1 / 10

Ionic bond

This overview on ionic bonds explains essential concepts such as ions, oxidation numbers, and the formation of ionic compounds. An ion is defined as an atom that has gained or lost electrons, leading to the formation of cations (positive ions) and anions (negative ions). It discusses the properties of ionic bonds formed between metals and nonmetals, their high melting and boiling points, and solubility in water. The guide includes steps for writing ionic compound formulas, naming compounds, and distinguishing between monoatomic and polyatomic ions.

samuru
Télécharger la présentation

Ionic bond

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Ionic bond Pg. 53

  2. Ions • An ion is an element that has gained or lost electrons • Oxidation numbers are used to show the charge of an ion. • A positive ion is called a cation • A negative ion is called an anion

  3. Writing ions • Write the element symbol first • As a superscript, write the oxidation number • Ex. Ba2+ or Ba+2

  4. Ionic Bonds • Force that holds oppositely charged ions together is called an ionic bond • Between a metal and a nonmetal • Electrons are lost or gained • High melting and boiling points • Can dissolve in water to produce electrolytes (produces an electric current) • Example: NaCl

  5. Writing Ionic compound formulas • Lowest ratio called a formula unit • First write the ions with their oxidation numbers • The charges on each elements switch and become the subscripts on the other element • Take just the numbers, NOT THE CHARGES • Simplify • Examples: • Na and Cl • Mg and F • K and P • Be and O

  6. Lewis Dot diagrams • Na and Cl • Mg and F • K and P • Be and O

  7. Naming Ionic compounds • The cation is written as normal • The anion drops the last part of the element and add –ide • Example: Sodium + Chlorine = Sodium Chloride

  8. Polyatomic ions • Ions made up of more than one element • Charge applies to the entire ion • Written in parenthesis in ionic formulas • Ex. Mg(OH)2

  9. Ionic formulas with transition metals • Transition metals can have multiple oxidation numbers • When writing the name, the charge of the transition metal must go in parenthesis using Roman numerals • Ex. Iron (III) oxide • Cu3P2 • MnO

More Related