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Preliminary Chemistry
Metals
Lesson 1: History of Metals and Alloys
0466 342 939 [email protected] www.synergyhsc.com
Name: _____________________
LESSON 1: Metals Preliminary CHEMISTRY
Copyright © HSC Synergy Education 2015 2
Summary of Key Words
Account Account for: state reasons for, report on. Give an account of: narrate a series of events or transactions
Analyse Identify components and the relationship between them; draw out and relate implications
Apply Use, utilise, employ in a particular situation
Assess Make a judgement of value, quality, outcomes, results or size
Calculate Ascertain/determine from given facts, figures or information
Clarify Make clear or plain
Classify Arrange or include in classes/categories
Compare Show how things are similar or different
Construct Make; build; put together items or arguments
Contrast Show how things are different or opposite
Deduce Draw conclusions
Define State meaning and identify essential qualities
Demonstrate Show by example
Describe Provide characteristics and features
Discuss Identify issues and provide points for and/or against
Distinguish Recognise or note/indicate as being distinct or different from; to note differences between
LESSON 1: Metals Preliminary CHEMISTRY
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Evaluate Make a judgement based on criteria; determine the value of
Examine Inquire into
Explain Relate cause and effect; make the relationships between things evident; provide why and/or how
Extract Choose relevant and/or appropriate details
Extrapolate Infer from what is known
Identify Recognise and name
Interpret Draw meaning from
Investigate Plan, inquire into and draw conclusions about
Justify Support an argument or conclusion
Outline Sketch in general terms; indicate the main features of
Predict Suggest what may happen based on available information
Propose Put forward (for example a point of view, idea, argument, suggestion) for consideration or action
Recall Present remembered ideas, facts or experiences
Recommend Provide reasons in favour
LESSON 1: Metals Preliminary CHEMISTRY
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Lesson Dotpoints By the end of the lesson, you should understand the following concepts: History of metals x Outline and examine some uses of different metals through history, including
contemporary uses, as uncombined metals or as alloys x Analyse information to relate the chronology of the Bronze Age, the Iron Age
and the modern era and possible future developments x Identify why there are more metals available for people to use now than there
were 200 years ago Extracting Metals x Explain why energy input is necessary to extract a metal from its ore Producing Alloys x Describe the use of common alloys including steel, brass and solder and
explain how these relate to their properties
x Gather, process, analyse and present information from secondary sources on the range of alloys produced and the reasons for the production and use of these alloys
LESSON 1: Metals Preliminary CHEMISTRY
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1. The History of Metals
CHECKPOINT:
Metals Through History
x Gold was the earliest of the metals to be discovered (Stone age), and people
used it to make jewelry.
- Explain why the use of gold was limited.
x Copper was the first metal used to make tools and weapons as it was stronger
and harder then gold
x Outline and examine some uses of different metals through history, including contemporary uses, as uncombined metals or as alloys
x Analyse information to relate the chronology of the Bronze Age, the Iron Age and the modern era and possible future developments
x Identify why there are more metals available for people to use now than there were 200 years ago
LESSON 1: Metals Preliminary CHEMISTRY
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- Define annealing and explain why it was used on copper.
Smelting of Copper and other Metal Ores x Smelting is process where the ore is reduced through used a reducing agent
- For smelting copper the reducing agent was charcoal
- Explain how charcoal reduces copper on an atomic level.
The chemical equation for smelting copper is:
LESSON 1: Metals Preliminary CHEMISTRY
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Applications 1.1 Question 1 Name 2 early metals used by humans and assess the reason for their uses. (3 marks)
Question 2 Explain why smelting is a chemical process. (2 marks)
LESSON 1: Metals Preliminary CHEMISTRY
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The Bronze and Iron Age Bronze Age x Bronze is an alloy – a mixture of copper and tin x Discuss why bronze is more superior then copper in building weapons.
x Bronze with 10% tin had a melting point of 950℃
x Copper had a melting point of 1083℃ x Recasting and the shaping of bronze was easier then copper Iron Age
x During the middle ages the use of bronze declined as the technology for
producing iron became more efficient and cheaper
x How do we produce iron?
