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Chemistry > Elements of Life > Flashcards

Elements of Life Flashcards

1
Q

Define Atomic number

A

The Atomic number of an atom is the number of protons within an atom, and in a non charged atom the number of electrons.

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2
Q

Define Mass number

A

The Mass number of an atom in the combined number of protons and neutrons in the nucleus of an atom.

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3
Q

What is an isotope?

A

An isotope an atom with the same number of protons and electrons but a different number of neutrons, no change in any properties.

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4
Q

What is Avogadro constant?

A

Avogadro Constant is 6.02 x 10^23

It represent to number of atoms in one mole of a substance.

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5
Q

Define relative isotopic mass.

A

The relative mass of an isotope of an element.

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6
Q

Define relative atomic mass.

A

The average mass of an element (and its isotopes) taking into account abundance. This is on a scale where an atom of Carbon-12 is 12.

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7
Q

How do you calculate relative atomic mass?

A

relative isotopic mass x abundance
—————————————————
100

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8
Q

What are the 7 diatomic elements?

A

Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, Bromine.

Use acronym:
Have No Fear Of Ice Cold Beer

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9
Q

What are the mole equations?

A 
Moles = Mass / Mr (solids)
Moles = Concentration x Volume (liquids)
Moles = Volume (dm^3) x 24 (gases)
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10
Q

What is empirical formula?

A

Is the simplest whole number ratio of atoms of each element present in a compound.

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11
Q

What is molecular formula?

A

The true number of each atom of each elements in a molecule.

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12
Q

What is water of crystallisation?

A

When molecules have a crystalline structure allowing them to hold water within them.
Anhydrous - no water within the structure.
Hydrated - water within the structure.

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13
Q

How do you calculate percentage yield?

A

Percentage Yield = (Actual Yield/Theoretical Yield) x 100

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14
Q

What is and how do you calculate percentage composition?

A

Percentage composition is the percentage of how much an element makes up a molecule.
Percentage Composition = (Mr of Element/Mr of compound) x 100

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15
Q

What are the 4 state symbols?

A

s - solid
l - liquid
g - gas
aq - aqueous (dissolved in water)

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16
Q

Write an ionic equation for:

HCl (aq) + NaOH(aq) –> NaCl (aq) + H20(l)

A

Write out the Ions present:
H+ + Cl- + Na+ + OH- –> Na+ + Cl- + H20
Sodium and Chlorine are unchanged so must be SPECTATOR ions.
H+ + OH- –> H20
This is the ionic equation for this reaction.

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17
Q

What is a titration?

A

A titration is a practical method where a standard solution with a known concentration is reacted with a substance with an unknown concentration in order to determine the unknown concentration.

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18
Q

How is an acid-base titration carried out?

A

1) A solution of the unknown compound is made in a volumetric flask diluted by a known factor.
2) The standard solution is poured into the burette.
3) A pipette is used to measure 25 cm^3 of unknown solution and pour into a conical flask.
4) Add universal indicator or methyl orange to the conical flask.
5) Titrate until the indicator has faintly but definitely change colour.
6) Record titre.
7) Repeat this until you get 2 or 3 concordant results.

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19
Q

What is the maximum number of electrons allows in the first for shells/energy levels?

A

n=1: 2 electrons
n=2: 8 electrons
n=3: 18 electrons
n=4: 32 electrons

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20
Q

What are the 4 sub shells and how many electrons can they hold?

A

s - 2 electrons
p - 6 electrons
d - 10 electrons
f - 14 electrons

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21
Q

What are orbitals and their corresponding shapes?

A 
Orbitals are what make up sub shells, they are composed of 2 electrons spinning in opposite directions.
Sub shells:
S: has 1 orbital
P: has 3 orbitals
D: has 5 orbitals
F: has 7 orbitals
There shape of orbitals:
S- Spherical
P- Dumb-bell/ figure eight (found on the x, y and z axis)
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22
Q

What are the orbital blocks and what do they represent?

A

The orbital blocks are blocks on the periodic table, representing elements with their outermost shell in the same sub shell.
The S block is groups 1,2.
The P block is groups 3,4,5,6,7,8.
The D block are the transition metals.
The F block are the lanthanides and actinides.

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23
Q

How do you express and element in its electronic configuration?

A

The energy of orbitals increases from s to d meaning electrons are filled in this order.
An example: Sodium
1s2 2s2 2p6 3s1

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24
Q

What are some exception with electronic configuration?

A

The energy level for the 3d sub shell and the 4s sub shell overlap, this means that the 4s orbital fills up before the 3d orbitals.
This is further complicated for chromium and copper.
A sub shell is more stable if it is half filled or completely filled, rather than being inbetween,
This means:
Chromium: 1s2 2s2 2p6 3s2 3p6 3d5 4s1
Half fills both 3d 4s.
Copper: 1s2 2s2 2p6 3s2 3p6 3d10 4s1
Completely fills 3d and half fills 4s.

