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Fundamentals Of Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Types of chemical bonds?

A

Ionic
Covalent
Dative/co-ordinate covalent
Metallic

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2
Q

Types of physical bonds?

A

Van der Waals’ forces
Dipole-dipole interaction
Hydrogen bonds

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3
Q

What is an ionic bond?

A

An electrostatic force of attraction between positive and negative ions, usually between a metal and a non-metal

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4
Q

Structure of ionic compounds?

A

Each ion attracts oppositely charged ions in all directions. Resulting in a giant ionic lattice structure containing billions of atoms

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5
Q

Properties of ionic bonds in regards to melting/boiling?

A

Most are solids at room temperature as there is insufficient energy to overcome the strong electrostatic forces of attraction so most have high melting and boiling points
the greater the ionic charge the higher the point
The larger the ion the lower the point as weaker bonds due to being spread over a large surface

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6
Q

Properties of ionic bonds in regards to solubility?

A

Most soluble in polar solvents such as water. Ionic lattice is broken down and solvent molecules surround the ions. The stronger the lattice the less soluble to compound.

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7
Q

Properties of ionic bonds in regards to electrical conductivity?

A

Can conduct electricity it only if charged ions can move. So solids cannot but molten/ dissolved compounds can.

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8
Q

What is a covalent bond?

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms. Occurs in non metals elements, non metal compounds and poly atomic ions

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9
Q

What is a simple covalent molecule?

A

A few atoms held together by covalent bonds

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10
Q

What are giant covalent structures?

A

Contain many atoms, each joined to adjacent atoms by covalent bonds. Usually arranged into giant regular lattices

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11
Q

Properties of simple covalent structure in regards to temperature?

A

Low melting and boiling points as less energy needed to break weak intermolecular forces (not strong covalent bond)

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12
Q

Properties of simple covalent structure in regards to solubility?

A

They can either be polar or non-polar.
Polar molecules dissolve in polar solvents.
Non-polar molecules dissolve in non-polar solvents

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13
Q

Properties of simple covalent structure in regards to electrical conductivity?

A

Do not conduct electricity as they do not have any free electrons or an overall electric charge

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14
Q

What is an allotrope?

A

A different form of the same element in the same state. E.g. graphite and diamond

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15
Q

Properties of giant covalent structure in regards to temperature?

A

High melting and boiling points due to presence of strong covalent bonds in the structures

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16
Q

Properties of giant covalent structure in regards to electrical conductivity?

A

Depends if there are any delocalised electrons. E.g. graphite will conduct but diamond will not

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17
Q

Properties of giant covalent structure in regards to solubility?

A

They are not soluble as covalent bonds in the lattices are too strong to be broken

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18
Q

What is metallic bonding?

A

Electrostatic interaction between positive metal ions and delocalised electrons. The atoms are ionised and these ions occupy fixed positions in the lattice. Outer shell electrons are delocalised and shared between all atoms within the structure

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19
Q

Properties of metallic bonds in regards to electrical conductivity?

A

Most conduct electricity in solid and liquid state. The delocalised electrons can move through the structure carrying a charge

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20
Q

Properties of metallic bonding in regards to temperature?

A

Most metals have high melting and boiling points. Depends upon the strength of metallic bonds within the structure. High temperatures are needed to overcome strong electrostatic attraction between the cations and electrons. The higher the ionic charge of the metal the higher the melting point

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21
Q

Properties of metallic bonds in regards to solubility?

A

Metals do not dissolve. Any interaction between polar solvents and changed in metallic lattice would lead to reaction rather than dissolving

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22
Q

Properties of metallic bonds in regards to malleability/ductile?

A

Metals can be hammered and pressed into shape as atoms can roll over each other into new positions without the bonds breaking
Metals can be drawn out into a wire again due to atoms rolling over each other

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23
Q

What is an alloy?

A

Mixtures containing metals. Not a compound as there can be different ratios of metals. They can modify a metals properties e.g. ions may be different sizes to stop layers moving past each other making it harder

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24
Q

What is a dative/coordinate bond?

A

Very similar to a covalent bond apart from both electrons involved in the bond are from the same atom.

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25
Q

Intramolecular forces definition?

A

The forces that hold atoms together within a molecule

26
Q

Intermolecular forces definition?

A

Forces that exist between molecules

27
Q

Three categories of of intermolecular bonding?

A

Induced dipole-dipole interactions (London/ Van der Waals)
Permanent dipole/dipole interactions
Hydrogen bonding

28
Q

Which type of force is weaker?

A

Intermolecular

29
Q

What is electronegativity?

A

A measure of the tendency of an atom to attract a bonding pair of electrons in a covalent bond. The greater the electronegativity the greater the attraction.

30
Q

What did Linus Pauling invent in 1932?

