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Chemistry > Experimental techniques and Stoichiometry > Flashcards

Experimental techniques and Stoichiometry Flashcards

1
Q

How will oxygen be represented as if there are 3 elements in a compound and one of them is oxygen

A

compound name will end in ate or ide

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2
Q

Order of two elements in compound

A

element further to left on periodic table comes first in name

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3
Q

How will the compound end if there are only 2 elements

A

second element will end in -ide

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4
Q

Exception to rules (Hydroxide) (2)

A

hydroxide usually exists as a compound with 3 elements

however it ends with -ide

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5
Q

Exception to rules (Ammonium) (2)

A

Ammonium exists as a compound with 3 elements

however it ends with -ide

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6
Q

Cations and Anions order in compound name (2)

A

cations come first

anions come second

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7
Q

How does a prefix help in a chemical formula

A

prefix helps to show the number of atoms for an element

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8
Q

Prefix for one

A

mono

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9
Q

prefix for 2

A

di

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10
Q

prefix for 3

A

tri

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11
Q

prefix for 4

A

tetra

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12
Q

prefix for 5

A

penta

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13
Q

prefix for 6

A

hexa

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14
Q

When is valency method used

A

when compound has no prefix

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15
Q

What does a roman numeral signify of an element

A

the valency of the element

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16
Q

When is radical method used

A

when compound has more than 2 elements

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17
Q

What is a radical (2)

A

group of elements bonded together

exist as ions

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18
Q

Name the radicals (7)

A

Hydroxide

Hydrogen Carbonate

Nitrate

Ammonium

Carbonate

Sulfate

Phosphate

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19
Q

What is the overall charge of an ion

A

0

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20
Q

Hydroxide radical

A

OH -

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21
Q

Hydrogen carbonate radical

A

HCO - 3

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22
Q

Nitrate radical

A

NO - 3

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23
Q

Ammonium radical

A

NH + 4

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24
Q

Carbonate radical

A

CO 2- 3

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25
Q

Sulfate radical

A

SO 2- 4

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26
Q

Phosphate radical

A

PO 3- 4

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27
Q

Purpose of word equations

A

represent what happened during chemical reaction

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28
Q

Definition of reactants

A

chemicals at the start of the reaction

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29
Q

Definition of products

A

new substances formed during reaction

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30
Q

Order of word equations (3)

A

reactants start

products end

seperated by arrow

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31
Q

Define a chemical equation

A

names of chemicals within word equations replaced with chemical formulae

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32
Q

Name the Diatomic elements (7)

A

Hydrogen

Nitrogen

Fluorine

Oxygen

Iodine

Chlorine

Bromine

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33
Q

State symbol for solid

A

s

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34
Q

State symbol for liquid

A

l

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35
Q

State symbol for gas

A

g

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36
Q

State symbol for solution (aqueous)

A

aq

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37
Q

Why are chemical equations balanced

A

law of conservation of mass - mass cannot be created or destroyed

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38
Q

Define Ionic equations

A

Equations which show reactions involving ions

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39
Q

Define spectator ions (2)

A

ions present in reaction but don’t take part

appear unchanged on both sides of chemical equation

40
Q

Unit given to mass of atom (3)

A

called atomic mass unit

symbol : u

can also be called Dalton (Da)

41
Q

Define relative atomic mass (3)

A

measured in relation to carbon-12 atom : because carbon-12 mass is exactly 12

mass number on periodic table

average mass of naturally occurring isotopes of element

42
Q

Define relative molecular mass

A

overall mass of compound

43
Q

Purpose of percentage of mass calculations

A

determine percentage of certain element in compound

44
Q

Percentage by mass formula

A

m/Mr x 100

45
Q

Define the independent variable (4)

A

variable deliberately changed during investigation

is cause

is on x-axis

is on left column for table

46
Q

Define the dependent variable (4)

A

variable measured during investigation

is effect

is on y-axis

is on right column of table

47
Q

Define a control variable

A

factors controlled during investigation

48
Q

Define a fair investigation

A

investigation in which only one variable is changed (independent variable)

49
Q

Measuring cylinder function

A

measure volume of liquid to be used in reaction

50
Q

Pipette function

A

transfers volume of liquid from one vessel to another

51
Q

Burettes function (4)

A

used in titration reactions

allow volumes of liquid to be added to another

addition of liquid controlled by tap

scientist able to measure how much liquid needed in reaction

52
Q

Define precise results

A

set of results close to each other

53
Q

Define accurate results

A

results close to actual value

54
Q

How does filtration work (2)

