Halogens: These are highly reactive elements, which are mainly used for chemical industries
Noble Gases: These elements are chemically unreactive
P1 task 2
Periodicity: in simple definition is something which refers to trends and frequent variations in the element properties with increasing atomic number. Periodicity is caused by expected and predictable typical amount in its atomic structure.
Atomic number: the amount of protons in the heart of an element which is called the nucleus.
Mass Number: Is the total of number of protons and neutrons which are present in a atom is called mass number.
Isotopes: are atoms of an element with standard number of protons and electrons, but the number of neutrons differing; Isotopes consist of same number of atomic number but is different with the mass numbers.
P1 Task 3
There are 7 groups in the periodic table which all have different and similar kinds of elements, which all have electrons. From looking at the periodic table is it very easy to conclude how many electrons the element contains in its outer shell, see how group 1 alkaline metals all have electrons, from looking at the group number it tells us how many electrons the elements have in its outer shell, here are a few examples of what my intended meaning is:
Lithium- contains 3 protons, 3 neutrons and 3 electrons, so from looking at the amount of electrons the Lithium has I can now draw up what the electronic structure would look like so it would have 2 electrons in its first shell which is the maximum number of electrons in the first shell, which leaves behind another electron which will be in the most outer shell, instead of drawing the electronic structure to see how many electrons it has in its most outer shell I can look over to the group number and it would tell me like now Lithium has 1 electron in its most outer shell and is from group 1,there is no reason why this happens it just is like that which makes it very easier. Here are some more examples to get the gist of how it works:
- Nitrogen- belongs to group 5, contains 7 protons,7 neutrons and 7 electrons, so the electronic structure will be 2,5. This again relates group 5 and 5 number of electrons in outer shell
- Fluorine- belongs to group 7, contains 10 neutrons, 9 protons and 9 electrons so the electronic structure would be 2,7. Same as before group number 7 and 7 electrons in outer shell.
P1 task 4
4 groups and its main properties
- Transitional metals- These are placed in the centre of the periodic table, most likely to be dense and hard, Transitional metals are reactive but not as much as alkali metals, There are many transitional metals out there but there are a few main ones which are iron, copper, silver and gold these are important metals. List of chemical properties of transitional metals:
- These are hard and tough at most times.
- They can be hammered or bent into shapes very easily, making them malleable.
- Have high melting points due to the fact they are metals
- Mainly formed as coloured compounds
- Can make useful catalysts
- Highly conductor of electricity
- Noble gases- These elements are chemically unreactive in other words inert, They have little trend to gain or lose electrons, The chemical properties of noble gases:
- Fairly no reactive
- They are non metals
- Colourless
- Single atom
- Halogens- contains elements which exist as molecules with pairs of atoms, that is the reason why they diatomic, The chemical properties of Halogens:
- They have low melting and boiling points
- These can get highly reactive with alkali metals and alkaline earths
- Halogens get darker as you go down the elements
- Alkali metals- The alkali metals, found in group 1 of the periodic table, are very reactive metals that do not come about freely in nature. These metals have only one electron in their outer shell. Therefore, they are ready to lose that one electron in ionic bonding with other elements. Chemical properties of alkali metals:
- Have low melting and boiling points
- Having that they have low boiling and melting points I can conclude they are good conductors of heat.
- Good conductors of electricity
- Softer than most metals
M1 task 1
Ionic bonding happens between a metal and a non metal when a metal transfers electrons to a non metal to form ions, Here are some examples of what I mean when they are transferred to form ions:
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calcium + chlorine → calcium chloride
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sodium + chlorine → sodium chloride
Basically the metal atom gives electrons to the non metal to atoms which makes the metal atoms positive ions and non metal atoms to become negative ions.
Here are 2 examples of Ionic bonding which I understand:
- This is ionic bonding between sodium chloride. So see how sodium has got an electron structure of 2,8,1 and the chlorine has got a electronic structure of 2,8,7. So now I know that chlorine needs 1 electron to make its outer shell a full shell, The sodium loses an electron and the chlorine gains the electronic leaving the sodium ion with a positive charge and the chlorine ion negatively charged.
2. Ionic bonding between magnesium oxide, See how the magnesium has an electronic structure of 2,8,2 and oxygen has an electronic structure of 2,6. I know from this magnesium will lose 2 electrons making it postivly charged and the oxygen will gain 2 electrons making it negativly charged
M1 task 3
Ammonia nh3- each nitrogen is bonded to 3 hydrogen’s with 3 lone pairs and they’re fore has the shape trigonal pyramidal with a bond angle of 107.5 degrees. H20 each oxygen is bonded to two hydrogen’s giving a h2o molecule the shape of non-linear with two lone pairs and a bond angle of 105 degrees hence they do not have the same bond angle as methane (ch4) because each carbon is bonded to 4 hydrogen’s and has a bond angle of 109.5 degree so they do not have the same bond angles given that each molecule varies due to electron repulsion.
