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Higher Chemistry > Unit 1: Chapter 4 - Bonding Compounds > Flashcards

Unit 1: Chapter 4 - Bonding Compounds Flashcards

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1
Q

What is the definition of an ionic bond?

A

The ionic bond is the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.

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2
Q

What do ionic compounds form?

A

Three dimensional structures called lattices.

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3
Q

In each ionic structure what are there equal numbers of and what does this produce?

A

In each structure there is equal numbers of positive and negative ions to produce the neutral compound. For example NaCl contains a sodium atom for every chlorine atom.

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4
Q

What does the large difference in electronegativities allow to happen in the NaCl compound and what does this mean for the sodium and chlorine atom?

A

The large difference allows the chlorine atom to completely strip away sodium’s outer electron. This leaves chlorine with a strong negative charge and sodium with a strong positive charge.

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5
Q

What are most covalent compounds formed by?

A

Most covalent compounds are formed by a combination of non-metallic elements.

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6
Q

What can covalent compounds be in the form of?

A

Discrete molecules or network structures.

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7
Q

In the discrete molecule form in covalent bonding, What is the main bond?

A

The main bond is the strong intramolecular covalent bond with the weaker bond being the intermolecular bond of the London Dispersion Forces which has an impact on the properties of the molecule.

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8
Q

When there is little difference in electreronegativities between atoms what is produced?

A

A pure covalent bond.

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9
Q

When a pure covalent bond is formed what are the electrons in the atom?

A

equally shared

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10
Q

In the network structure of covalent compounds, is there any effect from London Dispersion Forces?

A

No

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11
Q

What is the compound made from in the network structure of covalent compounds?

A

Strong covalent bonds only.

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12
Q

What are are polar covalent bonds?

A

An unequal sharing of electrons in the covalent bond.

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13
Q

What determines the polar covalent bond?

A

The electrons moving towards the more electronegative atom.

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14
Q

What does the term “dipole” refer to?

A

A molecule that carries a slightly positive and slightly negative part.

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15
Q

Why can some molecules carry a permanent dipole?

A

Due to the unsymmetrical nature of the molecule.

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16
Q

Describe how ammonia is a permanent dipole?

A

Nitrogen the more electronegative atom pulls the bonding electrons towards itself leaving the molecule with slightly positive and slightly negative poles.

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17
Q

Name two types of symmetric molecules containing dipoles?

A

Carbon dioxide and tetrachloromethane.

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18
Q

What happens to the dipoles in a symmetrical molecule?

A

The dipoles cancel each other out. i.e. there is no slightly positive or negative ends.

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19
Q

Do symmetrical molecules containing dipoles have polar covalent properties?

A

NO!!!

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20
Q

What are at opposite ends of the bonding continuum?

A

Pure covalent bonding and pure ionic bonding.

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21
Q

Why are pure covalent and pure ionic bonding at opposite ends of the bonding continuum?

A

Pure ionic bonds have electronegativitie values of around 3 whereas pure covalent has electronegativitie values of around 0.5.

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22
Q

What molecules have greater ionic character?

A

Molecules with higher electronegativity values.

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23
Q

If there is a larger difference in electronegativities in a molecule what will the bond in the molecule be?

A

More polar.

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24
Q

If the elcetronegativity is greater between molecule what happens to the electrons and what does this result in?

A

If the difference is large, then the movement of bonding electrons from the element of lower electronegativity to the element of higher electronegativity is complete, resulting in the formation of ions.

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25
Q

What is an inconsistency in the bonding continuum?

A

Tin(IV) Chloride, a metal compound which has polar covalent properties.

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26
Q

What are the types of bonding as the electronegativities decrease in the bonding continuum?

A

Pure/strongly ionic, ionic, polar covalent, covalent ,strongly/pure covalent.

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27
Q

What is the bonding between polar molecules known as?

A

Permanent Dipole to Permanent Dipole interactions.

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28
Q

Are permanent dipole to permanent dipole interactions stronger than the London dispersion forces?

A

YES

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29
Q

What are examples of polar molecules?

A

Ethanol, Trichloromethane and water.

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30
Q

Why are polar molecules attracted to electrical charges?

A

They are attracted to electrical charges as the polar molecules have a slightly negative and positive atoms present.

31
Q

What is an experiment to show how polar molecules are attracted to electrical charges?

A

Rub a plastic rod (which makes it charged, then slowly let the polar liquid like water run and it will be attracted to the plastic rod. If you repeat this experiment with a non polar liquid like hexane the liquid will not be affected.

32
Q

When does hydrogen bonding occur?

A

between strongly electronegative atoms.

33
Q

What are the main atoms involved in hydrogen bonding?

A

Fluorine, Nitrogen and Oxygen.

34
Q

How does hydrogen bonding occur in water?

A

The hydrogen bonding in water occurs between the slightly negative oxygen and a slightly positive hydrogen from another molecule.

35
Q

How does hydrogen bonding occur in ammonia?

A

Th hydrogen bonding occurs between the nitrogen and a hydrogen from another molecule.

36
Q

When with the elements nitrogen,oxygen and fluorine, hydrogen are commonly known as?

A

Hydrides

37
Q

What are intermolecular forces acting between molecules known as?