A

insoluble solid get stuck in filter paper

liquid easily passes through

55
Q

Filtration function

A

separates insoluble solid from solution

56
Q

Define residue

A

insoluble solid left after filtration

57
Q

Define filtrate

A

liquid seperated

58
Q

Function of evaporation (2)

A

separates soluble solid from liquid

liquid evaporated to leave soluble solid behind

59
Q

Define a pure substance

A

substance having only one type of particle

60
Q

Define an impure substance

A

substance which has more than one type of particle

61
Q

Melting/boiling point for a pure substance (2)

A

sharp melting/boiling point

set temperature at which IMFs break (as they are all the same)

62
Q

What is the melting/boiling point for an impure substance (2)

A

differing melting/boiling point

separate components melt at different temperatures

63
Q

Pure substance molecular structure

A

specific arrangement of atoms/molecules

64
Q

Impure substance molecular structure (2)

A

contains more than one type of particle

original arrangement of pure substance altered

65
Q

Impure solid melting and boiling point compared to pure solid

A

impure solids will have a lower melting point

66
Q

What happens during melting of a pure substance (3)

A

particles arranged in regular pattern held together by intermolecular forces

intermolecular forces begin to break as substance begins to melt

molecules aren’t held as tightly as before which disorders arrangement of atoms

67
Q

What happens during melting of an impure substance (3)

A

substance begins to melt before melting point reached

other substances get in between original substance, breaking intermolecular forces

substance begins turning into a liquid as intermolecular forces begin to break

68
Q

Why is purity important (2)

A

important for food and pharmaceutical industries

impurities can be harmful and need to be checked

69
Q

Define crystals

A

small, regularly shaped solids which reflect light

70
Q

Examples of crystals (2)

A

salt

copper sulfate

71
Q

Are crystals usually soluble

A

yes

72
Q

Function of crystallisation

A

allows pure crystals of solid to be obtained from solution

73
Q

How does crystallisation work (3)

A

crystals form when temperature of solution decreases

as a result, solid particles have less space in the liquid

solid particles are pushed out of solution and grow as crystals

74
Q

Function of distillation (3)

A

separate liquid from soluble solid

obtain liquid solvent

separates mixture of liquids with different boiling points (however temperature difference between mixtures must be 50 degrees C or above)

75
Q

How distillation works (3)

A

solvent boils in solution, turning into a gas

travels into condenser where it meets cool atmosphere and condenses into liquid

solute remains in flask while solvent collected as distillate

76
Q

Purpose of fractional distillation (2)

A

separate more complex liquid mixtures

used when difference in boiling point of separate components is roughly 25 degrees C

77
Q

How fractional distillation works (5)

A

same set up with distillation

components of mixture have similar boiling points and vaporise at same time

components travel up flask and meet cool glass beads

glass beads condense liquid with higher boiling point and cause it to drop back in round bottom flask

liquid with lower boiling point travels along condenser

78
Q

Where is fractional distillation used (2)

A

crude oil industry to separate crude oil

separated into petrol, diesel and kerosene

79
Q

Chromatography purpose

A

used to separate small quantities of substance from a solution

80
Q

Define stationary phase in chromatography (2)

A

part that doesn’t move

e.g filter paper

81
Q

Define the mobile phase in chromatography (2)

A

part that moves

e.g solvent which moves spots up paper

82
Q

Setting up chromatography procedure (4)

A

solvent used must start below baseline - otherwise spots travel into solvent

baseline done in pencil

paper sits vertically and is upright by a wooden splint

spots travel up stationary phase at different rates causing them to separate

83
Q

What is responsible for how far spots travel (2)

A

mass of spots - smaller mass greater distance

solubility of spots - more solubility greater distance

84
Q

Purpose of Rf values (2)

A

substances have unique Rf values

known Rf values compared to unknown Rf value to find substance

85
Q

Rf formula

A

distance moved by spot from baseline/distance moved by solvent front from baseline

86
Q

Conditions for keeping Rf values the same (3)

A

same type of chromatography

same conditions

same solvent used

87
Q

Purpose of paper chromatography (2)

A

used to test for impurities in substance

impure substance has more spots than expected

88
Q

What does 0K equal to in degrees celsius

A

-273 degrees celsius

89
Q

What does 1 L equal to in decimetres cubed

A

1

90
Q

What does 1 L equal to in cm cubed

A

1000

91
Q

SI measurement for mass

A

kilogram

92
Q

SI measurement for length

A

metre

93
Q

SI measurement for time

A

second

94
Q

SI measurement for amount of substance

A

mole (mol)

95
Q

SI measurement for electric current

A

ampere (A)

96
Q

SI measurement for temperature

A

kelvin (K)

Chemistry (3 decks)

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