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General and Inorganic Chemistry: Matter, Properties, Atomic Models, and Chemical Bonding, Study notes of Psychology

A comprehensive overview of fundamental concepts in general and inorganic chemistry, covering topics such as matter and its properties, atomic models, chemical bonding, and chemical reactions. It explores the nature of matter, its states, and the properties that define it. The document delves into the evolution of atomic models, from dalton's billiard ball model to the modern quantum mechanical model. It explains the concept of chemical bonding, including ionic and covalent bonds, and provides examples of chemical formulas and equations. The document also discusses the concept of solutions and their properties, including solubility, saturation, and supersaturation. It concludes with a brief overview of chemical reactions and the importance of balancing chemical equations.

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2023/2024

Available from 12/07/2024

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GENERAL AND INORGANIC CHEMISTRY
CHAPTER 1 | INTRODUCTION TO CHEMISTRY
1.1 CHEMISTRY AND ITS IMPORTANCE
- chemistry has enabled us to
design all kinds of materials
such as metals, glass and
plastics, which are widely used
in our life.
- Using the knowledge of
chemistry, we have created
many useful processes. Even
the water that we drink would
not be safe without chemical
treatment.
HISTORY OF CHEMISTRY
- Chemistry already existed since
ancient times. Humans had
already known how to extract
metals such as copper and iron,
and how to make ceramics and
glasses. However, they did not
know the chemical processes
involved.
- The systematic study of
chemistry as a subject only
began about 1700 years ago. It
revolved around alchemy, an art
of transforming common metals
such as lead into precious
metals, such as gold or silver.
Even though no one ever
succeeded in doing so, a
number of important chemical
processes such as distillation
were discovered
- alchemy refers to both an early
form of the investigation of
nature and an early
philosophical and spiritual
discipline, both combining
elements of chemistry,
metallurgy
- In fact, the word `chemistry' is
believed to originate from
`al-kimiya', the Arabic word for
alchemy.
- Modern chemistry began to be
founded during the 17th century.
The works of scientists of that
time laid the foundation for
today's chemistry
(a) ANTOINE LAVOISIER
- a French chemist, is considered
the founder of modern
chemistry. He did many
experiments on combustion and
the composition of water.
(b) ROBERT BOYLE
- an English philosopher, is also
considered as one of the
founders of modern chemistry.
He separated chemistry from
alchemy and introduced
experimental methods and the
idea that elements are the basic
building blocks of matter.
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CHAPTER 1 | INTRODUCTION TO CHEMISTRY

1.1 CHEMISTRY AND ITS IMPORTANCE

  • chemistry has enabled us to design all kinds of materials such as metals, glass and plastics, which are widely used in our life.
  • Using the knowledge of chemistry, we have created many useful processes. Even the water that we drink would not be safe without chemical treatment. HISTORY OF CHEMISTRY
  • Chemistry already existed since ancient times. Humans had already known how to extract metals such as copper and iron, and how to make ceramics and glasses. However, they did not know the chemical processes involved.
  • The systematic study of chemistry as a subject only began about 1700 years ago. It revolved around alchemy, an art of transforming common metals such as lead into precious metals, such as gold or silver. Even though no one ever succeeded in doing so, a number of important chemical processes such as distillation were discovered
  • alchemy refers to both an early form of the investigation of nature and an early philosophical and spiritual discipline, both combining elements of chemistry, metallurgy
  • In fact, the word chemistry' is believed to originate fromal-kimiya', the Arabic word for alchemy.
  • Modern chemistry began to be founded during the 17th century. The works of scientists of that time laid the foundation for today's chemistry (a) ANTOINE LAVOISIER
  • a French chemist, is considered the founder of modern chemistry. He did many experiments on combustion and the composition of water. (b) ROBERT BOYLE
  • an English philosopher, is also considered as one of the founders of modern chemistry. He separated chemistry from alchemy and introduced experimental methods and the idea that elements are the basic building blocks of matter. NAV | 0

