Bonding, structure and properties of matter

Question 1

Ions are

Answer 1

charged particles - they can be single atoms of group. They are made when electrons are transferred.

Question 2

When metals

Answer 2

form ions , they lose electron from outer shell to form positive ions

Question 3

When non-metals ion

Answer 3

they gain electrons to form negative ions.

Question 4

Group 1 and 2 elements

Answer 4

lose electrons to form positive

Question 5

Group 6 and 7 elements

Answer 5

gain electrons to form negative

Question 6

ionic bonding

Answer 6

non-metal + metal when ions are oppositely charged ions and strongly attracted to each other by electrostatic forces

Question 7

ionic compounds

Answer 7

have a regular lattice structure and giant ionic lattice.

Question 8

with ionic compounds

Answer 8

the ions form a closely packed regular lattice arrangement and very strong electrostatic forces of attraction between oppositely charged ions .

Question 9

A single crystal of sodium chloride

Answer 9

is one giant ionic lattice .

Question 10

Ionic compounds have similar properties

Answer 10

They all have high melting points and boiling points. When solid - ions are in place so they cants conduct electricity . When melted the ions are free to move and carry an electric charge .

Question 11

Covalent bonding

Answer 11

non- metal bonds together and share pairs of electrons. Positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces making bond strong

Question 12

Simple molecular substances

Answer 12

are made up of molecules containing a few atoms joined together by covalent bonds

Question 13

Examples of simple molecule substances

Answer 13

Hydrogen - 1 electron
Oxygen - need 2 electron for full outer shell
Methane - can form four covalent bonds with hydrogen atoms to fill its outer shell

Question 14

Properties of simple molecular substances

Answer 14

To melt of boil you need to break the feeble intermolecular forces and not the covalent bond . As molecules get bigger the strength of the forces increase. Melting point and boiling points are very low . Molecular compounds don’t conduct electricity

Question 15

Substances with covalent bonds .

Answer 15

usually have simple molecular structures

Question 16

Polymers

Answer 16

are long chains of small units which are linked together to form a long molecule that have repeating section

Question 17

Intermolecular forces between polymer molecules

Answer 17

are larger than between simple covalent molecules , so more energy is need to break them.

Question 18

Giant covalent structures are

Answer 18

macromolecules . All the atoms are bonded to each other by strong covalent bonds. very high melting and boiling points as lots of energy is needed to break covalent bonds.`

Question 19

Diamond - Giant covalent structure

Answer 19

each carbon atom forms four covalent bonds a in a very rigid giant covalent structure. It doesn’t conduct electricity because there is no free electrons or ions

Question 20

Graphite - Giant covalent structure

Answer 20

each carbon atom turns three covalent bonds to create layers of hexagons and one delocalised electron. High melting point Only three out of each carbons four outer electron are used in bonds, Conducts electricity and thermal energy

Question 21

Silicon dioxide - Giant covalent structure

Answer 21

this is what sand is made of . each grain of sand is one giant structure of silicon and oxygen.

Question 22

Allotropes are different structural forms of the same element in the same state . Carbons got lots

Answer 22

diamond
graphene
fullerenes

Question 23

Fullerenes

Answer 23

are molecules of carbon shaped like hollow balls. Mainly arranged in hexagons. They have a huge surface area so they could help make great industialil catalysts .

Question 24

Fullerenes can form

Answer 24

nanotubes . Nanotube can conduct both electricity and thermal energy. They also have high tensile strength

Question 25

Graphene

Answer 25

one layer of graphite. Graphene is a sheet of carbon atoms together in hexagons. Like graphite it contains delocalised electrons so can conduct electricity through the whole structure.

Question 26

Metallic bonding

Answer 26

involves delocalised electrons. Metals consist of a giant structure . Electrons in outer shell of metal are delocalised. Strong forces of electrostatic attraction between positive metal ions and negative electrons which hold the atoms in a regular structure.

Question 27

Intermolecules forces between polymers

Answer 27

are larger than simple covalent molecules so more energy is needed to break them

Question 28

Giant covalent structures are macromolecules

Answer 28

high melting and boiling points as lots of energy is needed to break the covalent bonds between the atoms

Question 29

examples of covalent bonding

Answer 29

diamond - four covalent bonds graphite - three covalent bonds , one delocalised electron silicon dioxide - one giant structure of silicon and oxygen