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Chem 2 (2.2 Electrons, Bonding & Structure) > 2.2.2 Bonding & Structure > Flashcards

2.2.2 Bonding & Structure Flashcards

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1
Q

What are the 3 types of bonding

A

Metallic
Ionic
Covalent

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2
Q

What materials does metallic bonding give rise to

A

Ones with a giant metallic structure

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3
Q

What compounds does ionic bonding give rise to

A

Giant ionic lattice

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4
Q

What 2 structures does covalent bonding give rise to

A

Simple covalent (molecular) structures

Giant covalent (macromolecular) structures

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5
Q

E.g of giant metallic structures

A

All metals on periodic table

Mg, Na, Zn

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6
Q

What’s giant ionic structure made from

E.gs

A

Metal + non metal

E.g NaCl, MgO

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7
Q

What’s simple covalent structure made from

E.g

A

Non metal + non metal

E.g H2O, CO2

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8
Q

What’s giant covalent (macromolecular) structure made from

E.g

A

Non metal + non metal

C- graphite, C-diamond, SiO2 (sand)

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9
Q

What type of melting + boiling points do simple covalent (molecular) structures have

Why

A

Low

As they have weak IMFs

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10
Q

What are electrons like in a metal element

A

They’re delocalised (outer electrons merge + aren’t associated with any one atom no more)

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11
Q

What does metallic bonding involve

A

A lattice of positive ions surrounded by a ‘sea’ of delocalised electrons e.g Mg

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12
Q

How do positive metal ions act towards the sea of delocalised electrons

A

They are attracted to the delocalised electrons by electrostatic attraction

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13
Q

Why is metallic bonding very strong and hard to break

A

As there are no individual bonds to break

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14
Q

Why are metals malleable

A

As the layers can slide over each other

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15
Q

What must particles be like to conduct electricity (2)

A

Carry charge

Move freely

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16
Q

Why can metals conduct

A

As the delocalised electrons are negatively charged and can move

17
Q

What’s the MP + BP of metals like

A

High

The atoms are difficult to separate as there is a strong attraction between the metal ions + the delocalised electrons

18
Q

What’s ionic bonding between

A

A metal + non metal

19
Q

What happens during ionic bonding

A

Electrons are transferred from the metal to the non metal so they can both have a full outer shell

20
Q

What happens to the metal and non metal in ionic bonding

What do they become

A

Metal becomes positively charged
Non metal becomes negatively charged

They become ions

21
Q

What force allows a bond to be formed in ionic bonding

A

Electrostatic attraction

22
Q

What’s an ionic bond

A

Electrostatic force of attraction between positive + negative ions

23
Q

What forms when ionic bonds are made

E.g

A

A giant ionic lattice

E.g NaCl

24
Q

How are the ions positioned in an ionic NaCl diagram

A

Oppositely charged ions are adjacent to each other

25
Q

What’s the melting point like in NaCl

Why

A

High

As each Cl- ion is attracted to Na+ ions so it takes lots of energy to break and is very strong

26
Q

What would need to happen to melt/break NaCl

A

Many strong ionic bonds would need to be broken (strong electrostatic attraction) between oppositely charged ions must be broken

27
Q

When do ionic compounds only conduct

A

They only conduct when molten/dissolved in water as the ionic bonds are broken and ions are free to move

28
Q

When don’t ionic compounds conduct

Why

A

They don’t conduct when solid as the ions can’t move freely although they are charged

29
Q

What’s covalent bonding between

A

Non metal + non metal

30
Q

What happens to the electrons in covalent bonding

A

They’re shared between the non-metals to gain a full outer shell

31
Q

What a covalent bond made from

A

A shared pair of electrons

32
Q

How does a covalent bond work

A

The shared electrons in the pair are attracted to the positive nuclei of both atoms

33
Q

When does a co-ordinate bond form

A

When both electrons are donated from 1 again (donor atom)

34
Q

What does co-ordinate (dative) bonding rely on

A

That the donating atom has an available pair of outer electrons to contribute (lone pair)

35
Q

What’s the co-ordinate bond represented by

A

Arrow

36
Q

What’s the atom that receives the donated electrons in co-ordinate (dative) bonding , said to be

A

Electron deficient

Chem 2 (2.2 Electrons, Bonding & Structure) (4 decks)

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