3.1.1.3 Metallic Bonding & Melting Point Flashcards Preview

Chemistry - 3.1 The periodic table and energy > 3.1.1.3 Metallic Bonding & Melting Point > Flashcards

Flashcards in 3.1.1.3 Metallic Bonding & Melting Point Deck (13)
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1

What is metallic bonding

Its the electrostatic interactions between positive metal ions and delocalised electrons

2

How are the atoms in metallic bonding

they are ionised:
> Positive ions occupy fixed position in a lattice
> the outer shell electron are delocalised - they are shared between all the atoms in he metallic structrure

3

What are the three properties of giant metallic structure?

> High melting & boiling point
> Good electrical conductor
> Malleable & Ductile

4

Describe giant metallic structure as having high melting & boiling point

Due to the attraction between the positive ions and negative electrons therefore high temp is needed to overcome the metallic bonds

5

Describe giant metallic structure as a good electrical conductor

as delocalised electrons can move anywhere within the lattice, allowing the current to flow

6

Describe giant metallic structure as Malleable & Ductile

as the atoms are able to roll over one another and go into a new position without breaking the metallic bond.

7

How are solid giant covalent lattices of carbon ( Diamond, Graphite and graphene) and silicon bonded by?

They are networks of atoms bonded by strong covalent bonds

8

What structure do period 2 & 3 elements have Li, Be, Na, Mg, Al

> Structure: Giant metallic
> Forces: Strong attraction between the positive ions and negative electrons
> Bonding: Metallic

9

What structure do period 2 & 3 elements have B, C, Si

> Structure: Giant covalent
> Forces: Strong forces between atoms
> Bonding: Covalent

10

What structure do period 2 & 3 elements have N2, O2, F2, Ne, P4, S8, Cl2, Ar

> Structure: simple molecular
> Forces: Weak intermolecular forces between molecules
> Bonding: Covalent bonding within molecules, intermolecular bonding between molecules

11

What happens to the melting point between group 1 and 14?

Melting point increases as they have giant structures.
> If an element has a giant metallic structure the Nuclear charge increases & the number of electrons in the outer shell which causes a stronger attraction
> If it has a giant covalent lattice, each successive group has more electrons with which to form covalent bonds

12

What happens to the melting point between group 14 and 15?

Decrease in melting point. This is because the element have simple molecular structures - each individual molecule is attracted to other by relatively weak intermolecular forces

13

What happens to the melting point between group 15 and 18?

The melting points remain relatively low - the element have simple molecular structures