2p9 metals and acids 121110
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This document discusses metals reacting with acids to form salts and hydrogen gas. The key points are: 1) Metals react with acids according to the general equation: Metal + Acid → Salt + Hydrogen. 2) Salts have the metal as the first name and acid as the last name, such as magnesium chloride from magnesium and hydrochloric acid. 3) Copper is less reactive than magnesium and zinc based on experiments showing these metals reacting with hydrochloric and sulfuric acids to form salts and hydrogen while copper did not react.
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1) Metals have high melting points and conduct heat and electricity well, whereas non-metals have lower melting points and do not conduct well. Metals are strong but can bend, while non-metals are usually brittle or snap.
2) When metals react with oxygen, they form metal oxides, such as magnesium reacting with oxygen to form magnesium oxide. Metals reacting with water form metal hydroxides or oxides along with hydrogen gas.
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3. Aluminum appears less reactive in the series due to the formation of a protective oxide layer. This layer prevents further reaction, unlike the soft oxide layers of less reactive metals.
Metals and non-metals.pptx CLAA 8 COLLINS
This chapter discusses the physical and chemical properties of metals and non-metals. It defines metals as hard, shiny, malleable and ductile materials, while non-metals are dull, brittle materials. The chapter describes the physical properties of metals and non-metals such as state, hardness, lustre, malleability, conductivity. It also discusses their chemical properties including reactions with oxygen, water, acids, and bases. Finally, it outlines some common uses of metals like in machinery and non-metals like oxygen in breathing and iodine as an antiseptic.
Single & double replacement reactions
1. The document discusses single and double replacement reactions, including the activity series of metals and halogens that can be used to predict products.
2. Single replacement reactions involve one element replacing another in a compound, following the activity series.
3. Double replacement reactions, also called metathesis reactions, involve two compounds exchanging ions when a new substance like water, gas, or precipitate is formed.
minerals
The document discusses minerals found in the Earth's crust, describing minerals as either natural elements or natural compounds. It provides examples of common elements like carbon and compounds like calcium carbonate that make up minerals. Properties of minerals like hardness and solubility in water are also examined, along with how heating can decompose some mineral compounds.
Metals and Non-metals revision.pptx
Metals and non-metals differ in their physical and chemical properties. Physically, metals are typically solid, hard, shiny, malleable and ductile with high melting and boiling points, while non-metals can be solid, liquid or gas with varying hardness, luster, malleability and melting/boiling points. Chemically, metals react with oxygen to form metal oxides, with water to form metal hydroxides and hydrogen gas, and with acids to form salts and hydrogen gas. Metals also displace less reactive metals in salt solutions. Non-metals gain electrons to form negative ions while metals lose electrons to form positive ions. Ionic bonds form when positive metal ions attract negative non-
Metalsandnonmetals 130623010725-phpapp02
Metals react with oxygen, water, and acids to form metal oxides, hydroxides, or salts. They lose electrons and become positively charged ions. Non-metals react with oxygen to form non-metal oxides, generally do not react with water or acids, and gain electrons to become negatively charged ions. Corrosion occurs as metals react with substances like oxygen and water, forming coatings like rust. Corrosion can be prevented by applying protective coatings like oil, paint, zinc plating, or by alloying metals.
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2p9 metals and acids 121110
- 1. Reactions of Metals and Acids 2P9: Friday 12th November
- 2. Homework review • Uses of metals in the home…
- 3. Review previous learning: hands up please! • Metals react with an acid to produce a chemical called a salt. Hydrogen gas is also produced in this reaction. • The general equation for a metal reacting with an acid is: Metal + Acid Salt + Hydrogen
- 4. Naming Salts Salts have a first name and a last name: First Name – comes from the metal Last Name – comes from the acid Acid name Salt produced Hydrochloric acid chloride Sulphuric acid sulphate Nitric acid nitrate
- 5. Examples of Salts From our experiments, the reactions which worked were: • Magnesium + Hydrochloric acid • Zinc + Hydrochloric acid • Magnesium + Sulphuric acid • Zinc + Sulphuric acid Magnesium Chloride + Hydrogen Zinc Sulphate + Hydrogen Magnesium Sulphate + Hydrogen Zinc Chloride + Hydrogen
- 6. Updating our reactivity series Copper metal did not react with either Hydrochloric acid or Sulphuric acid. Copper is therefore not as reactive as Magnesium or Zinc. We can add these metals to our reactivity series: Potassium Most reactive Sodium Calcium Magnesium Zinc Copper Least reactive
- 7. And now for more fun… • On your table is a reactivity series jigsaw… • In your groups come up with a mnemonic to remember the reactivity series: – Remember ROYGBIV (Richard of York gave battle in vain) to remember the colours of the rainbow – Potassium, Sodium, Calcium, Magnesium, Zinc, Copper
- 8. Remembering the reactivity series… • Please Potassium (K) • Send Sodium (Na) • Lions, Lithium (Li) • Cats, Calcium (Ca) • Monkeys, Magnesium (Mg) • And Aluminium (Al) • Zebras Zinc (Zn) • Into Iron (Fe) • Lovely Lead (Pb) • Hot Hydrogen (H) (non-metal) • Countries, Copper (Cu) • Signed Silver (Ag), • General Gold (Au) • Penguin. Platinum (Pt) Most reactive Least reactive
- 9. Next steps… • Next Wednesday you will be doing the Metal Displacement Experiment • Some metals are more reactive than others • A more reactive metal can displace a less reactive metal from a salt solution • When a displacement reaction occurs we see an chemical reaction taking place – Name three things we might see happening…
- 11. Review our learning: • How do we produce a salt? • Where does the first name of a salt come from? • Where does the last name of a salt come from? • Which salt will Hydrochloric acid produce? • Which acid would give a Sulphate salt?
Editor's Notes
- Literacy in science!