INTRODUCTION TO CHEMISTRY

  • Boyle (Irish: Robaird Ó Bhaoill) ( 25 January 1627 – 30 December 1691 ) was an Irish natural philosopher, chemist, physicist, inventor , and early gentleman scientist, noted for his work in physics and chemistry. He is best known for the formulation of Boyle's law. Although his research and personal philosophy clearly has its roots in the alchemical tradition, he is largely regarded today as the first modern chemist, and therefore one of the founders of modern chemistry. Among his works, The Sceptical Chymist is seen as a cornerstone book in the field of chemistry
  • Now, chemistry is acknowledged as a branch of science that deals with matter. MEANING OF CHEMISTRY
  • Chemistry is the study of the composition structure, properties and inter matter - In chemistry, all matter is considered chemical. Thus, chemicals are not only found in bottles in laboratories, but also in common substances such as air, water, soil and metals - We use chemicals in almost every part of our life. Here are some examples. (a) Sodium chloride is the salt that we use in cooking. (b) Vinegar is a dilute solution acid (acetic acid). It is widely used in preserving food. (c) Calcium carbonate in the marble tiles is widely used in furniture and flooring. (d) Lime or calcium oxide is used in the preparation of cement and mortar. (e) Silicon chips are used in a wide range of electronic devices such as computer, televisions and mobile phones (f) Pure copper is made into wire due to its extremely high electrical conductivity. - In chemistry, we study what these chemicals are made of, what are their properties, how they interact among each other and how to use this knowledge to produce useful new chemicals. CHEMISTRY RELATED CAREERS
  1. CHEMISTS are found in nearly all industries - food, textiles, detergents, paints, water treatment and others. They are not only doing analysis work but also in research and

INTRODUCTION TO CHEMISTRY

Detergent industry Detergents and fabric softeners industry

  • Some of the chemicals produced are directly used by local consumers in their daily lives. The products have helped them to improve their health and standard of living.
  • Others are exported overseas, thus earning foreign exchange for the country.
  • Some chemical-based industries support other industries in the country. For example, the production of rubber, steel and plastics support our national automobile industry.
  • Thus, chemical-based industries contribute greatly to our economy. On top of that, they also provide jobs to millions of people. 1.2 SCIENTIFIC METHOD
  1. As in all other fields of science, knowledge of chemistry is gathered through a systematic method used by scientists in their investigations.
  2. Generally, the scientific method starts with careful observations on a situation. Based on the observations, an inference is made.
  3. An inference is just a smart guess. To verify it, a hypothesis is formulated and tested through a carefully planned and controlled procedure called an experiment. 4. The following shows the steps involved in the scientific method. ➢ MAKING AN OBSERVATION - Gathering information about a phenomenon using our five senses, namely sight, hearing, smell, taste and touch. ➢ MAKING AN INFERENCE - Making a smart guess or a tentative explanation about the phenomenon based on the observation ➢ IDENTIFYING THE PROBLEM - Asking a question based on the inference made ➢ MAKING A HYPOTHESIS - Making a general statement about the relationship between a manipulated variable and a responding variable to explain the question asked. ➢ IDENTIFYING THE VARIABLES - A variable is a factor that affects the results of an experiment. ➢ MANIPULATED VARIABLE - the factor that is purposely changed in an experiment. ➢ RESPONDING VARIABLE - the factor that changes with the manipulated variable.

INTRODUCTION TO CHEMISTRY

➢ CONTROLLED VARIABLES

  • the factors that are kept constant throughout an experiment. ➢ CONTROLLING THE VARIABLES
  • Deciding how to manipulate the chosen variable, what to measure and how to keep the controlled variables constant. - PLANNING AN EXPERIMENT
    • Determining the list of materials and apparatus, the exact procedure of the experiment, the method of collecting data and ways to analyze and interpret the collected data. - COLLECTING DATA
    • Making observations or measurements and then recording them systematically. - INTERPRETING THE DATA
    • Organizing and analyzing data. Calculations, graphs or charts are usually drawn to look for any relationship between the variables.

