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Chemistry - Edexcel - GCSE > Topic 1 - Bonding and Structure > Flashcards

Topic 1 - Bonding and Structure Flashcards

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1
Q

When are atoms most stable?

A

When they have a full outer shell

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2
Q

In which two groups are the bible gases?

A

Group 0 and 8

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3
Q

Why are the Nobel gases so unreactive?

A

Because they all have a full outer shell of 8 electrons

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4
Q

Atoms that do not have a full outer shell will react forming what and why?

A

Chemical bonds with other atoms in order to gain a full outer shell, which is then stable

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5
Q

What are the 3 types of bonding?

A
  • Ionic Bonding
  • Covalent Bonding
  • Metallic Bonding
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6
Q

Ionic bonding forms between what?

A

Metal and non metal atoms

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7
Q

What happens to the electrons in ionic bonding?

A

Involves electrons being transferred to gain full outer shells

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8
Q

Where is ionic bonding found? Give examples:

A

Found in ionic compounds such as sodium chloride (NaCl) and Aluminium Oxide (Al2O3)

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9
Q

What does ionic bonding result in?

A

The oppositely charged ions are attracted together, forming a regular arrangement called a lattice or a giant structure

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10
Q

Covalent bonding forms between what?

A

Non metal atoms

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11
Q

What happens to the electrons in covalent bonding?

A

Involves electrons being shared to gain full outer shells

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12
Q

Where is covalent bonding found? Give examples:

A
  • Found in covalent compounds such as carbon dioxide (CO2) and ammonia (NH3)
  • Also found in some non metal elements e.go H2, Cl2, N2, O2
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13
Q

What does covalent bonding result in?

A

Simple molecular or giant covalent structures

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14
Q

Metallic bonding is formed between what?

A

Metal atoms

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15
Q

What happen to electrons in metallic Bonding?

A
  • The outer shell electrons from each atom become delocalised
  • The structure is held together by the strong electrostatic forces between the positive ions and the “sea” of free electrons
  • This means metals have high melting points
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16
Q

Where is metallic bonding found? Give examples:

A

Found in metals such as potassium (K), copper (Cu), iron (Fe) and aluminium (Al)

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17
Q

What does metallic bonding result in?

A

Giant Metallic structures

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18
Q

Definition of metallic bonding:

A

Metallic bonding is the strong electrostatic attraction between the positive ions and the delocalised electrons

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19
Q

Metals, eg. copper, consist of what kind of arrangement?

A

They consist of a regular arrange to of atoms called a giant structure

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20
Q

What makes metals malleable?

A

The layers of atoms/ions slide over each other when a force is applied but the structure does not break apart because it is held together by the delocalised electrons. This makes metals malleable

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21
Q

What does malleable mean?

A

It can be hammered into shape

22
Q

Why can metals conduct electricity and heat?

A

Due to the delocalised electrons being able to move freely throughout the structure

23
Q

What is an alloy?

A

Alloys are less amoebae than pure metals, so cannot easily be pressed into shape

24
Q

Why are alloys less malleable than pure metals?

A
  • In pure metals, the regular structure of atoms is arranged in layers. When a force is applied, the layers of atoms can slide over each other —> malleable
  • In alloys, there are atoms of other element, disrupting the layers. When a force is applied, the layers cannot slide over each other —> not so malleable
25
Q

What type of Bonding do dot and cross diagrams represent?

A

Ionic and covalent bonding and substances

26
Q

Definition of Ionic Bonding:

A

Ionic Bonding is the strong electrostatic attraction between the positive ions and the negative ions

27
Q

Examples of Ionic Bonding:

A
  • Magnesium Oxide (MgO), made from magnesium (metal) and oxygen (non-metal), therefore must contain ionic bonding
  • Aluminium Fluoride (ALF3), made from aluminium (metal) and fluorine (non-metal), therefore must contain ionic bonding
28
Q

What happens in magnesium oxide as it is Bonding?

A
  • Mg has 2 electrons in its outer shell so needs to lose 2 for a full outer shell
  • O has 6 electrons in its outer shell so needs to gain 2 for a full outer shell

——> 2 electrons from Mg transferred to O ——>

  • Mg has lost 2 negative charges (electrons) so becomes an ion with a charge of +2
  • O has gained 2 negative charges (electrons) from Mg so Beckens an ion with a charge of -2
29
Q

What happens to Aluminium fluoride as it is Bonding?

