Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| An acid with an anion that ends in -ide |
|
Definition
| Hyrdo__ic acid (ex: HCl= hydrochloric acid)\ |
|
|
Term
| An acid with an anion that ends in -ite |
|
Definition
| ___ous acid (ex: HNO2=nitrous acid)\ |
|
|
Term
| An acid with an anion that ends in -ate |
|
Definition
| ____ic acid (HC2H3O2=acetic acid)\ |
|
|
Term
|
Definition
| Salts with the alkali metals and ammonium are soluble\ |
|
|
Term
|
Definition
| Most chloride, bromide, and iodide salts are soluble except when they contain Ag+, Pb+2, and Hg2 +2.\ |
|
|
Term
|
Definition
| Most sulfate salts are soluble except for BaSO4, PbSO4, HgSO4, and CaSO4.\ |
|
|
Term
| When zero is and isn't a sig fig |
|
Definition
| Yes when it is in the middle of a number, no when it's at the beginning of a number, and sometimes when at the end of a number (only with a decimal place or in scientific notation)\ |
|
|
Term
| Sig Figs in multiplication and division |
|
Definition
| The final answer must have as many sig figs as the number with the lowest amount of sig figs that is not an exact number or conversion\ |
|
|
Term
|
Definition
| The final answer goes as many digits as the number with the least digits place.\ |
|
|
Term
|
Definition
|
|
Term
|
Definition
| How much the product the reactants actually form\ |
|
|
Term
|
Definition
| The amount of product that should be created according to stoichiometry.\ |
|
|
Term
|
Definition
| actual yield divided by theoretical yield\ |
|
|
Term
|
Definition
| the simplest whole number ratio of atoms in a compound\ |
|
|
Term
|
Definition
| the exact formula of a molecule, giving the types of atoms and the numbers of each type.\ |
|
|
Term
| The five classifications of reactions |
|
Definition
| Single replacement, double replacement, combination, decomposition, and combustion.\ |
|
|
Term
|
Definition
| With a metal, it makes an ionic compound. If there's carbon, it makes carbon dioxide. If there's hydrogen, it makes water.\ |
|
|
Term
|
Definition
| A double replacement where a cation falls in love with an anion.\ |
|
|
Term
|
Definition
|
|
Term
|
Definition
| HCl (Hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), H2SO4 (sulfuric acid), H2NO3 (nitric acid), HClO4 (perchloric acid), HClO3 (chloric acid)\ |
|
|
Term
|
Definition
| Less electrons oxidized, greater electrons reduced\ |
|
|
Term
|
Definition
| H is +/-1, O is -2 except when bonded with F, a pure element is 0, sum of all the oxidation sates of a polyatomic ion is equal to the total charge\ |
|
|
Term
|
Definition
| a compound that produces OH- when dissolved in water. It's strong when with Group 1 or lower Group 2 metals\ |
|
|
Term
|
Definition
| ions not charged in the reaction\ |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
R=0.0821 L*atm/mol*K
or 8.31 L*kPa/mol*K\
or 62.4 L*torr/mol*K |
|
|
Term
|
Definition
|
|
Term
|
Definition
| The ideal and combined gas laws go under this.\ |
|
|
Term
| Assumptions of kinetic theory |
|
Definition
| Gas particles are much smaller than the space between them so their volume is negligible, and gas particles are neither attracted nor repelled to one another.\ |
|
|
Term
|
Definition
| Ions are non-ideal, very polar molecules are somewhat non-ideal, and nonpolar molecules are the most ideal. Large molecules are more non-ideal and smaller particles (like noble gases) are more ideal\ |
|
|
Term
|
Definition
| if particles are attracted to each other, volume smaller than expected. If particles too close together, their mass not negligible, V bigger than expected.\ |
|
|
Term
| If a compound has a larger molar mass, it will effuse out... |
|
Definition
|
|
