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Chemistry A Level > Bonding - Chapter 3 > Flashcards

Bonding - Chapter 3 Flashcards

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1
Q

What types of bonding are there

A

Ionic
Covalent
Metallic

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2
Q

What are the three types of covalent bond

A

Simple Covalent e.g. H2
Giant Covalent e.g. Diamond
Coordinate (dative covalent)

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3
Q

What is a bond

A

An attractive force holding particles together

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4
Q

What is ionic bonding

A

Bonding between a metal and a non-metal

Where electrons are transferred from the metal to the non metal

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5
Q

What is an ionic bond

A

The electrostatic attraction between oppositely charged ions

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6
Q

What is a covalent bond

A

It is a bond between non-metals
where electrons are shared between the atoms

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7
Q

What is a covalent bond

A

It is a shared pair of electrons, and the electron pair is attracted by both nuclei so resists separation

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8
Q

What is a coordinate bond

A

It is a covalent bond where both electrons in the shared pair originate from the same atom

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9
Q

What is metallic bonding

A

It is attraction inside a metal between the positive metal ions and the sea of delocalised electrons

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10
Q

Why is there a sea of delocalised electrons in a metal

A

Outer electron is only weakly held so it becomes delocalised

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11
Q

What determines the shape of a molecule or ion

A

The number of electron pairs in the outer shell of the central atom

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12
Q

Why do species containing only bonding pairs have regular molecular shapes

A

Because bonding pairs of electrons exert equal repulsion on each other

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13
Q

What is the shape of an molecule with 2 bonding pairs

A

It is linear
Bond angle of 180 degrees
Shape of a straight line

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14
Q

What is the shape of molecule with 3 bonding pairs

A

Trigonal Planar
Bond angle of 120 degrees
Triangle shape

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15
Q

What is the shape of a molecule with 4 bonding pairs

A

Tetrahedral
Bond angle of 109.5 degrees
Triangular based pyramid

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16
Q

What is the shape of a molecule with 5 bonding pairs

A

Trigonal Bipyramidal
Bond angles of 90 degrees and 120 degrees
Triangle with another atom opposite the top of the triangle

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17
Q

What is the shape of a molecule with 6 bonding pairs

A

Octahedral
Bond angle of 90 degrees
Square with two atoms above and below

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18
Q

What does the shape of a molecule also depend on

A

The presence of non-bonding electron pairs (lone pairs)

Lone pairs take up more space because they are held closer to the nucleus so repel more strongly

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19
Q

What is the shape of a lone pair in a trigonal planar

A

Bent
Two atoms are slightly bent and at an angle

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20
Q

What are the two shapes of lone pairs in a tetrahedral

A

1 Lone Pair: Trigonal pyramidal
2 Lone Pair: Bent

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21
Q

What are the 3 shapes with lone pairs in a Trigonal Bipyramidal

A

1 Lone Pair: Sawhorse
2 Lone Pair: T- shaped, Lone pairs in the middle
3 Lone Pair: Linear

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22
Q

What are the 4 shapes with lone pairs in an Octahedral

A

1 Lone Pair: Square Pyramidal
2 Lone Pair: Square Planar
3 Lone Pair: T-shaped
4 Lone Pair: Linear

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23
Q

What is the order of decreasing replusion between electron pairs

A

Lone pair - Lone pair
Lone pair - Bonding pair
Bonding pair - Bonding pair

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24
Q

What is the method to find the shape of a molecule without double bonds

A
  1. Count number of outer electrons on the central atom
  2. add 1 for every atom bonded to the central atom
  3. For ions add 1 if singly negative, subtract 1 if singly positive
  4. Total then divide by 2 to get number of electron pairs
  5. Deduce the regular shape taken up by this number of pairs
  6. If any of the pairs are lone pairs alter the shape
25
Q

What happens when two different elements are bonded together

A

The electron pair is not equally attracted to both nuclei because the elements have different electronegativities

26
Q

What is electronegativity

A

It is the power of an atom to attract the pair of electrons in a covalent bond

27
Q

What affects electronegativity

A

Nuclear charge
As nuclear charge goes up so does electronegativity
Atomic radius
As atomic radius increases so does shielding which causes electronegativity to decrease

