1) It's in the middle of the atom
2) It contains protons and neutrons
3) It has a positive charge because of the protons
4) Almost the whole mass of the atom is concentrated in the nucleus
1) Move around the nucleus in electron shells
2) They're negatively charged
3) They're tiny, but they cover a lot of space
4) Electrons have virtually no mass
Number of Protons equals the number of Electrons
a) the atomic number tells you how many protons there are (bottom number)
b) To get the number of neutrons subtract the atomic number from the mass number(top)
c) The mass ubmer is always the biggest number
Elements and Isotopes
a) The modern periodic table shows the elements in order of ascending atomic number
b) periodic table is laid out so that elements with similar properties form colums
c) Vertical colums are called groups, the group tells you the number of electrons it has in its outer shell
d) The rows are called periods. These represent the shell number
Isoptopes have an Extra Neutron
Isotopes are different forms of the same element, which have the same number of protons but a dfferent number of neutrons.
1) Isotopes have the same atomic umber but different mass numbers.
2) If they different atomic numbers, they'd be different elements
3) common example: carbon 12 , carbon 14
Electron Cell Rules
1) Electrons always occupy shells
2) The lowest shell are always filled first
3) Only a certain number of electrons are allowed in a shell, 1st: 2, 2nd: 8, 3rd: 8
Learn the first 20 from science book!
In ionic bonding, atoms lose or gain electrons to form charge particles which are then strongly attracted to one another.
1) If an atom has one or two electrons in their outer shell they lose them to have a full shell
2) If it loses an electron it becomes a positive ion
3) Ions are very reactive and will leap at the first passing ion with an opposite charge and stick to it like glue.
4) If an atom has a shell which is nearly full then they try to fill that shell becoming negative ions.
Ionic Compounds Form Giant Ionic Lattices
1) Ionic bonds form between metals and non-metals and always produce giant ionic structures.
2) The ions form a closely packed regular lattic arrangement. The ions are not free to move though, so these compounds do not conduct electricity when solid
3) There are very strong chemical bonds between all the ions
Ions and Ionic Compounds
1) When metals form ions, they lose electrons to form positive ions.
2) When non-metals form ions, they gain electrons to form negative ions.
3) So when a metal and a non-metal combine, they from ionic bonds.
4) The number of electrons lost or gained is the same as the charge on the ion
Covalent Bonds - Sharing Electrons
1) When non-metal atoms combine together they form covalent bonds by sharing pairs of electrons
2) Each covalent bond provides one extra shared electron for each atom
3) Each atom involved has to make enough covalent bonds to fill up its outer shell
Simple Molecular Substances
1) Substances formed from covalent bonds usually have simple molecular structures like COv2
2) The atoms within the molecules are held together by very strong covalent bonds.
3) By contrast, the forces of attraction between these molecules are very weak
4) This results in the melting and boiling points being very low because the molecules can be easily parted
5) Molecular substances don't conduct electricity because there are no free electrons.
Group 1 - Alkali Metals
Includes: lithium, sodium, potassium, rubidium and caesium
a) as you go down group 1, the alkali metals become more reactive because the outer electron is more easily lost as its further from the nuclues so less energy is needed to remove it.
b) the alkali metals all have one outer electron making them very reactive and gives them all similar properties.
c) All have the following physical properties:
-low melting point and boiling point
Oxidation is the loss of electrons
1) When alkali metals are put in watert they react and produce hydrogen
2) Alkali metal compounds burn with the following colours:
Lithium - Red flame
Sodium - Yellow/orange flame
Potassium - lilac flame
Group 7 - Halogens
Group 7 contains fluorine, chloring, bromine, iodine and astatine.
a) All group 7 elements have 7 electrons in their outer shell so they all react by gaining one electron
b) As you go down group 7, the halogens become less reactive as there's less force to gain an extra electron because it's further away from the nucleus.
c) As you go down group 7 the meting points and boiling points of the halogens increase.
Reduction is the gaining of electrons
Halogens react with alkali metals to form salts
1) More reactive halogens will displace less reactive ones
2) Chlorine can displace bormine and iodine from a soluton of bromide or iodide
Metals have a crystal structure
1) All metals have the same basic properties due to the specia type of bonding that exists in metals
2) Metals are held together with metallic bonds which allow the outer electrons of each atom to move freely
Most have high melting and boiling points, and high density
1) Metals are very hard, dense and lustrous
2) There's a strong attraction between the free electrons and the closely packed postive ions causing very strong metallic bonding.
3) Metals have a high tensile strength in other words they're strong and hard to break
4) They're also malleable
5) Metals are good conductors of heat and electricity because of the free electrons.
Superconductors and Transition Metals
1) If you make some metals cold enough, their resistance disappears completely, that metal becomes a superconductor.
2) Without any resistance, none of the electrical energy is turned into heat, so none of it's wasted.
Using superconducting wires you can make:
a) Power cables that transmit electricity without any loss of power
b) Really strong electromagnets that don't need a constant power source
c) electronic circuits that work really fast because there's no resistance to slow them down
However metals only start superconducting at -265 Celsius
Metals in the middle of the periodic table are transition metals
1) Transition metals and their compounds make good catalysts e.g iron is he catalyst used in the haber process.
Thermal Decomposition and Precipitation
1) Thermal decomposition is when a substance breaks down into atleast two other substances when heated.
2) Transition metal carbonates break down into a metal oxide and carbon dioxide.
1) A precipitation reaction is where two solutions reaact and an insoluble solid forms in the solution