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A Level Physical Chemistry > Section 3 - Bonding > Flashcards

Section 3 - Bonding Flashcards

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1
Q

What is Ionic Bonding?

A

Bonding that occurs between Metals and Non-Metals, when ions are held together by electrostatic attraction.

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2
Q

How are ions formed?

A

When one or more electrons are transferred from one atom to another.

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3
Q

Do metals lose or gain electrons when they become ions?

A

They lose them.

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4
Q

Do non-metals lose or gain electrons when they become ions?

A

They gain them.

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5
Q

What is the formula for a sulfate ion?

A

SO₄²⁻

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6
Q

What is the formula for a hydroxide ion?

A

OH⁻

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7
Q

What is the formula for a nitrate ion?

A

NO₃⁻

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8
Q

What is the formula for a carbonate ion?

A

CO₃²⁻

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9
Q

What is the formula for a ammonium ion?

A

NH₄⁺

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10
Q

What is the structure of an ionic bond?

A

A giant ionic lattice.

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11
Q

What is the melting point of ionic bonds?

A

High - lots of strong forces of attraction between +ive and -ive ions.

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12
Q

Are ionic lattices good conductors of electricity?

A

Yes.

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13
Q

How do you make a giant ionic lattice conduct electricity?

A

Make the ions move by heating it up or dissolving it if it can be dissolved.

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14
Q

Why do giant ionic lattices need to be molten or dissolved to conduct electricity?

A

In a solid the ions are fixed by strong ionic bonds.

They need to be free to move and carry a charge.

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15
Q

Do ionic compounds dissolve in water?

A

Generally yes - water molecules are polar and the charged parts on them pull ions away from the lattice.

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16
Q

What is the order of mpts in LiCl, LiBr and LiF? And why?

A

Because LiF is the smallest so has the strongest FoA.

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17
Q

How many Cl- ions is each Na+ bonded to?

A

6

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18
Q

What is Covalent Bonding?

A

Bonding that occurs between non-metals, when two or more atoms share a pair of electrons.

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19
Q

What is a co-ordinate/dative covalent bond?

A

A shared pair of electrons provided by one atom.

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20
Q

What are the two types of covalent bonds?

A

Molecular and Giant Covalent.

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21
Q

What are giant covalent structures?

A

Huge networks of covalently bonded atoms.

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22
Q

What is the structure of graphite?

A
  • Each carbon is covalently bonded to 3 other carbons.

- The 4th outer electron of each carbon is delocalised.

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23
Q

What are the properties of graphite?

A
  • Soft and brittle - layers slide.
  • Conducts electricity - free electrons.
  • Low density - layers are far apart.
  • Very high mpt - very strong covalent bonds.
  • Insoluble - covalent bonds are too strong to break.
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24
Q

What is the shape of graphite?

A
  • Hexagonal planar sheets of bonded carbons.

- Delocalised electrons and Van der Waals between layers.

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25
Q

What is the structure of Diamond?

A
  • Each carbon is bonded to 4 other carbons.

- Not layered.

26
Q

What are the properties of diamond?

A
  • Doesn’t conduct electricity - no free electrons.
  • Insoluble - covalent bonds are too strong to break.
  • Very high mpt - very strong covalent bonds.
  • Extremely hard.
27
Q

What is the shape of diamond?

A

It is arranged in a tetrahedral shape.

28
Q

What is the structure of Iodine?

A

It is molecular.

Pairs of iodine atoms are covalently bonded and held together by weak intermolecular forces.

29
Q

What is Iodine’s mpt/bpt?

A

Low - only need to overcome weak IMFs.

30
Q

What is the structure of Ice?

A

It is molecular - H2O molecules are held together by IMFs between Hs and Os.

31
Q

What is the shape of a molecule/ion with 2 bonding pairs of electrons? And what is the bond angle?

A

Linear. 180.

32
Q

What is the shape of a molecule/ion with 3 bonding pairs of electrons? And what is the bond angle?

A

Trigonal Planar. 120.

33
Q

What is the shape of a molecule/ion with 2 bonding pairs and 1 lone pair of electrons? And what is the bond angle?

A

Bent. 117.5.

34
Q

What is the shape of a molecule/ion with 4 bonding pairs of electrons? And what is the bond angle?

A

Tetrahedral. 109.5.

