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Chapter 1 – Matter and Change Taken from Modern Chemistry written by Davis, Metcalfe, Williams & Castka.

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Presentation on theme: "Chapter 1 – Matter and Change Taken from Modern Chemistry written by Davis, Metcalfe, Williams & Castka."— Presentation transcript:

1 Chapter 1 – Matter and Change Taken from Modern Chemistry written by Davis, Metcalfe, Williams & Castka

2 Chemistry is a Physical Science – Define chemistry – List examples of the branches of chemistry – Compare and Contrast Basic research Applied research Technological development Section 1 - Objectives

3 Section 1-1 Chemistry is the study of the composition, structure, and properties of matter and the changes it undergoes. What is it made of? Makeup and internal arrangement? What happens when we heat? cool? Mix with other materials? Why does this behavior occur?

4 Section 1-1 (continued) Six main Branches of Chemistry Organic – deals with carbon containing compounds Inorganic – study of substances not classified as organic, mainly those that don’t contain carbon Physical – study of properties, changes and relationship between energy and matter Analytical – identification of components and composition of materials Biochemistry – study of substances and processes occurring in living things Theoretical – using math and computers to design and predict the properties of new compounds

5 Section 1-1 (continued) A Chemical is any substance that has a definite composition.

6 Section 1-1 (continued) Basic Research - carried out for the sake of increasing knowledge (ex. Teflon, sticky notes) Technological developments – production of products to improve our lives (ex biodegradable material) Applied research – is carried out to solve problems (ex ozone depletion) The 3 often overlap – understanding of crystals and basic light allowed lazers to be created which lead to fiber optics

7 Matter and Its Properties – Distinguish between the physical properties and chemical properties of matter. – Classify changes of matter as physical or chemical. – Explain the... states in terms of particles Gas Liquid Solid – Distinguish between a mixture and a pure substance Section 2 - Objectives

8 Section 1-2 M & M Mass is a measure of the amount of matter. Measured in Kg, g and for the less educated ☺ in lbs and ozs. So...Matter is anything that has mass and takes up space.

9 Section 1-2 (continued) An Atom is the smallest unit of an element that maintains the properties of that element. and...an element is a pure substance made of one only kind of atom. and...a compound is a substance that is made from the atoms of two or more elements that are chemically bonded. Basic Building Blocks of Matter

10 Section 1-2 (continued) An molecule is the smallest unit of an element or compound that retains the properties of that element or compound. Basic Building Blocks of Matter (continued) EXAMPLES O2O2 H2OH2O

11 Section 1-2 (continued) Extensive properties depend on the amount of matter present – Volume – Mass – Amount of Energy Properties and Changes in Matter Intensive properties do not depend on the amount of matter present – Melting pt. – Boiling pt. – Density – Ability to conduct: – Heat – Electricity

12 Section 1-2 (continued) Physical Properties and Physical Changes Physical property is a characteristic that can be observed without changing the identity of the substance – Melting pt. – Boiling pt. A change in a substance that does not involve a change in the identity of the substance is called a physical change – Grinding – Cutting – Melting & Boiling

13 Section 1-2 (continued) Physical Properties and Physical Changes (continued) Change of state is a physical change of a substance from one state to another. Solid has definite volume and definite shapeLiquid has definite volume but an indefinite stateGas has neither a definite volume or a definite shape

14 Section 1-2 (continued) Chemical Properties and Chemical Changes A Chemical property relates to a substances ability to undergo changes that transform it into different substances. – Ability to burn in air – Iron rusting by combining with the oxygen in air A change in which one or more substances are converted into different substances is called a chemical change.

15 Section 1-2 (continued) Chemical Properties and Chemical Changes (continued) Carbon plus oxygen yields (or forms) carbon-dioxide Carbon + oxygen  carbon-dioxide C + O 2  CO 2 The substances that react in a chemical change are called the reactants. The substances that are formed in a chemical change are called the products.

16 Section 1-2 (continued) Chemical Properties and Chemical Changes (continued) Chemical changes and reactions, such as combustion and decomposition, form products whose properties differ greatly from those of the reactants. However, chemical changes do not affect the total amount of matter present before and after a reaction. The amount of matter, and therefore the total mass, remains the same.

17 Section 1-2 (continued) Energy and Changes in Matter When physical or chemical changes occur, energy is almost always involved. The energy can take several different forms, such as heat or light. Although energy can be absorbed or released in a change, it is not created or destroyed. It simply assumes a different form.

