GCSE Chemistry- C2 Bonding, Structure and Properties of Matter

What is the process of going from solid to gas?

sublimation

What is the process of going from gas to solid?

deposition

What is the process of going from solid to liquid?

melting

What is the process of going from liquid to solid?

freezing

What is the process of going from liquid to gas?

boiling

What is the process of going from gas to liquid?

condensation

What are properties of solids?

particles close together, cannot be squashed, vibrates on spot, regular arrangement

What are properties of gases?

particles close together, cannot be squashed, particles move around each other, random arrangement

What are properties of liquids?

particles far apart, can be squashed, particles move freely in all directions, random arrangement

What is an aqueous solution?

a solution in which water is the solvent & something is dissolved in water

what is a non-newtonian fluid?

A liquid which doesn't follow Newton's law of viscosity

What are the limitations of the particle model?

2 dimensional, no movement of particles, cannot see intermolecular forces, shown as a solid sphere- inaccurate to reality, not to scale, cannot see properties.

What is the melting point?

the temperature at which a solid changes to a liquid

What is the boiling point?

The temperature at which a liquid changes to a gas

What is the melting point equal to?

melting point = freezing point

What is the boiling point equal to?

boiling point = condensing point

What makes atoms bond together?

the movement of electrons

What are the three types of bonding?

covalent, ionic, metallic

What does 'delocalised' mean?

(electrons) free to move

What does a stronger force of attraction mean?

Higher melting point, due to force of attraction requiring more force to overcome.

What is metallic bonding?

metals having a giant metallic structure and electrons in outer shell of each metal atom delocalised and can move throughout entire structure, meaning the positive ions arrange in regular pattern surrounded by 'sea' of delocalised electrons.

what are the properties of metals?

malleable- layers can slide over each other, strong, ductile- layers of atoms can slide over each other, high melting + boiling point, good conductors of electricity- has charges and delocalised electrons that can move, shiny, good conductors of heat- delocalised electrons can transfer thermal energy

Why are metals good conductors of electricity?

It has charges and delocalised electrons that can move, therefore current can pass through.

why are metals good conductors of heat?

The delocalised electrons can transfer thermal energy throughout the metal

Why are metals malleable and ductile?

The atoms are arranged in layers that are able to slide over each other

What does a compound with .........ide mean?

only one element

What does a compound with .........ate mean?

bonded with oxygen

What is an alloy?

a mixture with a metal and at leat one other element

Why are alloys harder and stronger than pure metals?

the atoms are different sizes due to the different elements, therefore layers cannot slide over each other easily. this makes alloys harder and stronger than most pure metals.

What are examples of alloys?

Steel- iron + carbon, bronze- copper + tin, brass

What is a stable atom?

an atom with a full outer shell

What is an unstable atom?

an atom with a outer shell not full

What is reacitivty?

How easily an electron is lost or gained

What is ionic bonding?

bonds between metals and non-metals

What happens to electrons in ionic bonding?

they are transferred, atoms involve will lose or gain electrons and become ions

What happens to non-metals ionic bonding?

they always gain electrons and become a negative ion (anion)

What happens to metals and hydrogen in ionic bonding?

They always lose electrons and become a positive ion (cation)

What forces are involved in ionic bonding?

strong electrostatic forces of attraction between the oppositely charged ions are formed in Ionic bonding.

Examples of ionic bonding

what are giant ionic lattices?

ions held in a structure with many ionic bonds. They have strong electrostatic forces of attraction between positively charged and negatively charged ions in all directions.

what is an empirical formula?

the simplest whole number ratio of atoms present in a compound

What are properties of ionic compounds?

high melting and boiling points, soluble in water, brittle, can conduct electricity when molten or dissolved

Why do ionic compound have high melting and boiling points?

there are strong electrostatic forces of attraction between ions, so it takes lots of energy to break the bonds

Why are ionic compounds soluble in water?

H2O molecules pull ions apart to make a solution because it is made up of H+ and OH- ions

What are ionic compounds brittle?

when the lattice structure is hit, the ions with the same charges are lined up together these same charges repel and split the lattice structure.

