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AQA A Level Chemistry > 1.3 Bonding > Flashcards

1.3 Bonding Flashcards

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1
Q

What is ionic bonding

A

Strong electrostatic forces of attraction between oppositely charged ions held in a lattice

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2
Q

Give an example of an ionically bonded substance

A

NaCl

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3
Q

How high are ionically bonded substances mp and bp? Why?

A

High - takes lots of energy to break strong electrostatic forces of attraction between oppositely charged ions

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4
Q

Do ionic compounds conduct electricity? Why?

A

Yes, when molten / in solution as the ions are free to move and carry charge (don’t conduct when solid)

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5
Q

What is simple molecular covalent bonding?

A

Strong covalent bonds between atoms, weak Van de Waals forces of attraction between molecules

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6
Q

Are there any lone electrons in simple covalent bonding

A

No - all involved in bonding

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7
Q

Can simple molecular covalent molecules conduct electricity? Why?

A

No - all electrons used in bonding and aren’t free to move

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8
Q

Do simple molecular substances have a high/low mpt and bpt? Why?

A

Low - weak van de Waals forces of attraction between molecules that don’t take much energy to overcome (these are overcome rather than covalent bonds)

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9
Q

Describe macromolecular covalent bonding

A

Lattice of many atoms held together by strong covalent bonds

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10
Q

Do substances with macromolecular covalent bonds have high/low mpt and bpt ? Why?

A

High, as it takes a lot of energy to overcome many strong covalent bonds

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11
Q

Do substances with macromolecular covalent bonds conduct electricity?

A

Most don’t as all electrons are used in bonding

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12
Q

Describe the structure of diamond

A

3D tetrahedral structure of C atoms with each C atom bonded to 4 others

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13
Q

Describe the structure of graphite

A

Similar to diamond but each atom is only bonded to 3 others so it is in layers
Weak van de Waals forces of attraction between layers allow them to Slide Over each other —> soft and slippery
One electron of each carbon is delocalised and can carry charge —> can conduct electricity

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14
Q

Describe metallic bonding

A

Lattice of positive metals ions strongly attracted to a sea of delocalised electrons. Layers slide over each other - malleable

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15
Q

Do metallic compounds have high mpt / bpt ? Why ?

A

High as strong forces of attraction between positive metal ions and negatively charged sea of delocalised electrons

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16
Q

Do metallic compounds conduct electricity ? Why?

A

Yes as delocalised electrons can move throughout the metal to carry charges

17
Q

How does the strength of metallic bonding change across the periodic table? Why?

A

Increases - higher mpt and bpt, stronger
Higher charge on metal ions
More delocalised electrons per metal ion
Stronger forces of attraction between

18
Q

Define electronegativity

A

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

19
Q

What affects electronegativity ? (3)

A

Atomic radius
Nuclear charge
Electron shielding

20
Q

What is the most electronegative element?

A

Fluorine (F) - 4.0 on paulings scale
Largest nuclear charge for its electron shielding, smallest atomic radius

21
Q

How do you get a non-polar bond?

A

Both bonding elements have the same electronegativity

22
Q

When do you get a polar bond?

A

When both bonding atoms have different electronegativity

23
Q

What is the strongest form of inter-molecular force?

A

Hydrogen bonding

24
Q

What is the weakest form of intermolecular force?

A

Van de Waals forces

25
Q

Describe Van de Waals forces of attraction

A

Temporary dipole is created by random movement of electrons —> induces dipole in neighbouring molecule —> temporary induced dipole dipole attraction aka Van de Waals forces of attraction

26
Q

Are Van de Waals forces greater or smaller in larger molecules

A

Larger - more electrons

27
Q

Describe permanent dipole-dipole attraction

A

Some molecules with polar bonds have permanent dipoles —> forces of attraction between those dipoles and the dipoles of neighbouring molecules

28
Q

What conditions are needed for hydrogen bonding to occur?

A

O-H, N-H or F-H bond, lone pair of electrons on O, F, N
Because O, F and N are highly electronegative, H nucleus is left exposed
Strong force of attraction between H nucleus and lone pair of electrons on O, F or N of a neighbouring molecule

29
Q

Why is ice less dense than liquid water

A

In liquid water, hydrogen bonds constantly break and reform as molecules move about
In ice, the hydrogen bonds hold the molecules in fixed positions; this makes them slightly further apart than in water, making ice less dense than water

30
Q

What is a dative/ coordinate covalent bond? When is it formed?

A

Formed when an electron deficient atom/ion accepts a lone pair of electrons from an atom with a lone pair of electrons (not used in bonding)

31
Q

What does the shape of molecules depend on?

A

Number of electrons in the valence shell of the central atom
Number of these electrons which are bonded or in lone pairs

32
Q

What does the electron pair repulsion theory state?

A

That electrons will take up positions as far away from each other as possible, to minimise the repulsive forces between them

33
Q

Which experience the strongest repulsion
Lone pair - lone pair
Lone pair - bonded pair
Bonded pair - bonded pair

A

LP-LP strongest repulsion
LP-BP middle repulsion
BP-BP weakest repulsion

34
Q

What is the shape, diagram and bond angle in a shape with 2 bonded pairs and 0 lone pairs?

A

Linear
180 degrees
•—•—•

35
Q

What is the shape, diagram and bond angle in a shape with 3 bonded pairs and 0 lone pairs

A

Trigonal planar
120 degrees

36
Q

What is the shape, diagram and bond angle in a shape with 4 bonded pairs and 0 lone pairs?

A

Tetrahedral
109.5 degrees

37
Q

What is the shape diagram and bond angle in a shape with 5 bonded pairs and 0 lone pairs

A

Trigonal bipyramid
90 and 120 degrees

38
Q

What is the shape diagram and bond angle in a shape with 6 bonded pairs and 0 lone pairs

A

Octahedral
90 degrees

AQA A Level Chemistry (34 decks)

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