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)

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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)