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Chemistry 2017 > Electron Configuration and Experimental skills > Flashcards

Electron Configuration and Experimental skills Flashcards

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1
Q

What is a systematic error

A

A recurring error which is inherent in the apparatus or experimental method used. Repeating the procedure and averaging results doesn’t eliminate random errors

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2
Q

3 ways to reduce systematic error

A

Re-calibrate instrument, change apparatus or procedure, use new standards

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3
Q

What are random errors

A

Chance variations between successive Measurements.

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4
Q

Random errors are indicated by ‘…’ In the measure values

A

Scatter

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5
Q

How to reduce the effect of random errors

A

Taking the average of repeated measurements or drawing a ‘line of best fit’ through the plotted points on a graph

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6
Q

The precision of a series of measurements is indicated by the degree of uniformity - the more ‘…’ The less precise

A

Scatter

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7
Q

A measurement is ‘…’ to the extent that random errors have been minimised

A

Precise

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8
Q

A measurement is ‘…’ To the extent that systematic errors have been minimised

A

Accurate

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9
Q

What is the formula for K, L, M and N

A

2n^2

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10
Q

How many electrons can K, L, M and N

A

2, 8, 18, 32

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11
Q

What can an orbital be visualised as

A

A blurry cloud of negative charge: the charge is most dense where the probability of finding the electron is the largest

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12
Q

How many orbitals and electrons does the S subshell contain

A

1 orbital - 2 electrons

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13
Q

How many orbitals and electrons does the subshell p contain

A

3 orbitals - 6 electrons

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14
Q

How many orbitals and electrons does the subshell d hold

A

Orbitals 5, Electrons 10

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15
Q

How many orbitals and electrons does the subshell f hold

A

Orbitals 7, Electrons 14

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16
Q

What is Hund’s Rule

A

When electrons occupy orbitals of equal energy, one electron enters each orbital until all orbitals contain one electron

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17
Q

What two elements do not follow the usual pattern

A

Chromium, Copper

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18
Q

What are the last two subshells of chromium

A

3d^5, 4s^1

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19
Q

What are the last two subshells of copper

A

3d^10 4s^1

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20
Q

Which electrons should be deleted first and second to create ion subshell notation

A

4s and 3D

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21
Q

How to figure out the group and period using subshell configuration

A 
Period = number of occupied electron shells 
Group = number of electrons in the valence shell (Roman numerals)
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22
Q

Define Energy sequence of orbitals

A

Electrons enter orbitals of lowest energy first

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23
Q

define Pauli Exclusion Principal

A

Orbitals can only accommodate a maximum of 2 electrons, and these must have opposite spins

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24
Q

Metals ‘…’ Electrons in chemical reactions

A

Lose

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25
Q

Non-metals “…” Or “…” Electrons in chemical reactions

A

Gain or share

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26
Q

Metalloids ‘…’ Or ‘…’ In chemical reactions

A

Lose or share

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27
Q

What can atoms of periods 3 and 4 do with elements from group V to VII

A

Share all their outer shell electrons

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28
Q

Where do extra electrons go when expanding the octet

A

3d shell

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29
Q

In group 1 elements what is the charge of a monatomic ion and the oxidation state of elements

A

1+ & +1

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30
Q

In group II elements what is the charge of a monatomic ion and the oxidation state of elements

A

2+ & +2

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31
Q

In group III elements what is the charge of a monatomic ion and the oxidation state of elements

A

3+ & +3

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32
Q

In group IV elements what is the charge of a monatomic ion and the oxidation state of elements

A

2+ or 4+ and +4, +2 or -4

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33
Q

In group V elements what is the charge of a monatomic ion and the oxidation state of elements

A

3- & +5, +3, or -3

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34
Q

In group VI elements what is the charge of a monatomic ion and the oxidation state of elements

A

2- & +6, +4, +2 or -2

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35
Q

In group VII elements what is the charge of a monatomic ion and the oxidation state of elements

A

1- & +7, +5, +3, +1 or -1

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36
Q

What is electronegativity

A

Ability of an atom to attract electrons to itself

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37
Q

An ‘…’ Substance can donate or accept protons

A

Amphiprotic

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38
Q

An ‘…’ Substance can react with an acid or a base

A

Amphoteric

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39
Q

What are acidic oxides oxides of

A

Non-metals

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40
Q

What do acidic oxides react with hydroxide ions to form

A

Oxyanions

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41
Q

What is an ionic bond

A

Between metal and non-metal atoms

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42
Q

What is a metallic bond between

A

Metal atoms

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43
Q

What are covalent bonds between

A

Non-metals

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44
Q

What are the bonds between atoms called

A

Primary bonds

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45
Q

What are bonds between molecules

A

Secondary or intermolecular

46
Q

3 types of secondary bonds

A

Dispersion forces, dipole-dipole and hydrogen Bonding

47
Q

7 properties of ionic compounds

A
  1. Usually crystalline solids 2. High melting and boiling points 3. Dissociate in water 4. Solids won’t conduct electricity 5. Conduct electricity as a molten or in aqueous solution 6. Hard 7. Brittle
48
Q

