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Chemistry💁🏻 > Atomic Structure > Flashcards

Atomic Structure Flashcards

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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
Q

Hydrated

A

With water

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26
Q

Anhydrous

A

Without water

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27
Q

Water of crystallization

A

Exactly how much water is part of the crystal structure

28
Q

Things that could affect epsom salt practical results

A

Leaving crucible lid off
Not fully letting water evaporate
*Humidity
*Getting soot under crucible

29
Q

Ionic bonds contain

A

Actions and anions held together by strong electrostatic forces

30
Q

Difference between alkali and base

A

Alkali is type of base alkalis are soluble bases are insoluble

31
Q

Soluble compounds

A

Group one compounds
Ammonium compounds
All nitrates
(Most ionic compound)

32
Q

Insoluble compounds

A

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
Q

Dissolving

A

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
Q

Ioinic equations

A

Write out dissolved subsastances separately (aq)

Cross our same things on both sides and you’re done

35
Q

Why do we need to know the mass of the sample as well as the elements in it

A

To make sure they are the only elements in the compound

36
Q

What is standard solution?

A

A solution of accurately known concentration

37
Q

Group two melting point trend

A

Melting points decrease as you go down the group except magnesium

38
Q

Why does magnesium not follow the melting point pattern

A

I’m magnesium there is a change in its crystal structure meaning that the ions are not packed as closely together

39
Q

Precipitate colour of fe 3+ with sodium hydroxide

A

Orange /brown

40
Q

Brine with silver nitrate

A

Cream precipitate

41
Q

Copper with sodium hydroxide

A

Blue precipitate

42
Q

Most carbonates are insoluble except

A

Potassium ammonium lithium and sodium carbonates

43
Q

Metal hydroxide plus acid

A

Salt plus water

44
Q

Metal plus water

A

MEtal hydroxide plus hydrogen

45
Q

Two things you need to add to test for sulfates

A

Barium chloride and hydrochloric acid

Gives white precipitate of barium sulfate

46
Q

Standard enthalpy change for combustion

A

Enthalpy change when one mole of fuel burns completely in excess oxygen in its standard state under standard conditions

47
Q

Standard enthalpy change for formation

A

Enthalpy change when one mole of substance is formed from its constituent elements in their standard states under standard conditions

48
Q

Standard enthalpy change for reaction

A

Enthalpy change when molar quantities as stated In the equation react completely under standard conditions

49
Q

Enthalpy change for neutralization

A

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
Q

Explain the differences of carbon dioxide and silicon dioxide in terms of bonding

A

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
Q

Periodic trends and patterns :melting points

A

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
Q

Wave speed is

A

Frequency x wavelength

53
Q

Change in energy is

A

Planck’s constant x frequency

54
Q

Structural isomer

A

Same molecular formula different structure

55
Q

Octane rating measures what and why is it good

A

Measures tendency to auto ignite
High rating is good as there is a low auto ignition rate
so prevents damage to engine

56
Q

Nitrogen molecule needs lots of energy because

A

Has a strong triple bond
So lots of energy needed to break the bond
Nucleus attracted strongly to bonding electrons

57
Q

Would a branched or a straight chain isomer have a higher octane rating

A

Branched

58
Q

Nuclear fusion

A

Two lighter nuclei fusing together to form a heavier nucleus

59
Q

What colour is hexa aqua copperii and give structure

A

(Cu(h2o)6)(2+)

Blue

60
Q

Colour and structure of testers chloro cupprate ii

A

(Cu(cl)4)2-

Green blue

61
Q

Colour and structure if terra Amina copper ii

A

(Cu(nh3)4)2+

Deep blue

62
Q

Colour and structure of hexa aqua iron ii

A

(Fe(h2o)6)2+

Green

63
Q

Colour and structure of hexa aqua iron iii

A

Fe(h2o)6 3+

Brown

64
Q

Vo2^+ oxidation state and colour

A

Yellow +5

65
Q

Vo^2+ oxidation state and colour

A

Blue +4

66
Q

V3+ colour

A

Green

67
Q

V2+ colour

A

Violet

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