Chemistry (CH.1)

Basic definitions, terms, and other things needed that we discussed within the first week

Chemistry

The study of what substances are made of and how they behave

Matter

Anything that has mass and takes up volume

Atom

The fundamental unit of matter

Element

Made of only one type of atom

Compound

Composed of more than one element, bound in a fixed ratio

Molecules

Groups of atoms that bind tightly together and behave as a single unit

Diatomic Molecules

Molecules made up of just two atoms, chemically bonded together

Pure substances

Contains only one type of element or compound

Mixture

contains more than one substance, not bound in a fixed ratio

Bronze is an example of…

…a mixture of copper and tin

Homogeneous Mixtures

Components are mixed evenly and appear to be uniform throughout

Heterogeneous Mixtures

Components do not mix evenly

Sand and water, when combined is an example of a…

heterogeneous mixture

Salt and water, when combined is an example of a…

homogeneous mixture

atoms → elements and compounds → pure substances →matter← mixtures←homogeneous and heterogeneous

Gatorade is an example of …

a homogeneous mixture

Crystalline sugar is an example of…

a pure substance

Led wire is an example of …

a pure substance

Salsa is an example of

a heterogeneous mixture

Solid to Liquid

Melting

Liquid to Gas

Vaporization

Solid to Gas

Sublimation

Gas to Liquid

Condensation

Liquid to Solid

Freezing

Gas to Solid

Deposition

Physical Properties

Can be measured without changing the identity of the substance

What are the five main physical properties?

Color, Hardness, Mass, Temperature, and Volume

Physical changes

don’t change the identity of the substance

Chemical Properties

Can NOT be measured without changing the identity of the substance

Chemical Changes

Change the identity of the substance — also called chemical reactions

Elements combining to form compounds is an example of a …

chemical change

A change that forms new compounds is…

a chemical change

Intensive properties

do not depend on the amount of matter in a sample

(I, do not depend)

Extensive properties

depend on how much matter a sample contains

Examples of Intensive Properties

Boiling point, concentration, temperature, luster

Examples of Extensive Properties

Entropy, Length, Weight, Volume

Units of measurement

quantities with accepted values that can be communicated between people

SI Units

The relationship between some common english and metric units

Mass

Kilograms (kg)

Length

Meters (m)

Time

Seconds (s)

Temperature

Kelvin (K)

Amount

Moles (mol)

Light Intensity

Candela (cd)

Electric Current

Ampere (A)

Volume

m³

Velocity

m/s

Density

kg/m³

tera-, T

10¹², 1,000,000,000,000

giga-, G

10⁹, 1,000,000,000

Mega -, M

10⁶,1,000,000

Kilo-, k

10³,1,000

Deci-, d

10^-1, 1/10

Centi-, c

10^-2,1/100

Milli-, m

10^-3,1/1,000

Micro-, μ

10^-6, 1/1,000,000

Nano-, n

10^-9, 1/1,000,000,000

Pico-, p

10^-12, 1/1,000,000,000,000

Boiling point of water

212 F, 100 C, 373 K

Freezing point of water

32 F, 0 C, 273 K

Absolute Zero

-460F, -273C, 0K

Equation for Fahrenheit

F= 9/5 C+32

Equation for Kelvins

K= C+ 273.15