Chemistry Flashcards
name the mass and charge of each atomic particle
proton (mass=1 charge=+1) neutron (mass=1 charge=0) electron (mass=0 charge=-1)
define an isotope
Atoms of the same element and same atomic number with different numbers of neutrons and different mass number
define relative molecular mass
total mass of all the atoms in the ionic formula
how to work out moles
mass/Ar or Mr
what is concentration measured in
g/dm^3 or mol/dm^3
how to calculate the number of moles in a solution
concentration (mol.dm^-3) X volume (cm^3)
how to calculate the volume
volume (dm^3)=24 X moles
how do you measure atomic radius
measure the distance between two nuclei and divide by two
what happens to atomic radius across a period
decreases
what happens to atomic radius as you go down a group
increases
what is ionisation energy
electrons being removed from atoms and the energy it takes to remove them can be measured. Atoms become positive ions.
what does the ionisation energy of an element depend on
atomic radius nuclear charge (number of protons) number of electron shells
what is a molecular formular
refers specifically to a covalently bonded molecule and shows the number of atoms of each element in molecules of a particular compound
what is a empirical formula
refers to ionic or covalent compounds and is the simplest ratio of atoms of different elements in a compound
how do you work out the volume in an ideal gas equation
v= nRT/P
how do you work out the number of moles n of a gas in an ideal gas equation
n=PV/RT
Structure of diamond
- Tetrahedral structure
- Each carbon is bonded to 4 other carbons
- Carbons are covalently bonded
properties of diamond
- very hugh melting point (2000°C)
- no charged oarticles, does not conduct electricty
- dosen’t dissolve in any olvent
structure of giant covalent:graphit
- hexagonal arrangment of carbons
- each carbon bonds to 3 other carbons
- covalent bond
- forms layer
structure of graphene
- single layer of graphite
- giant covalent lattice, high melting and boiling point
- dosen’t dissolve in any solvent
- conduct electricty, delocalised electrons
- transparent, extremely thin
properties of graphite
- high melting point
- does not dissolve in any solvent
- soft and sippery
- conduct electricty
structure of fullerenes
- 60 carbon atoms joined together to form a ball
- giant lattice, high melting and boling point, insoluble
- conducts electricty
properties of ilicion dioxide
- lagre number of strong covalent bonds
- high melting and boiling point
- had crystaline structure
- cannot conduct electricty
Metal atoms …. outer ecltrons and become …..
- loose
- positive
Free elctrons are called
What are the properties of metallic bonding?
- High melting points
- Hard and strong
- Solid at room temperature
- Conduct elctricty and heat
