Notes, summaries, assignments, exams, and problems for Chemistry

Halogenation

Halogenation: The reaction of an alkane with a halogen (X2 = F, Cl, Br, I) occurs when a mixture of the two is irradiated with ultraviolet light.

Combustion

Combustion: The reaction of an alkane with O2 occurs during combustion when the alkane is used as a fuel. Carbon dioxide and water are formed as products, and a large amount of heat is released.

An example of a combustion reaction:

CH4 + 2 O2 → CO2 + 2 H2O + Energy

Complete

Complete: C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) + Energy

Incomplete

Incomplete: C3H8 (g) + O2 (g) → H2O (g) + CO2 (g) + CO (g) + C (s) + Energy

Petroleum

Petroleum: Complex mixture of alkanes that can be separated into fractions by distillation. Separating molecules based on differences in boiling points is called... Continue reading "Halogenation, Combustion, Complete and Incomplete Reactions, Petroleum, Refining, Alkenes" »

Water Properties and Ocean Chemistry

Water's High Heat Capacity

21. Coastal Climate Moderation

Which property of water causes coastal communities to have only moderate differences in daily highs and lows when compared to inland communities?

Answer: A) High heat capacity.

22. Water's Heat Capacity Compared to Other Liquids

In comparison to most other liquids, the heat capacity of water is:

Answer: A) Higher than other liquids.

Seawater Composition and Buffering

23. Principle of Constant Proportions

The Principle of Constant Proportions states that:

Answer: D) The relative concentration of seawater ions does not change.

25. Seawater Buffer Ion

The ion in seawater that serves as a buffer is:

Answer: D) HCO3-.

Water Phase Changes

24. Temperature Change During

Metal Corrosion

Corrosion is the rusting of metal or alloy due to moisture and air. When it contacts air and water, a reaction forms a layer on the surface. For example, when an iron rod contacts air and moisture, it reacts and forms ferric oxide (Fe₂O₃) on its surface. It can be prevented by using alloys like stainless steel, brass, or bronze, painting the metal, applying oil, or coating with galvanized zinc.

Chemical Reactions

Some reactions happen very fast, like the precipitation of silver chloride, which occurs immediately after mixing aqueous solutions of silver nitrate and sodium chloride. Other reactions, like the rusting of iron in the presence of air and moisture, are very slow. Some reactions have a moderate rate.

The rate of a chemical... Continue reading "Metal Corrosion, Chemical Reactions, and Electrochemistry" »

Scalars and Vectors

What is a scalar? A scalar is a quantity that is fully described by a magnitude only. It is described by just a single number. Some examples of scalar quantities include speed, volume, mass, temperature, power, energy, and time.

What is a vector? A vector is a quantity that has both a magnitude and a direction. Vector quantities are important in the study of motion. Some examples of vector quantities include force, velocity, acceleration, displacement, and momentum.

Endothermic and Exothermic Reactions

An endothermic reaction takes place when energy is absorbed from the surroundings in the form of heat. An exothermic reaction is when energy is released from the system into the surroundings.

Endothermic reactions must be supplied... Continue reading "Scalars, Vectors, Endothermic & Exothermic Reactions Explained" »

Atomic Structure

Elements are a type of atom. Atoms are made up of protons, neutrons, and electrons. The nucleus is the center of an atom.

• Proton: +1 charge
• Electron: -1 charge
• Neutron: 0 charge (neutral)

Rutherford (1911) conducted the gold foil experiment.

Different elements have different numbers of protons in the nucleus.

• Atomic number (Z): Number of protons
• Mass number (A): Number of protons + Number of neutrons

Z

Chemical Symbol

A

Neutron number = Mass number - Atomic number

The number of neutrons can change (protons stay the same) in a given atom, making them isotopes.

Atomic mass is the total mass of elements and all its isotopes. U represents atomic mass units.

A radioactive isotope consists of nuclides whose nuclei undergo spontaneous decay.

Three

What is Surface Engineering?

Definition: It is the sub-discipline of material science which deals with the surface of solid matter.

Objectives: Involves altering the properties of the surface phase to reduce degradation over time, making it robust to the environment.

Applications: Automotive, aerospace, missile, power, electronic, biomedical, textile, petroleum, chemical, steel, power. Used in almost all types of materials.

Describe SEM and TEM

SEM: Scanning Electron Microscopy images the sample surface by scanning it with a high-energy beam of electrons. Advantages include 3D imaging and greater depth of focus. Disadvantages include low resolution and expensive equipment. Applications include gunshot residue analysis and firearms identification.... Continue reading "Surface Engineering and Microscopy Techniques in Material Science" »

Kinetic Theory of Matter

• Matter is made up of particles.
• These particles are constantly moving because they have kinetic energy.
• There are spaces between the particles.
• There are attractive forces between particles, and these become stronger as the particles move closer.
• All particles have energy. The temperature of a substance is a measure of the average kinetic energy of the particles.
• A change in phase may occur when the energy of the particles is changed.

Boyle's Law

The pressure of a fixed quantity of gas is inversely proportional to the volume it occupies, as long as the temperature remains constant. P₁ × V₁ = P₂ × V₂

Gay-Lussac's and Charles's Law

The volume of an enclosed sample of gas is directly proportional to its absolute temperature, provided... Continue reading "Matter: Kinetic Theory, Properties, and Classifications" »

Scientific models used to explain why and how atoms form molecules:

• Lewis dot structure
• Valence bond theory

Valence bond theory describes a covalent bond as the overlap of half-filled atomic orbitals (each containing a single electron) that yield a pair of electrons shared between the two bonded atoms. According to valence bond theory, a covalent bond results when two conditions are met: (1) an orbital on one atom overlaps an orbital on a second atom and (2) the single electrons in each orbital combine to form an electron pair.

• Molecular orbital theory

model that describes the behavior of electrons delocalized throughout a molecule in terms of the combination of atomic wave functions. It describes the distribution of electrons in molecules in much... Continue reading "Atomic Models, Periodic Trends, and Chemical Bonding" »

IONIC: thet are solids at room temperatures and have medium to high meltin and boiling points. Ionic bond is strong because it is electrostatic. They are very hard. It is not eassy to scratch an ionic compound. They are fragile. Hitting them forces ions with the same signs together, and they repel and break the crystal. Most disolve well in water, water molecules may surround the ions,weakening their bonds and separating them from the crystal lattice. This is called solvation. They do not conduct electricity well in solid state but hey do in solution or liquid state. SODIUM CHLORIDE

Mixing and Measuring

Agitator

An agitator is a machine used for mixing liquids, typically with an electromagnet.

Beaker

A beaker is a cylindrical container made of glass that is very commonly used in the laboratory, mainly to prepare or heat substances.

Burette

A burette is used for decantation and for transferring and dispensing liquids or fluids.

Graduated Cylinder

A graduated cylinder is used to measure volumes of liquids.

Micropipettes

Micropipettes are used to measure and extract very small amounts of liquids from a solution.

Pipette

A pipette is used to accurately measure volumes of liquids.

Volumetric Flask

A volumetric flask is used to prepare solutions and to know the volume.

Heating and Support

Bunsen Burner

A Bunsen burner is used to heat chemical... Continue reading "Essential Lab Equipment: Uses and Functions" »