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CH106: Chemistry Principles and Practice 1 > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

1
Q

What are the four fundamental forces ?

A
  • Strong Nuclear force
  • Weak Nuclear force
  • Electromagnetic force
  • Gravity
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2
Q

What force(s) bind Protons and Neutrons and only goes the distance of an atom ?

A
  • Strong nuclear force
  • Weak nuclear force
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3
Q

What force(s) is responsible for the attraction between positive and negative charge ?

A

Electromagnetic force

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4
Q

What distance can Electromagnetic force travel ?

A

Its infinite

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5
Q

What force(s) cause the attraction of matter to other matter ?

A

Gravity

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6
Q

What elements were formed through the big band and what is the proportion of these elements ?

A

Hydrogen (89%)
Helium (11%)

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7
Q

2 hours After the big band, the universe cooled, what happened next ?

A

The Strong nuclear force bound protons and neutrons into atomic nuclei and the electromagnetic force pulled the nuclei and electrons together to from atoms.

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8
Q

What happened during Stellar Nucleosynthesis ? and what elements did this create

A

Gravity brough H and He close together and they compressed which meant the density and heat rose and gave stars. Lighter atoms fused by nuclear fusion- this process also releases energy.
Created elements until Fe

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9
Q

What happened during Supernova Nucleosynthesis ? and what elements did this create

A

Old stars became very dense and heavier elements such as Oxygen and silicon fused to give very heavy elements. They formed and very ejected by explosion along any previously formed lighter elements.
Elements from Ni to U

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10
Q

What are the ways elements were created ?

A
  • The big bang
  • Steller nucleosynthesis
  • Supernova nucleosynthesis
  • Radioactive decay
  • Human interference
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11
Q

What is a group ?

A

Elements going down the periodic table

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12
Q

What is a period ?

A

Elements going across a periodic table

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13
Q

What is the ‘Periodic Law’ ?

A

The properties of elements are periodic functions of their atomic number

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14
Q

Why do elements in the same group have similar chemical properties ?

A

They have the same number of valence shell electron configuration

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15
Q

Valence shell definition

A

Outer shell

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16
Q

What is the max. number of electrons in an atomic orbital ?

A

2

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17
Q

What are the four different types of atomic orbital ?

A

s, p, d, f

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18
Q

Degenerate

A

equal energy

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19
Q

What gives the periodic table its structure ?

A

order of atomic orbitals

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20
Q

What are the three groups of elements?

A

metals, non-metals and semi-metals

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21
Q

what elements are semi- metals ? (use the periodic table to help)

A

B, Si, Ge, As, Sb, Te, At

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22
Q

What is ‘Effective Nuclear Charge’ ?

A

The positive charge than an electron experiences from the nucleus.

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23
Q

What is the trend for effective nuclear charge going across a period ?

A

ENC increases as nuclear charge increases

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24
Q

What is the trend for effective nuclear charge going down a group ?

