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AS Chemistry > Topic 1 - Elements of Life > Flashcards

Topic 1 - Elements of Life Flashcards

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1
Q

What other group has similar properties to group 2?

A

Group 1

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2
Q

Describe the reactivity of group 2 hydroxides

A

Increases going down the periodic table (Calcium Hydroxide is least reactive)

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3
Q

Describe the reactivity of group 2 sulfates

A

Decreases going down the periodic table (Barium Sulfate is least reactive)

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4
Q

Describe the trend of ionisation energy in group 2

A

Decreases down group
- Less electrostatic attraction
-Outermost shell is further from the nucleus

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5
Q

Describe the trend of reactivity in group 2 metals

A

Increases down the group - outermost shell gets further away from nucleus

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6
Q

Describe the trend of melting points in group 2 metals

A

Decreases down group

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7
Q

Describe thermal stability of group 2 carbonates

A

Increases down group
-Depends on charge density
-Smaller ion = higher charge density
-Higher charge density = less thermal stability, more CO3 distortion (products: CO2 and O2-) and forms more moles of carbonate

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8
Q

What is a spectrometer?

A

A machine that works out the atomic mass and formula mass of a sample

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9
Q

1st stage of spectrometry

A

Injection
-sample injected

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10
Q

2nd stage of spectrometry

A

Vaporisation
-sample heated to a gas

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11
Q

3rd stage of spectrometry

A

Ionisation chamber
-hit with high energy electrons - turns into cations

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12
Q

4th stage of spectrometry

A

Acceleration area
-ions accelerated to same KE as an electric field

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13
Q

5th Stage of spectrometry

A

Drift region
-ions travel through magnetic field

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14
Q

6th stage of spectrometry

A

Detector
-time to reach detector is measured
-cations gain electrons and create current

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15
Q

What does the current created say about the number of ions?

A

High = lots of ions

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16
Q

What does the speed that the ions hit the detector show?

A

Slow speed = heavier ions

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17
Q

Define periodicity

A

Regular variation of properties of elements with their position in the periodic table

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18
Q

What is first ionisation energy?

A

Energy required to remove 1 mole of electrons from 1 mole of a gaseous element
Example: Na(g) –> Na+(g) + e-

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19
Q

Why is ionisation energy always measured in gaseous state?

A

Eliminates energy for melting/boiling

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20
Q

Trend of atomic radius in period 3

A

-Electrons added to same shell
-More protons in nucleus, stronger attraction between nucleus and outermost shell
-Atomic radius decreases

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21
Q

Trend of melting/boiling points in period 3

A

Starts high - giant metallic and covalent structures
Then decreases - simple covalent

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22
Q

Define successive ionisation energy

A

A measure of the energy required to remove 1 mole of electrons in turn from 1 mole of gaseous atoms/ions

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23
Q

Define energy (/shell) level

A

Electrons at the same energy level are in the same shell
(Number)

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24
Q

Define sub shell

A

Within a shell. Successive subshells have extra subshells
(Letter)

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25
Q

Define orbital

A

Region of space where 2 electrons spend 98% of their time. Within a subshell
(Boxes/superscript numbers)

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26
Q

What are the orbitals?

A

1 s-orbital
3 p-orbitals
5 d-orbitals

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27
Q

Shape of an s-orbital?

A

Spherical

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28
Q

Shape of a p-orbital?

A

Dumbell (drawn like figure of 8 on xyz-axis)
Can be any orientation

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29
Q

Shape of a d-orbital?

A

Various shapes and orientation

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30
Q

How many s-orbitals are in each electron shell?

A

1

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31
Q

How many p-orbitals are in each electron shell?

A

3, from 2nd shell onward

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32
Q

How many d-orbitals are in each electron shell?

A

5, from 2nd shell onward

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33
Q

Full electron configuration of potassium?

A

1s2 2s2 3p6 3s2 3p6 4s1

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34
Q

Noble gas configuration of potassium?

A

[Ar] 4s1

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35
Q

What is VESPR theory?

A

Explains the shape of electrons based on the number of ares of electron density around the central atom

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36
Q

Considered points in VESPR theory

A

-Central atom
-Number of areas of electron density (bonds and lone pairs)
-Electrons repel as far as possible (AFAP)
-Lone pairs repel more than bonding pairs

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37
Q

Define dative covalent bond

A

A covalent bond where both electrons are supplied by one bonding atom

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38
Q

Bond angle for 2 areas of electron density

A

180°

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39
Q

Bond angle for 3 areas of electron density

A

120°

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40
Q

Bond angle for 4 areas of electron density

A

109.5°

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41
Q

Bond angle for 5 areas of electron density

A

120° and 90°

42
Q

Bond angle for 6 areas of electron density

A

90°

43
Q

Shape for 2 areas of electron density

A

Linear

44
Q

Shape for 3 areas of electron density

A

Trigonal Planar

45
Q

Shape for 4 areas of electron density

A

Tetrahedral

46
Q

Shape for 5 areas of electron density

A

Trigonal bipyramidal

47
Q

Shape for 6 areas of electron density

A

Octahedral

48
Q

What does a wedge mean in drawing VESPR?