A

The Pauling scale to measure electronegativity of atoms

31
Q

Electronegativity…….. across a period

A

Increases

32
Q

How does atomic radius affect electronegativity?

A

As the radius increases the bonding pair of electrons becomes further from the nucleus. They are therefore less attracted to the nucleus. So the greater the radius the lower the electronegativity.

33
Q

How does the number of unshielded protons affect electronegativity?

A

Full energy levels of electrons shield the electrons in the bond from the increased attraction of the greater nuclear charge, reducing electronegativity

34
Q

Electronegativity …… down a group?

A

Decreases

35
Q

What a non-polar bonds?

A

The electronegativity in both atoms of the covalent bond is identical so the electrons are equally attracted to them both. This cause symmetrical distribution of electron density around the two atoms.

36
Q

What is a polar bond?

A

When a covalent bond is formed by atoms with different electronegativities.

37
Q

Dipoles meaning?

A

When there is asymmetrical distribution of electron density because one atom attracts the electrons more strongly this created an imbalance in the charges in the bond.

38
Q

What symbol is used to show charges between bonds?

A

Delta positive and delta negative

39
Q

Polar bonds have a more …….. character?

A

Ionic

40
Q

Non-polar bonds have a more ……… character?

A

Covalent

41
Q

What is a non-polar molecule?

A

If the polar bonds are arranged symmetrically, the partial charges cancel each other

42
Q

What is a polar molecule?

A

If polar bond are asymmetrically arranged, the partial charges do not cancel each other out

43
Q

What are van der Waals forces?

A

Resulting weak forces of attraction between the small charges (temporary dipoles)

44
Q

How does atomic radius affect van der Waals forces?

A

As the radius increases the electrons are less attracted to the nucleus so temporary dipoles are easier to induce

45
Q

How do the points of contact between molecules affect van der Waals forces?

A

The more points of contact between the molecules the stronger the van der Waals forces

46
Q

What a permanent dipole-dipole forces?

A

If molecules contain bonds with a permanent dipole the molecules may align so there is electrostatic attraction between the opposite charges on neighbouring molecules

47
Q

What is a hydrogen bond?

A

A special type of permanent dipole-dipole bond interaction found between molecules containing:
An electronegative atom with a lone pair of electrons e.g. oxygen, nitrogen, fluorine
A hydrogen atom attached to the electronegative atom.
The hydrogen bond acts between the hydrogen atom in one molecule and the lone pair of electrons in an electronegative atom of another molecule

48
Q

Strength of intermolecular forces from highest to lowest?

A

Hydrogen
Permanent dipole/dipole
Van der Waals

49
Q

Why is solid water less dense that liquid water?

A

Hydrogen bonds hold water molecules further apart in an open lattice structure when solid. So the water molecules in ice are further apart than in water

50
Q

What influences the shape of a molecule?

A

The total number of electron pairs around the central atom. Lone pairs repel more than bonding pairs.

51
Q

What is bond length?

A

The distance between the nuclei of two bonded atoms

52
Q

What is bond angle?

A

The angle between two covalent bonds

53
Q

Basic principles of electron pair repulsion theory?

A

The electron pairs around the central atom determine the shape of the molecule or ion
The electrons pairs repel electrons each other so they are arranged as far apart as possible
The arrangement of electron pairs minimise repulsion and therefore holds the bonded atoms in a definite shape
Different number of electron pairs result in different shapes

54
Q

What is a tetrahedral shape molecule?

A

Four bonded pairs repel each other as far as possible
Bond angle of 109.5
e.g. methane

55
Q

What is a pyramidal shape molecule?

A

Contains 3 bonded pairs and one lone pair of electrons. Since the lone pairs repel more strongly than bonded pairs this means the bonded angles are closer together decreasing the bond angle
Bond angle of 107
e.g. ammonia

56
Q

What is a non-linear molecule?

A

Two bonded pairs and two lone pairs. The lone pairs repel more strongly creating the V-shape
Bond angle of 104.5
E.g. water

57
Q

What is a linear shaped molecule?

A

Molecules that contain 2 bonding regions but not lone pairs
Bond angle 180
E.g. CO2

58
Q

What is a triagonal planar shape molecule?

A

Contains 3 bonded pairs and no lone pairs.
Bond angles of 120
E.g. boron trifluoride

59
Q

What is an octahedral shape molecule?

A

6 bonded pairs and no lone pairs
Bond angle of 90
E.g. SF6

60
Q

How to predict molecular shape and angles?

A

1) work out number of valance electrons of central atom
2) take into account any charges for ions
3) work out the number of covalent bonds made by the central atom
4) work out amount of electron pairs
5) determine the shape

61
Q

What is a triagonal bipyramidal shape molecule?

A

5 bonded pairs and no lone pairs
2 x 90
3 x 120

Fundamentals Of Chemistry (10 decks)

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