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
Neutrons
Mass number-atomic number
Metallic character
Easily lose electrons, conducts electricity and shiny
Non- metallic character
Non- metals, gain electrons
how many electrons can occupy subshells 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f
1s=2
2s=2
2p=6
3s=2
3p=6
3d=10
4s=2
4p=6
4d=10
4f=14
Maximum number of electrons for each shell
Shell1:2
Shell2:8
Shell3:18
Shell4:32
covalent bond=
non-metals
where are the metals, metalloids and non-metals
metalloids =boron, silicon, arsenic, tellurium, astatine, germanium and antimony
on the right side of the metalloids are the non-metals
on the left side of metalloids are metals
with electron subshell configuration when do you stop
stop on the element
reactivity=
how easy it is for an atom to lose of gain electrons
allotropes
two or more physical forms an element can exist example graphite diamond
when an element is in its excited state…
it means it is not fully filled the shells and moved on to other shells
why are metals more reactive than non metals
because are more reactive than non-metals because have many free electrons to give away .
what info does 3 occupied electron shells and 2 valence electrons give us
that the element is in period 3 and group 2
how to find out which element has a larger atomic radius
the one with more electron shells occupied
what does unsaturated mean when referring to hydrocarbons
is one that has one or more carbon to carbon double or triple bonds
what ion does non-metals form
negative ion
when something is a lattice what does it experiences
intermolecular forces
what are alkanes and alkenes (bond? polarity)
they are non polar and experience dispersion forces
molecular formula
molar mass of a compound / molar mass of one empirical formula unit the answer is what u times the empirical formula by
what is the ratio of calcium ions to fluorine ions
each calcium atom needs to lose 2 electrons to achieve stability but each fluorine needs to gain one so two fluorine to atoms to 1 calcium
if it gains 2 it comes…
if it loses 2 it becomes
negative
positive
atomic number represents
the electrons and protons neutrons are diff
vitamin C contains 54.5% oxygen by mass. how many atoms of oxygen in one molecule of vitamin C? when given the gmol and percentage
Step 1: Calculate the mass of oxygen in one mole of Vitamin C
Since Vitamin C contains 54.5% (divide by 100) oxygen by mass, we can find the mass of oxygen in one mole of Vitamin C by multiplying the molar mass by the percentage of oxygen.
Mass of oxygen = 176.14 g/mol x 0.545 = 95.95 g/mol
Step 2: Calculate the number of moles of oxygen in one mole of Vitamin C
To find the number of moles of oxygen, we need to divide the mass of oxygen by the molar mass of oxygen.
Number of moles of oxygen = 95.95 g/mol / 16.00 g/mol = 6 moles
how to find the molar mass of the empirical formula
empirical formula:
C5H6
(12x5)+(6x1)= molar mass
ionic bonding properties
The properties of ionic bonding include high melting and boiling points, poor conductivity in the solid state, and high conductivity in molten/ liquid form
tetrachloromethane
Tetrachloroethene has a higher boiling point than tetrachloromethane because it has stronger intermolecular forces.
properties of hydrocarbons
-non-polar
-strong intramolecular bonds=covalent
-intermolecular forces are weak dispersion forces
-larger molecules high boiling points due to strong forces
haloalkanes:
BR
I
F
C
bromo-
iodo-
flouro-
chloro-
what do you add when naming a alcohol
-ol is the ending ex. ethanol
carboxylic acids ending
-onic acid
