CHEMISTRY-1CHAPTER 1

CHEMISTRY—THE SCIENCE OF MATTER

Chemistry is the study of matter and energy. In this chapter, you will examine the physical and chemical properties of matter. You will perform experiments and record data. You will learn how to classify matter as either a pure substance or a

mixture. You will also be introduced to the chemical language of symbols and formulas.

is also known as the central science

• Chemists are employed in dozens of occupations

• Whatever your career choice is, chances are you will need some

knowledge of chemistry!!!!

Anything that takes up space and has mass

Can be classified as solid, liquid, gas or plasma

Matter

Is it matter?

What is not matter?

ENERGY, HEAT, LIGHT, ELECTROMAGNETIC WAVES, MAGNETIC FIELDS, IDEAS, ETC.

Properties of MatterDescribe the characteristics and behavior

of matter, including the changes that matter undergoes

Observing Matter Macroscopic Observations: Observations made with the

5 senses

Microscopic Observations: Observations made with a microscope

Submicroscopic Observations: Observations of substances so small they cannot even be seen with a microscope

Macroscopic Microscopic Submicroscopic

Mass

Units: grams or kilogramsMeasured with: Triple Beam Balance

Scientific Model•Thinking device used to explain and represent macroscopic observations.

•Important in chemistry because the atom is so small we must study it at a submicroscopic level

Scientific model of an atom

Scientific model of a water molecule

Qualitative Observation: Describes the properties of a substance

Quantitative Observation: An observation that involves a numerical value.

PURE SUBSTANCEPURE SUBSTANCE

Matter with the same fixed Matter with the same fixed composition and propertiescomposition and properties– First Type of Pure SubstanceFirst Type of Pure Substance

ElementElement– The Periodic Table:The Periodic Table: A chart that lists the chemical A chart that lists the chemical

name and chemical symbol for each elementname and chemical symbol for each element– Chemical Symbol:Chemical Symbol: A shorthand abbreviation for A shorthand abbreviation for

the name of an elementthe name of an element

Aluminum = ___ Aluminum = ___ Tin = ____ Tin = ____

Carbon = ____ Carbon = ____ Xenon = ____Xenon = ____

PURE SUBSTANCEPURE SUBSTANCE

Matter with the same fixed Matter with the same fixed composition and propertiescomposition and properties– Second Type of Pure SubstanceSecond Type of Pure Substance

CompoundCompound– Chemical Formula:Chemical Formula: A combination of chemical A combination of chemical

symbols that show what elements make up a symbols that show what elements make up a compound and the number of atoms of each compound and the number of atoms of each elementelement

Subscript:Subscript: A number written to the lower right A number written to the lower right of an element symbol to indicate the number of of an element symbol to indicate the number of atoms of thatatoms of that

NaHNaH22COCO33 Mg(OH)Mg(OH)22

MIXTURES

Two or more elements physically combined.

Homogeneous Mixtures

• The prefix “homo-” means “the same”

• A mixture that is the same throughout

• You cannot see the phases (parts) of the mixture.

Solutions• Solute: The substance being dissolved in a

solution• Solvent: The substance that dissolves the

solute• Aqueous Solution: A solution in which water

is the solvent

ALLOY

NAME OF ALLOY % MAKE UP EXAMPLE

Stainless Steel 73-79% Fe14-18% Cr7-9% Ni

Sterling Silver 92.5% Ag7.5% Cu

18-karat white gold 75% Au12.5% Ag12.5% Cu

14 karat gold 58% Au14-28% Ag14-28% Cu

Heterogeneous Mixtures

• The prefix “hetero” means “different”

• A mixture with different compositions throughout

• You can see each phase (part) of the mixture

Methods to Separate Mixtures

• Filtration: Separates a solid from a liquid

Separating…

• Magnet: Separates Fe, Co, or Ni

Separating…

• Crystallization: Separates crystalline solids from a saturated liquid

Separating…

• Distillation: Separates two or more liquids with different boiling points.

Separating…

• Chromatography: Separates different types of liquids

Properties & Changes of Properties & Changes of MatterMatter

States of Matter

• Depends on:

• Solid:

• Liquid:

• Gas:

PLASMA

Free electrons and ions of an element.

The most common form of matter

Energy is needed to strip atoms of their electrons.

Plasmas can be steered and controlled by magnetic and electric fields.

PLASMA TV’S•Xenon and Neon in each cell

•Intersecting electrodes charged causing electric current through the gas in that cell

•Electric current = rapidly flowing charged particles causing the release of UV photons

•Photons interact with the phosphor coating giving off colored light

Because each cell is lit individually, the image is bright and looks good from almost any angle.

Physical Properties

What are the physical properties represented in the images above?

chara

cteris

tic

s

quantitative

qualitative

Volatile Substances

Density

To calculate Density

Density = Mass ÷ Volume

Chemical Properties

Chemical Reaction: A Chemical Change

• After a chemical reaction: The original substance no longer has the same identity

• Chemical reactions can be used to:

Is it a chemical reaction?

Law of Conservation of Matter

•Matter cannot be created nor destroyed in a chemical reaction.

•Developed by: Antoine Lavoisier

•Mathematically:Mass of the reactants = Mass of the products

(starting materials) (ending materials)

ENERGY IN CHEMICAL REACTIONS

• Most chemical reactions involve changes in energy.– The unit for energy is the Joule (J)

• This is because bond breaking requires energy and bond forming releases energy.

• Almost all chemical reactions either release or absorb energy

• This energy flow results in heat, either being absorbed or released.

EXOTHERMIC REATIONS• To the touch an exothermic reaction would

feel HOT because heat is being released to the surroundings

ENDOTHERMIC REACTIONS

• To the touch an endothermic reaction would feel cold because heat is being absorbed from the surroundings.

Law of Conservation

of EnergyEnergy

cannot be created nor destroyed!

Type of Energy Examples

Kinetic Sound, Wind, Spinning Wheel

Potential Ball held above ground, water before a dam

Radiant Light, Microwaves, X-rays, Gamma waves

Electrical Electricity, static cling, lightning

Magnetic Magnets, compasses

Mechanical Pistons in a car engine

Thermal Heat

Nuclear Nuclear fission, nuclear fusion, heavy water

Chemical Gasoline, oil, batteries, food

Spring Stretched rubber band, bungee cord, spring scale

Law of Conservation of EnergyEnergy cannot be created nor

destroyed!

Any situation

where energy

is transferred

from one object

to another…

…or from one kind

of energy into another kind.

Webster's Dictionary definition of "rube goldberg”: Accomplishing by extremely complex, roundabout

means what seemingly could be done simply.

Draw your final sketch today. Label all 10 forms of energy associated with your machine.

Objective: Make a drawing of a Rube Goldberg device of your own creation which includes examples of each of the 10 basic types of energy and 10 different energy changes.  

10 energies - these should be clearly labeled and numbered in blue next to where the energy occurs in the drawing.

10 different energy changes - arrows should be drawn connecting each energy in the drawing to the next in red to show how one type of energy is changing into another.