ionic compounds

atoms

• basic building block of all matter in the universe

elements

• a pure substance (cannot be broken down) and is made of one type of atom

arrangement of elements

1. monoatomic

2. molecules

3. lattices

monoatomic

• unbonded single atoms

• noble gases

compounds

• 2 or more DIFFERENT elements chemically bonded together

  • e.g. molecules: non-metallic elements

    • H₂O, CO₂

  • lattices: metallic + non-metallic elements

  • ionic compounds: metal transfer electrons to non-metals

molecule

• a cluster or group of atoms joined together

  • either element / compound

    • e.g. molecule when one element: Cl₂

    • molecule when compound: CO₂

lattice

• an array of atoms (same or different) bonded together

  • e.g. metallic lattice: Na

  • metal + non-metal: NaCl

mixture

• 2 or more pure substances (element or compound) combined without reacting chemically

subatomic particles

• protons → positive charge → weight: 1 atomic mass unit

• neutrons → no charge → 1 atomic mass unit

• electrons → negative charge → 1/1840 atomic mass unit

atomic number

• number of protons

mass number

• number of protons AND neutrons

  • therefore–

  • number of neutrons = mass number - atomic number

electron shells

• where electrons orbit the nucleus

valence electron

• electrons in the outermost energy shell

isotope

• atoms of the same element with the same number of protons but different numbers of neutrons in the nuclei

  • same atomic number, different mass number

chemical property

• isotopes have the same chemical property → chemical property is dependent on the number of electrons

ions

• a charged atom that has either gained or lost an electron

cation

• lose electrons → positive charge

anion

• gain electrons → negative charge

groups in periodic tables

• direction: ↓

  • represents valence electrons

periods in periodic tables

• direction: →

  • represents number of electron shells

polyatomic ion

• group of two or more ions bound together by covalent bonds

  • multiple ions joined together that have an overall charge

ionic compounds

• compounds bound together by ionic bonds

  • ionic bond = chemical link formed through electrostatic attraction

    • contain metal ion (cation) that is chemically combined with a non-metal

    • e.g. NaCl

characteristics of ionic compounds

1. brittle

2. conducting electricity

3. hard

4. high melting and boiling points

why are they attracted to each other?

• wants a full outer shell

  • stable state, lowest energy

• oppositely charged ions are attracted to teach other

• involves electrostatic reaction

  • transfer of electrons

solubility

• maximum amount of solute that can dissolve in a solvent

soluble

• substance that can dissolve into a liquid

solute

• substance that dissolves

solvent

• substance that dissolves another substance

solution

• uniform mixture of two substances

  • the mixture you get after the solute dissolves

equation

• solute + solvent → solution

precipitation

• solid produced in a reaction

  • two soluble (aq) ionic compounds mix to form an insoluble solid (precipitate)

atomic radius

• distance between the nucleus and the valence electron shell

when atomic radius increases, reactivity…

increases

• large atomic radius → easier to lose electrons