chadwick ( ): confirmed existence of Henri Bequerel (1896) French Chemist essentially discovered (alpha, beta, and gamma particles discovered later) Ernest Rutherford (1911) experiment Important Observations Inferences A. Rutherford s Hypothesis B. Rutherford s Model
4 Modern View of Atomic Structure/ Molecules and Ions - Relative Relative Actual Actual COMPONENTS Mass Charge Location Mass Charge Proton 1 +1 nucleus x g x C Neutron 1 0_ nucleus x g 0 Electron 0_ -1_ outside nucleus x g x C Nuclear Symbol A Z X (X = element symbol) ex C or 74 As 3- Z = Atomic Number = number of protons and is UNIQUE A = Mass Number = sum of neutrons and protons is NOT unique Atoms - electrically neutral (#p + = #e - ) Isotopes atoms of the same element with different number of neutrons (thus diff mass #). Molecules multiple atoms; covalently bonded; electrically neutral # protons = # electrons Methane, CH 4 Propane, C 3 H 8
5 Ions - Have an electrical charge due to gain/loss of electrons cations positive (lost e-) anions negative (gained e-) Insert images pf sodium ion and chloride ion a) Covalent Bonding b) Ionic Bonding Polyatomic ion multiple atoms; covalently bonded; NOT electrically neutral # protons # electrons
6 isoelectric species that have the same electron arrangement. (For monatomic atoms/ions this simply means they have the same number of electrons. Ex. K +, Ca 2+, P 3-, S 2-, Cl -, Ar are isoelectric (all 18 electrons arranged 1s 2 2s 2 2p 6 3s 2 3p 6 ) Na + is isoelectric with The Periodic Table Know the general organization of periodic table in terms of Groups/families Period/series alkali metals, alkaline earth metals, halogens, noble gases, transition metals, inner transition metals (lanthanides & actinides) metals/non-metals/metalloids (general metallic character increases toward Francium) radioactive elements synthetic elements atomic size (decreases across periods and increases down families) Naming Ionic Cpds, Molecular Cpds, & Acids see next page
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