Why can ionic compounds conduct electricity when molten or dissolved?

the charges can move, therefore, current can pass through

what is covalent bonding?

bonding of particles between non-metals with the sharing of electrons

What is a structural formula?

a formula that shows the arrangement of atoms in the molecule of a compound.

What is a chemical formula?

a combination of symbols that shows the ratio of elements in a compound

Example of a covalent bond

What do simple covalent structures contain?

strong covalent bonds within each molecule, weak intermolecular forces between molecules

What are most simple covalent structures at room temperature?

they are gases

What does the strength of intermolecular forces increasing mean?

the size of molecules increase, therefore more energy taken to melt and boil the molecule, higher melting and boiling points.

Why can's simple covalent structures conduct electricity?

they are neutral=have no charges, therefore cannot conduct electricity

What are physical properties of simple covalent structures?

soft as solid- weak intermolecular forces, brittle- weak intermolecular forces

What are polymers?

simple covalent structures which are chains or repeating units (monomers).

What does a larger polymer mean?

higher melting point due to more energy needed to break down larger size

example of polymer

Polythene

Why is a 3D model best to show the structure of simple covalent structures?

shows structure in different views and atoms are seen in 3D

what are giant covalent structures?

non-metals held together in lots of covalent bonds

what are allotropes?

different structural forms of the same element, eg. diamond and graphite, made from Carbon. Same chemical properties because same number of electrons, different physical properties because electrons are shared in different ways

what does structure mean?

how a compound looks

What does bonding mean?

How it is put together

what is the structure of graphene?

an allotrope of carbon with a single layer (2D) of graphite, has 3 strong covalent bonds between each carbon atom

What are the properties of graphene?

very strong (covalent bonds), high melting and boiling points (covalent bonds), can conduct electricity ( a free electron to carry a charge), transparent- too thin for the human eye

What is graphene often used as?

phone screens- transparent + strong, electronics- conducts electricity

What is the structure of graphite?

an allotrope of carbon with 3 strong covalent bonds between each carbon atom and weak intermolecular forces between each layer of graphene

What are the properties of graphite?

grey/black colour, layered structure, soft

What is graphite often used as?

pencil lead, lubricant

What is the structure of a fullerene?

an allotrope of carbon with hollow structure, based on rings of carbon atoms joined by a covalent bond. Weak intermolecular forces between fullerenes

What is the structure of Buckminster fullerene?

60 carbon atoms held together with covalent bonds (known as C60), weak intermolecular forces between buckminster fullerene molecules, spherical, hollow shape.

What are properties of Buckminster fullerene?

low melting and boiling points- weak intermolecular forces, slippery- weak intermolecular forces

What is the structure of a carbon nanotube?

layers of graphene rolled into a cylinder, one delocalised electron per carbon atom, very long compared to its width (high length to diameter ratio)

What are properties of a carbon nanotube?

high tensile strength (resist tension and being stretched), strong, can conduct electricity- delocalised electron

What is a kilo...?

10^3 or 1000 of a unit (K...)

What is a deci...?

10^-1 or 0.1 of a unit (d...)

What is a centi....?

10^-2 or 0.01 of a unit (c...)

What is a milli....?

10^-3 or 0.001 of a unit (m...)

What is a micro....?

10^-6 or 0.000001 of a unit (µ...)

What is a nano....?

10^-9 or 0.000000001of a unit (n...)

what is a pico...?

10^-12 or 0.000000000001 of a unit (p...)

What is the typical diameter of an atom?

O.1nm or 1 x 10^-10m

What is the particle matter of a coarse particle (dust)?

PM 10, diameter between 2500 nm to 10,000 nm

What is the particle matter of a fine particle?

PM 0.1-2.5, diameter between 100nm to 2500nm

What is the particle matter of a nanoparticles?

N/A, diameter between 1nm to 100nm

What is PM?

particulate matter

What is percentage by mass?

Mass of 100(element/Mr)