CHAPTER 1 Units of measure Dimensional Analysis conversions Sig Fig Rules Volume Density Giga mega kilo METER deci centi milli micro nano pico 109 106 103 10 1 10 2 10 3 10 6 10 9 10 12 Sig Fig Rules Density g cm3 mass volume Volume cm3 area 3 Ex A cube of Aluminum Al metal measures 15 6mm on a side It weighs 10 25g What is the density CHAPTER 2 Atoms are made up of protons neutrons and electrons are mostly empty space o Nucleus contains all of the weight protons neutrons Element contains only one type of atom o Defined by the number of protons in the nucleus o Designated by blocks ex S block P block o Can be either a gas liquid or solid most are metals solid Rare earth metals found in batteries motors etc Lanthanides Liquids Hg Cs Br2 Ga I2 Gases N2 He H2 X2 halogen Molecule contains 2 or more different atoms bonded together o Is an independent unit o Ex H20 CO NO2 hydrogen h h Compound contains 2 or more different elements bonded together o Are not independent units o Ex H20 CO2 NaCl GaAs TiN CaCO3 Mixture 2 substances physically intermingled and must be separable o Ex O2 N2 2 NO not a mixture Diatomic Gases Have No Fear Of Ice Cold Beer o H2 N2 F2 O2 I2 Cl2 Br2 Ion an atom with a different charge caused by the loss or gain of an electron o All Alkalide metals group 1 form 1 charge o All Alkaline metals group 2 form 2 EXCEPT Be 1 Cation positively charged ions lose electrons Ex Ca calcium Ca2 calcium ion 2 Anion negatively charged ion gain electrons Ex Cl chlorine Cl chloride O oxygen O2 oxide N nitrogen N2 nitride Isotope 2 different forms of the same element have different masses o different number of neutrons causes the mass to differ protons don t change o Name isotopes by their mass and element name EXCEPT hydrogen 1H hydrogen 2H Deuterium 3H Tritium Ex Isotopic mass approximate not exact protons neutrons Atomic Mass Unit amu equals 1 12 the mass of 1 atom of Carbon 12 a 1amu 1 66 x 10 24g mass of proton and electron Atomic Mass is composed of protons and neutrons in the nucleus mass 1 amu b Mass on the periodic table is the weighted average of naturally occurring isotopes Ex Carbon 12 is 98 89 abundant in nature with a mass of 12 000amu Carbon 13 is 1 11 abundant in nature with a mass of 13 003amu Based on the isotopes find the atomic mass Ex Chloride z 17 has two isotopes Find the atomic mass of Cl 35Cl 34 9689amu 75 774 37Cl 36 9659amu 24 226 Ex The mass of Chlorine is 35 45amu There are two naturally occuring isotopes Chlorine 35 has a mass of 34 9689amu and Chlorine 37 has a mass of 36 9659amu Find their abundance in nature Percent Composition Mass Atom Volume Pressure Atom of X atoms total atoms x 100 Mass mass X molecular weight Molecular weight sum of atomic weights Mole of carbon 12 atoms in 12 grams of 12C o Avogadro s number 6 022 x 1023 Represents the number of molecules in 1 mole molecules 1 mole One mole of ANY SUBSTANCE contains 6 02 x 10 23 units GRAMS PER MOLE ARE EQUAL TO THE MOLECULAR MASS 1amu 1g mol o 1 mole of B has mass of 10 81 grams o 1 atom of B 10 81 amu Ex How many grams are in 1 mole of water H20 Ex How many carbon atoms are in a 0 0265g diamond Ex H20 has a density of 1 g mL molecule has mass of 18 01amu One mole of H20 a Has a mass of 18 01g b Has 6 02 x 1023 molecules Occupies 18mL c d All of the above Periodic Table Arranged according to periods on left and families on top columns Organized according to chemical activity Group 1 Alkalide metals 1 charge Group 2 Alkaline earth metals 2 charge Group 15 Pntiogens Group 16 Chalcogens Group 17 Halogens Group 18 Noble inert gases Lanthanides aka rare earth metals Nomenclature Chemical symbol has capitalized 1st letter lowercase 2nd letter An element is defined by the number of protons in the nucleus