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Chemistry A level > Bonding > Flashcards

Bonding Flashcards

1
Q

What are ionic bonds?

A

Electrostatic forces of attraction between oppositely charged ions

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2
Q

What are covalent bonds?

A

Shared pair of electrons between atoms

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3
Q

What are metallic bonds?

A

Attraction in a lattice between the positive nuclei of the metal atoms and the negative delocalised outer shell electrons

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4
Q

What does the strength of an ionic bond depend on?

A
  • The smaller the ions, the stronger the attraction between positive and negative ions
  • The greater the charge on the ions, the stronger the attraction between positive and negative ions
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5
Q

What does the strength of a covalent bond depend on?

A
  • The shorter the bond, the stronger the bond
  • Double bonds are stronger than single bonds, triple bonds are stronger than double bonds
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6
Q

What does the strength of a metallic bond depend on?

A
  • The smaller the atoms, the stronger the bonds
  • The more delocalised electrons there are, the stronger the bonds
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7
Q

What is the order of size of some commonly asked about ions? (there are 11)

A

Beryllium
Aluminium
Lithium
Magnesium
Sodium
Calcium
Fluorine
Oxygen
Potassium
Chlorine
Sulfur

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8
Q

What is a co-ordinate bond?

A

A dative covalent bond
Where both the electrons come from the same species
Once formed, they are identical to other covalent bonds

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9
Q

What is the structure of simple molecules?

A
  • They are compounds of a non metal with a non metal
  • The atoms within molecules are joined by covalent bonds however the forces between molecules are very weak
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10
Q

What is the structure of giant covalent molecules?

A

A lattice structure in which all atoms are joined together in a network by covalent bonds

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11
Q

What are the melting and boiling points of giant covalent molecules?

A

Very high as lots of energy is needed to break the many strong covalent bonds

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12
Q

Do giant covalent molecules conduct electricity?

A

Only when there are delocalised electrons in their structure e.g. graphite does conduct but diamond doesn’t

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13
Q

What is the structure of ionic compounds?

A

A lattice structure of positive and negative ions - it’s held together by the strong electrostatic force of attraction between the positive and negative ions

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14
Q

What are the melting and boiling points of ionic compounds?

A

Very high as a lot of energy is needed to break the strong electrostatic forces of attraction

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15
Q

Do ionic compounds conduct electricity?

A

Only when molten or in solution so the electrons are free to carry charge

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16
Q

What is the structure of metallic bonds?

A

Lattice structure of metal atoms where the outer shell electrons from each atom are delocalised and there is a strong attraction between the positive nucleus of the atoms and the cloud of delocalised electrons

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17
Q

What are the melting and boiling points of metallic bonds?

A

Very high as it requires a lot of energy to overcome the strong electrostatic forces of attraction between the positive nucleus of the metal atoms and the delocalised electrons

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18
Q

Do ionic compounds dissolve in water (or any other polar solvent)?

A

Yes, as attractions form between the polar water molecules and the ions

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19
Q

Do ionic compounds dissolve in non polar solvents (e.g. alkanes)?

A

No

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20
Q

Do compounds with hydrogen bonding (like alcohols and simple sugars) dissolve in water?

A

They usually dissolve in water as the hydrogen bonds in the compounds can form attractions through the hydrogen bonds of the water

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21
Q

Do compounds with hydrogen bonding (like alcohols and simple sugars) dissolve in non polar solvents (e.g. alkanes)?

A

Not usually, or they are only slightly soluble

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22
Q

Do non polar substances dissolve in water (or any other polar solvents)?

A

Not usually, or they are only slightly soluble

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23
Q

Do non polar substances dissolve in non polar solvents (e.g. alkanes)?

A

Yes usually, as intermolecular forces form between the solvent and solute molecules

24
Q

Why do molecules have particular shapes?

A

Because pairs of electrons will experience mutual repulsion with other pairs of electrons as they are all negatively charged; this mutual repulsion is minimised when the pairs of electrons are as far away as possible from each other

25
Q

What is the bond angle of a linear molecule?

