AP Chemistry unit 1 Flashcards

10997708865	stoichiometry	the area of study that examines that quantities of substances involved in chemical reactions	0
10997714163	chemical reaction	a process by which one or more substances are converted to other substances	1
10997719173	chemical equations	use chemical formulas to symbolically represent chemical reactions	2
10997753847	balanced chemical equation	has an equal number of atoms of each element on each side of the arrow	3
10997793751	g,l,s,aq	are all symbols used to designate the physical state of each reactant and product	4
10997863834	decomposition reaction	one reactant changes to two or more products	5
10997881369	combustion reaction	involves oxygen, often from air, reacting with hydrocarbons or other organic molecules containing carbon, hydrogen, and oxygen to produce carbon dioxide and water.	6
10997927785	avogadro's number	6.02 X 10^23 of atoms in that element	7
10997937434	a mole	the amount of matter that contains 6.02 X 10^23 atoms, ions, molecules, or formula units	8
10997947705	molar mass	the mass in grams of one mole of that substance. to calculate: add the atomic mass of all the atoms in its formula	9
10997970166	molar road		10
10998021025	percentage composition	the percentage by man contributed by each element in the compound % composition= 100 x (molar mass of element x subscript for element) / (molar mass of substance)	11
10998047747	empirical forumla	expresses the simplest ratio of atoms in the formula. can be calculated from the percentage composition.	12
10998056819	molecular formula	tells exactly how many atoms are in one molecule of the compound	13
10998071957	ionic compounds	often form crystal structures called hydrates by acquiring one or more water molecules per formula unit	14
10998078972	stoichometry	the quantities of substances involved in chemical reactions	15
10998096767	limiting reactant	the reactant that is completely consumed in a chemical reaction. limits the amount of products formed	16
10998103432	excess reactant	some is left unreacted when the limiting reactant is completely consumed	17
10998114345	theoretical yield	the quantity of product that is calculated to form	18
10998119646	actual yield	the amount of product actually obtained and is usually less than the theoretical yield	19
10998126129	percent theoretical yield	related the actual to the theoretical yield percent theoretical yield= (actual yield) / (theoretical yield) x 100	20
10998145546	solution	a homogenous picture of two or more substances	21
10998148553	solvent	the dissolving medium, usually the substance present in the greatest quantity in a solution	22
10998153948	aqueous solution	solutions in which water is the solvent	23
10998164895	solutes	other substances in the solution	24
10998167736	electrolyte	a substance whose aqueous solution contains ions. the solution conducts electricity because the ions are free to migrate throughout the solution	25
10998180219	strong electrolyte	substances that exist in solution, completely ionized. ionic compounds and some molecular compounds called strong acids are strong electrolytes	26
10998194825	strong acids	can react readily with metals	27
10998198566	strong bases	dissociate completely	28
10998204391	weak electrolytes	exist mostly as molecules in solution. molecular compounds called weak acids and weak bases are weak electrolytes.	29
10998218517	ionic compounds	are always strong electrolytes if they're on the chart	30
10998226929	nonelectrolyte	a substance that does not form ions in solution and its solution does not conduct electricity. usually consists of a molecular compound, which when dissolved in water, usually consists of intact, un-ionized molecules.	31
10998255566	precipitate	an insoluble solid formed by a reaction in solution	32
10998292804	complete ionic equation	if the soluble strong electrolytes are shown as ions write it as a complete ionic equation	33
10998413576	spectator ions	ions that appear in identical form among both reactants and products of a complete ionic equation	34
10998455138	net ionic equation	omits spectator ions because they do not change from reactants to products	35
10998468171	the cations and anions that generally DO NOT form precipitates are	ammonium: NH4+ sodium: Na+ potassium: K+ nitrate: NO3-	36
10998485194	general rules for writing net ionic equations	1. write all the reactants that are indicated to be solids, liquids, or gasses 2. rewrite the formulas of the aqueous reactants, omitting the spectator ions (NH4+, Na+, K+, NO3-) 3. predict and write the product 4. if necessary, use ions to balance the mass and charge. then balance using coefficients. check to see if the charges are balanced.	37
10998541012	acids	substances that ionize in quests solution to form H+ ions	38
10998545703	bases	substances that react with H+ ions	39
10998554174	strong acids and strong bases are strong electrolytes	the completely ionize in solutions	40
10998727442	neutralization reaction	water is usually a product. because strong-acids and bases are strong electrolytes, their ions are usually spectator ions in acid-base reactions.	41
10999460821	ionic compounds	containing carbonate, sulfite, or sulfide ions produce gases when they react with acids	42
10999474863	metal carbonates and metal hydrogen carbonates	react with acids to produce carbon dioxide gas and water	43
10999488653	oxidation-reduction reactions	also called redox reactions are reactions that transfer electrons between reactants oxidation: losing negative charge and gaining positive charge reduction: gained negative charge and losing positive charge	44
10999527819	oxidation	is the loss of electrons, becomes more positive	45
10999537503	reduction	the gain of electrons, becomes more negative	46
10999587837	metals	also react with metal ions to exchange electrons	47
10999816431	activity series	a list of metals arranged in order of decreasing ease of oxidation	48
10999854984	oxidation state	also called oxidation number. A positive or negative whole number assigned to an element in a chemical formula based on set formal rules. used to track electron transfer in redox reactions.	49
10999914183	a solution	a homogeneous mixture consisting of a solvent and one or more solutes	50
10999927090	concentration	the amount solute dissolved in a given amount of solvent or solution	51
10999943552	molar concentration	also called molarity. the number of moles of solute dissolved in a liter of solution molarity= moles of solute/volume of solution in liters	52
10999993497	dilution	adding water to a solution decreases the molar concentration of each substance in the solution by a factor called the dilution factor. a ratio of the original volume to the new volume old volume/new volume	53
11000115769	solution stoichiometry	involved calculations that relate moles of reactants and products to the volumes of solutions of their molar concentrations.	54
11000150253	titration	an analytical technique used to determine the unknown concentration of a solution by reacting it with a solution of known concentration called a standard solution. Equivalence point of the titration is the only point at which the moles of a substance dissolved in the unknown solution completely react with the moles of a substance in the standard solution.	55