Exam revision Flashcards
1 carbon
2 carbons
3 carbons
4 carbons
5 carbons
meth-
eth-
prop-
but-
pent-
6 carbons
7 carbons
8 carbons
9 carbons
10 carbons
hex-
hept-
oct-
non-
dec-
branch with one group
branch with two groups
branch with three groups
methyl
ethyl
propyl
What does M stand for and what is it?
It is the molar mass (gmol-1) it can be found out using Ar(x)+Ar(b)
(Ar is found on the periodic table)
What does n stand for and how can it be found?
Number of moles(mol)
It can be found using n=m(mass g)/M(gmol-1)
n=N/NA
What does N stand for and how is it found
Number of particles
If we know the mole(n)
N=nxNA
If we know the mass(m)
1.n=m/M
2.N=nxNA
What does m stand for and how can it be found
It is mass(g)
If we know the number of particles (N)
1.n=N/NA
2.m=nxNA
If we know the mole(n)
m=nxNA
what is NA
Advogadros constant (mol-1)
6.02x10^23
Empirical formula
Composition/ mass found in pt
Then divide by the smallest answer
times by something that can make them full numbers if needed
when asked for the amount of substance
mol
n=N/Na
when asked for the number of molecules
N=nxNa
when asked for the number of atoms
N=(how much elements there are ex. H2O=3)xnxNa
Ar formula
(no. of pt)x(abundance)/100
percentage composition
(how much of the element) /the no. found on pt x 100
Electronegativity trends
High for non metals
Group 18 no electronegativity
Less pull when valence electrons further from nucleus
First Ionisation Trends
Decreases going down a group
Increases across a period
Reactivity trends
Group 1 most reactive followed by group 2 in the metals but in the non metals it’s group 17 followed by group 16
Group 18 no reactivity
The reactivity of an element belonging to metals increases on moving from top to bottom in a group of the periodic table. While moving from top to bottom in a group of the periodic table, the reactivity of non-metals decreases.
Atomic radii trends
Decrease from left to right across a period to group 18
Increase as you go down a group
Electronegativity trends
Group 18 has no electronegativity
Increase across a period and up a group
intramolecular
bonds that hold atoms within molecules
-covalent bonds
-ionic bonds
intermolecular
bonds that occur between molecules and hold them together
-h-bonding
~FON
-dipole-dipole
-dispersion forces
metallic bonding properties
-due to mobile electrons being able to reflect light they are lustre
-electrons are able to gain kinetic energy in hotter areas of the metal and are able to transfer it to other parts of the metal lattice (bc of free moving electrons they bump into each other=transfer)
-high density because metallic lattices are closed packed
- high melting point and hardness:
–strong bonding
–increase the number of outer shell electrons (bc greater attraction force between the cation and the electrons)
-when an electrical field is applied one end becomes positive and the other negative .electrons experience a force toward the positive end (this is called an electric current )
-not brittle malleable
Graphite Properties
is solid with a high melting point due to strong covalent bonds
conducts both electricity and heat due to the presence and movement of delocalised electrons
is slippery to the touch because weak dispersion forces between layers allow the layers to slide over each other
has a metallic sheen due to the interaction between light and the delocalised electrons.
Mass number
Number of protons-number of neutrons
