Matter Chapter 2.1 Sept 22, 2015 - PowerPoint Presentation

Matter Chapter 2.1

Sept 22, 2015 Objective: Distinguish between elements and compounds and categorize materials as pure substances or mixtures Lab safety: do not touch or taste anything without permission that is not yours Do now: Read the definitions of chemistry and matter . Create a list for matter and a list for changes you’ve seen matter undergo.

Matter Anything that has mass and occupies space. Chemistry is the study of matter and how it changes.

Solids

Liquids

Classification of matter

Pure Substances Uniform and definite composition Formed and separated chemically 2 types Elements & compounds

Pure Substance Elements – a substance that cannot be broken down into smaller substances. Atoms – smallest particle that has properties of an element.

Elements

Pure Substance Compounds – a substance formed when two or more elements chemically combine together. The smallest unit of a substance that exhibits all of the properties characteristic of that substance (compound) . Two or more atoms chemically combined

Chemical Formulas Ex. C 16 H 10 N 2 O 2 Ex. C 6 H 12 O 6 Ex. H 2 O

Mixtures A physical combination of more than one substance. (Two Types)

Homogeneous Mixtures Solutions Look the same throughout ex: flat soda, salt water, black coffee

Heterogeneous Mixtures Not uniformly mixed, different parts Substances that need to be shaken ex: noodle soup, granite

Classifying Liquid Mixtures: miscible -dissolve into each other immiscible -don’t mix into each other. You can see layers ex: oil and water.

Liquids Mix with Gas Can you think of a very common example???

SODA!

Station activity: which matter is which? Each group will start at a station Each station has a substance. Label the station you are at and identify the substance at that station (most have labels) With your teammates identify if the substance is a pure substance or a mixture Then, identify if the substance is an element, compound, heterogeneous mixture or homogeneous mixture.

Matter and Energy 2.2

Sept 23, 2015 Objective: Describe the properties and structures of the different states of matter using the kinetic theory. Do now: Identify the following as an element, compound, homogenous mixture, heterogeneous mixture – Water - gold Salad - olive oil c 6 h 12 o 6 Review station activity

Kinetic Theory All matter is made of atoms and molecules that act like tiny particles.

Kinetic Theory 2. These tiny particles are always in motion. The higher the temperature, the faster the particles move.

Kinetic Theory 3. At the same temperature, heavier particles move slower than lighter particles.

Phases/States of Matter Gas liquid solid plasma

Molecular workbench lab Virtual lab/ demonstration of phases of matter and kinetic energy Directions: Open tablets and go to http://mw.concord.org/modeler / (Phase change) Must read all directions and look at buttons before pressing play. Answer questions in complete sentences!When finished, click “create a report of my work,” then click “print without logging in.” include both last names.

Sept 24, 2015 Objective: Describe the properties and structures of the different states of matter using the kinetic theory. Do now: In a short paragraph, described what you have learned from the simulation so far (what did you see? What did you do?). How does this apply to kinetic theory?

Sept 25, 2015 Objective: Describe the energy transfers in each state of matter. Distinguish between physical changes and chemical changes Do now: compare and contrast solids and liquids. Include facts about shape, volume, movement of particles, attraction of particles.

States of Matter - Gases no definite shape. no definite volume. easy to compress. most random arrangement of particles. Most spread out.

Gases Property of gases is called pressure. the force exerted per unit area of a surface

Liquids Definite volume no definite shape (takes shape of container) Difficult to compress disorderly arrangement on particles Close together

Liquids Property of Liquids is called viscosity. the resistance of a fluid to flow

Solids Definite shape Definite volume Difficult to compress Orderly arrangement of particles close together Smallest amount of movement of particles.

Energy The ability to change state or move matter. Changing state does not change composition of the substance

liquid gas solid Changes of State

Law of conservation of matter (mass) Matter (mass) cannot be created or destroyed. It only changes its state or rearranges its atoms.

Law of conservation of energy Energy cannot be created or destroyed. It converts from one form to another during chemical or physical changes.

Physical or Chemical change? 1 2 3 4 5 6

Properties of Matter 2.3

Physical Property A characteristic of a substance that can be observed or measured without changing the composition of the substance.

Physical Property Melting and freezing points. Solubility Dissolving of a solid into a liquid. Density

Why do some things float while others sink? https:// www.youtube.com/watch?v=MzsORE0ae10

Density mass/volume (D=m/V) UNITS: mass – (g) Volume – (mL) or (cm 3 ) density – (g/mL) or (g/cm 3 )

Density Buoyancy - The force with which a more dense fluid pushes a less dense substance upward. ex. floating ice.

Example An unknown metal is measured to be 36 grams. What is it’s density if it has a volume of 15.5 cm 3 ? D=m/v d= 36 g/ 15.5 cm 3 D = 2.322 g/cm 3 Last point is sig. figs. 2.3 g/cm 3 +1 +1 +1 +1 +1

Sept 29, 2015 Objective: Perform observations and calculations involving density. Do Now: solve the following problems on page 56 of your textbk : 1. A piece of tin has a mass of 16.52g and a volume of 2.26 cm 3 . What is the density of the tin? 5. The mass of a 125cm 3 piece of material is 83.75g. Determine the density of this material.

Chemical Properties The way a substance reacts with others to form new substances with different properties.

Chemical Properties Flammability Reactivity corrosion

Physical Changes A change in the physical form or properties of a substance that occurs without a change in composition.

Chemical Change A change that occurs when a substance changes composition by forming one or more new substances.

Chemical Change 4 signs: Evolution heat or light Color change Formation of gas Formation of a precipitate (solid residue)