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Higher Chemistry > Bonding & Structure > Flashcards

Bonding & Structure Flashcards

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1
Q

What does it mean if there is a large difference in electronegativity between 2 elements

A
  • the movement of bonding e- from the element of lower electronegativity to the element of higher electronegativity is complete
  • results in formation of ions
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2
Q

ionic compounds form between

A

Metals and non-metals

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3
Q

What are ionic bonds

A

The electrostatic attraction between positive and negative ions

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4
Q

What do ionic compounds form

A

Lattice structures of oppositely charged ions

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5
Q

What are covalent bonds

A

A shared pair of electrons between atoms

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6
Q

What is the covalent bond a result of

A

2 positive nuclei being held together by their common attraction for the shared pair of electrons

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7
Q

What do pure covalent bonds form between

A

Atoms of identical electronegativity

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8
Q

When do polar covalent bonds form

A

When the atoms attraction for the pair of bonding e- are different

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9
Q

What does δ- indicate

A

The partial negative charge of an atom which causes a dipole

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10
Q

What does δ+ indicate

A

The partial positive charge of an atom which causes a dipole

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11
Q

What does the difference in electronegativities between bonded atoms show

A

Gives an indication of the ionic character

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12
Q

The larger the difference in electronegativities…

A
  • the more polar the bond will be

- greater ionic character

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13
Q

What can we use to deduce the type of bonding and structure in the compound

A

Physical properties e.g. state at room temp, MP/BP, solubility and electrical conductivity.

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14
Q

What are Van der Waals forces

A

Intermolecular forces acting between molecules

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15
Q

What are the different types of Van der Waals forces

A
  • London dispersion forces

- permanent dipole - permanent dipole interactions (includes hydrogen bonding)

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16
Q

What are london dispersion forces

A

Forces of attraction that can operate between ALL atoms and molecules

17
Q

What is the strength of london dispersion forces

A

Weaker than all other types of bonding

18
Q

Why do london dispersion forces form

A

As a result of electrostatic attraction between temporary and induced dipoles

19
Q

What is the strength of london dispersion forces related to

A

The number of electrons within an atom or molecule

20
Q

What is a polar molecule

A

It has a permanent dipole

21
Q

What else can make a molecule polar

A

The spatial arrangement of polar covalent bonds (3D symmetry)

22
Q

What are permanent dipole - permanent dipole interactions

A

Additional electrostatic forces of attraction between polar molecules

23
Q

What is the strength of permanent dipole - permanent dipole interactions compared to LDFS

A

Permanent dipole-permanent pole interactions are stronger than London dispersion forces

24
Q

What is a hydrogen bond

A

Electrostatic forces of attraction between molecules that contain these highly polar bonds

25
Q

What do highly polar bonds consist of

A

A hydrogen atom bonded to an atom of a strongly electronegative element (such as fluorine, oxygen or nitrogen)

26
Q

Strength of hydrogen bonds

A
  • Stronger than permanent dipole - permanent dipole interactions
  • weaker than a covalent bond
27
Q

How do we make predictions about the strength of the intermolecular forces

A

By considering the polarity and number of electrons present in molecules

28
Q

The MP & BPs of polar substances are …

A

Higher than the MP & BPs of non-polar substances

29
Q

What properties of substances are affected by hydrogen bonding

A
  • boiling point
  • melting point
  • viscosity
  • solubility in water
30
Q

What are the irregular boiling points of ammonia, water and hydrogen fluoride a result of

A

Hydrogen bonding

31
Q

What causes the density of ice to be less than water at low temperatures

A

Hydrogen bonding between molecules in ice results in an expanded structure

32
Q

What are ionic compounds and polar molecules soluble in

A

Polar solvents e.g. water (like dissolves like)

33
Q

What are ionic compounds and polar molecules insoluble in

A

Non-polar solvents

34
Q

What are non-polar molecular substances soluble in

A

Non-polar solvents (like dissolves like)

35
Q

What are non-polar molecular substances insoluble in

A

Polar solvents

36
Q

What are the key features to consider when predicting the solubility of a compound

A
  • presence of hydrogen bonding in molecules (O-H or N-H)

- spatial arrangement of polar covalent bonds

Higher Chemistry (11 decks)

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