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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

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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)
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3
Q

1.2a- Bonding in Elements

Covalent molecular solids?

A
  • Phosphorus (P)
  • Sulfur (S)
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4
Q

1.2a- Bonding in Elements

Define: “Covalent Network”

A

Structure consists of a giant lattice of covalently bonded atoms

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5
Q

1.2a- Bonding in Elements

What elements form Covalent Networks?

A
  • Boron (B)
  • Carbon (C)
  • Silicon (Si)
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6
Q

1.2a- Bonding in Elements

Define: “Metallic Bonding”

A

Structure consists of
* Positively charged ions
* Delocalized outer electrons

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7
Q

1.2a- Bonding in Elements

What elements form Metallic bonds?

A

Any metal

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8
Q

1.2a- Bonding in Elements

Define: “Monatomic”

A

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

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9
Q

1.2a- Bonding in Elements

Define: “Discrete”

Chemistry-wise

A

Separate

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10
Q

1.2a- Bonding in elements

What forms of Carbon are Covalent Networks?

A
  • Diamond
  • Graphite
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11
Q

1.2a- Bonding in Elements

What form of Carbon is a covalent molecular?

A

Fulerene
(C60)

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12
Q

1.2a- Bonding in elements

How do the following exist?
* Phosphorus
* Sulfur

A
  • P4
  • S8
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13
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

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14
Q

1.2b- Intramolecular bonding

Define: “Covalent bonding”

A

Formed when atoms of elements share electrons

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15
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

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16
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
17
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
18
Q

1.2b- Intramolecular bonding

What do the following mean?
* δ+
* δ-

A
  • δ+ = slightly positive
  • δ- = slightly negative
19
Q

1.2c- Intermolecular bonding

What are the different van der Waals’ forces?

A
  • London Dispersion Forces (LDFs)
  • Dipole-Dipole interactions
  • Hydrogen bonding
20
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
21
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
22
Q

1.2c- Intermolecular bonding

Define in the context of polarity:
* Symmetrical
* Asymmetrical

A
  • Polar
  • Non-polar
23
Q

1.2c- Intermolecular bonding

Define: “Dipole-Dipole interactions”

A

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

24
Q

1.2c- Intermolecular bonding

What bonds cause Hydrogen bonding?

A
  • H-F
  • H-N
  • H-O
25
# 1.2d- Properties Why do Metallic, Ionic, & Covalent Networks have high MP/BPs?
The many strong interactions that need to be overcome for the substances to change state
26
# 1.2d- Properties Why is the MP/BP of a covalent molecule < than a Covalent network?
Only weak van der Waals' forces need to be overcome
27
# 1.2d- Properties Why do larger molecules have > MP/BPs?
* More electrons to cause larger temporary dipoles & LDFs * LDF strength increases with molecular mass
28
# 1.2d- Properties Why do Polar Molecules have MP/BPs > than non-polar ones?
More energy required to overcome D-D interactions
29
# 1.2d- Properties Why do molecules containing H-F/N/O have high MP/BPs?
More energy needed to overcome strong Hydrogen Bonds
30
# 1.2d- Properties Strength of van der Waals' forces
Hydrogen > D-D > LDF (30 kJ mol) > (5-25 kJ mol) > (4 kJ mol)
31
# 1.2d- Properties Elaborate on: "Like dissolves like"
* Polar solvent: polar/ ionic solute * Non-polar solvent: non-polar solute
32
# 1.2d- Properties Define: * "Solvent" * "Solute"
* The dissolver * Thing being dissolved
33
# 1.2d- Properties Why do (-OH) groups cause increasing viscosity?
They allow Hydrogen-bonding between molecules & increase viscosity through intermolecular attraction
34
# 1.2d- Properties How does intermolecular attraction affect viscosity?
The **stronger** the **intermolecular atttraction**, the more **viscous** a liquid will be

Chemistry (14 decks)

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