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BMAT > Chem > Flashcards

Chem Flashcards

1
Q

Diameter of nucleus compared to diameter of atom

A

less than 1/20000 that of an atom

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2
Q

Energy shells around nucleus

A

Concentric circles

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3
Q

How to find number and abundances of isotopes of an element

A

Mass spec

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4
Q

Mass spec graph

A

X axis - m/z

Y axis - relative abundance

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5
Q

Reactivity trend - group 1/2

A

Reactivity increases

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6
Q

Reactivity trend - group 6/7

A

Less reactive

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7
Q

Lithium with cold water observations

A
  • slow
  • floats but does not melt
  • dissolves to form alkaline solution of LiOH
  • hydrogen gas
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8
Q

Sodium with cold water observations

A
  • more strongly than lithium
  • moves around surface + melts + quickly dissolves
  • alkaline solution of NaOH
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9
Q

Potassium with water reaction

A
  • moves rapidly on the surface
  • very quickly dissolves to produce an alkaline solution of KOH
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10
Q

Period number…

A

Number of shells

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11
Q

Group number…

A

Number of outermost electrons

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12
Q

Lithium

A

Li+

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13
Q

Sodium

A

Na+

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14
Q

Potassium

A

K+

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15
Q

Magnesium

A

Mg2+

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16
Q

Calcium

A

Ca2+

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17
Q

Barium

A

Ba2+

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18
Q

Aluminium

A

Al3+

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19
Q

Copper (II)

A

Cu2+

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20
Q

Silver

A

Ag+

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21
Q

Zinc

A

Zn2+

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22
Q

Sulfide

A

S2-

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23
Q

sulfuric acid

A

H2SO4

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24
Q

ethanoic acid

A

CH3COOH

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25
Q

buckminsterfullerene

A

C60

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26
Q

nitrogen

A

N2

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27
Q

acid + carbonate ionic

A

2H+(aq) + CO32−(aq) → H2O(l) + CO2(g)

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28
Q

Acid + ammonia ionic

A

H+(aq) + NH3(aq) → NH4+(aq)

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29
Q

Avagadros symbol

A

NA (a is subscript)

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30
Q

Avogadros number

A

6.022 × 1023 mol−1

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31
Q

Define concentration

A

measure of the number of solute particles in a given volume of solution.

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32
Q

Saturated solution

A

no more solute will dissolve at a given temperature.

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33
Q

Gases + solubility + temp

A

gases become less soluble as temperature increases

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34
Q

Reasons % yield not 100

A

the reaction will not go to completion if it is reversible

some of the product may be lost when it is separated from the reaction mixture

some of the reactants may also react in ways different to the expected reaction.

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35
Q

Oxidation

A

Gain of oxygen or LOSS OF HYDROGEN

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36
Q

Oxidation states in H2O2

A

oxygen atoms have an oxidation state of −1

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37
Q

Oxidation states in OF2

A

oxygen atom has an oxidation state of +2.

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38
Q

Oxidation state of hydrogen

A

always +1.

The exception is when hydrogen is part of a metal hydride, for example MgH2, and in this case the hydrogen atoms have an oxidation state of −1.

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39
Q

Giant covalent properties

A

Very high melting and boiling points

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40
Q

Why do giant covalent have a high melting + boiling point

A

all of the strong covalent bonds have to be broken

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41
Q

Graphite

A

Soft + conducts electricity

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42
Q

Melting point of simple covalent

A

Low

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43
Q

Order of group 1 - going down

A
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44
Q

Trend in boiling points - 1

A

Decrease

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45
Q

Trend in densities- 1

A

Increase

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46
Q

Trend in hardness - 1

A

Decrease

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47
Q

How to prevent group 1 reacting

A

stored in oil

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48
Q

Metal + water

A

Metal hydroxide + hydrogen

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49
Q

The metal hydroxide is…

A

Soluble = makes solution alkaline

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50
Q

2K(s) + Cl2(g)

A

2K(s) + Cl2(g) → 2KCl(s)

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51
Q

Group 17 order

A
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52
Q

F2

A

Pale yellow gas

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53
Q

Why does boiling point decrease down 1

A

distance of the delocalised electrons to the 1+ ion core within the metallic solid will increase as the ions get larger, causing a decrease in the metallic bond strength.

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54
Q

Iodine colour when displaced

A

Brown liquid

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55
Q

Bromine is more reactive than iodine. Bromine can…

A

OXIDISE an iodide ion because it REMOVES an electron

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56
Q

Trend in boiling points - 18

A

Low anyway - increases down group

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57
Q

Why do densities increase down group

A

increasing mass of the atoms.

