Chapter 6 Ionic Compounds

How to name Tenary compounds?

- A group of atoms that as a group have a charge Ex: Po4 3- -> phosphate

False statements

- A positively charged ion is called an anion - Elements tend to react so they acquire the electron structure of a halogen - A Cl- ion is an example of a cation - Nonmetals form a stable outer electron configuration by losing electrons and becoming anions - Binary ionic compounds are generally composed of a metal and a polyatomic ion - If a compound is soluble in water, then it is always anionic compound - Elements tend to react so they acquire the electron structure of a halogen

True statements

- Elements in Group 1 lose one valance electron, forming an ion with a 1+ charge - A sodium atom tends to lose one electron when it reacts - The ending -ide is used to designate an anion - The unpaired valence electrons are those involved in bonding

How to name binary compounds?

- Name cation 1st - Anion must end with -ide

Isoelectronic

2 atoms or ions with the same number of electrons; ions with the same electron configuration as noble gas atoms

Lewis electron dot structure

A diagram for a chemical substance in which each element is represented by its symbol and each valance electron is represented by a single dot

Ionic bond

A force that holds together that are oppositely charged (metal loses and nonmetal gains/ complete transfer ) The resulting attraction between the positively charged cations and negatively charged anions - After the exchange of electrons, they bond together - One is positive because it just lost the electron and the other one is negative because it just gain its electron

Anion

A negatively charged ion (gains electron)

Cation

A positively charged ion (loses electron)

Define polar covalent bond

Bonding electrons SHARED unequally between two atoms. (partial charges on atoms)

Noble gases are unreactive because...

Due to the octet rule - Exception: 1st row elements are stable

Define nonpolar covalent bond

Electrons shared qually between two atoms (no charges on atoms)

How to name transition metals?

FeCl3 -> 3 iron = Iron III chloride

When electronegativities of two bonded atoms differ greatly, the bond is

Ionic - The less reactive (low valance) element gives up 1 or more electrons to another atom to create a stable compounds

What are hydrates?

Ionic compounds with water molecules attached - Heat or putting stronger compounds to get rid of H2O Prefix: Mono, di- ,tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-

Binary compounds

Made up of 2 different elements

Tenary ionic compounds

Made up of 3 or more (polyatomic ion) elements

Metals and non metals properties to become stable

Metal: loses electrons Non-metal: gains electrons

Formula unit

Smallest collection of atoms from which the formula of a compound can be established (ionic compound) (NaCl)

Octet rule

States that elements tend to form compounds in ways that give each atom 8 valance electrons (share or transfers V.E.)

Describe the general properties of ionic compounds

Structure: Solids/ Crystal at room temp & brittle Melting points: Generally high Boiling points: Generally high Electrical conductivity: Excellent conductors (electrolyte) & conducts them in molten state Solubility: Soluble - Crystal lattice is created due to minimzing repulsion between negative and positive ions

What holds ionic compounds together?

The electrostatic attraction between the + & - ions - It forms a crustal lattice structure

Chemical bond

The force that holds two atoms together

Empirical formula

The ionic formula of a compound that shows the ratio of elements present in the compound but not the actual #s of atoms found in the molecule - The smallest/ lowest whole # ratio of elements in the compound

Dissolution

When a solute in a solvent forms a solution - A process in which a solid substance becomes dissolved in a given solvent (transfer of solute from the solid surface to the liquid phase) - Ionic compounds would go through dissolution to show conductivity in the water - occurs when water interacts with the ions in the crystal lattice, causing the lattice to break apart