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Physical Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is ionic bonding?

A

Electrons are transferred from metals to non metals to achieve a full outer shell.

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2
Q

Why are melting points and boiling points high in ionic bonding?

A

The positive and negative charged ions are attracted to each other by electrostatic forces. This takes a great deal of energy to overcome.

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3
Q

What makes ionic bonds easy to overcome electrostatic forces?

A

They are soluble in polar substances such as water. Many ionic compounds dissolve in polar solvents.

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4
Q

When does solubility decrease?

A

As charges get higher.

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5
Q

Why don’t ionic compounds conduct electricity when solid?

A

The ions are locked in place by electrostatic forces. Since they can’t move, they can’t carry a charge.

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6
Q

What is covalent bonding?

A

Electrons are shared between non-metals and non-metals to gain a full outer shell.

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7
Q

What is expansion of the octet?

A

Elements can have more than 8 electrons on the outer shell.

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8
Q

What is a dative covalent bond?

A

When an atom uses a lone pair of electrons to form a covalent bond.

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9
Q

How is a dative bond shown?

A

As an arrow pointing away from the central atom.

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10
Q

What does the dotted line in shapes of molecules mean?

A

The bond goes behind.

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11
Q

What does the wedge mean?

A

The bond goes forward.

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12
Q

Why are the atoms around the central pair far from each ohter?

A

Electrons repel all other electron pairs, atoms around the central atom move as far apart as possible to minimise repulsion.

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13
Q

2 B.P 0 L.P?

A

Linear -> 180 degrees

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14
Q

3 B.P 0 L.P?

A

Trigonal Planar -> 120 degrees.

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15
Q

4 B.P 0 L.P?

A

Tetrahedral -> 109.5 degrees.

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16
Q

5 B.P 0 L.P?

A

Trigonal Bypyramidal -> 120 degrees and 90 degrees.

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17
Q

6 B.P 0 L.P?

A

Octahedral -> 90 degrees.

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18
Q

Do bonding pairs or lone pairs repel more strongly than the other?

A

Lone pairs.

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19
Q

What happens due to repulsion?

A

Bond angles decrease by 2.5 degrees.

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20
Q

3 B.P 1 L.P?

A

Pyramidal -> 107 degrees.

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21
Q

2 B.P 1 L.P?

A

V Shape -> 107 degrees.

22
Q

2 B.P 2 L.P?

A

V Shape -> 104.5 degrees.

23
Q

4 B.P 1 L.P?

A

See saw -> 114 degrees and 89 degrees.

24
Q

3 B.P 2 L.P?

A

T Shape -> 120 degrees or 89 degrees.

25
Q

5 B.P 1 L.P?

A

Square pyramid -> 89 degrees

26
Q

4 B.P 2 L.P?

A

Square Planar -> 90 degrees.

27
Q

Describe metallic bonding?

A

Lattice of positively charged ions surrounded by sea of delocalised electrons provides strong electrostatic forces of attraction between oppositely charged particles.

28
Q

What happens as the charge on the positive ion gets greater in metallic bonding?

A

Attractive forces get stronger as more electrons released into the sea.

29
Q

What happens as the ions get larger in size in metallic bonding?

A

Weaker attraction due to the larger atomic radius.

30
Q

What are the 4 crystal structures?

A

Metallic
Ionic
Macromolecular
Simple molecular

31
Q

Describe the forces in simple molecular?

A

Weak van der waal forces. Not much energy required to overcome them. Low melting and boiling points.

32
Q

Why does water have a high boiling point?

A

Due to hydrogen bonding.

33
Q

Are simple molecular structures good conductors of electricity? Why?

A

No, they have no charged particles.

34
Q

Describe the macromolecular structure.

A

Giant lattice structure.

35
Q

Why does macromolecular structure have high melting point?

A

Multiple strong covalent bonds.

36
Q

Why is diamond rigid?

A

Each carbon atom is bonded to 4 other carbon atoms.

37
Q

Why is graphite a good conductor of electricity?

A

Carbons bond to 3 others in flat sheets. So there are free electrons moving between layers which conduct electricity.

38
Q

What is electronegativity?

A

The power of an atom to attract negative charge towards itself within a covalent bond.

39
Q

Where does electronegativity increase and decrease?

A

Along a period increases because atomic radius decreases. Down a group decreases because of shielding increasing.

40
Q

What happens if two atoms with different electronegativities bond?

A

A polar bond forms. (Permanent Dipole)

41
Q

When does an induced dipole form?

A

When there is an influence by another charged particle.

42
Q

What scale measures electronegativity?

A

Pauling Scale.

43
Q

What are the most electronegative elements?

A

Fluorine
Chlorine
Oxygen
Nitrogen

44
Q

What 3 factors does electronegativity depend on?

A

Size of the positive charge on the nucleus.
Atomic Radius
Shielding

45
Q

What is a dipole?

A

A separation of charge.

46
Q

What are the 3 Intermolecular Forces?

A

Van der Waal Forces
Hydrogen Bonding
Permanent Dipole-Dipole

47
Q

Strongest to weakes IMF forces?

A

Hydrogen
Permanent Dipole-Dipole
VDW

48
Q

What are van der waal forces caused by?

A

Random electron movement.

49
Q

What happens when there are higher number of electrons (VDW)?

A

Stronger VDW forces.

50
Q

Where does the Hydrogen bond occur?

A

Directly from hydrogen to lone pair of electrnos.

51
Q

What elements do Hydrogen bond with in hydrogen bonding?

A

Nitrogen
Oxygen
Fluorine.

Physical Chemistry (4 decks)

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