Unit 1. Matter and Change

Do Now: What are the parts of the scientific method and

explain each part?

Objective Identify the common steps of scientific

methods Identify types of variables Describe the difference between a

theory and a scientific law Identify the characteristics of a

substance Distinguish between physical and

chemical properties Differentiate among the physical states

of matter

Objectives Continued Define physical and chemical changes and

list common changes Apply the law of conservation of mass to

chemical reactions

Activities: Q&A Solve problems Exit Ticket

Scientific Method (p12)

Systematic approach used in scientific study

Method for scientists to verify the work of others

Steps of Scientific Method Observation Hypothesis Experiments Conclusion

Theory/ Scientific Law

Observation Act of gathering information

Qualitative Data- color, shape, odor other physical characteristics

Quantitative Data – some type of measurement. It is numerical. Ex. Height, weight, how fast, how slow etc.

Hypothesis Tentative explanation for what has been

observed.

Experiment Set of controlled observations used to

test the hypothesis Must carefully plan and set up one or

more laboratory experiments in order to change and test one variable at a time.

Independent Variable – Variable that you plan to change. ( what you can control)

Dependent Variable – variable that changes based on the independent variable

Conclusion Judgment based on the information

obtained

Ch. 3 - Matter

I.

Kinetic Molecular Theory

States of Matter

A. Kinetic Molecular Theory

KMT

Particles of matter are always in motion.

The kinetic energy (speed) of these particles increases as temperature increases.

Three States of Matter

Solidsvery low KE - particles

vibrate but can’t move around

fixed shape fixed volume

Three States of Matter

Liquids low KE - particles can

move around but are still close together

variable shapefixed volume

Three States of MatterGases

high KE - particles can separate and move throughout container

variable shapevariable volume

Vapor- Gaseous state of a substance that is a solid or liquid at room temperature.

Matter and its Properties It’s Classified!

Physical vs. Chemical Physical Property

can be observed without changing the identity of the substance Extensive or intensive properties

Chemical Property describes the ability of a substance to

undergo changes in identity

Extensive vs. Intensive Extensive Property

depends on the amount of matter present

ex,.-

Intensive Property depends on the identity of substance, not

the amount

Ex.-

Extensive vs. Intensive Extensive Property

depends on the amount of matter present

ex,.- Volume, mass, Energy

Intensive Property depends on the identity of substance, not the

amount

Ex.- melting point, boiling point, conduct electricity or heat

WHAT ABOUT DENSITY??

A. Extensive vs. Intensive Examples:

boiling point

volume

mass

density

conductivity

A. Extensive vs. Intensive Examples:

boiling point…… intensive

Volume …. extensive

Mass ….. extensive

Density ….. intensive

Conductivity ….. intensive

Physical vs. Chemical Physical Change

changes the form of a substance without changing its identity

properties remain the same

Chemical Change changes the identity of a substance products have different properties

Signs of a Chemical change in color or odor

formation of a gas

formation of a precipitate (solid)

change in light or heat

B. Physical vs. ChemicalExamples:

melting point

flammable

density

magnetic

tarnishes in

air

physical

chemical

physical

physical

chemical

B. Physical vs. ChemicalExamples:

melting point

flammable

density

magnetic

tarnishes in

air

physical

chemical

physical

physical

chemical

B. Physical vs. Chemical Examples:

rusting iron

dissolving in water

burning a log

melting ice

grinding spices

B. Physical vs. Chemical Examples:

rusting iron

dissolving in water

burning a log

melting ice

grinding spices

chemical

physical

chemical

physical

physical

Law of Conservation of Mass Mass is neither created nor destroyed

during a chemical reaction. It is conserved

In a chemical reaction, the mass of the reactants must equal the mass of the products

Law of Conservation of MassPg. 78#7 A student carefully placed 15.6 g of sodium in a reactor supplied with an exess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7f of sodium chloride. Calculate how many grams of chlorine gas reacted. How many grams of sodium reacted?

Law of Conservation of MassPg. 78#7 A student carefully placed 15.6 g of sodium in a reactor supplied with an exess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7f of sodium chloride. Calculate how many grams of chlorine gas reacted. How many grams of sodium reacted?

24.1 g of chlorine gas, 15.6 of sodium

Law of Conservation of MassPg. 78#7 A student carefully placed 15.6 g of sodium in a reactor supplied with an exess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7f of sodium chloride. Calculate how many grams of chlorine gas reacted. How many grams of sodium reacted?

24.1 g of chlorine gas, 15.6 of sodium

HW Pg 79 (10 and 13 only)

Do Now:

DO NOW: What is a solution? Describe the difference between a

heterogeneous and homogenous mixture Calculate % by Mass

Objective: SWBAT:

Contrast Mixtures and substances Classify mixtures as homogeneous or

heterogeneous List and describe several techniques used

to separate mixtures. Distinguish between elements and

compounds

Activities Q&A Solve problems Exit Ticket

Objective: Activities:

A. Matter Flowchart

MATTER

Can it be physically separated?

