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Higher Chemistry Unit 1 > (b) Structure and bonding > Flashcards

(b) Structure and bonding Flashcards

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1
Q

Is there a large or small difference in electronegativities between the atoms in an ionic bond?

A

Large.

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2
Q

What happens to metal atoms when they become ions and what type of ions do they become?

A

Metal atoms loose electrons to form positive ions.

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3
Q

What happens to non-metal ions when they become ions and what type of ions do they become?

A

They gain electrons to form negative ions.

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4
Q

What is the definition of an ionic bond?

A

Ionic bonding is the electrostatic force of attraction between positively and negatively charged ions.

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5
Q

Are ionic lattices: Strong or weak?

High or low melting points?

A

Strong

High.

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6
Q

When there are more electrons involved in the transfer in an ionic bond is the bond strong or weak?

A

Strong.

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7
Q

How does the size of ions impact the strength of the ionic bond?

A

Smaller ions get closer together and therefore the electrostatic force of attraction is stronger meaning that the bond is stronger and has higher melting and boiling points.

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8
Q

Are ionic bonds usually soluble or insoluble in water?

A

Soluble.

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9
Q

In what states does an ionic substance conduct electricity?

A

Molten or in solution.

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10
Q

Why do ionic substances conduct when they are molten or in solution but not when they are solid?

A

Ions are only free to move when the substance is molten or in solution.

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11
Q

What are the 2 types of covalent bonding?

A

Non-polar (or pure) covalent bonding and

Polar covalent bonding.

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12
Q

What is the definition of a covalent bond?

A

The electrostatic force of attraction between the positively charged nuclei and the negatively charged outer electrons.

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13
Q

What must be equal in both atoms for a non-polar covalent bond to form?

A

Electronegativity.

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14
Q

What does it mean for the sharing of the electrons if both atoms have the same electronegativity?

A

They are shared equally.

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15
Q

What is different in the atoms in a non-polar covalent bond?

A

Electronegativity.

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16
Q

What does it mean if a molecule is polarised?

A

It has a slightly negatively charged side and a slightly positively charged side.

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17
Q

What properties allow us to decide wether a bond is ionic or covalent?

A

State at room temperature
Melting and boiling points
Solubility
Electrical conductivity.

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18
Q

What is an intermolecular bond? Give an example.

A

Intermolecular bonds occur between molecules. An example is LDF’s.

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19
Q

What is an intramolecular bond? Give an example.

A

Intramolecular bonds occur between atoms. An example is covalent, ionic, or metallic bonds.

20
Q

What are the attractions between atoms called?

A

Van der Waals.

21
Q

Where do Van Der Waals occur?

A

In molecules with pure and polar covalent bonding.

22
Q

What are the 3 main types of intermolecular forces?

A

London dispersion forces
Permanent dipole dipoles
Hydrogen bonds.

23
Q

Which of the intermolecular forces is the weakest?

A

London Dispersion Forces (LDF)

24
Q

What type of covalent bonds only have LDF’s between the molecules?

A

Non-polar (pure) covalent bonds.

25
Q

What does the fact that non-polar bonds only having LDF’s between their molecules mean for their melting and boiling points?

A

They are low.

26
Q

What increases the strength of LDF’s?

A

More electrons.

27
Q

How do LDF’s arise?

A

The molecule gets slightly charged ends, known as a temporary dipole.
This change can introduce an opposite charge onto a neighbouring molecule called an induced dipole.
The oppositely charged ends attract each other creating the intermolecular force.

28
Q

What type of molecules may have permanent dipole dimples between their molecules?

A

Polar molecules.

29
Q

What molecules have higher melting and boiling points, polar or non-polar?

A

Polar.

30
Q

What does polarity do to the strength of the intermolecular bonding?

A

Increases it.

31
Q

What is the strongest intermolecular force?

A

Hydrogen bonding.

32
Q

When do hydrogen bonds arise?

A

When a hydrogen is bonded to a NOF.

33
Q

What are the 3 NOF’s?

A

Hydrogen, Oxygen, and Fluorine.

34
Q

What is special about the 3 NOF’s?

A

They have very high electronegativities and so create strong polar bonds.

35
Q

What are the boiling points in molecules which contain hydrogen bonding said to be?

A

Higher than normal.

36
Q

Do polar or non-polar bonds have higher melting and boiling points and why?

A

Polar molecules due to stronger intermolecular forces of attraction.

37
Q

Will polar or non-polar substances be attracted to a charged rod?

A

Polar molecules will be attracted to a charged rod.

38
Q

What is viscosity?

A

The thickness of a liquid.

39
Q

Which type of intermolecular bonds impact viscosity?

A

Hydrogen bonds.

40
Q

If there are more hydrogen bonds in a molecule will the substance be more or less viscous?

A

More.

41
Q

What substances will polar molecules dissolve in?

A

Polar substances.

42
Q

What substances will non-polar molecules dissolve in?

A

Non-Polar substances.

43
Q

Will polar substances dissolve in non-polar substances?

A

No.

44
Q

What substances will ionic molecules dissolve in?

A

Polar substances.

45
Q

What are the unusual qualities of water due to?

A

Hydrogen bonding.

46
Q

Why does solid ice have a lower density than liquid water?

A

Water expands when it freezes. The hydrogen bonds cause the molecules to adopt an open hexagonal shape. This means that ice is less dense in water and is why it floats.

47
Q

What does it mean if a compound has all of its atoms with full valances?

A

They will not be able to conduct as no free charged particles that can move.

Higher Chemistry Unit 1 (3 decks)

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