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MATTER & PROPERTIES

MATTER & PROPERTIES. Dr Mehmet Gökhan ÇAĞLAYAN 09/2019. Why Chemistry is Important?. In Our Daily Lives New Materials New Pharmaceuticals New Energy Sources Food Supplies Solutions to environmental problems Develop polymers for clothing, cooking utensils, artificial organs, and toys

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MATTER & PROPERTIES

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  1. MATTER & PROPERTIES Dr Mehmet Gökhan ÇAĞLAYAN 09/2019

  2. Why Chemistry isImportant? • In Our Daily Lives • New Materials • New Pharmaceuticals • New Energy Sources • Food Supplies • Solutions toenvironmentalproblems • Developpolymersforclothing, cooking utensils, artificial organs, and toys • Can you think of others?

  3. What is Chemistry? • The science that deals with the materials of the universe and the changes these materials undergo • The Central Science • Understanding most other fields of science requires an understanding of Chemistry • Duetoitsdiverse applications, chemistry is often called the “central science.”

  4. What is scientificmethod? A systematic approach to research in short. A process of studying natural phenomena that involves making observations, forming laws and theories, and testing theories by experimentation.

  5. Ahypothesis is a proposed explanation for an observation. A hypothesisneedsto be tested. • A scientific theory consists of one or more hypotheses that have been supported by repeated testing. Theories are one of the pinnacles of science and are widely accepted in the scientific community as being true. • Alaw is a concise verbal ormathematical statement of a relationship between phenomena that is always the sameunderthesameconditions

  6. Basic terms • Matter: is anything that occupies space and displays the properties of massand inertia. • Composition refers to the parts or components of a sample of matterand their relative proportions. • Properties are those qualities or attributes that we can use to distinguish onesample of matter from others • Energy is the part of the universe that has the ability to do work • Chemistry is the study of matter • The properties of different types of matter • The way matter behaves when influenced by other matter and/or energy

  7. When liquid water freezes into solid water (ice), it certainly looks different and, in manyways, it is different. Yet, the water remains same amount of hydrogen and oxygen by mass Properties of Matter • Physical Properties are the characteristics of matter that can be changed without changing its compositionoridentity. • Characteristics that are directly observable • Whenliquidwater freezes into solid water (ice), it certainly looks different and, in manyways, it is different. Yet, the water remains sameamount of hydrogen and oxygenbymass. Thereforrmeltingpoint of a substance is a physicalproperty.

  8. Properties of Matter • Chemical Properties are the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy. • Sochemicalchangeoccurs: one or more kinds of matter areconverted to new kinds of matter with different compositions. • Characteristics that describe the behavior of matter • Hydrogenandoxygenreactingto form water.

  9. Classify Each of the following as Physical or Chemical Properties • The boiling point of ethyl alcohol is 78°C. • Physical property – describes inherent characteristic of alcohol – boiling point • Diamond is very hard. • Physical property – describes inherent characteristic of diamond – hardness • Sugar ferments to form ethyl alcohol. • Chemical property – describes behavior of sugar – forming a new substance (ethyl alcohol)

  10. PhysicalandChemicalChanges in Matter • Physical Changes are changes to matter that do not result in a change the fundamental components that make that substance • State Changes – boiling, melting, condensing • Chemical Changes involve a change in the fundamental components of the substance • Produce a new substance • Chemical reaction • Reactants  Products

  11. Classify Each of the following as Physical or Chemical Changes • Iron is melted. • Physical change – describes a state change, but the material is still iron • Iron combines with oxygen to form rust. • Chemical change – describes how iron and oxygen react to make a new substance, rust • Burning of thepaper • Chemical change – newsubstances

  12. Matter • Matter is anything that occupies space and has mass, and chemistry is the study of matterand the changes it undergoes. • All matter, at least in principle, can exist in three states: solid, liquid, and gas. • The three states of matter can be interconverted without changing the composition of thesubstance.

  13. The three states of matter forwater: solidice, liquidwater, andgaseoussteam.

  14. States of Matter • solid, liquid, gas

  15. Classification of Matter • Matter is made up of very tiny units called atoms. • Each different type of atom isthe building block of a different chemical element. An element is a substance thatcannot be separated into simpler substances by chemical means(118 elements) • Chemical compounds are substances comprising atoms of two or more elementschemically united in fixed proportions. (water, H2) • Amoleculeis the smallest entity having the same proportions of the constituent atoms asdoes the compound as a whole.

