Structure, Bonding and Properties (copy)

Na

________ has 1 electron in its outer shell Cl has 7 electrons in its outer shell.

Metals

________ lose electrons to become positively charged.

Graphite

________ is made up of layers of carbon arranged in hexagons.

Ionic bonding

________ occurs between a metal and a non- metal.

Dot

________ and cross diagrams are useful to show the bonding in simple molecules.

Ionic compounds

________ are solid at room temperature because they are arranged in a giant lattice structure that is held together with strong electrostatic attraction.

Solid ionic compounds

________ can not conduct electricity unless they are molten or dissolved in water.

Stick diagrams

________ are easy to draw however they dont show any electrons or the shape of the atoms.

carbon atom

Each ________ is bonded to four other carbon atoms making a diamond very hard.

Covalent

________ bonding occurs between non- metals only, the atoms share a pair of electrons so they can both have a full outer shell.

Ionic compounds form structures

________ called giant lattices.

Silicon dioxide

________ has a similar structure to diamond- there are four bonds for each silicon atom and 2 bonds for each oxygen has a high melting and boiling point.

Ionic compounds

________ are brittle (they shatter break when they are hit)

Na

________ loses one electron, and Cl gains one electron.

Cl forms a Cl

ion

Silicon dioxide has a similar structure to diamond

there are four bonds for each silicon atom and 2 bonds for each oxygen has a high melting and boiling point