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36 Cards in this Set
- Front
- Back
Chemical Bonds:
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result of interactions between the charged particles-- electrons and protons--- that compose atoms.
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Ionic bonds:
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occur between metals and nonmentals-- involve the transfer of e-s from one atom to another
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The formation of an ionic compound:
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Covalent bonds:
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occur between two or more nonmetals-- involve the sharing of e-s between two atoms.
- the shared electrons interact with the nuclei of both atoms, lowering their potential energy through electrostatic interactions with the nuclei. |
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Chemical formula:
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- indicates the elements present in the compound and the relative # of atoms or ions of each.
- the formula contains the symbol for each element and a subscript indicating the relative # of atoms of the element. - normally list the more metallic (or more (+) charged) elements first, followed by the less metallic (or more (-) charged) element. |
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Empirical Formula:
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simply gives the relative # of atoms of each element in a compound
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Molecular formula:
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gives the actual # of atoms of each element in a molecule of a compound
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Structural Formula:
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uses lines to represent the covalent bonds, shows how atoms in a molecule are connected or bonded to each other.
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Molecular models:
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table representing molecular models of Benzene, Acetylene, Glucose, and Ammonia:
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atomic elements:
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those that exist in nature with single atoms as their basic units.
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A molecular view of elements and compounds:
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Molecular Elements:
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do not normally exist in nature with single atoms as their basic units. Instead, exist as molecules, two or more atoms of the element bonded together.
- most exists as diatomic molecules - a few exists as polyatomic molecules. |
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Molecular compounds:
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usually composed of two or more covalently bonded nonmetals.
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Ionic compounds:
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composed of cations and anions bound together by ionic bonds
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formula unit:
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the smallest, electrically neutral collection of ions.
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polyatomic ions:
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an ion composed of two or ore atoms
ex: ClO- |
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summary for writing formulas for ionic compounds:
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- ionic compounds always contain positive and negative ions
- in a chemical formula, the sum of the charges of the positive ions (cations) must always equal the sum of the charges of the negative ions (anions). - the formula reflects the smallest whole-number ratio of ions. |
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Procedure for writing formulas for ionic compounds:
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naming an ionic compound:
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- identify it as an ionic compound (usually formed between nonmetals and metals)
- can be divided into two types depending on the metal in the compound. |
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Binary Compounds:
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are those containing only two different elements
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some common anions:
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naming binary ionic compounds containing a metal that forms more than one kind of cation:
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some metals that form cations with different charges:
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some common polyatomic ions:
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how ionic compounds are named if there are only 2 ions in the series:
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how ionic compounds are named if there are more than two ions in the series:
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hypo =
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less than
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per=
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more than
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hydrate:
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compound containing a specific number of water molecules associated with each formula unit.
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Binary molecular compounds have the following form:
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Acids:
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- molecular compounds that release hydrogen ions (H+) when dissolved in water.
- composed of hydrogen, usually written first in their formula, and one/more nonmetals written second. - are characterized by their sour taste and their ability to dissolve many metals. |
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aqueous (aq) =
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dissolved in water
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Binary acids:
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are composed of hydrogen and a nonmetal.
the names for binary acids have this form. |
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oxyacids:
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contain hydrogen and an oxyanion
- simply a combination of one or more H+ ions with an oxyanion. ex: HNO3 (aq) = nitric acid |
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Formula mass:
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the average mass of a molecule
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