Unit 1 - Introduction to Chemistry. What Matters? 1.A.2(b) use appropriate SI units describe the relationship among SI unit prefixes

Transcription

1 Unit 1 - Introduction to Chemistry What Matters? 1.A.2(b) use appropriate SI units describe the relationship among SI unit prefixes

2 SI Base Units 1.A.2(b) use appropriate SI units describe the relationship among SI unit prefixes Length meter Mass kilogram Time second Temperature Kelvin Quantity of Matter mole Volume - liter This will be on the test

3 SI Derived Units Combinations of base units Ex velocity = meters/second (m/s) acceleration = meters/second second m/s 2 ) density = kg/m m m (kg/m 3 )

4 Non-SI Units Length foot, mile, Mass ounce Temperature Centigrade, Celsius, Fahrenheit Volume - gallon

5 Commonly Used Prefixes Centi- 1/100 or 0.01 Kilo or 1.0 x 10 3 Milli- 1/1000 or 0.001

6 States of Matter II.B.1(a) compare the definition of matter and energy and the laws of conservation of matter and energy

7 Matter Def- anything that has mass and occupies space 3 States of matter Solid Liquid Gas

8 Solids, Liquids, and Gases Solids have both definite volume and shape Liquids have definite volume but not shape Gases have neither definite volume or shape Particles have increasing velocity from solids to liquids to gases

9 Changes of State II.B.2(c) describe the phase and energy changes associated with them

10 Phase Changes Melting Freezing Vaporization/Evaporation Condensing Sublimation Deposition

11 Melting/Freezing Energy must be ADDED for a substance to melt Energy must be REMOVED for a substance to freeze

12 Vaporization & Condensation Energy must be ADDED for a substance to boil Energy must be REMOVED for a substance to condense

13 Deposition/Sublimation Energy must be ADDED for a substance to sublime Energy must be REMOVED for a substance to undergo deposition

14 Law of Conservation of Energy Energy cannot be created or destroyed Energy of a reaction MUST be conserved

15 Law of Conservation of Matter Matter cannot be created or destroyed Mass of a chemical reaction MUST be conserved

16 Elements, Compounds & Mixtures II.A.2(b) compare the characteristics of elements, compounds and mixtures

17 Elements An element is matter in its simplest form Cannot be broken down by chemical means Periodic Table (118 elements)

18 Compounds Are combinations of elements Have the same composition Can be broken down by chemical means

19 Mixtures Have variable composition Can be separated physically or chemically Homogeneous Mixtures are the same throughout Heterogeneous Mixtures have different regions

20 Separatory Techniques IV.A.1(b) describe and perform common separation techniques

21 Filtration Used for separating undissolved solids Pour through a mesh (filter paper)

22 Distillation Used to separate dissolved solids or liquid mixtures Uses physical changes

23 Chromatography Uses chemicals to separate the pigments of plant or chemicals Various Methods Gas chromatography Liquid chromatography Thin-layer chromatography Ion-exchange chromatography

24 Chemical vs Physical II.B.1(e) define chemical and physical properties and compare them by providing examples

25 Physical Properties Physical Properties Can be observed without changing a substance into another substance. Boiling point, density, mass, volume, etc. Odor Color Volume State Density Boiling point Melting point

26 Chemical Properties Chemical Properties Can only be observed when a substance is changed into another substance. Flammability, corrosiveness, reactivity with acid, etc. Wood burning Iron rusting Digestion photosynthesis

27 Chemical and Physical Changes II.B.1(d) explain the difference between chemical and physical changes and demonstrate how these changes can be used to separate mixtures and compounds into their components

28 Physical Change These are changes in matter that do not change the composition of a substance. Changes of state, temperature, volume, etc.

29 Chemical Change Chemical changes result in new substances. Combustion, oxidation, decomposition, etc.

30 Indicators of Chemical Change Formation of a gas (bubbles) Formation of a precipitate (solid) Change in temperature Exothermic Endothermic Color change

31 Properties Extensive Properties depend on the amount of substance present Volume Mass Energy present Intensive Properties do NOT depend on the amount of substance present Melting point Boiling point Density Conductivity

32 Elements & The Periodic Table Periods horizontal rows Groups vertical columns Group 1A alkalai metals Group 2A alkalai earth metals Group 3A-12A transition metals Group 16A chalcogens Group 17A halogens Group 18A noble gases

33 Group 1 Alkali Metals

34 Group 2 Alakali Earth Metals

35 Transition Metals

36 Chalcogens

37 Halogens

38 Noble Gases

39 The Periodic Table

40

41 Metals Conduct heat and electricity Malleable Ductile Luster (shiny)

42 Non-metals Poor conductors of heat Poor conductors of electricity Many are gases at room temp 5 solid non-metals Phosphorous Sulfur Carbon Selenium Iodine

43 Metalloids Have some characteristics of both metals and non-metals

44 Noble Gases Least reactive of all elements All gases at room temp