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Bonding Flashcards

1
Q

What is the definition of Ionic bonding?

A

An electrostatic force of attraction between oppositely charged ions

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2
Q

What two factors affect the strength of an ionic bond

A

-ionic radius
-size of charge

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3
Q

As ionic radius increases…

A

Ions become less charge dense so there are weaker ESFA between cations and Cl- ions

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4
Q

Smaller more …… charged ions are more ………, so attract oppositely charged ions more ……….

A

-highly
-charge dense
-strongly

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5
Q

What is the perfect ionic model?

A

-ions are perfectly spherical
- no electron density between them

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6
Q

Ionic radius decreases across the period because…

A

Shielding stays the same but ionic charge increases

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7
Q

What is covalent bonding?

A
  • the electrostatic force of attraction between a shared pair of electrons and two positive nuclei
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8
Q

What do we use to measure the strength of a covalent bond?

A

Bond enthalpy (kJ mol)

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9
Q

The longer the covalent bond…

A

The weaker the bond

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10
Q

Why do covalent bonds get weaker when atomic radius increases?

A

-As atomic radius increases covalent bonds get longer
-Atoms cannot approach as closely so there is a weaker ESFA between the two nuclei and the shared electrons

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11
Q

Multiple covalent bonds are…

A

Shorter and stronger than single bonds.
(Stronger ESFA between 2 nuclei and multiple pairs of electrons)

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12
Q

What is octet expansion?

A

-elements in period 3 and beyond can accommodate up to 18 electrons in their outer shell

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13
Q

What is a dative covalent bond?

A

-one atom supplies both electrons required to form a covalent bond.

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14
Q

What are the two requirements for the formation of a dative covalent bond?

A

-one atom must have a vacant orbital
-another atom must have a lone pair of electrons

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15
Q

A dimer is when…

A

Two of the same molecule join together to form a larger molecule via dative covalent bonding

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16
Q

What is metallic bonding?

A

An electrostatic force of attraction between a positive metal cation and delocalised electrons

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17
Q

What are the factors that affect the strength of a metallic bond?

A

-size of charge
-ionic radius
(Charge denisty)
-# of electrons in the sea

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18
Q

Ionically bonded molecules have a ………. Structure

A

Giant Ionic Lattice

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19
Q

Why do ionic compounds have high melting/boiling points?

A

-strong ESFA between oppositely charged ions that require a lot of energy to overcome

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20
Q

Ionic compounds can only conduct when……………..

A

-molten or dissolved in a solvent
- this is because ions can move and carry charge allowing current to flow

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21
Q

Why can’t ionic compounds conduct when solid?

A

-ions are held in place

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22
Q

Simple molecular structure has ___________ bonding

A

Covalent

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23
Q

Describe simple molecular structure

A

-strong covalent bonds between atoms
-weak intermolecular forces of attraction between molecules

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24
Q

Why is the melting/boiling point of simple molecular structures low?

A

-weak forces of attraction between molecules that are easy to overcome with little energy

