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Chemistry (Physical) > Bonding > Flashcards

Bonding Flashcards

1
Q

What is a dative bond

A

A bond where the shared pair of electrons in a covalent bond come from one atom

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2
Q

How do we display a dative bond

A

With an arrow in the direction towards the atom accepting the electrons

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3
Q

What are the conditions for a dative bond to form

A

The atom that is donating must have a lone pair, and the other must have space to gain two electrons (6 electrons in outer shell)

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4
Q

What is an ionic compound

A

Oppositely charged ions held together by electrostatic forces of attraction

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5
Q

What is electronegativity

A

The tendency for an atom to attract the pair electrons in a covalent bond

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6
Q

When does a permanent dipole form

A

When there is a difference in electronegativity between two atoms in a molecule , meaning the delta negative end of one molecule is attracted to the delta positive end of the adjacent molecule

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7
Q

What determines the strength of a permanent dipole

A

The difference in electronegativity between atoms in a molecule

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8
Q

Explain the 4 stages as to how van der waals forces occur

A
  • Electrons move around randomly in an oscillating motion
  • If at any moment in time there are more electrons on one side of an atom, the side with more electrons will be delta negative (causing a temp. dipole)
  • This will force electrons on neighbouring atoms to repel (induced dipole).
  • The attraction between the atoms due to the dipoles is called VDW
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9
Q

Can VDW forces occur between molecules?

A

Yes

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10
Q

What are the 2 conditions for not having a permanent dipole when atoms aren’t identical in a molecule

A
  • Molecule must be symmetrical (dipoles cancel)
  • All the surrounding atoms are the same in the molecule
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11
Q

Give 3 characteristics of giant ionic structures

A

Regular structure
Cubic shape
Giant repeating pattern

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12
Q

Give 4 characteristics of graphite

A

Layers slide
Conduct electricity
Low density (layers far apart)
High melting point

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13
Q

What is H bonding between

A

H bonding is between the lone pair on N, O, F and a delta positive hydrogen

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14
Q

What determines the strength of a H bond

A

The more electronegative the atom bonded to the hydrogen, the more delta positive the hydrogen will be due to greater pulling of electrons towards N, O, F

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15
Q

Why doesn’t Cl form H bonds

A

The p orbitals that the electrons are in are of less dense negative charge

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16
Q

What type of I.M.F do we get when a molecule has no dipole

A

VDW forces

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17
Q

When do VDW forces get stronger

A

When there are more electrons (bigger atom/molecule)

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18
Q

What type of IMF do we get when a molecule has a dipole

A

Either H bond
OR
Permanent dipole

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19
Q

Why does H2O have more bonding pairs than H-F

A
  • Per mole H2O will form more H bonds as there is a 1:1 ratio between lone pairs and hydrogens
  • In H-F, the number of H’s will limit the number of L.Ps which can attract, due to there being more L.Ps than Hs
20
Q

What holds a metallic lattice together

A

Sea of delocalised electrons holding positive cations

21
Q

What does VSEPR say

A

Pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible to minimise repilsion

22
Q

Write the order or repulsion strength between lone pairs and bonding pairs

A

LP-LP repulsion > LP-BP repulsion > BP-BP repulsion

23
Q

What is the name of the shape with 2BPs 0LPs (Draw too)

A

Linear

24
Q

What is the name of the shape with 3BPs 0LPs (Draw too)

A

Trigonal Planar

25
Q

What is the name of the shape with 2BPs 1LP (Draw too)

A

Bent

26
Q

What is the name of the shape with 4BPs 0LPs (Draw too)

A

Tetrahedral

27
Q

What is the name of the shape with 3BPs 1LP (Draw too)

A

Trigonal pyramidal

28
Q

What is the name of the shape with 2BPs 2LPs (Draw too)

A

Bent

29
Q

What is the name of the shape with 5BPs 0LPs (Draw too)

A

Trigonal bipyramidal

30
Q

What is the name of the shape with 4BPs 1LP (Draw too)

A

See-saw

31
Q

What is the name of the shape with 3BPs 2LPs (Draw too)

A

T-Shape

32
Q

What is the name of the shape with 6BPs 0LPs (Draw too)

A

Octahedral

33
Q

What is the name of the shape with 5BPs 1LP (Draw too)

A

Square pyramid

34
Q

What is the name of the shape with 4BPs 2LPs (Draw too)

A

Square planar

35
Q

What is the bond angle for a trigonal pyramidal molecule

A

107

35
Q

What is the bond angle for a trigonal planar molecule

A

120

36
Q

What is the bond angle for a linear molecule

A

180

37
Q

What is the bond angle for a bent molecule (2,1)

A

118

37
Q

What is the bond angle for a tetrahedral molecule

A

109.5

38
Q

What is the bond angle for a bent molecule (2,2)

A

104.5

38
Q

What are the angles for a trigonal bipyramidal molecule

A

90, 120

39
Q

What are the bond angles for a see saw molecule

A

89, 119

39
Q

What is the bond angle for a T shape molecule

A

89

39
Q

What is the bond angle for a square pyramid molecule

A

89

40
Q

What is the bond angle for a octahedral molecule

A

90

41
Q

What is the bond angle for a square planar molecule

A

90

Chemistry (Physical) (10 decks)

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