Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > 1.2 Structure & Bonding > Flashcards

1.2 Structure & Bonding Flashcards

1
Q

1.2a- Bonding in elements

Define: “Covalent molecular”

A

Structure consists of
* Discrete molecules
* Held together by WEAK forces of attraction
* Some elements normally exist as solids
* Others as diatomic gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

1.2a- Bonding in elements

What gases are diatomic?

A
  • Hydrogen (H)
  • Iodine (I)
  • Nitrogen (N)
  • Chlorine (Cl)
  • Bromine (Br)
  • Oxygen (O)
  • Fluorine (F)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

1.2a- Bonding in Elements

Covalent molecular solids?

A
  • Phosphorus (P)
  • Sulfur (S)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

1.2a- Bonding in Elements

Define: “Covalent Network”

A

Structure consists of a giant lattice of covalently bonded atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

1.2a- Bonding in Elements

What elements form Covalent Networks?

A
  • Boron (B)
  • Carbon (C)
  • Silicon (Si)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

1.2a- Bonding in Elements

Define: “Metallic Bonding”

A

Structure consists of
* Positively charged ions
* Delocalized outer electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

1.2a- Bonding in Elements

What elements form Metallic bonds?

A

Any metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

1.2a- Bonding in Elements

Define: “Monatomic”

A

Structure consists of:
* Discrete atoms
* Held together by van der Waals’ forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

1.2a- Bonding in Elements

Define: “Discrete”

Chemistry-wise

A

Separate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

1.2a- Bondin in elements

What forms of Carbon are Covalent Networks?

A
  • Diamond
  • Graphite
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

1.2a- Bonding in elements

How do the following exist?
* Phosphorus
* Sulfur

A
  • P4
  • S8
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

1.2b- Intramolecular bonding

Define: “Ionic Bonding”

A

The electrostaic force of attraction between the positive ions of 1 element & the negative ions of another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

1.2b- Intramolecular bonding

Define: “Covalent bonding”

A

Formed when atoms of elements share electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

1.2b- Intramolecular bonding

Define: “Pure Covalent” or “Non-Polar” bonds

A

When the atoms involved in the bond have an equal share of the bonding electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

1.2b- Intramolecular bonding

What molecules have Pure Covalent bonds?

A
  • Non-metals elements
  • Nitrogen Bromide (NBr) as both N & Br have eletronegativity values of 3.0
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

1.2b- Intramolecular bonding

Define: “Polar covalent bond”

A
  • A bond in which the atoms have different electronegatovity values
  • This means that 1 atom has an attraction for the bonded electrons > the other
17
Q

1.2b- Intramolecular bonding

What do the following mean?
* δ+
* δ-

A
  • δ+ = slightly positive
  • δ- = slightly negative
18
Q

1.2c- Intermolecular bonding

What are the different van der Waals’ forces?

A
  • London Dispersion Forces (LDFs)
  • Dipole-Dipole interactions
  • Hydrogen bonding
19
Q

1.2c- Intermolecular bonding

What causes LDFs?

A
  • An uneven distribution of the constantly moving electrons around the nuclei of atoms
  • The larger the atoms/molecule, the stonger LDFs can arise
  • Temporary imbalance causes a “Dipole” to form & be induced in neighbouring atoms/molecules
20
Q

1.2c- Intermolecular bonding

Why are symmatrical molecules with polar bonds non-polar overall?

A
  • δ- or δ+ cancel out polarity across the molecule
  • No one side is more ± than the other
21
Q

1.2c- Intermolecular bonding

Define in the context of polarity:
* Symmetrical
* Asymmetrical

A
  • Polar
  • Non-polar
22
Q

1.2c- Intermolecular bonding

Define: “Dipole-Dipole interactions”

A

The electrostatic attraction between the oppositely charged areas of 2+ polar molecules

23
Q

1.2c- Intermolecular bonding

What bonds cause Hydrogen bonding?

A
  • H-F
  • H-N
  • H-O
24
Q

1.2d- Properties

Why do Metallic, Ionic, & Covalent Networks have high MP/BPs?

A

The many strong interactions that need to be overcome for the substances to change state

25
Q

1.2d- Properties

Why is the MP/BP of a covalent molecule < than a Covalent network?

A

Only weak van der Waals’ forces need to be overcome

26
Q

1.2d- Properties

Why do larger molecules have > MP/BPs?

A
  • More electrons to cause larger temporary dipoles & LDFs
  • LDF strength increases with molecular mass
27
Q

1.2d- Properties

Why do Polar Molecules have MP/BPs > than non-polar ones?

A

More energy required to overcome D-D interactions

28
Q

1.2d- Properties

Why do molecules containing H-F/N/O have high MP/BPs?

A

More energy needed to overcome strong Hydrogen Bonds

29
Q

1.2d- Properties

Strength of van der Waals’ forces

A

Hydrogen > D-D > LDF
(30 kJ mol) > (5-25 kJ mol) > (4 kJ mol)

30
Q

1.2d- Properties

Elaborate on:

“Like dissolves like”

A
  • Polar solvent: polar/ ionic solute
  • Non-polar solvent: non-polar solute
31
Q

1.2d- Properties

Define:
* “Solvent”
* “Solute”

A
  • The dissolver
  • Thing being dissolved
32
Q

1.2d- Properties

Why do (-OH) groups cause increasing viscosity?

A

They allow Hydrogen-bonding between molecules & increase viscosity through intermolecular attraction

33
Q

1.2d- Properties

How does intermolecular attractionaffect viscosity?

A

The stronger the intermolecular atttraction, the more viscous a liquid will be

Chemistry (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions