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CHEMISTRY A-LEVEL > Bonding > Flashcards

Bonding Flashcards

(48 cards)

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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

Study These Flashcards
A

trigonal bipyramidal

21
Q

which simple molecular shape has

6 electron groups

6 bonding electron groups

0 lone pairs

22
Q

what is a free radical

Study These Flashcards
A

a species that has one unpaired electron

23
Q

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

Study These Flashcards
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

Study These Flashcards
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
How is a dative bond formed in ammonium ion
Ammonia donates its lone pair of electrons to a H+ ion making it NH4 +
26
What is electronegativity
Ability of an atom to withdraw electrons density towards itself In a covalent bond
27
Properties of diamond
giant covalent structures diamond is hard because of 3d structure Diamond carbon atoms joined to 4 other carbon atoms
28
Properties of graphite
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
Why is the melting point high for carbon and diamond
Covalent bonds must be broken Which requires a lot of energy
30
What is the difference between graphite and diamond
Diamond is a not a conductor of electricity and has no delocalised electron Graphite has delocalised electron and can conduct electricity
31
Name 3 types of bondings
Van der Waals Hydrogen Dipole dipole
32
Why is the energy needed to vaporise sodium chloride is much more than the energy needed to melt sodium chloride
Because vaporisation breaks all the bonds
33
Ionic compound conduct what when they are molten?
Electricity
34
Why to ionic compounds dissolve in water
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
What molecule shape has 5 electron pairs and 1 lone pair
Seesaw
36
What molecule shape has 5 electron pairs and 2 lone pairs
T-Shaped
37
What molecule shape had 6 electron pairs and 2 lone pairs
Square planar
38
What is the bonding angle of seesaw
102 degrees and 87 degrees
39
What are the bonding Angie of T-shaped
88 degrees
40
What is the bond angle of square planar
90 degrees
41
What is a dipole
A difference in charge between two atoms caused by an uneven shift in electron density
42
What causes a permanent dipole
In polar bonds the shift in electronegativity between two atoms causes a permanent dipole.
43
Explain van der waals
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
Name properties of ionic substances
- 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
Name properties of simple covalent substances
- 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
Giant covalent substance properties
-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
Metal is substance properties
High melting and bp Typically solid Can conduct electricity in solid and liquid state Not soluble in water
48
Explain why Nickle high mp
- contains positive metal ions - delocalised electron - strong attraction between metallic bonds

CHEMISTRY A-LEVEL (12 decks)

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