Chemistry - Introduction 1

• Very reactive, especially near water

• Malleable, ductile, and good conductors

• One Valence electron

• Typically extracted from compounds

What are the properties of alkali metals (1A)?

• Low electron affiliates and electromagnetism

• Two valence electrons

• Form divalent anions

• Have smaller atomic radii than alkali metals

What are the properties of Alkaline Earth metals (2A)?

• Fairly nonreactive—malleable

• High melting and boiling points

• Good for electrical conductivity

• Low ionization energies and very similar to one another

• Exhibit wide ranges of oxidation states

What are the properties of transition metals?

• High electronegatives

• Highly reactive with alkali and alkaline Earth metals

• Low ionization energies

• Form anions with one (-1) negative charge

What are the properties of Halogens?

• Solid at room temp (except mercury)

• Metalloids have both metal and nonmetal characteristics (brittle solids and gain elections easily)

What are the properties of metals, metalloids, gases, and nonmetals?

• Sliver-white metals

• Tarnish when exposed to air

• High melting and boiling points

• Highly reactive

• Strong reducing agents

What are the properties of lanthanides?

• Radioactive

• Highly electropositive

• Dense metals with distinctive structure

• Combine directly with most nonmetals

What are the properties of Actinides?

• Fairly nonreactive!

• Complete valence shell (8 electrons; depends on size of atom)

• Very low electronegatives

• Low boiling points

• gases at room temp.

What are the properties of noble gases?

Ion

An atom/molecule with a net electrical charge

• Created by the loss or gain of one or more electrons, resulting in an imbalance.

Cation

The loss of electrons in an ion

Anion

The gain of electrons in an ion

Net Electrical Charge

The total and overall change of an object or system

• The sum of all protons and electron changes

Ionization

The process of gaining or losing electrons to create a net electric charge

Electronegativity

An atom’s ability to attract electrons in a chemical bond

• Fluorine is the most electronegative element

Valence Electron

The atom’s outermost shell

• Responsible for chemical bonding and determining an element’s reactivity

• Influences the electronegativity and the type of bond formed (Ionic or covalent)

divalent anions

Ngeativiely charged ions that carry and -2 charge

• Gained two extra electrons (also called bivalent anions

• EX: Sulfate (SO) and Carbonate (CO)

oxidation states

The hypothetical charge an atom would have if all bonds were 100% Ionic, indicating electron loss (+state) or gain (-state)

• Oxidation number