Structure And Bonding

Question 1

Ionic bonding

Answer 1

Metal and non-metal. It’s a strong electrostatic attraction between oppositely charged ions.

Question 2

Covalent bonding

Answer 2

Non-metal only. A covalent bond is a shared pair of electrons, so they are very strong.

Question 3

Metallic bonding

Answer 3

Metals only. Consists of giant structure. Atoms are arranged in regular pattern. There are strong forces of electrostatic attraction between positively charged ions and negative electrons.

Question 4

Chemical Bonding

Answer 4

It involves changes in the electrons in the outer electron shell of the atoms. Metal atom donates electrons and non-metal receive electrons. This happens because they can achieve a stable electronic structure.

Question 5

Giant ionic lattice

Answer 5

Ions held together in a lattice. The strong electrostatic forces of attraction between the ions act in all directions. E.g sodium chloride(salt)NcCl

Question 6

Simple molecule

Answer 6

Molecules made up of just a few atoms. Covalent bonds. Very low boiling and melting point (intermolecular forces)E.g. hydrogen(H2), chlorine(Cl2)

Question 7

Macromolecules

Answer 7

Giant covalent structure. Many atoms are covalently bonded. E.g. silicon dioxide, diamond

Question 8

Double covalent bond

Answer 8

There are two pairs of electrons shared between two atoms.

Question 9

Delocalized electrons

Answer 9

Electrons aren’t associated with a particular atom or bond. They are free to move trough whole structure.

Question 10

Ionic compounds melting and boiling point

Answer 10

Ions arranged in a giant ionic lattice. All have high melting point and high boiling point, due to strong electrostatic attraction. A lot of energy required to break this attractions. When melted, it conduct electricity.

Question 11

Ionic compounds solubility

Answer 11

Dissolve in water easily. Ions separate and are free to move in the solution. Conduct electricity.

Question 12

Simple molecule properties

Answer 12

• Low melting and boiling point
• Mostly gases or liquids at room temperature
• do not conduct electricity- there are no ions or free electrons

Question 13

Simple molecular structure bonding

Answer 13

Intermolecular forces are very weak. This forces are broken down when the substance is boiled or melted.

Question 14

Giant covalent structure

Answer 14

There are no charged ions. All atoms are bonded to each other by covalent bond. Very high boiling and melting point. Most don’t conduct electricity. E.g. diamond, graphite, silicon dioxide.

Question 15

Diamond

Answer 15

Each carbon atom forms four covalent bonds in a very rigid giant covalent structure. Hardest natural substance. Does not conduct electricity, insolvable in water, colorless and clear.

Question 16

Graphite

Answer 16

Each carbon atom forms three covalent bonds. This create a layers of carbon atoms. The layers can easily slide over, since there is no covalent bonding between them (used in pencils). Conduct electricity.

Question 17

Nanoparticles

Answer 17

Really tiny particles. Contain roughly a few hundred atoms. Uses: huge surface are to volume. Used as industrial catalyst, to make stronger, lighter building materials, nanotubes conduct electricity, cannot be used in tiny electrical circuits

Question 18

Fullerenes

Answer 18

The carbon atoms are arranged in hexagonal rings. Shaped like hollow balls or closed tubes.

Question 19

Uses of fullerenes

Answer 19

• lubricant, catalyst
• can be used to deliver drugs into cells
• to form nanotubes

Question 20

Ions

Answer 20

A charged particle produced by the loss or gain of electrons. It has the electron arrangement of a noble gas.

Question 21

Nobel gas

Answer 21

Very unreactive gases found in group 0 of the periodic table.

Question 22

Intermolecular forces

Answer 22

The force of attraction between the individual molecules.

Question 23

The electrons in the highest occupied energy levels of metal atoms are…

Answer 23

delocalised and so free to move through the whole structure.

Question 24

Delocalised electrons in metals allow it…

Answer 24

to conduct electricity and heat.

Question 25

Conduction depends on the ability…

Answer 25

of electrons to move through the structure.