Changes in Matter. Introduction to Chemistry

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1 Changes in Matter Introduction to Chemistry

2 Classifying Matter Matter: is anything that has mass and volume. Volume: the amount of space that something takes up Property: a characteristic of a material that can be used in its identification e.g. colour,texture, state, density, boiling point, melting point etc.

3 Examples Give all properties you can think of for water Liquid Clear Boils at 100 C Freezes at 0 C Density is 1g/ml

4 All matter is composed of atoms. Atoms are the smallest complete building block of matter Atoms are composed of smaller particles called protons, neutrons, and electrons.

5 Inside the Atom.

6 Inside the Atom. neutral positive negative

7 Pure Substances A pure substance is something which is composed of only one type of particle Particle: an atom or molecule eg. copper wire, plastic

8 The Classification of Matter Elements: A pure substance that cannot be changed into anything simpler eg. gold, silver, oxygen

9 Elements When atoms of only one kind are grouped together you have an element. Elements are listed on the periodic table. There are just over 100 different elements in the universe.

10 Compounds. A pure substance that consists of two or more different types of atoms chemically bonded together to make one type of molecule The elements are in definite proportions and cannot be separated by physical means eg. Pure water or H 2 O Made of 2 hydrogen atoms and 1 oxygen atoms but the only molecule is H 2 O oxygen Hydrogen

11 Matter Mixture Pure Substance Compound two or more types of atoms but only one type of molecule e.g. H 2 O Element Only one type of atom e.g. Mg

12 Mixtures vs. Pure Substances Water is a compound and a pure substance. Kool Aid is a solution and a mixture. You can t change the properties of water like its taste or colour because it s only made up of one type of substance (H 2 O molecules). You can change the properties of Kool Aid. You can make it sweeter or lighter in colour because you can alter the amounts of each different type substance in it. E.g. more sugar, or more water etc. Not on your notes

13 Mixtures: Contain two or more pure substances Eg. salt dissolved in water Kool Aid is a mixture because it s made up of water molecules, sugar molecules, and food colouring molecules

14 Mixtures Variable combination of two or more pure substances. Heterogeneous Homogeneous Courtesy Christy Johannesson

15 Homogenous mixtures: Made up of substances that are evenly and microscopically mixed together These are called solutions (look like one thing). eg. Pop, chocolate milk

16 Mixtures Solution homogeneous very small particles no Tyndall effect Tyndall Effect particles don t settle EX: rubbing alcohol Courtesy Christy Johannesson

17 Mixtures - Solutions Solutions look like they re only made of one thing but Salt water (liquid Solution) made of salt molecules and water molecules Steel (Solid Solution) Made of iron atoms, nickel atoms, chromium atoms, carbon atoms Air (gas solution) made up of many different types of atoms and molecules such Oxygen, Carbon Dioxide and Nitrogen.

18 Component Symbol Volume Nitrogen N % Oxygen O % Argon Ar 0.9% Carbon Dioxide CO % 99.9% Composition of Air

19 Component Symbol Volume Nitrogen N % Oxygen O % Argon Ar 0.934% % Composition of Air Carbon Dioxide CO % Neon Ne 18.2 parts per million Helium He 5.2 parts per million Krypton Kr 1.1 parts per million Sulfur dioxide SO parts per million Methane CH parts per million Hydrogen H parts per million Nitrous Oxide N 2 O 0.5 parts per million Xenon Xe 0.09 parts per million Ozone O parts per million Nitrogen dioxide NO parts per million Iodine I parts per million Carbon monoxide CO trace Ammonia NH 3 trace

20 The Classification of Matter Heterogeneous Mixtures: A mixture that is not uniform in its composition A suspension is a liquid and solid that doesn t mix like flour and water A colloid are medium sized particles that don t settle like fog or milk. A mechanical mixture is a mixture of solids that can be seen. eg.salad

