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Thermal stability of nitrates and carbonates

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Thermal stability of nitrates and carbonates

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Explainer Video

Tutor: Alexander

Summary

Thermal stability of nitrates and carbonates

In a nutshell

The thermal stability of nitrates and carbonates increases as you go down Groups $1$ and $2$ . Thermal stability can be tested by producing gases and testing for them, $NO_2$ is tested for nitrates and $CO_2$ is produced from carbonates.

Thermal stability of nitrates and carbonates

Thermal stability is based on how much heat a substance can withstand before undergoing thermal decomposition. The higher the thermal stability the higher the temperature required to decompose the compound.

Thermal stability down a group

Thermal stability increases as you go down a group. Carbonates and nitrates are large negative ions (anions). They can be made unstable by the positive ions (cations). The greater the distortion the more this destabilises the anion.

Chemistry; Inorganic chemistry and the periodic table; KS5 Year 12; Thermal stability of nitrates and carbonates

The greater the charge on the cation the more this can destabilise the anion. As well as this the smaller the cation, the higher the charge density and the more this can distort the anion. Going down the group would mean a lower charge density and more thermal stability.

Group 2 are less thermally stable than Group 1

A higher charge density makes the anion more unstable. Group $2$ metals have a $2+$ charge compared to a $1+$ charge for Group $1$ metals which will cause more significant destabilisation. Group $2$ carbonates and nitrates are less thermally stable than Group $1$ .

Testing for thermal stability

Nitrate decomposition can be measured by...

How long it takes until a glowing split can be relit or how much brown gas $(NO_2)$ is produced. This must be done in a fume cupboard because $(NO_2)$ is toxic.

Example

Decomposition of Group $1$ and Group $2$ nitrates.

$2NaNO_3\ \rightarrow\ 2NaNO_2\ +\ O_2 \\2Ca(NO_3)_2\ \rightarrow \ 2CaO\ +\ 4NO_2\ +\ O_2$

Metals such as potassium and sodium, combust to form nitrite $(NO_2^-)$ salts. Metals such as; calcium, magnesium, aluminium, zinc, iron, lead and copper decompose to form a metal oxide and release $NO_2$ and $O_2$ gas.

Carbonate decomposition can be measured by...

Carbon dioxide is produced when carbonates are decomposed. This can be measured by testing with lime water (saturated $NaOH$ solution). A positive result is that the solution turns cloudy.

Example

Decomposition of Group $1$ and Group $2$ carbonates.

$K_2CO_3\ \rightarrow\ K_2O\ +\ CO_2 \\MgCO_3 \ \rightarrow\ MgO\ +\ CO_2$

Learn with Basics

Length:

Unit 1

The properties of metals

Unit 2

Group 1: properties and reactivity

Jump Ahead

Optional

Unit 3

Thermal stability of nitrates and carbonates

Final Test

Create an account to complete the exercises

FAQs - Frequently Asked Questions

What is an important factor in the thermal stability of an anion?

A lower charge density for a metal cation would increase the thermal stability of an anion.

How can you test for the decomposition of nitrates?

Metal nitrates thermally decompose and form nitrogen dioxide gas. This can be tested for by seeing how long it takes for a glowing splint to be relit.

How can you test for metal carbonates?

Thermal decomposition of metal carbonates produces carbon dioxide. Carbon dioxide can be bubbled through limewater (saturated NaOH solution) and this will turn the solution cloudy.

