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Chemistry Year 1 > Bonding And Shapes Of Molecules > Flashcards

Bonding And Shapes Of Molecules Flashcards

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1
Q

What is ionic bonding

A

The electrostatic attrition between oppositely charged ions formed by electron transfer in a lattice

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2
Q

Formula sulfate ion

A

So42-

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3
Q

Formula sulfate ion

A

So42-

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4
Q

Hydroxide ion

A

OH-

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5
Q

Hydroxide ion

A

OH-

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6
Q

Nitrate ion

A

No3-

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7
Q

Carbonate ion

A

CO32-

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8
Q

Carbonate ion

A

CO32-

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9
Q

Ammonium ion

A

NH4+

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10
Q

Where does ionic bonding take place in o

A

Metal to non metal

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11
Q

Are positive ions smaller or bigger compared to atoms and why

A

Smaller
Because it has one less shell of electrons
Ratio of P:e has increased so there is a greater net force on remaining electrons

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12
Q

Are negative ions smaller or bigger compared to atoms and why

A

Larger
More electrons but same number of protons
Nucleus electron attrition is less

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13
Q

Are negative ions smaller or bigger compared to atoms and why

A

Larger
More electrons but same number of protons
Nucleus electron attrition is less

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14
Q

Properties of ionic compounds

A

Solid @ room temp
Conduct electricity when molten/dissolved
Brittle shatter easily

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15
Q

What is the structure of an ionic compound and give an example

A

Giant ionic lattice
Sodium chloride magnesium oxide

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16
Q

Properties of an ionic lattice

A

High mp/bp due to the strong electrostatic forces
Soluble in water
Poorconductivity when solid
Good conductivity when molten

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17
Q

Properties of an ionic lattice

A

High mp/bp due to the strong electrostatic forces
Soluble in water
Poorconductivity when solid
Good conductivity when molten

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18
Q

What is a covalent bond

A

Shared pair of electrons

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19
Q

What IS A dative covalent bond/ coordinate bond

A

Shared pair of electrons with both electrons supplied by one atom

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20
Q

Atom accepting electron pair

A

Electron deficient

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21
Q

Atom donating electron pair

A

Lone pair

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22
Q

When drawing a CBq with an arrow, the direction of arrow goes from a to b

A

a - atom providing lone pair
b - atom that is deficient

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23
Q

Structures of a covalent bond and examples

A

Simple molecular eg iodine and ice
Macromelecular eg diamond and graphite

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24
Q

What do simple molecular structures contain and what are the properties

A

Intermolecular forces
Low mp/bp due to weak intermolecular forces
Poor solubility in water
Can’t conduct

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25
Q

Properties macromelecular

A

High mp I bp due to strong CB
Insoluble
Diamonds cannot conduct when sold
Graphite can conduct when solid
Cannot conduct when molten

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26
Q

What is metallic bonding

A

Attraction between delocalised electron And positive ions arranged in a lattice

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27
Q

Factors affecting metallic bonding

A

More protons, more stronger bond
More delocalised electron , more stronger bond
Smaller ion , more stronger bond

28
Q

Structure $ example of metallic bonding

A

Giant metallic lattice
Magnesium and sodium

29
Q

Properties of metallic

A

High mp/bp due to strong electrostatic forces and sea of delocalised elections
Insoluble
Conductor
Shiny
Malleable and ductile

30
Q

What are the two types of electron pairs

A

Shared pair
Lone pair

31
Q

What does the. Electron pair repulsion Theory state

A

Each part of electron around an atom will repel all other electron pairs.
The pairs of electronswill then take up positions far apart to minimise repulsion

