Ch 1, 2, 3 Review Flashcards
Subscripts in Chemical Formulas
tell number of atoms of an element in a compound
Coefficients in Chemical Formulas
tell number of molecules of the compound
Law of Multiple Proportions
when two elements form multiple compounds, you can find the ratio of each compounds’ masses and there will be a common whole number ratio between those ratios
Isotopes and number of protons
The number of protons in an element never changes; given carbon-26, we know that there are 12 carbon protons and therefore there are 14 neutrons in this isotope
Ionic vs Molecular Compounds
Ionic is between metal and nonmetal; a Molecular is between two nonmetals, aka Covalent
Covalent Compounds
formed by two nonmetals sharing electrons
Naming Ionic Compounds
metals with nonmetals; metal name + (IV) if a transition metal + nonmetal name + -ide
Naming Covalent Compounds
nonmetals with nonmetals; prefix based on number + first nonmetal (-ion charge) + prefix based on number + other nonmetal + -ide
Prefixes for naming covalent compounds
mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
Naming acids
When there is no oxygen involved: Hydro + root+ -ic
When there is oxygen: root of polyatomic + -ic/-ous
-ate becomes -ic, -ite becomes -ous
Calculating Number of Atoms or Molecules
multiply moles by Avogadros number
Percent Composition in a Compound
Molar Mass of Element looking for/ Total Molar Mass of Compound
How to calculate empirical formula from percent composition
Assume you have 100gs of solution and convert percents into masses. Convert masses to moles using the molar mass. Divide all moles by the lowest mole quantity to get the ratio.
Combustion Analysis: Empirical
Take product mass and convert to moles. Convert to moles of reactant (if looking for C moles, use CO2 as the product you focus on). Convert to mass. Repeat for all reactants. Using conservation of mass, solve for unknown mass. Find lowest moles and divide to get a common ratio.
Formula Weights vs Molar Mass vs Molecular Weight
same number, different units. in amu. the formula weight of a compound is it’s molar mass just in amu instead of g/mol; formula weight is for ionic compounds, molecular weight is for molecular compounds
Mass of n moles of an element
n*the element’s molar mass
Percent Error
abs(actual-theoretical)/theoretical
prefix hypo
means that it’s a polyatomic ion and it has one fewer oxygen than the -ite form of the ion.
prefix per
means that it’s polyatomic ion and it has one more oxygen than the -ate form of the ion
Avogadro’s Number
6.022e23
W
Tungsten
Sb
Antimony
Zr
Zirconium
Pu
Plutonium
Pt
Platinum
Mercury (I)
Hg2
Charge: +1
Mercury (II)
Hg2
Charge: +2
Acetate
C2H3O2
Charge: -1
Nitrate
NO3
Charge: -1
Carbonate
CO3
Charge: -2
Hydrogen Carbonate
HCO3
Charge: -1
Dichromate
Cr2O7
Charge: -2
Chromate
Cr2O4
Charge:-2
Oxalate
C2O4
Charge: -2
Peroxide
O2
Charge: -2
Charges on the periodic table
+1,+2,+3 …, -3, -2, -1
Copper Charge
+1, +2
Gold Charge
+1, +3
Silver Charge
+1
Thallium Charge
+1, NOT +3
Cobalt Charge
+2, +3
Iron Charge
+2, +3
Lead Charge
+2, +4
Manganese Charge
+2, +4
Nickel Charge
+2, +3
Bismuth Charge
+3
Chromium Charge
+3
