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Chemistry💁🏻 > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

Give charge mass and location of proton neutron and electron

A

Proton charge +1 mass 1 location is nucleus
Neutron charge 0 mass 1 location is in nucleus
Electron charge-1 mass almost 0 location in orbit

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2
Q

What’s an isotope

A

An isotope has the same number of protons and electrons but different number of neutrons.
So same proton number but different mass number

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3
Q

Isotopic abundance calculation

A

(Atomic mass1 x abundance%)
+ (atomic mass2 x abundance %)
All divided by 100

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4
Q

Mass spectroscopy-how a spectrometer works

A

Atoms put through sample inlet it’s hot to vaporise it

1) ionisation area-where atoms are knocked out by high energy electrons making all of them have 1+ charge
2) acceleration area-all ions given same energy
3) drift region-big space for ions to separate heavier ions travel slower bc ke=1/2mv^2
4) ion detector-calculates mass and gives it as mass/charge or m/z

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5
Q

What is mass number

A

The total number of protons and neutrons in a nucleus

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6
Q

Emission spectroscopy

A

Has a black background with colored lines.The lines represent a fixed and specific frequency of light energy being emitted.
The lines become close together as the frequency becomes higher.This is because the gaps between the energy levels become closer.

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7
Q

Absorption spectroscopy

A

Spectrum background with black lines.
Lines represent fixed and specific light energy being absorbed to go up an energy level.Lines become closer because gaps between energy levels become smaller.

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8
Q

Speed of light equation

A

C (3x10^8)=wavelength x frequency

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9
Q

Energy equation

A

Energy=plancks constant (6.63x10^-34)x frequency (s^-1)

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10
Q

Lithium flame color

A

Red

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11
Q

Sodium color flame

A

Yellow

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12
Q

Potassium flame

A

Lilac

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13
Q

Calcium flame

A

Brick red

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14
Q

Barium flame

A

Apple green

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15
Q

Copper flame

A

Blue green

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16
Q

RELATIVE atomic mass

A

(Ar) of an element is the mass of an atom compared to carbon 12

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17
Q

Relative formula/molecular mass

A

(Mr) of a substance is the mass of its formula unit relative to carbon 12 (sum of atomic masses in ratio of chemical formula)

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18
Q

Formula unit

A

The simplest whole particle of substance (atom,molecule,ion)

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19
Q

Mole

A

Amount of substance contained in atomic mass or molecular mass of the substance

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20
Q

Molar mass

A

The mass of one mole of that substance

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21
Q

Moles calculation

A

Mass/molar mass

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22
Q

Avagadros constant

A

The number of particles in a mole

6.02 x10^23

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23
Q

Empirical formula

A

Simplest ratio of numbers of different types of atom in a substance

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24
Q

Molecular formula

A

The actual number of different types of atoms in a molecule

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25
Hydrated
With water
26
Anhydrous
Without water
27
Water of crystallization
Exactly how much water is part of the crystal structure
28
Things that could affect epsom salt practical results
Leaving crucible lid off Not fully letting water evaporate *Humidity *Getting soot under crucible
29
Ionic bonds contain
Actions and anions held together by strong electrostatic forces
30
Difference between alkali and base
Alkali is type of base alkalis are soluble bases are insoluble
31
Soluble compounds
Group one compounds Ammonium compounds All nitrates (Most ionic compound)
32
Insoluble compounds
Ba Ca Pb and Ag sulfates Ag and Pb halides (cl’br,I) All metal carbonates Metal hydroxides (except group one and ammonium hydroxide)
33
Dissolving
When a substance dissolved the ionic lattice is broken down completely, completely separating ions making them no longer attract each other. Instead they are attracted to the water molecules. The solutions can conduct electricity becuase the ions are charged particles and are free to move.
34
Ioinic equations
Write out dissolved subsastances separately (aq) | Cross our same things on both sides and you’re done
35
Why do we need to know the mass of the sample as well as the elements in it
To make sure they are the only elements in the compound
36
What is standard solution?
A solution of accurately known concentration
37
Group two melting point trend
Melting points decrease as you go down the group except magnesium
38
Why does magnesium not follow the melting point pattern
I’m magnesium there is a change in its crystal structure meaning that the ions are not packed as closely together
39
Precipitate colour of fe 3+ with sodium hydroxide
Orange /brown
40
Brine with silver nitrate
Cream precipitate
41
Copper with sodium hydroxide
Blue precipitate
42
Most carbonates are insoluble except
Potassium ammonium lithium and sodium carbonates
43
Metal hydroxide plus acid
Salt plus water
44
Metal plus water
MEtal hydroxide plus hydrogen
45
Two things you need to add to test for sulfates
Barium chloride and hydrochloric acid | Gives white precipitate of barium sulfate
46
Standard enthalpy change for combustion
Enthalpy change when one mole of fuel burns completely in excess oxygen in its standard state under standard conditions
47
Standard enthalpy change for formation
Enthalpy change when one mole of substance is formed from its constituent elements in their standard states under standard conditions
48
Standard enthalpy change for reaction
Enthalpy change when molar quantities as stated In the equation react completely under standard conditions
49
Enthalpy change for neutralization
Enthalpy change when one mole of aqueous h+ ions react with one mole of oh- ions to form one mole of water.assuming one molar solutions and standard conditions
50
Explain the differences of carbon dioxide and silicon dioxide in terms of bonding
Carbon dioxide is simple molecular substance containing weak intermolecular forces which don’t need a lot of energy to overcome Silicon dioxide is a giant covalent lattice structure so to overcome its four strong covalent bonds more energy is needed and therefore higher temperatures
51
Periodic trends and patterns :melting points
Periods two and three have similar trends (increase to a high one then decrease even lower) This is because of the metallic bonds getting stronger due to increasing number of delocalised electrons and a higher charge density.Then it’s giant covalent structures. And the simple molecular substances have lower but it depends on their intermolecular forces.the noble gases have the lowest because they’re individual atoms with very weak imf
52
Wave speed is
Frequency x wavelength
53
Change in energy is
Planck’s constant x frequency
54
Structural isomer
Same molecular formula different structure
55
Octane rating measures what and why is it good
Measures tendency to auto ignite High rating is good as there is a low auto ignition rate so prevents damage to engine
56
Nitrogen molecule needs lots of energy because
Has a strong triple bond So lots of energy needed to break the bond Nucleus attracted strongly to bonding electrons
57
Would a branched or a straight chain isomer have a higher octane rating
Branched
58
Nuclear fusion
Two lighter nuclei fusing together to form a heavier nucleus
59
What colour is hexa aqua copperii and give structure
(Cu(h2o)6)(2+) | Blue
60
Colour and structure of testers chloro cupprate ii
(Cu(cl)4)2- | Green blue
61
Colour and structure if terra Amina copper ii
(Cu(nh3)4)2+ | Deep blue
62
Colour and structure of hexa aqua iron ii
(Fe(h2o)6)2+ | Green
63
Colour and structure of hexa aqua iron iii
Fe(h2o)6 3+ | Brown
64
Vo2^+ oxidation state and colour
Yellow +5
65
Vo^2+ oxidation state and colour
Blue +4
66
V3+ colour
Green
67
V2+ colour
Violet

Chemistry💁🏻 (15 decks)

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