Ionic Compounds Chapter 3

This set of flashcards covers the fundamental properties, naming conventions, structural characteristics, and common examples of ionic compounds and metals as presented in Chapter 3.

Law of Definite Proportions

A ground rule for compounds stating they have a consistent composition and whole number ratios.

Law of Multiple Proportions

A rule describing different molecules that are composed of the same elements.

Crystal lattice

The structural arrangement of ionic compounds, such as Halite ($NaCl$) or Fluorite ($CaF_2$).

Electrolytes

Aqueous ions that conduct electricity, formed when ionic compounds dissolve in water.

Neutral charge formula

The principle that the sum of the total positive charge and total negative charge in an ionic compound must equal $0$.

Cation

A positive ion typically formed by elements with a weak nuclear attraction for valence electrons.

Anion

A negative ion typically formed by elements with a strong nuclear attraction for valence electrons.

Metallic Bond

A type of chemical bond consisting of cations floating in a sea of electrons where electrons flow freely.

Native metal

A metal found in its pure state in nature.

Metal ore

Naturally occurring compounds from which metals are extracted.

Alloys

Man-made solutions of metals.

Brass

An alloy composed of Copper and Zinc.

Steel

An alloy composed of Iron and Carbon.

White gold

An alloy composed of Nickel, Palladium, Platinum, and Manganese.

Sodium chloride ($NaCl$)

An ionic compound commonly used as table salt.

Sodium bicarbonate ($NaHCO_3$)

An ionic compound commonly known as baking soda.

Sodium hydroxide ($NaOH$)

An ionic compound known as lye or drain cleaner.

Magnesium sulfate ($MgSO_4$)

An ionic compound commonly known as Epsom salt.

Sodium hypochlorite ($NaOCl$)

An ionic compound commonly used as bleach.

Polyatomic ions

Molecules that can form ions, such as Sulfate, Carbonate, Nitrate, and Phosphate.