Chemistry Terminologies

Chemistry

MatterProperty

Composition

Structure

Changes = Laws

Mass vs. Weight

• Unit of mass

• Amount of material in an object

• Constant

• Unit of force

• Force of gravity pulling on the object

• Depends on the location

Mass Weight

Temperaturehotness or coldness of

an object

Celsius vs. Fahrenheit vs. Kelvin

0C = (0F – 32)/ 1.8

0F = (1.8 X 0C) + 32

K = 0C + 273

0C 0F K

Normal body temperature

37 0C 98.6 0F ?

Boiling point 100 0C ? 373 K

Freezing point

? 32 0F 273 K

0C 0F K

Normal body temperature

37 0C 98.6 0F 310 K

Boiling point 100 0C 212 0F 373 K

Freezing point

0 0C 32 0F 273 K

Evaporation vs. Condensation

Evaporation vs. Condensation

Evaporation–Liquid to Gas

Condensation–Gas to Liquid

Sublimation vs. Condensation

Sublimation vs. Condensation

Sublimation–Solid to Gas

Condensation–Gas to Solid

Matter

Matter

Substance Mixture

Element

Compound

Homogenous

Heterogeneous

Solution

Suspension

Colloid

Matter

Space Mass

Pure Substance

Compose of the same kind of particles Has same color and taste Has definite properties and uniform

characteristics Has single phase

– Salt– Sugar– Pure water

Element

made up of only one kind of atoms having the same atomic number

cannot be further reduced to simpler substances by ordinary physical or chemical processes– Hydrogen– Oxygen

Compound

Formed by the combination two or more elements

Could not be separated into its constituents by mechanical or physical means

Properties of a compound differ entirely from those of its constituent elements

Mixture

Combination of two or more substances Each substance retains its own

properties– Air– Gasoline– Halo Halo– Fruit Salad

• Uniform characteristic

• Single phase

•Air

•Gasoline

• No uniform characteristic

• Two or more phase

•Fruit Salad

•Halo Halo

Homogenous Heterogeneous

Solution

Homogeneous mixture of two or more chemical substances

May be solid, liquid or gas– salt water (liquid solution)– air (gaseous solution)– alloy (solid solution)

Solute + Solvent = Solution

Suspension

Consists of particles of a solid suspended in a liquid medium

Has two distinct phases Particles of a suspension may not be visible

to the naked eye– Sand and water– Oil and water

Colloid

Represents an intermediate kind between true solution and suspension

Two-phase heterogeneous system – dispersed phase– dispersion medium

Dispersed phase = solute in a solution

Dispersed phase

 Dispersed medium

 Colloidal system

 Examples

 Solid  Solid  Solid solsColored glues, gem

stones, pearls,

 Solid  Liquid  Sols  Paints, starch,

 Liquid  Solid  Gels  cheese butter

 Liquid  Liquid  Emulsion  Milk, hair cream,

 Solid  Gas  Aerosols of

solids Smoke, dust in air,

smog

 Liquid  Gas Aerosols of

Liquids Insecticide sprays

 Gas  Solid  Solid foam Foam, Ice-cream,

Rubber

 Gas  Liquid  Foam, Froth Soda water, whipped

cream froth

Matter

Substance Mixture

Element

Compound

Homogenous

Heterogeneous

Solution

Suspension

Colloid

Acid vs. Base

• Latin “acidus”

• Sour

• Proton donor

• Blue to red

• Bitter

• Slippery

• Proton acceptor

• Red to blue

Acid Base

• Fruits

• Citric Acid

• Vinegar

• Acetic Acid

• Soft drinks

• Carbonic Acid

• Milk

•Lactic Acid

• Vomit

•Hydrochloric Acid

• Lye

• Baking soda

• Milk of magnesia

• Antacid

Acid Base

Indicator

Exhibits specific color in the presence of acid or base

pH – measure of acidity or basicity

pH paper

pH meter

pH Reading

Values 1-14Less than 7 = acidicHigher than 7 = basicEqual to 7 = neutral

pH = 5

Acidic

pH = 4

Acidic

pH = 7

Neutral

pH = 6

Acidic

pH = 8

Basic

Strong or Weak

Acid + Base = Neutralization

Atom

Atom

Smallest particle of an atomJohn Dalton : indivisible

Parts of an Atom

Proton Electron Neutron

Charge + - No charge

Location • In the nucleus

• Surrounds proton and neutron

• Near protons•Holds the protons together

Nucleus = center = proton and neutron

Atomic Number vs. Atomic Mass

Atomic Number Atomic weight

• Equal to the number of protons

• Equal to mass number

• Equal to the no. of neutron + no. of proton

S

Ga Ba

Isotope vs. Isotone vs. Isobar

Isotope

Same elementDifferent atomic mass

C CMg Mg

Isotone

Same number of neutrons

Neutrons = A. Mass – A. No.

C NCa K

Isobar

Same atomic massDifferent elements

Ne NaAr K

Isotope vs. Isotone vs. Isobar

C N

Pb Pb

Na Mg

Alpha vs. Beta vs. Gamma

Radioactivity

process whereby unstable atomic nuclei release energetic subatomic particles

subatomic particles released during the process

Charge Penetrating

Power

Ionizing

Power

Alpha + Least Maximum

Beta - Less Less

Gamma No charge Maximum Least

Penetrating Power

If you have three radioactive cookies alpha beta and gamma, what will you

Eat?

Place in your pocket?

Hold by your hand?

If you have three radioactive cookies alpha beta and gamma, what will you

Eat? Gamma

Place in your pocket? Beta

Hold by your hand? Alpha

End