A
  • Al has 3 electrons in its outer shell so needs to lose 3 for a full outer shell
  • F has 7 Electrons in its outer shell so needs to gain 2 for a full outer shell. 3 F atoms are needed to accept the 3 electrons from the outer shell of Al

——>

  • Al has lost 3 negative charges (electrons) so becomes an ion with a charge of +3
  • The F atoms have each gained 1 negative charge (electron) from Al so become ions with a charge of -1. 3 F ions are needed to balance the 3+ charge on Al and make the compound neutral
30
Q

When do Ionic compounds conduct electricity?

A

When they are molten or in a solution

31
Q

Why do Ionic compounds only conduct electricity when they are molten or in solution and not when solid?

A
  • Because the ions are free to move (many Ionic compounds dissolve in water)
  • Solid ionic compounds do not conduct because the ions are fixed in the lattice
32
Q

What gives Ionic compounds high melting points?

A

Strong electrostatic forces between oppositely charged ions

33
Q

Definition of Covalent Bonding:

A

Covalent Bonding is the strong electrostatic attraction between the nuclei and the shared pair of electrons

34
Q

Example of covalent Bonding:

A
  • Water (H2O), made from 2 hydrogen (non-metal) atoms and 1 oxygen (non-metal) atom, therefore must contain covalent
    bonding
  • Carbon dioxide (CO2), made from 1 carbon (non-metal) atom and 2 oxygen (non-metal) atoms, therefore must contain covalent bonding
  • Fluorine (F2) made from 2 fluorine (non-metal) atoms, therefore must contain covalent bonding. Note that several non-metal elements exist naturally as covalent molecules eg. H2, O2, N2, Cl2, Br2, I2
35
Q

What happen to water when it is bonding?

A
  • H has 1 electron in its outer shell so needs to gain 1 for a full outer shell (the 1st shell only holds 2 electrons
  • O has 6 electrons in its outer shell so needs to gain 2 for a full outer shell

——> pairs of electrons shared ——>

  • The O atom and both H atoms have gained full outer shells by sharing electron pairs. Each electron pair is a single bond, so the structure can also be drawn as H – O – H. The H2O molecule formed is neutral
36
Q

What happens to carbon dioxide when it is Bonding?

A
  • C has 4 electrons in its outer shell so needs to gain 4 for a full outer shell
  • O has 6 electrons in its outer shell so needs to gain 2 for a full outer shell

——> pairs of electrons shared ——>

  • The C atom and both O atoms have gained full outer shells by sharing electron pairs. Each electron pair is a single bond, so the structure can also be drawn as O = C = O. The CO2 molecule formed is neutral
37
Q

What happens to fluorine when it is Bonding?

A
  • F has 7 electrons in its outer shell so needs 1 electron for a full outer shell
  • This is achieved when the 2 F atoms share 1 pair of electrons to form a single covalent bond
38
Q

How do the vast majority of covalent substances exist?

A

As simple molecules

39
Q

What holds the atoms in the molecules together in a covalent substance?

A

Strong covalent bonds

40
Q

What does the weak intermolecular fiefs between the molecules in a covalent substance result in?

A

It results in the molecules being easy to pull apart so that they have low melting and boiling points

41
Q

What charge are the molecules in a covalent substance?

A

Neutral - they cannot carry any electrical charge - covalent substances made up of simple molecules do not conduct electricity

42
Q

How many covalent subsides exist as giant covalent structures?

A

A very small number

43
Q

Give examples of giant covalent structures:

A
  • Silicon dioxide (SiO2)
  • Graphite
  • Diamond
  • Fullerenes

⬆️All different forms of carbon ⬆️

44
Q

Why do covalent structures have high melting and boiling points?

A

Because all giant covalent structures have strong covalent bonds throughout the structure, they need
lots of energy to break these bonds

45
Q

In Diamond, each C atom is attached to how many others?

A

4 others

46
Q

Why is the structure hard in diamond?

A

Because there are string covalent bonds throughout the structure

47
Q

How are the C atoms arranged in graphite?

A

In layers

48
Q

Why can the layers easily slide over one another in graphite?

A

Because there are strong covalent bonds within the layers but only weak intermolecular forces between layers

49
Q

In graphite, each C atom is attached to how many others?

A

3, leaving 1 spade electric in the outer shell of each C atom

50
Q

Why can graphite conduct electricity?

A
  • Because in graphite, each C atom is attached to 3 others, leaving 1 spare electron in the outer shell of each C atom
  • This electron is free to move – it is delocalised enabling graphite to conduct electricity
51
Q

The structure of SiO2 is very similar to which other giant covalent structure, with the same properties?

A

Diamond

Chemistry - Edexcel - GCSE (1 decks)

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