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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Where does ionic bonding occur?

A
  • occurs between a non-metal and metal
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2
Q

Why does ionic bonding occur?

A
  • electrons are completely transferred from one atom to another to form ions
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3
Q

What is an anion?

A

Negative ion

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4
Q

What is an cation?

A

Positive ion

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5
Q

How many electrons does Group 1 gain or lose?

A

Loses 1 electron and becomes a +1 positive ion

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6
Q

How many electrons does Group 2 gain or lose?

A

Loses 2 electrons and becomes a +2 positive ion

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7
Q

How many electrons does Group 6 gain or lose?

A

Gain 2 electrons and becomes a negative 2- negative ion

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8
Q

How many electrons does Group 7 gain or lose?

A

Gain 1 electron and becomes a negative 1- negative ion

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9
Q

What holds ions together?

A

Strong electrostatic forces of attraction

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10
Q

Can ions conduct electricity?

A
  • when they are aqueous/molten

- ions are free to move and carry a charge

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11
Q

Are ions soluble?

A

Yes

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12
Q

Do ions have a low or high melting point?

A

High

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13
Q

Where does covalent bonding occur?

A
  • occurs between 2 non-metals
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14
Q

Why does covalent bonding?

A

When 2 atoms share electrons for a full stable outer shell

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15
Q

What is a dative bond?

A

When 2 electrons are shared but are from the same atom (arrow represents this)

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16
Q

What types of covalent structures are there?

A
  • small

- giant

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17
Q

What state are small covalent structures at room temperature an why?

A
  • gases as intermolecular forces are weak and don’t need much energy to break
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18
Q

Describe the shape of diamond’s structure?

A
  • tetrahedral structure

- 1 bonded to 4 others

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19
Q

Why is diamond hard?

A
  • strong covalent bonds between atoms (millions of carbon atoms)
20
Q

Why can’t diamond conduct electricity?

A
  • no free electrons to carry the charge
21
Q

Does diamond and graphite has a high or low melting point?

A

High

22
Q

Describe the shape of graphite’s structure?

A
  • hexagonal structure

- 1 bonded to 3 others

23
Q

Why is graphite soft?

A

Weak intermolecular forces between layers which are easily broken so they can slide past each other.

24
Q

How can graphite conduct electricity?

A

One spare electron on each carbon atom becomes delocalised between the layers and can carry a charge.

25
Q

Why can graphite only conduct electricity in certain directions?

A

Electrons can’t move through layers as they don’t have the energy so they conduct parallel to layers not perpendicular.

26
Q

Describe a charged cloud?

A

An area where you have a big possibility of finding an electron.

27
Q

Why do lone pairs make the shape of a molecules more oval?

A

They repel each other as they are closer to the central atom and more spread out so they take more space

28
Q

What size should all angles representing charge clouds be?

A

109.5

29
Q

What are the order of angles in charge clouds

A

biggest - lone/lone pair
second biggest - lone/bonding
smallest - bonding/bonding

30
Q

Describe electronegativity?

A

The ability to attract the bonding pairs in a covalent bond.

31
Q

Explain why electronegativity happens?

A
  • in a covalent bond, two different elements have different electron density that isn’t shared equally
32
Q

State the most electronegative elements?

A

FOClN

33
Q

State the factors affecting electronegativity?

A
  • nuclear charge
  • atomic radius
  • shielding
34
Q

Explain the effect of nuclear charge?

A
  • more protons = stronger attraction between nucleus and bonding electrons
  • high nuclear charge means high electronegativity
35
Q

Explain the effect of atomic radius?

A
  • as radius increases, bonding pairs become further away from nucleus = less attraction to positive nuclear charge
  • large atomic radius means lower electronegativity
36
Q

Explain the effect of shielding?

A
  • less shells between nucleus and electrons = less repulsion (shielding) = stronger attraction between nucleus and bonding pair of electrons
  • higher shielding means lower electronegativity
37
Q

Explain the trend down a group?

A
  • atomic radius increases
  • more shielding
  • less attraction between nucleus and bonding pair
38
Q

Explain the trends across a period?

A
  • atomic radius
  • more nuclear charge
  • stronger attraction between nucleus and bonding a pair
39
Q

Explain what a non-polar bond is?

A

If electronegativity in both atoms in a covalent are identical, the electrons in the bond will be equally attracted to both of them.

THIS RESULTS IN A SYMMETRICAL DISTRIBUTION OF ELECTRON DENSITY! (o2)

40
Q

Explain what a polar bond is?

A

If electronegativity of both atoms in a covalent bond is different (MORE THAT 0.5) the electrons in the bond will be pulled towards the more electronegative one.

THIS RESULTS IN A UNSYMMETRICAL DISTRIBUTION OF ELECTRON DENSITY! (HCl)

41
Q

State what a dipole is?

A

A difference in a charge between 2 atoms caused by a shift in electron density in the bond.

42
Q

Which type of bonding is more/less polar?

A
  • less polar have more covalent character

- more polar have more ionic character

43
Q

Why is it that even if a molecule has a polar bond it is not necessarily a polar molecules?

A

There was to be an uneven distribution of charge over the whole molecule - dipole

44
Q

State the three types of intermolecular forces?

A
  1. Instantaneous dipole - dipole forces (Van der Waal)
  2. Permanent dipole - dipole force
  3. Hydrogen bonds (STRONGEST)
45
Q

Describe a Van der Waal force?

A

When an instantaneous dipole induces another dipole so opposite charges attract.

46
Q

Describe when a permanent dipole - dipole force happens?

A

Dipoles are in a manner so the electrostatic attraction between opposite charges align

47
Q

When does hydrogen bond happen?

A

When hydrogen is bonded to fluorine, nitrogen and oxygen because they are small, polar and have lone pairs.

Chemistry (5 decks)

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