Ionic Bonding and Ionic compounds ( and metallic bonding)

what is an ion?

a charged particle formed by the gain or loss of electrons

all metals ____ electrons to become _____ly charged ions

lose, positive

all non metals ____ electrons to become ____ly charged ions

gain, negative

what is ionic bonding?

transfer of electrons from a metal to a non metal to form a positively charged metal ion and a negatively charged non metal ion

what holds ionic compounds together?

the positive and negative charges are held together by the strong electrostatic forces of attraction that act in all directions

what are the structures of ionic compounds?

they are composed of 100s of ions both positive and negative, held together by strong electrostatic forces, this forms 3D structures called a giant lattice structure

how can ionic compounds be represented?

using a ball and stick diagram

what are the properties of ionic compounds?

- can only conduct electricity when melted or dissolved in water as the ions are free to move/ flow and are no longer fixed

- very high melting point as lots of energy is needed to break the many strong bonds

how does metallic bonding work?

each metal atom donates its outer electron to become a positively charged ion and these electrons are free to move creating a sea of electrons. The metallic bond is the electrostatic force of attraction between these positive metal ions and the negative electrons. This holds the metal together in a regular lattice structure

what are alloys?

a mixture of two or more elements containing at least one metal

why are alloys stronger than regular metals?

the different sized atoms disrupt the regular structure so the layers can no longer slide over each other so it’s stronger

why do metals with a greater number of outer electrons have a higher melting point?

This is due to the increased positive charge on the metal ion and the increased number of electrons that are delocalised, resulting in stronger bonding.

how do metals conduct electricity

their outer electrons of each metal atom are delocalised so they are free to flow within the structure and carry charge