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A Level Chemistry > Bonding: Ionic+ Covalent+ Metallic 2.2.1, 2.2.2 > Flashcards

Bonding: Ionic+ Covalent+ Metallic 2.2.1, 2.2.2 Flashcards

1
Q

What is the structure of a metal

A

Giant Metallic Lattice

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2
Q

Types of particles involved in metallic bonding

A

Positive ions and delocalized electrons

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3
Q

Metallic Bonding= High or Low Melting and Boiling point ?

A

High Melting and Boiling point

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4
Q

Metallic Bonding: Conducts Electricity?

A

Yes, delocalized electrons are free to move and can carry charge

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5
Q

Giant metallic Lattice= Dissolves in water?

A

Doesn’t dissolve in water

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6
Q

Giant metallic Lattice= Dissolves in Covalent Solvents?

A

No

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7
Q

In metallic bonding what is special about the delocalized electrons

A

-delocalized electrons- not attached to one specific atom, they are free to move

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8
Q

How would you describe the Giant Metallic Lattice

A

lattice of regularly spaced positive ions, fixed in position surrounded by delocalized electrons

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9
Q

In metallic bonding are the metal ions able to conduct electricity

A

A metal contains delocalised electrons which are free to move, so it can conduct electricity in solid and molten states

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10
Q

How are the Positive metal ions in Metallic bonding attracted to each other and how does this affect the melting or boiling point

A

Electrostatic forces of attraction between positive ions and negative delocalized electrons.
A large amount of energy is needed to overcome the electrostatic forces so the melting point is high

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11
Q

What would affect the melting and boiling point in a metallic bonding

A

Metals with a high charge density (small ionic radius, high charge) have stronger electrostatic forces between positive ions and negative electrons so more energy is needed to overcome the strong electrostatic forces of attraction therefore increasing the m.p. and b.p.

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12
Q

What structure does Ionic bonding form

A

Giant Ionic Lattice

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13
Q

What types of Particles join to make ionic bonding

A

Positive metal ions and Negative metal ions

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14
Q

In Ionic Bonding is there high or low melting and boiling point

A

High melting + boiling point

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15
Q

In Ionic bonding do the ions conduct electricity

A

Not when solid but yes when Molten, because the negative ions are in a fixed position and are not free to move so cannot carry charge

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16
Q

In ionic bonding are the ions able to dissolve in water

A

Mostly

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17
Q

In Ionic bonding are the ions able to dissolve in Covalent Solvents

A

No

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18
Q

Give an example of a giant ionic lattice

A

NaCl
Sodium Chloride

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19
Q

What does the compound in ionic bonding consist of

A

Ions- cations+ anions, metals and non-metals

Compound contains metal + non-metal unless it contains an ammonium ion

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20
Q

What is an ion

A

A charged particle

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21
Q

What types of ions are there

A

They can be atomic ions e.g. Cl-, Na+

-Or molecular ions e.g. NO3 -, SO4 2-

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22
Q

Metals form…
Non-metals form…
Positive cations and negative anions attract and …

A

-metals form positive ions- cations
-non-metals form negative ions- anions
-positive cations and negative anions attract and form a giant ionic lattice structure

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23
Q

When do ions occur

A

When an element or molecule have either more electrons than protons or fewer electrons than protons

24
Q

Why do ionic compounds not conduct electricity when solid, but do conduct electricity when molten or dissolved in water?

A

-When solid, the ions are in a fixed position in a giant ionic lattice and are not free to move. The solid does not conduct electricity
- When molten or dissolved in water, the ions are free to move and conduct electricity

25
Q

What is ionic Bonding

A

An Ionic bond is the electrostatic force of attraction between oppositely charged ions

26
Q

How are the ions arranged in a Ionic solid

A

In an ionic solid the ions are arranged in a regular 3D pattern called giant ionic lattice

27
Q

Typical Physical Properties of Ionic Compounds

A

High melting points- strong electrostatic forces of attraction between oppositely charged ions int he lattice

Does not Conduct electricity- ions are in a fixed position+ are held together tightly and are not able to move therefore cannot carry charge

-Good conductor of electricity when in solution or molten- ions are free to move and therefore can carry charge when

-Usually soluble in aqueous solvents

28
Q

Which elements are so stable they exist as single atoms

A

Noble gases

29
Q

What can we say about the outer shells of noble gases

A

They have full outer shells and are therefore stable

30
Q

What 2 factors need to be considered when trying to work out the charge density of the ions

A

The charge of the ion and the size of the ion

31
Q

What 2 factors give an ion a high charge density (a high positive or negative charge per unit volume)?

