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Unit 1 Chemistry + Chromatography > Chemistry Test 2 > Flashcards

Chemistry Test 2 Flashcards

1
Q

How did Bohr confirm the existence of Electron shells?

A

He found the energy difference between levels by measuring the frequencies of emitted photons.

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2
Q

Bohr’s Discovery about Electrons and their Energy Levels

A
  • Electrons orbit the nucleus in fixed energy levels
  • Explained Electron Excitation, Electrons move up higher if they have more energy, shorter wavelength
  • Other energy shells exist but electrons do not occupy it
  • Electrons cannot be between levels
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3
Q

Electron configuration Maxes

A

1st Level Max: 2
2nd Level Max: 8
3rd Level Max: 8
4th Level Max: 2

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4
Q

Arrangement of Electrons effect?

A

The arrangement of the electrons into energy levels or shells is what determines the chemical behavior of an atom of an element.

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5
Q

Stability of the Valence shell effect?

A

The number of electrons in the valence shell of an atom determines its reactivity, tendency to form chemical bonds. A stable electron configuration is reached through the octet rule, this constitutes gaining or losing of electrons.

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6
Q

Isotopes Written Form IUPAC

A

Isotopes are written in the form with mass number in superscript to the left side of the element according to IUPAC

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7
Q

What properties of Isotopes are different?

A

Physical properties such as mass, inertia, density, melting, boiling and freezing point are different

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8
Q

Relative Atomic Mass

A

Relative Atomic Mass is defined as the ratio of the average mass of an atom (taking into account all isotopes and their natural abundances) compared to a 1/12 a Carbon-12 atom

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9
Q

Relative Atomic Mass formula

A

((%abundance of isotope x relative isotopic mass) + (%abundance x relative isotopic mass))/100

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10
Q

Mass Spectrometry Step 1: (Vapourised)

A

Sample is vapourised with extreme heat into gas form

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11
Q

Mass Spectrometry Step 2: (Ionised)

A

High Energy Electrons from an Electron gun bombard the sample atoms and knock off electrons ionizing them into cations.

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12
Q

Mass Spectrometry Step 3: (Acceleration)

A

Ions are accelerated so they all have the same kinetic energy (using accelerator plates)

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13
Q

Mass Spectrometry
Step 4: (Mass Tendency)

A

Inertia due to mass (tendency)

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14
Q

Mass Spectrometry:
Step 5: (Magnetism)

A

Amount of force ions feels from electromagnet is proportional to its charge.

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15
Q

Mass Spectrometry:
Step 6: (Deflection Part 1)

A

(Deflection due to charge)

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16
Q

Mass Spectrometry
Step 7: (Deflection Part 2)

A

Separated by mass (mass inertia comes in play with deflection due to charge)

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17
Q

Mass Spectrometry Step 8: (Detector)

A

Records Mass to charge ratios and isotopic. abundances

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18
Q

Mass Spectrum

A

A mass spectrum is the results produced by mass spectroscopy with relative abundance on y axis and mass to charge ratio (m/z) on x axis

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19
Q

Atomic Mass Calculation

A

Average of all isotopes of an atom

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20
Q

Relative Isotopic Mass

A

The ratio of the mass of an isotope of an element to 1/12 a Carbon-12 atom

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21
Q

How to calculate %abundance of an isotope from a Mass Spectra

A

Peak Height/Total Peak Height x 100

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22
Q

Properties of Elements Periodic table groups 7, 1, 2 and 8

A

Group 7 Halogens, Highly Reactive Group 1 and 2 metals are highly reactive Group 8 is inert, noble gases.

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23
Q

Atomic Radius Trend

A

Atomic Radius Trend is Increases down a group; as there are more energy levels and from right to left; decreased nuclear charge which leads to less pull of valence shells by lower positive charge

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24
Q

Electronegativity Definition and Trend w/ reason

A

Electronegativity is the ability for a neutral atom to attract valence electrons of an atom. Increase up a group; as there is less valence shells to disperse positive charge from nucleus which attracts electrons, increases from left to right; due to an increase nuclear charge which increase force of attraction.