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58
Q

Separating funnel use

A

to separate two immiscible liquid

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59
Q

Upper layer on separating funnel

A

Lower density

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60
Q

Purpose of narrowing walls on separating funnel

A

make it easier to close the tap the moment the last drop of the lower layer has passed through

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61
Q

Fractional distillation use

A

to separate miscible liquids (ones soluble in each other)

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62
Q

Why does the spot need to be above the solvent line in chromatography

A

so that it spreads up with the rising solvent rather than dissolves in the solvent at the bottom

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63
Q

Why lid on chromatography

A

ensure that the atmosphere in the tank has a saturated solvent vapour.

This prevents the solvent evaporating from the paper rather than rising.

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64
Q

What is centrifugation

A

used to separate heterogeneous mixtures based on their differences in particle mass

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65
Q

How does centrifugation work

A

If a liquid is mixed with a solid, the solid particles to settle to the bottom of a container as they are more dense than the liquid.

When the solid is small or finely divided, random motion and collisions of the particles causes them to settle much more slowly and in some cases they do not settle to the bottom.

Centrifugation encourages settling by spinning the mixture at high speed in a horizontal circle. As the mixture is spun, the heavier particles are brought to the end of the tube. The heaviest particles settle out first, becoming a pellet at the bottom of the tube.

The remaining liquid may be pure, a solution or still contain small solid particles. The remainder, called the supernatant may be decanted into a new tube and spun again at a higher speed to separate the smaller particles.

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66
Q

Remainder from centrifugation

A

supernatant

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67
Q

If the single solid component is wanted

A

decantation, filtration or centrifugation can be used.

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68
Q

Gas-gas mixtures can be separated by…

A

centrifugation or cyrogenic distillation.

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69
Q

Define acid

A

ability to donate H+ ions

70
Q

Salt definition

A

compound formed when the hydrogen ions in an acid are replaced by metal ions (or other cations)

71
Q

Reactions between metals and acids will only occur if…..

A

the metal is more reactive than hydrogen.

72
Q

Explain why silver sulfate cannot be prepared by adding silver metal to dilute sulfuric acid.

A

Silver is less reactive than hydrogen, so no reaction will take place under standard conditions.

73
Q

Weak acid

A

Carboxylic acid

74
Q

SO2(g) + H2O(l)

A

SO2(g) + H2O(l) → H2SO3(aq)

75
Q

2NO2(g) + H2O(l) →

A

2NO2(g) + H2O(l) → HNO3(aq) + HNO2(aq)

76
Q

Concentration 0.10

A

pH 1

77
Q

Concentration 0.01

A

pH 2

78
Q

Monoprotic acids

A

HCl, HNO3 and CH3COOH

  • only able to donate one acidic H+(aq) ion per acid molecule.
79
Q

HCl(aq) → (monoprotic)

A

HCl(aq) → H+(aq) + Cl−(aq)

80
Q

Diprotic

A

H2SO4(aq) → 2H+(aq) + SO42−(aq)

donate two acidic H+(aq) ions per acid molecule.

81
Q

Triprotic acid

A

H3PO4(aq) → 3H+(aq) + PO43−(aq)

can donate three acidic H+(aq) ions per acid molecule.

82
Q

Define base

A

can accept H+ ions, or one that has the ability to form OH−(aq) in solution.

83
Q

Weak base

A

Ammonia

84
Q

Strong base

A

sodium hydroxide and potassium hydroxide

85
Q

Cu(OH)2 is basic - why can’t form alkaline solutions

A

insoluble

86
Q

Neutralisation

A

Exothermic

87
Q

Why neutralisation is exothermic

A

there is no bond breaking (endothermic)

88
Q

Iodine clock

A

time taken for the starch indicator to form a blue-black colour with iodine, I2, is measured = proportional to the initial rate of reaction.

89
Q

10 degree increase

A

In many reactions, an increase in 10 °C will approximately double the rate of reaction as approximately twice as many particles will have sufficient energy to react.

90
Q

endothermic

A

melting of ice and
the boiling of water

91
Q

Bind energies only apply

A

When a gas

92
Q

Limitations of bond energies

A
  • average values
  • can only be done for reactions which take place entirely in the gaseous state.
93
Q

Assumptions in calorimetry - in aqueous solution

A
  • the density of solution is 1.00 g cm−3
  • SHC of solution is that of water
  • only the water has absorbed any heat and that the calorimeter does not absorb any energy
94
Q

Calorimeter material

A

Polystyrene = insulator = prevent heat loss to surroundings

95
Q

Calorimetry in combustion experiments

A

fuel is placed in a burner and when lit, the energy is used to heat water contained in a copper calorimeter.