- 𝐹𝑒2𝑂3 (Hematite) can be reduced by carbon at temperatures above 1100℃
1. Carbon monoxide is produced by reacting charcoal with oxygen
𝟔𝑪(𝒔) + 𝟑𝑶𝟐(𝒈) → 𝟔𝑪𝑶(𝒈)
2. The carbon monoxide reacts with the hematite to form:
x Producing iron ore was common in 1200BC
x To produce the high temperatures required workers forced air into the kiln to
encourage more rapid burning and therefore a faster release of heat
LESSON 1: Metals Preliminary CHEMISTRY
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Applications 1.2 Question 1 Justify why bronze was more commonly used then copper to produce weapons. (2 marks)
Question 2 Discuss why Iron became the more favoured then bronze. (2 marks)
LESSON 1: Metals Preliminary CHEMISTRY
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Metals in the Last 200 Years x There are three main reasons why there are more metals were discovered in
the last 200 years then ever before:
Technology
- High temperature environments could be created to extract metals that couldn’t be previously extracted
- Decomposition through electrolysis was discovered by Sir Humphrey Davy
- Before 1800, the main method to produce relatively high temperatures was carbon heating but these temperatures are not enough to produce the metals of today
Metallurgy
- The improvement of metallurgical skills for making and testing new alloys led to the incorporation of a wider range of metals into everyday products
- Scientists began to experiment with different metals to determine the outputs if two metals were combined e.g Titanium
- Titanium was not widely used on it’s own as a metal but when it was discovered that when titanium is combined with limited amounts of other metals, it becomes extremely hard, has high-tensile strength and is very light, its use expanded rapidly.
- Titanium alloys became the back-bone of modern jet and aircrafts. With the
improvement of metallurgical skills to create new alloys, a wider range of metals are available
Costs - In the past it was relatively expensive to extract metals from their ores - An example of this can be seen with aluminium. The major cost in extracting
aluminium is the electricity used for the electrolysis and for keeping the electrolyte molten
- During the twentieth century the price of electricity fell steadily and this
improved the competitive position of aluminium relative to steel, so it became used more prominently
- Thus the reducing cost of extracting the metal is another reason why more
metals are available for people to use now.
LESSON 1: Metals Preliminary CHEMISTRY
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Question 1 (5 marks) Assess the reasons for why more metals were discovered in the last 200 years then in the last 2000 years. (5 marks) Student Answer:
LESSON 1: Metals Preliminary CHEMISTRY
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Sample Answer:
LESSON 1: Metals Preliminary CHEMISTRY
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2. Extracting Metal
CHECKPOINT:
Definitions
Define the following terms: - Ore
- Mineral
- Alloy
x There are three steps in extracting a metal from ore: 1. Identification of metal ore deposit
2. The metal ore is mined 3. The metal ore is processed in which the metal is separated from the ore
x Explain why energy input is necessary to extract a metal from its ore
LESSON 1: Metals Preliminary CHEMISTRY
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x What are two main methods of extracting metal from ore?
Properties of Metal
x Energy is required to break bonds and to understand how metal ores break
bonds we need to look at the chemical property of metals: - How many valency electrons do metals have?
- Why are some metals found in combined and uncombined forms?
- When do metals become positive ions?
LESSON 1: Metals Preliminary CHEMISTRY
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Applications 1.3 Question 1 Draw a labeled diagram of what happens to metals when energy is absorbed and released. Question 2 a) When metals are smelted is it an oxidisation or reduction reaction? (1 mark)
b) Do you lose or gain electrons during reduction? (2 marks)
c) How are metals reduced during smelting and is energy released or used?