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25
1st Ionisation Energy Definition and Trend w/reason
1st Ionisation energy refers to the energy required to remove the most loosely bound electron of a neutral atom. Decreases down a group; due to increased number of valence shells occupied which results in valence electrons being removed with less resistance from nuclear positive charge. Increases left to right; due to an increased resistance from a high number of protons.
26
Electron affinity Definition and Trend w/o reason
Electron affinity is the potential energy change that occurs when electron/s are added to a gaseous atom. Increases to the right and up
27
Lewis Structures
Show they way that atoms share electrons when forming a molecule
28
What is a flame test?
A flame test is an analytical technique used to determine the presence of element in a salt or compound by colour. Elements absorb heat energy exciting electrons of different elements in different levels as they have distinct energy levels which causes the emission of specific discrete wavelengths only that element can emit when they return to ground state resulting in distinct colors which make up one main observable flame colour when state signifying the presence of a certain element. Uses nonluminous flame.
29
Flame Test Observed Colour (Absorption and Emission) and Electron Excitation Explanation
Flame tests rely on the transferring of energy by the electrons of the atoms through heat energy which excites electrons of a particular element in characteristic and distinct levels because they have distinct energy levels causing them to jump energy levels with the jump being proportional to energy absorbed. These excited electrons return back to ground state emitting the same energy absorbed in the form of visible light (photons) of specific wavelengths (emission spectra) which only that atom can emmit. These wavelengths are proportional to the jump back down to the ground state with a greater jump leading to a shorter wavelength and vice versa. These wavelengths emitted makes up the colour seen in the flame characterizing a specific elements presence.
30
Atomic Absorption Spectroscopy (AAS) (Absorption and Emission Excitation)
Atomic Absorption Spectroscopy is an analytical technique which is used to find the concentration of small traces of different elements in a solution. It utilizes the solution which is first aspirated through a spray chamber, combined with a fuel and its oxidant which allow combustion in the burner. The burner combusts the sample and atomizes it into gaseous free atoms in the flame. A cathode lamp of the specific element being analyzed is provided with electrical energy which excites the atoms in the element to specific energy levels which only that element can absorb due to their distinct energy levels which then is emitted in those specific wavelengths (emission spectra) which only that element can emit when the electrons return to ground state. These wavelengths are then absorbed by the free atoms which excites them as the wavelengths are nearly complementary to the element's own absorption spectra. The rest of the light that is not absorbed is turned into one specific wavelength by a monochromator to be photo multiplied which turns the light into an electrical signal which is sent to the computer which spits out an absorbance value used to calculate concentration for a main solution
31
Calibration Curves, Calibration values and calibration solutions
Calibration curves shows the proportionality between an element's absorbance value (y axis) and its concentration (x axis). A sample. Calibration solutions are a range of different solutions with set concentrations of the element being analyzed. These concentrations are called calibration values when the equivalent absorbance values are found. These values are used for the main solution when we have the absorbance but not the concentration so the concentration can be read off the calibration curve. A calibration curve is titled with the symbol for an element followed by the word calibration e.g. Au calibration
32
ppm and milligrams per liter equivalence point
When the solvent is water, these units are equivalent (density of 1 gm/ml)
33
What are pure substances? (Properties)
Pure substances are substances that contain only one type of compound or element. Homogenous. Holds a constant composition. They have distinct measurable physical properties. For example, water
34
What is a mixture?
Contains at least 2 physically combined substances. Can be homogenous or heterogenous.
35
What is a compound
A compound refers to two or more chemically combined elements
36
What is a solution?