Are polar bonds shared equally

A

No

49
Q

Two properties a molecule must have to be polar

A

Polar bonds, asymmetrical charge distribution

50
Q

Like dissolves in ?

A

Like

51
Q

What does the strength of dispersion forces depend on

A

The number of electrons, the more electrons the stronger the molecule

52
Q

How do dipole dipole reactions work

A

The positive end of one molecule is attracted to the negative end of another neighbouring molecule in polar molecules only

53
Q

What does hydrogen bonding form between

A

Hydrogen attached to nitrogen, oxygen or fluorine in one molecule and nitrogen, oxygen or fluorine in another molecule.

54
Q

How does hydrogen bonding work

A

When N, O and F are covalently bonded to hydrogen molecules leaving them exposed, this then strongly attracts the electronegative nitrogen, oxygen or fluorine in the neighbouring dipoles

55
Q

Would Nitrogen or CO2 have a higher boiling point

A

CO2

56
Q

Which would have a higher boiling point HF or HCL

A

HF

57
Q

Which has a higher boiling point SO2 and SF6

A

SO2

58
Q

Which would have a higher boiling point

A

NH3 and PF3

59
Q

Covalent molecules substance tend to have relatively ‘…’ Melting and boiling points

A

Low

60
Q

What is a continuous covalent lattice, give three examples

A

A giant structure in which no individual molecules exist, Silicon Dioxide/ Quartz (SiO2), Silicon Carbide (SiC) and Diamond (C)

61
Q

6 properties of covalent network lattices

A

Very hard, brittle, high melting and boiling points, non conductors (No free electrons), Insoluble

62
Q

What is decomposition

A

A chemical reaction in which a compound breaks down into simpler compounds or elements.

63
Q

What is aerobic respiration

A

The process in which foodstuffs are fully oxidised with the release of chemical energy. Process requires a ready supply of molecular oxygen

64
Q

Anaerobic respiration

A

Process by which foodstuffs are partially oxidised, with the release of chemical energy, in the absence of molecular oxygen.

65
Q

Alcoholic fermentation is a type of ‘…’ Respiration which one of the end products is ‘…’

A

Anaerobic, ethanol

66
Q

Aerobic products of Carbon, Hydrogen, Sulfur, Nitrogen, Phosphorus

A

Carbon Dioxide, Water, Sulfates, Nitrates, Phosphates

67
Q

Anaerobic products of Carbon, Hydrogen, Sulfur, Nitrogen, Phosphorus

A

Methane, Water, Hydrogen Sulphide, Ammonia, Phosphine

68
Q

Two key processes of the carbon and oxygen cycle and their equations

A

Photosynthesis: 6CO2 + 6H2O -(Sunlight & Chlorophyll)-> C6H12O6 + 6O2

Respiration: C6H12O6 + 6O2 –> 6CO2 + 6H2O + Energy

69
Q

What is nitrogen fixation

A

The conversion of atmospheric nitrogen into soluble nitrogen compounds such as nitrates and ammonium salts.

70
Q

What is the nitrogen cycle

A

The continuous chemical interchange between nitrogen in the atmosphere and the biosphere

71
Q

What is found in the nodules on the roots of legume plants

A

Nitrogen fixing bacteria which contain an enzyme that catalyses the conversion of atmospheric nitrogen into ammonia or ammonium compounds

72
Q

Other than microbes, what initiates nitrogen fixation and how do they do this

A

Lightening discharge and forest fires, high energy produced are sufficient to break the triple bond in the N2 molecule

73
Q

Two formulas related to natural nitrogen fixation through microbes, fires, lightening etc

A

N2 + O2 –> 2NO

2NO + O2 –> 2NO2

74
Q

Formula for forming nitrate ions which are deposited in the soil when it rains

A

2NO2 + H2O –> H(+) + NO3(-) + HNO2

75
Q

Causes of artificial nitrogen fixation

A

Combustion of fuels in the internal combustion engine and industrial furnaces produce the high temperatures needed

76
Q

What is the reaction the haber process uses high temperatures in artificial nitrogen fixation to bring about