18 Section 1-2 (continued) Classification of Matter - Mixture A mixture is a blend of two or more kinds of matter, each of which retains its own identity and properties. A mixture that is uniform in composition they are said to be homogeneous Examples salt-water solutions A mixture that is not uniform in composition is said to be heterogeneous Examples clay & water

19 Section 1-2 (continued) Classification of Matter – Pure substances A pure substance has a fixed composition and differ from a mixture in the following ways: 1.Every sample of a pure substance has exactly the same characteristic properties. 2.Every sample of a given pure substance has exactly the same composition.

20 Section 1-2 (continued) Classification of Matter – Laboratory Chemicals and Purity Chemicals in laboratories are generally treated as if they are pure. However all chemicals have some impurities. Purity ranking depends on the needs of the users.

21 Elements – Use a periodic table to name elements, given their symbols. – Use a periodic table to write the symbols of elements given their names. – Describe the arrangement of the periodic table. – List the characteristics that distinguish metals, nonmetals, and metaloids. Section 3 - Objectives

22 Section 1-3 Introduction to the Periodic Table The vertical columns of the periodic table are called groups. The horizontal rows of elements in the periodic table are called periods.

23 Section 1-3 (continued) Introduction to the Periodic Table (continued) Hydrogen Helium Oxygen Carbon Neon Iron Nitrogen Silicon Magnesium Sulfur Ten most common elements in the Milky Way GalaxyMilky Way Galaxy Oxygen Carbon Hydrogen Nitrogen Calcium Phosphorus Potassium Sulfur Chlorine Sodium Magnesium Iron Cobalt Copper Zinc Iodine Selenium Seventeen most common elements in the Human Body Oxygen Silicon Aluminum Iron Calcium Sodium Magnesium Potassium Titanium Hydrogen Ten most common elements in the Earth’s Crust

24 Section 1-3 Types of Elements - Metals An element that is a good conductor of heat and electricity is a metal. Most metals are malleable – they can be hammered or rolled into thin sheets They are also ductile which means they can be drawn in to fine wire. Metals that behave this way have a high tensile strength. The periodic table is divided into two main groups – metals and non-metals. Metals to the left and non-metals to the right.

25 Section 1-3 Types of Elements - Nonmetals A nonmetal is an element that is a poor conductor of heat and electricity. Many nonmetals are gas at room temperature, when solid they tend to be brittle.

26 Section 1-3 Types of Elements - metalloids A metalloid is an element that has some characteristics of metals and some characteristics of nonmetals. Metalloids tend to be semiconductors.

27 Section 1-3 Types of Elements – Noble Gases The elements in group 18 of the periodic table are generally unreactive.

28 Chapter Summary Questions HW – page 26 1,5-13,17,19, 20 & 23

29 Chapter Summary Questions 1 - Chemistry is the study of the compostion, structure and properties of substances and the changes they under go

30 5 a)A measure of the amount of matter b)the amount of space occupied by matter

31 6 The portions of elements in a pure substance are fixed.

32 7 a)A property is any characteristic of a substance or material. b)Properties can be compared in order to classify unknown materials as members of known groups or subgroups of substances, or to identify substances directly.

33 8 Extensive properties depend on the amount of matter that is present. Intensive properties do not.

34 9 a.a characteristic that can be observed or measured without changing the identity of the substance. b.Examples include color, odor, length, size, melting point & boiling point.

35 10 a.a property that describes the ability of a substance to undergo changes that alter its identity. b.Examples include the ability of coal to burn and the ability of iron (Fe) to rust.

36 11 A physical change is a change in a substance that does not involve a change in its identity. A chemical change is a change in which a substance is converted into other substances.

37 12 a.solids, liquids & gases b.A solid has a definite shape and fixed volume, whereas a liquid has a fixed volume but takes the shape of the vessel it is in. c.A gas has neither fixed volume or definite shape. d.Liquids and gases take the shape of the container they are in.

38 13 A change of a substance from one state of matter to another.

39 17 The reactants are potassium (K) and water (H 2 O) and the products are potassium hydroxide (KOH) and hydrogen (H 2 )

40 19 a.physical, wood still wood b.chemical, composition change think taste c.physical, butter still butter

41 20 a.potassium (K)  metal b.Silver (Ag)  metal c.Silicon (Si)  metalloid d.sodium (Na)  metal e.Mercury (Hg)  metal f.helium (He)  noble gas

42 23 a.Group 14, period 2 b.Group 18, period 3 c.Group 6, period 4 d.Group 2, period 6 e.Group 17, period 5 f.Group 11, period 6


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