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AS Chemistry Year 12 > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is ionic bonding?

A

Strong electrostatic force of attraction oppositely charged ions held in a lattice

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2
Q

Give an example of ionically bonded substance

A

NaCl(sodium chloride-salt)

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3
Q

Do ionically bonded substances have a high melting and boiling point?

A

High - it takes a lot of energy to break the strong electrostatic forces of attraction between opposite charged ions

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4
Q

Can ionic compounds conduct electricity?

A

Yes, when molten or aqueous as the ions are free to move and carry charge(don’t when in solid state)

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5
Q

What is simple molecular covalent bonding?

A

Strong covalent bonds between atoms, weak van der waals forces between molecule

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6
Q

Are there any lone pair electrons in simple covalent bonding?

A

No-all involved in bonding

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7
Q

Can simple molecular covalent molecules conduct electricity?

A

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

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8
Q

Do simple molecular substances have a high melting and boiling point?

A

Low-weak van der waals forces between molecules that don’t take much energy to overcome

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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 binds have high melting and boiling points?

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

What’s metallic bonding?

A

Lattice of positive metal ions strongly attracted to a sea of delocalised electrons

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13
Q

Do metallic compounds have a high melting and boiling point?

A

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

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14
Q

Do metallic compounds conduct electricity?

A

Yes, as delocalised electrons can move throughout the metal to carry charge

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15
Q

How does the strength of metallic bonds change across the perodic table?

A

Increases—>higher melting and boiling point, higher charge on metal ions, more delocalised electrons per ion, stronger forces of attraction between them

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16
Q

Define electronegativity

A

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

17
Q

What affects electronegativity?

A

Nuclear charge
Atomic radius
Electron shielding

18
Q

What is the most electronegative element?

A

Fluorine(4.0 on Paulings scale)
Largest nuclear charge for its electron shielding, small atomic radius

19
Q

How do you get a non-polar bond?

A

Both bonding elements have the same electronegativities

20
Q

When do you get a polar bond?

A

Bonding atoms have different electronegativities

21
Q

What is the strongest type of intermolecular force?

A

Hydrogen bonding

22
Q

What is the weakest type of intermolecular force?

A

Van der waal forces

23
Q

Describe van der waals forces of attraction

A

●Temporary dipoles are created by the random movement of electrons
●induces dipole in neighbouring molecule
●temporary induced dipole-dipole attraction aka van der waals forces

24
Q

Are van der waals forces greater in smaller or larger molecules?

A

Larger-more electrons

25
Q

Describe permanent dipole-dipole attraction

A

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

26
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,N,and F are highly electronegative, H nucleas is left exposed.
Strong force of attraction between H nucleas and lone pair of electrons on O,N,F

27
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 liquid water

28
Q

What is dative/ coordinating covalent bond? When is it formed?

A

A type of covalent bond where both the electrons in the shared pair come from the same atom

29
Q

What does the shape of molecule depend on?

A

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

30
Q

What does the electron pair repulsion theory state?

A

Electron pairs will take up positions as far away from each other as possible to minimise the repulsive forces between them

31
Q

Which experience the most repulsion?

A

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

32
Q

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

A

Linear
180°

33
Q

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

A

Trigonal planar
120°

34
Q

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

A

Tetrahedral
109.5°

35
Q

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

A

Trigonal Bipyramidal
90° and 120°

36
Q

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

A

Octahedral
90°

AS Chemistry Year 12 (15 decks)

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