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25
Q

What is a nuclear fusion reaction?

A

In a fusion reaction two light nuclei collide and form a larger nuclei.
It requires extreme temperature and pressure.
However, it releases large amounts of energy.
The energy release is due to the change in mass from the reacting nuclei and the product nuclei.

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26
Q

What is ionic bonding?

A
  • Electrostatic attraction between positive and negative ions.
  • Occurs between a metal and a non metal.
  • Only conduct electricity when molten or aqueous, as the ions need to be able to move.
  • Form giant ionic lattices as the oppositely charge ions attract through electrostatic forces.
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27
Q

What is a cation?

A

Positively charged ion, attracted to negatively cathode.

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28
Q

What is an anion?

A

Negatively charged ions, attracted to the positive anode.

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29
Q

What is covalent bonding?

A
  • Strong electrostatic attraction between a shared paired of electrons and the nuclei of bonded atoms.
  • Form between 2 two not metals.
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30
Q

What are dative covalent bonds?

A

When a covalent bond is form by 1 of the 2 elements supply both of the required electrons.
This is shown by using an arrow instead of a dash to represent the bond.

N - H Covalent
N -> H Dative

Dative Covalent bonds react the same as normal covalent bonds.

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31
Q

What is a simple covalent molecules?

A

A molecule comprised of only a covalent structure, and held together by intermolecular forces.

32
Q

What is a lone pair and what does it do?

A

Lone pairs are just a pair of unbonded electrons on the outermost shell of electrons on an atom.
They reduce the bond angle of an atom by 2.5°, they have repulsive forces.

33
Q

What are all the shapes of molecules?

A

Linear: 2 Bonding pairs, no lone pairs, 180° bond angle.
V - shaped: 2 Bonding pairs, 2 lone pairs, 104.5° bond angle.
Trigonal Planar: 3 Bonding pairs, no lone pairs, 120° bond angle.
Triangular Pyramid: 3 Bonding pairs, 1 lone pair, 107° bond angle.
Tetrahedral: 4 bonding pairs, no lone pairs, 109.5° bond angle.
Trigonal Bipyramidal: 5 bonding pairs, no lone pairs, 180° and 90° bond angle.
Octahedral: 6 bonding pairs, no lone pairs, 90° bond angle.

34
Q

What is a linear bond shape?

A

2 Bonding pairs
No lone pairs
180° bond angle

35
Q

What is V-Shaped bond shape?

A

2 Bonding pairs
2 lone pairs
104.5° bond angle

36
Q

What is Trigonal Planar bond shape?

A

3 Bonding pairs
No lone pairs
120° bond angle

37
Q

What is Triangular Pyramid bond shape?

A

3 Bonding pairs
1 lone pair
107° bond angle

38
Q

What is tetrahedral bond shape?

A

4 bonding pairs
No lone pairs
109.5° bond angle

39
Q

What is Trigonal Bipyramidal bond shape?

A

5 bonding pairs
No lone pairs
180° and 90° bond angle

40
Q

What is Octahedral bond shape?

A

6 bonding pairs
No lone pairs
90° bond angle

41
Q

How do you draw a 3D molecule in 2D?

A

Wedges - Show bonds coming put of the page.

Dash - Show bonds going into the page.

42
Q

What are Macromolecular covalent substances?

A
  • Covalently bonded giant lattices.
  • Each atom has multiple covalent bonds.
  • Very strong and very high melting points.

Examples: Diamond and graphite.

43
Q

Describe the structure of diamond.

A
  • Macromolecular
  • Carbon atoms are boned to 4 other carbon atoms.
  • Rigid tetrahedral structure.
44
Q

Describe the structure of Graphite.

A
  • Macromolecular.
  • Each carbon is bonded to 3 other carbon atoms.
  • Forms flat hexagonal layers.
  • 1 delocalised electron per carbon atom.
  • Weak intermolecular forces.
  • Layer can slide over each other.
45
Q

What is metallic bonding?

A
  • Giant lattice of positively charged ion surrounded by a sea of delocalised electrons.
  • Very strong electrostatic forces of attraction between positive ion and sea of electrons.
46
Q

What makes metallic bonding stronger/weaker?

A
  • If there is a greater charge on the positive ions, there is a stronger force of attraction since more electrons are released.
  • If large ions are there we be a weaker force of attraction, as the atomic radius will be greater and there will be higher shielding effect.
47
Q

What are some physical properties of metallic bonding?

A
  • Good conductors due to the sea of delocalised electrons.
  • Malleable because the uniform layers of positive ions are able to slide over eachother.
  • High melting and boiling points due to the strong electrostatic forces of attraction.
48
Q

What is Periodicity?

A

The study of trends on the period table.

49
Q

Describe the variation of Melting Points across Period 2.