Homogeneous Mixture(solution)

Heterogeneous Mixture Compound Element

MIXTURE PURE SUBSTANCE

yes no

Can it be chemically decomposed?

noyesIs the composition

uniform?

noyes

Colloids Suspensions

A. Matter Flowchart Examples:

graphite

pepper

sugar

(sucrose)

paint

soda

A. Matter Flowchart Examples:

graphite

pepper

sugar

(sucrose)

paint

soda

element

hetero. mixture

compound

hetero. mixture

solution

Pure Substances Element

composed of identical atoms EX: copper wire, aluminum foil

Pure Substances

Compound composed of 2 or more elements

in a fixed ratio

properties differ from those of individual elements

EX: table salt (NaCl)

Pure Substances Law of Definite Composition

A given compound always contains the same, fixed ratio of elements.

Law of Multiple Proportions Elements can combine in different ratios to form

different compounds.

Pure Substances For example…

Two different compounds, each has a definite composition.

Pure Substances(constant composition)

Elements Listed on the Periodic

Table Cannot be broken down

into unique components Na, Cl, Al, O2, S8

Compounds Made of elements that

are chemically joined Can be broken down NaCl, H2O, AlCl3, H2SO4

Diatomic Elements Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine Iodine

There are 7 diatomic elements

These atoms are never alone, if they are the pair up with the same atom

C. Mixtures Variable combination of 2 or more pure substances.

Heterogeneous Homogeneous

C. Mixtures Solution

homogeneous very small particles no Tyndall effect

Tyndall Effect

C. Mixtures Colloid

heterogeneous medium-sized particles Tyndall effect particles don’t settle EX: milk

C. Mixtures Suspension

heterogeneous large particles Tyndall effect particles settle EX: fresh-squeezed

lemonade

Mixtures(variable composition)

Homogeneous – Solutions evenly distributed

Heterogeneous not evenly distributed

Tea – Homogeneous Mixture

Air – Homogeneous Mixture

Alloys – Homogeneous Mixtures

Cereal – Heterogeneous Mixture

Sand – Heterogeneous Mixture

C. Mixtures Examples:

mayonnaise

muddy water

fog

saltwaterItalian salad dressing

C. Mixtures Examples:

mayonnaise

muddy water

fog

saltwaterItalian salad dressing

colloid

suspension

colloid

solution

suspension

% by Mass = Percent by Mass

AKA % composition

Example P 88 # 19 A 78.0 g sample of an unknown

compounds contains 12.4 g of hydrogen. What is the present by mass of hydrogen in the compound?

Example P 88 # 19 A 78.0 g sample of an unknown

compounds contains 12.4 g of hydrogen. What is the present by mass of hydrogen in the compound?

% mass = (12.4/78.0) * 100 = 15.9%

Extra problems: Pg 88 (# 22-23)

HW Pg 90 (28) Pg 94 (32, 37, 38, 40, 42, 43,44,50,52,

57,58,60, 62, 64, 76, 92)

Do Now: Look at your periodic table. What important information can you get

from the PTOE?

Objectives Find patterns in the Periodic Table Classify elements as metals, non-metals

or metalloids Distinguish between metals, non-metals

or metalloids

Activities PPT Group work

The Periodic Table

C. Johannesson

A. Mendeleev

Dmitri Mendeleev (1869, Russian) Organized elements

by increasing atomic mass.

Elements with similar properties were grouped together.

There were some discrepancies.

C. Johannesson

A. Mendeleev Dmitri Mendeleev (1869, Russian)

Predicted properties of undiscovered elements.

C. Johannesson

B. Moseley Henry Moseley (1913, British)

Organized elements by increasing atomic number.

Resolved discrepancies in Mendeleev’s arrangement.

C. Johannesson

MetalsNonmetalsMetalloids

How PTOE is organized

C. Johannesson

Main Group Elements

Transition MetalsInner Transition

Metals

B. Blocks

Periods and Families Periods: horizontal rows on the periodic

table physical and chemical properties change

somewhat regularly across a row. Elements closer to each other in the same

period tend to be similar than those that are farther apart.

Families: vertical rows of elements, aka groups Each group contains similar chemical

properties

Types of Elements METALS:

Shiny Conductors of heat and electricity

Most metals are malleable (can be pounded into thin sheets; a sugar cube sized chunk of gold can be pounded into a thin sheet which will cover a football field),

Most metals are ductile (can be drawn out into a thin wire).

All are solids at room temp (except Mercury, which is a liquid) Metals tend to have low ionization energies, and typically lose electrons

(i.e. are oxidized) when they undergo chemical reactions Alkali metals are always 1+ (lose the electron in s subshell) Alkaline earth metals are always 2+ (lose both electrons in s

subshell) Compounds of metals with non-metals tend to be ionic in nature.

Types of Elements NON- METALS:

Vary greatly in appearance Non-lustrous Poor conductors of heat and electricity The melting points of non-metals are generally lower than

metals Seven non-metals exist under standard conditions as diatomic

molecules: H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l) I2(l) (volatile liquid - evaporates readily) Nonmetals, when reacting with metals, tend to gain electrons

(typically attaining noble gas electron configuration) and become anions: Nonmetal + Metal -> Salt

Compounds composed entirely of nonmetals are molecular substances (not ionic)

Types of Elements Metalloids:

Elements may share properties of metals and non-metals.

Exit Ticket: Classify the following as either a METAL, NON-METAL or METALLOID:

a. Aub. Sic. Brd. An element that is brittle and conducts

electricitye. An element that is malleablef. An element that has tendency to become an

anion

Review of Unit List topics we have covered.

Study for test!