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AQA As Level Chemistry Unit One > Bonding > Flashcards

Bonding Flashcards

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0
Q

How are ionic compounds held together?

A

Electrostatic attraction between oppositely charged ions

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1
Q

What are ions and how are they removed?

A

When electrons are transferred from one atom to another

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2
Q

What crystal are giant ionic lattices?

A

Ionic crystals

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3
Q

Why is if called a ‘giant’ ionic lattice?

A

It is made up of the same basic unit repeated over and over

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4
Q

What is the electrical conductivity in ionic compounds?

A

Conduct electricity when they’re molten or dissolved

The ions are free to move then

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5
Q

What is the melting point of ionic compounds?

A

High melting points - strong electrostatic forces of attraction between oppositely charged ions, taking lots of energy to overcome

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6
Q

What is the solubility of ionic compounds?

A

Ionic compounds tend to dissolve in water. This is because water is polar and it pulls the ions away from the lattice causing it to dissolve

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7
Q

What are covalent bonds?

A

Two or more atoms sharing elections to gain a full outer shell. Both nuclei are electrostatically attracted to their sharing electrons

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8
Q

What is the electrical conductivity of simple covalent compounds?

A

Do not conduct electricity because there are no free ions to carry the charge

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9
Q

What is the melting point of simple covalent compounds?

A

Low melting points because the weak forces between molecules are easily broken

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10
Q

What are simple covalent compounds?

A

Strong covalent bonds between molecules but weak forces between molecules

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11
Q

What is the solubility of simple covalent compounds?

A

Some dissolve depending on how polarised the molecules are

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12
Q

What crystal type are simple covalent compounds?

A

Molecular crystal

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13
Q

What is another name for giant covalent structures?

A

Macromolecular structures

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14
Q

Describe the structure of graphite

A

Arranged in sheets of flat hexagonal carbon atoms. Each carbon is bonded to three others. The fourth outer electron of each carbon is delocalised. Each layer of atoms is held together by weak van der vaals forces

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15
Q

Why is graphite a good lubricant?

A

Layers can slide over each other due to weak van der vaals forces that are easily broken

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16
Q

What is the melting point of graphite?

A

High due to the strong covalent bonds

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17
Q

Can graphite conduct electricity?

A

Yes due to the delocalised electrons that are able to carry an electrical current

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18
Q

Is graphite soluble?

A

No as the covalent bonds are difficult to break

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19
Q

Why does graphite have a low density?

A

Layers are quite far apart compared to the length of the covalent bonds

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20
Q

Describe the structure of diamond?

A

Each carbon is covalently bonded to four others. This means they are arranged in a tetrahedral shape

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21
Q

What is the crystal of giant covalent structures?

A

Giant covalent?

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22
Q

What is the melting point of diamond and it’s hardness?

A

Extremely high, and extremely hard. This is because of strong covalent bonds

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23
Q

What is the electrical conductivity of diamond?

A

Does not conduct electricity. No ions and outer electrons are held in localised bonds

24
Q

What is the solubility of diamond?

A

Does not dissolve, strong covalent bonds

25
Q

Is diamond a good or bad thermal conductor?

A

Good, vibrations travel easily through the stiff lattice

26
Q

What is dative covalent bonding?

A

Also known as co-ordinate bonding, one of the atoms provides both of the shared electrons

27
Q

How do you identify dative covalent bonding in a molecule?

A

Identify the atom with the lone pair of electrons, this is the one that provides the bonding electrons

28
Q

What are charge clouds?

A

An area where there is a big chance of finding an electron pair

29
Q

Give two examples of where you will find a charge cloud

A

In bonding electrons

Lone pairs of electrons

30
Q

What electron pairs repel the most to least?

A

Lone pair and lone pair repel the most
Lone pair and bonding pair the second most
Bonding pair and bonding pair the least

31
Q

What is the bond angle of a molecule that look likes this:

O=S=O. This has one lone pair of electrons

A

120o

32
Q

What is electronegativity?

A

The tendency for atoms to attract bonding electrons towards itself in a covalent bond

33
Q

What is the most electronegative element?

A

Fluorine

34
Q

What is a polar bond?

A

In a polar bond, the difference in electronegativity between two atoms causes a dipole - slight differences in their charges caused by a shift in electron density in the bond

35
Q

If the difference between two bonding atoms’ electronegativity is greater, what affect does this have on how polar the bond is?

A

The greater the difference in electronegativity, the more polar the bond

36
Q

What is a dipole?

A

A difference in the charge between two bonding atoms caused by a shift in electron density in the bond

37
Q

What are intermolecular forces?

A

Forces between molecules

38
Q

Name the three types of intermolecular bonding

A

Van der waals
Dipole-dipole
Hydrogen bonds

39
Q

How are van der waals forces caused?

A

These are in all atoms and molecules. At any moment, the electrons are more likely to be on one side than the other. At this point, a temporary dipole is cause. This causes another temporary dipole in an adjacent molecule/atom which are attracted to each other.
Due to the constant movement of electrons, all the dipoles are only temporary

40
Q

What are permanent dipole-dipole forces?

A

The positive and negative delta charges cause weak electrostatic forces of attraction between molecules (it’s in HCl)

41
Q

What is hydrogen bonding?

A

It only occurs when hydrogen is covalently joined to fluorine oxygen or nitrogen. These are very electronegative so draw the bonding electrons away from the hydrogen atom. The bond is so polarised and as hydrogen has such a high charge density because it’s so small, the hydrogen forms weak bonds with the lone pair of electrons in the F O or N

42
Q

Put van der waals, hydrogen bonding and dipole-dipole in order from strongest to weakest intermolecular bonds

A

Hydrogen bonding
Dipole-dipole
Van der waals

43
Q

What effect do intermolecular forces have on molecules?

A

Increase melting or boiling point (hydrogen is strong) so require more never to break

44
Q

Why doe HI have a higher boiling point than HBR?

A

HI is a larger molecule, with more electrons and therefore will have more dipoles and van der waals forces, requiring more energy to over come

45
Q

Put these in order of highest to lowest boiling point:

HBR, HI, HF, HCl

A

HF
HI
HBr
HCl

46
Q

Describe the structure of metals

A

Metals exist as giant metallic lattice structures. The outermost shell of electrons of a metal is delocalised. This leaves positive metal ions in a sea of delocalised electrons

47
Q

What is the bonding in metals?

A

Positive metal ions attracted to sea of delocalised electrons

48
Q

What is the melting point of metals?

A

Amount of delocalised electrons have an effect on the metals boiling point. The more there are, the stronger the metallic bond due to greater electrostatic forces of attraction, the higher the melting point.

49
Q

How able to be shaped are metals?

A

Layers of metallic ions can slide over each other meaning they are malleable and ductile

50
Q

What does malleable mean?

A

The ability something has to be shaped

51
Q

What does ductile mean?

A

The ability for something to be drawn into a wire

52
Q

What is the electrical conductivity of metals?

A

Delocalised electrons can carry a charge so they make good electrical conductors

53
Q

What is the thermal conductivity of metals?

A

Delocalised electrons can pass kinetic energy to each other, making them good thermal conductors

54
Q

What is the solubility of metals?

A

Insoluble accept in liquid metals, due to strength of metallic bonds

55
Q

Who and when developed the periodic table?

A

Dmitri Mendeleev, 1800’s

56
Q

What do the periods show in the periodic table?

A

Elements within a period have the same number of electron shells

57
Q

What do the groups in the periodic table show?

A

Elements in the same group have the same number of electrons in the outer shell so they have similar chemical properties

AQA As Level Chemistry Unit One (6 decks)

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