Term
| Law of definite proportion |
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Definition
| compounds have a constant composition |
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Term
| Law of multiple proportions |
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Definition
| When two elements form a series of compounds, the rations of the masses of the seond element that combine with 1 gram of the first element can always be reduced to small whole numbers |
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Term
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Definition
- Each element is made up of tiny particles called atoms
- The atoms of a given element are identical
- Chemical compounds are formed whtn atoms combine with each other
- Chemical reactions involve reorganization of the atoms, or changes in the way they are bound together
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Definition
| A ray produced at teh negative electrode and repelled by the negative pole of an applied electric field; ray is a stream of negatively charged particals called electrons. |
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Definition
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| an atom with a dense center of positve charge (the nucleus) and electrons moving around the nucleus. |
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Definition
| the forces that hold atoms together |
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| A bond shared between atoms by sharing electrons. |
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| a bonded collection of two or more atoms of the same or different elements. |
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Definition
| the representation of a moleucle in which the symbols for the element are used to indicate the types of atoms present and subscripts are used to show the relative numbers of atoms |
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Definition
| the representation of a molecule in which the relative positions of the atoms are shown and the bonds are indicated by lines |
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Definition
| an atom or group of atoms that has a net positive or negative charge |
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Definition
| Members of Group 1A, on the periodic table. Are very active elements that readily form ions with a 1+ charge when they react with nonmentals. |
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Definition
| Members of Group 2A, on the periodic table. Form ions with a 2+ charge when they react with nonmetals. |
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Definition
| Members of Group 7A, on the periodic table. Form diatomic molecules |
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Definition
| In group 8A, on the periodic table. Exist under normal conditions as monatomic (single-atom) gases and have little chemical reactivity. |
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Term
| Binary ionic compounds (Type I) |
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Definition
| Contain a positive ion, always written first in the formula, and a negative ion. Cation keeps it's elemental name; whereas the anion ends with -ide. |
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Term
| Binary Compounds (Type II) |
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Definition
Contain a metal that can form more than one type of cation. The charge on the metal ion must be specified. The ion with the higher charge has a name ending in -ic, and the one with the lower charge has a name ending in -ous.
Fe^3+ iorn (III) or ferric
Fe^2+ iorn (II) ferrous |
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Term
| Ionic Compounds with Polyatomic ions |
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Definition
| Polyatomic ions are assigned special names that must be memorized. |
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Term
| Binary Compounds (Type III) |
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Definition
Formed between two nonmetals.
- The first element in the formula is named first
- The second element is named as if it were an anion
- Prefixes are used to denote the numbers of atoms present
- The prefix mono- is never used for the first element
ex: N_2O dinitrogen monoxide
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Term
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Definition
If the anion does not contain oxygen, the acid is named with the prefix hydro- and the suffix -ic.
ex: HF hydrofluoric acid |
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Term
| Naming acids containing oxygen |
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Definition
when the anion contains oxygen, the acid name is formed from the name of the anion with a suffix of -ic or -ous. If the anion name ends in -ate, then the acid name ends with -ic (e.g. HNO_3 nitric acid).
If the anion name ends in -ite, then the acid name ends in -ous (e.g. H_3PO_4 phosphoric acid). |
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Term
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Definition
| the weighted average mass of the atoms in a naturally occuring element |
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Term
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Definition
a sample of a natural element with a mass equal tot he element's atomic mass expressed in grams contains 1 mole of atoms.
ex: 6.022 x 10^23 atoms of Al = 26.98 grams |
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Term
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Definition
6.022 x 10^23
Counting number |
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Term
| molar mass / molecular weight |
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Definition
| the mass in grams of 1 mole of a compound |
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Term
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Definition
C2H5OH
Mass of C = 2 mol x 12.011 g/mol = 24.022 g
Mass of H = 5 mol x 1.008 g/mol = 6.048 g
etc.
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Term
| Solving a Stoichiometry Problem involving Masses of Reactants and Products |
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Definition
- Write and balance the equation
- Convert the known masses of substances to moles
- By compairing the mole ratio of reactants required by the balanced equation with the mole ratio, determine which reactant is limiting
- Using the amount of the LR and the appropriate mole ratios, compute the number of moles of the desired product
- Convert from moles to grams using the molar mass
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Term
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Definition
| a substance dissolved in a liquid to form a solution |
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| the dissolving medium in a solution |
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| a reaction in whcih an insoluble substance forms and separates from the solution |
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Definition
| a material that dissolves in water to give a solution that conducts an electric current |
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Definition
| the tendency of an atom in a molecule to attract shared electrons to itself |
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Definition
| measured in terms of the mass (grams) of solute that dissolve in a given volume of solution. |
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Term
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Definition
| M = Molarity = (mol of solute / L of solution) |
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Term
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Definition
| the process of adding water to acheive the molarity desired. |
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Term
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Definition
- soluble salt
- strong acids
- strong bases
Completely dissociates into ions
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Term
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Definition
| Weak acids and weak bases. Dissociates only to a slight extent in aqueous solutions. |
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Term
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Definition
| provide a way to keep track of electons in oxidation-reduction reactions |
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Definition
| an increase in oxidation state (loss of electrons) |
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Term
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Definition
| a decrease in oxidation state (gain of electrons). |
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