A
  • The melting points are vary due to the varying structures.
  • The boiling points increase from lithium to carbon, then drop massively for nitrogen to neon.
  • Lithium and beryllium have metallic bonding, beryllium has a higher charged ion so will have more delocalised electrons, therefore a higher boiling point.
  • Boron and Carbon form giant covalent lattices with strong covalent bonds.
  • Nitrogen, oxygen, fluorine and neon are all small simple covalent molecules, with weak intermolecular forces.
50
Q

What is the formula and charge of a nitrate ion?

A

NO3

Charge: -1

51
Q

What is the formula and charge of a sulfate ion?

A

SO4

Charge: -2

52
Q

What is the formula and charge of a carbonate ion?

A

CO3

Charge: -2

53
Q

What is the formula and charge of a hydroxide ion?

A

OH

Charge: -1

54
Q

What is the formula and charge of an ammonium ion?

A

NH4

Charge: +1

55
Q

What is the formula and charge of a bicarbonate ion?

A

HCO3

Charge: -1

56
Q

What is the formula and charge of a Copper ion?

A

Cu

Charge: +2

57
Q

What is the formula and charge of a zinc ion?

A

Zinc

Charge: +2

58
Q

What is the formula and charge of a Lead ion?

A

Pb

Charge: +2

59
Q

What is the formula and charge of a iron ion?

A

Fe

Charge: +2 or +3

60
Q

What happens when you react a group 2 metal with water?

A
  • Redox reaction.
  • Produces a metal hydroxide and hydrogen.
  • Product is an alkaline solution.
  • X + 2H20 –> X(OH)2 + H2
  • Reactivity increases down group 2.
61
Q

What happens when group 2 metals react with oxygen?

A
  • Forms metal oxide.
  • It is a vigorous reaction.
  • 2X + O2 –> 2XO
  • If there is a excess of oxygen the metal oxide can further react to form metal peroxide.
62
Q

What is the trend of Thermal Decomposition of Group 2 Carbonate?

A
  • Thermal stability is the ability of a substance to resist breaking down under heat.
  • Thermal Decomposition produces a metal oxide and carbon dioxide.
  • XCO3 –> XO + CO2
  • Thermal stability increases down group 2 carbonates.
  • The smaller molecules in group 2 have a higher charge density, which weakens the C-O bond.
63
Q

What is the trend in Solubility of Group 2 Carbonates?

A
  • Group 2 carbonates aren’t very soluble.

- However, solubility decreases down the group.

64
Q

What is the trend in Solubility of Group 2 Hydroxides?

A
  • Solubility increases down the group.
65
Q

Define First Ionisation Energy.

A

The minimum energy required to remove one mole of electrons from one mole of atoms in a gaseous state.

66
Q

What are Successive Ionisation energies?

A
  • Involve removing one mole of electrons from one mole of gaseous ions.
  • This is when more than 1 electrons are removed from an atom.
  • To remove another electron the energy required increases.
  • This is because when an electron is removed, the nuclear pull on the remaining electrons increases.
  • There can be an large jump in ionisation energy, when the outermost electron drops to a lower energy level/sub-shell.
67
Q

What are the trends of first ionisation energy across a period and down a group?

A

Down a group - First ionisation energy decreases as the there is an increasing atomic radius and electron shielding.

Along a period - First ionisation energy increases due to a decreasing atomic radius and an increasing nuclear charge. The trend can be screwed when the outermost electron jumps into a new sub shell.

68
Q

What is an Acid-Base equilibria?

A
  • They are a transfer of protons between substances.

- The involve a Brønsted-Lowry acid and a Brønsted-Lowry base.

69
Q

What is a Brønsted-Lowry acid?

A

Is a proton donor.

70
Q

What is a Brønsted-Lowry base?

A

A proton acceptor.

71
Q

What does amphoteric mean?

A

Reacts with acids and bases.

72
Q

What is the trend in pH of group 2 Oxides and Hydroxides?

A

The pH of group 2 oxides and hydroxides become more basic down a group.

73
Q

How do group 2 Hydroxides react with Dilute Acids?

A
  • Group 2 hydroxides react with dilute acids to form a salt and water.
  • This is a neutralisation reaction.
  • Hydrochloric acids form chloride salts.
  • Sulfuric acid forms sulfates salts.
  • Nitric acid forms bitrate salts.
  • Example:
    Ca(OH)2 + 2HCl –> CaCl2 + 2H2O
74
Q

What equation gives the energy of light?

A

E = hv
E- energy of light (J)
h- Planck Constant (Js)
v- frequency (Hz)

75
Q

What the the equation for the speed of light?

A

c = λv
c- speed of light (m/s)
λ- wavelength (m)
v- frequency (Hz)

76
Q

What the the EM spectrum in increasing frequencies?

A 
Royal Marines Invade Vietnam Using X-ray Guns
Radio
Micro
Infrared
Visible
Ultraviolet
X-ray
Gamma
77
Q

What is emission spectra?

A

Coloured Lines on a black background

Chemistry (7 decks)

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