When electrons in a metal ion absorb thermal energy during a flame test, what happens to their energy level?

They are promoted to higher energy levels

After excitation in a flame test, what do electrons do that results in light emission?

They fall back to lower energy levels

Why do different metal ions produce different flame colours?

Because photons of characteristic wavelengths are emitted when excited electrons return to lower energy levels, and different metals have different energy level spacings

Edexcel A-Level Chemistry 9CH0

Atomic Structure and the Periodic Table

Topic overview Protons, neutrons, electrons and isotopes Relative atomic mass and the mass spectrum Ionisation energy and the evidence for sub-shells Orbitals and electron configuration Periodicity across a period and down a group

Bonding and Structure

Topic overview Ionic bonding Covalent bonding, dative bonding and the shapes of molecules Electronegativity, polarity and intermolecular forces Structure and properties

Redox I

Topic overview Oxidation numbers Oxidation, reduction, disproportionation and half-equations

Inorganic Chemistry and the Periodic Table

Topic overview Flame tests and how they work Thermal decomposition of nitrates and carbonates Carrying out flame tests and testing the gases Group 2 elements and their compounds Trends in Group 7 and predicting fluorine and astatine Halogen displacement reactions Disproportionation and the reactions of chlorine Halides with concentrated sulfuric acid, and the hydrogen halides Testing for halide ions with silver nitrate Testing for carbonate and hydrogencarbonate ions Testing for sulfate and ammonium ions

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Organic Chemistry I

Topic overview Formulae, homologous series and functional groups IUPAC nomenclature Types of organic reaction and structural isomerism Stereoisomerism and E/Z nomenclature Practical techniques in organic chemistry Alkanes, crude oil and combustion pollutants Radical substitution Alkenes, the double bond and hydrogenation Electrophilic addition, Markovnikov's rule and the test for an alkene Addition polymers and waste polymers Nucleophilic substitution of halogenoalkanes Rates of hydrolysis and the SN1 and SN2 mechanisms Classifying and oxidising alcohols Alcohols: practical techniques and the core practicals

Modern Analytical Techniques I

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Acid-Base Equilibria

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Transition Metals

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Kinetics II

Topic overview Rate equations, orders and the rate constant Determining orders from experiments Rate-determining step and mechanisms Arrhenius equation and activation energy

Organic Chemistry II

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Organic Chemistry III

Topic overview The structure of benzene and the evidence for it Electrophilic substitution of benzene Nitration, halogenation, Friedel-Crafts and phenol Amines: structure and basicity Reactions of amines and preparing them Amides and condensation polymers Amino acids, zwitterions and proteins Empirical and molecular formulae from analytical data Grignard reagents and multi-step synthesis Purification techniques and the aspirin preparation

Modern Analytical Techniques II

Topic overview Carbon-13 and proton NMR Splitting, integration and the reference standard Chromatography High-resolution mass spectrometry

Inorganic Chemistry and the Periodic Table

Flame tests and how they work

2 things to know
Papers 1 and 3

Overview

How thermal energy promotes electrons in metal ions that emit light of characteristic wavelengths as they fall back, the flame colours of lithium, sodium, potassium, rubidium, caesium, calcium, strontium and barium compounds, and why magnesium compounds give no distinctive colour.

What you need to know

Answer each one before you reveal it.

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Key term

In a flame test, what is the initial energy source that causes electrons in metal ions to become excited?

Key term

Why is a flame test not useful for identifying magnesium compounds?

Questions from this subtopic

Each one with the model answer underneath.

1
In a flame test, what is the initial energy source that causes electrons in metal ions to become excited?
Model answer
Thermal energy from the flame
2
When electrons in a metal ion absorb thermal energy during a flame test, what happens to their energy level?
Model answer
They are promoted to higher energy levels
3
After excitation in a flame test, what do electrons do that results in light emission?
Model answer
They fall back to lower energy levels
4
Why do different metal ions produce different flame colours?
Model answer
Because photons of characteristic wavelengths are emitted when excited electrons return to lower energy levels, and different metals have different energy level spacings
5
What flame colour is produced by lithium compounds?
Model answer
Crimson/red
6
What flame colour is produced by sodium compounds?
Model answer
Yellow/orange

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Atomic Structure and the Periodic Table

Bonding and Structure

Redox I

Inorganic Chemistry and the Periodic Table

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AAtomisation turns each element into gaseous atoms.

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Flame tests and how they work

Overview

What you need to know

In a flame test, what is the initial energy source that causes electrons in metal ions to become excited?

Why is a flame test not useful for identifying magnesium compounds?

Questions from this subtopic

In a flame test, what is the initial energy source that causes electrons in metal ions to become excited?

When electrons in a metal ion absorb thermal energy during a flame test, what happens to their energy level?

After excitation in a flame test, what do electrons do that results in light emission?

Why do different metal ions produce different flame colours?

What flame colour is produced by lithium compounds?

What flame colour is produced by sodium compounds?

Other ways to work this

What is inside Levo

The 3-step method, run for you

Cram a whole paper in one sitting

Blank Blitz makes facts automatic

Build It gets the exam shape right

Test It catches misconceptions

Brain Breaks between sessions

Every question in Inorganic Chemistry and the Periodic Table, on a schedule.