Ionic and Covalent compounds Flashcards
Ion Definition
Metal atoms lose electrons to form positively charged ions.
Non metal atoms gain electrons to form negatively charged ions.
Cations
Positively charged ions
Anions
Negatively charged ions
Ionic bonds
Transferring electrons between metals and non metals to fill outer shells.
Ions in a ionic solid compound
Ions in a ionic solid compound are arranged in a regular, repeating arrangement. The regular pattern is formed with because oppositely charged ions attract.
Properties of ionic compounds
High melting and boiling points, conduct electricity (If it contains charged particles)
Polyatomic ions
Groups of atoms Cations - Ammonium, NH4+ Calcium, Ca2+ Sodium, Na+ Lead, Pb2+
Anions - Hydroxide OH- Nitrate, NO3- Carbonate Co3(2-) Sulfate SO4(2-)
The name of an ionic compound dependencies
If it contains 2 elements it ends in ide
If it contains 3 or more elements it ends in ate.
Covalent bonds
Sharing of electrons between atoms. eg: Silica (main compound in sand, joined together by covalent bonds in a regular arrangement)
Giant covalent structures
High melting + Boiling points, Most have no overall charge and cannot conduct electricity. They are also soluable in water.
Diamond and graphite properties
Diamond - Giant covalent substance. Each carbon atom is joined to four other carbon atoms. Carbon atoms form a tetrahedral network structure. There are no free electrons.
Graphite - each carbon atom is joined to 3 other carbon atoms by covalent bonds. The carbon atoms form a hexagonal layered network structure. They layers have weak forces between them and can slide over eachother. Each carbon atom has one un bonded outer electron.
Very large molecules
Graphene is another form of carbon. Its structure resembles a single layer of graphite. It has a high melting point and is very strong.
Fullerenes - A molecular form of the element carbon. Two examples of fullerenes are nanotubes and buckyballs.