  16. Substance • A substance is matter that has a definite or constant composition and distinct properties. • Forex: water, silver, ethanol, table salt (sodium chloride), and carbondioxide. • Substances differ from one another in composition and can be identified bytheir appearance, smell, taste, and other properties. • Presently, over 20 million substancesare known, the list is growing rapidly.

  17. Mixtures • A mixture is a combination of two or more substances in which the substancesretain their distinct identities. Ex: air, soft drinks, milk, and cement. • homogeneous mixture or a solution; uniform in composition and properties Air, seawater • heterogeneous mixtures the componentsseparate into distinct regions. Sandandwater

  18. homogeneousorheterogeneous? homogenizedmilkthrough a microscope

  19. Classificationsummary

  20. Different Physical Property Technique Boiling Point Distillation State of Matter (solid/liquid/gas) Filtration Adherence to a Surface Chromatography Volatility Evaporation Separation of Mixtures • Separate mixtures based on different physical properties of the components • Physical change

  21. Filtration Distillation

  22. Chromatography

  23. Measurement of Matter: SI (Metric) Units • Quantitative • Comparison Based on an Accepted Scale • e.g. Meter Stick • Has two Parts – the Number and the Unit • Number Tells Comparison • Unit Tells Scale • The scientific system of measurement is called the SystèmeInternationaled’Unités(International System of Units) and is abbreviated SI; a system based on the unit of length called ameter(m).

  24. SI units

  25. SI prefixes

  26. Mass • Measure of the quantityof matter in an object • SI unit = kilogram (kg) • Commonly measure mass in grams (g) or milligrams (mg) in chemistry • 1 kg = 2.2046 pounds, 1 lbs = 453.59 g • 1 kg = 1000 g = 103 g, 1 g = 1000 mg = 103 mg • 1 g = 0.001 kg = 10-3 kg, 1 mg = 0.001 g = 10-3 g • Weight is the force of gravity on an object. W = g * m

  27. Temperature Scales • Fahrenheit Scale, °F • Water’s freezing point = 32°F, boiling point = 212°F • Celsius Scale, °C • Temperature unit larger than the Fahrenheit • Water’s freezing point = 0°C, boiling point = 100°C • Kelvin Scale, K • Temperature unit same size as Celsius • Water’s freezing point = 273 K, boiling point = 373 K

  28. Conversions

  29. Question • (a) Solder is an alloy made of tin and lead that is used in electronic circuits. A certainsolder has a melting point of 224°C. What is its melting point in degrees Fahrenheit? 9°F/5°C *(224°C) + 32°F = 435°F • (b) Helium has the lowest boiling point of all the elements at -452°F. Convert thistemperature to degrees Celsius. (-452°F - 32°F)*5°C/9°F=-269°C • (c) Mercury, the only metal that exists as a liquid atroom temperature, melts at -38.9°C. Convert its melting point to kelvins. (-38.9°C + 273 .15°C) *1 K/1°C= 234.3 K

  30. DerivedUnits • Some derived units have special names. • the combination kg m-1 s-2 is called the pascal • the combinationkgm-2 s-2 is called the joule Non-SI Units • United States is one of the few countrieswhere most units used in everyday life are still non-SI. • Masses are given inpounds, room dimensions in feet, and so on.

  31. Density • What weighs more, a ton of bricks or a ton of cotton? • Density is the ratio of mass to volume • Density is a function of temperature because volume varies with temperature,whereas mass remains constant. • The mass of 1.000 L of water at 4 °C is 1.000 kg. The density of water at 4 °C is 1.000 g/mLor At 20 °C, the density of water is 0.9982 g/mL

  32. Question • Gold is a precious metal that is chemically unreactive. It is used mainly in jewelry,dentistry, and electronic devices. A piece of gold ingot with a mass of 257 g has avolume of 13.3 cm 3. Calculate the density of gold. • d= m/V = 257 g/13.3 cm3= 19.3 g/cm3

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