(Chem 200) 03- Molecules, Compounds, And Chemical Equations

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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