96
Q

Calorimetry in combustion experiments - assumptions extra q

A

Incomplete combustion can be a problem

Heat loss to the surroundings is more likely in this open system

Heat is lost to the calorimeter = conductor

97
Q

Electron movement in electrolysis

A

from the positive electrode to the negative electrode.

98
Q

Fractional distillation crude oil

A
  • vaporised
  • passed into the bottom of a long column (a fractionating column) which is hot at the bottom and cool at the top
  • different component molecules of the vapour rise until they reach a point where the temperature is below their boiling point; here they condense, and the liquid is run off.
99
Q

Small hydrocarbons

A

Low boiling point
Very volatile
Flow easily
Ignite easily

100
Q

Large molecules

A

High boiling point
Not very volatile
Do not flow easily
Do not ignite easily

101
Q

Viscous meaning

A

do not flow easily

102
Q

Larger molecules

A

more viscous (do not flow easily) and are less flammable.

103
Q

Second stage of refining

A

catalytic cracking.

104
Q

catalytic cracking.

A

longer chain molecules are passed over a heated catalyst and are broken down into shorter chain molecules

Random

105
Q

two main types of condensation polymers

A

polyesters and polyamides.

106
Q

Ester forms from

A

carboxyl group of a carboxylic acid combines with a hydroxyl group of an alcohol

107
Q

Amide linkage

A

carboxyl group of a carboxylic acid combines with an amine group, -NH2.

108
Q

Proteins

A

formed from long chains of amino acids joined by amide linkages

109
Q

Biodegradable polymers

A

down (degrade) after their intended use to produce such natural products as: CO2, N2, H2O

often contain ester or amide linkages.

110
Q

Non-biodegradable polymers

A

not broken down after their intended use

tend to consist of long chains of carbon and hydrogen atoms
= strong bonds

111
Q

Na + water vs Na + alcohol 🍺

A

When sodium is added to water, the reaction is fast and vigorous

When sodium is added to ethanol the reaction is much slower and more moderate.

112
Q

Na + alcohol

A

2Na + 2C2H5OH → 2C2H5ONa + H2

113
Q

2Na + 2C2H5OH → 2C2H5ONa + H2 = products

A

Sodium ethoxide

114
Q

Sodium ethoxide

A

Strong alkali

115
Q

Carboxylic acids

A

monoprotic

116
Q

Reaction between carboxylic acid + alcohol 🥃

A

Reversible + water gone

117
Q

Carboxylic acid + alcohol conditions

A

Concentrated sulfuric acid catalyst

118
Q

Ester naming

A

first part of the name comes from the alcohol and the second part of the name is the salt of the carboxylic acid

119
Q

Metal reactivity

A

Most reactive - group 1 (only one electron needed to go)

Then 2 = process of losing 2 electrons requires more energy

3 = even more energy needed

Transition metals are the least reactive

120
Q

Iron

A

Fe2+ and Fe3+

121
Q

Reactivity metals

A
122
Q

Reactivity metals

A
123
Q

Positive Electrode (anode) = aqueous

A

If halide ions (Cl-, Br-, I-) and OH- are present then the halide ion is discharged at the anode, loses electrons and forms a halogen (chlorine, bromine or iodine)

If no halide ions are present, then OH- is discharged at the anode, loses electrons and forms oxygen

124
Q

Negative Electrode (cathode) - aqueous

A

If the metal is above hydrogen in the reactivity series, then hydrogen will be produced and bubbling will be seen at the cathode

This is because the more reactive ions will remain in solution, causing the least reactive ion to be discharged

125
Q

Extract metals

A

NEEDS TO BE REDUCED

126
Q

How to extract metal x with carbon

A

Metals below carbon can be extracted from their ores by reduction using carbon or carbon monoxide, such as iron from iron ore (haematite) in a blast furnace.

BECAUSE CARBON IS MORE REACTIVE + CAN DISPLACE

127
Q

When to use electrolysis to extract metal

A

When more reactive then carbon

128
Q

Displacement reactions of metals

A

occur when a more reactive metal is added to a dissolved compound of a less reactive metal

129
Q

Why does Mg + H2SO4 → MgSO4 + H2 happen but Cu + H2SO4 → no reaction happens

A

magnesium is above hydrogen in the reactivity serie = can displace

copper is below hydrogen in the reactivity series = can’t displace

130
Q

Aluminium

A

silvery-white, lightweight

soft and malleable

corrosion resistant and non-toxic,

Low density

Electrical conductor

cans, kitchen foil and utensils

131
Q

Iron pure

A

Soft

132
Q

High carbon steel

A

strong but brittle and is used in cutting tools and drill bits.

