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)

24
Q

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

A

Trigonal Planar

25
What is the name of the shape with 2BPs 1LP (Draw too)
Bent
26
What is the name of the shape with 4BPs 0LPs (Draw too)
Tetrahedral
27
What is the name of the shape with 3BPs 1LP (Draw too)
Trigonal pyramidal
28
What is the name of the shape with 2BPs 2LPs (Draw too)
Bent
29
What is the name of the shape with 5BPs 0LPs (Draw too)
Trigonal bipyramidal
30
What is the name of the shape with 4BPs 1LP (Draw too)
See-saw
31
What is the name of the shape with 3BPs 2LPs (Draw too)
T-Shape
32
What is the name of the shape with 6BPs 0LPs (Draw too)
Octahedral
33
What is the name of the shape with 5BPs 1LP (Draw too)
Square pyramid
34
What is the name of the shape with 4BPs 2LPs (Draw too)
Square planar
35
What is the bond angle for a trigonal pyramidal molecule
107
35
What is the bond angle for a trigonal planar molecule
120
36
What is the bond angle for a linear molecule
180
37
What is the bond angle for a bent molecule (2,1)
118
37
What is the bond angle for a tetrahedral molecule
109.5
38
What is the bond angle for a bent molecule (2,2)
104.5
38
What are the angles for a trigonal bipyramidal molecule
90, 120
39
What are the bond angles for a see saw molecule
89, 119
39
What is the bond angle for a T shape molecule
89
39
What is the bond angle for a square pyramid molecule
89
40
What is the bond angle for a octahedral molecule
90
41
What is the bond angle for a square planar molecule
90
42
When does nuclear charge vs number of electron shells affect size of an atom/ion the most
More shells = larger size Electrons occupy orbitals further from the nucleus → naturally increases the radius 🧠 This is usually the dominant factor across a group (top to bottom) More protons = stronger attraction pulling electrons inward Especially significant when the number of shells is the same or similar 🧠 This is the dominant factor across a period (left to right)