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Chemistry > C3 - Bonding > Flashcards

C3 - Bonding Flashcards

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1
Q

An ionic bond occurs between what atoms?

A

A metal and a non-metal atom

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2
Q

A covalent bond occurs between what atoms?

A

2 non-metal atoms

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3
Q

A metallic bond occurs between what atoms?

A

2 metal atoms

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4
Q

In ionic bonds what are the 2 atoms attracted by?

A

Electrostatic force

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5
Q

Ionic compounds exist in what structure and why?

A

Lattices
It forms because each ion is electrostatically attracted in all directions to ions of the opposite charge.

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6
Q

In covalent bonds what are the 2 atoms attracted by?

A

Electrostatic force

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7
Q

What is a dative/co-ordinate bond?

A

A dative covalent bond is a covalent bond in which a shared pair of electrons has been supplied by one of the bonding atoms only.

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8
Q

How is a dative bond shown in a dot and cross diagram?

A

By → or ← with the arrow coming from the atom that provided the electrons

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9
Q

In metallic bonds what are the 2 atoms attracted by?

A

Electrostatic force between the metal ions and the electrons

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10
Q

How does metal ion size affect the strength of metallic bonds?

A

The smaller the metal ion, the closer the positive nucleus is to the delocalized electrons. This means there is a greater attraction between the two, which creates a stronger metallic bond.

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11
Q

Do ionic structures conduct electricty?

A

They conduct electricity when molten or dissolved in water as the ions are free to move

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12
Q

Do metallic structures conduct electricty?

A

They conduct electricity when solid or molten due to movement of delocalised electrons

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13
Q

Do marcomolecular structures conduct electricty?

A

They do not apart from graphite in a solid

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14
Q

Do molecular structures conduct electricty?

A

Does not conduct electricty as there are no charged particles

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15
Q

What is the boiling and melting point of ionic structures?

A

High as breaking strong ionic bonds requires lots of energy

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16
Q

What is the boiling and melting point of metallic structures?

A

High as breaking electrostatic forces of attraction requires lots of energy

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17
Q

What is the boiling and melting point of macromolecular structures?

A

Very high as they have many strong covalent bonds

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18
Q

What are the properties of ionic structures?

A

Hard due to strong electrostatic forces of attraction that hold ions together

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19
Q

What is the boiling and melting point of molecular structures?

A

Low as they are small structures with weak bonds

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20
Q

What is a molecular structure?

A

Simple covalent

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21
Q

What are the properties of metallic structures?

A

Malleable and Ductile as layers slide over each other

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22
Q

What are the properties of macromolecular structures?

A

Varies depending on the structure
E.g. rigid and hard for diamond but brittle for graphite

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23
Q

What are the properties of molecular structures?

A

Brittle as they don’t have strong bonds holding them together

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24
Q

What is macromolecular structure?

A

Giant covalent structure

25
Q

What is a bonding pair?

A

A pair of electrons in a covalent bond

26
Q

What is a lone pair?

A

Pairs of electrons that are not involved in bonding

27
Q

What is bond length?

A

The distance between the nuclei of two bonded atoms

28
Q

What is bond angle?

A

Angle between two covalent bonds

29
Q

What is a linear shaped molecule?

A

2 bonding pairs around the central atom, with the 2 pairs at an angle of 180*
As well as 2 bonding pairs and 3 lone pairs

30
Q

What is a traigonal planar shaped molecule?

A

3 bonding pairs around the central atom, with all 3 bonds on the same plane and a bond angle of 120*

31
Q

What is a tetrahedral shaped molecule?

A

4 bonding pairs around the central atom, with a bond angle of 109.5*

32
Q

What is a trigonal bipyramid shaped molecule?

A

5 bonding pairs around the central atom, 3 pairs in 1 plane have a bonding angle of 120, the 2 other pairs are 90 to this plane. (triagonal planar with one above and one below)

33
Q

What is a octahedral shaped molecule?

A

6 bonding pairs around the central atom, bond angle of 90* between all the bonds.

34
Q

How is the number of lone pairs calculated?

A

Total number of electron pairs - number of bonding pairs

35
Q

What is a pyramidal shaped molecule?

A

3 bonding pairs, 1 lone pair, bond angle of 107*

36
Q

What is a bent shaped molecule?

A

2 bonding pairs, 2 lone pairs, bond angle of 104.5*

37
Q

What is a T-shaped molecule?

A

3 bonding pairs, 2 lone pairs, bond angle of 86*

38
Q

What is a square planar shaped molecule?

A

4 bonding pairs, 2 lone pairs, bond angle of 90*

39
Q

What is electronegativity?

A

The ability of an atom to attract a bonded pair of electrons in a covalent bond

40
Q

If one atom is more electronegative than another in a covalent bond which atom are the electrons closer to?

A

The more electronegative atom

41
Q

What direction does electronegativity increase in the periodic table?

A

Increases going from bottom left to top right, with fluorine being the most electronegative
Increases across a period, Decreases down a group

42
Q

What 3 factors is electronegativity dependent on?

A

Atomic number
Atomic radius (shielding)

43
Q

If an atom has its electrons closer to itself than the other atom (is more electronegative) what is its charge?

A

δ- (delta negative) This means it has a slight negative charge

44
Q

If an atom is has its electrons further away and closer to the other atom (is less electronegative) what is its charge?

A

δ+ (delta positive This means it has a slight positive charge

45
Q

What happens if the electronegativity of both atoms in a covalent bond is identical?

A

The electrons in the bond will be equally attracted to both of them. This results in a symmetrical distribution of electron density around the two atoms. So a non-polar bond is formed

46
Q

What happens if the electronegativity of atoms in a covalent bond are different?

A

An asymmetrical distribution of electron density is created as one attracts electrons more strongly.

47
Q

What is an imbalance in the charges in the bond called?

A

A dipole

48
Q

If the electronegativity difference is 0 what is the bond type?

A

Covalent bond

49
Q

If the electronegativity difference is between 0 and 1.8 what is the bond type?

A

Polar covalent with more ionic character the higher the difference

50
Q

If the electronegativity difference is 1.8 or higher what is the bond type?

A

Ionic bond

51
Q

How are the bonds arranged in a non-polar molecule?

A

The polar bonds are symmetrical and the partial charges will cancel out

52
Q

How are the bonds arranged in a polar molecule?

A

The polar bonds are asymmetrical and the partial charges will not cancel out

53
Q

What are the 3 types of bonding between dipoles?

A

Van der Vaal forces
Permanent dipole dipole forces
Hydrogen bonds

54
Q

What are Van der Vaals forces

A

Forces of attraction due to induced dipole–dipole forces caused by movement of electrons in atoms and molecule

55
Q

How can a Van der Vaal force be stronger?

A

By being a bigger molecule with more electrons

56
Q

What are permanent dipole dipole forces?

A

Intermolecular force between 2 polar molecules and their δ+ and δ- charges

57
Q

How can permanent dipole dipole forces be stronger?

A

A higher electronegativity difference which makes the charges more positive or negative

58
Q

What is a hydrogen bond?

A

The attraction between a lone pair of electrons on one electronegative atom and an H atom bonded to either N, O of F

Chemistry (21 decks)

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