A

Drawing coming out infront of paper plane

49
Q

What does a dashed line mean in drawing VESPR?

A

Drawing going behind the plane of paper

50
Q

Drawing for 4 areas of electron density

A

2 normal lines
1 wedge
1 dashed line

51
Q

Drawing for 5 areas of electron density

A

3 normal lines
1 wedge
1 dashed line
90° between 2 normal lines
120° between middle normal and wedge

52
Q

Drawing for 6 areas of electron density

A

4 normal lines
1 wedge
1 dashed line

53
Q

Bond angle for 4 areas of electron density with 1 lone pair

A

107°

54
Q

Bond angle for 4 areas of electron density with 2 lone pairs

A

104.5°

55
Q

Shape for 4 areas of electron density with 1 lone pair

A

Trigonal pyramidal

56
Q

Shape for 4 areas of electron density with 2 lone pairs

A

(Linear) bent

57
Q

Drawing for 4 areas of electron density with 1 lone pair

A

1 normal line
1 wedge
1 dashed line

58
Q

Drawing for 4 areas of electron density with 2 lone pairs

A

2 normal lines

59
Q

What colour do copper ions go when burnt?

A

Blue-green

60
Q

What colour do lithium ions go when burnt?

A

Crimson

61
Q

What colour do potassium ions go when burnt?

A

Lilac

62
Q

What colour do sodium ions go when burnt?

A

Yellow

63
Q

What colour do calcium ions go when burnt?

A

Brick red

64
Q

What colour do barium ions go when burnt?

A

Green

65
Q

What colour precipitate is formed when copper (II) reacts with NaOH?

A

Blue

66
Q

What colour precipitate is formed when iron (II) reacts with NaOH?

A

Green

67
Q

What colour precipitate is formed when iron (III) reacts with NaOH?

A

Brown

68
Q

What colour precipitate is formed when calcium ions react with NaOH?

A

White

69
Q

What colour precipitate is formed when aluminum ions react with NH4OH?

A

White

70
Q

What colour precipitate is formed when zinc (II) ions react with NH4OH?

A

White

71
Q

What happens if excess NH4OH is added to zinc (II) ions?

A

Redissolves into a colourless solution

72
Q

What is used to test for lead (II) ions?

A

Potassium iodide

73
Q

What colour is the precipitate for a positive test for lead (II) ions?

A

Yellow

74
Q

What is used to test for sulfate ions?

A

Barium chloride

75
Q

What colour is the precipitate for a positive test for sulfate ions?

A

White

76
Q

What is used to test the halide ions?

A

Silver nitrate

77
Q

What colour is the precipitate for a positive test for chloride ions?

A

White

78
Q

What colour is the precipitate for a positive test for bromide ions?

A

Cream

79
Q

What colour is the precipitate for a positive test for iodide ions?

A

Yellow

80
Q

What is used to test ammonium ions?

A

Sodium hydroxide

81
Q

What is used to test nitrate ions?

A

Sodium hydroxide and aluminum

82
Q

How can the ammonia formed be tested?

A

Damp red litmus paper would be turned blue

83
Q

What is the result for a positive test for ammonium/nitrate ions?

A

When warmed ammonia is formed

84
Q

What is used to test for carbonate ions?

A

Acid

85
Q

What gas would form in a positive test for carbonate ions?

A

CO2

86
Q

How can the gas in the test for carbonate ions be tested?

A

Bubble gas through limewater. If CO2 present then limewater will go from clear to cloudy

87
Q

Define excited electron state

A

Electron placement after energy absorption

88
Q

Define ground electron state

A

Where electrons are normally

89
Q

What does an absorption spectra look like?

A

-Coloured background
-Black lines
-Lines get closer at higher frequencies

90
Q

What does an emission spectra look like?

A

-Black background
-Coloured lines
-Lines get closer at higher frequencies

91
Q

Why do the lines on absorption/emission spectra get closer at higher frequencies?

A

Energy levels decrease further from an atom’s nucleus

92
Q

What are the products formed when a metal and acid are reacted?

A

Salt and hydrogen

93
Q

What are the products formed when a metal hydroxide and acid are reacted?

A

Salt and water

94
Q

What are the products formed when a metal oxide and acid are reacted?

A

Salt and water

95
Q

What are the products formed when a metal carbonate and acid are reacted?

A

Salt, water and carbon dioxide

96
Q

How are insoluble salts made?

A

-Make precipitate from 2 soluble salts
-Filter
-Rinse in distilled water
-Dry

97
Q

How are soluble salts made using metals/insoluble bases?

A

-Add solid in excess
-Filter
-Heat solution
-Pat dry

98
Q

How are soluble salts made using acids and alkalis?

A

-Do a titration and using indicator
-Note the volumes for neutralisation
-Repeat using exact values (no indicator)
-Heat solution
-Pat dry

99
Q

Equation with Planck’s constant and frequency

A

E = hv

E - Energy/J
h - Planck’s constant/J Hz^-1
v - Frequency/Hz

100
Q

Equation with Planck’s constant and wavelength

A

E = hc/λ

E - Energy/J
h - Planck’s constant/J Hz^-1
c - Speed of light/m s^-1
λ - Wavelength/m

AS Chemistry (2 decks)

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