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Chemistry L6 > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is a covalent bond?

A

Sharing a pair of electrons between two atoms

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2
Q

What is electronegativity?

A

The power of an atom to attract the pair of electrons in a covalent bond

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3
Q

How does electronegativity increase throughout the periodic table?

A

It increases as you go to the right kf the period table
Also increases as you go up the table

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4
Q

What causes a polar bond?

A

When the more electronegative element in a covalent bond pulls the share of electrons closer to itself

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5
Q

What causes a non polar bond?

A

when two atoms in the bond are the same
they have an equal share of electrons
e.g. F2

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6
Q

What is ionic bonding?

A

strong electrostatic force of attraction between oppositely charged ions
NOT A BOND BUT AN ATTRACTION

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7
Q

What is the structure of an ionic bond?

A

giant ionic lattice

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8
Q

What are some properties of ionic compounds?

A
  • solid at room temp due to giant lattice
  • high melting/boiling point due to strong electrostatic attraction
  • don’t conduct electricity as solid bc ions arent free to move
  • brittle
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9
Q

What is metallic bonding?

A

strong electrostatic force of attraction between positive metal ions and the sea of delocalised electrons

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10
Q

What factors effect the strength of a metallic bond?

A
  • ionic charge (high=strong)
  • atomic radius (small=stronger)
  • number of delocalised electrons (more=stronger
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11
Q

What are some properties of metals?

A
  • good conductors as delocalised electrons are free to move
  • high melting/boiling point due to strong attraction between positive ions and delocalised electrons
  • malleable as layers of ions slide over each other
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12
Q

What is Co-ordinate bonding?

A

When one atom provides both electrons needed to form a covalent bond

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13
Q

LP-LP > BP- LP > BP-BP

A

idk just remember that

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14
Q

What are properties of a symmetrical (non polar) molecule?

A
  • bonded to the same atoms
  • NO lone pairs
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15
Q

What is a dipole?

A

occurs when there is an uneven distribution of electron density in a molecule

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16
Q

What is a Van der Waals force?

A

a temporary dipole in one molecule induces a dipole in another
there is an attraction between δ+molecule and δ-

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17
Q

What affects the strength of VDW forces?

A

Size/Mr of molecule (bigger=more forces)
Surface area contact (more SA = more forces)

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18
Q

What is a permanent dipole dipole force?

A

occurs between polar molecules

the δ+ on one molecule attracts the δ- on a neighbouring molecule

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19
Q

What is hydrogen bonding?

A

occurs between polar molecules which have a hydrogen directly bonded to oxygen nitrogen or fluorine
these are the most electronegative atoms, pulling pair if electrons closer to themselves leaving hydrogen very δ+

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20
Q

What are some features of a Hydrogen bonding diagram?

A
  • partial charges on ALL atoms
  • all lone lairs shld be clearly shown
  • hydrogen bond shown between lone pair and δ+ on other molecule
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21
Q

Why is ice less dense than liquid water? (hydrogen bonding)

A

there’s fewer particles of water per unit of volume in the a solid state

in ice water molecules are further apart than in liquid

so theres more gaps between molecules

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22
Q

Can a giant ionic lattice conduct electricity?

A

when molten or dissolved
this is because ions are free to move

but not when theyre solid

23
Q

What is the melting/boiling point of a giant ionic lattice?

A

HIGH
due to strong electrostatic attraction between opposite ions

24
Q

Dies a giant metallic lattice conduct electricity?

A

yes
delocalised electrons are free to move

25
Q

What is the boiling point if a giant metallic lattice?

A

HIGH
due to strong electrostatic attraction between positive ions and delocalised electrons

26
Q

Describe a simple molecular crystal structure?

A

weak intermolecular forces between molecules are broken
strong covalent bonds between atoms stay intact

27
Q

Can a simple molecular crystal structure conduct electricity?

A

NO
theres no delocalised electrons

28
Q

What is the boiling point of a simple molecular crystal structure?

A

LOW
due to weak intermolecular forces between molecules

29
Q

Describe the bonds in a Diamond?

A

strong covalent bonds between carbon atoms

30
Q

Can a diamond conduct electricity?

A

NO
no delocalised electrons

31
Q

What is the boiling point of a Diamond?

A

HIGH
strong covalent binds require alot of energy to break

32
Q

Describe the bonds in Graphite?

A

strong covalent bond between carbon atoms
weak VDW forces between layers

have delocalised electrons that can move between the layers

33
Q

Can Graphite conduct electricity?

A

YES
delocalised elctrons can move

34
Q

What is the boiling point of Graphite?

A

HIGH
strong covalent bonds require a lot of energy to break

35
Q

Describe the bonds in Graphene?

A

Strong covalent bonds between atoms
delocalised electrons across it’s surface

36
Q

Can graphene conduct electricity?

A

YES
delocalised electrons can move

37
Q

What is the boiling point of Graphene?

A

High
strong covalent bonds required alot of energy to break

38
Q

what shape has 2 bond pairs

A

linear

39
Q

What shape has 3 bond pairs?

A

Trigonal Planar

40
Q

What shape has 4 bond pairs?

A

Tetrahedral

41
Q

What shape has 3 bond pairs and 1 lone pair?

A

Trigonal Pyramid

42
Q

What shape has 2 bond pairs and 2 lone pairs?

A

V shaped

43
Q

What shape has 5 bond pairs?

A

Triganol Bipyramid

44
Q

What shape has 6 bond pairs?

A

Octahedral

45
Q

What shape has 4 bond pairs and 2 lone pairs?

A

Square planar

46
Q

What angle is in a linear shape

A

180°

47
Q

What angle is in a Trigonal Planar?

A

120°

48
Q

What angle is in a Tetrahedral shape?

A

109.5°

49
Q

What angle is in a trigonal pyramid?

A

107°

50
Q

What angle is in a V shaped?

A

104.5°

51
Q

what an angle is in a trigonal bipyramid

A

120° & 90°

52
Q

What angle is in an octahedral shape?

A

90°

53
Q

What angle is in a square planar shape?

A

90°

Chemistry L6 (17 decks)

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