bonding, structure and properties of matter (y10) Flashcards
what does a substance need to change from one state to another?
energy must be transferred
what are the properties of particles in a SOLID? (s)
- arranged in a regular pattern
- vibrate in a fixed position
- tightly packed together
- low amount of kinetic energy
- cannot be compressed
- fixed shape
what are the properties of particles in a LIQUID? (l)
- randomly arranged
- able to move around each other
- greater amount of kinetic energy compared to a solid
- can flow
-cannot be compressed
what are the properties of particles in a GAS? (g)
- randomly arranged
- able to move around quickly in every direction
- highest amount of kinetic energy
- gases can flow
- particles are FAR APART
- can be compressed
what is an ion?
a charged particle
how does an element become an ion?
when it loses or gains an electron
-metals lose an ion to become positively charged
-non-metals gain an electron to become negatively charged
properties of metals
- found on the left side of the periodic table
- strong, shiny, malleable
- good conductors of heat and electricity
properties of non- metals
- brittle, dull, not always solids at room temp
- poor conductors of heat and electricity
metallic bonding occurs between :
metals only
what are positive ions surrounded by in metallic bonding
a sea of delocalised electrons
describe the attraction between between ions and electrons in metallic bonding
there are strong electrostatic forces of attraction between the positive metal ions and negatively charged electrons
what does different sized atoms in metals do in metallic bonding
distorts the layers and prevents them sliding over each other, this makes it harder for alloys to be shaped like pure metals
ionic bonding occurs between :
a non metal and a metal
what happens in ionic bonds
metals LOSE electrons to become positively charged. opposite charges are attracted by electrostatic forces - an ionic bond.
what do ionic compounds form
giant lattices.
what makes up a giant ionic lattice
strong electrostatic forces that act in all directions and act between the oppositely charged ions that make up a giant ionic lattice
properties of ionic compounds :
- high melting point
- high boiling point
- cannot conduct electricity as a solid
- when molten or in a solution, can conduct electricity.
covalent bonding occurs between :
non- metals only
what is covalent bonding?
the sharing of a pair of electrons between atoms to gain a full outer shell.
what molecules does simple covalent bonding occur between ?
- chlorine
- oxygen
- nitrogen
- water
- ammonia
- hydrogen chloride
- methane
what do simple covalent structures have in common and why
- low melting and boiling points
- this is because the WEAK INTERMOLLECULAR forces that hold the molecules together break when a substance is heated, not the strong covalent bonds between atoms
- dont conduct electricity
- this si because they have no delocalised electrons
what are the properties of a diamond (Giant covalent structure)
- bonded by 4 other carbon atoms
- very strong
- high melting and boiling point
- does not conduct electricity
( this is very similar to silicon dioxide )
what are the properties of graphite in a giant covalent structure?
- made up of layers of carbon in hexagons
- each carbon is bonded to 3 other carbons
- has one free delocalised electrons that is able to move between layers
- layers are held together by weak intermollecular forces
- high melting point
-can conduct electricity
what are the properties of graphene in a giant covalent structure
- one layer of graphite
- very strong
- can conduct electricity
- each carbon is bonded with 3 others along with one delocalised electron
what is a polymer
long chain molecules that are made up of monomers.
what are atoms in a polymer chain held together by
strong covalent bonds
what do the intermollecular forces do in polymers?
attract polymers chains towards each other