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25
Do simple molecular compounds conduct electricity?
No
26
Name three types of compounds with giant covalent lattice structure
-Diamond -Graphite -Silicon dioxide
27
Diamond Each carbon atom is bonded to __ others. Atoms are held in ________ positions by ________________ bonds
-4 -fixed -strong covalent
28
Describe graphites structure
-each carbon atom is bonded to three others -atoms are arranged in layers -strong covalent bonds between atoms -weak forces of attraction between layers means they can slide over each other -delocalised electrons
29
Why do compounds with giant covalent lattice have high boiling/melting points?
Lots of strong covalent bonds between atoms that require lots of energy to break.
30
Why can’t diamond conduct electricity but graphite can?
-Diamond does not have delocalised electrons while graphite does
31
Some simple molecular _______ are soluble in water
-gases (Ammonia)
32
Giant metallic lattice has a regular…
-Close packed arrangement of positive metal ions surrounded by a sea of delocalised electrons. -layers of ions can slide over each other - delocalised electrons can move throughout the structure carrying charge
33
Why do metals have high boiling points
-strong ESFA between positive metal ions and delocalised electrons that requires a lot of energy to overcome
34
What are the shapes of molecules determined by?
-bonding and lone pairs of electrons
35
What is valence shell electron pair repulsion theory?
-bonding pairs repel other bonding pairs equally and as much as possible -lone pairs repel other lone pairs equally and as much as possible -lone pairs repel more than bonding pairs
36
What is the shape for 2 bonding pairs?
Linear
37
What is the shape for 3 bonding pairs?
Trigonal planar (120)
38
What is the shape for 2 bonding pairs and one lone pair?
Bent (117.5)
39
What is the shape for 4 bonding pairs?
Tetrahedral (109.5)
40
What is the shape for 3 bonding pairs and one lone pair?
Trigonal pyramidal (107)
41
What is the shape for 2bonding pairs and 2 lone pairs?
Bent (105.5)
42
What is the shape for 5 bonding pairs?
Trigonal bipyramidal (90 + 120)
43
What is the shape for 4 bonding pairs and one lone pair?
Sawhorse (87.5)
44
What is the shape for 3 bonding pairs and two lone pairs
T shaped (85 + 180)
45
What is the shape for two bonding pairs and three lone pairs?
Linear (180)
46
What is the shape for 6 bonding pairs?
Octahedral (90)
47
What is the shape for 5 bonding pairs and one lone pair?
-Square pyramidal (87.5 _ 90)
48
What is the shape for 4 bonding pairs and 2 lone pairs
Square planar (90)
49
What is the shape for 3 lone pairs and 3 bonding pairs?
T shaped (87.5)
50
What is the shape for 4 lone pairs and two bonding pairs
Linear
51
Name the 4 stages a bond goes through from ionic -> covalent
Ionic Distorted ions Polarized Covalent bond (has ionic character) Covalent bond
52
What is electronegativity?
The ability of an atom to withdraw electron density towards itself in a covalent bond
53
What are the two factors affecting electronegativity?
-Nuclear charge -Atomic radius (Small atoms with high nuclear charge are electronegative))
54
How does electronegativity change down a group?
-decreases -down the period atomic radius increases therefore extra energy levels, more shielding, weaker ESFA between nuclear and bond, e negativity decreases
55
What is the most electronegative element?
Fluorine
56
What are the requirements of the perfect ionic model?
Perfect spherical point charges -no electron density found between them -held together by ESFA
57
What are the two deviations from the perfect ionic model?
-A polarising cation (small highly charged ions such as Li+ and Al3+) -A polarisable anion (large diffuse ions (spread out) ) (Br- + I-)
58
Describe one example of how the perfect ionic model falls apart
-SIlver polarises the Iodide ion -distorting the electron cloud
59
What are the three types of intermolecular forces within simple molecular structures?
-Van der Waals forces of attraction -Dipole-dipole interactions -Hydrogen bonds
60
Intermolecular forces are found between simple molecules and they determine ……………. And ……………. Points.
-melting -boiling
61
When we melt/boil simple molecules we do not …..
-break covalent bonds -we overcome intermolecular forces
62
Van der Waals forces of attraction are caused by….
The movement of electrons within a molecule
63
What is the weakest intermolecular force?
-Van de Waals
64
How are Van der Waals forces formed?
-Electron movement in first molecule induces a dipole in another, resulting in a temporary attraction between d+ on one molecule and d- on another.
65
Strength of van der Waals forces are determined by..
-Size of the molecules (bigger mol. -> more electrons -> stronger VDW) -Shape of molecules (straight chain can pack closer together than branched)
66
Why does boiling point increase down the group of Group 0 gases?
-More energy level therefore more electrons each time so stronger vdw forces of attraction BETWEEN ATOMS that need more energy to overcome
67
The occurrence of dipole-dipole interactions depends on:
-presence of electronegative atoms resulting in polar bonds ( O, F, Cl , N, Br) -shape of the molecule (distribution of charge must be asymmetric)
68
If an atom is bigger…
Van de Waals will be stronger
69
What is the strongest type of intermolecular force?
Hydrogen bonding
70
For hydrogen bonding to occur between molecules..
-A hydrogen atom must be directly bonded to electronegative elements. -The electronegative element must have a lone pair of electrons. -The more electronegative the element the stronger the hydrogen bond.
71
Why does the strength of the hydrogen bond increase with electronegativity
-the greater the difference in electronegativity the greater the partial charges. -therefore, stronger attraction between s+ on one molecule and s- on another.
72
What are partial charges?
-difference in electronegativity causing an uneven share of electrons.
73
Boiling point increases as number of hydrogen bonds in a molecules…
Increases

Chemistry (18 decks)

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