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chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

How do you work out what IMF a molecule has ?

A

If it has O/N/F to H bond it is hydrogen bond
If not is it polar
Yes permanent dipole dipole
No induced dipole dipole

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2
Q

What is the formula for hydrogen carbonate ?

A

HCO3 -

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3
Q

What is the formula for carbonate ?

A

CO3 2-

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4
Q

What is the formula hydroxide ?

A

OH -

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5
Q

How do van der waal forces arise ?

A

There is random movement of electrons in a molecule leads to a uneven distribution of electrons which forms a temporary dipole this induces a temporary dipole on neighboring molecules which causes molecules to attract.

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6
Q

How do you work out if a molecule is polar ?

A

If the central atom is bonded to more than one type of atom e.g. CHCl3
If there is any lone pairs
If either is true then molecule is asymmetrical
Dipoles don’t cancel
Molecule is polar

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7
Q

Draw the structure of sodium.

A

2 rows of 3 +1 ions surrounded be e-

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8
Q

Draw NH3 giving bond angle and stating shape.

A

Use notes

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9
Q

Draw BeCl2 giving bond angle and stating shape.

A

Use notes

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10
Q

What is a lattice ?

A

Regular arrangement of particles.

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11
Q

What is the formula for dichromate ?

A

Cr2O7 2-

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12
Q

What is the formula for sulphate ?

A

SO4 2-

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13
Q

Draw SF6 giving bond angle and stating shape.

A

Use notes

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14
Q

What is a ionic bonding ?

A

ionic bond is strong electrostatic attraction between oppositely charged ions.

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15
Q

What is the most electronegative atom and why ?

A

F
Has low shielding
Has High nuclear charge

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16
Q

What are the IMf in CHCl3

A

Permanent dipole dipole

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17
Q

What is a non-polar bond ?

A

Bond where there is no difference in electronegativity between atoms.

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18
Q

Why does electronegativity increase across group 2 ?

A

Shielding remains the same
Nuclear charge increases
Therefore ability to attract electron in a covalent bond increases

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19
Q

What structure do ionic bonds form and draw it.

A

Giant ionic lattice
3D cube with + and - ions

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20
Q

Draw SF4 giving bond angle and stating shape.

A

Use notes

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21
Q

What are the IMF in NH3

A

Hydrogen bonding

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22
Q

What is the formula for phosphate ?

A

PO4 3-

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23
Q

What is a coordinate bond ?

A

A coordinate bond is a shared pair of electrons which come from the same atom.

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24
Q

Draw IF3 giving bond angle and stating shape.

A

Use notes

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25
Q

What is the bonding for simple molecular structure ?

A

Intermolecular Forces

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26
Q

What non-metals form a macromolecular structure ?

A

Carbon
Silicon
Silicon dioxide

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27
Q

Describe graphite.

A

Layers of Carbon with 3 covalent bonds
Each carbon has a delocalized electron
Layers held by weak intermolecular forces
conductor
High mp

28
Q

Draw ClF5 giving bond angle and stating shape.

A

Use notes

29
Q

Draw Hydrogen bonding ?

A

Use notes

30
Q

How does Hydrogen bonding arise ?

A

Very large difference in electronegativity between H and O/N/F
Creates a dipole on O/N/F - H
Lone pair on the atom strongly attracts a partially positive hydrogen atom in a different molecule.

31
Q

Draw KrF2 giving bond angle and stating shape.

A

Use notes

32
Q

what bonds form hydrogen bonds ?

A

H-F
H-O
H-N

33
Q

What is the structure of metallic bonding ?

A

Giant metallic lattice.

34
Q

How do permanent dipole dipole forces arise ?

A

Difference in electronegativity leads to bond polarity
dipoles don’t cancel giving a permanent dipole
There is attraction between δ- and δ+ in different molecules.

35
Q

What are the three types of intermolecular forces ?

A

Van der waal/Induced dipole dipole forces
Hydrogen bonding
permanent dipole dipole forces

36
Q

Draw permanent dipole dipole forces.

A

use notes

37
Q

What is a coordinate bond represented by ?

A

A arrow.

38
Q

What does it mean when a atom in a molecule δ-/δ+

A

It is slightly +/-

39
Q

What is the formula for chlorate (V)

A

ClO3 -

40
Q

Draw CCl2 giving bond angle and stating shape.

A

Use notes

41
Q

Draw a dot and cross diagram for oxygen.

A

each O has 2 lone pairs and 2 bonding pairs which forms a double bond.

42
Q

What is the formula for nitrate (V) ?

A

NO3 -

43
Q

Is NH3 polar or non-polar and why ?

A

Polar
Carbon is bonded to only H
Has one lone pair
Molecule is asymmetrical
Dipoles don’t cancel
Molecule is polar

44
Q

What structure do covalent bonds form ?

A

Simple molecular.

45
Q

Draw XeF4 giving bond angle and stating shape.

A

Use notes

46
Q

Draw CH4 giving bond angle and stating shape.

A

Use notes

47
Q

Why is the bonding in magnesium stronger than the bonding in sodium ?

A

Magnesium has a greater charge of 2+, Mg ions are smaller therefore have a higher charge density meaning the attraction between the delocalized electrons and ions are stronger.

48
Q

What is the formula for nitrate (III) ?

A

NO2 -

49
Q

Describe diamond.

A

Tetrahedral structure
Very high mp
Each carbon has 4 covalent bonds
Non-conductor

50
Q

Draw H2O giving bond angle and stating shape.

A

Use notes

51
Q

What are the properties of ionic compounds ?

A

High mp
conduct electricity only when molten/aqueous
Brittle

52
Q

Draw PF5 giving bond angle and stating shape.

A

Use notes

53
Q

What is a metallic bonding ?

A

Metallic bonding is strong electrostatic attraction between positive metal ions and a sea of delocalized electrons.

54
Q

What is the formula for ammonium ?

A

NH4 +

55
Q

Draw a fluorine molecule

A

Each F has 3 lone pairs and one bonding pair

56
Q

What are the properties of metals ?

A

Good conductors of heat and electricity due to delocalized electrons.
Strong due to Strong electrostatic attraction.
Malleable and ductile because layer of ions can slide over each other.
High mp and bp due to strong metallic bonds.

57
Q

What is a polar bond ?

A

Bond between atoms with differences in electronegativity so electrons are distributed towards the more electronegative atom.

58
Q

What is the formula for chlorate(I)

A

ClO -

59
Q

How are ionic bonds formed ?

A

Electrons are donated/accepted

60
Q

What is the order of strength in IMf from strongest to weakest ?

A

Hydrogen bonding ( can be I.D.D if it is a large molecule e.g. I )
permanent dipole dipole
induced dipole dipole

61
Q

What is the relationship between MP/BP and strength of IMF ?

A

Stronger IMF higher BP/MP

62
Q

What is a covalent bond ?

A

A covalent bond is a shared pair of electrons between two atoms (both non-metals)

63
Q

What are the IMF in BF3 ?

A

Van der waal

64
Q

What is electronegativity ?

A

An atoms ability to attract a pair of electrons in a covalent bond.

65
Q

How do you work out if a molecule is non-polar ?

A

If the central atom is bonded to only one type of atom e.g. CH4
If there is no lone pairs
If both are true then molecule is symmetrical
Dipoles cancel
Molecule is non-polar

66
Q

What is VSEPR ?

A

To minimise repulsion the electron pairs repel each other as far apart as possible

67
Q

Draw BF3 giving bond angles and stating shape.

A

Use notes

chemistry (17 decks)

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