133
Q

Low carbon steel

A

softer and more easily shaped, and is used in car bodies.

134
Q

Where does steel come from

A

Impure iron is purified and then mixed with controlled amounts of carbon to produce steel which is strong, malleable (can be shaped) and ductile (can be drawn into wires)

135
Q

Copper

A
  • good conductor
  • ductile
  • malware
  • strong
  • unreactive
  • wires
  • cooking
136
Q

Silver

A

Best thermal / electrical conductor
- jewellery
- lustre
- antimicrobial

137
Q

Gold

A
  • soft
  • heavy metal
  • ductile
  • malleable
  • conductor
138
Q

Titanium

A

As strong as steel but less dense

  • aircraft
139
Q

desired properties for a hip replacement

A

high strength, low density, corrosion resistance and biocompatibility.

140
Q

How do the properties of transition metals differ from Group 1 elements?

A

Compared to Group 1 metals, transition metals have high melting points and boiling points. They are also strong, hard and unreactive. Transition metals often form coloured compounds and form ions of different charges that enable them to be used as catalysts.

141
Q

Hydrogen

A
  • burning splint = produces water = goes out with a squeaky pop
142
Q

Oxygen

A

Glowing splint / burning splint is blown out to leave red glowing embers

Splint relights

143
Q

Carbon dioxide

A

Calcium hydroxide to form calcium carbonate

144
Q

Chlorine

A

piece of damp blue litmus or indicator paper is held in the gas. Chlorine forms an acidic solution in water which turns the litmus red. Chlorine is also a bleach so the red and blue colours will then both fade to leave a white colour

145
Q

Sulfate

A

dilute nitric or hydrochloric acid to the unknown solution, followed by a solution of barium nitrate or chloride.

146
Q

Order

A

1) Test for the presence of carbonate ions using a dilute acid

2) Test for the presence of sulfate ions using HCl/BaCl2(aq)

3) Test for halide ions using HNO3/AgNO3(aq)

147
Q

Why is nichrome wire used

A

Inert / high b.p = do it melt or give visible colour of their own

148
Q

Lithium - flame test

A

Crimson red

149
Q

Sodium - flame test

A

Yellow - orange

150
Q

Potassium - flame test

A

Lilac

151
Q

Calcium - flame test

A

Red-orange

152
Q

Copper - flame test

A

Green

153
Q

Solubility of metals

A

Increases down group

154
Q

Mg 2+ sodium hydroxide precipitate test

A

White

155
Q

Ca 2+ sodium hydroxide precipitate test

A

White

156
Q

Al 3+ sodium hydroxide precipitate test

A

White

157
Q

Cu 2+ sodium hydroxide precipitate test

A

Blue

158
Q

Fe 2+ sodium hydroxide precipitate test

A

Green

159
Q

Fe 3+ sodium hydroxide precipitate test

A

Brown

160
Q

Aluminium hydroxide sodium hydroxide precipitate test

A

also a white precipitate but this precipitate will dissolve in an excess of sodium hydroxide to leave a colourless solution

161
Q

testing for Fe2+

A

green precipitate of Fe(OH)2 that initially forms will turn brown on standing as it oxidises in the air to form Fe(OH)3

162
Q

Test for water

A

using solid copper(II) sulfate

white when anhydrous but blue when hydrated

163
Q

Test for water equation

A

CuSO4(s) + 5H2O(l) → CuSO4·5H2O(s)

If excess water is added, the copper(II) sulfate will dissolve to form a blue solution, CuSO4(aq).

164
Q

Quantitative analysis of Sulfate

A

concentration of the sulfate ions can be found by adding an excess of barium chloride solution.

The precipitate can be filtered, dried and weighed.

The number of moles of barium sulfate can be determined from the mass of dry solid.

From the volume of solution tested, the concentration of sulfate ions can be found.

165
Q

Nitrogen

A

N2

166
Q

N2

A

78.1

167
Q

02

A

20.95

168
Q

Argon

A

0.9

169
Q

Carbon dioxide

A

0.04 - percentage in dry air

170
Q

How to separate silicon dioxide and water

A

Filtration - silicon dioxide can not mix with water because it’s a giant covalent

BMAT (4 decks)

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