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chemistry A - level > Bonds > Flashcards

Bonds Flashcards

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1
Q

What is a covalent bond

A

Electrostatic attraction between the shared pair of electrons and the positive nuclei

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2
Q

Ionic bond

A

An electrostatic attraction between positive ions and negative ions

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3
Q

Metallic bond

A

An electrostatic attraction between positive ions and delocalised electrons

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4
Q

What happens in coordinate bonding

A

Both electrons are donated from 1 atom to the empty orbital of another

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5
Q

What is the shape of a simple molecule determined by

A

The electrons and bonds in it. This is because electron pairs repel each other and therefore try to get as far away as possible

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6
Q

Shapes of simple covalent molecules
2 pairs of electrons

A

Linear molecule
180 degrees

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7
Q

Shapes of simple covalent molecules
3 pairs of electrons

A

Trigonal planar
120 degrees

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8
Q

Shapes of simple covalent molecules
4 pairs of electrons

A

Tetrahedral
109.5 degrees

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9
Q

Shapes of simple covalent molecules
5 pairs of electrons

A

Trigonal bipyramidal
120 degrees & 90 degrees

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10
Q

Shapes of simple covalent molecules
6 pairs of electrons

A

Octahedral (8 faces)
90 degrees

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11
Q

What affects the shape of an atom

A

As well as bonding pairs of electrons repelling, any lone pairs that are around the central atom also affects the shape

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12
Q

What repels more lone pairs or bonding pairs

A

Lone pairs repel more

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13
Q

4 pairs of electron
3 bonding
1 lone pair

A

Pyramidal
107.5 degrees

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14
Q

4 pairs of electrons
2 bonding pairs, 2 lone pairs
( e.g. H20)

A

V - shaped / bent
104.5 degrees

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15
Q

5 pairs of electrons
4 bonding, 1 lone pair

A

Modified Trigonal bipyramid

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16
Q

5 pairs
3 bonding, 2 lone pairs

A

T shaped

17
Q

6 pairs
4 bonding, 2 lone pairs

A

Square planar

18
Q

How to determine the shape

A

1) group number of central atom
2) number of bonding atoms
3) charge
4) add up and divide by 2
5) work out lone pairs , total - bonding

19
Q

What is electronegativity

A

The ability of an atom to attract the pair of electrons(/electron density) in a covalent bond towards itself

20
Q

What would happen with Cl2 due to electronegativity

A

Nothing would happen because there is no difference in electronegativity, so we have a non-polar covalent bond

21
Q

Ht would happen in HCL due to electronegativity

A

Chlorine is more electronegative that hydrogen , this is a polar bond

22
Q

What does electronegativity depend on

A
  • nucleus charge
  • atomic radius
  • electron shielding
23
Q

What is the most electronegative element

A

F
Fluorine

24
Q

How to increase electronegativity

A

More protons and a smaller radius increases attraction from the nucleus

25
Q

What decreases electronegativity

A

More shielding decreases the attraction from the nucleus

26
Q

What elements are relatively electronegative

A

N , nitrogen
O , oxygen
Cl , chlorine

27
Q

where are intermolecular forces commonly found?

A

they exist between simple covalent molecules. these are the forces between individual molecules

28
Q

what are they 3 types of IMF?

A
  • van de Waals force (weakest)
  • dipole-dipole force
  • hydrogen bond ((strongest) but weak compared to real bonds)
29
Q

how is a van der waals force formed?

A

electrons in an atom are unevenly distributed making a temporary dipole. this induces a dipole in the nearby atom. this creates an attraction between them

30
Q

the affect of an atoms size on van der Waals forces

A

this bigger the Mr of the atom/molecule, the larger the van der Waal force is, which increases the boiling point

31
Q

which atoms have van der Waals forces

A

all atoms and molecules have van der Waals forces

32
Q

when does dipole-dipole forces occur

A

when the delta+ and the delta- in a molecule are permanent

33
Q

how are the dipole-dipole forces formed

A

the delta+ end of one molecule attracts the delta- end of an adjacent molecule

34
Q

what molecules can have dipole-dipole forces

A

asymmetric polar molecules as they have a net dipole moment

35
Q

when would hydrogen bonds occur

A

only happens when hydrogen is bonded to a small electronegative atom with in a molecule
N, O, F

36
Q

when drawing a hydrogen bond, what do you have to ensure

A
  • all delta charges on involved atoms
  • 180 degrees
  • all lone pairs are on the diagram

chemistry A - level (16 decks)

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