A

N2 + 3H2 –> 2NH3

77
Q

What can ammonia be used as after the Haber process

A

Plant fertiliser

78
Q

What is denitrification

A

The process by which diatomic nitrogen is returned to the atmosphere

79
Q

Reaction between rock phosphate and sulfuric acid which produces superphosphate

A

Ca3(PO4)2 + 2H2SO4 –> CaSO4 + Ca(H2PO4)2

80
Q

What is water pollution brought on by excess nutrients

A

eutrophication

81
Q

Photochemical smog is a form of …

A

Lower atmosphere air pollution

82
Q

Formula for general rain

A

CO2 + H2O -> H2CO3

83
Q

Oxides of Sulfur two equations

A

Compounds of Sulfur + O2 -> SO2

2SO2 + O2 -> 2SO3

84
Q

How does acid rain effect foliage

A

Causes damage that affects water loss from leaves, disrupts photosynthesis,

85
Q

How does acid rain effect soil

A

Leaches essential ions, can mobilise potentially toxic ions

86
Q

How does acid rain effect bacteria, include equation (aluminium)

A

Free aluminium ions can also damage bacteria that plants need

Al2O3 + 6H+ -> 2Al3+ + 3H2O-

87
Q

How does acid rain effect the fish population

A

Fish can suffer from excessive loss of sodium from the gills, free aluminium ions can restrict extraction of oxygen,

88
Q

How does acid rain effect human health

A

Toxic metal ions can be transported in solutions of drinking water eg dams and wells

89
Q

How does acid rain impact the built environment

A

Buildings made of limestone, marble and sandstone are washed away due to how they react with acid rain

90
Q

Two formulas for acid rain with calcium carbonate (Limestone and Marble)

A

CaCO3 + H2SO4 -> CaSO4 + CO2 + H2O

CaCO3 + HNO3 -> Ca(NO3)2 + CO2 + H2O

91
Q

Formula for pH

A

-Log[H3O+] [Concentration]

92
Q

Formula for concentration

A

10^pH OR -pH = log[H+]

93
Q

What is the waste product of the burning of fossil fuels

A

Carbon dioxide

94
Q

What role does carbon dioxide play in the earth

A

Regulates the temperatures on Earth

95
Q

How does carbon dioxide regulate the earths temperature and what is this process known as

A

Allows solar radiation, blocks heat radiated from the earths surface from escaping, acts like a one way blanket,
greenhouse effect

96
Q

What are the green house gases

A

Carbon dioxide, water vapour, methane, nitrous oxide and halocarbons

97
Q

What are the two primary pollutants of photochemical smog

A

Nitric Oxide and Hydrocarbons

98
Q

Equation of nitrous oxide and how is it created

A

N2 + O2 -> 2NO, formed within the combustion chamber of motor vehicle engines

99
Q

Equation for Nitrogen Dioxide and how is it formed

A

2NO + O2 -> 2NO2, nitric ochre is slowly oxidised to nitrogen dioxide in the atmosphere, nitrogen dioxide is yellowish brown gas

100
Q

Two equations for the production of Ozone

A

NO2 + UV -> NO + O

O + O2 -> O3

101
Q

Formula for when nitrogen dioxide is reformed from nitric oxide through the destruction of ozone

A

NO + O3 -> NO2 + O2

102
Q

3 equations involving Carbon monoxide, hydrocarbons and nitric oxide as a result of a catalytic converter

A

CO + O2 -> 2CO2

C8H18 + 25O2 -> 16CO2 + 18H2O

2NO + 2CO -> N2 + 2CO2

103
Q

Why does ammonium Sulfate provide nitrogen in a suitable form for use by plants

A

As its soluble and dissociates in water, ammonium ions are absorbed in aqueous solution through the roots

104
Q

Equation for the reaction of ammonium ion with water to form an acidic solution

A

NH4^+ + H2O ->

105
Q

If soluble in water what do acidic oxides react with water to form

A

Oxyacids

106
Q

Sulfur dioxide reaction with hydroxide ions and reaction with water

A

SO2 + 2OH^- -> SO3^2- + H2O

SO2 + H2O -> H2SO3 (sulfurous acid)

107
Q

Basic oxides are oxides of …

A

Metals

108
Q

Basic oxides react with acids or hydrogen ions to form

A

Metal cations and water molecules

109
Q

If soluble in water what do basic oxides form

A

Metal cations and hydroxide ions

110
Q

Sodium oxide reaction with hydrogen ions and water

A

Na2O + 2H+ -> 2Na+ + H2O

Na2O + H2O -> 2Na+ + 2OH-

Chemistry 2017 (5 decks)

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