C3 Structure and Bonding

Question 1

What is ionic bonding

Answer 1

This is bonding between a metal and a non metal where metals lose electrons and become positively charged and the non metal gains electrons becoming negatively charged. The atoms join by forces of electrostatic attraction and being a compound

Question 2

What is covalent bonding and how are the atoms drawn to one another

Answer 2

When non-metal atoms bond together, they share pairs of electrons to make covalent bonds. The positively charged nuclei of the atoms are attracted to the shared pair of electrons by electrostatic forces making the bond is very strong
When atoms bond covalently, they gain a full outer shell

Question 3

What is the group number and the ions they produce

Answer 3

1: 1+
2: 2+
3: 3+
4: 4+ or 4-
5: 3-
6: 2-
7: 1-
0: ❌

Question 4

What are ionic compounds

Answer 4

An ionic compound is a giant structure of ions. Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions. These forces act in all directions in the lattice and this is called ionic bonding.

Question 5

What are drawbacks to using the ionic diagrams

Answer 5

Dot and cross: doesn’t include three dimensional arrangements of the atoms and electron shell or the relative sizes of the atoms
Ball and stick: The atoms are placed far apart from each other, which in reality is not the case as the gaps between atoms are much smaller.
Displayed formula / 2D model: doesn’t show relative sizes of the atoms and bonds
3D model: it doesn’t show the electrons or how the electrons are transfered
Particle model: there are no forces, that all particles are represented as spheres and that the spheres are solid

Question 6

What do covalently bonded small moleculesmainly constist of

Answer 6

Smaller molecules Cl2, I2, Br2 ( common diatomics )

Question 7

Give example of giant covalent structures

Answer 7

diamond and silicon dioxide

Question 8

What do metals consist of

Answer 8

Metals consist of giant structures of atoms arranged in a regular pattern.

Question 9

How are metals bonded

Answer 9

The electrons in the outer shell of metal atoms are delocalised and so are free to move through the whole structure. The sharing of delocalised electrons gives rise to strong metallic bonds ( electrostatic )

Question 10

How are ionic compounds structured

Answer 10

Ionic compounds have regular structures (giant ionic lattices) in which there are strong electrostatic forces of attraction in all directions between oppositely charged ions

Question 11

Why do ionic compounds have high boiling points

Answer 11

These compounds have high melting points and high boiling points because of the large amounts of energy needed to break the many strong bonds

Question 12

When do ionic compounds conduct electricity

Answer 12

When melted or dissolved in water, ionic compounds conduct electricity because the ions are free to move and so charge can flow.

Question 13

What are the properties of small molecules

Answer 13

Substances that consist of small molecules are usually gases or liquids that have relatively low melting points and boiling points
These substances do not conduct electricity because the molecules do not have an overall electric charge

Question 14

Why do small molecules have the properties that they do

Answer 14

These substances have only weak forces between the molecules (intermolecular forces). It is these intermolecular forces that are overcome, not the covalent bonds, when the substance melts or boils.
The covalent bonds ( intramolecular forces ) are stronger

Question 15

Why do larger molecules have high boiling and melting points that smaller molecules

Answer 15

The intermolecular forces increase with the size of the molecules, so larger molecules have higher melting and boiling points

Question 16

What giant covalent structures and why do they have their properties, give examples

Answer 16

Substances that consist of giant covalent structures are solids with very high melting points.
All of the atoms in these structures are linked to other atoms by strong covalent bonds.
These bonds must be overcome to melt or boil these substances.
They do not conduct electricity not even when molten because the particles are not charged
Diamond and graphite (forms of carbon) and silicon dioxide (silica) are examples of giant covalent structures

Question 17

Why do metals have high melting and boiling points

Answer 17

Metals require a lot of energy to break the electrostatic forces of attraction between the ions and sea of delocalised electrons. This means that most metals have high melting and boiling points

Question 18

Why are metals malleable and ductile and why do alloying them change this

Answer 18

In pure metals, atoms are arranged in layers, they can slide over eachother, which allows metals to be bent and shaped.
Metals are too soft for certain jobs so alloying them makes them harder
The foreign atoms distort the regular arrangement so the metals’ atoms can no longer move over each other easily

Question 19

Why are metals good conductors

Answer 19

The delocalised electrons in the metal carry electrical charge through the metal. Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons.

Question 20

Why is diamond so rigid and non conductive

Answer 20

Each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, so diamond is very hard, has a very high melting point and does not conduct electricity (because it has no free electrons).

Question 21

What is significant about the structure of graphite

Answer 21

In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between the layers.
In graphite, one electron from each carbon atom is delocalised

Question 22

What are the properties of graphite

Answer 22

Good lubricant
High melting point
Conducts electricity and thermal energy

Question 23

What is graphene

Answer 23

Graphene is a sheet of carbon atoms joined in hexagons, it is a 2d substance that can be used in electronics due to it’s properties

Question 24

What are the properties of graphene

Answer 24

Light ( 1 atom thick )
Strong ( network of covalent bonds )
Conducts electricity ( delocalised electrons )

Question 25

What are fullenenes and what are their structure

Answer 25

Fullerenes are molecules of carbon atoms with hollow shapes. The structure of fullerenes is based on hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms. The first fullerene to be discovered was Buckminsterfullerene (C60) which has a spherical shape.

Question 26

What are carbon nanotubes

Answer 26

Carbon nanotubes are cylindrical fullerenes with very high length to diameter ratios.
Can conduct electricity and thermal energy
High tensile strength

Question 27

What is nanoscience

Answer 27

Nanoscience refers to structures that are 1–100 nm in size

Question 28

How are nanoparticles different to fine and coarse particles, give examples of fine and coarse particles

Answer 28

Nanoparticles, are smaller than fine particles (PM2.5), which have diameters between 100 and 2500 nm
Coarse particles (PM10) have diameters between 1 x 10-5 m and 2.5 x 10-6 m.
Coarse particles are often referred to as dust.

Question 29

What is the rule with SA : V ratio

Answer 29

As the side of cube decreases by a factor of 10 the surface area to volume ratio increases by a factor of 10.

Question 30

How can nanoparticles be useful in the future

Answer 30

Nanoparticles may have properties different from those for the same materials in bulk because of their high surface area to volume ratio.
It may also mean that smaller quantities are needed to be effective than for materials with normal particle sizes

Question 31

Shat are the uses of nanoparticles

Answer 31

Nanoparticles have many applications in medicine, in electronics, in cosmetics and sun creams, as deodorants, and as catalysts

Question 32

What are the worries with nanoparticles

Answer 32

Long term health impacts are not known

Environmental impacts are unknown