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Chemistry > 1.3 Bonding > Flashcards

1.3 Bonding Flashcards

1
Q

What is ionic bonding?

A
  • strong electrostatic forces of attraction between oppositely charged ions, held in a lattice
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2
Q

Give and example of an ionically bonded substance.

A

NaCl (Sodium chloride - salt)

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3
Q

How high are ionically bonded substances’ bp and mp? Why?

A
  • high
  • requires lots of energy to overcome the strong electrostatic forces of attraction between oppositely charged ions
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4
Q

Do ionic compounds conduct electricity? Why?

A
  • Yes
  • when molten/in solution as the ions are free to move and carry charge
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5
Q

What is simple molecular covalent bonding?

A
  • electrons are shared between the outer shells of two atoms to achieve full outer shells
  • weak van de waals forces of attraction between molecules
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6
Q

Can simple molecular covalent molecules conduct electricity? Why?

A
  • No, all electrons using in bonding and aren’t free to move
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7
Q

Are there any lone electrons in simple covalent bonding?

A
  • No, all involved in bonding
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8
Q

Do simple molecular substances have a high/low mpt and bpt? Why?

A
  • Low
  • weak van der waals forces of attraction between molecules that don’t require much energy to overcome
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9
Q

Describe macro-molecular covalent bonding?

A
  • lattice of many atoms held together by strong covalent bonds
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10
Q

Do substances with macromolecular covalent bonds have high/low mpt and bpts? Why?

A

-High
- as it requires a lot of energy to over many strong covalent bonds

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11
Q

Do substances with macromolecular covalent bonds conduct electricity?

A
  • Most don’t as all electrons are used in bonding
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12
Q

Draw and describe the structure of diamond…

A
  • tetrahedral structure of C atoms, with each C atom bonded to four others
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13
Q

Draw and describe the structure of graphite…

A
  • Similar to diamond, macromolecular covalent, but each C atom is bonded to 3 others (so its in layers)
  • weak van de waals forces of attraction between layers mean they can slide over each other (soft, slippery)
  • one electron from each carbon is delocalised, meaning it can conduct electricity
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14
Q

Describe and draw metallic bonding…

A
  • Lattice of positive metal ions strongly attracted to a sea of delocalised electrons
  • Layers can slide over each other (malleable)
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15
Q

Do metallic compounds have high/low bpt and mpts? Why?

A
  • High
  • due to strong forces of attraction between positive metal ions and sea of negatively charged delocalised electrons
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16
Q

Do metallic compounds conduct electricity? Why?

A
  • Yes
  • delocalised electrons can move throughout the metal to carry charge
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17
Q

How does the strength of metallic bonds change across the periodic table? Why?

A
  • Increases (higher melting and boiling points)
  • Greater charge on metal ions and more delocalised electrons per ions
  • stronger force of attraction between them
18
Q

Define electronegativity…

A
  • the ability of an atom to attract the pair of electrons (electron density) in a covalent bond
19
Q

What affect electronegativity? (3)

A
  • Nuclear charge
  • Atomic radius
  • Electron Shielding
20
Q

What is the most electronegative element?

A
  • Fluorine
  • because of it having the largest nuclear charge for its electron shielding and small atomic radius
21
Q

How do you get a non-polar bond?

A
  • both bonding elements have the same electronegativites
22
Q

When do you get a polar bond?

A
  • when the bonding atoms have different electronegativites
23
Q

What is the strongest type of intermolecular force?

A
  • Hydrogen Bonding
24
Q

What is the weakest type of intermolecular force?

A
  • Van de Waals forces
25
Q

Describe Van de Waals forces of attraction…

A
  • Temporary dipoles are created by the random movement of electrons
  • induces dipole in neighboring molecule
  • forces of attraction between them
26
Q

Are Van de Waals forces greater in smaller or larger molecules?

A
  • Larger, due to there being more electrons
27
Q

Describe permanent dipole-dipole attraction…

A
  • some molecules with polar bonds have permanent dipoles
  • forces of attraction arises between those dipoles and those of neighboring molecules
28
Q

What conditions are needed for hydrogen bonding to occur?

A
  • O-H, N-H or F-H bond and lone pair of electrons on O, F or N
  • Because O, N and F are highly electronegative, H nucleus is left exposed
  • Strong force of attraction between H nucleus and lone pair of electrons on O, N and F
29
Q

Why is ice less dense than liquid water?

A
  • in liquid water, hydrogen bonds constantly break and reform as molecules move about
  • in ice, the hydrogen bonds hold the molecules in fixed positions - this makes them slightly further apart
30
Q

What is a dative/co-ordinate covalent bond? When is it formed?

A
  • formed when an electron deficient atom/ion accepts a lone pair of electrons from an atom/ion with a lone pair of electrons
31
Q

Draw the formation of dative covalent bond in ammonia…

A
32
Q

What does the shape of molecules depend on?

A
  • number of electrons in the outer shell of the central atom
  • number of these electrons which are bonded or lone pairs
33
Q

What does the electron pair repulsion theory state?

A
  • that electron pairs will take up positions as far away from each other as possible, to minimize the repulsive forces between them
34
Q

Which experience the most repulsion:
Lone pair/lone pair
lone pair/bonded pair
bonded pair/bonded pair

A
  • LP - LP repulsion strongest
  • LP - BP repulsion middle
  • BP - BP repulsion weakest
35
Q

What is the shape, diagram and bond angle in a shape with 2BP and 0LP?

A
  • Linear
  • 180º
36
Q

What is the shape, diagram and bond angle in a shape with 3BP and 0LP?

A
  • Trigonal Planar
  • 120º
37
Q

What is the shape, diagram and bond angle in a shape with 4BP and 0LP?

A
  • Tetrahedral
  • 109.5º
38
Q

What is the shape, diagram and bond angle in a shape with 5BP and 0LP?

A
  • Trigonal Bipyramidal
  • 90º and 120º
39
Q

What is the shape, diagram and bond angle in a shape with 6BP and 0LP?

A
  • Octahedral
  • 90º
40
Q

What is the shape, diagram and bond angle in a shape with 3BP and 1LP?

A
  • Trigonal Pyramidal
  • 107º
41
Q

What is the shape, diagram and bond angle in a shape with 2BP and 2LP?

A
  • Bent
  • 104.5º
42
Q

What is the shape, diagram and bond angle in a shape with 4BP and 2LP?

A
  • Square Planar
  • 90º

Chemistry (24 decks)

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