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HIGHER CHEMISTRY > 1b)i) - Structure and bonding > Flashcards

1b)i) - Structure and bonding Flashcards

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1
Q

The first 20 elements in the periodic table are categorised according to binding and structure:

A

Metallic - (Li, Be, Na, Mg, Al, K, Ca)
Covalent molecular - (H2, N2, O2, F2, Cl2, P2, S8 and fullerenes C60)
Covalent network - B, C (diamond graphite) Si
Monoatomic - noble gases

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2
Q

What does the strength of metallic bonding depend on?

A

The strength of metallic bonding depends on the number of delocalised electrons per atom

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3
Q

Describe what happens to the strength of metallic bonding along a period and down a group

A

The strength of metallic bonding increases as you go along a period and decreases as you go down a group

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4
Q

What are the melting and boiling points of metals

A

The melting and boiling points of metals varies but is generally high (high hundreds to thousands of degrees C)

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5
Q

What are the noble gases (monoatomic)

A

the noble gases exist as single atoms with forces between the atoms

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6
Q

What are the melting and boiling points of covalent molecular

A

Covalent molecular elements have low melting and boiling points (low hundreds of degrees C)

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7
Q

What are the melting and boiling points of covalent network

A

Covalent network elements have very high melting points and boiling points (perhaps thousands of degrees C)

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8
Q

What are the different forms carbon can exist in

A

Carbon can exist in different forms, diamond and graphite have covalent network structures

Carbon fullerenes are covalent molecular structures c60

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9
Q

What is a covalent bond

A

In a covalent bond, atoms share pairs of electrons. The covalent bond is a result of two positive nuclei being held together by their common attraction for the shared pair of electrons

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10
Q

When is a polar covalent bond formed

A

Polar covalent bonds are formed when the attraction of the atoms for the pair of bonding electrons is different.

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11
Q

What should the electrons be in a covalent bond between two identical atoms

A

In a covalent bond between two identical atoms the electrons must be equally shared as each atom has the same attraction for the bonding electrons

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12
Q

What happens if the bond is between 2 different atoms (polar covalent bonds)

A

If the bond is between 2 different atoms the sharing will NOT be equal. The electrons in the bond will spend more time closer to the more electronegative atom

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13
Q

What are the signs of polar covalent bonds used for

A

(S+) - lower electronegativity

(S-) - higher electronegativity

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14
Q

Ionic bonds

A

Ionic bonds are the electrostatic attraction between positive and negative ions. Ionic compounds form lattice structures of oppositely charged ions

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15
Q

What is the melting and boiling points of noble gases

A

this gives low melting points and boiling points (low hundreds of degrees C)

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16
Q

How to determine which Intermolecular force a compound has

A

Firstly work out if it is , non polar, polar or has H-F H-O H-N bonds

Non polar - London dispersion forces
Polar - London dispersion force , permanent dipole - permanent dipole
Highly polar - London dispersion force, permanent dipole - permanent dipole , hydrogen bond

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17
Q

What is pure covalent bonding (3)

A
  • each atom has the same electronegativity value so no difference
  • this means the electrons will be shared equally
  • this is known as non-polar covalent bonding (pure covalent )
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18
Q

What is another way to say pure covalent bonding

A

Non-polar covalent

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19
Q

What is non polar covalent bonding

A

Non - polar bonding is when the atoms involved have no difference in electronegativity meaning the electrons are shared equally within the bond

  • usually questions with diatomics
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20
Q

When does a polar covalent bond occur

A

When the atoms involved have different electronegativity values, polar covalent bonding occurs

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21
Q

How are the electrons shared in a polar covalent bond

A

This is when the electrons are shared unequally in the bond so one atom has a larger electronegativity than the other

22
Q

What happens as a result of the electrons being shared unequally in a polar covalent bond

A

As the electrons are shared unequally this causes the bond to be partially charged

