Chemistry

Chemistry

The study of matter, its composition, properties, and changes.

States of Matter

Solid, Liquid, Gas, Plasma.

water

the most common element to change state of matter

Disciplines of Chemistry:

Physical, Organic, Inorganic, Analytical, Biochemistry,

Physical Chemistry

Studies macroscopic and atomic properties, energy transfers, and molecular structures.

Organic Chemistry

Focuses on carbon-containing chemicals, abundant in living organisms.

Inorganic Chemistry

Studies non-carbon-based chemicals, materials design, and properties.

Analytical Chemistry

Study of composition of matter, identifies, and quantifies chemicals in samples.

Uses complex instruments to analyze an unknown material to determine its components

Biochemistry

Examines chemical processes in living organisms, from cellular functions to disease mechanisms.

History of Chemistry

Evolution from practical uses to theoretical advancements, including early chemists' achievements and the development of chemical theories.

Soaps and Perfumes

Most common products in early chemistry

19th Century

When theories were developed

Robert Boyle (1637 - 1691)

Put chemistry on a solid foundation.

Developed basic ideas about behaviour of gases: could describe gases mathematically: helped form the idea that small particles could form molecules

Boyle’s Law

pressure of gas increases as volume decreases

John Dalton (1766 - 1844)

Developed Dalton Atomic Theory (1807)

Dalton Atomic Theory (1807)

All matter is composed of atoms

Atoms at a given element are identical whereas atoms of a different element are different

Atoms cannot be subdivided, created, or destroyed.

Joseph Priestley (1733 - 1804)

Isolated and characterised several gases: Oxygen, Carbon Dioxide, Nitrogen Oxide (laughing gas)

Laughing gas

first used for this purpose in 1844 during a tooth extraction

Carl Wilhelm Scheele or “C.W. Scheele” (1742 - 1786)

Discovered Chlorine

Antoine Lavoisier (1743 - 1794)

Father of Chemistry

Discovered Nitrogen and the role of Oxygen in combustion

Formulated the law of conservation of matter/mass

Amadeo Avogadro (1776 - 1856)

Laid the groundwork for a more quantitative approach to chemistry by calculating the number of particles in a given amount of gas

Allowed scientists to think of chemistry systematically

Alessandro Volta (1745 - 1827)

Most notable invention is batteries

Also invented voltage and discovered methane

Invented/began the field of electrochemistry

Humphry Davy (1778 - 1829)

Discovered sodium, potassium, calcium, and barium

Invented the Davy lamp

Michael Faraday (1791 - 1867)

Father of Electricity

Volta, Davy, and Faraday

all made significant contributions to electrochemistry

Charles Goodyear (1800 - 1860)

Discovered the process of vulcanization.

Louis Pasteur (1822 - 1895)

Made Pasteurization

Pasteurization:

the use of heat sterilisation to eliminate unwanted microorganisms in wine and milk.

Alfred Nobel (1833 - 1896)

Invented dynamite.

The fortune he made from his product was used to fund the nobel prizes in science and the humanities.

J.W. Hyatt (1837 - 1920)

Developed the first plastics.

Leo Baekeland (1863 - 1944)

Developed the first synthetic resin (widely used for inexpensive and sturdy dinnerware)

Crops need three things to grow:

Water

Nutrients from the Soil

Protection from Predators

Water Purification 

Uses chemical and physical techniques to remove salts and contaminants that would pollute the soil.

Chemistry and the Environment

Scientists used to dump waste in bodies of water/land: However, due to its harmful effects dumping was outlawed. 

“Lead”

a substance once commonly used in gasoline, paint, and plumbing: Now banned due to its link to brain damage and cancer.

