chem reactivity of metals

define the term reactive and reactivity series

‘reactive’ easily takes chemical reactions

‘reactivity series’ list of metals from most to least reactive, helps predictions as water and acid or displacement

explain how a metalic bond can gform when ve are free to move

electrons move between positive irons, and. the attractuon between holds the metals together

common properties of metals

• good conductors

• shiny

• malieable

• strong

• solid at room temp

describet he reactions of g1 and g2 metalic elements w water

Both are very reactive, but g1 is more reactive as it only has one valence electron, and g2 only has 2. As we go down the group, it gets weaker as the valence electron is further away from the nucleus and g2 valence electrons may need some heat to react

describe the metal displacement reactions and how tyhey can be used to compare the reactivity of metals

• More reactive metals take the place of the less reactive metal. By testing different metals, we can determine reactivity

• ex zinc +copper sulfate - zinc sulfate +copper ( more reactive than copper)

Describe how the thermite reaction involves the displacement of metals from an oxide compound

Aluminum reacts with iron oxide. Aluminum is more reactive than iron, so it displaces iron from iron oxide, alumina takes oxygen to form aluminum oxide, and molten iron is left behind. This reaction releases a large amount of heat, showing how strongly aluminum reacts with oxygen

how do we test for gas produced in the reaction between metals and water

pop test

why are some metals stored in oil

they are very reactive with water as pol and water do not mix togtehr

why is alluminum made for cans

need direct heat for it to react

what types of metals would be found in nature

unreactiove ones as they will not react to anything around them