periodic patterns of melting points, electrical conductivity, IE

periodic patterns of melting points, electrical conductivity, IE

By Yosefina Rahayu

the explanation will be depending on the bonding and structure of the elements

​

check table 10.5

​pattern of melting point

Multiple Select

check on Na to Al.

what are the reason(s) behind the increase in their melting point?

• metallic bonding from Na to Al is getting stronger

• Na donates 1 electron, while Al donates 3 electrons

• Na to Al have strong giant covalent structure

• more delocalized electrons in Al compared to Na

• increasing charge on the metal ions in the giant metallic lattice

electrical conductivity of Na-Al

similar to melting point, electrical conductivity is increasing from Na to Al, due to:

1. increase in no of electrons donated to the sea of delocalized electrons

2.​

Subject | Subject

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Multiple Select

tick on the boxes below, why Si (silicon) has the highest melting point?

• giant molecular structure

• giant ionic structure

• strong covalent bond (each Si connects to 4 other Si atoms)

Multiple Select

how about silicon's electrical conductivity?

tick some correct statements below

• Silicon is semimetal or metalloid

• has no delocalized electrons

• silicon is a very good electrical conductor

• silicon is able to conduct electricity when it is doped with other element

Multiple Select

melting point of Phosphorus to argon.

describe the reason why it has the shape as shown below

• P4, S8, Cl2 and argon are all non metal, with relatively small molecules

• they have giant covalent structure

• the covalent bond is strong but they have weak instanteneous dipole - induced dipole

​- Name of Author

" Replace this with a quote, words full of wisdom that someone important said and can inspire the reader. " 

decrease mp

Cl2 is smaller than S8

Ar exists as monoatomic gas

weaker id-id force​

​S8 to Cl2 to Ar

increase m.p

as molecules get bigger, more electrons present

stronger instantaneous dipole-induced dipole​

P4 to S8

P4 to S8 to Cl2 to Ar

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all of the nonmetals elements, from P4 to Ar are non electrical conductor

no delocalized electrons are present

Subject | Subject

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Multiple Choice

define ionisation energy

• energy needed to remove one mole of electron from its outermost shell in its gaseous state

• energy needed to remove one mole of electron from its outermost shell in its liquid state

• energy needed to remove one mole of electron from its outermost shell in its solid state

IE increases due to

1. increasing nuclear charge

2.electrons are filling the same shell/energy level /similar shielding effect

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across the period

IE decreases due to

1. increasing shielding effect/increasing quantum shell

2. increase shell has outweighed the increase in nuclear charge

3. weaker force of attraction​

​down the group

have it a review from section 2.6

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Multiple Select

why is there is dip from Be to B (which is similar to Mg to Al)?

• presence of p orbital in B (2s² 2p¹) or Al (3s² 3p¹)

• p orbital is slightly further from nucleus

• weaker force of attraction in B or Al

• spin spin paired repulsion in p orbital

Multiple Choice

why is there is dip from N to O (which is similar to P to S)?

• presence of p orbital in B (2s² 2p¹) or Al (3s² 3p¹)

• spin spin paired repulsion in p orbital in O or S