Bonding And Structure

Front 1

Melting and boiling point of giant ionic structures

Back 1

-high melting and boiling point

-it has a giant ionic structure hence a large amount of energy is needed to overcome the strong electrostatic forces of attraction between oppositely charged ions in the giant ionic lattice structure

Front 2

Hardness of giant ionic structures

Back 2

-hard and brittle

Front 3

Conductivity of giant ionic structures

Back 3

-unable to conduct electricity in solid state

- able to conduct electricity in molten and aqueous state

-it has a giant ionic structure. In solid state, the oppositely charged ions can only vibrate about their fixed positions due to strong electrostatic forces of attraction, therefore ions are not mobile to conduct electricity

-in the aqueous/molten state, the electrostatic forces between oppositely charged ions are weakened. Hence, ions become mobile and can conduct electricity

Front 4

Solubility of giant ionic structure

Back 4

- most ionic compounds are soluble in water except silver chloride (Ag+ and Cl-) and barium sulfate (Ba2+ and SO4 2-)

-usually insoluble in organic solvents like ethanol, petrol and turpentine

Front 5

Why does sodium chloride have a lower melting point than magnesium oxide? (NaCl and MgO)

Back 5

Mg2+ has a higher ionic charge than Na+. O2- has a higher ionic charge than Cl-. More energy is needed to overcome the stronger electrostatic forces of attraction between oppositely charged ions of Mg2+ and O2-, therefore MgO has stronger ionic bonds and thus has a higher melting point than NaCl

Front 6

Melting and boiling point of SIMPLE covalent structure

Back 6

- Low melting and boiling point

- It has simple covalent structure. Little energy is needed to overcome the weak intermolecular forces of attraction between simple discrete molecules

Front 7

Conductivity of SIMPLE covalent structures

Back 7

-Unable to conduct electricity in any state with the exception of ammonia, hydrogen chloride, sulfur dioxide

-it has a simple covalent structure. The molecules are electrically neutral so there are no mobile ions or electrons to conduct electricity

Front 8

Solubility of SIMPLE covalent structure

Back 8

- most simple covalent substances are insoluble in water except hydrogen chloride and ammonia

- usually soluble in organic solvents like ethanol, petrol and turpentine

Front 9

Melting and boiling point of diamond

Back 9

-high melting and boiling point

-It has a giant covalent structure. Each carbon atom is covalently bonded to 4 other carbon atoms in a giant covalent network. These strong covalent bonds require large amount of energy to overcome.

Front 10

Conductivity of diamond

Back 10

-diamond is unable to conduct electricity

-it has a giant covalent structure. Each carbon atom uses up all 4 of its valence electrons to form a covalent bonds with 4 other carbon atoms to form a giant covalent network. It does not have any mobile electrons to conduct electricity

Front 11

Hardness of diamond

Back 11

-diamond is a very hard natural substance. Used as a cutting tool/ drill bit to cut hard objects such as glass and rocks

-It has a giant covalent structure. Each carbon atom is covalently bonded to 4 other carbon atoms in a giant covalent network. These strong covalent bonds require large amounts of energy to overcome

Front 12

Melting and boiling point of graphite

Back 12

-It has a high melting hand boiling point

-It has a giant covalent structure. Each carbon atom is covalently bonded to 3 other carbon atoms in a giant covalent network. These strong covalent bonds require large amounts of energy to overcome.

Front 13

Conductivity of graphite

Back 13

-graphite is able to conduct electricity. Used as electrodes during electrolysis

-It has a giant covalent structure. Each carbon atom uses 3 out of 4 of its VALENCE ELECTRONS to form covalent bonds with 3 other carbon atoms to form a giant covalent network. Hence each carbon atom has one delocalised mobile valence electron that is able to conduct electricity

Front 14

Hardness of graphite

Back 14

-graphite is soft and slippery. Used as a lubricant and in pencil lead.

-it has a giant covalent structure. Each carbon atom is covalently bonded to 3 other carbon atoms in a giant covalent network. Graphite is soft and slippery because the layers of carbon atoms are held by weak intermolecular forces of attraction and can slide over each other easily.

Front 15

Metallic bond

Back 15

-strong electrostatic force of attraction between the metallic cations and the sea of delocalised electrons

Front 16

Melting and boiling point of giant metallic structures

Back 16

-generally high melting and boiling points with the exception of group 1 metals

-it has a giant metallic structure. A lot of energy is needed to overcome the strong electrostatic forces of attraction between the metallic cations and the sea of delocalised electrons

Front 17

Conductivity of giant metallic structure

Back 17

- able to conduct electricity

-It has a giant metallic structure. Metals are held together by strong electrostatic forces of attraction between the metallic cations and sea of delocalised electrons. The sea of delocalised electrons are Mobile and therefore metals can conduct electricity

Front 18

Hardness of giant metallic structure

Back 18

-pure metals are malleable and ductile. Alloys are harder and stronger then pure metals.

-the orderly layers of the same sized atoms can slide easily over each other without disrupting the structure. Alloys consists of atoms of different sizes. This disrupts the orderly arrangement of atoms and therefore the layers of atoms cannot slide past each other easily when a force is applied

Front 19

Hardness of giant metallic structure

Back 19

-pure metals are malleable and ductile. Alloys are harder and stronger then pure metals.

-the orderly layers of the same sized atoms can slide easily over each other without disrupting the structure. Alloys consists of atoms of different sizes. This disrupts the orderly arrangement of atoms and therefore the layers of atoms cannot slide past each other easily when a force is applied

Front 20

Solubility of giant metallic structures

Back 20

- insoluble in water with the exception of group 1 metals