Metal and Non-metal Oxides. An oxide is a compound of oxygen and one or more other elements.

Slides:

Advertisements

Similar presentations

Types of Chemical Reactions Special Cases of Synthesis & Decomposition

Advertisements

1 Chemical Reactions & Periodicity In the next sections periodicity will be applied to the chemical reactions of hydrogen, oxygen, and their compounds.

Acids in the Atmosphere - Unit 4C Unit 4.C. 1 Acid Rain.

ACID RAIN. Do Now What does pH scale measure? What pH value is considered “neutral”? Which pH values are “acidic”? Which pH values are “basic” or “alkaline”?

Chemistry of Acid Rain How it relates to elements, compounds, and mixtures…

Some of the gases present in our atmosphere dissolve in rain water and cause it to become acidic. Here we will examine some of these.

Hall © 2005 Prentice Hall © 2005 General Chemistry 4 th edition, Hill, Petrucci, McCreary, Perry Chapter Four 1 Synthesis Reactions Type 1: A metal combines.

 Acid-Base Reactions A “Basic” Introduction. Acids  Ionize in aqueous solutions to form H + ions  Memorize the 7 strong acids (completely ionize, never.

Chemical Reactions: Reactants change chemical and physical properties …. to become new substances made from the same elements; these are called products.

Unit 9 Notes Acids, Bases, and Salts. Acids An acid is a substance that produces Hydrogen ion H + or hydronium H 3 O + in solution.

Case Studies of Scientific and Technological Issues Nature and Development of Science and Technology.

© Oxford University Press 2008 Many power stations burn coal containing sulfur. The sulfur reacts with oxygen and produces acidic sulfur oxides. 5.7 Acid.

Chapter 6: Neutralizing the Threat of Acid Rain Is normal rain acidic? Is acid rain worse in some parts of the country?

6.6 But acid rain can have pH levels lower than 4.3 – where is the extra acidity coming from? The most acidic rain falls in the eastern third of the United.

Periodic Properties of the Elements Equations associated with periodic trends © 2009, Prentice-Hall, Inc.

Copyright © Marshall Cavendish International (Singapore) Pte. Ltd. Acid Rain Acid rain is formed when acidic air pollutants such as sulphur dioxide.

Acid Deposition. pH Scale 7 is neutral As numbers decrease, acidity increases As numbers increase, alkalinity increases.

Form Group 3G 4th December 2006.

Quiz #1 Chemical Rxns and Safety 1.If you don’t know what to do in a lab, what should you do? 2.What is the correct way to write the formula for oxygen?

5.2 Salts Salts are ionic compounds formed when acids & bases react OR when oxides or carbonates react with acids OR when metals react with acids. Table.

(c) McGraw Hill Ryerson Salts Salts are ionic compounds formed when acids and bases react.  Salts are also produced when oxides or carbonates.

Section 4: Acids and Bases in Solution Objectives: describe the ions formed when acids and bases are dissolved in water describe the pH scale and tell.

Neutralization Reactions & Environment

Balancing chemical equations. WRITING CHEMICAL EQUATIONS Chemical equations should show : (a) formulas of the reactants & products (b) their states of.

Converting Hydrogen Ion Concentrations to pH Practice Problems.

Introduction to Acids and Bases. Acid A substance that produces hydrogen ions, H + (aq), when it dissolves in water. Sour-tasting and good conductors.

PH & Acid Rain. What is an Acid? An acid is a substance which, when dissolved in water, releases protons. ([H + ] ions) The amount of protons ([H +

Adapted from “The Ultimate Chemical Equation Handbook, 2 nd Edition”

5.1 T HE C OMBUSTION OF H YDROCARBONS pp

CCBAB Compound ABCompound CD AD Compound ADCompound CB D ++ Magnesium Chloride MgCl 2 Calcium Hydroxide Ca(OH) 2 Magnesium Hydroxide Mg(OH) 2 Calcium Chloride.