- MAKING A CONCLUSION

  • Making a statement about the outcome of the experiment and whether the hypothesis is accepted or rejected. - WRITING A REPORT
  • Communicating the details of the experiment.
  1. Scientific attitudes and noble values should be inculcated in all chemistry investigations. For example: (a) An experiment is planned and carried out systematically and diligently. (b) All observations and collection of data must be done honestly and objectively. (c) Interpretation of data, inferences and conclusions are made with rational, critical and analytical thinking.

MATTER AND ITS PROPERTIES

STRUCTURE OF LIQUID

  • Liquid , another state of matter, has indefinite shape and definite volume.
  • Molecules will flow or glide over one another, but stay toward the bottom of the container.
  • Motion is a bit more random than that of a solid. STRUCTURE OF GAS
  • Gas , state of matter, has indefinite shape and volume.
  • A gas flows and takes the shape and fills the entire volume of its container.
  • The kinetic energy of the molecule is greater than the attractive force between them, thus they are much farther apart and move freely of each other. PROPERTIES OF SOLID, LIQUID, and GAS PHASE TRANSITION
  • A physical change where the substance undergoes changes without changing its chemical composition.

MATTER AND ITS PROPERTIES

PHYSICAL AND CHEMICAL

PROPERTIES OF MATTER

PROPERTIES OF MATTER

  • Properties are characteristics of matter that describe or distinguish them from one another.
  • Physical vs. Chemical
  • Extensive (extrinsic) vs. Intensive (intrinsic) PHYSICAL PROPERTIES
  • Characteristics of a material that can be observed without carrying out a chemical reaction on it.
  • Perceived by the senses and are generally measurable. CHEMICAL PROPERTIES
  • Described the ability of matter to be transformed into other materials different from the original composition and structure

PHYSICAL & CHEMICAL PROPERTIES

INTENSIVE AND EXTENSIVE

PROPERTIES

➢ INTENSIVE PROPERTIES

  • are substances that do not depend on the amount of the substance. - density, color,luster, malleability, conductivity, hardness, melting point,freezing point, boiling pointEXTENSIVE PROPERTIES
  • are properties that do depend on the amount of substance of the material. - weight, volume, length, mass **CLASSIFICATION OF MATTER
  • MIXTURES**
    • two or more substances that are not chemically combined with each other and can be separated by physical means. The substances in a mixture retain their individual properties. Physical Propertie s Color, odor, taste, texture, shape, density, melting and boiling points, solubility Chemical Propertie s Flammability, toxicity, reactivity to water and oxygen like rusting, heat combustion, pH, enthalpy of formation, oxidation states, chemical stability, types of chemical bonds that matter can form

MATTER AND ITS PROPERTIES

MIXTURE

  • two or more pure substances (elements or compounds) that are mixed together but NOT joined chemically
  • NOT a pure substance - examples: the air we breath, gasoline for cars, the sidewalk on which we walk
  • Uniform in composition and appearance
  • Same proportion of components throughout
  • Consists of two or more substances in the same phase
  • Also called SOLUTIONS HETEROGENEOUS MIXTURES
  • Variable appearance and composition

PURE SUBSTANCE

ELEMENTS COMPOUNDS

Elements are the simplest pure substances. Examples: •O-Oxygen •H- Hydrogen •Na- Sodium •C- Carbon •Fe- Iron •Pb- Lead The smallest particle of an element that has the properties of that element is an atom. Compounds are pure substances that are made of more than one element bound together. Examples: •H2O and CO A molecule is formed when two or more atoms chemically combine.

