Introduction to Science and Its Divisions

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Questions and Answers

What is the correct representation of valence electrons in the Lewis dot formula?

Using the element symbol with dots for each valence electron (correct)

Using a series of numbers next to the element symbol

Using the element symbol and circles around it

Using brackets around the element symbol

Which quantum number describes the shape of an electron's orbital?

Magnetic quantum number (m)

Principal Quantum number (n)

Secondary or azimuthal quantum number (l) (correct)

Magnetic spin quantum number (s)

What is the outcome of a loss of electrons from an atom?

The atom becomes a cation (correct)

The atom becomes an anion

The atom becomes neutral

The atom gains protons

Which method represents the expected distribution of electrons in energy levels?

Spectronic or spdf notation Signup and view all the answers

What is the range of values for the magnetic quantum number (m) when n = 2?

-1, 0, +1 Signup and view all the answers

According to the octet rule, how many valence electrons should an atom ideally have?

8 Signup and view all the answers

In orbital diagrams, what does a box or line represent?

An orbital Signup and view all the answers

What does the principal quantum number (n) indicate?

The number of electron clouds or shells Signup and view all the answers

Which principle states that no more than two electrons can occupy a single orbital?

Pauli's Exclusion Principle Signup and view all the answers

What does the Aufbau Principle dictate regarding the filling of electron orbitals?

Electrons fill the lowest energy levels before moving to the next level. Signup and view all the answers

What defines isotopes of an element?

Same number of protons and different numbers of neutrons. Signup and view all the answers

What is the maximum number of electrons that can occupy a single p orbital?

2 Signup and view all the answers

Which unit is used to express mass on an atomic scale?

Atomic mass unit (amu) Signup and view all the answers

Which of the following describes the probability of finding an electron in an orbital?

It is greatest at specific regions of space around the nucleus. Signup and view all the answers

If an electron transitions from a higher energy level to a lower energy level, what must occur?

The electron loses energy. Signup and view all the answers

Which of the following statements about electron configurations is correct?

Electrons fill orbitals according to increasing energy levels. Signup and view all the answers

According to Dalton's Atomic Theory, what can be said about atoms of the same element?

They have the same chemical properties. Signup and view all the answers

What is a defining characteristic of a molecule?

It acts as a single unit. Signup and view all the answers

Which principle is associated with the Law of Conservation of Mass?

The total mass before and after a reaction remains the same. Signup and view all the answers

What was one of Niels Bohr's contributions to atomic theory?

Formulated the planetary model of an atom. Signup and view all the answers

Which concept did Louis de Broglie introduce regarding electrons?

Electrons possess both wave and particle properties. Signup and view all the answers

The Law of Constant Composition states that:

Any compound is made up of elements in the same proportion by mass. Signup and view all the answers

Which scientists contributed to the development of the wave-mechanical model of the atom?

Werner Heisenberg, Louis de Broglie, and Erwin Schrodinger Signup and view all the answers

What role does quantum mechanics play in modern atomic theories?

It provides a framework for understanding the behavior of subatomic particles. Signup and view all the answers

Study Notes

Science

Science is the study of accumulated and accepted knowledge, systematized and formulated as a basis for discovering general truths.
Derived from the Latin word "scire," meaning to know or knowledge.
Chemistry plays a crucial role in many aspects of public concern, offering advantages like improved healthcare, resource conservation, environmental protection, and advancements in food, clothing, and shelter.
Disadvantages include some chemicals potentially harming health

Division of Science

Social Sciences: Study of human behavior. Includes Anthropology (study of man and culture), Economics (allocation of resources), and Sociology (origin and structure of society).
Natural Sciences: Study of natural objects and phenomena. Subdivided into Physical and Biological Sciences.

Physical Sciences

Astronomy: Study of celestial bodies
Chemistry: Study of the structure, properties, and composition of substances, and their transformations.
Geology: Study of Earth.
Mathematics: Study of quantities.

Biological Sciences

Microbiology: Study of microorganisms.
Botany: Study of plants.
Zoology: Study of animals.

Chemistry

Is the study of matter, its properties, and changes.
Aims to distinguish different kinds of matter, separate substances, influence changes in matter, and determine the energy involved.

