# CHM 1020 Final

 What is the value of a mole (mol)?
 6.022 x 10^23
 Who was the mole named after?
 What is the atomic mass unit?
 1/12 of the mass of carbon-12
 What is molar mass?
 The mass of 1 mol of atoms of an element
 Covert from moles to grams by:
 Multiply # moles by # molar mass
 Convert from grams to moles by:
 Divide # grams by # molar mass
 Convert grams to # of atoms by:
 Divide # grams by molar mass then multiply by 6.022 x 10^23
 Convert from molecules to grams by:
 Divide # molecules by 1 mol, then multiply by molar mass
 Convert grams of compound to grams of element by:
 Divide by total mass and multiply by mass of target element
 Mass percent composition
 Element’s percentage of the total mass of compound
 Calculate mass percent by:
 Divide target element by total compound in grams
 Convert grams of element to grams of compound by:
 Multiply initial element (g) by 100/(percentage)
 Calculate empirical formula by:
 Divide experimental mass of each element by molar mass of that element
 Calculate empirical formula from reaction data by:
 Subtracting given element mass from total compound mass
 n = ?
 Molar mass(usually bigger number) / empirical formula molar mass
 Compounds containing what are soluble?
 Li, Na, K, NH4, NO3, C2H3O2
 Compounds that may be soluble (Cl, Br, I)
 Cannot contain Ag, Hg2, Pb
 Compounds that may be soluble (SO4)
 Cannot contain Sr, Ba, Pb, Ca
 Slightly soluble if:
 Contains OH; but not Li, Na, K, NH4; but does have Ca, Sr, Ba
 What is a molecular equation?
 Shows complete, neutral formulas for every compound in a reaction
 What is a complete ionic equation?
 Shows all of the species as they are actually present in the solution
 What is a net ionic equation?
 Shows only the species that actually participate in the reaction
 What are the characteristics of oxidation-reduction reactions?
 Involve transfer of electrons
 What does OIL RIG stand for?
 Oxidation is loss, reduction is gain
 What is the law of constant composition?
 All samples of a given compound have the same proportions of their corresponding elements.
 NH4
 Ammonium
 C2H3O2
 Acetate
 Mg(NO3)2?
 Magnesium nitrate
 What is an empirical formula?
 It gives the relative number of atoms of each element in a compound.
 Atomic elements are:
 Single atoms of an element
 Molecular elements are:
 (Usually) doubled atoms of an element
 Molecular compounds are:
 Compounds formed from two or more nonmetals. (H2O)
 Ionic compounds are:
 Compounds that contain one or more cations paired with one or more anions. (NaCl)
 Cation is:
 Positively charged ions
 Anions are:
 Negatively charged ions
 What is an ion?
 It makes up the electric charge of an atom.
 You can assume a compound is ionic when:
 You have a metal and one or more nonmetals together in a chemical formula
 What is a Type I metal?
 It does have a charge that varies from one compound to another
 What is a Type II metal?
 It has a charge that differs in different compounds
 Binary compounds are:
 Those that contain only two different elements and end with -ide
 SO3
 Sulfite
 SO4
 Sulfate
 CO3
 Carbonate
 NO3
 Nitrate
 NO2
 Nitrite
 HCl
 Hydrochloric acid
 KOH
 Potassium hydroxide
 HNO3
 Nitric acid
 NaOH
 Sodium hydroxide
 NaNO3
 Sodium nitrate
x

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