C1-Atomic structure and the periodic table

the relative mass of particles protons, neutrons, and electrons

• 1- proton

• 1 proton

• very small (0-virtually no mass)

Charge of the subatomic particles

• Proton- +1

• Neutron- 0

• Electron- -1

What type of particle is charged

ions

The top number of a Nuclear symbol

Relative Atomic mass

Distillation

simple distillation- good for separating a liquid from a solution if they have very different boiling points

fractional distillation- used to seperated mixtures with or without similar boiling points

Properties of metals

• Metallic bonding

• Strong (hard to break), but can be bent or hammered into different shapes (malleable)

• Great conductors of heat and electricity

• shiny

• High boiling and melting points

Non metal properties

• Different properties to metals

• dull

• Aren’t always solid at room temperature

• Brittle

• Lower density

Trends of group 1

Reaction with Oxygen produces a metal oxide

Reaction with Chlorine produces salt

Reaction with water produces hydrogen gas (violent reaction) metal hydroxide

As you go down:

• Reactivity increases outer electron is more easily lost as it is further away from the nucleus of the atom meaning the electrons attraction to the nucleus is less strong

• Lower melting and boiling points

• higher relative atomic mass soft grey metals

Trends of group 7 (halogens)

Covalent bonding

As you go down:

• become LESS REACTIVE- it’s harder to gain an extra electron, because the outer shell’s further from the nucleus

• Higher melting and boiling points

• higher atomic masses

  Ions are called halides

• Displacement reactions

• Diatomic

Trends of group 0 (noble gases)

Full outer shell makes them non reactive

• All colourless gases at room temperature

• Non flammable

• Boiling points increases as you move down the table (due to greater intermolecular forces between them)