3.3 Metals
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Define ionic bonding
A strong electrostatic force of attraction between oppositely charged ions
Define metallic bonding
The electrostatic force of attraction between delocalised electrons and positive metal ions
Define giant structure
Lattic of atoms in a cloud//sea of delocatlised electrons
Give the word equation for the reactions of metals and water
(2) Metal + (2) Water –> (2) Metal hydroxide + hydrogen(2)
Give the word equation for the reactions of metals and steam
Metal + steam –> metal oxide + Hyrdrogen
Give the reactivicty series of metals from Potassium to Gold, and the acronym.
Please (Potassium; K) Stop (Sodium; Na) Calling (Calcium; Ca) My (Magnesium; Mg) Zebra (Zinc; Zn) In (Iron; Fe) Class (Copper; Cu) She (Silver; Ag) Grunts (Gold; Au)
Why do metals have high heating//boiling points?
Because all the thermal energy is going into brekaing the ionic bonds in the lattic structure, which are very strong
Are Ionic compounds brittle or malleable and why?
Brittle, because the lattice hits a layer of ions, anf that layer shifts, so when the ions with the same charges line up, the lattic shatters because like charges repel.
Why can’t ionic compounds conduct electricity when they’re in lattic form? (And give what form/s they CAN move in)
Because their ions are bonded together in the lattice. However, ions in solution//motlen state can.
What happens as you move down the periodic table, in terms of ionic bonding and atom structure? [3 points - SIZE, DISTANCE, LOSS]
• As we move down group 1 atomic size increases (SIZE) • Attration decreases between + nucleus and and the - outermost electron. (DISTANCE) • Therefore the atom loses an electron more easily. (LOSS)
Explain how particles are held together in a metal* [3 points]
atoms held together by electrstatic bonds. outer electrons form ‘sea’ (delocalised electrons) that flows freely around the + metal ions (lattic form)
Why are metals excellent conductors?
sea of electrons are free to move. can move about the metal’s network
Define Alloy
a mixture of metals (with at least one other element)
List the 4 most common acids, and give their chemical formulas.
HCl - Hydrochloric acid HNO3 - Nitric acid H2SO4 - Sulphuric acid H3PO4 - Phosphoric acid
Give the displacement reaction equation in the metal a + metal b formula
Metal A + Metal B –> Metal B oxide + Metal A
Give the word equation for the reaction fo a metal and an acid
Acid + metal –> Salt + Hydrogen
Give the test for Hydrogen
Hold a lit splint against the cource of Hydrogen. If there is a squeaky pop, the H is present.
How is a salt compound formed when a metal and an acid react?
when it is displaced from an acid
give the state of acid that is most commonly used
(aq)
Define the term acid
A substance that produces H+ ions when dissolved in water (H+ donor)
name the term for heat given off in a reaction
Exothermic
Define ‘ore’
A metal found in earth’s crust combined with other elements Impure form of metal
Define reduction [2 points]
Loss of oxygen OR gain of electrons
Define oxidation [2 points]
Gain of oxygen OR loss of electrons