Bonding,structure And Properties Of Matter

Question 1

What are solids

Answer 1

Particles of atoms of a substance that is tightly owcked together and vibrate in fixed positions

Question 2

Properties of solids

Answer 2

Fixed shape and volune

Lowest energy form of matter

Held by strong forces of attraction

Vibrate

Question 3

What are liquids

Answer 3

Made up of randomly arranged particles of a substance that is free to move around.

Question 4

Properties of liquids

Answer 4

No fixed shape but a fixed volume

No orderly arrangement

Partciles still close together

Question 5

What are gases

Answer 5

A state of matter where its particles are able to move around freely and spread out.

Question 6

Properties of gases

Answer 6

Mostly empty space, distance between particles

No fixed shape or volume

No order in particle arrangement

Highest energy state of matter

Question 7

Four main ways substances can change

Answer 7

Melting,boiling,condensing and freezing

Question 8

What is melting

Answer 8

Solid is heated up to its melting point, particles will gain enough energy to overcome the forces between them and break out its solid arrangement

Question 9

What is boiling

Answer 9

Liquid is heated up to its boiling point. The particles will gain enough energy to overcome the remaining forces between them and the structure of the liquid will seperate

Question 10

What is condensation

Answer 10

In condensation gas cools down to the condensation point and looses energy, changing from a gas to liquid

Question 11

What is freezing

Answer 11

Freezing is when a liquid cools down to its freezing point as it loses energy, changing from a liquid to solid state

Question 12

Limitations of particle theory

Answer 12

Doesn’t consider the forces between molecukes

Assumes that all particles are spheres,doesn’t account for complex molecule shapes

Assumes all spheres are solids and inelastic, doesn’t reflect atoms,ions and molecules

Question 13

What are ions

Answer 13

An atoms or a group of atoms that has an electric charge

Question 14

How are ions formed

Answer 14

When atoms gain or lose one or more electrons to form a charged particle.

Question 15

How are positive ions formed

Answer 15

Loss of electrons from the outermost shell

Question 16

What are positive ions always

Answer 16

They are always metals as they tend to lose electrons in its outermost shell

Question 17

What are negative ions

Answer 17

Formed by the gain of electrons in the outermost shell

Question 18

What are negatives almost always

Answer 18

They are almost always non-metals elements as they tend to have outer shells which need to gain electrons

Question 19

How are ionic bonds formed

Answer 19

Metal elements react with non-metal element to create a full outer shell for both elements

Ions are oppositley charged meaning there is a strong electrostatic attraction between them

Question 20

What is a giant ionic lattice

Answer 20

Giant: very large containing milliions of ions held by many bonds

Ionic: The particle that makes up the solid are ions,each with posiitve and negative charge

Lattice: Orderly structured and made up of repeating patterns.

Question 21

Properties of giant ionic lattices

Answer 21

Incredibly high melting points as a result of strong electrostatic attractions between oppositley charged ions. Requires lots of energy to break

Ionic solids easily soluble in water. The electrostatic attractions between the ions in the lattice and water molecules is stronger than between ions in the lattice

Ionic substances don’t conduct electricity when solid, this is due to ions in the lattice are fixed

Ionic substances will conduct when molten. When in the liquid state is ions are able to move around and as such carry a charge

Question 22

What are covalent binds

Answer 22

Strongs bonds formed between 2 or more atoms that are both non-metals elements

Question 23

How are covalent bonds formed

Answer 23

Covalent bonds form when two or more atoms of non-metal elements come together to form a molecule (one or more pair of electrons are shared)

Question 24

Dot and cross advantages/limitations

Line diagrams advantages/limitations

3 dimensional models advantages/limitations

Answer 24

Allows us to visualise how electrons are shared and which atoms they orginated from however does not tell us about the shape

Line diagrams can tell us more about the
2D shape of a molecules but fail to represent the space filled by atoms

Three dimensional models shows accurate shapes of molecules and the spaces filled by their constituent atoms. We lose info e.g the distribution of electrons within the molecule.

Question 25

Properties of simple covalent molecules

Answer 25

Bond between atoms are strong and difficult to break but the forces between the molecules are very weak

Weak intermolecular forces much easier to overcome than strong electrostatic forces of attraction

Covalent conpounds don’t conduct electricity as there are no charged particles ( balanced charges)

Question 26

What are polymers

Answer 26

Type of covalent molecule, made up of long chains of carbon, held by covalent bomds

Question 27

Properties of polymers

Answer 27

Stronger covalent bonds then simple covalent molecules however its intermolecular forces are still weaker than the electrostatic attractions found in ionic solids

Question 28

Properties of giant covalent structures

Answer 28

Made up if many covalent bonds making it very strong and hard

Lots of energy required to break it down (force)

Very high melting point

Question 29

Graphite : explain the structure and properties

Answer 29

Each carbon atom is bonded to 3 other atoms. Carbon atom with 3 electeons with a free delocalised electron. Carbon atoms arranged in flat sheets of connected hexagons

Delocalised electrons allow graphite to conduct electricity
Strong covalent bond= difficult to break (high melting point)
Weak intermolecular forces hold the sheets of strong graphite layers can slide over each other (slippery)

Question 30

Graphene: explain structure and properties

Answer 30

Singular layer of graphite

Light material (only 1 atom thick)
Many strong covalent bonds= very strong material
Graphene has a high melting point
Graphene can conduct electricity (delocalsied electrons)

Question 31

Fullerenes: explain structure and properties

Answer 31

Buckminsterfullerene is a hollow ball made up of 60 carbon atoms
Used for drug delivery

Carbon nanotubes are long hollow cyclinders made up of carbon atoms.

Excellent lubricants
Good conductors of electricity

Question 32

What can the giant covalent structures be used for and why

Answer 32

Graphite: layer of graphite can slide off the tip of the pencil onto the page

Graphene: Used in composites to make other materials stronger and electronics

Buckminsterfullerene: electronic applications

Carbon nanotube: They are used to deliver deugs inside the body or as a catalyst for chemical reactions

Question 33

What is metallic bonding

Answer 33

Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons.

Question 34

Properties of metals

Answer 34

Electrostatic attractions is very strong and requires lots of energy to overcome.

Metals have a high melting point

Metals are able to conduct electricity and heat easily when solid (delocalised electrons move freely)

Very ductile (metal ions can slide over each other) arranged in layers

Metal not soluble in water. Attraction between the positive metal lattice and negative sea of electrons much stronger between ions and water

Question 35

Diamond: explain structure and properties

Answer 35

Giant structure made up of carbon atoms with 4 covalent bonds

Diamonds are hard

They have a high melting point

No electricity conducted (no delocalised electrons)

Question 36

How are alloys created and why

Answer 36

Pure metals are too soft and may be required for certain jobs this can be done through creating an alloy

Alloy-mixture of 2 or more metals. They are usually harder due to the difference size atoms in the metal layer which distorts it thus making it more useful then pure metals.

Question 37

What are nano particles

Answer 37

Very small particles 1 and 100nm in size

Question 38

Fetaures and use of nanoparticles

Answer 38

SA:V increases by factor of 10
Some may conduct electricity

Used as a catalyst due to high SA

Healthcare such as polymers (masks), drug delivery vehixles

Development of tiny cirucits-some can conduct electricity

Question 39

What is the structure and properties of sodium chloride

Answer 39

Structure: 3 dimensionsl lattice, regular repeated patterns of positive sodium ions and negative chloride ions

Properties: large amounts of energy required to overcome electrostatic forces of attraction, high melting and boiling point. They can conduct electricity when melted or dissolved in water.