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Question
reactivity series
use your knowledge of reactions to complete the table below to show the reactions of metals in different reactions.
metals: potassium, sodium, calcium, magnesium, zinc, iron, lead, copper, silver, gold
reaction with acids: observation, products
heated in air: observation, product
reaction with water: observation, product
(handwritten products: copper, iron, zinc, magnesium, sodium, potassium, calcium, gold visible in product columns)
To complete the "Reactivity Series" table, we analyze each metal's reactions based on the reactivity series (most reactive to least: Potassium > Sodium > Calcium > Magnesium > Zinc > Iron > Lead > Copper > Silver > Gold) and chemical properties:
1. Reaction with Acids
Metals above hydrogen in the reactivity series react with acids (e.g., HCl, H₂SO₄) to produce a salt and hydrogen gas (\( \text{H}_2 \)). Metals below hydrogen do not react.
| Metal | Observation | Products |
|---|---|---|
| Sodium | Violent reaction, gas bubbles | Sodium salt (\( \text{NaX} \)) + \( \text{H}_2 \) |
| Calcium | Vigorous reaction, gas bubbles | Calcium salt (\( \text{CaX}_2 \)) + \( \text{H}_2 \) |
| Magnesium | Moderate reaction, gas bubbles | Magnesium salt (\( \text{MgX}_2 \)) + \( \text{H}_2 \) |
| Zinc | Slow reaction, gas bubbles | Zinc salt (\( \text{ZnX}_2 \)) + \( \text{H}_2 \) |
| Iron | Very slow reaction (with dilute acid) | Iron(II) salt (\( \text{FeX}_2 \)) + \( \text{H}_2 \) |
| Lead | No reaction (or very slow with concentrated acid) | No reaction (or \( \text{PbX}_2 \) + \( \text{H}_2 \) with conc. acid) |
| Copper | No reaction (below H in reactivity) | No reaction |
| Silver | No reaction | No reaction |
| Gold | No reaction | No reaction |
2. Heated in Air (Combustion/Oxidation)
Metals react with \( \text{O}_2 \) to form metal oxides. Reactivity determines reaction vigor.
| Metal | Observation | Product |
|---|---|---|
| Sodium | Violent reaction, burns with yellow flame | \( \text{Na}_2\text{O} \) (or \( \text{Na}_2\text{O}_2 \) with excess \( \text{O}_2 \)) |
| Calcium | Vigorous reaction, burns with brick-red flame | \( \text{CaO} \) |
| Magnesium | Burns brightly with white flame | \( \text{MgO} \) |
| Zinc | Burns with blue-green flame (when heated strongly) | \( \text{ZnO} \) |
| Iron | Glows red, forms scale | \( \text{Fe}_2\text{O}_3 \) (rust) or \( \text{Fe}_3\text{O}_4 \) (with intense heat) |
| Lead | Forms yellow oxide when hot, white when cool | \( \text{PbO} \) (or \( \text{Pb}_3\text{O}_4 \) with strong heating) |
| Copper | Forms black coating | \( \text{CuO} \) |
| Silver | No reaction (or tarnishes to \( \text{Ag}_2\text{S} \) in air with \( \text{S} \), but \( \text{O}_2 \) alone: no reaction) | No reaction (or \( \text{Ag}_2\text{O} \) with strong heating) |
| Gold | No reaction | No reaction |
3. Reaction with Water
Metals react with water (or steam) to form metal hydroxides (or oxides) and \( \text{H}_2 \). Reactivity determines reaction type (cold water, hot water, steam).
| Metal | Observation | Product |
|---|---|---|
| Sodium | Violent reaction, melts, moves on water | \( \text{NaOH} \) + \( \text{H}_2 \) |
| Calcium | Vigorous reaction, gas bubbles | \( \text{Ca(OH)}_2 \) + \( \… |
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To complete the "Reactivity Series" table, we analyze each metal's reactions based on the reactivity series (most reactive to least: Potassium > Sodium > Calcium > Magnesium > Zinc > Iron > Lead > Copper > Silver > Gold) and chemical properties:
1. Reaction with Acids
Metals above hydrogen in the reactivity series react with acids (e.g., HCl, H₂SO₄) to produce a salt and hydrogen gas (\( \text{H}_2 \)). Metals below hydrogen do not react.