Home

Chemistry

Inorganic chemistry and the periodic table

Thermal stability of nitrates and carbonates

Videos

Summary

Exercises

Select Lesson

Exam Board

Select an option

Practical skills

The scientific method

How to plan experiments

Improving repeatability and reproducibility

Presenting results using tables and graphs

Analysing results: anomalies and correlation

Evaluating experiments

Modern analytical techniques II

NMR spectroscopy

Proton NMR spectroscopy

Chromatography

Combining analytical techniques

Organic chemistry III

Benzene: structure and combustion

Electrophilic substitution

Friedel-Crafts reactions

Phenols

Aliphatic and aromatic amines

Reactions of amines

Forming amides

Condensation polymers

Amino acids and zwitterions

Grignard reagents

Synthetic routes

Practical techniques

Percentage composition and combustion analysis

Organic chemistry II

Optical isomers and chirality

Aldehydes and ketones

Carboxylic acids: properties and reactions

Esters: formation, properties and uses

Acyl chlorides: formation and reactions

Kinetics II

Measuring rates of reaction

Determining reaction orders

The initial rates method

Rate equations and the rate constant

The rate determining step

Halogenoalkane reaction mechanisms

Activation energy and the Arrhenius equation

Transition metals

Transition metals: electron configuration and oxidation number

Complex ions: formation, shape and isomerism

Colours of inorganic ions and complexes

Chromium and its reactions

Ligand substitution reactions

Transition metals as catalysts

Redox II

Electrochemical cells and redox

Electrode potentials and calculations

The electrochemical series

Energy storage cells and hydrogen fuel cells

Redox titrations

Energetics II

Lattice enthalpies and Born-Haber cycles

Polarisation and the Pauling scale

Enthalpy change in solution

Entropy and calculating entropy change

Gibbs free energy change

Acid-base equilibria

Acids and bases

pH calculations

The ionic product of water

pH curves and indicators

Buffer solutions and calculations

Equilibrium II

The equilibrium constant

Partial pressure and gas equilibria

Le Chatelier's principle and equilibrium constants

Equilibrium I

Reversible reactions

Le Chatelier's principle

Kinetics I

Collision theory and rates of reaction

Calculating the rate of reaction

Catalysts and the Maxwell-Boltzmann distribution

Energetics I

Enthalpy changes and reaction profiles

Standard enthalpy changes

Hess's Law and enthalpy cycles

Calculating bond enthalpies

Modern analytical techniques I

Mass spectrometry

IR spectroscopy

Organic chemistry I

Basic concepts of organic chemistry

Organic reactions and mechanisms

Structural isomerism

Alkanes and free radical substitution

Fractional distillation of crude oil

Fuels: combustion and emissions

Alkenes: bonding and reactivity

Stereoisomerism

Reactions of alkenes

Addition polymerisation

Halogenoalkanes and their reactions

Alcohol: classification and reactions

Oxidation of alcohols

Organic techniques

Formulae, equations and amounts of substances

The mole and Avogadro's constant

Calculations involving gases

Empirical and molecular formulae

Balancing equations

Acid-base titrations

Calculating uncertainty and errors

Atom economy and percentage yield

Inorganic chemistry and the periodic table

Group 2: ionisation energy and properties

Thermal stability of nitrates and carbonates

Chemical properties of Group 7

Reactions with halogens

Halide ion reactions

Testing for ions

Redox I

Calculating oxidation numbers

Oxidation, reduction and redox reactions

Bonding and structure

Ionic bonding

Covalent bonding

Shapes of molecules

Giant covalent and metallic structures

Electronegativity and polarisation

Intermolecular forces: types and examples

Hydrogen bonding

Solubility

Predicting structures and properties

Atomic structure and the periodic table

The atom: history, structure and isotopes

Relative masses and mass spectrometry

Electronic structure: shells and orbitals

Atomic emission spectra

Ionisation energies

Ionisation energy trends

Periodicity

Explainer Video

Tutor: Alexander

Summary

Thermal stability of nitrates and carbonates

In a nutshell

Thermal stability of nitrates and carbonates

Thermal stability down a group

Group 2 are less thermally stable than Group 1

Testing for thermal stability

Nitrate decomposition can be measured by...

How long it takes until a glowing split can be relit or how much brown gas $(NO_2)$ is produced. This must be done in a fume cupboard because $(NO_2)$ is toxic.

Example

Decomposition of Group $1$ and Group $2$ nitrates.

$2NaNO_3\ \rightarrow\ 2NaNO_2\ +\ O_2 \\2Ca(NO_3)_2\ \rightarrow \ 2CaO\ +\ 4NO_2\ +\ O_2$

Carbonate decomposition can be measured by...

Carbon dioxide is produced when carbonates are decomposed. This can be measured by testing with lime water (saturated $NaOH$ solution). A positive result is that the solution turns cloudy.

Example

Decomposition of Group $1$ and Group $2$ carbonates.

$K_2CO_3\ \rightarrow\ K_2O\ +\ CO_2 \\MgCO_3 \ \rightarrow\ MgO\ +\ CO_2$

Learn with Basics

Length:

Unit 1

The properties of metals

Unit 2

Group 1: properties and reactivity

Jump Ahead

Optional

Unit 3

Thermal stability of nitrates and carbonates

Final Test

Create an account to complete the exercises

FAQs - Frequently Asked Questions

What is an important factor in the thermal stability of an anion?

A lower charge density for a metal cation would increase the thermal stability of an anion.

How can you test for the decomposition of nitrates?

Metal nitrates thermally decompose and form nitrogen dioxide gas. This can be tested for by seeing how long it takes for a glowing splint to be relit.

How can you test for metal carbonates?

Thermal decomposition of metal carbonates produces carbon dioxide. Carbon dioxide can be bubbled through limewater (saturated NaOH solution) and this will turn the solution cloudy.