A

ENC decreases as shielding increases- through more occupied energy levels

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25
What is 'Atomic Radius' ?
Half the distance between the nuclei in an element
26
Why is measuring atomic radii trivial ?
They don't end abruptly as electrons 'fall away'
27
What is the trend for atomic radius going down a group?
Atomic Radius increases as a new shell of electrons is added
28
What is the trend for atomic radius going across a period ?
The Atomic radius decreases as the ENC increases hence there's more attraction to nucleus, pulling electrons closer to the nucleus.
29
What is ionisation energy ?
Minimum energy required to remove the outermost (highest energy) electrons from a neutral atom in the gaseous state.
30
Is an Ionisation reaction exothermic or endothermic ?
Endothermic
31
What is the trend for ionisation going across a period ?
The ionisation energy increases as the atom size decreases, valence electrons are closer to nucleus hence more energy is required to remove it
32
What is the trend for ionisation energy going down a group ?
Ionisation energy decreases as The electrons are further from the nucleus so are not tightly bound to the nucleus
33
Why does Boron have a smaller ionisation energy than Beryllium, even though the trend shows it should have a larger one ?
It is easier to remove Boron's 2p1 electron than one of Berylliums 2s2 electrons because this leave the subshell unstable.
34
What is electron affinity ?
Energy change of the process of adding electrons to neutral atoms in gaseous state to form negative ions.
35
What is electronegativity ?
A relative measure of the ability of an atom in a molecule to attract bonding electrons to itself.
36
What groups have the highest electronegativity ? (metals, non-metals or semimetals)
Non-metals
37
What is the trend for electronegativity going across a period ?
Electronegativity increases as the Effective nuclear charge increases
38
What is the trend for electronegativity going down a group ?
Electronegativity decreases as atom gets bigger hence valence/bonding electrons are further from attraction of nuclei
39
What type of bond has a low electronegativity ?
Covalent bonds
40
What type of bond has an intermediate electronegativity ?
Polar covalent bonds
41
What is an 'ionic bond'?
Chemical bonds formed by electrochemical attraction between positive and negative
42
Cations are...
positive (ions that have lost electrons)
43
Anions are...
negative (ions that have gained electrons)
44
What metal element can also form covalent bonds and why ?
Beryllium as it is the most electronegative metal.
45
What is 'Oxidation state' ?
Formal charge on an atom in a substance when the bonding electrons are assigned to the most electronegative atom in the bond.
46
What are the five oxidation state rules ?
1. Group 1 is always +1 2. Group 2 is always ++2 3. Oxygen is always -2 unless there's Fluorine 4. Fluorine is always -1 5. If there's no lighter Halide or Oxygen then Halide is -1
47
How can you check the oxidation states ?
The total of oxidation states adds up to 0 or the charge on the group ions
48
What makes a stable oxidation state ?
- Full electron shell - Half filled electron shell - Empty electron shell
49
Why is Chlorine (+7) highly reactive ?
It can't be oxidised further as it has no more electrons to give and wants to gain electrons (be reduced) as its a very strong oxidising agent.
50
How real is the oxidation states ?
Only true for Ionic bonds as its electrons are fully taken/shared but it does give accurate precisions of behaviour
51
What is the difference between Sulphurous acid and Sulfuric acid ?
Sulphurous acid is less acidic and has a less positive state than Sulfuric acid
52
Describe the three different Oxygen Anions
O2- / oxidation state of -2/ oxide O22-/ oxidation state of -1/ peroxide O21-/ oxidation state of -1/2/ superoxide
53
What is more reactive ? oxide ? peroxide ? superoxide ?
Peroxide and superoxide
54
What does VSEPR stand for ?
Valence Shell Electron Pair Repulsion
55
What are Bonding Pairs ?
Two electrons in a covalent bond
56
What are Lone Pairs ?
Two valence electrons centred on one atom, also known as non-bonding pair of electrons.
57
VSEPR applies to covalent compounds of main group elements. This is based on two separate ideas:
1. Minimise repulsion, electron pairs take up positions as wide apart from each other as possible 2. Molecular shape about a central atom will depend on valence electron pairs and bonded pairs and lone pairs
58
What are the 5 core shapes ?
2 pairs - Linear 3 pairs - Trigonal Planar 4 pairs - Tetrahedral 5 pairs - Trigonal Bipyramidal 6 pairs - Octahedral
59
What are the angles in each of the 5 core shapes ?
Linear - 180' Trigonal Planar - 120' Tetrahedral - 109.5' Trigonal Bipyramidal - 90', 120', 180' Octahedral - 90', 180'
60
What are the derived shapes ?
2 coordinate - Angular 3 coordinate - Trigonal Bipyramidal 3 coordinate - T - shaped 4 coordinate - Square planar 4 coordinate - Disphenoidal (see saw) 5 coordinate - Square Pyramidal
61
What are the size considerations for shapes ?
Lone pairs take up more room at the central atom compared to bonding pairs of electrons.
62
What is the most abundant element ?
Hydrogen (~89%)
63
What are the different ways for Hydrogen to react ?
1. Gain an electron to form H- (Ionic hydride) 2. Lose an electron to form H+ (acids) 3. Form normal covalent bonds by sharing electrons (covalent hydrides).
64
What is 'Amphoteric' ?
Acts as both an acid and base
65
What is an Acid, according to Bronsted Lowry ?
Species which donates a proton
66
What is a Base, according to Bronsted Lowry ?
Species which accepts a proton
67
What is a Lewis Acid ?
Accept an electron
68
What is a Lewis Base ?
Donates an electron
69
What are donor-acceptor bonds involving lone pairs called ?
Dative or Coordinate
70
What is Hydrogen Bonding ?
This can be either INTERmolecular or INTRAmolecular bonding
71
What is the donor group ?
Hydrogen bonded to an electronegative atom
72
What is the Acceptor atom ?
An atom with a negative charge
73
When is Hydrogen bonding strongest ?
When there is a large charge difference between Hydrogen and the Acceptor. The more electronegative Donor group is- the stronger the Hydrogen bonding.
74
What does the 'sea of electrons' describe ?
Metallic bonding model is NOT ionic or covalent. Metals share their valence electrons over ALL atoms.
75
What are the Alkali Metal reaction types ?
1. Reducing agents 2. Salts are strong bases 3. MR used in organic reactions
76
What group 2 element doesn't react similarly to the other elements in this group and why ?
Be as they are the Anomalous member of the group. They are not so reactive and are more selective
77
What molecule containing Be is Amphoteric ?
BeO (Beryllium Oxide)
78
What are the rules of thumb for the periodic table ?
1. Top elements in any group trends to be most difference. 2. Diagonal relationship - acts like pairs
79
What is different about Boron ?
Boron is electron deficient
80
Name some elements which are Allotropic
Carbon, Sulfur and Phosphorous
81
What is the definition of Allotropic ?
One of two or more distinct forms of an element in the same physical state
82
How does Carbon exist ?
Molecule, diamond, graphite layer, Buckministerfullerene

CH106: Chemistry Principles and Practice 1 (5 decks)

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