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AQA A Level Chemistry > Bonding > Flashcards

Bonding Flashcards

1
Q

Definition of Electronegativity

A

The ability of an atom to attract the pair of electrons in a covalent bond

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2
Q

The most electronegative Element

A

Fluorine

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3
Q

Shape and Bond angle for a Molecule with 2bp and 0lp

A

Shape: Linear
Bond Angle: 180

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4
Q

Shape and Bond angle for a Molecule with 2bp and 1lp

A

Shape: Bent/V-Shaped
Bond Angle:

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5
Q

Shape and Bond angle for a Molecule with 3bp and 0lp

A

Shape: Trigonal Planar
Bond Angle: 120

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6
Q

Shape and Bond angle for a Molecule with 3bp and 1lp

A

Shape: Pyramidal
Bond Angle: 107

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7
Q

Shape and Bond angle for a Molecule with 4bp and 0lp

A

Shape: Tetrahedral
Bond Angle: 109.5

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8
Q

Shape and Bond angle for a Molecule with 5bp and 0lp

A

Shape: Trigonal Bipyramidal
Bond Angle: 120, 90

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9
Q

Shape and Bond angle for a Molecule with 6bp and 0lp

A

Shape: Octahedral
Bond Angle: 90

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10
Q

Shape and Bond angle for a Molecule with 2bp and 2lp

A

Shape: Bent
Bond Angle: 104.5

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11
Q

Shape and Bond angle for a Molecule with 4bp and 1lp

A

Shape: Seesaw
Bond Angle: 102, 86.5

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12
Q

Shape and Bond angle for a Molecule with 3bp and 2lp

A

Shape: T-Shaped
Bond Angle: 87.5

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13
Q

Shape and Bond angle for a Molecule with 5bp and 1lp

A

Shape: Square Pyramidal
Bond Angle: 90

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14
Q

Shape and Bond angle for a Molecule with 4bp and 2lp

A

Shape: Square Planar
Bond Angle: 90

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15
Q

When ions are formed

A

When electrons are transferred from one atom to another

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16
Q

Names and charges of 5 common compound ions

A

Ammonium (NH4 +), Carbonate (CO3 2-), Hydroxide (OH-), Nitrate (NO3 -), Sulfate (SO4 2-)

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17
Q

Define Electrostatic Attraction

A

Attraction between + and -

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18
Q

Structure of Giant Ionic Lattice

A

Regular alternating structure of + and - ions

19
Q

Ionic Compounds’ Electrical Conductivity

A

Conduct electricity when molten or dissolved
Ions are free to flow in liquid

20
Q

Ionic Compounds’ Melting Point

A

High due to strong electrostatic forces

21
Q

Ionic Compounds’ Solubility

A

Tend to dissolve in water as water molecules are polar and pull ions appart

22
Q

When do molecules form?

A

When 2+ atoms bond together

23
Q

What does a single covalent bond contain?

A

a shared pair of electrons that are attracted to both positive nuclei

24
Q

Definition of Covalent Bonding

A

the electrostatic attraction between nuclei of two atoms and the bonding electrons of their outer shells

25
Q

Examples of Macromolecular Structures

A

Graphite
Diamond

26
Q

The structure of Graphite

A

Layers of sheets of hexagonal carbon rings with delocalised electrons flowing between them. the sheets are held together by weak van der waals

27
Q

The structure of Diamond

A

Carbon atoms arranged in a tetrahedral shape forming a crystalline lattice structure

28
Q

Definition of a co-ordinate bond

A

a type of covalent bond where one atom donates a pair of valence electrons to another atom/ion

29
Q

What is a charge cloud?

A

the area where electrons can be found around the nuclei

30
Q

What is Valence shell electron pair repulsion theory?

A

lp-lp>lp-bp>bp-bp

31
Q

What makes a molecule polar?

A

Asymmetrical arrangement of polar bonds

32
Q

What makes a bond polar?

A

a difference in electronegativity

33
Q

What are the three types of intermolecular forces?

A

Hydrogen Bonding
Dipole-Dipole
van der Waals

34
Q

What is Hydrogen Bonding?

A

forces of attraction between H and N,O, or F

35
Q

What are dipole-dipole forces?

A

forces between the + and - of neighbouring polar molecules

36
Q

What are van der Waals forces?

A

when electrons are randomly arranged on one side of the nucleus, this induces a temporary dipole in surrounding molecules creating a weak intermolecular force

37
Q

Simple covalent molecules’ electrical conductivity

A

no

38
Q

Simple covalent molecules’ melting point

A

low due to weak intermolecular forces

39
Q

Simple covalent molecules’ solubility

A

some dissolve in water depending on how polar the molecule is

40
Q

Definition of Metallic Bonding

A

the attraction between delocalised electrons and positive ions

41
Q

Metallic Structures’ Melting point

A

high due to strong electrostatic attraction

42
Q

Metallic Structures’ ability to be shaped

A

no bonds holding specific ins together so can slide and be molded

43
Q

Metallic Structures’ conductivity

A

delocalised electrons

44
Q

Metallic Structures’ solubility

A

insoluble except in liquid metals

AQA A Level Chemistry (9 decks)

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