Chem Flashcards

Question

buckminsterfullerene

Answer 1

2H+(aq) + CO32−(aq) → H2O(l) + CO2(g)

Answer 2

H+(aq) + NH3(aq) → NH4+(aq)

Answer 3

NA (a is subscript)

Answer 4

6.022 × 1023 mol−1

Answer 5

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

Answer 6

no more solute will dissolve at a given temperature.

Answer 7

gases become less soluble as temperature increases

Answer 8

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.

Answer 9

Gain of oxygen or LOSS OF HYDROGEN

Answer 10

oxygen atoms have an oxidation state of −1

Answer 11

oxygen atom has an oxidation state of +2.

Answer 12

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.

Answer 13

Very high melting and boiling points

Answer 14

all of the strong covalent bonds have to be broken

Answer 15

Soft + conducts electricity

Answer 16

stored in oil

Answer 17

Metal hydroxide + hydrogen

Answer 18

Soluble = makes solution alkaline

Answer 19

2K(s) + Cl2(g) → 2KCl(s)

Answer 20

Pale yellow gas

Answer 21

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.

Answer 22

Brown liquid

Answer 23

OXIDISE an iodide ion because it REMOVES an electron

Answer 24

Low anyway - increases down group

Answer 25

increasing mass of the atoms.

Answer 26

to separate two immiscible liquid

Answer 27

Lower density

Answer 28

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

Answer 29

to separate miscible liquids (ones soluble in each other)

Answer 30

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

Answer 31

ensure that the atmosphere in the tank has a saturated solvent vapour. This prevents the solvent evaporating from the paper rather than rising.

Answer 32

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

Answer 33

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.

Answer 34

supernatant

Answer 35

decantation, filtration or centrifugation can be used.

Answer 36

centrifugation or cyrogenic distillation.

Answer 37

ability to donate H+ ions

Answer 38

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

Answer 39

the metal is more reactive than hydrogen.

Answer 40

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

Answer 41

Carboxylic acid

Answer 42

SO2(g) + H2O(l) → H2SO3(aq)

Answer 43

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

Answer 44

HCl, HNO3 and CH3COOH - only able to donate one acidic H+(aq) ion per acid molecule.

Answer 45

HCl(aq) → H+(aq) + Cl−(aq)

Answer 46

H2SO4(aq) → 2H+(aq) + SO42−(aq) donate two acidic H+(aq) ions per acid molecule.

Answer 47

H3PO4(aq) → 3H+(aq) + PO43−(aq) can donate three acidic H+(aq) ions per acid molecule.

Answer 48

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

Answer 49

sodium hydroxide and potassium hydroxide

Answer 50

Exothermic

Answer 51

there is no bond breaking (endothermic)

Answer 52

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

Answer 53

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.

Answer 54

melting of ice and the boiling of water

Answer 55

When a gas

Answer 56

- average values - can only be done for reactions which take place entirely in the gaseous state.

Answer 57

- 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

Answer 58

Polystyrene = insulator = prevent heat loss to surroundings

Answer 59

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

Answer 60

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

Answer 61

from the positive electrode to the negative electrode.

Answer 62

- 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.

Answer 63

Low boiling point Very volatile Flow easily Ignite easily

Answer 64

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

Answer 65

do not flow easily

Answer 66

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

Answer 67

catalytic cracking.

Answer 68

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

Answer 69

polyesters and polyamides.

Answer 70

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

Answer 71

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

Answer 72

formed from long chains of amino acids joined by amide linkages

Answer 73

down (degrade) after their intended use to produce such natural products as: CO2, N2, H2O often contain ester or amide linkages.

Answer 74

not broken down after their intended use tend to consist of long chains of carbon and hydrogen atoms = strong bonds

Answer 75

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.

Answer 76

2Na + 2C2H5OH → 2C2H5ONa + H2

Answer 77

Sodium ethoxide

Answer 78

Strong alkali

Answer 79

monoprotic

Answer 80

Reversible + water gone

Answer 81

Concentrated sulfuric acid catalyst

Answer 82

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

Answer 83

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

Answer 84

Fe2+ and Fe3+

Answer 85

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

Answer 86

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

Answer 87

NEEDS TO BE REDUCED

Answer 88

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

Answer 89

When more reactive then carbon

Answer 90

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

Answer 91

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

Answer 92

silvery-white, lightweight soft and malleable corrosion resistant and non-toxic, Low density Electrical conductor cans, kitchen foil and utensils

Answer 93

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

Answer 94

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

Answer 95

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)

Answer 96

- good conductor - ductile - malware - strong - unreactive - wires - cooking

Answer 97

Best thermal / electrical conductor - jewellery - lustre - antimicrobial

Answer 98

- soft - heavy metal - ductile - malleable - conductor

Answer 99

As strong as steel but less dense - aircraft

Answer 100

high strength, low density, corrosion resistance and biocompatibility.

Answer 101

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.

Answer 102

- burning splint = produces water = goes out with a squeaky pop

Answer 103

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

Answer 104

Calcium hydroxide to form calcium carbonate

Answer 105

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

Answer 106

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

Answer 107

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)

Answer 108

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

Answer 109

Crimson red

Answer 110

Yellow - orange

Answer 111

Red-orange

Answer 112

Increases down group

Answer 113

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

Answer 114

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

Answer 115

using solid copper(II) sulfate white when anhydrous but blue when hydrated

Answer 116

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).

Answer 117

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.

Answer 118

0.04 - percentage in dry air

Answer 119

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

Chem Flashcards

(170 cards)