MATTER AND ITS PROPERTIES

MIXTURES

2 TYPES OF MIXTURE

- HETEROGENEOUS

MIXTURES

  • All components of the mixture are visible because they do not mix together
  • Particles not distributed evenly - ex: trail mix, vegetable soup, oil and water - HOMOGENEOUS MIXTURES
  • Components cannot be distinguished from each other, appear as one substance
  • Particles distributed evenly throughout - ex: air, salt water, 10 karat gold - Extras:
  • Homogeneous mixtures are also called solutions.
  • Separate particles are not visible because one dissolves in the other = dissolution
  • In salt water,
  • salt is the solute , gets dissolved
  • water is the solvent , dissolves other substance SOLUBILITY
  • Because different amounts of solute can be dissolved in a solvent, we look at a solution’s SOLUBILITY.
  • The maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature.
  • Usually expressed as the number of grams of solute per 100mL of solvent.
  • Every chemical substance which dissolves in water has a fixed solubility. - If it does not dissolve, solubility = zero.
  • Many of these solubilities have been measured and special charts are produced displaying solubility of many substances at once. HETEROGENOUS MIXTURES

HOMOGENOUS

MIXTURES

All components of the mixture are visible because they do not mix together Particles not distributed evenly EX: sand and water, vegetable soup, oil and water Homogeneous mixtures Components cannot be distinguished from each other, appear as one substance Particles distributed evenly throughout EX: air, salt water, 10 karat gold *SOLUTIONS

SEPARATING MIXTURES

ATOMIC MODELS

ATOMIC MODELS

  • This model of the atom may look familiar to you. This is the Bohr model. In this model, the nucleus is orbited by electrons, which are in different energy levels.
  • A model uses familiar ideas to explain unfamiliar facts observed in nature.
  • A model can be changed as new information is collected.
  • The atomic model has changed throughout the centuries, starting in 400 BC, when it looked like a billiard ball DEMOCRITUS (400 BC)
  • This is the Greek philosopher Democritus who began the search for a description of matter more than 2400 years ago.
  • He asked: Could matter be divided into smaller and smaller pieces forever, or was there a limit to the number of times a piece of matter could be divided?

ATOMOS

  • His theory: Matter could not be divided into smaller and smaller pieces forever, eventually the smallest possible piece would be obtained.
  • This piece would be indivisible.
  • He named the smallest piece of matter “atomos,” meaning “not to be cut.”
  • To Democritus, atoms were small, hard particles that were all made of the same material but were different shapes and sizes.
  • Atoms were infinite in number, always moving and capable of joining together. ARISTOTLE & PLATO
  • Aristotle and Plato favored the earth, fire, air and water approach to the nature of matter. Their ideas held sway because of their eminence as philosophers. The atomos idea was buried for approximately 2000 years. **- Aristotle’s Four (Plus One) Elements
  • Aristotle’s (384-322 BC)** natural philosophy elaborated in different works (On the Heavens, Physics, Metaphysics) sustains, that:

ATOMIC MODELS

  • Atoms of the same element can have different numbers of neutrons.
  • Thus, different mass numbers.
  • These are called isotopes. FREDERICK SODDY (1877-1956)
  • He proposed the idea of isotopes in 1912 (note this was close to 30 years after Dalton’s original idea)
  • Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons.
  • Soddy won the Nobel Prize in Chemistry in 1921 for his work with isotopes and radioactive materials. THE “BILLIARD BALL” MODEL
  • proposed by John Dalton in 1804
  • this theory proposed that matter was composed of small, spherical particles but evidence was later gathered that matter was composed of even smaller bits
  • during the 1900s evidence was discovered regarding charges:
  • atoms have positive (Rutherford’s contribution) and negative (Thomson’s contribution) parts
  • charges interact:
  • as a result, revisions to Dalton’s model had to be made J.J THOMSON’S PLUM PUDDING MODEL
  • In 1897, the English scientist Sir Joseph John Thomson ( December 1856 – 30 August
  1. provided the first hint that an atom is made of even smaller particles.
  • Thomson: “Plum Pudding” or “Chocolate Chip Cookie” Model
  • using available data on the atom, J.J. Thomson came up with the idea of having charges embedded with Dalton’s Billiard Balls