(1 mark)
LESSON 1: Metals Preliminary CHEMISTRY
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3. Producing Alloys
CHECKPOINT:
Alloys x An alloy is a ________________________________ of a metal with __________ or more
elements
x List some examples of alloys
x Alloys are formed by mixing substances together through a process of melting
and cooling - Are solid alloys homogenous or heterogeneous mixtures?
x Describe the use of common alloys including steel, brass and solder and explain how these relate to their properties
x Gather, process, analyse and present information from secondary sources on the range of alloys produced and the reasons for the production and use of these alloys
LESSON 1: Metals Preliminary CHEMISTRY
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Physical Properties of Alloys x The above diagram shows different types of alloys. Determine how they relate
to the physical properties of alloys.
x The advantages of alloys over pure metals include:
1. Harder
2. Resist Higher Temperatures
3. Resists Corrosion
4. High Tensile Strengths
x A disadvantage is that alloys are more brittle then pure metal
LESSON 1: Metals Preliminary CHEMISTRY
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Uses of Alloys
x Fill in the rest of the table.
Alloy Composition (%)
Properties Uses
Structural
Steel
99.8% Fe
0.2% C
x Hard x High Tensile Strength
x Railways x Beams
Stainless Steel
10-20% Cr 5 – 20% Ni
70 – 80% Fe
x Hard x Resists Corrosion x Shiny
Brass
50 – 60% Cu 40 – 50% Zn
x Musical
Instruments x Decorations x Door Knobs
Bronze
80 – 90% Cu 10 – 20% Sn
x Ship propellers x Statues x Door frames
Solder
30 – 60% Sn 40 – 70% Pb
x Low melting point x Adheres to other
metals when in molten form
18 Carat
White Gold
75% Au
25% Platinum
x Jewellery
Copper –
Nickel Alloy
75% Cu 25% Ni
x Silvery appearance x Resists corrosion x Shiny
x From the above table it can be concluded that alloys are ‘designed’ and can be
made depending on its uses
LESSON 1: Metals Preliminary CHEMISTRY
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Applications 3.1 Question 1 Which of the following properties most directly affects the reactivity of a metal? a) Malleability b) Melting Point c) First Ionisation Energy d) Electrical Conductivity Question 2 Which of these is not an alloy? a) 18 Carat Gold b) Aluminium c) Steel d) Solder Question 3 (Exam Choice 2009 – Qu 9) Identify the correct statement about aluminium. a) Aluminium is a renewable resource because its ore, bauxite, is formed
continuously by natural geological processes b) Aluminium mining and extraction consumes very little energy, and hence
makes only a small contribution to the enhanced greenhouse effect c) One of the most important reasons for recycling aluminium is that it consumes
approximately 20% of the energy required to obtain it from its ore d) Aluminium production is sufficiently inexpensive that there is no demand for
more expensive recycled material Question 4 Compare the use of alloys and pure metals in relation to their properties. (3 marks)
LESSON 1: Metals Preliminary CHEMISTRY
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Question 5 Explain why steel is suitable in making railways. (2 marks)
Question 6 Describe the properties and uses of an alloy. (3 marks)
Question 7 (James Ruse Half Yearly 2002 – Qu 7) a) Write a balanced chemical equation showing the extraction of an ancient metal.
(1 mark)
b) Australia is the world’s third largest producer of lead. Huge smelters are located at Mt Isa, Q and Port Pirie, SA where lead is extracted from lead (II) sulfide. Identify an environmental problem associated with this process. (1 mark)
LESSON 1: Metals Preliminary CHEMISTRY
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c) Explain why energy input is necessary to extract a metal from its ore. (1 mark)
d) Alloys of lead are used in the plumbing and electronics industries. Identify a
property of lead alloys, which relates to their use. (1 mark)
e) Pure lead plates immersed in dilute sulfuric acid are used in car batteries to
make electricity. (Write a balanced chemical equation showing the reaction of lead with sulfuric acid. (1 mark)