G8 Science Q3- Week 3-4- Protons and Atoms.pptx

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1. CLASSIFICATION OF MATTER PREPARED BY: MS. ELLEN ROSE D. PACARDO

2. S8MT - IIIa - b - 8 Explain the properties of solids, liquids, and gases based on the particle nature of matter;

3. Matter Pure substance Mixture Element Compound Homogeneous Heterogeneous Can it be separated by physical process? No Yes Can it be decomposed by chemical process? Is it uniform throughout? No No Yes Yes

4. INTRODUCTION Matter :  Anything that occupy space and has mass  made up of very tiny units calls atoms Substance : a form of matter with a definite composition and distinct properties Element :  a substance made up of one type of atoms Compound : substance formed by the combination of 2 or more different elements  definite and constant composition

5. Atom: s mallest particle in substance Molecule : The smallest uncharged individual unit of compound formed by the union of two or more atoms. Ion : An atom or molecule that has acquired a charge by either gaining or losing electrons. Cation : positive charge Anion : negative charge

6. Molecular compounds: are made of molecules each molecule has the same element composition and properties as the compound Ionic compounds: are made of cations and anions cations combine with anions in just the right numbers to give an electrically neutral compound Mixture: combination of two or more substances in which the substances retain their distinct identities.

7. atom A atom B molecule A molecule B molecule AB element compound

8. element compound mixture mixture element mixture Classify each of the following as an element, a compound or a mixture:

9. Homogeneous mixture: the mixing is uniform . have a constant composition throughout. Homogeneous mixture are called solution gaseous solution (e.g: pure air) liquid solution (e.g: syrup) solid solution (e.g: steel, bronze) alloy

10. Heterogeneous mixture the mixing is not uniform . have regions of different composition. consist of two or more physically distinct phases eg: concrete (a mixture of cement, gravel, sand)

11. Classify each of the following as an element, a compound, a homogeneous mixture or heterogeneous mixture: a) Sulfur dioxide gas  compound Chlorine gas  element CuSO 4 aqueous  homogeneous mixture Tomato juice  heterogeneous mixture e) Brass plate  homogeneous mixture Exercise

12. PROPERTIES OF MATTER Chemical properties : the ability of a substance to form new substances , either by reaction with other substances or by decomposition. E.g : rusting, combustion, decomposition Chemical change : the formation of a new substance with a different composition and properties than the initial substance.

13. Physical properties : a characteristic of a substance that can be measured and observed without changing the composition or identity of a substance. E.g : taste, odour , colour , temperature (melting/boiling points), density. Physical change : a change in which the physical appearance of a substance changes but the chemical composition stays the same.

14. Intensive properties : properties that do not depend on the amount of the sample. E.g : temperature (melting/boiling points), density. Extensive properties : relate to the amount of substance present. E.g : mass, volume.

15. Classify the following as physical or chemical properties of water a) density = 1.00 g/mL c) forms ice at 0°C b) release hydrogen gas when reacted with sodium metal d) Water is formed when wood is burned physical property: density can be measured without changing a substance to anything else physical property: freezing is just changing the physical state chemical property: hydrogen gas is a new compound formed from water chemical property

16. Does the following describe a physical change or a chemical change? Evaporation of water  physical change (changes of state) b) Hydrogen burns in air  chemical change (H 2 converted to H 2 O) c) A piece of sliced apple turn brown  chemical change

17. STATES OF MATTER Solid : molecules are held close together in an orderly structure with little freedom of motion. Liquid : molecules are close together but are not held so rigidly in position and can move past one another. Gas : molecules are separated by distances that are large compared with the size of the molecules, thus they are much farther apart and move freely of each other. solid liquid gas

18. Water Molecule Solid 0°C Vapor 100°C Liquid o C - 100°C

19. Kinetic Molecular Theory : matter consist of particles called molecule in constant movement colliding with each other. Heat given, matter will change states from solid to liquid to gas Each state will differ particle arrangement amount of kinetic energy difficulty to compress attractive forces between the particles movement of particles

20. GAS LIQUID SOLID Condensation Vaporization Sublimation Deposition Melting (Fusion) Freezing Process of Changes in State of Matter

21. Temperature ( o C) time -25 ° C ice water water steam vaporization (liquid and vapor in equilibrium) steam H fus H vap (0 ° C) melting point 100 ° C boiling point Ice water Melting (solid and liquid in equilibrium) Heating Curve of Ice

22. Cooling Curve of Steam Temperature ( o C) time 105 ° C steam steam water condensation water 100 ° C boiling point (0 ° C) melting point ice water ice freezing Super cooling

23. Super Cooling Cooling of a liquid below its freezing point without forming the solid Occur when heat is removed from liquid so rapidly that the molecules have no time to assume the ordered structure of a solid unstable

24. Phase Diagram of Water 0.01 o C 0.006 atm Vapor solid liquid Triple point critical point

25. A diagram showing the conditions at which a substance exists as a solid, liquid and vapor Each solid line between two phases specifies the conditions of P and T under which the two phases can exist in equilibrium Triple point:  the point at which all three phases can exist in equilibrium  0.006 atm , 0.01 o C

26. Critical Pressure  the minimum P that must be applied to bring about liquefaction at the critical T. (P c of water = 219.5 atm ) Critical Tempt.  the highest T at which a substance can exist as a liquid. ( T c of water =374.4 o C )  above T c , vapor phase cannot be made to liquefy, no matter how great the applied pressure Critical Point:

27. Question 1 Which is an example of a physical change?  *Steam from the boiling water condenses on the cooler part of the ceiling. The crude metal ore was first heated then combined with pure oxygen gas to make the oxide of the metal. A piece of paper burns in air with a smoky flame. The table salt in the warehouse was used to make some of the polymeric material.

28. Question 2 Which is an example of a chemical change?  Steam from the boiling water condenses on the ceiling. The solid metal is heated until it melts. The gas is cooled until it finally becomes a liquid. *A piece of paper burns in air with a smoky flame.

29. Question 3 Which is an example of both a physical and a chemical change?   The milk in the carton became frozen because the carton was accidentally placed in the freezing compartment overnight. The bit of scrap metal was removed to the junkyard after being crushed by the heavy machine. The old parchment became dry when it was placed in the warm oven for ten minutes. *Bubbles were seen on the egg shell soon after a sample of the vinegar was poured on it.

30. Question 4 In the process of attempting to characterize a substance, a chemist makes the following observation: ‘the substance is a silvery white metal. It melts at 649 o C and boils at 1105 o C. The substance burns in air, producing an intense white light. It react with chlorine to give a brittle white solid.’ Which of these characteristics are physical properties and which are chemical properties?

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