21 Mixtures Suspension heterogeneous large particles Tyndall effect particles settle EX: fresh-squeezed lemonade

22 Mixtures Colloid heterogeneous medium-sized particles Tyndall effect particles don t settle EX: milk

23 Matter Mixture Pure Substance Compound Element Atom A Atom B 1 kind of atom Mechanical Suspensions Solutions nuts n bolts salad flour and water Large particles air salt water Colloids Medium size particles

24 Physical and Chemical Changes In a physical change no new substances are formed Physical changes include changes of state. liquid to solid: Solidifying or Freezing solid to liquid: Melting liquid to gas: Evaporation or Boiling gas to liquid: Condensation gas to solid :Deposition solid to gas: Sublimation

25 gas condensing sublimation liquid evaporating deposition solid Changes of State

26 gas condensing sublimation solidifying / freezing liquid solid evaporating melting deposition Changes of State

27 Physical Change When a change of state occurs, molecules or atoms may move faster or slower, may spread out or clump together, but they do not change. i.e. An H 2 O molecule is still an H 2 O molecule!

28

29

30 Kinetic Molecular Theory 1) All matter is made up of tiny particles 2) Different substances have different particles 3) The particles are in constant motion 4) The more energy the particles have, the faster they move 5) The attraction between particles decreases with distance

31

32 Solids Particles are very close Particles are constantly vibrating in place Attraction between particles is high but decreases as vibration increases

33 Liquids Increase in energy from solids, increased amount of vibration Particles are still close together Particles can move freely within the container Attraction still quite high, but less than solids and decreasing with distance apart

34 Gases Increase in energy from liquids, increase in vibration & movement of particles Particle are very far apart Particles vibrate, rotate, bump into each other in a very rapid straight line motion

35 No attractive force between the particles, they are too far apart and moving too fast Increase in energy causes an increase in pressure Increase in speed and number of particles hitting the sides of containers

36 Chemical Change Chemical change results in a new substance being produced with different chemical and physical properties. In short, a chemical reaction takes place e.g. frying an egg

37 Chemical Change Physical changes can usually be reversed, whereas chemical changes cannot

38 Clues that a Chemical Reaction Might Have Occurred: Colour change Heat or light given off Odour given off Gas released Solid forming in a liquid Difficult to reverse

39 Identifying Chemical and Physical Change Physical Chemical Reversible Often Not usually New substance No Yes Properties Stay the same New Energy change May occur, but not noticeable May occur, often noticeable

40 Chemical Reactions A chemical change means that a chemical reaction has occurred. In a chemical reaction one or more substances (reactants) change to one or more new substances (products) Energy is either released OR absorbed in every chemical reaction

41 In a word equation, reactants are listed on the left and products on the right. They are separated by an arrow pointing to the right. H 2 + O 2 H 2 O reactants products The means reacts to form The + means and

42 Practice write the word equation Aluminum reacts with oxygen to form aluminum oxide. aluminum + oxygen aluminum oxide

43 Practice write the word equation In our bodies we use glucose and oxygen to produce carbon dioxide, water and ATP. glucose + oxygen carbon dioxide + water + ATP

44 Two Types of Chemical Reactions You Know About Corrosion: metal reacting with oxygen and water to form rust Combustion: is the burning of a substance (fuel) in the presence of oxygen. Products are carbon dioxide and water

45 In a chemical reaction atoms rearrange to form new substances. HCl + NaHCO 3 H 2 O + CO 2 + NaCl the total mass of the reactants is equal to the total mass of the products because no atoms are created or destroyed only rearranged! This is the Law of Conservation of Mass.

46 When the reaction involves gases it is difficult to prove that mass is conserved if you are using an open system because the gas can escape! A closed system (a sealed container) is needed to prove the Law of Conservation of Mass!

47 Endothermic vs Exothermic Reactions All reactions either give off energy or absorb energy. Endothermic reactions absorb energy and the surroundings can get cooler.

48 Exothermic reactions release energy the surroundings get warmer like in combustion and burning.

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