Acids/Bases/ & Acid Rain

Chapter 5 Compounds are classified in different ways

Types of Reactions Chapter 10. There are 5 Types of Reactions: 1. Synthesis 2. Decomposition 3. Single Displacement (replacement) 4. Double Displacement.

Chapter 6: Neutralizing the Threat of Acid Rain Is normal rain acidic? Is acid rain worse in some parts of the country? Is there a way to “neutralize”

Chapter 9 Acid Rain.

What are Acids? An acid is any compound that yields hydrogen ions (H + ) or hydronium ions (H 3 O + ) when dissolved in water. Hydronium ions are really.

Acid Rain. Educational Objectives To understand how the pH level of an environment affects living organisms. To understand the relationship between the.

Chemical Reactions: Chapter 9 Reactants change chemical and physical properties …. to become new substances made from the same elements; these are called.

E2 acid deposition State what is meant by the term acid deposition and outline its origins. Discuss the environmental effects of acid deposition and possible.

Chemical Reactions SCH 3U Unit 2 Part 3. Classifying Reactions Most chemical reactions can be grouped or organized into 5 categories. Synthesis Decomposition.

What are they???. What are they? Acids and bases are very common. Many familiar compounds are acids or bases. Acids are Sour, Bases are Bitter Classification.

Title: Lesson 13: Acid Deposition

ACID RAIN BY DYLON GOOKIN AND TODD RAMSEY

Acids, Bases, and Salts Get to know them!. Facts about Acids and Bases An acid is a substance that produces Hydrogen Ions ( H + ). A bases is a substance.

Acid Precipitation – A Global Concern Sulfur, nitrogen and carbon oxides emitted from industries (such as smelters) combine with water vapor in the air.

Acid and Bases Oxides Many acids and bases are formed by dissolving oxides in water.

Acid Deposition. process by which acid-forming pollutants are deposited on Earth’s surface by… – wet- rain, snow, fog – dry- smoke or dust particles impacts.

How to predict a Product. Synthesis Acid anhydride + water  acid Base anhydride + water  base Nonmetallic oxide is acid anhydride Metallic oxide is.

Acids and Bases. Have you ever wondered, “Why do foods taste sour or bitter?”

Acid Deposition. process by which acid-forming pollutants are deposited on Earth’s surface by… – wet- rain, snow, fog – dry- smoke or dust particles impacts.

(c) McGraw Hill Ryerson Acids and Bases Many familiar compounds are _______________________.  Classification as acids or bases is based on chemical.

5.2 - Salts Salts are a class of ionic compounds formed when:  acids and bases react  oxides or carbonates react with acids  metals react with acids.

The Chemistry of Acids and Bases

WJEC GCSE The ever-changing Earth

2-6 Acids/Base Chemistry

15.2 NOTES Acid Rain and Concentration

5.2-Salts, Metal Oxides, Non-Metal Oxides

CHEMICAL WEATHERING.

Introduction to Acids and Bases.

Acid Precipitation.

Acid Precipitation.

Chemical Weathering.

CWK CWK Acid Rain State the adverse effect of these common pollutants on buildings and why these pollutants are of global concern Relate the effects.

Acid Precipitation.

Acids and Bases.

Acids and Bases.

Acid Rain Menu A. What is Acid Rain? B. What Causes Acid Rain?

Synthesis Reactions!.

Presentation transcript:

Metal and Non-metal Oxides

An oxide is a compound of oxygen and one or more other elements.

Examples of oxides are carbon dioxide, CO 2,

An oxide is a compound of oxygen and one or more other elements. Examples of oxides are carbon dioxide, CO 2, sulfur trioxide, SO 3,

An oxide is a compound of oxygen and one or more other elements. Examples of oxides are carbon dioxide, CO 2, sulfur trioxide, SO 3, and sodium oxide, Na 2 O.

In Science 10, you are given this Periodic Table: METALSNON-METALS

An oxide formed by a metal and oxygen is called a metal oxide.