A

-The ion has a small radius
-The ion has a high charge

32
Q

Using the periodic table explain what happens to the ionic radius, for when you are trying to work out charge density

A

Ionic radius decreases across a period, and increases down a group

33
Q

Do ionic compounds have high or low melting and boiling points? Explain why.

A

High melting and boiling point because there is a strong electrostatic force of attraction between the oppositely charged ions , this needs a lot of energy to overcome the ionic bonds and separate the ions

34
Q

How does Charge density (amount of charge per unit volume) of an ion affect the melting or boiling point of the ionic compound?

A

An ion with a high charge density (high charge, small ionic radius) will form stronger ionic bonds. More energy will be needed to overcome the electrostatic attraction between ions to separate the ions. The melting or boiling point will be higher.

35
Q

The strength of the ionic bond increases when the…

A

charge on the ion increases

36
Q

As we move across a period the…

A

ions get smaller

37
Q

As we move down a group…

A

the ions get bigger

38
Q

What happens to the strength of the ionic bond when the ions get smaller

A

When the ions get smaller the ionic bond becomes stronger because there is a higher charge per the ions volume so it has a higher charge density, therefore stronger electrostatic forces of attraction between the bonds which need more energy to overcome the ionic bond and separate the ions

39
Q

What has a higher melting and boiling point, Calcium Chloride or Calcium Fluoride

A

Fluorine is a smaller ion than chlorine and has the same charge however because its a smaller ion and has a high charge density it will take more energy to overcome the ionic bond and separate the ions hence Calcium Fluoride has a higher melting point than Calcium Chloride

40
Q

What 2 processes do we have to consider when an ionic compound dissolves?

A

-Energy taken in by the compound to overcome the electrostatic attractions (ionic bonds) between ions in the lattice, and separate the ions
-Energy given out when intermolecular attractions are made between an ion and surrounding polar water molecules

41
Q

Why is it so hard to predict the solubility of an ionic compound

A

-If an ion has a high charge density, the electrostatic attractions will be stronger
SO
More energy will be needed to break the ionic bonds in the lattice

BUT also
-More energy will be given out when intermolecular attractions are made with water molecules

42
Q

What is the structure of covalent compounds

A

Simple molecular structure

43
Q

Types of particles involved in covalent bonding

A

Non-metal atom and a Non-metal atom

44
Q

Do covalent compounds have high or low melting and boiling points

A

Low melting and boiling points, weak intermolecular forces

45
Q

Do covalent compounds conduct electricity

A

No they do not have delocalized electrons or any ions to move freely and carry charge

46
Q

Can covalent compound dissolve in water

A

No

47
Q

Can covalent compounds dissolve in covalent solvents

A

Yes

48
Q

What is a covalent bond

A

Electrostatic force of attraction between the shared pair of negatively charged electrons and the 2 positively charged nuclei of the non-metal atoms

49
Q

What are lone pairs of electrons

A

Lone pair= pairs of electrons occupying orbital in an atom or molecule but not directly involved in bonding

50
Q

What are bonding pairs

A

Bonding pair= electron pairs of electrons being shared between atoms or molecules

51
Q

What are dative covalent bonds

A

Covalent bonds whereby all the shared pairs of electrons come from one atom

52
Q

What are molecules

A
  • small groups of non metal atoms
  • Can be elements or compounds
  • covalently bonded
53
Q

What is considered a perfect covalent bond

A

When the atoms sharing the pair of electrons have the same radii and the same nuclear charges. The ‘pull’ on the pair of electrons is equal and they are equally shared e.g. H2 O2, N2

54
Q

What is a polar molecule

A

The atoms sharing the pair of electrons have different radii or different nuclear charges. The shared electrons are more attracted to one of the nuclei- therefore one of the atoms gets a partial negative charge- delta minus

55
Q

Define electronegativity

A

The relative ability of an atom to attract the pair of electrons in a covalent bond is called its electronegativity.

56
Q

How can we distinguish electronegativity on a periodic table

A

Electronegativity increases across a period and up the group - Fluorine is the most electronegative element

57
Q
A

A Level Chemistry (10 decks)

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