23
Q

What are partially charged bonds shown by

A

Partially charged bonds are shown by using delta (s-) thingy

24
Q

What will happen to the atom with the higher electronegativity in a polar covalent bond

A
  • The atom that has the higher electronegativity value will pull the electrons closer to itself
    -this causes the atom to become partially negative (delta s-)
25
Q

What will happen to the atom with the lower electronegativity in a polar covalent bond

A

As the electrons in the bond are closer to the atom with the higher electronegativity, this causes the lower electronegativity atom to become partially positive (delta positive)

26
Q

What must each atom be in a polar bond

A

In a polar bond each atom must be partially charged

27
Q

How can a compound with polar bonds be non-polar?

A
  • if the structure has symmetrical structure the polarity cancels out as a whole molecule
28
Q

What happens if a polar molecule is not symmetrical

A

If the molecule is not symmetrical and the atoms have a difference in electronegativity the molecule is said to have a permanent dipole.

29
Q

Permanent dipole

A

This is when each end has a different charge

30
Q

What is ionic bonding instead of sharing of electrons

A

Ionic bonding is a transfer of electrons instead of sharing of electrons

31
Q

What does the bigger the difference in electronegativities make more likely

A

Bigger the difference the more likely they are to be ionic

32
Q

What happens as you move across the bonding continuum

A

As we go across the bonding continuum the ionic character increases so we are increasing the chance of the transfer of electrons opposed to sharing electrons

33
Q

What value is non-polar (pure) covalent on the bonding continuum

A

If the difference in electronegativity is less than 0.5 you’re going to have a non polar covalent bond

34
Q

What value is polar covalent on the bonding continuum

A

If the difference in electronegativity is between 0.5 and 1.7 you will have a polar covalent bond

35
Q

What value is ionic bonding on the bonding continuum

A

If the difference in electronegativity between the two atoms is more than or equal to 1.7 it will be ionic

36
Q

Do metals conduct electricity

A

Metals - copper iron - conducted

37
Q

Do covalent molecular structures conduct

A

Covalent - oil, wax , sugar sulfur - do not conduct

38
Q

Do ionic structures conduct

A

Ionic - conduct in solution

39
Q

What is the term to explain solubility of substances

A

Like dissolve like

40
Q

What happens if the distance is large on the bonding continuum

A

If the distance is large, then the movement of bonding electrons from the element of lower electronegativity to the element of higher electronegativity is complete, this results In the formation of ions

41
Q

What will any compound containing hydrogen and carbon only be

A

Non-polar

42
Q

What are single elements on the bonding continuum

A

Non-polar so only LDFS

43
Q

How do non metal atoms form ions

A

Non metal atoms with high electronegativity gain (accept) electrons to form negatively charged ions

44
Q

How do metal atoms for ions

A

Metal atoms with low electronegativity donate electrons to form positive ions

45
Q

Who to write an ionic formula

A
  • use SVSDF to get the chemical formula
  • determine whether it is non metal or metal
  • determine if it is a positive or negative ion
  • use the valency to get the charge
46
Q

How to ensure you’ve written the write ionic formula

A

Total charge should cancel each other out

If we do not know the valency of transition metals use the number that would cancel it

47
Q

What are ionic bonds

A

Ionic bonds are the electrostatic attraction between positive and negative ions.

48
Q

What type of structure do ionic compounds form

A

Ionic compounds form lattice structures of oppositely charged ions

49
Q

Why are ionic lattices soluble in water

A

Ionic lattices are soluble in water due to attraction between opposite charges

50
Q

What are polar molecules soluble in

A

Polar molecules will also be soluble in water because water is also polar molecule due to partial negative and positive charges

51
Q

What do non polar substances dissolve in

A

Non polar molecules will dissolve in non polar substances but will be insoluble in water because in non polar molecules there are no charged ends to be attracted to

52
Q

What determines melting and boiling points

A

Only Intermolecular forces can determine mp and bp covalent bonds are inside

HIGHER CHEMISTRY (21 decks)

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