3.3 Metals

Question 1

Define ionic bonding

Answer 1

A strong electrostatic force of attraction between oppositely charged ions

Question 2

Define metallic bonding

Answer 2

The electrostatic force of attraction between delocalised electrons and positive metal ions

Question 3

Define giant structure

Answer 3

Lattic of atoms in a cloud//sea of delocatlised electrons

Question 4

Give the word equation for the reactions of metals and water

Answer 4

(2) Metal + (2) Water –> (2) Metal hydroxide + hydrogen(2)

Question 5

Give the word equation for the reactions of metals and steam

Answer 5

Metal + steam –> metal oxide + Hyrdrogen

Question 6

Give the reactivicty series of metals from Potassium to Gold, and the acronym.

Answer 6

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)

Question 7

Why do metals have high heating//boiling points?

Answer 7

Because all the thermal energy is going into brekaing the ionic bonds in the lattic structure, which are very strong

Question 8

Are Ionic compounds brittle or malleable and why?

Answer 8

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.

Question 9

Why can’t ionic compounds conduct electricity when they’re in lattic form? (And give what form/s they CAN move in)

Answer 9

Because their ions are bonded together in the lattice. However, ions in solution//motlen state can.

Question 10

What happens as you move down the periodic table, in terms of ionic bonding and atom structure? [3 points - SIZE, DISTANCE, LOSS]

Answer 10

• 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)

Question 11

Explain how particles are held together in a metal* [3 points]

Answer 11

atoms held together by electrstatic bonds.
outer electrons form ‘sea’ (delocalised electrons) that flows freely around the + metal ions (lattic form)

Question 12

Why are metals excellent conductors?

Answer 12

sea of electrons are free to move.
can move about the metal’s network

Question 13

Define Alloy

Answer 13

a mixture of metals (with at least one other element)

Question 14

List the 4 most common acids, and give their chemical formulas.

Answer 14

HCl - Hydrochloric acid
HNO3 - Nitric acid
H2SO4 - Sulphuric acid
H3PO4 - Phosphoric acid

Question 15

Give the displacement reaction equation in the metal a + metal b formula

Answer 15

Metal A + Metal B –> Metal B oxide + Metal A

Question 16

Give the word equation for the reaction fo a metal and an acid

Answer 16

Acid + metal –> Salt + Hydrogen

Question 17

Give the test for Hydrogen

Answer 17

Hold a lit splint against the cource of Hydrogen. If there is a squeaky pop, the H is present.

Question 18

How is a salt compound formed when a metal and an acid react?

Answer 18

when it is displaced from an acid

Question 19

give the state of acid that is most commonly used

Answer 19

(aq)

Question 20

Define the term acid

Answer 20

A substance that produces H+ ions when dissolved in water (H+ donor)

Question 21

name the term for heat given off in a reaction

Answer 21

Exothermic

Question 22

Define ‘ore’

Answer 22

A metal found in earth’s crust combined with other elements
Impure form of metal

Question 23

Define reduction [2 points]

Answer 23

Loss of oxygen
OR
gain of electrons

Question 24

Define oxidation [2 points]

Answer 24

Gain of oxygen
OR
loss of electrons

Question 25

Define a REDOX rection

Answer 25

the simltaneous reduction and oxidation of species in a chemical reaction.

Question 26

Suggest why sodium wasn't discovered until 1807 [2 points]

Answer 26

It doesn't exist as a pure element – Sodium is highly reactive and always found in compounds (like salt). Lack of technology – Scientists couldn't isolate metals from their compounds before electrolysis was invented.

Question 27

Deifine galvanized

Answer 27

the process of applying a protective zinc coating to steel or iron, to prevent rusting

Question 28

name the main compound in rust

Answer 28

hydrated iron (iii) oxide

Question 29

how are metals with high reactivicty extracted? And why can't they be displaced by carbon?

Answer 29

Electrolosis Used because Carbon is not reactive enough to displace them

Question 30

Why are metals like Ag and Au not needed to be extracted from ores? [2 points]

Answer 30

Because they are chemically unreactve, and a native metal, thereofre can be found as pure elements

Question 31

Define the rterm 'native metal'

Answer 31

Chemically uncombined

Question 32

Explain why Lead can be extracted by heating with carbon

Answer 32

Because Lead is less reactive than Carbon, and can therefore be displaced

Question 33

Define covalent bonding

Answer 33

Where 2 non-metla atoms share a pair of electrons (electrons are in the outer shell of the electrons) An atom that shares 1 or more o its electrons will complete its outer shell

Question 34

What happend when an ionic substance dissolves in water? (short answer)

Answer 34

the ions separate

Question 35

WHy is Ag malleable?

Answer 35

As the layers of ions//particles can slide over each other when a force is applied

Question 36

give the menaing of the acronym OIL RIG

Answer 36

Oxidisation Is Loss Reduction Is Gain

Question 37

What is the chemical name for rust?

Answer 37

The chemical name for rust is hydrated iron(III) oxide

Question 38

Describe the appearance of a rusted iron nail [3 points]

Answer 38

Brown; dull; brittle

Question 39

Here is a list of metals: copper; iron; gold; magnesium; zinc. Which metal is least likely to be found as an uncombined element and why? [2 points]

Answer 39

Gold; it is the least reactive element on the list

Question 40

What accelerates the speed at which iron rusts? [2 points]

Answer 40

salt water; oxygen

Question 41

Magnalium is an alloy of aluminium and magnesium. Explain why it is less malleable than a pure aluminium metal. [2 points]

Answer 41

Any form the following list: - regular arrangement of atoms is distrupted - atoms are different sizes - Harder for atoms to slide over each other

Question 42

Why do metlas have a high melting point? [2 points]

Answer 42

- giant lattice structure - stong bonds within structure; requires lots of thermal energy to break

Question 43

Define sacrificial protection:

Answer 43

Attatch (block of) more reactive metal to the iron. [More reactive metals is attatched to the iron metal. The more reactive metal will corrode before the iron rusts.]

Question 44

true or false: salt increases rusting rate

Answer 44

true