A

180°

26
Q

What is the bond angle of a trigonal planar molecule?

A

120°

27
Q

What is the bond angle of a tetrahedral molecule?

A

109.5°

28
Q

What are the bond angles in a trigonal bipyramidal molecule?

A

90°
120°

29
Q

What is the bond angle of an octahedral molecule?

A

90°

30
Q

What is the bond angle of a bent molecule?

A

104.5°

31
Q

What is the bond angle of a T-shaped molecule?

A

87.5°

32
Q

What is the bond angle of a trigonal pyramidal molecule?

A

107°

33
Q

What are the bond angles of a seesaw shape molecule?

A

102°
86.5°

34
Q

What is the bond angle of a square planar molecule?

A

90°

35
Q

What is the bond angle of a square pyramidal molecule?

A

90°

36
Q

What can reduce bond angles?

A

Lone pairs as they repel more than bonding pairs

37
Q

What is the definition of electronegativity?

A

The power of an atom to attract the two electrons in a covalent bond

38
Q

How does nuclear charge affect electronegativity?

A

The negative electrons in the bonding pair are attracted to the nucleus, so the more protons the stronger the attraction

39
Q

How does atomic radius affect electronegativity?

A

The closer the bonding pair to the nucleus, the stronger the attraction so the smaller the radius, the greater the electronegativity

40
Q

How does shielding affect electronegativity?

A

The more shells between the bonding pair and the nucleus, the weaker the attraction because the more shells there are, the greater the repulsion is between the nucleus and the bonding pair

41
Q

What is the trend in electronegativity down a group and why?

A

It decreases because
- atoms get bigger
- more shielding
therefore weaker attraction between the bonding pair and the nucleus

42
Q

What is the trend in electronegativity across a period and why?

A

It increases because
- atoms get smaller
- greater nuclear charge / more protons
therefore stronger attraction between the bonding pair and the nucleus

43
Q

When does a non-polar covalent bond occur?

A

When the two atoms in a covalent bond have the same electronegativity and the two electrons are shared equally

44
Q

When does a polar covalent bond occur?

A

When the two atoms in a covalent bond have a different electronegativity and the two electrons are not shared equally

The more electronegative atom has a greater share of the two electrons

45
Q

What is a bond dipole moment?

A

It’s a measure of the strength and direction of the polarity in the bond of polar molecules
The bigger the difference in electronegativity, the bigger the bond dipole moment

46
Q

What shapes of molecules may be non polar overall despite having polar bonds?

A

Linear, trigonal planar, tetrahedral or octahedral

47
Q

What are Van der Waal’s forces and why do they occur?

A

Because electrons in an atom are always moving around, at any moment they are unlikely to be evenly spread, giving the atom or molecule a temporary dipole
This temporary dipole will induce a temporary dipole in a neighbouring atom by repelling / attracting its electron charge cloud

48
Q

What is the weakest kind of molecular force?

A

Van der Waal’s

49
Q

Are Van der Waal’s forces in every molecule?

A

Yes

50
Q

What can increase the magnitude of Van der Waal’s forces?

A

The forces increase as the size of the molecule increases
The strength of the forces is also larger in straight chain molecules as they can pack closer together

51
Q

What is hydrogen bonding?

A

The attraction between a lone pair of electrons on the N, O or F to the H on a neighbouring molecule

52
Q

What is the strongest kind of intermolecular force?

A

Hydrogen bonding

53
Q

Why does hydrogen bonding occur?

A

Because there is a strong attraction from the lone pair on the N / O / F of one molecule to the exposed H nucleus of another molecule because it only has one electron

54
Q

When does permanent dipole-dipole attraction occur?

A

Between polar molecules
(Permanent dipole-dipole attraction doesn’t occur when the overall molecule is non polar despite having polar bonds)

55
Q

What is the kinetic energy of particles directly proportional to?

A

The temperature

Chemistry A level (3 decks)

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