ATOMIC MODELS

  • Also used cathode ray experiment to discover the existence of the electron
  • Note: this model kept Dalton’s key ideas intact
  • Thomson Model
  • Thomson studied the passage of an electric current through a gas.
  • As the current passed through the gas, it gave off rays of negatively charged particles.
  • Thomson concluded that the negative charges came from within the atom.
  • A particle smaller than an atom had to exist.
  • The atom was divisible!
  • Thomson called the negatively charged “corpuscles,” today known as electrons.
  • Since the gas was known to be neutral, having no charge, he reasoned that there must be positively charged particles in the atom.
  • But he could never find them.

ROBERT MILLIKAN

  • Mass of the Electron
  • Robert Millikan (March 22, 1868
    • December 19, 1953) determined the mass of the electron: 1/1840 the mass of a hydrogen atom; it has one unit of negative charge. Mass of the electron is 9.11 x 10-28 g - The oil drop apparatus RUTHERFORD’S GOLD FOIL EXPERIMENT
  • In 1908, the English physicist Ernest Rutherford (30 August 1871 – 19 October 1937) was hard at work on an experiment that seemed to have little to do with unraveling the mysteries of the atomic structure.

ATOMIC MODELS

Rutherford reasoned that all of an atom’s positively charged particles were contained in the nucleus. The negatively charged particles were scattered outside the nucleus around the atom’s edge. BOHR’S MODEL

  • In 1913, the Danish scientist Niels Henrik David Bohr ( October 1885 – 18 November
    1. proposed an improvement. In his model, he placed each electron in a specific energy level.
  • According to Bohr’s atomic model, electrons move in definite orbits around the nucleus, much like planets circle the sun. These orbits, or energy levels, are located at certain distances from the nucleus. - Niels Bohr
  • Discovered that electrons exist in several distinct layers or levels
  • “Jimmy Neutron Model”
  • Travel around nucleus like planets travel around sun
  • Electrons Orbit
  • Electrons can jump between levels with energy being added/released - Bohr’s Model - Niels Bohr proposed that electrons revolve around the central positive nucleus (like planets in the solar system) - Niels Bohr also suggested that the electrons can only revolve in certain orbits, or at certain energy levels (i.e., the energy levels are quantized) WERNER HEISENBERG & ERWIN SCHRODINGER
  • Found that Electrons live in fuzzy regions or “clouds” not distinct orbits
  • Improved on Bohr’s findings
  • Electron location can not be predicted
  • Quantum Mechanical Model

ATOMIC MODELS

QUANTUM MECHANICAL MODEL

  • the current understanding of the atom is based on Quantum Mechanics
  • this model sees the electrons not as individual particles, but as behaving like a cloud - the electron can be “anywhere” in a certain energy level
  • Remember back to CPE with electrons behaving like bees in a beehive THE WAVE MODEL Today’s atomic model is based on the principles of wave mechanics.
  • According to the theory of wave mechanics, electrons do not move about an atom in a definite path, like the planets around the sun.
  • In fact, it is impossible to determine the exact location of an electron. The probable location of an electron is based on how much energy the electron has. - According to the modern atomic model, an atom has a small positively charged nucleus surrounded by a large region in which there are enough electrons to make an atom neutral. ● ELECTRON CLOUD: - A space in which electrons are likely to be found. - Electrons whirl about the nucleus billions of times in one second - They are not moving around in random patterns. - Location of electrons depends upon how much energy the electron has. - Depending on their energy they are locked into a certain area in the cloud. - Electrons with the lowest energy are found in the energy level closest to the nucleus - Electrons with the highest energy are found in the outermost energy levels, farther from the nucleus.