32
Q

Is lone pair -lone pair repulsion greater or lower than lone pair - bond pair

A

greater

33
Q

Lone pair - bond pair greater or lower than bond pair - bond pair

A

greater

34
Q

Linear bond pair and lone pair and bond angle

A

BP = 2
LP = 0
Angle = 180 degrees

35
Q

trigonal planar bond pair and lone pair and bond angle

A

BP = 3
LP = 0
Angle = 120 degrees

36
Q

Tetrahedral bond pair and lone pair and bond angle

A

BP = 4
LP = 0
Angle = 109.5 degrees

37
Q

Trigonal bipramidal bond pair and lone pair and bond angle

A

BP = 5
LP = 0
Angle = 120 and 90 degrees

38
Q

Octahedral bond pair and lone pair and bond angle

A

BP = 6
LP = 0
Angle = 90 degrees

39
Q

Bent bond pair and lone pair and bond angle

A

BP = 2
LP = 2
Angle = 104.5 degrees

40
Q

Trigonal pyramidal bond pair and lone pair and bond angle

A

BP = 3
LP = 1
Angle = 107 degrees

41
Q

Trigonal planar with 2 lone pair angle

A

BP = 3
LP = 2
Angle = 120 degrees

42
Q

Square planar bond pair and lone pair and bond angle

A

BP = 4
LP = 2
Angle = 90 degrees

43
Q

what is electronegativity

A

Power of an atom to attract the pairs of electrons in a covalent bond

44
Q

What is used to measure electronegativity

A

Pauling scale
Ranges from 0-4

45
Q

What are the most electronegative atoms and which is the most ?

A

F O N Cl
F is the most

46
Q

What factors affect electro negativity

A
  1. the nuclear charge
    2.the distance between the nucleus and the outer shell electrons
    3.the shielding of the nuclear charge by electrons in inner shells.
47
Q

What factors affect electro negativity

A
  1. the nuclear charge
    2.the distance between the nucleus and the outer shell electrons
    3.the shielding of the nuclear charge by electrons in inner shells.
48
Q

Across a period, electro negativity

A

increases

49
Q

Down agroup eletron negativity

A

Decreases

50
Q

When do polar covalent bonds form

A

when elements have different electronegativitys

51
Q

When do polar covalent bonds form

A

when elements have different electronegativity

52
Q

polarity

A

unequal sharing of electrons between atoms bonded covalently

53
Q

polarity

A

unequal sharing of electrons between atoms bonded covalently

54
Q

What are the three intermolecular forces?

A

Van der Waals forces
Permanent dipole dipole forces
Hydrogen bonding

55
Q

What are the three intermolecular forces?

A

Van der Waals forces
Permanent dipole dipole forces
Hydrogen bonding

56
Q

Explain van der walls forces 

A

Because between all simple covalent molecules and noble gases an induced dipole is always formed and it has the opposite sign to the original one

57
Q

What is the main factor which affects the size of VW forces?

A

The more electrons that are in the molecule the higher chance of the temporary dipole forming this makes the vDW stronger between molecules and so the boiling point will be greater

58
Q

Explain why there is an increase in boiling point going down group 7
Explain why there is an increase in boiling points going down the alkane homologous series
Relate to vW forces

A

 there is an increase in boiling point going down group 7 as there is an increase number of electrons in the bigger molecules which causes an increase in the size of both between the molecules. There is also a larger electron cloud can also explain why iodine is a solid and chlorine is a gas
There is an increase going down the alkane series as there is an increase number of electrons in the big molecules which causes an increase in the size of force between molecules

59
Q

How does the shape of a molecule affect the size of VW forces?

A

Long chain alkanes have a larger surface area between molecules so BW forces can form

60
Q

What is a permanent dipole dipole force?

A

It is a weak electrostatic force which occurs between polar molecules. It is stronger than VW forces so the compounds have a higher boiling point.

61
Q

Why do polar molecules have a permanent dipole?

A

Because of the difference in electronegativity between the atoms

62
Q

How can polar molecules be tested?

A

Placing a charged rod near a steady stream of a polar liquid. The liquid should bent towards the rod as the molecules align to face the opposite charged rod.

63
Q

Explain hydrogen bonding

A

It occurs in compounds which have a hydrogen attached to one of the three most electronegative atoms

64
Q

What are the three most electronegative atoms?

A

 nitrogen oxygen fluorine

65
Q

Why is ice less dense than water?

A

It has a regular structure held by hydrogen bonds and the molecules are further apart. This is what makes us less dance.

Chemistry Year 1 (16 decks)

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