Analytical Chemistry

Qualitative Analysis: Identification of the elements or compounds present in a sample.
Quantitative Analysis: Determination of the ratios and percentages of elements or compounds in a sample.

Matter

Anything that occupies space and has mass
Pure Substances: Fixed composition. Cannot be further purified. Classified as:
- Elements: Cannot be subdivided by chemical or physical means.
- Compounds: Elements united in fixed ratios.
Mixtures: Combination of two or more pure substances. Classified as: Homogeneous: Uniform composition throughout. Heterogeneous: Non-uniform composition.

Intensive and Extensive Properties

Intensive Property: Independent of the quantity of the substance (e.g., density, specific gravity).
Extensive Property: Depends on the quantity of the substance (e.g., mass, volume).

Classification of Matter

Elements: Substances composed of only one type of atom (e.g., carbon, hydrogen).
Compounds: Substances composed of two or more different types of atoms chemically bonded in a fixed ratio (e.g., water).
Mixtures: Combinations of elements or compounds not chemically bonded and not in a fixed ratio. Classified as homogenous or heterogeneous, meaning their properties are uniform or vary from place to place

Atoms, Molecules, and Atomic Structure

Atoms: The fundamental units of elements comprised of a nucleus and electrons orbiting the nucleus. The nucleus contains protons and neutrons.
Molecules: Tightly-bound combinations of two or more atoms that act as a single unit.
Atomic Models: Models illustrating the structure of atoms, such as the plum pudding model and the Bohr model (planetary model). Also, including the Wave Mechanical Model based on quantum mechanics.
Atomic number: Number of protons
Mass Number: Sum of protons and neutrons
Isotopes: Atoms of the same element with different numbers of neutrons, thus different masses.

Electron Configuration

Electronic configuration: Arrangement of electrons in energy levels, orbitals, and subshells surrounding the atom's nucleus..

Periodic Table

Elements are arranged in order of increasing atomic number.
Elements with similar chemical properties are grouped together in vertical columns (groups or families).
Horizontal rows are called periods. A families are representative elements. B families are called transition elements. 10-member sequences related to stepwise addition of electrons to d orbitals.
Elements are also categorized as metals, nonmetals, and metalloids based on their properties.

Chemical Bonding

Ionic bonding: Transfer of electrons between atoms creating ions that attract. The strong attraction between oppositely charged ions forms a crystal.
- An ion is an atom that has lost or gained electrons; when it loses electrons it becomes a cation; when it gains electrons it becomes an anion.
Covalent bonding: Sharing of electrons between atoms. Polar covalent bonds share electrons unequally, non-polar share them equally.
Metallic bonding: Sharing of electrons by many atoms in a sea of delocalized electrons, allowing metals to conduct heat and electricity.

Intermolecular Forces

London Dispersion Forces: Weak, temporary forces of attraction occurring between any two molecules.
Dipole-Dipole Forces: Permanent forces of attraction between polar molecules, caused by the attraction between partial positive and negative charges.
Hydrogen Bonds: Strong dipole-dipole interactions that result from attraction between hydrogen of one molecule and a highly electronegative atom (N, O, or F) in another molecule.

Chemical Reactions

Reactants: Substances undergoing a chemical change.
Products: Substances produced by a chemical change.
Chemical equations: Representation of chemical reactions using chemical symbols and formulas.
Balancing Chemical Equations: Ensuring the law of conservation of mass holds true by adjusting coefficients in front of formulas.
Typical Types of Chemical Reactions: - Combination/Composition Reactions - Decomposition Reactions - Single Replacement Reactions - Double Replacement Reactions

Oxidation-reduction (Redox) Reactions

Oxidation: Loss of electrons/increase in oxidation number.
Reduction: Gain of electrons/decrease in oxidation number.
Oxidation numbers: Arbitrary values assigned to elements in compounds to indicate their oxidation state during a reaction..

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Description

Explore the vast field of science, covering its definition, divisions, and the critical roles of chemistry and other physical sciences. Delve into the social sciences, such as anthropology, economics, and sociology, as well as the basic principles of natural sciences. This quiz will test your understanding of these fundamental concepts.