| Metal | Observation | Products |
|---|---|---|
| Sodium | Violent reaction, gas bubbles | Sodium salt (\( \text{NaX} \)) + \( \text{H}_2 \) |
| Calcium | Vigorous reaction, gas bubbles | Calcium salt (\( \text{CaX}_2 \)) + \( \text{H}_2 \) |
| Magnesium | Moderate reaction, gas bubbles | Magnesium salt (\( \text{MgX}_2 \)) + \( \text{H}_2 \) |
| Zinc | Slow reaction, gas bubbles | Zinc salt (\( \text{ZnX}_2 \)) + \( \text{H}_2 \) |
| Iron | Very slow reaction (with dilute acid) | Iron(II) salt (\( \text{FeX}_2 \)) + \( \text{H}_2 \) |
| Lead | No reaction (or very slow with concentrated acid) | No reaction (or \( \text{PbX}_2 \) + \( \text{H}_2 \) with conc. acid) |
| Copper | No reaction (below H in reactivity) | No reaction |
| Silver | No reaction | No reaction |
| Gold | No reaction | No reaction |
2. Heated in Air (Combustion/Oxidation)
Metals react with \( \text{O}_2 \) to form metal oxides. Reactivity determines reaction vigor.
| Metal | Observation | Product |
|---|---|---|
| Sodium | Violent reaction, burns with yellow flame | \( \text{Na}_2\text{O} \) (or \( \text{Na}_2\text{O}_2 \) with excess \( \text{O}_2 \)) |
| Calcium | Vigorous reaction, burns with brick-red flame | \( \text{CaO} \) |
| Magnesium | Burns brightly with white flame | \( \text{MgO} \) |
| Zinc | Burns with blue-green flame (when heated strongly) | \( \text{ZnO} \) |
| Iron | Glows red, forms scale | \( \text{Fe}_2\text{O}_3 \) (rust) or \( \text{Fe}_3\text{O}_4 \) (with intense heat) |
| Lead | Forms yellow oxide when hot, white when cool | \( \text{PbO} \) (or \( \text{Pb}_3\text{O}_4 \) with strong heating) |
| Copper | Forms black coating | \( \text{CuO} \) |
| Silver | No reaction (or tarnishes to \( \text{Ag}_2\text{S} \) in air with \( \text{S} \), but \( \text{O}_2 \) alone: no reaction) | No reaction (or \( \text{Ag}_2\text{O} \) with strong heating) |
| Gold | No reaction | No reaction |
3. Reaction with Water
Metals react with water (or steam) to form metal hydroxides (or oxides) and \( \text{H}_2 \). Reactivity determines reaction type (cold water, hot water, steam).
| Metal | Observation | Product |
|---|---|---|
| Sodium | Violent reaction, melts, moves on water | \( \text{NaOH} \) + \( \text{H}_2 \) |
| Calcium | Vigorous reaction, gas bubbles | \( \text{Ca(OH)}_2 \) + \( \text{H}_2 \) |
| Magnesium | No reaction with cold water; reacts with steam | \( \text{MgO} \) + \( \text{H}_2 \) (with steam) |
| Zinc | No reaction with cold/hot water; reacts with steam | \( \text{ZnO} \) + \( \text{H}_2 \) (with steam) |
| Iron | No reaction with cold/hot water; reacts with steam | \( \text{Fe}_3\text{O}_4 \) + \( \text{H}_2 \) (with steam) |
| Lead | No reaction with water/steam | No reaction |
| Copper | No reaction | No reaction |
| Silver | No reaction | No reaction |
| Gold | No reaction | No reaction |
Example Completion (Filling the Table):
For Potassium (Reaction with Acids):
- Observation: Violent bubbling, rapid gas release.
- Products: Potassium chloride (if acid is HCl) + \( \text{H}_2 \) → \( \text{KCl} + \text{H}_2 \).
For Copper (Heated in Air):
- Observation: Black coating forms on the metal.
- Product: Copper(II) oxide (\( \text{CuO} \)).
For Magnesium (Reaction with Water):
- Observation: No reaction with cold water; reacts with steam (requires heating).
- Product: Magnesium oxide (\( \text{MgO} \)) + \( \text{H}_2 \).
Use the reactivity series and chemical principles (metal + acid → salt + \( \text{H}_2 \); metal + \( \text{O}_2 \) → oxide; metal + \( \text{H}_2\text{O} \) → hydroxide/oxide + \( \text{H}_2 \)) to fill in observations and products for each metal.