Chemistry Quiz REview - Quiz material summary on ch 2 and 3 PDF

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Quiz material summary on ch 2 and 3...

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Chemistry Quiz #1 Review  

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09/17/2014

Chapter 2: -Element:  only one type of atom, these atoms not created/destroyed/divisible o not all atoms identical though- isotopes -Compound  2 or more elements bonded chemically, broken by chemical change  its properties are different from that of its elements  Both element and compounds are pure substance- fixed composition

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-Mixture  2 or more substances physically intermingled  separated by physical change -Mass Fraction  Mass of element X in compound A/ mass of compound A o Mass fraction fixed no matter size of the sample o Mass percent is this x100

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-Dalton’s Atomic theory  all matter consists of atoms

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-Electron Experiment  Cathode Ray experiment o negatively charged particles found in all matter

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JJ Thompson’s plum pudding model o Mass/charge ratio of electron

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Milikan’s oil drop experiment o Charge of electron and mass

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-Rutherford’s Gold foil experiment  some rays bounced back- discovered nucleus of positive charge that holds majority of an atom’s mass

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-Structure of Atom  proton and neutron in nucleus o proton p+ has positive charge  mass 1.0 amu aka 1.66054 x 10^(-24) g  charge: +1.602 x 10^(-19) 

electron is same charge but negative o neutron n0 has no charge  mass 1.0 amu o atom is neutral bc #protons = #electrons   

-Atomic #  number of protons, always the same for an element -Mass #  total number of protons and neutrons in nucleus -Isotopes  same atomic number but different mass number

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-Periodic Table  Mendeleev’s periodic table came first o arranged according to increasing atomic mass  Modern periodic table o In order of increasing atomic number o Groups and Periods  Groups     

Groups- similar chemical properties The 8 A groups- main group elements 10 B groups- transition elements 1A and 2A- highly reactive elements Halogens- high reactive nonmetals

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Noble Gases- unreactive metals Periods  Different chemical properties

o Metals, Metalloids, Nonmetals  Metals- most of table 

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-Compounds

Mercury only metal liquid at room temp Nonmetals  Not good conductors

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Ionic o Transferring electrons o Binary ionic compound  Metal and nonmetal  Metal loses electron- cation  Nonmetal gains electron- anion o 3D array

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Covalent o Sharing electrons o Distinct structures o Example: H2 o Mutual attraction between two nuclei and two electrons

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Polyatomic ions o

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-Coulombs law  energy of attraction is directly proportional to product of charges and inversely proportional to distance between them

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-Nomenclature  Binary Ionic compounds o Cation + anion with –ide ending o Charge of one ion becomes subscript of other  Compounds of metals that form more than one ion

o Example: Cobalt has Co 2+ and Co 3+ o Cation plus (roman numeral)  Lower charge- suffix –ous  Higher charge- suffix –ic 

Compounds w/polyatomic ions o Just memorize these o (NH4)+ ammonium o H3O+ hydronium o CH3CO2- acetate

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Acids o hydrogen containing o binary acids  hydrochloride dissolves in water (HCl) it becomes hydrochloric acid o oxoacids  ate becomes ic 

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ite becomes ous Binary Covalent Compounds o Example: H2O, NH3 o Element with lower group number comes first  If same group, higher period first o Greek Prefix for both

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-Organic compounds  contain carbon  hydrocarbons o contain only H and C

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-Molecular Mass  sum of atomic masses

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-Mixtures  heterogeneous  homogeneous

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-Weak acid/weak base are weak electrolyte, strong acid/ base are strong electrolyte

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Chapter 2: -Law of Multiple Proportions -isotopic mass

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-molecular v. covalent compound -coulombs law

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-Naming  oxoanions  hydrated ionic compounds -percent abundance of isotopes

Chapter 3- Stoichiometry 

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-Mole  SI unit for amount of substance  Contains 6.022x10^23 (avogadro’s number)  Atom has mass in amu, same as mol has mass in g -Molar mass  mass per mole  

monoatomic elements its just atomic mass molecular elements like O2- atomic massx2

09/17/2014...