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C = Structure and Bonding = > Covalent Bonding > Flashcards

Covalent Bonding Flashcards

1
Q

What determines the length of a single covalent bond?

A

The size of the atom - the distance between the nucleus and outer shell electron.

The charge density - which affect size.

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2
Q

Which out of single bonds, double bonds and triple bonds contain the longest and shortest bond?

A

Longest bond > single bond C——C
Middle length > double bond C==C
Shortest bond > triple bond C≡O

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3
Q

Predict which bond is longer…

P-P or S-S
C≡N or C≡C
Cl-H or Br-H
C-C or C=C
N-O or P-O

A

Longest bonds…

P-P or S-S > P-P

C≡N or C≡C > C≡C

Cl-H or Br-H > Cl-H

C-C or C=C > C-C

N-O or P-O > N-O

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4
Q

What increases the length of a covalent bond?

A

The greater the SIZE of the atom, the longer the covalent bond.

The greater the CHARGE density of the atom, the longer the covalent bond.

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5
Q

Describe the relationship between bond length and bond strength.

A

As bond length decreases, the bond strength increases.

As bond length increases, the bond strength decreases.

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6
Q

Predict which bond is the strongest and weakest…

C-C
N-N
N=N

A

Strongest > N=N

Weakest > C-C

An N-N bond should be stronger than a C-C bond since it is shorter, and an N=N bond is stronger than an N-N bond since double bonds are shorter.

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7
Q

What is a covalent bond?

A

When intermolecular forces of attraction form between atoms that share 1 or more pairs of electrons in a simple molecular or giant covalent structure.

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8
Q

What is the force of attraction formed between molecules?

A

Intermolecular forces of attraction.

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9
Q

What should I always remember about covalent bonds?

A

Covalent bonds are STRONG, not weak.

Intermolecular forces are WEAK.

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10
Q

What is a single bond?

A

When atoms share 1 pair of electrons.

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11
Q

What is a double bond?

A

When atoms share 2 pairs of electrons,

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12
Q

What is a triple bond?

A

When atoms share 3 pairs of electrons.

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13
Q

List everything about covalent bonding you can remember.

A

Non-metal and non-metal.

STRONG covalent bonds.
WEAK intermolecular forces of attraction.
Electrons are SHARED.

Simple molecular structure
Giant covalent structure

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14
Q

Give examples of simple molecules.

A

Cl₂
N₂
H₂
CO₂
H₂O
CH₄
NH₄
H₂O₂

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15
Q

Give examples of giant covalent structures.

A

Diamond (each carbon bonds to 4 other carbons)

Silicon dioxide (SiO₂)

Graphite (each carbon bonds to 3 other carbons)

Graphene (1 layer of graphite)

Buckminster fullerene (C₆₀)

Carbon nanotubes

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16
Q

What are some properties of simple covalent structures?

A

Low MP/BP

Do NOT conduct electricity

Insoluble (usually)

17
Q

What is a simple covalent molecule?

A

Molecules joined by covalent bonds with weak forces between them.

18
Q

Explain why simple covalent molecules have a low melting and boiling point. [2 marks]

A

Intermolecular forces of attraction are WEAK - requires less energy to overcome the forces.

19
Q

Explain why simple covalent molecules cannot conduct electricity.

A

Contains no charged particles (ions/delocalised electrons) that can move - molecules are neutral.

20
Q

What is a giant covalent structure?

A

Lattice structure where atoms are joined by covalent bonds.

21
Q

What are some properties of giant covalent molecules?

A

High MP/BP

DO NOT conduct electricity (except graphite)

Insoluble

22
Q

Explain why giant covalent molecules have a high melting and boiling point. [2 marks]

A

Contain MANY strong covalent bonds - requires more energy to overcome.

23
Q

Explain why giant covalent molecules cannot conduct electricity, and why graphite CAN conduct electricity.

A

Contains no charged particles (ions/delocalised electrons) that can move - molecules are neutral.

Graphite contains DELOCALISED ELECTRONS that move between the layers and carry charge through the substance, conducting electricity.

24
Q

What is a dative covalent bond?

A

Where one atom contributes BOTH electrons to the shared pair.

25
Q

How is a dative covalent bond represented using dots and crosses?

A

2 crosses

OR

2 dots

instead of 1.

26
Q

How is a dative covalent bond represented using a bonds as sticks diagram?

A

Instead of a line being shown between 2 atoms, it will be an arrow.

E.G.
Instead of B-N, it is B ←N

27
Q

What does forming a dative bond require?

A

A dative bond DONOR

and…

A dative bond ACCEPTOR

28
Q

What is a dative bond donor?

A

An atom that has a LONE PAIR of electrons.
An atom that CONTRIBUTES 2 electrons to the shared pair.

The pair of electrons on the side that aren’t joined with any other atom.

29
Q

What is a dative bond acceptor?

A

A substance that NEEDS a PAIR of electrons to form a full outer shell.

This is when an atom still doesn’t have a full outer shell despite bonding with other atoms.

30
Q

What are examples of macromolecules / giant covalent structures?

A

Diamond

Silicon dioxide

Graphite

31
Q

What are examples of simple molecular lattices?

A

Buckminster fullerene (C60)

Ice (H2O)

Iodine (I2)

32
Q

What are the properties of macromolecular covalent bonds?

A

High MP/BP =
Requires lots of energy to overcome MANY STRONG covalent bonds.

Do NOT conduct electricity (except graphite) =
No delocalised electrons or ions.

33
Q

Draw and describe the structure of diamond.

A

Each carbon atom is bonded to 4 other carbon atoms.

= Hard =
To break up diamond, you need to break the strong C-C bonds.

= Cannot conduct electricity =
no delocalised electrons as they’re all in covalent bonds.

= High melting point =

34
Q

Draw and describe the structure and function of graphite.

A

Each carbon atom is bonded to 3 other carbon atoms.
Arranged in layers.

= Soft =
WEAK van de Waals forces of attraction between layers mean they can slide over each other. Can be easily broken.

= Conducts electricity =
Each carbon has a spare electron in a 2p orbital so…
it contains delocalised electrons - can carry charge.

= High melting point =

35
Q

What are macromolecules?

A

A massive covalently-bonded MOLECULE which contains THOUSANDS of atoms.

36
Q

What is a lattice made up of macromolecules, and a lattice made up of smaller molecules known as?

A

Macromolecular lattice

Molecular lattice

37
Q

How many carbon atoms does one carbon atom bond to in diamond and graphite? What are they held by?

A

Diamond –> 4 other carbon atoms - held by covalent bonds

Graphite –> 3 other carbon atoms - held by intermolecular forces (van der waals) between graphene sheets.

38
Q

What are allotropes?

A

Structures where the atoms of the SAME element bond in DIFFERENT ways.

39
Q

Compare the properties of diamond and graphite.

A

= Diamond =
Cannot conduct electricity
Hard
High melting point

= Graphite =
Can conduct electricity
Soft
High melting point

C = Structure and Bonding = (6 decks)

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