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CHEMISTRY A-LEVEL > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is an ionic bond?

A

lonic bonding involves electrostatic attraction

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2
Q

What is a metallic bond?

A

The attraction between delocalised electrons and cations

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3
Q

Draw trigonal bipyramidal

A

[Draw it]

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4
Q

Draw an octahedral

A

[Draw it]

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5
Q

What is a covalent bond

A

The attraction between a pair of electrons and the nucleus it lies between

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6
Q

Draw tetrahedral

A

[Draw it]

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7
Q

Draw trigonal pyramidal

A

[Draw it]

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8
Q

what is the bonding angle in a linear molecule

A

the bonding angle in linear is 180 degrees

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9
Q

what is the bonding angle in trigonal planar

A

the bonding angle in trigonal planar is 120 degrees

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10
Q

what is the bonding angle in tetrahedral

A

the bonding angle in tetrahedral is 109.5 degrees

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11
Q

what is the bonding angle in trigonal pyramidal

A

the bonding angle in trigonal pyramidal 107

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12
Q

what is the bonding angle in bent

A

the bonding angle in bent 104.5 degrees

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13
Q

what is the bonding angle in trigonal bipyramidal

A

the bonding angle in octahedral is 90 degrees down and 120 degrees accross

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14
Q

what is the bonding angle in octahedral

A

the bonding angle in octahedral is 90 degrees

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15
Q

which simple molecular shape has

2 electron groups

2 bonding electron groups

0 lone pairs

A

Linear

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16
Q

which simple molecular shape has

3 electron groups

3 bonding electron groups

0 lone pairs

A

trigonal planar

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17
Q

which simple molecular shape has

4 electron groups

4 bonding electron groups

0 lone pairs

A

tetrahedral

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18
Q

which simple molecular shape has

4 electron groups

3 bonding electron groups

1 lone pairs

A

trigonal pyramidal

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19
Q

which simple molecular shape has

4 electron groups

2 bonding electron groups

2 lone pairs

A

Bent

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20
Q

which simple molecular shape has

5 electron groups

5 bonding electron groups

0 lone pairs

A

trigonal bipyramidal

21
Q

which simple molecular shape has

6 electron groups

6 bonding electron groups

0 lone pairs

A

octahedral

22
Q

what is a free radical

A

a species that has one unpaired electron

23
Q

why is NH4 (for example) tetrahedral
applies to similar questions

A
  • There are 4 bonding pairs that repel each other equally as far away as possible,
  • the bond angle is 109.5, the shape is tetrahedral
24
Q

why is H3O trigonal pyramidal

A

-There are 3 bonding pairs of electrons and 1 lone pair of electrons that repel each other as far away as possible

  • lone pairs repel more than bonding pairs

-the bonding angle is 107 the shape trigonal pyramidal

25
Q

How is a dative bond formed in ammonium ion

A

Ammonia donates its lone pair of electrons to a H+ ion making it NH4 +

26
Q

What is electronegativity

A

Ability of an atom to withdraw electrons density towards itself
In a covalent bond

27
Q

Properties of diamond

A

giant covalent structures

diamond is hard because of 3d structure
Diamond carbon atoms joined to 4 other carbon atoms

28
Q

Properties of graphite

A

Carbon atoms in graphite joined to 3 other carbon atoms

Graphite is soft because has layers that can Slide Over each other because of weak intermolecular forces

29
Q

Why is the melting point high for carbon and diamond

A

Covalent bonds must be broken
Which requires a lot of energy

30
Q

What is the difference between graphite and diamond

A

Diamond is a not a conductor of electricity and has no delocalised electron
Graphite has delocalised electron and can conduct electricity

31
Q

Name 3 types of bondings

A

Van der Waals

Hydrogen

Dipole dipole

32
Q

Why is the energy needed to vaporise sodium chloride is much more than the energy needed to melt sodium chloride

A

Because vaporisation breaks all the bonds

33
Q

Ionic compound conduct what when they are molten?

A

Electricity

34
Q

Why to ionic compounds dissolve in water

A

Water molecules are polar- part of water molecules have a small negative charge and others have positive so the charged parts pill ions away from the lattice

35
Q

What molecule shape has 5 electron pairs and 1 lone pair

A

Seesaw

36
Q

What molecule shape has 5 electron pairs and 2 lone pairs

A

T-Shaped

37
Q

What molecule shape had 6 electron pairs and 2 lone pairs

A

Square planar

38
Q

What is the bonding angle of seesaw

A

102 degrees and 87 degrees

39
Q

What are the bonding Angie of T-shaped

A

88 degrees

40
Q

What is the bond angle of square planar

A

90 degrees

41
Q

What is a dipole

A

A difference in charge between two atoms caused by an uneven shift in electron density

42
Q

What causes a permanent dipole

A

In polar bonds the shift in electronegativity between two atoms causes a permanent dipole.

43
Q

Explain van der waals

A

At any moment electrons are more likely to be on one side of an atom called an instantaneous dipole

This dipole can cause an induced dipole and the two dipoles are now attracted to each other

The second dipole caused another dipole in another atom

Electrons are always moving so dipoles are constantly created and destroyed

44
Q

Name properties of ionic substances

A
  • high mp and bp
  • typical state solid
  • can’t conduct electricity in solid state
  • can conduct electricity in liquid state
  • is soluble in water
45
Q

Name properties of simple covalent substances

A
  • Low melting and boiling points
  • is usually a liquid or gas
  • can’t conduct electricity in solid
  • can’t conduct electricity in liquid
  • is soluble in water depending on polarity of molecules
46
Q

Giant covalent substance properties

A

-high melting and boiling point
- typically solid at room tem
- solid cannot conduct electricity except for graphite
- does not melt, it sublimes
-is not soluble in water

47
Q

Metal is substance properties

A

High melting and bp
Typically solid
Can conduct electricity in solid and liquid state
Not soluble in water

48
Q

Explain why Nickle high mp

A
  • contains positive metal ions
  • delocalised electron
  • strong attraction between metallic bonds

CHEMISTRY A-LEVEL (11 decks)

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