P1 Task 1

Task 1 (P1)

The periodic table is laid out into groups and periods. They are also put into different blocks S-Block, D-Block, P-block and F-Block due to their energy levels. They are organised by their energy levels and chemicals properties. As the elements go along the periods in the periodic table the electronegativity increases but as the elements go down the groups the electronegativity decreases. Ionizing energy also increases as the elements go across the periods and also decreases when the elements go down the groups. The atomic radius does the opposite of electronegativity and ionization; it decreases as the elements go across the periods and increases when the elements go down the groups. The electronegativity increases as you go across the periods because the elements nucleus gains 1 more proton which means more protons more power to attract the electrons, the electronegativity decreases as you go down the groups because an extra shell is added every time this then causes an increase in nuclear charge due to more protons being added. This means that the nucleus is less able to attract electrons. Ionizing energy increases across a period because as the atoms radii is getting smaller the electrons get closer to the nucleus which creates a greater attraction for the electrons making it harder to remove them.

Covalent bonding - Covalent bonding is when two atoms share electrons this can only occur between two non-metals. They share electrons to fill up their outer shells, this makes the atoms stable. A Covalent bond can form up to one to three Covalent bonds with non-metals depending on how much electrons they possess. They don't always share electrons