A

Van der Waal’s forces

38
Q

What are the three types of Van der Waal’s forces?

A

London Dispersion forces, Permanent dipole to permanent dipole interactions and Hydrogen bonding.

39
Q

What forces of attraction can act between all atoms and molecules?

A

London Dispersion Forces.

40
Q

Are London dispersion the weakest of all the bonds?

A

Yes

41
Q

How are London Dispersion forces formed?

A

They are formed as a result of electrostatic attraction between temporary dipoles and induced dipoles caused by movement of electrons in atoms and molecules.

42
Q

What is the strength of the London Dispersion forces related to?

A

The number of electrons within the atom or molecule.

43
Q

What can result in a molecule being polar?

A

The spatial arrangement of polar covalent bonds.

44
Q

What are permanent dipole to permanent dipole interactions?

A

Additional electrostatic forces of attraction between polar molecules.

45
Q

What is the stronger force for molecules with a similar number of electrons. Permanent dipole to permanent dipole interactions or London Dispersion forces?

A

Permanent dipole to permanent dipole interactions.

46
Q

What are hydrogen bonds?

A

Hydrogen bonds are electrostatic forces of attraction between molecules that contain the highly polar bonds like that of the bonds consisting of a hydrogen atom bonded to an atom of a strongly electronegative
element such as fluorine,oxygen and nitrogen.

47
Q

What are hydrogen bonds stronger than and weaker than?

A

A hydrogen bond is stronger than other forms of permanent dipole permanent dipole interactions but weaker than a covalent bond.

48
Q

What are London Dispersion forces between?

A

London Dispersion forces are between all molecules and atoms but the only force between non polar molecules and monatomic elements.

49
Q

What are permanent dipole to permanent dipole interactions between?

A

Between Polar Molecules.

50
Q

What is hydrogen bonding between?

A

Polar molecules where a Hydrogen atom is directly bonded to an oxygen, nitrogen or fluorine atom.

51
Q

What can make a liquid more viscous?

A

Its mass/size and the polar bonds present.

52
Q

What interactions show a higher viscosity than permanent dipole to permanent dipole interactions?

A

Hydrogen bonding.

53
Q

What is the most used solvent in chemistry?

A

water

54
Q

Why is water capable of dissolving polar and ionic substances?

A

Water is capable of dissolving polar and ionic substances as it is polar.

55
Q

What is the general rule for polar solvents?

A

Polar solvent will dissolve polar or ionic substances. e.g. water will dissolve salts.

56
Q

What will non-polar solvents dissolve?

A

Non-polar

57
Q

How does water dissolve an ionic lattice?

A

Water is polar and has slightly negative and slightly positive ends. These ends are attracted to the positive and negative ions in the lattice. The attraction drags ion out of the lattice (the water molecules, when attached, then literally pull the lattice apart.) and the ions go into a solution surrounded with water molecules, held together by ELECTROSTATIC ATTRACTION. As the ions are taken out of the lattice the lattice reduces in size (dissolves).

58
Q

When the ions in an ionic lattice are surrounded with water molecules, what are they are said to be.

A

Hydrated

59
Q

When the polar covalent HCL molecule is dissolved in water, what does this result in?

A

An uneven breaking of the covalent bond (due to difference in electronegativity).

60
Q

As the breaking of the covalent bond in the polar covalent HCL is uneven. What does this result in for the electrons?

A

This results in both electrons within the covalent bond staying with the chlorine atom.

61
Q

As the electrons stay within the chlorine atom When the polar covalent HCL is dissolved in water, what does this result in the production of?

A

This results in on IONIC acid solution being made from a POLAR COVALENT substance.

62
Q

In a chemical equation what does the subscript (aq) denote?

A

The atom or compound is HYDRATED.

63
Q

What is miscibility?

A

The ability for two liquids to be mixed is called the miscibility of the liquids.

64
Q

What are examples of miscible compounds?

A

Water, ethanol and sugar.

65
Q

Why are water and ethanol miscible?

A

Water and ethanol are miscible as they both contain hydrogen bonding so they mix well leaving no visible boundary.

66
Q

Why is sugar miscible?

A

Sugar has intramolecular pure covalent bonding but has polar -OH groups allowing it to dissolve in water.

67
Q

What compounds are immiscible?

A

Hexane.

68
Q

Why is hexane immiscible?

A

Hexane is pure covalent.

69
Q

What does water do on cooling?

A

Contract

70
Q

What does water do at 4℃?

A

Expand

71
Q

At 0℃ what is ice less dense than?

A

Water

72
Q

Why is ice at 0℃ less dense than water?

A

This is due to the molecules arranging themselves into a LATTICE where HYDROGEN BONDING takes a full part.

73
Q

Explain how the structure of ice allows to float on water?

A

As water cools, the hydrogen bond overcomes the decreasing thermal motion of the molecules, and takes a greater part in the bonding structure. Effectively the hydrogen bond “locks” the water molecules in a hexagonal structure. This means that the molecules can move further away from each other which leads to a decrease in density, hence ice floats.

74
Q

What is the basic explanation of how ice floats on water?

A

Hydrogen bonding between molecules in ice results in an expanded structure that causes the density of ice to be less than that of water at low temperatures.

Higher Chemistry (19 decks)

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