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As level Chemistry > Bonding And Structure > Flashcards

Bonding And Structure Flashcards

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1
Q

What are the 3 main types of chemical bonds?

A

Ionic
Covalent
Metallic

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2
Q

Define ionic bonding

A

The electrostatic attraction between positive and negative ions.

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3
Q

Give an example of an ironically bonded substance

A

NaCl salt

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4
Q

Define covalent bonding

A

Electrostatic attraction between a shared pair of electrons and the nuclei

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5
Q

Define metallic bonding

A

Electrostatic attraction between the positive metal ions and the sea of delocalised electrons

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6
Q

Why does giant ionic lattices conduct electricity when liquid but not solid?

A

In solid state the ions are in fixed positions and therefore can’t move.
When they are in liquid state the ions are mobile and thus can freely carry the charge.

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7
Q

Giant ionic lattices have a high melting point, why?

A

Large amount of energy is required to overcome the strong electrostatic bonds.

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8
Q

In what type of solvents do ionic lattices dissolve?

A

Polar solvents

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9
Q

Why are ionic compounds soluble in water?

A

Water has a polar bond, hydrogen atoms have a positive charge and oxygen atoms have a negative charge. These charges are able to attract the charges ions.

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10
Q

What is it called when atoms are bonded by a single pair of shared electrons?

A

Single bond

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11
Q

How many covalent bonds does carbon form?

A

4

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12
Q

How many covalent bonds does oxygen form?

A

2

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13
Q

What is a lone Pair?

A

Electrons in the outer shell that are not involved in the bonding

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14
Q

What is formed when atoms share 2 pairs of electrons?

A

Double bond

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15
Q

What is formed when atoms share 3 pairs of electrons?

A

Triple bond

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16
Q

What is average bond Enthalpy ?

A

Measure the average energy needed to break the bond

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17
Q

What is a dative covalent bond?

A

A bond where both of the shared electrons are supplied by one atom

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18
Q

How are oxoniums ions formed?

A

Formed when acid is added to water H3O+

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19
Q

What does expansion of the octet mean?

A

When a bonded atom has more than 8 electrons in the outer shell.

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20
Q

What are the types of covalent structure?

A

Simple molecular lattice

Giant covalent lattice

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21
Q

Describe the bonding in simple molecular structures

A

Atoms within the same molecule are held by strong covalent bonds and different molecules are held by weak intermolecular forces.

22
Q

Why do simple molecular structures have low melting and boiling points?

A

Small amount of energy is enough to overcome the intermolecular forces.

23
Q

Can simple molecular structures conduct electricity ?

A

No because they have no free charged particles to move around.

24
Q

What type of solvent do simple molecular structures dissolve in?

A

Non polar

25
Q

Give examples of giant covalent structures

A

Diamond
Graphite
Silicon dioxide

26
Q

List some properties of giant covalent structures ?

A

High melting and boiling points.
Non conductors of electricity except graphite
Insoluble in polar and no polar solvents

27
Q

How does graphite conduct electricity?

A

Delocalised electrons present between the layers are able to move freely carrying the charge

28
Q

Why do giant covalent structures have Hugh melting and boiling points?

A

String covalent bonds within the molecules need to be broken which requires a lot of energy

29
Q

Draw and describe the structure of a diamond

A

3D tetrahedral structure of c atoms bonded with 4 other c atoms

30
Q

What does the shape of a molecule depend on?

A

Number of electron pairs in the outer shell

Number of these electrons which are bonded and lone pairs

31
Q

By how many degrees does each lone pair reduce the bond angle?

A

2.5

32
Q

Define electronegativity

A

The ability of an atom to attract the pair of electrons (the electron density) in a covalent bond.

33
Q

In which direction of the periodic table does electronegativity increase?

A

Top right, towards fluorine

34
Q

What does it mean when the bond is non-polar?

A

The electrons in the bond are evenly distributed

35
Q

What is the most electronegative element?

A

Fluorine

36
Q

How is a polar bond formed?

A

Binding atoms have different electronegativities

37
Q

Why is water polar but carbon dioxide is not?

A

Calvin dioxide is a symmetrical molecule, so therefore there is no overall dipole

38
Q

What is meant by intermolecular force?

A

Attractive force between neighbouring molecules?

39
Q

What are the 2 types of intermolecular forces?

A

Hydrogen bonding
Permanent dipole permanent dipole forces
Permanent dipole - induced dipole forces

40
Q

What is the strongest type of intermolecular forces?

A

Hydrogen bonding

41
Q

Describe permanent dipole - induced dipole interactions

A

When a molecule with a permanent dipole is close to the non polar molecules it causes the non polar molecule to become slightly polar leading to attraction.

42
Q

How does graphite conduct electricity?

A

Delocalised electrons are present between the layers and are able to move freely carrying the charge.

43
Q

Describe permanent dipole-dipole interactions

A

Some molecules with polar bonds have permanent dipoles. These forces of attraction between those dipoles and those of neighbouring molecules.

44
Q

Describe London forces

A

London forces are caused by random movements of electrons.
This leads to instantaneous dipoles
Instantaneous dipole induce a dipole on nearby molecules.
Induced dipoles attract one another

45
Q

Are London forces greater in smaller or larger molecules?

A

Larger due to more electrons

46
Q

Does boiling point increase down the noble gas group? Why?

A

B.p increases because the number of electrons increases and hence the strength of London forces also increases.

47
Q

What conditions are needed for hydrogen bonding to occur?

A

O-H N-H F-H bind
Lone pair of electrons on O,F,N
Because O, N,F at highly electronegative, the hydrogen nucleus is left exposed.
Strong force of attraction between the hydrogen nucleus and lone polar of electrons on N,O,F

48
Q

Why is ice less dense than liquid water

A

In ice, the water molecules are arranged in an orderly pattern. It has an open lattice with hydrogen bonds
In water the lattices is collapsed and the molecules are closer together,

49
Q

Why does water have a higher melting and boiling point than expected.

A

Hydrogen bonds are stronger than other intermolecular forces so extra strength is required to overcome the forces.

50
Q

Other important areas in the topic

A

Shapes of molecules

Drawing if hydrogen bonding

As level Chemistry (12 decks)

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