35
Q

What is the shape of a molecule/ion with 3 bonding pairs and 1 lone pair of electrons? And what is the bond angle?

A

Trigonal Pyramid. 107.

36
Q

What is the shape of a molecule/ion with 2 bonding pairs and 2 lone pairs of electrons? And what is the bond angle?

A

Bent. 104.5.

37
Q

What is the shape of a molecule/ion with 5 bonding pairs of electrons? And what are the 2 bond angles?

A

Trigonal Bipyramid. 90 and 120.

38
Q

What is the shape of a molecule/ion with 4 bonding pairs and 1 lone pair of electrons? And what are the 2 bond angles?

A

Seesaw. 87.5 and 117.5.

39
Q

What is the shape of a molecule/ion with 3 bonding pairs and 2 lone pairs of electrons? And what is the bond angle?

A

Trigonal Planar. 120. (lone pairs working in equal and opposite directions cancel each other out)
Or
T-shape. 85.

40
Q

What is the shape of a molecule/ion with 6 bonding pairs of electrons? And what is the bond angle?

A

Octahedral. 90.

41
Q

What is the shape of a molecule/ion with 5 bonding pairs and 1 lone pair of electrons? And what is the bond angle?

A

Helicopter. 87.5.

42
Q

What is the shape of a molecule/ion with 4 bonding pairs and 2 lone pairs of electrons? And what is the bond angle?

A

Square Planar. 90.

43
Q

What is a good method for working out shapes of molecules?

A
  • Add group number to number of bonds to charge. (a negative charge is a +1 and positive is -1)!!!!
  • Divide answer by 2 to get number of pairs.
  • Calculate how many bonded pairs and how many lone pairs.
44
Q

What is the most electronegative element?

A

Fluorine.

45
Q

What is the general trend in electronegativity?

A

Increases across periods.

Decreases down groups.

46
Q

What is a polar bond?

A

A bond between two atoms of different electronegativities where the electron pair is pulled closer to the more electronegative atom.

47
Q

Is H2 polar?

A

No - it’s non-polar.

48
Q

Is C-H polar?

A

No - C and H have practically the same electronegativity.

49
Q

How are permanent dipoles formed?

A

In a polar bond, the difference in electronegativity causes a delta positive and a delta negative charge.

50
Q

What is a polar molecule?

A

It is a molecule with polar bonds, which causes an uneven distribution of charge across the molecule.

51
Q

What happens if polar bonds are symmetrical in a molecule?

A

The molecule will be non-polar - the charges cancel out.

52
Q

What are the 3 types of IMFs?

A

1) Van der Waals
2) Permanent dipole-dipole forces
3) Hydrogen Bonding

53
Q

What are Van der Waal forces?

A

Instantaneous dipole dipoles.

54
Q

Define electronegativity

A

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

55
Q

When can Hydrogen Bonding occur?

A

When H is covalently bonded to N O or F.

56
Q

How is a dipole formed?

A

When electrons are grouped more on one side of an atom than the other for an instant.

57
Q

How do Van der Waals forces form?

A

An instant dipole causes an instant dipole on a neighbouring atom which causes an instant dipole on the next atom, etc. This causes a constant attraction.

58
Q

Why might a molecule have stronger VdWs and therefore higher mpts?

A
  • Larger molecules = larger electron clouds = stronger VdWs

- Long straight molecules can lie closer together = stronger VdWs

59
Q

What is the strength order of IMFs?

A
  • Hydrogen Bonding
  • Dipole Dipole
  • Van der Waals
60
Q

How does Hydrogen Bonding occur?

A
  • N, O and F are very electronegative
  • They draw electrons away from H creating a polar bond.
  • H has such a high charge density that the atoms form weak bonds with lone pairs on the N O or F.
61
Q

What is the structure of metallic bonding?

A
  • Giant Metallic Lattice
  • The outer shell of electrons of a metal atom is delocalised.
  • There is an attraction between positive metal ions and a sea of delocalised electrons.
62
Q

What are the properties of a metallic bond?

A
  • High melting point - strong FoA
  • The more delocalised electrons, the higher the mpt.
  • Good conductors of heat and electricity - electrons can carry a current.
  • Soft/malleable - layers can slide.
  • Insoluble (except liquid metals) - too strong.

A Level Physical Chemistry (9 decks)

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