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General Chemistry, 5th ed.Whitten, Davis & Peck

Chapter 4 DefinitionsLeft click your mouse to continue.

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DIRECTIONS

• This slide show presentation is designed to function like flash cards.

• To check your answer, and/or to move on to the next slide, simply left click your mouse.

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BASE

• A substance that produces OH- ions in aqueous solution.

• Strong soluble bases are soluble in water and are completely dissociated.

• Weak bases ionize only slightly.

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BINARY ACID

A binary compound in which H is bonded to one of the less metallic

nonmetals.

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BINARY COMPOUND

A compound consisting if two elements; may be ionic or molecular.

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CHEMICAL PERIODICITY

The variation in properties of elements with their positions in the

periodic table.

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COMBUSTION REACTION

A highly exothermic reaction (release heat) of a substance with oxygen,

usually with a visible flame.

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DISPLACEMENT REACTION

A reaction in which one element displaces another from a compound.

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DISPROPORTIONATION REACTION

A redox reaction in which the oxidizing agent and the reducing

agent are the same element.

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DISSOCIATION

In aqueous solution, the process in which a solid ionic compound

separates into its ions.

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ELECTROLYTE

• A substance whose aqueous solutions conduct electricity.

• Remember: ions are charged particles. Movement of charged particles conducts electricity.

• Ionic compounds are electrolytes

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FORMULA UNIT EQUATION

An equation for a chemical reaction in which all formulas are written as

complete formulas.

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GROUP (FAMILY)

• The elements in a vertical column of the periodic table.

• Elements in a group have similar chemical and physical properties

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IONIZATION

In aqueous solutions, the process in which molecular compound separates

to form ions.

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METALLOIDS

• Elements with properties intermediate between metal and nonmetals

• B, Si, Ge, As, Sb, Te, Po, and At

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NET IONIC EQUATION

• An equation that results from canceling spectator ions and eliminating brackets from a total ionic equation

• The net ionic equation for ALL reactions of strong acids with strong soluble bases that form salts and water is H+ + OH- H2O

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NEUTRALIZATION

The reaction of an acid with a base to form a salt.

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NONELECTROLYTE

• A substance whose aqueous solutions do not conduct electricity.

• Molecular compounds are nonelectrolytes

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OXIDATION

• Loss of electrons• Gain oxygen• Loss of hydrogen• An algebraic increase in oxidation number• Remember: electrons are negative, therefore if you

are losing electrons, you oxidation number will change in the positive direction

• If the item is being oxidized, then it serves as the reducing agent

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OXIDATION NUMBERS

Arbitrary numbers that can be used as mechanical aids in writing formulas

and balancing equations

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OXIDATION-REDUCTION REACTION

A reaction in which oxidation and reduction occur; also called redox

reactions

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PERIOD

• The element in a horizontal row of the periodic table

• Elements in a period have properties that change progressively across the table

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PERIODICITY

Regular periodic variations of properties of elements with atomic

number (and position in the periodic table)

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PERIODIC LAW

The properties of the elements are periodic functions of their atomic

numbers.

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PRECIPITATE

An insoluble solid that forms and separates from a solution.

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PSEUDOBINARY IONIC COMPOUND

A compound that contains more than two elements but is named like a

binary compound.

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REDUCTION

• Gain of electrons• Loss of oxygen• Gain of hydrogen• An algebraic decrease in oxidation number• Remember: electrons are negative, so if you are

gaining electrons, the oxidation number will be in the negative direction

• if an item is being reduced, then it serves as the oxidizing agent.

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REVERSIBLE REACTION

A reaction that occurs in both directions; indicated by double

arrows

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SALT

A compound that contains a cation other than H+ and an anion other than

OH- or O-2

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SEMICONDUCTOR

A substance that does not conduct electricity at low temperatures, but

does so at higher temperatures.

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SPECTATOR IONS

• Ions in solution that do not participate in a chemical reaction

• When looking at a total ionic equation, the spectator ions are the ones whose oxidation state does not change

• Are not shown in a net ionic equation

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STRONG ACID

• An acid that ionizes (separates into ions) completely, or very nearly completely, in dilute aqueous solutions

• EX: H2SO4, HNO3, HCl, HClO3, HClO4, HI, HBR

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STRONG ELECTROLYTE

• A substance that conducts electricity well in dilute aqueous solution.

• Three major classes of solutes are strong electrolytes: strong acids, strong soluble bases and most soluble salts

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STRONG SOLUBLE BASE

• Metal hydroxide that is soluble in water and dissociates completely in dilute aqueous solution

• EX: LiOH, NaOH, KOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

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TERNARY ACID

A ternary compound containing H, O, and another element, often a

nonmetal

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TOTAL ION EQUATION

An equation for a chemical reaction written to show the predominant form of all species in aqueous solution or

in contact with water.

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WEAK ACID

• An acid that ionizes only slightly in dilute aqueous solution

• EX: HF, HC2H3O2, HCN, HNO2, H2CO3, H3PO4, H2SO3, (COOH)2

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WEAK BASE

• A molecular substance that ionizes only slightly in water to produce an alkaline (base) solution

• EX: NH3, CH3NH2, C6H5NH2

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WEAK ELECTROLYTE

A substance that conducts electricity poorly in dilute aqueous solution.

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METALS

• Outer shells contain few electrons, usually three or four

• Form cations (positive ions) by losing electrons

• Form ionic compounds with nonmetals

• Solid state characterized by metallic bonding

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NONMETALS

• Outer shells contain four or more electrons• Form anions (negative ions) by gaining

electrons• Form ionic compounds with metals and

molecular (covalent) compounds with other nonmetals

• Covalently bonded molecules; noble gases are monatomic

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METALLIC CHARACTER

Increases from top to bottom and from right to left with respect to

position in the periodic table

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NONMETALLIC CHARACTER

Increases from bottom to top and from left to right in the periodic table

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HALOGENS

• Will displace less active (heavier) halogens from their binary slats

• Order of increasing activity: I2 < Br2< Cl2< F2