Some examples are:

An oxide formed by a metal and oxygen is called a metal oxide. Some examples are: Li 2 O

An oxide formed by a metal and oxygen is called a metal oxide. Some examples are: Li 2 O MgO

An oxide formed by a metal and oxygen is called a metal oxide. Some examples are: Li 2 O MgO CaO

An oxide formed by a non-metal and oxygen is called a non-metal oxide.

Some examples are:

An oxide formed by a non-metal and oxygen is called a non-metal oxide. Some examples are: CO 2

An oxide formed by a non-metal and oxygen is called a non-metal oxide. Some examples are: CO 2 NO 2

An oxide formed by a non-metal and oxygen is called a non-metal oxide. Some examples are: CO 2 NO 2 Cl 2 O

Metal oxides, and non-metal oxides have quite different properties.

One very important difference is what they produce when they are dissolved in water.

Metal oxides dissolve in water to form BASIC solutions.

Non-metal oxides dissolve in water to form ACIDIC solutions.

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l) 

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l)  2NaOH (aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l)  2NaOH (aq) sodium hydroxide

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l)  2NaOH (aq) sodium hydroxide (a base)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l) 

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq) magnesium hydroxide

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq) magnesium hydroxide (a base)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l) 

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Carbonic acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 2(g) + H 2 O (l) 

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 2(g) + H 2 O (l)  H 2 SO 3(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Sulfurous acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 3(g) + H 2 O (l) 

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 3(g) + H 2 O (l)  H 2 SO 4(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 3(g) + H 2 O (l)  H 2 SO 4(aq) Sulfuric acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l) 

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) Nitrous acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq) Nitric acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq) Nitric acid Nitrous Acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2HOCl (aq)

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2HOCl (aq) Hypochlorous Acid

Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2HOCl (aq)

Non-metal oxides dissolve in water to form ACIDIC solutions.

Acid Precipitation Non-metal oxides dissolve in water to form ACIDIC solutions.

CO 2(g) Naturally occurs in Earth’s atmosphere

Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq)

Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Carbonic acid

Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Carbonic acid A weak acid

Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Natural rainwater has a pH of about 5.6

Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Natural rainwater has a pH of about 5.6

Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Natural rainwater has a pH of about 5.6 Rainwater with a pH of 5.6 and above is NOT called Acid Rain

Natural rainwater has a pH of about 5.6 Rainwater is a pH lower than 5.6 is called Acid Rain Non-metal oxides dissolve in water to form ACIDIC solutions.

Thermal power generating plants burn large amounts of coal.

Non-metal oxides dissolve in water to form ACIDIC solutions. Thermal power generating plants burn large amounts of coal. Coal and other fossil fuels contain small amounts of sulfur.

S (s) + O 2(g) 

S (s) + O 2(g)  SO 2(g)

SO 2 is a non-metal oxide S (s) + O 2(g)  SO 2(g)

SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Sulfurous acid

S (s) + O 2(g)  SO 2(g) SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Dissolved sulfurous acid causes Acid Precipitation

SO 2(g) + H 2 O (l)  H 2 SO 3(aq) SO 3(g) + H 2 O (l)  H 2 SO 4(aq) Many industrial processes release SO 2 and SO 3 into the atmosphere

SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Aqueous sulfurous acid and sulfuric acid cause Acid Precipitation SO 3(g) + H 2 O (l)  H 2 SO 4(aq)

Non-metal oxides dissolve in water to form ACIDIC solutions. Vehicle exhaust releases nitrogen oxides like NO 2 to the atomosphere.

2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq) Nitric acid Nitrous Acid

Acid precipitation can have serious effects on freshwater organisms, crops, and forests.

Acid precipitation can also damage buildings and statues made of limestone or marble.

Limestone and marble are made up of calcium carbonate, CaCO 3(s).

Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs:

CaCO 3(s) + H 2 SO 4(aq) 

Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s)

Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s) + H 2 O (l)

Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s) + H 2 O (l) + CO 2(g)

Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s) + H 2 O (l) + CO 2(g) This slowly dissolves the CaCO 3 which makes up limestone or marble.