Unit 7 - Ionic Compounds

WOMENS HISTORY MONTH

Cations

Elements that lose electrons form positive (+) ions

cations

Transition metals tend to form ___, but are difficult to predict because of d and f orbitals

Anions

Elements that gain electrons form negative (-) ions

releases; requires/absorbs

When an atom picks up an electron, it ___ energy; when it releases an electron it ___ energy.

Explanation: Gaining an electron often results in a more stable configuration, releasing energy in the process. Losing an electron, on the other hand, requires energy to overcome the attraction between the electron and the nucleus.

Ionic Bond

Electrostatic force that holds oppositely charged particles together

cations (+); anions (-)

Ionic bonds form when ___ and ___ combine

Ionic Crystal

Regular and repeating patterns formed when Ionic compounds push positive and negative ions together

Monoatomic; valence electrons

___ ions form from a single atom: LI⁺, Ca²⁺, Br^-. Charge is based off ___.

space out

Positive and negative ions ___ to reduce repulsive forces

Oxidation Number

The charge of the ion

oxygen

Oxidation number is a reference to ___

Roman Numerals

Use ___ in the name of transition metals to represent its charge

Polyatomic Ions

ions made up of more than one atom

entire group

Charge of the polyatomic ion applies to the ___ of atoms.

crystal lattices

Ions are arranged in large ___.

Crystal Lattice

Formula Unit

Simplest ratio to represent Ionic compounds

zero

Positive and negatives charges must add up to net charge ___.

Chemical Nomenclature

Rules for naming compounds

first

Cations are named ___.

original element name

Cations use their ___

roots; -ide

Anions use ___ of the anion name plus ___ suffix.

roman numerals; oxidation numbers

Transition metals use ___ to define their oxidation numbers because they have can multiple ___.

crystal lattices

Strong attraction of ions results in 3D geometric arrangements of particles called ___.

strong; high melting, high boiling points, and significant hardness

Crystal lattices create ___ bonds in ionic compounds. They have ___ properties.

Endothermic

Reactions that absorb energy and make the temperature go down.

Exothermic

Reactions that release energy and make the temperature go up.

exothermic

Energy of Ionic compounds will always be ___.

Lattice Energy

Energy needed to separate ions of an Ionic compound

similar

Metals form bonds ___ to Ionic bonds

sea of electrons; valence electrons; act; cations

Metals create a ___ where they contribute their ___, and that bond makes those metals atoms ___ like ___.

delocalized electrons

Valence electrons that are in the “sea of electrons”, or electrons that are free to move.

Metallic bond

The attraction of a metallic cation for delocalized electrons.

melting points; boiling points; seperate

High ___ of metals can be explained by: atoms are easily able to slide past each other, but even higher ___ because they are hard to ___.

malleable; ductile

Metals are ___ and ___ because their atoms can be easily pushed and pulled around

conductors; delocalized electrons

Metals are excellent ___ because ___ can move heat around from place to place easily.

high; d-orbitals

Transition metals have ___ conductivity (better than normal metals) because of their loose ___.

Alloy

A mixture of elements that have metallic properties

Mixture

A material made up of two or more different chemical substances which can be separated by physical method

Sea of electrons surrounding lattice of positively charged metal ions, valence electrons in metals are delocalized and able to move throughout the crystal lattice structure

What do metallic bonds look like?

High electrical & thermal conductivity, malleability & ductility, high melting & boiling points, strong & hard

List some properties of metals that are due to the way metallic bonds form.