28
Q

What is electronegativity measured using

A

Pauling scale

29
Q

What happens to electronegativity across a period

A

There is an increasing nuclear charge which means the electron are more attracted to the nucleus so atomic radius reduces and electronegetivity increases

30
Q

What happens to electronegativity up a group

A

Fewer energy levels and the outer electrons are less shielded so electronegativity increases

31
Q

What is used to symbolise which element has a greater electronegativity

A

A lower case delta is used with a plus and a minus to show the stronger electrongetativity
The negative is used on the stronger one

32
Q

What is a polar molecule

A

It is one in which the electron density across the whole molecule is unevenly distributed

33
Q

What happens when the charge on the molecule isnt symetrical

A

It is polar overall and described as permanent dipole

34
Q

What are the 3 types of intermolecular forces

A

Dipole-Dipole interactions
Hydrogen bonding
Van der Waal’s forces

35
Q

What is dipole-dipole interactions

A

They are attractive forces between polar molecules
The polar molecules will flip to give an arrangement where the molecules attract

36
Q

What are hydrogen bonds

A

They are very strong intermolecular forces
It takes place when a hydrogen is bonded to a very electronegative element like Oxygen, Fluorine and Nitrogen and there is at least 1 lone pair

37
Q

What are Van der Waal’s forces

A

They are temporary dipole - induced dipole interactions
They happen in all molecules
Caused by the movement of electrons, so the more electrons the stronger the force is

38
Q

What is the order of strength of intermolecular forces at an increasing strength

A

Van der Waals
Dipole - dipole
Hydrogen bonding

39
Q

How do two sets of polar molecules or 2 sets of non-polar molecules interact as liquids

A

They are miscible
but different polar states means that they are non-miscible

40
Q

What are the 3 states of matter

A

Solid
Liquid
Gas

41
Q

What are solids like

A

They have an arrangement of close and regular and vibrate about a fixed position

42
Q

What are liquids like

A

They have an arrangement of random, close and can move past each other

43
Q

What are gases like

A

they have an arrangemnet of random, far-apart, rapid and random motion

44
Q

What is the process solid to liquid

A

melting

Fusion

45
Q

What is the process liquid to gas

A

Boiling

vaporisation

46
Q

What is the process Gas to liquid

A

Condensation

47
Q

What is the process liquid to solid

A

Freezing

Solidifying

48
Q

What is the process solid to gas

A

Sublimation

49
Q

What are crystals

A

they are solids that contain particles in a regular arrangement known as a lattice

50
Q

What are the 4 types of crystal lattices

A

Ionic
Metallic
Molecular (simple covalent)
Macromolecular (giant covalent)

51
Q

What are ionic crystals

A

They are positive and negative ions held together in a giant lattice by strong electrostatic attraction between oppositely charged ions

52
Q

Properties of ionic compounds

A

High MP - Strong electrostatic attraction
Conductors as liquid - Ions
Hard and Brittle - Like ions repel
Dissolve in water - Ions become surronded by water

53
Q

What are metallic crystals

A

A giant lattice of positive ions held together by a sea of delocalised electrons

54
Q

Properties of metals

A

High MP and BP - Strong metallic bonds
Conduct electricity - Sea of delocalised electrons
Malleable and ductile - Ions slide over eachother
Insoluble in water - Water can’t break bonds

55
Q

What are molecular crystals

A

Individual molecules held together by weak intermolecular forces

56
Q

Properties of molecular solids

A

Low MP - Weak intermolecular forces
Soft - Weak intermolecular forces
Dont conduct electricity - No ions or electrons

57
Q

What are Macromolecular crystals

A

A giant arrangement of atoms joined by covalent bonds

58
Q

Properties of Diamond

A

High melting point - Strong covalent bonds
Very Hard - Strong covalent bonds
Non-Conductor - No ions or electrons

59
Q

Properties of Graphite

A

High MP - Strong covalent bonds
Soft - Weak attraction between layers
Conducts electricity - delocalised 4th electron

Chemistry A Level (20 decks)

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