A solution is a special type of mixture with two phases (solvent and solute) and is usually homogenous. Solution is uniform (single phase).
37
States of Matter in a Solution with examples for each
gas in gas gas in liquid (soda) Co2 in water liquid in liquid (gasoline) solid in liquid (salt water) gas in solid (smoke) liquid in solid (Water in gelatin- jelly) solid in solid - alloys
38
What is heterogenous mixture? Two classes, Light scattering and an example
2 or more physically combined substances (elements/compounds) with distinct, detectable phases. Does not have uniform properties. Differently composed throughout. Yes, it is always. Colloids and Suspensions. Tyndall effect comes in play. Brick or Milk
39
What is homogenous matter
same throughout
40
What is heterogenous matter?
Different throughout
41
Three ways to separate a mixture by Particle Size
Gravitational Filtration, Vacuum Filtration, Sieving
42
What is homogenous mixture? Example
Constantly composed throughout (solutions) (sugar water, salt water)
43
3 classes of mixtures
Suspension, Colloids and Solutions
44
What is Gravitational Filtration
It is when you rely on the weight of the solid particles to filter the two materials
45
Tyndal Effect
Scattering of light by particles in a colloid or suspensions
46
What are Suspensions and their features with an example? Heterogenous or Homogenous
A suspension is a system that does not stay stable. Can be easily filtered out. Heterogenous Mixtures. Example is muddy water or aerosols (which are a suspension of fine liquid or solid particles in a gas)
47
What are Colloids and their features with an example? Heterogenous or Homogenous
Colloids are non-transparent (opaque), non-uniform, cloudy liquids with large particles but has a stable system. E.g. milk. Heterogenous Mixtures
48
What is Vacuum Filtration
It is faster than gravitational filtration and is Useful if the particles are light and you want to dry out the mixture.
49
Sieving
Sieving is used to separate the components of a mixture with different particles sizes (sand and gravel) (sand and water)
50
Separation of Mixtures by solubility
Filtration is used to separate an insoluble substance from the solvent. Used to separate heterogenous.
51
Separation by Densities techniques
Sedimentation, Decantation, Separation funnels
52
Sedimentation (Density Seperation)
Sedimentation is when the denser materials drop to the bottom.
53
Decantation after Sedimentation (Density Seperation)
Decantation is when your pour the top liquid away from the sediment
54
Separation funnels (Density Separation)
Separation funnels can be used to extract the sediment of two liquids that don't mix.
55
Centrifugation (Density Separation)
Centrifugation is when a mixture is spinned, which settles the finer particles which may otherwise not settle.
56
Separation by Boiling Point Techniques
- Evaporation - Distillation - Fractional Distillation
57
Evaporation
Evaporation is when you boil off a liquid (solvent) leaving behind the dissolved material (solute)
58
Distillation
Distillation uses evaporation but then collects the gas, the condenser converts the gas back into a liquid which is collected.
59
Fractional Distillation
Fractional Distillation is used for mixtures that have many different substances in them, that all have different boiling points.
60
Crystallisation
Separation technique that results in the formation of a pure solid particles from a solution contained the dissolved substances. As one substance evaporates the dissolved substance comes out and collects as crystals (highly pure solid)
61
Separation by electrical charge (What is Electrostatic Seperation)
Electrostatic separation can be used to separate charged solid particles from a gas.
62
Separation by electrical charge (What is Chromatography)
Chromatography is a separation is a technique that relies on how 'sticky' one material is to a static medium such as paper or resin that can separate components out of a mixture..
63
Magnetic seperation
Separates a magnetic substance from a non-magnetic substance
64
Flame colour for Potassium
Lilac
65
Flame Colour for Lithium
Pink-Red
66
Flame Colour for Sodium
Yellow
67
Copper Flame colour
Blue-Green
68
Barium Flame colour
Green
69
Calcium Flame colour
Brick red
70
Iron Flame Colour
Orange-brown
71
Strontium Flame Colour
Red
72
Write Hydroxide formula
OH-
73
Write Nitrite formula
NO2-
74
Write nitrate formula
NO3-
75
Write Carbonate Formula
CO3-2
76
Write Sulfate formula
SO4-2
77
Write sulfite formula
SO3-2
78
Write Phospate formula
PO4-3
79
Acid formula rule
Add on number of hydrogen at the front of the compound charge after
80
Other Polyatomic Ions
Learn From Appendix 2
81
Permanganate Formula
MNO4-

Unit 1 Chemistry + Chromatography (5 decks)

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