Though it is still used in car batteries that are safely recycled and processed

Chemists’ role in the environment

By analyzing the presence of harmful substances and study how these affect human and environmental health

Major Impacts of Chemistry (10)

1. Anaesthetics : First anaesthetics discovered (mid - 1800’s)

2. Antibiotics:  Discovered by Alexander Flemming - Discovered in the 1930’s

3. Batteries:  Helped progress I.T.

4. Birth Control: Became available (1960’s)

5. Catalytic Converters: Developed 1960’s - 70’s (Converts toxic gases to less harmful emissions)

6. Fertilizers : Vital for growing food

7. Fuels: 

8. Plastics: Used in day-to-day life

9. Screens: Different types of screens need materials developed by chemists

10. Water Treatment: Water chlorination started 1900’s - Prevents diseases from spreading

The development of new materials

Includes everything from stronger and lighter materials for use in construction to new materials for use in electronics and medicine (ex. Nickel-carbon-sulfur alloy)

The development of new medicines

Chemists work to understand how diseases work then develop drugs for cures (ex. Alzheimer’s disease treatment)

The understanding of environmental issues

By studying the impact of pollution on the environment and how to clean up pollution as well as developing sustainable energy resources

MATTER

Anything that has mass and volume. Includes atoms and anything made up of atoms, but not other energy phenomena or waves like light or sound.

a physical substance of which systems may be composed.

Macroscopic

Objects/phenomena are large enough to be visible practically with the naked eye, without magnifying optical instruments.

Microscopic

Objects and events are smaller than those that can easily be seen by the naked eye, requiring a lens or microscope to see them clearly.

Atoms

Make up everyday objects, consisting of interacting subatomic particles like protons and neutrons.

Tiny building blocks of matter.

liquid oxygen

(gas compressed such that it turned liquid)

Mass

the measure of the amount of matter in something. not a substance but a quantitative property of matter and other substances or systems.

Air (and all other gases)

invisible to the eye, have very small masses compared to equal volumes of solids and liquids, and are quite easy to compress (change volume).

mass of air

approximately 0.0002 pounds or 0.09 grams

Intermolecular Forces (IMF)

Force that causes molecules to move together

MOLECULES

The most important method that nature uses to organize atoms into matter are groups of two or more atoms that have been bonded together.

It has its own set of chemical properties, and it’s these properties with which chemists are most concerned

Physical States of Matter

• State that a given substance exhibits is also a physical property

• The physical state of everything depends on the temperature 

• All substances can be any state of matter

Solid

• Definite volume and shape

• Tightly packed; Particles vibrate around fixed axes

• Its molecules have fixed positions because there is not enough thermal energy to overcome the IMF interaction between the particles

Liquid

• Definite volume no definite shape

• Relatively dense or slightly loose

• Partially overcomes IMF but their particles are still in close contact

• Free to move over each other yet still attracted to each other

Gas

• Neither definite volume or shape

• Extremely far apart

• Completely overcomes IMF so its particles move in random motion with little to no interaction with each other

• Highly compressible

“crystal”

Constituent particles arranged in a regular, three-dimensional array

“Amorphous” (without form)

Some solids cannot organize their particles in such regular crystals

Mercury

• An anomaly, it is the only metal we know that is liquid at room temperature.

• (has a 357c boiling point)

Change from Liquid to Gas 

significantly increases the volume of a substance, by a factor of 1000 or more.

Plasma

• Also a state of matter yet rarely happens naturally on earth

Pure Substance

A form of matter with a constant composition and constant properties throughout the sample.

• Has a fixed chemical composition and distinct properties

• Is the same everywhere

• Can only be separated through chemical methods and rarely physical

Element

Fundamental substances that cannot be separated into simpler substances by chemical methods (ex. Aluminum)

Compound

• A substance composed of 2 or more elements in fixed proportions

• Can be separated into simpler substances only by chemical methods.

• A molecule made of atoms from different elements.

• (ex. Water, Sodium Chloride, Carbon Dioxide)

Mixture

• Matter consisting of two or more pure substances that retain their individual identities and could be separated by physical methods

Homogeneous (solution)

• Mixture that has a uniform composition and properties throughout

• Is composed of a single phase

• (ex. Coffee, Wine, Air, Saltwater)

Heterogeneous

• A mixture that is not uniform in composition and properties throughout

• Is composed of two or more phases

• (ex. Vegetable soup)

Phase

• Is any part of a sample that has a uniform composition and properties.

More than one phase

Does not mix into a uniform composition. (ex: oil and water)