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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
Properties macromelecular
High mp I bp due to strong CB Insoluble Diamonds cannot conduct when sold Graphite can conduct when solid Cannot conduct when molten
26
What is metallic bonding
Attraction between delocalised electron And positive ions arranged in a lattice
27
Factors affecting metallic bonding
More protons, more stronger bond More delocalised electron , more stronger bond Smaller ion , more stronger bond
28
Structure $ example of metallic bonding
Giant metallic lattice Magnesium and sodium
29
Properties of metallic
High mp/bp due to strong electrostatic forces and sea of delocalised elections Insoluble Conductor Shiny Malleable and ductile
30
What are the two types of electron pairs
Shared pair Lone pair
31
What does the. Electron pair repulsion Theory state
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
Is lone pair -lone pair repulsion greater or lower than lone pair - bond pair
greater
33
Lone pair - bond pair greater or lower than bond pair - bond pair
greater
34
Linear bond pair and lone pair and bond angle
BP = 2 LP = 0 Angle = 180 degrees
35
trigonal planar bond pair and lone pair and bond angle
BP = 3 LP = 0 Angle = 120 degrees
36
Tetrahedral bond pair and lone pair and bond angle
BP = 4 LP = 0 Angle = 109.5 degrees
37
Trigonal bipramidal bond pair and lone pair and bond angle
BP = 5 LP = 0 Angle = 120 and 90 degrees
38
Octahedral bond pair and lone pair and bond angle
BP = 6 LP = 0 Angle = 90 degrees
39
Bent bond pair and lone pair and bond angle
BP = 2 LP = 2 Angle = 104.5 degrees
40
Trigonal pyramidal bond pair and lone pair and bond angle
BP = 3 LP = 1 Angle = 107 degrees
41
Trigonal planar with 2 lone pair angle
BP = 3 LP = 2 Angle = 120 degrees
42
Square planar bond pair and lone pair and bond angle
BP = 4 LP = 2 Angle = 90 degrees
43
what is electronegativity
Power of an atom to attract the pairs of electrons in a covalent bond
44
What is used to measure electronegativity
Pauling scale Ranges from 0-4
45
What are the most electronegative atoms and which is the most ?
F O N Cl F is the most
46
What factors affect electro negativity
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
What factors affect electro negativity
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
Across a period, electro negativity
increases
49
Down agroup eletron negativity
Decreases
50
When do polar covalent bonds form
when elements have different electronegativitys
51
When do polar covalent bonds form
when elements have different electronegativity
52
polarity
unequal sharing of electrons between atoms bonded covalently
53
polarity
unequal sharing of electrons between atoms bonded covalently
54
What are the three intermolecular forces?
Van der Waals forces Permanent dipole dipole forces Hydrogen bonding
55
What are the three intermolecular forces?
Van der Waals forces Permanent dipole dipole forces Hydrogen bonding
56
Explain van der walls forces 
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
What is the main factor which affects the size of VW forces?
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
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
 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
How does the shape of a molecule affect the size of VW forces?
Long chain alkanes have a larger surface area between molecules so BW forces can form
60
What is a permanent dipole dipole force?
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
Why do polar molecules have a permanent dipole?
Because of the difference in electronegativity between the atoms
62
How can polar molecules be tested?
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
Explain hydrogen bonding
It occurs in compounds which have a hydrogen attached to one of the three most electronegative atoms
64
What are the three most electronegative atoms?
 nitrogen oxygen fluorine
65
Why is ice less dense than water?
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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