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HIGHER CHEMISTRY > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is the metallic bond

A

The electrostatic force of attraction between the positively charged ions and delocalised electrons.

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2
Q

Describe the structure of a metallic bond

A

a giant lattice of positively charged ions in a sea of delocalised electrons.

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3
Q

3 properties of a metallic bond

A

Electrical conductors
High mpts
Good thermal conductors

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4
Q

Metals going across the period trends and why

A

Conductivity increases as there are more delocalised electrons.

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5
Q

Metals going down a group trends and why

A

Mpts decrease as there are more occupied energy levels so the nucleus is further from the delocalised electrons.

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6
Q

What does a single covalent bond consist of

A

one shared pair of electrons

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7
Q

Define a pure covalent bond

A

when atoms of the same element form a covalent bond and the electrons are shared equally. This is because they have the same electronegativity.

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8
Q

Define a polar covalent bond

A

When atoms of different elements share electrons. Atoms with different electronegativity values will share the pair of bonding electrons unequally, forming partial changes or a permanent dipole.

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9
Q

In covalent bonds, what do the atom with the highest electronegativity do

A

will attract the bonding electrons closer towards it, therefore it turns slightly negative.

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10
Q

In covalent bonds what atom attracts the electrons (turns negative)

A

Highest electronegativity

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11
Q

Define the ionic bond

A

The ionic bond is the electrostatic attraction between positive and negative ions

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12
Q

Ionic bond structure

A

3D crystal lattice where oppositely charged ions surround each other.

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13
Q

What do elements far apart in the periodic table more likely to do

A

Form ionic rather than covalent bonds

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14
Q

4 properties of ionic bonds

A

Don’t conduct as solid ions are not free to move
High mpts
Conduct in molten or solution
Many are soluble

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15
Q

3 covalent networks

A

Boron
Carbon
Silicon

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16
Q

4 covalent network properties

A

High mpts
Hard substances
Don’t conduct
Insoluble

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17
Q

What state do van der Waals hold molecules

A

Liquid or solid

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18
Q

What atoms/molecules do vdw hold

A

Discrete atoms (noble gases)
Discrete molecules (diatomics)

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19
Q

Are VDW weak or strong

A

Weak

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20
Q

2 types of VDW

A

Permanent dipole - permanent dipole
London Dispersion Forces

21
Q

What is LDF in monatomics

A

a force caused by an uneven distribution of the constantly moving electrons around the nucleus.

22
Q

What does the uneven distribution of electrons do to monatomics

A

causes one side of the atom to have a temporary dipole.

23
Q

What is a temporary dipole

A

a slightly + charge and one side a slightly - charge

24
Q

Why do monatomics have low mpt/bpt

A

Their LDF are weak

25
Q

How are LDF formed in covalent moleculars

A

formed as a result of electrostatic attractions between the temporary dipoles and induced dipoles caused by the movement of electrons

26
Q

What is a polar covalent bond

A

a covalent bond in which the atoms have a difference in electronegativity.

27
Q

What is a permanent dipole

A

the difference in charge in polar bonds

28
Q

What forces of attraction between polar molecules

A

PD-PD

29
Q

What does the spatial arrangement of polar covalent bonds do

A

sometimes result in the overall molecule becoming non polar.

30
Q

Are hydrocarbons polar or nonpolar

A

Nonpolar

31
Q

When does hydrogen bonding occur

A

Between very polar molecules

32
Q

3 very polar molecules

A

F, N and O

33
Q

What are hydrogen bonds

A

electrostatic forces of attraction between molecules that contain highly polar bonds.

34
Q

What does a greater number of e/gfm mean for bpt and why

A

increases it as it makes a greater the chance of temporary and induced dipoles forming and therefore creating stronger LDF of attraction, so it requires more energy to separate the molecules.

35
Q

Why sulfur has larger bpt than phosphorus

A

-Sulfur has an S8 discrete molecule structure and phosphorus has a P4 discrete molecule structure.
-The sulfur molecule contains more electrons than phosphorus, so there are more temporary dipoles in sulfur.
-This creates stronger LDF between the sulfur molecules, requiring more energy to separate them.

36
Q

Fullerne/C60 mpt

A

280

37
Q

Why would fullerene have a higher mpt than sulfur

A

it has more atoms present in the structure and therefore more LDF.

38
Q

Why compare substances with similar electrons or gfms

A

because LDF are acting on all molecules, so same gfms/e means that the strength of the LDF will be similar. Means a bpt difference can be attributed to another type of van der Waal

39
Q

Polar behaviour in electric fields

A

If a charged rod is held in a stream of liquid, the PD of polar liquids are attracted to the rod. (The flow changes)

40
Q

Viscosity meaning

A

The resistance to flow

41
Q

What molecules bonds are typically more viscous

A

polar or hydrogen bonds

42
Q

Polar and nonpolar miscibility

A

Very polar molecules do not mix with nonpolar molecules

43
Q

Explain polar and nonpolar immiscibility

A

The stronger hydrogen bonds between the water (polar) molecules cannot be broken by the nonpolar molecules as they have no charge to attract the polar molecules.

44
Q

Ionic compounds and polar covalent compounds miscibility

A

tend to be soluble in polar solvents such as water.

45
Q

Nonpolar molecular substances solubility

A

soluble in nonpolar substances.

46
Q

If charge is evenly distributed the bonding is…

A

Nonpolar

47
Q

If charge is unevenly distributed…

A

Polar

48
Q

What type of bond/force is not a van der waal

A

Covalent

49
Q

What type of bonds/forces are van der waals

A

Hydrogen
LDF
PD-PD

HIGHER CHEMISTRY (6 decks)

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