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A Chemistry IGCSE course > Covalent bonding > Flashcards

Covalent bonding Flashcards

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1
Q

What is covalent bonding?

A

A covalent bond is an electrostatic attraction between the shared pair of electrons and the positively charged nuclei of two atoms

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2
Q

Why do simple covalent structures have low boiling points?

A

They have very low boiling point because the intermolecular forces between the molecules are weak and only need a small amount of energy to overcome.

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3
Q

What are the different types of covalent bonds?

A

Simple covalent
Giant covalent

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4
Q

How are covalent bonds represented?

A

A line between the atoms e.g. h-h

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5
Q

Why are covalent bonds formed?

A

To complete an outer shell

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6
Q

Why when Hydrogen bonds is Hydrogen not helium?

A

Because the identity of an element is based on the number of protons.

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7
Q

Why do bonds make the ions more stable?

A

When a chemical reaction takes place, energy is released leaving the product with less energy making it more stable.

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8
Q

What is the relation of a paired share of electrons to another (in terms of positioning)

A

The shared electrons move as far away as possible, because electrons repel each other

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9
Q

Can water be bent?

A

Water can be bent
Slightly polar ends
electrical charged object to water -> bend

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10
Q

how are double covalent bonds represented?

A

two lines

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11
Q

draw dot and cross diagrams

A
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12
Q

How are covalent structures held together between molecules?

A

Weak intermolecular forces

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13
Q

Trend between melting and boiling point of halogens

A

up the group
higher melting and boiling points

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14
Q

Do covalent ions conduct electricity

A

no except graphene or graphite

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15
Q

Do covalent structures dissolve in water?

A

Covalent structures usually do not dissolve in water.

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16
Q

arrangement in diamond

A

tetrahedral arrangement, giant covalent

17
Q

Graphite structure

A

Graphite’s structure is a bit like a layer structure, but still giant covalent structure with layers in between.

18
Q

structure of C60 fullerene

A

C60 fullerene is a simple covalent structure with a delocalised electron per carbon atom, but they cannot move between molecules.

19
Q

Trend between M(small r) and intermolecular forces

A

Usually intermolecular forces are stronger when there is a higher relative molecular mass but not always.

20
Q

Graphite’s structure

A

Layers with 3 shared electrons and delocalised electrons which means graphite can conduct electricity. There are weak intermolecular forces between the layers making graphite soft.

21
Q

Why is melting point of diamond high(around 4000 degrees celcius)?

A

Diamond has a very high melting point. This is because diamond is in a giant covalent structure (or macro molecular covalent). This means that there are millions of strong covalent bonds between the carbon atoms. This is a strong structure and is hard to break. This means that a lot of energy is needed to break all the bonds.

22
Q

Why does Fullerene have a low melting and boiling point?

A

Fullerene has a low melting point. This is because fullerene is in a simple molecular structure and there are weak intermolecular bonds between the atoms. This means that little energy is needed to overcome these bonds.

23
Q

Explain why simple covalent molecules have:

1) Low melting points
2) Cannot conduct electricity

A

Simple covalent molecules cannot conduct electricity as there are no delocalised electrons or oppositely charged ions. Simple covalent molecules have a low melting point because they have weak intermolecular forces. These forces are weak and easy to overcome.

24
Q

Explain why:

Giant covalent structures have high melting/boiling points?

A
  1. Giant covalent structures have a high boiling point
  2. This is because giant covalent have a giant covalent structure
  3. This means that there are many covalent bonds
  4. These bonds are strong and hard to break requiring a lot of thermal energy to break them
25
Q

List the:

Halogens

(including their colour and state of matter at room temperature)

A
  • Fluorine, yellow, gas
  • Chlorine, green, gas
  • Bromine, orange, liquid (amber gas)
  • Iodine, grey, solid, purple gas
26
Q

what is the bonding and structure of a metal?

A

metallic bond, strong electrostatic forces of attraction between the positive nuclei of the metal and the delocalised electron in the giant metallic lattice

27
Q

Explain why metals have a high boiling point, can conduct electricity, and are ductile/malleable

A
  1. Metals have a high melting point due to the strong electrostatic forces between the positive metal nucleus and the delocalised electron in the giant metallic lattice which is strong. This bond is hard to overcome.
  2. Metals are ductile and malleable. This is because the metal can slide over each other without breaking.
  3. Metals can conduct electricity. This is because of the free delocalised electrons that are free to move and can flow.
28
Q

Define the key term covalent bonding, give examples of simple covalent molecules

A

A covalent bond is electrostatic forces of attraction between the shared pair of electrons and the positively charged nuclei of two atoms

29
Q

Explain why halogens have a similar chemical reactivity

A

They have similar chemical reactivity because they have the same number of electrons on their outer shell. This means that the halogens will all react to gain 1 electron

30
Q

explain why Group 7 elements decrease in reactivity

A

Because the outer electron is further away from the positive nucleus so the force of electrostatic attraction of the nucleus is not as strong decreasing the reactivity.

31
Q

What is displacing? give examples

A

When a more reactive halogen displaces a less reactive halogen to bond with a metal.
2KI + Cl2 -> 2KCl + I2
2Br + Cl2 -> 2KCl + Br2

A Chemistry IGCSE course (16 decks)

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